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Chemistry Dawes Y12 > Module 3 > Flashcards

Module 3 Flashcards

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1
Q

what is periodicity

A

the repeating pattern seen across different periods

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2
Q

advantages and disadvantages of numbering the groups 1-7

A

+ve group number matches number of electrons in highest energy shell
-ve doesn’t include d-block

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3
Q

advantages of numbering groups 1-18

A

+ve numbers each column in the s, p and d blocks sequentially

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4
Q

what is the s block

A

groups 1 and 2

s-subshells being filled

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5
Q

what is the p block

A

groups 13-18
p-subshells being filled
group 18 are inert as their subshells are filled

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6
Q

what is the d block

A

transition metals

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7
Q

define first ionisation energy

A

energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms

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8
Q

factors affecting ionisation energy

A

atomic radius
nuclear charge
shielding

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9
Q

how does ionisation energy increase across the periodic table

A

from bottom left to top right

from bottom to top, from left to right

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10
Q

what evidence do ionisation energies provide

A

shell structure that supports the Bohr model of the atom

and that subshells fill in a particular order

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11
Q

why does hydrogen have a high 1st ionisation energy

A

as the electron is closest to the nucleus and has no shielding

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12
Q

what is second ionisation energy

A

energy needed to remove 1 electron from each ion In 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions

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13
Q

what happens to melting and boiling points across periods 2, 3 and 17

A

increases from Li to C
increases from Na to Si
increases from F2 to At2

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14
Q

what happens to melting and boiling points as you go down the periodic table

A

decrease

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15
Q

what happens to the atomic radius across a periodic table

A

decreases

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16
Q

what happens to the atomic radius as you go down the periodic table

A

increases

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17
Q

why does reactivity decrease down group 17

A

because its harder for it to attract an extra electron into its outer shell and be reduced to form a 1- ion, due to increased shielding and a larger atomic radius, which decrease the effective nuclear charge

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18
Q

what colour to the halide ions turn when silver nitrate is added

A

cl- white precipitate
br- cream precipitate
I- pale yellow precipitate

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19
Q

what happens to the halide ions when dilute and conc. ammonia are added

A

cl- dissolves in dilute
br- dissolves in conc.
I- insoluble

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20
Q

define disproportionation

A

oxidation and reduction of the same element in a redox reaction

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21
Q

chlorine and water equation

A

Cl2 + H2O –> HClO + HCl

can purify drinking water

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22
Q

chlorine and alkali equation

A

Cl2 + 2NaOH –> NaClO + NaCl + H2O

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23
Q

define enthalpy

A

amount of energy that a substance contains

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24
Q

what is an exothermic reaction

A

gives heat to surroundings

displayed as a -ve enthalpy

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25
Q

what is an endothermic reaction

A

energy being taken in from surroundings

displayed as a +ve enthalpy

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26
Q

what is the equation for energy transferred

A

q=mcΔT

27
Q

define activation energy

A

the minimum energy required for a reaction to take place

28
Q

how to calculate enthalpy of reaction

A

∑(bond enthalpies of reactants) - ∑(bond enthalpies of products)

29
Q

define enthalpy of neutralisation

A

enthalpy change when an acid and alkali react together to form 1 mole of water

30
Q

what is Hess’ law

A

if a reaction can take place by more than one route, the total enthalpy change is the same for each route

31
Q

describe the collision theory

A

particles constantly moving
reactant particles must collide
the particles must have a minimum amount of energy- activation energy- and the correct orientation for the collision to be effective

32
Q

factors that affect rate of reaction

A

concentration (pressure if reactants are gas)
temperature
catalyst
surface area

33
Q

how does concentration affect rate of reaction

A

more particles in a given volume, increasing frequency of successful collisions

34
Q

how can rate of reaction be measured

A

volume of gas produced
mass of reactants
colour change

35
Q

what is a homogenous catalyst

A

is the same physical state as the reactants

36
Q

what is a heterogeneous catalyst

A

different physical state to the reactants

37
Q

benefits of catalysts in terms of sustainability

A

lower temperatures required, so less energy demanded and less combustion of fossil fuels
this reduces CO2 emissions and sustainability is improved

38
Q

factors of the Boltzmann distribution curve

A

total area under the graph represents the total number of molecules
shaded area represents the number of molecules with enough energy to react if they collide

39
Q

what happens to the Boltzmann curve when temperature increases

A

curve gets broader and shaded area increases as more molecules have the activation energy or higher

40
Q

what is dynamic equilibrium

A

reversible reaction where rate of the forward reaction is equal to the rate of the backward reaction

41
Q

what is Le Chatelier’s principle

A

equilibrium shifts in position to favour the forward or backward reaction- opposes change

42
Q

what factors affect the position of equilibrium

A

change in concentration
change in pressure
change in temperature

43
Q

what way does equilibrium shift when pressure is increased

A

to the side with fewer gas molecules

44
Q

what way does equilibrium shift if temperature is increased

A

in the endothermic direction

45
Q

how to calculate equilibrium constant- Kc

A

concentration of products/ concentration of reactants
aA + bB — cC + dD
Kc= [C]c[D]d/[A]a[B]b

[A]= conc of A inn moldm-3
a= number of moles of A
46
Q

what does it mean if the value of K>1

A

the reaction is product-favoured

47
Q

what does it mean if the value of K<1

A

the reaction is reactant-favoured

48
Q

uses of cobalt chloride

A

humidity indicator in weather instruments

cobalt chloride paper tests for the presence of water

49
Q

what do catalysts do

A

provide an alternative route with a lower activation energy

50
Q

name for group 2 elements

A

alkaline earth metals

51
Q

name for group 17 elements

A

halogens

52
Q

standard conditions

A

298k

100KPa

53
Q

what is the atomic radius

A

the distance from the outer shell of electrons to the nucleus of the atom

54
Q

what is shielding

A

number of shells of electrons between the nucleus and outer shell of electrons

55
Q

what is nuclear charge

A

the attraction from the protons in the nucleus with the electrons

56
Q

what is the standard enthalpy change of a reaction

A

the enthalpy change when the amounts shown in the chemical equation react under standard conditions with the reactants and products in their standard states

57
Q

what is the standard enthalpy change of combustion

A

the enthalpy change when 1 mole of the substance completely burns in an excess of oxygen under standard conditions with the reactants and their products in their standard states

58
Q

what is the standard enthalpy change of formation of a compound

A

the enthalpy change when 1 mole of the compound forms from its elements under standard conditions with the elements in their standard states

59
Q

what is bond dissociation enthalpy

A

the enthalpy change on breaking 1 mole of a particular covalent bond in a gaseous molecule

60
Q

as you go down group 2 what happens to solubility

A

it increases

61
Q

which sulphate in group 2 is the most insoluble

A

BaSO4

62
Q

how to test for sulphates

A

add acid and BaCl

63
Q

what detects halogen ions

A

AgNO3

64
Q

what colour do the halogens go when hexane is added

A

Cl2- pale green
Br2- orange
I2- purple

Chemistry Dawes Y12 (4 decks)

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