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Chemistry I Review

Total questions: 86

Worksheet time: 2hrs 46mins

Name
Class
Date
1.

4.2 Physical properties of matter...

a)

can be measured or observed without changing to an entirely different substance.

b)

cannot be measured because you can't measure light, energy and sound.

c)

include all the chemical components of the elements on the periodic table.

d)

change when water is added to the mixture.

2.

4.3 Density is...

a)

is the emptiness of a container.

b)

reflects how closely packed the particles of matter are.

c)

is anything that is used to fill an empty space.

d)

is how big a container is regardless of what it is filled with.

3.

4.4 Chemical properties...

a)

are not measurable, therefore they are not observable.

b)

cannot be seen without a microscope.

c)

can be measured or observed only when matter undergoes a change to become an entirely different kind of matter.

d)

are not measurable because the changes happen extremely fast.

4.

4.5 A purse substance is called an...

a)

proton.

b)

electron.

c)

atom.

d)

element.

5.

4.8 In physical change,

a)

matter may change its size, shape or state, but its chemical properties do not change.

b)

matter does not change size, shape or state.

c)

matter changes it chemical properties to suit the need of an element.

d)

matter keeps it shape regardless of the temperature.

6.

4.9 Most chemical changes are not as dramatic as exploding fireworks, so how can you tell whether a chemical change has occurred?

a)

You can't. You can't see chemical changes.

b)

There needs to be bubbles release, a change of color, an odor produced or a loud sound.

c)

Chemical changes need to be chemically checked.

d)

Chemical changes only change shape, form or size.

7.

4.10 Chemical changes in matter...

a)

do not destroy matter.

b)

discards protons and electrons.

c)

destroy matter.

d)

disappear completely.

8.

4.16 What theory or law states that particles of matter are in constant motion?

a)

The Laws of Thermodynamics.

b)

The Kinetic Theory of Matter.

c)

The Law of Conservation of Mass.

d)

Newton's firs law.

9.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
10.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
11.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
12.
True or False: Gases can be compressed. 
a)
True
b)
False
13.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
14.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
15.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
16.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
17.
What causes pressure?
a)
The walls of the container
b)
The vacuum in the container
c)
The collisions of the particles
d)
Atmospheric pressure acting on the outside walls
18.
A series of steps used by scientists to solve a problem or answer a question. 
a)
scientific method
b)
recipe
c)
data collection
d)
metric system
19.
On this digital scale, which digit is the uncertain digit?
a)
1
b)
2
c)
6
d)
4
20.
Is this device used to make accurate volume measurements?
a)
Yes, erlenmeyer flasks are the best
b)
No, graduated cylinders are better
21.
Is this device used to make accurate volume measurements?
a)
Yes, beakers are the best
b)
No, graduated cylinders are better
22.
Is this device used to make accurate volume measurements?
a)
Yes, beral-type pipets are the best
b)
No, graduated cylinders are better
23.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
24.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
25.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
26.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
27.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
28.

What is the most electronegative element? (Just write the symbol)

(a)  

29.

How many liters does 2 moles of CO2 occupy at STP?

a)

44.8 L

b)

22.4 L

c)

11.2 L

d)

Cannot calculate from the given information.

30.

How many liters does 2 moles of CO2 occupy at 100 0C?

a)

44.8 L

b)

22.4 L

c)

11.2 L

d)

Cannot calculate from the given information.

31.
You have 100 grams of radioactive C-14. The half life of C-14 is 5730 years. 
How many grams are left after 1 half life? 
a)
100 grams
b)
25 grams
c)
2 grams
d)
50 grams
32.

What percentage of rubidium-87 atoms will be left after four half lives?

a)

25.0%

b)

12.5%

c)

6.25%

d)

3.125%

33.

Isotopes have a different number of

a)

protons

b)

neutrons

c)

electrons

34.

Ions of the same element have a different number of

a)

protons

b)

neutrons

c)

electrons

35.

Different elements have a different number of

a)

protons

b)

neutrons

c)

electrons

36.

Any substance that does not conduct electricity when in solution is called a(n) ―

a)

nonelectrolyte

b)

electrolyte

c)

conductor

d)

semiconductor

37.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
38.
In an exothermic process the surrounding looses heat. 
a)
True
b)
False
39.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
40.
_P4+_O2 →  _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
41.
_K + _Cl2 →_KCl
a)
2 K + 16 Cl2 → 8 KCl
b)
2 K + 1 Cl2 → 2 KCl
c)
3 K + 4 Cl2 → 3 KCl
d)
1 K + 1 Cl2 →1 KCl
42.
Balance this equation,            Al2O3 ---> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 ---> 2Al + 3O2 
c)
2Al2O3 ---> 4Al + 3O2 
d)
3Al2O3 ---> 2Al + O2 
43.
Substances that enter into a chemical reaction (found to the left side of the arrow) 
a)
product
b)
reactant
c)
chemical
d)
balanced equation
44.
The large number in front of a chemical formula or compound is the ___________. 
a)
coefficient
b)
product
c)
physical
d)
chemical
45.
In every balanced chemical equation, each side of the equation has the same number of ____.  
a)
coefficients
b)
moles
c)
molecules
d)
atoms of each element
46.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
47.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
48.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
49.

If the first and second energy levels of an atom are full, then what would be the total number of electrons in the atom?

a)

6

b)

8

c)

10

d)

18

50.

Which of the following sub-levels is correctly designated?

a)

1p5

b)

3f9

c)

2p6

d)

3d11

51.

If the 1st energy level is already filled up with 2 electrons, what level should be filled up next?

a)

Second

b)

Third

c)

Fourth

d)

Fifth

52.

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

a)

1

b)

2

c)

4

d)

8

53.

“An electron should occupy the lowest energy level first before the higher energy level” is stated in what rule?

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

All of the above.

54.

What rule states that single electrons must occupy each equal-energy orbital before additional electrons can occupy the same orbitals.

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

None of the choices.

55.

What are the shapes of p orbitals ?

a)

cloverleaf

b)

spherical

c)

dumbbell

56.

How many electrons can occupy any single subshell orbital?

a)

1

b)

2

c)

6

d)

10

57.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
58.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
59.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
60.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
61.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
62.

What geometry will this molecular structure have? PH3

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

63.

What geometry will this molecular structure have? H2S

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

64.
Is the following molecule polar or non-polar?
a)
non-polar
b)
polar
65.
IS this molecule polar or non-polar
a)
non-polar
b)
polar
66.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
67.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
68.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
69.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
70.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
71.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
72.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
73.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

74.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
75.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
76.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

77.

The _____ is the thing being dissolved.

a)

solute

b)

solvent

78.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

79.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

80.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

81.

What is the molarity of a solution if 2 moles of NaOH are dissolved in 1 L of water?

(a)  

82.

What is the molarity of a solution if 2.5 moles of HCl is dissolved in 5 L of water?

a)

2 M HCl

b)

0.5 M HCl

c)

1 M HCl

83.
A helium nucleus with two protons and two neutrons is called a(n) ____.  
a)
alpha particle
b)
electroscope
c)
beta particle
d)
gamma ray
84.
Alpha particles.....
a)
a) are positively charged.
b)
b) consist of two protons and four neutrons.
c)
c) can penetrate any thickness of matter
d)
d) All of the above 
85.

The mass number of Neptunium (Np) is (a)   .

86.

The best time to wear a striped sweater is

a)

All the time

b)

Some of the time

c)

Never

d)

Cannot determine based on the information given

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