Chapter 5-6 - Electrons and bonding & Shapes of molecules and intermolecular forces

Question 1

Define ionic bonding

Answer 1

the strong electrostatic attraction between oppositely charged ions

Question 2

can giant ionic lattices conduct electricity when solid?

Answer 2

No, ions are fixed in a lattice

Question 3

can giant ionic lattices conduct electricity when liquid/molten?

Answer 3

Yes, ions are mobile

Question 4

can giant ionic lattices conduct electricity when aqueous/dissolved?

Answer 4

Yes, ions are mobile

Question 5

Boiling points of ionic materials

Answer 5

High, lots of energy required to overcome the strong eletroststic attraction between the oppositely charged ions.

Question 6

Are ionic materials soluble?

Answer 6

Yes, Polar water molecules break apart the ionic lattice

Question 7

Define metallic bonding

Answer 7

The strong electrostatic attraction between cations (positive metal ions) and delocalised electrons

Question 8

can giant metallic lattices conduct electricity when solid?

Answer 8

Yes, delocalised electrons are free to move and carry charge

Question 9

can giant metallic lattices conduct electricity when liquid/molten?

Answer 9

Yes, delocalised electrons are free to move and carry charge

Question 10

Boiling points of metals

Answer 10

High, lots of energy required to overcome the strong electrostatic attraction between cations and delocalised electrons

Question 11

Are metals soluble?

Answer 11

Insoluble in water

Question 12

Define covalent bond

Answer 12

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

Question 13

Define dative covalent bond

Answer 13

A covalent bond where both of the electrons are donated by only one of the bonded atoms.

Question 14

can simple molecular structures conduct electricity?

Answer 14

No

Question 15

can giant covalent structures conduct electricity?

Answer 15

mostly no as no mobile charge carriers

Question 16

what are exceptions of giant covlent structures that can conduct electricty

Answer 16

graphite (contains free electrons) and silicon is a semi-conductor

Question 17

Boiling points of simple molecular structures

Answer 17

Low, intermolecular forces easily overcome

Question 18

Boiling points of giant covalent structures

Answer 18

High, lots of strong covalent bonds

Question 19

are simple molecular structures soluble?

Answer 19

depends on the structure

Question 20

are giant covalent structures soluble?

Answer 20

insoluble in water

Question 21

the 2 anomalous properties of ice

Answer 21

• high MP due to london forces and hydrogen bonds require a lot of energy to overcome
• less dense than water as hydrogen bonds cause it to have an open lattice (water molecules sit father apart)

Question 22

Define London force

Answer 22

weak attraction force between an instantaneous dipole and an induced dipole in a different molecule

Question 23

Define Permenant dipole-dipole force

Answer 23

Attractive force between permanent dipoles in neighbouring molecules

Question 24

Define Hydrogen Bonding

Answer 24

A strong dipole-dipole attraction between an electron deficient hydrogen atom and a lone pair of electrons on a highly electronegative atom on a different molecule

Question 25

Define Electronegativity

Answer 25

The ability of an atom to attract the electrons in a covalent bond

Question 26

Define a polar molecule

Answer 26

A covalent bond *(or asymmetrical molecule)* where the electron density is shifted more towards one side

Question 27

Define Permanent Dipole

Answer 27

A small charge difference across a bond caused by a difference in electronegativity in the bonded atoms

Question 28

Linear bond angle

Answer 28

180 degrees

Question 29

Trigonal Planar bond angle

Answer 29

120 degrees

Question 30

Non-linear bond angle

Answer 30

104.5 degrees

Question 31

Tetrahedral bond angle

Answer 31

109.5 degrees

Question 32

Trigonal Pyramidal bond angle

Answer 32

107 degrees

Question 33

Trigonal Bipyramidal bond angle

Answer 33

120 degrees & 90 degrees

Question 34

4 bonds, no lone pairs

Answer 34

tetrahedral - 109.5

Question 35

3 bonds, 1 lone pair

Answer 35

pyramidal - 107

Question 36

2 bonds, 2 lone pairs

Answer 36

non-linear 104.5

Question 37

2 bonds, no lone pairs

Answer 37

linear 180

Question 38

3 bonds, no lone pairs

Answer 38

trigonal planar - 120

Question 39

6 bonds, no lone pairs

Answer 39

octahedral 90