This document provides an introduction to biochemistry, covering topics like elements, atoms, ions, electron shells, chemical bonds, and organic macromolecules. It defines key terms and explores the building blocks of organic compounds like carbohydrates, lipids, proteins, and nucleic acids. The roles and examples of these macromolecules in the body are also summarized.

1. Chapter 2: Introductory
Biochemistry
Anatomy and Physiology

2. Chemistry
 Elements – cannot be broken down into
simpler form
 Chemical symbol – represented with letters
(first always capital and second is small)

3.  Atoms – smallest unit of matter
 Protons
 Neutrons
 electrons

4.  Atomic mass = mass of nucleus (protons +
neutrons)
 Atomic number =number of protons
 Number of electrons = # of protons
 Number of neutrons = atomic mass - #
protons
19
F
9
55
Mn
25
32
S
16
40
Ca
20
27
Al
13

5. Math Monkey Moment
How many protons, neutrons and electrons are in each
atom?
Protons Neutrons Electrons
Be
Na
Ca

6.  Electron shells – electrons move in layers
around the nucleus
 2 electrons in shell closest to nucleus
 8 electrons in the next shell

7.  Ions – atoms that give up or gain electrons
when bonding to another atom become
positive or negative (charge). i.e. Ca2+
or K-
 Molecule – 2 or more atoms share
electrons

8. Compound – 2 or more different
types of atoms bonded together.
H2O and C6H12O6 are compounds
and molecules
O2 and N2 are molecules not
compounds

9. Chemical Reactions
 Occurs when bonds are broken and
reformed
 Reactants
 Products
 Law of conservation of matter
Count the atoms in H2O and
C6H12O6
C6H12O6 + 6O2  6CO2 + 6 H2O

10.  Chemical energy - Energy stored in chemical
bonds and is a form of potential energy
 Anabolic reactions build substances and
generally require energy which is then stored
in their chemical bonds. i.e. glycogen
 Catabolic reactions break down substances
and release energy. i.e. fat catabolism
 ATP – adenosine triphosphate is the
compound of energy used for the work of
cells in living organisms

11. Chemical Bonds
 Valence shell – outer electron shell and electrons
involved with bonding to other atoms.
 Ionic bonds – atom gains or loses electrons; metal
bonds to a nonmetal (see periodic table)

12. Cation – positively charged ion
Anion – negatively charged ion
Electrolytes – ionic compound
that breaks apart into cations
and anions when dissolved

13.  Covalent bonds – atoms share
electrons in their valence shell
 (nonmetals only)
 Most common bonds in body
 Carbon can form 4 bonds

14. Hydrogen bonds – forms when
hydrogen atoms with a partial
positive charge bond with a
partial negative atom.
Weaker bond
Reason for properties of water

16. Vocabulary Cards
Anabolic
Catabolic
Cation
anion
Ionic bond
Covalent
bond
Hydrogen
bond

17. Inorganic Compounds Organic – carbon containing compounds
(except CO2)
 Inorganic – all others including CO2
 Water is most important and abundant
inorganic compound in living systems. 5
properties
 Excellent solvent

18. Solutes that are polar (slightly
charged) are hydrophilic and dissolve
in water.
Solutes that are nonpolar are
hydrophobic and do not dissolve in
water.

19.  Participates in chemical reactions
 Absorbs and releases heat slowly –
helps moderate changes in body
temp.
 Requires a lot of heat to change
from liquid to gas
 Serves as a lubricant: major
component of mucus

20. Acids and bases
 Acids break apart or dissociate into
one or more hydrogen ions (H+
)
 Bases break apart or dissociate into
one or more hydroxide ions (OH-
)
 Salt dissociates into cations and anions
that are neither H+
nor OH-

21.  pH
 Scale of 0-14
 Below 7, greater H+
than OH-
and are acids
 Above 7, greater OH-
than H+
and are bases
 7 is neutral

22. 10-1
10-4
10-8
10-14

23. Buffers
 Living systems are very sensitive to
changes in pH
 Buffer systems keep pH stable by giving
up H+
or OH-
depending on what is needed

24.  Blood pH is 7.35-7.45. Lethal is 6.8 and
7.8
 i.e. bicarbonate buffer system
CO2 + H2O H2CO3 HCO3
-
+ H+

25. Organic compounds
 Most common elements of living
organisms: CHNOPS
 Made of monomers or building blocks

26.  Monomers combined by dehydration
synthesis reaction and water is lost.
 Monomers break apart by hydrolysis and
water required.

27. Vocabulary Cards
Organic
Inorganic
Dehydration
synthesis
Hydrolysis
Buffer
pH

28. Organic Macromolecules
 Carbohydrates
 Lipids
 Proteins
 Nucleic Acids

29. Carbohydrates
 Monomer: monosaccharides
 Monomer components: C, H, O (2:1H-
C)

30.  Types
 Monosaccharides
 Disaccharides
 Polysaccharides
(starch)
 Function: energy

31. Proteins
 Monomers: amino acids
 Monomer components:
 amino group (-NH2), carboxyl
group (-COOH), and side chain
(R group)
 C, H, O, N, S

32.  Types:
 Peptide
 polypeptide
 Function(s): multiple
 Varies depending on type
 Generally responsible for structure
of body cells

34. Enzymes
 Proteins that are catalysts to
speed up chemical reactions
without being altered
themselves.

35.  Act as a lock and key
 Substrate is the key and binds
to the active site on the enzyme
 Enzyme is the lock or binding
site
 Form enzyme-substrate
complex

37. Lipids
 Monomers: fatty acids and glycerol
 Monomer components: C, H, O (H-O not
2:1)

38.  Types:
 Triglyceride
Saturated
unsaturated
 Steroids
 phospholipids
 Function(s)
 Triglycerides – energy
 Steroids – hormones
 Phospholipids-membranes

39. Nucleic Acids
 Monomer: nucleotide
 Monomer components: sugar, phosphate,
nitrogen base

40.  Types
 DNA: deoxyribonucleic acid
Adenine, thymine, cytosine, and guanine
Double stranded
helix
 RNA: ribonucleic acid
Adenine, uracil, cytosine, and guanine
Single stranded
 Function: hereditary information

43. Vocabulary
Cards
 Enzyme
 Lipid
 Carbohydrate
 Protein
 Nucleic acid

44. ANY QUESTIONS?