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Chemistry > Module 2: Atoms And Reactions 1 > Flashcards

Module 2: Atoms And Reactions 1 Flashcards

1
Q

What ions do group 1 elements form??

A

+1

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2
Q

What ions to group 2 elements form??

A

+2

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3
Q

What ions to group 3 elements form

A

+3

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4
Q

What ions to group 4 elements form??

A

Rarely form ions

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5
Q

What ions to group 5 ions form??

A

-3

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6
Q

What ions to group 6 ions form??

A

-2

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7
Q

What ions to group 7 elements form??

A

-1

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8
Q

What ions to group 0 elements from?

A

Do not form ions

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9
Q

Hydrogen ion

A

H+

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10
Q

Ammonium ion

A

NH4+

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11
Q

Silver ion

A

AG+

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12
Q

Lead (II) ion

A

Pb2+

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13
Q

Zinc ion

A

Zn2+

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14
Q

Iron (II) ion

A

Fe2+

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15
Q

Iron (III) ion

A

Fe3+

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16
Q

Copper (II) ion

A

Cu2+

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17
Q

Hydroxide ions

A

OH-

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18
Q

Nitrate ion

A

NO3-

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19
Q

Sulphate ion

A

SO42-

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20
Q

Sulphite ion

A

SO32-

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21
Q

Carbonate ion

A

CO32-

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22
Q

Hydrocarbonate ion

A

HCO3-

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23
Q

Phosphate ion

A

PO43-

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24
Q

Ethanoate ion

A

CH3CO2-

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25
Q

Hydrogen element

A

H2

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26
Q

Nitrogen element

A

N2

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27
Q

Oxygen element

A

O2

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28
Q

Fluorine element

A

F2

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29
Q

Chlorine element

A

Cl2

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30
Q

Bromine element

A

Br2

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31
Q

Iodine element

A

I2

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32
Q

Water compound

A

H2O

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33
Q

Ammonia compound

A

NH3

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34
Q

Methane compound

A

CH4

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35
Q

Carbon dioxide compound

A

CO2

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36
Q

Sulphur dioxide compound

A

SO2

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37
Q

Hydrogen chloride compound

A

HCL

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38
Q

Hydrogen peroxide compounds

39
Q

Acid + alkali

A

Salt + water

40
Q

Acid + base

A

Salt + water

41
Q

Acid + metal

A

Salt + hydrogen

42
Q

Acid + carbonate

A

Salt + water + CO2

43
Q

What ions do acids release in aqueous solutions??

44
Q

What ions do alkalis release in solutions??

45
Q

What is a base

A

A base is a substance that neutralises an acid

46
Q

Examples of bases

A

Metal oxides and metal hydroxides

47
Q

What is a salt?

A

Formed by replacing the H+ ion in an acid with another positive ion

48
Q

Common acids

A

Sulphuric acid

Nitric acid

Hydrochloric acid

Ethanoic acid

49
Q

Common alkalis

A

Sodium hydroxide

Potassium hydroxide

Ammonia

50
Q

1 mole of gas is equal to how many dm^3

51
Q

What do atoms consist

A

A number of fundamental particles

52
Q

Proton relative mass

53
Q

Proton relative charge

54
Q

Neutron relative mass

55
Q

Neutron relative charge

56
Q

Electron relative mass

57
Q

Electron relative charge

58
Q

Atomic number

A

Number of protons in the nucleus of an atom

59
Q

Mass number

A

Sum of the protons and neut one in the nucleus

60
Q

Relative atomic mass

A

The mass of an atom relative to the 12C isotope having a value of 12.000

61
Q

Ar equation

A

Ar = average mass per atom of an element/mass of one atom of carbon-12 x12

62
Q

What is carbon-12

A

The international standard isotope on which all other atomic masses are based

63
Q

Relative isotopic mass

A

The mass of an isotope relative to 1/12th the mass of an atom of carbon-12

64
Q

Isotopes definition

A

Atoms with some atomic number but different mass number

Same number of protons but different number of neutrons

65
Q

Properties of an isotope

A

Chemical properties are identical

Physical properties can differ

66
Q

Heavy water D2O

A

I’m heavy water, all molecules of H2O contain the second isotope of hydrogen called Deuterium

67
Q

Binary compounds

A

Contain 2 elements only

68
Q

Empirical formula

A

Simplest whole number ratio of the numbers of each kind of atom or ion in a compound

69
Q

A molecular formula

A

Total numbers of each kind of atom in a molecule

70
Q

Volumes of gases

A

1 mol of any gas occupies the same volume as a given temp and pressure

71
Q

When is material lost during a chemical reaction

A

Filtering, distilling, transferring or purifying chemicals

Many reactions do not go to completion

Side reactions may have occurred

72
Q

Percentage yield

A

Actual/theoretical x 100

73
Q

What does a high % yield mean?

A

Efficient conversion of starting materials into product

74
Q

Avogadros law

A

A temperature at a constant temperature and pressure

75
Q

Boyle’s law

A

For a fixed mass of gas at constant temperature

76
Q

Charles’ Law

A

For a fixed mass of gas at constant pressure

77
Q

Ideal gas equation

A

pV = nRT

V = volume

P = pressure

n = number of moles of gas

R = ideal gas equation

T = temperature

78
Q

Atom economy equation

A

Atom economy = sum of Mr of desired products/sum of Mr of all products x 100

79
Q

Benefits of a high atom economy

A

Most of the product is useful and there is little waste product

80
Q

What is atom economy

A

A measure of how well atoms have been utilised in a chemical reaction

81
Q

Limiting reagent

A

When using two reactants and one is in excess, the other will be completely used up and stop the reaction

82
Q

Properties of an ideal gas

A

Gas particles have negligible size or volume

No intermolecular forces (no attraction between molecules)

Elastic collisions

Random motion

83
Q

What happens when real gases are at low temp and high pressure

A

Particles are moving more slowly and are closer together

84
Q

What does a chemical bond hold together?

A

Atoms, ions and molecules

85
Q

What do the physical properties of a substance depend on??

A

Strength of the bonds that must be broken

86
Q

Metals and non-metals have what bonding?

87
Q

Non metals only have what bonding?

88
Q

Metals only have what type of bonding??

A

Metallic bonding

89
Q

What is ionic bonding??

A

An ionic bond is an electrostatic attraction between oppositely charged ions

90
Q

How are ionic bonds formed??

A

Formed by the transfer of electrons from one atom to the next

91
Q

What does the strength of the ionic bond depend upon??

A

The charge densities of the ions

92
Q

What is the relationship between charge densities and bond strength??

A

The greater the charge density, the stronger the ionic bonds will be

93
Q

What structure do strong electrostatic forces result in??

A

Result in a regular lattice

94
Q

Why are atoms electrically neutral??

A

Because they contain the same number of protons and electrons

Chemistry (7 decks)

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