Explain how the structure of a copper atom changes when it forms a copper ion, Cu2+.
The copper atom loses two electrons
The copper atom loses two protons
The copper atom gains two electrons
The copper atom gains two protons
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Which element normally reacts to form an ion with a 2+ charge?
Sodium
Magnesium
Oxygen
Fluorine
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An oxygen atom has an atomic number of 8 and a mass number of 16.
This oxygen atom forms the ion O2-.
Which lettered row shows the number of protons and the number of neutrons in this oxide ion, O2-?
|
| number of protons | number of neutrons |
☐ | A | 8 | 8 |
☐ | B | 8 | 10 |
☐ | C | 10 | 8 |
☐ | D | 10 | 10 |
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How is a sulfate ion different to a sulfide ion?
A sulfide ion contains more atoms in it
A sulfate ion contains oxygen, a sulfide ion does not contain oxygen
A sulfide ion is more common
A sulfate ion has the formula S2-, a sulfide ion has the formula SO42-
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Ions are electrically charged atoms or groups of atoms.
Which statement about how ions are formed is true?
Protons and electrons are gained or lost
Neutrons are gained or lost
Electrons are gained or lost
Protons are gained or lost
The table below shows three statements about the charge of an atom.
Put a tick (✓) next to the correct statement.
Atoms have no overall charge because the number of protons and electrons are equal |
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Atoms have no overall charge because the number of protons and neutrons are equal |
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Atoms have an overall positive charge because the number of protons is greater than the number of neutrons |
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Atoms have an overall negative charge because the number of electrons is greater than the number of neutrons |
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Figure 1 shows some statements about ionic bonding.
Put ticks (✓) in the boxes in Figure 1 to show which statements are true and which statements are false
| True | False |
Positively and negatively charged ions are held together by strong covalent bonds |
|
|
Positive and negatively charged atoms are held together by strong forces |
|
|
Positively and negatively charged ions are held together by strong forces of electrostatic attraction |
|
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The formation of positively and negatively charged ions involves the transfer of electrons |
|
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Figure 1
Use the words from the box to complete the sentences about ionic lattices.
random protons regular ions positively atoms |
Ionic lattices involve the organisation of ___________ and negatively charged ________ in a __________, repeating arrangement.
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The ions present in iron(III) sulfate are:
iron(III) Fe3+
sulfate SO42-.
Write the formula of iron(III) sulfate using this information.
Fe2SO4
Fe3(SO4)2
Fe2(SO4)3
(Fe)2(SO4)3
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Sodium has an atomic number of 11.
A sodium atom has a mass number of 23.
This sodium atom is ionised to form a sodium ion with the formula Na+.
Which option shows the number of protons, electrons and neutrons in this sodium ion?
11 protons, 11 electrons, 12 neutrons
10 protons, 10 electrons, 12 neutrons
11 protons, 10 electrons, 12 neutrons
11 protons, 12 electrons, 12 neutrons
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Ionic compounds contain ions.
The numbers of electrons, neutrons and protons in four particles, W, X, Y and Z, are shown in Figure 15.
particle | electrons | neutrons | protons |
W | 9 | 10 | 9 |
X | 10 | 14 | 12 |
Y | 16 | 16 | 16 |
Z | 18 | 18 | 16 |
Figure 15
Explain which particle, W, X, Y or Z, is a negative ion.
Lithium fluoride, LiF, is an ionic compound. It contains lithium cations and fluoride anions. The electronic configurations of a lithium atom and of a fluorine atom are shown in Figure 16.
Figure 16
Complete Figure 17 to show the electronic configurations and charges of the ions in lithium fluoride.
Figure 17
(4)
Figure 18 shows the ability of different substances to conduct electricity.
substance | conducts electricity |
solid calcium chloride | no |
molten calcium chloride | yes |
diamond | no |
zinc | yes |
Figure 18
Explain these results by referring to the structures of the substances.
2 marksCalcium nitrate contains calcium ions and nitrate ions.
Calculate the relative formula mass of calcium nitrate, Ca(NO3)2. (relative atomic masses: Ca = 40, N = 14, O = 16)
relative formula mass = .....................................................
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Sodium fluoride is an ionic compound containing sodium ions, Na+, and fluoride ions, F-.
The electronic configurations are show below:
| electronic configuration of atoms |
sodium | 2.8.1 |
fluorine | 2.7 |
Which statement explains how sodium and fluorine atoms form the ions in sodium fluoride?
The sodium atom gains one electron from the fluorine atom
The sodium atom and the fluorine atom share one electron each
The sodium atom transfers one electron to the fluorine atom
The sodium atom and the fluorine atom both lose one electron
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The formula of lead(IV) oxide is PbO2.
What is the charge of the lead ion in lead(IV) oxide?
4-
2-
2+
4+
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Potassium reacts with chlorine to form potassium chloride.
The electronic configuration of the potassium atom is 2.8.8.1 and the electronic configuration of the chlorine is 2.8.7.
What are the electronic configurations of the ions formed?
| K+ | Cl- | |
A | 2.8.8.2 | 2.8.7 | |
B | 2.8.8.2 | 2.8.8 | |
C | 2.8.8 | 2.8.7 | |
D | 2.8.8 | 2.8.8 |
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An aluminium atom has the atomic number 13 and the mass number 27.
Which row shows the numbers of subatomic particles present in an aluminium ion, Al3+?
| protons | neutrons | electrons | |
A | 13 | 14 | 13 | |
B | 13 | 14 | 10 | |
C | 14 | 13 | 10 | |
D | 14 | 13 | 17 |
Magnesium burns in excess oxygen to form magnesium oxide.
The balanced equation for this reaction is
2Mg + O2 → 2MgO
Starting with 1.35 g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction.
(relative atomic masses: O = 16.0, Mg = 24.0)
You must show your working.
mass of magnesium oxide = .............................. g
Chlorine reacts with hydrogen to form hydrogen chloride.
Write the balanced equation for this reaction.
Sodium chloride is an ionic compound, containing sodium ions, Na+, and chloride ions, Cl–.
Figure 15 shows the electronic configuration of sodium and chlorine.
| |
sodium | 2.8.1 |
chlorine | 2.8.7 |
Figure 15
Explain how sodium and chlorine atoms form the ions in sodium chloride and how the ions are arranged in the solid sodium chloride.
You may wish to use diagrams in your answer.
Sodium reacts with chlorine to form sodium chloride.
The electronic configuration of the sodium atom is 2.8.1 and the electronic configuration of the chlorine atom is 2.8.7.
Give the electronic configurations of the ions formed.
Na+ ...............................................
Cl– ...............................................
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Ionic compounds contain ions.
The numbers of electrons, neutrons and protons in four particles A, B, C and D are shown below.
Which one is the negative ion?
| particle | electrons | neutrons | protons | |
☐ | A | 6 | 6 | 6 | |
☐ | B | 10 | 12 | 11 | |
☐ | C | 10 | 14 | 13 | |
☐ | D | 18 | 20 | 17 |
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The structure of an ionic compound, sodium chloride, is a lattice structure.
Which of the following statements about an ionic lattice structure is not true?
There is a regular arrangement of ions in the lattice
The layers of ions slide over each other easily in the lattice
The ions are arranged with alternating anions and cations
Strong electrostatic forces of attraction occur between oppositely charged ions
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The name of an ionic compound can be used to deduce its formula.
Draw one straight line from each name of an ionic compound to its correct formula.
What is meant by the term ion?
When sodium and chlorine react together, they form the ionic compound, sodium chloride.
Use words from the box to complete the sentences about how sodium chloride is formed.
lose |
| electrostatic |
| negative |
|
| positive |
| gain |
| intermolecular |
Sodium atoms ...................... one electron to form ...................... ions and chlorine atoms ...................... one electron to form ...................... ions. There are ...................... forces of attraction between the oppositely charged ions which hold the compound together.
Which substance does not have ionic bonding?
lithium sulfide
calcium carbonate
carbon dioxide
magnesium oxide
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