Final Review Sheet

Final Review Sheet - Chapter 9: Chemical Bonding I: Lewis...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 9: Chemical Bonding I: Lewis Theory 1) Bond Relationships -the shorter the bond, the stronger the bond -relative strength: single bond < double bond < triple bond -increased electron density in bonding internuclear region -single bond rotation allowed, double bond no rotation 2) Polar Covalent, Nonpolar Covalent, and Ionic Bonds electronegativity difference bond type example small (0 - 0.4) covalent Cl 2 intermediate (0.4 - 2.0) polar covalent HCl large (2.0+) ionic NaCl -electronegativity trends -electron density models -red (negative), blue (positive) - 3) Lewis Structures -drawing structures 1) sum all valence electrons 2) write atom symbols to show connectivity 3) draw a single bond between each atom pair bonded together 4) complete octets 5) place leftover electrons on central atom 6) not enough electrons to give to central atom an octet, try multiple bonds -octet exceptions -less than octet: B, Be, H -more than octet: P, S, I, As (3 rd period or below) -resonance structures (example: CO
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

Final Review Sheet - Chapter 9: Chemical Bonding I: Lewis...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online