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BMAT Revision > Chemistry > Flashcards

Chemistry Flashcards

1
Q

How do you calculate the retention factor (Rf)?

A

distance travelled by sample / distance travelled by solvent

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2
Q

Describe a displacement reaction

A

Occurs when a react metal is added to a dissolved compound of a less reactive metal.

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3
Q

How can you find the rate of reaction?

A

Measure either the rate at which a reactant is used up
or
the rate at which one of the products is formed.

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4
Q

Describe the process of covalent bonding

A

Occurs when non-metals react with each other by sharing electrons.

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5
Q

What is a mixture?

A

A mixture contains more than one element or compound.

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6
Q

What is a compound?

A

Substance made from different elements bonded together.

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7
Q

Define an element.

A

A substance made from only one type of atom.

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8
Q

Name the following elements:
Br2
Cl2
F2
I2
N2

A

Bromine
Chlorine
Flourine
Iodine
Nitrogen

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9
Q

Name the properties and group of noble gases.

A

Group 18
Unreactive
Low melting/boiling point.
Monoatomic

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10
Q

Describe an endothermic reaction.

A

A reaction which takes in heat from its surrounding, the products have more energy than the reactants.

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11
Q

Describe an exothermic reaction.

A

A reaction which gives off heat to its surrounding. Products have less energy than the reactants.

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12
Q

Name factors affecting the rates of reaction.

A

Concentration
Temperature
Surface area
Catalysts

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13
Q

What elements are in group 1?

A

Alkali metals with 1 electron in outer shell.

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14
Q

What elements are in group 2?

A

Alkaline earth metals with 2 electrons in outer shell.

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15
Q

Name the parts of the atomic structure

A

Nucleus
Shells
Electrons

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16
Q

What is the mass number of an element?

A

The mass number is the number of protons and neutrons in an atom.

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17
Q

What is the atomic number of an element?

A

The number of protons in the nucleus.

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18
Q

How would you find the number of electrons in an element?

A

You would look at the number of protons.
The number of protons is the same as the number of electrons.

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19
Q

Why do reactions happen quicker at higher concentrations?

A

Because there is a greater number of particles to collide, making for more successful collisions.

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20
Q

What is a catalyst?

A

It is a substance that affects the rate of reaction without being used up in the reaction itself.

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21
Q

What are bond energies

A

Bond energies are a measure of the average bond strength for a particular covalent bond.

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22
Q

Describe the process of electrolysis

A

The process where a molten ionic substance is decomposed by an electrical current.

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23
Q

What are the relative atomic masses and charges of subatomic particles?

A

Protons 1 mass / +1 charge
Neutrons 1 mass / 0 charge
Electrons negligible / -1 charge

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24
Q

What are some properties of giant covalent bonds?

A

High melting/boiling point
Graphite conducts electricity
diamond and silicon is very hard.

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25
Q

What do amino acids consist of?

A

Carboxyl group -COOH
Amino group NH2
Organic R group

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26
Q

What are the key features of polymerisation?

A

Small reactant alkene molecules are unsaturated called monomers.
The large product molecule is saturated called a polymer.

27
Q

Define a base.

A

A base is a substance that can accept H+ ions or the ability to form OH-.
Sometimes called alkalis

28
Q

Describe the process of ionic bonding

A

Occurs when a metal reacts with a non-metal.
Metals lose electrons and non-metals gain electrons.
Creating an ionic bond.

29
Q

Describe the properties of ionic compounds.

A

Solids at room temperature.
Strong overall attraction.
Do not conduct electricity.
Many compounds dissolve in water.

30
Q

Define an acid.

A

An acid is a substance which has the ability to donate H+ ions.

31
Q

Define activation energy.

A

The minimum amount of energy for particles to successfully react upon collision.

32
Q

How do you calculate the % composition by mass of a compound.

A

Number of atoms of compounds / Mr of compound.

33
Q

How to calculate number of moles of a molecule?

A

Mass / Molar mass

Mass must always be in grams.

34
Q

What is Avogadro’s constant?

A

It gives the number of particles in 1 mole.
value of 6.022x10^23

35
Q

Describe the properties of halogens.

A

Group 17
Non-metals
Poor conductors
Low melting/boiling point.

36
Q

Define hydrocarbons.

A

Compounds which consist of only hydrogen and carbon.

37
Q

Give some examples of hydrocarbons.

A

Ethene
Butane
Methane
Octane

38
Q

What ions are attracted to the cathode during electrolysis?

A

+ ions are attracted to the cathode which gains electrons.

39
Q

What ions are attracted to the anode during electrolysis?

A

-Ions are attracted to the anode which loses electrons.

40
Q

What are some physical properties of group 1 alkali metals?

A

Shiny solids at room temp
Low melting/boiling point
Soft metals
Good conductors

41
Q

How would you calculate the percentage yield?

A

Actual yield / predicted yield * 100

42
Q

What is an alloy?

A

An alloy is two or more metals mixed together to combine properties.

43
Q

What do proteins consist of?

A

Proteins are formed from long chains of amino acids, joined by amino linkages.

44
Q

What are the chemical properties of group 1 alkali metals?

A

Very reactive with oxygen/water.
react with non-metals to form ionic compounds.

45
Q

What are alkanes?

A

Series of hydrocarbons with no functional group.
Methane and ethane.

46
Q

What are the limitations of bond energies?

A

Just an average value so not specific.
Can only be calculated for reactions in a gaseous state,

47
Q

How do you calculate enthalpy change?

A

Sum of energy in - sum of energy out.

48
Q

What’s a key point to remember of distillation?

A

The particles are closer/further away from each other depending on which state the solution is in.

49
Q

What is dentrification?

A

The conversion of nitrates into nitrogen gas.

50
Q

What are alcohols?

A

Homologous compounds that contain hydroxyl group.

51
Q

What do alkenes have at least one off?

A

There is at least one carbon to carbon double bond.

52
Q

What are the three main types of extractions of metals from ores?

A

Reduction with carbon.
Molten by electrolysis
Reduction of ore with a more reactive metal.

53
Q

Name the following formulae:
HCL
HNO3
H2SO4
CH3COOH

A

Hydrochloric acid
Nitric acid
Sulfuric acid
Ethanoic acid

54
Q

Describe collision theory.

A

For two particles to collide, they must collide at the correct orientation and have sufficient energy.

55
Q

What is enthalpy change?

A

it is the amount of heat given out or taken in during a reaction carried out.

56
Q

Name the following formulae:
NH3
CO2
CO
NO2
SO3

A

Ammonia
Carbon dioxide
Carbon monoxide
Nitrogen dioxide
Sulphur trioxide

57
Q

Name the properties of hydrogen.

A

An element
Produced when metal reacts with water/alcohol.
Burns with a pop when ignited.

58
Q

Name the properties of oxygen.

A

Testing oxygen - glowing split will relight.
It is an element.

59
Q

Why do reactions happen quicker at higher temperatures?

A

The particles will have more kinetic energy so more frequent successful collisions.

60
Q

What are some characteristics of carbon dioxide?

A

Testing - extinguishes a lit splint.
Limewater turns cloudy in presence of CO2.

61
Q

How would you test for carbonate ions.

A

This can be tested using limewater which turns cloudy in presence of CO2.

62
Q

How would you test for halide ions?

A

It will react with silver if there are halide ions present.

63
Q

What are the distinct colours of each silver halide participate?

A

Sliver iode goes Yellow
Silver chloride goes white
Silver bromide goes cream

64
Q

What’s the specific order you test for unknown ions?

A

1st - carbonates with dilute acid
2nd - presence of sulphate ions
3rd - halide ions using silver.

BMAT Revision (3 decks)

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