Unit-4 Periodic Table and Periodicity of Properties
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Unit-4 Periodic Table and Periodicity of Properties
Answer: Group 1 (IA) elements are the alkali metals.
Answer: Down a group, larger atoms accept electrons less readily.
Answer: Group 2 (IIA) elements are the alkaline earth metals.
Answer: Larger atoms attract shared electrons less strongly.
Answer: Halogens are the reactive non-metals of Group 17.
Answer: Oxygen is smaller and higher in the group, so it is more electronegative.
Answer: Noble gases occupy Group 18 and have complete valence shells.
Answer: Sodium is farther left in the period, so it is more metallic.
Answer: Halogens have seven valence electrons and need one more for an octet.
Answer: Moving right, elements gain electrons more easily, becoming non-metallic.
Answer: Noble gases have eight valence electrons, a stable configuration.
Answer: Inner shell electrons shield outer electrons from nuclear attraction.
Answer: Metals have low ionization energies and readily form positive ions.
Answer: Each new shell adds electrons that screen the valence electrons.
Answer: Non-metals gain electrons to complete their valence shell.
Answer: Same-shell electrons shield poorly, so the nucleus pulls harder across a period.
Answer: Metalloids like silicon and boron show intermediate properties.
Answer: Noble gases have stable complete shells, needing the most energy to lose an electron.
Answer: Atomic radius measures the distance from the nucleus to the outermost shell.
Answer: Silicon lies on the zigzag line with mixed properties.