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CHEM-1315 > Unit 4.1: Identify trends in effective nuclear charge, atomic size, ionic size, ionization energy, and relate trends to properties displayed in the periodic table > Flashcards

Unit 4.1: Identify trends in effective nuclear charge, atomic size, ionic size, ionization energy, and relate trends to properties displayed in the periodic table Flashcards

Identify trends in effective nuclear charge, atomic size, ionic size, ionization energy, and relate trends to properties displayed in the periodic table. [Readings 3.9, 3.10]

1
Q

Reading 3.9: Atomic and Ionic Sizes

What two things determine the sizes of ions and atoms?

A
  1. Electronic configuration
  2. Interactions between the nucelus and the electrons
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2
Q

Reading 3.9: Atomic and Ionic Sizes

Principles pertaining to the forces of attraction or repulsion in charged species

A

Electrostatic Principles

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3
Q

Reading 3.9: Atomic and Ionic Sizes

What is the first electrostatic principle?

A
  1. Oppositely charged particles attract each other
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4
Q

Reading 3.9: Atomic and Ionic Sizes

What is the second electrostatic principle?

A
  1. Like-charged particles repel each other
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5
Q

Reading 3.9: Atomic and Ionic Sizes

What is the third electrostatic principle?

A
  1. As charges increase, so does the attraction or repulsion
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6
Q

Reading 3.9: Atomic and Ionic Sizes

What is the fourth electrostatic principle?

A
  1. As two charged bodies get closer together, the force of attraction or repulsion gets stronger.
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7
Q

Reading 3.9: Atomic and Ionic Sizes

In an atom or ion with multiple electrons there are both _ between the negatively charged electrons and _ forces between the electrons and the positively charged protons in the nucleus.

A
  1. Repulsions
  2. Attractive
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8
Q

Reading 3.9: Atomic and Ionic Sizes

The net positive charge from the nucleus that a valence electron experiences.

A

Effective nuclear charge (Zeff)

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9
Q

Reading 3.9: Atomic and Ionic Sizes

The effective nuclear charge is (higher/lower) than the actual nuclear charge, Z.

A

Lower

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10
Q

Reading 3.9: Atomic and Ionic Sizes

Effective nuclear charge equation

A

Zeff=Z-S

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11
Q

Reading 3.9: Atomic and Ionic Sizes

A set of rules that provides a numerical value for the shielding constant S when calculating effective nuclear charge

A

Slater’s Rules

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12
Q

Reading 3.9: Atomic and Ionic Sizes

Is the particular electron included in the calculation of the shielding constant?

A

No

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13
Q
A
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14
Q

Reading 3.9: Atomic and Ionic Sizes

What does S represent?

A

Shielding constant

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15
Q

Reading 3.9: Atomic and Ionic Sizes

How do you calculate the shielding constant?

A
  1. For a given valence electron, electrons in the same principal quantum number orbital each contribute a value of 0.35 toward the value
  2. Electrons in shells with lower n values each contribute a value of 0.85
  3. Add the two together
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16
Q

Reading 3.9: Atomic and Ionic Sizes

For a given valence electron, electrons in the same principal quantum number orbital each contribute a value of _ toward the shielding constant.

A

0.35

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17
Q

Reading 3.9: Atomic and Ionic Sizes

Electrons in shells with lower n values each contribute a value of _ towards the shielding constant.

A

0.85

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18
Q

Reading 3.9: Atomic and Ionic Sizes

Effective nuclear charge _ across a period of the periodic table

A

Increases

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19
Q

Reading 3.9: Atomic and Ionic Sizes

Effective nuclear charge _ down a group of the periodic table

A

Decreases

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20
Q

Reading 3.9: Atomic and Ionic Sizes

Calculate the effective nuclear charge experienced by the valence electrons of sodium

A

+2.5

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21
Q

Reading 3.9: Atomic and Ionic Sizes

Calculate the effective nuclear charge experienced by the valence electrons of Magnesium

A

+3.15

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22
Q

Reading 3.9: Atomic and Ionic Sizes

Calculat the effective nuclear charges experienced by the valence electrons of
1. K
2. Ca

A
  1. +3.7
  2. +4.35
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23
Q

Reading 3.9: Atomic and Ionic Sizes

Calculate the effective nuclear charges experienced by the valence electrons of
1. Be
2. B+

A
  1. +1.95
  2. +2.95
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24
Q

Reading 3.9: Atomic and Ionic Sizes

Atomic radius generally _ moving from left to right across a period on the periodic table

A

Decreases

25
Q

Reading 3.9: Atomic and Ionic Sizes

Atomic radius generally _ moving down a group of the periodic table

A

Increases

26
Q

Reading 3.9: Atomic and Ionic Sizes

Compare the relative sizes of oxygen and sulfur

A

A sulfur atom is larger than an oxygen atom.

Both are in group 16, but sulfur is farther down the group than oxygen is.

27
Q

Reading 3.9: Atomic and Ionic Sizes

Determine whether an atom of aluminum or an atom of argon would have a larger radius.

A

An aluminum atom should have a larger radius than an argon atom.

An aluminum atom should have a larger radius than an argon atom.The effective nuclear charge experienced by an element’s valence electrons increases from left to right across a period. This increase in effective nuclear charge results in a decrease in atomic radius. As a result, an

28
Q

Reading 3.9: Atomic and Ionic Sizes

All cations have (smaller/larger) radii than their corresponding neutral atoms.

A

Smaller

29
Q

Reading 3.9: Atomic and Ionic Sizes

All anions have (smaller/larger) radii than their corresponding neutral atoms.

A

Larger

30
Q

Reading 3.9: Atomic and Ionic Sizes

Compare the relative sizes of Cl and Cl-

A

Cl- is significantly larger than Cl

Cl- is significantly larger than Cl because it has an extra electron but the same nuclear charge of +17. The net negative charge of Cl- allows for greater electron-electron repulsions and results in an increase in size.

31
Q

Reading 3.9: Atomic and Ionic Sizes

Compare the relative sizes of Co, Co2+, and Co3+

A

Co > Co2+ > Co3+

In each case, the nucleus has 27 protons and, therefore, a charge of +27. Co has 27 electrons, Co2+ has 25 electrons, and Co3+ has 24 electrons.

32
Q

Reading 3.9: Atomic and Ionic Sizes

Compare the sizes of Cl-, K+, and Ca2+

A

Ca2+ < K+ < Cl-

The three species each have 18 electrons and are isoelectronic. The Ca2+ nucleus has 20 protons and a nuclear charge of +20, however, resulting in a stronger attractive force on the electrons than in K+ 919 protons) and Cl- (17 protons). Therefore, Ca2+ is the smallest of the three species. Additionally, Ca2+ and K+ are both in the fourth row of the periodic table, but Ca is to the right of K, so Ca2+ should be smaller than K+
Cl- is the largest of the three species because it has more electrons than protons, and the resulting electron-electron repulsions allow the valence electrons to occupy a position farther from the nucleus.

33
Q

Reading 3.9: Atomic and Ionic Sizes

Compare the sizes of O2-, F-, and Na+

A

Na+ < F- < O2-

34
Q

Reading 3.10: Ionization Energy and Electron Affinity

The energy required to remove an electron from a gaseous atom to produce a gaseous cation is called _

A

Ionization Energy

35
Q

Reading 3.10: Ionization Energy and Electron Affinity

As effective nuclear charge decreases, and atom gets larger, so (more/less) energy is needed to remove an electron.

A

Less

36
Q

Reading 3.10: Ionization Energy and Electron Affinity

The ionization energy of the elements tends to _ across a row of the periodic table.

A

Increase

37
Q

Reading 3.10: Ionization Energy and Electron Affinity

The ionization energy of the elemends tends to _ down a group on the periodic table.

A

Decrease

38
Q

Reading 3.10: Ionization Energy and Electron Affinity

Ionization energy generally _ as effective nuclear charge increases and as atomic radius decreases.

A

Increases

39
Q

Reading 3.10: Ionization Energy and Electron Affinity

Which group of elements requires the least amount of energy to remove an electron?

A

The alkali metals, group 1

40
Q

Reading 3.10: Ionization Energy and Electron Affinity

Which group of elements are most difficult to remove an electron from?

A

The noble gases

41
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. K
2. Ga
3. Se

A

Se

42
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. O
2. S
3. Se

A

O

43
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. In
2. As
3. Cl

A

Cl

44
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. Be
2. C
3. N

A

N

45
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. Sn
2. Se
3. F

A

F

46
Q

Reading 3.10: Ionization Energy and Electron Affinity

Identify the element with the highest first ionization energy:
1. Mg
2. Ca
3. Sr

A

Mg

47
Q

Reading 3.10: Ionization Energy and Electron Affinity

What are the two exceptions to the ionization energy trend?

A
  1. Each time a new subshell begins, the ionization energy lowers
  2. Half-filled subshells are particuarly stable
48
Q

Reading 3.10: Ionization Energy and Electron Affinity

The energy requried to remove an electron from the +1 gaseous ion

A

Second ionization energy

49
Q

Reading 3.10: Ionization Energy and Electron Affinity

The energy required to remove an electron from the +2 gaseous ion.

A

Third ionization energy

50
Q

For every element, the second ionization energy is (higher/lower) than the first.

A

Higher

It is more difficult to remove a negatively charged electron from a positively charged species than from the corresponding neutral atom.

51
Q

Reading 3.10: Ionization Energy and Electron Affinity

Ionization energy (increases/decreases) dramatically when a noble gas configuration of electrons will be disrupted.

A

Increases

52
Q

Reading 3.10: Ionization Energy and Electron Affinity

Does the largest increase in ionization energy for potassium occur between removing the first and second electrons or the second and third electrons?

A

The second ionization energy is much greater than the first.

K+ (electron configuration = [Ar]) has a filled valence shell that is disrupted furing its ionization to K2+.
The actual values for the first three ionization energies are 418, 3050, and 440 kJ/mol, respectively. So the largest increase in IE for K occurs between removing the first and second electrons.

53
Q

Reading 3.10: Ionization Energy and Electron Affinity

Which of the first three ionizations of calcium has the greatest increase in ionization energy?

A

The third ionization of calcium is much greater than the first two.

54
Q

Reading 3.10: Ionization Energy and Electron Affinity

The energy liberated when an electron is added to a gaseous atom to form a gaseous anion.

A

Electron affinity, EA

55
Q

Reading 3.10: Ionization Energy and Electron Affinity

Negative electron affinities represent an (subtraction/addition) in energy.

A

decrease

56
Q

Reading 3.10: Ionization Energy and Electron Affinity

Positive electron affinities reflect an (subtraction/addition) in energy to the gaseous atoms.

A

Addition

57
Q

Reading 3.10: Ionization Energy and Electron Affinity

Main group elements that have common anions often have (positive/negative) afinities.

A

Negative

58
Q

Reading 3.10: Ionization Energy and Electron Affinity

Noble gases and some other elements have (positive/negative) affinities.

A

Positive

59
Q

Reading 3.10: Ionization Energy and Electron Affinity

Which group of elements have the most negative electron affinities of all the elements?

A

Halogens

CHEM-1315 (27 decks)

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