I have the answers for these but can you please explain to me how to get them? Thanks.
Place the following in order of decreasing lattice energy.
KBr RbI MgS
a. KBr > RbI > MgS
b. KBr > MgS > RbI
c. RbI > KBr > MgS
d. MgS > KBr > RbI
e. MgS > RbI > KBr
I am confused about lattice energy or even how to figure it out?
Which of the following species are paramagnetic?
a. Ca
b. S2-
c. Zn2+
d. Sr2+
e. None of the above are paramagnetic.
Are paramagnetic the ones that have unpaired electrons???
According to valence bond theory, the sigma bond between C and H in C2HCl is formed from the overlap of which two orbitals?
Carbon Hydrogen
a. sp s
Here is a site that give you some insight on lattice energy.
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch7/lattice.html
Yes, paramegnetic species will be those that have unpaired electrons.
s and p.
To determine the order of decreasing lattice energy, you need to consider the charges and sizes of the ions involved. Lattice energy is a measure of the energy required to break apart one mole of a solid ionic compound into its constituent ions in the gas phase.
When comparing the lattice energies of different compounds, the following factors generally apply:
1. Ion charges: Greater charges on the ions generally result in higher lattice energies. This is because stronger electrostatic attractions are present between ions of higher charge.
2. Ion size: Smaller ions usually have higher lattice energies. Smaller ions can come closer together, leading to stronger electrostatic attractions between them.
In the given compounds, KBr, RbI, and MgS, the ions present are K+, Rb+, Br-, I-, Mg2+, and S2-. Comparing the charges, both K+ and Rb+ have the same charge, while Br- is larger than I- and Mg2+ is larger than S2+. Therefore, we can eliminate options c and d because they suggest RbI having the highest lattice energy.
Now, we need to choose between options a, b, and e. Since KBr and MgS both have ions of the same charge, we need to compare the sizes. Br- is larger than S2+, so KBr should have a higher lattice energy than MgS.
Therefore, the correct answer is option b: KBr > MgS > RbI.
Regarding the second question, yes, paramagnetic species are those that have unpaired electrons. Paramagnetism arises when there is an uneven distribution of electrons, resulting in a net magnetic moment.
Analyzing the options:
a. Ca: Calcium (Ca) loses two electrons to achieve a stable configuration, resulting in a filled electron shell. It does not have any unpaired electrons, so it is not paramagnetic.
b. S2-: Sulfur (S) gains two electrons to achieve a stable configuration, resulting in a filled electron shell with paired electrons. It does not have any unpaired electrons, so it is not paramagnetic.
c. Zn2+: Zinc (Zn) loses two electrons to achieve a stable configuration, resulting in a filled electron shell. It does not have any unpaired electrons, so it is not paramagnetic.
d. Sr2+: Strontium (Sr) loses two electrons to achieve a stable configuration, resulting in a filled electron shell. It does not have any unpaired electrons, so it is not paramagnetic.
Therefore, the correct answer is e: None of the above are paramagnetic.
For the third question, according to valence bond theory, the sigma bond between C and H in C2HCl is formed from the overlap of two orbitals: the sp orbital of carbon and the s orbital of hydrogen.
The hybridization of carbon in this molecule is sp because it forms two sigma bonds with two hydrogen atoms and one sigma bond with a chlorine atom. The s orbital of hydrogen overlaps with one of the hybridized sp orbitals on carbon to form a sigma bond.
Therefore, the correct answer is a: sp s.