1. Basic Chemistry
Chapter 2

2. MATTER & ENERGY Matter Anything that occupies space and can be weighed
Chemistry examines the nature of matter
Energy
No mass
Ability to do work
Matter is the substance that is moved by energy

3. Matter Building blocks: solid, liquid, gas
Physical change –nature of substance is unchanged
Chemical change –nature of substance is changed

4. ENERGY No mass We measure the effect of energy on matter
Two types: Kinetic and Potential

5. ENERGY Forms: Chemical -stored within bonds, released as heat
Electrical -movement of charged partials (e-)
Mechanical -direct movement of matter
Radiant -electromagnetic waves
Energy is converted from one form to another, any not used is released as heat.

6. COMPOSITION OF MATTER Elements Atoms Opposites attract!
Protons (p+) –positive charge
Neutrons(n0) –neutral or no charge
Electrons (e-) –negative charge
Opposites attract!

7. ELEMENTS OF THE HUMAN BODY

8. ATOMS Orbital Model –electron cloud Atomic number –number of protons
Atomic mass –sum of all protons and neutrons
Isotopes –vary in number of neutrons
Radioisotopes –radioactivity, heavy isotopes

9. CHEMICAL BONDS & REACTIONS
Molecules, Compounds, Reactions, OH MY!
Molecules =same
Compounds =different
Reactions =associations or dissociations of atoms
Bonds form between molecules and compounds
Energy relationships

10. CHEMICAL BONDS Bonds are energy relationships
Opposites attract while “like” or same repels
Role of electrons
Occupy fixed regions called electron shells or energy levels
Valence shell electrons participate in bonds

11. ENERGY LEVELS

12. ENERGY LEVELS Valence Shells (energy levels) Outer shell
If fewer than 8 electrons will try to: share, gain, lose

13. ENERGY LEVELS

14. CHEMICAL BONDS Ionic –one atom gains electron and second loses
Covalent –electrons are shared between atoms
Hydrogen –form bridge between two electrically negative atoms

15. CHEMICAL REACTIONS Synthesis –larger molecule formed
Decomposition –larger molecule is degraded
Exchange –synthesis and decomposition; switch

16. BIOCHEMISTRY Inorganic compounds do not contain carbon atoms
Water, salts (electrolytes), acids and bases
Organic compounds contain carbon atoms
Carbohydrates, lipids, proteins and nucleic acids

17. INORGANIC COMPOUNDS
Water –thermoregulatory, universal solvent, reactivity, cushioning, lubrication
Salts –cations other than H+, electrolytes
Acids –H+, proton donors
Bases –OH-, proton acceptors
pH –concentration of acid; [protons]
pH 7 =1 x 10-7 pH2 =1 x 10-2 pH12 =1 x 10-12

18. pH 7 =1 x 10-7=
pH6 =1 x 10-6 =
pH1 =1 x 10-1 =0.1
pH14 =1 x =

19. ORGANIC COMPOUNDS Large, complex molecules
Functional groups are reactive parts
Monomers combine to form polymers
Carbohydrates, Lipids, Proteins, Nucleic Acids, ATP

20. CARBOHYDRATES “Hydrated Carbon” Monosaccharides are building blocks
Disaccharides –double sugars
Polysaccharides –branching chains

21. LIPIDS More carbon & hydrogen than oxygen Insoluble in water
Saturated or unsaturated
Triglycerides –fatty acids + glycerol
Phospholipids –contain phosphorus
Steroids –flat with interlocking rings

23. PROTEINS Amino acids are building blocks
Amine + acid group + functional group (R)
Most are complex in structure
Tertiary
Primary
Secondary

24. PROTEINS Fibrous or Globular Function depends on shape
Enzymes (end in –ase)

25. NUCLEIC ACIDS Building blocks are nucleotides Code for genes
5 types: adenine, guanine, cytosine, thyamine, uracil
Deoxyribonucleic Acid (DNA) & Ribonucleic Acid (RNA)

26. ADENOSINE TRIPHOSPHATE
Chemical energy
Adenine base + ribose sugar + 3 phosphates
Phosphate bonds are high energy