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Review for EAS fall semester final exam

Total questions: 107

Worksheet time: 54mins

Name
Class
Date
1.

What type of physical property does not depend on the amount of matter present?

a)

Intensive property

b)

Extensive property

c)

Chemical property

d)

Chemical change

2.

What type of physical property is dependent on the amount of matter present?

a)

Intensive property

b)

Extensive property

c)

Chemical property

d)

Chemical change

3.

Which of the following is not an example of an intensive property?

a)

Luster

b)

Malleability

c)

Volume

d)

Density

4.

Which of the following is not an example of an extensive property?

a)

Mass

b)

Volume

c)

Density

d)

Length

5.

What state of matter has no definite shape, no definite volume, and whose atoms atoms move freely?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

6.

What state of matter has no definite shape, definite volume, and whose atoms flow freely?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

7.

What state of matter has a definite shape, definite volume, and whose atoms can only vibrate in place?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

8.

What state of matter is not compressible, doesn't expand, and has very little kinetic energy (energy of motion)?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

9.

What state of matter is readily compressible, has a great ability to expand, and a lot of kinetic energy (energy of motion)?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

10.

What state of matter has almost no compressibility, a moderate ability to expand, and low to moderate kinetic energy (energy of motion)?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

11.

What do all of the elements in a group/family have in common?

a)

Same number of electrons

b)

Same number of valence electrons

c)

Same atomic mass

d)

Same atomic number

12.

What do the periods (rows) on the periodic table tell us about the electron configuration?

a)

The energy levels

b)

The shapes

c)

How many electrons are present

d)

How many protons are present

13.

Why do the elements in a group have similar properties?

a)

They have the same number of protons

b)

They have the same number of neutrons

c)

They have the same number of total electrons

d)

They have the same number of valence electrons?

14.

Color, odor, luster, density, and ductility are all examples of

a)

Chemical properties

b)

Intensive properties

c)

Extensive properties

d)

Chemical changes

15.

What is the coefficient ratio for the following equation:

_ B (s) + _ O2 (g) --> _ B2O3 (s)

a)

2, 3, 4

b)

3, 4, 2

c)

4, 3, 2

d)

4, 2, 3

16.

Size, mass, volume, length, and weight are all examples of

a)

Chemical properties

b)

Intensive properties

c)

Extensive properties

d)

Chemical changes

17.

What rule for electron orbital diagrams says that electrons enter the orbital of lowest energy levels first?

a)

Aufbau principle

b)

Pauli exlusion principle

c)

Hund's rule

d)

Dalton's theory

18.

What rule for electron orbital diagrams says that an atomic orbital may have at most 2 electrons?

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

d)

Dalton's postulates

19.

What rule for electron orbital diagrams says that electrons in the same orbital will spin in opposite directions?

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

d)

Mendeleev's rule

20.

What rule for electron orbital diagrams says that when electrons enter orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins?

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

d)

Mendeleev's rule

21.

How many orbitals does the s-block have for an energy level?

a)

1

b)

3

c)

5

d)

7

22.

How many electrons can each orbital have?

a)

1

b)

2

c)

6

d)

10

23.

How many orbitals does the p-block have?

a)

1

b)

3

c)

5

d)

7

24.

How many orbitals does the d-block have?

a)

1

b)

3

c)

5

d)

7

25.

How many orbitals does the f-block have?

a)

1

b)

3

c)

5

d)

7

26.

What element has the Noble Gas Configuration (Notation) of

[Ne] 3S2 3P4

a)

Oxygen

b)

Phosphorus

c)

Sulfur

d)

Chlorine

27.

What is the correct name for the following compound?

Cr2O3

a)

Chromium (III) oxide

b)

Chromium (II) oxide

c)

Chromium oxide

d)

Dichromium Trioxide

28.

What is the correct name for the following compound?

ZnO

a)

Zinc (I) oxide

b)

Zinc (II) oxide

c)

Zinc oxide

d)

Monozinc monoxide

29.

What is the correct chemical formula for magnesium nitrate?

a)

MgNO3

b)

Mg(NO3)2

c)

Mg2(NO3)2

d)

Mg2(NO3)

30.

What is the formula for sodium sulfate?

a)

NaSO4

b)

Na(SO4)2

c)

Na2SO4

d)

Na2(SO4)2

31.

What type of reaction involves a hydrocarbon reacting with oxygen to produce carbon dioxide and water?

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Combustion

32.

What are the reactants in a combustion reaction?

a)

Hydrocarbon and oxygen

b)

Hydrocarbon and water

c)

Hydrocarbon and carbon dioxide

d)

Carbon dioxide and water

33.

What are the products of a combustion reaction?

a)

Hydrocarbon and oxygen

b)

Carbon dioxide and oxygen

c)

Carbon dioxide and water

d)

Water and oxygen

34.

What type of property can be observed without changing the identity of the substance?

a)

Physical property

b)

Chemical property

c)

Chemical change

d)

Physical change

35.

What property describes the ability of a substance to undergo changes in identity where a new substance is produced?

a)

Physical property

b)

Chemical property

c)

Chemical change

d)

Physical change

36.

Change in state, solubility, mass, volume, freezing point, and boiling point are examples of

a)

Physical change

b)

Chemical change

c)

Physical property

d)

Chemical property

37.

Reactivity, flammability, combustibility, and toxicity are examples of a

a)

Physical change

b)

Chemical change

c)

Physical property

d)

Chemical property

38.

Which element below has 6 valence electrons, gains 2 electrons as an ion and has a charge (oxidation number) of -2?

a)

Nitrogen

b)

Carbon

c)

Sulfur

d)

Chlorine

39.

Which element below has 2 valence electrons, loses 2 electrons to become an ion, and has a charge (oxidation number) of +2?

a)

Chlorine

b)

Oxygen

c)

Sodium

d)

Magnesium

40.

Which element below has 7 valence electrons, gains 1 electron to become an ion, and has a charge (oxidation number) of -1?

a)

Chlorine

b)

Sulfur

c)

Nitrogen

d)

Sodium

41.

Which element has 1 valence electron, loses 1 electron to become an ion, and has a +1 charge (oxidation number?

a)

Chlorine

b)

Sulfur

c)

Magnesium

d)

Sodium

42.

What is the correct name Na2S?

a)

Sodium sulfide

b)

Disodium monosulfide

c)

Sodium sulfur

d)

Sodium (II) sulfide

43.

What is the correct name for Rb3P?

a)

Rubidium (II) Phosphide

b)

Rubidium (III) Phosphide

c)

Trirubidium monophosphide

d)

Rubidium Phosphide

44.

What happens to the wavelength when frequency and energy decrease?

a)

It increases

b)

It decreases

c)

It remains the same

45.

What happens to wavelength if the frequency and energy increase?

a)

It increases

b)

It decreases

c)

It remains the same

46.

Horizontal rows are called _________

a)

Groups

b)

Families

c)

Periods

d)

none of the above

47.

The vertical columns on the periodic table are called

a)

Groups

b)

Families

c)

Periods

d)

Groups or Families

48.

High melting points, good conductors of heat and electricity, and malleability are all properties of

a)

Nonmetals

b)

Metals

c)

Gases

d)

Metalloids

49.

Brittle, dull, and poor conductors of heat and electricity are properties of

a)

Metals

b)

Nonmetals

c)

Gases

d)

Metalloids

50.

What is the correct formula for calcium bromide?

a)

CaBr

b)

CaBr2

c)

Ca2Br

d)

Ca2Br3

51.

What is the correct formula for sodium sulfide?

a)

Na2S

b)

NaS2

c)

Na3S2

d)

NaS

52.

Who did the gold foil experiment to discover the dense positive nucleus?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Schrodinger

53.

Who came up with the plum pudding model to describe the structure of an atom?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Schrodinger

54.

Who did the cathode ray tube experiment to discover that electrons have a negative charge?

a)

JJThomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Shrodinger

55.

Who made the Quantum Mechanical Model?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Shrodinger

56.

Who said that electrons are found in energy levels (shells) around the nucleus like planets revolving around the sun?

a)

JJThomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Schrodinger

57.

Who said that he could predict the probability of finding electrons in the "electron cloud"?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Erwin Schrodinger

58.

In the nuclear symbol, what is the number on the top, left of the chemical symbol?

a)

Atomic number

b)

Mass Number

c)

Number of neutrons

d)

Number of protons

59.

What is the number on the bottom left of the nuclear symbol?

a)

Atomic number

b)

Mass number

c)

Number of neutrons

60.

If you have Carbon-12, how many protons, electrons, and neutrons does it have respectively?

a)

12, 6, 6

b)

6, 6, 12

c)

6, 6, 6

d)

6, 6, 8

61.

If you have Carbon-14, how many protons, electrons, and neutrons does it have respectively?

a)

12, 6, 6

b)

6, 6, 12

c)

6, 6, 6

d)

6, 6, 8

62.

What type of reaction is the following equation:

Zn (s) + Cu(NO3)2 (aq) --> Zn(NO3) (aq) + Cu (s)

a)

Synthesis

b)

Decomposition

c)

Single-Replacement

d)

Double-Replacement

63.

The atomic number is the same as the number of

a)

Protons

b)

Neutrons

c)

Electrons

d)

Ions

64.

When a compound is formed, a ____________ ____________ occurs.

a)

Physical change

b)

Chemical change

c)

Physical property

d)

Chemical property

65.

What is the coefficient ration for the following chemical equation:

_ H2 + _ O2 --> _ H2O

a)

1, 1, 1

b)

2, 2, 1

c)

2, 1, 2

d)

1, 2, 2

66.

What is the name for the following compound?

P2S3

a)

Phosphorus disulfide

b)

Diphosphorus disulfide

c)

Diphosphorus trisulfide

d)

Triphosphorus trisulfide

67.

What is the name for the following chemical compound?

CF4

a)

Carbon tetrafluoride

b)

Monocarbon tetrafluoride

c)

Tetracarbon monofluoride

d)

Carbon fluoride

68.

What is the charge of elements in group 7A?

a)

+7

b)

+1

c)

-7

d)

-1

69.

What is the charge of elements in group 5A?

a)

+3

b)

-3

c)

+5

d)

-5

70.

What is the charge of elements in the group 3A?

a)

+3

b)

-3

c)

+5

d)

-5

71.

What is the charge of elements in group 1A?

a)

+1

b)

-1

c)

+7

d)

-7

72.

The three main types of elements are _______________.

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

All answers are correct

73.

What kinds of matter are composed of 2 or more substances?

a)

Mixtures

b)

Compounds

c)

Both answers are correct

d)

Neither answer is correct

74.

Elements in the same group of the periodic table have similar properties because they have the same ______________________.

a)

Number of atoms

b)

Number of protons

c)

Valence electrons

d)

Number of neutrons

75.

What does the number represent in the isotope selenium-79?

a)

Mass number

b)

Atomic number

c)

Average atomic mass

d)

All answers are correct

76.

What is the atomic number of the element with the electron configuration of

1s2 2s2 2p6 3s2 3p6 4s2

a)

Magnesium

b)

Potassium

c)

Calcium

d)

Strontium

77.

What is the density of a 120g object that has a volume of 15cm3?

D = m/v

a)

1800 g/cm3

b)

8 g/cm3

c)

0.125 g/cm3

d)

Not enough information is given to answer this question

78.

What is a pure substance that cannot be broken down into simpler substances by physical or chemical means?

a)

Element

b)

Compound

c)

Heterogeneous mixture

d)

Homogeneous mixture

79.

What is a substance that is composed of two or more elements that can only be broken down into simpler substances by chemical means and has properties different than the substances that it is made up of?

a)

Element

b)

Compound

c)

Heterogeneous mixture

d)

Homogeneous mixture

80.

Change in color, change in odor, formation of a gas, formation of a precipitate, change in temperature, and production of light are ways that we can determine that a ______________________ has occurred.

a)

Physical property

b)

Physical change

c)

Chemical property

d)

Chemical change

81.

Dmitri Mendeleev arranged the first periodic table in order of __________________.

a)

Increasing atomic mass

b)

Decreasing atomic mass

c)

Increasing atomic number

d)

Decreasing atomic number

82.

Henry Moseley arranged the periodic table in order of _________________.

a)

Increasing atomic mass

b)

Decreasing atomic mass

c)

Increasing atomic number

d)

Decreasing atomic number

83.

What family do the group 1A elements on the periodic table belong to?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

84.

What family do the group 2A elements on the periodic table belong to?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

85.

What family do the 8A elements on the periodic table belong to?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

86.

What family do the group 7A elements on the periodic table belong to?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

87.

If a 4 g/cm3 cube is cut precisely in half, what is the density of each of the cubes?

a)

4 g/cm3

b)

2 g/cm3

c)

8 g/cm3

d)

16 g/cm3

88.

What is the average atomic mass for an element that has two isotopes? Isotope 1 has a mass of 62.9396 amu and is 69.17% abundant and isotope 2 has a mass of 64.9278 amu and is 30.83% abundant.

a)

63.93 amu

b)

63.55 amu

c)

64.31 amu

89.

Using VSEPR theory, what is the molecular geometry (shape) of CCl4?

a)

Linear

b)

Bent

c)

Trigonal pyramidal

d)

Tetrahedral

90.

Using VSPER theory, what is the bond angle for CCl4?

a)

180⁰

b)

105⁰

c)

107⁰

d)

109.5⁰

91.

Using VSEPR theory, what is the molecular geometry (shape) of H2O?

a)

Linear

b)

Bent

c)

Trigonal pyramidal

d)

Trigonal planar

92.

Using VSEPR theory, what is the bond angle for H2O?

⁰

a)

180⁰

b)

105⁰

c)

107⁰

d)

120⁰

93.

Using VSEPR theory, what is the molecular geometry (shape) for CO2?

a)

Linear

b)

Bent

c)

Trigonal pyramidal

d)

Trigonal planar

94.

How many electrons are located on the Lewis dot structure for Phosphorus?

a)

3

b)

5

c)

8

d)

15

95.

How many electrons are located on the Lewis dot structure for Oxygen?

a)

2

b)

6

c)

8

d)

18

96.

How many electrons are located on the Lewis dot structure for Magnesium?

a)

2

b)

6

c)

8

d)

18

97.

How many electrons are located on the Lewis dot structure for Fluorine?

a)

1

b)

2

c)

7

d)

8

98.

Identify the element using the noble gas (shorthand) electron configuration below:

[Ar] 4s2 3d10 4p3

a)

Germanium (Ge)

b)

Arsenic (As)

c)

Selenium (Se)

d)

Antimony (Sb)

99.

Identify the element below using noble gas (shorthand) electron configuration:

[Ne] 3s2 3p5

a)

Chlorine (Cl)

b)

Sulfur (S)

c)

Argon (Ar)

d)

Fluorine (F)

100.

What type of reaction is the following equation

_Ca(s) + _LiNO3(aq) --> _Ca(NO3)2(aq) + Li(s)

a)

Synthesis

b)

Single-Replacement

c)

Double-Replacement

d)

Combustion

101.

What is the coefficient ratio for the following balanced chemical equation?

_Ca(s) + _LiNO3(aq) --> _Ca(NO3)2(aq) + Li(s)

a)

2, 1, 2, 1

b)

2, 1, 1, 2

c)

1, 2, 2, 1

d)

1, 2, 1, 2

102.

What is the correct chemical formula for the following

titanium (IV) sulfide

a)

Ti2S

b)

Ti4S2

c)

TiS2

d)

Ti2S4

103.

What is the correct chemical formula for the following

iron (II) oxide

a)

Fe2O

b)

FeO

c)

Fe2O

d)

Fe2O2

104.

What is the average atomic mass of an element that has two isotopes? Isotope 1 has a mass of 78.92 amu and a percent abundance of 50.69%. Isotope 2 has a mass of 80.92 amu and a percent abundance of 49.31%.

a)

79.91 amu

b)

79.92 amu

c)

79.93 amu

105.

What periodic trend increases as we move from right to left on the periodic table and as we move from top to bottom on the periodic table?

a)

Ionization energy

b)

Electronegativity

c)

Atomic radii

d)

All answers are correct

106.

What element has the smallest atomic radius?

a)

Francium

b)

Helium

c)

Fluorine

d)

Calcium

107.

What element has the largest atomic radius?

a)

Francium

b)

Helium

c)

Fluorine

d)

Calcium

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