Lesson 10.5 - 10.7

Non Polar Molecules: 

  • Made up of only one element (Monatomic and Diatomic atoms). For example: N2, O2, CI2, H2, F2, He, Ne, Ar, Xe

  • Molecules that contain only Carbon and Hydrogen. Example: CH4, C2H6

  • The compound has symmetry. Example: CF4, SBr6, CO2, BH3

  • If there is no symmetry (only two atoms), check the Electronegativity difference. If the electronegativity difference is less than 0.5, it is nonpolar. 


Polar Molecules:

  • If Hydrogen is directly bonded to N, O, F,  (H-N,  H-O,  H-F),  it is polar

  • If the molecule lacks symmetry, it is polar. 

  • If the electronegativity difference is larger than 0.5, it is polar

- If a molecule has one polar bond, and multiple nonpolar bonds, it is still considered to be polar.


σ Bonds = only single bond

𝛑 bonds = double and triple bonds




Hybridization:

  • A single bond, a double bond, a triple bond, and a lone pair all have a value of one (1) bond. 

  • 6 points = sp3d2,  5 bonds = sp3d,  4 points = sp3,   3 points = sp2,   2 points = sp

  • Example: Methane - have 4 single bonds around the Central atom, Carbon,  therefore being sp3 hybridized: