Question

10. Indicate whether the following properties increase or decrease from top to bottom down a group on the periodic table. a. atomic radius: ____________________ b. Valence electrons: ____________________ c. electronegativity (not including noble gasses): __________________ d. Ionization energy: ______________________

Answer 1

Answer: Atomic radius increases, valence electrons remain the same, electronegativity decreases, ionization energy decreases.

Step-by-step explanation:

Atomic radius increases due to increasing number of electron shells. (Think bigger shell = bigger atom)

Valence electrons = group number, so they stay the same.

Electronegativity decreases. As more shells are added (greater atomic radius), the ability to attract electrons decreases as the distance between nucleus and outer shells gets smaller, the electromagnetic force decreases. Therefore usually larger atomic radius = lower electronegativity.

ionization decreases. The outermost electron is not held on to tightly, taking little energy to remove. Caused by shielding effect.

Hope this helped!