1. CHEMISTRY The Chemical Basis of the Body

2. MATTER Anything that has mass and occupies space Anything that has mass and occupies space Three states: solid - liquid - gas Three states: solid - liquid - gas Made up of chemical building blocks called ELEMENTS Made up of chemical building blocks called ELEMENTS

3. Elements Composed of the same atoms. Composed of the same atoms. Cannot be broken down into simpler substances by ordinary chemical means. Cannot be broken down into simpler substances by ordinary chemical means. 117 Elements (98 occurring naturally). 117 Elements (98 occurring naturally). 26 Elements found in the human body. 26 Elements found in the human body. C, H, O, N - 96% of the human body. C, H, O, N - 96% of the human body. S and P make up 99% of the body. S and P make up 99% of the body.

4. Major Elements in the Body The four major elements in the body are: The four major elements in the body are: C – carbon C – carbon H – hydrogen H – hydrogen O – oxygen O – oxygen N - nitrogen N - nitrogen

6. Atoms The smallest unit of matter that can enter into chemical reactions. The smallest unit of matter that can enter into chemical reactions. Composed of two basic components: Composed of two basic components: –Nucleus –Outer energy levels or clouds

7. Structure of an Atom

8. Nucleus Protons (+ charge) Protons (+ charge) # of protons is element’s atomic number Neutrons (uncharged) Neutrons (uncharged) # of protons plus # of neutrons form the element’s atomic weight # of protons plus # of neutrons form the element’s atomic weight

9. Electrons Negatively charged particles that orbit around the nucleus. Negatively charged particles that orbit around the nucleus. # of electrons always equals the # of protons in an atom. # of electrons always equals the # of protons in an atom.

11. Atoms

12. Ions (Electrolytes) Most atoms have too many or too few electrons in their outermost energy level which is not complete. Most atoms have too many or too few electrons in their outermost energy level which is not complete. Valance is the number of extra or deficient electrons in outermost orbital. Valance is the number of extra or deficient electrons in outermost orbital. Anions - extra electrons in outermost orbital which creates a net negative charge. Anions - extra electrons in outermost orbital which creates a net negative charge. Cation - deficient electrons in outermost orbital which creates a net positive charge. Cation - deficient electrons in outermost orbital which creates a net positive charge. Electrolytes - ions in solution Electrolytes - ions in solution

13. Anions and Cations Anions Anions An anion is formed when an atom gains an electron or electrons from another atom creating an overall negative charge. Example: Cl - An anion is formed when an atom gains an electron or electrons from another atom creating an overall negative charge. Example: Cl -

14. Cations Cations Cations are formed when an atom loses an electron or electrons to another atom creating an overall positive charge. Cations are formed when an atom loses an electron or electrons to another atom creating an overall positive charge. Example: Na + Example: Na +

15. Molecules The combination of two or more elements in a chemical reaction. The combination of two or more elements in a chemical reaction. –May be atoms of the same element H 2, O 2, N 2, etc. H 2, O 2, N 2, etc. –May be atoms of different elements NaCl, HCl etc. NaCl, HCl etc.

16. Molecule Examples

17. Compounds A substance that can be broken down into two or more elements by chemical means. A substance that can be broken down into two or more elements by chemical means. Molecules of a compound always contain atoms of two or more different elements. Molecules of a compound always contain atoms of two or more different elements. ***All compounds are molecules but not all molecules are compounds*** ***All compounds are molecules but not all molecules are compounds***

18. Chemical Bonding Chemical bonds are formed between atoms when electrons in the outermost orbital are gained, lost, or shared

19. Types of Chemical Bonds Ionic Bonding Ionic Bonding Covalent Bonding Covalent Bonding Hydrogen Bonding Hydrogen Bonding

20. Ionic Bonding Bonding when one atom gains an electron and another atom loses an electron. Bonding when one atom gains an electron and another atom loses an electron. Transfer electrons from one atom to another. Transfer electrons from one atom to another. Bonds together two oppositely charged ions. Bonds together two oppositely charged ions. Strongest type of chemical bonding. Strongest type of chemical bonding.

21. Ionic Bond Example

22. Covalent Bonding Sharing of electron pairs by more than one atom Sharing of electron pairs by more than one atom –single covalent bond: share one pair of electrons –double covalent bond: share two pairs of electrons –triple covalent bonds: share three pairs of electrons

23. Hydrogen Bonds A hydrogen atom covalently bonded to another atom. A hydrogen atom covalently bonded to another atom. Very weak bond. Very weak bond. Often serves as a bridge between molecules. Often serves as a bridge between molecules. Many large molecules can contain hundreds of these bonds. Many large molecules can contain hundreds of these bonds.

25. pH pH is the term used to describe the degree of acidity or alkalinity determined by the relative amounts of H+ and OH- found in a solution. pH is the term used to describe the degree of acidity or alkalinity determined by the relative amounts of H+ and OH- found in a solution. Biochemical reactions are extremely sensitive to small changes in the acidity or alkalinity of the environment in which they occur. Biochemical reactions are extremely sensitive to small changes in the acidity or alkalinity of the environment in which they occur.

26. A Acidic, basic, or neutral solutions The pH scale has values ranging from 0-14. It is determined primarily upon the number of hydrogen ions (H+) or hydroxyl ions (OH-) in a solution. The pH scale has values ranging from 0-14. It is determined primarily upon the number of hydrogen ions (H+) or hydroxyl ions (OH-) in a solution. An acidic solution forms hydrogen ions, H+, when in solution. On the pH scale, the numbers are below 7.0. Examples include lemons or HCl with a pH of 2.0, tomatoes with a pH of 4.0 or milk with a pH of 5.0. An acidic solution forms hydrogen ions, H+, when in solution. On the pH scale, the numbers are below 7.0. Examples include lemons or HCl with a pH of 2.0, tomatoes with a pH of 4.0 or milk with a pH of 5.0. A neutral solution has a pH of 7.0. The best example is distilled water. A neutral solution has a pH of 7.0. The best example is distilled water. A basic (or alkaline) solution forms hydroxide ions (OH-) when in solution. The pH scale numbers are above 7.0. Examples include eggs with a pH of 8.0 and drain cleaner with a pH of 13.0. A basic (or alkaline) solution forms hydroxide ions (OH-) when in solution. The pH scale numbers are above 7.0. Examples include eggs with a pH of 8.0 and drain cleaner with a pH of 13.0.

27. Neutral pH and pH of Blood Neutral pH is considered to be 7.0 on the pH scale. This is distilled water which has equal concentrations of H + and OH -. Neutral pH is considered to be 7.0 on the pH scale. This is distilled water which has equal concentrations of H + and OH -. The pH of blood is slightly basic (alkaline) ranging from 7.35 to 7.45. The pH of blood is slightly basic (alkaline) ranging from 7.35 to 7.45.

28. A Acidic, basic, or neutral solutions

29. Acids – Bases - Salts

30. Water Water is the universal solvent which provides an excellent suspension medium for the transport of nutrients and wastes. Water is the universal solvent which provides an excellent suspension medium for the transport of nutrients and wastes. A solvent describes a liquid or gas in which some other material has been dissolved. A solvent describes a liquid or gas in which some other material has been dissolved. The solute is the atom, molecule, or compound that has been dissolved in a solvent. The solute is the atom, molecule, or compound that has been dissolved in a solvent. A solution is the combination of a solute and a solvent. A solution is the combination of a solute and a solvent.

31. Water Participates in or is essential in many chemical reactions Participates in or is essential in many chemical reactions Absorbs and releases heat very slowly Absorbs and releases heat very slowly Important transport medium Important transport medium Functions as a lubricant in various regions of the body Functions as a lubricant in various regions of the body

32. Classification of Chemical Compounds Inorganic Compounds Inorganic Compounds –Small ionically bonded molecules –Generally lack a carbon atom –Vital to normal physiological functioning

33. Inorganic Compounds Water Water Acids Acids Bases Bases Salts Salts

34. Organic Compounds * Contains one or more carbon atoms * Contains hydrogen atoms * Almost exclusively held together by covalent bonds

35. Organic Compounds Carbohydrates (sugars & starches) Carbohydrates (sugars & starches) Lipids (fats) Lipids (fats) Proteins Proteins Nucleic Acids (DNA & RNA) Nucleic Acids (DNA & RNA)

36. Carbohydrates Includes sugars and starches. Includes sugars and starches. Account for about 2% of body mass. Account for about 2% of body mass. Contain C, H, and O molecules in a general formula of (C H 2 O)n. Contain C, H, and O molecules in a general formula of (C H 2 O)n. Functions of carbohydrates: Functions of carbohydrates: –structural units of DNA and RNA –energy source (4.5 kcal/gm) –only energy source for brain and nerve cells

37. Lipids (FATS) Most are insoluble in water. Most are insoluble in water. Most highly concentrated energy source Most highly concentrated energy source (9.2 kcal/gm). (9.2 kcal/gm). Less efficient as a body fuel than carbs. Less efficient as a body fuel than carbs. Made up of C, H, and O in structural units called fatty acids and glycerols (triglycerides). Made up of C, H, and O in structural units called fatty acids and glycerols (triglycerides). Common types include triglycerides, steroids and phospholipids. Common types include triglycerides, steroids and phospholipids.

38. Types of fats Types of fats Types of fats are determined by the types of hydrogen bonds in the molecule. Saturated – each carbon is saturated with hydrogen atoms – solid at room temp. – solid at room temp. - Mostly in meats and dairy products(whole milk, cheese, and butter Monounsaturated – not completely saturated with hydrogen bonds - Olive oil, peanut oil, most nuts and avocados - Reduce risk of heart disease Polyunsaturated – Margarine and vegetable shortening (Increase risk of heart disease)

39. Functions of Lipids - Energy Storage - Energy Storage - Insulation and Protection - Insulation and Protection - Cell Membrane structure - Cell Membrane structure - Helps create hormones like Estrogen and Progesterone - Digestion and absorption of important nutrients & Fat Soluble Vitamins (A,D,E, & K)

40. Fat Molecules

41. Phospholipid Molecule

42. Proteins All contain C, H, O, and N (many also contain S and P). All contain C, H, O, and N (many also contain S and P). Composed of molecules called amino acids (20). Composed of molecules called amino acids (20). Type of protein is determined by the number and sequence of amino acids. Type of protein is determined by the number and sequence of amino acids. Amino acids are joined together at the N atoms in a chemical bond called a peptide bond Amino acids are joined together at the N atoms in a chemical bond called a peptide bond

43. Amino Acids

44. Protein Structure

45. Types and Functions of Proteins Structural Proteins Structural Proteins –Form the structural framework of various body parts (muscle, skin, hair, nails, etc.) Regulatory Proteins Regulatory Proteins –Function as hormones to control a variety of physiological processes (insulin) Contractile Proteins Contractile Proteins –Serve as the contractile elements in muscle tissue (actin and myosin)

46. Types and Functions of Proteins Immunological Proteins Immunological Proteins –Serve as anti-bodies to protect the body (gamma globulin) Transport Proteins Transport Proteins –Transports vital substances throughout the body (hemoglobin) Enzymatic Proteins Enzymatic Proteins –Alter the rate or activation energy of chemical reactions (amylase, lipase, lactase)

47. Enzyme Function

48. Nucleic Acids (Structure) Nucleic Acids include DNA (deoxyribonucleic acid) and RNA (ribonucleic acid). Nucleic Acids include DNA (deoxyribonucleic acid) and RNA (ribonucleic acid). Contain the atoms C, H, O, N, and P. Contain the atoms C, H, O, N, and P. Nucleic acids are composed of structural units called nucleotides. A nucleotide is formed by a sugar ( deoxyribose or ribose ), a phosphate, and a nitrogen base. Nucleic acids are composed of structural units called nucleotides. A nucleotide is formed by a sugar ( deoxyribose or ribose ), a phosphate, and a nitrogen base.

49. Nucleic Acids (Function) DNA stores the genetic code within structures called chromosomes. They are found within the nucleus of the cell. DNA stores the genetic code within structures called chromosomes. They are found within the nucleus of the cell. DNA and RNA assist with protein synthesis. DNA and RNA assist with protein synthesis. RNA is responsible for transporting the genetic code from the DNA in the nucleus to the ribosomes where the needed proteins are synthesized by bonding the appropriate amino acids together. RNA is responsible for transporting the genetic code from the DNA in the nucleus to the ribosomes where the needed proteins are synthesized by bonding the appropriate amino acids together.

50. DNA (Deoxyribonucleic Acid) Formed by a double helix of nucleotides. Formed by a double helix of nucleotides. The sides of the double helix contain a phosphate group which alternates with the deoxyribose forming the sides of the helices. The sides of the double helix contain a phosphate group which alternates with the deoxyribose forming the sides of the helices. The sugar is deoxyribose. The nitrogen base is attached to the deoxyribose. Forms the sides of the helices. The sugar is deoxyribose. The nitrogen base is attached to the deoxyribose. Forms the sides of the helices. The nitrogen bases form the rungs of the DNA molecule. The nitrogen bases form the rungs of the DNA molecule. The four nitrogen bases found in DNA include: The four nitrogen bases found in DNA include: adenine (A) adenine (A) thymine (T) thymine (T) cytosine (C) guanine (G) Nitrogen bases are paired together (A-T) and (C-G)(Apple-Tree, Chewing- Gum). Nitrogen bases are paired together (A-T) and (C-G)(Apple-Tree, Chewing- Gum).

51. Structure of DNA

52. RNA Ribonucleic Acid Molecule is a single strand of nucleotides. Molecule is a single strand of nucleotides. The sugar portion of the molecule is a pentose sugar, ribose. The sugar portion of the molecule is a pentose sugar, ribose. Nitrogen base thymine in DNA is replaced by uracil in RNA. Nitrogen base thymine in DNA is replaced by uracil in RNA.

53. Adenosine Triphosphate (ATP) High energy compound that supplies energy for most chemical reactions. High energy compound that supplies energy for most chemical reactions. Found in all living systems. Found in all living systems. Formed during a process called cellular respiration which takes place in the cytoplasm and the mitochondria of cells. Formed during a process called cellular respiration which takes place in the cytoplasm and the mitochondria of cells.

54. Structure of ATP Adenine unit composed of an adenine molecule and a five carbon sugar (ribose). Adenine unit composed of an adenine molecule and a five carbon sugar (ribose). Three phosphate groups attached to the end of the molecule. Three phosphate groups attached to the end of the molecule. Tremendous amount of energy is released when the terminal phosphate is removed. Tremendous amount of energy is released when the terminal phosphate is removed.

55. Structure of ATP

56. ATP ADP + P + ENERGY