Question

1. why does electronegativity increase when you move from left to right across a row of the periodic table?

the force the nucleus exerts on electrons decreases.

the distance from the nucleus to the bond increases.

the number of protons in the nucleus increases.

the number of electron shells decreases.

1. which neutral atom in row 3 of the periodic table is the least likely to lose an electron?

sodium (na)

aluminum (al)

phosphorus (p)

argon (ar)

Explanation:

Question 5

To determine why electronegativity increases across a period (row) of the periodic table, we analyze each option:

• Option 1: If the nuclear force on electrons decreases, electronegativity (attraction for electrons) should decrease, so this is incorrect.
• Option 2: If the distance from the nucleus to the bond increases, the attraction for electrons (electronegativity) should decrease, so this is incorrect.
• Option 3: As we move left to right across a row, the number of protons in the nucleus (atomic number) increases. This increases the positive charge of the nucleus, which increases its attraction for electrons (electronegativity). This is correct.
• Option 4: The number of electron shells remains the same across a period (row), so this is incorrect.

To find the atom least likely to lose an electron, we consider ionization energy (the energy required to remove an electron). Atoms with full valence shells (noble gases) have the highest ionization energy and are least likely to lose electrons. In Row 3, Argon (Ar) is a noble gas with a full valence shell. Sodium (Na), Aluminum (Al), and Phosphorus (P) are more likely to lose electrons (Na and Al are metals, P is a non - metal but does not have a full valence shell like Ar).

Answer:

C. The number of protons in the nucleus increases.

Question 6