4 ORGANIC COMPOUNDS

 ORGANIC COMPOUNDS ARE COMPOUNDS THAT CONTAIN THE ELEMENT CARBON.  _{THERE ARE EXCEPTIONS: CO, CO}

2, AND

CARBONATES.

 ALL LIVING THINGS CONTAIN THE

ELEMENT CARBON. NOT EVERYTHING

THAT CONTAINS THE ELEMENT CARBON IS ALIVE.

 WHY ARE THERE SO MANY CARBON COMPOUNDS?

 1) CARBON HAS 4 VALENCE ELECTRONS. THIS MEANS THAT EACH CARBON ATOM CAN FORM FOUR COVALENT BONDS WITH OTHER CARBON ATOMS OR ATOMS OF

 2) THERE ARE SINGLE, DOUBLE, AND TRIPLE BONDS AND ARRANGEMENTS. MORE ON THIS LATER…

 HYDROCARBONS: A COMPOUND MADE OF CARBON AND HYDROGEN ATOMS ONLY.

 NATURAL GAS IS A HYDROCARBON.

METHANE. THE CHEMICAL FORMULA FOR METHANE IS CH₄. ITS STRUCTURAL

FORMULA IS 1 CARBON ATOM

SURROUNDED BY 4 HYDROGEN ATOMS. THE LINE REPRESENTS A SINGLE

COVALENT BOND.

 OTHER EXAMPLES:

 ETHANE: C₂H₆

 PROPANE: C₃H₈

 BUTANE: C₄H₁₀

 ALL OF THE EXAMPLES JUST GIVEN ARE ALSO CALLED SATURATED

HYDROCARBONS. THEY ALL HAVE SINGLE BONDS AND THE CARBON ATOMS ARE



ISOMERS: COMPOUNDS THAT HAVE THE

SAME CHEMICAL/MOLECULAR FORMULA

AND A DIFFERENT STRUCTURAL SHAPE.



BUTANE AND ISOBUTANE BOTH HAVE

THE MOLECULAR FORMULA C

H

, BUT

THE CARBON/HYDROGEN ATOMS FORM

DIFFERENT SHAPES. SOME OF THEIR

 SATURATED HYDROCARBONS: CARBON AND HYDROGEN ONLY AND SINGLE

BONDS ONLY. (METHANE)

 UNSATURATED HYDROCARBON:

HYDROCARBONS THAT HAVE AT LEAST ONE DOUBLE OR TRIPLE BOND.

 SUBSTITUTED HYDROCARBONS:

COMPOUNDS WHERE HYDROGEN ATOMS ARE REPLACED BY ATOMS OF OTHER

ELEMENTS.  EXAMPLES:

 1) ALCOHOLS: THE OH GROUP. OH REPLACES HYDROGEN ATOMS.

 ETHANOL: C₂H₅OH (molecular formula)

 ETHANOL IS ALCOHOL PRODUCED BY THE FERMENTATION OF SUGAR IN CORN AND FRUITS.

 STRUCTURAL FORMULA NEXT SLIDE.

 2) ORGANIC ACIDS: THE COOH GROUP REPLACES HYDROGEN ATOMS.

 EXAMPLE:

 ACETIC ACID (IN VINEGAR) CH₃COOH

 BIOLOGICAL COMPOUNDS:

 1) PROTEINS: POLYMERS FORMED FROM ORGANIC COMPOUNDS CALLED AMINO ACIDS.

 POLYMERS ARE LARGE MOLECULES MADE FROM SMALLER MOLECULES CALLED

 THERE ARE MILLIONS OF PROTEINS MADE FROM ONLY 20 AMINO ACIDS.

 PROTEINS MAKE UP MUSCLE, HEMOGLOBIN, AND ENZYMES.

 TRYPTOPHAN C₁₁H₁₂N₂O₂

 IT IS AN ESSENTIAL AMINO ACID (MUST BE OBTAINED IN YOUR DIET)

 TRYPTOPHAN IS IN CHOCOLATE, MILK, AND CHEESE. ONE FUNCTION IS TO

PRODUCE SEROTONIN, A

NEUROTRANSMITTER. A DECREASE IN TRYPTOPHAN YIELDS A DECREASE IN

 2) NUCLEIC ACIDS: POLYMERS THAT CONTROL THE ACTIVITIES AND

REPRODUCTION OF CELLS.

 DNA AND RNA ARE EXAMPLES OF NUCLEIC ACIDS.

 THE BUILDING BLOCKS OF NUCLEIC ACIDS ARE MONOMERS CALLED

 DNA: CODES AND STORES GENETIC INFORMATION AND CONTROLS THE PRODUCTION OF RNA.

 RNA: CONTROLS THE PRODUCTION OF PROTEINS.

 3) CARBOHYDRATES: SUCROSE,

GLUCOSE AND STARCH…1:2:1 RATIO OF CARBON- HYDROGEN- OXYGEN ATOMS.  _C

6H12O6 IS A MOLECULE OF GLUCOSE.

 USED IN CELLULAR RESPIRATION FOR THE PRODUCTION OF ATP FOR ENERGY. PRODUCED BY PLANTS DURING

PHOTOSYNTHESIS.

 4) LIPIDS: FATS AND OILS… SAME ELEMENTS AS CARBOS, BUT IN

 ANIMAL FATS ARE SATURATED FATS. OILS FROM PLANTS ARE UNSATURATED.

 TOO MUCH SATURATED FAT CAN CAUSE HEART DISEASE.

 ACIDS: A SUBSTANCE THAT PRODUCES HYDROGEN IONS (H+) IN SOLUTION.

 THE PRODUCTION OF HYDROGEN IONS IS WHAT GIVES ACID COMPOUNDS THEIR

PROPERTIES.

 PROPERTIES OF ACIDS:  1) A SOUR TASTE

 2) ARE ELECTROLYTES

 ELECTROLYTES ARE SOLUTIONS THAT CONDUCT ELECTRICITY.

 3) CORROSIVE

 SULFURIC ACID: H₂SO₄

 USED IN BATTERIES, MANUFACTURE OF FERTILIZER.

 PHOSPHORIC ACID: H₃PO₄

 FERTILIZERS

 HYDROCHLORIC ACID: HCl

 NITRIC ACID: HNO₃

 BASES: SUBSTANCE THAT PRODUCES (OH-) HYDROXIDE IONS IN A SOLUTION.

 THE HYDROXIDE IONS OF BASES ARE

 PROPERTIES OF BASES:  BITTER TASTE

 CORROSIVE

 ELECTROLYTES  FEEL SLIPPERY

 COMMON BASES:

 SODIUM HYDROXIDE: NaOH

 DRAIN CLEANERS, MAKING SOAP

 AMMONIA: NH₃

 FERTILIZER, HOUSEHOLD CLEANERS

 ALUMINUM HYDROXIDE: Al(OH)₃

 ACIDS: ANY COMPOUND THAT CAN BE

IONIZED IN WATER TO FORM HYDRONIUM IONS.

 _{HCl + H}

2O YIELDS H30+ + Cl

- _H

3O+ IS THE HYDRONIUM ION

 WHEN THE ACID IS DISSOLVED IN WATER, THE NEGATIVELY CHARGED AREA OF THE WATER MOLECULE (O) ATTRACTS THE

 IF A SOLUTION CONTAINS MORE OH

-HYDROXIDE IONS THAN H₃O+ HYDRONIUM

IONS, IT IS A BASE.

 NH₄ AMMONIA IS A BASE THAT DOESN’T HAVE THE OH- HYDROXIDE, BUT,

DISSOLVED IN WATER, STILL PRODUCES OH- HYDROXIDE IONS.

 NH₃ + H₂O YIELDS NH₄+ + OH

 STRONG ACID: IONIZES COMPLETELY IN A SOLUTION.

 HCl + H₂O YIELDS H₃O+ + Cl

- WEAK ACID: PARTLY IONIZES IN SOLUTION.

- STRONG BASE: DISSOCIATES COMPLETELY IN SOLUTION.

 NaOH YIELDS Na+ + OH

- WEAK BASE: PRODUCES FEW IONS.

 NH₃ + H₂O YIELDS NH₄+ + OH

 PH: THE MEASURE OF THE

CONCENTRATION OF HYDRONIUM IONS IN A SOLUTION.

 THE PH SCALE IS O-14  PH < 7 IS ACID

 ACID RAIN:

 SULFUR + OXYGEN PRODUCES SULFUR DIOXIDE + OXYGEN YIELDS SULFUR

TRIOXIDE + WATER YIELDS SULFURIC ACID.

 S + O₂  SO₂

 NEUTRALIZATION: A CHEMICAL REACTION BETWEEN AN ACID AND A BASE.

 HYDRONIUM IONS FROM THE ACID

COMBINE WITH HYDROXIDE IONS FROM THE BASE TO PRODUCE WATER.

(NEUTRALIZATION)

 SALTS: A COMPOUND FORMED WHEN THE NEGATIVE IONS FROM AN ACID

COMBINE WITH THE POSITIVE IONS FROM THE BASE.

 THE MOST FAMILIAR SALT IS SODIUM

CHLORIDE NaCl OR COMMON TABLE SALT.  WHAT HAPPENS WHEN HCl COMBINES

WITH NaOH?

 MOST SALTS ARE COMPOSED OF A METAL AND A NONMETAL OTHER THAN OXYGEN.  SOME SALTS ARE COMPOSED OF A METAL

AND A POLYATOMIC ION.

 AMMONIUM SALTS CONTAIN THE

POLYATOMIC ION NH₄+ INSTEAD OF A

METAL.

 WHEN ACIDS REACT WITH METALS, HYDROGEN GAS IS RELEASED.

 EXAMPLES:

 H₂SO₄ + Zn YIELDS ZnSO₄ + H₂

 HCl + Fe YIELDS FeCl + H₂

 COMMON SALTS:

 NaCl: SODIUM CHLORIDE FOODS

 NaHCO₃: SODIUM HYDROGEN CARBONATE (BAKING SODA OR BICARB) FOODS

 CaCO₃: CALCIUM CARBONATE (CHALK)

 SOAPS ARE ORGANIC SALTS. THEY ARE

MADE BY REACTING FATS OR OILS WITH A STRONG BASE SUCH AS SODIUM

 ESTER: AN ORGANIC COMPOUND FORMED BY THE REACTION OF AN ORGANIC ACID AND AN ALCOHOL.  AN EXAMPLE IS ACETIC ACID PLUS

METHYL ALCOHOL YIELDING AN ESTER CALLED METHYL ACETATE.