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Chemistry Final Study Guide

Total questions: 144

Worksheet time: 1hrs 24mins

Name
Class
Date
1.

These are all examples of what?:

-Kool-aid

-Hot coffee (Plain, no milk, no suger, no grounds in it)

-Fresh milk

a)

Homogeneus mixture

b)

Heterogenous mixture

c)

element

d)

compound

2.

These are all examples of what?:

-Vegetable soup

-Pizza

a)

Homogeneus mixture

b)

Heterogenous mixture

c)

element

d)

compound

3.

These are all examples of what?:

-Silver

-Carbon dioxide

-Oxygen

a)

Homogeneus mixture

b)

Heterogenous mixture

c)

element

d)

compound

4.

These are all examples of what?:

-Sugar

-Caffeine

a)

Homogeneus mixture

b)

Heterogenous mixture

c)

element

d)

compound

5.

These properties are ?

-Color

-Boiling point

-Density

-Malleability

-Ability to conduct electricity

a)

Physical and intensive

b)

Physical and extensive

c)

Chemical

6.

This property is?

-20 kg of bricks

a)

Physical and intensive

b)

Physical and extensive

c)

Chemical

7.

These properties are ?

-Tendency to rust

-Ability to burn

a)

Physical and intensive

b)

Physical and extensive

c)

Chemical

8.

Everything is made up of:

a)

cells

b)

carbon

c)

matter

d)

water

9.

What law states that regardless of the amount, a compound is always composed of the same elements in the same proportion by mass.

a)

law of multiple proportions

b)

law of conservation of mass

c)

law of definite proportions

d)

law of conservation of energy

10.

A physical property (like density or color) that is independent of the amount of the substance that is present is called:

a)

a chemical property

b)

an indeterminate property

c)

an extensive property

d)

an intensive property

11.

Which would be the easiest way to separate a heterogenous mixture of solids and a liquid?

a)

chromatography

b)

crystallization

c)

distillation

d)

filtration

12.

All of the elements in the same group on the periodic table share similar:

a)

mass

b)

radioactivity

c)

horizontal row on the table

d)

chemical properties

13.

A compound...

a)

is 2 or more elements chemically combined

b)

is generally stable, requiring some energy to break it apart.

c)

usually shows properties different than the properties of its component elements.

d)

all of the above

14.

Matter is anything that has ________ and takes up ________

a)

mass, area

b)

space, mass

c)

mass, space

d)

volume, space

15.

these are examples of...

-burning paper

-dissolving salt in water

-iron rusting

-milk turning sour

a)

Chemical change

b)

Physical change

16.

these are examples of...

-melting ice

-boiling water

-separating iron from sand with a magnet

-steam condensing

a)

Chemical change

b)

Physical change

17.

(ch 3) Name the elements in the following compound:

MgO

(a)  

18.

(ch 3) Name the elements in the following compound:

HCl

(a)  

19.

(ch 3) Name the elements in the following compound:

CaCO3

______, ______, ______

(a)  

20.

(ch 3) Name the elements in the following compound:

CuS

(a)  

21.

These are examples of ....:

-Has the greatest charge

-Can be stopped by paper

-Produces the greatest change in the mass #

-Is the lightest particle

a)

Alpha

b)

Beta

c)

gamma

22.

These are examples of ....:

-Can travel through paper, but not aluminum foil

-Produces the greatest change in atomic number

a)

Alpha

b)

Beta

c)

gamma

23.

These are examples of ....:

-Has no charge

-Can even travel through lead or concrete if it is not thick enough

-Particle produces the least change in the mass number

-A high-energy ray that has no electrical charge and no mass is called a...

a)

Alpha

b)

Beta

c)

gamma

24.

Which of the following is NOT part of Dalton's atomic theory?

a)

All elements are composed of atoms.

b)

Atoms are always in motion.

c)

Atoms of the same element are identical.

d)

Atoms that combine to form compounds do so in simple whole-number ratios.

25.

The nucleus of an atom is...

a)

Positively charged and contains the most mass.

b)

Negatively charged and contains the most mass.

c)

Positively charged and contains the least mass.

d)

Negatively charged and contains the least mass.

26.

Which of these statements is false?

a)

The neutron is found in the nucleus of an atom.

b)

The nucleus of an atom is positively charged.

c)

Electrons are negatively charged and have a mass of 1 AMU.

d)

Protons are positively charged.

27.

All atoms of the same element have the same...

a)

mass

b)

number of neutrons

c)

mass numbers

d)

number of protons

28.

The sum of the number of protons plus the number of neutrons in an atom equals the...

a)

mass number

b)

atomic mass

c)

atomic number

d)

nucleus number

29.

The atomic mass of an element, as seen on the periodic table...

a)

depends upon the number of isotopes of that element.

b)

depends upon the mass of each isotope of that element.

c)

depends upon the relative abundance of each isotope of the element.

d)

all of the above

30.

Which of the statements is false?

a)

atoms of the same element can have different masses

b)

atoms are mostly empty space

c)

the nucleus of an atom has a positive charge

d)

isotopes of an element have different numbers of protons

31.

Different isotopes of one element contain different number of...

a)

protons

b)

neutrons

c)

electrons

d)

nucleotides

32.

What is the charge of an electron?

a)

+1

b)

+2

c)

-1

d)

-2

e)

no charge

33.

What is the charge of a neutron?

a)

+1

b)

+2

c)

-1

d)

-2

e)

no charge

34.

What is the charge of a proton?

a)

+1

b)

+2

c)

-1

d)

-2

e)

no charge

35.

The mass of a neutron is...

a)

about the same as a proton

b)

double that of a proton

c)

about the same as an electron

d)

half that of an electron

36.

Atoms are electrically neutral because...

a)

protons and neutrons are equal in number

b)

protons and electrons are equal in number

c)

neutrons and electrons are equal in number

d)

protons, neutrons, and electrons are equal

37.

What type of reaction involves changes in the nucleus of an atom?

a)

nuclear reactions

b)

chemical reactions

c)

combustion reactions

d)

replacement reactions

38.

Which is the highest energy (most harmful) type of radiation external to the body?

a)

alpha radiation

b)

beta radiation

c)

gamma radiation

d)

all are equally bad!

39.

Unstable radioactive atoms undergo radioactive decay until...

a)

they are turned completely into energy

b)

they become a different radioisotope

c)

they form a stable, non-radioactive atoms.

d)

They form stable atoms of the same element.

40.

Which scientist developed a model known as the "plum pudding model?" He also did cathode ray tube experiments to discover the electron.

a)

Marie Curie

b)

JJ Thomson

c)

Ernest Rutherford

d)

Niels Bohr

41.

Which scientist is called the "father of modern chemistry?"

a)

Marie Curie

b)

Lavosier

c)

ernest rutherford

d)

niels bohr

42.

Which scientist coined the term radioactivity?

a)

Marie Curie

b)

Lavosier

c)

Ernest Rutherford

d)

Niels Bohr

43.

An atom with the same number of protons, but different number of neutrons is...

a)

A radioactive atom

b)

An isotope

c)

A nuclear reaction

d)

Fallout

44.

When one nucleus splits into two or more smaller nuclei it undergoes a process called...

a)

ionization

b)

fission

c)

fusion

d)

half-life

45.

When two nuclei join together to form one large nucleus it undergoes a process called...

a)

ionization

b)

fission

c)

fusion

d)

half-life

46.

Radioactive material from nuclear weapons is called...

a)

ionization

b)

cosmic rays

c)

fallout

d)

geiger counters

47.

Radiation detectors that detect x-rays and ionizing rays are called...

a)

ionization

b)

cosmic rays

c)

fallout

d)

geiger counters

48.

Two electrons can occupy the same orbital only if they have opposite spins

a)

Hund's rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Bohr model

e)

Modern theory

49.

Electrons have wave-like and particle-like properties, and are found in "fuzzy clouds" called orbitals.

a)

Hund's rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Bohr model

e)

Modern theory

50.

Each electron occupies the lowest energy orbital available (for example, the "s" orbital must be filled before "p" orbitals in the same energy level.)

a)

Hund's rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Bohr model

e)

Modern theory

51.

Electrons go around the nucleus in specific circular orbit, like planets around the sun.

a)

Hund's rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Bohr model

e)

Modern theory

52.

This ↑↑↑ is okay but this ↑↓ ↑ isn't.

a)

Hund's rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Bohr model

e)

Modern theory

53.

Photons of light are emitted from a metal's surface when light of a certain frequency shines on the surface.

a)

principle quantum number

b)

atomic emission spectrum

c)

photoelectric effect

d)

electromagnetic radiation

e)

electromagnetic spectrum

54.

Indicates the relative sizes and energies of atomic orbitals.

a)

principle quantum number

b)

atomic emission spectrum

c)

photoelectric effect

d)

electromagnetic radiation

e)

electromagnetic spectrum

55.

A form of energy exhibiting wavelike behavior as it travels through space

a)

principle quantum number

b)

atomic emission spectrum

c)

photoelectric effect

d)

electromagnetic radiation

e)

electromagnetic spectrum

56.

A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors.

a)

principle quantum number

b)

atomic emission spectrum

c)

photoelectric effect

d)

electromagnetic radiation

e)

electromagnetic spectrum

57.

Includes all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths.

a)

principle quantum number

b)

atomic emission spectrum

c)

photoelectric effect

d)

electromagnetic radiation

e)

electromagnetic spectrum

58.

The lowest energy state of an electron is called its _______ state

a)

initial

b)

photon

c)

excited

d)

ground

59.

Electrons located in the outermost shell of an atom (outer s and p orbitals) are called _____ electrons

a)

quantum

b)

fixed

c)

valence

d)

configuration

60.

A photon is...

a)

A "particle" of light or other electromagnetic radiation with no mass but a specific amount of energy

b)

the name given to any valence electron

c)

the lowest energy state of an electron

d)

part of the Bohr model, now proven to be incorrect.

61.

Which of the following orbitals is spherical shaped?

a)

3p

b)

2s

c)

4d

d)

5f

62.

Two electrons can occupy the same orbital only if they...

a)

have the same spin

b)

have opposite charges

c)

have opposite spins

d)

have enough energy

63.

The 3s orbital differs from the 2s orbital because the 3s orbital is:

a)

smaller

b)

larger

c)

a different shape

d)

more crowded

64.

how many electrons can the d orbitals hold?

a)

four

b)

five

c)

ten

d)

fourteen

65.

How can you tell when electrons "excited" by heat or other energy return to their ground state

a)

you can't

b)

they give off light

c)

the atoms become radioactive

d)

the atoms get hotter

66.

Which rule is being broken? ↑↑ ↑↓ ↑↓ /2p

a)

hund'e rule

b)

aufbau principle

c)

pauli exclusion principle

d)

none of the above

67.

The atomic orbitals represent

a)

the exact location of electrons

b)

2-dimensional views of how electrons move

c)

a wave and a phase

d)

the probable location of an electron

68.

light can act as both

a)

a particle and an ion

b)

a particle and a wave

c)

a wave and a phase

d)

phase and a particle

69.

Waves that have a longer wavelength have a ____ frequency

a)

higher

b)

similar

c)

lower

d)

broader

70.

The heisenburg uncertainty principle states that it is impossible to know both the position and the ___ of a particle at the same time.

a)

angular momentum

b)

frequency

c)

wavelength

d)

velocity

71.

Developed the law of octaves

a)

Moseley

b)

Mendeleev

c)

Newlands

72.

Arranged the elements in order of increasing atomic number

a)

Moseley

b)

Mendeleev

c)

Newlands

73.

Arranged the elements in order of increasing atomic mass.

a)

Moseley

b)

Mendeleev

c)

Newlands

74.

The only noble gas that does not have a full octet is:

a)

hydrogen

b)

helium

c)

argon

d)

neon

75.

When elements are arranged by increasing ____, elements with similar properties re-occur at regular intervals.

a)

neutrons

b)

radius

c)

atomic number

d)

charge

76.

The ____ play the largest role in determining chemical properties

a)

protons

b)

electrons

c)

neutrons

d)

valence electrons

77.

An atom's ability to attract electrons is called:

a)

electronegativity

b)

ionization energy

c)

atomic radius

d)

electron affinity

78.

The energy required to remove an electron is called:

a)

electronegativity

b)

ionization energy

c)

atomic radius

d)

electron affinity

79.

The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is called the:

a)

atomic theory

b)

periodic table

c)

chemical law

d)

periodic law

80.

The most electronegative element is:

a)

H

b)

At

c)

Rn

d)

F

81.

What period is carbon in?

a)

2

b)

4

c)

6

d)

14

82.

What group is calcium in?

a)

2

b)

4

c)

6

d)

14

83.

At room temperature, which of the following elements does not exist in the gaseous state?

a)

I

b)

F

c)

O

d)

Cl

84.

how many valence electrons does sodium have?

a)

1

b)

3

c)

7

d)

11

85.

How many valence electrons does aluminum have?

a)

1

b)

3

c)

13

d)

26

86.

Which element has the largest atomic radius

a)

Li

b)

N

c)

O

d)

C

87.

Which element has the highest ionization energy?

a)

Be

b)

O

c)

F

d)

Ne

88.

What is the force that holds two atoms together?

a)

energy level

b)

ions

c)

electron bond

d)

chemical bond

89.

What is a polyatomic ion that is negatively charged and includes one or more oxygen atoms?

a)

a cation

b)

an electron

c)

an oxyanion

d)

an anionide

90.

What are the ions made up of more than one atom called?

a)

cations

b)

anions

c)

polyatomic ions

d)

anionides

91.

What is the bond between two oppositely charged ions?

a)

ionic bond

b)

covalent bond

c)

acidic bond

d)

molecular bond

92.

What is the name of an ion that is formed from a single atom?

a)

a polyatomic ion

b)

a binary ionic compound

c)

a monatomic ion

d)

an oxyanion

93.

What is another name for the charge of the ion that shows how many electrons were gained or lost?

a)

ionic number

b)

oxidation number

c)

pseudo-noble gas formation

d)

monatomic number

94.

The formula unit of an ionic compound shows the...

a)

numbers of atoms within each molecule

b)

total number of each kind of ion in a sample

c)

simplest whole number ratio of the ions

d)

number of nearest neighboring ions surrounding each kind of ion

95.

Elements tend to react so that they can acquire...

a)

a full octet

b)

more electrons

c)

the structure of a halogen

d)

less electrons

96.

What ending designates a monatomic ion?

a)

-ide

b)

-ite

c)

-ate

d)

-ium

97.

What is the formula for copper (II) chloride?

a)

Cu2Cl

b)

CuCl2

c)

CuCl

d)

Cu4Cl2

98.

Which shows the oxidation number of sodium?

a)

1+

b)

1-

c)

7+

d)

7-

99.

Which shows the oxidation number of silver

a)

1+

b)

1-

c)

7+

d)

7-

100.

what oxidation number would the element with the electron configuration 1s2 2s2 2p6 3s2 3p4 have?

a)

16

b)

6+

c)

2-

d)

6-

101.

Which gets named first when naming an ionic compound?

a)

the anion

b)

the cation

c)

the binary ion

d)

the electron

102.

the group 2 elements would form...

a)

anions

b)

cations

c)

protons

d)

electrons

103.

Which shows the oxidation number of iodine?

a)

17

b)

7+

c)

1+

d)

1-

104.

What is the name of the compound TiI4?

a)

titanium iodide

b)

titanium (IV) iodide

c)

titanium iodide (IV)

105.

Which noble gas electron configuration does a sodium ion have?

a)

Neon

b)

Argon

c)

Krypton

d)

Helium

106.

Ionic compounds have _____ conductivity when _____.

a)

high, dissolved in water

b)

high, solid

c)

low, dissolved in water

d)

low, solid

107.

The overall charge of a formula unit for an ionic compound...

a)

is always zero

b)

is always negative

c)

is always positive

d)

may have any value

108.

Metals _____ electrons and form _____.

a)

gain, cations

b)

lose, cations

c)

gain, anions

d)

lose, anions

109.

The roman numerals in a compound's name represents:

a)

the number of nonmetal ions

b)

the number of metal ions

c)

the oxidation state of the nonmetal

d)

the oxidation state of the metal

110.

A three dimensional arrangement of particles in an ionic solid is called:

a)

a crystal lattice

b)

formula unit

c)

the electron sea

d)

an electrolyte

111.

When ions form, which of the following is correct?

a)

the metal atom gains electrons from the nonmetal

b)

the nonmetal atom gains electrons from the metal

c)

both atoms gain electrons

d)

neither atom gains electrons

112.

Ionic compounds have ____ melting points and ____ boiling points

a)

low, low

b)

high, low

c)

low, high

d)

high, high

113.

Alkali metals make ions with a ____ charge.

a)

+1

b)

-7

c)

+2

d)

-2

114.

A _____ alloy is an alloy where smaller elements fit in between the metallic cations.

a)

substitutional

b)

mixed

c)

uniform

d)

interstitial

115.

reactions that absorb energy from their surroundings are said to be ___.

a)

entropic

b)

endothermic

c)

exothermic

d)

enthalpic

116.

Mark ALL of the following choices that are ionic compounds.

a)

NaI

b)

PO4

c)

NH4Cl

d)

Mg(OH)2

e)

C6H12O6

117.

Electrons that are not bound to any one metallic cation are said to be _____.

a)

delocalized

b)

localized

c)

electrolytes

d)

conducting

118.

Given the name write the formula for the following ionic compound:

Sodium nitrate

(a)  

119.

Given the name write the formula for the following ionic compound:

Silver nitride

(a)  

120.

Given the name write the formula for the following ionic compound:

Barium hydroxide

(a)  

121.

Given the name write the formula for the following ionic compound:

Iron (III) phosphate

(a)  

122.

Given the name write the formula for the following ionic compound:

Tin (IV) bromide

(a)  

123.

Given the formula write the name for the following ionic compound:

NH4I

(a)  

124.

Given the formula write the name for the following ionic compound:

Zn(NO2)2

(a)  

125.

Given the formula write the name for the following ionic compound:

FeF2

(a)  

126.

Given the formula write the name for the following ionic compound:

Ca(CLO3)2

(a)  

127.

Given the formula write the name for the following ionic compound:

K2O

(a)  

128.

What is the maximum amount of electrons a hydrogen atom can hold in its bonding orbitals?

a)

1

b)

2

c)

8

d)

10

129.

According to VSEPR theory, molecules, adjust their shapes to keep which of the following as far apart as possible?

a)

Pairs of valence electrons

b)

Inner shell electrons

c)

Mobile electrons

d)

The electrons closest to the nuclei

130.

Intermolecular forces tend to be ______ than covalent bonds between atoms.

a)

Weaker

b)

Stronger

c)

Closer

d)

Larger

131.

Hydrogen bonding can occur between hydrogen and all of the following, except:

a)

O

b)

F

c)

Cl

d)

N

132.

If electrons are shared unequally, a __________ bond is formed.

a)

Polar

b)

Non-polar

133.

Electrons repel each other

a)

True

b)

False

134.

The strongest intermolecular force is a dispersion force.

a)

True

b)

False

135.

Lone pairs do not affect the molecules molecular geometry.

a)

True

b)

False

136.

VSEPR stands for the Valence Shell Electron Pair Resonance theory

a)

True

b)

False

137.

A covalent bond is the electrostatic attraction that binds oppositely charged ions.

a)

True

b)

False

138.

In a covalent bond, the orbitals overlap.

a)

True

b)

False

139.

Ionic compounds and covalent bonds have similar melting points

a)

True

b)

False

140.

Both ionic and covalent compounds are electrolytes

a)

True

b)

False

141.

Polar molecules are very good at dissolving nonpolar molecules.

a)

True

b)

False

142.

Dipole-dipole intermolecular forces can occur in a nonpolar covalent bond

a)

True

b)

False

143.

Ionic bonding involves electron _______

a)

Exchange

b)

Sharing

144.

Covalent bonding involved electron ________

a)

Exchange

b)

Sharing

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