Question

instructions: for each of the following pairs, determine which atoms will form a positive ion more easily. 14.___ mg, sr 15._ k, ca 16._ li, b 17.___ rb, sn

Explanation:

• For 14. Mg vs Sr:
• As we move down a group in the periodic table, the atomic radius increases.
• Larger atoms have less attraction for their valence electrons.
• Strontium (Sr) is below Magnesium (Mg) in Group 2. So, Sr will lose electrons more easily to form a positive ion.
• For 15. K vs Ca:
• Potassium (K) is in Group 1 and Calcium (Ca) is in Group 2.
• Group 1 elements have a lower ionization energy (energy required to remove an electron) than Group 2 elements in the same period.
• K has one valence electron and Ca has two. K will lose its single valence electron more easily to form a positive ion.
• For 16. Li vs B:
• Lithium (Li) is in Group 1 and Boron (B) is in Group 13.
• Group 1 elements have a much lower ionization energy than Group 13 elements.
• Li will lose its valence electron more easily to form a positive ion.
• For 17. Rb vs Sn:
• Rubidium (Rb) is in Group 1 and Tin (Sn) is in Group 14.
• Group 1 elements have a very low ionization energy compared to Group 14 elements.
• Rb will lose its valence electron more easily to form a positive ion.

Answer:

1. Sr
2. K
3. Li
4. Rb