Compare and contrast the bonding found in the H2( g) and HF(g) molecules with that found in NaF(

Compare and contrast the bonding found in the H2( g) and...

Key Concepts

Covalent Bonding

Covalent bonding involves the sharing of electrons between atoms to achieve a more stable electron configuration. This type of bonding is common in molecules where the atoms have similar electronegativities, allowing them to share electrons fairly equally. The electron sharing forms molecular orbitals that hold the atoms together and is key to the structure and properties of many compounds.

Polar Covalent Bonding

Polar covalent bonding is a type of covalent bonding where the electrons are shared unequally between the atoms due to a difference in electronegativity. One atom attracts the bonding electrons more strongly than the other, creating a dipole moment within the molecule. This polarity affects the physical properties and reactivity of the molecule by introducing regions of partial positive and partial negative charge.

Ionic Bonding

Ionic bonding occurs when one atom transfers one or more electrons to another atom, leading to the formation of positively and negatively charged ions. These oppositely charged ions are held together by strong electrostatic forces, forming an ionic compound. Ionic bonds are typically found in compounds formed between elements with a large difference in electronegativity.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons when forming bonds. Differences in electronegativity between bonding atoms determine whether a bond will be nonpolar covalent, polar covalent, or ionic. Understanding these differences is essential for predicting the types of bonds that form and the resulting distribution of charges within a molecule or compound.

Crystal Lattice and Lattice Energy

In ionic solids, the individual ions are arranged in a repeating, three-dimensional pattern known as a crystal lattice. The stability of these compounds is largely due to the lattice energy, which is the energy released when the ions come together to form the lattice. This lattice energy is a measure of the strength of the ionic bonds and contributes to the overall stability and high melting points typically observed in ionic compounds.

Transcript

00:01 So we're going to analyze some different forms of chemical bonding here.

00:06 Now first we're going to look at diatomic hydrogen gas, and hydrogen is two.

00:11 We're going to have h2, which is two non -metals.

00:15 So we know that this is covalently bonded, where each hydrogen has one electron, one valence electron, which they're going to want to share.

00:24 And together, they share this one electron, and then you have our h2 gas here.

00:30 Now the h2 gas, since the two hydrogens have the exact same electric negativity, this is a non -polar molecule.

00:40 So h2 is non -polar covalently bound.

00:47 So we have non -polar covalent bond here between h2.

00:51 Now if we look at our hydrofluoric acid here is a gas, we're going to see again, we're going to have a hydrogen atom, and we're going to have a fluoride atom or fluorine.

01:03 Now, fluorine is a halide.

01:06 It is a non -metal, and it has seven valence electrons.

01:10 And we know that hydrogen has one.

01:13 So again, we have two non -metals, fluorine and hydrogen.

01:17 So they're going to covalently bond by sharing electrons here.

01:21 So the hydrogen shares one, and the fluorine shares one.

01:26 So now their system with eight valence electrons, they have the octet they desire.

01:30 So this is an example of covalent bonding.

01:34 Now if we look at the electronegativity, fluorine is extremely electronegative compared to the much lesser hydrogen.

01:42 So there's going to be a pole...