Presentation is loading. Please wait.

Presentation is loading. Please wait.

3.7: Polar Covalent Bonds and Electronegativity

Published bySucianty Pranoto Modified over 5 years ago

Similar presentations

Presentation on theme: "3.7: Polar Covalent Bonds and Electronegativity"— Presentation transcript:

1 3.7: Polar Covalent Bonds and Electronegativity
5

2 Electronegativity Electronegativity is a measure of an element to attract electrons toward itself when bonded to another element. An electronegative element attracts electrons. An electropositive element releases electrons. 2

3 Pauling Electronegativity Scale
Electronegativity increases from left to right in the periodic table. Electronegativity decreases going down a group. 5

4

5 Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. F : .. H—H : N nonpolar bonds connect atoms of the same electronegativity 7

6 Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. O .. H d+ d- d- d+ d- F : .. H d+ d- : O C O : .. .. polar bonds connect atoms of different electronegativity 7

7 3.7 Molecular Dipole Moments
1

8 (expressed in Debye units)
Dipole Moment A substance possesses a dipole moment if its centers of positive and negative charge do not coincide. m = e x d (expressed in Debye units) + — not polar 17

9

10

11

12 (expressed in Debye units)
Dipole Moment A substance possesses a dipole moment if its centers of positive and negative charge do not coincide. m = e x d (expressed in Debye units) — + polar 17

13 Molecular Dipole Moments
molecule must have polar bonds necessary, but not sufficient need to know molecular shape because individual bond dipoles can cancel 18

14 Molecular Dipole Moments
Carbon dioxide has no dipole moment; m = 0 D 18

15 Comparison of Dipole Moments
Carbon tetrachloride Dichloromethane m = 0 D m = 1.62 D 20

16 Carbon tetrachloride m = 0 D
Resultant of these two bond dipoles is Resultant of these two bond dipoles is m = 0 D Carbon tetrachloride has no dipole moment because all of the individual bond dipoles cancel. 20

17 Dichloromethane Resultant of these two bond dipoles is Resultant of these two bond dipoles is m = 1.62 D The individual bond dipoles do not cancel in dichloromethane; it has a dipole moment. 20

Download ppt "3.7: Polar Covalent Bonds and Electronegativity"

Similar presentations

MOLECULAR SHAPE HOW DOES SHAPE AND POLARITY DETERMINE FUNCTION AND PROPERTIES OF MOLECULES?

MOLECULAR SHAPE HOW DOES SHAPE AND POLARITY DETERMINE FUNCTION AND PROPERTIES OF MOLECULES?
Polar Molecules H F electron rich region electron poor region d+ d-

Polar Molecules H F electron rich region electron poor region d+ d-
NELSON CHEMISTRY 12 SECTION 4.4 POLARITY What is the name of 007’s Inuit cousin? Polar Bond.

NELSON CHEMISTRY 12 SECTION 4.4 POLARITY What is the name of 007’s Inuit cousin? Polar Bond.
Sections 3.3 & 3.4 Covalent Bonding and Lewis Structures

Sections 3.3 & 3.4 Covalent Bonding and Lewis Structures
Polarity of Bonds Molecular Polarity. Equal Pull on Electrons If there is no difference in the electronegativity of the atoms forming a covalent bond,

Polarity of Bonds Molecular Polarity. Equal Pull on Electrons If there is no difference in the electronegativity of the atoms forming a covalent bond,
Molecular Compounds Unit 7. Covalent Bonds Sharing pairs of electrons Sharing pairs of electrons Covalent bonds are the intra-molecular attraction resulting.

Molecular Compounds Unit 7. Covalent Bonds Sharing pairs of electrons Sharing pairs of electrons Covalent bonds are the intra-molecular attraction resulting.
Molecular Polarity AP Chemistry.

Molecular Polarity AP Chemistry.
Polar vs. Non Polar Molecules. Covalent/Molecular Compounds All molecular compounds are either polar or nonpolar.

Polar vs. Non Polar Molecules. Covalent/Molecular Compounds All molecular compounds are either polar or nonpolar.
3.3 Polar bonds and Polar Molecules. Polar Bonds Polar covalent bonds have 0 < ∆En < 1.7 ∆En = 0Pure covalent 0 < ∆En < 0.4Slightly polar 0.5 < ∆En

3.3 Polar bonds and Polar Molecules. Polar Bonds Polar covalent bonds have 0 < ∆En < 1.7 ∆En = 0Pure covalent 0 < ∆En < 0.4Slightly polar 0.5 < ∆En
 Electronegativity Electronegativity  Polarity of Bonds Polarity of Bonds  Dipole Moment Dipole Moment  Dipole Moment of Polar Covalent Bond Dipole.

 Electronegativity Electronegativity  Polarity of Bonds Polarity of Bonds  Dipole Moment Dipole Moment  Dipole Moment of Polar Covalent Bond Dipole.
Molecular Polarity Boiling point = 100 ˚C Boiling point = -161 ˚C

Molecular Polarity Boiling point = 100 ˚C Boiling point = -161 ˚C
Predicting Molecular Polarity  When there are no polar bonds in a molecule, there is no permanent charge difference between one part of the molecule and.

Predicting Molecular Polarity  When there are no polar bonds in a molecule, there is no permanent charge difference between one part of the molecule and.
1 Electronegativity? The ability of an atom in a molecule to attract shared electrons to itself. The ability of an atom in a molecule to attract shared.

1 Electronegativity? The ability of an atom in a molecule to attract shared electrons to itself. The ability of an atom in a molecule to attract shared.
Polar Bears and Penguins Making Sense page 135. Unit 2 Investigation IV The ability of an atom to attract electrons shared between two atoms is called.

Polar Bears and Penguins Making Sense page 135. Unit 2 Investigation IV The ability of an atom to attract electrons shared between two atoms is called.
Section 12.1 Characteristics of Chemical Bonds 1.To learn about ionic and covalent bonds and explain how they are formed 2.To learn about the polar covalent.

Section 12.1 Characteristics of Chemical Bonds 1.To learn about ionic and covalent bonds and explain how they are formed 2.To learn about the polar covalent.
Covalent Bonding Chapter 6 Section 1. Covalent Bonds Ionic bond – transfer of e- Ionic bond – transfer of e- Covalent bond – a bond formed when atoms.

Covalent Bonding Chapter 6 Section 1. Covalent Bonds Ionic bond – transfer of e- Ionic bond – transfer of e- Covalent bond – a bond formed when atoms.
Polar Bonds and Molecules Chapter 8.4. Learning Objectives Be able to use electronegativity to identify polar vs. non-polar covalent bond Draw correct.

Polar Bonds and Molecules Chapter 8.4. Learning Objectives Be able to use electronegativity to identify polar vs. non-polar covalent bond Draw correct.
Bond Polarity. Electronegativity Trend Page 161 in textbook.

Bond Polarity. Electronegativity Trend Page 161 in textbook.
Section 12.1 Characteristics of Chemical Bonds 1.To understand the nature of bonds and their relationship to electronegativity 2.To understand bond polarity.

Section 12.1 Characteristics of Chemical Bonds 1.To understand the nature of bonds and their relationship to electronegativity 2.To understand bond polarity.
ml.

ml.

Similar presentations

Ads by Google