consider the following substances Fe(s); O2(g); H2o(l). which of the following is the corrrect order to show decreasing attractions between irons atoms, oxygen molecules, and water molecules?
I posted an answer, removed it, and I'm re posting. I had it straight in my mind but I didn't type it in that way.
If we go with boiling points, we will have
Fe, H2O, O2.
To determine the correct order of decreasing attractions between iron atoms (Fe), oxygen molecules (O2), and water molecules (H2O), we need to compare their intermolecular forces.
1. Iron atoms (Fe) - Metallic Bonding: Iron atoms are metal atoms, which form metallic bonds. Metallic bonds are formed by the sharing of electrons between all the atoms in a metal. This results in a "sea of electrons" that allows for strong attractions between metal atoms. However, Fe(s) is not an intermolecular substance, so it does not exhibit intermolecular attractions.
2. Oxygen molecules (O2) - London Dispersion Forces: Oxygen molecules are nonpolar and interact through London dispersion forces, which are the weakest type of intermolecular force. London dispersion forces arise from temporary fluctuations in electron distribution, resulting in temporary dipoles that create attractions between molecules.
3. Water molecules (H2O) - Hydrogen Bonding: Water molecules are polar due to the difference in electronegativity between oxygen and hydrogen atoms. This polarity gives rise to hydrogen bonding, which is a strong intermolecular force. Hydrogen bonding occurs when a hydrogen atom bonded to an electronegative atom (such as oxygen) interacts with another electronegative atom.
Based on the strength of intermolecular forces:
Water molecules (H2O) > Oxygen molecules (O2)
Since Fe(s) does not exhibit intermolecular attractions, it can be excluded from the order. Therefore, the correct order of decreasing attractions is:
Water molecules (H2O) > Oxygen molecules (O2)