Question

1. what happens to the valence electrons as you go right on a period in the periodic table?

• a. they are closer to the nucleus
• b. they are further from the nucleus
• c. their number increases
• d. their number decreases

1. which of the following has the largest atomic radius?

• a. lithium (li)
• b. rubidium (rb)
• c. iodine (i)
• d. fluorine (f)

1. when comparing elements, which will have more metallic character?

• a. elements with lower ionization energy
• b. elements with smaller atomic radius
• c. elements with higher electronegativity
• d. elements with fewer electron shells

Explanation:

8.

• Option a: As we move right in a period, the effective nuclear charge increases, pulling valence electrons closer.
• Option b: Incorrect as electrons are pulled closer.
• Option c: In a period, from left to right, the number of valence electrons increases (e.g., in period 2, Li has 1, Be has 2, …, Ne has 8).
• Option d: Opposite of the actual trend.

• Atomic radius increases down a group (due to more electron shells) and decreases across a period (due to increasing effective nuclear charge).
• Li and Rb are in Group 1 (alkali metals). Rb is below Li, so Rb has a larger radius than Li.
• I is in Group 17. It has fewer electron shells than Rb (Rb has 5 shells, I has 5 shells but higher effective nuclear charge pulling electrons in more).
• F is in Group 17, period 2 (very small radius).

• Metallic character is related to the ability to lose electrons.
• Ionization energy is the energy required to remove an electron. Lower ionization energy means easier to lose electrons (more metallic).
• Smaller atomic radius: Electrons are held more tightly (less metallic).
• Higher electronegativity: Atoms tend to gain electrons (more non - metallic).
• Fewer electron shells: Electrons are held more tightly (less metallic as in smaller atoms across a period).

Answer:

c. Their number increases

9.