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Worksheets

Fall exam

Total questions: 79

Worksheet time: 40mins

Name
Class
Date
1.

How many electrons should Carbon have around its Lewis dot model?

a)

1

b)

3

c)

4

d)

5

2.

How many electrons should Oxygen have around its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

3.

Solid particles are

a)

A

b)

B

c)

C

4.

Liquid particles

a)

A

b)

B

c)

C

5.

Which statement correctly describes BOTH gases and liquids?

a)

Their volumes change in different containers.

b)

Their shapes change in different containers.

6.

As a sample of matter is heated, its particles…

a)

Slow down

b)

Stay the same

c)

Move more quickly

d)

Stop

7.

What letters show a phase change

a)

A, B, and C

b)

A and E

c)

B and D

d)

A, C, and E

8.

On which portion(s) of the graph is only a liquid present?

a)

A

b)

B

c)

C

d)

D

9.

How many phase changes are in the diagram?

a)

1

b)

2

c)

3

d)

4

10.

When a substance goes from a gas to a liquid state, the process is known as _____________, while a change

from a gas directly to a solid state is __________________.

a)

Deposition, sublimation

b)

condensation, deposition

c)

Condensation, sublimation

d)

Sublimation, deposition

11.

Which diagram to the right represents the change of water from solid to a gas vapor?

a)

A

b)

B

c)

C

d)

D

12.

Mixtures can be either heterogeneous or homogeneous. Which of the following is characteristic of a

homogeneous mixture?

a)

cement

b)

Salt and pepper

c)

Chocolate chip cookies

d)

Salt water

13.

What is the definition of homogeneous mixture?

a)

A mixture in which large particles are suspended

b)

A mixture in which two or more substances are evenly distributed/uniform throughout

14.

KCl is an example of which type of material?

a)

Colloid

b)

Compound

c)

Element

d)

Mixture

15.

Which of the following mixtures display the Tyndall effect?

a)

Suspension

b)

Solution

c)

Colloid

16.

This picture shows _________ and __________

a)

Solid and Colloid

b)

Suspension and Solution

c)

Solution and Colloid

d)

Suspension and Colloid

17.

Which of the following substances is NOT an element?

a)

Aluminum (AL

b)

Table Salt (NaCl)

c)

Hydrogen (H)

d)

Iron (Fe)

18.

You are about to open a container of orange juice, but notice that there are instructions to “shake well before serving.” The orange juice is most likely a…

a)

Colloid

b)

Pure substance

c)

Solution

d)

Suspension

19.

Which of the following is a heterogeneous mixture?

a)

Bowl of cereal

b)

Tea

c)

Sugar water

d)

Swimming pool water

20.

All of the following are indicators of a chemical reaction EXCEPT

a)

Bubbles are formed by a gas

b)

The Tyndall effect is seen

c)

Light and heat is produced

d)

A colorful, insoluble solid forms when two solutions are mixed

21.

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

a)

Shiny Penny

b)

Iron becomes rust in the presence of oxygen

c)

Painting a wall

d)

Mass of aluminum

22.

What is the scattering of light as a light beam passes through a colloid. The individual suspension particles scatter and reflect light, making the beam visible.

a)

Tyndall effect

b)

Phase Change

c)

Condensation

d)

Sublimation

23.

A beaker contains 0.73 L of water. The beaker’s volume is how many milliliters?

a)

7.30

b)

73

c)

0.73

d)

730

24.

Elements form chemical bonds in order to have

a)

neutrality.

b)

chemical stability.

c)

personality.

d)

gravity.

25.

Florine forms an ion by

a)

gaining an electron.

b)

losing an electron.

c)

gaining two electrons.

d)

losing two electrons.

26.

Aluminum forms an ion by

a)

gaining two electron.

b)

losing an electron.

c)

gaining three electrons.

d)

losing three electrons.

27.

In order to become chemically stable, a metallic atom will

a)

gain electron(s).

b)

share electron(s).

c)

lose electron(s).

d)

accept electron(s).

28.

are diagrams that represent the valence electrons of atoms within a molecule.

a)

Tyndall effect

b)

Lewis Structure

c)

Hyphen Notation

d)

Isotope Notation

29.

This diagram shows

a)

The valence electrons

b)

The protons

c)

Neutrons

30.

How many valence electrons does Calcium have?

a)

One

b)

Two

c)

Three

d)

Four

31.

How many valence electrons does Neon have?

a)

Five

b)

Six

c)

Seven

d)

Eight

32.

Which type of chemical bond involves the sharing of valence electrons between nonmetals?

a)

Ionic

b)

Covalent

c)

Metallic

d)

None of the above

33.

Which type of chemical bond would form between Hydrogen and Oxygen?

a)

Metallic

b)

Ionic

c)

Covalent

d)

None of the above

34.

What do we call the attractive force that holds atoms of different elements together?

a)

chemical neutrality

b)

chemical stability

c)

chemical bond

d)

none of the above

35.

Which type of chemical bond involves the transfer of electrons from a metal to a nonmetal?

a)

Ionic

b)

covalent

c)

metallic

d)

none of the above

36.

How do we correctly write an ionic compound’s chemical formula?

a)

Lowest whole number ratio of cation to anion to form a neutral compound

b)

Highest ratio of metal to nonmetal to form a neutral compound

c)

Same number of metallic atoms as nonmetallic atoms

d)

Same number of cations as the number of anions.

37.

What is the proper way to write the compound between Chlorine and Sodium?

a)

SC

b)

ClNa

c)

NaCl

d)

Na2Cl

38.

What are the Greek prefixes for 4, 7, and 10

a)

penta, hepta, and nona

b)

tetra, hexa, and deca

c)

tetra, hepta, and deca

d)

tri, hepta, and deca

39.

How do we correctly write a covalent compound’s chemical formula?

a)

Greek prefixes represent the number of atoms of each nonmetal

b)

Same number of each atom.

c)

Lowest whole number ratio of the first nonmetal to the second nonmetal.

d)

Lowest whole number ratio of cation to anion to form a neutral compound.

40.

Which of the following are properties of ionic compounds?

a)

High melting point

b)

Crystalline solids

c)

conductive when molten or dissolved in water

d)

all of the above are correct

41.

Select the correct chemical formula for dinitrogen trioxide?

a)

N2O3

b)

N10O3

c)

2N3O

d)

None of the above

42.

Select the correct chemical formula for Magnesium Bromide.

a)

Mg2Br

b)

MgBr2

c)

MgBr

43.

Select the correct chemical formula for Lithium Oxide.

a)

LiO

b)

LiO2

c)

Li2O

44.

Select the correct chemical name for AlCl3.

a)

Aluminum Chloride

b)

Aluminum TriChloride

c)

Aluminum (III) Chloride

45.

Select the correct chemical name for Fe2O3.

a)

Iron oxide

b)

diiron trioxide

c)

iron (III) oxide

d)

iron (II) oxide

46.

What is the ionic charge (or oxidation state) of a Strontium ion?

a)

1+

b)

2+

c)

1-

d)

2-

47.

What is the ionic charge (or oxidation state) of a Selenium ion?

a)

1+

b)

2+

c)

1-

d)

2-

48.

How do you know that a chemical reaction (also called a chemical change) has taken place?

a)

Energy is released or absorbed

b)

Gas is given off

c)

a precipitate is formed

d)

all of the above is correct

49.

What is endothermic?

a)

absorption of heat

b)

release of heat

50.

Fireworks is an example of ________.

a)

Endothermic

b)

Exothermic

51.

A candle burning is an example of __________.

a)

Endothermic

b)

Exothermic

52.

Photosynthesis is an example of __________.

a)

Endothermic

b)

Exothermic

53.

What type of reaction requires more energy to form the new bonds of a product than the energy released by the broken bonds of the reactants?

a)

Endothermic

b)

Exothermic

c)

Exergonic

d)

None of the above

54.

What type of reaction involves a single compound breaking down into two or more smaller parts?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

55.

What type of reaction involves the replacement of a metal in a compound with another metallic element?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

56.

What type of reaction involves the replacement of a metal in a compound with another metallic element?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

57.

What type of reaction involves many elements forming a single product?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

58.

What happens to the atoms during a chemical reaction?

a)

Bonds are broken

b)

Atoms are rearranged

c)

new bonds are formed

d)

all of the above is correct

59.

What part of a reaction contains the new substances with new properties that are formed from the chemical change?

a)

reactant

b)

product

c)

subscript

d)

coefficient

60.

What part of a reaction tells you the number of atoms that are bonded together in a chemical compound?

a)

reaction

b)

product

c)

subscript

d)

coefficient

61.

What chemical reaction is - 2 KCl(s) → 2 K(s) + Cl2(g)

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

62.

What chemical reaction is AgNO3 + NaCl → AgCl + NaNO3?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

63.

What reactions is 2Li (s) + 2H2O (l) -----> 2LiOH + H2 (g)

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

64.

What reaction is 2 H2(g) + O2(g) → 2 H2O(g)

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

65.

What elements only exist in pure form in nature as two atoms of the same element covalently bonded together?

a)

Alkali metals

b)

Halogen

c)

Diatomic molecules

d)

Polyatomic molecules

66.

What theory explains why some reactions do or do not take place when molecules come in contact with one another?

a)

Law of conservation of mass

b)

Collision Theory

c)

Tyndall Effect

d)

Atomic Theory

67.

In order for reactions to occur, the reactants must collide with

a)

Sufficient energy

b)

correct orientations

c)

all of the above

d)

none of the above

68.

A catalyst can be used to do all of the following EXCEPT

a)

Increase rate of a reaction

b)

Lower activation energy of a reaction

c)

start a reaction

d)

slow down a reaction

69.

Identify the coefficients needed to correctly balance the following reaction:

KBr + Fe(OH)3 ---> KOH + FeBr3

a)

2,1 2,1

b)

3,1 3,1

c)

3,3 3,1

d)

2,3 2,3

70.

usually solid at room temperature (mercury is an exception)

a)

metals

b)

non-metals

c)

metalloid

71.

high luster (shiny)

a)

metals

b)

nonmetals

c)

metalloid

d)

A & B

72.

Semiconductor

a)

metals

b)

nonmetals

c)

metalloid

73.

brittle

a)

metal

b)

nonmetal

c)

metalloid

d)

B & C

74.

poor conductors of heat and electricity

a)

metals

b)

nonmetals

c)

metalloid

d)

A & C

75.

ductile (can be drawn into wire) and malleable (can be bent and pounded into thin sheets)

a)

metal

b)

nonmetal

c)

metalloid

d)

A & B

76.

What type of elements can exist as gases, brittle solids and a liquid under normal conditions?

a)

metals

b)

nonmetals

c)

metalloids

d)

A & B

77.

Which of the following statements is TRUE for an element in the noble gas family?

a)

It is unreactive

b)

It is chemically reactive

c)

Can form an anion

d)

Has seven valence electrons

78.

The most reactive family of metals are known as the

a)

Alkali metals

b)

Alkaline Earth metals

c)

Transition metals

d)

Halogen

79.

An atom is electrically neutral because

a)

neutrons balance the protons and electrons.

b)

the numbers of neutrons and electrons are equal.

c)

the numbers of protons and electrons are equal.

d)

the numbers of neutrons and protons are equal.

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