Answer:
Here's what I get.
Explanation:
The MO diagrams of KrBr, XeCl, and XeBr are shown below.
They are similar, except for the numbering of the valence shell orbitals.
Also, I have drawn the s and p orbitals at the same energy levels for both atoms in the compounds. That is obviously not the case.
However, the MO diagrams are approximately correct.
The ground state electron configuration of KrF is
KrF⁺ will have one less electron than KrF.
You remove the antibonding electron from the highest energy orbital, so the bond order increases.
The KrF bond will be stronger.
mass percent concentration = 15.7 %
molar concentration of glucose solution 1.03 M
Explanation:
To calculate the mass percent concentration of the solution we use the following formula:
concentration = (solute mass / solution mass) × 100
solute mass = 60.5 g
solution mass = solute mass + water mass
solution mass = 60.5 + 325 = 385.5 g (I used the assumption that the solution have a density of 1 g/mL)
concentration = (60.5 / 385.5) × 100 = 15.7 %
Now to calculate the molar concentration (molarity) of the solution we use the following formula:
molar concentration = number of moles / volume (L)
number of moles = mass / molecular weight
number of moles of glucose = 60.5 / 180 = 0.336 moles
molar concentration of glucose solution = 0.336 / 0.325 = 1.03 M
Learn more about:
molarity
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Drawbacks of Dalton's Atomic Theory. The indivisibility of an atom was proved wrong: an atom can be further subdivided into protons, neutrons and electrons. However an atom is the smallest particle that takes part in chemical reactions. According to Dalton, the atoms of same element are similar in all respects.
The most abundant carbon isotope is carbon-12.
The relative atomic mass of carbon is 12.011, which is extremely close to 12.0. This means that the masses C-13, and C-14 are practically negligible when contributing to the relative atomic mass of carbon.
the C-12 isotope makes up 98.9% of carbon atoms, C-13 makes up 1.1% of carbon atoms, and C-14 makes up just a trace of carbon atoms as they are found in nature.
