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Chemistry Flashcards

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1
Q

Describe the properties of metals. (7)

A

Lustrous (1)
High melting points (1)
High boiling points (1)
Good conductors of electricity (1)
Good conductors of heat (1)
High density (1)
Malleable and ductile (1)

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2
Q

Are Metals
Oxides basic (alkaline)?

A

Yes.

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3
Q

Describe the properties of non - metals (7)

A

Dull (1)
Low melting points (1)
Low boiling points (1)
Poor conductors of electricity (1)
Poor conductors of heat (1)
Low density (1)
Brittle (1)

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4
Q

Are nonmetals oxides acidic (1)

A

Yes (1)

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5
Q

List the Reactivity Series and include carbon. (14)

A

Potassium (1)
Sodium (1)
Calcium (1)
Magnesium (1)
Aluminium (1)
(Carbon) (1)
Zinc (1)
Iron (1)
Lead (1)
(Hydrogen) (1)
Copper (1)
Silver (1)
Gold (1)
Platinum (1)

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6
Q

Define an ore and give some examples. (4)

A

Ores are naturally occurring rocks that contain metals or metal compounds in sufficient amounts to make it worthwhile extracting them. (1)
Iron ore (1)
Magnetite (1)
Platinum (1)

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7
Q

How metals are extracted from their ores using different
methods depending on their place on the reactivity
series.

A

Metals more reactive than carbon, such as aluminium, are extracted by electrolysis, (1)

While metals less reactive than carbon, such as iron, may be extracted by reduction with carbon. (1)

As gold is so unreactive, it is found as the native metal and not as a compound. It does not need to be chemically separated. (1)

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8
Q

Thermal Decomposition. (1)

A

Thermal decomposition is a chemical reaction that happens when a compound breaks down when heated.. (1)

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9
Q

Reactions of Metals with, oxygen, water and acid.

A

Water
When a metal reacts with water, a metal hydroxide and hydrogen are formed. (1)

Oxygen
Many metals react with oxygen to form metal oxides. (1)

Acids
Acids react with most metals. · When an acid reacts with a metal, the products are a salt and hydrogen. (1)

EXAMPLES on PPT pg 39, 40, 42

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10
Q

What is the test for Oxygen?

A

Oxygen supports combustion. If oxygen is present in a test tube, a glowing splint relights when it is held inside. (1)

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11
Q

Displacement reactions and how to write out the relevant
word equations.

A

In displacement reactions a more reactive metal will displace a less reactive metal from its compound. (1)

Iron + copper sulfate → copper + iron sulfate. (1)

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12
Q

Define an atom and element, giving examples. (4)

A

Atoms are the building blocks of everything. (1) Hydrogen Atom (1)

An element is a substance that is made up of only one kind of atom. (1) Hydrogen (1)

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13
Q

Structure of an atom and a brief description of the sub
atomic particles; protons, neutrons, and electrons. (5)

A

Atoms are made up of three smaller particles called protons + (1), electrons -(1) and neutrons o (1).
(+, - and o: represent charge)

The protons and neutrons are contained in the nucleus, the tiny centre of an atom, (1) with smaller electrons orbiting outside the nucleus (1).

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14
Q

Recognise the most common elements from the periodic
table and their symbols. (6)

A

Hydrogen (1) H (1)
Helium (1) He (1)
Iron (1) Fe (1)
…

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15
Q

Define a mixture and give examples. (4)

A

A mixture is formed when two or more elements or compounds are present without being chemically bonded together. (1)

Peas + Sweetcorn (1)
Mixture of Sweets (1)
Mixure of Coins (1)

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16
Q

Distinguish between a solute, solvent and solution. (3)

A

A solution is made when a substance dissolves into a liquid. (1) The liquid is called the solvent. (1) The substance that has been dissolved is called the solute. (1)

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17
Q

Describe how to separate mixtures using filtration. Be able to fully label a diagram of filtration. (2)

A

Filtration is a method for separating an insoluble solid from a liquid. When a mixture of sand and water is filtered:

  1. The sand stays behind in the filter paper (it becomes the residue)
  2. The water passes through the filter paper (it becomes the filtrate)
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18
Q

Describe how to separate mixtures using evaporation. Be able to fully label a diagram of evaporation. (2)

A

Evaporation is used to separate a soluble solid (i.e. a solid that dissolves) from a liquid.

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19
Q

Describe how to separate mixtures using simple distillation. Be able to fully label a diagram of distillation. (2)

A

Simple distillation is a method for separating the solvent from a solution. (2)

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20
Q

Describe how to separate mixtures using fractional distillation. Be able to fully label a diagram of fractional distillation. (2)

A

Fractional distillation is a method for separating a liquid from a mixture of two or more liquids.

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21
Q

Describe how to separate mixtures using chromatography. Be able to fully label a diagram of chromatogrophy. (2)

A

Paper chromatography is a method for separating dissolved substances from one another.

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22
Q

Define a compound and give examples of common
compounds.

A

A compound is a pure substance that is made from more than one element. In a compound, elements are chemically bonded together, which makes it very difficult to separate them. (1)
Water - H2O (1)
Carbon Dioxide - CO2 (1)
Sodium Chloride - NaCl (1)

23
Q

Does a chemical reaction must occur for a compound to occur? (1)

A

Yes. (1)

24
Q

Define a chemical change and give examples of chemical
changes. (3)

A

A chemical change is a change of materials into another, new materials with different properties and one or more than one new substances are formed. (1)

Wood Burning. (1)
…

25
Q

List some ways you can observe a chemical reaction has
taken place. (3)

A

Bubbles – Many chemical reactions you see in the science lab make a chemical which is a gas, so you see bubbles. (1)

A colour change – If the new chemicals are a different colour from the original chemicals, there will be a colour change. (1)

A large energy change – Many chemical reactions give off lots of energy, like burning, and a few absorb energy, so they feel cold. (1)

26
Q

How to write a word equation and what a reactant and a
product are. (4)

A

A word equation represents a chemical reaction using the names of the substances involved. Word equations do not show any chemical symbols or formulae. (1) The reactants are on the left of the chemical equation, and the products on the right. (1)

In a chemical reaction, reactants are the substances that react together, and products are the substances formed. (1)

27
Q

How to name compounds, ‘ide’ and ‘ate’ and the
exceptions of diatomic elements such as chlorine. (9)

A

When 2 elements mix their name ends with -ide.

Iron + Oxygen → Iron Oxide (1)

When 3+ elements mix and one is Oxygen, their name ends with - ate.

Copper + Sulphur + Oxygen→ Copper Sulphate. (1)

Diatomic elements are not compunds! They are elements that are rarely found separate in nature. They are:

Hydrogen, Nitrogen, Flourine, Oxygen, Chlorine, Iodine, and Bromine. (7)

28
Q

State the Conservation of Mass in a reaction. (1)

A

The Conservation of Mass states that no atoms are created or destroyed in a chemical reaction. The total mass of the products in a chemical reaction will be the same as the total mass of the reactants. (1)

29
Q

Write word equations for combustion and incomplete
combustion. (2)

A

Complete combustion reaction is:
Fuel + O2 → CO2 + H2O. (1)

Incomplete combustion is:
Fuel + O → CO + C + H2O. (1)

30
Q

Label the Bunsen burner and how to light and use it
safely. (7)

A
  1. Make sure there are no breaks or holes in the gas hose.
  2. Ensure lab rules.
  3. Put the Bunsen burner on a heat-resistant mat, making sure it isn’t near the edge of the bench.
  4. Turn the collar to ensure the air hole of the Bunsen burner is closed.
  5. Hold a lit splint 1-2 cm above the top of the barrel of the burner.
  6. Turn on the gas at the gas tap, and the Bunsen burner will burn with a yellow flame.
  7. Extinguish the splint and place it on the heat-resistant mat. (7)

Use BBC BITESIZE for image (2)

31
Q

Distinguish between a control, independent and dependent variable. (3)

A

Independent variables – the variable that is being changed during the experiment. (1)

Dependent variables – the variable being tested or measured during the experiment. (1)

Control variables - the variable that you do not change during an experiment. (1)

32
Q

Draw and label the most common apparatus used in
chemistry

A

Beaker:

A cylindrical container with a flat bottom and a lip for pouring. It is used for mixing, stirring, and heating liquids.
Flask (Erlenmeyer Flask):

A conical-shaped container with a narrow neck. It is used for titration, mixing, and holding liquids.
Test Tube:

A small cylindrical tube with an open top. Used for holding, mixing, and heating small quantities of liquids.
Burette:

A long, graduated tube with a stopcock at the bottom. It is used for delivering precise volumes of liquid in titrations.
Pipette:

A slender tube used to transfer small amounts of liquid. There are different types, such as volumetric pipettes and micropipettes.
Graduated Cylinder:

A tall, narrow cylinder with calibrated markings for measuring volumes of liquids.
Funnel:

A cone-shaped device with a narrow neck, used to channel liquids into containers with smaller openings.
Evaporating Dish:

A shallow, flat-bottomed dish used for evaporating liquids to leave behind solutes.
Watch Glass:

A circular, flat glass dish with a slight lip. It is used as a cover for beakers or evaporating dishes and for holding small amounts of substances.
Crucible and Cover:

A small, heat-resistant container with a lid used for heating substances to high temperatures.
Mortar and Pestle:

A pair of tools used to grind and mix substances into a fine powder.
Bunsen Burner:

A gas burner used for heating, sterilization, and combustion reactions in the laboratory.
Thermometer:

An instrument used to measure temperature.
Retort Stand and Clamp:

A support structure with a clamp used to hold glassware and other apparatus securely.
Centrifuge:

A machine used to separate components of a liquid mixture based on their densities, typically used in biochemistry and molecular biology.
These are just a few examples of the many apparatus used in chemistry laboratories. Each piece serves a specific purpose in carrying out experiments, measurements, and analyses.

33
Q

Define matter and state the particle theory. (2)

A

Matter is anything which occupies space and has a mass. (1)

The particle theory of matter is a model that describes the arrangement and movement of particles in a substance. The model is used to explain the physical properties of solids, liquids and gases. (1)

34
Q

Distinguish between the three main states of matter, solid, liquid and gas in terms of their particle arrangement. Give examples of each. (4)

A

PPT 4 (3)

Ice - Solid: Water - Liquid: Steam - Gas (1)

35
Q

What is a physical change? (1)

A

A physical change is when substance changes without becoming a new chemical. It can be reversed easily. (1)

36
Q

Define melting, boiling, evaporation, condensation
freezing and sublimation. (5)

A

Melting is when a solid turns into a liquid. (1)

Boiling is when bubbles of gas form throughout the liquid. (1)

Evaporation is when a liquid turns into a gas. (1)

Freezing is when a liquid turns into a solid. (1)

Sublimation is when a solid turns straight into a gas. (1)

PPT 4 for more info.

37
Q

Define boiling and melting point. (2)

A

A boiling point is the temperature at which a liquid changes into a gas. (1)

A melting point is the temperature at which a solid changes into a liquid. (1)

38
Q

Is energy (usually thermal energy)
required for a change of state to occur? (1)

A

Yes. (1)

39
Q

Define diffusion. (1)

A

Diffusion is the movement of a substance from an area of high concentration to an area of lower concentration. (1)

40
Q

Describe gas pressure in terms of volume and
temperature. (1)

A

Gas pressure is the name given to the force exerted by gas particles colliding with the wall of their container. (1)

41
Q

Define an indicator and give examples

A

A substance that changes colour in relation to the pH of another substance.
Examples:
Plant Dyes
Litmus Paper
Universal Indicator

42
Q

Describe how to make red cabbage indicator

A

To make your own indicator, you will need:

Red cabbage
A kettle and water
Household substances to test, such as lemonade, vinegar, baking powder or toothpaste. These are your substance samples.

  1. Chop up the red cabbage into small pieces and place it in a mug.
  2. Add freshly boiled water from the kettle.
  3. Stir the cabbage and boiling water until a deep purple solution is made.
  4. Put drops of your substance sample onto a white plate and then add your red cabbage solution.
  5. Use the colour comparison chart to find the pH of your substances.
43
Q

The pH scale and where on the scale I would find a weak
or strong acid or alkali

A

The pH scale is a logarithmic scale that measures the acidity or alkalinity (basicity) of a solution. The scale ranges from 0 to 14, with 7 being considered neutral. Here’s a breakdown of where you would find weak or strong acids and alkalis on the pH scale:

pH Scale:

0-6: Acidic range
7: Neutral
8-14: Alkaline (basic) range

44
Q

Neutralisation Reactions, what are the reactants and
products

A

A neutralisation reaction is a chemical reaction between an acid and a base, resulting in the formation of water and a salt.

The general chemical equation for a neutralization reaction is:

acid + base → water + salt

In a chemical reaction, reactants are the substances that undergo a chemical change to form new substances. They are written on the left side of a chemical equation.

In a chemical reaction, products are the substances that are formed as a result of the chemical change. Products are written on the right side of a chemical equation.

45
Q

Uses of neutralisation everyday such as farmers liming
soils and antacid tablets.

A

Neutralization reactions have several practical applications in everyday life. Here are two examples:

Farmers Liming Soils:

Farmers often use neutralization reactions to improve soil quality. Soils can become acidic due to factors such as rainfall, leaching of basic minerals, or the decomposition of organic matter.

Antacid Tablets:

Antacid tablets are commonly used to relieve indigestion and heartburn, which are often caused by an excess of stomach acid. These tablets typically contain compounds that undergo neutralization reactions with the acidic stomach contents. For example, many antacids contain aluminum hydroxide or magnesium hydroxide.

46
Q

How to name salts using the acid for example HCL –
Hydrogen Chloride

A

Naming salts:
1. hydrochloric acid produces chloride salts.
1. nitric acid produces nitrate salts.
1. sulfuric acid produces sulfate salts.

47
Q

All metal oxides are bases, some bases dissolve in water
to from hydroxides (Alkalis) for example calcium oxide
forms the alkali calcium hydroxide. True Or False?

A

True

48
Q

Using the name of the base, how else can you name a salt?

A

When a base neutralises an acid you use the first name of
the base and it becomes the first name of the salt.
Copper oxide + sulphuric acid -> copper sulfate and water

49
Q

Can Carbonates make salts?

A

Yes
All carbonates make CO2
when added to acids. Acid = carbonate – Salt + water and
CO2.

50
Q

Do Metals react with acids to form salt and hydrogen?

A

Yes
Metal + acid – salt and hydrogen.

51
Q

Define acid rain and describe how it is formed by the
burning of fossil fuel. List some of its effects.

A

Acid rain refers to precipitation, such as rain, snow, or fog, that has become acidic due to the presence of pollutants in the atmosphere.

Acid rain can harm aquatic ecosystems, leading to the acidification of lakes and rivers. This negatively affects fish and other aquatic life.

52
Q

The test for CO2

A

Carbon dioxide reacts with calcium hydroxide solution to produce a white precipitate of calcium carbonate. Limewater. It turns milky in the presence of carbon dioxide.

53
Q

Test for Hydrogen

A

Test for Hydrogen: Place a lighted splint in a test tube containing the gas. If the gas is hydrogen, there will be a squeaky pop.

54
Q

Define weathering.

A

The process of wearing or being worn by long exposure to the atmosphere.

CE Science at 13+ (3 decks)

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