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Shapes of molecules & ions

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Page 1: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

Shapes of molecules & ions

Page 2: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

VSEPR theory

VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and ions

Page 3: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

VSEPR theory

VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and ions

It states that because of the repulsion between pairs of electrons around the central atom in the molecule or ion, the pairs of electrons are arranged to be as far away from each other as possible

Page 4: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

Negative Charge Centres

For VSEPR, multiple bonds (double, triple) count as if they are just one pair of electrons

Page 5: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

Negative Charge Centres

For VSEPR, multiple bonds (double, triple) count as if they are just one pair of electrons

So VSEPR uses repulsion between negative charge centres rather than between pairs of electrons

Page 6: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

4 bonding pairs - tetrahedral

Bond Angle =

109.5º

E.g methane - CH4, CCl4, SiCl4

4 negative charge centres

From: http://library.thinkquest.org/3659/structures/commonstructures.html

www.chemvc.com/~tim/VSEPR.html , http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter4section8.rhtml

Page 7: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

3 bonding pairs (& 1 non-bonding pair) trigonal pyramid

Bond Angle = 107º

E.g. ammonia - NH3, PCl3

4 negative charge centres

From: http://library.thinkquest.org/3659/structures/commonstructures.html

www.chemvc.com/~tim/VSEPR.html , http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter4section8.rhtml

Page 8: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

The bond angle decreases because the non-bonding pair of electrons exerts a greater repulsion than the bonding pair(s)

From: http://www.examstutor.com/chemistry/resources/studyroom/bonding/shapes_of_molecules/

Page 9: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

2 bonding pairs ( 2 non-bonding pairs)

bent or v-shaped

Bond angle = 105º

E.g. H2O, H2S

4 negative charge centres

From: http://library.thinkquest.org/3659/structures/commonstructures.html

www.chemvc.com/~tim/VSEPR.html , http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter4section8.rhtml

Page 10: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

2 negative charge centres

Shape is always linear

Bond angle is 180º

E.g.

From: www.physchem.co.za/Bonding/Shape.htm

www.tulane.edu/~bmitche/book/structrj.html

Page 11: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

3 negative charge centres 3 bonding electron

pairs, no non-bonding pairs

Trigonal planar

Bond angle is 120°

e.g. BF3, ethene, CO32-

2 bonding pairs, 1 non-bonding pair

Bent or v-shaped Bond angle is 120°

E.g. SO2, ozone - O3

From: http://library.thinkquest.org/3659/structures/commonstructures.html ,

www.chm.bris.ac.uk/motm/so2/so2h.htm

Page 12: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

5 and 6 charge centres

Elements in the third period can have more than 8 electrons in their outer shell because the 3 d orbitals are close in energy to the 3p orbitals.

The VSEPR theory also applies

You do not have to know specific bond angles

Page 13: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

5 negative charge centres (HL)

Trigonal bipyramidal e.g. PCl5

From: http://library.thinkquest.org/3659/structures/commonstructures.html

Page 14: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

5 negative charge centres (HL)

4 bonding pairs and 1 non-bonding pair

Distorted tetrahedral

From: www.chemvc.com/~tim/Predictions.html

Page 15: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

6 negative charge centres (HL)

Octahedral

e.g. SF6

From: http://library.thinkquest.org/3659/structures/commonstructures.html

Page 16: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

6 negative charge centres (HL)

4 bonding pairs and 2 non-bonding pairs as far apart as possible (above & below plane)

Square planar

e.g. XeF4

From: www.chemvc.com/~tim/Predictions.html

Page 17: Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and

VESPR theory

All the previous molecular shapes are based on VSEPR theory

VSEPR=Valence Shell Electron Pair Repulsion theory

Pairs of electrons arrange themselves around the central atom so that they are as far apart from each other as possible


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