Chemistry

Chemistry Overview

• Inorganic• Organic• Biochemistry• Analytical

Matter

• Define• Composition

– Fundamental Elements

– Atomic Particles

States of Matter

Energy

• Components– Te = Ke + Pe

• Forms– Chemical– Electrical– Mechanical– Electromagnet

ic

• Conversions

Matter and Energy Relationship

Atoms

• Define• Subatomic

Particles– Name– Charge– Location– Function

• Atomic Symbol– Atomic Number– Mass Number– Atomic Weight– Charge

Atomic Nucleus

• Protons = AN– Electrically neutral– P = E

• Neutrons = AW– Variable number– Isotopes

Energy Levels

• Electrons• Orbitals

– Maximum e- number• 2n to 2nd power• n is 1, 2, 3 etc orbital

– Sublevels • 2 electrons each• s, p, d, f

– Valence• Outermost • Determines Chemical

property of atom

Electron Valence Shells

• Gain electrons

• Loose electrons

• Share electrons

Reactive vs. Inert Atoms

Molecules and Compounds

• Define– molecule of an

element• Define

– molecule of a compound

• Define solution– Solvent– Solute

Chemical Bonds Overview

Covalent Bonds

• Strong• Electrons shared• Electrically

neutral• Types

– Single– Double– Triple

Polar Covalent Bonds

• Slightly weaker than covalent

• Unequal electron sharing

• Allow for hydrogen bonds between other elements

Ionic Bonds

• Do not share electrons– Electrons gained or

lost– Create ions

• Cations• Anions

• Stable – Electron orbitals

full– Salts

• Dissociate– Ions in solution– Electrolytes

Hydrogen Bonds

Chemical Reactions

• Reaction components– Reactants– Products– Direction indicated by

arrows

• Types– Decomposition– Synthesis– Displacement– Reversible

• Reaction Rates– Temperature– Particle size– Concentration of

reactants– Enzymes– Energy requirements

Inorganic Compounds

• No carbon-hydrogen as primary structure

• Small molecules• Majority have ionic

bonds• Examples

– Water– Salts– Acids– Bases– Buffers

Water

• 2/3 body weight• 75% of cell

volume• Bonds

– Polar covalent– Hydrogen

• Chemistry– Dehydration

synthesis– Hydrolysis

• Properties– Temperature– Solvent– Reactant– pH– Surface tension– Solubility

pH

• Define• Math equation• Scale• Normal range• Problems

– Acidemia, acidosis– Alkalemia,

alkalosis– Compensated– Uncompensated

pH and pH Scale

Buffers

Chemical Buffer Systems

• Define• Types

– Chemical– Respiratory– Renal

Organic Compounds

• Contain – Carbon-Hydrogen– Oxygen

• Covalent bonds • Macromolecule

classes– Carbohydrates– Lipids– Proteins– Nucleic Acids

Organic Functional Groups

Carbohydrates

• Source• Function• Structure

– Formula– Combinations

• Mono-• Di-• Poly-

Glucose Chemical Structure

Carbohydrate Interactions

GlucoseC6H12O6

Fatty Acid Structure

Lipid Structure

Saturated vs. Unsaturated

Lipids

• Basic Structure• Class Types

– Fatty Acids– Glycerides– Prostaglandins– Steroids– Phospholipids– Glycolipids

• Function

Proteins

• AA structure• Bonds• Shape• Types

– Short chain– Long chain

• Functions– Fibrous– Globular

Amino Acid Structure

Amino Acid named for its structure

Amine group Carboxylic acid group

Amino Acid Groups

Peptide Bonds

Fibrous Proteins

• Structure• Support• Movement/

Contraction• External Defense

Elastin and collagen

Globular Proteins

• Transport– Albumin– Hemoglobin– Hormones

• Metabolic– enzymes

• Defense– Immunoglobuli

ns

Enzymatic Reaction

Enzyme Saturation Curve

Enzyme Interactions

Protein Denatured

Nucleotide Structure

Nucleic Acids

Nitrogen Base Pairing

• DNA– A-T– T-A– C-G– G-C

• RNA– U-A– A-U

Nucleic Acid Comparison

• DNA– Double stranded– Alpha Helix– AT and CG base pairs– Nucleus (eukaryotes)– Semi-conservative

replication creates daughter strands during S phase of cell cycle

• RNA– Single stranded– Different for each

type– AU and CG base

pairs– Cytoplasm– Created from DNA

for transcription and translation for protein synthesis

DNA

mRNA

rRNA

tRNA

DNA Replication

Transcription

Translation

Protein Synthesis

High Energy Compounds

Questions?