Bonding

Question 1

Atom

Answer 1

Smallest particle that characterizes a chemical element

Question 2

Octet Rule

Answer 2

When bonds form between atoms, the atoms gain, lose, or share electrons in a way that they create outer energy levels w/ 8 electrons

Question 3

Bonding occurs when….where….why…

Answer 3

Valence electrons are shared or transferred at the highest energy level to make it more stable
- Electrons in lower energy lvls are not involved w/ bonding

Question 4

Define orbitals

Answer 4

Space around an atoms nucleus where an electron may exist

Question 5

Define Valence Orbitals

Answer 5

Volume of space that can be occupied by electrons in atoms highest energy lvl (outer layer)

Question 6

Define Bonding Electrons

Answer 6

Un-paired electrons that can be shared w/ other atoms

Question 7

Define Lone Pair

Answer 7

Two electrons occupying same orbital

Question 8

Define Valence Electrons

Answer 8

Electrons in highest energy lvl in atom

Question 9

Define Ionic Bond

Answer 9

Attraction between pos. and neg. ions resulting in transfer of one or more valence electrons

Question 10

Define Covalent Bond

Answer 10

Two or more electrons are shared among the atoms

Question 11

Which bond is stronger, (covalent or ionic)

Answer 11

Ionic is stronger

Question 12

Define Electronegativity

Answer 12

Ability of atom to attract pair of bonding electrons in valance lvl
- Increase as you go up or right of the periodic table

Question 13

Define Non-polar Molecule

Answer 13

A molecule w/ symmetrical electron distribution

NOTE: Hydrocarbons are always non-polar

Question 14

Define Polar Molecule

Answer 14

Molecule in which negative charges are not distributed symmetrically among atoms causing partial negative and partial positive charge on both sides of atom

Question 15

Electronegativity for ionic compound

Answer 15

Difference in electronegativities is usually greater than 1.7 causing electrons to be transferred.

Question 16

Difference in Electronegativity (DEN)

Answer 16

DEN = 0 - Nonpolar covalent bond
DEN between 0.1-1.7 - Polar Covalent bond
DEN between 1.7-4 - Ionic bond

Question 17

Bond Dipole

Answer 17

When arrow points towards more electronegativity end of compound

Question 18

Define Intramolecular Forces

Answer 18

• Forces within the molecule

- Responsible for physical behaviour of molecule substance

Question 19

What are the two types of intramolecular forces?

Answer 19

1. Ionic Bonds: within crystal lattice

2. Covalent Bonds: within a molecule

Question 20

Define Intermolecular Forces

Answer 20

• Forces between molecules
• Responsible for physical properties in molecules
• Present between covalent compunds

Question 21

Types of Intermolecular Forces

Answer 21

1. Van der Waals Forces
   - London Dispersion Forces
   - Dipole-Dipole Forces
2. Hydrogen Bonding

Question 22

London Dispersion Forces

Answer 22

• Always present between all molecules, does not matter if there are different attractions
• Any electron movement within molecule can produce momentary dipole
• Force gets stronger as # of electrons in molecule increases
• More electrons = more LDF

Question 23

Relationship between Boiling point and Intermolecular bonds

Answer 23

• Stronger LDF = greater strength of intermolecular forces

- Greater strength of intermolecular forces = higher BP of substance

Question 24

Dipole - Dipole Forces

Answer 24

• Exist between polar bonds ONLY

- Strength of Dipole force is dependent on overall polarity, more polar = greater DD force

Question 25

Hydrogen Bonding

Answer 25

- Strongest intermolecular force - Only occurs when hydrogen bonds to: Oxygen, Nitrogen, or Fluorine - Must have at least one lone pair

Question 26

Intermolecular forces of non-polar molecule, polar molecule, and polar molecule w/ H bonded w/ N,O, F

Answer 26

Non-polar = LDF Polar = LDF, DD Polar w/ H bonded N,O, F = LDF, DD, HB

Question 27

List the strengths of attractions for intermolecular and intramolecular forces (weakest to strongest)

Answer 27

1. LDF 2. DD 3. HB 4. Covalent Compounds 5. Ionic compunds

Question 28

What does VSEPR stand for

Answer 28

Valence Shell Electron Pair Repulsion Theory

Question 29

Shape of AXE3 and polarity

Answer 29

- Linear - 2 Atoms are the same = non polar - 2 atoms are different = polar

Question 30

Shape of AX2 and polarity

Answer 30

- Linear - Peripheral atoms are same = non polar - Peripheral atoms are different = polar

Question 31

Shape of AX2E2 and polarity

Answer 31

- V- shaped | - Central atom has lone pairs = polar

Question 32

Shape of AX3E and polarity

Answer 32

- Trigonal Pyramidal | - Central atom has lone pairs= polar

Question 33

Shape of AX4 and polarity

Answer 33

- Tetrahedral - Peripheral atoms are same = non polar - Peripheral atoms are different = polar

Question 34

Shape of AX3 and polarity

Answer 34

- Trigonal Planar - Peripheral atoms are same = non polar - Peripheral atoms are different = polar