CHEM 1113 Study Guide - Final Guide: Lone Pair, Trigonal Bipyramidal Molecular Geometry, Trigonal Planar Molecular Geometry

119 views19 pages

tealhedgehog29

13 Dec 2016

School

Department

Course

Professor

For unlimited access to Study Guides, a Grade+ subscription is required.

Document Summary

Chem 1113 fall 2016 final exam new material study sheet. Chapter 11 - chemical bonding and molecular structure: Concept area 2 - molecular architecture: hybrid orbitals, molecular orbitals, and the structure of some simple. Organic molecules: given a molecule, you should be able to draw the lewis structure and determine the hybridization at the central atom and types of bonds ( - or -bonds) contained within the molecule. Hybrid orbitals: number of atomic orbitals put in equals the number of hybrid orbitals created: sp: linear edg 2 hybrid orbitals formed shape: linear, 180 , sp2: trigonal planar edg 3 hybrid orbitals formed shape: 1 lone pair: bent, <120 : sp3: tetrahedral edg 4 hybrid orbitals formed shape: 2 lone pairs: bent, <109. 5 : sp3d: trigonal bipyramidal edg 5 hybrid orbitals formed shape: No lone pairs: trigonal bipyramidal, 90 and 120 . 1 lone pair: see-saw, <90 and <120 .

Related Questions

Use valence bond theory to describe the bonding and geometry in theSeF4 molecule.

A. The central atom is Se, which has five electron groups around it(four bonding pairs and one nonbonding/lone pair). Theelectron-group geometry is trigonal bipyramidal (and the moleculargeometry is see-saw). To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3d orbitals. Four of these hybridorbitals contain one of Se's 6 valence electrons each, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The fifth hybrid orbital of Se contains a lone pair ofelectrons. There are 4 sigma bonds and 0 pi bonds in thismolecule.
B. The central atom is Se, which has six electron groups around it.The electron-group geometry is octahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3d2 orbitals.Four of these hybrid orbitals contain one of Se's 6 valenceelectrons each, and these hybrid orbitals overlap with unhybridizedp orbitals of the four F atoms. The fifth and sixth hybrid orbitalsof Se contain lone pairs of electrons. There are 4 sigma bonds and0 pi bonds in this molecule.
C. The central atom is Se, which has four electron groups aroundit. The electron-group geometry is tetrahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3 orbitals.These hybrid orbitals overlap with unhybridized p orbitals of thefour F atoms. There are 4 sigma bonds and 0 pi bonds in thismolecule.
D. The central atom is Se, which has four electron groups aroundit, two single bonds and two double bonds. The electron-groupgeometry is tetrahedral. To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3 orbitals. These hybrid orbitalscontain one electron each of Se's 6 valence electrons, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The final 2 electrons of Se's 6 valence electrons reside inunhybridized p orbitals, which overlap with unhybridized p orbitalsof the F atoms. There are 4 sigma bonds and 2 pi bonds in thismolecule.

Antibonding molecular orbitals can be used to make bonds to other atoms in a molecule. For example, metal atoms can use appropriate d orbitals to overlap with the
π^*_2p orbitals of the carbon monoxide molecule. This is called d-π backbonding. (a) Draw a coordinate axis system in which the y-axis is vertical in the plane of the paper and the x-axis horizontal. Write “M” at the origin to denote a metal atom. (b) Now, on the x axis to the right of M, draw the Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the x-axis. (c) Draw the CO π^*_2p orbital, with phases (see the “Closer Look” box on phases) in the plane of the paper. Two lobes should be pointing toward M. (d) Now draw the d_xy orbital of M, with phases. Can you see how they will overlap with the π^*_2p orbital of CO? (e) What kind of bond is being made with the orbitals between M and C, σ or π? (f) Predict what will happen to the strength of the CO bond in a metal–CO complex compared to CO alone.

turquoisemink562

CHEM 1113 Study Guide - Final Guide: Lone Pair, Trigonal Bipyramidal Molecular Geometry, Trigonal Planar Molecular Geometry

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 1113 Study Guide - Final Guide: Alkene, Alkyne, Cycloalkane

CH 101 Study Guide - Final Guide: Orbital Hybridisation, Lewis Structure, Metallic Bonding

CHEM 200 Chapter Notes - Chapter 11: Orbital Hybridisation, Atomic Orbital, Bond Energy

Related Questions