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WorksheetsC1 Lessons 1-12
Total questions: 50
Worksheet time: 25mins
What is an atom?
The smallest part of an element that can still be recognised as that element
A substance made of only one type of atom
A substance made of two or more different atoms chemically bonded together
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
What is an element?
The smallest part of an element that can still be recognised as that element
A substance made of only one type of atom
A substance made of two or more different atoms chemically bonded together
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
What is a compound?
A substance made of only one type of atom
A substance made of two or more different atoms chemically bonded together
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
A substance made of more than one thing not chemically bonded together
What is a molecule?
A substance made of only one type of atom
A substance made of two or more different atoms chemically bonded together
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
A substance made of more than one thing not chemically bonded together
What is a mixture?
A substance made of only one type of atom
A substance made of two or more different atoms chemically bonded together
A substance made of more than one atom chemically bonded together (can be atoms of the same type!)
A substance made of more than one thing not chemically bonded together
Name the three subatomic particles
Protons, quarks, electrons
Protons, neutrons, electrons
Borons, neutrons, electrons
Protein, neutral, electricity
State the masses of the subatomic particles
Protons: 1, neutrons: 0, electrons: 1
Protons: 0, neutrons: 1, electrons: 0
Protons: 1, neutrons: 1, electrons: 1
Protons: 1, neutrons: 1, electrons: 0
How are the subatomic particles arranged in an atom?
Protons and neutrons in the nucleus, electrons orbiting in shells
Neutrons and electrons in the nucleus, protons orbiting in shells
Electrons and neutrons in the nucleus, protons orbiting in shells
Protons in the nucleus, electrons orbiting in shells
What is the plum pudding model of the atom?
A ball, similar to a snooker ball.
A ball of negative charge with positive protons embedded into it.
A central mass of positive charge with negative electrons orbiting in shells.
A ball of positive charge with negative electrons embedded into it
What did the gold foil experiment prove?
That atoms have a dense nucleus with a neutral charge.
That atoms have a dense nucleus with a positive charge.
That atoms have a do not have a nucleus.
That atoms have a dense nucleus with a positive and negative charge.
What is the atomic number of an atom?
The number of protons and neutrons in an atom
The number of protons and electrons in an atom
The number of neutrons in an atom
The number of protons in an atom
What is the mass number of an atom?
The number of protons + the number of electrons in an atom.
The number of protons in an atom.
The number of neutrons in an atom.
The number of protons + the number of neutrons in an atom.
Why is the number of electrons in an atom equal to the number of protons?
To give the atom a positive charge
To give the atom a negative charge
As their charges cancel out
As their mass numbers cancel out
How do you calculate the number of neutrons in an atom?
Mass number - atomic number
Mass number + atomic number
Atomic number - atomic number
Atomic number + atomic number
What did Chadwick discover?
The proton
The neutron
The electron
The electron orbits
What did Bohr's experiments show?
That protons are located in the central nucleus.
That neutrons existed.
That electrons are in specific shells.
That protons and neutrons have a mass of 1.
What are isotopes?
Atoms of the same element with the same number of neutrons
Atoms of the same molecule with a same number of protons
Atoms of the same molecule with a different number of protons
Atoms of the same element with a different number of neutrons
What is the mass number of magnesium?
6
12
18
24
How are the electrons arranged in atoms?
Orbiting the nucleus in shells, specifically arranged.
Randomly arranged in the nucleus
Specific arrangement in the nucleus
Randomly arranged in shells
How many electrons can go in the first shell?
2
4
6
8
How many electrons can go in the second and third shells?
2
4
6
8
What are groups in the periodic table?
The rows, numbered 1, 2, 3, 4, 5, 6, 7, 0
The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0
The sections, numbered 2, 4, 6, 8
The segments, numbered 2, 4, 6, 8
What can the group tell you about the electrons in an atom?
How many electron shells there are. E.g. carbon is in period 2 and has 2 electron shells
How many electrons in the outer shell. E.g. carbon is in group 4 so has 4 electrons in the outer shell
What are periods in the periodic table?
The columns in the periodic table
The sections in the periodic table
The rows in the periodic table
The segments in the periodic table
What can the period tell you about the electrons in an atom?
How many shells an atom has. E.g. carbon is in the second period so has two shells
How many electrons are in the outer shell of an atom. E.g. carbon has 4 electrons in its outer shell and is in group 4.
Why did Mendeleev put some elements in groups?
Because they were solid/liquid/gas
Because they looked the same colour
Because they had different properties (e.g. they reacted differently with water)
Because they had similar properties (e.g. they reacted violently with water)
Why did Mendeleev leave gaps in his periodic table?
For elements that had not been discovered yet
To make space between groups in the table
Just in case there were mistakes, he could move the elements about.
For compounds that were being investigated on
How many electrons are in calcium?
5
10
15
20
How are the electrons in sulfur atoms arranged?
2,8,5
2,8,6
2,8,7
2,8,8
What is the formula of magnesium oxide?
MgO2
Mg2O
MgO
MGO2
In terms of electrons, what do group 1 elements have in common?
1 electron shell
1 electron in the outer shell
1 neutron
1 proton in the nucleus
In terms of electrons, what do group 7 elements have in common?
7 protons in the nucleus
7 electron shells
7 neutrons
7 electrons in the outer shell
In terms of electrons, what do group 0 elements have in common?
All shells have 8 electrons in them
Full inner shell
Full outer shell
Why is sodium more reactive than lithium?
Because the outer electron is further away from the nucleus, so is easier to lose.
Because the outer electron is closer to the nucleus, so is easier to lose.
Because there is only 1 electron in its outer shell.
Because there are more shells in sodium.
Why is chlorine more reactive than bromine?
Because there are only 7 electrons in its outer shell.
Because chlorine has less electron shells than bromine.
Because the outer shell is closer to the nucleus, so it is easier to gain an electron.
Because the outer shell is further away from the nucleus, so it is easier to gain an electron.
Explain why the noble gases are inert
They are unreactive gases
They have full outer shells, so do not need to gain or lose electrons
They have incomplete outer shells, so need to gain or lose electrons
They are used for lighting.
State the trend in the melting points of the alkali metals
They all have similar melting points
Gets lower down the group
Gets higher down the group
What state is fluorine at room temperature?
gas
liquid
solid
What state is chlorine at room temperature?
gas
liquid
solid
What state is bromine at room temperature?
gas
liquid
solid
What state is iodine at room temperature?
gas
liquid
solid
Name LiOH
Lithium oxide
Lithium hydride
Lithium hydroxide
Lithium dihydroxide
Name KOH
Potassium oxide
Potassium hydride
Potassium hydroxide
Potassium dihydroxide
Explain why the group 1 elements are called alkali metals
They are metals that form acids when they react with water
They all produce a purple colour
They produce substances with a pH of 1-6
They are metals that form alkalis when they react with water
What is a displacement reaction?
A reaction in which elements form a compound
A reaction in which a more reactive element takes the place of all the elements in a compound
A reaction in which a more reactive element takes the place of a less reactive element in a compound
A reaction in which a less reactive element takes the place of a more reactive element in a compound
Explain why the following reaction does not proceed: KBr + I₂
Iodine is less reactive than bromine so cannot displace it
Potassium is less reactive than bromine so cannot displace it
Iodine is less reactive than potassium so cannot displace it
Bromine is less reactive than iodine so cannot displace it
Where are transition metals found in the periodic table?
At the top
In the middle
On the left
On the right
Compare the melting point, density, strength, hardness and reactivity of transition metals with group 1 metals
Lower for all the transition metals except reactivity
Higher for all the transition metals except hardness
Higher for all the transition metals except reactivity
Lower for all the transition metals except hardness
What is distinctive about compounds formed from transition metals?
They are coloured
They are white
They are black
They are brown
What can transition metals be used for?
Catalysts
Pharmaceuticals
Fertilisers
Explosives
