Electronegativity and Ionization Energy Quiz

Match the following descriptions with their corresponding terms.

• Electron shielding

• The ability of an atom to accept an electron

• Electron affinity

• The shielding of valence electrons by inner electrons

• Ionization energy

• The amount of energy needed to remove an electron

• Electronegativity

• The measure of attraction an atom has for bonding electrons

How does electronegativity change across a period?

• Decreases from left to right

• Increases from left to right

• Remains constant

• Decreases and then increases

Answer explanation

Electronegativity increases from left to right across a period due to increasing nuclear charge, which attracts electrons more strongly. This trend reflects the greater ability of atoms to attract bonding electrons as you move across the periodic table.

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What happens to electronegativity as you move down a group?

• It increases

• It decreases

• It remains constant

• It fluctuates

Answer explanation

As you move down a group in the periodic table, the electronegativity decreases due to the increasing distance between the nucleus and the valence electrons, which reduces the nucleus's ability to attract bonding electrons.

What is ionization energy?

• The ability of an atom to accept an electron

• The measure of attraction an atom has for bonding electrons

• The amount of energy needed to remove an electron

• The shielding of valence electrons by inner electrons

Answer explanation

Ionization energy is defined as the amount of energy needed to remove an electron from an atom. This makes the correct choice the one that accurately describes this concept.

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Why do noble gases have very high first ionization energy?

• They have incomplete valence shells

• They have full valence shells

• They have low electronegativity

• They have high electron affinity

Answer explanation

Noble gases have full valence shells, making them stable and less likely to lose electrons. This stability results in very high first ionization energy, as removing an electron requires significant energy.

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What is electron affinity?

• The ability of an atom to accept an electron

• The measure of attraction an atom has for bonding electrons

• The amount of energy needed to remove an electron

• The shielding of valence electrons by inner electrons

Answer explanation

Electron affinity refers to the ability of an atom to accept an electron, which indicates how much an atom wants to gain an electron to form a negative ion. This makes the first answer choice the correct one.

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What is the trend in first ionization energy down a group?

• Increases

• Decreases

• Remains constant

• Fluctuates

Answer explanation

The trend in first ionization energy decreases down a group due to increased atomic size and shielding effect, making it easier to remove the outermost electron.

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(a)   do not follow electronegativity trends due to their complexity.

• Transition metals

• Lanthanides and actinides

• Noble gases

• Halogens

Answer explanation

Lanthanides and actinides do not follow electronegativity trends due to their complex electron configurations and f-orbital involvement, which leads to irregularities in their chemical behavior compared to other groups.

What is the trend in electron affinity down a group?

• It increases

• It decreases

• It remains constant

• It fluctuates randomly

Answer explanation

The trend in first electron affinity decreases down a group due to increased atomic size and shielding effect, making it less favorable for an atom to gain an electron. Thus, the correct answer is that it decreases.

Metallic character (a)   down a group.

• It increases

• It decreases

• It remains constant

• It fluctuates randomly

Answer explanation

Metallic character increases down a group due to the addition of electron shells, which enhances the ability of atoms to lose electrons, making them more metallic in nature.

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