NURS 1310

Course: Biochemistry for nursing (NURS 1310)

Course time: Sunday , Tuesday: 9:30 – 11 L 403

Instructor: Dr. Tarek Zaida; tarekzaida@iug.edu

Office location: B304

Office hours: To be announced

Introduction

1

At the end of the course the student is expected to have:

gained a solid back ground on carbon based molecules

(organic chemistry) regarding their structures,

nomenclature, functional groups and basic reactions.

learnt the fundamentals of the structure as well as functions

of biological molecules (amino acids, proteins,

carbohydrates, lipids, nucleic acids).

learnt the basic concepts of enzyme catalysis and

intermediary metabolism.

NURS 1310Course Objectives

2

Course schedule NURS 1310

Weeks TopicsWeek 1 Introduction to organic chemistry Week 2 Saturated Hydrocarbons (Alkanes, and their

halogen derivatives

Week 3 Unsaturated hydrocarbons, and their halogen derivatives

Week 4 Alcohols, thiols, phenols, and ethersWeek 5 Aldehydes, ketones and carboxylic acids

BiochemistryWeek 6-7 CarbohydratesWeek 8-9 LipidsWeek 10-11 Proteins Week 12-13 Nucleic acids Week 14 Enzymes and basic concepts of analysis Week 15 Introduction into metabolism3

Organic Chemistry, a short course; 13th edition (2012); David Hart, Christopher Hadad, Laslie Craine, and Harold Hart.

Biochemistry, a short course; 1st edition (2010); John L. Tymoczko and Jeremy M. Berg, and Lubert Stryer.

Chemistry for the health sciences; 8th (1998); Georg Sackheim, Dennis Lehmann.

NURS 1310Textbooks

4

Course attendance and course activities: 15 %

Participating in different Electronic tools 5%

Midterm exam: 30 %

Final exam: 50 %

NURS 1310Evaluation

5

Organic Chemistry

Chapter 1Introduction to organic

chemistry

6

Introduction to organic chemistry

• History:• Earlier in the eighteenth century it was

believed that in order to produce compounds by living cells, a “vital force” was needed.

• These compounds were classified as organic compounds.

• A german chemist, Friedrich Woehler in 1828 has shown this belief was incorrect

7

How did Woehler end this belief?

• He prepared urea, a compound normally found in both blood and urine, by heating a solution of ammonium cyanate, which is considered an inorganic compound:

NH4CNO heat NH2-CO-NH2

8

• Later on many other organic compounds were produced in the laboratory.

• This has led to the subdivision of chemistry into 2 parts:

• Organic• Inorganic

9

Organic Chemistry

• Definition:

With the simplest definition, organic chemistry is known as the chemistry of carbon compounds.

10

What makes Carbon so special to give it a whole branch of chemistry and place all

other elements in the other branch?

1. Carbon is unique in that it forms covalent bonds to other carbon atoms as well as to other elements.

2. There are millions of organic compounds known today

11

Importance of organic chemistry

• It’s importance comes from its association with all living matter in both plants and animals

Examples:Proteins, carbohydrates, lipids, hormones,

vitamins, enzymes, and many other drugs are organic compounds.

12

Comparison of organic and inorganic compounds

organic inorganic

Flammable yes no

Melting point low high

Boiling point low high

Solubility in water No (most) yes

Solubility in nonpolar liquids

yes no

Types of bonding covalent ionic

Reactions occur between

molecules ions

Atoms per molecules many few

structure complex simple

Electrolyte no yes

13

Carbon and the Covalent Bond C usually forms covalent bonds with other

atoms by sharing electrons. Covalent bond: an evenly strong bond formed

between 2 atoms by sharing electrons. Carbon atom has 4 electrons so it can form a

maximum of 4 covalent bonds.

14

Carbon–Carbon Single Bonds C has ability to share electrons not only

with different elements but also with other carbon atoms. In this case the electrons are shared equally between

the two identical carbon atoms As shown below in the example two C atoms may be

bonded to one another, and each of these carbon atoms may be linked to other atoms (Chains).

15

16

Polar Covalent Bonds A polar covalent bond is a covalent bond in

which the electron pair is not shared equally between the two atoms.

Example: Hydrogen chloride molecule (HCl)

In case of HCl, the shared electron pair is attracted more toward the chlorine, which therefore is slightly negative (partial negative charge) with respect to the hydrogen.

17

18

Multiple Covalent Bonds In a double bond, two electron pairs are

shared between two atoms. Nonbonding electrons, or unshared electron

pairs, reside on one atom. In a triple bond , three electron pairs are

shared between two atoms.

19

Hydrocarbons are compounds composed of just hydrogen and carbon atoms.

20

Valence The valence of an element is the number of

bonds that an atom of the element can form. The number is usually equal to the number of

electrons needed to fill the valence shell. Oxygen, for example, has six valence

electrons but a valence of only 2.

21

IsomerismThe molecular formula of a substance

gives the number of different atoms present.

The structural formula indicates how those atoms are arranged.

Isomers are molecules with the same number and kinds of atoms but different arrangements of the atoms.

22

Structural (or constitutional ) isomers have the same molecular formula but different structural formulas.

23

Writing Structural Formulas In a continuous chain, atoms are bonded one after

another. In a branched chain , some atoms form branches from

the longest continuous chain.

24

Abbreviated Structural Formulas In a continuous chain, atoms are bonded one after

another. In a branched chain , some atoms form branches from

the longest continuous chain.

25 Line segment structure

Classification According to Molecular Framework

The three main classes of molecular frameworks for organic structures are acyclic, carbocyclic, and heterocyclic compounds.

Acyclic compounds contain no rings. Carbocyclic compounds contain rings of carbon

atoms. Heterocyclic compounds have rings containing

at least one atom that is not carbon.

26

27

Acyclic compounds

28

Carbocyclic compounds

29

Heterocyclic compounds

Allotropic Forms of Carbons

• Three forms are know:• Graphite: soft, dark black solid with good

electrical conduction.• Diamond: formed over long geologic time

periods, when graphite is subjected to extreme underground pressures. Diamond is clear, and is the hardest natural substance known.

• Fullerenes: the most common being C60 have shapes similar to soccer balls

30

Graphite

31

Diamond

32

Fullerene

33

Classification According to Functional Group

Functional groups are groups of atoms that have characteristic chemical properties regardless of the molecular framework to which they are attached.

34

Classification According to Functional Group

Functional groups are groups of atoms that have characteristic chemical properties regardless of the molecular framework to which they are attached.

35

36

37