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Chemistry > Periodic Table And Energy > Flashcards

Periodic Table And Energy Flashcards

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1
Q

How are elements arranged in a periodic table

A

They’re arranged in the order of increasing atomic numbers

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2
Q

What is meant by periodicity

A

Repeating trends in chemical and physical properties

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3
Q

Define first ionisation energy

A

The energy required to remove one electron from each atom in one mole of the gaseous element to form one mole of gaseous 1+ ions

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4
Q

What are the factors that effect ionisation energy

A

Atomic radius
Nuclear charge
Electron shielding of screening

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5
Q

Why does first ionisation energy decrease between group 2 to 3

A

In group 3 outermost electrons are in p orbital whereas in group 2 they’re in s orbital so electrons are easier to remove

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6
Q

Does first ionisation increase or decrease between the end of one period and the start of the next

A

Decrease because
Increase in atomic radius
Increase in electron shielding

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7
Q

Does first ionisation Increase or decrease down a group

A

Decrease because
Shielding increases
Atomic radius increases

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8
Q

What’s the most reactive metal of group 2

A

Barium

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9
Q

3 physical properties of group 2 metals

A

High melting and boiling points
Low density metals
Form colorless compounds

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10
Q

Does reactivity increase or decrease down group 2

A

Increases- electrons are lost more easily because larger atomic radius and more shielding

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11
Q

What are the products when group 2 elements react with water

A

Hydroxide and hydrogen gas

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12
Q

What is oxidised and what is reduced in a reaction between group 2 metal and water

A

Metal- oxidised
Hydrogen from each water - reduced

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13
Q

What is formed when group 2 oxides react with water

A

Metal hydroxide

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14
Q

List 2 properties of halogens

A

Low melting and boiling points
Exist as diatomic molecules

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15
Q

Trend in boiling point down group 7

A

Increases because size of atom increases
More electrons(more London forces)

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16
Q

Trend in reactivity down group 7

A

Decreases because
Atomic radius increases
Electron shielding increases
Ability to gain electron decreases

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17
Q

Define disproportionation

A

The oxidation and reduction of the same element in a redox reaction

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18
Q

Why is chlorine added to drinking water

A

Kills bacteria in the water and makes it safer to drink

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19
Q

How can you test for carbonate Ions

A

Add strong acid to the sample
Collect the gas produced
Pass through lime water

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20
Q

Positive test- carbonate ions

A

Fizzing

Lime water turns cloudy

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21
Q

Test for sulfate ions

A

Dilute hydrochloric acid and barium chlorine to the sample

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21
Q

Test for sulfate ions

A

Dilute hydrochloric acid and barium chlorine to the sample

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22
Q

Positive test- sulfate ions

A

White precipitate

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23
Q

Test for halide ions

A

Dissolve sample in water
Add aqueous silver nitrate
Record colour change
If difficult to distinguish colour add aqueous ammonia
Note solubility

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24
Q

Positive result- halide ions

A

Cl-: white precipitate
Br-: cream precipitate
I-: yellow precipitate

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25
Q

Order or qualitative tests

A

Carbonate,sulfate,halide

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26
Q

Test for ammonium ions

A

Sodium hydroxide and warm
Test gas with red litmus paper

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27
Q

Positive ammonium test

A

Red litmus paper turns blue
Ammonia smells

28
Q

What does a system mean in a chemical reaction

A

The atoms and bonds involved in the chemical reaction

29
Q

Explain the law of conservation

A

The amount of energy I am isolated system remains the same. Energy cannot be destroyed or created if can only be transferred

30
Q

What energy change is breaking bonds associated with

A

Energy is taken in to break bonds- endothermic

31
Q

What energy change is making bonds associated with

A

Energy is released to make bonds- exothermic

32
Q

What is an endothermic reaction

A

A reaction with an overall positive enthalpy change

33
Q

What is an exothermic reaction

A

A reaction with an overall negative enthalpy change

34
Q

What does activation energy mean

A

The minimum energy required for a reaction to take place

35
Q

What are standard conditions

A

100kPa
298K

36
Q

What does in standard state mean

A

The state an element/ compound exists at in standard conditions

37
Q

Define enthalpy change of formation

A

The energy change that takes place when 1 mole of a compound is formed from its constituent elements in their standard state under standard conditions

38
Q

Define enthalpy change of combustion

A

The energy change that takes place when 1 mole of a substance is completely combusted

39
Q

Define enthalpy change of neutralisation

A

The energy change that takes place when 1 mole of water is formed from a neutralisation reaction

40
Q

What does enthalpy change of reaction mean

A

The energy change associated with a given reaction

41
Q

How can you calculate enthalpy change from experimental data

A

Q=mc🔺️T where m is mass of substance being heated c is the specific heat capacity of that substance and 🔺️T is the change in temperature

42
Q

What are the advantages of using a bomb calorimeter

A

Minimises heart loss
Pure oxygen used ensures complete combustion

43
Q

Why might experimental methods for enthalpy determination not be accurate

A

Heat is lost to surroundings
Not in standard conditions
Reaction may not go to completion

44
Q

What does average bond enthalpy mean

A

The mean energy required to break 1 mole of bonds in gaseous molecules

45
Q

How to calculate enthalpy change of reaction using average bonds enthalpies

A

🔺️H=sum of(bond enthalpies of reaction)- sum of (bond enthalpies of products)

46
Q

What is the equation used to calculate rate

A

Rate=change in concentration/ time

47
Q

Unit for rate of reaction

A

Mol dm^-3 s ^-1

48
Q

What must particles do in order to react

A

Collide with sufficient energy and correct orientation

49
Q

Do most collisions result in a reaction

A

No

50
Q

Factors that effect rate of reaction

A

Temperature
Pressure
Concentration
Surface area
Catalyst

51
Q

Affect of temperature on rate

A

Higher proportion of particles have energy greater than the activation energy so more successful collisions

52
Q

Increasing pressure/ concentration on rate

A

More particles in a given volume

53
Q

How to calculate rates from a concentration time graph

A

Draw a tangent
Work out gradient
Change in y/ change in x

54
Q

What is catalyst

A

A substance which increases the rate is reaction but is not used up in the reaction

55
Q

How do catalysts work

A

They provide an alternate reaction pathway so more particles have sufficient energy so increases the reaction rate

56
Q

Homogenous catalyst

A

A catalyst in the save phase as reactants

57
Q

heterogeneous catalyst

A

Catalyst in a different phase to reactants

58
Q

Catalytic convertors

A

Present in vehicles to reduce toxic emissions and prevent photochemical smog

59
Q

Define activation energy

A

Minimum energy needed for a reaction to occur

60
Q

Features of Boltzmann distribution

A

Area under curve=total number of molecules
Curve starts at the origin
Curve does not touch energy axis
Only molecules with energy more than the activation energy can react

61
Q

Dynamic equilibrium

A

Rate of forward reaction equals rate of reverse reaction and concentration of reactants and products remain constant in a closed system

62
Q

What factors effect the position of equilibrium

A

Concentration of reactants/ products
Pressure
Temperature

63
Q

Le Chatelier’s principle

A

If a system at equilibrium is disturbed the equilibrium moves in the direction that tends to reduce the disturbance

64
Q

What effect does a catalyst have on the position of equilibrium

A

No effect

65
Q

What condition effects the value of Kc

A

Temperature

66
Q

What type of system is Kc relevant for

A

Homogenous systems in equilibrium

67
Q

What does Kc mean for the position of equilibrium

A

Greater than one = over to the right
Less than one= to the left

68
Q

Effect of temperature on equilibrium

A

Increase temp= shifts to endothermic reaction

Chemistry (3 decks)

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