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HPS First Nine Weeks Review

Total questions: 132

Worksheet time: 3hrs 1mins

Name
Class
Date
1.

Convert 62 miles/hour to feet/second

a)

5,456 feet/second

b)

0.003 feet/second

c)

90.9 feet/second

d)

909 feet/second

2.

Convert 50 decimeters/week to kilometers/year

a)

0.026 kilometers/year

b)

2.6 kilometers/year

c)

0.26 kilometers/year

d)

26 kilometers/year

3.

Convert 6 centigrams/day to kilograms/year

a)

2.19 kilograms/year

b)

21.9 kilograms/year

c)

0.0219 kilograms/year

d)

219 kilograms/year

4.

How many millimeters are in 65.4 centimeter

a)

254ml

b)

654ml

c)

365ml

d)

456ml

5.

How many minutes are in four hours?

a)

175min

b)

280min

c)

240min

d)

325min

6.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
7.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
8.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
9.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
10.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
11.
How many significant figures: 0.001 g
a)
4
b)
3
c)
2
d)
1
12.
How many significant figures: 4.20 cm
a)
1
b)
2
c)
3
d)
4
13.
How many significant figures: 0.010 L
a)
1
b)
2
c)
3
d)
4
14.

Which of these has a negative charge?

a)

Proton

b)

Neutron

c)

Electron

d)

Oatmeal

15.

Which charge does a proton have?

a)

Neutral

b)

Negative

c)

No charge- battery is dead

d)

Positive

16.

Neutrons have a ____________ charge.

a)

Neutral, or no charge

b)

Positive

c)

Negative

d)

Neutron? I don't know what that is!

17.

True or false: Atoms make up everything around you.

a)

True

b)

False

18.
What is at the center of every atom?
a)
An electron
b)
A compound
c)
A molecule
d)
A nucleus
19.
Which two particles make up the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Molecules and Compounds
d)
Neutrons and Electrons
20.

Letter A is showing

a)

Neutrons

b)

Electrons

c)

Protons

d)

Nucleus

21.

Which subatomic particles make up the mass of an atom?

a)

protons only

b)

protons and neutrons

c)

protons, neutrons and electrons

d)

protons and electrons

22.

Label the atomic parts., their charge, and location.

(a)  

23.

The atomic number is the number of _______ in an atom.

a)

protons

b)

neutrons

c)

protons and neutrons

d)

neutrons and electrons

24.

The mass number is the _______ inside one atom.

a)

number of electrons

b)

number of electrons and protons

c)

number of neutrons and protons

d)

number of neutrons

25.

To find the number of neutrons, you must

a)

Subtract atomic number from mass number. (Example: 14-7=7 neutrons)

b)

Subtract mass number from atomic number. (Example: 7-14= -7 neutrons)

26.

How many protons are in Sodium?

a)

11

b)

22

c)

12

d)

33

27.

How many electrons are in Aluminium?

a)

40

b)

27

c)

13

d)

14

28.

How many neutrons are in Magnesium?

a)

36

b)

12

c)

24

d)

6

29.

How many neutrons are in Argon?

a)

18

b)

40

c)

58

d)

22

30.

How many protons, neutrons, and electrons are in Oxygen?

a)

Protons = 8; Neutrons = 16; Electrons = 8

b)

Protons = 8; Neutrons = 8; Electrons = 8

c)

Protons = 16; Neutrons = 8; Electrons = 16

d)

Protons = 16; Neutrons = 24; Electrons = 16

31.
How many protons does this atom have?
a)
2.5
b)
6
c)
5
d)
10.811
32.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
33.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
34.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

35.

What type of atom is this?

a)

Neutral atom

b)

Cation

c)

Anion

d)

Isotope

36.

What type of atom is this?

a)

Normal Atom

b)

Cation

c)

Anion

d)

Isotope

37.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

38.
Negative ions are called
a)
Cations
b)
Electrons
c)
Anions
d)
Neutrons
39.

How many protons does this isotope of titanium have?

a)

22

b)

26

c)

48

d)

70

40.

How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?

a)

2

b)

34

c)

36

d)

40

41.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
42.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
43.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
44.
An element with 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389amu.
a)
51.99 amu
b)
52.19 amu
c)
53.45 amu
d)
17.33 amu
45.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
46.
How does heat flow?
a)
Always from cold to warm
b)
Always from warm to cold
c)
Both warm to cold & cold to warm
d)
It depends on the temperature
47.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
48.
When a  piece of aluminum foil is taken out of the oven and cools from 100° C to 50°C, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
49.
The specific heat of aluminum is 0.21 cal/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
d)
50 J
50.
20 g of water. specific heat of water is 4.18 J/g°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
51.
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
52.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
53.
True or False: Gases can be compressed. 
a)
True
b)
False
54.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
55.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
56.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
57.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
58.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
59.

Find the volume occupied by 22.0 g of helium gas at 25.0 o C and 1.18 atm .

a)

123 L

b)

9.57 L

c)

114 L

d)

159 L

60.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
61.

Temperature should always be expressed in Kelvin (K). If A 600 mL sample of nitrogen is heated from 27 °C to 77 °C at constant pressure. What is the final volume of nitrogen?

a)

210.4mL

b)

514.3 mL

c)

700 mL

d)

1,711.1 mL

62.

A 132 mL of gas is measured at 380C. If the pressure remains constant, what will be the volume of the gas at 100C?

a)

34.74 mL

b)

120. 12 mL

c)

311.15 mL

d)

37, 375.8 mL

63.
a)

Student A

b)

Student B

c)

Student C

d)

Cannot be determined

64.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
65.

This bullseye demonstrates...

a)

High Accuracy & High Precision

b)

High Accuracy & Low Precision

c)

Low Accuracy & High Precision

d)

Low Accuracy & Low Precision

66.

Describe the accuracy and precision of the image

a)

Very accurate and somewhat precise

b)

Very accurate but not precise at all

c)

Not accurate at all but very precise

d)

not accurate and not very precise

67.
This image is an example of...
a)
precision ONLY
b)
accuracy ONLY
c)
BOTH precision and accuracy
d)
NEITHER precision and accuracy 
68.
What line segment represents only the solid state?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
69.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
70.

Between which two points is Heat of Fusion?

a)

A <----> B

b)

B <----> C

c)

C <----> D

d)

D <----> E

e)

E <----> F

71.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
72.

What letter on the diagram represents the substance only in the gas phase?

a)

A

b)

B

c)

C

d)

D

73.

What letter on the diagram represents a substance only in the liquid?

a)

A

b)

B

c)

C

d)

D

74.

What letter on the diagram represents a substance only in the solid phase?

a)

A

b)

B

c)

C

d)

D

75.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

76.

What is the melting point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

77.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

78.

What would the state of this substance be at 0.5 ATM of pressure at a 100 degrees Celsius?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

79.

The average atmospheric pressure in Michigan is close to 1 ATM. What state of matter would this substance be in if it was a nice summer day with a temperature of 80 o F (27 o C)?

a)

Solid

b)

Liquid

c)

Gas

d)

Michigan

80.

What happens along the AC line?

a)

Melting/Freezing

b)

Boiling/Condensing

c)

Boiling/melting

d)

freezing/condensing

81.

What happens along the BC line?

a)

Melting/Freezing

b)

Boiling/Condensing

c)

Boiling/melting

d)

freezing/condensing

82.

The critical point is found at point.....

a)

A

b)

B

c)

C

d)

D

83.

What is the name of the compound with chemical formula FeCl₂?

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

84.

What is the name of the compound with chemical formula FeCl₂?

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

85.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen 

86.

What is the name of the compound Na2SO4?

a)

sodium sulfate

b)

sodium sulfide

c)

sodium sulfite

d)

Sodium sulfuroxide

87.

Which of these combinations is an ionic compound made of?

a)

metal and metal

b)

nonmetal and nonmetal

c)

metal and nonmetal

d)

cation and Cation

88.

When naming ionic compounds with transition metals you need to include roman numerals to show the ___ of the metal.

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

89.

When metals bond with non-metals they form what type of bonds?

a)

covalent

b)

ionic

c)

cooperative

d)

lewis

90.

When two or more different elements are chemically combined, it forms a ___.

a)

mixture

b)

element

c)

solution

d)

compound

91.

When naming ionic compounds, you always write the name of the positive element ___.

a)

first

b)

second

c)

with "ide"

d)

with a prefix

92.

When naming binary ionic compounds, you change the ending of the second element to ___.

a)

-ate

b)

-ite

c)

-ide

d)

-ine

93.

What is the formula for magnesium carbonate?

a)

MgCO3

b)

Mg(CO3)2

c)

Mg2CO6

d)

Mg2CO3

94.

Which is true of ionic compounds?

a)

They are electrically neutral when dissolved in a solution

b)

They are made by sharing electrons

c)

They are made of metals and nonmetals

d)

They are good conductors as solids

95.
A negatively-charged ion.
a)
atom
b)
cation
c)
anion
d)
electron
96.
Cations are
a)
positive
b)
negative
c)
on the right side of the periodic table.
d)
nonmetals
97.
Na +  and  S -2
a)
Na2S
b)
NaS2
c)
Na2S2
d)
NaS
98.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
99.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
100.
When naming ionic compounds, the cation is always named first and the anion is always named second.
a)
False
b)
True
101.
 Li2O
a)
Dilithium oxideDilithium oxide
b)
Lithium oxide
c)
Lithium dioxide
102.
CsCl
a)
Monocesium monochloride
b)
Cesium monochloride
c)
Cesium Chloride
103.
MgS 
a)
Magnesium sulfide
b)
Monomagnesium monosulfide
c)
Magnesium monosulfide
104.
Na2S
a)

Disodium sulfide

Disodium sulfide

b)
Sodium sulfide
c)
Sodium monosulfide
105.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
106.
Name this compound: 
NaBr
a)
Bromide sodide
b)
Sodium bromide
c)
Sodium bromate
d)
Sodium bromite
107.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
108.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
109.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
110.
What is the charge on the simple (single atom) ion that sulfur forms?
a)
1-
b)
2+
c)
3+
d)
2-
111.
What is the formula for the compound formed by magnesium ions and nitrogen ions?
a)
MgN
b)
Mg2N3
c)
Mg3N2
d)
MgN3
112.
Li+ combines with P3-  to form
a)
LiP
b)
Li3P
c)
LiP3
d)
Li3P3
113.

The formula for this binary ionic compounds

Aluminum phosphide is

a)

Al P

b)

Al3P3

c)

Al3F3

114.

Why do all bonds form?

a)

to fill the outermost energy level

b)

so an atom can be unstable

c)

so the number of protons and electrons can equal.

d)

so they can gain neutrons.

115.

Valence electrons are found

a)

outermost energy level

b)

innermost energy level

c)

some where in the electron cloud

116.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

nothing

b)

gain 7

c)

lose 1

117.

How do covalent bonds form?

a)

by sharing electrons between atoms

b)

by donating or receiving electrons

118.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

119.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

120.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

121.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

122.

Atoms are most stable when their outer shell is full or complete.

a)

true

b)

false

123.

How are ionic bonds formed?

a)

transfer of electrons

b)

sharing of electrons

124.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

125.

Water is an example of what?

a)

molecular compound (covalent compound)

b)

ionic compound

126.

Salt is an example of what?

a)

ionic compound

b)

covalent compound

127.

Atoms involved in a covalent bond are not charged, while atoms involved in an ionic bond are charged (negative or positive)

a)

true

b)

false

128.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
129.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
130.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

131.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

132.

What charge will a Neon ion have?

a)

+1

b)

-1

c)

-8

d)

Neon does not form ions.

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