1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
11)
12)
13)
14)
15)
16)
17)
18)
19)
20)
lithium acetate
LiC2H3O2
iron (II) phosphate
Fe3(PO4)2
titanium (II) selenide
TiSe
calcium bromide
CaBr2
gallium chloride
GaCl3
sodium hydride
NaH
beryllium hydroxide
Be(OH)2
zinc carbonate
ZnCO3
manganese (VII) arsenide
Mn3As7
copper (II) chlorate
Cu(ClO3)2
cobalt (III) chromate
Co2(CrO4)3
ammonium oxide
(NH4)2O
potassium hydroxide
KOH
lead (IV) sulfate
Pb(SO4)2
silver cyanide
AgCN
vanadium (V) nitride
V3N5
strontium acetate
Sr(C2H3O2)2
molybdenum sulfate
Mo(SO4)3
platinum (II) sulfide
PtS
ammonium sulfate
(NH4)2SO4
Ionic/Covalent Compound Naming Solutions
1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
Na2CO3
sodium carbonate
P2O5 diphosphorus pentoxide
NH3
ammonia
FeSO4
iron (II) sulfate
SiO2
silicon dioxide
GaCl3
gallium chloride
CoBr2
cobalt (II) bromide
B2H4
diboron tetrahydride
CO
carbon monoxide
P4
phosphorus
11)
12)
13)
14)
15)
16)
17)
18)
19)
20)
dinitrogen trioxide
nitrogen
methane
lithium acetate
phosphorus trifluoride
vanadium (V) oxide
aluminum hydroxide
zinc sulfide
silicon tetrafluoride
silver phosphate
N2O3
N2
CH4
LiC2H3O2
PF3
V2O5
Al(OH)3
ZnS
SiF4
Ag3PO4
(Still) More Naming Practice - Answers
1)
2)
3)
4)
5)
6)
7)
BBr3
boron tribromide
CaSO4
calcium sulfate
C2Br6
dicarbon hexabromide
Cr(CO3)3 chromium (VI) carbonate
Ag3P
silver phosphide
IO2
iodine dioxide
VO2
vanadium (IV) oxide
8)
9)
10)
PbS
CH4
N2O3
lead (II) sulfide
methane
dinitrogen trioxide
Write the formulas of the following chemical compounds:
11)
tetraphosphorus triselenide
P4Se3
12)
potassium acetate
KC2H3O2
13)
iron (II) phosphide
Fe3P2
14)
disilicon hexabromide
Si2Br6
15)
titanium (IV) nitrate
Ti(NO3)4
16)
diselenium diiodide
Se2I2
17)
copper (I) phosphate
Cu3PO4
18)
gallium oxide
19)
tetrasulfur dinitride
S4N2
20)
phosphorus
P4
Ga2O3
Answers – Naming Chemical Compounds
1)
NaBr
sodium bromide
2)
Ca(C2H3O2)2
calcium acetate
3)
P2O5
4)
Ti(SO4)2
titanium(IV) sulfate
5)
FePO4
iron(III) phosphate
6)
K3N
potassium nitride
7)
SO2
8)
CuOH
9)
Zn(NO2)2
10)
V2S3
diphosphorus pentoxide
sulfur dioxide
copper(I) hydroxide
zinc nitrite
vanadium(III) sulfide
Write the formulas for the following chemical compounds:
11)
silicon dioxide
SiO2
12)
nickel (III) sulfide
Ni2S3
13)
manganese (II) phosphate Mn3(PO4)2
14)
silver acetate
AgC2H3O2
15)
diboron tetrabromide
B2Br4
16)
magnesium sulfate heptahydrate
17)
potassium carbonate
18)
ammonium oxide
(NH4)2O
19)
tin (IV) selenide
SnSe2
20)
carbon tetrachloride
CCl4
MgSO4.7H2O
K2CO3
Naming Acids
Name the following acids.
1.
HIO3
iodic acid
2.
HI
hydroiodic acid
3.
H2SO4
sulfuric acid
4.
H2SO3
sulfurous acid
5.
H2S
hydrosulfuric acid
Convert the following names of acids to formulas.
6.
iodous acid
HIO2
7.
sulfurous acid
H2SO3
8.
sulfuric acid
H2SO4
9.
perchloric acid HClO4
10. phosphoric acid H3PO4
Metallic Bonding
1)
What are the two types of alloy, and how do they differ from one another?
Interstitial alloys are alloys in which one element takes up the spaces
between the atoms of the other metal. Substitutional alloys are
alloys in which the atoms of one element in the lattice are replaced
by atoms of other elements.
2)
How is bonding in metals different than bonding in either ionic or covalent
compounds?
In metals, the bonding electrons are delocalized among all of the
atoms. As a result, the most common analogy for discussing
metallic bonding is the “electron sea theory” in which the nuclei are
islands of positive charge that are floating in a big ocean of electrons
that hold them all together.
Precipitate Reactions
1. LiCl ( ) + AgNO3 ( ) AgCl ( ) + LiNO3 ( )
2. Na2S ( ) + CaCl2 ( ) 2NaCl ( ) + CaS ( )
3. ZnCl2 ( ) + 2KOH ( ) Zn(OH)2 ( ) + 2KCl ( )
4. Na2CO3 ( ) + Co(NO3)2 ( ) 2NaNO3 ( ) + CoCO3 ( )
Compare and contrast ionic and covalent compounds.
Ionic Compounds
1.
2.
3.
4.
Crystalline solids (made of ions)
High melting and boiling points
Conduct electricity when melted
Many soluble in water but not in nonpolar
liquid
Covalent Compounds
1.
2.
3.
4.
Gases, liquids, or solids (made of
molecules)
Low melting and boiling points
Poor electrical conductors in all phases
Many soluble in nonpolar liquids but not in
water
VSEPR
For the following molecules, find the following.

Draw the Lewis structure

Determine the ABE formula

State the electron pair geometry and molecular geometry

Find formal charges
1. Water (dihydrogen monoxide)
2. Nitrogen triiodide
3. Carbon disulfide
4. Silicon tetrafluoride
5. Arsenic tribromide
6. Dihydrogen monosulfide
Polarity
For the following molecules:

Draw the Lewis Structure

Determine the molecular geometry

Determine if the bonds are polar/nonpolar/ionic.

Determine if the overall molecule is polar.
7. Oxygen gas
8. Selenium dibromide
9. Iodine pentachloride
10. Sulfur tetrafluoride
11. Xenon trichloride
12. Hydrochloric acid