11. Answer any two of the parts (a), (b) and (c) - Leaving Cert Chemistry - Question 11 - 2019
Question 11
11. Answer any two of the parts (a), (b) and (c).
(a) (i) Define electronegativity.
(ii) Account for the increase in electronegativity values across the second per... show full transcript
Worked Solution & Example Answer:11. Answer any two of the parts (a), (b) and (c) - Leaving Cert Chemistry - Question 11 - 2019
Step 1
Define electronegativity.
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Answer
Electronegativity is defined as the number expressing the relative (measure of) attraction of an atom for shared pairs of electrons in a covalent bond.
Step 2
Account for the increase in electronegativity values across the second period of the periodic table.
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Answer
The increase in electronegativity values across the second period is attributed to several factors: the effective nuclear charge increases due to the increasing number of protons, while the atomic radius decreases. This results in a stronger attraction of the nucleus for the bonding electrons.
Step 3
Use electronegativity values to predict the type of bonding in oxygen difluoride (OF2).
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Oxygen difluoride (OF2) has slightly polar covalent bonding. This is due to the difference in electronegativity between oxygen and fluorine.
Step 4
State and account for the shape of the OF2 molecule.
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The shape of the OF2 molecule is V-shaped planar, or bent. This is due to the presence of two bond pairs and two lone pairs surrounding the oxygen atom.
Step 5
Select, giving your reasons, which of these angles is the most probable value for the bond angle in oxygen difluoride.
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Answer
The most probable value for the bond angle in oxygen difluoride is 103°. This is because the repulsion between two bond pairs (2 b.p.) and two lone pairs (1 l.p.) reduces the bond angle, making it less than the typical 109.5° for tetrahedral arrangements.
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