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Chemistry > Chapter 7 Review > Flashcards

Chapter 7 Review Flashcards

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1
Q

Effective Nuclear Charge is equal to

A

Atomic number - Core electrons

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2
Q

Effective Nuclear Charge is smaller than the ________

A

Charge of the nucleus (Z)

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3
Q

In an isoelectric series, ionic charge _____ while nuclear charge _____

A

Decreases , increases

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4
Q

Chemical properties are determined by: . . .

A

The number of valence electrons and how strongly the valence electrons are attracted to the nucleus

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5
Q

Though electrons are attracted to the nucleus, the __________, also known as “shield” electrons “shield” the valence electrons from the force of the nucleus

A

core electrons

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6
Q

What is “S”?

A

“S” is the number of core electrons

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7
Q

What is “Z”?

A

“Z” is the atomic number of an atom

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8
Q

What is “Zeff”

A

“Zeff” is the effective nuclear charge of an atom

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9
Q

What is “Zeff” in terms of valence electrons?

A

“Zeff” is the charge “felt” by the valence electrons of an atom

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10
Q

Atomic radii is the . . .

A

Distance between the nucleus and outermost electron

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11
Q

The unit for Atomic radii is the . . .

A

Angstrom or “Å”

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12
Q

As the amount of valence electrons increases, the attraction of the nucleus decreases, causing the electrons to “spread out”. This means that Atomic radii . . . from left to right.

A

decreases

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13
Q

As we go step down rows, the Atomic radii . . . because the amount of electron shells is increasing

A

increases

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14
Q

The greater the Zeff, the . . .

A

greater the attraction of the nucleus

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15
Q

Because there are fewer electrons in a cation compared to the parent atom, a cation is . . . than the parent atom

A

smaller

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16
Q

Because there are more electrons in an anion compared to the parent atom, an anion is . . . than the parent atom

A

larger

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17
Q

The Zeff of cations is . . . than the Zeff of the parent atom

A

greater

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18
Q

The Zeff of anions is . . . than the Zeff of the parent atom

A

less

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19
Q

In an isometric series, Atomic radii . . . with an increasing nuclear charge

A

decreases

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20
Q

In an isoelectric series, the largest ion will have the . . . number of protons

A

smallest

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21
Q

In an isoelectric series, the smallest ion will have the . . . number of protons

A

largest

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22
Q

An isoelectric series is a series of . . .

A

ions with the same number of electrons

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23
Q

Ionization energy is . . .

A

the minimum energy required to REMOVE one electron from an atom or ion

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24
Q

Ionization energy makes . . .

A

cations

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25
Q

Second ionization energy is always . . . than first ionization energy

A

greater

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26
Q

The correct way to show the first ionization energy of an atom (X) is . . .

A

X –> X(+) + e(-)

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27
Q

There is a sharp increase in ionization energy when you . . .

A

remove a core electron

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28
Q

For transition metals, if s and p orbitals have electrons, ___ electrons are removed first, then ___ electrons, before ___ electrons

A

p, s, and d

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29
Q

The exception groups for ionization energy are groups ___ and ___

A

3A and 6A

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30
Q

The more the amount of valence electrons, the easier it is to remove one, which means that ionization energy . . . from left to right

A

increases

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31
Q

As we move from top to bottom of the table of elements, valence electrons are farther and farther away, making it easy to remove one. This means that ionization energy . . . from top to bottom.

A

decreases

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32
Q

Electron Affinity’s symbol is ___

A

ΔE

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33
Q

Electron Affinity is . . .

A

The CHANGE in energy to ADD one electron to form an ANION

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34
Q

The more negative the Electron Affinity, the . . .

A

more stable the anion

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35
Q

The more stable the anion, . . .

A

the greater attraction between an atom and the added electron

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36
Q

If the Electron Affinity is positive, . . .

A

the less stable the anion

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37
Q

The correct way to show the Electron Affinity of an atom (X) is . . .

A

X + e(-) –> X(-)

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38
Q

The most non-metallic
elements have the . . . values

A

most negative

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39
Q

Groups where the electron affinities are near positive are Groups ___, ___, and ___

A

2A, 5A, and 8A

40
Q

From left to right, electron affinity . . .

A

increases

41
Q

From top to bottom, electron affinity . . .

A

stays the same

42
Q

The period with generally the largest electron affinity is . . .

A

period 3

43
Q

Electron Negativity’s symbol is . . .

A

EN

44
Q

Electron Negativity is . . .

A

the ability of an atom, that is bonded to
another atom, to attract electrons to itself

45
Q

Electron Negativity . . . from left to right

A

increases

46
Q

Electron Negativity . . . from top to bottom

A

decreases

47
Q

The exception to the Electron Negativity is . . .

A

Group 8A

48
Q

Metals have . . . ionization energies

A

low

49
Q

Metal oxides are . . .

A

bases, which
1. react with acids to form salt
and water
2. dissolve in water and react to form metal hydroxides.

50
Q

Metal oxide + acid –>

A

salt + water

51
Q

Metal oxide + water –>

A

metal hydroxide

52
Q

Alkali metals have low . . .

A

densities, melting points, and ionization energies

53
Q

Compared to Alkali metals, Alkaline metals have higher . . .

A

densities, melting points, and ionization energies

54
Q

As you go down the group of Alkaline metals, ________ tends to increase

A

reactivity

55
Q

The melting points of nonmetals are generally . . . than those of metals

A

lower

56
Q

These elements occur naturally as diatomic

A

H, N, O, F, Cl, Br, and I

57
Q

Nonmetals tend to . . .

A

gain electron and become anions

58
Q

Nonmetal oxides are . . .

A

acids, which
1. dissolve in basic solutions to form a salt
and water
2. dissolve in water react to form acids

59
Q

nonmetal oxide + base –>

A

salt + water

60
Q

nonmetal oxide + water –>

A

oxyacid

61
Q

Hydrogen is a . . .

A

nonmetal gas

62
Q

Hydrogen typically likes to form . . .

A

the +1 ion

63
Q

The ionization energy of Hydrogen is . . . than the Alkali metals

A

higher

64
Q

When Hydrogen is part of an ionic compound with a metal, Hydrogen becomes a . . .

A

H(-)

65
Q

Ionic compounds with H(-) are called . . .

A

Metal hydrides

66
Q

Under extreme pressure, Hydrogen can . . .

A

act like a metal, conduct electricity, and conduct heat

67
Q

One or more forms of a chemical element that occur in the same
physical state are known as . . .

A

Allotropes

68
Q

Allotropes form because of the . . .

A

different ways atoms may be bonded together

69
Q

Allotropes may display . . . chemical and physical properties

A

very different

70
Q

In response to changes in pressure,
temperature, and exposure to light, elements may change ________

A

Allotrpoes

71
Q

What elements are all nonmetals and have highly negative electron affinities?

A

F, Cl, Br, and I

72
Q

What element removes electrons from almost any substance it contacts (very
exothermic), including water, and is very reactive?

A

Fluorine

73
Q

The halogens react directly with most metals to form . . .

A

Ionic halides

74
Q

The halogens also react with diatomic H to form gaseous

A

Hydrogen halide compounds

75
Q

The Noble Gases are . . .

A

gaseous, monatomic nonmetals

76
Q

Noble gases are very unreactive because they have full . . .

A

s and p subshells

77
Q

The only noble gases to form chemical compounds are . . .

A

the heaviest because of the lower ionization energies

78
Q

Metals tend to ____ electrons

A

lose

79
Q

Metals tend to lose electrons because of . . .

A

low ionization energies

80
Q

Nonmetals tend to ____ electrons

A

gain

81
Q

Nonmetals tend to lose electrons because of . . .

A

high electron affinities

82
Q

Compounds formed between metals and nonmetals tend to be _____

A

ionic

83
Q

An element’s reactivity is characterized by its . . .

A

metallic character

84
Q

Metals are on the left side of the Table while Nonmetals are on the right side of the Table, which means Metallic Character _________ from left to right

A

decreases

85
Q

Because Ionization
energy decreases down a
group, making it easier for an atom to lose an electron, Metallic Character _________ from top to bottom

A

increases

86
Q

Group 1A is

A

Alkali Metals

87
Q

Group 2A is

A

Alkaline Earth Metals

88
Q

Group 8A is

A

Noble Gases

89
Q

Group 7A is

A

The Halogens

90
Q

Group 6A is

A

The Chalcogens

91
Q

Group 1A elements include . . .

A

Li, Na, K, Rb, Cs, and Fr

92
Q

Group 2A elements include . . .

A

Be, Mg, Ca, Sr, Ba, and Ra

93
Q

Group 8A elements include . . .

A

He, Ne, Ar, Kr, Xe, and Rn

94
Q

Group 7A elements include . . .

A

F, Cl, Br, I, and At

95
Q

Group 6A elements include . . .

A

O, S, Se, Te, and Po

Chemistry (17 decks)

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