Ionization Energy and Atomic Structure Quiz

How does ionization energy change across a period and down a group on the periodic table?

• Increases across a period, decreases down a group

• Decreases across a period, increases down a group

• Remains constant across a period, increases down a group

• Increases across a period, remains constant down a group

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What is the relationship between atomic number and ionization energy as shown in the graph?

• Ionization energy decreases as atomic number increases

• Ionization energy increases as atomic number increases

• Ionization energy remains constant as atomic number increases

• Ionization energy fluctuates randomly as atomic number increases

Explain how the graph supports the claim that ionization energy is influenced by atomic structure.

• The graph shows a random pattern unrelated to atomic structure

• The graph shows a consistent increase in ionization energy with atomic number

• The graph shows a decrease in ionization energy with atomic number

• The graph shows no clear pattern related to atomic structure

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What is the trend in ionization energy as you move from left to right across a period on the periodic table?

• Ionization energy decreases

• Ionization energy remains constant

• Ionization energy increases

• Ionization energy fluctuates randomly

Which of the following describes the effect on ionization energy when moving down a group?

• The ionization energy increases

• The ionization energy decreases

• The valence electrons are in energy levels farther from the nucleus

• The shielding effect is less

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Why do noble gases have high ionization energies, and what does this suggest about their chemical stability?

• They have low electron affinity, indicating instability

• They have a full valence shell, indicating high stability

• They have a high electron affinity, indicating instability

• They have an incomplete valence shell, indicating high stability

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What is the relationship between atomic size and electronegativity as described in the text?

• Larger atomic radius leads to higher electronegativity.

• Smaller atomic radius leads to higher electronegativity.

• Larger atomic radius leads to lower electronegativity.

• Atomic size does not affect electronegativity.

According to the text, how does the position of sulfur and phosphorus on the periodic table relate to their electronegativity?

• Sulfur is to the left of phosphorus and has higher electronegativity.

• Sulfur is to the right of phosphorus and has higher electronegativity.

• Sulfur is above phosphorus and has lower electronegativity.

• Sulfur is below phosphorus and has higher electronegativity.

What does the text suggest about the relationship between shared electrons and electronegativity?

• Shared electrons are more attracted to atoms with lower electronegativity.

• Shared electrons are more attracted to atoms with higher electronegativity.

• Shared electrons are equally attracted to all atoms.

• Shared electrons are not affected by electronegativity.

How is electronegativity calculated?

• By measuring the atomic mass directly

• By using the average energy required to remove an electron and the energy given off when an electron is added

• By counting the number of protons in an atom

• By measuring the volume of the atom

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