Principles of chemistry Flashcards

1
Q

Properties of a solid?

forces between particles, particle positioning, type of shape, movement

A

Strong forces of attraction between particles
Fixed positions in lattice arrangement
Keep definite shape and volume
vibrate about positions

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2
Q

Properties of liquids?

forces between particles, type of shape, movement

A

Weak forces of attraction between particles
Don’t keep a definite shape, but do keep a definite volume
Moving with random motion

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3
Q

Properties of gasses?

forces between particles, type of shape, movement

A

Forces of attraction between particles are very weak
Don’t have definite shape or volume
Moving constantly with random motion

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4
Q

What’s going from a solid to a gas called?

A

Subliming

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5
Q

How do states change from to another?

A

Gain energy, so they vibrate more and break or weaken the bonds

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6
Q

What’s diffusion?

A

The gradual movement of particles from an area of high concentration to low

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7
Q

What can you use to show diffusion?

A

Potassium manganite in water, bright purple spreads out

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8
Q

How can ammonia and hydrogen chloride show diffusion?

A

Put at 2 sides of a tube, white ring will form where they meet, closer to hydrogen chloride, because ammonia diffuses faster

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9
Q

What happens when bromine gas (brown) mixes with air in a tube?

A

Bromine diffuses making the air browner

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10
Q

Features of a nucleus?

location, what it contains, what charge, mass

A

Middle of atom
Contains protons and neutrons
Positive charge due to protons
Small compared to rest of atom, but contains all mass

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11
Q

Features of electrons?

A

Move around the nucleus in shells
negatively charged (-1)
Very small
No mass

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12
Q

Features of protons?

A

Relative mass=1

Relative charge = 1

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13
Q

The number of protons equals?

A

The number of electrons

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14
Q

Features of a neutron?

A

Relative mass=1

No charge

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15
Q

What’s the mass number?

A

Total number of protons and neutrons

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16
Q

What’s the atomic number?

A

Number of protons

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17
Q

How do you find the amount of neutrons?

A

Mass number subtract atomic number

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18
Q

What are molecules?

A

Groups of atoms held together by covalent bonds

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19
Q

Elements consist of?

A

1 type of atom

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20
Q

What’s a diatomic molecule?

A

A molecule with 2 atoms

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21
Q

What’s a compound?

A

2 or more different elements chemically bonded together

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22
Q

What’s a mixture?

A

When there’s no chemical bond between parts, and they can be separated by physical methods

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23
Q

What’s filtration used for?

A

To separate an insoluble solid from a liquid (filter paper)

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24
Q

What’s crystallisation used for?

A

Separating a soluble solid from a soloution

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25
Q

Method for crystallisation?

A

Pour solution into evaporating dish
Heat solution
Place in warm place to allow evaporation from the crystals
Dry in drying oven

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26
Q

How can you use filtration and crystallisation to separate rock(Insouluble)Salt(solouble)?

A

Grind up
dissolve in beaker
Filter
Crystallise

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27
Q

What’s paper chromatography?

A

Putting dots of ink on a piece paper, placing it in a solvent and seeing how soluble the dyes are by how far they move up the paper

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28
Q

What’s simple distillation used for?

A

Separate solutions

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29
Q

What’s fractional distillation used for?

A

Separating a mixture of liquids, different boiling point come out at different fractions

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30
Q

What are groups on the periodic table?

A

Amount of outer electrons

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31
Q

What are group 1 elements called?

A

alkali metals

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32
Q

What are group 7 elements called?

A

halogens

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33
Q

What are group 0 elements called?

A

Noble gases

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34
Q

What are the electron shell rule?

A

they fill up shells in the form 2:8:8
Happiest when they have a full shell
Want to react when it’s not full

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35
Q

What’s ionic bonding?

A

When atoms bond and lose or gain electrons to become strongly attracted to each other through electrostatic attraction

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36
Q

What’s oxidation?

A

When an atom loses electrons

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37
Q

What’s reduction?

A

When an atom gains electrons

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38
Q

What are positive ions called?

A

Cations

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39
Q

What are negatively charged ions called?

A

Anions

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40
Q

When does ionic bonding occur?

A

When an atom wants to get rid of electrons, and another atom wants to gain an electrons

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41
Q

Why do giant ionic structures have high melting and boiling points?

A

closely packed 3D lattice arrangement,

oppositely charged ions mean strong forces if attraction

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42
Q

What’s covalent bonding?

A

When atoms share electrons to fill each others outer shell

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43
Q

What are the atoms within a molecule bonded by?

A

Strong covalent bonds

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44
Q

What are the forces between molecules like?

A

Very weak

45
Q

Features of giant covalent structures?

type of bonds, melting point, do they conduct, are they soluble

A

Bonded by strong covalent bonds
Lots of bonds so high boiling/melting point
Don’t conduct electricity
insoluble in water

46
Q

Features of diamond?

A

Each carbon atom has 4 covalent bonds

very hard

47
Q

Features of Graphite?

A

Each carbon atom only makes 3 bonds, creating layers which can slide over each other making it a good lubricant
this leaves free electrons so it’s the only non metal which can conduct electricity

48
Q

What does aqueous mean?

A

Dissolved in water

49
Q

What does a balanced equation require?

A

Even amount of atoms on each side of the equation

50
Q

What’s an isotope?

A

Different atomic forms of the same element, which have the same number of protons but different amount of neutrons

51
Q

How to find the average mass of an isotope, when given 2 relative masses and 2 relative abundances?

A

(relative abundance 1 x mass 1) + (Relative mass 2 x mass2) /(relative abudance 1 + relative abundance 2)= average mass

52
Q

How to find the relative mass?

A

Add up the masses from all the atoms in the subject

53
Q

How to find the empirical formula?

A

1) write all elements
2) Write the experimental masses or percentages
3) Divide each mass by their RFM
4) turn these numbers into a ratio
5) Write out the formula

54
Q

How to find the molecular formula?

A

1) Work out the mass of the empirical formula of the elements you’ve been given
2) See how that compares to the RFM of the full molecule
3) divide or multiply the elements to get the mlecularformula

55
Q

How to find masses in reactions?

A

1) Work out the RFM of the 2 things which create each other

2) Multiply and divide the masses until you get the ratio which allows you to answer the question

56
Q

What’s the actual yield?

A

The actual amount of product you get when doing the experiment

57
Q

What’s the theoretical yield?

A

The yield you get when you work out masses you a balanced symbol equation

58
Q

What’s the percentage yield?

A

The actual yield compared to the theoretical yield

59
Q

Formula for percentage yield?

A

Percentage yield= actual yield (grams) / theoretical yield (grams). then x answer by 100

60
Q

What’s a mole

A

The number (6.023 x 10 to the power of 23), making an elements mass in grams equal to its RFM

61
Q

How do you find moles when given RFM and mass?

A

Moles = mass in g / RFM

62
Q

What do salts consist of?

A

Lattice arrangement of positive and negative ions

63
Q

A solid salt containing water of crystallisation is?

A

Hydrated

64
Q

A solid salt containing no water of crystallisation is?

A

Anhydrous

65
Q

How to calculate how much water of crystallisation a salt contains?

A

Work out the mass of the anhydrous salt with and without water

Calculate the moles of water lost

Calculate the moles of anhydrous salt made (using the mass and rfm)

Find the ratio of moles of anhydrous salt to water (using the mass and rfm)

Put these ratios in the Formula for the hydrated salt

66
Q

What’s Avodaros law?

A

One of mole of any gas occupies 24dm(cubed) at room temperature and pressure

67
Q

How to find the moles of a gas?

A

Moles of gas= Volume dm(cubed) / 24

68
Q

How to find the volume of a gas if given the mass of the gas?

A

Volume (dm cubed) = (mass of gas / RFM of gas) x 24

69
Q

How to calculate volumes of gases in reactions if you know the masses?

A

Write balanced equation

Write down the RFM for each part

Divide and multiply to get the mass the question wants

Put the new information into the formula Volume (dm cubed) = (mass of gas / RFM of gas) x 24, to find the required element

70
Q

What’s concentration?

A

The amount of stuff per unit volume

71
Q

Equation for concentration?

A

Concentration (mol/dm3)= moles/volume

72
Q

What’s an ion?

A

A positively or negatively charged atom

73
Q

What’s an electric current?

A

A flow of electrons or ions

74
Q

What state can ionic compounds conduct electricity?

A

Molten or in a solution

75
Q

Why can’t solid ionic compounds conduct electricity?

A

Ions aren’t free to move around

76
Q

Why can an ionic compound conduct electricity when In a solution or molten?

A

when dissolved the ions separate, and are free to move in the soloution, so they can carry a current and conduct electricity

77
Q

Why don’t covalent compounds conduct electricity?

A

Don’t contain ions, so no charge carriers

78
Q

Structure of metal?

A

Lots of positive metal ions, surrounded by a sea of delocalised electrons

79
Q

What’s metallic bonding?

A

The attraction between the positive ions and the sea of electrons, giving metals their properties

80
Q

Why are metals good conductors of heat and electricity

A

Free electrons carry them effectively

81
Q

Why are most metals malleable?

A

Layers in the atom can roll over each other, do they can be rolled into flat sheets

82
Q

What’s electrolysis?

A

Passing an electric current through a molten or in solution ionic substance, to make new substances

83
Q

What’s the liquid required to conduct the electricity in electrolysis called?

A

The electrolyte

84
Q

How are electrolytes made?

A

Dissolving or melting a substance, so it has free ions to conduct electricity

85
Q

What’s the positive electrode called?

A

The anode

86
Q

What’s the negative electrode called?

A

The cathode

87
Q

What’s required for the electrolysis circuit to be complete?

A

A flow of electrons, electrons taken away from ions at the anode, and electrons given to other ions at the cathode

88
Q

What happens to ions as they gain or lose electrons?

A

Become atoms or molecules

89
Q

How to test whether a liquid is a electrolyte?

A

Use a conductivity probe to see if it produces a current

90
Q

How are electrolytes made?

A

By dissolving or melting a ionic compounds so they have free electrons

91
Q

What does there have to be in electrolysis for the circuit to be complete?

A

A flow of electrons

92
Q

What’s the positive electrode called?

A

The anode

93
Q

What happens at the anode?

A

electrons are taken away from the ions

94
Q

What’s the negative electrode called?

A

The cathode

95
Q

What happens at the cathode?

A

Electrons given to ions

96
Q

What happens in the electrolysis molten lead bromine?

A

Lead cations go to cathode and gain 2 electrons and the molten lead then sinks to bottom

Bromine anions go to anode to make bromine, bromine gas goes to the top

97
Q

Why don’t the electrodes react?

A

They are inert

98
Q

why’s electrolysis different in a aqueous solution?

A

There will be hydrogen ions (H+), and hydroxide ions (OH-)

99
Q

In an aqueous solution, what happens if H+ ions and metal ions are present?

A

At the cathode if the metal ions are more reactive that H+ ions then Hydrogen gas will be made. If their not then the pure metal will be produced then

At the anode, if OH- and halide ions (Cl-, Br-, I-) are present there halides molecules will be formed. If there are no halides oxygen will be made

100
Q

In an aqueous solution, what’s produced in the electrolysis of Sulphuric acid?

A

Cathode: Hydrogen gas
Anode: Oxygen and water

101
Q

In an aqueous solution, what’s produced in the electrolysis of Sodium chloride?

A

Cathode: Hydrogen gas
Anode: Chlorine gas

102
Q

In an aqueous solution, what’s produced in the electrolysis of copper Sulphate

A

Cathode: Copper metal
Anode: Oxygen and water

103
Q

What does the amount of product made by electrolysis rely on?

A

The amount of electrons transferred

104
Q

How to increase the amount of electrons transferred?

A

Longer electrolysis

Increase the current

105
Q

Equation for charge?

A

Charge= amps x time

106
Q

What’s one faraday?

A

96,000 coulombs, and one mole of electrons

107
Q

How do you know how many moles of electrons an ion needs to make an atom?

A

The same amount as the ions charge

108
Q

How to work out masses from electrolysis?

A

Write out balanced equation of lead
Calculate the number of faradays
Calculate the number of moles of product made ( Divide the amount of faradays by the amount of electrons)
Work out the RFM to be able to use the moles equation to find the mass