Periodic Table

Elements with stable electronic configuration e.g. neon have an electron affinity value of 0.

Increase in nuclear charge of an atom decreases the tendency of the atom to lose electrons.

With increase in nuclear charge the nuclear attraction for outer electrons increases, hence ionization potential increases.

Atomic size across a period decreases with increase in nuclear charge of the element.

Atomic size of neon is more than the atomic size of fluorine.

The nuclear charge of an atom is the positive charge on the nucleus of an atom, equivalent to the atomic number of an atom.

Across a period the nature of oxides and hydrides varies from basic to acidic while the strength of oxy-acids increases from left to right.

Periodicity in properties is observed in elements after definite intervals due to similar electronic configuration.

The element in group 17 [VIIA] which is a liquid at room temperature is Br.

Elements of group 1 [IA] are strong reducing agents since they are electron donors.