Chapter 4 discusses the importance of carbon in biological molecules, highlighting its unique ability to form diverse and complex compounds that are foundational to life. It covers concepts such as organic chemistry, bonding configurations, molecular diversity, isomer types, and functional groups crucial for chemical reactions. Additionally, it emphasizes the role of adenosine triphosphate (ATP) in cellular energy transfer.

1. Chapter 4
Carbon and the Molecular
Diversity of Life

2. Overview: Carbon—The Backbone of
Biological Molecules
• Although cells are 70–95% water, the rest
consists mostly of carbon-based compounds
• Carbon is unparalleled in its ability to form
large, complex, and diverse molecules
• Proteins, DNA, carbohydrates, and other
molecules that distinguish living matter are all
composed of carbon compounds

3. Concept 4.1: Organic chemistry is
the study of carbon compounds
• Organic compounds range from simple molecules to
colossal ones
• Most organic compounds contain hydrogen atoms in
addition to carbon atoms
• Vitalism, the idea that organic compounds arise only in
organisms, was disproved when chemists synthesized
the compounds
• Mechanism is the view that all natural phenomena are
governed by physical and chemical laws

4. 1953—Stanley Miller

5. Concept 4.2: Carbon atoms can
form diverse molecules by bonding
to four other atoms (valence of 4)
• Electron configuration is the key to an atom’s
characteristics
• Electron configuration determines the kinds
and number of bonds an atom will form with
other atoms

6. The Formation of Bonds with
Carbon
• With four valence electrons, carbon can form four
covalent bonds with a variety of atoms
• This tetravalence makes large, complex molecules
possible
• In molecules with multiple carbons, each carbon
bonded to four other atoms has a tetrahedral shape
• However, when two carbon atoms are joined by a
double bond, the molecule has a flat shape

7. LE 4-3
Molecular
Formula
Structural
Formula
Ball-and-Stick
Model
Space-Filling
Model
Methane
Ethane
Ethene (ethylene)

8. • The electron configuration of carbon gives it
covalent compatibility with many different
elements
• The valences of carbon and its most frequent
partners (hydrogen, oxygen, and nitrogen) are
the “building code” that governs the
architecture of living molecules

9. LE 4-4
Hydrogen
(valence = 1)
Oxygen
(valence = 2)
Nitrogen
(valence = 3)
Carbon
(valence = 4)
Valence electrons
1 6 5 4
Note the difference between valence electrons and valence. Do not get
mixed up.

10. Molecular Diversity Arising from
Carbon Skeleton Variation
• Carbon chains form the skeletons of most
organic molecules
• Carbon chains vary in length and shape

11. LE 4-5
Length
Ethane Propane
Butane 2-methylpropane
(commonly called isobutane)
Branching
Double bonds
Rings
1-Butene 2-Butene
Cyclohexane Benzene

12. Hydrocarbons
• Hydrocarbons are organic molecules consisting
of only carbon and hydrogen
• Many organic molecules, such as fats, have
hydrocarbon components
• Hydrocarbons can undergo reactions that
release a large amount of energy

13. Figure 4.6
Nucleus
Fat droplets
(b) A fat molecule(a) Part of a human adipose cell
10 μm

14. Isomers
• Isomers are compounds with the same
molecular formula but different structures and
properties:
– Structural isomers have different covalent
arrangements of their atoms
– Geometric isomers have the same covalent
arrangements but differ in spatial arrangements
– Enantiomers are isomers that are mirror images
of each other

15. LE 4-7
Structural isomers differ in covalent partners, as shown in
this example of two isomers of pentane.
Geometric isomers differ in arrangement about a double
bond. In these diagrams, X represents an atom or group of
atoms attached to a double-bonded carbon.
cis isomer: The two Xs
are on the same side.
trans isomer: The two Xs
are on opposite sides.
L isomer D isomer
Enantiomers differ in spatial arrangement around an
asymmetric carbon, resulting in molecules that are mirror
images, like left and right hands. The two isomers are
designated the L and D isomers from the Latin for left and
right (levo and dextro). Enantiomers cannot be
superimposed on each other.

16. • Enantiomers are important in the
pharmaceutical industry
• Two enantiomers of a drug may have different
effects
• Differing effects of enantiomers demonstrate
that organisms are sensitive to even subtle
variations in molecules

17. Figure 4.8
Drug Effects
Effective
Enantiomer
Ineffective
Enantiomer
Ibuprofen
Albuterol
Reduces
inflammation
and pain
Relaxes bronchial
(airway) muscles,
improving airflow
in asthma
patients
S-Ibuprofen
R-AIbuterol S-AIbuterol
R-Ibuprofen

18. 4. What type of isomer is propanal
compared to acetone?
a. cis-trans isomer
b. structural isomer
c. enantiomer
d. none of the above; these are not isomers

19. 4. What type of isomer is propanal
compared to acetone?
a. cis-trans isomer
b. structural isomer
c. enantiomer
d. none of the above; these are not isomers

20. Concept 4.3: Functional groups are the
parts of molecules involved in chemical
reactions
• Distinctive properties of organic molecules
depend not only on the carbon skeleton but
also on the molecular components attached
to it
• Certain groups of atoms are often attached to
skeletons of organic molecules

21. The Functional Groups Most
Important in the Chemistry of Life
• Functional groups are the components of
organic molecules that are most commonly
involved in chemical reactions
• The number and arrangement of functional
groups give each molecule its unique
properties

22. LE 4-9
Estradiol
Testosterone
Male lion
Female lion

23. • The seven functional groups that are most
important in the chemistry of life
– Hydroxyl group
– Carbonyl group
– Carboxyl group
– Amino group
– Sulfhydryl group
– Phosphate group
– Methyl group
– also primary amide and acetyl

24. Figure 4.9
Chemical Group Compound Name Examples
Ethanol
PropanalAcetone
Acetic acid
Glycine
Cysteine
Glycerol phosphate
Organic
phosphate
Thiol
Amine
Carboxylic acid, or
organic acid
Ketone
Aldehyde
AlcoholHydroxyl group (—OH)
Carboxyl group (—COOH)
Amino group (—NH2)
Sulfhydryl group (—SH)
Phosphate group (—OPO3
2−
)
Methyl group (—CH3) Methylated
compound
5-Methyl cytosine
Carbonyl group ( C ＝
O)
——

25. Others
• R-CH2-CH3 alkyl
O
• R-C-CH3 acetyl
O
• R-C-N-H primary amide
H

26. ATP: An Important Source of Energy
for Cellular Processes
• One phosphate molecule, adenosine
triphosphate (ATP), is the primary energy-
transferring molecule in the cell
• ATP consists of an organic molecule called
adenosine attached to a string of three
phosphate groups

27. Figure 4.UN04
Adenosine

28. Figure 4.UN05
Reacts
with H2O
Inorganic
phosphate
ADP
EnergyAdenosine Adenosine
ATP
P P P P PP i

29. The Chemical Elements of Life:
A Review
• The versatility of carbon makes possible the
great diversity of organic molecules
• Variation at the molecular level lies at the
foundation of all biological diversity

30. 5. Based on these results, how many molecules of
methionine are present per mole of glycine?
a. 1.08 x 1070
molecules
b. 1.8 x 103
molecules
c. 1.08 x 1021
molecules
d. 6.02 x 1023
molecules

31. 5. Based on these results, how many molecules of
methionine are present per mole of glycine?
a. 1.08 x 1070
molecules
b. 1.8 x 103
molecules
c. 1.08 x 1021
molecules
d. 6.02 x 1023
molecules
Moles methionine/moles glycine x 6.023 x
1023
molecules methionine/mole
methionine