Atoms electron poor region electron rich region e

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: r region electron rich region e- poor e- rich H F δ+ H F δ- Bond polarity: depends on the difference in electronegativity between the two atoms forming the bond. Electronegativity Electronegativity: the ability of an atom to attract electrons in a chemical bond. Electron affinity: the energy changes that occurs when an electron energy is added to a gaseous atom or ion. Electronegativity: -the relative ability, -Unmeasurable F is the highest Electron Electron Affinity: - measurable, Cl is the highest Cl X (g) + e- X-(g) Electrons are shared but not equally Ionization energy Electron Electron Affinity Polar covalent bonds Bond polarity: depends on the difference in electronegativity between the two atoms forming the bond. electronegativity If the difference in electronegativity •less than < 0.5 non-polar covalent •greater than > 2 ionic •between 0.5 and 2 polar covalent Electrons are shared but not equally Exercise Decide which of these bonds are polar polar C–H EN difference = 2.5 –2.1 = 0.4 NonNon-polar covalent bond K – Cl Ionic bond H – Cl EN difference = 3.0-0.8 = 2.2 K+ – Cl- complete charge separation EN difference = 3.0- 2.1 = 0.9 3.0Hδ+ – Clδpartial charge polar covalent bond separation Bond polarity---Dipole Bond polarity---Dipole Moment (µ) Dipole moment: quantifies the polarity related to polarity partial partial charge separations Dipole moment = charge (Q)× distance (d) µ= Q×d +Q d Q Unit of Q = “coulomb” 1 electron charge = 1...
View Full Document

Ask a homework question - tutors are online