1. LO 6 Chemical bonding

2. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. The bonding pairs of electrons in covalent bonds are pulled between the nuclei of the atoms sharing the electrons Bond Polarity Covalent bonds differ in terms of how the bonded atoms share the electrons.

3. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. When the atoms in the bond pull equally (as occurs when identical atoms are bonded), the bonding electrons are shared equally, and each bond formed is a nonpolar covalent bond. 6.2

4. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. The more electronegative atom attracts more strongly and gains a slightly negative charge. The less electronegative atom has a slightly positive charge. 6.1 A polar covalent bond, known also as a polar bond, is a covalent bond between atoms in which the electrons are shared unequally.

5. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. The higher the electronegativity value, the greater the ability of an atom to attract electrons to itself. When polar molecules are placed between oppositely charged plates, they tend to become oriented with respect to the positive and negative plates. 6.1

6. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Describing Polar Covalent Bonds The polar nature of the bond may also be represented by an arrow pointing to the more electronegative atom. H—Cl Polar molecules have unequal distribution of electrons while non-polar molecules have equal distribution of electrons https://www.youtube.com/watch?v=72CQe-_PJU4

7. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 6.3+ 6.4- Bond Polarity Electronegativity Differences and Bond Types Electronegativity difference range Most probable type of bondExample 0.0–0.4Nonpolar covalentH—H (0.0) 0.4–1.0Moderately polar covalent δ+ δ– H—Cl (0.9) 1.0–1.7Very polar covalent δ+ δ– H—F (1.9) > 1.7IonicNa + Cl – (2.1) Describing Polar Covalent Bonds The electronegativity difference between two atoms tells you what kind of bond is likely to form.

8. 6.3+ 6.4 (contd.)- Bond Polarity Describing Polar Covalent Bonds There is no sharp boundary between ionic and covalent bonds. As the electronegativity difference between two atoms increases, the polarity of the bond increases. If the difference is more than 1.7, the electrons will likely be pulled away completely by one of the atoms. –In that case, an ionic bond will form.

9. Questions. Q1. Use electronegativity differences and the table on slide 7 to classify bonding between sulfur, S, and the following elements: hydrogen, H; cesium, Cs; chlorine, Cl. In each pair, which atom will be more negative? Q2. Which type of bond (nonpolar covalent, moderately polar covalent, very polar covalent, or ionic) will form between each of the following pairs of atoms? a. N and H b. F and F c. Ca and Cl d. Al and Cl

10. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. In a polar molecule, one end of the molecule is slightly negative, and the other end is slightly positive. Dipole moment is a measure of the polarity of the molecule. The larger the difference in electronegativity, the larger the dipole moment. 6.5- Bond Polarity Describing Polar Covalent Molecules Molecules that are polar are also said to be dipoles. Di- means 2 and pole means it has + and – electrostatic poles.

11. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. – The hydrogen chloride molecule is a dipole. For a molecule to be polar, it must have dipoles and the net dipole moment must not be equal to zero. 6.5- Bond Polarity Describing Polar Covalent Molecules In the hydrogen chloride molecule, for example, the partial charges on the hydrogen and chlorine atoms are electrically charged regions, or poles.

12. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. A carbon dioxide molecule has two polar bonds and is linear. O C O Carbon dioxide molecule has no dipole moment and therefore is is nonpolar. Bond Polarity Describing Polar Covalent Molecules The effect of polar bonds on the polarity of an entire molecule depends on the shape of the molecule and the orientation of the polar bonds.

13. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. The water molecule also has two polar bonds. Bond Polarity Describing Polar Covalent Molecules However, the water molecule is bent rather than linear. Therefore, the bond polarities do not cancel and a water molecule is polar.

14. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Carbon monoxide (CO) is an example of a type of covalent bonding different from that seen in water, ammonia, methane, and carbon dioxide. It is possible for both carbon (which needs to gain four electrons) and oxygen (which needs to gain two electrons) to achieve noble-gas electron configurations by a type of bonding called coordinate covalent bonding. 6.6- Coordinate Covalent Bonds

15. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Coordinate Covalent Bonds Look at the double covalent bond between carbon and oxygen. With the double bond in place, the oxygen had a stable electron configuration, but the carbon does not.

16. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. As shown below, the dilemma is solved if the oxygen also donates one of its unshared pairs of electrons for bonding. A covalent bond in which one atom contributes both bonding electrons is a coordinate (dative) covalent bond. Coordinate Covalent Bonds

17. 6.6- Contd. Examples- H 3 O +, NH 4 +, BF 4 -, NH 3 BF 3 The ammonium ion forms when a positively charged hydrogen ion (H + ) attaches to the unshared electron pair of an ammonia molecule (NH 3 ).