1. Which of the following is a physical property?
A. corrosion of aluminum metal B. melting of ice
C. burning a match
D. an acid and base reacting
2. Which of the following solutions is the most acidic?
A. 0.5 M NH3
B. 0.3 M HNO3
C. 0.4 M HI
D. 0.7 M CH3OH
3. How many grams are in 1.45 L of a substance if the density
is 0.564 g/mL?
1.45 L x1000 mL/L = 1450 mL
D=m/V
0.564 g/mL = ‘x’ g/ 1450 mL
‘x’ = 818 g (sig figs)
4. You are given a bottle that contains 4.59 cm3 of a metallic
solid. The total mass of the bottle and solid is 35.66 g. The
empty bottle weighs 14.23 g. What is the density of the
solid?
35.66 g – 14.23 g = 21.43 g metallic solid
21.43 g / 4.59 mL (cm3) = 4.67 g/mL
5. _Polymers__ are made up of many smaller parts called
monomers. The element _C_ forms the backbone of nearly
all of these.
6. What is the correct atomic symbol for potassium-40?
A. 19K
B. 19K
C. 40K
D. 40K
7. Complete the following table.
Symbol
56
Fe3+
192
Os2+
197
Au3+
Protons
26
76
79
Neutrons
30
116
118
Electrons
23
74
76
Net
charge
3+
2+
3+
8. The element Mg has three naturally occurring isotopes.
The isotopic masses (amu) and % abundances are listed in
the table below. Find the average atomic mass.
Isotope
24
Mg
25
Mg
26
Mg
Abundance
78.99 %
10.00 %
11.01 %
Atomic
mass
(amu)
23.98504
24.98584
25.98259
.7899 x 23.98504 +
.1000 x 24.98584 +
.1101 x 25.98259 =
24.31 amu
9. Which of the following ions (denoted by their charge) have
the strongest attraction?
A. +1, +2, r=2
B. -2, +3, r=3
C. -1, -1, r=1
D. -2, +2, r=1
10.
Compound
Name
lithium nitrate
phosphorous
pentafluoride
silicon
tetrachloride
mercury (II)
bromide
aluminum
hydroxide
Compound
Formula
LiNO3
ionic or
molecular?
ionic
PF5
molecular
SiCl4
molecular
HgBr2
ionic
Al(OH)3
ionic
11. Write the correct molecular formula for this compound.
C22H28ON2
12. Which of the following is not a type of chemical bond?
A. molecular
B. ionic
C. metallic
D. covalent
Bad question! B,C, and D are the main names we talked
about,though.
13. Which of the following is a halogen?
A. bromine
C. potassium
B. sodium
D. oxygen
14. Complete and balance the following reaction.
2C3H6(g) + 9O2(g)
6CO2 + 6H2O
15. How many atoms of N are present in 3.1 mg N2O?
3.1 mg x 1 g/1000 mg x 1 mol N2O/44.0128 g x
2 mol N/1 mol N2O x 6.022x1023/mol =
8.5 x 1019 atoms N
16. How many grams of solute are present in 37.2 mL of
0.471 M HBr?
0.471 M = x mol/ .0372 L
‘x’ = .0175 mol HBr x 80.9 g/mol = 1.417 g HBr
17. What ion would you have to add to increase the acidity
(decrease the pH) of a solution? H+
18. Complete the following equation, then write the
complete and net ionic equations. Are there any
spectators? Is there a precipitant?
Ba(NO3)2 + Na2SO4
BaSO4(s) + 2 NaNO3(aq)
net ionic: Ba2+(aq) + SO42-(aq)
BaSO4(s)
spectators are Na+ and NO3-. Precipitant is the solid.
19. How many grams of aluminum sulfate are produced when
2.64 g of aluminum hydroxide is reacted with excess
sulfuric acid?
2Al(OH)3(s)
+
3H2SO4(aq)
Al2(SO4)3(aq) +
6H2O(l)
2.64 g Al(OH)3 x 1 mol x 1 mol Al2(SO4)3 x 342.14 g = 5.79 g Al2(SO4)3
78.01 g
2 mol Al(OH)3
1 mol
20. A compound consists of 75.69% C, 8.80% H, and 15.51% O
by mass. Determine the empirical formula as well as the
molecular formula if the molar mass is determined to be 412
g/mol. .
*Assume 100 g
75.69g C x 1 mol/12.01 g = 6.30 mol C
8.80g H x 1 mol/1.01 g = 8.71 mol H
15.51g O x 1 mol/16.00 g = 0.97 mol O
*divide all by 0.97 to equal 6.5 mol C, 9 mol H, 1 mol O, times by 2
Emp. formula = C13H18O2
Mol. formula= C26H36O4