Promos

Question 1

Formula for deflection

Question 2

Definition of orbital

Question 3

How to draw s, p, and d orbitals

Question 4

Exceptions to Aufbau’s Principle

Question 5

Factors affecting IE

Question 6

General trend across a period + exceptions

Question 7

General trend down a group

Question 8

General trend of successive IE

Question 9

Definition of Metallic, Covalent and Ionic bonds

Question 10

Factors affecting metallic bonds

Question 11

Arrangement of ions in ionic lattice

Question 12

Factors affecting ionic bond.

Question 13

How to atoms in Period 3 or higher accommodate more than 8 valence electrons

Question 14

Sigma vs Pi bonds, and which is stronger

Question 15

Factors affecting covalent bond

Question 16

Description of Silicon (IV) Oxide and Diamond

Answer 16

Diamond has a giant covalent (lattice) structure as it has a tetrahedral arrangement of atoms extensively held together by strong electrostatic forces of attraction b/w nuclei of each carbon atom and its shared electron pair.

Question 17

Description of Graphite

Answer 17

Each carbon atom in the layer is bonded to three other carbon atoms via strong covalent bonds, forming a hexagonal arrangement of carbon atoms. The fourth valence electron of each carbon atom is delocalised in b/w the layers. Layers are held together by weak id-id forces.

Question 18

VSEPR Theory BP-LP

Question 19

Effect of electronegativities of central/non-central atoms on bond angle

Question 20

Factors affecting pd-pd

Question 21

How id-id interactions come about

Answer 21

At any moment in time, due to electrons continuously moving, there is a temporary distortion in the electron cloud of the molecule, giving rise to an instantaneous dipole in the molecule. This then induces a dipole in the neighboring molecule. Thus molecules are held together by the id-id interactions b/w them.

Question 22

Factors affecting id-id

Question 23

Definition of Hydrogen bonds and factor affecting its strength (know how to draw H bonds)

Question 24

Ionic molecules with covalent character formation

Answer 24

Cation has high charge density, highly polarising
Anion has large electron cloud, highly polarizable
Distortion of electron cloud of anion, electron density may be shared between anion and cation, thus giving the molecule covalent character. Extent to sharing of electrons equal to extent of covalent character.

Question 25

How does solubility work

Answer 25

Energy released from forming favourable interactions b/w solute and solvent molecules is able to compensate for energy needed to overcome existing interactions b/w solute particles

Question 26

Definition of Ion-Dipole interactions

Answer 26

Electrostatic forces of attraction between charged ions in a ionic compound and oppositely charged dipoles of polar molecules in solvent.

Question 27

Solubility of giant and simple covalent structures

Question 28

Assumptions of Ideal Gas (three)

Answer 28

Size of gas particles is negligible compared to size of the container Negligible intermolecular forces exerted by gas particles on one another Average kinetic energy of gas particles is directly proportional to absolute temperature

Question 29

Daltons Law of partial pressure

Answer 29

The total pressure in a mixture of non reacting gases is the sum of partial pressures exerted by the constituent gases.

Question 30

Factors affecting deviation from Ideal gas behavior (four)

Question 31

(Optional) Definition of enthalpy change of atomisation

Answer 31

Enthalpy change when one mole of gaseous atoms is formed from the element in its standard state under standard conditions

Question 32

(optional) Definition of enthalpy change of formation

Answer 32

Enthalpy change when one mole of substance is formed from its constituent elements in their standard states under standard conditions

Question 33

(optional) Enthalpy change of combustion

Answer 33

Enthalpy change when one mole of a substance is completely burnt in oxygen under standard conditions

Question 34

(optional) IE definition

Answer 34

Enthalpy change when one mole of electrons is removed from one mole of gaseous atom/singly charged cation

Question 35

(optional) EA definition

Answer 35

Enthalpy change when one mole of gaseous atom/singly charged anion accepts one mole of electrons

Question 36

Why is first EA is negative and second EA is positive

Answer 36

- Attraction of electron = negative EA Energy is needed to overcome repulsion b/w anion and electron to be added as both are negative.

Question 37

(optional) BE

Answer 37

Average enthalpy change when one mole of covalent bonds between atoms of gaseous molecules is broken

Question 38

(optional) H of neutralization

Answer 38

Enthalpy change when one mole of water is formed from the reaction of an acid and alkali under standard conditions

Question 39

(optional) H of hydration

Answer 39

Enthalpy change when one mole of gaseous ions is hydrated under standard conditions

Question 40

(optional) H of solution

Answer 40

Enthalpy change when one mole of a substance is completely dissolved to give an infinitely dilute solution under SC, such that there is no further enthalpy change when more solvent is added.

Question 41

Formula for H of solution

Question 42

Why spontaneous reaction does not mean reaction will actually take

Answer 42

Might not be kinetically favorable as there could be a very high Ea that prevents reaction from proceeding at a reasonable rate.

Question 43

Definition of dynamic eqm

Question 44

LCP

Question 45

Effect of change in conc, pressure (volume), temperature, catalyst

Question 46

Factors affecting ROR (know how to draw maxwell curve)

Question 47

Definition of catalyst

Question 48

Characteristics of catalyst (three)

Question 49

Mode of action of heterogeneous catalyst

Question 50

Common Ion effect

Answer 50

Due to a common ion in the solution, POE shift left and backward rxn is favored, thus reducing the solubility of the salt (sparingly soluble)

Question 51

Complex Ion effect

Answer 51

Due to addition of a complex ion that reacts with a product of the reaction, the conc of the product decreases, thus IP

Question 52

Conditions for enantiomers to form and definition

Question 53

Enantiomer pair and how it affects plane polarised light

Question 54

Idea of stability of a radical/carbocation

Question 55

Why is trans-isomer more stable than cis-isomer

Question 56

Why cis-isomer has higher bp than trans-isomer

Question 57

Why cis-isomer has lower mp than trans-isomer

Answer 57

Cis-isomer has lower symmetry, does not pack as well into a crystalline solid compared to trans-isomer. As a result, there is less extensive intermolecular forces and thus less energy is needed to melt the solid.

Question 58

Name of the four main reactions

Question 59

Reagent and conditions for each sub-reaction

Answer 59

excess conc h2so4, heat ethanolic naoh, heat under reflux Ni catalyst, heat, H2 room temp, Br2 in CCl4 H3PO4, heat at high pressure excess conc h2so4, then heat with water cold Kmno4 (aq), dilute Naoh hot KmO4 (aq) with dilute h2so4

Question 60

Why are alkanes generally unreactive

Question 61

Factors for similarity and differences b/w orbitals

Answer 61

size, shape, energy level, distance from nucleus, electrons cant be found in center at centre of orbital