Bonding

Question 1

Metallic bonding definition

Answer 1

Strong electrostatic attraction of positive metal ion surrounded by sea of delocalised electrons

Question 2

Metallic structure

Answer 2

Giant metallic lattice

Question 3

Comparing strength of metallic bonds
Mg 2+ and Na +
CRAM

Answer 3

MG has a greater charge of 2+
MG has twice as many electrons in sea of delocalised electrons
MG ions are smaller meaning greater charge identity
Therefore, attraction between MG 2 plus and delocalised electrons are stronger

Question 4

Four properties of metals

Answer 4

1. Conductivity.= good and electrical and thermal conductors as a delocalised electrons help transfer energy through metal very efficiently and delocalised electrons can also flow hence metals also good conduct electricity very well
2. Strength of metal= very strong and strong electrostatic attraction between positive metal ions and delocalised electrons
3. Malleable and ductile= metals can be hammered into shape which means they are malleable and can be pulled into wires which means they are ductile because of layers of metal ions can slide past one another
4. Melting point and boiling point= high melting and boiling points because of strength of metallic bonds

Question 5

Covalent bond definition

Answer 5

Shared pair of electrons between two atoms

Question 6

Two types of covalent structures

Answer 6

Macromolecular or simple molecular

Question 7

Three macromolecular structures

Answer 7

C
Si
SiO2
Strong covalent bonds between atoms

Question 8

What is diamond and graphite known as?

Answer 8

AlloTropes as there are different structural forms of the same element

Question 9

Diamond structure

Answer 9

Carbon atoms form 4 covalent bonds
Arrangement is tetrahedral
Very high melting point
Doesn’t conduct a electricity as no free electrons to carry a flow of charge

Question 10

Graphite structure

Answer 10

Layers of carbon atoms forming three covalent bonds
Delocalised electrons between layers
Separate layers are held by a induced dipole forces
Fairly soft as each layer can slide over each other
Conducts electricity due to delocalised electrons
Still has a high melting point

Question 11

Simple molecular structures

Answer 11

They have weak intermolecular forces between molecules

Question 12

Ionic bond definition

Answer 12

Strong electrostatic forces of attraction between oppositely charged ions

Question 13

Physical properties of ionic compounds

Answer 13

1. High melting point on boiling point.
2. Electrical conductivity =. Only when aqueous or molten
3. Structural properties= Tend to be brittle and shatter easily

Question 14

Ammonium formula

Answer 14

NH4 +

Question 15

Hydroxide formula

Answer 15

OH-

Question 16

Nitrate(v) formula

Answer 16

NO3 -

Question 17

Nitrate (III) formula

Answer 17

NO2 -

Question 18

Hydrogen carbonate formula

Answer 18

HCO3 -

Question 19

Chlorate (I) formula

Answer 19

CLO -

Question 20

Chlorate ( V) formula

Answer 20

CLO3-

Question 21

IDE …, instead of ate

Answer 21

No oxygen

Question 22

Carbonate formula

Answer 22

CO3 2-

Question 23

Sulphate formula

Answer 23

SO4 2-

Question 24

Dichromate formula

Answer 24

CR2O7 2-

Question 25

phosphate formula

Answer 25

PO4 3-

Question 26

Silver formula

Answer 26

Ag+

Question 27

Zinc formula

Answer 27

Zn2+

Question 28

Coordinate bond definition

Answer 28

Shared power electron that both come from the same atom

Question 29

Three bonding pairs

Answer 29

Trigonal planar 120

Question 30

Four bonding pairs

Answer 30

Tetrahedral 109.5

Question 31

Five bonding pairs

Answer 31

Trigonal bipyrimidal 90 and 120

Question 32

Six bonding pairs

Answer 32

Octahedral 90

Question 33

One lone pair Two bonding pairs

Answer 33

V - shape 117.5

Question 34

1 lone pair 3 bonding pairs

Answer 34

Pyrimidal 107

Question 35

1 lone pair 4 bonding pairs

Answer 35

See saw 89 119

Question 36

One lone pair Five bonding pairs

Answer 36

Square pyramidal 89

Question 37

Two lone pairs Two bonding pairs

Answer 37

V - shape 104 ,5

Question 38

2 lone pairs 3 bonding pairs

Answer 38

Trigonal planar 115

Question 39

Two lone pairs 4 bonding pairs

Answer 39

Square planar 90

Question 40

Electronegativity

Answer 40

Ability to attract a pair of electrons in a covalent bond

Question 41

What atom is most electronegative?

Answer 41

Fluorine The closer element is the f the more electronegative it is

Question 42

Three factors that affect electronegativity

Answer 42

Distance from nucleus. Shielding. Nuclear charge

Question 43

What does it mean if a molecule is non polar?

Answer 43

Molecule is symmetrical Dipoles cancel out Induced dipole forces of attraction

Question 44

What does it mean if a molecule polar

Answer 44

Molecule is not symmetrical and dipoles don’t cancel out as atoms have different electronegativities Permanent dipole forces of attraction

Question 45

Hydrogen bonding

Answer 45

O-H N-H F-H

Question 46

How does hydrogen bonding arise?

Answer 46

1. Large difference in electronegativity between atoms. ( STATE WHCH ATOMS ) 2. Creates a dipole on the EG O-H BOND ( State the bond ) 3. Lone pair on oxygen atom in one molecule attracted to to partially positive hydrogen atom on another molecule

Question 47

How does permanent dipole-dipole arise?

Answer 47

1. Difference in electronegativity lead to bond polarity. 2. Dips don’t cancel out there for molecule has an overall permanent dipole 3. Attraction between partially positive delta plus on one molecule and partial -delta minus on another

Question 48

How does induced dipole dipole forces arise?

Answer 48

RUTID 1. Random movement of electrons and one molecule lead 2. Uneven distribution of electrons creating a 3. Temporary dipole in one molecule 4. Induce is a dipole in a neighbouring molecule 5. Dipoles a attract All molecules have induced dipole dipole forces of attraction and therefore can be even stronger than permanent if more atoms which means more electrons

Question 49

Points to make sure when drawings hydrogen bonding

Answer 49

1. Make sure it’s in a straight line. 2. Make sure hydrogen bond is labelled 3. Make sure hydrogen bond is in a dashed line 4.Make sure you draw all lone pairs on oxygen 5. Make sure all charge are shown