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Draw Lewis electron dot structures for oxygen and ozone - HSC - SSCE Chemistry - Question 18 - 2008 - Paper 1
Question 18
Draw Lewis electron dot structures for oxygen and ozone. Account for the differences in the properties of oxygen and ozone on the basis of their molecular structure... show full transcript
Worked Solution & Example Answer:Draw Lewis electron dot structures for oxygen and ozone - HSC - SSCE Chemistry - Question 18 - 2008 - Paper 1
Step 1
Draw Lewis electron dot structures for oxygen and ozone.
Answer
To draw the Lewis dot structure for oxygen (O₂):
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Oxygen has 6 valence electrons.
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Each oxygen atom shares two electrons, forming a double bond.
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The structure can be represented as:
O = O
Each oxygen has 4 unshared electrons (2 pairs).
For ozone (O₃):
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Ozone has a total of 18 valence electrons (3 oxygens, 6 each).
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Arrange it with one double bond and one single bond:
O || O - O
The resonance structures should be indicated, showing that the double bond can be between either pair of oxygen atoms.
Step 2
Account for the differences in the properties of oxygen and ozone on the basis of their molecular structure and bonding.
Answer
Oxygen (O₂) is a diatomic molecule with a double bond between the two oxygen atoms, resulting in a linear shape. This structure leads to a higher reactivity and is essential for combustion processes.
Ozone (O₃), on the other hand, has a bent molecular geometry due to the presence of a resonance structure, where one oxygen atom is bonded to the other two via a double bond and a single bond. This bent structure alters its physical properties, such as being a pale blue gas at room temperature, and it has different chemical properties, including strong oxidizing capabilities.
In summary:
- O₂: linear structure, non-polar, can efficiently bond with other substances.
- O₃: bent structure, polar, has stronger intermolecular forces due to its geometry, which impacts its boiling point and reactivity.