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WorksheetsAQA Higher Tier Chemistry Ppaer
Total questions: 100
Worksheet time: 2hrs 55mins
Define atom.
The smallest part of an element that can still be recognised as that element
A molecule made up of two or more elements
A substance that cannot be broken down into simpler substances
A particle that carries a positive charge
Define element.
A substance made of only one type of atom
A mixture of different substances
A compound made of two or more elements
A substance that can be separated by physical means
Define compound.
A substance made of two or more different atoms chemically bonded together
A single atom with no bonds
A mixture of elements not chemically combined
A physical blend of substances
Define molecule.
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
A single atom not bonded to any other atom
A mixture of different substances not chemically combined
A group of atoms physically mixed but not bonded
Define mixture.
A substance made of more than one thing not chemically bonded together
A pure substance made of only one type of atom
A substance formed by a chemical reaction between two elements
A liquid that cannot be separated into other substances
Define a chemical reaction.
Chemical reactions involve the formation of one or more new substances.
Chemical reactions do not change any substances.
Chemical reactions only involve physical changes.
Chemical reactions always produce heat.
Name the 4 separating techniques.
filtration, crystallisation, distillation, chromatography
filtration, evaporation, condensation, precipitation
sublimation, melting, freezing, boiling
decantation, sieving, magnetism, centrifugation
State the three subatomic particles.
Protons, neutrons, electrons
Protons, photons, electrons
Neutrons, electrons, positrons
Protons, neutrons, quarks
State the masses of the subatomic particles.
State the relative charges of the subatomic particles.
Protons: +1, neutrons: 0, electrons: -1
Protons: 0, neutrons: -1, electrons: +1
Protons: -1, neutrons: +1, electrons: 0
Protons: +1, neutrons: -1, electrons: 0
How are the subatomic particles arranged in an atom? (3 marks) ________
Protons and neutrons in the nucleus, electrons orbiting in shells
Protons and electrons in the nucleus, neutrons orbiting in shells
Electrons and neutrons in the nucleus, protons orbiting in shells
All particles are randomly distributed throughout the atom
What is the plum pudding model of the atom?
A ball of positive charge with negative electrons distributed into it
A nucleus surrounded by orbiting electrons
A solid sphere with no internal structure
A cloud of positive and negative charges mixed together
What is the Bohr model of the atom?
Electrons orbit the nucleus in shells
Electrons are fixed inside the nucleus
Atoms do not have a nucleus
Protons orbit electrons in shells
What did the gold foil experiment prove?
That atoms have a dense nucleus with a positive charge
That electrons are found only in fixed orbits
That atoms are indivisible
That atoms do not contain empty space
What is the atomic number of an atom? ________
The number of protons in an atom
The number of neutrons in an atom
The number of electrons in an atom
The sum of protons and neutrons in an atom
What is the mass number of an atom? ________
The number of protons + the number of neutrons in an atom
The number of electrons in an atom
The number of protons in an atom
The number of neutrons in an atom
How do you calculate the number of neutrons in an atom?
How are the electrons arranged in atoms?
Orbiting the nucleus in shells
Randomly scattered throughout the atom
Fixed at the center of the nucleus
Grouped together in pairs outside the atom
How many electrons can go in the first shell?
2
4
6
8
How many electrons can go in the second and third shells?
(a)
What are groups in the periodic table?
The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0
The rows, numbered 1 to 7
The diagonal elements in the table
The elements with similar atomic masses
What links the group number of an atom and the electron distribution?
What are periods in the periodic table?
What can the period tell you about the electrons in an atom?
Why did Mendeleev put some elements in groups?
Because they had similar chemical properties (e.g. they reacted violently with water)
Because they had similar atomic numbers
Because they were discovered at the same time
Because they had the same color
Why did Mendeleev leave gaps in his periodic table?
For elements that had not been discovered yet
To make the table look symmetrical
Because he ran out of element names
To separate metals from non-metals
Where are the non metals located on the periodic table?
Top right of the periodic table
Bottom left of the periodic table
Center of the periodic table
Top left of the periodic table
What is an ion?
an atom which has lost or gained an electron
an atom which has gained a proton
an atom which has lost a neutron
an atom which has gained a nucleus
How many electrons does calcium have?
20 (same as atomic number!)
18
22
12
How many electrons does silicon have?
14 (same as atomic number!)
12
16
18
How are the electrons in sulphur arranged?
How are the electrons in magnesium arranged?
How many electrons are in the outer shell of boron?
How many electrons are in the outer shell of phosphorous?
How many electrons are in the outer shell of sodium?
An element has three shells and three electrons in the outer shell. What element is it?
Aluminium (group 3, period 3)
Sodium (group 1, period 3)
Magnesium (group 2, period 3)
Silicon (group 4, period 3)
How many electrons are in the outer shell of Gallium?
What charge do electrons have?
(a)
What charged ion will a group 3 metal form?
3+ (three electrons in the outer energy level)
1+ (one electron in the outer energy level)
2- (two electrons gained)
0 (no charge)
What charged ion will a group 2 metal form?
2+ (two electrons in the outer level)
1+ (one electron in the outer level)
2- (two electrons gained)
0 (no charge)
What charged ion will a group 1 metal form?
1+ (one electron in the outer level)
2+ (two electrons in the outer level)
1- (one electron in the outer level)
0 (no charge)
Name the force of attraction between ions in an ionic compound.
What charged ion will a group 6 non-metal form?
-2 (requires two electrons to complete outer energy level)
+2 (loses two electrons to complete outer energy level)
-1 (requires one electron to complete outer energy level)
+1 (loses one electron to complete outer energy level)
What charge will an ion of beryllium take?
What charge will an ion of barium take?
What charge will an ion of fluorine take?
1- (7 electrons in the outer shell, needs to gain one)
2+ (7 electrons in the outer shell, needs to lose two)
1+ (7 electrons in the outer shell, needs to lose one)
2- (7 electrons in the outer shell, needs to gain two)
If something has gained electrons, what charge will it have?
Negative
Positive
Neutral
No charge
If something has lost electrons, what charge will it have?
Positive (because they have lost a negative!)
Negative (because they have gained a positive!)
Neutral (because electrons do not affect charge)
No charge (because electrons are not important)
What charge will an ion of oxygen take?
What charge will an ion of Selenium take?
2- (group 6, so has 6 electrons in the outer shell and needs to gain two)
1+ (group 1, so has 1 electron in the outer shell and needs to lose one)
3- (group 5, so has 5 electrons in the outer shell and needs to gain three)
2+ (group 2, so has 2 electrons in the outer shell and needs to lose two)
Explain in terms of electrons what occurs when lithium bonds with chlorine.
Why do atoms transfer electrons in ionic bonding?
So that they can have full outer shells
To increase their size
To lose all their electrons
To become radioactive
Explain in terms of electrons what occurs when lithium bonds with fluorine.
One electron transferred from lithium to fluorine
One electron transferred from fluorine to lithium
Electrons are shared equally between lithium and fluorine
No electrons are transferred or shared
Explain in terms of electrons what occurs when magnesium bonds with oxygen.
Two electrons transferred from magnesium to oxygen
Two electrons transferred from oxygen to magnesium
Magnesium shares electrons with oxygen
No electrons are transferred between magnesium and oxygen
Explain in terms of electrons what occurs when beryllium bonds with oxygen
Explain in terms of electrons what occurs when magnesium bonds with chlorine.
Explain in terms of electrons what occurs when sodium bonds with oxygen.
Two electrons transferred to an oxygen atom from two different sodium atoms
One electron is shared between sodium and oxygen
Oxygen donates two electrons to sodium atoms
Electrons are equally shared between sodium and oxygen atoms
Why do sodium ions and chlorine ions form an ionic bond?
There is an electrostatic force of attraction between oppositely charged ions
They share electrons equally between them
They form a covalent bond by overlapping orbitals
They have the same number of protons and neutrons
Why don't sulphur ions and oxygen ions form ionic bonds with each other?
Both have negative charges so would repel
They are both metals and cannot bond
They have the same number of protons
They are too far apart on the periodic table
What is the name for a substance made of billions of oppositely charged ions joined together?
Giant ionic lattice
Covalent molecule
Metallic crystal
Simple molecular structure
Define giant ionic lattice
A crystalline structure made of alternating positive and negative ions held together by electrostatic forces of attraction
A structure made of molecules held together by covalent bonds
A metallic structure with delocalized electrons
A network of atoms bonded by hydrogen bonds
State the melting points of ionic substances
(a)
Explain why ionic substances have high melting points.
Strong forces of attraction between oppositely charged ions require large amounts of energy to overcome (break)
Ionic substances are made up of small molecules that easily separate when heated
Ionic substances contain weak covalent bonds that break at low temperatures
Ionic substances are gases at room temperature, so they melt easily
Will NaCl(s) conduct electricity?
(a)
Will NaCl (aq) conduct electricity?
Will NaCl (l) conduct electricity?
(a)
What does molten mean?
A solid which has melted is described as molten
A gas that has condensed is described as molten
A liquid that has frozen is described as molten
A solid that has evaporated is described as molten
Explain why ionic compounds do not conduct electricity when solid
Because the ions are not free to move
Because they contain no charged particles
Because they are made of molecules
Because they are always insoluble in water
Explain why ionic compounds conduct electricity in solution
Because the ions are free to move
Because the molecules are tightly packed
Because the electrons are fixed in place
Because the atoms share electrons
Explain why ionic compounds conduct electricity when molten
Because the ions are free to move
Because the electrons are fixed in place
Because the molecules are neutral
Because the atoms are bonded covalently
What does soluble mean?
What does insoluble mean?
Does not dissolve in water
Dissolves quickly in water
Turns into a gas in water
Changes color in water
Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity?
Melt it
Dissolve it in water
Crush it into powder
Cool it to a very low temperature
Why does solid lead(II) bromide not conduct electricity?
Ions are in fixed positions and cannot move.
It contains free electrons that cannot move.
It is a good conductor in solid state.
It is made up of neutral atoms only.
Why does molten lead(II) bromide conduct electricity?
Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is.
Dissolve it in water because this does not require high temperatures.
Melt it at a very high temperature to allow conduction.
Mix it with oil to increase its conductivity.
Grind it into a fine powder and heat it gently.
In terms of electrons, what do group 1 elements have in common?
1 electron in the outer shell
2 electrons in the outer shell
A full outer shell
No electrons in the outer shell
In terms of electrons, what do group 7 elements have in common?
7 electrons in the outer shell
8 electrons in the outer shell
1 electron in the outer shell
2 electrons in the outer shell
In terms of electrons, what do group 0 elements have in common?
Full outer shell
One electron in outer shell
Half-filled outer shell
No electrons in outer shell
What happens to the reactivity of the group 1 elements as you go down the group?
Increases
Decreases
Remains the same
Becomes unpredictable
What happens to the reactivity of the group 7 elements as you go down the group?
Decreases
Increases
Remains the same
Becomes unpredictable
Explain why the noble gases are unreactive.
They have full outer shells, so do not need to gain or lose electrons.
They have empty outer shells, so they are unstable.
They easily form bonds with other elements.
They have more protons than other elements.
What is a trend?
A pattern in properties
A type of chemical reaction
A measurement of mass
A unit of temperature
State the trend in the melting points of the alkali metals as you go down the group.
(a)
State the trend in the melting points of the halogens as you go down the group.
(a)
What is produced when group 1 elements react with oxygen?
Metal oxide
Metal hydroxide
Metal carbonate
Metal chloride
Explain why universal indicator turns purple when added to water which has reacted with a group 1 element.
A metal hydroxide / alkali is produced
A gas is released
The temperature decreases
A salt is formed
What gas is produced when the alkali metals react with water?
Hydrogen
Oxygen
Carbon dioxide
Nitrogen
Balance the equation: Li + H₂O → LiOH + H₂
Balance the equation: K + H₂O → KOH + H₂
Name Li₂O
Lithium oxide
Lithium peroxide
Lithium hydroxide
Lithium carbonate
Name KOH
Potassium hydroxide
Sodium hydroxide
Calcium hydroxide
Magnesium hydroxide
What charge do group 1 ions have?
(a)
What charge do group 7 ions have?
-1
+1
-2
+2
What is a displacement reaction?
Explain why the following reaction does not proceed: KBr + I₂
Iodine is less reactive than bromine so cannot displace it
Bromine is less reactive than iodine so cannot displace it
Potassium reacts with iodine to form a stable compound
Iodine forms a precipitate with potassium bromide
Balance the below equation and explain why it is a displacement reaction: KBr + Cl₂ → KCl + Br₂
Explain why fluorine is more reactive than chlorine.
Fewer shells/electrons, less shielding (or stronger attraction from nucleus), easier to gain electrons
Fluorine has more protons than chlorine, making it more reactive
Fluorine is a gas at room temperature, while chlorine is a liquid
Fluorine has a larger atomic radius than chlorine, making it more reactive
Explain why potassium is more reactive than lithium
More shells/electrons, less shielding (or weaker attraction from nucleus), easier to lose electrons
Potassium has a smaller atomic radius than lithium, making it more reactive
Potassium has more protons, which makes it harder to lose electrons
Potassium is a transition metal, so it reacts more easily
Explain why bromine is less reactive than chlorine
