CHM 130
PRACTICE WORKSHEET #2
1. Write the electronic configuration for:
a) bromine, b) iron, c) carbon, d) Na+1, e) neon
2. Write the Lewis structures for:
a) argon, b) aluminum, c) sulfur, d) fluoride (F-1), e) Ca+2
3. A 25.0 gram rock was placed in a graduated cylinder containing 36.5 mL. The
water level in the graduated cylinder now reads to 44.0 mL. Calculate the
density of the rock in g/cc.
4. Convert -20.00F to degrees Celsius.
5. Calculate the volume of alcohol needed to obtain 100.0 g if it has a
density of 0.80 g/cc.
6. Complete the following nuclear reactions.
2
4
a)
H + He

________
1
2
=========================================================
236
144
1
b)
U 
Cs + _______ + 2 n
92
55
0
=========================================================
239
4
c)
Pu 
_________
+ He
94
2
=========================================================
14
0
d)
_________

N +
e (beta -)
7
-1
========================================================
27
4
30
e)
Al + He -------->
P
+ ______
13
2
15
7.
What would be the mass of 50 mL of concentrated sulfuric acid
(specific gravity = 1.8)?
8.
Write the Lewis structure for:
9.
A sample of metal having a mass of 6.25 grams was found to react with
exactly 2.85 grams of oxygen. Calculate the percentage of oxygen in the
metal oxide.
10.
Calculate the number of grams in 5.5 moles of isopropyl alcohol, C3H7OH.
11.
An organic compound has a chemical composition of 82.7% carbon and 17.3%
hydrogen. Calculate the Empirical formula for the compound.
12.
Write the Lewis structure for:
a) C, b) Na, c) Br, d) He, e) Al
a) K, b) arsenic, c) S, d) argon, e) neon
13.
Write the electron configuration for: a) Cl, b) Si, c) P, d) Na, c)Ne
14.
Calculate the percentage of water in NiSO4 .6H2O.
15.
A sample of metal having a mass of 5.40 grams was found to react with
exactly 3.10 grams of oxygen. Calculate the percentage of oxygen in the
metal oxide.
16.
Calculate the molecular mass of (NH4)2 CO3.
17.
Calculate the number of grams of isopropyl alcohol, C3H7OH, in 3.50 moles
of the alcohol.
18.
An alloy of copper and zinc contains 25.0 percent zinc.
amount of alloy that contains 48.0 grams of zinc.
Calculate the
19.
Butane is an organic compound made of carbon and hydrogen.
It has a
molecular mass of 58.0 grams/mole and a composition of 82.7% carbon and
17.3% hydrogen. Calculate the simplest formula and the true formula for
butane.
20.
Write the Lewis structure for:
a) aluminum, b) sulfur, c) krypton, d) Cl-1, e) barium
21.
Write the electron configuration for:
a) calcium, b) neon, c) Br, d) Na+1, e) K
22.
Calculate the mass of 400. mL of concentrated sulfuric acid
(specific gravity = 1.8).
23.
A 3.60 gram sample of hydrated salt was found to have a mass of 2.20
grams after heating. Calculate the percent water in the hydrated salt.
24.
What is the Celsius equivalent to 20.00F?
25.
A rock having a mass of 18.65 grams was placed into a graduated cylinder
containing 42.6 mL of water. The water level rose to 49.7 mL. Calculate the
density of the rock in gm/cc.
26.
Find the volume occupied by 48.0 grams of alcohol (Sp. G. =
27.
A copper-zinc alloy contains 30.0% copper. Calculate the mass of copper
contained in 150. grams of the alloy.
28.
Calculate the molecular mass of aluminum sulfate,
Al2(SO4)3.
29.
Calculate the percent hydrogen in phosphorous acid, H3PO3.
30.
What is the empirical formula of a compound that has the following percent
composition: 14.6% C, 39.0% O and 46.4% F?
0.80).
31.
Calculate the percent oxygen in an oxide if 6.8 grams of metal reacts with
5.4 grams of oxygen to form the metal oxide.
32.
Calculate the number of grams equivalent to 0.25 moles of CaCO3.
33.
Convert 20.00F to degrees Celsius.
34.
A compound contains 78.3% boron and 21.7% hydrogen. The molecular mass
of the compound is 27.6 grams/mole. Calculate the empirical and molecular
formulas for the compound.
35.
Write the electron configurations for the following:
a) fluorine, b) Mg+2, c) Kr(36), d) potassium, e) nickel
36.
Calculate the molecular mass of aluminum hydroxide, Al(OH)3.
37.
Calculate the percent hydrogen in nitrous acid, HNO2.
38.
What is the empirical formula of a compound that has the following percent
composition: 41.0% K, 33.7% S and 25.3% O?
39.
Calculate the percent oxygen in an oxide if 6.8 grams of metal reacts with
oxygen to form 12.4 grams of the metal oxide.
40.
Draw the Lewis structures for:
a) phosphorus, b) K+1, c) bromine, d) Ne(10), e) S-2
41.
Calculate the number of moles equivalent to 50.0 grams CaCO3.
42.
Convert -15.00F to degrees Celsius.
43.
A compound contains 73.7% carbon, 3.8% hydrogen and 10.7% nitrogen. The
molecular mass of the compound is 235 grams/mole. Calculate the empirical
and molecular formulas for the compound.
43.
Calculate the percent of water in CuSO4 .5H2O.
44.
A sample of metal sulfide having a mass of 4.60 grams was found to contain
2.20 grams of sulfur. Calculate the percent of sulfur in the metal sulfide.
45.
Calculate the number of grams of H2SO4 and the number of moles of
H2SO4 in 100. mL of concentrated sulfuric acid. (Density = 1.8 g/mL)
47.
Calculate the number of grams of ethyl alcohol, C2H5OH. In 8.0 moles of the
alcohol.
48.
An alloy of gold and nickel contains 25.0 percent gold.
of nickel needed to make 48.0 grams of the alloy.
49.
Butane is a organic compound made of carbon and hydrogen.
It has a
molecular mass of 58.0 grams/mole and a composition of 82.7% carbon and
17.3% hydrogen. Calculate the simplest formula and the true formula for
butane.
50.
Write the electron configuration for: a) Ca, b) Zn, c) Ar, d) Br, e) Fe
Calculate the mass