1. Chapter 2
Chemistry of Life

2. Outline
Basic Chemistry
Atoms
Molecules and Compounds
Chemical Reactions
Properties of Water
Acids and Bases
Macromolecules
ATP

3. Basic Chemistry
There are 92 naturally-occurring elements.
Over 90% of human body is composed of four elements. (CHON)
Carbon.
Hydrogen.
Oxygen.
Nitrogen.

4. Atoms
An atom is the smallest unit of matter that retains an element’s physical and chemical properties.
Positively-charged protons and neutral neutrons are located in the nucleus.
Negatively-charged electrons orbit the nucleus in shells.

5. Atoms
An element’s atomic number is designated by its number of protons.
An element’s atomic weight is designated by its protons and neutrons.

6. Elements and Atoms

7. Molecules and Compounds
A molecule and compound is a group of atoms bonded together.

8. Ionic Reactions
During an ionic reaction, atoms give up or take on an electron to stabilize their outer shells of the atom.
Ions are particles that carry a positive (+) or negative (-) charge.
The attraction between oppositely charged sodium ions and chloride ions forms an ionic bond.

9. Ionic “electron stripping” Reaction

10. Covalent “electron sharing” Reactions
In covalent reactions, atoms share electrons in covalent bonds instead of losing or gaining them.
A single bond is formed when atoms share a single pair of electrons.
A double bond is formed when atoms share two pairs of electrons.
A triple bond is formed when atoms share three pairs of electrons.

11. Covalent Reactions

12. Water and Living Things and a Third type of bond- Hydrogen bond
The electrons in water spend more time circling the larger oxygen atom than the smaller hydrogen atom.
Water is a polar molecule with the oxygen end being slightly negative and the hydrogen end being slightly positive.
A hydrogen bond occurs when a covalently bonded hydrogen is positive and is attracted to a negatively charged atom.

13. Hydrogen Bonding between Water Molecules

14. Some Properties of Water
liquid at room temperature.
solvent for polar molecules.
cohesive.
temperature rises and falls slowly.

16. Acids and Bases
Acids break down in water and release hydrogen ions (H+).
Bases/alkaline take up hydrogen ions (H+) or release hydroxide ions (OH-).
Buffers help keep the pH within normal limits by taking up excess hydrogen ions or hydroxide ions.

17. Water can break down to form Ions (atoms with a + or – charge)
Fig. 2.p022a

18. pH Scale
The pH scale measures acidity or alkalinity of a solution.
Neutral = 7.
Acidic < 7.
Basic > 7.
Logarithmic Scale.

19. Log scale
Fig. 2.p022b

20. The pH Scale

21. Molecules of Life
Four categories of molecules are unique to cells.
Carbohydrates.
Lipids.
Proteins.
Nucleic Acids.
Macromolecules are synthesized by a dehydration reaction, and degraded by a hydrolysis reaction.

22. pg.24a
Fig. 2.p024a

23. Fig. 2.9

24. Synthesis of larger product (macromolecule)
Fig. 2.9a

25. Breakdown of Molecule to simpler subunits
Fig. 2.9b

26. Carbohydrates
Carbohydrates function for quick and short-term energy storage.
Monosaccharide (simple sugar).
Glucose.
Disaccharide.
Fructose.

27. Complex Carbohydrates
Polysaccharides.
Starch (plants).
Glycogen (animals).
Cellulose (plant cell walls).

28. Glucose molecule in various forms
Fig. 2.p024b

29. A Disacharride
Fig. 2.p025

30. Plant Polysaccharide
Fig. 2.11

31. Animal polysaccharide
Fig. 2.12

32. Lipids
Lipids contain more energy per gram than any other biological molecule.
Do not dissolve in water.
Absence of polar groups.
Fats.
Animal origin, solid at room temperature.
Oils.
Plant origin, liquid at room temperature.

33. Synthesis and breakdown of Fat
Fig. 2.13

34. Phospholipids and Steroids
Phospholipids contain a phosphate head and fatty acid tails.
Polar head and non-polar tails.
Soluble in water.
Steroids are lipids with a backbone of four fused carbon rings.
Estrogen and testosterone.

35. Another Example of a lipid
Fig. 2.14

36. Cell membrane
Fig. 2.14c

37. Other lipid examples
Fig. 2.15ab

38. Fig. 2.15bb
Fig. 2.15bb

39. Emulsyfier
Bile salts
Tween

40. Emulsyfication
Fig. 2.p026

41. Proteins
Proteins are macromolecules with amino acid subunits.
An amino acid has a central carbon atom bonded to a hydrogen and three groups.
Peptide bond - Any bond joining two amino acids.
Polypeptide - Single amino acid chain.

42. Building block of proteins
Fig. 2.p028a

43. Fig. 2.16a
Fig. 2.16a

44. Peptide bond- bond between two amino acids
Fig. 2.p028b

45. Levels of Protein Organization
Primary Structure.
Linear sequence of amino acids.
Secondary Structure.
Polypeptide takes on orientation in space.
Tertiary Structure.
Final three-dimensional shape.
Quaternary Structure.
Proteins with more than one polypeptide.

46. Fig. 2.16b

47. Nucleic Acids
Nucleic acids are huge macromolecules composed of nucleotides.
A nucleotide is constructed of a phosphate, a pentose sugar, and a nitrogenous base.
Deoxyribonucleic acid (DNA).
Double-stranded helix.
Ribonucleic acid (RNA).
Single stranded.

48. Building block of an Nucleic Acid- A Nucleotide
Fig. 2.p031

49. DNA Structure

50. (ATP) Adenosine Triphosphate
ATP is the primary cellular energy carrier.
Energy currency of cells.
Breaks down to adenosine diphosphate (ADP) and a molecule of inorganic phosphate, releasing energy to drive cellular metabolism.

51. Another nucleic acid example- ATP and ADP (cell energy)
Fig. 2.18

52. Lecture Review Give an example of ionic bonding and explain it.
Give an example of covalent bonding and explain it.
Relate the characteristics of water to its polarity and hydrogen bonding.
List the four molecules of life and examples of each.
Fat /triglyceride is composed of______ and ______.
The subunits of Proteins are _______ _______.
List some functions of proteins. What is a polypeptide?
The subunits of Nucleic acids are ____________.