Consider the following orders : (i) HF > HCl > HBr > HI : Lewis basic character (ii) CH4 < CCl4 < CF — Periodic Table and Periodicity Chemistry Question
Question
Consider the following orders : (i) HF > HCl > HBr > HI : Lewis basic character (ii) CH4 < CCl4 < CF4: Electronegativity of central 'C'-atom (iii) Mg2+ < K+ < S2- < Se2-: Ionic radius (iv) Ni > Pd > Pt : Ionisation energy (v) As5+ > Sb5+ > Bi5+: Stable oxidation state (vi) LiF > NaF > KF > RbF: Lattice energy (vii) F-(aq.) > Cl-(aq.) > Br-(aq.) > I-(aq.): Electrical conductance (viii) Li+ < Mg2+ < Al3+: Hydration energy (ix) Cl > Br > F > I : Electron affinity (x) BeCl2 < AlCl3 < SiCl4: Lewis acidic character. Then calculate value of \
💡 Solution & Explanation
Step 1: Write down the electronic configuration for each element to determine the number of unpaired electrons in their ground states. Step 2: Nitrogen (N: 1s2 2s2 2p3) has 3 unpaired electrons; Oxygen (O: 1s2 2s2 2p4) has 2 unpaired electrons; Aluminum (Al: [Ne] 3s2 3p1) has 1 unpaired electron; Calcium (Ca: [Ar] 4s2) has 0 unpaired electrons. Step 3: Paramagnetic behavior increases with the number of unpaired electrons. Therefore, the correct decreasing order of paramagnetism is N (3) > O (2) > Al (1) > Ca (0).