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Chapter 7. Keefe 1415. Valence electrons. These are the electrons that are available to participate in reactions: they are always in the OUTSIDE shell of electrons The number of valence electrons determines the chemical properties of the element. Valence Electrons. - PowerPoint PPT Presentation
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Chapter 7Keefe 1415
Valence electrons
• These are the electrons that are available to participate in reactions: they are always in the OUTSIDE shell of electrons• The number of valence electrons determines the
chemical properties of the element
Valence Electrons• Lithium and sodium each have 1 outer electron, so they have
similar properties. For example, they are soft metals and they corrode easily in air.
Valence Electrons• In forming compounds, atoms tend to achieve the electron
configuration of a noble gas• Octet- a set of 8 valence electrons
Valence electrons
• Exceptions to the OCTET RULE include H, He, and B:• H and He are happy with just TWO electrons• B is happy with SIX electrons
Valence Electrons• Atoms of metals tend to LOSE all of their valence electrons to
leave a complete octet in the next-lower energy level• Atoms of nonmetals tend to GAIN electrons or SHARE
electrons with another nonmetal to achieve an octet
Valence electrons
Anions Versus Cations
Anions versus Cations• Cations want to LOSE electron(s) and therefore have a net
POSITIVE charge:
Anions Versus Cations• Name of a cation is the same as the element name, then add
the word ‘ion’:
ion
Anions Versus Cations• Some transition metals have multiple possible oxidation states
(charges). To name them, you add a ROMAN NUMERAL after the name of the element to indicate the charge:
ion
Anions versus Cations• Anions want to GAIN electron(s) and therefore have a
NEGATIVE charge
Anions Versus Cations• Name of an anion is usually the name of the element, BUT
drop the last syllable and add ‘ide’:• Clorine atoms form chloride anions• Oxygen atoms for oxide anions
Lewis dot structures of atoms• Simply put the symbol of the element and add dots around it
until you have represented all the valence electrons:
Valence Electrons
Compound:
•any substance made up of two or more elements.
Binary Compounds
“Binary” means “two”, as in there are two different elements involved.•There are two types:• Ionic•Covalent
Ionic Compounds • Ionic Compounds are made from a Metal and a Non-metal.
Ionic Compounds
•Naming: metal cation first, then non-metal anion with –ide at the end.• Example: NaCl:
Sodium Chloride• In this Ionic Compound, there is one
Sodium atom for every Chlorine atom.
Balancing Ionic Compounds
•Sometimes an Ionic Compound will have little numbers included in its formula:• Ex. Magnesium Chloride = MgCl2
Balancing Ionic Compounds
• These numbers are called subscripts, and they tell you how many of the previous atoms you have.• One magnesium, two chlorines• Magnesium Chloride = MgCl2
Balancing Ionic Compounds
•Beryllium Fluoride: how do you know whether or not subscripts are needed?
Balancing Ionic Compounds
• There is nothing in their name that indicates that numbers are necessary in the formula• You need the:• Oxidation Number (we call it the
charge)
Balancing Oxidation State Numbers• We’re trying to get these two numbers to add up to zero:
•Be2+ and F-
• BeF2 = Beryllium Fluoride
A visual representationBe2+ F-
We need two “minus ones” to balance out “plus two”
Another Trick:
• How about Aluminum Oxide?• First, find their oxidation numbers:• Al3+ and O-2
• How can we balance out a 3+ and a -2?• Trick: Swap the numbers!• Al2O3 = Aluminum Oxide
Write the formula for the ionic compound that will form between Ba2+ and Cl.Solution:1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the
negative ion Ba2+ Cl
Cl
3. Write the number of ions needed as
subscripts BaCl2
Writing a Formula
Write the correct formula for the compounds containing the following ions:1. Na+, S2-
2. Al3+, Cl-
3. Mg2+, N3-
Learning Check
1. Na+, S2-
Na2S
2. Al3+, Cl-
AlCl3
3. Mg2+, N3-
Mg3N2
Solution
• 1. Cation first, then anion
• 2. Monatomic cation = name of the element• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide• Cl- = chloride
• CaCl2 = calcium chloride
Naming CompoundsNaming Compounds
Binary Ionic Compounds:
Examples:NaCl
ZnI2
Al2O3
Naming Binary Ionic Compounds
sodium chloride
zinc iodide
aluminum oxide
Complete the names of the following binary compounds:Na3N sodium ________________
KBr potassium ________________
Al2O3 aluminum ________________
MgS _________________________
Learning Check
Complete the names of the following binary compounds:
Na3N
KBr
Al2O3
MgS
Solution
sodium nitride
potassium bromide
aluminum oxide
magnesium sulfide
Elements that can have more than one possible charge
MUST have a Roman Numeral to indicate the charge on
the individual ion.
1+ or 2+ 2+ or 3+Cu+, Cu2+ Fe2+, Fe3+
copper(I) ion iron(II) ion copper (II) ion iron(III) ion
Transition Metals
These elements REQUIRE Roman Numerals because they can have more than one possible charge:anything except Group 1A, 2A, Ag, Zn, Cd, and Al
Names of Variable Transition Ions
Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3 (Fe3+) iron (III) chlorideCuCl (Cu+ ) copper (I) chlorideSnF4 (Sn4+) tin (IV) fluoridePbCl2 (Pb2+) lead (II) chlorideFe2S3 (Fe3+) iron (III) sulfide
Names of Variable Ions
Examples of Older Names of Cations formed from Transition Metals(you do not have to memorize these)
Complete the names of the following binary compounds with variable metal ions:
FeBr2 iron (_____) bromide
CuCl copper (_____) chloride
SnO2 ___(_____ ) ______________
Fe2O3 ________________________
Hg2S ________________________
Learning Check
Complete the names of the following binary compounds with variable metal ions:
iron ( II ) bromide
copper ( I ) chloride
tin (IV) oxide
iron (III) oxide
mercury (I) sulfide
Solution
FeBr2
CuCl
SnO2
Hg2S
Fe2O3
Polyatomic ions: MEMORIZE (and I have a trick to help)
Naming polyatomic ions YAS THERE ARE MOAR“ate” anions have one more oxygen then the “ite” ion, but the same charge. If you memorize the “ate” ions, then you should be able to derive the formula for the “ite” ion and vice-versa:
• Examples: • sulfate is SO4 2- , so sulfite has the same charge
but one less oxygen (SO3 2-)
• nitrate is NO3 -, so nitrite has the same charge but one less oxygen (NO2
-)
Naming Polyatomics
• A sulfate ion is SO42- . To get the formula
for hydrogen sulfate ion, you add a hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge on the new ion is less negative by one.
Naming polyatomics• Add one more hydrogen to the mix and you get:
Naming polyatomics
• Similarly, adding/subtracting oxygens results in: