shapes of molecules and ions with 5 and 6 negative centers section 14.1

Shapes of Molecules and Ions with 5 and 6 negative centers •Section 14.1

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Shapes of Molecules and Ions with 5 and 6 negative

centers

•Section 14.1

Sulfur Hexafluoride Octahedral with bond angles of 90º and 180º Notice there are 12 electrons around the

sulfur atom

Page 3: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

VSEPR Theory Can be used for 5 and 6 negative centers Elements in the 3rd and lower periods of the

p-block can promote one or more electrons from a filled s or p orbital to an unfilled, low energy d orbital

More unpaired electrons are available for bonding

Page 4: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Continued Have an expanded valence shell with more

than 8 electrons Usually occurs when the atoms are

relatively small and very electronegative so they can fit around the central atom

Lewis structures are a little more challenging as you have to consider the total number of electrons available

Examples: SF6, PCl5, XeF4, PF6-

Page 5: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Phosphorus Pentachloride Trigonal bipyramidal with angles of 90º and

120º

Page 6: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Xenon Tetrafluoride Unshared (lone) pairs of electrons distort the

shape to make it a square planar with bond angles of 90º

Page 7: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Sulfur Hexafluoride Shape is an octahedron See pages 107 or 375 for additional pictures

and examples

Page 8: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Resonance Structures Consider the nitrate ion and its Lewis

structure It has three possible structures Note the use of lines and dots whereas you

must use one or the other

Page 9: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Continued Experiments have shown that the bonds do

not really switch back and forth Instead, all the bonds have the same length

and energy A better structure is called a resonance

hybrid:

Page 10: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Continued The shape is trigonal planar The electrons are said to be delocalized as in

they are shared evenly and not with just one nucleus

Consider the nitrite ion. The resonance structures are:

Page 11: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

More on the Nitrite Ion The shape is bent The resonance hybrid is:

Page 12: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Consider the Carbonate Ion Has three resonance structures The resonance hybrid is trigonal planar

Page 13: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Ozone (O3) Has two resonance structures The resonance hybrid is bent

Page 14: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

RCOO-

R represents a combination of CH3 with a number of CH2 attached (or not)

The important part is that the two oxygens experience resonance

The shape is trigonal planar

Page 15: Shapes of Molecules and Ions with 5 and 6 negative centers Section 14.1

Benzene Ring The resonance structures are called Kelule

structures

Resonance structures can be drawn as any of the examples below

Shapes of molecules The shapes of molecules and ions can be described by valence shell electron pair repulsion VSEPR predicts the shapes and bond

Indicator 14.1

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