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Chemistry 1 > Chapter 9 Periodic Properties of the Elements > Flashcards

Chapter 9 Periodic Properties of the Elements Flashcards

1
Q

Necessary for the rapid electrical signaling in these cells

A

ion channels

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2
Q

Establish and control a voltage gradient in neurons

A

ion channels

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3
Q

properties whose values can be predicted based on the element’s position on the periodic table.

A

periodic properties

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4
Q

what is medeleev known for?

A

look at notes

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5
Q

when the elements are
arranged in order of increasing atomic
mass, certain sets of properties recur
periodically.

A

periodic law

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6
Q

allows us to predict
the properties of an element based on its
position on the table.

A

Mendeleev’s Periodic Law

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7
Q

what doesn’t Mendeleev’s Periodic Law explain?

A

why the pattern exists.

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8
Q

is a theory that explains
why the periodic trends in the properties exist.

A

Quantum mechanics

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9
Q

the location of electrons in atoms

A

electron configurations.

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10
Q

A description of the orbitals occupied by electrons is called
an

A

electron configuration.

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11
Q

which gives similar information but symbolizes the electron as an arrow and the orbital as a box.

A

Orbital Diagrams

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12
Q

Spinning charged particles generates a what?

A

magnetic field.

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13
Q

is a fundamental property of all electrons.

A

Spin

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14
Q

The electron’s spin adds a fourth quantum
number to the description of electrons in an atom, called the

A

spin quantum number, m(s)

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15
Q

what values does m(s)

A

can have values of +½ or −½.

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16
Q

what is pauli exclusion principle

A

*No two electrons in an atom may have the same set of
four quantum numbers.
*Therefore, no orbital may have more than two electrons,
and they must have opposite spins.

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17
Q

how many electrons are in an orbital

A

2

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18
Q

how may electrons can s sublevel have?

A

2

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19
Q

how may electrons can p sublevel have?

A

6

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20
Q

how may electrons can d sublevel have?

A

10

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21
Q

how may electrons can f sublevel have?

A

14

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22
Q

Electron-Electron interactions lead to:

A

–Shielding
–Penetration

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23
Q

describes the attractions
and repulsions between charged particles.

A

Coulomb’s law

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24
Q

what is important about Coulomb’s law

A

on notes

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25
Q

These repulsions cause the electron to have
a net reduced attraction to the nucleus;

A

shielding

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26
Q

The total amount of attraction that an
electron feels for the nucleus is called the

A

effective nuclear charge

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27
Q

The what an electron is to the nucleus,
the more attraction it experiences.

A

closer

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28
Q

The better an outer electron is at what
through the electron cloud of
inner electrons, the more attraction it will
have for the nucleus.

A

penetrating

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29
Q

related to the orbital’s radial distribution
function.

A

degree of penetration

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30
Q

Penetration and shielding cause the energies of sublevels in the same principal level to what?

A

not be degenerate

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31
Q

where are the effects of penatration important

A

in the forth and fifth prinicple levels

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32
Q

The energy separations between one set of orbitals
and the next become smaller beyond the

A

4s

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33
Q

For multi-electron atoms, the energies of the
sublevels are

A

split not degenerate

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34
Q

why are multi-electron atoms, the energies of the
sublevels split?

A

shielding and penetration

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35
Q

what do orbitals in sublevels do?

A

degenerate

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36
Q

energy levels and sublevels fill from what to what

A

low to high

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37
Q

energy levels and sublevels fill from lowest energy to
high:

A

energy levels and sublevels fill from lowest energy to
high:

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38
Q

no more than two electrons per orbital.

A

Pauli exclusion principle

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39
Q

When filling degenerate orbitals, place one electron in
each orbital before completing electron pairs.

A

Hund’s Rule

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40
Q

listing of the
sublevels in order of filling with the number of
electrons in that sublevel written as a
superscript.

A

The electron configuration

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41
Q

Electrons in all the sublevels with the
highest principal energy shell are called the

A

valence electrons

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42
Q

electrons in lower energy shells are called

A

core electrons

43
Q

One of the most important factors in the
way an atom behaves, both chemically and
physically, is the what?

A

number of valence electrons.

44
Q

corresponds to the number of valence electrons.

A

group number (main group elements)

45
Q

corresponds to the principal
energy level of the valence electrons.

A

period number

46
Q

is the maximum
number of electrons the sublevel can hold.

A

length of each “block”

47
Q

slide 55-65

A
48
Q

explains this because
the number of valence
electrons and the types of
orbitals they occupy are
also periodic.

A

quantum mechanical model

49
Q

eight valence electrons.

A

noble gases

50
Q

which noble has only two valence

A

helium

51
Q

nonreactive.

A

noble gases

52
Q

practically inert

A

He and Ne

53
Q

The reason the noble gases are so
nonreactive is that the

A

electron
configuration of the noble gases is
especially stable.

54
Q

have one more electron
than the previous noble gas.

A

alkali metals

55
Q

tend to lose one electron,

A

alkali metal

56
Q

Forming a cation with a 1+ charge

A

alkali metal

57
Q

one fewer electron than the next
noble gas

A

halogens (7A)

58
Q

forming an anion with charge 1−.

A

halogens

59
Q

In their reactions with nonmetals, they tend
to share electrons with the other
nonmetal so that each attains the electron
configuration of a noble gas.

A

halogen

60
Q

what eclectron configurations with result from ions

A

the same as the
nearest noble gas.

61
Q

are formed when nonmetal atoms gain
enough electrons to have eight valence electrons

A

anions

62
Q

are formed when a metal atom loses all its
valence electrons, resulting in a new lower energy level
valence shell.

A

cations

63
Q

Electron configurations that result in unpaired
electrons mean that the atom or ion will have a
net magnetic field;

A

paramagnetism.

64
Q

Electron configurations that result in all paired
electrons mean that the atom or ion will have no
magnetic field; this is called

A

diamagnestism

65
Q

measuring the radius of nonbonding pairs

A

Van der Waals Radius

66
Q

measuring the radius of bonding pairs

A

Covalent Radius

67
Q

is an average radius of an atom based on
measuring large numbers of elements and compounds.

A

Atomic Radius

68
Q

is the trend for atomic radius?

A

Atomic radius decreases across period (L to R)

Atomic radius increases down group

69
Q

is a net positive charge that is attracting a particular electron.

A

effective nuclear charge

70
Q

is the nuclear charge (i.e. atomic number),

A

Z

71
Q

is the number of electrons in lower energy
levels.

A

S

72
Q

what is the size of an atom is related to what?

A

the distance the valence electrons are from the nucleus.

73
Q

The larger the principal
energy level of an orbital, the
larger its what?

A

volume

74
Q

predicts the atoms should
get larger down a column.

A

Quantum-mechanics

75
Q

The larger the effective nuclear charge
an electron experiences, the what?

A

the stronger the attraction it will have for the
nucleus.

76
Q

The stronger the attraction the valence
electrons have for the nucleus, the what?

A

closer their average distance will be to
the nucleus.

77
Q

predicts the atoms should get smaller across a
period.

A

Quantum-mechanics

78
Q

Atomic radii of transition
metals are what?

A

roughly the same
size across the dblock.

79
Q

the ionic radii trends, what are the sizes of the ions and exceptions

A

anions > neutral > cations

Except Rb+ and Cs+ bigger or same size as F− and O2− .

80
Q

the larger positive charge the what?

A

smaller cation for isoelectronic species

81
Q

same electron configuration

A

isoelectronic

82
Q

The larger the negative charge what?

A

the larger the anion for isoelectronic species

83
Q

When atoms form cations, the valence
electrons are what?

A

removed

84
Q

These “new valence electrons” of a cation also experience what?

A

a larger effective nuclear charge

85
Q

When atoms form anions, electrons are what?

A

added to the valence shell

86
Q

These “new valence electrons” of a anion also experience what?

A

a smaller effective nuclear charge

87
Q

Minimum energy needed
to remove an electron from an atom or ion in
the gas phase

A

Ionization Energy

88
Q

energy to remove the first electron from
the neutral atom

A

First IE

89
Q

energy to remove an electron from the
1+ ion

A

Second IE

90
Q

what is the trend for atomic radius

A

down column increases
across period decreases

91
Q

what is the trend for ionic radius

A

down column increases
across period decreases

92
Q

what is the trend for first ionization energy

A

down column decreases
across period increases

93
Q

predicts the atom’s first ionization energy should get larger across a period and decrease down the group

A

Quantum-mechanics

94
Q

Atomic size decreases due
to what?

A

having more protons
than electrons

95
Q

when core electrons are
removed what happens?

A

here’s a large increase in
energy

96
Q

what kind of process is ionization energy?

A

endothermic

97
Q

Energy released when a
neutral atom gains an electron in the gas phase.

A

electron affinity

98
Q

is defined as exothermic
(−H), but can be endothermic (+H).

A

electron affinity

99
Q

the more negative the number the what the EA?

A

the larger

100
Q

is how closely an element’s
properties match the ideal properties of a metal.

A

metallic character

101
Q

what is the trend for metallic character

A

down column increases
across period decreases

102
Q

predicts that metallic character should increase down a column because the valence electrons are not held as strongly.

A

Quantum-mechanics

103
Q

predicts that metallic character should
decrease across a period because the valence electrons are held more strongly and the electron affinity increases.

A

Quantum-mechanics

Chemistry 1 (14 decks)

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