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.ppt for ionic bonds and metallic bonds. Chapter 7.
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1
Ionic Bonding and Ionic Compounds
Or How I Learned to Love Electrostatic Forces
2
Ionic Bonds
The periodic table is based upon the properties of the elements After the discovery of the electron scientists found that all elements in the same group have the same number of valence electrons
Valence electrons are the electrons in the highest occupied energy level of an elementrsquos atoms
The number of valence electrons determines the chemical properties of an element
The number of valence electrons is related to the group numbers in the periodic table
3
The elements in Group 1A (hydrogen lithium etc) all have one valence electron
H 1s1 Na 1s22s22p63s1
Li 1s22s1 K 1s22s22p63s23p64s1
Carbon and silicon in Group 4A have four valence electrons
C 1s22s22p2
Si 1s22s22p63s23p2
Groups 5A has five (5) valence electrons and Group 6A has six (6) valence electrons etc
4
Valence electrons are usually the only electrons used in the formation of chemical bonds A shorthand way of showing valence electrons is through electron dot structures
Electron dot structures show valence electrons as dots The inner electrons are represented by the symbol for the element being considered
P188
5
Formation of Cations amp AnionsAs we have talked about before noble gases are quite unreactive This is because they have filled outer energy levels
Atoms form ions amp molecules for this reason they want filled outer energy levels
As such they follow a rule called the octet rule
The octet rule states that atoms in compounds tend to have the stable electron configuration of a noble gas
Na -- 1s22s22p63s1 Namiddot
Na+ -- 1s22s22p6 Na+ octet
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
2
Ionic Bonds
The periodic table is based upon the properties of the elements After the discovery of the electron scientists found that all elements in the same group have the same number of valence electrons
Valence electrons are the electrons in the highest occupied energy level of an elementrsquos atoms
The number of valence electrons determines the chemical properties of an element
The number of valence electrons is related to the group numbers in the periodic table
3
The elements in Group 1A (hydrogen lithium etc) all have one valence electron
H 1s1 Na 1s22s22p63s1
Li 1s22s1 K 1s22s22p63s23p64s1
Carbon and silicon in Group 4A have four valence electrons
C 1s22s22p2
Si 1s22s22p63s23p2
Groups 5A has five (5) valence electrons and Group 6A has six (6) valence electrons etc
4
Valence electrons are usually the only electrons used in the formation of chemical bonds A shorthand way of showing valence electrons is through electron dot structures
Electron dot structures show valence electrons as dots The inner electrons are represented by the symbol for the element being considered
P188
5
Formation of Cations amp AnionsAs we have talked about before noble gases are quite unreactive This is because they have filled outer energy levels
Atoms form ions amp molecules for this reason they want filled outer energy levels
As such they follow a rule called the octet rule
The octet rule states that atoms in compounds tend to have the stable electron configuration of a noble gas
Na -- 1s22s22p63s1 Namiddot
Na+ -- 1s22s22p6 Na+ octet
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
3
The elements in Group 1A (hydrogen lithium etc) all have one valence electron
H 1s1 Na 1s22s22p63s1
Li 1s22s1 K 1s22s22p63s23p64s1
Carbon and silicon in Group 4A have four valence electrons
C 1s22s22p2
Si 1s22s22p63s23p2
Groups 5A has five (5) valence electrons and Group 6A has six (6) valence electrons etc
4
Valence electrons are usually the only electrons used in the formation of chemical bonds A shorthand way of showing valence electrons is through electron dot structures
Electron dot structures show valence electrons as dots The inner electrons are represented by the symbol for the element being considered
P188
5
Formation of Cations amp AnionsAs we have talked about before noble gases are quite unreactive This is because they have filled outer energy levels
Atoms form ions amp molecules for this reason they want filled outer energy levels
As such they follow a rule called the octet rule
The octet rule states that atoms in compounds tend to have the stable electron configuration of a noble gas
Na -- 1s22s22p63s1 Namiddot
Na+ -- 1s22s22p6 Na+ octet
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
4
Valence electrons are usually the only electrons used in the formation of chemical bonds A shorthand way of showing valence electrons is through electron dot structures
Electron dot structures show valence electrons as dots The inner electrons are represented by the symbol for the element being considered
P188
5
Formation of Cations amp AnionsAs we have talked about before noble gases are quite unreactive This is because they have filled outer energy levels
Atoms form ions amp molecules for this reason they want filled outer energy levels
As such they follow a rule called the octet rule
The octet rule states that atoms in compounds tend to have the stable electron configuration of a noble gas
Na -- 1s22s22p63s1 Namiddot
Na+ -- 1s22s22p6 Na+ octet
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
5
Formation of Cations amp AnionsAs we have talked about before noble gases are quite unreactive This is because they have filled outer energy levels
Atoms form ions amp molecules for this reason they want filled outer energy levels
As such they follow a rule called the octet rule
The octet rule states that atoms in compounds tend to have the stable electron configuration of a noble gas
Na -- 1s22s22p63s1 Namiddot
Na+ -- 1s22s22p6 Na+ octet
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
6
Metals lose electrons to obey this rule and nonmetals share or gain electrons to obey this rule
Sodium is a metal and as such loses electrons to form a cation amp have eight valence electrons
Nonmetals like chlorine gain electrons amp form anions
Cl -- 1s22s22p63s23p5
Cl- -- 1s22s22p63s23p6 Cl- octet
This is the same electron configuration as argon
It is easier for nonmetals to gain electrons to become an anion to have a filled outer energy level than to lose electrons
Oxygen atoms have six valence electrons By gaining two more they have the same electron configuration as neon
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
7
Ionic Bond Formation
Anions and cations have opposite charges They attract one another by electrostatic forces
The forces of attraction that bind oppositely charged ions together are called ionic bonds
Ionic compounds are also called salts
In any sample of an ionic compound the positive charges of the cations must equal the negative charges of the anions
Sodium chloride is a good example of how ionic bonds are formed
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
8
The chemical formula NaCl is a formula unit It shows that one sodium ion combines with one chlorine ion
1s22s22p63s1 1s22s22p63s23p5
Na+ Cl- or NaClChemical formula
Namiddot
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
9
Predict the formula when aluminum combines with bromine to make aluminum bromide
Al
+ Br
Three bromine react with one aluminum ion
The formula is therefore AlBr3 and the name always ends in ldquo-iderdquo aluminum bromide (metal first then nonmetal with -ide ending)
ExamplePredict the formula and name using electron dot structures for (a) potassium and oxygen
(b) magnesium and nitrogen
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
10
Kmiddot
Kmiddot
K+
K+O2-+ or K2O
potassium oxide
Mg bullbull
Mg bullbull
Mg bullbull
+
Mg2+
Mg2+
Mg2+
N3-
N3-
Mg3N2
magnesium nitride
Website orsquounderstanding
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
11
Polyatomic ions
Now that we have studied some of the more simple ionic bonds let us review and study some of the more complex ionic elements
We have learned that the group ldquoArdquo elementsrsquo ionic charge is determined by its group (ie Group 1A = +1 Group 2A = +2 etc)
On your paper make a chart of all of the Group A elements and their ionic charges
1A 2A 3A (ignore 4A) 5A 6A 7A
Li+ Be2+ Al3+ etc
p190
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
12
Unlike the cations of Group 1A 2A and 3A metals many of the transition metals have more than one common ionic charge
PR52
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
13
Notice that lead Pb Iron Fe Tin Sn Copper Cu and Mercury Hg have more than one charge
Pb = +2 and +4
Tin = +2 and +4
etc
These are known as the ldquoCMILTrdquo ions (C=copper M=mercury etc)
When you say the name of these ions you say the element plus whatever is in parentheses (ie Pb4+ = ldquolead fourrdquo ion) = lead (IV)
Example lead(II) oxide = PbO = Pb2+ + O2-
All of the ions mentioned so far have been single atoms Such ions are called monoatomic ions
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
14
Ions made of two or more atoms are called polyatomic ions Polyatomic ions are a tightly bound group of atoms that behave as a unit and carry a charge
Example
NO3 - 1 = nitrate ion
NO2 - 1 = nitrite ion
Most polyatomic ions end in ldquo-iterdquo or ldquo-aterdquo ldquo-iterdquo indicates one less oxygen atom than ldquo-aterdquo Charge is still the same for both however
Some common polyatomic ions
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
15
Polyatomic Ion Formation
In writing the formula of a compound that contains a polyatomic ion if more than one of that ion is needed parentheses are written around it
Example
Determine the formula for calcium nitrate
Calcium ion = Ca+2 Nitrate ion = NO3-1
Calcium nitrate = Ca(NO3)2
The () means 2 NO3-1rsquos are needed Without () it
would look like ldquoCaNO32rdquo or that there are 32
Orsquos
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
16
Determine the formula of calcium phosphate
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
17
copper(I) nitrite tin(II) perchlorate
Cu+1 NO2-1 Sn2+ ClO4
-1
CuNO2 Sn(ClO4)2
Write the name for the following compounds
PbCl2
Sn3N4
Lead(II) chloride
Tin(IV) Nitride
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
18
20 When an ionic bond is formed the atom that transfers its valence electron becomes an ion with 1) positive charge and more protons 2) positive charge and no change in the number of protons 3) negative charge and more protons 4) negative charge and no change in the number of protons
22 What monoatomic ion has 26 protons 30 neutrons and 24 electrons 1) chromium (II) 2) copper (II) 3) iron (II) 4) zinc (II)
19 Which part of the atom is involved in chemical bonding 1) only the nucleus 2) only the protons 3) only the electrons 4) only the valence electrons
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
19
Properties of Ionic Compounds
Most ionic compounds are crystalline solids at room temperature
Other properties of ionic compounds are
1 High melting point
2 Soluble (dissolves) in water
3 Well-defined crystals
4 Molten form conducts electricity
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
20
Each ion is strongly attracted to its neighbor and repulsions are minimized
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
21
Metallic Bond
Another bond that deals with cations but is no where similar to ionic bonds is the metallic bond
Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions
The electrons are often referred to as forming an electron sea
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
22
Metals are thought to have electrons that are delocalized - they donrsquot belong to any one atom but are free to move about
Another view
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
23
This model of metals explains several physical properties
Metals are good conductors of electrical current (flow of electrons) because as electrons enter one end of a bar of metal an equal number leave the other end
Another physical property that has revolutionized the industrial world is the fact that metals are ductile
Being ductile means that it can be drawn into thin wires
24
25
Metals are also malleable - they can be hammered into different shapes
24
25
Metals are also malleable - they can be hammered into different shapes
25
Metals are also malleable - they can be hammered into different shapes
