RHS Chemistry Review December 2014
Give a definition and example of each of the following:
This section you should have been able to do without help.
Major Topics
1. Atomic Theory: Describe what each scientist contributed to the atomic theory:
a. Dalton-Created the atomic theory, know the points from your notes and that he
thought atoms were indivisible, which is wrong.
b. Thompson-Discovered the electron and had the plum pudding model
c. Rutherford-gold foil experiment, discovered the nucleus
d. Bohr-Planetary Model (Saturn) showing how electrons are arranged around the
nucleus
2. The atom: Give the charge, location and mass of the following subatomic particles:
a. Proton-Positive, inside the nucleus, 1 a.m.u
b. Neutron-Neutral, inside the nucleus, 1 a.m.u
c. Electron-Negative, outside the nucleus, 0 a.m.u
3. Periodic trends: Explain the general trends of the following:
a. Electronegativity-. It is how strong an atom can pull electrons away from another
atom. (Does not include noble gases). Increases as you go from left to right across the
periodic table and bottom to top
b. Atomic Radius- How big the atom is. Increases as you from right to left across the
periodic table and top to bottom, Francium is largest atomic radius.
c. Ionic Radius-When an atom loses/gains electrons, it changes the size of the atom. If it
gains, it gets bigger, if it loses, it gets smaller. There are different trends for each type
of ion. Anions get larger as you go from right to left and down the periodic table.
Cations get smaller as you go from right to left and down the periodic table.
d. Ionization Energy- How easily an atom ionizes. follows the same pattern as
electronegativity.
4. Radioactivity: Give the symbol of each and an example equation for each
a. Alpha;

+
b. Beta- ;

+
c. Gamma
;

+
+
5. Radioactivity: List these in order of increasing penetrating power: Beta, Gamma, Alpha
Alpha, Beta, Gamma
Skills:
1. Sig Figs:
a. How many sig figs are in the following numbers:
i. 0.000023
2
ii. 5690
3
iii. 451.005
6
iv. 0.001020
4
3
v. 4.20 x 10
3
b. Answer the following in correct sig figs:
i. 332.968 cm + 894.85 cm
1227.82 cm
ii. 87.50 cm – 10 cm
78 cm
iii. 2.30 L x 6.1 L
14 L
iv. 89.5 g/783.1 g
0.114 g
c. Put these in correct scientific notation:
i. 509000000000
5.9 x 1011
ii. 0.000000040
4.0 x 10-8
iii. 0.003
3 x 10-3
iv. 10000000
1 x 107
d. Put these in correct decimal form:
i. 6.02 x 108
602000000
-5
ii. 5.6 x 10
0.000056
2. Metric Conversions
a. 1000L = ________mL
1000000 mL
b. 723 km = _______cm
73200000 cm
c. 67.0 mm = _______m
0.067 m
d. 9 m = ________nm
9 x 109 nm
3. Density:
a. Use the Density equation in the following (in correct sig figs):
i. Mass = 15 g; Volume = 5 L
= 3 g/mL
ii. Mass = 100g; Density = 2.15 g/mL
= 47 mL
iii. Volume = 54 mL; Density = 1.56 g/mL
= 84 g
4. Average Atomic Mass
Isotopes of Magnesium
Percent abundance
Mg - 24
78.99%
=18.9576
Mg – 25
10.00%
=2.5
Mg - 26
11.01%
=2.8626
a. Calculate the average atomic mass using the table above
Add the three numbers together to get  24.32
5. Radioactive Decay: Fill in the missing particle in the nuclear equation.
a.
 __________ +
b.

6. Wave Problems:
+ _________
a. A light wave has a frequency of 8.75 x 1015 Hz. What is its wavelength?
C = f x λ; Rearrange to λ = C/f  3.00 x 108 / 8.75 x 1015 = 3.4 x 10-8 m.
b. A light wave has a frequency of 6.35 x 1015 Hz. What is its energy?
E = h x f (no rearranging needed)  h = is given to you on formula chart
6.63 x 10-34 x 6.35 x 1015 =4.21 x 10-18 J
c. A red light is found to have a wavelength of 674 nm. Calculate its frequency.
Convert 674 nm to meters  6.74 x 10-7 m
C = f x λ; Rearrange to f = C/ λ 3.00 x 108 / 6.74 x 10-7 m = 4.45 x 1014 hz
7. Electron Configurations:
a. Write out the electrons configuration for the following elements:
i. Magnesium
1s22s22p63s2
ii. Indium
1s22s22p63s23p64s23d104p65s24d105p1
iii. Strontium
1s22s22p63s23p64s23d104p65s2
b. Name the element for the following electron configurations
i. 1s22s22p63s23p64s23d5
Mn, Manganese
ii. 1s22s22p63s23p4
S, Sulfur
iii. 1s22s22p63s23p64s23d104p65s24d105p3
Sb, Antimony
c. Write out the ion electron configuration of the following elements
i. Fluorine
1s22s22p6
ii. Calcium
1s22s22p63s23p6
8. Ionic Bonding and Compounds:
a. Binary (Give the opposite):
i. BaS
Barium Sulfide
ii. Li3N
Lithium Nitride
iii. Magnesium phosphide,
Mg3P2
iv. Cesium chloride
CsCl
b. Polyatomics (Give the opposite):
i. NaOH
Sodium Hydroxide
ii. Fe2(SO4)3
Iron (III) Sulfate
iii. Potassium dichromate
K2Cr2O7
iv. Ammonium Carbonate
(NH4)2CO3
c. Transition Metals
i. CuO
Copper (II) Oxide
ii. MnS2
Manganese (IV) Sulfide
iii. Nickel (II) Arsenide
Ni3As2
iv. Cobalt (III) Acetate
Co(C2H3O2)3
d. Mixed:
i. Ca(OH)2
Calcium Hydroxide
ii. K2Cr2O7
Potassium Dichromate
iii. Ag3P
Silver Phosphide
iv. (NH4)2SO4
Ammonium Sulfate
v. Chromium (II) Borate
Cr3(BO3)2
vi. Sodium Chlorite
NaClO2
vii. Ammonium Sulfite
viii. Lead (II) Carbonate
(NH4)2SO3
PbCO3
9. Lewis Structures:
a. Single Element Dot Diagrams-Draw the dot diagrams for these elements
i. Nitrogen
ii. Oxygen
iii. He
iv. Mg
b. Bonding Diagrams (Draw the dot diagrams of each compound):
i. NaCl
ii. Aluminum Sulfide
iii. BeCl2
iv. Lithium Nitride