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U2 92 q

Total questions: 91

Worksheet time: 2hrs 34mins

Name
Class
Date
1.

A sample composed only of atoms having the same atomic number is classified as

a)

compound

b)

element

c)

solution

d)

isomer

2.

4 students were tasked with classifying air as a whole sample, and then selecting one of its components to classify. Given the following, which student(s) is/are correct and why?

A sample of air was found to have:

78% N2

97% O2

.93% Ar

.04% CO2

a)

Student A

Air: Heterogeneous mixture (different gases and different amounts of each gas)

N2 = element (2 identical atoms)

b)

Student B

Air: Homogeneous mixture (different components/types of gas but uniform composition).

O2 = compound, 2 atoms chemically combined.

c)

Student C

Air: Homogeneous mixture (different types of gas hard to detect and separate giving it a uniform consistency)

N2 = element (2 atoms of the same element combined diatomic element)

d)

Student D

Air: Heterogeneous mixture (made of different components)

CO2 = compound (2 different elements chemically combined)

3.

A dilute, aqueous potassium nitrate solution is best classified as a

a)

homogeneous compound

b)

homogeneous mixture

c)

heterogeneous compound

d)

heterogeneous mixture

4.

At which Celsius temperature does lead change from a solid to a liquid?

Use Reference Table S & T

a)

874°C

b)

328°C

c)

601°C

d)

0°C

5.

The table shows mass and volume data for four samples of substances at 298 K and
1 atmosphere.

Which two samples could consist of the same substance?

a)

A & B

b)

A & C

c)

B & C

d)

C & D

6.

Which statement describes a chemical property of hydrogen gas?

a)

Hydrogen gas burns in air.

b)

Hydrogen gas is colorless.

c)

Hydrogen gas has a density of 0.000 09 g/cm3 at STP.

d)

Hydrogen gas has a boiling point of 20. K at standard pressure.

7.

Which statement describes a chemical property of the element magnesium?

a)

Magnesium is malleable (flexible/bendable).

b)

Magnesium conducts electricity

c)

Magnesium reacts with an acid

d)

Magnesium has a high boiling point.

8.

A 10.0-gram sample of which element has the smallest volume at STP?

a)

Aluminum (Al)

b)

Magnesium (Mg)

c)

Titanium (Ti)

d)

Zinc (Zn)

9.

At room temperature, a mixture of sand and water can be separated by

a)

ionization

b)

combustion

c)

filtration

d)

sublimation

10.

Which particle diagram represents a sample of one compound, only?

a)

1

b)

2

c)

3

d)

4

11.
 Which of the following is a pure substance?
a)
   tea
b)
   brass
c)
   ocean water
d)
 carbon dioxide
12.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
13.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

14.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
15.
energy in exothermic reactions are
a)
released
b)
absorbed
16.
Endothermic reactions feel
a)
warm
b)
cold
17.

When a bond is broken in compounds, energy is generally

a)
released, and the reaction is exothermic
b)
released, and the reaction is endothermic
c)
absorbed, and the reaction is exothermic
d)
absorbed, and the reaction is endothermic
18.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
19.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
20.

During which phase change does a substance absorb energy?

a)

freezing

b)

condensation

c)

evaporation

d)

deposition

21.

During which phase change does a substance release energy?

a)

condensation

b)

evaporation

c)

melting

d)

sublimation

22.

Which phase change is endothermic?

a)

condensation

b)

deposition

c)

melting

d)

freezing

23.

What is happening to the kinetic energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

24.

What is happening to the potential energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

25.

What is happening to the kinetic energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

26.

Which particle diagram shows a solid?

a)
b)
c)
27.

When particles of a substance move faster, their kinetic energy...

a)

increases

b)

decreases

c)

stays constant

28.

When temperature increases, kinetic energy...

a)

increases

b)

decreases

c)

stays constant

29.

At what time interval is the substance melting?

a)

AB

b)

BC

c)

CD

d)

DE

30.

At what time interval is the substance evaporating?

a)

AB

b)

BC

c)

CD

d)

DE

31.

Which particle diagram shows a liquid?

a)
b)
c)
32.

Which particle diagram shows a gas?

a)
b)
c)
33.

The diagram represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Which element is not present in the mixture?

a)

A

b)

D

c)

X

d)

Z

34.
Which grouping lists the states of matter in order of increasing distance between particles?
a)
gas, liquid, solid
b)
liquid, solid, gas
c)
solid, gas, liquid
d)
solid, liquid, gas
35.
Which phrase best describes the particles in a solid?
a)
not moving
b)
very far apart
c)
vibrating in place
d)
able to slip past one another
36.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
sour milk
37.
A change in which NEW substances are formed.
a)
Chemical change
b)
Physical change
c)
Casual change
d)
Formal change
38.
A copper penny turning greenish after a few years is an example of ...
a)
Chemical Change
b)
Physical Change
39.
What is the name of a single type of atom?
a)
cell
b)
proton
c)
element
d)
atom
40.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
41.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
42.
Carbon is considered an element while carbon dioxide is considered a compound. This is because carbon dioxide is –
a)
a gas at room temperature.
b)
made of two different elements.
c)
given off by green plants.
43.
Which of the following chemical formulas represents a compound? 
a)
C3
b)
O2
c)
CH3CHO
d)
H2
44.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

45.

A student measures the mass and volume of a sample of aluminum at room temperature, and calculates the density of Al to be 2.85 grams per cubic centimeter. Based on Table S in the Chemistry Reference Table, what is the percent error for the student's calculated density of Al?

% Error = [(Measured - Real) / Real] x 100

a)

2.7%

b)

5.3%

c)

5.6%

d)

95%

46.

A large sample of solid calcium sulfate is crushed into smaller pieces for testing. Which two physical properties are the same for both the large sample and one of the smaller pieces?

a)

mass and density

b)

mass and volume

c)

solubility and density

d)

solubility and volume

47.

Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion?

a)

solution

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

48.

Compared to a 26-gram sample of NaCl(s) at STP, a 52-gram sample of NaCl(s) at STP has

a)

a different density

b)

a same mass

c)

the same chemical properties

d)

the same volume

49.

A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture?

a)

The mixture is homogeneous and can be separated by filtration.

b)

The mixture is homogeneous and cannot be separated by filtration.

c)

The mixture is heterogeneous and can be separated by filtration.

d)

The mixture is heterogeneous and cannot be separated by filtration.

50.

Which statement describes the type of change and the chemical properties of the product and reactants?

a)

The equation represents a physical change, with the product and reactants having different chemical properties.

b)

The equation represents a physical change, with the product and reactants having identical chemical properties.

c)

The equation represents a chemical change, with the product and reactants having different chemical properties.

d)

The equation represents a chemical change, with the product and reactants having identical chemical properties.

51.

Bronze contains 90 to 95 percent copper and 5 to 10 percent tin. Because these percentages can vary, bronze is classified as (Select ALL that apply)

Hint 1: We MOST COMMONLY describe solutions as homogeneous mixtures that are liquids- that's how we most commonly can distinguish between different types of mixtures and how we use it when working with solutes and solvents.

However, we actually can have other states of matter classified as solutions - if they fit the description of a homogeneous mixture.

Hint: 2: Which choices ALWAYS have a FIXED ratio of whatever makes it up AND, therefore, have the same composition in every sample no matter what?

 Hint 3: Which ONE COULD have a VARIABLE composition?

a)

a compound

b)

an element

c)

a mixture

d)

a pure substance

e)

a solid solution

52.

Bronze contains 90 to 95 percent copper and 5 to 10 percent tin. Because these percentages can vary, bronze is classified as (Select ALL that apply)

Hint: 1: Which choices ALWAYS have a FIXED ratio of whatever makes it up AND, therefore, have the same composition in every sample no matter what?

 Hint 2: Which ONE COULD have a VARIABLE composition?

a)

a compound

b)

an element

c)

a mixture

d)

a pure substance

53.

Which sample of matter is a mixture?

(aq) = aqueous: generally refers to water as a solvent (something dissolved in water)

Spanish "agua" means water

a)

Br2 (l)

b)

K (s)

c)

KBr (s)

d)

KBr (aq)

54.

Which statement describes H2O(l) and H2O2(l)?

a)

Both are compounds that have the same properties.

b)

Both are compounds that have different properties.

c)

Both are mixtures that have the same properties.

d)

Both are mixtures that have different properties.

55.

Green bananas turning yellow on their own as they ripen. This is a:

a)

chemical change.

b)

physical change.

56.

Sugar dissolving in water is an example of a:

a)

chemical change.

b)

physical change.

57.

Which of the following is NOT an example of a physical change?

a)

crumpled paper

b)

pencil sharpening

c)

glass breaking

d)

mold growing on cheese

58.

Bleaching your hair is an example of a:

a)

physical change.

b)

chemical change.

59.

Hammering wood together to build a house is an example of a:

a)

chemical change.

b)

physical change.

60.

Which of the following is a physical property?

a)

Combustion

b)

Electronegativity

c)

Color

d)

PH Level

61.

Which of the following is a chemical property of water?

a)

Reacts with pure sodium.

b)

Boils at 100 oC.

c)

Dissolves sugar easily.

d)

Has a density of 1 gm/mL

62.

Which of the following is a physical change?

a)

Burning a match

b)

Vinegar reacting with baking soda

c)

Melting butter

d)

Cooking an egg

63.

Which of the following is an example of a chemical change?

a)

Ripping paper in half

b)

Boiling an egg

c)

Cracking an egg

d)

Dissolving sugar in water

64.

Which of the following is NOT a sign that a chemical change has occurred?

a)

Change in color

b)

Change in shape

c)

Formation of a gas

d)

Change in odor

65.

Which of the following is a physical property?

a)

Heat of combustion

b)

Boiling point

c)

Flammability

d)

Reactivity

66.

Chicken noodle soup is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

67.

Methane (CH4) is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

68.

Tap water (water, salt & minerals) is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

69.

How would you classify the matter in the picture above?

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

70.

Does this image represent a chemical or physical change?

a)

Chemical change

b)

Physical change

71.

Does this image represent a chemical or a physical change?

a)

Chemical change

b)

Physical change

72.

Is this image showing a homogeneous or a heterogeneous mixture? Image: Milk

a)

homogeneous

b)

heterogeneous

73.

Does this particle view show an element or a compound?

a)

element

b)

compound

74.

What is an example of a chemical change?

a)

Tearing paper

b)

Dissolving salt in water

c)

Melting ice

d)

Burning wood

75.

What is an example of a physical property?

a)

Silver is shiny

b)

Alcohols are flammable

c)

Alkali metals are reactive with water

d)

Acids are sometimes corrosive

76.

What is the best classification of this substance? CO2 & H2S

a)

An element

b)

A compound

c)

A mixture of 2 compounds

d)

A mixture of many elements

77.

What is the best classification of this substance, sulfuric acid? H2SO4

a)

An element

b)

A compound

c)

A mixture

78.

What is the best classification of this substance?

a)

An element

b)

A compound

c)

A mixture of 2 elements

d)

A mixture of 2 compounds

79.

Is this a pure substance?

a)

Yes

b)

No

80.

What particle view below is a mixture?

a)

A

b)

B

c)

C

d)

D

81.

How many TYPES of MOLECULES are in this image?

a)

1

b)

2

c)

4

d)

5

82.

How many TOTAL MOLECULES in the sample in this image?

a)

4

b)

5

c)

15

d)

2

83.

How can this sample be best classified?

a)

Compound-

Pure Substance

b)

Element-

Pure Substance

c)

Mix of elements and compounds-

Homogeneous Mixture

d)

Mix of compounds-

Heteroeneous Mixture

84.

How many different TYPES of ATOMS are in this image?

a)

1

b)

2

c)

3

d)

4

85.

Which below shows a CHEMICAL change?

a)

b)

c)

86.

Which form of energy is transferred when an ice cube at 0°C is placed in a beaker of water at 50°C?

a)

chemical

b)

electrical

c)

nuclear

d)

thermal

87.

5 A beaker contains a dilute sodium chloride solution at 1 atmosphere. What happens to the number of solute particles in the solution and the boiling point of the solution, as more sodium chloride is dissolved?

a)

The number of solute particles increases, and the boiling point increases.

b)

The number of solute particles increases, and the boiling point decreases.

c)

The number of solute particles decreases, and the boiling point increases.

d)

The number of solute particles decreases, and the boiling point decreases.

88.

The average kinetic energy of the particles in a sample of matter is expressed as

a)

density

b)

volume

c)

pressure

d)

temperature

89.

Given the equation: I2(s) → I2(g)

Which phrase describes this change?

a)

endothermic chemical change

b)

exothermic chemical change

c)

endothermic physical change

d)

exothermic physical change

90.

Which term identifies a factor that will shift a chemical equilibrium?

a)

atomic radius

b)

catalyst

c)

decay mode

d)

temperature

91.

  1. At room temperature, a student determines the density of a sample of nickel to be 9.79 g/cm3. Based on Table S, what is the student’s percent error for the density of nickel?

  2. % Error = [(Measured Value - Real Value)/Real Value ] x 100

a)

0.091%

b)

0.10%

c)

9.1%

d)

10.%

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