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OrganicOrganic CompoundsCompounds & &

InorganicInorganic Substances Substances in Living Thingsin Living Things

ksuweb.kennesaw.edu/~vking2/Chemistry%20of%20Life%20Post.ppt www.wyalusingrams.com/53942041017952357/lib/53942041017952357/UNIT_2_chemistry.ppt www.wyalusingrams.com/53942041017952357/lib/53942041017952357/UNIT_2_chemistry.ppt 

faculty.sgc.edu/asafer/BIOL1107/chapt02_lecture.pptfaculty.sgc.edu/asafer/BIOL1107/chapt02_lecture.ppt   

b) Inorganic substances also are important to organisms, but do NOT contain carbon

a) Organic compounds are carbon-based and are the key substances that make up living things.

Introduction

1. All living things are made MOSTLY of organic compounds!

2. Yes, you’re organic!

c) Organic (Carbon) Compounds

The 4 Types of Organic (C) Compounds

3. Organic compounds are made of repeating units called monomers

4. Organic compounds FORM by dehydration synthesis (condensation)

5. Organic compounds are BROKEN DOWN by hydrolysis (decomposition)

1) Carbohydrates

Main Use: immediate energy –contain C, H, and O –polysaccharide is a long chains of monomers

Part 1: Types of Organic (C) Compounds

a) Monosaccharides:• glucose (main source of energy for cells)• fructose (in fruit)

b) Disaccharides•sucrose (table sugar)•lactose (in milk)

Examples of carbohydrates: sugars & starches

c) Polysaccharides (starches)

• glycogen starch stored in liver• cellulose fibers in plants

2) Lipids (fats; triglycerides)

Main Use: long term energy storage–contains C, H, and O–composed of glycerol + long fatty acid chains

a) Saturated fats – contain single bonds

- solid fats (related to heart disease)

e.g. butter, lard, coconut oil, palm oil

b) Unsaturated fats – contain double bonds

- liquid oils (healthier)

e.g. peanut, corn, olive oils

c) Steroids – have a four ring structure

Examples: cholesterol (LDL, HDL) sex hormones (testosterone, estrogen), cell membrane bile

3) ProteinsMain Uses:

Structural –muscle protein fibers

Enzymes – catalysts to speed up chemical reactions

Energy– only if starvation occurs

–contains C, H, O, N–monomer = amino acids–polypeptide is a long chain of amino acids linked by peptide bonds

Examples of proteins hemoglobin (in red blood cells) digestive enzymes

hydrolysis or decomposition (e.g. digestion)

Enzymes speed up chemical reactions!

dehydration synthesis- assembles larger organic compounds

4) Nucleic AcidsMain Use: store and carry genetic information

–C, H, O, N and P–monomer = nucleotide

Examples of nucleic acids DNA (deoxyribonucleic acid) is double

stranded RNA (ribonucleic acid) is single stranded

MATCHING

Monomer Organic compound

1. nucleotides carbohydrates

2. monosaccharides lipids

3. amino acids proteins

4. glycerol + fatty nucleic acids acid chains

Part 2: Inorganic Substances in Living

Things(no carbon)

I. Water & Organisms about two-thirds (2/3) of the human body is

water!!!

Water is essential for cell function; it is required in chemical reactions to sustain life

Water is the only common substance in nature in all 3 physical states of matter– solid, liquid and gas

A) Polarity of Water

Water is a polar molecule with positive (+) and negative (-) ends

this leads to easy formation of hydrogen (H) bonds between water molecules

Water is a polar molecule

Oxygen

H H

Oxygen

H

Hydrogen (H) bondsform between watermolecules

H H

H H

H

H bond

H bond

1. cohesion--water molecules H bond to one another easily and “cling” together

B) Properties of Water

cohesion surface tension

water strider (or skater)

2. adhesion--water molecules easily form H bonds to other non-water substances

e.g. water travels UP through plant stems & tree trunks

adhesion capillary action

3. high specific heat! Water has high specific heat and resists changes in temperature

e.g. sweat absorbs some of the heat of your body

4. high heat of vaporization

* It takes a significant temperature increase for water to evaporate!

5. Water is less dense as a solid!

water E X P A N D S when it freezes Therefore, ice FLOATS in water!! and cells die when the cytoplasm

(fluid) inside freezes!

e.g. frostbite

Euphausid shrimp under ice

Ice fishing

6. High solubility

water molecules surround molecules

water is practically a universal solvent

• Many substances are dissolved in biological fluids (vitamins, glucose, oxygen, salts, carbon dioxide, wastes)

• Detection by blood & urine tests

II. Acids & Bases1. Acids are substances that form

hydrogen ions (H+) in water

2. Bases are substances that form hydroxide ions (OH-) in water

3. The pH scale measures the acidity & alkalinity.

pH scale

_________________________________________0 7

14

acids bases pH < 7 pH > 7

neutralpH = 7

III. Oxygen (O2)

• cells use O2 to breakdown food into ATP energy molecules during cellular aerobic respiration

• You need to breathe O2 for energy!

• No O2, no energy, no life!

IV. Salts – dissolve easily in water– form ions (electrolytes) for metabolism

(chemical reactions for cell activities)

e.g. Na+, Mg2+, Ca2+, K+, Cl-

Assignment #27:

Create a thinking map entitled,

“Chemicals in Living Things”

Enzymes Enzymes are proteins that function as catalysts for

chemical reactions– they speed up the rate of reactions by lowering the

activation energy needed for a chemical reaction to happen

Lock and Key Model– Each enzyme has a specific shape (lock)– Substrate (key)

the reactant that must fit into active site of enzyme for reaction to occur

One enzyme one specific reaction– Enzymes are not changed during the reaction; “re-

usable”

Coenzymes – smaller organic molecules that are needed for a proper fit of an enzyme to substrate e.g. vitamins

Cofactors – ions needed for proper fit of enzyme/substrate

e.g. Minerals Denaturation – the change of a protein’s shape

– Change the shape, change (usually ruin) the function– possible causes: high temperatures, wrong pH or salt

concentration