Ionization energy generally decreases down a group because:
A. Atomic radius increases and shielding effect increases
B. Number of valence electrons increases
C. Nuclear charge decreases
D. Electron affinity increases
Answer: Option A
Solution (By JKExamLibrary)
Down a group, number of shells increases, atomic radius increases, and inner electrons shield the outermost electron from the nucleus. The effective nuclear charge experienced by valence electron decreases, making it easier to remove. Thus ionization energy decreases. For example, IE of Cs
Explanation:
The ion-exchange process (using cation and anion exchange resins) removes all dissolved cations and anions from water, producing completely demineralized (deionized) water. Distillation removes most impurities but may still contain trace dissolved gases or volatile organics.
Explanation:
Unsaturated hydrocarbons contain at least one double or triple bond between carbon atoms. Benzene (C6H6) has a ring structure with alternating double bonds (delocalized pi electrons), making it highly unsaturated. Cyclohexane, propane, and methane contain only single bonds and are saturated hydrocarbons.
Explanation:
Mg goes from 0 to +2 oxidation state, losing electrons – oxidized. Oxygen is reduced (0 to -2). This is a combustion/combination redox reaction.
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