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A-level Chemistry > Chapter 4: Acids and redox > Flashcards

Chapter 4: Acids and redox Flashcards

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1
Q

what is the main characteristic of an acid

A

acids donate H+(aq) in aqueous solution

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2
Q

what does a strong acid do

A

strong acid dissociates fully there H+ ions

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3
Q

what is a monoprotic acid

A

acid that breaks up and dissociates to form one proton

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4
Q

what is a diprotic acid

A

acid that breaks up and dissociates to form two proton

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5
Q

what is a tripotic acid

A

acid that breaks up and dissociates to form three protons

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6
Q

what does concentrated and dilute refer to in acids

A

refers to how much acid there is in a set volume

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7
Q

what is the pH scale in terms of mathematical formula

A

pH = -log[H+]

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8
Q

what is a weak acid

A

acid that only partially dissociates in aqueous solution

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9
Q

what is a Base

A

substance that neutralises an acid and accepts H+ ions to form water and salt

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10
Q

what is an alkali

A

a base that dissolves to form OH-(aq) ions

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11
Q

what is the general neutralisation formula

A

Acid + base –> Salt + Water + (Carbon Dioxide)

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12
Q

what do titrations always need

A

Aqueous solution

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13
Q

what is a spectator ion

A

it is an ion that during the reaction nothing happens to

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14
Q

what does an ionic equation do

A

get rid of spectator ion and show what is actually happening during the reaction

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15
Q

what is the first step for writing an ionic equation

A

write a ‘normal’ balanced equation

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16
Q

what is the second step for writing an ionic equation

A

ionic compounds in aqueous solution will split into separate hydrated ions which react independently

17
Q

what is the third step for writing an ionic equation

A

look for the spectator ions and remove from the equation

18
Q

what are the two things you do to spot the spectator ions

A

are they in an aqueous solution
are they unchanged
if yes to both they are spectator ions

19
Q

what is the fourth step for writing an ionic equation

A

write out the remaining ionic equation with state symbols

20
Q

what is quantitative analysis

A

all about measuring amounts then analyse and evaluate date

21
Q

what is volumetric analysis

A

involves using volumes

22
Q

what is the percentage purity formula

A

(mass of pure substance / mass of impure sample) x 100

23
Q

what is a REDOX reaction

A

a reaction where both oxidisation and reduction happen

24
Q

what is an ionic half equation

A

where you split an ionic equation in half to show what is happening to each ion

25
Q

what is an Oxidising Agent

A

A chemical species that causes something else to be oxidised and is itself reduced

26
Q

what is a Reducing Agent

A

A chemical species that causes something else to be reduced and is itself oxidised

27
Q

what are Oxidation Numbers

A

Theoretical numbers of electrons involved in bonding of an atom to a separate element, whether ionic or covalent

28
Q

what is the element oxidation number

A

any element in its elemental form has an oxidation number of 0

29
Q

what is the simple ion oxidation number rule

A

in a simple ion the oxidation number is equal to the charge

30
Q

what does an increase in the oxidation number mean

A

the element is being oxidised

31
Q

what does a decrease in the oxidation number mean

A

the element is being reduced

32
Q

what is the compound oxidation number rule

A

in a compound the total oxidation number of each atom add up to 0

33
Q

what is the complex ion oxidation number rule

A

in a complex ion the oxidation numbers of all the atoms add up to the remaining charge

34
Q

what do Roman numerals in Chemistry represent

A

Roman numerals show the oxidation number where an element can have more than one oxidation state

35
Q

what are the three special cases for oxidation states

A

> Hydrogen in metal hydrides
Oxygen in peroxides
Halogens can vary

36
Q

explain how metal hydrides are special cases for oxidation states

A

Hydrogen has a negative oxidation number

e.g. NaH H has an oxidation state of -1

37
Q

explain how peroxides are special cases for oxidation states

A

Oxygen has an oxidation state of -1

e.g. H2O2 Oxygen has an oxidation number of -1

38
Q

explain how halogens are special cases for oxidation states

A

Halogen can have varying oxidation state from usual -1

e.g. HClO Cl has an oxidation state of +1

39
Q

what is disproportionation

A

where an element is both oxidised and reduced in the same reaction

A-level Chemistry (19 decks)

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