Bio Week 2

• breaking and reforming of bonds
• reactants to products
• all chemical reactions must be balanced

6CO₂+6H₂O----> C₆H₁₂O₆ + 6O<sub>2

yield = light</sub>

4

• cohesive behavior
• ability to moderate temperature
• expansion upon freezing
• versatility as a solvent

the tendency of a substance to stick to itself b/c of hydrogen bonds b/c of polar covalent bonds

• the tendency of a substance to stick to some other substance
• ex. water sticks to cellulose and it climbs up trees

• cohesion + adhesion working together
• it is an unbroken bond of water; one air bubble would ruin it

• property of cohesion + adhesion
• the amount of force required to break the surface
• water has high surface tension relative to other liquids.

• kinetic energy= energy of motion
• heat= the total amount of kinetic energy due to molecular motion
• temperature= average kinetic energy of molecules
• ex. high flame will break hydrogen bonds (boiling water)
• breaking hydrogen bonds=gas molecules absorb heat
• when things are colder, hydrogen bonds form
• forming hydrogen bonds releases heat to the air
• large bodies of water moederate temp

hydrogen bonds-when cool- makes an ordered crystal shape, "arm's length", so that it's less dense than water

heat is released to the water below and air above.

amount of heat required to raise the temperature of 1g of water by 1 degree celcius

heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degree celcius

1 cal/g/degree celcius

due to high specific heat

a liquid that is a homogenous mixture of a substance

dissolving agent of solution

substance thats dissolved

where water is solvent

wet

• substance must be ion or polar to get shell
• ex. NaCl in water

too much solute, not enough water (solvent)

water solubile (charged/polar)

• not water solubile
• contains no polar bonds or charges
• ex. C+H

• sum of all the masses of all atoms in a molecule
• ex. water is 1+1+16=18

1 mol per Liter

1 out of 10 million times in pure water there is one hydronium (H₃O⁺) ion and one hydroxide (OH^-) ion

• donates H⁺ to the solution
• 1-6 acidic

• donates OH^- to solution or removes H⁺ from solution
• 8-14 basic

resists changes in pH

weak acid and the salt of a weak acid

ionize 100 %, but weak acids do not

• replication
• communication
• function
• objectivity

• used worldwide
• based on tens
• volume, mass, length are tied together for easier calculations

• transfer pipette has no measurements. it is used as a guide to add one drop at a time
• serological pipette is used as a measuring device for volume and it has lines on it for 5 ml 10 ml etc.

• weak bonds keep proteins together
• hydrogen bonds, van der waals, ionic
• if its too acidic, protein loses structure + function and it denaturates because H⁺ break the bonds

• lung pH is 7.4
• leg pH is 7.2
• when hemoglobin gets to legs, its shape slightly changes so that the O leaves the protein and enters tissue

carbonic acid

• it increases H protons in oceans
• which removes CO₃^2- ion, coral reefs cant build and they die

carbon makes 4 bonds and it can form 3-D molecules

single bonds, double bonds, triple bonds, long chains, branch, rings, fused rings

• same formula, same MW, different structure in space
• ex. pentane C₅H₁₂

cannot rotate

• cis-isomer = same side
• trans-isomer = different side

• mirror images
• ex. your two hands
• there is two: levo (left side) and dexar (right side)
• all amino acids are L in nature
• all sugars are D

• carboxylic acid or organic acid
• R-C--O
• -O-H

• monomors for proteins
• very polar molecule
• put on organic molecule and it makes it basic
• R-N-H
• -H

S-H