2 Basic Chemistry

Power Point Assignment For all the items marked with an * fill in the indicated information using Chapter 2 information. Do not look up these items in the glossary. The professor will not necessarily review these items so it is critical to your understanding of the material that you complete these notes on your power point. It is a good idea to download and print the powerpoint out and bring it to class.

I. Introduction A. Matter and Energy 1. Matter:* Define 2. Energy:* Define a. Chemical b. Electrical c. Mechanical d. Radiant

B. Composition of Matter 1. Elements:* Define 96 percent of the body = four elements C * What does this letter stand for? O * What does this letter stand for? H * What does this letter stand for? N * What does this letter stand for? 2. Atoms—building blocks of elements

3. Subatomic Particles a. Nucleus *Where is it and what does it contain Protons * Charge & location: Neutrons * Charge & location: b. Electrons: Orbiting the nucleus Electrons * Size, Charge & Location c. Atomic Number = Number of protons (equals numbers of electrons) in an atom; different for each d. Atomic mass number: Helium atom e- e- Proton Neutron

How many protons, neutrons, and electrons does Hydrogen normally have? Helium? Lithium? Figure 2.2

4. Isotopes Isotopes = Atoms of an element vary in the number of ______________ Isotopes have the same number of? Atomic Weight of Isotopes

Radioactivity Radioisotope = Stability? Decomposes: Radioactivity: Examples: Uranium, Iodine, …

5. IONS = Positive & Negative Ions Properties as compared to atoms: Table Salt

Ions Examples… Cl ¯1 ion or Cl ¯ ion A Chlorine Atom gains an electron from another atom Cl ¯1 ion or Cl ¯ ion

Properties of atoms compared to their ions … Figure 2.4

C. Making Larger Chemicals out of the Atoms or Elements 1 C. Making Larger Chemicals out of the Atoms or Elements 1. Chemical Formulas 2. Molecules and Compounds Molecule—two or more atoms, of the same or different elements, combined chemically H2O O2 NaCl b. Compound—two or more atoms of different elements combined chemically

One CHEMICAL BOND = ____ electrons 3. Chemical Bonds Bonding involves interactions between electrons in outer part of 2 atoms One CHEMICAL BOND = ____ electrons a. Ionic Bonds (Electrovalent Bonds) Bond Formed When: Example: SALT Na atom Cl atom Na+ Cl ¯

b. Covalent Bonds i) Bonds occurs when: ii) Types Non Polar—electrons are:

The Oxygen: Polar Covalent Bonds Bond– electrons are: Example: WATER The Hydrogens: Polarity Polar Molecule Attraction between Polar Molecules -1/2 Oxygen +1/2 +1/2 2 Hydrogens -1/2 Figure 2.8 +1/2 +1/2

Polar Molecules … Example: Attraction between Water Molecules -- creates surface tension Hydrogen Bonds Figure 2.9

D. Chemical Reactions c. Process of making Products a. Reactants = b. Products = c. Process of making Products Bonds broken in ______________ Atoms rearranged New bonds in _______________ H2O + CO2 ---> H2CO3 Reactants ---> Products

2. Types of Chemical Reactions a. Synthesis reaction = Example: Synthesis of Proteins

b. Decomposition Reactions = Example: Glycogen is broken down into ______

c. Exchange reaction: Parts moved around Example:

E. SOLUTIONS SOLUTION = a mixture of chemicals in a liquid - AQUEOUS SOLUTIONS = the liquid is WATER 1. Solvent: the liquid 2. Solute: the dissolved chemicals 3. The Concentration of a Solution: can use percentages % Solvent + % Solutes = 100%

4. Movement of chemicals in Solutions a. Diffusion: b. Osmosis: water solute

II. Biochemistry: Essentials for Life TWO TYPES Organic Inorganic A. Inorganic compounds No “C” framework simpler Examples

Inorganic Compounds … Water -- STUDENTS READ IN TEXT 2. Salts ions Vital some conduct electrical currents Examples:

+ H – O H + Na+ Na+ Cl– Cl– Salt crystal Ions in solution Water molecule Na+ Na+ Cl– Cl– Salt crystal Ions in solution Figure 2.11

Release ______________ (H+) 4. Bases Release hydroxyl ions (OH–) Inorganic Compounds … 3. Acids Release ______________ (H+) 4. Bases Release hydroxyl ions (OH–) Are ______________ acceptors Neutralization reaction Acids + bases - water + salt

pH concentration of hydrogen ions Neutral = Acidic = Basic = Buffers—regulate pH change

B. ORGANIC CHEMICALS = framework of ____________ Types Fossil Fuels Biochemicals Carbohydrates Lipids Proteins Nucleic Acids

Biochemicals 1. Carbohydrates Elements: General Function: Ratio of Hydrogen to Oxygen: General Function: Classification Monosaccharides Disaccharides Polysaccharides

2. Lipids Elements: Ratio of H to C: Solubility in water: Types Organic Compounds … 2. Lipids Elements: Ratio of H to C: Solubility in water: Types

Lipids Types Neutral fats (triglycerides) Location: Function: Composed of: Glycerol & 3 Fatty Acids

Saturated Fats Figure 2.16a

Un-Saturated Fat Figure 2.16b

Important Characteristic: Lipids … Types … Phospholipids Composition: Function: Important Characteristic: Glycerol + 2 Fatty Acids Phosphate (Charged)

Cholesterol is the basis for all steroids made in the body Function: Lipids … Steroids Have rings Cholesterol is the basis for all steroids made in the body Function:

Important Organic Compounds … 3. Proteins Elements: Subunit: structure R group

Level of Complexity in Structure Primary structure. sequence of amino acids. Amino acids Hydrogen bonds Amino acids Secondary structure. Initial Folding into 2-D structure -pleated sheet Alpha- helix Figure 2.18a-b

Two or more polypetides Tertiary Structure 3-D Quaternary Structure Two or more polypetides Figure 2.18c-d

Proteins– Structure & Function Fibrous proteins, Structural proteins Function Stability Examples:

Figure 2.19a

Proteins 3-D proteins have specific Functions Stability– Denaturation Carriers Long-distance transport Hormones Enzymes

(b) Hemoglobin molecule composed of the Heme group Globin protein (b) Hemoglobin molecule composed of the protein globin and attached heme groups. (Globin is a globular or functional protein.) Figure 2.19b

Enzymes Function: How Function: active site

Substrates bind to active 2 Structural changes Enzyme (E) Product (P) e.g., dipeptide Substrates (S) e.g., amino acids Energy is absorbed; bond is formed. Water is released. Peptide bond + H2O Active site Enzyme-substrate complex (E-S) Enzyme (E) 1 Substrates bind to active 2 Structural changes Enzyme (E) site. Enzyme changes shape to hold substrates in proper position. occur, resulting in the product. 3 Product is released. Enzyme returns to original shape, ready to catalyze another reaction. Figure 2.20

Organic Compounds … 4. Nucleic Acids Types: Built from nucleotides Pentose (5 carbon) sugar A phosphate group A nitrogenous base A = Adenine G = Guanine C = Cytosine T = Thymine U = Uracil.

(a) Adenine nucleotide (Chemical structure) Deoxyribose Phosphate sugar Adenine (A) (a) Adenine nucleotide (Chemical structure) KEY: Thymine (T) Cytosine (C) Adenine (A) Guanine (G) Figure 2.21a

Nucleic Acids DNA Location Structure: Type sugar: deoxyribose Bases: Function:

(d) Diagram of a DNA molecule Hydrogen bond Deoxyribose sugar Phosphate (d) Diagram of a DNA molecule KEY: Thymine (T) Cytosine (C) Adenine (A) Guanine (G) Figure 2.21c-d

Nucleic Acids Ribonucleic acid (RNA) Structure: Sugar Bases Types Released mRNA Nucleic Acids Ribonucleic acid (RNA) Structure: Sugar Bases Types Function:

Nucleic Acid Derivatives Adenosine triphosphate (ATP) Modified Nucleotide of adenine with three phosphate groups Function: __________________________ Examples

(a) Adenosine triphosphate (ATP) Adenosine diphosphate (ADP) (b) Hydrolysis of ATP Figure 2.22a-b