Is bromine (Br) a metal, a nonmetal, or a metalloid? Does bromine have a higher or lower electron affinity than selenium

element X has an electron affinity of 295.3 kJ/mol and the following ionization energies (in kJ/mol): IE1 = 1.008e3, IE2 = 1.846e3, IE3 = 3.20e3. In what column of the periodic table is this element probably found?

In a plot of IE1 for the Period 3 elements , why do the values for elements in Groups 3A(13) and 6A(16) drop slightly below the generally increasing trend?

Consider the figure in Chapter 7 of your textbook which shows the periodic trends in electron affinity.  When you look across a period (row),  why are the electron affinities of the Group 4A elements more negative than the electron affinities of the Group 5A elements? Group of answer choices The ratio of bonding radius to first ionization energy is smaller in 4A Atomic radii of the Group 4A elements are bigger than their corresponding group 5A elements Group 4A elements are more electronegative than the elements of Group 5A Group 5A half-filled p-subshells discourage the addition of an electron None of these choices explain the question

Rank the following isoelectronic species in order of decreasing size: Argon atom (Ar), Calcium ion (Ca+2), chloride ion (Cl-1), Potassium ion (K+1), Sulfide ion (S-2).

Give the name and symbols for three ions that are isoelectronic with an unknown element whose electron configuration is [ Kr] 5s², 4d10, 5p6.

Explain why sulfur has a larger first ionization energy than silicon.

Write the complete ground-state electron configuration of magnesium.

Using the concept of effective nuclear charge, explain how the ionization energy varies on the 3rd line of the periodic table (from Na to Cl).