Ions & Ionic Bonds

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Formation of Ions

An ion is an electrically charged atom or group of atoms formed by loss or gain of electrons.
Atoms lose or gain electrons to obtain a full outer shell (noble gas configuration).
Cations are positive ions formed when atoms lose electrons (metals).
Anions are negative ions formed when atoms gain electrons (non-metals).
Group 1 elements form 1+ ions; Group 2 form 2+ ions.
Group 6 elements form 2– ions; Group 7 form 1– ions.

Bohr-shell diagrams of a sodium atom and the sodium ion it forms.

Ionic Bonding

Ionic bonding occurs between metal and non-metal atoms.
Metal atoms lose electrons to non-metal atoms, forming positive and negative ions.
The oppositely charged ions are held together by strong electrostatic forces of attraction.
This electrostatic attraction is the ionic bond.
The overall charge of an ionic compound is zero.

Sodium loses one electron and chlorine gains an electron.

Dot-and-Cross Diagrams

Dot-and-cross diagrams show the arrangement of outer-shell electrons only.
Electrons from one atom are shown as dots, from the other as crosses.
Each ion is enclosed in square brackets with the charge written at the top right.
Example: NaCl – Na loses one electron (becomes Na⁺), Cl gains one electron (becomes Cl⁻).

Ionic bonding in sodium chloride.

Ionic Lattice Structure (Extended)

Ionic compounds form a giant lattice structure.
The lattice consists of a regular arrangement of alternating positive and negative ions.
Strong electrostatic forces act in all directions between oppositely charged ions.
Example: NaCl lattice – each Na⁺ is surrounded by Cl⁻ and vice versa.

The lattice structure of NaCl.

Properties of Ionic Compounds

Ionic compounds are solid at room temperature.
They have high melting and boiling points due to strong electrostatic forces.
They conduct electricity when molten or in aqueous solution (ions free to move).
They do not conduct electricity when solid (ions fixed in lattice).
Higher charge on ions leads to stronger forces and higher melting point (e.g., MgO > NaCl).

Electrical conductivity of ionic compounds.

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1.What change occurs to an atom when it forms a negative ion?
Easy
- AIt loses electrons.
- BIt gains protons.
- CIt gains electrons.
- DIt loses protons.
2.Which of the statements describes ionic bonding?
Easy
- AElectrostatic attraction between atoms
- BElectrostatic attraction between positively charged particles and delocalised electrons
- CElectrostatic attraction between oppositely charged ions
- DElectrostatic attraction between the nuclei of two atoms and a shared pair of electrons
3.The electronic configuration of an ion was determined to be 2.8.8. What could the identity of the ion be?
Medium
- ACa²⁺
- BS²⁻
- CBoth Ca²⁺ and S²⁻
- DNeither Ca²⁺ nor S²⁻
4.Calcium reacts with fluorine to form calcium fluoride. Which statement describes what happens to calcium atoms in this reaction?
Medium
- ACalcium ions lose electrons to form positive charges.
- BCalcium atoms gain 3 electrons to form positive ions.
- CCalcium ions gain 2 electrons to form positive ions.
- DCalcium atoms lose 2 electrons to form positive ions.
5.Three statements about sodium chloride are shown. 1. Sodium chloride has a low melting point because the attractive forces between the ions in the lattice are weak. 2. Sodium chloride conducts electricity in aqueous solution because the ions are free to move. 3. Sodium chloride conducts electricity when solid because the ions can carry an electric current through the lattice. Which statements are correct?
Medium
- A1 and 2
- B2 only
- C2 and 3
- D3 only
6.Ionic compounds are formed when a metal reacts with a nonmetal. Which two elements combine to form this kind of compound? Element Q: electronic structure 2.4 Element R: electronic structure 2.8 Element S: electronic structure 2.8.1 Element T: electronic structure 2.8.7
Medium
- AS and T
- BR and S
- CQ and R
- DQ and T
7.Ionic compounds are formed when metals react with nonmetals. Which row correctly describes the electron transfer when an ionic bond is formed and the nature of the bond?
Easy
- AMetal to nonmetal; Opposite ions attract
- BMetal to nonmetal; Opposite ions repel
- CMetal to metal; Same ions repel
- DNonmetal to metal; Opposite ions attract
8.Potassium and bromine chemically combine to form the compound potassium bromide. During formation, each bromine atom …..1….. one electron which is completely …..2….. from the outer shell of the potassium atom. The …..3….. force of attraction is formed from the attraction between the opposite charges on each ion. What words correctly fill gaps 1, 2 and 3?
Medium
- Aloses; shared; electrical
- Bloses; transferred; intermolecular
- Cgains; shared; electrostatic
- Dgains; transferred; electrostatic

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9.The bonding present in a substance determines the structure and properties of that substance. Which of the following statements is a correct description of the structure of an ionic compound?
Medium
- AA lattice structure with an irregular arrangement of alternating positive and negative ions
- BA lattice structure with a regular arrangement of alternating positive and negative ions
- CA random structure with a regular arrangement of alternating positive and negative ions
- DA random structure with an irregular arrangement of alternating positive and negative ions
10.Extended Only: The ionic lattice structure of potassium chloride is shown below. Which of the following statements best describes the bonding and structure of KCl?
Medium
- AA small lattice structure held together by electrostatic forces between oppositely charged ions which act in all directions.
- BA small lattice structure held together by electrostatic forces between like charged ions which act in all directions.
- CA giant lattice structure held together by electrostatic forces between oppositely charged ions which act in all directions.
- DA giant lattice structure held together by electrostatic forces between oppositely charged ions which act in one direction only.
11.What is an ion?
Easy
- AAn atom that has gained or lost protons
- BAn atom that has gained or lost neutrons
- CAn electrically charged atom or group of atoms formed by the loss or gain of electrons
- DA neutral atom with a full outer shell
12.What is the charge on an ion formed from a Group 2 element?
Easy
- A1+
- B2+
- C1-
- D2-
13.The table shows the melting points and electrical conductivities of four substances. Which substance is most likely an ionic compound? | Substance | Melting point (°C) | Conducts electricity when solid | Conducts electricity when molten | |-----------|--------------------|--------------------------------|----------------------------------| | W | 3550 | no | no | | X | 801 | no | yes | | Y | -91 | no | no | | Z | 3410 | yes | yes |
Medium
- AW
- BX
- CY
- DZ
14.An atom of element X has electronic configuration 2.8.2. An atom of element Y has electronic configuration 2.8.7. What is the formula of the ionic compound formed when X and Y react?
Medium
- AXY
- BXY2
- CX2Y
- DX2Y3
15.The electronic configurations of atoms P and Q are shown. P: 2.8.1 Q: 2.8.7 P and Q combine by ionic bonding. What is the formula of the compound produced?
Medium
- AP2Q
- BPQ2
- CPQ
- DP2Q3
16.Which statement explains why ionic compounds have high melting points?
Easy
- AThey have weak intermolecular forces between molecules.
- BThey have strong electrostatic forces between oppositely charged ions in a giant lattice.
- CThey have strong covalent bonds between atoms.
- DThey have weak forces between ions that require little energy to overcome.
17.Which two elements are most likely to form an ionic compound? Element A: electronic configuration 2.8.1 Element B: electronic configuration 2.8.7 Element C: electronic configuration 2.8.8 Element D: electronic configuration 2.4
Medium
- AA and B
- BA and C
- CB and D
- DC and D
18.The diagram shows the electronic configurations of two atoms. Which dot-and-cross diagram correctly represents the ionic compound formed? (Assume the outer shells are shown: Atom X: 2.8.2, Atom Y: 2.8.6)
Medium
- AX loses 2 electrons to Y, forming X2+ and Y2-, with both ions having full outer shells.
- BX gains 2 electrons from Y, forming X2- and Y2+.
- CX loses 1 electron to Y, forming X+ and Y-.
- DX shares 2 electrons with Y, forming a covalent bond.
19.Which statement about the lattice structure of an ionic compound is correct?
Easy
- AIt consists of a regular arrangement of alternating positive and negative ions.
- BIt consists of a random arrangement of positive and negative ions.
- CIt consists of a regular arrangement of molecules held by intermolecular forces.
- DIt consists of a giant covalent network of atoms.
20.What is the charge on an ion formed from a Group 6 element?
Easy
- A1+
- B2+
- C1-
- D2-
21.A student measures the electrical conductivity of an ionic compound at different temperatures. The results show no conductivity at 25°C, but conductivity increases sharply at 800°C. What is the most likely explanation?
Hard
- AAt 25°C the ions are fixed in the lattice; at 800°C the compound has melted and ions are free to move.
- BAt 25°C the compound is a gas; at 800°C it becomes a liquid.
- CAt 25°C the electrons are delocalised; at 800°C they become localised.
- DAt 25°C the compound is covalent; at 800°C it becomes ionic.
22.Which statement describes what happens to a chlorine atom when it forms a chloride ion?
Easy
- AIt loses one electron.
- BIt gains one electron.
- CIt loses one proton.
- DIt gains one proton.
23.What is the formula of the ionic compound formed between calcium and oxygen?
Medium
- ACaO
- BCaO2
- CCa2O
- DCa2O3
24.A student tests the electrical conductivity of an ionic compound in three states: solid, molten, and dissolved in water. Which row shows the correct results?
Medium
- ASolid: no, Molten: yes, Dissolved: yes
- BSolid: yes, Molten: no, Dissolved: no
- CSolid: no, Molten: no, Dissolved: yes
- DSolid: yes, Molten: yes, Dissolved: no
25.Which of the following dot-and-cross diagrams correctly shows the arrangement of electrons in lithium sulfide?
Medium
- ATwo Li atoms each lose one electron to a S atom, forming Li⁺ and S²⁻, with S showing 8 outer electrons.
- BOne Li atom loses one electron to a S atom, forming Li⁺ and S⁻.
- CTwo Li atoms each gain one electron from a S atom, forming Li⁻ and S²⁺.
- DOne Li atom gains one electron from a S atom, forming Li⁻ and S⁺.
26.A student measures the electrical conductivity of an ionic compound at different temperatures. The results show no conductivity at 25°C, but conductivity increases as temperature rises above the melting point. Which statement explains this?
Medium
- AAt 25°C the ions are fixed in the lattice; when molten, the ions are free to move and carry charge.
- BAt 25°C the ions are free to move; when molten, the ions become fixed.
- CAt 25°C the electrons are delocalised; when molten, the electrons are localised.
- DAt 25°C the compound is covalent; when molten, it becomes ionic.
27.Extended Only: A student analysed an ionic compound and a covalent compound using a melting point apparatus. She found the ionic compound had a much higher melting point than the covalent compound. Which statement explains this observation?
Medium
- AIonic compounds are formed from metals only.
- BIonic compounds are formed from nonmetals and nonmetals.
- CThere are strong electrostatic forces of attraction in ionic compounds.
- DThere are strong intermolecular forces in ionic compounds.
28.Extended Only: A Group 2 metal atom reacts with a Group 6 non-metal atom to form an ionic compound. Which of the following dot-and-cross diagrams correctly represents the ionic compound formed? (Assume the outer shell electrons only are shown.)
Medium
- AThe metal atom (Group 2) loses two electrons, shown as dots, to the non-metal atom (Group 6), shown as crosses, resulting in a 2+ metal ion and a 2- non-metal ion, each with full outer shells.
- BThe metal atom gains two electrons from the non-metal atom, forming a 2- metal ion and a 2+ non-metal ion.
- CThe metal atom shares two electrons with the non-metal atom, forming a covalent bond.
- DThe metal atom loses one electron to the non-metal atom, forming a 1+ metal ion and a 1- non-metal ion.
29.Which of the following describes the formation of a positive ion?
Easy
- AAn atom gains electrons
- BAn atom loses electrons
- CAn atom gains protons
- DAn atom loses protons
30.Which of the following is the correct definition of an ionic bond?
Easy
- AThe sharing of electrons between atoms
- BThe electrostatic attraction between oppositely charged ions
- CThe attraction between a positive ion and delocalised electrons
- DThe force between molecules
31.An atom of element X has electronic configuration 2,8,2. An atom of element Y has electronic configuration 2,8,7. What is the formula of the ionic compound formed between X and Y?
Medium
- AXY
- BXY2
- CX2Y
- DX2Y3
32.Extended Only: Which of the following statements about the electrical conductivity of ionic compounds is correct?
Easy
- AIonic compounds conduct electricity in solid state because ions are free to move
- BIonic compounds conduct electricity in molten state because ions are free to move
- CIonic compounds do not conduct electricity in any state
- DIonic compounds conduct electricity only when dissolved in water, not when molten
33.Extended Only: Magnesium oxide has a higher melting point than sodium chloride. Which statement explains this?
Medium
- AMagnesium oxide has stronger electrostatic forces because the ions have higher charges
- BSodium chloride has stronger electrostatic forces because the ions are smaller
- CMagnesium oxide has weaker electrostatic forces because the ions are larger
- DSodium chloride has a giant lattice structure while magnesium oxide does not
34.Extended Only: In a dot-and-cross diagram for lithium sulfide (Li2S), which of the following is correct?
Medium
- AEach lithium atom loses one electron and sulfur gains two electrons; lithium ions are shown as Li+ and sulfide ion as S2-
- BEach lithium atom gains one electron and sulfur loses two electrons
- CLithium atoms share electrons with sulfur atoms
- DLithium atoms gain two electrons and sulfur loses two electrons
35.Which of the following pairs of elements is most likely to form an ionic compound?
Easy
- ACarbon and oxygen
- BSodium and chlorine
- CNitrogen and hydrogen
- DSilicon and carbon
36.A student measures the electrical conductivity of an ionic compound at different temperatures. The results show no conductivity at 25°C, but conductivity increases as the temperature rises above 800°C. Which statement explains this observation?
Medium
- AAt 25°C the ions are fixed in the lattice and cannot move; above 800°C the compound melts and ions are free to move.
- BAt 25°C the ions are fixed in the lattice and cannot move; above 800°C the electrons become delocalised.
- CAt 25°C the ions can move freely; above 800°C they become fixed.
- DAt 25°C the compound is a liquid; above 800°C it becomes a gas.
37.The table shows the properties of four substances. Which substance is most likely an ionic compound? | Substance | Melting point (°C) | Boiling point (°C) | Conducts electricity when solid | Conducts electricity when liquid | |-----------|-------------------|-------------------|-------------------------------|--------------------------------| | W | 3410 | 5930 | yes | yes | | X | 801 | 1413 | no | yes | | Y | 3550 | 4830 | no | no | | Z | -91 | 98 | no | no |
Medium
- AW
- BX
- CY
- DZ
38.Negative ions are called cations.
Easy
True or false?
39.Which group of elements forms ions with a 2+ charge?
Easy
- AGroup 1
- BGroup 2
- CGroup 6
- DGroup 7
40.Which of the following are properties of ionic compounds? (Select all that apply)
Medium
- AHigh melting points
- BConduct electricity when solid
- CConduct electricity when molten or in solution
- DUsually solid at room temperature
- ELow boiling points
41.In a dot-and-cross diagram for sodium chloride, what is shown?
Easy
- AOnly the outer-shell electrons of sodium and chlorine
- BAll electrons of sodium and chlorine
- CThe nucleus and all electrons of both atoms
- DThe inner-shell electrons only
42.Ionic compounds have a giant lattice structure consisting of alternating positive and negative ions.
Easy
True or false?
43.Match each group with the charge on the ion it forms.
Easy
- Group 1
- Group 2
- Group 6
- Group 7
- 1+
- 2+
- 2-
- 1-
44.Arrange the steps in the formation of an ionic bond between sodium and chlorine in the correct order.
Easy
- Sodium loses one electron to become a Na+ ion
- Chlorine gains one electron to become a Cl- ion
- The Na+ and Cl- ions are attracted by electrostatic forces
- Sodium and chlorine atoms come together
45.Match each group of the periodic table with the charge on the ion it typically forms.
Easy
- Group 1
- Group 2
- Group 6
- Group 7
- 1+
- 2+
- 2−
- 1−
46.Arrange the following steps in the correct order for the formation of an ionic bond between sodium and chlorine.
Easy
- Sodium atom loses one electron to become a Na+ ion.
- Chlorine atom gains one electron to become a Cl− ion.
- The Na+ and Cl− ions are held together by electrostatic forces.
- Sodium and chlorine atoms come into contact.
47.The table shows the melting points and electrical conductivities of four substances. Which substance is most likely an ionic compound? | Substance | Melting point (°C) | Conductivity when solid | Conductivity when molten | |---|---|---|---| | A | 113 | poor | poor | | B | 3550 | poor | good | | C | 801 | poor | good | | D | -39 | good | good |
Medium
- AA
- BB
- CC
- DD
48.Complete the sentences about ionic bonding.
Easy
Ionic compounds are formed when ____ atoms react with ____ atoms. Metal atoms ____ electrons to become positively charged ions, while non-metal atoms ____ electrons to become negatively charged ions.
49.How many electrons does a calcium atom (Group 2) lose to form a calcium ion?
Easy
50.State the term for the electrostatic attraction between oppositely charged ions in an ionic compound.
Easy
51.Complete the following sentences about ionic bonding.
Easy
Ionic compounds are formed when ____ atoms react with ____ atoms. Metal atoms ____ electrons to become positively charged ions.
52.A student measures the electrical conductivity of an ionic compound at different temperatures. The results show no conductivity at 25°C, but conductivity increases sharply at 801°C. What is the melting point of the compound in °C?
Medium
53.Explain why magnesium oxide has a higher melting point than sodium chloride.
Hard
54.How many electrons does a calcium atom (Group 2) lose to form a calcium ion?
Easy
- A2
- B4
- C1
- D3
55.A student measures the electrical conductivity of an ionic compound at different temperatures. The results show no conductivity at 25°C, but conductivity increases sharply at 801°C. What is the melting point of the compound in °C?
Medium
- A801 °C
- B721 °C
- C881 °C
- D961 °C

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