+ DOR: What’s in a name?
Write the element symbol
WITHOUT the periodic table
1) Lithium
6) Magnesium
2) Fluorine
7) Lead
3) Oxygen
8) Manganese
4) Copper
9) Potassium
5) Mercury
10) Iron
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What’s in a
name?
+
LOL
ASAP
FYI
BRB
Binary
Compounds—Writing
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Chemical formulas
1) Cation, Anion
2) Write oxidation number/charge on
each element.
3) Balance charges by the smallest
common multiplier between the two
elements. Charges must add to 0 for a
neutral compound.
4) Add the subscripts for each
element in the chemical compound.
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Example 1: Sodium chloride
“salt”
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Example 2: Aluminum oxide
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You try…..
1)
Magnesium bromide
2)
Lithium chloride
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5) If the first element is a transition
element, the oxidation number or
charge of the element is given by a
Roman numeral (I, II, III, IV, etc.)
following the element name.
Exceptions: Ag+1 and Zn+2—they will
always have these charges.
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1)
Magnesium chloride
2)
Sodium sulfide
3)
Calcium sulfide
4)
Potassium bromide
5)
Barium chloride
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Example 3: Tin (IV) sulfide
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You Try…..
1) Zinc oxide
2) Mercury (II) fluoride
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Example 4: Iron (III) oxide
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Try…..
1)
Calcium chloride
2)
Copper (I) oxide
3)
Sodium bromide
4)
Potassium sulfide
5)
Calcium oxide
Binary
Homework—Due
Friday
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2/8, write chemical formula
with chemical name.
 1)
Iron (II) oxide
2) Potassium bromide
 3)
Magnesium chloride
4) Chromium (III) oxide
 5)
Calcium fluoride
6) Iron (III) sulfide
 7)
Manganese (IV) sulfide
 9)
Zinc bromide
8) Strontium sulfide
10) Copper (II) oxide
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DOR: Binary Naming
1)
Cobalt (II) nitride
2)
Calcium chloride
3)
Barium sulfide
4)
Chromium (VI) oxide
5)
Beryllium sulfide
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Binary Compounds—Writing
Chemical formulas (Cont.)
6) If a binary compound has a prefix
or prefixes in front of an element
name, these prefixes are the
subscripts for that element in the
chemical formula. Prefixes
represent the number of element
atoms present in a molecule of the
chemical compound.
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Prefixes
1
mono
6 hexa
2
di
7 hepta
3
tri
8 octa
4
tetra
9 nona
5
penta
10 deca
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Example 1: Carbon monoxide
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Example 2: Carbon dioxide
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You Try…..
Diphosphorus
Iodine
trioxide
heptafluoride
Carbon
tetrachloride
Polyatomic
Chemical
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Compounds—Writing Chemical
Formulas.
1) Cation, Anion—reference table
2) Write the oxidation number/charge on each element
and polyatomic ion.
3) Balance charges by the smallest common multiplier
between the cation and anion. Charges must add to 0 for
a neutral compound.
4) Add the subscripts for each element/polyatomic ion
to the chemical compound.
*Polyatomic ions: place polyatomic ions in
parentheses when adding subscript (ex. (NO3)2)
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Example 1: Silver nitrate
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Example 2: Magnesium acetate
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You try…..
1)
Ammonium chloride
2) Calcium carbonate
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 1)
Potassium sulfate
11. Mercury (II) hydroxide
 2)
nitrogen dioxide
12. Sodium phosphate
 3)
sulfur tetrabromide
13. Dinitrogen pentaoxide
 4)
magnesium phosphate
14. Carbon tetrahydride
 5)
sodium sulfate
15. Calcium nitrate
 6)
phosphorus pentachloride
 7)
selenium trichloride
 8)
chromium (III) nitrite
 9)
iodine dioxide
 10)
magnesium hydroxide
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DOR Regular: Chemical
Formulas
1)
Barium sulfate
2) calcium sulfide
3) Cobalt (II) carbonate
4) sulfur hexafluoride
5) Carbon tetrabromide
6) tin (IV) chloride
7) Potassium chloride
8) zinc fluoride
9) Strontium iodide
10) magnesium carbonate
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Can we go in reverse?
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Binary Compounds: Chemical
Nomenclature
1) Write an element’s oxidation number
over the element symbol.
2) Cation, Anion—write the element name
3) Add the ending -IDE to the second
element/anion
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Example 1: Al2S3
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Example 2: LiCl
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Try……
1) MgO
2) CaBr2
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Transition Elements
4) Place a Roman numeral
matching the charge/oxidation # on
an element after the positive
element’s name. Roman numeral is
put in () (ex. (II)). Roman numeral
indicates the oxidation number on
an element can vary.
-Go back to Step #3
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Example 1: CuS
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Example 2: CoBr2
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You Try….
1)
SnO
2)
CrCl3
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5) If both elements are found on
the RIGHT side of the periodic
table, use the appropriate prefix
for a given element.
-Go back to Step #3
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Example 1: CO2
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Example 2: CCl4
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You Try….
1) SO2
2) SBr3
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Compounds with Polyatomic
Ions: Chemical Nomenclature
1) Write oxidation # for each element/polyatomic ion in the
formula
2) Write the element and/or polyatomic ion names.
3) If a transition element (an element where the oxidation #
varies), use a Roman numeral to indicate an element’s
oxidation # in the chemical name.

*NO –IDE ENDING!!!!
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Example 1: ZnCO3
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Example 2: CuSO4
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You Try……Mg(CN)2
Sr(NO3)2
1)
Mg(CN)2
2) Sr(NO3)2
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Regular Classwork
1) Ni3(PO4)2
6) Mg3N2
2) AgBr
7) BiI3
3) SnCl4
8)(NH4)2SO4
4) (NH4)2 S
9) ZnCO3
5) HgF2
10) Cu2S
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DOR : Nomenclature and
Formulas
1) Cobalt (II) carbonate
2) sulfur hexafluoride
3) Tin (IV) chloride
4) calcium sulfide
5) Ammonium phosphate
6) K2S
7) MgF2
8) Al2O3
9) CuO
10) Fe2O3
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Law of Conservation of Matter:
Matter
cannot be created or
destroyed.
AMOUNT
OF REACTANTS =
AMOUNT OF PRODUCTS ! ! ! !
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Guidelines for Balancing
Chemical Equations:

1) Do NOT change the subscripts !

2) Every element MUST have the same amount of atoms
on both sides of the equation.

3) To balance, coefficients (numbers) are added in front of
the chemical formula until we have the same atom
amount on both sides of the equation.

4) Once a coefficient is added, go back and check the rest
of the equation5) Balance every element EXCEPT Hs and
Os. Then balance Hs, Os are balanced last.

6) CHECK EQUATION TO BE SURE EVERYTHING
BALANCES/CANCELS OUT ON BOTH SIDES ! ! !
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Example 1:
Mg +
HCl 
MgCl +
H2
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Example 2:
KI (aq) +
Pb(NO3)2 
KNO3 +
PbI2
+
Example 3:
FeI3 +
K2SO4 
KI +
Fe2(SO4)3
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Practice
 1)
Zn + CrCl3  CrCl2 + ZnCl2
 2)
Cu + H2SO4  CuSO4 + SO2 + H2O
 3)
LiAlH4 + H2O  LiOH + Al(OH)3 + H2
 4)
CaSO4 + Al(NO3)3  Ca(NO3)2 + Al2(SO4)3
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Honors Homework

Worksheet