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Atomic Structure & Bonding Study Guide, Exams of Geometry

Geometry

(a) Draw the Lewis structure (electron-dot diagram) of each of the four species. ... (ii) The bond angles in SeCl4 are less than 90° and less than 120°.

Typology: Exams

2022/2023

Uploaded on 03/01/2023

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Atomic Structure & Bonding Study Guide
1. Use principles of atomic theory, along with the photoelectron spectroscopy data shown
below, to answer the following questions.
(a) Write the electron configuration for this element.
(b) How many valence electrons are present in this element?
(c) What is the identity of this element?
(d) Identify the sublevel associated with the peak at 104 MJ/mol.
(e) Explain for the large difference in energy between the peak at 104 MJ/mol and 6.84
MJ/mol.
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Atomic Structure & Bonding Study Guide

  1. Use principles of atomic theory, along with the photoelectron spectroscopy data shown below, to answer the following questions. (a) Write the electron configuration for this element. (b) How many valence electrons are present in this element? (c) What is the identity of this element? (d) Identify the sublevel associated with the peak at 104 MJ/mol. (e) Explain for the large difference in energy between the peak at 104 MJ/mol and 6. MJ/mol.

GeCl 4 SeCl 4 ICl 4 −^ ICl 4 +

  1. The species represented above all have the same number of chlorine atoms attached to the central atom. (a) Draw the Lewis structure (electron-dot diagram) of each of the four species. Show all valence electrons in your structures. (b) Identify the molecular geometry of each compound. (c) On the basis of the Lewis structures drawn in part (a), answer the following questions about the particular species indicated. (i) What is the Cl-Ge-Cl bond angle in GeCl 4? (ii) The bond angles in SeCl 4 are less than 90° and less than 120°. Explain why these bond angles are less than those of a molecule with trigonal bipyramidal geometry. (iii) Is SeCl 4 polar? Explain your reasoning. (iv) What is the hybridization of the Ge atom in GeCl 4?
  2. Answer the following questions related to sulfur. (a) Consider the two chemical species S and S^2 -. (i) Write the electron configuration of each species. (ii) Explain why the radius of the S^2 -^ ion is larger than the radius of the S atom. (b) The S^2 -^ ion is isoelectronic with the Ar atom. From which species, S^2 -^ or Ar, is it easier to remove an electron? Explain.
  1. Use principles of molecular structure to answer the following questions. (a) A complete Lewis electron-dot diagram of a molecule of ethyl methanoate is given below. (i) Identify the hybridization of the valence electrons of the carbon atom labeled Cw. (ii) Estimate the numerical value of the Hy-Cx-O bond angle in an ethyl methanoate molecule. Explain the basis of your estimate. (iii) Determine the number of sigma and pi bonds in ethyl methanoate. (b) Ethyl methanoate, CH 3 CH 2 OCHO, is synthesized in the laboratory from ethonal, C 2 H 5 OH, and methanoic acid, HCOOH, as represented by the following equation. C 2 H 5 OH(l) + HCOOH(l) ↔ CH 3 CH 2 OCHO(l) + H 2 O(l) In the box below, draw the complete Lewis electron-dot diagram of a methanoic acid molecule.