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Honors Chemistry > Module 4 Test > Flashcards

Module 4 Test Flashcards

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1
Q

What were categories in Lavoisier’s Table of Simple Substances?

A

Metals and nonmetals

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2
Q

What significantly helped chemists organize the many facts associated with the elements?

A

Agreeing on how to determine atomic masses

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3
Q

Who noticed that by arranging the elements in order of increasing atomic mass, their properties repeated every eighth element?

A

John Newlands

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4
Q

What were features of Mendeleev’s periodic table?

A

Blank spaces predicted elements yet to be discovered

Elements in columns had similar properties

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5
Q

Moseley improved the periodic table by arranging the elements in order of atomic _____ rather than atomic _____.

A

Number, mass

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6
Q

About how many the chemical elements were known by 1870?

A

Over 60

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7
Q

Chemists were better able to organize facts about the elements after they agreed upon a method for accurately determining the atomic _____ of the elements

A

Mass

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8
Q

When John Newlands arranged the elements by atomic mass, he noticed that their properties repeated every
_____ element.

A

Eighth

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9
Q

What is the periodic repetition of properties when the elements are arranged by increasing atomic number?

A

Periodic law

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10
Q

Arrange the statements relating to the development of the periodic table in chronological order.

A

Elements arranged by increasing atomic mass
Repetition noticed in properties of every eighth element
Existence and properties of undiscovered elements predicted
Discovered that atoms contain a unique number of protons called the atomic number
Elements arranged in order of increasing atomic number

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11
Q

Moseley improved the pattern of properties in the periodic table by arranging elements by ______.

A

Atomic number

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12
Q

What events played major roles in the advancing the number of known elements?

Multiple select question.

A

Advent of electricity

Development of the spectrometer

The industrial revolution

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13
Q

The statement that there is a periodic repetition of properties of the elements when they are arranged by increasing atomic number is called the ____ ____.

A

Periodic Law

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14
Q

The modern periodic table consists of boxes, each containing an element name, symbol, atomic ____, and atomic ____.

A

Number, mass

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15
Q

What scientists contributed to the development of the periodic table?

A

Henry Moseley
Dmitri Mendeleev
John Newlands
Lothar Meyer

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16
Q

What are key features of the modern periodic table?

A
  1. The elements in groups 3 to 12 are called the transition elements.
  2. The boxes are arranged into a series of columns, called groups or families, and rows, called periods.
  3. The elements in groups 1, 2, and 13 to 18 are referred to as the main group, or representative elements.
  4. It consists of boxes, each containing an element name, symbol, atomic number, and atomic mass.
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17
Q

What is a vertical column of elements in the periodic table arranged in order of increasing atomic number?

A

Group

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18
Q

What elements have been known since prehistoric times?

A

Carbon
Gold
Silver

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19
Q

What is a horizontal row of elements in the modern periodic table?

A

Period

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20
Q

The elements in groups 1, 2, and 13 to 18 possess a wide range of chemical and physical properties. For this reason, they are often referred to as the main group elements or what other term?

A

Representative elements

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21
Q

What term describes the elements in groups 3 through 12 on the periodic table?

A

Transition elements

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22
Q

What were categories in Lavoisier’s Table of Simple Substances?

A

Metals
Nonmetals
Gases
Earths

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23
Q

What are elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity?

A

Metals

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24
Q

What are examples of metals?

A

calcium (Ca)

sodium (Na)

mercury (Hg)

lithium (Li)

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25
Q

Elements in groups 3 through 12 (with the exception of the lanthanide series and actinide series) are called the _____ metals.

A

Transition

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26
Q

The transition elements included in the lanthanide series and actinide series are called the _____ transition metals.

A

Inner

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27
Q

What are the transition elements (with the exception of the lanthanide series and actinide series) located in groups 3 through 12 on the periodic table?

A

Transition metals

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28
Q

Elements 57 through 71 in the sixth period are known as the ______ series.

A

Lanthanide

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29
Q

What term refers to elements 89 through 103 in the seventh period of the periodic table?

A

Actinide series

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30
Q

What are examples of nonmetals?

A

carbon (C)

radon (Rn)

helium (He)

bromine (Br)

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31
Q

What term refers to the lanthanide series and actinide series, located at the bottom of the periodic table?

A

Inner transition metals

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32
Q

What is the group of elements that are generally gases or brittle, dull looking solids, and poor conductors of heat and electricity?

A

Nonmetals

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33
Q

The highly reactive elements in group 17 of the periodic table are known as ____.

A

Halogens

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34
Q

What term describes the extremely unreactive group 18 gases?

Multiple choice question.

A

Noble gases

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35
Q

Many nonmetals have interesting properties and applications. For example, the only nonmetal that is a liquid at room temperature is _______ the most abundant element in the human body is the nonmetal
_____ and the element commonly added to toothpaste and drinking water to prevent tooth decay is
______

A

Bromine
Oxygen
Fluorine

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36
Q

What are examples of metalloids?

A

antimony (Sb)

germanium (Ge)

arsenic (As)

silicon (Si)

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37
Q

What are elements that have the physical and chemical properties of both metals and nonmetals?

A

Metalloids

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38
Q

Elements in the same group have similar chemical properties because they have the same _____ __ ______ _______.

A

number of valence electrons

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39
Q

Two important metalloids that are used extensively in computer chips and solar cells are _____ and ______.

A

Silion, germanium

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40
Q

The energy level of an element’s valence electrons indicates the _____ on the periodic table in which it is found.

A

Period

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41
Q

What can be determined from the period in which an element appears on the periodic table?

A

energy level of valence electrons

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42
Q

The group 18 elements are extremely stable because the ___ and ____ orbitals are completely filled.

A

S, P

43
Q

The periodic table is divided into sections, or blocks, representing the atom’s energy sublevel being filled with valence electrons. These are known as the ___, ____, ___, and _____ blocks.

A

S, P, D, F

44
Q

What characterize the electron configurations of the d-block elements?

A

filled outermost s orbital of energy level n

filled or partially filled d orbitals of energy level n – 1

45
Q

What explains the stability of the electron configurations of the group 18 elements?

A

The s and p orbitals are completely filled.

46
Q

Elements in the f-block of the periodic table are characterized by a filled or partially filled outermost ____ orbital and filled or partially filled 4f and 5f orbitals.

A

S

47
Q

Most d-block elements in period 4 have partially filled d orbitals of energy level ____.

A

3

48
Q

For metals such as sodium, atomic radius is defined as

A

half the distance between nuclei in a crystal of the element.

49
Q

What is an observed trend in atomic radii?

A

atomic radii decrease across a period from left to right

50
Q

Atomic radii decrease across a period because the valence electrons are all in the same energy level but are attracted more strongly by the greater number of _____ in the nucleus.

A

Protons

51
Q

What is an observed trend in atomic radii?

A

atomic radii increase down a group

52
Q

Atomic radii generally increase moving down a group because the increased distance of valence electrons from the nucleus offsets the pull of the increased _____ charge.

A

Positive

53
Q

In general, there is a(n) ______ in atomic radii as you move from left to right across a period.

A

decrease

54
Q

What are reasons for atomic radii decreasing across a period?

A

no new energy levels are added

more protons are added to the nucleus

no additional electrons come between the valence electrons and the nucleus

55
Q

An atom or group of bonded atoms that has a positive or negative charge is called a/an ____.

A

ion

56
Q

Atoms always become smaller when they _____ electrons and form ions with a _____ charge.

A

Lose, positive

57
Q

What factors explain why atomic radii generally increase when moving down a group?

A

electrons in inner orbitals shield the outer electrons from the nucleus

increased distance of valence electrons from the nucleus offsets the pull of increased nuclear charge

added principal energy levels are farther from the nucleus

58
Q

An atom that gains an electron and forms an ion with a ______ charge becomes _____ in size.

A

Negative, bigger

59
Q

Moving across a period, the change from positive to negative ions causes a sudden _____ in ionic radii at group 15 or 16.

A

Growth

60
Q

How do ionic radii vary moving down a group?

A

Both positive and negative ionic radii increase.

61
Q

True or false: Atoms always become larger when they lose electrons and form positively charged ions.

A

False

62
Q

Why is this false: Atoms always become larger when they lose electrons and form positively charged ions.

A

They become smaller because losing a valence electron results in a completely empty outer orbital or in valence electrons experiencing less electrostatic repulsion and therefore a greater nuclear charge.

63
Q

The energy required to remove an electron from a gaseous atom is called the ______ energy.

A

Ionization

64
Q

Atomic radii generally increase moving down a group because the increased distance of valence electrons from the nucleus offsets the pull of the increased _____ charge.

A

Positive

65
Q

When atoms gain electrons, they ______.

A

form negatively charged ions and become larger

66
Q

What of these are correct descriptions of trends in ionic radii moving from left to right across a period?

A

radii of negative ions decrease

radii increase at the dividing line between positive and negative ions

radii of positive ions decrease

67
Q

Ionic radii of both positive and negative ions ____ moving down a group.

A

Increase

68
Q

What are characteristics of atoms with high ionization energy?

A

They are unlikely to form positive ions.

They have a strong hold on electrons.

69
Q

What factors explain why atomic radii generally increase when moving down a group?

A

electrons in inner orbitals shield the outer electrons from the nucleus

added principal energy levels are farther from the nucleus

increased distance of valence electrons from the nucleus offsets the pull of increased nuclear charge

70
Q

The third ionization energy is the energy required to remove ______.

A

one electron from a 2+ ion

71
Q

How do ionic radii vary moving down a group?

A

Both positive and negative ionic radii increase.

72
Q

Ionization energy generally _____ across a period.

A

Increases

73
Q

Atoms that have a low ionization energy are likely to form ______ ions.

A

Positive

74
Q

What explains the decrease in ionization energy moving down a group?

A

The valence electrons are farther from the nucleus.

75
Q

True or false: For a given atom, the second ionization energy is always less than the first ionization energy.

A

False

76
Q

Why is this false: For a given atom, the second ionization energy is always less than the first ionization energy.

A

Each successive electron requires more energy to remove than the previous one.

77
Q

When atoms gain electrons, they ______.

A

form negatively charged ions and become larger

78
Q

Which rule states that atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons?

A

octet rule

79
Q

The relative ability of atoms to attract electrons in a chemical bond is called ______.

A

Electronegativity

80
Q

True or false: Electronegativity increases moving down a group.

A

False

81
Q

Why is this false: Electronegativity increases moving down a group.

A

Electronegativity decreases moving down a group because electrons are farther from the nucleus.

82
Q

What did John Newlands do?

A

He discovered the law of octaves

83
Q

What did Mendeleev contribute to the periodic table?

A

He provided the base to organize the elements on the table, predicted undiscovered elements

84
Q

What is the periodic table?

A

A table that organizes elements by their properties

85
Q

Elements in groups 3-12 are called?

A

Transition metals

86
Q

Elements on the periodic table are in order of increasing _____?

A

Both atomic number and number of protons

87
Q

Mendeleev organized his periodic table according to what?

A

Atomic mass

88
Q

Elements with similar outer electron configurations have what in common?

A

They have similar reactivities because they have similar numbers of valence electrons

89
Q

Why are alkali metals so reactive?

A

They have exactly one electron on their outer shell

90
Q

What are metalloids?

A

Semi-conductors

91
Q

Where are metalloids located?

A

They are located along the “staircase”

92
Q

Is Ge a metal, nonmetal, or metalloid?

A

Metalloid

93
Q

Is Na a metal, nonmetal, or metalloid?

A

Metal

94
Q

Is Xe a metal, nonmetal, or metalloid?

A

Nonmetal

95
Q

Is Rn a metal, nonmetal, or metalloid?

A

Nonmetal

96
Q

What is electron shielding?

A

Inner electrons shield the valence electrons on the shell from protons or the nucleus

97
Q

Elements in the same group on the periodic table have similar?

A

Properties

98
Q

Groups on the periodic table are arranged?

A

Vertically

99
Q

The rows of a periodic table are called?

A

Periods

100
Q

What is a Lewis dot diagram?

A

A diagram showing the number of valence electrons

101
Q

Electron affinity is?

A

The amount of energy required to add an electron to an atom

102
Q

Electronegativity is?

A

The measure of the tendency to attract electrons

103
Q

Ionization energy is?

A

The amount of energy needed to remove an electron from the atom

Honors Chemistry (13 decks)

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