ionization energy Flashcards
(117 cards)
1
Q
What is ionization energy?
A
The energy required to remove an electron from an atom or ion in the gaseous state.
2
Q
True or False: Ionization energy increases across a period in the periodic table.
A
True
3
Q
What trend in ionization energy is observed down a group in the periodic table?
A
Ionization energy decreases down a group.
4
Q
Fill in the blank: The first ionization energy is the energy required to remove ______ electron(s).
A
one
5
Q
Which element has the highest first ionization energy: Helium, Lithium, or Sodium?
A
Helium
6
Q
What factor primarily affects ionization energy?
A
Nuclear charge and electron shielding.
7
Q
True or False: Noble gases have high ionization energies.
A
True
8
Q
What is the general trend of ionization energy in relation to atomic radius?
A
Ionization energy increases as atomic radius decreases.
9
Q
What is meant by ‘successive ionization energies’?
A
The energies required to remove additional electrons from an atom after the first has been removed.
10
Q
Multiple Choice: Which element would have a lower second ionization energy: Magnesium, Sodium, or Aluminum?
A
Sodium
11
Q
What does a large jump in successive ionization energies indicate?
A
That an electron is being removed from a new, inner shell.
12
Q
Fill in the blank: The second ionization energy is always ______ than the first.
A
greater
13
Q
True or False: Ionization energy is always a positive value.
A
True
14
Q
What is the unit of ionization energy?
A
Kilojoules per mole (kJ/mol)
15
Q
Multiple Choice: Which of the following has the lowest first ionization energy: Beryllium, Boron, or Carbon?
A
Boron
16
Q
What role does electron shielding play in ionization energy?
A
It reduces the effective nuclear charge felt by the outermost electrons.
17
Q
What is the relationship between ionization energy and reactivity in metals?
A
Lower ionization energy generally means higher reactivity.
18
Q
True or False: Transition metals generally have higher ionization energies than alkali metals.
A
True
19
Q
What happens to ionization energy as you move from left to right across a period?
A
It increases.
20
Q
Fill in the blank: Ionization energy is a measure of how strongly an atom ______ its electrons.
A
holds
21
Q
Which group of elements typically has the lowest ionization energies?
A
Alkali metals.
22
Q
Multiple Choice: Which element would likely have a higher ionization energy: Chlorine, Fluorine, or Bromine?
A
Fluorine
23
Q
What effect do nonmetals generally have on ionization energy compared to metals?
A
Nonmetals tend to have higher ionization energies than metals.
24
Q
True or False: Ionization energy can be affected by the presence of other electrons in an atom.
A
True
25
What is the general trend of ionization energy in relation to electron affinity?
Higher ionization energy usually correlates with higher electron affinity.
26
What determines the position of an element in the periodic table in relation to its ionization energy?
The number of protons and the distance of the valence electrons from the nucleus.
27
Fill in the blank: The first ionization energy of an element is generally ______ than the second.
lower
28
Which has a higher first ionization energy: Oxygen or Nitrogen?
Oxygen
29
True or False: Ionization energy is directly proportional to the number of protons in the nucleus.
True
30
What is the effect of increasing nuclear charge on ionization energy?
It increases ionization energy.
31
Multiple Choice: Which of the following elements would you expect to have the highest ionization energy: Lithium, Sodium, or Potassium?
Lithium
32
What is the significance of measuring ionization energy?
It helps to understand the reactivity and chemical properties of an element.
33
Fill in the blank: The removal of an electron from an atom is called ______.
ionization
34
True or False: The first ionization energy for helium is higher than that for hydrogen.
True
35
What are the two main factors that affect the ionization energy of an element?
Nuclear charge and electron shielding.
36
What is the general trend of ionization energy in period 2 elements?
It increases from left to right across the period.
37
Multiple Choice: Which element has a lower first ionization energy: Calcium, Strontium, or Barium?
Barium
38
What is the relationship between ionization energy and the ability to form cations?
Lower ionization energy makes it easier to form cations.
39
Fill in the blank: The energy required to remove an electron from a gaseous atom is called ______ energy.
ionization
40
True or False: All elements have the same first ionization energy.
False
41
Which group of elements has the highest first ionization energies?
Noble gases.
42
What is the effect of atomic size on ionization energy?
Larger atomic size generally results in lower ionization energy.
43
Multiple Choice: Which element would have a lower ionization energy: Aluminum, Silicon, or Phosphorus?
Aluminum
44
What does a high ionization energy suggest about an element's reactivity?
It suggests the element is less reactive.
45
Fill in the blank: The process of an atom losing an electron is known as ______.
ionization
46
True or False: Ionization energy is affected by the electron configuration of an atom.
True
47
What happens to ionization energy as you go from group 1 to group 18?
Ionization energy increases.
48
Multiple Choice: Which element has a higher second ionization energy: Magnesium or Calcium?
Magnesium
49
How does the presence of inner shell electrons affect ionization energy?
They cause shielding, reducing ionization energy.
50
Fill in the blank: The energy needed to remove an electron from the outermost shell is called the ______ ionization energy.
first
51
True or False: Elements with full outer shells have high ionization energies.
True
52
What is the relationship between ionization energy and electronegativity?
Higher ionization energy usually correlates with higher electronegativity.
53
Multiple Choice: Which of the following has the highest ionization energy: Iron, Copper, or Zinc?
Copper
54
What is the role of ionization energy in determining an element's position in the periodic table?
It helps predict the element's reactivity and bond formation.
55
Fill in the blank: A large increase in ionization energy indicates that the electron is being removed from a ______ shell.
core
56
True or False: Ionization energy can be used to predict the types of ions an element will form.
True
57
What is the relationship between ionization energy and the formation of anions?
Higher ionization energy makes it less likely to form anions.
58
Multiple Choice: Which element has a lower first ionization energy: Fluorine, Chlorine, or Bromine?
Bromine
59
What is the significance of the first ionization energy for alkali metals?
It indicates their high reactivity and tendency to lose one electron.
60
Fill in the blank: The second ionization energy is usually ______ than the first.
higher
61
True or False: Ionization energy is a key concept in understanding chemical bonding.
True
62
What happens to ionization energy as you move from top to bottom in a group?
It decreases.
63
Multiple Choice: Which element has a higher first ionization energy: Barium, Strontium, or Calcium?
Calcium
64
What is the effect of increased atomic number on ionization energy?
It generally increases ionization energy due to greater nuclear charge.
65
Fill in the blank: Ionization energy is essential for understanding ______ behavior in elements.
reactive
66
True or False: The first ionization energy is always less than the second ionization energy.
True
67
Which element is expected to have the highest second ionization energy: Sodium or Magnesium?
Magnesium
68
What is the effect of electron-electron repulsion on ionization energy?
It can decrease ionization energy by making it easier to remove an electron.
69
Multiple Choice: Which element would likely have a lower ionization energy: Neon, Argon, or Krypton?
Krypton
70
Fill in the blank: The trend of ionization energy can be explained using ______ theory.
atomic
71
True or False: Ionization energy is unrelated to an element's position in the periodic table.
False
72
What does a low ionization energy indicate about an element's ability to lose electrons?
It indicates that the element can easily lose electrons.
73
Multiple Choice: Which of these has the highest first ionization energy: Lithium, Sodium, or Potassium?
Lithium
74
What is the relationship between ionization energy and the ability to form covalent bonds?
Higher ionization energy can facilitate the formation of covalent bonds.
75
Fill in the blank: The ionization energy of an atom is influenced by its ______ configuration.
electron
76
True or False: Atoms with full outer electron shells have low ionization energies.
False
77
Which group in the periodic table has the highest ionization energies?
Noble gases.
78
What is the effect of increased distance between the nucleus and the outermost electron on ionization energy?
It decreases ionization energy.
79
Multiple Choice: Which of the following has the lowest ionization energy: Magnesium, Barium, or Calcium?
Barium
80
Define the term First Ionisation Energy (IE)
The first ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms, forming one mole of gaseous unipositive ions.
## Footnote
Atoms must be in the gaseous state. Measured in kJ mol⁻¹.
81
What is the equation for the first ionisation energy?
X(g) → X⁺(g) + e⁻
82
What is the equation for the second ionisation energy?
X⁺(g) → X²⁺(g) + e⁻
83
What is the equation for the third ionisation energy?
X²⁺(g) → X³⁺(g) + e⁻
84
What trend is observed in ionisation energy across a period?
IE increases
85
What causes the increase in ionisation energy across a period?
↑ Nuclear charge, ↓ Atomic radius, Same shielding, Stronger attraction between nucleus and outer electron
86
What trend is observed in ionisation energy down a group?
IE decreases
87
What factors contribute to the decrease in ionisation energy down a group?
↑ Atomic radius, ↑ Electron shielding, Weaker nuclear attraction on outer electron
88
What is the pattern of successive ionisation energies of an element?
Ionisation energies increase with each successive electron removed. Big jumps occur when electrons are removed from a new inner shell.
89
What is the reason for the existence of ionisation energies?
Ionisation energy is due to the electrostatic attraction between the positive nucleus and the negative outer electron.
90
What effect does nuclear charge have on ionisation energy?
↑ Protons = ↑ attraction = ↑ IE
91
What effect does atomic/ionic radius have on ionisation energy?
↑ Radius = ↓ attraction = ↓ IE
92
How does electron shielding influence ionisation energy?
More inner shells = ↑ shielding = ↓ IE
93
What is the effect of subshell structure on ionisation energy?
Half-filled or full subshells are more stable.
94
What is the impact of electron repulsion on ionisation energy?
2 electrons in the same orbital repel, making it easier to remove an electron, leading to ↓ IE
95
How can you deduce electron configuration from ionisation energies?
Look at successive ionisation energy values and identify large jumps.
96
What does a large jump in ionisation energy indicate?
It indicates the beginning of an inner shell.
97
What is the method to deduce periodic table position from successive ionisation energy data?
Count electrons before the big jump to determine Group number and total number of electrons for Atomic number.
98
What are the factors that increase ionisation energy?
* ↑ Nuclear charge
* Full/half subshell
99
What are the factors that decrease ionisation energy?
* ↑ Shielding
* ↑ Atomic radius
* Paired electrons
100
Define the term First Ionisation Energy (IE)
The first ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms, forming one mole of gaseous unipositive ions.
## Footnote
Atoms must be in the gaseous state. Produces 1+ ions. Measured in kJ mol⁻¹.
101
What is the equation for the first ionisation energy?
X(g) → X+(g) + e−
## Footnote
Always remove 1 electron at a time. Keep the state symbol as (g).
102
What is the equation for the second ionisation energy?
X+(g) → X2+(g) + e−
103
What is the equation for the third ionisation energy?
X2+(g) → X3+(g) + e−
104
What is the trend in ionisation energy across a period?
IE increases
## Footnote
Due to ↑ nuclear charge, ↓ atomic radius, same shielding, and stronger attraction between nucleus and outer electron.
105
What is the trend in ionisation energy down a group?
IE decreases
## Footnote
Due to ↑ atomic radius, ↑ electron shielding, and weaker nuclear attraction on outer electron.
106
What happens to ionisation energies with successive removals of electrons?
Ionisation energies increase with each successive electron removed.
## Footnote
Big jumps in values occur when electrons are removed from a new (inner) shell, closer to the nucleus and less shielded.
107
What is the reason for ionisation energy?
Ionisation energy is due to the electrostatic attraction between the positive nucleus and the negative outer electron.
108
What factors influence ionisation energies?
Factors include:
* Nuclear charge (protons)
* Atomic/ionic radius
* Electron shielding
* Subshell structure
* Electron repulsion (spin-pair repulsion)
109
Fill in the blank: The stronger the attraction between the nucleus and the outer electron, the _______ energy is needed to remove the electron.
more
110
How can you deduce electron configuration from ionisation energies?
Look at successive ionisation energy values and identify large jumps, which indicate the beginning of an inner shell.
111
What does a large jump in ionisation energy indicate?
It indicates that the inner shell begins and helps identify the number of valence electrons.
112
How can you deduce the periodic table position from successive ionisation energy data?
Count electrons before the big jump to determine the group number and the total number of electrons to find the atomic number.
113
What is the effect of increased nuclear charge on ionisation energy?
Increases ionisation energy.
114
What is the effect of increased shielding on ionisation energy?
Decreases ionisation energy.
115
What is the effect of increased atomic radius on ionisation energy?
Decreases ionisation energy.
116
What effect do full or half-filled subshells have on ionisation energy?
Increase ionisation energy.
117
True or False: Paired electrons in the same orbital increase ionisation energy.
False
## Footnote
Paired electrons experience spin repulsion, making it easier to remove them, thus decreasing ionisation energy.
