Unit 1 AP Bio Chemistry of Life

the world is composed of ____, anything that has mass and takes up space

matter

mass is then broken down into ____, two or more atoms

molecules

the smallest units of mass are

atoms

atoms are broken down into subatomic particles such as 

protons, electrons, neutrons

an ___ is a substance that cannot be broke down further using a chemical reaction

element

elements are defined by their ___

atomic number or the number of protons

the ___ number is the number of protons added to the number of neutrons, gives the total amount of subatomic particles in the nucleus

mass

___ are outside the nucleus, orbiting it

electrons

when the number of protons isn’t equal to the number of neutrons

isotope

atoms are joined together through bonds, these bonds ___

make both atoms more stable

an ___ bond is when electrons are given up or gained, occurs when the ___ of one atom is higher than another atom

ionic, electronegativity

the result of an ionic bond is both atoms becoming ___, an atom or molecule with an unequal number of protons and electrons, giving it a net positive or negative electrical charge.

ions

a ___ bond is when electrons are shared, is more likely to occur than ionic bond in living organisms

covalent

types of covalent bonds

polar covalent, when electrons are unequally shared, results in an atom having a slightly positive (δ+) and a slightly negative (δ-) side of a single molecule

nonpolar Covalent, when electrons are equally shared, occurs when the electronegativity is equal

an ___, a substance with a high concentration of H+ ions

acid

a ___, a substance with a low concentration of H+ ions

base (alkaline)

pH scale goes from __ to __

0 to 14

the pH scale is not ___, but rather a ___ scale, meaning the change of one pH number means a tenfold change in the number of hydrogen ions

linear, logarithmic (ex. 3 pH is 10 times more acidic than 4 pH)

any number equivalent to or relatively close is classified as a __ pH

7.0, neutral

any number above 7 is called a ___, and any number below 7 is called an __

base, acid

our blood and pure water are abt 7 pH, any fluctuations in pH can __

kill an organism

our ___ have a low pH, but can survive bc they have ___ cells, cells that die in 7 to 10 days and replace easily

stomachs, disposable 

to prevent pH fluctuation, ___ exist… they either add or remove H+ ions depending on the situation 

buffers, (ex. anti-acid reflux drugs remove H+ ions to lower acidity)

__ an essential component of life, is composed of __& __, making a tetrahedral shape, and makes up abt 60-70% of all living organisms (cytosol)

water, two hydrogens and one oxygen

oxygen is slightly more __, and __

electronegative and hogs electrons

hydrogen is __

slightly more positive (δ+)

due to these slight electronegative differences between the two sides of a water molecule, the molecule is said to be __

polar covalent (unequal sharing of electrons)

due to this property of water, it can become the universal solvent of life - separating substances into two categories

Hydrophilic: substances that can dissolve in water (“water-loving”)

Hydrophobic: substances that cannot dissolve in water (“water-fearing”)

A ___, a weak intermolecular force, gives water its many unique properties…

hydrogen bond

water is both __, attracted to molecules similar to it, and _, attracted to molecules different than it 

cohesive, adhesive 

__ give water’s ability to a high _, the force needed to rupture the surface of a liquid

cohesion, surface tension

__ and __work together in __ moving upward in a small tube while working against gravity

cohesion, adhesion, capillary action 

_ allows for high specific heat and allows ice to be less dense, thus float

cohesion

_ allows water to be a universal solvent

adhesion

Water is densest at _ and least dense at _ or the freezing point

4°C, 1°C

why is ice less dense than water?

because the distance between the water molecules in each hydrogen bond expands in ice 

when does water freeze?

when it loses its kinetic energy which forces it to stop breaking and reforming hydrogen bonds and instead stick with their current mates

water has a high __, the amount of hear needed to raise the temp of a gram of liquid by  1°C because

specific heat capacity, it uses the majority of the heat given to it for breaking and reforming its hydrogen bonds

Sometimes when the amount of heat is large enough, the liquid can vaporize in a process called _, the amount of heat needed to convert a gram of liquid into a gas (100°C for water)

heat of vaporization

a biological process where water changing from liquid to gas absorbs heat from its surroundings, thereby cooling the surface.

evaporative cooling

__, the backbone of most organic molecules, takes up 18% of our body. it is a good backbone because it follows __, which requires four bonds to reach the octet rule, and the bonds it forms are stable and durable

carbon, tetravalent rule

__, molecules composed of only carbon and hydrogen, are a great source of energy due to the strong bonds that hold them together

hydrocarbons

__ are different molecules that have the exact same chemical formula but differ in the way their atoms are arranged

isomers 

Although there are many elements, 96% of the mass of all living things is made of just four elements:

oxygen, carbon, hydrogen, and nitrogen

There are also __: elements that all organisms require, but in small quantities (ex:/ iron)

trace elements

A molecule with a carbon skeleton is considered an _, but those without are considered __

organic molecule, inorganic molecules

a molecule that stores genetic information

Deoxyribonucleic Acid (DNA)

DNA is a polymer (large molecule) made up of repeating monomer units called nucleotides

DNA is composed of

one nucleic base, a phosphate group, and a sugar

is a nucleic acid that is used for protein and ribosomal synthesis

Ribonucleic Acid (RNA)

a macromolecule composed of carbon, hydrogen, and oxygen, typically in a 1:2:1 ratio

carbohydrates

The monomer of carbohydrate is called a — (“one sugar”) and there are three types…

monosaccharide

glucose, galactose, and fructose

A __, two monosaccharides, is created through a glycosidic linkage

disaccharide

maltose, lactose, fructose

__,  are large, complex carbohydrates

polysaccharide

starch, glycogen, chitin 

energy-rich organic compounds, such as fats, oils, and waxes, that are made of carbon, hydrogen, and oxygen.

lipid

lipid function

long term energy storage, source of energy, and insulation

Building blocks of lipids

fatty acids and glycerol

Fats are mainly synthesized by...

animals

Oils are mainly synthesized by...

plants

an energy-rich compound made up of a single molecule of glycerol and three molecules of fatty acid.

triglyceride

Oils are ______ at room temperature

liquid, unsaturated

A fatty acid in which all carbons in the hydrocarbon tail are connected by single bonds. Additionally, their structures are straight chains.

saturated fatty acid

A fatty acid possessing one or more double bonds between the carbons in the hydrocarbon tail.

unsaturated fatty acid

Types of lipids

triglycerides, phospholipids, steroids

found in cell membranes

phospholipids

What happens in phospholipids are mixed with water?

when mixed with water, they create a phospholipid bilayer. The head of phospholipid is polar and the tails are nonpolar.

lipids characterized by a carbon skeleton consisting of four fused rings.

Steroids

A type of lipid molecule consisting of one fatty acid linked to an alcohol; functions as a waterproof coating on many biological surfaces such as apples and other fruits.

waxes

Polymers of many amino acids (monomers) bonding together in a condensation reaction

protein

What are proteins made of?

C, H, O, N, (S)

Function of proteins

Communication, transport of genetic info, immune defense, enzymes structure

Basic Amino Acid Structure

Amino group and carboxyl group bonded to a carbon atom.

A long chain of amino acids that folds up to become the functional protein

Polypeptide

Bonds between amino acids via dehydration synthesis

peptide bonds

Two amino acids bonded together

dipeptide

Three or more amino acids bonded together

polypeptide

sequence of a chain of amino acids

primary protein structure

local folding of the polypeptide chain into helices or sheets

secondary protein structure

complete, three-dimensional (3D) folded shape

tertiary protein structure

the highest level of protein organization, where two or more separate polypeptide chains, called subunits, assemble to form a larger, functional protein complex

quaternary protein structure