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Chemistry mock > Particles and mixtures > Flashcards

Particles and mixtures Flashcards

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1
Q

what are the 3 states of matter

A

solid, liquid, and gas

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2
Q

how strong forces are depend on what 3 things?

A
  • material
  • temperature
  • pressure
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3
Q

do particles move in a solid? why?

A
  • no they don’t move.

- they don’t move so that the solid can keeps its definite shape and volume.

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4
Q

how strong are the forces of attraction between particles in solids? why?

A
  • the forces of attraction is solids are strong.

- this force causes the particles to be close together in fixed positions to form a very regular lattice arrangement.

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5
Q

do particles vibrate about their position in a solid? why?

A
  • yes, they vibrate about their position.

- because as a solid gets hotter, the more the solid vibrates (causing solids to expand slightly when heated).

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6
Q

how strong are the forces of attraction between particles in liquids? why?

A
  • the force of attraction between liquids is weak.
  • this is because they are randomly arranged and free to move past each other, but they do tend to stick closely together.
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7
Q

do liquids have a definite volume and shape?

A
  • liquids do have a defined volume

- liquids don’t have a defined shape

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8
Q

how do particles move in a liquid?

A

they constantly move with a random motion.

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9
Q

what happens when a liquid is heated?

A

the hotter a liquid gets, the faster they move. This causes liquids to expand slightly when heated.

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10
Q

how strong are the forces of attraction between particles in gases? why? how do they travel?

A
  • the force of attraction between the particles in gases is very weak.
  • they are free to move but they move far apart.
  • particles in gases travel in a straight line.
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11
Q

do gases have a definite volume and shape?

A
  • they don’t have a definite shape or volume and it will always feel any container.
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12
Q

how do particles move in a gas?

A
  • the particles move constantly with random motion.
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13
Q

what happens when a gas is heated?

A
  • when a gas is heated the faster it moves.

- particles either expand when heated or their pressure increases

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14
Q

do physical changes change particles?

A

no it just changes the arrangement on their energy

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15
Q

what is the cycle of the change of one state to another? (there are 6 points)

A
  1. when a solid is heated, its particles gain more energy.
  2. this makes its particles vibrate more which weakens the force that hold the solid together, this makes the solid expand.
  3. at a certain temperature, the particles have enough energy to break free from their positions. This is called melting, the solid turns into a liquid.
  4. when a liquid is heated, their particles get even more energy.
  5. this energy causes particles to move faster, which weakens and breaks the bonds holding the liquid together.
  6. at a certain temperature, particles have enough energy to break their bonds. This is called evaporating and the liquids turns into gas.
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16
Q

what is the process of a solid turning into gas called?

A

subliming.

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17
Q

what is the process of a solid turning into liquid called?

A

melting

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18
Q

what is the process of a liquid turning into gas called?

A

evaporating

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19
Q

what is the process of a gas turning into liquid called?

A

condensing

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20
Q

what is the process of a liquid turning into solid called?

A

freezing

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21
Q

what is diffusion?

A

it is the gradual movement of particles from places where there are lots of them to places where there are fewer of them. It is the natural tendency for stuff to spread out.

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22
Q

how to test for diffusion? (in this test we will use potassium manganate)
there are going to be 3 points made

A
  1. take a beaker of water and place some potassium manganate at the bottom of it, the purple colour will slowly spread out to fill the beaker.
  2. the chemicals in the particle potassium manganate are diffusing out among the particles of water.
  3. it is the random motion of the particles in a liquid that causes the purple colour to eventually be evenly spread out through the water.
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23
Q

what is dilution?

A

when you add more water to the solution

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24
Q

what is a mixture?

A

it is a solution of solvent and dilute

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25
Q

what is a solution?

A

a mixture of a solute and a solvent that does not separate out.

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26
Q

what is a solute?

A

a substance being dissolved

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27
Q

what is a solvent?

A

what the liquid is dissolving into

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28
Q

what is a saturated solution?

A

it is where the maximum amount of solute has been dissolved, so no more solute will dissolve in the solution

29
Q

what are the 3 subatomic particles atoms contain?

A
  • protons
  • neutrons
  • electrons
30
Q

describe protons

A

they are heavy and positively charged

31
Q

describe neutrons

A

they are heavy and neutral

32
Q

describe electrons

A

they have hardly any mass and are negatively charged

33
Q

what is a nucleus (tell me 5 facts about it)

A
  • it is the middle of the atom
  • it contains protons and neutrons
  • it has a positive charge because of the protons
  • almost the whole mass of the atom is concentrated in the nucleus
  • compared to the overall size of the atom, the nucleus is tiny.
34
Q

what are electrons (tell me 5 facts about it)

A
  • electrons move around the nucleus in energy levels called shells.
  • they are negatively charged
  • they are tiny, but their orbitals cover a lot of space
  • the size of their orbitals determines the size of the atom
  • electrons have virtually no mass
35
Q

do neutral atoms have any charge?

A

no they don’t have any charge overall

36
Q

what is the charge size of electron equal to?

A
  • the charge of electrons is the same size is equal to the number of protons (but the opposite)
  • this means the number of electrons always equals the number of protons in a neutral atom
37
Q

what happens if some electrons are added or removed from an atom

A

the atom becomes charged and is then an ion

38
Q

the number of electron is equal to what?

A

it is equal to the number of protons

39
Q

what does the atomic number and atomic mass describe?

A

it describes an atom

40
Q

what does the atomic number tell you?

A

how many protons there are

41
Q

what do atoms of the same element have the same number of?

A
  • it has the same number of protons.

- this means that with different elements will have different numbers of protons.

42
Q

what is the mass number total to?

A

it is total of protons and neutrons in the atom

43
Q

how do you get the number of neutrons?

A

subtract the atomic number from the mass number.

44
Q

what are molecules

A

they are group of atoms

45
Q

what can atoms do to form molecules

A

they can join together

46
Q

how many elements molecules can be made of?

A

it can be made up of 1 or more
e.g
1 element = H2, N2
2 elements = H2O, CO2

47
Q

what are isotopes?

clues to remember how to answer this:

  • isotopes must have the same proton number but different mass numbers.
  • if they had different proton number, they’d be different elements altogether
  • e.g of isotopes: carbon- 12, carbon-13
A

isotopes are different atomic forms of the same element, which have the same number of protons but different number of neutrons.

48
Q

what is relative atomic mass (Ar)?

A

how heavy different atoms are compared with the mass of an atom of carbon-12

49
Q

what is relative abundance?

A

it is how much there is of each isotope compared to the total amount of the element in the world. This can be a ratio, a fraction or a percentage

50
Q

how to calculate the relative atomic mass?

A
  • multiply the mass of each isotope by its relative abundance.
  • add those together.
  • divide by the sum of the relative abundances
51
Q

what is a compound?

A

it is a substance made of two or + different elements which are chemically joined (bonded) together.

52
Q

which one is harder to separate mixtures or compounds?

A

compounds

53
Q

what are the properties of a mixture?

A

the properties of a mixture is the mixture of the properties of the separate parts

54
Q

what causes a substance not to be pure?

A

if it is not made up of a single element or compound.

55
Q

what do pure substance have? (related to temperature)

A

specific melting and boiling points.

56
Q

why are mixtures not pure?

A

because it will melt or boil gradually over a range of temperatures.

57
Q

why do we use Simple distillation?

A

to separate a liquid from a solution (e.g water from a solution of salt water)

58
Q

how to do Simple distillation?

A
  • Solution is heated and water vapors will rise and evaporate
  • Water vapors pass through the condenser where it cools and condenses, turning into a liquid that is collected in a beaker.
  • After all water is evaporated from solution, solute will be left behind
59
Q

why do we use Fractional distillation?

A

to separate 2 or more liquids that are mixed with one another (E.g Ethanol and Water from a Mixture of the Two).

60
Q

how to do Fractional distillation?

A
  • Solution is heated to the temperature of the substance with the lowest boiling point and vapors of this substance will rise and evaporate.
  • Vapors pass through a condenser where it cools and condenses, turning into a liquid that is collected in a beaker.
  • After all of the substance is evaporated and collected, a mixture of substance will be left behind.
61
Q

why do we use Filtration?

A

To separate an undissolved solid from a mixture of the solid and a liquid / solution ( E.g Sand from a mixture of Sand and Water)

62
Q

how to do Filtration?

A
  • Filter paper is placed in a filter tunnel, which is placed above another beaker
  • A mixture of insoluble solids and liquids is poured into the filter tunnel, which only allows small liquids particles to pass through as filtrate
  • Solid particles are too large to pass through as filtrate, so this particles will stay behind as residue
63
Q

why do we use Crystallization?

A

to separate a dissolved solid from a solution (solids are more soluble in hot solved than in cold ones) (e.g copper sulphate from a solution of copper sulphate in water)

64
Q

how to do Crystallization?

A
  • The solution is heated, allowing solvent to evaporate and leave a saturated solution
  • The saturated solution is left to cool down, and solids will start coming out of the solution to grow into crystals
  • Crystal are collected and allowed to dry
65
Q

why do we use Paper chromatography?

A

to separate substances that have different solubilities in a given solvent (e.g different coloured inks mixed to form black ink)

66
Q

how to do Paper chromatography?

A
  • Draw a line with a pencil on chromatography paper and the concentrated spot of ink/dye is placed on it.
  • Lower the paper into a bucket of solvent, which allows the solvent to travel up the paper taking the particles of coloured substances with it.
  • Different substances have different solubilities so the solvent will travel at different rates, causing the substance to be spread along the vertical length of paper.
  • This will show the different components of the ink/ dye.
67
Q

how does chromatogram provide information about the composition of a mixture?

A
  • Chromatogram shows the composition of a mixture as different coloured substances. It will spread apart as they have different solubilities so it will travel at different rates.
  • Pure substances will only produce one spot on a chromatogram during paper chromatography.
68
Q

how to calculate Rf values?

A

Rf = distance of dye from baseline/ distance of solvent front from baseline

69
Q

Practical: investigate paper chromatography by using inks/food colourings
(there are 6 points you need to make for this question)

A
  1. Draw a line 1 cm (baseline) from the bottom of the paper (use pencil not ink. Ink dissolves into the solvent and a pencil doesn’t).
  2. One drop of dye of each sample must be dropped at different points along the baseline.
  3. The paper must be then suspended in a beaker which contains a small amount of solvent. The bottom of the paper must be touching the solvent , but the baseline with the dyes should be above the level of the solvent (this is so that the dryer doesn’t simply dissolve into the solvent in the beaker).
  4. Put a lid to cover the beaker so that the atmosphere becomes saturated with the solvent (and so that the solvent does not evaporate from the surface of the beaker).
  5. When the solvent is near the top, the paper should be removed from the solvent and a pencil line drawn (and labelled) should reach up the paper. This is called the solvent font.
  6. The chromatography is then left to dry so that all the solvent evaporates.

Chemistry mock (3 decks)

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