Give the first three ionization equation for Br and determine the process with the least energy

Rank the following from lowest to greatest first ionization energy

Ca, Ge, Br, Ga, Se

Consider the following electron configurations for three atoms: 

(a) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

(b) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²

(c) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³

Identify the atom that will have the largest 2nd ionization energy and the atom that will have the smallest 7th ionization energy.

Consider the following successive ionization energies for an element in the third period of the periodic table. Determine the name of the element.

E_a1 = 577.5 kJ/mol
E_a2 = 1,816.7 kJ/mol
E_a3 = 2,744.8 kJ/mol
E_a4 = 11,577 kJ/mol
E_a5 = 14,842 kJ/mol
E_a6 = 18,379 kJ/mol
E_a7 = 23,326 kJ/mol

Predict the element with the highest second ionization energy among the following: Rb, Al, K, Mg.

Choose the process that will release the greatest amount of energy

Arrange the following elements in decreasing order of the energies released from the addition of an electron in their outermost shell: Si, Mg, Na, Al

One way to give a relative value of electronegativity is based on the ionization energy and the electron affinity of the element. The EN value can be calculated using the equation:  EN = k(I - EA). Identify the statements that correctly describe why electronegativity is based on ionization energy and electron affinity.

(i) Ionization energy measures how difficult it is to remove electrons, which can be a reflection of how strong an electron in the atom is attracted to its nucleus.
(ii) Electron affinity measures how difficult it is to add electrons, which can be a reflection of how strong an electron in another atom is attracted to its nucleus.
(iii) Ionization energy and Electron affinity both measure how negative the energies are in the addition and removal of electrons.
(iv) Electron affinity and electronegativity are the same.

Arrange the following elements from most electronegative to least electronegative:

K   C   F   Si   O

Identify the statement that would be a good adjustment to Slater's rules to account for the difference in electronic penetration of the nucleus for 3s, 3p, and 3d orbitals. Use the radial probability distribution curve below as a reference.

Arrange the following elements from the highest to lowest values of their effective nuclear charge (Z_eff):

Po, Rn, Cs, Bi, Pb

Detailed calculations show that the value of Z_eff for the outermost electrons in Si and Cl atoms is 4.29+ and 6.12+, respectively. (a) What value do you estimate for Z_eff experienced by the outermost electron in both Si and Cl by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant?

Calculate the change in energy for the given reactions based on the ionization energy and electron affinity of the involved elements.

(A) Li (s) + Cl (g) → Li^- (g) + Cl⁺ (g)

(B) Li (s) + Cl (g) → Li⁺ (g) + Cl^- (g)

a. Arrange the following elements in descending order of their first ionization energies.

F
K
S
Ca
Si

b. Arrange the following in ascending order of their ionic radii.

O₂^-
N₃^-
Mg²⁺ 
F^-
K⁺

c. Arrange the following elements in descending order of their atomic radii.

Ca
K
F
Si
Ge
S