review 3 - key

review 3 - key - Chapter 9: Geometry 1. Determine the...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Chapter 9: Geometry 1. Determine the electron-domain geometry and molecular shape (geometry) for any molecule or ion. i) which of the following molecule has a trigonal planar molecular shape . (a) CO (b) CF 4 (c) CO 3 2- (d) NH 3 ii) what is the parent structure and molecular shape for ClO 3- , respectively? (a) trigonal planar and trigonal planar (b) trigonal planar and bent (c) tetrahedral and trigonal pyramidal (d) tetrahedral and tetrahedral (e) tetrahedral and bent 2. Give approximate bond angles and predict how angles may deviate (larger or smaller) from these approximate values. Draw the Lewis Structure of water. What is the parent structure? What is the molecular shape? What approximate angle(s) do you expect for the molecular shape? Parent structure: TETRAHEDRAL Molecular shape: BENT H-O-H bond angle is approximately 109.5 (or slightly less due to repulsion by lone pair electrons) 3. Identify a molecule as being polar or nonpolar. Define molecular polarity. i) Which of the following molecules is polar? (a) BCl 3 (b) SiF 4 (c) H 2 S (d) CO 2 ii) For an ABn type of molecule, indicate which of the following molecular geometries would be result in a polar molecule and which would be non-polar: Trigonal planar Nonpolar Tetrahedral Nonpolar Trigonal pyramidal Polar Bent Polar T-shape Polar Linear Nonpolar Square planar Nonpolar Octahedral Nonpolar Trigonal bipyramidal Nonpolar 4. Determine the hybridization for all central atoms in a molecule Valence Electron Pair Geometry Number of Orbitals Hybrid Orbitals Linear 2 sp Trigonal Planar 3 sp 2 Tetrahedral 4 sp 3 Trigonal Bipyramidal 5 sp 3 d Octahedral 6 sp 3 d 2 H 2 O Hybridization Involving d Orbitals Atoms in the third period and higher can utilize d orbitals to form hybrid orbitals PF 5 i) What is the electron pair geometry (EPG) for a central atom with sp 3 d hybridization? (a) Linear (b) Octahedral (c) Tetrahedral (d) Trigonal bipyramidal (e) Trigonal planar ii) For the following molecules, specify the hybrid orbitals of the central atom: AsF 5 2- , CCl 4 AsF 5 2- sp 3 d 2 CCl 4 sp 3 iii) Draw a Lewis Structure for the ammonium ion (NH 4 + ). Draw an orbital diagram to indicate the hybrid orbitals for the central Nitrogen iv) Draw the Lewis Structure for the SCl 5- ion. Draw an orbital diagram to indicate the hybrid orbitals for the central Sulfur 5. Determine the number of sigma and pi bonds in a molecule. How do and bonds differ? Which types of orbitals are used for each? i) How many bonds and bonds are there in the O 3 molecule? (a) 1 bonds, 1 bonds (b) 1 bonds, 2 bonds (c) 2 bonds, 1 bonds (d) 2 bonds, 2 bonds ii) Warm apple pi Give the electron pair geometry, expected hybrid orbitals and molecular geometry for the atoms in the following structure 6. Explain why rotation does not occur about double bonds ....
View Full Document

Page1 / 13

review 3 - key - Chapter 9: Geometry 1. Determine the...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online