VSEPR

Question 1

valence shell electron pair repulsion theory

Answer 1

predicts shapes of molecules and atoms by assuming that valence shell electron pairs are arranged around so that electron pairs are kept as far away from each other as possible. Double or triple bonds will not change this.

Question 2

Dipole moment

Answer 2

Arrows that point to the more electronegative ion. If they oppose, they cancel out. If they go towards each other, they add together.

Molecules with zero dipole moments are non polar

Question 3

Polar molecules

Answer 3

Non symmetrical, with a dipole moment

Question 4

Bond theory

Answer 4

Bonds form when two orbitals overlap

Total number of electrons in each orbital is no more than two

Strength of the bonds depends on the amount of overlap, orbitals bond in the directions in which they protrude a point to obtain maximum overlap

Question 5

Hybrid orbitals

Answer 5

Orbitals used to describe bonding that are obtained by taking combinations of atomic orbitals. Number of hybrid orbitals is always equal to the number of orbitals used

Question 6

sp shape

Answer 6

Linear

Question 7

sp2 shape

Answer 7

trigonal planar

Question 8

sp3 shape

Answer 8

tetrahedral

Question 9

sp3d

Answer 9

trigonal biprymidal

Question 10

2p3d2

Answer 10

Octahedral

Question 11

Sigma bonds

Answer 11

Formed when there is a single bond, when two 2 orbitals overlap

Question 12

Pi bonds

Answer 12

Electron distribution above and below the bond axis- formed by a sideways gap of 2 p orbitals. Will have a sigma bond with it

Question 13

Diatomic molecules

Answer 13

Non polar if the two atoms are identical

Polar if they are different

Question 14

Triatomic molecules

Answer 14

If they are linear with the same atoms bonded to the central atom, non polar

if terminal atoms are different they are polar

If the molecule is bent, it is polar

Question 15

Steric number

Answer 15

The number of atoms bonded to an electron