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Introduction and Quantitative Chemistry Quiz

Total questions: 122

Worksheet time: 6hrs 37mins

Name
Class
Date
1.
Define the term allotropes
a)
Atoms with same proton number but different number of neutrons
b)
Atoms with same proton number but different mass number
c)
Atoms in different arrangement in structure
d)
Atoms in different arrangement and different physical form
2.
Define the term metallic bonding
a)
Attraction between positive nuclei and electrons
b)
Forces attraction between nuclei and electron
c)
Forces attraction between nuclei and sea of electrons
d)
Electrostatic attraction between nuclei and sea of electrons
3.
Electronegativity is...
a)
how good an atom is at attracting 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. 
4.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
5.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
6.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
7.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
8.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
9.

An ionic compound forms between a _______ and _______.

a)

metal and non-metal

b)

two metals

c)

two non-metals

10.

Name the ionic compound, CaCO3

a)

calcium carbide

b)

calcium carbon trioxide

c)

calcium carbon oxide

d)

calcium carbonate

11.

Name the ionic compound, FeBr3

a)

Iron (II) bromide

b)

Iron (III) bromide

12.

Name the molecular compound CO

a)

carbon monoxide

b)

monocarbon monoxide

c)

carbide

d)

oxygen carbide

13.

Name the following compound:

CO2

a)

monocarbon dioxide

b)

carbon oxide

c)

carbon dioxide

d)

oxygen carbonide

14.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine
15.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

16.

What is the name for AlBr3?

a)

aluminum bromide

b)

aluminum tribromide

c)

aluminum bromine

d)

monoaluminum tribromide

17.
Name this compound.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
18.
Name this formula: 
Al2O3
a)
Aluminum Oxide
b)
Aluminum Oxygen
c)
Antimony Oxide
d)
Aluminum (VII) Oxide
19.
Name the compound Na2O
a)
Sodium Oxide
b)
Sodium Dioxide
c)
Sodium Oxygen
d)
Natride Oxide
20.
What is the formula for sulfur pentoxide?
a)
SO2
b)
SO3
c)
SO4
d)
SO5
21.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

22.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

23.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

24.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

25.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

26.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

27.
This is the correct dot diagram for nitrogen, group 15.
a)
true
b)
false
28.
How many electrons should Nitrogen, group 15, have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
29.
What is a cation? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
30.
What is a anion? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
31.
Why does K become positive when it bonds to Cl to form KCl?
a)
Because it loses an electron to have a full valence shell 
b)
Because it gains an electron to have 2 valence electrons
c)
Because it loses an electron to become negatively charged
d)
Because Cl gives away its 7 electrons to Na to form an equal charge 
32.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
33.
(NO3) - 
a)
Ionic
b)
Covalent
c)
Polyatomic Ion
d)
Metallic 
34.
O3
a)
Covalent
b)
Ionic
c)
Metallic
d)
Polyatomic Ion 
35.
Which of the following is nitrate?
a)
NO-
b)
NO2-
c)
NO3-
d)
NO4-
36.

What is the correct name for this polyatomic ion: OH–

a)

hydrogen carbonate

b)

oxonium

c)

hydroxide

d)

acetate

37.

What is the correct formula for the polyatomic ion called hydrogen carbonate?

a)

HCO3–

b)

CO32–

c)

CrO42–

d)

CN–

38.

What is the correct formula for the polyatomic ion called ammonium?

a)

NH3+

b)

NH3

c)

CN+

d)

NH4+

39.

CO32-

a)

carbonate

b)

sulfate

c)

phosphate

d)

ammonium

40.

SO42-

a)

carbonate

b)

sulfate

c)

phosphate

d)

ammonium

41.

PO43-

a)

carbonate

b)

sulfate

c)

phosphate

d)

ammonium

42.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
43.
What is the molar mass of sodium?
a)
11
b)
23
c)
45.98
d)
3
44.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
45.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
46.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
47.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
48.
What is the definition for Avogadro's number?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
49.
Which has a greater mass: 1 mole of scandium or 2 moles of boron?
a)
scandium
b)
boron
c)
neither
d)
more information is needed.
50.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40 g
b)
80 g
c)
16 g
d)
32 g
51.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
52.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
53.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
54.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
55.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
56.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
57.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
58.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
59.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
60.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
61.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
62.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
63.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
64.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
65.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
66.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
d)
Left side is balanced
67.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
68.
Which side of a chemical equation is the product side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
69.
Which problem is balanced?
a)
PbO2 + 2H2--> H2SO4
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
d)
2Na + 2H2O --> 2NaOH + H
70.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
71.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
6
c)
8
d)
24
72.
Which elements are(is) not balanced?
LiNO3 +CaBr2 --> Ca(NO3)2 +  LiBr   
a)
Li
b)
Ca and Li
c)
O and N
d)
Ca
73.
Balance the equation:
Si(OH)4+NaBr--> SiBr4+NaOH
a)
Si(OH)4+2NaBr--> SiBr4+NaOH
b)
Si(OH)4+4NaBr--> SiBr4+4NaOH
c)
Si(OH)4+NaBr--> SiBr4+4NaOH
d)
Si(OH)4+2NaBr--> SiBr4+2NaOH
74.
 Mg  +  ___ HCl  →   MgCl2  +   H2
a)
1
b)
2
c)
3
d)
4
75.

Concentration is

a)

the amount of solute in the solvent

b)

the amount of solvent in the solute

c)

density

d)

particle size

76.

Which solution is more concentrated?


Solution 1:

20 mL of water

5 g of salt


Solution 2:

20 mL of water

10 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally concentrated

77.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
78.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
79.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
80.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
81.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
82.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
83.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
84.

You need to make 200 mL of a 0.20 M aqueous solution of sodium chloride. The only available solution is 1.0 M. Determine how to make the needed dilution.

a)

Add 160 mL to the initial volume

b)

Add 160 grams to the initial volume

c)

Evaporate 160 mL from the initial volume

d)

the experiment cannot be conducted with the materials provided

85.

A dilution is when

a)

solute is added to the volume of stock solution

b)

water is added to the volume of stock solution

c)

solute is removed from the volume of stock solution

d)

water is removed from the volume of stock solution

86.

How many liters would you need to make a 1 M solution if you have 6 moles of Sodium Hydroxide?

a)

2

b)

3

c)

4

d)

6

87.

If I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if I add 560 mL more water to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

88.

If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

a)

2 M

b)

0.02 M

c)

0.03 M

d)

0.08 M

89.
When the temperature is constant (k) inside a balloon, if you add pressure on it, the volume will ..... 
a)
Decrease
b)
Increase
c)
Not Change at all
d)
Particles will solidify 
90.
For example, if you increase the temperature of a gas inside a balloon, the balloon will....
[pressure is constant (k)]
a)
Expand (increase in volume)
b)
Deflate (decrease in volume) 
91.
What is the name of the law that involves these two variables:
Temperature increases // Pressure increases 
a)
Gay-Lussac's Law
b)
Boyle's Law
c)
Charles' Law
d)
Ideal Gas Law 
92.
What is the name of the law that involves these two variables:
Pressure decreases // Volume increases 
a)
Boyle's Law
b)
Charles' Law
c)
Gay-Lussac's Law
d)
Ideal Gas Law 
93.
What 2 variables are used in a Hot Air Balloon? 
[Hint:  Space and Heat]
a)
Pressure and Volume
b)
Volume and Temperature
c)
Temperature and Pressure
d)
Pressure, Temperature and Volume 
94.
What Gas Law would a Hot Air Balloon "follow"  
[Hint:  Space and Heat]
a)
Gay-Lussac's Law
b)
Charles' Law
c)
Boyle's Law
d)
Ideal Gas Law
95.

How do you convert C to Kelvin (K)?

a)

C + 273

b)

C x 273

c)

C / 273

d)

C + 32 + 273

96.

What is the equation to solve for Boyle's Law?

a)

P1 (P2) = V1 (V2)

b)

P1 (V1) = P2 (V2)

c)

P1 / V1 = P2 / V2

d)

P1-V1 = P2 - V2

97.

What is the equation to solve for Charles' Law?

a)

P1 (P2) = V1 (V2)

b)

V1 / T1 = V2 / T2

c)

P1 / T1 = P2 / T2

d)

V1 / V2 = T1 / T2

98.

What variable is constant (k) in Boyle's Law?

a)

Pressure

b)

Volume

c)

Temperature

d)

# of moles

99.

What variable is constant (k) in Charles' Law?

a)

Pressure

b)

Volume

c)

Temperature

d)

# of moles

100.

What variable is constant (k) in Gay-Lussac's Law?

a)

Pressure

b)

Volume

c)

Temperature

d)

# of moles

101.

Select all gas laws that are directly proportional?

a)

Boyle's

b)

Charles

c)

Gay-Lussac's

d)

Ideal Gas Law

102.
Calculate:
I have 130 liters of gas in a piston at a temperature of 2500 C.  If I cool the gas until the volume decreases to 85 liters, what will temperature of the gas be? 
a)
163 K
b)
342 K
c)
800 K
103.
Calculate:
How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atmospheres and a temperature of  340 K? 
a)
9.89 atm
b)
5.48 atm 
c)
.10 atm
104.
What happens to the average kinetic energy of matter when it is heated?
a)
It increases
b)
It decreases 
c)
It doesn't change
d)
It cannot be determined
105.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
106.
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
107.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
108.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
109.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
110.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
111.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
112.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
113.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
114.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
115.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
116.
What is oxidation number of H in CaH2?
a)
+1
b)
-1
c)
0
d)
+2
117.

Defined as the gain of electrons.

a)

oxidation

b)

redox

c)

reduction

d)

LEO GER

118.

Defined as the loss of electrons.

a)

oxidation

b)

reduction

c)

redox

d)

OIL RIG

119.

Substance that reduces another substance by losing electrons.

a)

reducing agent

b)

half-reaction

c)

electronegative atom

d)

oxidizing agent

120.

Substance that oxidizes another substance by accepting its electrons.

a)

reducing agent

b)

oxidation number

c)

combustion

d)

oxidizing agent

121.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
122.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2

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