Unit 6

Question 1

What is the VSEPR theory?

Answer 1

valence shell electron pair repulsion
electrons don’t want to be next to each other

Question 2

what does the VSEPR theory determine

Answer 2

the shape of an atom/molecule

Question 3

when the central atom has unshared electrons, the angles between bonding pairs will be ______ than when all central atom’s electrons are shared

Answer 3

smaller

Question 4

What are electron domains?

Answer 4

the bonding regions which determine the shape

Question 5

which elements are ok with more than 8 valence electrons?

Answer 5

row 3 and below

Question 6

which elements are ok with less than 8 valence electrons?

Answer 6

B and Be

Question 7

double, single, and triple bonds only count as ___ region

Answer 7

1

Question 8

several atomic orbitals mix to form the same total number of equivalent hybrid orbitals whatever you mix you need to get the same number back out

Answer 8

orbital hybridization

Question 9

linear, trigonal planar, tetrahedral, trygonal bipyramidal, and octahedral are all what?

Answer 9

types of hybridization

Question 10

Name, draw electron dot structure, find shape, and hybridization of the following
NBr3
CO2
BF3

Question 11

what makes a molecule nonpolar?

Answer 11

The molecules shape has no lone pairs or if it does it’s either square planar or linear.

Question 12

What are inTRAmolecular forces? And draw a picture of it

Answer 12

attractive forces that occur inside the molecule.

Question 13

What are inTERmolecular forces? And draw a picture of it

Answer 13

attractive forces between two molecules

Question 14

What determines the boiling and melting points of a molecular compounds?

Answer 14

inTERmolecular bond

Question 15

Rank these from strong to weak molecular force
liquids, solids, and gases

Answer 15

solids, liquids, gases

Question 16

The two weakest attractions between molecules are collectively called______. These two forces are _________ _____ and _________ _____.

Answer 16

Vander Waals
dispersion forces
dipole interactions

Question 17

REMEMBER TO PUT BRACKETS ON CHARGED LEWIS DOT STRUCTURES

Question 18

Draw an example of dispersion forces

Question 19

Would a hydrogen molecule with dispersion force or Neon molecule with dispersion force have a stronger pull and higher boiling point

Answer 19

Neon because it has more valence electrons

Question 20

If an atom or molecule has electrons then they are engaging in _______________.

Answer 20

dispersion

Question 21

draw a picture of dipole interactions using H and Cl

Question 22

draw a picture of hydrogen bonding and an example of something that’s not

Question 23

List the substances BaCl2, H2, CO, HF, and Ne in order of increasing boiling points

Answer 23

H2 Ne CO HF BaCl2

Question 24

What are the steps to organizing substances in order of increasing boiling points

Answer 24

find an ionic compound (metal paired with non-metal)
Hydrogen bonding
Dipole (polar bond)
Dispersion (more number of electrons= higher boiling point)