2. Valence electrons in an atom of phosphorus are closer to the nucleus than the valence electrons of aluminum because: (A) P has a greater effective nuclear charge and a greater shielding than Al. (B) P has a greater effective nuclear charge with the same shielding as Al. (C) P has the same effective nuclear charge with greater shielding than Al. (D) P has the same effective nuclear charge and the same shielding as AI.

Find Zeff using Slater's Rules:

7.125. How do ionization energies change with increasing atomic number (a) down a group of elements in the periodic table and (b) from left to right across a period of elements?

6) (a) The solubility of carbon tetrachloride (CCI4) in water at 25°C is 1.2 g/L. The solubility of chloroform (CHCI3) at the same temperature is 10.1g/L. Why is chloroform almost 10 times more soluble in water than is carbon tetrachloride? (b) Explain the difference between the Bohr model for the hydrogen atom and the quantum-mechanical model. Is the Bohr model consistent with Heisenberg's uncertainty principle? (Ctrl)

What does the magnetic quantum number, ml, describe?        (a)  the orientation in space of the orbital        (b) the average distance of the electron from the nucleus        (c)  the shape of the orbital        (d) the direction of spin of the electron

(a) Write the equation representing the 3rd ionization energy for Cr.(b) The electron affinity of K is 48 kJ/mol. Write the equation for which this is the energy change.

Knowing that atomic radius and ionization energy are two important properties of an atom that are periodic in nature. First, (i) define the term ionization energy. Then, (ii) state the directions along the periodic table (up, down, left, right) that a) atomic radius and b) ionization energy increase and (iii) explain the factors that lead to each of these trends.

Use an orbital diagram to describe the electron configuration of the valence shell of each of the following atoms. (Let n stand for the highest occupied principal quantum level, and m for the principal quantum level right below it. Complete each energy level from left to right. Enter for an unoccupied orbital, 1 for a singly occupied orbital, and 14 for a doubly occupied orbital.) (a) I (b) Cl (c) Rb (d) Ni (e) Ag