CC13,14,15 - rates, energy, groups and heat changes Flashcards

1
Q

what are group 1 elements known as?

A

alkali metals

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2
Q

properties of group 1

A

one electron in the outer shell
low melting and boiling points
very soft
low density
form ionic compounds

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3
Q

why do group 1 elements get more reactive going down the group?

A
  • atomic radius gets larger
  • less electrostatic attration between nucleus and outermost electron
  • outermost electron is more easily lost (to gain a full outer shell)
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4
Q

what happens when group 1 is reacted with water?

A

reacts vigorously producing hydrogen gas and a hydroxide of the metal
Li, Na, K - move around surface + fizz
K - ignites
Na, K - can melt in the heat of the reaction

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5
Q

saftey regarding reacting group 1 with water

A
  • gloves, goggles, lab coat - protects eyes and clothing , prevents metals reacting w moisture on hands
  • behind screen
  • stand away (spitting)
  • dont touch metal
  • put everything in water to react unreacted metal at end
  • small amount of metal
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6
Q

what are group 7 known as?

A

halogens

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7
Q

properties of halogens?

A
  • 7 electrons in outer shell
  • diatomic, share electrons in a covalent bond
  • melting and bp increase going down group
  • more reactive going up group
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8
Q

describe state and colour of halogens at room temp?

A

Flourine- gas- pale yellow
chlorine- gas- green
bromine - liquid- red/ brown
iodine- grey- soild

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9
Q

explain state of group 7 elements

A

intermolecular forces of attraction get stronger going down the group therefore boiling and melting point increase.

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10
Q

how to test for chlorine

A

hold damp blue litmus paper over it, chlorine will bleach it red then white as chlorine is acidic

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11
Q

why does reactivity of group 7 decrease going down the group

A

need to gain 1 electron for a full outer shell, it is harder for elements further down the group to attract the electron as the outer shell is further from the nucleus therefore theyre less reactive

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12
Q

explain displacement

A

more reactive halogens displace less reactive halogens

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13
Q

what is a hydrogen halide

A

hydrogen and a halogen, when dissolved in water it always forms an acid

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14
Q

what is a redox reaction?

A

reduction - gain of electrons
oxidation - loss of electrons
(when both happen)
OIL RIG

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15
Q

what are group 0 elements known as?

A

noble gases

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16
Q

properties of group 0

A

inert - unreactive, already have a full outer shell of electrons
all gases
bp increases going down group as they get bigger and heavier
density increases going down

17
Q

what needs to happen in order for particles to react?

A

collide with enough energy

18
Q

what are reactants?

A

variables that react

19
Q

what are products?

A

variables that are made

20
Q

ways to speed up a reaction?

A
  • increase acid concentration
  • increase surface area
  • increase temperature
  • use a catlyst
21
Q

how does increasing temp speed up a reaction?

A

particles gain more energy and they can move faster, they collide more often and harder.

22
Q

how does increasing acid concentration speed up a reaction?

A

particles remain w same energy and at same speed but there are more particles per cm3 therefore collisions are more likley and frequent.

23
Q

how does increasing SA speed up a reaction?

A

particles will only collide with the outside of a variable, cant get to the middle. if it is in smaller peices, particles have more area to collide with and there are more collisions per second.

24
Q

what is activation energy?

A

the energy required to break bonds between atoms in reactant molecules

25
Q

what is a catalyst?

A

a substance that speeds up a reaction by lowering the activation energy. doesnt get used up so it can be reused - only a small amount is needed

26
Q

what is exothermic?

A

gives out energy

27
Q

what is endothermic?

A

takes energy in

28
Q

what is a 2 stage reaction?

A

stage 1: break bonds (endo)
stage 2: make new bonds (exo)

29
Q

how do catalysts speed up a reaction?

A
  • provides a different pathway with a lower activation energy
  • more particles exceed this activation energy and undertake successful collisions
  • catalyst increases rate of reaction
30
Q

what do catalytic converters do?

A

reduce pollution by turning harmful gases into less harmful gases

31
Q

why must catalyst be spread thinly over a honeycomb in a catalytic converter?

A

higer SA - more collisions

32
Q

What is a reagent

A

a substance or compound added to a system to cause a chemical reaction, or test if one occurs

33
Q

Examples of exothermic reactions

A
  • displacement reactions
  • precipitation reactions
  • most neutralisation reactions
34
Q

Examples of endothermic reactions

A
  • Ethanoic acid and sodium carbonate
  • dissolving ammonium chloride
35
Q

How to calculate overall energy change

A

Energy required to break bonds - energy released when new bonds are formed

36
Q

What does a positive energy change mean

A

An endothermic reaction

37
Q

What does a negative energy change mean

A

An exothermic reaction