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Test 3 Review

Total questions: 75

Worksheet time: 6hrs 41mins

Name
Class
Date
1.

How many significant figures does the following number have: 0.002040

a)

6

b)

4

c)

3

d)

2

2.

How many significant figures does the following number have: 1740200

a)

4

b)

7

c)

3

d)

5

3.

Calculate 12.34 + 1.234 + 0.1234 and give your answer with the correct number of significant figures.

a)

13.6974

b)

13.697

c)

13.70

d)

13.7

4.

Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.

a)

1.0 m2

b)

1.1 m2

c)

1.0947 m2

d)

1.095 m2

5.

All of the following have one significant figure except:

a)

100 cm

b)

0.0001 cm

c)

2 cm

d)

2.00 cm

6.
a)

6.5

b)

6.60

c)

6

d)

6.65

7.

Which is the more precise measurement?

a)

4 mL

b)

4.3 mL

c)

4.30 mL

d)

4.300 mL

8.

To make a proper measurement...

a)

write down only the certain digits.

b)

write down all certain digits and one estimated digit.

c)

write down all certain digits and a few estimated digits.

d)

look at the instrument carefully

9.

An experimental measurement was taken of 10.4 mL and the actual measurement was 9.7 mL. What is the percent error? Round to the nearest tenth of a percent.

a)

5.2%

b)

9%

c)

7.2%

d)

8.8%

10.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

11.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

12.

At which temperature is the vapor pressure of ethanol equal to the vapor pressure of propanone at 35oC?

a)

35oC

b)

60oC

c)

82oC

d)

95oC

13.

When the atmospheric pressure equals the equilibrium vapor pressure ___ occurs.

a)

freezing

b)

melting

c)

boiling

d)

sublimation

14.

What is the normal boiling point of water

a)

0oC

b)

100oF

c)

50oC

d)

100oC

15.

Which model represents a LOWER Vapor Pressure?

a)

A

b)

B

16.

As pressure decreases, boiling point___

a)

decreases

b)

increases

c)

decreases then increases

d)

increases then decreases

17.

Which model represents STRONGER Intermolecular Forces?

a)

A

b)

B

18.

Imagine A & B represent the same substance. Which model would be at a HIGHER temperature?

a)

A

b)

B

19.

When the vapor pressure of water is 70 kPa the temperature of the water is

a)

20oC

b)

40oC

c)

60oC

d)

91oC

20.

Which is an example of a chemical change?

a)

distillation

b)

filtration

c)

combustion

d)

freezing

21.

Which describes a chemical change?

a)

sugar dissolving in tea

b)

sunshine warming a sidewalk

c)

scissors cutting paper into pieces

d)

acid in the stomach digesting food

22.

Contains two or more different substances that are physically, not chemically, combined

a)

a mixture

b)

an element

c)

a compound

d)

a chemical formula

23.

What type of substance is pictured?

a)

element

b)

compound

c)

mixture

d)

solution

24.

A substance that can NOT be broken down by physical or chemical means

a)

element

b)

compound

c)

mixture

25.

Matter that is composed of one type of atom is ...

a)

an element

b)

a compound

c)

a molecule

d)

a mixture

26.

Which is a mixture of compounds?

a)
b)
c)
d)
27.

Which is a pure substance?

a)
b)
c)
d)
28.

Which picture(s) represents a mixture between two elements?

a)

A

b)

B

c)

C

d)

A and C

29.

Which picture(s) represents a mixture between an element and a compound?

a)

A

b)

B

c)

D

d)

B and D

30.

Heterogeneous mixture is

a)

A mixture with a composition that varies from point to point

b)

A mixture with a uniform composition and appears visually the same throughout

31.

Homogeneous mixture is

a)

A mixture with a composition that varies from point to point

b)

A mixture with a uniform composition and appears visually the same throughout

32.

Name the separation technique shown in the diagram.

a)

evaporation

b)

distillation

c)

filtration

33.

Dyes in water soluble markers may be separated by means of..

a)

crystallization

b)

sublimation

c)

chromatography

d)

sedimentation

34.

Water and alcohol are easily separated by distillation because of their

a)

 different melting points

b)

different colours

c)

different densities

d)

different boiling points

35.

Look at the apparatus setup. It CANNOT be used to separate which of the following mixtures?

a)

Marble chips from oil

b)

Alcohol and water

c)

Chalk from sugar solution

d)

Sand and sea water

36.

Matter can be classified by analyzing its composition as it is shown in the diagram. Steel is a material that contains two elements: iron (Fe) and carbon (C). Two different samples of steel have different quantities of these two elements, but both have uniform composition. Using the diagram above, how would you classify steel?

a)

As pure substance, because it has uniform composition and it is a compound

b)

As a heterogeneous mixture, because is formed by two different elements

c)

As a homogeneous mixture, because is formed by two different elements and it is uniform

d)

As pure substance, because different samples have different composition

37.

What is the correct order for obtaining salt from a mixture of sand and salt?

a)

Dissolving in water - filtration – evaporation

b)

Evaporation - filtration - dissolving in water

c)

Filtration - dissolving in water - evaporation

d)

Dissolving in water – evaporation - filtration

38.

Which part of a filtration is the "filtrate"?

a)

The filter paper

b)

The solid material left in the funnel

c)

The liquid that has gone through

d)

The conical flask

39.

This diagram represents...

a)

An element

b)

A molecule

c)

A compound

d)

A mixture of elements and compounds

40.
a)
element
b)
compound
c)
mixture of elements
d)
mixture of compounds
41.

Water and alcohol are easily separated by distillation because of their

a)

different densities

b)

different boiling points

c)

different colours

d)

different melting points

42.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1,200 g of water from 23 °C to 39 °C?

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

43.

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

44.

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

a)

37.8 °C

b)

-19.8 °C

c)

19.8 °C

d)

55.8 °C

45.

How many Joules of energy are required to make 50.0 grams of ice at 0 οC completely melt?

a)

334 J

b)

0 J

c)

33,400 J

d)

16,700 J

46.

The temperature of a 6.0 g sample of glass changed from 20.0°C to 45.0°C when it absorbed 550 J of heat. What is the specific heat of this glass?

a)

0.27 J/g °C

b)

3.7 J/g °C

c)

130 J/g °C

d)

12 J/g °C

47.

Specific heat of water is  4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more heat energy to raise the temperature?

a)

Water

b)

Wood

c)

Both are same

48.

Calculate the energy needed to completely boil away 30 g of water at 100 ⁰C .

a)

67,800 J

b)

2260 J

c)

226,000 J

d)

100 J

49.

What are the characteristics of a solid?

a)

Solids do not have a definite shape but have a definite volume

b)

Solids have a definite shape and no definite volume

c)

Solids do not have a definite shape and no definite volume

d)

Solids have a definite shape and definite volume

50.

5. What is it called when a solid turns directly into a gas?

a)

Sublimation

b)

Condensation

c)

Liquid

51.

Between which two points is the solid cooling?

a)

A <---- B

b)

B <----> C

c)

C <---- D

d)

D <----> E

e)

E <---- F

52.

A substance's heating curve is shown in the graph.  What is its boiling point?

a)

100 C

b)

60 C

c)

80 C

d)

20 C

53.

Which two phases changes takes away energy?

a)

Freezing, Melting

b)

Condensation, Evaporation

c)

Freezing, Condensation

d)

Melting, Evaporation

54.

Endothermic phase changes include

a)

conduction, convection and radiation

b)

freezing and condensation

c)

vaporization and condensation

d)

melting, boiling, evaporation and sublimation

55.

Temperature is the measure of _______________ energy.

a)

potential

b)

kinetic

c)

thermal

d)

mechanical

56.

Absolute zero happens when particles -

a)

move very fast

b)

move very slowly

c)

stop moving

d)

melt

57.

The food that plants make during the process called photosynthesis is what form of energy?

a)

electrical

b)

chemical

c)

mechanical

d)

light

58.

What does the law of conservation of matter and energy say?

a)

that matter changes phase when it absorbs thermal or heat energy

b)

that all matter melts when heated

c)

that matter and energy cannot be created or destroyed, but just transformed from one form into another

d)

that energy causes motion in matter

59.
Which direction is heat flowing in the picture?
a)
from the hand to the ice
b)
from the ice to the hand
c)
heat is not being transferred
d)
there is no way to tell
60.

As part of a lab experiment, Tasha drops a metal cube into a beaker of water, as shown in the figure below.


After energy in the form of heat transfers between the substances, what is the final temperature of the water?

a)

The final temperature is 25 °C because there is more water than metal.

b)

The final temperature is 50 °C because the metal warms the water to the temperature of the metal.

c)

The final temperature is between 25 °C and 50 °C because energy is transferred from the metal to the water.

d)

The final temperature is between 25 °C and 50 °C because most of the thermal energy is lost to the air around the substances.

61.

When calcium reacts with water, the temperature changes from 18°C to 39°C. Which statement is correct?

a)

The solution at the end is acidic

b)

The reaction is reversible

c)

The reaction is exothermic

d)

The reaction is endothermic

62.
Convert: 253 C to K:
a)
526 K
b)
625 K
c)
0 K
d)
186 K
63.

Convert

450 K450\ K  to Celsius

a)

723oC723^oC  

b)

277oC277^oC  

c)

177 oC177\ ^oC  

d)

623oC623^oC  

64.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
65.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
66.

Type of intermolecular force present between I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

67.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

68.

Intermolecular forces for: NH3

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

69.

Intermolecular forces for: CO2

a)

London dispersion Forces

b)

Dipole dipole

c)

Hydrogen bonding

70.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

71.

Which molecule: Br2, HCl, H2S, or NH3, will most likely have London dispersion forces as the MOST important IMF considered when determining melting/boiling points?

a)

Br2, it only has dispersion forces when interacting

b)

HCl, it can participate in dipole-dipole interactions and also dispersion forces

c)

H2S, it can participate in dipole-dipole interactions and also dispersion forces

d)

NH3, it can participate in hydrogen bonding and also dispersion forces

72.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

73.

Which of the following will have the lowest melting point?

a)
b)
c)
d)
74.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Attraction

b)

Molecule-Ion Attraction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

75.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

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