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AS- Chemistry > 2.1- Atoms and reactions > Flashcards

2.1- Atoms and reactions Flashcards

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
At room temperature and preassure, a mole of gas will have the volume......?
24dm^3
26
What is the equation that links moles and volume of gasses?
Moles=volume/24
27
When we perform gas volume calculations, what do we assume?
That any intermolecular forces are negligible | it is at room temperature and pressure
28
What is the value of 0K?
-273 degrees Celsius
29
What is the ideal gas equation?
PV=nRT
30
What are the units of the ideal gas equation, PV=nRT?
``` P=pascals V=m^3 n=Moles R=j/k/mol T=Kelvin ```
31
What is the definition of empirical formula?
The simplest whole number ratio of atoms of each element in a compound
32
What is the definition of molecular formula?
The number and type of atoms of each element in a molecule
33
What is the definition of a crystal?
A substance whose atoms are regularly arranged in a 3d pattern
34
What is a hydrated salt?
A salt which contains the water of crystalisation. | We express this using the dot formulae
35
What is an anhydrous salt?
a salt which contains no water in the structure
36
What does the xH2O represent in a hydrated salt?
the number of waters of crystallisation
37
What is the definition of concentration?
How much solute is dissolved in a given volume of solvent
38
What is the formula that links concentration, moles and volume?
concentration=moles/volume
39
What is stoichiometry?
The quantitative relationship between reactants and products in a balanced chemical reaction
40
What is the formula for percentage yield?
actual yield ----------------- Theoretical yield
41
Why is percentage yield not always 100%?
Side reactions may occur Some reactants may remain unreacted Some reactants may be lost Reaction may be reversible and not proceed to completion
42
What is the limiting reactant?
The reactant that isnt in excess and dictates the amount of product formed
43
Processes with high atom economys are more........?
Sustainable
44
What is a strong acid? | What is an example of a strong acid
An acid that fully dissociates in soloution | Hydrochloric
45
What is a weak acid? | Give an example of a weak acid
An acid that only partially disscociates in soloution | Ethanoic acid
46
Acid+Base=
Salt+water
47
Acid+Carbonate=
Salt+Water+CO2
48
Acid+Metal Oxide=
Salt+Water
49
What is the definition of an acid?
A substance that produces H+ ions in an aqueous solution
50
What is the definition of an alkali?
A soluble base that produces OH- ions in an aqueous solution
51
What are the two indicators we use when performing titrations?
Methyl Orange | Phenolpthalein
52
What happens to methyl orange when an alkali is neutralised?
It turns from yellow to orange and to red when it becomes acidic
53
What happens to Phenolphthalein when an alkali is neutralised?
It turns from Pink to colourless
54
What is a standard solution?
A solution that has a precisely known concentration
55
What are polyprotic acids?
Acids that donate more than one Proton
56
What is an acid that donates 2 protons called?
Diprotic | eg. Sulfuric acid
57
What is an acid that donates 3 protons called?
A triprotic acid | eg. Phosphoric acid
58
What does an oxidation number tell you?
How many electrons an atom has donated or accepted to form an ion or part of a compound
59
What is the oxidation number of Ag?
0
60
What is the oxidation number of H2?
0
61
What is the oxidation number of Na+?
+1
62
What is the oxidation number of Mg2+?
+2
63
What is normally the oxidation number of oxygen?
-2
64
What is normally the oxidation number of hydrogen?
+1
65
What order do we apply oxidation number rules in?
1,2,3 Fluorine, hydrogen, oxygen, chlorine
66
What is the oxidation number of fluorine?
-1
67
What is normally the oxidation number of chlorine?
-1 except when bonded to oxygen
68
A compound ends in -ate. What does this suggest about the compound?
It contains oxygen and another element
69
What is a loss of electrons called?
Oxidation
70
What is a gain in electrons called?
Reduction
71
What is the reaction called if oxidation and reduction happen simultaneously?
Redox
72
As electrons are lost, what happens to the oxidation number?
It will increase
73
As electrons are gained, what happens to the oxidation number?
It will decrease
74
When are metals oxidised?
When they react with acids
75
What happens to the oxidation number of metals when they react with acid?
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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