Name: Orlando Nica
Student ID: 20413435
Qualification: Pearson BTEC Level 3 National Extended Diploma in
Applied Science
Unit number and title: Unit 14: Applications of Organic Chemistry
Learning aim A: Understand the structures, reactions and properties of
functional group compounds.
Functional group chemistry for designer molecules
Scenario: I am a research assistant working for Reckitt Benckiser at their
research and development base in Hull (UK). The products made by this
company include Vanish and Mr Sheen. Each year the research laboratories
invite a small group of ‘A’ level and ‘BTEC’ students in for two weeks of work
experience. This year I have been given the responsibility of preparing an
instructional video or presentation and accompanying handbook that will be
used on the first day of the student’s work experience. The purpose is to ensure
the work experience students have the basic knowledge they will need about the
structure, reactions and properties of carbonyl and non-carbonyl organic
compounds.
Aim: The aim of this write up is to create a handbook that explains the
functional groups and their relevance to reactivity of organic compounds.
The handbook will be then filled up with balanced equations that will illustrate
the importance of functional groups reactions in organic and inorganic
chemistry. In addition to that a multi-step synthesis will be planned for an
organic molecule. The planned synthesis will include reagents, reaction
conditions and intermediate products involved in each step.
1
, CONTENT PAGE:
1.1 FUNCTIONAL GROUPS
1.1.1 What are functional GROUPS:
1.1.2 Halogenoalkanes and their reactions (Nucleophilic Substitution and
Elimination)
1.1.3 Alcohols ( Primary, Secondary , Tertiary and their Reactions)
1.1.4 Amines (Bases and Nucleophiles Reactions)
1.1.5 Aldehydes and Ketones (Their reactions)
1.1.6 Carboxylic acids ( Addition-Elimination to form Esters)
1.1.7 Acyl Chlorides, Acid Anhydrides, Amides ( Their reactions)
1.2 MECHANISM
1.2.1 Addition
1.2.2 Substitution
1.2.3 Elimination
1.2.4 Addition-Elimination
1.3 PLAN A MULTI-STEP SYNTHESIS
1.3.1 ethyl ethanoate (CH 3 CO 2 CH 2 CH 3 ), starting from ethanol and
ethanal
2
, Halogenoalkanes
Halogenoalkanes are compounds in which one or more hydrogen atoms in an
alkane have been replaced by halogen atoms (fluorine, chlorine, bromine or
iodine)
The carbon-halogen bonds (apart from the carbon-iodine bond) are polar,
because the electron pair is pulled closer to the halogen atom than the carbon.
This is because (apart from iodine) the halogens are more electronegative than
carbon.
The electronegativity values are:
C 2.5 F 4.0
Cl 3.0
Br 2.8
I 2.5
This means that in addition to the dispersion forces there will be forces due to
the attractions between the permanent dipoles (except in the iodide case). The
size of those dipole-dipole attractions will fall as the bonds get less polar (as
you go from chloride to bromide to iodide, for example). Nevertheless, the
boiling points rise! This shows that the effect of the permanent dipole-dipole
attractions is much less important than that of the temporary dipoles which
cause the dispersion forces.
3
Student ID: 20413435
Qualification: Pearson BTEC Level 3 National Extended Diploma in
Applied Science
Unit number and title: Unit 14: Applications of Organic Chemistry
Learning aim A: Understand the structures, reactions and properties of
functional group compounds.
Functional group chemistry for designer molecules
Scenario: I am a research assistant working for Reckitt Benckiser at their
research and development base in Hull (UK). The products made by this
company include Vanish and Mr Sheen. Each year the research laboratories
invite a small group of ‘A’ level and ‘BTEC’ students in for two weeks of work
experience. This year I have been given the responsibility of preparing an
instructional video or presentation and accompanying handbook that will be
used on the first day of the student’s work experience. The purpose is to ensure
the work experience students have the basic knowledge they will need about the
structure, reactions and properties of carbonyl and non-carbonyl organic
compounds.
Aim: The aim of this write up is to create a handbook that explains the
functional groups and their relevance to reactivity of organic compounds.
The handbook will be then filled up with balanced equations that will illustrate
the importance of functional groups reactions in organic and inorganic
chemistry. In addition to that a multi-step synthesis will be planned for an
organic molecule. The planned synthesis will include reagents, reaction
conditions and intermediate products involved in each step.
1
, CONTENT PAGE:
1.1 FUNCTIONAL GROUPS
1.1.1 What are functional GROUPS:
1.1.2 Halogenoalkanes and their reactions (Nucleophilic Substitution and
Elimination)
1.1.3 Alcohols ( Primary, Secondary , Tertiary and their Reactions)
1.1.4 Amines (Bases and Nucleophiles Reactions)
1.1.5 Aldehydes and Ketones (Their reactions)
1.1.6 Carboxylic acids ( Addition-Elimination to form Esters)
1.1.7 Acyl Chlorides, Acid Anhydrides, Amides ( Their reactions)
1.2 MECHANISM
1.2.1 Addition
1.2.2 Substitution
1.2.3 Elimination
1.2.4 Addition-Elimination
1.3 PLAN A MULTI-STEP SYNTHESIS
1.3.1 ethyl ethanoate (CH 3 CO 2 CH 2 CH 3 ), starting from ethanol and
ethanal
2
, Halogenoalkanes
Halogenoalkanes are compounds in which one or more hydrogen atoms in an
alkane have been replaced by halogen atoms (fluorine, chlorine, bromine or
iodine)
The carbon-halogen bonds (apart from the carbon-iodine bond) are polar,
because the electron pair is pulled closer to the halogen atom than the carbon.
This is because (apart from iodine) the halogens are more electronegative than
carbon.
The electronegativity values are:
C 2.5 F 4.0
Cl 3.0
Br 2.8
I 2.5
This means that in addition to the dispersion forces there will be forces due to
the attractions between the permanent dipoles (except in the iodide case). The
size of those dipole-dipole attractions will fall as the bonds get less polar (as
you go from chloride to bromide to iodide, for example). Nevertheless, the
boiling points rise! This shows that the effect of the permanent dipole-dipole
attractions is much less important than that of the temporary dipoles which
cause the dispersion forces.
3
