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Secondary 3 Chemistry Atomic Structure Bonding Quiz

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Secondary 3 Chemistry Quiz - Atomic Structure Bonding

Name: __________________________
Class: __________________________
Date: __________________________
Score: ________ / 40

Duration: 45 minutes
Total Marks: 40

Instructions:

Answer all questions.
Write your answers in the spaces provided.
For questions requiring diagrams, use a pencil for clarity.
The number of marks for each question is given in brackets [ ] at the end of the question.

Section A: Atomic Structure and Isotopes (Questions 1–5)

1. The table below shows the number of protons, neutrons, and electrons in four different particles, W, X, Y, and Z.

Particle	Protons	Neutrons	Electrons
W	6	6	6
X	6	8	6
Y	7	7	7
Z	6	6	8

(a) Which two particles are isotopes of the same element? Explain your answer.
[2]

(b) Which particle is a negative ion? Give a reason for your answer.
[1]

2. Chlorine exists as two isotopes: $^{35}\text{Cl}$ and $^{37}\text{Cl}$ . The relative atomic mass of chlorine is 35.5.

(a) Define the term isotope.
[2]

(b) Explain why the relative atomic mass of chlorine is not a whole number.
[1]

3. An atom of element Q has the electronic configuration 2, 8, 3.

(a) Deduce the group and period of element Q in the Periodic Table.
[2]
Group: _______________ Period: _______________

(b) Element Q reacts with oxygen to form an oxide. Deduce the formula of this oxide.
[1]
Formula: _______________

4. Complete the table below for the subatomic particles.

Particle	Relative Mass	Relative Charge	Position in Atom
Proton	1	+1	Nucleus
Neutron	_______	_______	Nucleus
Electron	1/1840	_______	_______________

[3]

5. Why do isotopes of the same element have identical chemical properties?
[1]

Section B: Chemical Bonding (Questions 6–12)

6. Magnesium chloride ( $\text{MgCl}_2$ ) is an ionic compound.

(a) Describe, in terms of electron transfer, how a magnesium atom reacts with chlorine atoms to form magnesium chloride. You may use a diagram to help your answer.
[3]

(b) Draw the 'dot-and-cross' diagram for magnesium chloride. Show only the outer shell electrons. Include the charges on the ions.
[2]

Answer space

7. Carbon dioxide ( $\text{CO}_2$ ) is a covalent compound.

(a) Draw the 'dot-and-cross' diagram for a molecule of carbon dioxide. Show only the outer shell electrons.
[2]

Answer space

(b) Explain why carbon dioxide has a low boiling point despite having strong covalent bonds.
[2]

8. The table below shows the properties of three substances: A, B, and C.

Substance	Melting Point (°C)	Electrical Conductivity (Solid)	Electrical Conductivity (Molten)
A	801	No	Yes
B	-78	No	No
C	1083	Yes	Yes

(a) Identify the type of structure and bonding in Substance A.
[1]
Structure: __________________________ Bonding: __________________________

(b) Explain why Substance A conducts electricity when molten but not when solid.
[2]

9. Graphite and diamond are both allotropes of carbon.

(a) Explain why graphite is soft and can be used as a lubricant.
[2]

(b) Explain why diamond is very hard.
[1]

10. Silicon(IV) oxide ( $\text{SiO}_2$ ) has a giant covalent structure.

(a) Describe the arrangement of atoms in silicon(IV) oxide.
[1]

(b) Explain why silicon(IV) oxide has a very high melting point.
[2]

11. Ammonia ( $\text{NH}_3$ ) is a simple molecular substance.

(a) How many shared pairs of electrons are there in one molecule of ammonia?
[1]
Answer: _______________

(b) Ammonia has a low melting point. Explain why.
[1]

12. Brass is an alloy of copper and zinc.

(a) Draw a diagram to represent the structure of brass. Label the copper and zinc atoms.
[2]

Answer space

(b) Explain why brass is harder than pure copper.
[2]

Section C: Structure and Properties (Questions 13–20)

13. Substance X is a white solid. It dissolves in water to form a solution that conducts electricity. Substance Y is a white solid. It does not dissolve in water and does not conduct electricity in any state.

Suggest the type of bonding in:
Substance X: __________________________ [1]
Substance Y: __________________________ [1]

14. Explain why ionic compounds generally have high melting points.
[2]

15. Consider the following substances: Sodium chloride, Water, Diamond, Copper.

Which substance:
(a) Has a giant metallic structure? __________________________ [1]
(b) Has a simple molecular structure? __________________________ [1]
(c) Has a giant covalent structure? __________________________ [1]

16. A student states: "Covalent bonds are weak because covalent compounds like methane have low melting points."

Is this statement correct? Explain your answer.
[2]

17. Fullerenes (e.g., $\text{C}_{60}$ ) are forms of carbon.

(a) What is the shape of a $\text{C}_{60}$ molecule?
[1]

(b) Unlike diamond, $\text{C}_{60}$ is soluble in some organic solvents. Suggest why, referring to its structure.
[1]

18. Explain why metals are malleable (can be hammered into shape).
[2]

19. The diagram below represents the lattice structure of sodium chloride.

Image pending generation for this question.

(a) What is the ratio of sodium ions to chloride ions in the lattice?
[1]
Ratio: _______________

(b) Why is the formula written as NaCl and not $\text{Na}_2\text{Cl}_2$ ?
[1]

20. Compare the electrical conductivity of solid lead(II) bromide and molten lead(II) bromide. Explain the difference.
[3]

[End of Quiz]

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Answers

Secondary 3 Chemistry Quiz - Atomic Structure Bonding (Answer Key)

1.
(a) W and X. [1]
They have the same number of protons (6) but different numbers of neutrons. [1]
(b) Z. [1]
It has more electrons (8) than protons (6), giving it a net negative charge.
(c) 14. [1]
(6 protons + 8 neutrons).

2.
(a) Atoms of the same element (same proton number) [1] with different numbers of neutrons (different nucleon numbers). [1]
(b) It is a weighted average of the masses of its isotopes based on their relative abundances. [1]
(c) Let $x$ be the abundance of $^{35}\text{Cl}$ . Then $(100-x)$ is the abundance of $^{37}\text{Cl}$ .
$35x + 37(100-x) = 35.5 \times 100$
$35x + 3700 - 37x = 3550$
$-2x = -150$
$x = 75$
Abundance of $^{35}\text{Cl}$ is 75%. [2]
(1 mark for correct setup, 1 mark for correct answer)

3.
(a) Group 13 (or III), Period 3. [2]
(b) $\text{Q}_2\text{O}_3$ . [1]
(Q has valency 3, O has valency 2).

4.
Neutron Relative Mass: 1 [1]
Neutron Relative Charge: 0 [1]
Electron Relative Charge: -1 [1]
Electron Position: Shells / Orbitals / Around the nucleus [1]
(Note: Only 3 marks available, accept any 3 correct entries)

5.
They have the same number of electrons in the outer shell (valence electrons). [1]
(Chemical properties depend on electronic configuration)

6.
(a) Magnesium atom loses 2 electrons [1] to form $\text{Mg}^{2+}$ ion. Each chlorine atom gains 1 electron [1] to form $\text{Cl}^-$ ion. Electrostatic attraction between oppositely charged ions forms the bond. [1]
(b) Diagram:

Mg ion shown with empty outer shell (or inner shell shown as 8), labeled $[\text{Mg}]^{2+}$ . [1]
Two Cl ions shown with 8 electrons in outer shell (7 crosses/dots + 1 transferred), labeled $[\text{Cl}]^-$ . [1]
Correct use of dots and crosses to distinguish origin.

7.
(a) Diagram:

Central C atom double bonded to two O atoms. [1]
C shares 4 electrons (2 pairs) with each O. Each O has 4 non-bonding electrons. Total 8 electrons around C, 8 around each O. [1]
(b) $\text{CO}_2$ consists of simple molecules. [1]
The forces between the molecules (intermolecular forces) are weak and require little energy to overcome. [1]
(Note: Do not say covalent bonds break)

8.
(a) Structure: Giant Ionic [1] Bonding: Ionic [1]
(b) In solid state, ions are fixed in position and cannot move. [1]
In molten state, ions are free to move and carry charge. [1]
(c) Structure: Lattice of positive metal ions. [1]
Bonding: Attraction between positive ions and a 'sea' of delocalized electrons. [1]

9.
(a) Graphite has a layered structure. [1]
Weak van der Waals forces between layers allow them to slide over each other. [1]
(b) Diamond has a giant covalent structure where each carbon atom is strongly bonded to 4 others in a rigid 3D network. [1]
(c) In graphite, each carbon atom has one delocalized electron that is free to move and conduct charge. [1]
In diamond, all 4 outer electrons are used in covalent bonds, so there are no free/delocalized electrons. [1]

10.
(a) Each silicon atom is covalently bonded to 4 oxygen atoms, and each oxygen atom is bonded to 2 silicon atoms in a giant lattice. [1]
(b) Many strong covalent bonds must be broken to melt the substance. [1]
This requires a large amount of heat energy. [1]

11.
(a) 3. [1]
(b) Weak intermolecular forces between ammonia molecules. [1]

12.
(a) Diagram showing a regular lattice of atoms of two different sizes (Cu and Zn). [1]
Labels clearly indicating Copper and Zinc atoms. [1]
(b) The different sized atoms (Zn) disrupt the regular lattice structure of copper. [1]
This prevents layers from sliding over each other easily. [1]

13.
Substance X: Ionic [1]
Substance Y: Covalent (Giant or Simple Molecular) [1]
(Accept Covalent for Y as it doesn't conduct. If it were giant covalent like SiO2, it wouldn't dissolve. If simple molecular, it might not dissolve or conduct. Given "white solid" and insoluble/non-conducting, Covalent is the key distinction from Ionic).

14.
There are strong electrostatic forces of attraction between oppositely charged ions. [1]
A large amount of energy is required to overcome these forces. [1]

15.
(a) Copper [1]
(b) Water [1]
(c) Diamond [1]

16.
No, the statement is incorrect. [1]
Covalent bonds within the molecule are strong. It is the weak intermolecular forces between molecules that are broken during melting, not the covalent bonds. [1]

17.
(a) Spherical / Ball-shaped / Buckyball. [1]
(b) $\text{C}_{60}$ consists of discrete molecules with weak intermolecular forces, allowing solvent molecules to interact/separate them. (Unlike giant structures). [1]

18.
Layers of positive ions can slide over each other. [1]
The delocalized electrons maintain the bonding throughout the structure, preventing it from breaking. [1]

19.
(a) 1:1 [1]
(b) NaCl represents the simplest ratio (empirical formula) of ions in the giant lattice. [1]

20.
Solid lead(II) bromide does not conduct electricity. [1]
Molten lead(II) bromide does conduct electricity. [1]
In the solid, ions are fixed in position. In the molten state, ions are free to move and carry charge. [1]