Brainscape's Knowledge GenomeTM

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


See full index

OCR A-Level Chemistry Salters B > Elements of Life > Flashcards

Elements of Life Flashcards

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

What are isotopes

A

Atoms of the same element with a different number of neutrons in the nucleus

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

Relative Atomic Mass = ?

A

(Relative isotopic mass x Relative abundance)/100

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

Speed of light in a vacuum

A

3x10^8 m/s

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

Wavespeed = ?

A

Wavelength x Frequency

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

Energy of a photon = ?

A

Planck constant x Frequency

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

Flame colours of lithium, sodium, potassium, calcium, barium, and copper

A 
Li+ -- Bright red
Na+ -- Yellow
K+ -- Lilac
Ca2+ -- Brick red
Ba2+ -- Apple green
Cu2+ -- Blue green
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The four main points of Bohr’s theory

A
  • Electrons only exist in certain definite energy levels or electron shells
  • A photon of light is emitted when electrons change from one energy level to another
  • The energy of the photon is equal to the different between the two energy levels
  • E = hv
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How many electrons can an orbital hold and how many orbitals per subshell

A

Each orbital can hold two electrons

  • 1 orbital in s sub-shell
  • 3 orbitals in p sub-shell
  • 5 orbitals in d sub-shell
  • 7 orbitals in f sub-shell
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Which elements have a strange electronic structure?

A

Copper and chromium. The 4s orbital contains only one electron rather than two

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

Melting and boiling points across period 3

A

Both melting and boiling points initially increase but fall dramatically after silicon. This means the bonds in phosphorous must be weaker and easier to overcome than those between silicon

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

Covalent bonding

A

A bond in which electrons are shared between atoms

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

Four points needed to answer a shape and bond angle question

A
  • The shape and the bond angle
  • The number of areas of electron density
  • Electrons repel to get as far away as possible
  • Lone pairs repel more than bond pairs
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

2 x bond pairs

A

180 degrees, linear

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

3 x bond pairs

A

120 degrees, trigonal planar

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

4 x bond pairs

A

109.5 degrees, tetrahedral

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

2 x bond pairs, 1 x lone pair

A

107 degrees, bent

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

2 x bond pairs, 2 x lone pairs

A

104.5 degrees, bent

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

3 x bond pairs, 1 x lone pair

A

107 degrees, trigonal pyramidal

19
Q

5 x bond pairs

A

120 degrees and 90 degrees, trigonal bipyramidal

20
Q

4 x bond pairs, 2 lone pairs

A

90 degrees, square planar

21
Q

Moles = ?

A

Mass (g) / Relative Formula Mass (g/mol)

Concentration (mol/dm3) x Volume (dm3) x 1000

22
Q

Water of crystallisation

A

The crystals of some ionic lattices include molecules of water. To remove, heat the substance to a constant mass

23
Q

Percentage yield = ?

A

(Experimental yield / Theoretical yield) x 100

24
Q

Factors which reduce the amount of product produced

A
  • Loss of products from reaction vessels
  • Side reactions occurring, producing unwanted by-products
  • Impurities in the reactants
  • Changes in temperature and pressure
  • If the reaction is an equilibrium system
25
Q

Acid + alkali –>
Acid + base –>
Acid + carbonate –>
Acid + metal –>

A

Salt + water
Salt + water
Salt + water + carbon dioxide
Salt + hydrogen

26
Q

Test for Cu2+

A

Add sodium hydroxide, if present then blue precipitate will form

27
Q

Test for Fe2+

A

Add sodium hydroxide, if present then ‘dirty’ green precipitate will form

28
Q

Test for Fe3+

A

Add sodium hydroxide, if present then orange/brown precipitate will form

29
Q

Test for Pb2+

A

Add potassium iodide, if present then bright yellow precipitate will form

30
Q

Test for Cl-

A

Add silver nitrate, if present then white precipitate will form

31
Q

Test for Br-

A

Add silver nitrate, if present then cream precipitate will form

32
Q

Test for I-

A

Add silver nitrate, if present then yellow precipitate will form

33
Q

Test for SO4 2-

A

Add barium chloride, if present then white precipitate will form

34
Q

Ionic bonding. Melting and boiling point, hardness, electrical conductivity, and solubility

A
  • Occurs between a metal and a non-metal
  • Typically have high melting and boiling points
  • Typically hard
  • Will conduct when molten and dissolved
  • Often soluble in water
  • Insoluble in non-polar solvents
35
Q

Giant covalent lattice. Melting and boiling points, hardness, electrical conductivity, and solubility

A
  • Occurs between two non-metals
  • Very high melting and boiling points
  • Very hard (except for graphite)
  • Do not conduct (except graphite)
  • Insoluble in water
  • Insoluble in non-polar solvents
36
Q

Metallic bonding. Melting and boiling points, hardness, electrical conductivity, and solubility

A
  • Occurs between metals
  • Generally high melting and boiling points (except mercury)
  • Conducts when solid or liquid
  • Insoluble in water
  • Insoluble in non-polar
37
Q

Simple covalent bonding. Melting and boiling points, hardness, electrical conductivity, and solubility

A
  • Low melting and boiling points
  • Soft
  • Do not conduct
  • Usually insoluble in water unless they contain groups which can hydrogen bond
  • Usually soluble in non-polar solvents
38
Q

First ionisation enthalpy

A

The energy needed to remove one electron from every atom in one mole of isolated gaseous atoms of the element

39
Q

Trend in ionisation enthalpy

A
  • Ionisation enthalpy increases across a period
  • Nuclear charge increases across a period which holds the electrons with a stronger force
  • Smaller atomic radii across the period which means electrons are closer to the nucleus
  • Electron shielding would decrease the ionisation enthalpy but not enough to counteract the nuclear charge and atomic radii
40
Q

Group 2 reaction with oxygen

A

Assuming M is the group two element

2M + O2 –> 2MO

41
Q

Group 2 reactions with carbonates

A

Assuming M is the group two element

MCO3 –> MO + CO2

42
Q

Explain the trend in thermal stability down the group 2 carbonates

A

The thermal stability of the group two carbonates increases down the group as the charge density of the cations increases meaning they can polarise the negative charge cloud around the carbonate ion making it less stable and easier to break down

43
Q

Trends down group 2

A
  • Increasing reactivity
  • Increasing thermal stability
  • Increasing pH of hydroxide
  • Increasing solubility of hydroxide
  • Decreasing solubility of carbonates
44
Q

Concentration = ?

A

(1000 x Moles)/Volume

OCR A-Level Chemistry Salters B (10 decks)

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