Indicate the type of intermolecular forces expected with each of the following compounds.
H2
Li2CO3
LiOH
C3H7OH
choices include: Hydrogen Bonding,Ion-Molecule and
vanDerWaals.
help me! please!!!! im so stuck!
http://www.ausetute.com.au/intermof.html
The above site is a basic way to get started. First, inter means between molecules, not between atoms. Therefore, the forces your question is asking is NOT the H-H bond in H2 but the attraction of one H atom to another H atom of an adjacent H2 molecule. For diatomic molecules, this is always van der Waals forces. van der Waals forces are the weakest of the three. The strongest of the three is hydrogen bonding and that occurs when there is an H in one molecule being attracted to an O, N, or F in another molecule. Therefore, for hydrogen bonding, look for compounds, with -OH, -NH2, or -F. (Hydrogen bonding is just a special case of dipole-dipole attractions but it is given a special name because it involves those three highly electronegative atoms of F, O, or N with H.) C3H7OH is an example. I'm not exactly sure what "ion-molecule" means but I assume it is ion-dipole. Li2CO3 is an example. ion-dipole or dipole-dipole forces are intermediate between van der Waals and hydrogen bonding.
thank you!!!!!!
I can certainly help you with that! Let's go through each compound one by one:
1. H2 (hydrogen molecule): The intermolecular forces in H2 would be van der Waals forces. Since H2 is a nonpolar covalent molecule, the only intermolecular forces it can exhibit are London dispersion forces, which are a type of van der Waals forces.
2. Li2CO3 (lithium carbonate): In Li2CO3, the intermolecular forces can be a combination of ion-molecule and van der Waals forces. Li2CO3 is an ionic compound, so it has strong ionic bonding within the molecule. However, when dissolved in a solution, the individual ions (Li+ and CO3 2-) can interact with water molecules through ion-dipole interactions, which is a type of ion-molecule force. Additionally, there can also be some weak London dispersion forces between the carbonate ions and other nearby molecules.
3. LiOH (lithium hydroxide): Similar to Li2CO3, LiOH also exhibits both ion-molecule and van der Waals forces. The strong ionic bonding within the LiOH molecule gives rise to ion-dipole interactions when dissolved in a solution. Additionally, there can also be weak London dispersion forces between the hydroxide ions and other nearby molecules.
4. C3H7OH (isopropyl alcohol): In C3H7OH, the main intermolecular forces are hydrogen bonding and van der Waals forces. C3H7OH is a polar molecule due to the presence of the hydroxyl (OH) group. This allows for hydrogen bonding between the Oxygen atom in one molecule and the hydrogen atom in another molecule. In addition to hydrogen bonding, there can also be some weak London dispersion forces present.
To summarize:
- H2: van der Waals forces (London dispersion forces).
- Li2CO3: a combination of ion-molecule forces (ion-dipole) and van der Waals forces (London dispersion forces).
- LiOH: a combination of ion-molecule forces (ion-dipole) and van der Waals forces (London dispersion forces).
- C3H7OH: hydrogen bonding and van der Waals forces (London dispersion forces).
I hope this helps you understand the types of intermolecular forces present in each of the compounds! Let me know if you have any more questions.
No problem, I'm here to help! To determine the type of intermolecular forces present in each compound, we need to consider the different types of bonds and the polarity of the molecules.
Let's go through the compounds one by one:
1. H2 - This compound consists of two hydrogen atoms bonded together. Since both atoms in H2 have similar electronegativity, the bond is nonpolar. Therefore, the intermolecular forces present in H2 are van der Waals forces.
2. Li2CO3 - This compound, known as lithium carbonate, is a salt. It contains ions: Li+ and CO32-. The intermolecular forces between ions and polar molecules are called ion-dipole forces. So, the expected intermolecular forces in Li2CO3 are ion-molecule forces.
3. LiOH - Similar to Li2CO3, LiOH also contains ions (Li+ and OH-) due to the presence of a metal (Li) and a polyatomic ion (OH-). Hence, the intermolecular forces present in LiOH are ion-molecule forces.
4. C3H7OH - This compound is known as propanol or isopropyl alcohol. It consists of a long carbon chain (C3H7) with an -OH group attached to it. The oxygen atom in the -OH group is more electronegative than carbon, making the molecule polar. As a result, the intermolecular forces present in C3H7OH are hydrogen bonding in addition to the usual van der Waals forces.
To summarize:
- H2: van der Waals forces
- Li2CO3: ion-molecule forces
- LiOH: ion-molecule forces
- C3H7OH: hydrogen bonding and van der Waals forces
Remember that these are the expected intermolecular forces based on the molecular structure and polarity of the compounds.