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Page 1: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 2: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

I. AtomsA. Subatomic Particles

• Protons (+) in nucleus• Neutrons (0) in nucleus• Electrons (-) in orbitals energy

levels• 1st- 2electrons 2nd- 8 electrons• 3rd orbital 8 or 18 electrons

B. Atomic number – number of protonsC. Atomic mass – protons & neutronsD. Isotopes – same element w/

different number of neutronsE. Chemical properties – reactivity, F. Physical properties – descriptive

solid shape color

Page 3: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 4: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

G. Elements1. C H O N Na Cl S Mg K Ca Fe P2. Periodic table

• 6 – atomic number = # of protons• C – element symbol• 12 – atomic mass = # of protons

+ # of neutronsII. Chemical Compounds – 2 or

more elements combined A. Molecules “compounds”

• H20, O2, NaCl “salt”, CO2, C6H12O6- monosaccharide (glucose)

• HCl – “hydrochloric acid • C12H22O11 – disaccharide (sucrose)

Page 5: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 6: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

B. Ionic Bonds – elements lose or gain electrons, become ions

C.Covalent Bonds – shared electrons

Page 7: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 8: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

III. Water – most common solventA. Solubility – how well something

dissolves, like dissolves likeB. Solvent dissolves soluteC. Cohesion-tension – water attracted

to water• Capillary action – surface

tension, attraction tension H2O to H2O

D. Specific heat – water has a high specific heat, it takes a lot of energy to change water’s temp.

Page 9: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

IV. pH – relative concentration of H+ and OH-

A. Acids – pH 1-6, more H+ ions, hydrogen ions, sour taste, urine 5.5, sweat 5.5, pop 3.5, gastric juice 2.0

B. Bases – “alkaline” pH 8-14, more OH- ions, hydroxide ions, bitter taste, bile 8, ammonia 11.5, bleach 12.5, pancreatic juice 8

C. Neutral – pH 7, H+ = OH-, water, blood, salivaD. Buffers – baking soda NaOH,

neutralize excess acid to create pH 7

Page 10: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 11: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

I. Molecules of living things

A. Organic chemistry – contain carbonB. Chemical groups pg 38

• Hydroxyl – OH• Carboxyl – COOH,in lipids & proteins• Amino – NH3, NH2,in proteins• Phosphates – PO4, In nucleic acids, DNA, RNA

Page 12: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 13: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

II. Macromolecules A. Polymer – repeating monomers

“chains”B. Biological polymers

1. Condensation reactionsDehydration synthesis, anabolic = smaller largerC6H12O6 + C6H12O6 C12H22O11 + H2O2. Hydrolysis – catabolic = larger smaller,

digestion breaking downC12H22O11 + H2O C6H12O6 +

C6H12O6

Page 14: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 15: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 16: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

III. Carbohydrates – sugars and starches used for energy, 4 calories / gram,

contain C, H, O, 2H: 1 oxygenA. Monosaccharides – single sugars

(C6H12O6)• Glucose• Fructose – fruit sugar• Galactose Isomers – same formula different

arrangementB. Disaccharides – double sugar

(C12H22O11)• Sucrose – “table” fructose + glucose• Lactose – “milk” glucose + galactose• Maltose – “malt” glucose + glucose

Page 17: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 18: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

C.Polysaccharides – “many sugars”1. Starch – breads, potatoes, grains2. Glycogen – stored glucose in muscles

and liver3. Cellulose – cell walls “wood”

Page 19: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 20: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

IV. Proteins – C H O N & sometimes S, used for growth maintenance and repair (4 calories / gram)

A. Amino acids – (20) base unit of proteins, examples: lysine, argenine, tyrosine

B. Peptide bonds • Polypeptides – 3 or more amino

acids form proteins: albumin, keratin, collagen, enzymes, skin, hair, muscles, organs

C. Prosthetic groups – another element will replace H, hemoglobin, H-C-C-C-C-Fe

Page 21: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 22: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 23: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

V. Lipids – C H O (9 calories / gram) fats ,waxes, oils used for energy storage, insulation, padding

A. Fatty acids – base unit of lipids (linoleic acid)

Unsaturated – liquid – plants, double bonds, HDL’s

Saturated – solid – animals, single bonds, LDL’s

B. Triglycerides & neutral lipids – 3 fatty acids & glycerol, “adipose” fat

C. Phospholipids – cell membranes D. Sterols – fats in a ring, cholesterol,

testosteroneE. Waxes – fatty acids & alcohol,

resistant to water

Page 24: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 25: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

VI. Nucleic Acids – C, H, O, N, and P

A. DNA – deoxyribonucleic acid, genetic code of life

B. RNA – ribonucleic acid, codes for proteins

C. Nucleotides & ribose & phosphates

• Guanine• Adenine• Thymine• Cytosine• Uracil

Page 26: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 27: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

I. EnergyA. Potential – stored

Chemical – stored in chemical bonds

B. Kinetic – energy of motion, break bonds

II. Energy in chemical reactionsA. Reactants and products

(left of equation and right ofEquation will equal each other- balanced equations Conservation of matter and energy

Page 28: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons

B. Chemical balance of energy1.ATP – adenosine triphosphate,

A-P~P~P contains high energy bonds

2.ADP – adenosine diphosphate, A-P~P

3.ATP/ADP cycle –

Page 29: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons
Page 30: I.Atoms A. Subatomic Particles Protons (+) in nucleus Neutrons (0) in nucleus Electrons (-) in orbitals energy levels 1 st - 2electrons 2 nd - 8 electrons