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Chemistry Dawes Y12 > Module 3 > Flashcards

Module 3 Flashcards

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
what is an endothermic reaction
energy being taken in from surroundings | displayed as a +ve enthalpy
26
what is the equation for energy transferred
q=mcΔT
27
define activation energy
the minimum energy required for a reaction to take place
28
how to calculate enthalpy of reaction
∑(bond enthalpies of reactants) - ∑(bond enthalpies of products)
29
define enthalpy of neutralisation
enthalpy change when an acid and alkali react together to form 1 mole of water
30
what is Hess' law
if a reaction can take place by more than one route, the total enthalpy change is the same for each route
31
describe the collision theory
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
factors that affect rate of reaction
concentration (pressure if reactants are gas) temperature catalyst surface area
33
how does concentration affect rate of reaction
more particles in a given volume, increasing frequency of successful collisions
34
how can rate of reaction be measured
volume of gas produced mass of reactants colour change
35
what is a homogenous catalyst
is the same physical state as the reactants
36
what is a heterogeneous catalyst
different physical state to the reactants
37
benefits of catalysts in terms of sustainability
lower temperatures required, so less energy demanded and less combustion of fossil fuels this reduces CO2 emissions and sustainability is improved
38
factors of the Boltzmann distribution curve
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
what happens to the Boltzmann curve when temperature increases
curve gets broader and shaded area increases as more molecules have the activation energy or higher
40
what is dynamic equilibrium
reversible reaction where rate of the forward reaction is equal to the rate of the backward reaction
41
what is Le Chatelier's principle
equilibrium shifts in position to favour the forward or backward reaction- opposes change
42
what factors affect the position of equilibrium
change in concentration change in pressure change in temperature
43
what way does equilibrium shift when pressure is increased
to the side with fewer gas molecules
44
what way does equilibrium shift if temperature is increased
in the endothermic direction
45
how to calculate equilibrium constant- Kc
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
what does it mean if the value of K>1
the reaction is product-favoured
47
what does it mean if the value of K<1
the reaction is reactant-favoured
48
uses of cobalt chloride
humidity indicator in weather instruments | cobalt chloride paper tests for the presence of water
49
what do catalysts do
provide an alternative route with a lower activation energy
50
name for group 2 elements
alkaline earth metals
51
name for group 17 elements
halogens
52
standard conditions
298k | 100KPa
53
what is the atomic radius
the distance from the outer shell of electrons to the nucleus of the atom
54
what is shielding
number of shells of electrons between the nucleus and outer shell of electrons
55
what is nuclear charge
the attraction from the protons in the nucleus with the electrons
56
what is the standard enthalpy change of a reaction
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
what is the standard enthalpy change of combustion
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
what is the standard enthalpy change of formation of a compound
the enthalpy change when 1 mole of the compound forms from its elements under standard conditions with the elements in their standard states
59
what is bond dissociation enthalpy
the enthalpy change on breaking 1 mole of a particular covalent bond in a gaseous molecule
60
as you go down group 2 what happens to solubility
it increases
61
which sulphate in group 2 is the most insoluble
BaSO4
62
how to test for sulphates
add acid and BaCl
63
what detects halogen ions
AgNO3
64
what colour do the halogens go when hexane is added
Cl2- pale green Br2- orange I2- purple

Chemistry Dawes Y12 (4 decks)

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