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Definitions/common equations Flashcards

(60 cards)

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1
Q

*Relative isotopic mass

A

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

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2
Q

*relative atomic mass

A

The weighted mean mass compared with 1/12th mass of carbon-12

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3
Q

how to calculate Mr

A

((isotope mass x percentage) + (isotope mass x percentage)) / 100

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4
Q

*Isotopes

A

Atoms of an element with the same number of protons but different number of neutrons.

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5
Q

*Molar Mass

A

mass per mole, units g mol–1

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6
Q

*Mole

A

The unit of amount of substance, 1 mole is 6.02 x 1023 particles

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7
Q

*Acid

A

Releases H+ ion aqueous solution, proton donor

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8
Q

*Alkali

A

A soluble base that releases OH- ions in an aqueous solution.

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9
Q

*Strong acid

A

Fully dissociates in solution

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10
Q

*Weak acid

A

Partially dissociates in solution

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11
Q

Oxidation

A

increase in oxidation number due to the loss of electrons

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12
Q

Reduction

A

decrease in oxidation number due to the gaining of electrons

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13
Q

Salt

A

A compound produced when an H+ ion of an acid is replaced by a metal ion or an ammonium ion.

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14
Q

Base

A

accepts a proton (H+)

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15
Q

water of crystallization

A

is the water incorporated into the lattice of a crystal

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16
Q

Anhydrous

A

A salt without water of crystallization

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17
Q

hydrated

A

A salt with water of crystallisation

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18
Q

empirical formula

A

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

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19
Q

molecular formula

A

The actual number of atoms of each element in a molecule

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20
Q

atom economy

A

Mr desired products/Mr all products x100

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21
Q

How to calculate moles in a solid

A

Moles = mass /molar mass (for solids)

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22
Q

How to calculate moles in a solution

A

Moles = concentration x volume (for solutions)

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23
Q

How to calculate moles in a gas (at rtp)

A

Moles = volume / 24dm3 (for gas)

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24
Q

How to calculate moles from no. of particles

A

Moles = number of particles / Avogadro’s constant

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25
How to calculate % error
% error = (uncertainty in equipment x no of uses / measured value) x 100
26
How to calculate Mr
Mr = ( (relative mass of isotope A x % of isotope A) + (relative mass of isotope B x % of isotope B)) /100
27
How to calculate % yield
% yield = (actual yield/ theoretical yield) x100
28
How to calculate atom economy
Mr of desired products/Mr of all products (include molar ratio)
29
what is the ideal gas equation
pV = nRT (p in Pascal’s, v in m3, T in Kelvin)
30
nitrate ion
NO3 –
31
Hydroxide ion
OH–
32
Carbonate ion
CO3 2–
33
Sulphate ion
SO4 2–
34
Ammonium ion
NH 4+
35
Zinc ion
Zn 2+
36
Silver ion
Ag+
37
Hyrdrochloric acid
HCl
38
Sulphuric acid
H2SO4
39
Nitric acid
HNO3
40
Ethanoic acid
CH3COOH
41
Sodium hydroxide
NaOH
42
Potassium hydroxide
KOH
43
Ammonia
NH3
44
Acid + Metal
Acid + Metal --> Salt + Hydrogen
45
Acid + Metal Oxide
Acid + Metal --> Salt + Water
46
Acid + Metal Hydroxide
Acid + Metal --> Salt + Water
47
Acid + Metal Carbonate
Acid + Metal --> Salt + Water + carbon dioxide
48
order of assigning oxidization states
``` 1 (1+) 2 (2+) 3 (3+) F (-1) H (nearly always +1) O (nearly always -2) Cl (nearly always -1 expect when bonded to O) ```
49
what are the 4 state symbols
(s) - solid (l) - liquid (g) - gas (aq) - aqueous (solution in water)
50
what is an ionic equation
an equation that doesn't include spectator ions
51
how to convert from m3 to dm3
x1000
52
how to convert from dm3 to cm3
x1000
53
how to convert from dm3 to m3
divide by 1000
54
how to convert from cm3 to dm3
divide by 1000
55
how to convert from celcius to kelvin
kelvin= celcius+273
56
reasons for low yield
- reaction at equilibrium - side reactions - left in apparatus - impure reactants - lost in separation and purification
57
why is higher atom economy good
- less waste so higher profit | - more sustainable as raw materials are in limited supply
58
what do roman numerals stand for
charge of the positive ion
59
what does the OS of ions equal
the charge of that ion
60
what is the OS of elements and molecules
add to zero

Chemistry (12 decks)

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