CHEMISTRY REVIEW
1. Name 4 families on the periodic table. Why do elements in these families have similar properties?
Alkali Metals (H, Li, Na, K, Rb, Cs, Fr)
Alkali Earth Metals (Be, Mg, Ca, Sr, Ba, Ra)
Halogens (F, Cl, Br, I At)
Noble Gases (He, Ne, Ar, KR, Xe, Rn)
- All members of a family have the same number of valence shell electrons!
2. Describe the structure of an atom – what it’s made of, where those particles reside, properties of those
particles.
Sub-atomic
Particles
Located where?
Charge
AMU (atomic mass
unit)
Calculated by
Protons
Nucleus
+
1
Electrons
Orbital/electron
shells
-
0
(so small, it’s
considered 0
compared to the
mass of a neutron
or proton)
Neutrons
nucleus
Neutral
1
Atomic number =
# protons, which
gives the atom its
identity
Atomic number =
# electrons for a
neutrally charge
atom. (Ions have
less or more
electrons than
normal.)
Atomic mass/mass
number/atomic
weight (all mean
the same thing) =
protons + neutrons,
therefore:
Atomic mass –
atomic number =
#neutrons
3. How many protons does 20782Pb have? How many neutrons? Electrons?
Protons = 82, electrons = 82,
neutrons = 207-82= 125
4. Draw a Bohr diagram for chlorine, helium, potassium, carbon.
5. Draw Lewis diagrams for the same atoms.
6. What is the difference between an ionic and a covalent bond? What is the reason for any bond, ionic
or covalent, to form at all?
Ionic: metal + non-metal, electron transfer
Covalent: non-metal + non-metal, electron sharing
7. Explain how to figure out what ions are formed when ionic compounds dissolve, and what their charges
are.
When an ionic compound dissolves, the ions separate individually. You can write a dissolving equation by
looking at the formula and the charges of each ion.
e.g. Na2O  (dissolves) Na+ + Na+ + O2or, simplified:
Na2O  (dissolves) 2Na++ O28. Explain the difference in how covalents and ionics are named.
See notes from last class.
9. Write the correct formulas for the following compounds:
a. sodium bromide
NaBr
d. iron (II) nitride
Fe3N2
e. iron (II) nitrate
Fe(NO3)2
h) silicon dioxide
SiO2
j) carbon tetraiodide
CI4
l) chlorine gas
Cl2
(It’s one of the seven diatomic covalent compounds you memorized last year: Cl2, F2, Br2, I2, O2, N2, H2. All
of these elements exist diatomically – two atoms together – when they are not combined with other
elements.)
10. Write the correct names for the following compounds:
a) Ag2O
silver oxide
b) CuSO4
copper(II) sulfate
c) K2O
potassium oxide
d) LiOH
lithium hydroxide
e) Ni2O3
nickel (III) oxide
11. What makes an acid an acid? What makes a base a base?
Acids donate hydrogen and bases accept hydrogen in neutralization reactions.
12. Explain how water is formed in a neutralization reaction.
The acid and base combine to form a “salt” (a neutral ionic compound) and water.
e.g. LiOH + HCl  LiCl + H2O
base acid
“salt” water
13. Write a balanced neutralization reaction for the following acid/base combo:
2 HNO3 + Ca(OH)2  2 H2O + Ca(NO3)2
14. Balance and classify the following reactions:
a) single displacement: 2 Al + 6 HCl → 2 AlCl3 + 3 H2
b) synthesis: 2 Sr + O2 → 2 SrO
c)
combustion: C6H12O6 +
6 O2 →
6 CO2 +
6 H2O
d) tin(IV) hydroxide produces tin(IV) oxide and water
decomposition: Sn(OH)4  SnO2 +2 H2O
e)
double displacement: Al2(SO4)3 +
3 K2CrO4 → 3 K2SO4 +
Al2(CrO4)3
15. Predict the products of the following equations and balance them:
a) SD:
F2 +
2 NaCl → 2 NaF + Cl2
b) SD:
Cu +
AgNO3 → CuNO3 + Ag
or
Cu +
if you assumed Cu was copper(I)
2 AgNO3 → Cu(NO3)2 +2 Ag if you assumed Cu was copper (II)
c) DD:
3 NH4OH +
d) DD:
SrBr2 +
H3PO4 → (NH4)3PO4 +3 H2O
(NH4)2CO3 → SrCO3 + 2 NH4Br
IONIC COMPOUNDS (SEE POWERPOINT)
A combination between:
Which ion goes first?
How to figure out their formulas OR
What ratios elements will combine in?
e.g.
How to write their names:
e.g.
When to use Roman numerals:
e.g.
Where do Roman numerals go in the name?
e.g.
What is a polyatomic ion?
How do polyatomic ions change naming rules?
The only polyatomic ion to end in “ide”:
COVALENT COMPOUNDS
A combination between:
How are the naming rules different than ionic compounds?