Bonding

Question 1

How do you work out what IMF a molecule has ?

Answer 1

If it has O/N/F to H bond it is hydrogen bond
If not is it polar
Yes permanent dipole dipole
No induced dipole dipole

Question 2

What is the formula for hydrogen carbonate ?

Answer 2

HCO3 -

Question 3

What is the formula for carbonate ?

Answer 3

CO3 2-

Question 4

What is the formula hydroxide ?

Answer 4

OH -

Question 5

How do van der waal forces arise ?

Answer 5

There is random movement of electrons in a molecule leads to a uneven distribution of electrons which forms a temporary dipole this induces a temporary dipole on neighboring molecules which causes molecules to attract.

Question 6

How do you work out if a molecule is polar ?

Answer 6

If the central atom is bonded to more than one type of atom e.g. CHCl3
If there is any lone pairs
If either is true then molecule is asymmetrical
Dipoles don’t cancel
Molecule is polar

Question 7

Draw the structure of sodium.

Answer 7

2 rows of 3 +1 ions surrounded be e-

Question 8

Draw NH3 giving bond angle and stating shape.

Answer 8

Use notes

Question 9

Draw BeCl2 giving bond angle and stating shape.

Answer 9

Use notes

Question 10

What is a lattice ?

Answer 10

Regular arrangement of particles.

Question 11

What is the formula for dichromate ?

Answer 11

Cr2O7 2-

Question 12

What is the formula for sulphate ?

Answer 12

SO4 2-

Question 13

Draw SF6 giving bond angle and stating shape.

Answer 13

Use notes

Question 14

What is a ionic bonding ?

Answer 14

ionic bond is strong electrostatic attraction between oppositely charged ions.

Question 15

What is the most electronegative atom and why ?

Answer 15

F
Has low shielding
Has High nuclear charge

Question 16

What are the IMf in CHCl3

Answer 16

Permanent dipole dipole

Question 17

What is a non-polar bond ?

Answer 17

Bond where there is no difference in electronegativity between atoms.

Question 18

Why does electronegativity increase across group 2 ?

Answer 18

Shielding remains the same
Nuclear charge increases
Therefore ability to attract electron in a covalent bond increases

Question 19

What structure do ionic bonds form and draw it.

Answer 19

Giant ionic lattice
3D cube with + and - ions

Question 20

Draw SF4 giving bond angle and stating shape.

Answer 20

Use notes

Question 21

What are the IMF in NH3

Answer 21

Hydrogen bonding

Question 22

What is the formula for phosphate ?

Answer 22

PO4 3-

Question 23

What is a coordinate bond ?

Answer 23

A coordinate bond is a shared pair of electrons which come from the same atom.

Question 24

Draw IF3 giving bond angle and stating shape.

Answer 24

Use notes

Question 25

What is the bonding for simple molecular structure ?

Answer 25

Intermolecular Forces

Question 26

What non-metals form a macromolecular structure ?

Answer 26

Carbon Silicon Silicon dioxide

Question 27

Describe graphite.

Answer 27

Layers of Carbon with 3 covalent bonds Each carbon has a delocalized electron Layers held by weak intermolecular forces conductor High mp

Question 28

Draw ClF5 giving bond angle and stating shape.

Answer 28

Use notes

Question 29

Draw Hydrogen bonding ?

Answer 29

Use notes

Question 30

How does Hydrogen bonding arise ?

Answer 30

Very large difference in electronegativity between H and O/N/F Creates a dipole on O/N/F - H Lone pair on the atom strongly attracts a partially positive hydrogen atom in a different molecule.

Question 31

Draw KrF2 giving bond angle and stating shape.

Answer 31

Use notes

Question 32

what bonds form hydrogen bonds ?

Answer 32

H-F H-O H-N

Question 33

What is the structure of metallic bonding ?

Answer 33

Giant metallic lattice.

Question 34

How do permanent dipole dipole forces arise ?

Answer 34

Difference in electronegativity leads to bond polarity dipoles don't cancel giving a permanent dipole There is attraction between δ- and δ+ in different molecules.

Question 35

What are the three types of intermolecular forces ?

Answer 35

Van der waal/Induced dipole dipole forces Hydrogen bonding permanent dipole dipole forces

Question 36

Draw permanent dipole dipole forces.

Answer 36

use notes

Question 37

What is a coordinate bond represented by ?

Answer 37

A arrow.

Question 38

What does it mean when a atom in a molecule δ-/δ+

Answer 38

It is slightly +/-

Question 39

What is the formula for chlorate (V)

Answer 39

ClO3 -

Question 40

Draw CCl2 giving bond angle and stating shape.

Answer 40

Use notes

Question 41

Draw a dot and cross diagram for oxygen.

Answer 41

each O has 2 lone pairs and 2 bonding pairs which forms a double bond.

Question 42

What is the formula for nitrate (V) ?

Answer 42

NO3 -

Question 43

Is NH3 polar or non-polar and why ?

Answer 43

Polar Carbon is bonded to only H Has one lone pair Molecule is asymmetrical Dipoles don't cancel Molecule is polar

Question 44

What structure do covalent bonds form ?

Answer 44

Simple molecular.

Question 45

Draw XeF4 giving bond angle and stating shape.

Answer 45

Use notes

Question 46

Draw CH4 giving bond angle and stating shape.

Answer 46

Use notes

Question 47

Why is the bonding in magnesium stronger than the bonding in sodium ?

Answer 47

Magnesium has a greater charge of 2+, Mg ions are smaller therefore have a higher charge density meaning the attraction between the delocalized electrons and ions are stronger.

Question 48

What is the formula for nitrate (III) ?

Answer 48

NO2 -

Question 49

Describe diamond.

Answer 49

Tetrahedral structure Very high mp Each carbon has 4 covalent bonds Non-conductor

Question 50

Draw H2O giving bond angle and stating shape.

Answer 50

Use notes

Question 51

What are the properties of ionic compounds ?

Answer 51

High mp conduct electricity only when molten/aqueous Brittle

Question 52

Draw PF5 giving bond angle and stating shape.

Answer 52

Use notes

Question 53

What is a metallic bonding ?

Answer 53

Metallic bonding is strong electrostatic attraction between positive metal ions and a sea of delocalized electrons.

Question 54

What is the formula for ammonium ?

Answer 54

NH4 +

Question 55

Draw a fluorine molecule

Answer 55

Each F has 3 lone pairs and one bonding pair

Question 56

What are the properties of metals ?

Answer 56

Good conductors of heat and electricity due to delocalized electrons. Strong due to Strong electrostatic attraction. Malleable and ductile because layer of ions can slide over each other. High mp and bp due to strong metallic bonds.

Question 57

What is a polar bond ?

Answer 57

Bond between atoms with differences in electronegativity so electrons are distributed towards the more electronegative atom.

Question 58

What is the formula for chlorate(I)

Answer 58

ClO -

Question 59

How are ionic bonds formed ?

Answer 59

Electrons are donated/accepted

Question 60

What is the order of strength in IMf from strongest to weakest ?

Answer 60

Hydrogen bonding ( can be I.D.D if it is a large molecule e.g. I ) permanent dipole dipole induced dipole dipole

Question 61

What is the relationship between MP/BP and strength of IMF ?

Answer 61

Stronger IMF higher BP/MP

Question 62

What is a covalent bond ?

Answer 62

A covalent bond is a shared pair of electrons between two atoms (both non-metals)

Question 63

What are the IMF in BF3 ?

Answer 63

Van der waal

Question 64

What is electronegativity ?

Answer 64

An atoms ability to attract a pair of electrons in a covalent bond.

Question 65

How do you work out if a molecule is non-polar ?

Answer 65

If the central atom is bonded to only one type of atom e.g. CH4 If there is no lone pairs If both are true then molecule is symmetrical Dipoles cancel Molecule is non-polar

Question 66

What is VSEPR ?

Answer 66

To minimise repulsion the electron pairs repel each other as far apart as possible

Question 67

Draw BF3 giving bond angles and stating shape.

Answer 67

Use notes