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Chemistry > Chapter 7 Review > Flashcards

Chapter 7 Review Flashcards

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
Second ionization energy is always . . . than first ionization energy
greater
26
The correct way to show the first ionization energy of an atom (X) is . . .
X --> X(+) + e(-)
27
There is a sharp increase in ionization energy when you . . .
remove a core electron
28
For transition metals, if s and p orbitals have electrons, ___ electrons are removed first, then ___ electrons, before ___ electrons
p, s, and d
29
The exception groups for ionization energy are groups ___ and ___
3A and 6A
30
The more the amount of valence electrons, the easier it is to remove one, which means that ionization energy . . . from left to right
increases
31
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.
decreases
32
Electron Affinity's symbol is ___
ΔE
33
Electron Affinity is . . .
The CHANGE in energy to ADD one electron to form an ANION
34
The more negative the Electron Affinity, the . . .
more stable the anion
35
The more stable the anion, . . .
the greater attraction between an atom and the added electron
36
If the Electron Affinity is positive, . . .
the less stable the anion
37
The correct way to show the Electron Affinity of an atom (X) is . . .
X + e(-) --> X(-)
38
The most non-metallic elements have the . . . values
most negative
39
Groups where the electron affinities are near positive are Groups ___, ___, and ___
2A, 5A, and 8A
40
From left to right, electron affinity . . .
increases
41
From top to bottom, electron affinity . . .
stays the same
42
The period with generally the largest electron affinity is . . .
period 3
43
Electron Negativity's symbol is . . .
EN
44
Electron Negativity is . . .
the ability of an atom, that is bonded to another atom, to attract electrons to itself
45
Electron Negativity . . . from left to right
increases
46
Electron Negativity . . . from top to bottom
decreases
47
The exception to the Electron Negativity is . . .
Group 8A
48
Metals have . . . ionization energies
low
49
Metal oxides are . . .
bases, which 1. react with acids to form salt and water 2. dissolve in water and react to form metal hydroxides.
50
Metal oxide + acid -->
salt + water
51
Metal oxide + water -->
metal hydroxide
52
Alkali metals have low . . .
densities, melting points, and ionization energies
53
Compared to Alkali metals, Alkaline metals have higher . . .
densities, melting points, and ionization energies
54
As you go down the group of Alkaline metals, ________ tends to increase
reactivity
55
The melting points of nonmetals are generally . . . than those of metals
lower
56
These elements occur naturally as diatomic
H, N, O, F, Cl, Br, and I
57
Nonmetals tend to . . .
gain electron and become anions
58
Nonmetal oxides are . . .
acids, which 1. dissolve in basic solutions to form a salt and water 2. dissolve in water react to form acids
59
nonmetal oxide + base -->
salt + water
60
nonmetal oxide + water -->
oxyacid
61
Hydrogen is a . . .
nonmetal gas
62
Hydrogen typically likes to form . . .
the +1 ion
63
The ionization energy of Hydrogen is . . . than the Alkali metals
higher
64
When Hydrogen is part of an ionic compound with a metal, Hydrogen becomes a . . .
H(-)
65
Ionic compounds with H(-) are called . . .
Metal hydrides
66
Under extreme pressure, Hydrogen can . . .
act like a metal, conduct electricity, and conduct heat
67
One or more forms of a chemical element that occur in the same physical state are known as . . .
Allotropes
68
Allotropes form because of the . . .
different ways atoms may be bonded together
69
Allotropes may display . . . chemical and physical properties
very different
70
In response to changes in pressure, temperature, and exposure to light, elements may change ________
Allotrpoes
71
What elements are all nonmetals and have highly negative electron affinities?
F, Cl, Br, and I
72
What element removes electrons from almost any substance it contacts (very exothermic), including water, and is very reactive?
Fluorine
73
The halogens react directly with most metals to form . . .
Ionic halides
74
The halogens also react with diatomic H to form gaseous
Hydrogen halide compounds
75
The Noble Gases are . . .
gaseous, monatomic nonmetals
76
Noble gases are very unreactive because they have full . . .
s and p subshells
77
The only noble gases to form chemical compounds are . . .
the heaviest because of the lower ionization energies
78
Metals tend to ____ electrons
lose
79
Metals tend to lose electrons because of . . .
low ionization energies
80
Nonmetals tend to ____ electrons
gain
81
Nonmetals tend to lose electrons because of . . .
high electron affinities
82
Compounds formed between metals and nonmetals tend to be _____
ionic
83
An element's reactivity is characterized by its . . .
metallic character
84
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
decreases
85
Because Ionization energy decreases down a group, making it easier for an atom to lose an electron, Metallic Character _________ from top to bottom
increases
86
Group 1A is
Alkali Metals
87
Group 2A is
Alkaline Earth Metals
88
Group 8A is
Noble Gases
89
Group 7A is
The Halogens
90
Group 6A is
The Chalcogens
91
Group 1A elements include . . .
Li, Na, K, Rb, Cs, and Fr
92
Group 2A elements include . . .
Be, Mg, Ca, Sr, Ba, and Ra
93
Group 8A elements include . . .
He, Ne, Ar, Kr, Xe, and Rn
94
Group 7A elements include . . .
F, Cl, Br, I, and At
95
Group 6A elements include . . .
O, S, Se, Te, and Po

Chemistry (17 decks)

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