Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Edexcel > 4th Form > Flashcards

4th Form Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Why do high surface area increase rate of reaction?

A

More of the solid is exposed to the other particles
So there are more particles per unit volume
So the collision frequency is higher
So there are more successful collisions per unit time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why does a higher concentration increase rate of reaction?

A

There are more particles per unit volume
So the collision frequency is higher
So there are more successful collisions per unit time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Why does a higher temp increase rate of reaction?

A

The particles have more kinetic energy
So the percentage of collisions with energy above activation energy is higher
So there are more successful collisions per unit time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why does a catalyst increase rate of reaction?

A

They provide an alternative route with a lower activation energy
So the percentage of collisions with energy above activation energy is higher
So there are more successful collisions per unit time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define covalent bonding

A

The electrostatic attraction between protons in two nuclei and a shared pair of electrons between them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why do simple molecular covalent substances boil easily?

A

Although simple molecules contain very strong covalent bonds, there are also weak intermolecular forces (IMFs) between the molecules.
When simple molecular substances boil, it’s the weak IMFs which break

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why can a simple molecular substance not condunt electricity?

A

Electrical conductivity requires charged particles that can move freely
But in a simple molecular substance, there aren’t any charged particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Why does diamond have a high melting point?

A

Covalent bonds are very strong
There are lots of bonds in the giant lattice
Lots of energy is required to break all the bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why can diamond not conduct electricity, but graphite can, since they are both types of carbon?

A

Diamond cannot conduct electricity, as there are no free moving charged particles, as all the electrons are stuck inside an atom or a bond. Graphite has free moving charged particles between the layers, so it can.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Name the structure and essential properties of an ionic bond.

A

Giant lattice
High mp/bp
Insulator when solid
Conductor when liquid
Conductor when in an aqeous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Name the structure and essential properties of a convalent bond.

A

Simple molecular substance
Low mp/bp
insulator

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Name the structure and essential properties of a metallic bond

A

Giant lattice
High mp/bp
Conductor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens when halogens (group 7) react with metals?

A

Form ionic compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why is it harder for halogens lower down the group to bond?

A

Atoms have more electron shells
The extra electron is further from the nucleus
So its attraction to the nucleus is weaker
(Harder for the atom to pull in an extra electron.)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Chlorine test

A

Damp blue litmus paper → turns white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

As you go down in groups halogens get ……. …………..
As you go down in groups noble gases get ……. …………

A

Less reactive
More reactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How to calculate RFM?

A

By adding the relative atomic masses (RAMs) of the atoms or ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How to find percentage by mass of an element in a compound?

A

(Mass of element/RFM)x100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

equation for moles

A

mass/RFM

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

table to calculate moles:

A

Element 1 Element 2
Mass:
RFM:
Moles:
Ratio:

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How to calculate mole ratio in a formula?

A

Only look at big numbers: eg
2Na+S
If you were asked to find the mole ratio of Na to S, it would be 2:1 respectivly

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Describe a metallic structure

A

A sea of delocalised electrons
A lattice of positive metal ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

How can metals conduct electricity?

A

Delocalised electrons can pass through the lattice

24
Q

Define metallic bonding

A

The electrostatic attraction between the positive metal ions and the negative delcalised electrons.

25
Q

Table of reactivity

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper

26
Q

Structure of Diamond

A

Every carbon makes 4 covalent bonds
Tetrahedral

27
Q

Structure of graphite

A

Layers of Carbon
Every carbon makes 3 covalent bonds
Weak inter molecular forces between layers
Delocalised electrons between layers

28
Q

Isotope definition

A

Atoms of the same element with different numbers of neutrons

29
Q

What colour change occurs when copper carbonate is heated

A

Green to black

30
Q

Discuss the differences between diamond and graphite. Refer to bonding,structure, electrical conductivity, and hardness.

A

Diamond (structure):
Tetrahedral structure
Graphite (structure)
Hexagonal structure made up of layers
Diamond (conductivity)
Diamond does not conduct electricity (1)
Because it has no delocalised electrons (1)
Graphite (hardness)
Graphite is malleable (1)
Because it has layers that can slide over each other (1)

31
Q

Why does C60 fullerene have a much lower melting point than diamond and graphite

A

C60 fullerene has weak intermolecular forces
which are easily overcome
whereas diamond has strong covalent bonds
which require lots of energy to overcome

32
Q

What obervations would you see when magnesium reacts to form magnesium oxide

A

bright white light
effervesence

33
Q

chromatography experiment

A
  1. Draw a start line in pencil near the bottom of the paper
  2. Place the samples on the start line
  3. Put the paper in the beaker with the start line above the water level
  4. Mark the solvent front
34
Q

HCL Formula, name of Salt, Anion formula

A

HCL, Chloride Cl-

35
Q

Nitic Formula, name of salt, and Anion Formula

A

HNO3, Nitrate, No3-

36
Q

Sulphuric formula, name of Salt, and Anion formula

A

H2So4, Sulphate, So4-

37
Q

Ethanoic formula, name of salt and Anion formula

A

CH3COOH, Ethanate, Ch3COO

38
Q

Sodium Hydroxide

A

NaOh

39
Q

Potassium hydroxide

A

KOH

40
Q

Ammonium Hydroxide

A

NH4OH

41
Q

Molecular and structural formula of Methane

A

CH4, CH4

42
Q

Molecular and structural formula of Ethane

A

C2H6, CH3CH3

43
Q

Propane molecular formula and structural formula

A

C3H8, CH3CH2CH3

44
Q

Butane Molecular formula and structural formula

A

C4H10,CH3CH2CH2CH3

45
Q

Pentane

A

C5H12,CH3CH2CH2CH2CH3

46
Q

Define homologous series

A

a collection of compounds with the same general formula that only changes with the Carbon chain lengh.

47
Q

List the order for Cracking

A

refinery gases
gasoline
kerosene
diesel
bitumen
fuel oil

48
Q

What is the catalyist in cracking reactions

A

aluminium Dioxide

49
Q

What temperature is cracking performed at

A

650 degrees C

50
Q

Give the general formula for alkanes

A

CnH2n

51
Q

use of kerosene

A

jet fuel

52
Q

use of bitumen

A

road surfacing

53
Q

give a reason for the importance of a catalytic cracking reaction

A

shorter chain molecules are in higher demand (eg for petrol)

54
Q

unsautrated in alkenes meaning

A

they contain a double carbon bond

55
Q

test for unsaturation

A

bromine water turns from orange to colorless

56
Q

Ammonium test

A

Add NaOH
Damp red litmus paper will turn blue

Chemistry Edexcel (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions