1. Anatomy and Physiology
This PPT Adapted from
Hole’s Human
Anatomy and Physiology
Eleventh Edition
Shier w Butler w Lewis
Chapter 2
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

2. Chapter 2 Chemical Basis of Life
Why study chemistry in an Anatomy and Physiology class?
- body functions depend on cellular functions
- cellular functions result from chemical changes
- biochemistry helps to explain physiological processes, and develop new drugs and methods for treating diseases

3. Structure of Matter
Matter – anything that takes up space and has weight; composed of elements
Elements – composed of chemically identical atoms
bulk elements – required by the body in large amounts
trace elements – required by the body in small amounts
Atoms – smallest particle of an element

4. Atomic Structure Atoms - composed of subatomic particles:
proton – carries a single positive charge
neutron – carries no electrical charge
electron – carries a single negative charge
Nucleus
central part of atom
composed of protons and neutrons
electrons move around the nucleus

5. Atomic Number and Atomic Weight
number of protons in the nucleus of one atom
each element has a unique atomic number
equals the number of electrons in the atom
Atomic Weight
the number of protons plus the number of neutrons in one atom
electrons do not contribute to the weight of the atom

6. Isotopes
Isotopes
atoms with the same atomic numbers but with different atomic weights
atoms with the same number of protons and electrons but a different number of neutrons
oxygen often forms isotopes (O16, O17, O18)
unstable isotopes are radioactive; they emit energy or atomic fragments

7. Molecules and Compounds
Molecule – particle formed when two or more atoms chemically combine
Compound – particle formed when two or more atoms of different elements chemically combine
Molecular formulas – depict the elements present and the number of each atom present in the molecule
H C6H12O H2O

8. Bonding of Atoms bonds form when atoms combine with other atoms
electrons of an atom occupy regions of space called electron shells which circle the nucleus
each shell can hold a limited number of electrons
for atoms with atomic numbers of 18 or less, the following rules apply:
the first shell can hold up to 2 electrons
the second shell can hold up to 8 electrons
the third shell can hold up to 8 electrons

9. Bonding of Atoms lower shells are filled first
if the outermost shell is full, the atom is stable

10. Ions
Ion
an atom that gains or loses electrons to become stable
an electrically charged atom
Cation
a positively charged ion
formed when an atom loses electrons
Anion
a negatively charged ion
formed when an atom gains electrons

11. Ionic Bond Ionic Bond an attraction between a cation and an anion
formed when electrons are transferred from one atom to another atom

12. Covalent Bond Formed when atoms share electrons
Hydrogen atoms form single bonds
Oxygen atoms form two bonds
Nitrogen atoms form three bonds
Carbon atoms form four bonds
H ― H
O = O
N ≡ N
O = C = O

13. Ionic Compounds Covalent Compounds Made of metal and non-metals
Two or more Non-metals
Dissolve ready in water
Many do not dissolve in water
Dissociate into + or – ions surrounded by hydration shells
Remain intact molecules
Many inorganic compounds
All organic compounds
Electrolytes in water
Non-electrolytes
Crystalline structure
Amorphous

14. Structural Formula
Structural formulas show how atoms bond and are arranged in various molecules (covalent compounds)

15. Polar Molecules Polar Molecule ( polar covalent molecules)
molecule with a slightly negative end and a slightly positive end
results when electrons are not shared equally in covalent bonds
water is an important polar molecule

16. Polarity of Water Responsible for properties of water
Adhesion, cohesion, surface tension
Capillary action
“Universal solvent” can dissolve ionic and some covalent compounds

17. Hydrogen Bonds Hydrogen Bond
a weak attraction between the positive end of one polar molecule and the negative end of another polar molecule
formed between water molecules
important for protein and nucleic acid structure

18. Chemical Reactions
Chemical reactions occur when chemical bonds form or break among atoms, ions, or molecules
Reactants are the starting materials of the reaction- the atoms, ions, or molecules
Products are substances formed at the end of the chemical reaction
NaCl ’ Na+ + Cl-
Reactant
Products

19. Types of Chemical Reactions
Synthesis Reaction – more complex chemical structure is formed
A + B ’ AB
Decomposition Reaction – chemical bonds are broken to form
a simpler chemical structure
AB ’ A + B
Exchange Reaction – chemical bonds are broken and new bonds are formed
AB + CD ’ AD + CB
Reversible Reaction – the products can change back to the reactants
A + B n AB

20. Acids, Bases, and Salts
Electrolytes – substances that release ions in water
NaCl  Na+ + Cl-
Acids – electrolytes that dissociate to release hydrogen ions
in water
HCl  H+ + Cl-
Bases – substances that release ions that can combine with hydrogen ions
NaOH  Na+ + OH-
Salts – electrolytes formed by the reaction between an acid and a base
HCl + NaOH  H2O + NaCl

21. Buffers
Buffers are the salts of weak acids. They can keep the pH of a solution from shifting too rapidly. The can help maintain pH within a narrow range.
A buffer can neutralize either an acid or a base. With an acid it acts as a base. With a base it can act as an acid.
An example is NaHCO3

22. Acid and Base Concentrations
pH scale - indicates the
concentration of hydrogen ions in
solution
Neutral – pH 7; indicates equal concentrations of H+ and OH-
Acidic – pH less than 7; indicates a greater concentration of H+
Basic or alkaline – pH greater than 7;
indicates a greater concentration of OH-

23. Organic Versus Inorganic
Organic molecules
contain C and H
usually larger than inorganic molecules
dissolve in water and organic liquids
carbohydrates, proteins, lipids, and nucleic acids
Inorganic molecules
generally do not contain C
usually smaller than organic molecules
usually dissociate in water, forming ions
water, oxygen, carbon dioxide, and inorganic salts

24. Inorganic Substances Water most abundant compound in living material
two-thirds of the weight of an adult human
major component of all body fluids
medium for most metabolic reactions
important role in transporting chemicals in the body
absorbs and transports heat
Oxygen (O2)
used by organelles to release energy from nutrients
in order to drive cell’s metabolic activities
necessary for survival

25. Inorganic Substances Carbon dioxide (CO2)
waste product released during metabolic reactions
must be removed from the body
Inorganic salts
abundant in body fluids
sources of necessary ions (Na+, Cl-, K+, Ca2+, etc.)
play important roles in metabolism

26. Organic Substances Carbohydrates
provide energy to cells
supply materials to build cell structures
water-soluble
contain C, H, and O
ratio of H to O close to 2:1 (C6H12O6)
monosaccharides – glucose, fructose
disaccharides – sucrose, lactose
polysaccharides – glycogen, cellulose

27. Organic Substances Carbohydrates

28. Dehydration synthesis

29. Hydrolysis

30. Organic Substances Lipids
soluble in organic solvents; insoluble in water
fats (triglycerides)
used primarily for energy; most common lipid in the body
contain C, H, and O but less O than carbohydrates (C57H110O6)
building blocks are 1 glycerol and 3 fatty acids per molecule
saturated and unsaturated

31. Organic Substances Lipids
phospholipids
building blocks are 1 glycerol, 2 fatty acids, and 1 phosphate per molecule
hydrophilic and hydrophobic
major component of cell membranes
2-25

32. Organic Substances Lipids
steroids
four connected rings of carbon
widely distributed in the body, various functions
component of cell membrane
used to synthesize hormones
cholesterol

33. Organic Substances Proteins
structural material
energy source
hormones
receptors
enzymes
antibodies
amino acids held together with peptide bonds
building blocks are amino acids
2-27

35. Organic Substances Nucleic Acids
carry genes
encode amino acid sequences of proteins
building blocks are nucleotides
DNA (deoxyribonucleic acid) – double polynucleotide
RNA (ribonucleic acid) – single polynucleotide

36. Organic Substances Nucleic Acids

37. DNA
RNA
A-T and G-C
A-U and G-C
Double helix
Single strand
Can’t leave nucleus
Active in cytoplasm
Replication and Transcription
Translation of proteins
1 kind
Many types

38. Macro-molecule
Elements
Building blocks (monomers)
Example monomers
Bonding
Use
Key vocabulary
Example polymers
Polymer formula
Chemistry
Carbo-hydrates
C1H2O1
Monosaccharides Or
simple sugars
Glucose,
Fructose, Ribose
Covalent
COH to COH producing
-C-O-C-
bonds
Short term energy from
Cellular respiration
Disaccharides,
Polysaccharides
Amylose or Plant Starch,
Glycogen,
Cellulose
(C1H2O1)n – (H2O)n-1
Dehydration synthesis and
Hydrolysis
Enzymes =
-ase
Lipids
CHO (P)
Glycerol and fatty acids
Glycerol and
Essential fatty acids such as linoleic acid and alpha linoleic acid
COH to COOH or
POOH
producing
COOC or
COOP bonds
Long term energy storage,
Insulation,
Cushioning
Low density lipids LDL
High density Lipids HDL
Saturated, unsaturated, polyunsaturated fatty acids
Cholesterol
Triglycerides,
Steroids, Waxes
Phospholipids
Proteins
CHON (S)
Amino Acids
20 essential amino acids , groups acidic, basic, neutral, and rings
COH to NH2 producing C-N bond
Energy use, enzymes, Transport, cell markers, muscle
Dipeptides,
Polypeptides,
Enzymes, Transport proteins, Hormones
Linear proteins, globular proteins
(Aa)n – (H2O)n-1
Nucleic Acids
CHONP
Nucleotides
Adenine, Thymine Guanine
Cytosine
Uracil
Covalent COC
COOP and
Hydrogen bonds
Making DNA and RNA, information storage
Double Helix,
Genes, Genomes,
Ribosomes
DNA, mRNA tRNA, rRNA, and other RNA’s NA