CHEM 11b Lecture Notes - Lecture 1: Trigonal Bipyramidal Molecular Geometry, Trigonal Planar Molecular Geometry, Valence Bond Theory

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viridiancrow586

30 Jan 2017

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Document Summary

The shape of a molecule is determined by the electron groups around the central atom that repel one another. Single bond, multiple bond, lone pair, single electron. Arrange themselves to be as far away from one another as possible. *to show 3d: solid wedge(bond) comes out of paper, hashed wedge goes into paper, line is in the plane of the paper. A trigonal planar group (equatorial atoms) with a linear group up and down in it (axial atoms) 120o with equatorial atoms and 90o bond angles with the axial bonds. Antimony pentachloride - sbcl5 trigonal bipyramidal geometry. Double bonds have more electron density so they repel single bonds slightly more. Electron-group geometry is determined by the total number of electron groups (of any kind) around an atom . Molecular geometry is the shape created by the bonding groups and the angles between them. Molecular geometry is influenced by the number of lone electron pairs around an atom.

Related Questions

Select all molecular geometries (shapes) that are possible for a molecule with five electron groups an the central atom.

Do not include molecular geometries that can only be produced by having a single bonding group on the central atom (all but one of the electron groups are lone pairs.)

ocahedral
	T-shaped
	linear
	bent
	trigonal pyramidal
	trigonal bipyramidal
	seesaw
	square pyramidal
	trigonal planar
	tetrahedral
	square planar

Part A

Select all molecular geometries (shapes) that are possible for a molecule with five electron groups an the central atom.

Do not include molecular geometries that can only be produced by having a single bonding group on the central atom (all but one of the electron groups are lone pairs.)

	T-shaped
	square pyramidal
	ocahedral
	tetrahedral
	square planar
	linear
	bent
	trigonal planar
	trigonal bipyramidal
	trigonal pyramidal
	seesaw

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Draw the Lewis structure for , then answer the following questions:

a. How many valence electrons does this compound have?

b. How many bonded electrons does this compound have?

c. How many lone pairs of electrons does this compound have?

d. How many single bonds does this compound have?

e. How many double bonds does this compound have?

f. What is the electron group arrangement (aka electron pair geometry) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)?

g. What is the molecular arrangement (aka shape) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar)?

h. Predict the approximate bond angle (enter e.g. 90, 109.5, 120, 180, <109.5, >109.5).