AP Bio Unit 1; Chp 1-5

Based on Study Guides

Organic Compound

made of carbon & hydrogen, may include elements like oxygen, nitrogen & sulfur

Isomer

molecules w/ the same chemical formula, same number of atoms but different structures

Structural Isomer

Same empirical formula, different shape

Sterioisomer

Same empirical formula, same shape, different arrangement

Enantiomer

molecules that are mirror images of each other

Cis-Trans Isomer

Atoms differ in spatial arrangements due to inflexibility in double bonds

Hydrocarbon

organic compounds composed solely of hydrogen and carbon atoms, hydrophobic

Functional Group

Behavior of organic molecules depends on it, they're specific clusters of atoms within a longer molecule, dictating chemical properties & reactivity

Hydroxyl Group

functional group consisting of -OH

Carbonyl Group

functional group consisting of C=O

Carboxyl Group

functional group consisting of -COOH

Amino Group

functional group consisting of -NH2

Sulfhydryl Group

functional group consisting of -SH or HS-

Phosphate Group

functional group consisting of -PO3

Methyl Group

functional group consisting of -CH3

Aldehyde Group

type of carbonyl groups: functional group at the end of a carbon chain

Ketone Group

type of carbonyl groups: functional group at the middle of a carbon chain

Hydrolysis

Chemical reaction where water is added, causing it to split (opposite of dehydration synthesis)

Dehydration Synthesis

formation of large molecules via removal of water molecules

Polymer

Many units, many monomers

Monomer

Single subunit of a polymer

Macromolecule

large molecules or carbohydrates, lipids, nucleic acids, proteins

Monosaccharide

monomer of carbohydrate, typically 6 carbons, simple sugars (glucose, fructose, galactose)

Disaccharide

formed by a dehydration reaction between two monosaccharides, e.x., sucrose

Polysaccharide

Polymers with a few hundred to thousands of monosaccharides joined by glycosidic linkages - lots of sugar molecules bonded together

Glycosidic Linkage

Bonds between sugar molecules, between monosaccharides through dehydration synthesis

Glucose

primary energy source for the body, monosaccharide, level is low we feel hunger

Fructose

isomer of glucose, fruit of sugars

Sucrose

Disaccharide formed from glucose and fructose - held by a glycosidic linkage

Glycogen

carbohydrate found in animal tissue, a ton of branches of glucose chains - big boost of energy and then dropped

Amylose

edible starch, found in plants, alpha linkage, the simplest branch of a glucose chain

Cellulose

found in plant cell walls, non-edible starch, polysaccharide, beta linkage

Starch

polymers of glucose molecules, energy storage for plants, alpha linkage

Chitin

found in shells of arthropods and in cell walls of fungi, structural polysaccharide, beta linkage

Lipid

includes fats, oils, waxes; even distribution of electrons, hydrophobic, no monomer

Fatty Acid

long carbon skeleton, usually 16 or 18 carbon atoms in length, with a carboxyl group at the end

Saturated Fatty Acid

contains as many hydrogen atoms as possible, no double bonds between carbon atoms

Unsaturated Fatty Acid

contains one or more double bonds, with one fewer hydrogen atom on each double-bonded carbon

Triacylglycerol (Triglyceride)

formed by a dehydration reaction between three fatty acids linked to one glycerol molecule

Phospholipid

similar to triglycerides but has only 2 fatty acids attached to a phosphate group

Steroid

lipids characterized by a carbon skeleton consisting of four fused rings

Cholesterol

type of steroid, crucial molecule in animals, found in animal cell membranes

Peptide

short chains of amino acids, typically less than 20

Peptide Bond

bond between amino acids formed by a dehydration reaction

Polypeptide

polymer of amino acids, typically folded into a specific shape

Amino Acid

monomer of protein, organic molecule with both an amino group and a carboxyl group

Nucleic Acid

macromolecule, includes DNA, RNA, ATP

Nucleotide

monomer of nucleic acid, consisting of a phosphate, sugar, and nitrogenous base

DNA

contains instructions to make proteins, double-stranded, AT & GC

RNA

single-stranded, can leave nucleus and make proteins, AU & GC

Pyrimidine

type of nitrogenous base with one six-membered ring of carbon and nitrogen atoms, cytosine & thymine& uracil

Purine

type of nitrogenous base with two rings, a six-membered ring fused to a five-membered ring, adanine & guanine

Oligosaccharide

short chain of carbohydrates (3-10) - functions like cell recognition

Cis functional group

functional group on the same side of a carbon structure

trans functional group

functional group on opposite sides of a carbon structure

primary structure of a protein

sequence of amino acids

secondary structure of protein

alpha helices and beta sheets formed by the backbone

tertiary structure of protein

shape of the amino acid chain

quaternary structure of protein

shape/interaction of more than one amino acid chain

mass number

number of protons+neutrons for an atom

valence electrons

electrons found in outermost orbital - bonding sites

polar covalent bond

bond between atoms where electrons are shared but not evenly distributed - creates charged sides; i.e. water

elements

substances that cannot be broken down into other substances by a chemical reaction

-atom with specific amount of protons

dalton

unit of measurement for atomic mass

• 1 proton = 1 Dalton

• 1 electron = (1/2000) Dalton

Potential Energy (PE)

energy matter has due to its position or structure/phase

Non-Polar covalent Bond

bond between atoms where they share electrons evenly, meaning the charge is the same all the way around the molecule

Compound

substance consisting of 2 or more unique elements combined in a fixed ratio

• different characteristics from parent elements

isotope

when element contains a different number of neutrons from protons

• protons stay the same and determine type of element

• behave identically in chemical reactions

• typically more neutrons than protons

orbital

3D region around an atomic nucleus that contains the electrons

Cation

positively charged ion

Proton

positively charged particle found in nucleus of an atom

radioactive isotope

Isotope where nucleus is unstable and spontaneously decays, giving off energy

Covalent Bond

bond between atoms where electrons are shared

Anion

negatively charged ion

neutron

neutral particle found in nucleus of an atom

• contains both positive and negative charge

half-life

the time it takes for half of a parent isotope to decay

• only applies to radioactive isotopes

molecule

2 or more atoms that are covalently bonded

ionic bond

electron is transferred between two atoms

• creates 2 ions with opposite charges that are now attracted to each other

• weaker than covalent bond

electron

negatively charged particle found outside the nucleus of an atom

radiometric dating

used to calculate the number of half-lives that have passed since organic matter has been fossilized

single bond

one pair of shared electrons

double bond

2 pairs of shared electrons

triple bond

3 pairs of shared electrons

hydrogen bond

covalently bonded H atoms are partially positive, resulting in an attraction to electronegative particles

• attraction is the H bond

• easily broken

Atomic nucleus

densely packed protons and neutrons found at the center of an atom

energy

capacity to do work (cause change)

electronegativity

measure of how strongly an atom attracts electrons (mainly in chemical bonds)

• high electronegativity = stronger pull on electrons

Van der Waals Reaction

caused by randomly moving electrons creating regions with +/- charges that enable atoms to stick together

-individually weak bonds that happen in close proximity 

Specific heat

The resistance to change in temperature

Product

The resulting material in a chemical reaction

Reactant

Starting material in a chemical reaction

Acid

High level of hydrogen ions (H⁺) and low levels of hydroxide (OH^-)

pH under 7

Base

Low levels of hydrogen ions (H⁺) and high levels of hydroxide (OH^-)

pH over 7

Creation of Hydroxide

when H⁺ ion in water bonds to another water molecule leaving behind a water molecule that lost a proton (OH^-) with a charge of 1-

Buffer

substance that minimizes changes in concentration of H⁺ and OH^- by accepting H ions from solution when there is an excess and donating when H⁺ has been deplted

• i.e. carbonic acid in the blood

pH scale

reverse logarithm measure of H⁺ ions in an aqueous solution

Solution

Homogeneous mixture of 2 or more substances

Solvent

dissolving agent in a solution

Solute

the substance being dissolved in a solution

hydrophilic

water loving

• polar molecules (ions)

• dissolve in water