Questions and Answers
What trend is observed in ionization energy as you move down group 1 from Na to Rb?
Why does the first ionization energy of Na exceed that of Rb?
What effect does increased shielding have on ionization energy as you go down the group?
How does the atomic size change as you move from Na to Rb?
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What is the primary reason for the decrease in ionization energy down the group?
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Study Notes
Ionization Energy in Group 1
- Ionization energy decreases as one moves down the alkali metals group (Group 1) due to increasing atomic radius.
- Increase in atomic size leads to a weaker attraction between the nucleus and valence electrons.
- The shielding effect also plays a significant role, as more inner electron shells reduce nuclear charge experienced by valence electrons.
Comparison Between Sodium (Na) and Rubidium (Rb)
- Sodium (Na) has a smaller atomic radius compared to Rubidium (Rb).
- As a result of the smaller size, Na exhibits a larger first ionization energy than Rb.
- This trend reflects the general behavior of ionization energy within the group, confirming that lighter elements require more energy to remove their outermost electrons.
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Description
This quiz explores the ionization energy of group 1 elements, specifically comparing sodium (Na) and rubidium (Rb). It explains the trends in ionization energy as atomic size increases down the group, highlighting the effects of atomic radius and the shielding effect. Test your understanding of these fundamental concepts in chemistry.
