Question

1. indicate the trends for the following properties: atomic radius net attractive force 1st ionization energy electronegativity metallic character nonmetal reactivity

Explanation:

Atomic Radius

• Trend: Increases down a group (due to addition of electron shells) and decreases across a period (increasing nuclear charge pulls electrons closer).

Net Attractive Force

• Trend: Increases across a period (higher nuclear charge with same - shell electrons) and decreases down a group (electrons in higher shells are less strongly attracted).

1st Ionization Energy

• Trend: Decreases down a group (electrons in higher shells are easier to remove) and increases across a period (higher nuclear charge makes it harder to remove electrons).

Electronegativity

• Trend: Decreases down a group (electrons in higher shells are less attracted) and increases across a period (higher nuclear charge attracts electrons more).

Metallic Character

• Trend: Increases down a group (easier to lose electrons) and decreases across a period (more non - metallic behavior as nuclear charge increases).

Nonmetal Reactivity

• Trend: For non - metals, reactivity first increases then decreases across a period (halogens are very reactive). Down a group of non - metals (e.g., halogens), reactivity decreases (as atomic size increases, it is harder to gain electrons).

Answer:

• Atomic Radius: Increases down a group, decreases across a period.
• Net Attractive Force: Increases across a period, decreases down a group.
• 1st Ionization Energy: Decreases down a group, increases across a period.
• Electronegativity: Decreases down a group, increases across a period.
• Metallic Character: Increases down a group, decreases across a period.
• Nonmetal Reactivity: Across a period (for non - metals), first increases then decreases; down a group (of non - metals), decreases.