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- Draw a Lewis structure for each of the following molecules and ions. In each case, the atoms can be connected in only one way. (a) Br2 (b) H2S (c) N2H4 (d) N2H2 (e) CN- (f) NH4+ (g) N2 (h) O2Predict the best choice in each of the following. You may wish to review the chapter on electronic structure for relevant examples.(a) the most metallic of the elements Al, Be, and Ba(b) the most covalent of the compounds NaCl, CaCl2, and BeCl2(c) the lowest first ionization energy among the elements Rb, K, and Li(d) the smallest among Al, Al+, and Al3+(e) the largest among Cs+, Ba2+, and XeWhich of the following statements is true? (A) Because HCl is a strong acid, the bond dissociation energy of HCl is smaller than that of Cl₂. (B) The Cl₂ bond cannot cleavage by increasing temperature. (C) Yellow light cannot cleavage Cl2 bond, you can do it well by increasing amplitude of yellow light. (D) The electromagnetic wavelength required to cleavage Cl2 bond is greater than that to cleavage Br2 bond (E) The oxygen atoms are found easily far away from earth surface than it be found in earth surface.
- Draw the Lewis structures and describe the geometry for the following:(a) PF4+(b) PF5(c) PF6−(d) POF3Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+(b) CF4(c) BF3(d) SiF5−(e) BeCl216. What is the molecular geometry of PH3? (A) Trigonal planar (B) T-shaped (C) Trigonal pyramidal (D) Tetrahedral 17. The correct Lewis structure for BF3 would have exactly: (A) 1 double bond (B) 2 double bonds (C) No double bonds (D) 1 triple bond 18. Nitrogen has a greater first ionization energy than phosphorus. What is the best evidence to support this observation? (A) Nitrogen has a greater effective nuclear charge. (B) A nitrogen atom is larger than a phosphorus atom. (C) The electron ionized from nitrogen is in a lower energy level closer to the nucleus. (D) The electron ionized from nitrogen is not from a valence energy level.
- Please don't provide handwritten solution ....Mixing SbCl3 and GaCl3 in a 1;1 molar ratio (usingliquid sulfur dioxide as a solvent) gives a solid ioniccompound of empirical formula GaSbCl6. A controversyarises over whether this compound is ( ) SbCl2 + ( ) GaCl 4 - or( ) GaCl+ 2 ( ) SbCl 4 -(a) Predict the molecular structures of the two anions.(b) It is learned that the cation in the compound has abent structure. Based on this fact, which formulationis more likely to be correct?Write a Lewis structure for each of the following molecules and ions:(a) (CH3)3SiH(b) SiO44−(c) Si2H6(d) Si(OH)4(e) SiF62−
- Give the Lewis structure of each of the following:(a) SF4(b) K2SO4(c) SO2Cl2(d) H2SO3(e) SO3Draw the Lewis structures for CO2 and CO, and predict the number of σ and π bonds for each molecule.(a) CO2(b) COPredict the electron pair geometry and the molecular structure of each of the following ions:(a) H3O+(b) PCl4−(c) SnCl3−(d) BrCl4−(e) ICl3(f) XeF4(g) SF2