Graded Assignment
Unit Assessment, Part 2: Bonds
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Describe electronegativity, and explain the trend of electronegativity in the Periodic Table.
1. Answer:
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Describe polar covalent bonds using water as an example.
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What are bonds in metals like?
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Electronegativity is a qualitative measure of how much an atom attracts electrons in a covalent bond. In the Periodic Table, electronegativity generally increases from left to right across a period and decreases down a group. For example, in Group 17 (halogens), electronegativity increases as you move from top to bottom.

Polar covalent bonds result from differences in electronegativity between atoms. Water (H2O) is an example of a polar covalent bond because oxygen is significantly more electronegative than hydrogen, leading to a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms.

Metallic bonds involve a lattice of positive metal ions immersed in a sea of delocalized electrons. These bonds are characterized by the sharing of electrons among a large number of metal atoms, giving metals their unique properties like conductivity and malleability.

Learn more about Chemical Bonds here:

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