This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — here is the solution to Q1 and Q2. Q1. The properties of hydrogen are unique, leading to its placement in a separate position in the periodic table, though it shares characteristics with both Group 1 and Group 17 elements. a) Hydrogen is similar to Group 1 (alkali metals) because: • It has one valence electron (1s^1) in its outermost shell. • It can lose this electron to form a positive ion (H^+), similar to how alkali metals form M^+ ions. b) Hydrogen can also be considered to belong to Group 17 (halogens) because: • It needs one electron to achieve a stable electron configuration (a duet, like helium). • It can gain one electron to form a negative ion (H^-), known as a hydride ion, similar to how halogens form halide ions (X^-). • It exists as a diatomic molecule (H_2) at room temperature, similar to halogens (F_2, Cl_2, etc.). c) Hydrogen does not fully fit into Group 17 because: • Unlike halogens, hydrogen has a much lower electronegativity and a weaker tendency to gain electrons. • Hydrogen's H^+ ion is a bare proton, which is extremely reactive and does not exist freely in aqueous solutions, unlike the larger, less reactive alkali metal cations. • Hydrogen forms predominantly covalent bonds, whereas halogens readily form ionic bonds with metals. Q2. a) The basis of the electropositive nature of Group 1 elements (alkali metals) is their strong tendency to lose electrons and form positive ions. This is due to: • Having only one valence electron in their outermost shell. • Possessing large atomic radii and relatively low ionization energies. These factors make it energetically favorable for them to readily donate their single valence electron to achieve a stable noble gas electron configuration, resulting in a +1 oxidation state. b) The differentiation between Group 1 and Group 2 elements is as follows: • Valence Electrons: Group 1 elements have one valence electron, while Group 2 elements have two valence electrons. • Oxidation State: Group 1 elements typically form ions with a +1 oxidation state, whereas Group 2 elements form ions with a +2 oxidation state. • Reactivity: Group 1 elements are generally more reactive than Group 2 elements due to their lower first ionization energies. • Hardness and Density: Group 1 metals are typically softer and less dense than Group 2 metals. Drop the next question.