Periodic Table, Periodic Properties and Variations of Properties — Question 1
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(a) The element below sodium in the same group would be expected to have a ............... (lower/higher) electro-negativity than sodium and the element above chlorine would be expected to have a (lower/higher) ionization potential than chlorine.
(b) On moving down a group, the number of valence electrons ............... (remains the same/increases/ decreases).
(c) Metals are good ............... (oxidising agent/ reducing agent) because they are electron ............... (acceptors/donors).
(d) Down the group, electron affinity ............... [increases, decreases, remains same].
(e) Electronegativity across the period ............... [increases/ decreases].
(f) Non-metallic character down the group ............... [increases/ decreases].
(g) In a period, increase in electron affinity increases ............... (oxidation/reduction).
(h) On descending a group, ............... (increase/decrease) in ionisation potential as well as electron affinity ............... (increases/decreases) oxidising capacity.
(i) If an element has a low ionization energy then it is likely to be ............... (metallic/non metallic).
(j) If an element has seven electrons in its outermost shell then it is likely to have the ............... (largest/smallest) atomic size among all the elements in the same period.
(a) The element below sodium in the same group would be expected to have a lower (lower/higher) electro-negativity than sodium and the element above chlorine would be expected to have a higher (lower/higher) ionization potential than chlorine.
(b) On moving down a group, the number of valence electrons remains the same (remains the same/increases/ decreases).
(c) Metals are good reducing agent (oxidising agent/ reducing agent) because they are electron donors (acceptors/donors).
(d) Down the group, electron affinity decreases [increases, decreases, remains same].
(e) Electronegativity across the period increases [increases/ decreases].
(f) Non-metallic character down the group decreases [increases/ decreases].
(g) In a period, increase in electron affinity increases reduction (oxidation/reduction).
(h) On descending a group, decrease (increase/decrease) in ionisation potential as well as electron affinity decreases (increases/decreases) oxidising capacity.
(i) If an element has a low ionization energy then it is likely to be metallic (metallic/non metallic).
(j) If an element has seven electrons in its outermost shell then it is likely to have the smallest (largest/smallest) atomic size among all the elements in the same period.