Indicate the bond polarity (show the partial positive and...

Key Concepts

Dipole Moment

The dipole moment is a quantitative measure of the separation of charge in a bond or molecule, arising from bond polarity. It is represented as a vector pointing from the positive to the negative charge and its magnitude indicates the degree of polarity. The dipole moment plays a significant role in dictating the physical properties of substances, such as solubility and boiling point, as well as their interactions with electric fields and other dipoles.

Partial Charges

Partial charges are the small positive and negative charges that develop on atoms as a result of unequal sharing of electrons in a polar bond. When one atom attracts electrons more strongly than another, it gains a partial negative charge while the other atom becomes partially positive. These localized charges are crucial in determining intermolecular interactions and the overall polarity of a molecule.

Bond Polarity

Bond polarity refers to the unequal distribution of electron density between two atoms in a bond, resulting in the formation of partial positive (?+) and partial negative (??) charges. This occurs when atoms with different electronegativities are involved in bonding, and it has important implications for the behavior, reactivity, and physical properties of molecules.

Electronegativity

Electronegativity is a fundamental property of atoms that describes their ability to attract electrons within a chemical bond. The greater the difference in electronegativity between two bonded atoms, the more uneven the electron distribution, leading to bond polarity. This concept is essential for understanding how electrons are shared in covalent bonds and why certain bonds exhibit significant partial charges.

Transcript

00:01 So in this video, we're going to talk about question 38 from chapter 8, which says, indicate the bond polarity, show the partial positive and partial negative ends, in the following bonds.

00:12 So in a, we have a carbon -oxygen bond.

00:15 So let's take a look at the periodic table to decipher what our electronegativities are.

00:21 So remember, as we go from left to right across a periodic table, as we cross one row of the periodic table, we're gradually increasing our nuclear charge.

00:30 We're increasing the number of protons in our nucleus.

00:33 And because of that, increased nuclear charge, the more positive charge, you have a stronger pull on your electrons.

00:40 You're becoming more electronegative from left to right.

00:44 Now from top to bottom, you're gradually adding more shells of electrons.

00:50 So as you do that, any electron that atom might attract is going to be further away from the nucleus.

00:58 And remember, the further away two positive and negative charges are, the weaker that attractive force between them is.

01:06 So as we get farther from the nucleus, our electronegativity decreases.

01:11 And that's also because as you have more shells of electrons in between the nucleus and your outermost electrons, you have increased shielding effects as well.

01:21 So we're increasing electronegativity from left to right and from bottom to top.

01:28 And now we're talking about a carbon -oxygen bond.

01:30 So we know that oxygen is more electronegative than carbon, because it's further to the right on the periodic table.

01:37 So oxygen is going to take our partial negative charge.

01:40 It's going to attract electrons more effectively than carbon, which will have a partial positive charge...

Please give Ace some feedback