1. Basic Chemistry
Chapter 2

2. Introduction
Since chemicals compose the body, & the sum of the chemical reactions that takes place in the body is called metabolism, it is important to be familiar with basic chemistry.

3. Anything that has mass & occupies space
Matter
Energy
Capacity to do work
2 Types – kinetic (motion) & potential (stored)
4 Forms the body uses – Chemical – stored in bonds of chemicals - food
Electrical – movement of charged particles – ions
Mechanical – moving matter - muscles
Radiant – travels in waves – EM spectrum
Anything that has mass & occupies space
3 States – solid, liquid, gas

4. 112 elements are known with certainty.
A chemical element is a pure substance that consists entirely of one type of atom.
112 elements are known with certainty.
96% of the mass of a human is made up of Carbon, Hydrogen, Oxygen, and Nitrogen.
Copyright Pearson Prentice Hall

5. The study of chemistry begins with the basic unit of matter, the atom.
Atoms
The study of chemistry begins with the basic unit of matter, the atom.
Copyright Pearson Prentice Hall

6. The subatomic particles that make up atoms are Protons (+)
Neutrons (0)
Electrons (-)
Electrons
Copyright Pearson Prentice Hall
Protons and Neutrons

7. The number of protons in an atom of an element is the element's atomic number
Copyright Pearson Prentice Hall

8. Mass number is the number of protons and neutrons in the nucleus of an atom

9. Atoms of the same element that differ in the number of neutrons they contain are known as isotopes.
Copyright Pearson Prentice Hall

10. Because they have the same number of electrons, all isotopes of an element have the same chemical properties.
Copyright Pearson Prentice Hall

11. Radioisotopes Isotopes that exhibit radioactive behavior
Used to tag biological molecules so that they can be traced through the body for medical diagnosis and treatment
Xrays, Nuclear Medicine, PET Scans, CT Scans, MRI

12. Molecules Compounds two or more atoms held together by chemical bonds.
H (atom) + H (atom) → H2 (molecule)
two or more different elements, the atoms of which are chemically united
4H + C = CH4 (methane)

13. Chemical Bonds
The atoms in compounds are held together by chemical bonds.
The electrons that are available to form bonds are called valence electrons.
Copyright Pearson Prentice Hall

14. The main types of chemical bonds are: ionic bonds covalent bonds
Copyright Pearson Prentice Hall

15. Ionic Bonds
An ionic bond is formed when one or more electrons are transferred from one atom to another.
These positively and negatively charged atoms are known as ions.
Ionic bonds are common in salts.
Copyright Pearson Prentice Hall

16. A covalent bond forms when electrons are shared between atoms.
single covalent bond
double bond
triple bond
Copyright Pearson Prentice Hall

17. Hydrogen Bonds
Weak bonds that bind water molecules or different parts of the same molecule. They are common in large, complex organic molecules (proteins & nucleic acids).
Copyright Pearson Prentice Hall

18. Patterns of Chemical Reactions
Synthesis – A+B = AB; Two or more atoms form a larger atom
Decomposition - AB→ A+B; Molecules are broken down
Exchange – AB + C →AC + B; A switch is made

19. Factors Increasing the Rate of Reactions
Increase Temperature
Increase Concentration of reacting particles
Decrease particle size
Presence of Catalyst

20. Biochemistry Inorganic Lack Carbon Small, simple molecules
Ex: Water, Salts, Acids, Bases
Organic
Have Carbon
Fairly large, covalently boned molecules
Carbohydrates, Lipids, Proteins, Nucleic Acids

21. Water Most abundant inorganic compound in the body
Accounts for about two-thirds of body weight
Properties
High heat capacity
Polarity/solvent properties
Chemical reactivity
Cushioning

22. Salts
Ionic compound that dissociates into charged particles (other than hydrogen or hydroxyl ions) when dissolved in water
Called electrolytes
Vital to body functioning

23. Acids, Bases, and pH
A water molecule is neutral, but can react to form hydrogen and hydroxide ions.
H2O   H+ + OH-
pH – measure of how acidic or basic a solution is
Copyright Pearson Prentice Hall

24. Acids and Bases Like salts, acids and bases are electrolytes.
That is, they ionize and then dissociate in water and can then conduct an electrical current.

25. The pH scale 
Chemists devised a measurement system called the pH scale to indicate the concentration of H+ ions in solution.
The pH scale ranges from 0 to 14.
Copyright Pearson Prentice Hall

26. Acid below 7; more H+ than OH- Base above 7; less H+ than OH-
The pH Scale
At a pH of 7, the concentration of H+ ions and OH- ions is equal - Neutral
Acid below 7; more H+ than OH-
Base above 7; less H+ than OH-
Copyright Pearson Prentice Hall
The concentration of H+ ions determines whether solutions are acidic or basic.

27. Buffers
Living cells are extraordinarily sensitive to even slight changes in pH; and acid-base balance is carefully regulated by the kidneys, lungs, and a number of chemicals called buffers, which are present in body fluids.
Buffer - a substance or substances that help to stabilize the pH of a solution.

28. Types of Organic Compounds
4 main types of organic compounds are:
Carbohydrates – known as sugars, polar molecules, most dissolve in water
Lipids – fats, nonpolar, do not dissolve in water
Nucleic acids – DNA and RNA
Proteins – amino acids, muscles, enzymes and hair

29. 3 Types of Carbohydrates
Monosaccharide: one simple sugar. Examples are glucose, fructose(fruit sugar), galactose(milk sugar)
The formula for glucose is C6H12O6. Plants use this during photosynthesis

30. 3 Types of Carbohydrates
Disaccharide: two simple sugars joined by a saccharide bond.
Examples are sucrose(table sugar), lactose(milk sugar), and maltose (malt beverage sugar)
Polysaccharide: three or more monosaccharides combined.
Examples are cellulose(cell walls), chitin (exoskeleton), glycogen (stores glucose in liver cells), starch (stores glucose in roots of plants)

31. Lipids Lipids are fats, waxes, phospholipids, and steroids.
Lipids contain carbon, hydrogen and oxygen but have fewer oxygen atoms than carbohydrates
Building blocks are glycerol and three fatty acids.

32. Lipids are used for protection, cushion, structure, insulation, and energy storage.
Fats
Saturated contains the maximum amount of hydrogens – solid at room temperature – animal fats
Unsaturated does not contain maximum amounts of hydrogen so double bonds exists – liquids at room temperature- oils

33. Phospholipids make up cell membranes
Consists of two fatty acids and a phosphate group
Steroids contain a 4-ringed backbone
Examples: cholesterol and steroids (hormones)
Waxes – used to form waterproof coverings on leaves, skin, or fur
Example: beeswax, ear wax

34. Proteins are composed of carbon, hydrogen, oxygen, and nitrogen (sulfur is found in two amino acids)
The building blocks of protein are amino acids held together by a peptide bond.
Proteins

35. Proteins
Function in immunity, building structures, hormones, enzymes, transporting substances
Examples of proteins are antibodies, muscles, ligaments, tendons, and hair.

36. Enzyme Enzymes are made of proteins
Enzymes biological catalysts that enables chemical reactions to take place in the body
End in –ase
Enzymes speed up chemical reactions that take place in cells
Enzyme

37. Nucleic Acids
polymers assembled from individual monomers known as nucleotides.
Copyright Pearson Prentice Hall

38. Nucleic Acids Nucleotides consist of three parts:
a 5-carbon sugar (Carbon, hydrogen, & oxygen)
a phosphate group
a nitrogenous base
adenine, cytosine, guanine, and thymine for DNA and adenine, cytosine, guanine, and uracil for RNA
Copyright Pearson Prentice Hall

39. Nucleic acids store and transmit hereditary, or genetic information.
Examples:
ribonucleic acid (RNA)
deoxyribonucleic acid (DNA)
Copyright Pearson Prentice Hall

40. ATP
a modified nucleotide; it consists of an adenine base, ribose sugar, and three phosphate groups
the universal energy compound used by all cells of the body