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AS- Chemistry > 2.1- Atoms and reactions > Flashcards

2.1- Atoms and reactions Flashcards

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1
Q

What is Relative Atomic Mass?

A

The weighted mean mass of an atom of an element compared to 1/12th the mass of an atom of carbon 12

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2
Q

What is Relative Isotopic Mass?

A

The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon 12

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3
Q

When describing a giant compound structure, you should use…

A

Relative formula mass

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4
Q

When describing a simple molecule, you should use…

A

Relative Molecular Mass

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5
Q

What can mass spectrometers do?

A

Identify unknown compounds
Find relative isotopic abundances
determine structural information about molocules

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6
Q

When a metal atom becomes an ion, what happens to its electrons and charge?

A

it loses electrons and becomes positively charged

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7
Q

When a non-metal atom becomes an ion, what happens to its electrons and charge?

A

It gains electrons and becomes negatively charged

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8
Q

What is an atom?

A

the smallest particle of a chemical element

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9
Q

What is an isotope?

A

a different form of an atom with the same number of protons but a different number of neutrons

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10
Q

In mass spectrometry, what are ions sorted on?

A

their mass to charge ratio

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11
Q

What is the acronym we use to remember the steps in mass spectrometry?

A 
Vapourisation
Ionisation
Acceleration
Deflection
Detection
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12
Q

What are ions?

A

atoms or molecules with a net charge

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13
Q

Why dont noble gasses form ions?

A

they have a stable outer shell and are unreactive

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14
Q

What is the charge on an NH4 Ion?

A

+1

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15
Q

What is the charge on a OH ion?

A

-1

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16
Q

What is the charge on a NO3 ion?

A

-1

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17
Q

What is the charge of a CO3 ion?

A

-2

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18
Q

What is the charge of a SO4 ion?

A

-2

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19
Q

Why do we use ionic equations?

A

To show the useful components of a chemical equation

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20
Q

Why dont we write solids in ionic equations?

A

they are spectator ions

only aqueous components dissociate into ions

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21
Q

Which type of elements form multiple ions?

A

Transition metals

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22
Q

What is the definition of a mole?

A

the amount of substance that contains the same number of atoms as 12g of carbon 12

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23
Q

what is avogadros constant?

A

6.02x10^23

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24
Q

What is the equation that links moles, mass and Mr?

A

Moles=Mass/Mr

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25
Q

At room temperature and preassure, a mole of gas will have the volume……?

A

24dm^3

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26
Q

What is the equation that links moles and volume of gasses?

A

Moles=volume/24

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27
Q

When we perform gas volume calculations, what do we assume?

A

That any intermolecular forces are negligible

it is at room temperature and pressure

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28
Q

What is the value of 0K?

A

-273 degrees Celsius

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29
Q

What is the ideal gas equation?

A

PV=nRT

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30
Q

What are the units of the ideal gas equation, PV=nRT?

A 
P=pascals
V=m^3
n=Moles
R=j/k/mol
T=Kelvin
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31
Q

What is the definition of empirical formula?

A

The simplest whole number ratio of atoms of each element in a compound

32
Q

What is the definition of molecular formula?

A

The number and type of atoms of each element in a molecule

33
Q

What is the definition of a crystal?

A

A substance whose atoms are regularly arranged in a 3d pattern

34
Q

What is a hydrated salt?

A

A salt which contains the water of crystalisation.

We express this using the dot formulae

35
Q

What is an anhydrous salt?

A

a salt which contains no water in the structure

36
Q

What does the xH2O represent in a hydrated salt?

A

the number of waters of crystallisation

37
Q

What is the definition of concentration?

A

How much solute is dissolved in a given volume of solvent

38
Q

What is the formula that links concentration, moles and volume?

A

concentration=moles/volume

39
Q

What is stoichiometry?

A

The quantitative relationship between reactants and products in a balanced chemical reaction

40
Q

What is the formula for percentage yield?

A

Theoretical yield

41
Q

Why is percentage yield not always 100%?

A

Side reactions may occur
Some reactants may remain unreacted
Some reactants may be lost
Reaction may be reversible and not proceed to completion

42
Q

What is the limiting reactant?

A

The reactant that isnt in excess and dictates the amount of product formed

43
Q

Processes with high atom economys are more……..?

A

Sustainable

44
Q

What is a strong acid?

What is an example of a strong acid

A

An acid that fully dissociates in soloution

Hydrochloric

45
Q

What is a weak acid?

Give an example of a weak acid

A

An acid that only partially disscociates in soloution

Ethanoic acid

46
Q

Acid+Base=

A

Salt+water

47
Q

Acid+Carbonate=

A

Salt+Water+CO2

48
Q

Acid+Metal Oxide=

A

Salt+Water

49
Q

What is the definition of an acid?

A

A substance that produces H+ ions in an aqueous solution

50
Q

What is the definition of an alkali?

A

A soluble base that produces OH- ions in an aqueous solution

51
Q

What are the two indicators we use when performing titrations?

A

Methyl Orange

Phenolpthalein

52
Q

What happens to methyl orange when an alkali is neutralised?

A

It turns from yellow to orange and to red when it becomes acidic

53
Q

What happens to Phenolphthalein when an alkali is neutralised?

A

It turns from Pink to colourless

54
Q

What is a standard solution?

A

A solution that has a precisely known concentration

55
Q

What are polyprotic acids?

A

Acids that donate more than one Proton

56
Q

What is an acid that donates 2 protons called?

A

Diprotic

eg. Sulfuric acid

57
Q

What is an acid that donates 3 protons called?

A

A triprotic acid

eg. Phosphoric acid

58
Q

What does an oxidation number tell you?

A

How many electrons an atom has donated or accepted to form an ion or part of a compound

59
Q

What is the oxidation number of Ag?

A

0

60
Q

What is the oxidation number of H2?

A

0

61
Q

What is the oxidation number of Na+?

A

+1

62
Q

What is the oxidation number of Mg2+?

A

+2

63
Q

What is normally the oxidation number of oxygen?

A

-2

64
Q

What is normally the oxidation number of hydrogen?

A

+1

65
Q

What order do we apply oxidation number rules in?

A

1,2,3 Fluorine, hydrogen, oxygen, chlorine

66
Q

What is the oxidation number of fluorine?

A

-1

67
Q

What is normally the oxidation number of chlorine?

A

-1 except when bonded to oxygen

68
Q

A compound ends in -ate. What does this suggest about the compound?

A

It contains oxygen and another element

69
Q

What is a loss of electrons called?

A

Oxidation

70
Q

What is a gain in electrons called?

A

Reduction

71
Q

What is the reaction called if oxidation and reduction happen simultaneously?

A

Redox

72
Q

As electrons are lost, what happens to the oxidation number?

A

It will increase

73
Q

As electrons are gained, what happens to the oxidation number?

A

It will decrease

74
Q

When are metals oxidised?

A

When they react with acids

75
Q

What happens to the oxidation number of metals when they react with acid?

A

The metals lose electrons and the metal atoms are oxidised

The hydrogen ions are reduced as they gain electrons

AS- Chemistry (7 decks)

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