Unit-4 Periodic Table and Periodicity of Properties
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Unit-4 Periodic Table and Periodicity of Properties
Answer: Alkali metals lose their single outer electron most easily.
Answer: Francium and caesium at the lower left are the most metallic.
Answer: Sodium and potassium are s-block alkali metals.
Answer: Greater nuclear charge pulls electrons closer, shrinking the atom.
Answer: Francium's large size and low ionization energy make it most metallic.
Answer: Chlorine is a p-block element; its last electron enters the p-subshell.
Answer: Each new period adds an outer shell, increasing atomic size.
Answer: Effective nuclear charge equals nuclear charge minus the shielding constant.
Answer: Transition elements have their last electrons in the d-subshell.
Answer: Smaller radius and stronger nuclear attraction make electrons harder to remove.
Answer: Actinides are in the seventh period and the f-block.
Answer: s- and p-block elements are known as representative (normal) elements.
Answer: Larger atoms hold outer electrons more loosely, lowering ionization energy.
Answer: Francium loses its single valence electron most readily.
Answer: Lanthanides and actinides are inner transition elements of the f-block.
Answer: K is lowest in Group 1, so it has the largest atomic radius.
Answer: Transition metals show only slight variations in atomic size across a period.
Answer: Alkali metals readily lose one valence electron, making them most reactive.
Answer: Across a period, atoms gain electrons more readily, increasing electron affinity.
Answer: Tellurium lies on the zigzag line and shows metalloid properties.