shapes of molecules

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  • Created by: NicoleAD
  • Created on: 25-04-16 22:10
Give the bond/lone pairs, bond angle and an example of a tetrahedral molecule
Four bond pairs, no lone pairs. Has a bond angle of 109.5 degrees and an example is an ammonium molecule.
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Give the bond/lone pairs, bond angle and an example of a linear molecule.
2 bond pairs, no lone pairs, has a bond angle of 180 degrees. An example of this is beryllium chloride.
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Give the bond/lone pairs, bond angle and an example of a trigonal planar molecule.
Three bond pairs and no lone pairs, has a bond angle of 120 degrees. An example of this is boron trifluoride.
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Give the bond/lone pairs, bond angle and an example of a non linear molecule.
2 bond pairs 2 lone pairs and a bond angle of 104,5 degrees. An example of this is water.
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Give the bond/lone pairs, bond angle and an example of a trigonal pyramidal molecule.
3 bond pairs, 1 lone pair, has a bond angle of 107 degrees. An example of this would be an ammonia molecule.
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Give the bond/lone pairs, bond angle and an example of a trigonal bipyramidal molecule.
5 bond pairs no lone pairs, has bond angles of 90 and 120 degrees and an example is phosphorus pentachloride.
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Give the bond/lone pairs, bond angle and an example of a seesaw molecule.
4 bond pairs, 1 lone pair, has bond angles of 86.5 and 102 degrees. An example of this is sulfur tetrafluoride.
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Give the bond/lone pairs, bond angle and an example of a t-shape molecule.
3 bond pairs, 2 lone pairs, a bond angle of 87.5 degrees. An example of this would be chlorine trifluoride.
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Give the bond/lone pairs, bond angle and an example of an octahedral molecule.
6 bond pairs no lone pairs , a bond angle of 90 degrees and an example is sulfur hexafluoride.
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Give the bond/lone pairs, bond angle and an example of a square pyramidal molecule.
5 bond pairs 1 lone pair, bond angle of 90 degrees and an example is chlorine pentafluoride.
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Give the bond/lone pairs, bond angle and an example of a square planar molecule.
4 bond pairs 2 lone pairs, bond angle of 90 degrees and an example is xenon tetrafluoride.
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How do we predict the shape of a molecule?
1.Find the central atom (take how many electrons in the outer shell) 2. how many other atoms is the central atom bonded to. 3. If it has a negative charge +1 if it has a positive charge -1 4. add values together then divide by 2.
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Define 'charge cloud'.
A charge cloud is an area where there is a large possibility of finding an electron.
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Define electronegativity.
Electronegativity is the ability to attract the bonding electrons in a covalent bond.
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What is a dipole?
The difference in electronegativity between two atoms causes a dipole.
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Briefly explain valence shell electron pair repulsion theory.
Lone pair/lone pair have the greatest repulsion. Lone pair/bond pair second greatest repulsion and bond pair/bond pair has the weakest repulsion.
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Other cards in this set

Card 2

Front

Give the bond/lone pairs, bond angle and an example of a linear molecule.

Back

2 bond pairs, no lone pairs, has a bond angle of 180 degrees. An example of this is beryllium chloride.

Card 3

Front

Give the bond/lone pairs, bond angle and an example of a trigonal planar molecule.

Back

Preview of the front of card 3

Card 4

Front

Give the bond/lone pairs, bond angle and an example of a non linear molecule.

Back

Preview of the front of card 4

Card 5

Front

Give the bond/lone pairs, bond angle and an example of a trigonal pyramidal molecule.

Back

Preview of the front of card 5
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