Explain how the structure of a copper atom changes when it forms a copper ion, Cu2+.
| ☐ | A | The copper atom loses two electrons | |
| ☐ | B | The copper atom loses two protons | |
| ☐ | C | The copper atom gains two electrons | |
| ☐ | D | The copper atom gains two protons |
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Which element normally reacts to form an ion with a 2+ charge?
| ☐ | A | Sodium | |
| ☐ | B | Magnesium | |
| ☐ | C | Oxygen | |
| ☐ | D | 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 | A sulfide ion contains more atoms in it | |
| ☐ | B | A sulfate ion contains oxygen, a sulfide ion does not contain oxygen | |
| ☐ | C | A sulfide ion is more common | |
| ☐ | D | 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?
| ☐ | A | Protons and electrons are gained or lost | |
| ☐ | B | Neutrons are gained or lost | |
| ☐ | C | Electrons are gained or lost | |
| ☐ | D | 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.
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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
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True |
False |
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Positively and negatively charged ions are held together by strong covalent bonds |
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Positive and negatively charged atoms are held together by strong forces |
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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.
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random protons regular ions positively atoms |
Ionic lattices involve the organisation of ___________ and negatively charged ________ in a __________, repeating arrangement.
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The diagram shows the chemical symbol for lithium.
Explain why lithium ions have a charge of +1.
Explain why calcium oxide, CaO, has a very high melting point.
Compare the ionic formula of lithium chloride, LiCl, with the ionic formula of magnesium chloride, MgCl2.
Explain the electron transfer when barium reacts with oxygen.
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Sodium chloride has a melting point of around 800oC.
Magnesium oxide has a melting point of around 2850oC.
Explain the difference in melting points of these ionic compounds.
Deduce and explain the chemical formula for lithium bromide.
The diagram below shows the chemical symbol for fluorine.
Explain why a fluoride ion has a charge of 1-.
Describe what is meant by the term “ionic lattice”.
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Explain why iron (III) sulfate has a formula of Fe2(SO4)3.
Explain the electronic configuration of the ions in sodium fluoride.
Explain why the melting point of magnesium fluoride is higher than the melting point of sodium fluoride.
Explain why a magnesium atom loses electrons instead of gaining electrons.
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Explain why lithium bromide has ionic bonding rather than covalent bonding.
The diagram below shows a lithium ion.
Discuss the accuracy of the diagram.
Explain why lithium bromide has a high melting point.
Explain why there is a difference in ionic formula for the compound lithium bromide and lithium oxide.
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The diagram shows the electronic structures of a lithium atom and a fluorine atom.
Describe how the two atoms will react to form lithium fluoride.
A student stated that:
‘Magnesium atoms form Mg2- ions during a reaction’
The diagram below shows the chemical symbol of magnesium.
Explain why the student is incorrect.
You should refer to the number of subatomic particles in magnesium in your answer.
Ionic compound X has a melting point of 300oC and ionic compound Y has a melting point of 2000oC.
Explain why the two ionic compounds have different melting points.
A different ionic compound consists of atom X and atom Y.
Atom X forms ions with 3+ charge. Atom Y forms ions with 2- charge.
Deduce and explain the formula of this ionic compound.
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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.
| ☐ | A | Fe2SO4 | |
| ☐ | B | Fe3(SO4)2 | |
| ☐ | C | Fe2(SO4)3 | |
| ☐ | D | (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?
| ☐ | A | 11 protons, 11 electrons, 12 neutrons | |
| ☐ | B | 10 protons, 10 electrons, 12 neutrons | |
| ☐ | C | 11 protons, 10 electrons, 12 neutrons | |
| ☐ | D | 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.
Complete Figure 17 to show the electronic configurations and charges of the ions in lithium fluoride.
(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 |
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?
| ☐ | A | The sodium atom gains one electron from the fluorine atom | |
| ☐ | B | The sodium atom and the fluorine atom share one electron each | |
| ☐ | C | The sodium atom transfers one electron to the fluorine atom | |
| ☐ | D | 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?
| ☐ | A | 4- | |
| ☐ | B | 2- | |
| ☐ | C | 2+ | |
| ☐ | D | 4+ |
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