Mix stuff to remember

Question 1

Aldehyde

Answer 1

R-CHO)
(-al)

Question 2

Ketone

Answer 2

R-CO-R
(-one)

Question 3

Ether

Answer 3

R-O-R
(Alkoxy-)
(Methoxy-)

Question 4

Esters

Answer 4

R-COO-R
(-oate)

Question 5

Amines

Answer 5

R-NH2
(-amine)
(amino-)

Question 6

Amides

Answer 6

R-CONH2
(-amide)

Question 7

Bromine water

Answer 7

Alkenes react with Bromine water (brown to clear)

Question 8

How to Know if it’s SN1

Answer 8

Tertiary (Positive induction of 3 alkyl groups to spread the charge)
Maybe Secondary

SN1 reactions are favoured by protic polar solvents
Polar protic solvents have O–H or N–H bonds

Question 9

How to Know if it’s SN2

Answer 9

Primary (Tertiary too many bulky attached groups therefore cannot accomodate 5 groups)

Maybe Secondary

SN2 reactions are favoured by aprotic polar solvents
These solvents lack O–H or N–H bonds and are not able to form hydrogen bonds.

Question 10

SN2 vs SN1 states

Answer 10

SN2 has a transition state
SN1 has an intermediate

Question 11

SN2 Diargram (transition state)

Answer 11

Question 12

SN1 Diagram Step 2. (intermediate)

Answer 12

Question 13

SN1 Diagram Step 1. (intermediate)

Answer 13

Question 14

Electrophilic Addition

Answer 14

Question 15

Electrophilic substitution reactions

Answer 15

Question 16

Oxidation Tertiary alcohol

Answer 16

Question 17

Oxidation Secondary alcohol

Answer 17

Question 18

Oxidation Primary alcohol

Answer 18

Question 19

Buffers

Answer 19

Akali buffers are made up of a weak base and a salt which can fully dissociate into the conjugate acid.

Acidic buffers are made up of weak acid and a salt which can fully dissociate into the conjugate base.

Question 20

Halogenatation

Answer 20

Halogenatation is where the hydrogen is replaced by a halogen, a UV light is required to break the initial Cl-Cl bond

Question 21

Naming which side

Answer 21

In alkene the double bond takes priority over the functional group in deciding which side to go from
Saturated carbons have no double or triple bonds

Question 22

k units

Answer 22

The units of k are (mol dm-3sec-1)

Everytime the Overall order increases you divide by (mol dm-3)

Question 23

Arrhenius Equation

Question 24

Breaking bonds (endo/exo)

Answer 24

Endothermic

Question 25

Forming Bonds (endo/exo)

Answer 25

Exothermic

Question 26

Gibbs negative

Answer 26

Spontaneous

Question 27

Gibbs Positive

Answer 27

Non-Spontaneous

Question 28

Conformational isomerism

Answer 28

Question 29

Eclipsed vs Staggered Conformational isomerism

Answer 29

Question 30

cis–trans isomerism

Answer 30

Question 31

EZ

Answer 31

both the highest priority groups are on the same side, therefore, it is the Z-isomer. highest priority groups are on a different side, therefore, it is the E-isomer.

Question 32

Optical isomerism

Answer 32

Question 33

Secondary to Ketone (oxidation)

Answer 33

Question 34

Ketone to Secondary (reduction)

Answer 34

Question 35

Primary to Aldehyde (Oxidation)

Answer 35

Question 36

Aldehyde to Carboxylic (Oxidation)

Answer 36

Question 37

Carboxylic to Ester (Oxidation)

Answer 37

Question 38

Carboxylic to Primary (Reduction)

Answer 38

Question 39

ammonium

Answer 39

(NH4)+

Question 40

Nitrate

Answer 40

(NO3)-

Question 41

Bicarbonate

Answer 41

(HCO3)-

Question 42

Phosphate

Answer 42

(PO4)3-

Question 43

Bent Angle

Answer 43

105

Question 44

Pyramidal

Answer 44

107

Question 45

Tetrahedral

Answer 45

109.5

Question 46

Bronsted Lowry

Answer 46

A Bronsted Lowry acid is a proton donor (it must have a hydrogen ion present) A Bronsted Lowry base is a proton acceptor (it must have a pair of lone electrons to accept the hydrogen)

Question 47

Electrolysis

Answer 47

Inert Electrodes

Question 48

Voltaic Cell

Answer 48

2 Beakers Spontaneous The direction of electron depends on E* Electrons Anode to cathode More reactive metals, such as zinc, have a greater tendency to lose electrons as they are stronger reducing agents.

Question 49

Voltaic Cell Notation

Answer 49

Question 50

HNMR splitting patterns

Answer 50

neighbours + 1

Question 51

Hybridization

Answer 51

sp orbitals are single ponds p orbitals are double and triple bonds

Question 52

Ligand

Answer 52

Lewis base (lone pair donor) forms coordinate bond (dative covalent) with a transition metal ion.

Question 53

Transition metal complex colour

Answer 53

The electron transition between split d orbitals of lower energy to higher energy requires the absorption of specific frequencies of light due to the discrete nature of nuclear energy level. Thus the complementary colour will be observed.

Question 54

Transition metal

Answer 54

Partially filled d orbitals allows for varying amount of oxidation state.

Question 55

Nitration of Benzene

Question 56

Delocalised electrons Compounds

Answer 56

compounds which have resonance structures

Question 57

Lewis Acids and Bases

Answer 57

Lewis Acid Electron pair acceptor Lewis Base Electron pair donator

Question 58

Solubility and Volatility of Hydrocarbons

Answer 58

Stronger intermolecular forces eg. hydrogen bonds means more soluble and less volatile

Question 59

Electrolysis of Dilute NaCl

Answer 59

Oxidation - O2- Reduction - 2H+

Question 60

Electrolysis of Concentrated NaCl

Answer 60

Oxidation - Cl- Reduction - 2H+

Question 61

Melting point of Alkali Halides

Answer 61

Higher Charge = Higher Melting point Lower electron radius = Higher Melting point

Question 62

When do Real Gasses act like Ideal Gasses

Answer 62

Very low Pressure High Temperature

Question 63

Period 3 Oxides Acidity trend

Answer 63

basic to acidic across the period

Question 64

Van der Waals

Answer 64

Umbrella term for Dipole Dipole and London Dispersion Forces

Question 65

London Dispersion

Answer 65

Induced Dipoles Weak

Question 66

Electron Affinity

Answer 66

The first electron affinity is the energy released when one mole of electrons are added to one mole of gaseous atoms to form one mole of gaseous 1− ions

Question 67

Born Haber Cycle

Answer 67

Question 68

Formal Charge Equation

Answer 68

FC = (valence) - (non bonding valence electrons) - (total number of electrons shared in bonds)

Question 69

Formal Charge Rule

Answer 69

Closest to Zero is Favoured FC or everything is Zero (most Favoured)

Question 70

Hunds Rule

Answer 70

Every orbital in a sub level is singly occupied before fully occupied

Question 71

Covalent Bonds

Answer 71

have electronegativity difference of less than 1.8 and more than 0.4 then its a polar covalent bond

Question 72

Allotropes

Answer 72

Allotropes are different physical forms of the same element.

Question 73

Fullerene Hybridisation

Answer 73

sp2

Question 74

Graphine Hybridisation

Answer 74

sp2

Question 75

Titration peak

Answer 75

Draw two Straight Lines

Question 76

Equivalence Point

Answer 76

Very middle of vertical part of pH graph

Question 77

Redox Equation Balance

Answer 77

1. Half Equations 2. Add electrons 3. Hydrogens to balance charge 4. Water to Balance Hydrogen 5. Cancel out electrons in two equations.

Question 78

Electrode Potential Definition

Answer 78

Potential Difference obtained when a half cell is connected to Standard Hydrogen Electrode under standard conditions

Question 79

Redox which reaction occurs

Answer 79

Most Positive occurs Least Positive is reacts

Question 80

Dichromate

Answer 80

Cr2O7^2-

Question 81

Half Equivalence point

Answer 81

pH = pKa of original base/acid

Question 82

Vinegar molecular Formula

Answer 82

CH₃COOH

Question 83

Activity Series

Answer 83

Most Reactive - Most Likely to Oxidise Least Reactive - Most Likely to Reduce

Question 84

Electrolysis E*(direction)

Answer 84

For Reduction Potentials (in data booklet) the most positive reduction potential will happen and the other will reverse.

Question 85

phosphorus(V) oxide

Answer 85

P₄O₁₀

Question 86

Enantiomer

Answer 86

Optical Isomer (mirror)

Question 87

Ionic Structure

Answer 87

lattice structure