Periodic TableIonization Energy Trend6Choose the best answerThe first ionization energy generally decreases down a group mainly because of an increase in: (1) Atomic radius (2) Nuclear charge (3) Electron affinity (4) Number of shielding electronsA(1) and (2)B(1) and (4)C(2) and (3)D(3) and (4) Like 0 Discuss 0Share
Periodic TableAtomic Radius Trend7Choose the best answerThe correct decreasing order of atomic radii in Period 3 is:ACl > S > P > SiBSi > P > S > ClCP > Si > Cl > SDSi > S > P > Cl Like 0 Discuss 0Share
Periodic TableIonic Radius8Choose the best answerWhich statement correctly compares the sizes of Cl and Cl⁻?ACl⁻ is smaller because it gains an electron.BCl and Cl⁻ have the same radius.CCl⁻ is larger because electron–electron repulsion increases.DCl is larger because it is neutral. Like 0 Discuss 0Share
Periodic TableIsoelectronic Species and Ionic Radius9Choose the best answerAr, K⁺ and Ca²⁺ are isoelectronic. Their radii increase in the order:AAr < K⁺ < Ca²⁺BCa²⁺ < Ar < K⁺CCa²⁺ < K⁺ < ArDK⁺ < Ar < Ca²⁺ Like 0 Discuss 0Share
Periodic TableIonization Energy and Metallic Character10Choose the best answerWhich information cannot be concluded simply from a low ionization energy?AThe element is likely metallicBIt readily forms positive ionsCIt may form ionic bondsDIt belongs to the p-block Like 0 Discuss 0Share