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A.1 Determination of Structure

A.2 Rate Expression.

A.3 Reaction Mechanism

A.4 Nucleophilic Substitution Reactions

A.5 Acids, Bases and Buffers

A.1 Determination of Structure (5hr)

A.1.1 State that the structure of a compound can be determined by using information from a variety of spectroscopic and chemical techniques.

A.1.2 describe and explain hoe information from an infrared spectrum can be used to identify functional groups in a compound.

• restrict to using infrared spectra to show the presence of alcohols acids, ketones aldehydes, alkenes and alkynes
• Match the fingerprint region to a known spectra

A.1.3 describe and explain how information from a mass spectrum can be used to determine the structure of a compound.

• restrict to using mass spectra to determine the relative molecular mass of a compound and to identify simple fragments
• (Mr-15) loss of CH3
• (Mr-29) loss of C2H5 or CHO
• (Mr-31) loss of CH3O
• (Mr-45) loss of COOH

A.1.4 Describe and explain how information from a H NMR spectrum can be used to determine the structure of a compound.

• restrict this to using NMR spectra to determine the number of different environments in which hydrogen is found and the number of hydrogen atoms inn each environment. Splitting pattern are not required.

A.1.5 Describe and explain the structure of benzene using chemical and physical evidence.

• Consider the special stability of the ring system (heat of combustion or hydrogenation of C6H6 in comparison to that of cyclohexene, cyclohexadiene and cyclohexatriene), as well as benzene's

A.2 Rate Expression. (3hr)

A.2.1 Define the terms rate constant and order of reaction. 

A.2.2 Derive the rate expression for a reaction from data.

• Rate = k[A]^m[B]ⁿ
• where k = rate constant, [A] = concentration in mol dm^-3

A.2.3 Draw and analyze graphical representations for zero, first and second order reactions.

A.2.4 Define the terms half life and calculate the half life for first-order reactions

• The half-life should be calculated from graphs and by using the integrated form of the rate equation. Integrated form of 2nd order is not required.

A.3 Reaction Mechanism (1hr)

A.3.1 Define the terms "rate determining step" , 'molecularity' and 'activated complexes'.

A.3.2 Describe the relationship between mechanism, order, rate determining step and activated complex.

• Restrict examples to 1 or 2 step reactions where mechanism is known.

A.4 Nucleophilic Substitution Reactions(2hr)

A.4.1 Distinguish between primary, secondary and tertiary halogenoalkanes.

A.4.2 Describe and explain the Sn1 and Sn2 mechanisms in nucleophilic substitution.

• Students must be able to draw a stepwise mechanism. Examples of nucleophiles should include -CN, -OH, and NH3.

A.4.3 describe and explain the molecularity for the Sn1 and Sn2 mechanisms.

• The predominant mechanism for tertiary halogenoalkanes is Sn1 and for primary halogenoalkanes it is Sn2. Both mechanisms occur for secondary halohenoalkanes

A.4.4 Describe how the rate of nucleophilic substitution in halogenoalkanes depends on both the identity of the halogen and whether the halogenoalkane is primary, secondary tertiary.

A.5 Acids, Bases and Buffers (4hr)

A.5.1 State the expression for the ionic product constant of water.(Kw)

A.5.2 Define pH, pOH, and pKw

A.5.3 Calculate the pH, pOH, [H+(aq)] and [OH-(aq)] from specified concentrations

A.5.5 State the equation for the reaction of any acid or base with water and hence derive the ionization constant expression for any weak acid or base in water.

• HA<--> H⁺ + A^-
• B + H₂O <--> BH⁺ + OH^-

A.5.6 State and explain the relationship between Ka and pKa.

A.5.7 Determine the relative strengths of acids or their conjugate bases from Ka or pKa values

A.5.8 Apply Ka or pKa in calculations.

• Calculations can be performed using various forms of the acid ionization constant expression. Student should state when approximations are used in equilibrium calculations. Use of quadratic expression is not required

 A.5.9 Calculate the pH of a specified buffer system.

• Calculations will involve the transfer of only one proton.