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Questions and Answers
Which of the following statements best describes the effect of increasing the number of electrons on the nucleus charge in a negative ion?
Which of the following statements best describes the effect of increasing the number of electrons on the nucleus charge in a negative ion?
- The effect of the nucleus charge on the electrons' attraction decreases, resulting in a decrease in the energy level radius.
- The repulsion force between the electrons decreases, leading to a decrease in the energy level radius.
- The effect of the nucleus charge on the electrons' attraction increases, resulting in an increase in the energy level radius.
- The repulsion force between the electrons increases, leading to an increase in the energy level radius. (correct)
What trend is observed for ionization energy (IE) as we move down a group in the periodic table?
What trend is observed for ionization energy (IE) as we move down a group in the periodic table?
- Ionization energy fluctuates
- Ionization energy decreases (correct)
- Ionization energy increases
- Ionization energy remains constant
What is the relationship between effective nuclear charge and the pulling of electrons closer to the nucleus?
What is the relationship between effective nuclear charge and the pulling of electrons closer to the nucleus?
- A larger effective nuclear charge pulls electrons closer to the nucleus (correct)
- A larger effective nuclear charge pushes electrons away from the nucleus
- A larger effective nuclear charge has an unpredictable effect on electron position
- Effective nuclear charge has no effect on electron position
What effect does increasing the number of electrons have on the nucleus charge in a negative ion?
What effect does increasing the number of electrons have on the nucleus charge in a negative ion?
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What happens to the ionization energy as we move from up to down in a group?
What happens to the ionization energy as we move from up to down in a group?
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