Macromolecules

• Most confusing of concepts.

• What are they?

• Use of Macromolecules

• Differentiate

• Human need

Etymology

• 1886, from macro- + molecule. Apparently coined in "On Macro-molecules, with the Determinations of the Form of Some of Them," by Anglo-Irish physicist G. Johnstone Stoney (1826–1911). Originally of crystals.

Etymology

Macro- meaning “large,” “long,” “great,” “excessive,”

AND….

Molecule – Combination of elements

Meaning "molecule composed of many atoms" is from 1935, from German makromolekul (1922).

A macromolecule - is a very large molecule commonly created by polymerization of smaller subunits. In biochemistry, the term is applied to the four conventional Biopolymers •nucleic acids •proteins•carbohydrates•as well as non-polymeric molecules with large molecular mass such as lipids and macrocycles.

• The individual constituent molecules of macromolecules are called monomers (mono=single, meros=part).

SPONCH

What is SPONCH?

SPONCH

• S= Sulfur• P= Phosphorus• O= Oxygen• N= Nitrogen• C= Carbon• H= Hydrogen

6 most important elements to life

Matter

• Anything that occupies space and has mass

Element

• Simplest form of matter, cannot be broken down chemically into a simpler kind of matter

Periodic Table of Elements

• Organized table of elements discovered so far

• Organized according to atomic structure and chemical characteristics

Atoms and Atomic Structure

• Atoms are the simplest form of an element that keeps all the properties of the element

Model of the Atom• Parts of the atom:

– Protons (+), Neutrons and Electrons (-)

– Nucleus: central core of the atom that contains

• Protons • Neutrons

– Electrons orbit the nucleus

Determining Atomic Structure Using the Periodic Table

• Atomic number = # of protons and is smaller number by the symbol

• Atomic mass number = # of protons + # of neutrons

• Assume for now that protons =electrons

PracticeElement # protons # neutrons # electrons

hydrogen 1 0 1

helium

carbon

oxygen

sodium

chlorine

argon

sulfur

Practice

Element # protons # neutrons

# electrons

hydrogen 1 0 1

helium 2 2 2

carbon 6 6 6

oxygen 8 8 8

sodium 11 12 11

chlorine 17 18 17

argon 18 22 18

sulfur 16 16 16

Types of Bonds

• COVALENT – strong bond between elements

• IONIC- attraction between elements due to opposite charges (weaker than covalent)

• HYDROGEN – weakest type of bond

Covalent

• Sharing of electrons to fill the valence shell

• Examples– methane (CH4) and carbon dioxide (CO2)

Ionic

• One element gains electrons becoming ____

• The other element loses electrons becoming _____________

• Opposites attract• Ionic compoundsDissolve easily in water

– EX. NaCl

Hydrogen bonds

• Caused by partial positive and negative charges

• Water is best example

+ ہ- ہ

How does salt dissolve in water?

• Na+ and Cl –

• Ions become attracted to the partial charges on water

Biology

I know the following…

*atomic mass

*atomic number

*how to find # of protons

*how to find # of neutrons

*how to find # of electrons

*atomic structure (drawings)

*types of bonds

Today’s Agenda:

•QUIZ on Basic Chem.

•2-1

Chemistry Basics Quiz

Element Atomic Mass

Atomic Number

# of protons

# of neutrons

# of electrons

Li

Lithium

He

Helium

B

Boron

Na

Sodium

Draw the following atoms

• Carbon • Oxygen

WATER H2O

CARBON – the building block of life!

• DRAW Carbon

Carbon is able to covalently bond with up to four other elements or form double and triple bonds with other carbon atoms.

Carbon

• Carbon chains make up many structures of living organisms.

• Varying carbon chains’ structure and/or adding various atoms and molecules to the carbon chain will change it’s function

• MAKE CH4

* MAKE C2H6

* MAKE C2H4

Group of 4 Make…

• C4H10 – two different ways

Ring Forms of Carbons

• Make C4H8 with NO DOUBLE BONDS

FUNCTIONAL GROUPS

• Add a hydroxyl group (-OH) to a 2 carbon chain

•You just made ethanol – an alcohol that destroys liver cells

MACROMOLECULES

• 4 Large Molecules Important to Life– Carbohydrates– Lipids– Proteins– Nucleic Acids

Stuff to know!Chapter 2-1•Atomic #•Atomic mass•Atomic structure•Ionic bonds•Covalent bonds•Hydrogen bonds•Water chemistry

–Solutions,Solvents,pH– polarity

Chapter 2-3

•Carbon chem

•Carbohydrates

•Lipids

•Proteins

•Nucleic Acids

CARBOHYDRATES (CH2O)n

• Monomers = monosaccharides– Examples = glucose, fructose and galactose

(all 3 = C6H12O6 so they are isomer)

•Functions= provides energy (glucose is energy source for cells

• Two linked = disaccharides– Examples = sucrose (glucose and fructose)

and lactose

• Polymer = polysaccharides– Examples = glycogen (animals) starch

(plants)

Why “bulk-up” on carbs?

Why not eat carbs?

CONDENSATION REACTION

HOW WOULD THIS GET BROKEN DOWN?

HYDROLYSISH20

PROTEINS

• Monomers = amino acids

• All amino acids have– Amine group (NH2)

– Carboxyl group (COOH)

• R-groups differ

Dipeptide

FUNCTIONS of PROTEINS

• Structural

• Hormones

• Transport

• Histones

• ENZYMES!!!

Lock and Key Model

What symptoms would you have if you had sickle cell anemia?

1 amino acid is wrong in the hemoglobin sequence = mis-shaped RBCs

LIPIDS

• MONOMERS = fatty acids

• Saturated

• Unsaturated

COMPLEX

• TRIGLYCERIDES

• PHOSPHOLIPIDS

• WAXES

FUNCTIONS

• TRIGLYCERIDES – insulation and energy storage

• PHOSPHOLIPDS – main component in cell membranes

HARDENING OF THE ARTERIES

• Fats such as cholesterol and saturated fatty acids build up in arteries

• What other factors contribute to arteriosclerosis?

include

that consist of

which contain

that consist of that consist of that consist of

which contain which contain which contain

Section 2-3

Concept Map

CarbonCompounds

include

that consist of

which contain

that consist of that consist of that consist of

which contain which contain which contain

Section 2-3

Concept Map

Carbohydrates Lipids Nucleic acids Proteins

Sugars and starches

Fats and oils Nucleotides Amino Acids

Carbon,hydrogen,

oxygen

Carbon,hydrogen,

oxygen

Carbon,hydrogen,oxygen, nitrogen,

phosphorus

Carbon,hydrogen,oxygen,

nitrogen,

WATER CHEMISTRY

2-2

• 2–2 Properties of WaterA.The Water Molecule

1. Polarity

2. Hydrogen Bonds

B.Solutions and Suspensions1. Solutions

2. Suspensions

C.Acids, Bases, and pH1. The pH Scale

2. Acids

3. Bases

4. Buffers

Section 2-2

Section Outline

Hydrogen bonds

• Caused by partial positive and negative charges

• Water is best example

+ ہ- ہ

Cl-

Water

Cl-

Na+

Water

Na+

Section 2-2

Figure 2-9 NaCI Solution

Section 2-2

Figure 2-9 NaCI Solution

Cl-

Water

Cl-

Na+

Water

Na+

Solutions

• Ions break away from each other and form hydrogen bonds with water (because its polar)

• Solute- the substance that is dissolved

• Solvent- almost always water, substance in which the solute is dissolved

• Ex. Koolaid– Solute- koolaid powder– Solvent- water

Suspension

• Materials do not dissolve when placed in water, instead the water molecules keep them floating

• Blood- cells are floating in water solution

H2O sometimes breaks down into H+ and OH-

Oven cleaner

Bleach

Ammonia solution

Soap

Sea water

Human bloodPure waterMilkNormalrainfall

Acid rainTomatojuice

Lemon juice

Stomach acid

NeutralIn

crea

sing

ly B

asic

Incr

easi

ngly

Aci

dic

Section 2-2

pH Scale indicates the concentrion of H+ ions in water

Acids have higher concentration of H+, bases have higher concentration of OH-

The higher the pH, the more BASIC the solution. The lower the pH, the more ACIDIC the solution.

Buffers

• Weak acids and bases that reacts with other acids and bases to change the pH.

• In the body, buffers help maintain homeostasis

• Ex. Blood needs to stay within 6.5 to 7.5. Stomach needs to stay around 3. Peptobismo (buffer) raises stomach acid if your stomach is too acidic.

• 1. What are the reactants when wood burns?

• Reactants are oxygen and cellulose.

• 2. What are the products when wood burns?

• Products are carbon dioxide and water

• 3. What kinds of energy are given off when wood burns?• Light and heat are given off. Some students may also mention

sound (the crackling of a fire).

• 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy?

• To start a fire, you must light it with a match and kindling. You are giving the wood some energy in the form of heat.

• 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire?

• Once the fire gets going, it gives off enough heat to start more of the wood burning.

Section 2-4

Interest Grabber continued

• 2–4 Chemical Reactions and EnzymesA.Chemical Reactions

B.Energy in Reactions1. Energy Changes

2. Activation Energy

C. Enzymes

D. Enzyme Action1. The Enzyme-Substrate Complex

2. Regulation of Enzyme Activity

Section 2-4

Section Outline

Reaction pathwaywithout enzyme Activation energy

without enzyme

Activationenergywith enzymeReaction pathway

with enzyme

Reactants

Products

Section 2-4

Effect of Enzymes

Energy-Absorbing Reaction Energy-Releasing Reaction

Products

Products

Activation energy

Activation energy

Reactants

Reactants

Section 2-4

Figure 2-19 Chemical Reactions

Energy-Absorbing Reaction Energy-Releasing Reaction

Products

Products

Activation energy

Activation energy

Reactants

Reactants

Section 2-4

Figure 2-19 Chemical Reactions

Enzyme/Substrate Complex

CATALASE AND H2O2