Period 2 and 3

Last updated: 12/03/2020

Edexcel A-Level Chemistry Atomic structure and the periodic table Period 2 and 3

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Question 1 of 20

1. Question
What is the correct described trend moving across periods 2 and 3?
- Metal elements to non-metal elements
- Non-metal elements to metal elements
- Metal to gases
- Non-metals to gases
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Question 2 of 20

2. Question
What type of molecular structure do elements between groups 1 – 13 have within periods 2 and 3?
- Giant metallic
- Simple molecular
- Giant covalent
- Giant ionic
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Question 3 of 20

3. Question
What type of molecular structure do elements in group 14 have within periods 2 and 3?
- Giant covalent
- Simple molecular
- Giant metallic
- Giant ionic
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Question 4 of 20

4. Question
What type of molecular structure do elements between groups 15 – 18 have within periods 2 and 3?
- Simple molecular
- Giant metallic
- Giant covalent
- Giant ionic
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Question 5 of 20

5. Question
What is the overall melting point trend across groups 1 – 14 in period 2 and 3?
- Steady increase
- Sharp increase
- No change
- Sharp decrease
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Question 6 of 20

6. Question
Explain the melting point trend across groups 1-14 in period 2 and 3.
- Steady increase, as elements have giant structures with increasing nuclear charge as well as an increasing number of electrons in their outer shell. This results in stronger nuclear attraction, as more bonds can be made.
- Steady decrease, as elements have simple structures with decreasing nuclear charge as well as a decreasing number of electrons in their outer shell. This results in weaker nuclear attraction, as less bonds can be made.
- Sharp increase, as elements have giant structures with increasing nuclear charge as well as an increasing number of electrons in their outer shell. This results in stronger nuclear attraction, as more bonds can be made.
- Sharp decrease, as elements have simple structures with decreasing nuclear charge as well as a decreasing number of electrons in their outer shell. This results in weaker nuclear attraction, as less bonds can be made.
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Question 7 of 20

7. Question
What is the overall melting point trend across groups 14 – 15 in period 2 and 3?
- Sharp decrease
- Steady inrease
- Sharp increase
- No changes
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Question 8 of 20

8. Question
Explain the melting point trend across groups 14 – 15 in period 2 and 3.
- A sharp decrease, as elements have simple molecular structures therefore containing weaker intermolecular forces that need less energy break.
- A sharp increase, as elements have giant molecular structures therefore containing stronger intermolecular forces that need more energy break.
- A steady decrease, as elements have simple molecular structures therefore containing weaker intermolecular forces that need less energy break.
- A steady increase, as elements have giant molecular structures therefore containing stronger intermolecular forces that need more energy break.
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Question 9 of 20

9. Question
What is the overall melting point trend across groups 15 – 18 in period 2 and 3?
- Remain low
- Remain high
- Sharp increase
- Remain the same
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Question 10 of 20

10. Question
Explain the melting point trend across groups 15 – 18 in period 2 and 3.
- Remain low, as elements have simple molecular structures therefore containing weaker intermolecular forces that need less energy to break.
- Remain high, as elements have giant molecular structures therefore containing stronger intermolecular forces that need more energy to break.
- Sudden increase, as the elements are changing from simple molecular structures to giant molecular structures.
- Sudden decrease, as the elements are changing from giant molecular structures to simple molecular structures.
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Question 11 of 20

11. Question
What type of bonding do elements between group 1 – 13 have within periods 2 and 3?
- Metallic bonding
- Ionic bonding
- Covalent bonding
- Covalent bonding, with intermolecular bonding between molecules
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Question 12 of 20

12. Question
What type of bonding do elements in group 14 have within periods 2 and 3?
- Covalent bonding
- Ionic bonding
- Metllic bonding
- Covalent bonding, with intermolecular bonding between molecules
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Question 13 of 20

13. Question
What type of bonding do elements between group 18 – 13 have within periods 2 and 3?
- Covalent bonding, with intermolecular bonding between molecules
- Ionic bonding
- Metallic bonding
- Covalent bonding
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Question 14 of 20

14. Question
What type of forces do elements between groups 1 – 13 have within periods 2 and 3?
- Strong intermolecular forces between positive ions and delocalised electrons
- Weak intermolecular forces between molecules
- Strong intermolecular forces between atoms
- Weak intermolecular forces between positive ions and delocalised electrons
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Question 15 of 20

15. Question
What type of forces do elements in group 14 have within periods 2 and 3?
- Strong intermolecular forces between atoms
- Weak intermolecular forces between positive ions and delocalised electrons
- Weak intermolecular forces between molecules
- Strong intermolecular forces between positive ions and delocalised electrons
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Question 16 of 20

16. Question
What type of forces do elements between groups 15 – 18 have within periods 2 and 3?
- Weak intermolecular forces between molecules
- Strong intermolecular forces between positive ions and delocalised electrons
- Strong intermolecular forces between atoms
- Weak intermolecular forces between positive ions and delocalised electrons
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Question 17 of 20

17. Question
Describe the overall melting point trend continuing through the following elements. Na, Mg, Al
- Increases, as the nuclear charge increases resulting in ionic size decreasing.
- Increases from Na-Mg as the nuclear charge increases. However, the nuclear charge then decreases from Mg-Al.
- Stays the same, as nuclear charge does not change throughout the elements.
- Decreases, as the nuclear charge decreases resulting in the ionic size increasing. As the number of outer shell electrons are decreases there is a weaker nuclear attraction.
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Question 18 of 20

18. Question
Describe the overall melting point trend continuing throughout the following elements. Li, Be, B
- Increases, as the nuclear charge increases resulting in ionic size decreasing.
- Increases from Na-Mg as the nuclear charge increases. However, the nuclear charge then decreases from Li-Be.
- Stays the same, as nuclear charge does not change throughout the elements.
- Decreases, as the nuclear charge decreases resulting in the ionic size increasing. As the number of outer shell electrons are decreases there is a weaker nuclear attraction.
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Question 19 of 20

19. Question
Out of the following, which lattice is made from carbon?
- Diamond
- Sodium chloride
- Lead
- Water
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Question 20 of 20

20. Question
Out of the following, which lattice is made from carbon?
- Graphite
- Benzene
- Aluminium fluoride
- Sodium chloride
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