CHEMISTRY THE CHEMICAL BASIS OF THE BODY
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1 CHEMISTRY THE CHEMICAL BASIS OF THE BODY
2 MATTER Anything that has mass and occupies space Three states: solid liquid gas Made up of chemical building blocks called ELEMENTS
3 Elements Composed of the same atoms. Cannot be broken down into simpler substances by ordinary chemical means. 109 Elements (92 occurring naturally). 26 Elements found in the human body. C, H, O, N - 96% of the human body.
4 Elements Top Six Elements = 98% of the human body (Oxygen, Carbon, Hydrogen, Nitrogen, Calcium, Phosphorous) Next Six Elements = 0.8% of the human body (Potassium, Sulfur, Sodium, Chloride, Magnesium, Iron) Trace Elements (12) = 0.7% of the human body
5 Yellow Boxes = 5 most abundant elements present in the human body Green Boxes = Next most abundant elements present in the human body Blue Boxes = Trace elements that are required by the human body Violet Boxes = Elements that cause damage to the human body.
6 What are the elements in the human body? Most of the human body is made up of water, H2O, with cells consisting of 65-90% water by weight. Therefore, it isn't surprising that most of a human body's mass is oxygen. Carbon, the basic unit for organic molecules, comes in second. 99% of the mass of the human body is made up of just six elements: oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus. Oxygen (65%) Carbon (18%) Hydrogen (10%) Nitrogen (3%) Calcium (1.5%) Phosphorus (1.0%) Potassium (0.35%) Sulfur (0.25%) Sodium (0.15%) Magnesium (0.05%) Copper, Zinc, Selenium, Molybdenum, Fluorine, Chlorine, Iodine, Manganese, Cobalt, Iron (0.70%) Lithium, Strontium, Aluminum, Silicon, Lead, Vanadium, Arsenic, Bromine (trace amounts)
7 Atoms The smallest unit of matter that can enter into chemical reactions. Composed of two basic components: Nucleus Outer energy levels or clouds
8 Structure of an Atom
9 Nucleus Protons (+ charge) # of protons is element s atomic number Neutrons (uncharged) # of protons plus # of neutrons form the element s atomic weight (or atomic mass)
10 Electrons Negatively charged particles that orbit around the nucleus. # of electrons always equals the # of protons in an atom. Ions are different, we will discuss those later
11 Electron Shells Electrons closest to the nucleus are most strongly attracted Each shell has distinct properties Number of electrons has an upper limit Shells closest to nucleus fill first
12 Atoms
13 Ions (Electrolytes) 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. Anions - extra electrons in outermost orbital which creates a net negative charge. Cation - deficient electrons in outermost orbital which creates a net positive charge. Electrolytes - ions in solution
14 Ions and Ionization Ions -carry a charge due to an unequal number of protons and electrons Ionization = transfer of electrons from one atom to another ( stability of valence shell)
15 Anions and Cations Anions An anion is formed when an atom gains an electron or electrons from another atom creating an overall negative charge. Example: Cl -
16 Cations Cations Cations are formed when an atom loses an electron or electrons to another atom creating an overall positive charge. Example: Na +
17 Molecules 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. May be atoms of different elements NaCl, HCl etc.
18 Atoms vs. Molecules
19 More Molecule Examples
20 Compounds 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. ***All compounds are molecules but not all molecules are compounds***
21 Chemical Bonding CHEMICAL BONDS ARE FORMED BETWEEN ATOMS WHEN ELECTRONS IN THE OUTERMOST ORBITAL (VALENCE) ARE GAINED, LOST, OR SHARED. FULL VALENCE ORBITALS DO NOT FORM BONDS.
22 Chemical Bonds Follow the Octet Rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell in order to become stable
23 Types of Chemical Bonds Ionic Bonding Covalent Bonding Hydrogen Bonding
24 Ionic Bonding Bonding when one atom gains an electron and another atom loses an electron. Transfer electrons from one atom to another. Bonds together two oppositely charged ions. Strongest type of chemical bonding in inorganic compunds
25 Ionic Bond Example
26 Covalent Bonding 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 Strongest chemical bond in organic compounds
27 Properties of Ionic vs. Covalent Bonds
28 Hydrogen Bonds A hydrogen atom covalently bonded to another atom. Very weak bond. Often serves as a bridge between molecules. Many large molecules can contain hundreds of these bonds
29 Review of Ionic and Covalent Bonds
30 Water and Hydrogen Bonding
31 Water Universal solvent Solvent = liquid or gas in which some other material has been dissolved Solute = the atom, molecule, or compound that has been dissolved in a solvent Solution = the combination of a solvent and solute
32 Water Participates in or is essential in many chemical reactions Absorbs and releases heat very slowly Important transport medium Functions as a lubricant in various regions of the body
33 Water Image retrieved from
34 ph Scale MEASURE OF ACIDITY OR ALKALINITY OF A SOLUTION
35 ph Scale Descibes the degree of acidity or alkalinity (basicity) of a solution. Expressed on a logrhythmic base 10 scale that runs from 0-14 with 7 being a neutral ph: > 7 is a basic or alkaline solution < 7 is a acidic solution Actually represents the number of H+ ions or OH- ions in solution.
36 ph Scale
37 Specific Examples
38 Acids A substance that dissociates into one or more hydrogen ions (H+) and one or more negative ions (anions) Acids are proton donors
39 Bases A substance that dissociates into one or more hydroxyl ions (OH-) and one or more positively charged ions (cations) Bases are proton acceptors
40 Salts When you mix a base with an acid you form water and a salt. As a result of our cellular metabolism, our cells produce acids (H+). Acids need to be eliminated from the body. We combine H+ to bicarbonate (HCO 3 ) to form carbonic acid (H 2 CO 3 ) which dissociates to form water and carbon dioxide (CO 2 ), which we then excrete through our lungs! This is one way we can remove H+ from our body.
41 Acids Bases - Salts
42 Buffers A solution that resists changes in ph when acid or alkali is added to it. Buffers typically involve a weak acid or alkali together with one of its salts Buffers stop massive changes in ph levels The main buffer system of the human body is Carbonic Acid-Bicarbonate Buffer
43 Buffers
44 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 -. The ph of blood is slightly basic (alkaline) ranging from 7.35 to 7.45.
45 Classification of Chemical Compounds Inorganic Compounds Small ionic bonded molecules Generally lack a carbon atom If carbon is present, there is no hydrogen Vital to normal physiological functioning Organic Compounds Contains one or more carbon atoms Contains hydrogen atoms Almost exclusively held together by covalent bonds
46 Inorganic Compounds Water Acids Bases Salts
47 Organic Compounds Carbohydrates (sugars & starches) Lipids (fats) Proteins Nucleic Acids (DNA & RNA)
48 Carbohydrates Includes sugars and starches. Account for about 2% of body mass. Contain C, H, and O molecules in a general formula of (C H 2 O). Functions of carbohydrates: structural units of DNA and RNA energy source (4.5 kcal/gm) only energy source for brain and nerve cells
49 Glucose Molecule Storage form of Carbohydrates
50 Lipids (FATS) Most are insoluble in water. Most highly concentrated source of energy (9.2 kcal/gm). Less efficient as a body fuel than carbs. Made up of C, H, and O in structural units called fatty acids and glycerols (triglycerides). Types of fats determined by the types of hydrogen bonds in the molecule saturated fat unsaturated fat (mono or poly)
51 Function of Lipids Insulates Protects body organs Secondary source of energy Cell membranes (phospholipid bilayer)
52 Common lipids in the human body Neutral fats (triglycerides) Found in fat deposits Composed of fatty acids and glycerol Source of stored energy Phospholipids Form cell membranes Steroids Include cholesterol, bile salts, vitamin D, and some hormones
53 Fat Molecules
54 Phospholipid Molecule
55 Proteins All contain C, H, O, and N (many also contain S and P). Composed of molecules called amino acids (20). 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
56 Amino Acids
57 Protein Structure
58 Types and Functions of Proteins Structural Proteins Form the structural framework of various body parts (muscle, skin, hair, nails, etc.) Regulatory Proteins Function as hormones to control a variety of physiological processes (insulin) Contractile Proteins Serve as the contractile elements in muscle tissue (actin and myosin)
59 Types and Functions of Proteins Immunological Proteins Serve as anti-bodies to protect the body (gamma globulin) Transport Proteins Transports vital substances throughout the body (hemoglobin) Enzymatic Proteins Alter the rate or activation energy of chemical reactions (amylase, lipase, lactase)
60 Enzyme Function
61 Nucleic Acids DNA and RNA Building blocks of life All contain C, H, O, N, and P Made up of structural units called nucleotides DNA contains the genetic code DNA and RNA assist with protein synthesis
62 DNA Deoxyribonucleic Acid Nucleotides are molecules composed of C, H, O, and a nitrogen base of: thymine guanine - adenine - cytosine Contains a pentose sugar called deoxyribose Contains a phosphate group
63 Structure of DNA A two stranded molecule that twists around each other (double helix). looks like a twisted ladder Sides or uprights of the ladder are made of alternating phosphates and the deoxyribose section of the molecule. The rungs of the ladder contain the paired nitrogen bases. thymine (T) guanine (G) - adenine (A) - cytosine (C)
64 Structure of DNA
65 RNA Ribonucleic Acid Molecule is a single strand of nucleotides. The sugar portion of the molecule is a pentose sugar, ribose. Nitrogen base thymine in DNA is replaced by uracil in RNA.
66 Adenosine Triphosphate (ATP) High energy compound that supplies energy for most chemical reactions. Found in all living systems. Formed during a process called cellular respiration which takes place in the cytoplasm and the mitochondria of cells.
67 Structure of ATP Adenine unit composed of an adenine molecule and a five carbon sugar (ribose). Three phosphate groups attached to the end of the molecule. Tremendous amount of energy is released when the terminal phosphate is removed.
68 Structure of ATP
69 ATP ADP + P + Energy
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