Exam code: 1CH0
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-?
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| 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 |
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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.
random protons regular ions positively atoms |
Ionic lattices involve the organisation of ___________ and negatively charged ________ in a __________, repeating arrangement.
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This question is about lithium and chlorine.
Which group of the periodic table is chlorine in?
Lithium reacts with chlorine to produce lithium chloride.
lithium + chlorine lithium chloride
The diagram in Figure 1 shows how the reaction happens.
Only the outer electrons are shown.
Figure 1
Use the words in the boxes to complete the sentences:
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A lithium atom becomes an ion by ............................................... one electron.
A lithium ion has a ............................................... charge.
The lithium ion now has the electronic structure of a ............................................... element.
The ions in lithium chloride are held together by strong ............................................... forces.
Why do lithium and chlorine react in this way?
Magnesium and bromine will form an ionic compound, like lithium and chlorine.
What is the formula of the ionic compound formed from magnesium and bromine?
Tick (✓) one box.
MgBr |
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MgBr2 |
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Mg2Br |
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Magnesium atoms have 12 protons and 12 electrons.
Which statement about Mg2+ ion is true?
Mg2+ contains 12 protons and 14 electrons
Mg2+ contains 12 protons and 10 electrons
Mg2+ contains 10 protons and 12 electrons
Mg2+ contains 14 protons and 10 electrons
Magnesium and oxygen atoms react together to form an ionic compound.
Put two ticks (✓) next to the correct statements that describe what happens for this ionic compound to form.
Oxygen loses two electrons to form ions with a +2 charge |
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Magnesium loses two electrons to form ions with a +2 charge |
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Magnesium gains two electrons to form an ion with a -2 charge |
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Oxygen gains two electrons to form ions with a a -2 charge |
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Ionic compounds have an overall charge of 0. When magnesium and chlorine react, magnesium forms an Mg2+ ion and chlorine forms a Cl- ion
What is the correct ionic formula of magnesium chloride?
MgCl2
MgCl
Mg2Cl
MgCl3
Ionic compounds have very high melting and boiling points.
Put a tick (✓) next to the correct statement that describe why ionic compounds have such high melting and boiling points.
Positively charged and negatively charged ions are arranged in a regular, repeating arrangement |
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Positively charged and negatively charged ions have strong electrostatic forces of attraction between them |
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Positively charged and negatively charged atoms have strong electrostatic forces of attraction between them |
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Sodium chloride, NaCl, is an ionic compound.
Put a tick (✓) next to the correct statement that describes the structure of solid sodium chloride.
Positively charged and negatively charged ions are arranged in a regular, repeating lattice arrangement |
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Positively charged and negatively charged atoms arranged in a giant covalent structure |
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Positively charged and negatively charged atoms arranged in a giant metallic structure |
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Ions are electrically charged atoms or groups of atoms.
Which statement about how sodium ions are formed is true?
A sodium atom gains one electron
A sodium ion gains one electron
A sodium atom loses one electron
A sodium ion loses one electron
Ionic compounds have an overall charge of 0. Sodium forms an Na+ ion and chlorine forms a Cl- ion, when they react to form sodium chloride.
What is the ionic formula of sodium chloride?
NaCl2
NaCl
Na2Cl
NaCl3
Sodium chloride has a melting point of 801oC.
Put two ticks (✓) next to the correct statements that explain the high melting point of sodium chloride.
Sodium chloride has strong covalent bonds |
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Sodium chloride has giant structure |
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Sodium chloride has strong forces of electrostatic attraction between oppositely charged ions |
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Sodium chloride has strong forces of electromagnetic attraction between oppositely charged ions |
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Lithium and magnesium are both metals. Lithium atoms form Li+ ions and magnesium atoms form Mg2+ ions.
Which statement about the formation of both these ions is true?
Magnesium atoms gain 2 electrons and lithium atoms gain 1 electron
Magnesium atoms lose 2 electrons and lithium atoms lose 1 electron
Magnesium atoms lose 1 electron and lithium atoms lose 2 electrons
Both atoms lose 2 electrons each
Lithium reacts with bromine to form an ionic compound.
What is the name of the ionic compound formed?
Lithium bromate
Lithium bromide
Lithium bromine
Lithium brominide
Lithium bromide is an ionic compound.
Put a tick (✓) next to the correct statement that describes the bonding within solid lithium bromide.
Positively charged and negatively charged ions are attracted to each other via electrostatic forces of attraction |
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Positively charged and negatively charged atoms share a pair of electrons |
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Positively charged and negatively charged atoms are attracted to each other via electrostatic forces of attraction |
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Lithium forms Li+ ions and bromine forms Br- ions to form an ionic compound.
What is the correct formula of lithium bromide?
LiBr2
LiBr
Li2Br
LiBr3
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Fluorine and chlorine are both non- metals.
Fluorine atoms form F- ions and chlorine atoms form Cl- ions.
Which statement about the formation of these ions is true?
Fluorine gains 1 electron and chlorine loses 1 electron
Fluorine loses 1 electron and chlorine gains 1 electron
They both lose 1 electron
They both gain 1 electron
Calcium reacts with fluorine to form an ionic compound.
What is the name of the ionic compound formed?
Calcium fluorate
Calcium carbonate
Calcium fluoride
Calcium fluorine
Calcium forms Ca2+ ions and chlorine forms F- ions to form an ionic compound.
What is the correct ionic formula for the compound formed?
CaF2
CaF
Ca2F
CaF3
All Group 2 elements lose electrons to become ions.
Which statement about the formation of Group 2 metal ions is true?
Group 2 elements lose 1 electron to form ions with +1 charge
Group 2 elements lose 2 electrons to form ions with +2 charge
Group 2 elements lose 2 electrons to form ions with -2 charge
Group 2 elements lose 1 electron to form ions with -1 charge
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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.
Calcium 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?
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| 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+?
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| 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 |
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| 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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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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A student made the statement:
“Sodium forms ions with a 2+ charge”.
Explain why the student’s statement is incorrect.
Compare the bonds formed by ionic and covalent compounds.
Describe the electron transfer when strontium reacts with oxygen.
Compare the structure of sodium chloride, NaCl, with calcium chloride, CaCl2 in terms of their ionic lattice.
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Explain why fluorine atoms form F- ions.
Explain the electron transfer in the formation of sodium fluoride, NaF.
Explain how the ionic lattice of sodium chloride influences its physical properties.
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Explain why aqueous sodium fluoride is able to conduct electricity but solid sodium fluoride is not.
Figure 1 shows the electronic configuration of a fluoride ion.
Figure 1
Explain why the electronic configuration diagram of fluoride ion is incorrect.
Explain why Dalton’s model of the atom would not have been able to explain the formation of ions.
Explain why the ionic compound formed from sodium and fluorine atoms is called “sodium fluoride” and not “florate sodium”.
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