Attachments
unit1FlowChartforClassifyingMatter.doc
UNIT1ClassificationofMatter.doc
UNIT1UnderlyingStructureofMatter.doc
atomsandionsworksheet.rtf
atomsandionsworksheetans.rtf
isotopeworksheet.doc
unit1scaleassignment.doc
electronconfighandout.doc
electronconfigurationworksheet.doc
summaryoftrendshandout.doc
valenceelectronsworksheet.doc
UNIT1ElementsandCompounds.doc
NamingIonicCompounds.doc
compoundnamingassignment.doc
namingmolecularcompounds.doc
IonicCompoundNaming.doc
namingassign.doc
namingacidsworksheet.doc
namingacidsworksheet2.doc
Flow Chart for Classifying Matter
Flow Chart for Classifying Matter
SMART Notebook
Classification of Matter (6 hours):
It is expected that students will:
Define and classify matter according to its composition (pure
substances or mixtures)
Define and distinguish between chemical and physical
properties
Define and classify matter as elements and compounds, and as
heterogeneous mixtures and solutions.
Use the periodic law as illustrated by the periodic table to
identify and distinguish metals and non metals, periods and groups,
representative and transition elements, and families.
Describe the factors which contribute to the unique position of
hydrogen on the periodic table.
Identify the elements that are most prevalent in living
systems.
Research ingredients and additives in consumer products.
Identify consumer products and investigate claims made by
companies about the products.
SMART Notebook
Underlying Structure of Matter (8 hours):
It is expected that students will:
Use standard atomic notation to represent atoms, define isotopes
and use isotopic notation.
Predict ionic charges from position on the periodic table.
Define atomic mass, explain the relative nature of atomic
mass.
Provide definitions and examples of atoms, ions, and molecules,
including subatomic particles, atomic mass, atomic number, mass
number, valence electrons, and isotopes.
Identify the inadequacies in the Rutherford and Bohr Models.
Identify the new proposal in the Bohr model of the atom.
Describe the energies and positions of electrons according to
the quantum mechanical model.
Describe how the shapes of orbitals differ as it relates to
different sublevels.
Write electron Configuration diagrams using Hunds rule, Pauli
exclusion Principle and Aufbau principle (diagonal rule)
LEVEL 1:
Demonstrate an understanding of modern atomic theory.
Demonstrate an introductory understanding of Quantum Theory.
Demonstrate an understanding of periodicity of IE,
electronegativity and atomic radii.
SMART Notebook
chapter 2 page 84
atomic theory: atoms and ions
Complete the following table.
English Name
International Symbol
Number of Protons
Number of Electrons
Number of Electrons Lost or Gained
Net Charge
1.
neon atom
2.
lithium ion
lost 1
3.
47
1 +
4.
18
2-
5.
Si
6.
33
36
7.
54
lost 1
8.
30
28
9.
1
0
10.
P
11.
Ca2+
12.
selenide ion
13.
13
3+
14.
Rb+
15.
18
18
16.
8
10
17.
iodine atom
53
18.
Pu
94
19,
52
54
gained 2
20.
Gold Ion
79
Lost 2
E-12 ADDITIONAL EXERCISE MASTERS
nelson canada, A division of thomson canada limited, 1996
SMART Notebook
chapter 2 page 84
atomic theory: atoms and ions
Complete the following table.
English Name
International Symbol
Number of Protons
Number of Electrons
Number of Electrons Lost or Gained
Net Charge
1.
neon atom
Ne
10
10
0
0
2.
lithium ion
Li+1
3
2
lost 1
1+
3.
silver ion
Ag+
47
46
lost 1
1 +
4.
sulfide ion
S-2
16
18
gained 2
2-
5.
silicon atom
Si
14
14
0
0
6.
arsenide ion
As-3
33
36
gained 3
3-
7.
cesium ion
Cs+
55
54
lost 1
1+
8.
zinc ion
Zn+2
30
28
lost 2
2+
9.
hydrogen atom
H
1
1
0
0
10.
phosphorus atom
P
15
15
0
0
11.
calcium ion
Ca2+
20
18
lost 2
2+
12.
selenide ion
Se-2
34
36
gained 2
2-
13.
aluminum ion
Al+3
13
10
lost 3
3+
14.
rubidium ion
Rb+
37
36
lost 1
1+
15.
argon atom
Ar
18
18
0
0
16.
oxide ion
0-2
8
10
gained 2
2-
17.
iodine atom
I
53
53
0
0
18.
plutonium atom
Pu
94
94
0
0
19,
telluride ion
Te-2
52
54
gained 2
2-
20.
Gold Ion
Au+2
79
77
Lost 2
2+
E-12 ADDITIONAL EXERCISE MASTERS
nelson canada, A division of thomson canada limited, 1996
SMART Notebook
SMART Notebook
Chem 112
Scale Assignment
Trace this image onto a sheet of graph paper.
Now, use the graph paper to draw the same atom 100 times
smaller.
(Compare the diameters of the circles, are they 100 times
smaller? Discuss what youve done with groups around you)
If youve successfully drawn an atom that is 100 times smaller,
then do it again with your new picture.
How much smaller is the new picture than the original?
About how many times would you have to reduce your picture to
get to the size of an actual Helium atom? (The diameter of a Helium
atom is 60 pm, which is 60 pico meters, which is 60 x 10-12 m)
Use your diagram and the information above to estimate the size
of a proton.
Given that a proton is thought to be about 1.5x10-18 m is the
drawing above done to scale?
SMART Notebook
SMART Notebook
Electron Configurations Worksheet
Write the complete ground state electron configurations for the
following:
1)lithium ________________________________________
2)oxygen ________________________________________
3)calcium ________________________________________
4)titanium ________________________________________
5)rubidium ________________________________________
6)lead ________________________________________
7)erbium ________________________________________
Write the abbreviated ground state electron configurations for
the following:
8)helium ________________________________________
9)nitrogen ________________________________________
10)chlorine ________________________________________
11)iron ________________________________________
12)zinc ________________________________________
13)barium ________________________________________
14)polonium ________________________________________
Electron Configurations Worksheet - Answers
Write the complete ground state electron configurations for the
following:
1)lithium 1s22s1
2)oxygen 1s22s22p4
3)calcium 1s22s22p63s23p64s2
4)titanium 1s22s22p63s23p64s23d2
5)rubidium 1s22s22p63s23p64s23d104p65s1
6)lead
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2
7)erbium 1s22s22p63s23p64s23d104p65s24d105p66s24f12
Write the abbreviated ground state electron configurations for
the following:
8)helium 1s2 (this one cannot be abbreviated)
9)nitrogen [He] 2s22p3
10)chlorine [Ne] 3s23p5
11)iron
[Ar] 4s23d6
12)zinc
[Ar] 4s23d10
13)barium [Xe] 6s2
14)polonium [Xe] 6s24f145d106p4
For more practice, visit www.chemfiesta.com
2006 Cavalcade Publishing. All Rights Reserved
SMART Notebook
SMART Notebook
Finding the number of valence electrons of an element
This is easier than you might think. First of all, let's go
through a couple of terms:
Octet rule: The rule that says that all elements want to have
the same electron configurations as the nearest noble gas to them.
This is because the noble gases are really stable, and all elements
want to be stable in the same way. Elements become like the nearest
noble gas by gaining or losing electrons, or by sharing electrons
with other atoms.
Valence electrons: The number of s- and p- electrons in the
outermost energy level. You can find the number of valence
electrons by counting backwards from the element you're interested
in to the last noble gas. However, and this is important for some
elements, when you're counting backwards, you want to skip over the
d- and f- parts of the periodic table. For example, sulfur has 6
valence electrons, as does selenium. Why does selenium have six
valence electrons when there are more elements between it and the
last noble gas? It's because we skip over the entire d-block of
elements.
Of course, anybody who's read this far is probably curious as to
why we need to worry about the octet rule or the number of valence
electrons. Well, I'm glad you asked.
The octet rule allows us to determine the charge that an element
will have when it forms ionic compounds. To find this charge,
you'll count from the element that you're interested in to the
nearest noble gas. If counting backwards takes you to the nearest
noble gas (as in the case of lithium and magnesium), the charge is
equal to +[however many elements you need to count across]. For
example, since you count backwards one element from lithium to
reach the nearest noble gas (which is helium), the charge is +1. If
counting forwards takes you to the nearest noble gas (as in the
case of oxygen and chlorine), the charge is equal to -[the number
of elements you need to count across]. For example, since you count
forwards two elements from oxgyen to reach neon, the charge of
oxygen when it forms ionic compounds is -2.
The number of valence electrons allows us to determine how many
electrons an element has that can do covalent bonding, and for this
reason is extremely important for nonmetals. For example, when
oxygen bonds with two hydrogen atoms, we know that our resulting
Lewis structure will need to show eight electrons, as oxygen has
six valence electrons (determined by counting backwards to He) and
the two hydrogens each have one valence electron
Questions:
1. Draw the Lewis structures (Which is the Element symbol
surrounded by its valence electrons in the proper positions) for
each of the following.
a) Sodium
b) Beryllium
c) Nitrogen
d) Sulfure) Fluorine
2. Determine the number of electrons that will be added or
removed from each of the elements above to make them have a
complete shell. Write the resulting charge of the ion.
3. One potassium atom and a chloride atom combine to form
potassium chloride. Draw each atoms Lewis structure and show how
the electron could be shared to make a bond.
4. How many potassium atoms would be needed to satisfy an oxygen
atoms needs? Draw it.
SMART Notebook
Elements and Compounds (8 hours):
It is expected that students will:
Define and differentiate between ionic and molecular compounds,
including acids and bases, using conductivity and indicators
Identify, name and write formulas for ionic (binary,
multivalent, polyatomic, and hydrates) and molecular compounds, and
acids using IUPAC and classical systems.
Elements and Compounds (8 hours):
It is expected that students will:
Define and differentiate between ionic and molecular compounds,
including acids and bases, using conductivity and indicators
Identify, name and write formulas for ionic (binary,
multivalent, polyatomic, and hydrates) and molecular compounds, and
acids using IUPAC and classical systems.
Elements and Compounds (8 hours):
It is expected that students will:
Define and differentiate between ionic and molecular compounds,
including acids and bases, using conductivity and indicators
Identify, name and write formulas for ionic (binary,
multivalent, polyatomic, and hydrates) and molecular compounds, and
acids using IUPAC and classical systems.
Elements and Compounds (8 hours):
It is expected that students will:
Define and differentiate between ionic and molecular compounds,
including acids and bases, using conductivity and indicators
Identify, name and write formulas for ionic (binary,
multivalent, polyatomic, and hydrates) and molecular compounds, and
acids using IUPAC and classical systems.
SMART Notebook
Naming Ionic Compounds
1. Name the following ionic compounds:
a) NH4Cl b) Fe(NO3)3
c) TiBr3 d) Cu3P e) SnSe2 f) GaAs
g) Pb(SO4)2 h) Be(HCO3)2 i) Mn2(SO3)3 j) Al(CN)3 k) NaBr l)
Sc(OH)3
m) V2(SO4)3 n) NH4F
o) CaCO3 p) NiPO4 q) Li2SO3 r) Zn3P2
s) Sr(C2H3O2)2 t) Cu2O
u) Ag3PO4 v) YClO3 w) SnS2 x) Ti(CN)4
y) KMnO4 z) Pb3N2
2. Write the formulas for each of the ionic compounds
listed.
a) chromium (VI) phosphate
b) vanadium (IV) carbonate
c) tin (II) nitrite
d) cobalt (III) oxide
e) titanium (II) acetate
f) vanadium (V) sulfide
g) chromium (III) hydroxide
h) lithium iodide
i) lead (II) nitride
j) silver bromide
k) lithium acetate
l) iron (II) phosphate
m) titanium (II) selenide
n) calcium bromide
o) gallium chloride
p) sodium hydride
q) beryllium hydroxide
r) zinc carbonate
s) manganese (VII) arsenide
t) copper (II) chlorate
u) cobalt (III) chromate
v) ammonium oxide
w) potassium hydroxide
x) lead (IV) sulfate
y) silver cyanide
z) vanadium (V) nitride
Naming Ionic Compounds
1. Name the following ionic compounds:
a) NH4Cl b) Fe(NO3)3
c) TiBr3 d) Cu3P e) SnSe2 f) GaAs
g) Pb(SO4)2 h) Be(HCO3)2 i) Mn2(SO3)3 j) Al(CN)3 k) NaBr l)
Sc(OH)3
m) V2(SO4)3 n) NH4F
o) CaCO3 p) NiPO4 q) Li2SO3 r) Zn3P2
s) Sr(C2H3O2)2 t) Cu2O
u) Ag3PO4 v) YClO3 w) SnS2 x) Ti(CN)4
y) KMnO4 z) Pb3N2
2. Write the formulas for each of the ionic compounds
listed.
a) chromium (VI) phosphate
b) vanadium (IV) carbonate
c) tin (II) nitrite
d) cobalt (III) oxide
e) titanium (II) acetate
f) vanadium (V) sulfide
g) chromium (III) hydroxide
h) lithium iodide
i) lead (II) nitride
j) silver bromide
k) lithium acetate
l) iron (II) phosphate
m) titanium (II) selenide
n) calcium bromide
o) gallium chloride
p) sodium hydride
q) beryllium hydroxide
r) zinc carbonate
s) manganese (VII) arsenide
t) copper (II) chlorate
u) cobalt (III) chromate
v) ammonium oxide
w) potassium hydroxide
x) lead (IV) sulfate
y) silver cyanide
z) vanadium (V) nitride
SMART Notebook
Chem 112
Name:
Naming Compounds Assignment
Date:
For each of the following questions, determine whether the
compound is ionic or covalent and name it appropriately.
1)Na2CO3 _________________________________________
2)P2O5 _________________________________________
3)NH3 _________________________________________
4)FeSO4 _________________________________________
5)SiO2 _________________________________________
6)GaCl3 _________________________________________
7)CoBr2 _________________________________________
8)B2H4 _________________________________________
9)CO _________________________________________
10)P4 _________________________________________
For each of the following questions, determine whether the
compound is ionic or covalent and write the appropriate formula for
it.
11)dinitrogen trioxide
_________________________________________
12)nitrogen _________________________________________
13)methane _________________________________________
14)lithium acetate _________________________________________
15)phosphorus trifluoride
_________________________________________
16)vanadium (V) oxide
_________________________________________
17)aluminum hydroxide
_________________________________________
18)zinc sulfide _________________________________________
19)silicon tetrafluoride
_________________________________________
20)silver phosphate
_________________________________________
SMART Notebook
SMART Notebook
Compound Naming Assignment
Chem 112
Ch. 9 Worksheet
Directions: Answer all of the following questions on this sheet.
Use your periodic tables and the sheet of complex ions to do it. It
is a good idea to check your answers with me after you have
completed the first 10 to see if they are good.
1)copper (II) acetate _________________ 2)sodium hydroxide
__________________
3)lithium oxide __________________ 4)cobalt (III) carbonate
__________________
5)aluminum sulfide __________________ 6)ammonium cyanide
__________________
7)iron (III) phosphide _________________ 8)vanadium (V)
phosphate ________________
9)sodium permanganate ______________ 10)manganese (III) fluoride
________________
11)beryllium nitrate __________________ 12)nickel (III) sulfite
__________________
13)potassium oxide __________________ 14)silver bromide
__________________
15)zinc phosphate __________________ 16)copper (II) bicarbonate
_________________
17)nickel (II) selenide _________________ 18)manganese (IV)
carbonate ______________
19)lead (IV) nitride __________________ 20)tin (II) hydroxide
__________________
21)lithium arsenide __________________ 22)chromium (VI) sulfate
__________________
23)calcium bromide __________________ 24)ammonium sulfate
__________________
25)copper (II) oxide __________________ 26)platinum (IV)
phosphate ________________
27)aluminum carbonate _______________ 28)silver nitrate
__________________
29)magnesium acetate ________________ 30)nickel (III) cyanide
__________________
31)vanadium (IV) phosphate ____________32)silver sulfate
__________________
33)cobalt (III) sulfide __________________ 34)iron (II) sulfite
__________________
35)copper (II) nitrite __________________ 36)nickel (II)
hydroxide __________________
37)zinc nitride __________________ 38)manganese (VII) nitrate
________________
39)gallium sulfate __________________ 40)sodium nitrate
__________________
ANSWER STRIP
1) Cu(CH3COO)2 2) NaOH
3) Li2O4) Co2(CO3)35) Al2S3
6) NH4CN
7) FeP
8) V3(PO4)59) NaMnO4
10) MnF3
Compound Naming Race - Solutions
Be the first team in the room to correctly get all the names on
this sheet right. When you have finished the first ten problems,
bring them up to the teacher to be checked. Once these have been
checked, move to the second ten. Once all forty problems have been
solved, youre the winner!
1)copper (II) acetate
Cu(CH3COO)2
2)sodium hydroxide
NaOH
3)lithium oxide
Li2O
4)cobalt (III) carbonate
Co2(CO3)3
5)aluminum sulfide
Al2S3
6)ammonium cyanide
NH4CN
7)iron (III) phosphide
FeP
8)vanadium (V) phosphate
V3(PO4)5
9)sodium permanganate
NaMnO4
10)manganese (III) fluoride
MnF3
11)beryllium nitrate
Be(NO3)2
12)nickel (III) sulfite
Na2(SO3)3
13)potassium oxide
K2O
14)silver bromide
AgBr
15)zinc phosphate
Zn3(PO4)2
16)copper (II) bicarbonate
Cu(HCO3)2
17)nickel (II) selenide
NiSe
18)manganese (IV) carbonate Mn(CO3)2
19)lead (IV) nitride
Pb3N4
20)tin (II) hydroxide
Sn(OH)2
21)lithium arsenide
Li3As
22)chromium (VI) sulfate
Cr(SO4)3
23)calcium bromide
CaBr2
24)ammonium sulfate
(NH4)2SO4
25)copper (II) oxide
CuO
26)platinum (IV) phosphate
Pt3(PO4)4
27)aluminum carbonate
Al2(CO3)2
28)silver nitrate
AgNO3
29)magnesium acetate
Mg(CH3COO)2
30)nickel (III) cyanide
Ni(CN)3
31)vanadium (IV) phosphate
V3(PO4)4
32)silver sulfate
Ag2SO4
33)cobalt (III) sulfide
Co2S3
34)iron (II) sulfite
FeSO3
35)copper (II) nitrite
Cu(NO2)2
36)nickel (II) hydroxide
Ni(OH)2
37)zinc nitride
Zn3N2
38)manganese (VII) nitrate
Mn(NO3)7
39)gallium sulfate
Ga2(SO4)3
40)sodium nitrate
NaNO3
SMART Notebook
Chem 112
Name:
Ch. 9 Assignment
Date:
For the list on the left, name the compound. For the list on the
right, give the chemical formula that corresponds to the name
1)NaF
13)potassium fluoride
2)K2CO3
14)ammonium sulfate
3)MgCl2
15)magnesium iodide
4)Be(OH)2
16)copper (II) sulfite
5)SrS
17)aluminum phosphate
6)Cu2S
18)lead (II) nitrite
7)ZnI2
19)cobalt (II) selenide
8)Ca3(PO4)2
20)silver cyanide
9)NH4I
21)copper (II) hydrogen carbonate
10)Mn(NO3)3
22)iron (II) oxide
11)FePO4
23)lithium cyanide
12)CoCO3
24)lead (IV) sulfite
Compound Names and Formulas Solution Key
Formula to name problems:
1)NaF is sodium fluoride
2)K2CO3 is potassium carbonate
3)MgCl2 is magnesium chloride
4)Be(OH)2 is beryllium hydroxide
5)SrS is strontium sulfide
6)Cu2S is copper (I) sulfide
7)ZnI2 is zinc iodide
8)Ca3(PO4)2 is calcium phosphate
9)NH4I is ammonium iodide
10)Mn(NO3)3 is manganese (III) nitrate
11)FePO4 is iron (III) phosphate
12)CoCO3 is cobalt (II) carbonate
Name to formula problems:
13)potassium fluoride is KF
14)ammonium sulfate is (NH4)2SO4
15)magnesium iodide is MgI2
16)copper (II) sulfite is CuSO3
17)aluminum phosphate is AlPO4
18)lead (II) nitrite is Pb(NO2)2
19)cobalt (II) selenide is CoSe
20)silver cyanide is AgCN
21)copper (II) bicarbonate is Cu(HCO3)2
22)iron (II) oxide is FeO
23)lithium cyanide is LiCN
24)lead (IV) sulfite is Pb(SO3)2
Compound Names and Formulas
SMART Notebook
Formula
IUPAC name
Common Name
hydrofluoric acid
H2SO3
H2S
Hydrogen phosphate
hydroselenic acid
HCN
carbonic acid
nitrous acid
H3P
sulfuric acid
hydrobromic acid
Chem 112
Naming Acids Worksheet.
SMART Notebook
Formula
IUPAC name
Common Name
hydrofluoric acid
H2SO3
H2S
Hydrogen phosphate
hydroselenic acid
HCN
carbonic acid
nitrous acid
H3P
sulfuric acid
hydrobromic acid
Chem 112
Naming Acids Worksheet.
SMART Notebook
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