In a periodic table
How would the tendency to gain electrons change as you go down a group?

How does electron affinity vary down a group ?

How does ionisation energy vary along a period and down a group ?

Use the periodic table to answer the following questions. a) Identify elements with five electrons in the outer shell. b) Identify elements that would tend to loose two electrons. c) Identify elements that would tend to gain two electrons. d) Identify the group having metal, non-metal, liquid as well as gas at the room temperature.

Carbon (atomic number 6) and silicon(atomic number 14) are elements in the same group of the periodic table give the electronic arrangemetns of the carbon and silicon atoms and state the groups in which these elements occur.

Why does bond angle decreases in the hydrides of nitrogen family while going down a group ?

Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.

Which of the following pairs of elements would have a more negative electron gain enthalpy? i) O or N ii) F or Cl

By considering their position in the periodic table, which one of the following elements would you expect to have the most metalllic characteristics? Ga Ge As Se Be.