Rank the following 4 compounds in order of lowest to highest freezing point.

Enter the formulas in the spaces provided.
For example, enter CH4 as CH4.

H2O MgO CH4 H2S

CH4

H2S
H2O
MgO

Oh, I love freezing point jokes! Here's the order, from lowest to highest freezing point:

CH4 (methane) - It's so cool that it freezes at a nice low temperature!
H2O (water) - Ah, water, the classic, freezing at 0 degrees Celsius. No surprises there.
H2S (hydrogen sulfide) - Just a tad colder than water, freezing at a slightly lower temperature.
MgO (magnesium oxide) - The "O" in the formula stands for "Oh no!" because it has the highest freezing point. Sorry, MgO!

Remember, these rankings are just in terms of freezing point, not actual fun factor. Stay frosty!

To rank the compounds based on freezing point from lowest to highest, we need to consider the strength of intermolecular forces in each compound. Generally, compounds with stronger intermolecular forces will have higher freezing points.

Let's analyze each compound:

1. CH4 (methane): The molecule is nonpolar, and it participates in London dispersion forces (also known as van der Waals forces). Compared to the other compounds, CH4 has the weakest intermolecular forces.

2. H2S (hydrogen sulfide): H2S is also a nonpolar molecule but has a slightly higher boiling point than CH4 due to the presence of sulfur. It engages in London dispersion forces, which are slightly stronger in H2S than in CH4.

3. H2O (water): Water is a polar molecule and exhibits hydrogen bonding, which is a very strong type of intermolecular force. Hydrogen bonding causes water to have a higher freezing point compared to nonpolar compounds.

4. MgO (magnesium oxide): MgO is an ionic compound formed by a metal (Mg) and a nonmetal (O). Ionic compounds have strong electrostatic forces between oppositely charged ions, leading to higher freezing points. Therefore, MgO is expected to have the highest freezing point among the four compounds.

Ranking the compounds in order of lowest to highest freezing point, we have:

CH4 < H2S < H2O < MgO

To rank the compounds in order of lowest to highest freezing point, we need to consider their molecular structures and intermolecular forces. The strength of intermolecular forces determines the freezing point, with stronger forces leading to higher freezing points. Here's how we can determine the ranking:

1. CH4 (methane): CH4 is a non-polar molecule with only weak London dispersion forces between molecules. These forces are relatively weak, so CH4 has the lowest freezing point among the given compounds.

2. H2S (hydrogen sulfide): H2S is a polar molecule due to the difference in electronegativity between hydrogen and sulfur. This polarity allows for dipole-dipole interactions, which are stronger than London dispersion forces. Therefore, H2S has a higher freezing point than CH4.

3. H2O (water): H2O is a highly polar molecule, and it exhibits strong hydrogen bonding between its molecules. Hydrogen bonding is the strongest intermolecular force among the molecules listed here. As a result, water has a higher freezing point than both CH4 and H2S.

4. MgO (magnesium oxide): MgO is an ionic compound composed of Mg2+ and O2- ions. Ionic compounds have very strong electrostatic forces between oppositely charged ions, known as ionic bonds. These forces are much stronger than the intermolecular forces present in the other compounds. Therefore, MgO has the highest freezing point among the given compounds.

So, the ranking in order of lowest to highest freezing point is: CH4, H2S, H2O, MgO.