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semester 2 final review

Total questions: 80

Worksheet time: 3hrs 7mins

Name
Class
Date
1.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
2.

Classify the following molecule.

a)

polar

b)

nonpolar

3.

Classify the following molecule.

a)

polar

b)

nonpolar

4.

Classify the following molecule.

a)

polar

b)

nonpolar

5.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

6.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

7.

What type of bond would form between O and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

8.

Match the charge with the groups.

a)

-1

1.

Group 17

b)

-3

2.

Group 15

c)

-2

3.

Group 16

9.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

10.

In a(n) ________ electrons are transferred from one atom to another

a)

ionic compound

b)

covalent compound

11.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
12.
Carbonate
a)
Cr2O4-2
b)
CH3COO-
c)
CO3-2
d)
CN-
13.
Hydroxide
a)
Cr2O4-2
b)
Cr2O4-2
c)
O3-2
d)
OH-
14.
Sulfate
a)
S2O3-2
b)
O2-2
c)
SO4-2
d)
SO3-2
15.
The elements on the left side of the periodic table are generally always ______ and the elements on the right side of the periodic table are generally always ______.
a)
cations; anions
b)
anions; cations
c)
reactive; non-reactive
d)
non-reactive; reactive
16.
An example of a polyatomic ion is:
a)
O2-
b)
Na+
c)
CO32-
d)
Ag+
17.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
18.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
19.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
20.

What is the correct name for the compound NaNO₃?

a)

sodium nitride

b)

sodium nitrogen trioxide

c)

sodium nitrate

d)

sodium nitrogen oxide

21.

What is the correct name for CO₂?

a)

carbon monoxide

b)

carbon dioxide

c)

monocarbon monoxide

d)

carbon oxide

22.

Name the ionic compound, LiCl

a)

lithium chlorine

b)

lithium chloride

c)

lithium chlorate

d)

lithium monochloride

23.

What is the correct name for the compound NaCl?

a)

sodium chloride

b)

sodium chlorate

c)

sodium carbonate

d)

sodium nitrate

24.

What is the correct name for the compound MgSO4?

a)

magnesium sulfate

b)

magnesium sulfite

c)

magnesium sulfide

d)

manganese sulfate

25.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
26.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
27.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
28.
Where do you look to calculate the molar mass?
a)
avogadros number
b)
periodic table 
29.
What is the molar mass of one molecule of Nitrogen N2?
a)
14.01 amu
b)
14.01 g
c)
28.02 g
d)
28.02 amu
30.
What is the molar mass of Carbon Dioxide (CO2)?
a)
12 amu
b)
12 g
c)
44 g
d)
44 amu
31.
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%
32.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
33.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

0.8291 moles

d)

0.0829 moles

34.
If an atom of Fluorine has an atomic mass of 19 amu, it has a Molar mass of ____
a)
19 lbs.
b)
19 kg
c)
How am I supposed to know?
d)
19 g/mol
35.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
36.
Which has more atoms, 12.0 mol of C or 12.0 mol of Ca?
a)
12.0 mol C
b)
12.0 mol Ca
c)
They are equal
37.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
38.

What is the mass percentage of Carbon in Carbon dioxide (CO2)?

a)

27.27%

b)

42.86%

c)

72.73%

d)

72.72%

39.

What is the empirical formula of a substance with the molecular formula C2H4?

a)

C2H2

b)

C2H2

c)

C1H1

d)

CH2

40.

If the empirical formula of a compound is C2H4 and its molar mass is 56 g/mol, what is its molecular formula?

a)

C4H8

b)

C2H6

c)

C3H6

d)

C6H12

41.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

42.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
43.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
44.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
45.
a)

A

b)

B

c)

C

d)

D

46.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
47.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
48.

Which particles are transferred during a redox reaction?

a)

atoms

b)

electrons

c)

neutrons

d)

positrons

49.

Given the equation representing a reaction: 2Ca(s) + O2(g) → 2CaO(s), during this reaction, each element changes in

a)

atomic number

b)

oxidation number

c)

number of protons per atom

d)

number of neutrons per atom

50.

Given the equation representing a reaction:

3CuCl2(aq) + 2Al(s) → 3Cu(s) + 2AlCl3(aq)

the oxidation number of copper changes from

a)

+1 to 0

b)

+2 to 0

c)

+2 to +1

d)

+6 to +3

51.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

52.

What is the oxidation number of: Br2?

a)

-1

b)

+1

c)

-2

d)

0

53.

What is the oxidation number of Sr+2?

a)

-2

b)

0

c)

+2

d)

+1

54.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
55.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
56.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
57.
2NaClO3 (s) → 2NaCl (s) + 3O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
58.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
59.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
60.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
61.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
62.

Which of these is the shape of CCl4?

a)
b)
c)
d)
e)
63.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
64.

Which of the following shapes has an unshared pair of electrons on the central atom?

a)

linear

b)

trigonal pyramidal

c)

trigonal planar

d)

tetrahedral

65.

What geometry is shown here?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Tetrahedral

d)

Seesaw

66.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

67.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

68.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

69.

Which is true for the reaction below?

Na + Cl --> ___

a)

Na will donate an electron to Cl

b)

Cl with share electrons with Na

c)

a polar bond will form

d)

a metallic bond would form

70.

If the substance is neutral, what would the pH be?

a)

3

b)

5

c)

7

d)

9

e)

11

71.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

72.

Is this substance acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

73.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)

Cl-

74.

Name the following acid based on the molecular formula: HI

a)

ionic acid

b)

hydroiodic acid

c)

ioditic acid

d)

iodine acide

75.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
76.
NaCl is a ...
a)
acid
b)
base
c)
salt
d)
water
77.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

78.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

79.

A 0.050L solution of Ba(OH)2 is neutralized by 0.072L of a 0.55 M HNO3 solution. What is the concentration of the Ba(OH)2 solution?

a)

2 M

b)

0.40 M

c)

1.2 M

d)

None of the above

80.

What is the main purpose of acid-base titrations?

a)

To test if reactants react.

b)

To calculate the concentration of unknown acid or base.

c)

To test quality of reactants.

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