Shapes of Molecules Flashcards

1
Q

What can be used to predict the shapes of molecules and polyatomic ions?

A

VSPER ( valence shell electron pair repulsion )

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2
Q

Why is the shape of a molecule important?

A

It will determine its properties and uses.

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3
Q

How do you work out the shape of a molecule?

A
  1. the number of electron pairs ( outer electrons, same as group number )
  2. How many of the electron pairs are bonded to other atoms and non-bonded.
  3. the number of atoms attached to the central atom.
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4
Q

How do you work out the number of electron pairs in a molecule or polyatomic ion?

A

(number of valence e ( group number ) of the central atom (usually first atom)
+ number of atoms attached to central atom ) / 2

** if it is an ion, you subtract the charge if its a positive charge from the top row and you add thew charge if its a negative charge.

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5
Q

What are the shapes of molecules where al e- are bonding pairs?

A

Linear - 2 bonding pairs
Trigonal planer - 3 bonding pairs
Tetrahedral - 4 bonding pairs
Trigonal bipyramidal - 5 bonding pairs
Octahedral - 6 bonding pairs

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6
Q

How are shapes of molecules determined?

A

The shapes adopted by the atoms present based on the arrangement of electron pairs

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7
Q

Describe how electron pair repulsions decrease in strength in the order.

A

Greatest Atrraction/ smallest angle - (non-bonding pair/ non-bonding pair) > (non-bonding pair/ bonding pair) > (bonding pair/bonding pair) Weakest attraction / greatest angle

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8
Q

How are bond angles kept as far apart as possible?

A

Electron pairs are negatively charged and repel each other. They are arranged to minimise repulsion and maximise separation.

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9
Q

How many electron pairs gives you an angle of 90 degrees?

A

6

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