Chemicals of Life A Unit on Biochemistry What is biochemistry???? The study of the different types of chemicals found that make up all living organisms

Review of terms: Atoms: Basic building block of matter.

Composition of an atom: Made up of three subatomic particles: Protons + in the nucleus Neutrons neutral Electrons --- electron shell

Elements: Substance made up of all one type of atom. Six most common elements found in living organisms: C, H, N, O, P, S

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

Molecules/compounds:

Molecules/compounds: -Two or more atoms bonded together to create a new substance with new properties. Example: Sodium + Chlorine = Sodium Chloride Table Salt -silvery white solid -explosive in water -green gas -poisonous -white solid -not explosive -not poisonous

5 most common compounds in a living organism: Carbohydrates Lipids Proteins Nucleic Acids Water

Two types of compounds: Inorganic compounds: Do not contain carbon-hydrogen bonds Can not be decomposed Must be recycled Examples: Sand, glass, Styrofoam Soil, rocks, metals and Water Carbon dioxide CO2

Organic Compounds: Contain at least one carbon-hydrogen bond Can be decomposed or broken down Examples: Anything living or once living Dead plants and animals Proteins, lipids, carbs/C6H12O6 and nucleic acids

The C, H, N, O, P, S found in organic molecules must be decomposed and recycled continuously through our biosphere.

Lets start with INORGANIC:

The most common inorganic compound found in all living organisms is: WATER: -classified as being inorganic -Why? -does not contain…. carbon and hydrogen bonds -cannot be…….. decomposed -must be………. recycled

Recycling of water:

Water: H2O 2. The atoms bond to form an angular molecule 1. Made up of two hydrogen atoms bonded to one oxygen atom. Turn the page!!! 2. The atoms bond to form an angular molecule

- + 3. Water is classified as a polar molecule. Like a bar magnet it has a partial positive and a partial negative end. +

One of the most important rules in biology is that: …………opposites attract

+ - + - + - + -

Therefore, one molecule of water is attracted to another molecule of a water, as long as the + end of one is next to the – end of another thus giving water many unique properties. + -

Temporary, weak hydrogen bonds form between the two water molecules “holding” the two molecules together + -

Lab Time

Water’s unique properties: -1. Is an inorganic molecule -Contains no carbon-hydrogen bonds -2. Made up of two hydrogen atoms and one oxygen 3. -forms an angular molecule 4. - Is a POLAR MOLECULE -has a + and a – end -5. Covers 75% of the Earth’s surface -6. Makes up 70% to 80% of a living organism + -

7. -Occurs in three phases -Solid -molecules have a small amount of energy -a little movement (just vibrating) -Liquid -molecules gain some energy and some movement -Gas -molecules gain a lot of energy and a lot of rapid movement (enough to escape the surface )

PHASE DIAGRAM OF WATER

Phase Change Diagram of Water

Water displays cohesion. to work together Hesion or hesive (think tape) = to stick together Cohesion is: the attraction between like molecules. (one water molecule to another water molecule. - This occurs because water is a polar molecule and opposites attract.

9. Water displays adhesion. What is adhesion? -waters attraction to other types of molecules (like waters attraction to a paper towel)

10. Water expands when frozen. When frozen, the water molecules slow down their movement and due to their polarity they will line themselves up + end to – end thus taking up more room and lowering its density.

Water expands when frozen. Density is : Mass/volume Liquid: 1g/1cm3 = density of 1.0 Solid: 1g / 1.2 cm3 = density of .83 Solid ice with .83 density will float in liquid water with a 1.0 density Liquid: water molecules have more energy/more movement thus they are constantly moving , regardless of the + and – charges, they take up less volume Solid: molecules are only vibrating, they arrange themselves + end to – end taking up more volume.

- - + + O H H H H O H O O H H H Liquid Solid Occupies less volume . . - O H H H + H - O H O O H H H + Occupies less volume Liquid Occupies more volume Solid

It dissolves more substances on Earth than any other 11. Water is known as the UNIVERSAL SOLVENT It dissolves more substances on Earth than any other substance

To dissolves means the molecules of one substance are picked up and surrounded by another type of molecule.

Demo of salt dissolving In water.

Lab Results

Mixtures: - 2 or more substances combined but not chemically. -each substance retains it’s own properties. -each substance can be separated from the other. Examples??????? Salt water, kool aid, trail mix

12. Due to its polarity, water can create 2 types mixtures: - Suspensions - Solutions

Suspensions: Example: Oil and water A substance is mixed with water and the 2 substances separate. The less dense substance is “suspended above” the more dense substance. This happens because water is POLAR and oil is NONPOLAR (oil has no + or – ends)

Blood is a suspension: Red blood cells, white blood cells and platelets are float around in the liquid plasma

Solutions: One substance dissolves into another substance. Examples: Kool aid Salt water

Cytoplasm is a solution: All of the digested food molecules from the food we eat and all of the Oxygen molecules from the air we breathe are dissolved in the liquid component of our cell’s blood.

Likes dissolve likes The Rule::: SO: Polar substances dissolve other polar substances Polar water will dissolve salt because salt is polar Nonpolar substances dissolve other non polar substances Nonpolar oil will dissolve in gas because gas is non polar

Parts of a solution: Solvent: Substance doing the dissolving. (water) Solute: Substance being dissolved. (salt) Solution: Created when the solute DISSOLVES in the solvent. (salt water)

Water is known as the Universal Solvent. -dissolves more substances than any other solvent including all items that need to be dissolved in living organisms.

Aqueous solution: water is the solvent Saline solution: salt is the solute Tincture: alcohol is the solvent

Types of water solutions: 1.Acids 2.Bases 3.Neutral

Acids: A substance that release +H ions when dissolved in water. HCl / Hydrogen chloride dissociates into H+ ions and Cl- ions when placed in water + -

HCl is Hydrogen Chloride H is +1 and Cl is – 1 therefore it is neutral Not dangerous to us and our tissues When HCl is dissolved into water, the H and Cl ions separate. HCl is now known as Hydrochloric Acid It is now very dangerous to us and our tissues

- Acidic Solutions: + HCl / Hydrogen chloride dissociates into H+ ions and Cl- ions when placed in water Opposites attract so the + H is attracted to the – end of water and -Cl is attracted to the positive end of water Free H+ ions are present now so it is now an ACID Cl- + - H+

Base: A substance that release -OH ions when dissolved in water. NaOH/Sodium hydroxide dissociates into Na+ ions and OH- ions when placed in water

NaOH, sodium hydroxide is now very dangerous to us and our tissues NaOH is Sodium Hydroxide Na is +1 and OH is – 1 therefore it is neutral Not dangerous to us When NaOH is dissolved into water, the Na and OH ions separate. NaOH, sodium hydroxide is now very dangerous to us and our tissues

- Basic Solution: + NaOH/Sodium hydroxide dissociates into Na+ ions and OH- ions when placed in water Opposites attract so the + Na is attracted to the – end of water and -OH is attracted to the positive end of water Free OH- ions are present now so it is now an BASE OH- + - Na+

Neutral: A substance that release no +H or –OH ions when dissolved in water A when a substance releases an equal amount of both the +H and the – OH ions and they cancel each other out. OR

- Neutral Solution: + NaCl /sodium chloride dissociates into +Na and –Cl ions There is NO +H or –OH ions so therefore it is NOT an acid or a base so it is NEUTRAL Cl- + - Na+

Review of acids and bases:

pH Scale: -measures the strength and weaknesses of an acid (%H+) and of bases (%OH-) -based on a scale of 0 to 14

pH and common substances:

Neutralization Reaction: When an acid and a base of equal strength are mixed and cancel each other out creating a neutral substance. HCl + NaOH ---- NaCl + HOH Strong Strong neutral neutral acid base no H or OH H = OH

Buffer: A substance which guards against shifts in the pH level. Our blood is an example of a buffer. Blood uses extra H+ and OH- ions substances to help resist pH changes in our body.

Indicator Test: -special chemicals that can show whether a substance is an acid, a base or is neutral. -Two type of indicators: -pH paper: Used to determine the strength or weakness of an acid or a base.

pH paper: Classroom pH paper ranges from 1 to 12 and not 0 to 14 for safety reasons

2. Litmus Paper: -Two types of litmus paper. -RED and BLUE Used to determine the presence of +H ions and OH- ions NOT the strength of the acid or base.

Red litmus determines the presence of +H ions Blue litmus determines the presence of –OH ions

Dip the red litmus paper into the solution and record the color Dip the red litmus paper into the solution and record the color. Did it stay red or did it turn blue?

Dip the blue litmus paper into the solution and record the color Dip the blue litmus paper into the solution and record the color. Did it stay blue or did it turn red?

Results: Red litmus paper Blue litmus paper Stays red… contains H+ ions Red litmus paper Blue litmus paper Turns blue….contains 0H- Blue (start with a “B”) indicates OH- ions/base Red (think of a burn) indicates H+ ions/acid Stays blue… contains OH- ions Turns red….contains H+ ions

Substance Blue Litmus (red or blue) Red Litmus pH paper (range 1-12) Strong or weak acid Strong or weak base Or neutral Windex Saliva