Europium can have a 2+ or a 3+ charge. which one of the following below is not possible
1. EuSO4
2.Eu2(SO4)3
3.EuPO4
4.Eu(NO3)3
5.EuHCO3
Which of the compounds below would not have hydrogen bonding as an intermolecular attractive force
1. H-O-CH3
2CH3-CH2-Ch2-O-CH3
3.NH3
4.H2O
5.CH3-NH2
I answered both of these for you. The first one last night and the second one about 10 minutes ago.
they all have a H or a OH on the end are am im missing something
You are missing something although I didn't give very good directions. #2 is an ether and has the O in the middle. Most ethers are not low on the totem pole as polar compounds.
What about the first question?
To determine which one of the following compounds is not possible for europium with a 2+ or 3+ charge, we need to consider the charges of the ions and the rule regarding the charges of compounds.
In compound formulas, the sum of the charges of the ions must be zero.
1. EuSO4: Since sulfate ion (SO4^2-) has a charge of 2-, europium (Eu) cannot have a 2+ charge in this compound. This is because the sum of the charges would be (2+) + (2-) = 0. Therefore, EuSO4 is not possible.
2. Eu2(SO4)3: In this compound, we have two europium ions (Eu) and three sulfate ions (SO4^2-). The total charge of sulfate ions is (2-) * 3 = 6-. Therefore, each europium ion must contribute a charge of 3+, which is possible for europium. So, Eu2(SO4)3 is possible.
3. EuPO4: Since phosphate ion (PO4^3-) has a charge of 3-, europium (Eu) cannot have a 2+ charge in this compound. This is because the sum of the charges would be (3+) + (3-) = 0. Therefore, EuPO4 is not possible.
4. Eu(NO3)3: Nitrate ion (NO3^-) has a charge of 1-, therefore, europium (Eu) must have a 3+ charge in order to balance the charges. This means Eu(NO3)3 is possible.
5. EuHCO3: Hydrogen carbonate ion (HCO3^-) has a charge of 1-, therefore, europium (Eu) must have a 2+ charge in order to balance the charges. This means EuHCO3 is possible.
Therefore, the compound that is not possible for europium is EuSO4 (option 1).
Moving on to the second question regarding hydrogen bonding as an intermolecular attractive force:
Hydrogen bonding occurs between a hydrogen atom bonded to a highly electronegative element (such as oxygen, nitrogen, or fluorine) and another electronegative atom. It is a strong intermolecular force.
1. H-O-CH3: This compound has a hydrogen atom bonded to an oxygen atom, so it can form hydrogen bonding. Hydrogen bonding is possible in H-O-CH3.
2. CH3-CH2-CH2-O-CH3: This compound does not have a hydrogen atom directly bonded to an oxygen, nitrogen, or fluorine atom. Therefore, hydrogen bonding is not possible in CH3-CH2-CH2-O-CH3.
3. NH3: Ammonia has a hydrogen atom bonded to a nitrogen atom, so it can form hydrogen bonding. Hydrogen bonding is possible in NH3.
4. H2O: Water has a hydrogen atom bonded to an oxygen atom, so it can form hydrogen bonding. Hydrogen bonding is possible in H2O.
5. CH3-NH2: This compound has a hydrogen atom bonded to nitrogen, so it can form hydrogen bonding. Hydrogen bonding is possible in CH3-NH2.
Therefore, the compound that would not have hydrogen bonding as an intermolecular attractive force is CH3-CH2-CH2-O-CH3 (option 2).