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AA Chemistry > Paper 1 - Topics 1-5 (Year 10) > Flashcards

Paper 1 - Topics 1-5 (Year 10) Flashcards

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1
Q

What is the first step of writing an ionic equation?

A

Step 1: Write an equation and balance it.

2Na(s) + 2HCl(aq) -> 2NaCl(aq) + H2(g)

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2
Q

What is the second step of writing an ionic equation?

A

Step 2: Split the ions. (Only compounds that are aqueous are split into ions.)

2Na(s)+2H+(aq)+2Cl-(aq) → 2Na+(aq)+2Cl-(aq)+H2(g)

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3
Q

What is the third step of writing an ionic equation?

A

Step 3: Cancel out spectator ions. (Spectator ions are ions that remain the same in their original states before and after a chemical reaction.)

2Na(s)+2H+(aq)+2Cl-(aq) → 2Na+(aq)+2Cl-(aq)+H2(g)
Turns into:
2Na(s) + 2H+(aq) → 2Na+(aq) + H2(g)

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4
Q

What is the last step of writing an ionic equation?

A

Step 4: Write a balanced ionic equation

2Na(s) + 2H+(aq) → 2Na+(aq) + H2(g)

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5
Q

What is a mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together. The chemical properties of each substance in the mixture are unchanged.

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6
Q

How can mixtures be separated?

A

Filtration, crystallisation, simple distillation, fractional distillation, and chromatography.

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7
Q

What were atoms thought of being before electrons were discovered?

A

Before the discovery of the electron, atoms were thought to be tiny spheres that could not be divided.

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8
Q

What did the plum pudding model suggest?

A

The plum pudding model suggested that the atom is a ball of positive charge with negative electrons embedded in it.

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9
Q

What did the alpha particle scattering experiment lead to?

A

The results from the alpha particle scattering experiment led to the conclusion that the mass of an atom was concentrated at the centre (nucleus) and that the nucleus was charged. This nuclear model replaced the plum pudding model.

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10
Q

What was Niels Bohr change about the nuclear model?

A

He adapted the nuclear model by suggesting that electrons orbit the nucleus at specific distances. The theoretical calculations of Bohr agreed with experimental observations.

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11
Q

What are the three subatomic particles in an atom, and what are their charges and masses?

A

Proton: Charge: 1 Mass: 1
Neutron: Charge: 0 Mass: 1
Electron: Charge: -1 Mass: Almost 0

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12
Q

What is an atomic number?

A

The number of protons in an atom of an element is its atomic number. All atoms of a particular element have the same number of protons.

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13
Q

What is an atoms mass number?

A

The sum of the protons and neutrons in an atom is its mass number.

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14
Q

What are isotopes?

A

Atoms of the same element can have different numbers of neutrons; these atoms are called isotopes of that element.

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15
Q

How are elements in a periodic table ordered?

A

They are arranged in order of their atomic numbers.

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16
Q

What is similar about the atoms in the same group of the periodic table?

A

Elements in the same group in the periodic table have the same number of electrons in their outer shell (outer electrons) and this gives them similar chemical properties.

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17
Q

Before the discovery of subatomic particles, how did scientists order the elements on the periodic table?

A

Before the discovery of protons, neutrons, and electrons, scientists attempted to classify the elements by arranging them in order of their atomic weights.

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18
Q

Why is the periodic table widely accepted by scientists today?

A

Elements with properties predicted by Mendeleev were discovered and filled the gaps. These correct predictions allowed scientists to believe Mendeleev’s table.

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19
Q

What are elements that form into positive ions?

A

Metals.

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20
Q

What are the elements that do not form positive ions?

A

Non-metals.

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21
Q

In which group are the noble gases?

A

Group 0 or Group 8.

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22
Q

Why are noble gases unreactive?

A

They are unreactive and do not easily form molecules because their atoms have stable arrangements of electrons. The noble gases have eight electrons in their outer shell, except for helium, which has only two electrons.

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23
Q

What are the group 1 metals known as?

A

The elements in Group 1 of the periodic table are known as the alkali metals.

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24
Q

Why do group 1 metals have specific characteristics?

A

They have characteristic properties because of the single electron in their outer shell.

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25
Q

What is the approximate size of an atom?

A

About 0.1 nanometers.

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26
Q

How does the number of protons relate to the number of electrons?

A

The number of electrons and the number of protons are the same.

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27
Q

If an ion has a 2- charge, how is it’s number of electrons different to protons?

A

It has two more protons than electrons.

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28
Q

What is the definition of an isotope?

A

Different forms of the same element, which have the SAME number of PROTONS, but a DIFFERENT number of NEUTRONS.

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29
Q

What is the difference between carbon 12 and 13?

A

Carbon-13 has one more neutron than carbon-12.

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30
Q

What is the formula for relative atomic mass?

A

sum of (isotope abundance x isotope mass number)
/
sum of abundances of all the isotopes.

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31
Q

How does ionic bonding work?

A

The metal atom loses electrons to form positive ions and the non-metal atom gains electrons to form negative ions. The opposite charges make them extremely attracted to each other. (the metal gives an electron).

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32
Q

How does covalent bonding work?

A

Each non-metal atom shares an electron with the other.

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33
Q

What is the formula for Sodium Carbonate?

A

Na2Co3

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34
Q

What is the formula for Ammonia?

A

NH3

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35
Q

What is the formula for Calcium chloride?

A

CaCl2

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36
Q

What is the difference between mixtures and compounds?

A

There’s no chemical bond between molecules in a mixture, there is in compounds.

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37
Q

Summarise the steps of paper chromatography.

A

1 - Draw pencil line at bottom of filter paper
2 - Add spot/s of ink on line
3 - Place paper in solvent (usually water)
4 - Solvent goes up paper (osmosis)
5 - Solvent brings dye with it - dye seperates.

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38
Q

What does filtration do?

A

Filtration seperates insoluble solids from liquids.

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39
Q

What are the two ways to seperate soluble solids from solutions?

A

Evaporation

Crystallisation

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40
Q

Describe the evaporation method of filtration.

A

Put solution in evaporating dish and heat, solvent will evaporate leaving crystals.

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41
Q

Describe the crystallisation method of filtration.

A

Pour solution in evaporating dish and heat a little, solution will concentrate and crystals start to form. Salt should start to form crystals once taken off heat as it becomes insolublein the cold highly concentrated solution. Then filter the crystals out.

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42
Q

What are the 4 processes of seperating rock salt?

A

1 - Grinding the mixture
2 - Dissolving it
3 - Filtering it
4 - Evaporating it

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43
Q

When is simple distillation used?

A

To seperate mixtures which contain liquids.

44
Q

What are the 3 main stages of simple distillation?

A
  • Solution is heated. Lowest boiling point evaporates 1st.
  • The vapour cools, condenses and is collected (CCC)
  • The rest of solution is left behind.
45
Q

What are the 5 main stages of fractional distillation?

A

1 - Put mixture in a flask and stick a fractionating column on top. Heat it.
2 - Different liquids have different boiling points, will evaporate at different temps.
3 - The liquid with the lowest boiling point evaps first. It will reach the top of the column.
4 - Liquids with higher boiling points may evaporate but will not reach top of column.
5 - Once first liquid has been collected, increase temp to get 2nd.

46
Q

What was the plum pudding model of the atom?

A

It showed the atom as a ball of positive charge with electrons stuck in it.

47
Q

How did Ernest Rutherford disprove the plum pudding model?

A

He used the famous alpha particle scattering experiments. From the plum pudding model they expected the particlats to pass straight through the gold sheet or be slightly deflected at most. Whilst most followed this idea, some were deflected more than expected, even backwards! Therefore the plum pudding model could no be right.

48
Q

What model did Ernest Rutherford come up with instead of the plum pudding model? And how?

A

The nuclear model of the atom, because of the results of his alpha particle scattering experiments, the alpha particles must have been deflecting backwards for a reason, and this reason was because of the NUCLEUS!

49
Q

What is another name for a shell (atoms)?

A

Energy levels.

50
Q

When are atoms much happier?

A

When they have FULL electron shells. In most atoms if the outer shell is not full this makes it want to fill it.

51
Q

Are most elements metals or non-metals?

A

Metals.

52
Q

What are the physical properties of metallic bonding?

A
  • Strong but malleable
  • Great conductors of heat and electricity.
  • High boiling and melting points.
53
Q

What are 3 properties of transition metals?

A
  • More than one ion
  • Often coloured - compounds more colourful
  • Often make for good catalysts.
54
Q

What are group 1 elements?

A

They are reactive, soft metals. They are alkali metals.

55
Q

What are the trends of alkali metals as you go down group 1?

A

1) Increasing reactivity as you go down (outer electron is more easily lost)
2) Lower melting and boiling points.
3) Higher relative atomic mass.

56
Q

What type of ions do group 1 metals make?

A

They readily form 1+ ions with non-metals!

57
Q

How do alkali metals react with water?

A

They react vigourously to produce hydrogen gas and metal hydroxides (salts that dissolve in water to produce alkaline solutions).

58
Q

How do alkali metals react with chlorine?

A

React vigourously and form white metal chloride salts.

59
Q

How do alkali metals react with oxygen?

A

The group 1 metals can react with oxygen to form a metal oxide. (Lithium oxide, Sodium oxide, Potassium peroxide etc.)

60
Q

What are the 2 main differences between group 1 metals and transition metals?

A
  • Group 1 metals are more more reactive.

- Much less dense, strong, and hard.

61
Q

What are the halogens?

A

Group 7 - All non-metals with coloured vapours!

62
Q

As you go down, what are the trends of the halogens?

A

1) Become less reactive - harder to gain extra electron because the outer shell’s further from nucleus.
2) Higher melting and boiling points.
3) Higher relative atomic masses.

63
Q

What do halogens form ionic bonds with? How so and what are they called?

A

Metals, they gain an electron (1- ion) and the metal loses an electron (1+). They are called halides.

64
Q

As you go down group 0, how do the boiling points differ?

A

They increase as you go down.

65
Q

What are ions?

A

Ions are charged particles. They can be single or groups of atoms!

66
Q

Why do atoms gain or lose electrons to form an ion?

A

All they are trying to do is get a full outer shell, which makes them much more stable, like a noble gas.

67
Q

What happens to metals when they form ions?

A

They lose electons from their outer shell to form POSITIVE ions!

68
Q

What happens to non-metals when they form ions?

A

They gain electrons to form NEGATIVE ions!

69
Q

What is the relation between the number of electrons lost or gained and the charge on the ion in ionic bonding.

A

They are the same! e.g is 2 electrons are lost the charge is 2+ (LP), or if 3 electrons a gained the charge is 3- (GL)

70
Q

What are the elements that most readily form ions?

A

Groups 1 & 2 and 6 & 7.

71
Q

What type of ions to group 1 elements form?

A

1+ ions.

72
Q

What type of ions to group 2 elements form?

A

2+ ions.

73
Q

What type of ions to group 6 elements form?

A

2- ions.

74
Q

What type of ions to group 7 elements form?

A

1- ions.

75
Q

What do dot and cross diagrams show?

A

They show how bonds are formed.

76
Q

RE-READ PAGE 49 OF TEXTBOOK ON DOT AND CROSSDIAGRAMS.

A

Whats the difference between a lampost and a firelighter? I don’t know why i thought of this joke lol hehehehehehhehehehehhehehehe

77
Q

What type of structure to ionic compounds have?

A

A regular/giant lattice structure.

78
Q

What are the 4 main traits of ionic compounds? (and explain them :D)

A
  • High melting and boiling points because of many strong bonds between the ions.
  • When solid, ions held in place so cannot conduct electricity.
  • When they melt the ions are free to move so they can conduct electricity.
  • Some can dissolve in water, free to move and therefore can carry an electric current!
79
Q

What is an empirical formula?

A

It is a formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms. For example, K2O or CsCl.

80
Q

How do you work out the empirical formula of a ionic compound?

A
  • Look at a/the diagram to work out what ions are in the compound. (K ion and O ion).
  • Work out what charges the ions will form (e.g K would form 1+ or Oxygen - 2- ions)
  • Balance the charges so the charge of the emperical formula is 0. (K2O)
81
Q

What happens to electrons in covalent bonding?

A

They are shared between the two or more atoms that are bonding.

82
Q

What diagrams can be used to show the bonding in covalent bonds?

A
  • Dot and cross diagrams - Electrons drawn in the overlap of the orbitals are shared between two atoms.
  • Displayed formulas
  • 3D Model of covalent bonds.
83
Q

Advantages and disadvantages of dot and cross diagrams?

A

Good at showing which atoms the electrons in a covalent bond come from, but don’t sow the relative sizes of the atoms or how the atoms are arranged in space.

84
Q

Advantages and disadvantages of displayed formulas diagrams?

A

Great way of showing how atoms are connected in large molecules, however they don’t show the 3D structure of the molecule or which atoms the electrns in the covalent bond have come from.

85
Q

Advantages and disadvantages of 3D model diagrams?

A

Hrood at showing the atoms and the covalent bonds arrangement in space next to each other, buy cna quickly get confusing for large molecules, and they don’t show where the electrons in the bonds have come from either.

86
Q

What is the formula for methane?

A

CH4

87
Q

What are the properties of simple molecular structures? (usuallly substances containing covalent bonds)

A
  • To melt/boil a substance, only need to break weak intermolecular forces and not bonds, so melting and boiling points are looooooooooow.
  • Most are gases or liquids at room temperature.
  • As they get bigger, more energy needed to break the forces, higher boiling/melting points.
  • Don’t conduct electricity, no charge.
88
Q

What are polymers?

A

Polymers are long chains of repeating units (monomers)

89
Q

What are the intermolecular forces of polymers like?

A

They are larger/stronger than simple covalent molecules, so more energy is needed to break them apart. Most polymers are solid at room temp. They are still weaker than covalent and ionic bonds tho.

90
Q

How do you write the molecular formula for a polymer?

A

Write down the moleculare formula of the repeating unit (e.g C2H4) and put them in brackets with an n on the outside!

e.g: (C2H4)n

91
Q

How are giant covalent structures bonded together?

A

Each atom is bonded together by strong covalent bonds! This makes their melting/boiling points very high as a lot of energy is needed to overcome the bonds.

92
Q

Name 3 examples of giant covalent bonds and what are their properties?

A
  • Diamond (Carbon atoms, all bonded together, 4 bonds)
  • Graphite (Carbon atoms, layers, delocalised electrons as each carbon atom only bonds 3 times not 4)
  • Silicon dioxide (like diamond but with silicon and oxygen)
93
Q

Why does graphite conduct electricity?

A

Only 3 out of carbon’s 4 outer electrons are bonded in graphite, which leaves 1 electron free (delocalised) and therefore can conduct electricity and thermal energy

94
Q

What is graphene? And how thick is it?

A

Graphene is a single layer of graphite! It is just one atom thicc.

95
Q

What is buckminsterfullerene?

A

It is the first fullerene to be discovered. It is a hollow sphere of carbon atoms, with the molecular formula C60.

96
Q

What are some uses of fullerenes?

A
  • Fullerenes can be used to essentially trap other molecules inside them, can be used to deliver drugs into the body.
  • Huge surface area - great industrial catalysts.
  • Make great lubricants.
97
Q

What are the allotropes of carbon we need to know?

A

Diamond;
Graphite;
Graphene;
Buckminsterfullerene.

98
Q

What are 3 properties of metal?

A
  • Most are solid at room temperature.
  • Good conductors of electricity and heat.
  • Most metals are malleable.
99
Q

What are alloys and why are they stronger than pure metals?

A

Alloys are a mixture of 2 or more metals, and they are stronger than pure metals because of the different sized atoms. When another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms, making it more difficult for them to slide over each other!

100
Q

What produce all the properties of metals?

A

Their delocalised electrons.

101
Q

How does metallic bonding work?

A

Metals are giant structures with delocalised electrons. There are strong forces of electrostatic attraction between the +metal ions and the -electrons. These forces of attraction hold the atoms together in a regular structure. This is very strong.

102
Q

What are the 3 things that change how strong the forces are between the particles of the material? (SLG)

A
  • the material
  • the temperature
  • and the pressure!
103
Q

What does aqueous mean?

A

Dissolved in water.

104
Q

How small are nanoparticles?

A

About 1 x 10^-9 m or 1nm

105
Q

Surface area to volume ratio = …?

A

surface area / volume

106
Q

What are the uses of nanoparticles?

A
  • Huge surface area to volume ratio, can be used as catalysts.
  • ## Nanomedicine - could deliver drugs where needed.

AA Chemistry (3 decks)

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