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Chemistry > Unit 1.1 - Formulae and equations > Flashcards

Unit 1.1 - Formulae and equations Flashcards

1
Q

Sulfur dioxide

A

SO2

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2
Q

Methane

A

CH4

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3
Q

Hydrocloric acid

A

HCL

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4
Q

Sulfuric acid

A

H2SO4

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5
Q

Nitric acid

A

HNO3

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6
Q

Ethanoic acid

A

CH3CO2H

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7
Q

Ammonium (the ion)

A

NH4+

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8
Q

Ammonium chloride

A

NH4CL

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9
Q

Which compounds can I figure out myself?

A

All of the sodiums, coppers and calciums

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10
Q

Which ions have a +1 charge that can’t be figured out using the Periodic Table?

A

Silver (Ag+) and Ammonium (NH4+)

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11
Q

Which ions have a 2+ charge that can’t be worked out with the Periodic table?

A

Copper (II) (Cu2+)
Iron (II) (Fe2+)
Zinc (Zn2+)
Lead (Pb2+)

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12
Q

Which ions have a +3 charge that cannot be worked out with the Periodic table?

A

Iron (III) (Fe3+)

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13
Q

Which ions have a 1- charge that cannot be worked out using the Periodic Table?

A

Hydrogencarbonate (HCO3-)
Hydroxide (OH-)
Nitrate (NO3-)

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14
Q

Which ions have a 2- charge that cannot be worked out using the Periodic table?

A

Carbonate (CO3 2-)

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15
Q

Nitrates symbol and solubility rule

A

NO3-
All are soluble

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16
Q

Chloride, Bromide and Iodide symbols and solubility rule

A

ALL SOLUBLE
Except…..
Ag+ and PB2+
OH AND COPPER TOO NOW APPARENTLY

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17
Q

Which ions go together in a group of three to share the same solubility rule?

A

Chlorides, Bromides and Iodides

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18
Q

Carbonates symbol and solubility rule

A

CO3 2-
ALL INSOLUBLE
Except…..
Na+, K+, NH4+

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19
Q

Symbol for sulphates and solubility rule

A

SO4 2-
ALL SOLUBLE
Except……
Pb2+, Ba2+, Sr2+
Ca2+ is sparingly soluble

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20
Q

Symbol for hydroxides and solubility rule

A

OH-
ALL INSOLUBLE
Except…… Na+ and K+
Ba2+ and Ca2+ are slightly soluble

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21
Q

What do you do with a solid compound (s) if writing an ionic equation and why?

A

Leave it whole as it cannot dissolve in water to form ions

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22
Q

What does (aq) mean in an equation?

A

That it’s aqueous in water and can thereofore be dissolved in water

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23
Q

Steps to writing ionic equations

A

1- Word + chemical formula
2 - Write formula of ions formed (remember solids cannot dissolve to form ions)
3 - Omit spectator ions (if they appear on both sides, they do not take part in the reaction and can be cancelled)

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24
Q

Ammonia (the compound)

A

NH3

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25
Q

What are four things to remember when writing ionic equations?

A

1 - state symbols (aq or s)
2 - use the correct little ion charges
3 - numbers that were only there for balancing purposes in the compound turn into large ones when split into its separate elements, for example when compounds dissolve in aqueous solution
4 - numbers that are actually part of the compound remain the same, still written as little numbers

(For example for 3 and 4 - Ba(NO3)2 (s) (the two should be small)
Would be Ba 2+ + 2NO3 (the threes should be small lol)

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26
Q

Atom

A

The smallest part of matter that can exist on its own

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27
Q

Molecule

A

Two or more atoms combined chemically. Can be the same elements or different ones

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28
Q

Ion

A

A charged particle

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29
Q

Compound

A

A substance in which two or more elements are chemically combined - may be covalent or ionic compounds

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30
Q

Which three ions go together with the same solubility rule as eachother? Plus, what is this rule?

A

Chloride, Bromide and Iodide
All are soluble in water, expect for lead and silver

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31
Q

What do you call the substances that react?

A

Reagents

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32
Q

What type of equations always require state symbols?

A

Ionic

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33
Q

What do you call the solid that forms when two solutions react? How would this be written in an ionic equation?

A

Precipitate
With an (s), without charge as it hasn’t dissolved in the water to form ions

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34
Q

Percipitate

A

Solid that forms as two solutions react

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35
Q

Which formulas are written without charge in ionic equations?

A

Elements
Covalent compounds (H20 for example)
Insoluble compounds (CuO for example)

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36
Q

What are the diatomic elements? How can we remember them?

A

Hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, bromine
(have no fear of ice cold beer)

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37
Q

What are oxidation states used in?

A

Molecules or ions
Also covalent structures, where complete transfer of electrons does not occur

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38
Q

What do oxidation states show?

A

Used to show how many electrons the atom has used in bonding

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39
Q

What’s the first oxidation rule?
(give an example)

A

The oxidation state of an uncombined element is always zero
O2 = 0

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40
Q

What’s the second rule of oxidation states?

A

In a compound (contains two elements), 1 element has a positive oxidation state whilst the other has a negative oxidation state
The negative oxidation state is assigned to the more electronegative element
The sun of the oxidation state is zero

41
Q

In a compound, which element has the negative oxidation state?

A

The more electronegative element

42
Q

What is the sum if the oxidation state in compounds?

A

zero

43
Q

Give an example of the oxidation states in a compound

A

NaCl
Na oxidation state = 1
Sum of oxidation states = 0
Therefore, Cl = -1

44
Q

What’s the third oxidation state rule?

A

In ions, the sum of oxidation states is equal to the charge of the ion

45
Q

Give an example of oxidation states in ions

A

VO2+
Sum of oxidation states = 2
O oxidation states = -2
Therefore, V oxidation state = 4

46
Q

What’s the fourth oxidation states rule?

A

Some elements have specific oxidation states

47
Q

Which group one elements have an oxidation state of 1?

A

Li, Na, K

48
Q

Which group 2 elements have an oxidation state of 2?

A

Mg, Ca, Sr, Ba

49
Q

What group three elements have an oxidation state of 3?

A

Al

50
Q

Hydrogen oxidation state

A

+1
(except in metal hydrides)

51
Q

Oxygen oxidation state

A

-2 (except hydrogen peroxide- H202-1)

52
Q

Chlorine oxidation state

A

-1 (except with oxygen (variable) eg. chlorate)

53
Q

Which elements have exceptions with their oxidation states?

A

Hydrogen and Chlorine and Oxygen

54
Q

Which elements have specific oxidation states?

A

Some group 1, 2 and 3, hydrogen, oxygen and chlorine

55
Q

Redox reaction

A

A reaction in which both oxidation and reduction take place

56
Q

Oxidation

A

Removal (loss) of electrons = more positive species
= oxidised

57
Q

Reduction

A

Gain of electrons = more negative species
=reduced

58
Q

Oxidising agent

A

A species that oxidises another and is reduced in the process

59
Q

Reducing agent

A

A species that reduces another and is oxidised in the process

60
Q

What’s the pneumonic to remember the redox reactions?

A

OIL RIG

61
Q

How many elements are we expected to say the oxidation state of if there’s multiple?

A

Just one

62
Q

What signs do you need to remember to use when writing oxidation states?

A

Plus or minus

63
Q

What do we ignore when working out whether oxidation and reduction happened?

A

The big numbers in front

64
Q

Disproportionation

A

When the same element gets oxidised and reduced during the reaction

65
Q

What do you call when the same element gets oxidised and reduced during a reaction?

A

Disproportionation

66
Q

Can you put 1/2 in front of a compound in a formula?

A

Apparently, an official WJEC past paper said so so we’re going with yes

67
Q

Oxides symbol and solubility rules

A

O2-
Insoluble
except
Na, K, Sr, Ba
Ca sparingly soluble

68
Q

What IS hydrogen peroxides oxidation state?

A

-1

69
Q

Which element should you leave until last to make balancing equations easier?

A

Oxygen

70
Q

Phosphate ion

A

Po43-

71
Q

Lead ion

A

Pb2+

72
Q

Phosphoric acid

A

H3PO4

73
Q

Which numbers do we ignore when looking at redox reactions to figure out oxidations and reductions?

A

The big AND small numbers. Just look at the charges

74
Q

Do we have to balance the oxidation states in a compound when working out whether elements have been oxidised or reduced?

A

No, just look at their charges on the periodic table
(but still follow uncombined elements rules)

75
Q

What forms basic oxides?

A

Group 1, 2 and lanthanides

76
Q

What is the oxidation state of hydrogen in metal hydrides?

A

-1

77
Q

Oxygen oxidation state exception

A

-2 except in hydrogen peroxide H202, where it’s -1

78
Q

What’s the oxidation state exception with chlorine?

A

-1 usually except with oxygen (variable) eg- chlorate

79
Q

Which other element always has the same oxidation state and what is this?

A

Florine, that’s always -1

80
Q

What’s a shortcut for working out oxidation states in complex ions like Cr(H20)6^3+?

A

The compound’s oxidation state is 0
So (H20) = 0
That leaves Cr6^3+
Which is an uncombined element and an ion with a 3+ charge, so it’s just 3+

81
Q

Do you use the little numbers when working with oxidation states?

A

Yes lol

82
Q

What’s important to remember when writing out nuclear decay equations?

A

Whatever is decaying gets it’s own side of the equation

83
Q

Which ions have the same solubility rules as carbonates?

A

Phosphates and sulphides (s - not to be confused with sulphates!)

84
Q

What’s an element?

A

a substance with only 1 type of atom (has its own symbol on the periodic table)

85
Q

What do I need to stop forgetting for compound formulas?

A

Brackets! (Especially with hydroxide)

86
Q

What’s the rule to remember for zeros in significant figures?

A

Zeros are only significant after a figure

87
Q

What significant figure do we round to if asked to round to an ‘appropriate’ number of significant figures?

A

The least amount seen in the question

88
Q

How do we convert from cm^3 to m^3?

A

Divide by 100^3
(So, divide by 1,000,000)

89
Q

With what type of compounds do you take into account the big numbers when calculating the molecular mass?

A

Hydrides - include water
(E.g - Cuso4.7H20 DOES take into account the 7)

90
Q

Metal hydride

A

Metal with covalently bound hydrogen

91
Q

Zinc ions

A

Zn2+

92
Q

Under what conditions is oxygen’s oxidation state no longer -2?

A

-In peroxides
-In F20
(Both -1 instead)

93
Q

Where are the halogens on the periodic table?

A

Group 7

94
Q

What are the halogens common oxidation states?

A

-1 (as expected)

95
Q

Spectator ions

A

The same on both sides of the reaction - can cross them out of ionic equations as they’re not involved in the reaction

96
Q

In which order to we write out the letters in compound equations?

A

CHO
(the rest in alphabetical order)

97
Q

What is the compound formed from CO3 and H2?

A

NOT H2CO3 but…
CO2 and H2O

98
Q

What are two things to remember about the diatomic elements?

A

-Only write them as diatomic if they’re existing alone
-No need to be diatomic as ions

99
Q

Do we split water into its ions? Why?

A

No, we write its state symbol as (l) for liquid, which has the same effect as (s)

Chemistry (39 decks)

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