chemistry AQA GCSE triple paper 1

C1 1) What are the three states of matter?

Solid, liquid, gas

C1 2) What is the particle theory?

Explains properties of solids, liquids and gases in terms of movement particles and distance between particles.

C1 3)What is a solid?

Particles held close together. Strong forces between. Particles do not move from position, only slightly vibrate.

C1 4)What is a liquid?

Particles randomly arranged and free to move past each other, but stick closely together. Weaker forces. Don't keep a definite shape.

C1 5)What are gases?

Particles are free to move and do so randomly. Particles are very far apart. Very weak forces between particles.

C1 6)What is melting?

When a solid goes to a liquid by heating.

C1 7)What is boiling?

What a liquid goes to a gas by heating.

C1 8)What is condensing?

When a gas goes to a liquid by cooling.

C1 9)What is freezing?

When liquid goes to a solid by cooling.

C1 10)Why do substances have different melting points?

Depends on amount of energy needed to break bonds in substance.

C1 11)Define atom

Smallest part of an element that can still be recognised as an element.

C1 12)Define element

A substance made up of only one type of atom

C1 13)Define compound

A substance made of two or more different atoms chemically bonded together.

C1 14) What are chemical symbols?

Symbols (One or two letters) to represent an atom so it can universally recognised around the world.

C1 15)What are chemical equations?

They show what happens during a chemical reaction. Reactants go on left, products on the right.

C1 16)What are word equations?

Show what happens during a chemical reaction using the words of the substances involved.

C1 17)What are symbol equations?

Show what happens during a chemical reaction using the symbols of the substances involved.

C1 18)What is a balanced equation?

An equation with the same number of atoms of each element on both sides.

C1 19) What are state symbols?

Symbols that represent what state the substances are in. s for solid, l for liquid, g for gas, aq for aqueous.

C1 20)Define mixture

A substance made of more than one things not chemically joined together.

C1 21)What is chromatography?

Used to separate mixtures of different colours.

C1 22)What is filtration?

Used to separate an insoluble solid from a liquid. Like sand and water.

C1 23)What is crystallisation?

Used to separate a soluble solid and a solution. Gently heat a solution and some of the solvent will evaporate.

C1 24)What is simple distillation?

Separate out a liquid from a mixture. Only be used to separate substances with boiling point significantly apart from each other.

C1 25)How does simple distillation work?

Heat the mixture. Liquid with lowest boiling point will boil and evaporate. As this passes condenser, it condenses back into a liquid and is collected.

C1 26)What is fractional distillation?

Separating a mixture of different liquids and useful when boiling points are close together.

C1 27)How does fractional distillation work?

Mixture heated. Lowest boiling point evaporates first. If others evaporate, top of column is cooler so will condense back down. Once first liquid is collected, next is collect and so on.

C1 28) How does chromatography work?

Works because some mixtures will dissolve better than others in the solvent chosen. The more soluble a substance is in the solvent, the further up the paper it is carried.

C1 29) What did John Dalton believe the atom to look like?

Tiny, hard spheres (like snooker balls). He believed they could not be split any further.

C1 30) What model came after Dalton's sphere model?

Plum pudding model

C1 31)What is the plum pudding model?

States that the atom was a ball of positive charge with negative electrons stuck in it.

C1 32)What is the gold foil experiment?

Fired alpha particles at an extremely thin sheet of gold foil. Most went through but some bounced back.

C1 33)What did the gold foil experiment prove?

That atoms have a nucleus with a positive charge.

C1 34)Who did the gold foil experiment?

Geiger and Marsden

C1 35)What is the nuclear model of the atom?

Neils Bohr's model that suggested electrons were contained in shells and they orbit the nucleus.

C1 36)Who discovered neutrons?

James Chadwick.

C1 37)State the three subatomic particles (what makes up an atom?)

Electrons, protons and neutrons

C1 38)State the masses of the subatomic particles

Electrons 0, protons 1, neutrons 1

C1 39)State the charges of the subatomic particles

Electrons -1, protons +1, neutrons 0

C1 40)How are the subatomic particles arranged?

Protons and neutrons in the nucleus (in the middle), electrons orbiting in shells.

C1 41)How do you calculate the number of protons and electrons in an atom?

The proton number on the periodic table (the smaller number)

C1 42)How do you calculate the number of neutrons in an atom?

Mass number (big number) - proton number (small number)

C1 43)What is the mass of an atom?

The number of Protons add neutrons

C1 44) Why does an atom have no overall charge?

Same number of protons and electrons

C1 45)What are isotopes?

Different forms of the same element, which have the same number of protons but different number of neutrons. Same atomic number but a different mass.

C1 46)What are ions?

Charged particles.

C1 47)How are ions made?

They are made when electrons are either lost or gained.

C1 48)What are positive ions?

When an atom has lost an electron/electrons

C1 49)What is a negative ion?

When an atom has gained an electron/electrons.

C1 50)What ions do metal atoms form?

Positive ions (cations) - they lose electrons

C1 51)What ions do non-metal atoms form?

Negative ions (anions) - they gain electrons.

C1 52)Why are ions formed?

To get a full outer shell to be a more stable structure.

C1 53)How many electrons do group 1 elements lose?

1

C1 54)How many electrons do group 2 elements lose?

2

C1 55)How many electrons do group 6 gain?

2

C1 56)How many electrons do group 7 gain?

1

C1 57)How are electron arranged in an atom?

Orbiting the nucleus in shells.

C1 58)How many electrons can go in the first shell?

2

C1 59)How many electrons can go in the second and third shells?

8

C1 60)Magnesium has 12 electrons. What is the electronic configuration?

2,8,2

C1 61) How many electrons do group 1 elements have in their outer shell?

1

C1 62) How many electrons do group 6 elements have in their outer shell?

6

C1 63)What is the conservation of mass?

During a chemical reaction, no atoms are made or destroyed, so the mass of the produces is the same as the mass of the reactants.

C2 18) How many electrons do group 1 have in their outer shell?

1

C2 19) Why are alkali metals so reactive?

Only have 1 electron to lose to get a stable structure.

C2 20) What happens to the reactivity of elements as you go down the group 1?

Reactivity increases

C2 21) Why does reactivity increase as you go down group 1?

Outer electron is further away from the positive pull of the nucleus. Electron can be pulled away easier.

C2 22) Why do the alkali metals fizz when you add them to water?

When added to water, they form hydrogen gas.

C2 23) What is the word equation for sodium reacting with water?

Sodium + water à sodium hydroxide and hydrogen

C2 8) Why do elements in the same group react in similar ways?

Because they have the same amount of electrons in their outer shells.

C2 9) How many electrons do group 3 have in their outer shell?

3

C2 10) How many shells do the elements have in period 2?

2

C2 11) What are two differences between metals and non-metals?

Metals conduct electricity but non-metals generally do not. Metals tend to have higher melting and boiling points.

C2 12) Where do you find metals on the periodic table?

Left hand side and centre of the periodic table

C2 13) Where do you find non-metals on the periodic table?

Right hand side of staircase.

C2 14 What are the elements in group 0 called?

Noble gases

C2 15) Why are group 0 elements so unreactive

Already have a stable outershell. Do not need to lose or gain electrons.

C2 16) What does monoatomic mean?

Single atom. Exist on their own.

C2 17) What happens to the boiling point as you go down group 0?

It increases

C2 18) How many electrons do group 1 have in their outer shell?

1

C2 19) Why are alkali metals so reactive?

Only have 1 electron to lose to get a stable structure.

C2 20) What happens to the reactivity of elements as you go down the group 1?

Reactivity increases

C2 21) Why does reactivity increase as you go down group 1?

Outer electron is further away from the positive pull of the nucleus. Electron can be pulled away easier.

C2 22) Why do the alkali metals fizz when you add them to water?

When added to water, they form hydrogen gas.

C2 23) What is the word equation for sodium reacting with water?

Sodium + water à sodium hydroxide and hydrogen

C2 24) What are group 7 elements called?

Halogens

C2 25) How many electrons do group 7 have in their outer shell?

7

C2 26) Why are group 7 elements so reactive?

Only need to gain 1 electron to have full outer shell.

C2 27) What happens to the melting and boiling points as you go down group 7?

They increase

C2 28) What does diatomic mean?

Molecules made up of a pair of atoms

C2 29) What happens to the reactivity as you go down group 7?

It decreases

C2 30) Why do elements get more reactive as you go down group 1?

Outer electron attracted less strongly to positive nucleus with larger atom, larger atoms have shielding affects from other shells from outer electron and nucleus, amount of positive pull increases in larger atoms.

C2 31) Why do elements get less reactive as you go down group 7?

Outer electron attracted less strongly to positive nucleus with larger atom, larger atoms have shielding affects from other shells from outer electron and nucleus, amount of positive pull increases in larger atoms.

C2 32) Give three physical properties of transition elements

good conductors of electricity and thermal energy, hard and strong, high desnties, high melting points

C2 33) Give two chemical properties of transition elements

less reactive, slowly corrode

C2 34) What is 1 use of transition elements

industrial catalysts

C2 35) Compare the reaction in water between transition elements and alkali metals

alkali metals react much more vigorously with water

C2 36) Compare the reaction in oxygen between transition elements and alkali metals

alkali metals react much more vigorously with oxygen

C2 37) True or false. A transition element can form ions with different charges

TRUE

C3 1) What are the three states of matter?

Solid, liquid, gas