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Final Review

Total questions: 56

Worksheet time: 4hrs 48mins

Name
Class
Date
1.

why would O2 effuse faster than CO2 in the same room

a)

because it has more energy

b)

because it has a smaller molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

2.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
3.
On the basis of the pH curve, the pKa value of the acid is closest to 
a)
4
b)
5
c)
8
d)
12
4.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
5.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
6.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
7.

Which of the following is a correctly written balanced equation of synthesis?

a)

2Na + Br2 -->2 NaBr

b)

Na + 2Br --> NaBr2

c)

HgO + Cl2-->HgCl + O2

d)

Cl2 +Na--> NaCl2

8.

Which BALANCED equation correctly represents the decomposition of sodium chloride?

a)

Na +Cl2 → 2NaCl

b)

NaCl →Na +Cl

c)

2NaCl →2Na +Cl2

d)

NaCl →Na +Cl

9.
Find the percent composition of N2S2.
a)
N: 69.6%  S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
10.
How many moles are in 88 g of propane, C3H8. 
a)
2.0
b)
16.0
c)
0.051
d)
3,872
11.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
12.

Yellow dye is separated from a mixture using a polar stationary phase (filter paper) and non-polar mobile phase (solvent). The yellow dye is:

a)

polar

b)

nonpolar

13.
Which of the following is a general characteristic of a nonmetal?
a)
Low Density
b)
Nonconductor of heat
c)
Brittle
d)
All of the above
14.
Which one of the following elements has the greatest ionization energy?
a)
Al
b)
Cl
c)
Br
d)
S
15.
Which of the following is true of an element in an excited state?
a)
It has emitted a photon and its energy has decreased
b)
It has emitted a photon and its energy has increased
c)
It has absorbed a photon and its energy has increased
d)
It has absorbed a neutron and its energy has increased
16.
Which one of these molecules has a trigonal pyramidal molecular geometry?
a)
SO3
b)
NF3
c)
IF3
d)
BF3
17.
Which molecular geometry tends to be nonpolar?
a)
Bent
b)
Trigonal Pyramidal
c)
Trigonal Bipyramidal
d)
Square Pyramidal
18.
What is the name for the force holding two atoms together in a chemical bond?
a)
Gravitational force
b)
Strong nuclear force
c)
Weak nuclear force
d)
Electrostatic force
19.
Which of the following molecules is polar?
a)
SO3
b)
SO2
c)
CO2
d)
CH4
20.
An alkaline earth metal is expected to have a _____ ionization energy and a _____ electron affinity.
a)
small; large
b)
small; small
c)
large; small
d)
large; large
21.
Which of the following compounds will have the lowest boiling point?
a)
CH4
b)
CHCl3
c)
CH3CH2OH
d)
NH3
22.
Under which conditions does a real gas behave most nearly like an ideal gas?
a)
High Temperature and High Pressure
b)
High Temperature and Low Pressure
c)
Low Temperature and Low Pressure
d)
Low temperature and High Pressure
23.
A 2.50 L sample of He gas has a pressure of 0.925 atm.  What is the pressure of the gas if the volume is reduced to 0.350 L?
a)
6.61 atm
b)
0.661 atm
c)
0.130 atm
d)
0.946 atm
24.
Which of the following solid compounds is insoluble in water?
a)
barium sulfate
b)
barium hydroxide
c)
barium chloride
d)
barium chlorate
25.
Which of the following elements will form a covalent network solid?
a)
C
b)
O
c)
Mg
d)
S
26.
Which of the following would be a weak electrolyte in a solution?
a)
HBr
b)
KCl
c)
KOH
d)
HC2H3O2
27.

Which of the following is NOT true about ionic compounds?

a)

They conduct electricity when in the liquid state

b)

They are comprised of positive and negative ions

c)

They are ductile (can be made into wire)

d)

They are brittle (break easily)

28.

What type of hybridization does C have in CH2OH?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

29.

How many sigma and pi bonds are in C2H2?

a)

3 sigma and 1 pi

b)

3 sigma, 2 pi

c)

4 sigma, 1 pi

d)

4 sigma, 2 pi

30.

Which of the following is NOT isoelectronic with the other species?

a)

S2-

b)

Br-

c)

Kr

d)

Sr2+

31.

Which Lewis dot structure shows exactly two unshared pairs of valence electrons?

a)

H2S

b)

CO2

c)

NH3

d)

CBr4

32.

What is the correct coefficient for O2 when this reaction is balanced?

a)

3

b)

5

c)

6

d)

10

33.

Identify the reaction type:

C2H6 + O2 --> CO2 + H2O

a)

Double replacement

b)

Synthesis

c)

Acid base

d)

Combustion

34.
Identify the following element:
1s22s22p63s23p64s23d10
a)
nickel
b)
copper
c)
zinc
d)
gallium
35.
If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?
a)
6.59 x 10^-28 m
b)
1.01 x 10^-6 m
c)
3.32 x 10^-3 m
d)
301 m
36.

What is the molecular weight of this compound?

a)

29

b)

87

c)

54

d)

15

37.
What do the peaks on the mass spectrum represent?
a)
anions
b)
different isotopes
c)
atoms with differing numbers of electrons
d)
numbers of electrons
38.
What do the heights of the peaks represent in the mass spectrum?
a)
number of isotopes
b)
relative abundance of each isotope
c)
average atomic mass
d)
charge:mass ratio
39.
Which of the following type of electromagnetic radiation affects the bonds,vibrating ,stretching rocking...
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
40.
Which of the following type of electromagnetic radiation affects spin of the nucleons
a)
infrared
b)
ultraviolet
c)
microwaves
d)
radiowaves
41.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL?
a)
4.88 M
b)
4.880 M
c)
2.440 M
d)
2.44 M
42.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
43.
A sample of iron receives 50J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?
a)
25g
b)
30g
c)
20g
d)
50g
44.
Which of the following is not a strong acid?
a)
HCl
b)
HF
c)
HBr
d)
HNO3
45.
How much does 100,000,000 (1 * 108) atoms of gold weigh?
a)
2.617 * 10-13 g
b)
1.308 * 10-13 g
c)
3.271 * 10-14 g
d)
6.542 * 10-14 g
46.
What is the endpoint of a titration
a)
Where the amount of acid and base are equal as shown by a colour change 
b)
Where there is no base
c)
When the volume of base in the burette is used up 
d)
When there is no acid
47.
What are the products of the neutralization shown below?
Ca(OH)2  +  H2CO3  -->  
a)
H2O  +  Ca2CO3
b)
CaO +  CO3
c)
H2O  +  CaCO3
48.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
49.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
50.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
51.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
52.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
53.
When two nonmetals do not share electrons evenly, the resulting covalent bond will be
a)
nonpolar
b)
polar
c)
ionic
d)
metallic
54.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
55.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
56.

The question below is about the Maxwell–Boltzmann distribution shown for a sample of a gas, X, at two different temperatures.


Which statement is correct for the higher temperature?

a)

The area under the curve to the left of Ea decreases.

b)

The total area under the curve increases.

c)

The activation energy decreases.

d)

More molecules have the mean energy.

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