1

In development of the Periodic Table, explain why it was essential to be able to measure the mass of gases.

2

State Dalton’s concept of atoms.

3

Explain how Avogado’s postulate that a Mole of every pure element had the same number of atoms was used to define Gram Atomic Weight.

4

Which chemist lead the search for atomic weight values ?

5

Describe the pattern oif properties observed when elements are put in order of increasing atomic weight.

6

Explain how this linear graph was rearranged by Mendeleev into the Periodic Table.

7

What experiment showed that were divisible ?

8

How was the atomic structure of small positive nucleus and large surrounding electron cloud first demonstrated ?

9

Describe the Bohr “planetary model” of atomic structure. Explain why it could not accommodate many electrons of equal mass and charge.

10

Explain why Heisenberg”s Uncertainty Principle made the Bohr theory obsolete.

11

Explain how energy becomes “quantized” as standing waves in a confined system.

12

Show how the quantum numbers n, l and m_l identify the basic structural aspects of an orbital.

13

How did Schoedinger use this standing wave behaviour to set up a Position Space model of Atomic Structure ?

14

Define the concepts of Normality and Orthogonality of the standing waves used to define atomic orbitals.

15

Write these conditions in the Schroedinger integral format.

16

Define the Spherical Polar Coordinate system used to describe these orbitals.

17

Show how to calculate the number of separate orbital lobes in a shell of principal quantum number n.

18

Determine the lowest value of n for which m_l could have a value of +4.

19

Identify the orbital that has n = 5 and l = 1 and the one with n = 6 and l = 0.

20

Define the following features of orbital structure, angular node, radial node, nodal surface.

21

Define the radial probability functions, the angular probability functions and the contour maps of the 2s and 2p orbitals.

22

Define the three forces acting together on electrons bound within atomic orbitals.

23

Show how the magnetic forces lead to the Pauli Exclusion Principle.

24

Show how these forces together lead to the concept of the “orbital configurations” of atomic electronic structure.

25

Define the concept of “shielding” of the least stable electrons by the more stable electrons in an atom. Show the shielding of the “core” electrons against the (2p) electron in the atom Boron.

26

Define the complementary concept of “penetration” by the least stable electrons. Show the penetration through the core by the (2p) electron in the atom Boron

27

Define the concept of the Effective Nuclear Charge Z_Eff acting on the least stable electron.

28

Define the Slater Shielding Constant for the least stable electrons in an atom.

29

List Slater's Rules for shielding.

30

Use these Rules to estimate Z_Eff for the least stable electrons in B, Na, Cl and Sc.

31

Write noble gas core ground-state electron configurations for the atoms or ions Na, Ca, K, Cl, Sc³⁺, Cr, Mn⁴⁺, Co²⁺; Ni, Cu, Cu²⁺ and Pb .

32

Explain why C has its two valence electrons in different p orbitals with parallel spins rather than any other arrangement.

33

Explain why Be has a ground state electron configuration of (1s)²(2s)² rather than (ls)²(2s)¹(2p)¹.

34

Determine the number of unpaired electrons in neutral atoms of N, Si, Cr, Br and element 113.

35

Give the ground-state electron configurations of the following atoms or ions; C, F, Ca, Ga³⁺, Sc, V³⁺, V⁵⁺, Mn²⁺, Cr²⁺, Co³⁺, Cr⁶⁺, Cu, Mo⁴⁺, W, Rh³⁺, Eu³⁺, Eu²⁺, Gd³⁺ Bi, and Pb²⁺.

36

Draw the form of the periodic table with the numbers of the groups and the periods. Identify the s-, p-, and d- blocks and give their chemical names

37

Compare the periodic trends in element ionization energies and atomic radii. Show any repeating behaviour on a graph against atomic number Z.

37

Compare the first ionization energy of calcium with that of zinc. Explain the difference in terms of the balance between shielding with increasing numbers of d electrons and the effect of increasing nuclear charge. Define the concept of Transition Element Contraction

38

Compare the first ionization energies of Sr, Ba and Ra. Relate the irregularity to the Lanthanide Contraction.

39

Define the concept of the Stable Oxidation Numbers of an element.

40

Use the Auf Bau and Pauli Principles and the Slater shielding trends to predict the Stable Oxidation Numbers of the elements Tl, Ag, Zr and Sn from their electronic configurations.