LiF, BeF2, PCl3, CCl4, F2
1. which is likely to conduct electricity when aqueous:
2. which is most likely to be a gas in room temp.
3. which is likely to be very soluble in water
4. which is a polar molecule?
may have more than one answer
Do you know which are ionic and which covalent? That is the secret to answering this question. LiF is ionic, it dissolves in H2O and because the ions are in solution it conducts electricity.
which one is at room temperature then ?
The one most likely to be a gas at room T is F2
LiF is likly to be soluble in water because both are polar; polar solutes dissolve in polar solvents.
LiF is polar; PCl3 is polar. F2, BeF2, CCl4 are not polar.
To identify which compounds are likely to fulfill each requirement, we can analyze their chemical properties and bond types. Here's how to determine the answers to each question:
1. Which compound is likely to conduct electricity when aqueous?
To conduct electricity in an aqueous solution, a compound must dissociate into ions. Ionic compounds are the typical conductors. In this case, LiF and BeF2 are ionic compounds, whereas PCl3, CCl4, and F2 are covalent compounds. Therefore, LiF and BeF2 are likely to conduct electricity when dissolved in water.
2. Which compound is most likely to be a gas at room temperature?
At room temperature, compounds with weaker intermolecular forces and low boiling points tend to be in a gaseous state. Among the provided compounds, F2 is most likely to be a gas at room temperature because it consists of diatomic molecules held together by relatively weak van der Waals forces.
3. Which compound is likely to be very soluble in water?
To determine solubility, one must consider the polarity of the compound. Polar compounds tend to dissolve in polar solvents, like water. LiF and PCl3 are polar compounds due to the electronegativity differences between the bonded atoms (Li-F, P-Cl). Therefore, LiF and PCl3 are likely to be very soluble in water.
4. Which compound is a polar molecule?
Polarity in molecules arises due to differences in electronegativity between the bonded atoms. If the molecule has polar covalent bonds and an asymmetrical molecular shape, it will be polar. Among the given compounds, LiF does not have an asymmetrical molecular shape and is an ionic compound, making it nonpolar. BeF2 is also nonpolar because it has a linear molecular shape. On the other hand, PCl3 has a trigonal pyramidal shape, which leads to an asymmetrical distribution of charge, making it polar. CCl4 and F2 are nonpolar due to their symmetrical structures. Therefore, PCl3 is the polar molecule among the provided compounds.
In summary:
1. Likely to conduct electricity when aqueous: LiF, BeF2
2. Most likely to be a gas at room temperature: F2
3. Likely to be very soluble in water: LiF, PCl3
4. Polar molecule(s): PCl3