Question I. Answer as required:

(a) Draw the orbital diagram for each of Ca⁺ and Cl^2-. Explain why both ions are not stable?

b) Write the basic physical processes that could be used in chemical laboratories.

(c) Define the following:

1. Pauli exclusion principle.                          2. Isotopes.

(d) What is/are the difference/s between:

1- 3d and 3p sub-orbitals.                      2- Mass number and atomic mass.

3- Core and valence electrons.
 
 

Question II: Answer with FALSE or TRUE, If the statement is False, correct it.

1. The electronic configuration 1s¹, describe the excited state of H atom, and allow it to emit energy.

2. Each of the following species has as many electrons as it has neutrons.

        a) H⁺          b) Ca²⁺          c) C          d) F              e) Cl^-

3. The outer most shell electrons in Ga are the same as those of Al.

4. The short hand electronic configuration of In is:[Kr] 5s² 4P¹

5. Orbital 3p has the quantum numbers n=3, l=0 & m_l=0.

6. Pauli exclusion principle stated that "no two electrons in the same atom can have the same set of three quantum numbers" .

7. 1s²2s²2p⁶3s²3p⁷is the electronic configuration of Ca⁺.

8. Each of the following has an incompletely filled d suborbital:

            a) Ag          b) Ba          c) Cu          d) Se              e) Ni

9. Each of the following is an stable isotope of ₁₇Cl³⁵.

        a) ₁₇X³⁴          b) ¹⁷X³³          c) ₁₇X³⁷              d) ₁₇X³⁶

10. The rule of n+l explains the paramagnetism of the elements.

Question III A) For Mn, P, Br, Mg and In answer questions (1 -4)

1) Write the short hand (noble gas inner core) electronic configuration for each of these elements

2) Identify the group of elements (Block) corresponding to each of these elements.

3) For each of these elements, state the number of unpaired electrons.

4) How many valence electrons are in P, in Mg, in Br and in In ?

B) Give example/s that may explain each of the following statements:

1) Atoms may lose or gain one or more electron in order to have the same electronic structure of the

nearest noble gas.

2) ¹¹₆C is not a stable isotope of Carbon.

Question VI. Consider the given information when answering the following questions.

An ion having a 2+ charge and a mass of 65.400 amu, has 2 electrons with n (principal Q.#) =1, 8 elec trons with n=2, and 18 with n=3. In forming ions, the 4s electrons are lost before the 3d electrons. Has only two isotopes of 35 and 36 neutrons.

a) What is the atomic number ?

b) What are the total number of s electrons ?

c) What are the total number of p electrons ?

d) What is the abundance (percentage) of each isotope?

e) Explain (using orbital diagrams) why neither the neutral atom nor the 2+ ion form are                  paramagnetic.

f) Write all possible quantum numbers for electrons in the outer most shell of the neutral atom.

Question VI- Answer as required:

A) For each of the following electron configurations, determine the element to which it corre-sponds and determine number of valence electrons and determine whether it is a ground or excited state

a) [He] 2s¹2p⁴ ........ ......... ........

b) [Ar] 4s²3d¹⁰4p⁵ ..... ......... ........

c) [Ne] 3s²3p⁵4s¹ ..... ......... ........

d) [Kr] 5s³4d¹⁰4p⁷ ..... ......... ........