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Chemical Bonding (C - Dot and Cross Diagrams (Non-metals that has a…
Chemical Bonding
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B - Polarity
In solutions, atoms may or may not be able to exist independently and they have to form molecules.
Ions can exist independently in solutions.
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0 - 0.4 electronegativity difference means its covalent
0.4 - 2 electronegativity difference means its polar covalent.
2 - 4 electronegativity difference means its ionic.
Polar covalent bonds happens when 1 atom is more electronegative than the other so it tends to pull the charged electron closer to its nucleus making it delta negative leaving the other atom as delta positive.
In non-polar covalent bonds, the differences isn't high so they attract the electron at the equal strength so no one is slightly positive or negative.
Ionic bonds happens when 1 atoms is so much more electronegative that it comepletely removes the electron from the other atom making it self negative and the other positive.
Dative covalent bonds is when an atom bonds to a lone pair of electrons on another atom.
Since there are less electrons the the cation, it means that the positive nucleus can pull harder on the existing electrons making the radius smaller. This means it is more polarising which distorts the electron field around the anion. Pulling electrons closer to the cation
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D - Metallic bonding
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Because the metallic ions are arranged in a general structure, they have layers of metallic ions on top of more layers which can easily slide across another.
They have a sea of delocalised electrons that can move freely and carry a charge. Therefore they can conduct electricity.
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