Question

1. in general, the atomic radius (increases, decreases) from top to bottom in a group. in general, the atomic radius (increases, decreases) form left to right across a period. in general, the ionization energy (increases, decreases) from top to bottom in a group. in general, the ionization energy (increases, decreases) form left to right across a period. 8. compare the bohr models for a and b only. which would have the highest ionization energy? a. a because it is easier to remove a valence electron from a. b. b because it is easier to remove a valence electron from b. c. a because it is harder to remove a valence electron from a. d. b because it is harder to remove a valence electron from b. 9. which would have the highest electronegativity? a. b because it is a metal and wants to lose electrons. b. c because it is a metal and wants to lose electrons. c. b because it is a nonmetal and wants to gain electrons. d. c because it is a nonmetal and wants to gain electrons. 10. put the letter in the blank above that matches the lewis dot diagram: a) halogen b) alkali metal c) noble gas d) carbon e) nitrogen 11. refer to the bohr models above: element c is in period____. element b is in period__. element b has (lower, higher) shielding effect compared to element c. element a is in group__. element b is in group__. element c is in group__. 12. what is the oxidation number (charge) for each of the following? __rb __br __n __al __mg ____s 13. put these elements in order of smallest to largest: sulfur, tellurium, oxygen 14. which element has the largest ionization energy? mg or si 15. which element has the smallest electronegativity? c or sn

Explanation:

Step1: Recall periodic - trend rules

Atomic radius increases from top to bottom in a group and decreases from left to right across a period. Ionization energy decreases from top to bottom in a group and increases from left to right across a period.

Step2: Analyze Bohr - model for ionization energy (Question 8)

The more electron shells an atom has, the easier it is to remove a valence electron (lower ionization energy). B has fewer electron shells than A, so it is harder to remove a valence electron from B, and B has higher ionization energy.

Step3: Analyze electronegativity (Question 9)

Non - metals want to gain electrons and have higher electronegativity. Assuming B is a non - metal and C is a metal (from the context), B has higher electronegativity as non - metals have a greater tendency to attract electrons.

Step4: Match Lewis dot diagrams (Question 10)

A halogen has 7 valence electrons, an alkali metal has 1, a noble gas has 8 (except He with 2), carbon has 4, and nitrogen has 5. Match the number of dots in the Lewis dot diagrams accordingly.

Step5: Analyze Bohr models for period and group (Question 11)

The number of electron shells is the period number. The number of valence electrons determines the group number (for main - group elements).

Step6: Determine oxidation numbers (Question 12)

Rb is an alkali metal with an oxidation number of + 1, Br is a halogen with an oxidation number of - 1, N can have multiple oxidation numbers but common ones are - 3, + 3, + 5, Al has an oxidation number of + 3, Mg has an oxidation number of + 2, S can have - 2, + 4, + 6.

Step7: Order elements by atomic radius (Question 13)

Atomic radius increases down a group. Oxygen is in period 2, sulfur is in period 3, and tellurium is in period 5. So the order from smallest to largest is oxygen, sulfur, tellurium.

Step8: Compare ionization energies (Question 14)

Si is to the right of Mg in the same period. Ionization energy increases from left to right across a period, so Si has a larger ionization energy.

Step9: Compare electronegativities (Question 15)

Sn is below C in the periodic table. Electronegativity decreases down a group, so C has a larger electronegativity, and Sn has the smallest electronegativity.

Answer:

1. Increases; Decreases; Decreases; Increases
2. d. B because it is harder to remove a valence electron from B.
3. c. B because it is a nonmetal and wants to gain electrons.
4. (Answers depend on the actual Lewis - dot diagrams, but follow the valence - electron rules: 1 for alkali metal, 7 for halogen, 8 for noble gas, 4 for carbon, 5 for nitrogen)
5. (Answers depend on the actual Bohr models, but period is number of electron shells and group is number of valence electrons for main - group elements)
6. + 1 (Rb); - 1 (Br); - 3 (common for N); + 3 (Al); + 2 (Mg); - 2 (common for S)
7. oxygen, sulfur, tellurium
8. Si
9. Sn