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Unit 1+2 Review

Total questions: 97

Worksheet time: 2hrs 51mins

Name
Class
Date
1.

A property of a substance that is observed when the substance undergoes a change in identity is known as

a)

a physical property

b)

a chemical property

c)

a mixture

2.

A property of a substance that can be observed without the substance changing identity is known as

a)

a physical property

b)

a chemical property

c)

a mixture

3.

A box has a mass of 10 kg and a volume of 2 m3.  What is the box’s density?

a)

5 oz/mi

b)

0.2 kg/m3

c)

5 km/m3

d)

0.2 oz/mi

4.

Which of the following is NOT a physical property?

a)

Rust

b)

Color

c)

Magnetic

d)

Texture

5.

Which two factors make up density?

a)

weight and volume

b)

size and weight

c)

mass and size

d)

mass and volume

6.

​

A student collected thermal data for acetic acid (CH3CO2H) and water (H2O) and graphed the heating curves for the two substances. ​​​​ Which comparison can be made about a phase change common to acetic acid and water based on the graph?

​(Think about water's state of matter)

a)

More heat energy is required to melt a gram of acetic acid than to melt a gram of water.

b)

More heat energy is required to vaporize a gram of water than to vaporize a gram of acetic acid.

c)

Given the same rate of added heat, the temperature of a gram of water will increase at a faster rate than a gram of acetic acid.

7.

​

The illustration shows the lab equipment set up by a student to find the melting and freezing points for naphthalene, a chemical used as an insect repellent. ​​​​

A small sample of solid naphthalene (C10H8) is placed in the capillary tube attached to the thermometer and is heated in the water bath until the white solid melts. The student then turns the heat off and observes the sample as it cools, recording the temperature at regular intervals. What happens to the particles in naphthalene as it cools?

​

a)

the kinetic energy of the particles remains the same

b)

the kinetic energy of the particles increases

c)

the kinetic energy of the particles decreases

8.

During which period of time is the substance completely in the liquid phase?

a)

B-C

b)

C-D

c)

A-B and B-C

9.

​

A student is shown a model of the particles that make-up a liquid. ​​​​

How should the model be changed to show the particles of a solid?

​

a)

Increase the speed of the particles, and decrease the space between the particles

b)

Decrease the speed of the particles, and increase the space between the particles

c)

Decrease the speed of the particles, and decrease the space between the particles

10.

Consider the four phases of matter. How is a liquid different than a solid?

a)

the particles are farther apart

b)

energy has decreased

c)

molecules begin to vibrate

11.

Which of the following best describes the particles of a solid?

a)

The particles are far apart and moving slowly.

b)

The particles are closely packed and vibrate in place.

c)

The particles are far apart and moving fast.

12.

What is the boiling point of the substance?

a)

150 degrees

b)

90 degrees

c)

50 degrees

13.

What is the freezing point of this substance?

a)

150 degrees

b)

200 degrees

c)

90 degrees

14.

What happens to temperature and thermal (heat) energy during a phase change (ex: freezing)?

a)

The potential (thermal) energy changes, but the temperature remains constant.

b)

The temperature changes, but the potential (thermal) energy remains constant.

c)

Both the potential (thermal) energy and temperature remain constant.

15.

An element is heated to a temperature high enough to raise the kinetic energy of the molecules to a level where all of the molecules completely break free of the binding forces holding them together. What term is used to describe that temperature?

a)

melting point

b)

boiling point

c)

decomposition

d)

freezing point

16.

How many significant figures are in 127.500?

(a)  

17.

How many significant figures are in 670?

(a)  

18.

How many significant figures are in 300900?

(a)  

19.

How many significant figures are in 1200?

(a)  

20.

How many significant figures are in 0.0730?

(a)  

21.

Give the answer to the correct number of significant figures to

3.419 + 3.912 + 7.0518 + 0.00013

a)

14.383

b)

14.382

c)

14.3829

d)

14.38293

22.

Give the answer to the correct number of significant figures to

145.63 - 28.9

a)

116.73

b)

116.7

c)

116.70

d)

117

23.

Give the answer to the correct number of significant figures to

17.3 x 6.2

(a)  

24.

Give the answer to the correct number of significant figures to

247.89 ÷ 43.5

a)

5.70

b)

5.7

c)

5.699

d)

5.69

25.

Matter can be classified in:

a)

Mixtures and Compounds

b)

Substances and Elements

c)

Mixtures and Substances

d)

Elements and compounds

26.

Substances are classified in Elements and (a)  

27.

NH3 is a:

a)

Mixture

b)

Element

c)

Compound

d)

Particle

28.

Mixtures are divided in homogeneous and (a)  

29.

Water and sugar dissolved is an example of:

a)

Compound

b)

Homogeneous mixture

c)

Substance

d)

Heterogeneous mixture

30.

A chocolate chip cookie is an example of:

a)

Substance

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

31.

What mixture is an heterogeneous mixture?

a)

Soluble coffee in water

b)

Sand and water

c)

Perfume

d)

Apple juice

32.

The mixtures where the components can be distinguished at simple sight

a)

Homogeneous

b)

Heterogeneous

c)

Homogeneous and heterogeneous

d)

None

33.

Filtration can be used to separate...

a)

an insoluble solid from a solution

b)

a soluble solid from a solution

c)

a dissolved solid from a solution

34.

Combination of multiple substances is a...

a)

pure substance

b)

mixture

c)

colloid

d)

suspension

35.

The liquid that condenses during distillation is called the

a)

residue

b)

filtrate

c)

distillate

d)

suspension

36.

The change of a liquid to a gas to remove solvent and collect solute is called

a)

Decantation

b)

Filtration

c)

Evaporation

d)

Centrifuge

37.

what type of mixture can be separated using the arrangement shown?

a)

salt dissolved in water

b)

ink components

c)

saw dust and iron fillings

d)

sand mixed with water

38.
Which one of these pictures represents a mixture? 
a)
1
b)
2
c)
3
d)
1, 2 and 3
39.
This picture represents: 
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
40.
This picture represents: 
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
41.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
42.
Why is the composition of every element fixed?
a)
Because it contains only one type of atom.
b)
Because the ratio of atoms is always the same.
c)
Because the atoms are so small.
d)
Because God said so.
43.

Which one of the following does not have an indicator for chemical change?

a)

Two clear liquids form precipitate after mixing

b)

The milk smells when you leave it out of the refrigerator

c)

Fireworks explode with different shapes and colors

d)

Prepare a cold Kool-Aid in a hot summer day.

44.

1.Particles cannot change position in a ________

a)

solid state

b)

liquid state

c)

gas state

45.
This picture represents: 
a)
Element
b)
Compound
c)
Mixture of Elements
d)
Mixture of Compounds
46.

A marshmallow is toasted over a campfire is;

a)

Physical Change

b)

Chemical Change

47.

A classification of matter that is made up on only 1 type of particle is called

a)

a heterogeneous mixture

b)

a pure substance

c)

a homogeneous mixture

d)

a blender

48.

In identifying a sample of a pure substance, which may be its chemical property?

a)

Its mass is 26.87 g

b)

It melts when heated

c)

It burns in air

d)

It is a good heat conductor

49.

What is the unit for density ?

a)

g/ mL

b)

g

c)

gcm3\frac{g}{cm^3}  

d)

cm4cm^4  

50.

Which box has a higher density?

a)

A

b)

B

c)

They both have the same density.

51.

If a block of wood has a density of 0.6 g/cm3 and a mass of 120 g, what is its volume?

a)

300 cm3

b)

200 cm3

c)

100 mL

d)

150 cm3

52.

Find the density of a 2 cm x 2 cm x 2 cm cube with a mass of 64 g.  

(Hint: find the volume first!)

a)

13 g/cm3

b)

2 g/cm3

c)

10 g/cm3

d)

8  g/cm3

53.
A mechanical pencil has the density of 3.000 g/cm3.  The volume of the pencil is 15.8 cubic centimeters.  What is the mass of the pencil?
a)
47.4 g
b)
50 g
c)
0.190  g
d)
5.27 g
54.
If you have a gold brick that is 2 cm by 3 cm by 4 cm and has a density of 19.3 g/cm3, what is its mass?
a)

263.5 g/cm3

b)
463.2 g
c)
0.804 kg
d)

2.804 g

55.

TRUE or FALSE: In order to change the state of matter, you need increase or decrease the energy (heat).

a)

TRUE

b)

FALSE

56.

TRUE or FALSE: The particles in solids move around a lot and spread out.

a)

TRUE

b)

FALSE

57.

TRUE or FALSE: Liquids have a fixed volume but not a fixed shape.

a)

TRUE

b)

FALSE

58.

TRUE or FALSE: Gases have the least kinetic energy out all 3 states of matter.

a)

TRUE

b)

FALSE

59.

Phase change from liquid to gas is called:

a)

Freezing

b)

Condensation

c)

Vaporization

d)

Sublimation

60.

Phase change from solid to gas is called:

a)

Freezing

b)

Condensation

c)

Vaporization

d)

Sublimation

61.

Phase change from gas to liquid is called:

a)

Melting

b)

Freezing

c)

Deposition

d)

Condensation

62.

Phase change from liquid to solid is called:

a)

Melting

b)

Freezing

c)

Deposition

d)

Condensation

63.

When changing a substance from liquid to solid, the energy has to...

a)

INCREASE

b)

DECREASE

64.

When changing a substance from gas to liquid, the energy has to...

a)

INCREASE

b)

DECREASE

65.

Which of the following statements is NOT true about gases?

a)

Gases do not have fixed shape or volume

b)

Gas particles do not move much, but vibrate

c)

Gas particles have a lot of free space

d)

Unlike solids, gases can be compressed

66.

Which of the following statements is true about liquids?

a)

Particles do not move around much, but vibrate

b)

Particles have a lot of free space and spread out

c)

Liquids have fixed shape & volume

d)

Particles are less closely packed than solids

67.

Look at the picture. Which state of matter is in beaker A?

a)

Solid

b)

Liquid

c)

Gas

d)

Blue thingys

68.

Which of the following statements is true about solids?

a)

Particles do not move around much, but vibrate

b)

Particles have a lot of free space and spread out

c)

Solids have fixed shape but not volume.

d)

Particles are less closely packed than gas.

69.

Are the particles moving faster or slower as time goes on?

a)

Faster

b)

Slower

70.

The melting point of the sample is

a)

-60 ºC

b)

-100 ºC

c)

60 ºC

d)

100 ºC

71.

Given the heating curve of a solid being heated at a constant rate, what is the boiling point of this substance?

a)

20°C

b)

50°C

c)

110°C

d)

170°C

72.

What term goes on the y-axis? (A)

a)

Heat(Energy)

b)

Temperature

c)

Phase

d)

Type of Matter

73.

What phase of matter exists in part C of the graph?

a)

Gas

b)

Liquid

c)

Solid

d)

Plasma

74.

What phase change occurs when you start at D and end at C?

a)

Freezing

b)

Melting

c)

Condensing

d)

Vaporization

75.

On which parts of the graph does the temperature remain the same?

a)

Between C and D

b)

Between D and E

c)

At C, D, or E

d)

On both flat sections

76.

What values represent standard temperature and pressure?

a)

273K

83 atm

b)

100K

1atm

c)

273K

1atm

d)

0K

1atm

77.
When iron nails get rusty, heat is released.  What process is this?
a)
Exothermic
b)
Endothermic
78.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
79.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
80.

What energy is stored and waiting to be used?

a)

Kinetic Energy

b)

Potential Energy

81.
Heat transfers from an area of ____temperature to an area of ___ temperature.
a)
high to low
b)
low to high
c)
high to high
d)
It can travel high to low and low to high. 
82.

The law of conservation of energy states that

a)

energy can be created or destroyed

b)

energy cannot be created or destroyed

c)

energy can be potential or kinetic only

d)

heat energy is kinetic energy

83.

What would likely happen if you were to touch the flask in which an exothermic reaction was occurring?

a)

The flask would feel cooler

b)

The flask would feel warmer

c)

The flask would feel the same before and after a reaction

d)

None of the above

84.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
85.
In an exothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released
86.

What instrument would you use to detect an endothermic or exothermic reaction?

a)

triple beam balance

b)

ruler

c)

thermometer

87.
Energy is transferred as heat between two objects of ___________ temperatures. 
a)
differing
b)
same
88.
The measure of average kinetic energy of all the particles within an object is called ____________. 
a)
temperature
b)
conduction
c)
radiation
d)
heat 
89.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
90.
When you measure the temperature of hot soup, you are measuring the:
a)
thermal energy given off by the bowl
b)
specific heat of the bowl
c)
average kinetic energy of the particles in the soup
d)
thermal expansion of the particles in the soup
91.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
92.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
93.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

a)

0.46 J/goC

b)

1.654 J/goC

c)

2,567,446.875 J/goC

94.

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22.0°C to 55.0°C, if the specific heat of aluminum is 0.903 J/g°C?

a)

298 Joules

b)

0.003 Joules

c)

297 J/g°C

d)

0.003 J/g°C

95.

A 300.0 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 0.3845 J/g 0C, what is the change of the copper's temperature? (INPUT THE NUMBER WITHOUT UNITS)

(a)  

96.
How many Joules of energy are required to make 100 grams of ice at 0 οC completely melt? The specific latent heat of fusion of ice is 334000 J/kg
a)
200 J
b)
400 J
c)
33,400 J
d)
2,000,000 J
97.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J

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