Molecular Geometry

Question 1

Bond Angles

Answer 1

Based on electron domain geometries (number of domains).

Question 2

What is bond angle of linear?

Answer 2

180 Degrees

Question 3

What is bond angle of trigonal planar?

Answer 3

120 Degrees

Question 4

What is bond angle of tetrahedral?

Answer 4

109.5 Degrees

Question 5

What is the bond angle of trigonal bipyramidal

Answer 5

The whole thing is 180 degrees, however up and down is 90 degrees, side to side is 120 degrees.

Question 6

What is the bond angle of octahedral?

Answer 6

90 Degrees

Question 7

2 types of trigonal bipyramidal, what are they?

Answer 7

Equatorial and Axial positions.

Question 8

What is an equatorial position?

Answer 8

Three bonds arranged in a trigonal plane.

Question 9

What is an axial position?

Answer 9

Perpendicular to the trigonal plane.

Question 10

What is molecular geometry?

Answer 10

The shape the atoms themselves make.

Question 11

Do lone pairs affect the shape?

Answer 11

Yes, but not used in the descriptive name of the shape.

Question 12

How to determine molecular geometry?

Answer 12

Number of domains + number of lone pairs on the central atom.

Question 13

Electronic Geometry

Answer 13

Arrangement of electron pairs around a central atom.

Question 14

Molecular Geometry

Answer 14

Arrangement of atoms instead of electrons.

Question 15

Bond Angles

Answer 15

The angle between the two bonds, based on electron domain geometries.

Question 16

Multiple bonds occupy how much space?

Answer 16

A lot of pace, more space than single bonds.

Question 17

How do bonds and electrons affect shape?

Answer 17

The bonds and electron density causes higher repulsions, causing other bond angles to compress.

Question 18

Multi-Center Molecules

Answer 18

Molecules that does not contain a single central atom.

Question 19

What makes a bond polar covalent?

Answer 19

If the difference in electronegativity between the two atoms in the bond is between 0.4 - 1.8

Question 20

Bond Dipole

Answer 20

Partial charges on the atoms in covalent bond due to electronegativity.

Question 21

How to calculate dipole moment (µ)?

Answer 21

µ = Q x r

Question 22

What does Q stand for in dipole moment?

Answer 22

Q is the magnitude of the partial charge and r is the distance between the charges.

Question 23

How to calculate overall dipole moment for the molecule?

Answer 23

The vectors for each bond in a molecule can be added to find the overall dipole moment for the molecule.

Question 24

What are the factors that affect polarity of of a molecule/compound?

Answer 24

Direction of bonds, and magnitudes of electronegativity. Remember vectors have direction and magnitude.

Question 25

If all terminal atoms are the same and there are no lone pairs on the central atom, the molecule is what?

Answer 25

Always nonpolar

Question 26

If terminal atoms are not all the same, the molecule is what?

Answer 26

Probably polar

Question 27

If there are lone pairs on the central atom, the molecule is what?

Answer 27

Probably polar

Question 28

Molecules with bent, trigonal pyramidal, see-saw, T-shaped or square pyramidal is always what?

Answer 28

Polar

Question 29

Molecules with square planar or linear is what?

Answer 29

Nonpolar if all terminal atoms are the same since all lone pairs and atoms cancel out in 3D structures.