Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.

Explain whether the cation formed from an atom is larger or smaller and why. Then, explain whether the anion formed from an atom is larger or smaller and why. We would predict that the alkaline earth metals would have a higher electron affinity than the alkali metals, but they do not. Why Why does beryllium have a higher ionization energy than we would predict and a lower electron affinity than we would predict?

Which of the following atoms and ions is (are) isoelectronic with S²+? A B C D Ar As 3+ Si4+ C13+

Which element has the smallest electron affinity Rb, Tc , Sb

Write the electron configuration for Si7+ ion.

it is clear that the first ionization energy of He is very large.  Would you expect the first ionization energy of H– (hydride ion) to be larger, smaller, or about the same as the first ionization energy of He, and why?

Summarize the acid-base behavior of the main-group metal and nonmetal oxides in water. How does oxide acidity in water change down a group and across a period?

Arrange these elements according to first ionization energy.   Highest ionization energy to lowest ionization energy     Br, Ca, As, Kr, K, Se, Ge, Ga

Draw the electron configuration for a neutral atom of vanadium.

Chemistry Write orbital diagrams for each ion. Determine if the ion is diamagnetic or paramagnetic. Cd2+ Au+ Mo6+ Zr4+