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Science - continued > Groups in the periodic table > Flashcards

Groups in the periodic table Flashcards

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1
Q

What do the elements in groups and periods share?

A

Chemical and physical properties

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2
Q

What is group 1 called?

A

Alkali metals

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3
Q

What are some chemical properties of alkali metals?

A

They’re malleable and conduct electricity (same as usual metals)

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4
Q

What properties do alkali metals have that make them unique?

A
  • Relatively low melting points

- Soft and easily cut

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5
Q

What is the reactivity of alkali metals?

A

High reactivity and readily form compounds with non-metals

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6
Q

What is the oxidation of alkali metals like?

A

Easily oxidised and burn brightly in air

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7
Q

What is the trend of reactivity in alkali metals?

A

Increases down the group

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8
Q

What are the products of a alkali metal and water reaction?

A

Metal hydroxide (an alkali) and hydrogen

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9
Q

Explain why the reactivity increases down the alkali metals group

A
  • Each element has one electron in its outer shell
  • The period number is how many electron shells the element has
  • The force between the outer electron and nucleus become weaker further down the group due to a larger gap between them
  • The further the outer electron is to the nucleus, the easier it is to lose it to form a compound with another element
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10
Q

What are group 7 elements called

A

The halogens

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11
Q

What are all halogens?

A

Diatomic

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12
Q

Are halogens good or bad conductors of heat and electricity and why?

A

Bad, they’re non-metallic

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13
Q

Why does care need to be taken with halogens

A

They’re all corrosive and toxic

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14
Q

What is the trend for melting, boiling points and densities in halogens

A

They all increase down the group

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15
Q

What is the appearance of chlorine, bromine and iodine?

A

Chlorine- green gas
Bromine- brown liquid
Iodine- purple/brown solid

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16
Q

What do halogens form when reacting with metals?

A

They form salts that contain halide ions

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17
Q

Give some uses of halide salts

A

Sodium chloride- table salts
Sodium fluoride- used in toothpaste
Sodium bromide- used as a disinfectant in pools
Sodium iodide- added in salts to prevent iodine deficiency

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18
Q

What can all halogens be used as?

A

Disinfectants and bleaches - as they kill microorganisms and remove colour

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19
Q

What is the test for chlorine?

A

Damp blue litmus paper dipped in chlorine gas, if it turns red and then bleaches white

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20
Q

What does a reaction between hydrogen and a halide form?

A

A hydrogen halide (u wouldn’t think…) which dissolves in water to form an acidic solution

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21
Q

Give an explanation of the reaction between hydrogen and chloride

A
  • Hydrogen and chlorine molecules collide and the covalent bonds holding the chlorine atoms together breaks
  • The chlorine and hydrogen atoms covalently bond to form hydrogen chloride
  • When the hydrogen chloride is placed in water, the bonds break in Cl- and H+ meaning the solution is now acidic due to the H+
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22
Q

What is the trend in reactivity for halogens?

A

Decrease going down the group

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23
Q

What is a displacement reaction

A

A more reactive element takes the place of a less reactive element in an ionic compound

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24
Q

What can displacement reactions be used for?

A

Finding out the reactivity order in a group

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25
Q

Explain why the reactivity of halogens decreases down the group

A
  • Down the group, the distance between the outermost shell containing electrons and the nucleus increases
  • Meaning the force of attraction between the positive nucleus and the incoming negative electron (gains one electron when reacts) decreases
  • So the ions do not form as readily and reactivity decreases
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26
Q

What is oxidation in terms of electrons?

A

Loss of electrons (OILRIG)

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27
Q

What is reduction in terms of electrons?

A

Gain of electrons (OILRIG)

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28
Q

When do oxidation and reduction occur

A

At the same time in displacement reactions making them redox reactions

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29
Q

Why does oxidation and reduction have to occur at the same time?

A

Because the electrons lost from one element, needs to be gained by another

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30
Q

What are group 0 elements called?

A

Noble gases

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31
Q

Give three properties of noble gases

A
  • colourless
  • very low melting and boiling points
  • poor conductors of electricity and heat
32
Q

What does inert mean and how does this tie in with noble gases?

A

Unreactive, and all of the noble gases are inert

33
Q

What is the trend of density, melting point and boiling point in noble gases

A

They increase down the group

34
Q

Why were noble gases hard to find?

A

Because they don’t react with anything, they exist as single atoms

35
Q

How much of the noble gases are there in our atmosphere?

A

Very minuscule

36
Q

What is Krypton used in?

A

Photography lighting due to its brilliant white light when electricity is passed through it

37
Q

What is Argon used in?

A

It’s denser than air so it’s added to the space above the wine in wine barrels to stop the oxygen in the air from reacting with the wine

38
Q

What is Helium used in?

A

Helium has a very low density and is non-flammable and so is used in weather balloons and airships

39
Q

What is Neon used in and why?

A

Long-lasting illuminated light signs because it produces a distinctive red-orange colour when electricity is passed through it

40
Q

Why are noble gases unreactive?

A

Noble gases are already stable because they already have a full outer shell of electrons and so do not need to gain or lose any to become stable

41
Q

What is the rate of reaction?

A

The rate at which reactants are turned into products

42
Q

How can you control the rate of reactions?

A

Using variables (e.g concentration)

43
Q

What do you need to measure to investigate the reaction rates?

A

How the reactants or products change with time or measuring the mass changes in the reactants or products

44
Q

Why are reaction rates usually the fastest at the beginning of a reaction?

A

That is when the concentration of the reactants is highest

45
Q

How do you know a reaction is faster based on a graph?

A

It will have a steeper gradient

46
Q

Only when can chemical reactions occur?

A

When the reactant particles collide with enough energy to react

47
Q

What is the activation energy

A

The minimum amount of energy needed for a reaction to occur

48
Q

What happens in successful collisions?

A

The activation energy helps to break bonds so the atoms can be rearranged to make new substances (the products)

49
Q

What happens when methane and air mix

A

Nothing until a spark or flame provides the energy for a reaction. The reaction then keeps going until it releases energy, which then provides the activation energy

50
Q

What is an exothermic change

A

A reaction that releases energy

51
Q

What reactions will not continue unless energy is constantly being supplied to it?

A

Endothermic changes

52
Q

In general, when are reaction rates increased?

A

When the energy of the collisions and the frequency (the number of collisions in a certain set of time) increases

53
Q

When do more collisions occur

A

When the particles are closer together and moving faster

54
Q

How does concentration affect reaction rates?

A

Increasing the concentration of the solution increases the rate of reaction because there are more reacting particles in the same volume so collisions are more frequent

55
Q

How does surface area affect reaction rates?

A

Increase the surface area to volume ratio, and the reaction rate increases because there is more surface area for collisions to happen o they’re more often

56
Q

How does gas pressure affect reaction rates?

A

Increasing the gas pressure increases the rate of reaction because the reactant particles are squeezed closer together so collisions are more often

57
Q

How does temperature affect reaction rates?

A

Increasing the temperature increases the reaction rate because the reactant particles speed up and have more energy and so, therefore, collide more often

58
Q

What are catalysts

A

Substances that speed up reaction rates without affecting themselves and altering the products of the reaction

59
Q

Why do catalysts save money in the industry world?

A

They make products faster and allow reactions to occur at a lower temperature

60
Q

Why do catalysts never get replaced?

A

Because they’re never used up

61
Q

What are reaction profiles used for?

A

Comparing catalytic and noncatalytic reactions

62
Q

Why are more collisions successful with a catalyst?

A

Because the catalyst does not actually alter the energy change between the reactants and products, but because less energy is needed to start the reaction, there is more energy and so there are more collisions

63
Q

What catalysts are used in catalytic converters in car exhausts and what do they do?

A

Platinum and palladium - lower the energy needed to convert harmful gases into harmless gases

64
Q

How is an alcohol made?

A

An enzyme in yeast catalyses the reaction of glucose into ethanol and carbon dioxide

65
Q

How does a reaction profile work?

A

Shows the energy change in a reaction. the energy stored in bonds is represented by a horizontal line, the greater the energy stored, the higher the line (refer to a diagram in case it comes up)

66
Q

What happens to the energy in a reaction

A

It is transferred to the surroundings (usually by heating esp in solutions)

67
Q

How would you know if a reaction is exothermic or endothermic

A

Temperature increases in exothermic

Temperature decreases in endothermic

68
Q

What ‘thermic’ is precipitation reactions?

A

Endothermic or exothermic, depending on the substances involved

69
Q

Give two examples of reactions that are always exothermic

A
  • Displacement

- Neutralisation

70
Q

How much activation energy is needed for neutralisation and precipitation reactions?

A

Very little as the reactions start as soon as the reactants are mixed

71
Q

What reaction requires a higher activation energy

A

Combustion reactions

72
Q

What thermic is breaking and making bonds

A

Breaking - endothermic (energy transferred to reactants to break their bonds)
Making- exothermic (energy transferred to surroundings as bonds form)

73
Q

What is bond energy

A

The amount of energy needed to break a particular bond measured in Kilojoules per mole - kJ/mol

74
Q 
What are the bond energies for the following bonds: 
C-O 
C-H
H-H
O-H
O=O
C=O
A 
C-O 358
C-H 413
H-H 436
O-H 464
O=O 498
C=O 805
75
Q

How do you work out bond energy change

A

ITS NOT HARD I PROMISE, YOU JUST NEED TO GO AND SEE ON ACTIVE LEARN PAGE 147 BECAUSE I WONT EXPLAIN IT VERY WELL ON HERE :)

Science - continued (9 decks)

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