Ionization Energy & Periodic Trends

Why does ionization energy increase across a period in the periodic table?

• The atomic radius and nuclear charge both increase.

• The atomic radius decreases and nuclear charge increases.

• The atomic radius increases and nuclear charge decreases.

• The atomic radius and nuclear charge both decrease.

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What happens to the atomic radius as you move from left to right across a period?

• It increases due to decreased nuclear charge.

• It decreases due to increased nuclear charge.

• It remains constant due to equal protons and electrons.

• It increases due to more electron shells.

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What is the effect of increasing nuclear charge on valence electrons?

• Valence electrons are repelled.

• Valence electrons are unaffected.

• Valence electrons are held more tightly.

• Valence electrons are held more loosely.

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Which factor is relatively constant across a period, affecting ionization energy?

• Valence electron count

• Shielding effect

• Atomic radius

• Nuclear charge

What is the relationship between electron proximity to the nucleus and ionization energy?

• Closer electrons are easier to remove.

• Closer electrons require less energy to remove.

• Proximity has no effect on ionization energy.

• Closer electrons require more energy to remove.

How does the atomic radius change as you move down a group in the periodic table?

• It decreases due to increased nuclear charge.

• It increases due to additional electron shells.

• It remains constant due to equal protons and electrons.

• It decreases due to more electron shells.

What is the effect of electron shielding with atomic size?

• Electron shielding decreases atomic size.

• Electron shielding increases with atomic size.

• Electron shielding makes atomic size constant.

• Electron shielding has no effect on atomic size.

Why does electronegativity generally increase across a period?

• Due to decreasing atomic radius and increasing nuclear charge.

• Due to increasing atomic radius and decreasing nuclear charge.

• Due to constant atomic radius and nuclear charge.

• Due to increasing atomic radius and nuclear charge.

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What is the trend in electronegativity as you move down a group in the periodic table?

• Electronegativity increases due to decreased atomic radius.

• Electronegativity increases due to increased nuclear charge.

• Electronegativity decreases due to increased atomic radius and electron shielding.

• Electronegativity remains constant due to balanced forces.

How does the ionization energy change as you move down a group in the periodic table?

• Ionization energy remains constant due to equal protons and electrons.

• Ionization energy decreases due to increased atomic radius and electron shielding.

• Ionization energy increases due to decreased atomic radius.

• Ionization energy increases due to increased nuclear charge.