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Year 10 Chemistry > Unit 1 chemistry > Flashcards

Unit 1 chemistry Flashcards

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1
Q

Arrangement in a Solid?

A

Fixed and compact (all touching and must be organized/fixed in a line)

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2
Q

Movement in a Solid?

A

Vibrating

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3
Q

Energy Level in a Solid?

A

Low

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4
Q

Arrangement in a Liquid?

A

Spaced (some are still touching each other but some aren’t and they are fairly close to each other)

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5
Q

Movement in a Liquid?

A

Free (slow)

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6
Q

Energy level in a liquid?

A

Medium

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7
Q

Arrangement in a Gas?

A

Random (free)

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8
Q

Movement in a Gas?

A

Free to move

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9
Q

Energy level in a Gas?

A

High

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10
Q

What is DIffusion?

A

It is the movement of gasses from a high concentration (lots of them in a certain volume) to a low concentration (there are lower amount of them in a certain volume)

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11
Q

What are the factors that affect diffusion and how do they affect it?

A

1) The concentration gradient (greater gradient, fast)
2) The Surface area (Greater SA, fast)
3) Length of diffusion pathway (Greater pathway, SLOWER)
4) Higher temp (high temp, fast because more kinetic energy)

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12
Q

What causes diffusion?

A

In gasses and liquids, particles move freely which causes them to collide with each other (or with their container) and this makes them change directions which causes particles to spread around a place (or container)

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13
Q

Explain the process of a solid to a liquid

A

This is called melting. You do this by heating a solid until it melts. When a solid is heated, particles gain kinetic energy which lets them vibrate faster. When the temperature is high enough, the vibration becomes strong enough to overcome forces of attraction in a solid which lets them move freely and slide past each other.

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14
Q

Explain the process of liquid to solid

A

This is called freezing. You do this by cooling a liquid until it freezes. When a liquid is cooled, the particles lose their kinetic energy and when the temp is low enough, the particles don’t have any more energy to slide past each other, and the forces of attraction hold particles together.

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15
Q

Explain the process of a liquid to a gas

A

This is called evaporation. You do this by heating a liquid until it boils. As it is heated, particles gain kinetic energy, and move further apart and forces of attraction in the liquid are then broken.

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16
Q

Explain the process of a gas to a liquid

A

This is called condensation. You do this by cooling the gas until it condenses and when the gas is cooled, the particles lose kinetic energy, and forces of attraction between particles become weaker so they are now just close enough like a liquid

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17
Q

Explain process of a solid to a gas

A

This is called sublimation. You do this by heating the solid until it sublimes and the solid particles gain energy which lets them vibrate faster and the forces of attraction are completely broken between the particles and become a gas

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18
Q

What is an element?

A

A substance made up of only 1 type of atom

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19
Q

What is a compound?

A

A substance made up of 2 or more different elements which are chemically bonded

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20
Q

What is a mixture?

A

A combination of 2 or more substances that are physically mixed but not chemically bonded (substance is classified as a mixture as long as the 2 substances are NOT chemically bonded so it doesn’t matter if they can dissolve with each other or not, if not chemically bonded then it is classified as a mixture)

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21
Q

Mixtures vs compounds - Are the elements bonded to each other?

A

Mixture - No they aren’t
Compound - Yes they are

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22
Q

Mixtures vs compounds - Properties?

A

Mixture - Elements still have their own properties
Compound - Has its own unique properties (different to elements)

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23
Q

Mixtures vs compounds - Chemical formula?

A

Mixture - Atoms can be in any ratio
Compound - Formula is fixed with atoms in fixed ratios

24
Q

Mixtures vs compounds - Is it easy to separate elements and why?

A

Mixture - Easy to separate elements as atoms are not bonded together
Compound - Very hard to separate elements as atoms are bonded together

25
Q

Mixtures vs compounds - Methods used to produce them

A

Mixture - Filtration, distillation, chromatography, funnel, etc
Compound - Thermal decomposition, Electrical decomposition (electrolysis)

26
Q

What is simple distillation and how do you do it?

A

We use simple distillation to separate a liquid from a soluble solid in a solution (dissolved). The solution is heated and the liquid turns into vapour as it evaporates and rises. Vapour will pass through a condenser and it cools down later and condenses into a liquid which is then collected in a beaker. All the liquid is now evaporated and a solute is left. An example of this experiment is separating water from salt.

27
Q

What is fractional distillation and how do you do it?

A

We use fractional distillation to separate 2 or more liquids that are miscible (capable of being mixed together). The solution is heated at temp of substance with the lowest boiling point and this causes one of the liquids to evaporate up through a fractionating column which is filled with lots of glass rods and is cold at the top (some of the other liquid with high boiling point will also evaporate but when it goes up, the cool temp cools it down so it wont go all the way up) and only the vapour with low boiling point will pass though a condenser where it cools down and condenses which turns into a liquid and is collected in a beaker and this leaves a substance or mixture behind. An example for this experiment is separating water from ethanol.

28
Q

What is filtration and how do you do it?

A

We use filtration to separate insoluble solids from liquids in a mixture (not dissolved). We first need to put a funnel with filter paper on top of a conical flask and then pour the substance into the funnel. The filter paper will only allow small liquid particles to pass the funnel and it will filter out large solid particles as they stay behind. The substance left behind is called the residue and the liquid is the filtrate. An example of this experiment is separating tea leaves from water.

29
Q

What is crystalization and how do you do it?

A

We use crystalization to separate a solute from a solvent (dissolved because it separates a solution). First place your substance into an evaporation dish and put it into a water bath to heat it. Some of the solvent will then evaporate and then crystals start to form in the solution so you then stop heating it and leave it to cool. More crystals will form because solids are less soluble at colder temperatures. Then filter out crystals using filtration method and then dry your crystals.

30
Q

What is chromatography and how do you do it (important) ?

A

We use chromatography to separate substances that have different solubilities (dissolved because it separates a solution). Take a piece of filter paper and use a pencil to draw a line near the bottom of the sheet, then put a dot of sample of ink to pencil line. Then fill a beaker with a shallow amount of solvent. Place filter paper in beaker with solvent but don’t submerge the pencil line and ink. Also place a lid on top of beaker to stop solvent from evaporating. Solvent and ink will move up and the place where solvent stops moving is called a solvent front (draw a line). Different dyes that make up ink will also move up with solvent, the dyes move at different speeds which shows that each one is a different substance (dye with higher solubility moves faster) and this shows us components of the ink/dye.

31
Q

Chromatography - What is the stationary phase?

A

The paper because it doesn’t move

32
Q

Chromatography - What is the mobile phase?

A

The solvent because it moves

33
Q

How does a chromatogram (the pattern produced on paper) provide information about the composition of a mixture?

A

It shows the components of a mixture as they travel at different speeds which makes then get separated on the paper and the number of spots indicate the amount of compositions in the original mixture. The Rf value also indicates the distance each substance travels and the colour and size also indicate their identity.

34
Q

Chromatography - Why do samples move at different speeds during the experiment?

A

Different substances have different forces of attraction/affinities for the mobile and stationary phases. A substance with stronger attraction to mobile phase will move faster and closer with the solvent front whilst a substance with a weaker attraction to mobile phase but stronger attraction to stationary phase (paper) will move slower and further away from solvent front.

35
Q

What is an Rf value and what is the formula?

A

An Rf value shows how far a substance moves compared to the solvent. The Rf value is also very specific to a compound so you can identify a compound in an unknown mixture. (main important one)

Formula:
Distance travelled by substance
RF = ———————————————-
Distance travelled by solvent

36
Q

Where is the proton located, whats its charge, and whats its mass?

A

Location = Nucleus
Charge = 1+
Mass = 1

37
Q

Where is the neutron located, whats its charge, and whats its mass?

A

Location = Nucleus
Charge = Neutral (no charge)
Mass = 1

38
Q

Where is the electron located, whats its charge, and whats its mass?

A

Location = Electron shell
Charge = 1-
Mass = Negligible

39
Q

What does the mass number represent?

A

Represents number of protons + neutrons

40
Q

What does the atomic number represent?

A

Represents number of protons

41
Q

How do you find the number of protons, neutrons and electrons from an element on periodic table?

A

Proton = Atomic number
Electron = Atomic number
Neutron = Atomic mass - Atomic number

42
Q

Definitions of:
- Atom
- Molecule

A
  • Atom = Smallest particle of element
  • Molecule = Atoms join together by chemical bonds
43
Q

What is an isotope?

A

2 or more atoms of the same element which have same atomic number but different mass numbers which means that they have same number of protons but different number of neutrons between the 2 atoms of same element

44
Q

What is the formula for average atomic mass for isotopic abundances?

A

Formula:
Ar of element =
(mass 1 x abundance%) + (mass 2 x abundance%) / 100

45
Q

Definition of abundance?

A

Relative amount of an element or isotope present in a sample. (usually as percentage)

46
Q

Definition of solute?

A

Substance that is dissolved in a solvent to form a solution (usually smaller amount than solvent and usually in all 3 states of matter)

47
Q

Definition of solvent?

A

Substance that dissolves a solute to form a solution (usually liquid and in larger amounts than a solute)

48
Q

Definition of solution?

A

A mixture of a solute dissolved in a solvent (must be dissolved to be called a solution and this is a type of mixture so they are not chemically bonded)

49
Q

Definition of soluble?

A

When a substance can dissolve in a solvent

50
Q

Definition of solubility?

A

Ability of a solute to dissolve in a solvent

51
Q

Definition of insoluble?

A

Substance that doesn’t dissolve in a solvent

52
Q

Definition of saturated?

A

Something which has a maximum amount of solute as it can hold so if you add more, it wont dissolve

53
Q

Definition of unsaturated?

A

Something which CAN dissolve more solute because theres room for it

54
Q

Explain the dilution of coloured solutions

A

When you dilute a solution, the particles which give its colour start to spread out and as they start to spread, the colour becomes more lighter as the colours intensity starts to decrease because the concentration of the particles in each part of the liquid is lower. More you dilute, the weaker the colour intensity is so now theres a lighter colour.

55
Q

Definition of dilute/dilution?

A

It is when you reduce the concentration of a substance by adding more solvent. Example: adding more water to orange juice makes the colours concentration weaker and also makes taste weaker.

56
Q

Explain why a pure substance has a fixed melting and boiling point but a mixture doesn’t.

A

A mixture contains 2 or more different substances and because of this, mixtures don’t have a fixed melting or boiling points as their melting and boiling point temperatures depend on the proportions of each substance

57
Q

What is meant by the term:
“solubility in g/per 100g of solvent” ?

A

It means the maximum mass of solute that is dissolved in 100g of solvent

Year 10 Chemistry (1 decks)

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