So this is the case: liquid methanol, CH3OH is being prepared to be poured into a beaker of water.
(THERE CAN BE MORE THAN ONE ANSWER FOR Q1-3)
1) What intermolecular forces are broken in the methanol when these substances are mixed?
-hydrogen-bonding
-dispersion forces
-dipole-dipole interactions
-ion-ion interactions
2) What intermolecular forces are broken in the water when these substances are mixed?
-hydrogen-bonding
-dispersion forces
-dipole-dipole interactions
-ion-ion interactions
3) What intermolecular forces are formed in the solution when these substances are mixed?
-hydrogen-bonding
-dispersion forces
-dipole-dipole interactions
-ion-ion interactions
Look up each of the four types of forces in your text and answer the best you can giving reasons for your answer. We shall be happy to provide comment.
1) i think this one is hydrogen bonding because in CH3OH, the H is bonded to an O. I think my teacher said all bonds have a tiny bit of dispersion force, but the main force is the H-bond. I am also confused, isn't h-bond also considered a dipole-dipole interaction? it's polar.
but i think i would answer hydrogen-bond + dispersion force
(based on what teacher said that all bonds have some kind of dispersion force) OR is he wrong? dispersion is only for non-polar?
2) i think i would answer h-bond and dispersion again.
again, if it was INTRmolecular force then it would be dipole-dipole but it is talking about INTERmolecular so it would be h-bond. i based the dispersion that all molecules contain a tiny bit of dispersion force.
3) i don't really get this one. so is this saying CH3OH + h20 = what type of force formed?
i think h-bond since the O can be connected to the H?
GAHHHH I AM SO CONFUSED
To answer questions 1-3, we need to understand the intermolecular forces present in each substance.
1) When liquid methanol (CH3OH) is mixed with water:
- Methanol can establish hydrogen bonding due to the presence of an oxygen atom bonded to a hydrogen atom. Hydrogen bonding involves the attraction between the partially positive hydrogen atom and the partially negative oxygen atom.
- Methanol also exhibits dispersion forces, also known as London dispersion forces. These occur due to temporary fluctuations in electron distribution and result in the creation of temporary dipoles. This force is present in all molecules, regardless of polarity.
- It does not have dipole-dipole interactions, as methanol is not significantly polar.
- Methanol does not have ion-ion interactions because it is a covalent compound.
2) When water is mixed with methanol:
- Water molecules are capable of hydrogen bonding due to the presence of two hydrogen atoms bonded to an oxygen atom. This force is stronger in water than in methanol.
- Water also exhibits dispersion forces, as mentioned earlier, since all molecules exhibit this force.
- Like methanol, water lacks significant dipole-dipole interactions with methanol.
- Water does not experience ion-ion interactions.
3) When the substances are mixed, several intermolecular forces are formed in the solution:
- Hydrogen bonding occurs between methanol and water molecules. The partially positive hydrogen atoms in the methanol molecules form attractive interactions with the partially negative oxygen atoms in the water molecules.
- Dispersion forces are still present in the solution as both methanol and water molecules can establish these temporary attractions.
- Dipole-dipole interactions between methanol and water are not significant due to the relatively low polarity of methanol compared to water.
- Ion-ion interactions are not formed in this solution as neither methanol nor water dissociate into ions.
Therefore, the possible answers for questions 1-3 are:
1) Methanol experiences hydrogen bonding and dispersion forces.
2) Water experiences hydrogen bonding and dispersion forces.
3) The solution formed experiences hydrogen bonding and dispersion forces.