11.3, 11.4 VSEPR Theory: The Effect of Lone Pairs, Predicting Molecular Geometries

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11.3 VSEPR Theory: The Effect of Lone Pairs, 11.4 VSEPR Theory: Predicting Molecular Geometries

Last updated 12:21 AM on 10/19/26
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18 Terms

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electron geometry

the geometrical arrangement of electron groups in a molecule

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molecular geometry

the geometrical arrangement of atoms in a molecule

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trigonal pyramidal geometry

the molecular geometry of a molecule with tetrahedral electron geometry and one lone pair

<p>the molecular geometry of a molecule with tetrahedral electron geometry and one lone pair</p>
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is

Electron geometry ___ (is/is not) relevant to the molecular geometry; lone pair(s) exerts influence on the bonding pair(s).

<p>Electron geometry ___ (is/is not) relevant to the molecular geometry; lone pair(s) exerts influence on the bonding pair(s).</p>
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1, 2

A lone electron pair is more spread out in space than a bonding electron pair because a lone pair is attracted to ____ nucleus/nuclei while a bonding pair is attracted to ___ nucleus/nuclei.

<p>A lone electron pair is more spread out in space than a bonding electron pair because a lone pair is attracted to ____ nucleus/nuclei while a bonding pair is attracted to ___ nucleus/nuclei.</p>
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greater, decrease

Lone pair electrons typically exert slightly _______ (greater/lesser) repulsions than bonding electrons, causing bond angles to _________ (increase/decrease).

<p>Lone pair electrons typically exert slightly _______ (greater/lesser) repulsions than bonding electrons, causing bond angles to _________ (increase/decrease).</p>
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bent geometry

a molecular geometry in which the angle between 3 bonded atoms is approximately 109 degrees (could be less)

<p>a molecular geometry in which the angle between 3 bonded atoms is approximately 109 degrees (could be less)</p>
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lone pair-lone pair, lone pair-bonding pair, bonding pair-bonding pair

Electron group repulsions between lone pairs and bonding pairs in order from most to lease repulsions

<p>Electron group repulsions between lone pairs and bonding pairs in order from most to lease repulsions</p>
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seesaw geometry

aka irregular tetrahedron, the molecular geometry of a molecule with trigonal bipyramidal electron geometry and one lone pair in an equatorial position

<p>aka irregular tetrahedron, the molecular geometry of a molecule with trigonal bipyramidal electron geometry and one lone pair in an equatorial position</p>
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T-shaped

the molecular geometry of a molecule with trigonal bipyramidal electron geometry and two lone pairs in equatorial positions

<p>the molecular geometry of a molecule with trigonal bipyramidal electron geometry and two lone pairs in equatorial positions</p>
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linear

________ geometry also occurs when 3 of 5 electron groups around the central atoms are lone pairs, and lone pairs occupy all 3 of the equatorial positions

<p>________ geometry also occurs when 3 of 5 electron groups around the central atoms are lone pairs, and lone pairs occupy all 3 of the equatorial positions</p>
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square pyramidal geometry

molecular geometry of a molecule with octahedral electron geometry and one lone pair

<p>molecular geometry of a molecule with octahedral electron geometry and one lone pair</p>
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square planar geometry

molecular geometry of a molecule with octahedral electron geometry and two lone pairs

<p>molecular geometry of a molecule with octahedral electron geometry and two lone pairs</p>
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more

Bond angles can vary from idealized angles because double and triple bonds occupy ____ (more/less) space than single bonds (they are bulkier even though they are shorter), and lone pairs occupy _____ (more/less) space than bonding groups.

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straight line

bond in plane of paper

<p>bond in plane of paper</p>
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hatched wedge

bond going into the page

<p>bond going into the page</p>
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solid wedge

bond coming out of the paper

<p>bond coming out of the paper</p>
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interior

To predict the shape of larger molecules, we determine the geometry of each _______ (interior/terminal) atom.

<p>To predict the shape of larger molecules, we determine the geometry of each _______ (interior/terminal) atom.</p>