BASIC CHEMISTRY / BIOCHEMISTRY

1. BASIC CHEMISTRY / BIOCHEMISTRY Reference: Chapter 2 of text THE CHEMISTRY OF LIFE

2. BASIC CHEMISTRY

3. MEET THE ELEMENTS

4. ATOMIC THEORY OF MATTER(vocabulary) • Atoms = building blocks of matter that cannot be divided any further by ordinary chemical means • Molecule = two or more atoms combined that act as a single particle, the smallest particle that retains the properties • Elements = substances made of only one kind of atom

5. ATOMIC THEORY OF MATTER(vocabulary) • Compounds = two or more kinds of atoms in a substance in definite proportions • Isotopes = varieties in the normal number of neutrons on the nucleus (The atomic number stays the same, the mass number changes) • Radioactivity = a nuclear process in which an atom is undergoing changes by emitting charged particles

6. STRUCTURE OF THE ATOM particle charge mass location proton (+) 1 amu in nucleus electron (-) 0 in orbitals neutron ( ) 1 amu in nucleus A “Happy Atom” has all its orbital places filled. • Atomic number = # of protons (also the number of electrons in a neutral atom) • Atomic mass or mass number = number of protons plus the number of neutrons in the nucleus.

7. ATOMIC ORBITALS(energy levels) Level 1 2 electrons orbit nucleus Level 2 8 electrons orbit Level 3 8 electrons orbit Remember: A “Happy Atom” has all its orbital places filled.

8. CHEMICAL BONDING 1. Chemical bond = force of attraction that holds atoms together There are two kinds of bonds between atoms • Covalent Bonds = chemical bond that is formed by the sharing of electrons • Ionic Bonds = chemical bond that is formed by transfer of electrons

9. COVALENT BOND HYDROGEN ATOM HYDROGEN ATOM OXYGEN ATOM Covalent Bond = chemical bond that is formed by the sharing of electrons (covalent bonds form molecules) Remember: A “Happy Atom” has all its orbital places filled.

10. IONIC BOND Ionic bond = chemical bond that is formed by transfer of electrons Remember: A “Happy Atom” has all its orbital places filled Sodium (Na) has 1 electron in its outer energy level – is it happy? Chlorine (Cl) has 7 electron in its outer energy level – is it happy?

11. IONIC BOND Sodium and Chlorine ions are formed – What is an ion? 2. Ion = atom with an excess charge by the loss or gain of electrons Sodium has lost one electron (one less (–) charge) so it now has a net charge of +1 Na Cl Na Cl Chlorine has gained one electron (one more (–) charge) so it now has a net charge of -1 The (+) charge of Na is attracted to the (-) of the Cl and this attraction forms an ionic bond!

12. CHEMICAL FORMULAS Each elements (symbol) and its proportions (subscripts) are represented information All elements are listed in the periodic table • 6 atoms of Carbon (C) • 12 atoms of hydrogen (H) • 6 atoms of oxygen (O) For example C6H12O6means:

13. CHEMICAL FORMULAS Examples are: H2O CO2 C6H12O6 CH4

14. STRUCTURAL FORMULAS 4. A Structural formulashows the kinds and number of atoms as well as the chemical bonds glucose H H C C H O acetylene H water benzene

15. CHEMICAL EQUATIONS 5. Reactants = the original substances before a chemical reaction (left of the arrow) 6. Products = new substances formed after a chemical reaction (right of the arrow)

16. 7. Law of Conservation of Mass= mass can neither be created or destroyed (chemical reaction formulas must balance) + 2 molecules of hydrogen (2H2) + 1 molecule of oxygen (O2) 2 molecules of water (2H2O)

17. Complete pages 6 and 7 in your packet

18. BIOCHEMISTRYThe Chemical Compounds of Life

19. BIOLOGICALLY IMPORTANT COMPOUNDS ORGANIC COMPOUNDS: • Species that naturally contain carbon and hydrogen (living organisms and their products) • Most also contain O (oxygen) and N (nitrogen) • Only a few elements are found in organic compounds • May also have P (phosphorous), S (sulfur), Fe (iron), Ca (calcium), Na (sodium), Cl (chlorine), Mg (magnesium), K (potassium)

20. BIOLOGICALLY IMPORTANT COMPOUNDS INORGANIC COMPOUNDS: • DO NOT CONTAIN CARBON (with hydrogen) • May have carbonate compounds (CO2, CaCO, etc.) but not carbon with hydrogen. • Living organisms do contain inorganic compounds

21. IMPORTANT INORGANIC COMPOUNDS • WATER • The most important inorganic compound in living organisms • 65% of the body • Many biological processes require water • SALTS • Help maintain water balance in the cells • Provide ions for many biological processes • ACIDS and BASES • Help maintain homeostasis

22. The Structure of Organic Compounds • Organic compounds are large and complex because of the carbon atom • Four vacancies for electrons allow 4 covalent bonds Carbon has an atomic # of 6 which means it has 6 protons and 6 electrons It has 4 vacancies in the outer energy level 2. 1. 6 + 3. 4.

23. CHEMICAL COMPOUNDS OF LIFE Living organisms depend upon a variety of molecules for their survival. Some are used to build complex parts of an organism; some supply energy; while others provide instructions for the operation of the organism. There are many organic compounds found in organisms, but they can be classified into 4 main types: • CARBOHYDRATES • LIPIDS • NUCLEIC ACIDS • PROTEINS

24. CARBOHYDRATES • Carbohydrates are compounds of C (carbon), H (hydrogen), and O (oxygen) • They have the same ratio H:O as in water (H2O) = 2:1 (twice as many H as O) • Monosaccharides = simple sugars = C6H12O6 • ALWAYS END IN “OSE” EX: MALTOSE, FRUCTOSE, GLUCOSE • RELEASE ENERGY WHEN BREAKING DOWN GLUCOSE INTO CO2 AND H2O • C6H12O2 CO2 + H2O • MOST ORGANISMS USE GLUCOSE AS A SOURCE OF ENERGY

25. CARBOHYDRATES THIS IS A MONOSACCHARIDE MOLECULE! THIS IS A SIMPLE SUGAR! THIS IS GLUCOSE! THIS IS C6H12O6 !

26. CARBOHYDRATES DISACCHARIDE = two simple sugars joined POLYSACCHARIDE = several simple sugars joined POLYMERS = long chains of repeating molecules (many) (molecules)

27. CARBOHYDRATES Sugars stored in plants are called STARCH Sugars stored in the liver of animals are called GLYCOGEN Glycogen will be changed into glucose when the body needs it for energy!

28. CARBOHYDRATES BUILDING BLOCKS OF CARBOHYDRATES ARE SIMPLE SUGARS OR MONOSACCHARIDES

29. LIPIDS(fats, oils, and waxes) • Made of carbon, oxygen, and hydrogen (there is less oxygen in lipids than in carbohydrates) • Reserve energy supply in an organism 2 times as much energy as carbohydrates • Plants store oils in seeds • Mammals store fats under the skin • Waxes are formed from fatty acids and substances similar to glycerol • Fats and oils are formed from fatty acids and glycerol

30. LIPIDS(fats, oils, and waxes) BUILDING BLOCKS of LIPIDS (fats and oils) ARE 1 GLYCEROL + 3 FATTY ACIDS

31. The Structure of a Fatty Acid Lipid molecule The Fatty Acid has 2 parts: Chain of carbon atoms with hydrogen atoms bonded (hydrocarbon chain) Carboxyl group

32. SATURATED vs UNSATURATED FATTY ACIDS • SATURATED FATTY ACIDS: • Fats that have all single carbon-to-carbon bonds • Tend to be solids at room temperature (ie. butter) • Tend to increase the amount of cholesterol in the body • Cause deposits that lead to hardening and narrowing of arteries

33. SATURATED vs UNSATURATED FATTY ACIDS • UNSATURATED FATS • Fats that have a double or triple carbon-to-carbon bond • Tend to be oils at room temperature • Tend to decrease blood cholesterol • Polyunsaturated fats = a chain that has more than one double or triple bond

34. Complete the crossword puzzle on page 11 in your packet

35. NUCLEIC ACIDS • Compounds that contain phosphorus (P) and nitrogen (N) • Also carbon, hydrogen, and oxygen Two types of Nucleic Acids: • DNA • RNA

36. NUCLEIC ACIDS(DNA) DNA = deoxyribonucleic acid • Found in the nucleus of the cell • Directs and controls heredity information and the development and activities of the cell

37. THE STRUCTURE OF DNA DNA is made of: Repeated chains of nucleotides Nucleotides are made of: • 5 carbon sugar (deoxyribose) • Phosphate group (PO4) • Nitrogenous base (A,T,C,G)

38. THE STRUCTURE OF DNA DNA • The DNA molecule is made of repeating chains of nucleotides • The sugar and phosphate groups are the sides of the ladder • Nitrogenous base pairs are the rungs of the ladder • The bases are adenine (A), thymine (T), cytosine (C), and guanine (G) • adenine (A) always pairs with thymine (T) • cytosine (C) always pairs with Guanine (G)

39. RNA RNA = ribonucleic acid RNA structure: • A single strand or chain of bases • The sugar is ribose • The base thymine is replaced with uracil • RNA is involved with protein synthesis

40. PROTEINS • Compounds that contain nitrogen, carbon, hydrogen, and oxygen • Many contain sulfur and phosphorus • Great range of properties that give life complexity • 20 different amino acids found in proteins AMINO ACIDS ARE THE BUILDING BLOCKS OF PROTEINS

41. STRUCTURE OF AN AMINO ACID • One central carbon atom (C) • One carboxyl group (COOH) • One amino group (NH3) • One hydrogen atom (H) • One side chain (R) GLYCINE is the simplest amino acid – the side chain is only one H atom

42. Examples of the different amino acids

43. PROTEIN VOCABULARY Dipeptide = two amino acids bonded together The peptide bond = the bond between amino acids Polypeptide = a long chain of amino acids

48. Complete page 15 in your packet

49. DEHYDRATION SYNTHESIS DEHYDRATION = to remove water SYNTHESIS = to make more complex H and OH are removed from the glucose molecules (to make water), this is the dehydration part Then the two glucose molecules have open bonding sites so they can join together to make more complex, this is the synthesis part. Dehydration synthesis = to make more complex by removing water

50. HYDROLYSIS To break down by adding water