Chemical Bonding Chapter 4

Question 1

What does VSEPR stand for

Answer 1

Valence Shell Electron Pair Repulsion Theory

Question 2

A region of space in which there is a high probability of finding an electron

Answer 2

Orbital

Question 3

What is the shape of the p orbital?

Answer 3

Dumbbell

Question 4

What is the shape of the s orbital?

Answer 4

Sphere

Question 5

What is the shape of the d orbital

Answer 5

“Four-leaf Clover”

Question 6

What is the most electronegative element

Answer 6

Fluorine

Question 7

What is the least electronegative element

Answer 7

Francium

Question 8

-They are three-dimensional

-They can contain a maximum of two electrons

-Their shapes are predicted by Schrodinger’s equation

Answer 8

Orbital

Question 9

Substances that are non-conductors and soluble in water
(if not too large)

Answer 9

Molecular Crystals

Question 10

A substance is a solid that is ductile and malleable and conducts electricity and heat in the solid state.

Answer 10

Metal

Question 11

Dissolves in water and conducts electricity when dissolved or in the molten state

Answer 11

Ionic Substance

Question 12

According to VSEPR theory, molecules adjust their shapes to keep what as far apart as possible?

Answer 12

Pairs of valence electron orbitals

Question 13

A partial positive charge at one end of a molecule combined with a partial negative charge at the other end of a molecule

Answer 13

Dipole

Question 14

What causes high surface tension in water?

Answer 14

Hydrogen Bonding

Question 15

Must have this in order to form double and triple bonds

Answer 15

p-orbital

Question 16

Bond type in double and triple bonds only

Answer 16

pi-bond

Question 17

Uneven sharing of electrons

Answer 17

Polar Bond

Question 18

A combination of at least two different orbitals

Answer 18

Hybrid Orbital

Question 19

3-D arrangement of covalent bonds between atoms

Answer 19

Covalent Network

Question 20

Weak forces between all molecules

Answer 20

London Dispersion Forces

Question 21

Attraction associated with the transfer of electrons

Answer 21

Ionic Bond

Question 22

Attraction between polar molecules

Answer 22

Dipole-Dipole Force

Question 23

Any force occurring between molecules

Answer 23

Intermolecular Forces

Question 24

Forces that hold atoms together

Answer 24

Intramolecular Forces

Question 24

A regular repeating pattern of atoms, ions, or molecules

Answer 24

Crystal Lattice

Question 25

If the electronegativity difference is 0 to 0.4 inclusive

Answer 25

Nonpolar Covalent

Question 26

If the electronegativity difference is >0.4 to 1.7 inclusive

Answer 26

Polar Covalent

Question 27

if the electronegativity difference is >1.7 to 4.0 inclusive

Answer 27

Ionic

Question 28

How do you find the bond polarity?

Answer 28

Calculate the electronegativity difference between a bond of a molecule

Question 29

How do you find the polarity of a molecule?

Answer 29

Step 1: find the EN difference between each bond Step 2: does the molecule have only non-polar bonds if so then the molecule is non-polar. If the molecule has polar bonds move to next step Step 3: If the molecule is diatomic(1 bond)then the molecule is polar. If the molecule is polyatomic( more than 1 bond) then move on to step 4 Step 4: If the shape of the molecule is not symmetrical then the molecule is polar. If the shape of the molecule is symmetrical move to step 5 Step 5: if the molecules bonded to the central atom are not the same then the molecule is polar. If the molecules bonded to the central are the same the molecule is non-polar

Question 30

Ionic Crystals properties?

Answer 30

-positive metal and nonmetal ions -primary force of attraction is ionic bonds through electrostatic forces -High boiling and melting points -Conducts electricity when liquid(molten) or dissolved in solution -Does not conduct as a solid -Hard Brittle Solid -Transfer of electrons is necessary to be formed Examples: NaCl MgO CaCO3

Question 31

Metallic Crystals properties?

Answer 31

-Closely packed metal atoms -Mettalix bonding through electrostatic interactions of free moving electrons -Boiling and melting point varies from low to high (mercury and tungsten) - Good conductor of both heat energy and electricity when solid -Sheen: silver and shiny, Malleability & Hardness: Gold is soft and Al is hard -the condition necessary to form is the “electron sea theory” Examples: Au, Al, Cu

Question 32

What causes Metallic Crystals to have properties?

Answer 32

-Sheen: Mobile valence electrons absorb and emit light energy of many wavelengths of light -Malleability: The “electron sea” allows atoms to slide over each other. Electrical conductivity: Mobile valence electrons produce an electric current when a metal is connected to a battery -Hardness: The “electron sea” surrounding the positive nuclei produces strong electrostatic attractions that hold the nuclei together.

Question 33

Molecular Crystal properties?

Answer 33

-molecules create the crystals -Inter molecular forces such as h-bonding, dipole-dipole and LDF are the primary force of attraction -Lower melting points than ionic crystals as IMF are weaker than ionic bonds -Does not conduct well as solid or when dissolved in a solution -Softer than ionic crystals -composed of neutral molecules in order to form Examples: Ice, Dry Ice, Iodine

Question 34

Covalent Network Crystal properties?

Answer 34

-Atoms are involved in creating this crystal -Covalent bonds between the atoms is primary force of attraction -High melting point because of the strong covalent bonds - Does not conduct electricity well as the electrons are unable to move freely. They are also insoluble so can’t dissolve in solutions - Extreme Hardness -Has a interlocking network structure which allows it to form -Examples: Diamond, C

Question 35

What does the polarity of a molecule define?

Answer 35

-surface tension -melting and boiling point temperatures -solubility in certain solvents.

Question 36

How do Polar molecules interact?

Answer 36

Polar molecules interact through intermolecular forces such as hydrogen bonding or dipole-dipole bonding.