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Chemistry S2 Practice Test

Total questions: 110

Worksheet time: 7hrs 19mins

Name
Class
Date
1.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

2.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

3.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
4.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
5.

Identify the element for

[Kr] 5s2 4d3

a)

Vanadium (V)

b)

Iron (Fe)

c)

Niobium (Nb)

d)

Tantalum (Ta)

6.

What is the electron configuration for boron?

a)

1s22s2

b)

1s22s22p2

c)

1s22s22p1

d)

[Li]2s22p1

7.

What is the (shorthand) noble gas configuration for beryllium?

a)

[He]1s2

b)

[He]2s2

c)

[Li]2s1

d)

[Li]2s2

8.

What is the (shorthand) noble gas configuration for Sulfur?

a)

[Ar] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

9.

1s22s22p4 is the electron configuration for which element?

a)

oxygen

b)

sulfur

c)

phosphorus

d)

fluorine

10.

the lowest energy level an electron occupies is the ______

a)

ground state

b)

excited state

c)

stable state

d)

neutral state

11.

Which element has the lowest ionization energy?

a)

Ca

b)

K

c)

O

d)

F

12.

The electron configuration of an atom is 1s22s22p6. The total number of electrons in the atom is

a)

3

b)

6

c)

8

d)

10

13.

An s orbital can hold a maximum of how many electrons?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

14.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
15.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
16.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
17.

An atom that gains or loses an electron becomes

a)

an isotope

b)

a new element

c)

an ion

d)

a molecule

18.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
19.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

20.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

21.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

22.

A compound forms between a metal and a nonmetal. It is

a)

ionic

b)

metallic

c)

covalent

23.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

24.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

25.

According to the Octet Rule, atoms want ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

26.

Which compound has high melting point?

a)

Ionic

b)

Covalent

27.

Which of these are properties of Covalent Bonds?

Categorize the following

High Boiling point

High Melting Point

Share Electrons

Non-Conductive

Low Melting Point

Low Boiling Point

Conductive

Only conductive when dissolved

Transfer Electrons

Property of Covalent Bonds
Not A property of covalent bonds
28.

Which is the correct structure for NH3 (ammonia)? (Top picture is A, bottom picture is D.)

a)
Option A
b)
Option B
c)
Option C
d)
Option D
29.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
30.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
31.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
32.

Which of the following is the correct Lewis Dot Diagram for Hydrogen Cyanide, HCN?

a)

A

b)

B

c)

C

d)

D

33.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
34.
 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
35.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
36.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
37.
What is the Molecular Geometry of the molecule?
a)
Linear
b)
Bent, 120o
c)
Bent, 109.5o
d)
Trigonal Planar
38.
What is the Molecular Geometry of the molecule?
a)
Linear
b)
Bent, 120o
c)
Bent, 109.5o
d)
Trigonal Planar
39.
The water droplets on this glass of water is showing the following phase change
a)
melting
b)
evaporation
c)
freezing 
d)
condensation
40.

Which section of the phase change diagram is indicated?

a)

liquid

b)

solid

c)

melting

d)

freezing

41.

Which section of the phase change diagram is indicated?

a)

Gas

b)

Liquid

c)

Vaporization

d)

Condensation

42.

Which section of the phase change diagram is indicated?

a)

Freezing

b)

Melting

c)

Solid

d)

Liquid

43.

Which section of the phase change diagram is indicated?

a)

Condensation

b)

Vaporization

c)

Liquid

d)

Gas

44.
What state of matter is Y?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
45.
What state of matter is Z?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
46.
What change occurs from F to E?
a)
sublimation
b)
deposition
c)
melting
d)
condensation
47.
What is point A?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
48.
At 0.10 atm, what phase(s) can exist?
a)
solid, liquid or gas
b)
liquid or gas
c)
solid only
d)
gas only
49.
Does H2O have hydrogen bonding?
a)
yes
b)
no
50.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
51.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
52.
Chemical reactions that absorb energy are called
a)
endothermic
b)
fast
c)
slow
d)
exothermic
53.
An endothermic reaction feels _____ to the touch
a)
warm
b)
cool
54.
The slower molecules move, 
a)
the higher the temperature
b)
the less temperature
c)
the same temperature
d)
I don't know
55.
The faster molecules move, 
a)
the higher the temperature
b)
the less temperature
c)
the same temperature
d)
I don't know
56.
Device/Object that measures temperature. 
a)
Thermal energy
b)
Temperature
c)
Thermometer
d)
Heat
57.

What would be the effect on the molecules if more heat is supplied to the system?

a)

They would slow down

b)

They would stop moving

c)

They would speed up

d)

There would be no effect

58.

The average Kinetic Energy of a substance represents the ___________ of a substance

a)

Density

b)

Heat

c)

Thermal Energy

d)

Temperature

59.

Heat is a form of____________________and can do work.

a)

energy

b)

heat

c)

atoms

d)

water

60.

Convert 10780 J to "nutritonal" Calories.

(1 Cal = 1000 cal) (1 cal = 4.184 J)

a)

2576 Cal

b)

45.10 Cal

c)

2.576 Cal

d)

10.78 Cal

61.

How much energy is required to heat up 12000. g of copper from 10.0 °C to 120.0 °C. The specific heat capacity is 0.390 J/g °C.

a)
46800 J
b)

562000 J

c)

515000 J

62.

Energy (Heat) is measured in 

a)
joules
b)
grams
c)
degrees celcius
d)
mililiters
63.

How much heat is required to melt 26.0 g of ice at 0∘C? The Hf of water is 334 J/g.

a)

5.88 x 104 J

b)

8680 J

c)

109000 J

d)

0 J

64.

How much heat is required to vaporize 150. g of water at 100∘C? The Hv is 2260 J/g.

a)

62700 kJ

b)

50100 kJ

c)

150. J

d)

339000 J

65.

Observe the diagram. Which statement is true about the kinetic energy of the molecules in the containers?

a)

The molecules are moving faster in Diagram A

b)

The molecules are moving slower in Diagram A

c)

The molecules are moving at the same rate in both diagrams

66.

The specific heat of aluminum is 0.9025 J/g°C. How much heat(Q) is released when a 10.0 g piece of aluminum foil is taken out of the oven and cools from 100.0° to 50.0°?

a)

451 J

b)

45.1 J

c)

400 J

67.

The pressure on a tank containing 0.3 moles of oxygen is 4.5 atm, and the temperature is 150 K. What is the volume of the gas?

(R = 0.0821)

a)

0.821 L

b)

8.21 L

c)

82.1 L

d)

821 L

68.

What does the unit Kelvin, K, measure?

a)

Pressure

b)

Volume

c)

Mass

d)

Temperature

69.

A sealed container holds a mixture of Neon and Helium. The Neon has a Pressure of 2.25 atm. If the total Pressure in the container is 7 atm, what is the Partial Pressure of Helium?

a)

4.75 atm

b)

9.25 atm

c)

3.11 atm

d)

15.75 atm

70.

What does the unit Liters, L, measure?

a)

Volume

b)

Pressure

c)

Temperature

d)

Moles

71.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

72.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

73.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

74.
What is 50 °C in Kelvin?
a)

223

b)

323

c)

100

d)

50

75.

Match the following units to their names.

a)

Pressure

1.

mmHg

b)

Volume

2.

L

c)

Temperature

3.

K

d)

Pressure

4.

atm

e)

Moles

5.

mol

76.

Absolute zero is

a)

0 K

b)

where there is no molecular movement

c)

the coldest temperature possible

d)

all of these

77.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

78.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

79.

Grace, Priya, and Benjamin are conducting a science experiment in their school lab. They have a gas sample which they are holding at constant pressure. Initially, the gas occupies 3.62 L of volume when the temperature is 294.8 K. They are trying to determine the temperature at which the volume of the gas would be 3.42 L. Can you help them find out?

a)

312K

b)

278.5K

c)

20.4K

d)

295K

e)

552K

80.

Match the following gas laws with corresponding mathematical relationship:

a)

Boyle's Law

1.

P1V1 = P2V2

(n & T are constant)

b)

Charles' Law

2.

V1T1=V2T2\frac{V_1}{T_1}=\frac{V_2}{T_2}

(n & P are constant)

c)

Avogadro's Law

3.

V1n1=V2n2\frac{V_1}{n_1}=\frac{V_2}{n_2}

(p and T are constant)

d)

Ideal Gas Law

4.

PV = nRT

81.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
82.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
83.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
84.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

85.

You make a Kool Aid drink using Kool Aid powder, sugar, & water & you notice your drink still has to much powder sitting at the bottom. What will happen if you add more water to the drink?

a)

decrease the solubility of your drink

b)

decrease the solubility rate of your drink

c)

increase the solubility rate of your drink

d)

increase the solubility of your drink

86.
When no more sugar will dissolve in a glass of water, the solution is...
a)
unsaturated
b)
saturated
c)
supersaturated
87.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

88.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

89.

What is the pH of a solution where the [H+] is 1.0 x 10-11?

a)

11

b)

13

c)

14

d)

1

90.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
91.

Bases have a pH of

a)

7

b)

Less than 7

c)

More than 7

92.

Which of the following are properties of acids but not bases? Select all that apply.

a)

Sour taste

b)

Reacts with metals to produce hydrogen gas

c)

Feels slippery

93.

Which of the following will conduct electricity? Select all that apply

a)

Acidic solutions

b)

Basic solutions

c)

Ionic solutions

d)

Neutral covalent solutions

94.

The table shows the pH of several solutions. Which solution has the greatest concentration (amount) of H+ ions?

a)

vinegar

b)

milk

c)

water

d)

bleach

95.

The table shows the pH of several solutions. Which solution has the greatest concentration (amount) of OH- ions?

a)

vinegar

b)

milk

c)

water

d)

bleach

96.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
97.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
98.

The [H+] of orange juice is 0.00020 M. Find the pH of orange juice.

a)

1

b)

3.7

c)

10.3

d)

13

99.

How many liters are in 200 mL?

a)

0.2

b)

2

c)

20

d)

200

100.

How many milliliters equals 1 liter?

a)

10

b)

100

c)

1,000

101.

Which relationship is correct?

a)

1 calorie = 1 Calorie

b)

1 calorie = 1000 Calories

c)

1 Calorie = 4.184 Joules

d)

1 calorie = 4.184 Joules

102.

A piece of candy has 200 Calories per serving. How many calories of heat will be released when it is broken down?

a)

200 calories

b)

200,000 calories

c)

836,800 calories

d)

836.8 calories

103.

A snack item has 180 Calories per serving. How much heat energy (Joules) will be released when it is broken down?

a)

0.75312 Joules

b)

43,021 Joules

c)

43.02 Joules

d)

753,120 Joules

104.

How many moles is in 25.0 g of calcium?

a)

25.0 moles

b)

0.62 moles

c)

1.60 moles

d)

40.0 moles

105.

Determine the number of moles in 25.0 grams of potassium sulfide (K2S).

a)

0.23 moles

b)

4.41 moles

c)

110.3 moles

d)

25.0 moles

106.

Determine the number of moles in 1.50 grams of copper metal.

a)

1.50 grams

b)

0.023 moles

c)

42.4 moles

d)

6.02x1023

107.

Convert: 186.5 K to C (a)  

Choose from the below words
-86.4 C
-50 C
-68.4 C
180 K
108.

Convert 20.0⁰C to Kelvin. (a)  

Choose from the below words
293 K
273 K
298 K
20 K
109.

Convert 273K to ⁰C (a)  

Choose from the below words
0 ⁰C
546 ⁰C
-273 ⁰C
0 K
110.

What do both the Jedi and the Sith use as their source of power?

a)

Space magic

b)

Politics

c)

Money

d)

The Force

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