Free Printable Chem Fall Final Study Practice

1.

The positive particles of an atom are

a)

electrons

b)

positrons

c)

neutrons

d)

protons

2.

Where are an atom's neutrons and protons located?

a)

nucleus

b)

electron cloud

c)

core

d)

center

3.

An atom with atomic number 6 would have how many protons?

a)

6

b)

12

c)

3

d)

Not enough information

4.

Particles in an atom that are neutral and have no charge are

a)

negatrons

b)

electrons

c)

neutrons

d)

protons

5.

True or False? Neutrons have a negative charge

a)

True

b)

False

6.

What is the atomic number for an element with three protons?

a)

2

b)

1

c)

3

d)

6

7.

In this image, what does 1.00794 stand for?

a)

Hydrogen

b)

atomic number

c)

atomic mass

d)

atomic explosion

8.

What is the number of protons that the element in this image contains?

a)

14

b)

7

c)

15

d)

18

9.

What is the atomic mass of "F"

a)

9

b)

18

c)

17

d)

19

10.

Where are electrons of an atom found?

a)

Nucleus

b)

Electron Cloud

c)

Some are in the nucleus and some in the electron cloud.

d)

They are moving everywhere.

11.

"C" is the element symbol for which element?

a)

Calcium

b)

Carbon

c)

Chlorine

d)

Cadmium

12.

How many neutrons are in the atom "K"?

a)

7

b)

2

c)

39

d)

20

13.

How is an atom's mass number determined?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

14.

Which state of matter does this picture best represent?

a)

Solid

b)

Liquid

c)

Gas

15.

Which state of matter does this picture best represent?

a)

Solid

b)

Liquid

c)

Gas

16.

What do scientists believe all matter is made up of?

a)

dust

b)

particles

c)

water

d)

grains

17.

What happens to the particles when you “cool off” a substance?

a)

speed up

b)

sink

c)

slow down

d)

run over each other

18.

What happens to a substance when you decrease its temperature?

a)

expands

b)

breaks down

c)

dissolves

d)

contracts

19.

When heating up a substance, the particles begin to ________________________ and _______________________.

a)

expand; slow down

b)

spread apart; move faster

c)

contract; speed up

d)

come closer together; move slower

20.

You trap particles inside a syringe then push the plunger down.

a)

There are the same amount of air particles in the syringe.

b)

There are more particles in the compressed syringe.

c)

There are fewer particles in the compressed syringe.

d)

The particles in the compressed syringe get smaller.

21.

You trap particles inside a syringe then pull the plunger up.

a)

There are an equal number of particles in the syringe.

b)

There are more particles in the syringe.

c)

There are fewer particles in the syringe.

d)

The particles in the syringe are expanded.

22.

You compress a closed syringe and then let it go. Why does the plunger return to its original position?

a)

More air particles rush into the syringe and push the plunger up.

b)

The air particles outside the syringe pull the plunger back.

c)

The air particles inside the syringe push the plunger back.

d)

The air inside tried to get out.

23.

Why doesn't the ball fit into the ring after being heated?

a)

particles are moving slower

b)

particles have expanded due to the heat

c)

the ring got smaller

24.

Heat flows from _______ to ______ objects.

a)

cooler; warmer

b)

warmer; warmer

c)

warmer; cooler

d)

cooler; cooler

25.

Heat is usually measured in

a)

Joules

b)

grams

c)

degrees Celcius

d)

atmospheres

26.

The specific heat (c) of copper is 0.39 J/g °C. What is the temperature change (∆T) when 100 Joules of heat (Q) is added to 20 grams of copper?

a)

12.82 °C

b)

24.12°C

c)

351 °C

27.

A(n) _____________ is a device for measuring temperature.

a)

thermometer

b)

barometer

c)

anemometer

d)

psychrometer

28.

For the formula:
Q= m c ∆T
The units for specific heat are:

a)

g /J C

b)

°C/g J

c)

kJ/g

d)

J/g°C

29.

Endothermic reactions feel

a)

warm

b)

cold

30.

Exothermic reactions feel

a)

warm

b)

cold

31.

Energy is ___________ in endothermic reactions.

a)

released

b)

ended

c)

absorbed

32.

Energy is _________ in exothermic reactions.

a)

released

b)

absorbed

c)

unchanged

33.

If you focus on a cup that is in your hand, the cup is considered the _______ and you are considered the _________.

a)

system, surrounding

b)

surrounding, system

c)

suspect, victim

d)

object, universe

34.

What is the relationship between degrees Celsius and Kelvin?

a)

Kelvin + 273.15 = Degrees Celsius

b)

Degrees Celsius + 273.15 = Kelvin

c)

Degrees Celsius multiplied by 273.15 = Kelvin

d)

Kelvin divided by 273.15 = Degrees Celsius

35.

Which of the following best describes temperature?

a)

a measure of the speed (average kinetic energy) of particles in a sample of matter

b)

the energy transferred between samples of matter because of a difference in their temperature

c)

the energy stored (potential energy) in a sample of matter

36.

If a piece of copper is heated from 130K to 185K, what is the value of ΔT?

a)

55 K

b)

- 55 K

c)

315 K

d)

none of the above

37.

In what units is temperature measured?

a)

degrees Celsius

b)

Kelvin

c)

both Kelvin and degrees Celsius

d)

neither

38.

As a reaction is taking place, a student notices that the temperature has dropped. This indicates that the system has increased in energy. What type of process is this?

a)

Endothermic

b)

Exothermic

39.

A sample of iron receives 50 J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

40.

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 cal

b)

10.5 cal

c)

1.05 cal

41.

A material was cooled from 100ºC to 40ºC. What is the temperature change?

a)

60ºC

b)

40ºC

c)

-60ºC

d)

-40ºC

42.

___________________________ is the amount of heat energy required to raise the temperature of one gram of a substance by one degree.

a)

Specific heat capacity

b)

Thermochemistry

c)

Enthalpy

d)

Heat

43.

An atom's overall charge on the periodic table is

a)

positive

b)

depends on its mood

c)

neutral

d)

negative

44.

The smallest particle of any particular type of matter is known by which of the following terms?

a)

Compound

b)

Atom

c)

Chemical

d)

Element

45.

If the number of protons in an atom equals the number of _______, the atom will have no charge.

a)

protons

b)

neutrons

c)

electrons

d)

nucleus

46.

How is an atom's atomic number determined?

a)

the number of protons

b)

the sum of protons and neutrons

c)

the number of neutrons

d)

the difference between protons and electrons

47.

Two atoms of the same element but with different mass numbers are ________.

a)

relatives

b)

isotopes

c)

variables

d)

unstable

48.

How many neutrons does the isotope of lithium have?

a)

8

b)

3

c)

4

d)

5

49.

Where are electrons of an atom found?

a)

Nucleus

b)

Electron Cloud

c)

Some are in the nucleus and some in the electron cloud.

d)

They are moving everywhere.

50.

What is the atomic symbol for sodium?

a)

Na

b)

So

c)

NaCl

d)

S

51.

An atom has 10 protons, 15 neutrons and 10 electrons. What is its mass number?

a)

20

b)

10

c)

5

d)

25

52.

Which particle determines what element you have (the element's identity)?

a)

nucleus

b)

proton

c)

neutron

d)

electron

53.

Which particles make up the nucleus of an atom?

a)

protons and neutrons

b)

electrons and protons

c)

electrons, protons, and neutrons

d)

electrons and neutrons

54.

What is true of molecules of gas that are exposed to heat in a fixed volume container?

a)

They move faster and they cause the pressure to increase

b)

They move slower and pressure will decrease

c)

The volume increases and pressure increases

d)

The volume decreases and the pressure decreases.

55.

What about gasses can be measured?

a)

Pressure and Volume

b)

Temperature, Volume, and Pressure

c)

Volume and Temperature

d)

Pressure, Temperature, Volume, and Number of Particles

56.

If you increase the pressure of a constant volume of gas, what will happen to the temperature?

a)

Increase

b)

Decrease

c)

Stay the same

d)

It will Blow Up

57.

What is 323 Kelvin in degrees Celcius?

a)

-50 ^oC

b)

50 ^oC

c)

100 ^oC

d)

25 ^oC

58.

How are pressure and volume related?

a)

Directly

b)

Indirectly

c)

They aren't related

59.

You have a gas that has a pressure of 2 atm and a volume of 10 L. What would be the new volume if the pressure was decreased to 1 atm?

a)

5 L

b)

20 L

c)

It would stay at 10L

d)

1 L

60.

Which of the following would increase the pressure on a system?

a)

Increase the Temperature

b)

Pump in more gas

c)

Decrease the volume

d)

All of these

61.

What law combines all 3 factors (pressure, temperature, and volume)

a)

Combined Gas Law

b)

Charles's Law

c)

Boyle's Law

d)

Guy-Lussac's Law

62.

If a balloon is cooled what will happen to the volume?

a)

Volume will increase

b)

Volume will decrease

c)

Volume will not change

63.

When is it OK to eat or drink at the lab tables?

a)

Always

b)

During group work, but not during lab activities

c)

Never

d)

During lab activities

64.

What should you do if you break glass in the lab?

a)

Tell the teacher, sweep up the glass, and put it in the broken glass container

b)

Tell the teacher, sweep up the glass, and dump it into the garbage

c)

Pick up the glass with your hands

d)

Ignore it; the teacher will clean it up

65.

Keeping your work area neat and clean is important because:

a)

My teacher is a neat-freak

b)

I won't lose my supplies in the clutter.

c)

It keeps the room from looking messy.

d)

It helps prevent accidents.

66.

Disrupting other students in the laboratory with horseplay in the lab is:

a)

helpful.

b)

allowed

c)

dangerous.

d)

the quickest way to do a job.

67.

Helping to clean up the lab or classroom is the job of

a)

old students.

b)

transfer students.

c)

each and every student.

d)

only the teacher.

68.

Which of the following IS considered safety equipment in our classroom?

a)

Eyewash Station

b)

Emergency Shower

c)

Fire Extinguisher

d)

All of the Above.

69.

You should report accidents to the teacher __.

a)

after the class is over

b)

immediately

c)

the following day

d)

never

70.

When should you look over the experiment instructions?

a)

After starting the lab

b)

When your teacher tells you to

c)

Before starting the lab

d)

It doesn't really matter. Instructions are silly!

71.

It's fine to smell chemicals directly from their containers.

a)

True

b)

False

72.

Hot glass looks the same as cold glass.

a)

True

b)

False

73.

Beakers are used

a)

to measure volume with high accuracy and precision

b)

to hold small amounts of dry chemicals

c)

to recover dissolved solids

d)

to measure approximate volumes and observe reactions

74.

When should you use the safety shower?

a)

After P.E.

b)

After spilling chemicals onto your body

c)

Before going out on a date

d)

Never

75.

Identify the equipment shown here:

a)

beaker

b)

Erlenmeyer flask

c)

Florence flask

d)

volumetric flask

76.

What is special about graduated cylinders?

a)

They hold large quantities of liquid safely. We use them to store chemicals.

b)

They measure small amounts very accurately. We use them when precision is important.

c)

They are easily heated. We use them to heat liquids.

77.

Identify the equipment shown here:

a)

beakers

b)

flasks

c)

decanters

d)

graduated cylinders

78.

In a lab report, what do you call the list of numbered steps explaining what you did, or will do?

a)

Data Analysis

b)

Hypothesis

c)

Procedure

d)

Evaluation

79.

How is an atom's net charge determined?

a)

sum of protons and neutrons

b)

difference between protons and electrons

c)

number of electrons

d)

number of neutrons

80.

What does this picture likely represent?

a)

solid

b)

liquid

c)

gas

d)

plasma

81.

Which of the following best describes heat?

a)

a measure of the speed (average kinetic energy) of particles in a sample of matter

b)

a measure of the stored energy (potential energy) within particles

c)

a measure of energy related to the speed and mass of particles in a sample of matter

82.

Which of the following best describes pressure?

a)

a measure of the speed (average kinetic energy) of particles in a sample of matter

b)

the number of collisions between particles and the walls of a container

c)

a measure of energy related to the speed and mass of particles in a sample of matter

83.

Isotopes of an element have the same number of ______, but a different number of ______.

a)

protons; electrons

b)

neutrons; protons

c)

protons; neutrons

d)

electrons; protons

84.

How are pressure and temperature related?

a)

Directly

b)

Indirectly

c)

They aren't related

85.

How are volume and temperature related?

a)

Directly

b)

Indirectly

c)

They aren't related

86.

In a lab report, what do you call your prediction of what will happen in your experiment?

a)

Data Analysis

b)

Hypothesis

c)

Purpose

d)

Evaluation

87.

In a lab report, where do you provide Claim-Evidence-Reasoning (CER)?

a)

Data Analysis

b)

Conclusion

c)

Purpose

d)

Evaluation

88.

In a lab report, where do you discuss errors?

a)

Data Analysis

b)

Conclusion

c)

Hypothesis

d)

Evaluation

89.

What pressure is 1.43 kPa in mmHg?

a)

1.43 mmHg

b)

10.7 mmHg

c)

101.325 mmHg

d)

760 mmHg

90.

What pressure is 2.65 atm in kPa?

a)

268 kPa

b)

0.0261 kPa

c)

39.0 kPa

d)

265 kPa

91.

What pressure is 1.4 atm in mmHg?

a)

1064 mmHg

b)

1108 mmHg

c)

120 mmHg

d)

14005 mmHg

92.

1000 grams = _____ kilograms

a)

0.0001

b)

1,000,000

c)

10

d)

1

93.

42 L = ___mL

a)

4,200

b)

.0042

c)

4.20

d)

42,000

94.

1 L = _______ mL

a)

1

b)

10

c)

100

d)

1000

95.

What pressure is 6.8 atm in psi?

a)

100 psi

b)

110 psi

c)

205 psi

d)

80 psi

96.

What pressure is 0.9 psi in mmHg?

a)

900 mmHg

b)

273.15 mmHg

c)

46.5 mmHg

d)

58.2 mmHg

97.

You are performing an experiment in class to explore how mass of a substance affects heat transfer in a reaction. You perform 3 trials with different masses of a chemical in a beaker with 50 mL of water. After each trial, you measure the change in temperature of the water. What is your independent (manipulated) variable?

a)

volume of water

b)

mass of chemical

c)

container

d)

change in temperature

98.

You are performing an experiment in class to explore how mass of a substance affects heat transfer in a reaction. You perform 3 trials with different masses of a chemical in a beaker with 50 mL of water. After each trial, you measure the change in temperature of the water. What is your dependent (responding) variable?

a)

volume of water

b)

mass of chemical

c)

container

d)

change in temperature

99.

You are performing an experiment in class to explore how mass of a substance affects heat transfer in a reaction. You perform 3 trials with different masses of a chemical in a beaker with 50 mL of water. After each trial, you measure the change in temperature of the water. What is your control variable? Select all that apply.

a)

volume of water

b)

mass of chemical

c)

container

d)

change in temperature

100.

Determine the new temperature if 2.9 L of a gas at pressure of 5 atm and a temperature of 50 ℃ is changed to decrease the volume of the gas to 2.4 L and decrease the pressure to 1 atm.

a)

8.3 K

b)

12 K

c)

54 K

d)

78 K

Chem Fall Final Study Practice

Total questions: 100

Worksheet time: 2hrs 0mins

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