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Question

1

Predict the change in the Hardness and Electronegativity values of elements down Groups.

2

Define the core and valence electrons for the neutral atoms in the forst and second rows of the Periodic Table.

3

Draw the shapes of these (ns) and (np) valence orbitals, including all orbital phases.

4

Draw the shapes of the Molecular Orbitals formed by allowed overlap of these atomic valence orbitals. Show all phase conditions.

5

Define the range of SON’s defined for 1A elements by the Octet Rule.

6

Are the electronegativity values of 1A elements low enough to allow formation of the cations with the SON of the previous rare gas configuration?

7

Are the electronegativity values of 1A elements high enough to allow formation of the anions with the SON of the next rare gas configuration?

8

From these limits on the allowed SON range, define the SONs of 1A elements.

9

Assuming purely ionic bonding, give the theoretical formula for calculating the lattice energy, U, of a 1A-halide salt.

10

During dissolution of a salt by a polar solvent, describe how solvent molecules attack and weaken the solid state bonds between the ions.

11

Identify which components of a solvated ion are the “Donor” and the “Acceptor”.

12

Define the type of bonding in which the terms Donor and Acceptor are used to describe the system

13

In solvated ions, identify which components are the Lewis acid and Lewis base.

14

Define the Coordination Number of a solvated ion.

15

How does the Coordination Number vary with ionic radius?

16

The hydrated proton is usually written H₃O⁺. What is the actual Coordination Number for this cation?

17

Write the equilibrium equations for the successive addition of water molecules to a cation to form a solvated cation.

18

Define the formation constants for each of these steps.

19

From the difference in electronegativity between H and C describe the bond type in methane..

20

Describe the bond type for Li and C and describe the bond type in LiCH₃

21

Compare the Hardness and Electronegativity values of 2A elements to 1A elements along each period.

22

Predict the change in the Hardness and Electronegativity values of 2A elements down the Group.

23

Use the Diagonal rule to predict the Hardness and Electronegativity values of 2A elements from those of the 1A elements.

24

Define the Stable Oxidation Number identified by the Octet Rule for 2A elements .

25

Describe the change in bond type from a hydated 1A ion to a hydrated 2A ion.

26

Describe how the change in (M-O) bond strength from a 1A to a 2A hydrated ion affects the strength of the internal (O-H) bond in the coordinated water molecule.

27

Describe how this change in bonding leads to Hydrolysis of the bound water.

28

Describe why hydrolysis of these bound water molecules is equivalent to Bronstead acid dissociation of a polyprotic acid.

29

Use the Octet Rule and the electronegativity trends to define the SONs of the 3A elements.

30

From the periodic electronegativity trend, describe the Bond Type in BH₃.

31

Draw the structure and describe the bonding in the diborane molecule.

32

Identify the bridge and terminal H atoms.

33

From the Octet Rule, predict the Lewis behaviour of BX₃ compounds.

Use shielding to explain why the chemical properties of Al are different from those of B.

34

Draw the structure and describe the bonding of the Al₂Cl₆ dimer.

35

Define the pH ranges for formation of Al(OH₂)₆³⁺ cations, Al(OH₂)₃(OH)₃ and AlO₂^- anions.

36

Define the equilibrium reactions for this sequence of hydrolysis reactions.

37

Define the hydrolysis constants for these steps.

38

Give the chemical definition of metal ions which permit all of these 3 conditions.

39

Describe the common physical form of the neutral compounds in this sequence.

40

Use shielding to explain why C can have SON values from -IV to +IV.

41

Draw the SON-Hydration Table for Carbon.

42

Explain why C atoms dehydrate more readily with increasing SON values.

43

Explain why methanol is a mild base but hydrated CO₂ is a weak acid

44

Use shielding to explain why the chemical properties of Si are similar to those of B.

45

On a reaction coordinate diagram, show the difference between an equilibrium reaction path and a transition state reaction path.

46

Describe the three concepts used to identify the reaction mechanisms of inert reagents.

47

Define the essential properties of electrophilic and nucleophilic reagent molecules.

48

Describe the difference in bond rearrangements between unimolecular and bimolecular reactions.

49

Use the Octet Rule and the electronegativity trends to define the SONs of the 5A elements.

50

Use shielding to explain why N can have SON values from -III to +V.

51

Draw the SON-Hydration Table for Nitrogen.

52

Show and name the reaction that leads to formation of NO₂

53

Use shielding to explain the large change in electronegativity from N to P.

54

Draw the SON-Hydration Table for P from PH₃ to P₂O₅.

55

Draw the shape of the P₄O₁₀ molecule.

56

Explain why the electronegativity of As is is similar to that of P.

57

Define the concept of Alternation of chemical properties down any Group.

58

Use the Octet Rule and the electronegativity trends to define the SONs of the 6A elements.

59

Draw the energy level diagram for the O₂ molecule and calculate its Bond Order.

60

Illustrate the allotropy of elements with the solid forms of S.

61

Use shielding to explain the large change in electronegativity from O to S.

62

Draw the SON-Hydration Table for S from SH₂ to SO₃.

63

Draw the energy level diagram and use the Aufbau Principle to define the bonding in H₂S

64

Compare bond overlaps to explain why the bond angle decereases from 109 in H₂O to 90 degrees in H₂S.

65

Give the structures of the SX _n molecules.

66

Explain why PF₅ is a Lewis acid but SF₆ is an inert gas.

67

Use shielding to explain the large change in electronegativity from F to Cl.

68

Draw the SON-Hydration Table for S from HCl to Cl₂O₇

69

Define the structures and Bond Types of the family of Interhalogen molecules.

70

Use shielding to explkain why ClF₇ and IF₇ exist but BrF₇ does not.

71

Explain why the acid strength of fully rediced elements increases from AlH₃ to HCl.

72

Use the Diagonal Rule to predict the chemical behaviour of the Noble Gas Xenon.

73

Draw the SON-Hydration Table for Xe.

74

Describe the Bond Type in Xenon compunds.

75

Why are some Xenon compunds used as reagents in organic syntesis reactions?