Chapter 2 Bio

Front 1

Matter

Back 1

The matter that makes up every object consists of one or more elements that organize into atoms and molecules.

Front 2

Energy

Back 2

physics, the capacity for doing work. It may exist in potential, kinetic, thermal, electrical, chemical, nuclear, or other various forms.

Front 3

Element

Back 3

a substance that cannot be broken down by chemical means into other substances.

Front 4

Periodic table

Back 4

List all known elements

Front 5

Bulk element

Back 5

Living organisms contain relatively large amounts of oxygen, carbon, hydrogen, nitrogen, and sulfur (these five elements are known as the bulk elements), along with sodium, magnesium, potassium, calcium, chlorine, and phosphorus

Front 6

Trace elements

Back 6

a chemical element present only in minute amounts in a particular sample or environment.

Front 7

Atoms

Back 7

the smallest piece of an element that retains the characteristics of the element.

Front 8

Proton

Back 8

a stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal in magnitude to that of an electron, but of opposite sign.

Front 9

Neutron

Back 9

a subatomic particle of about the same mass as a proton but without an electric charge, present in all atomic nuclei except those of ordinary hydrogen.

Front 10

Electron

Back 10

surround the atomic nucleus. They are very small and move very fast.

Front 11

Nucleus

Back 11

an organelle found in eukaryotic cells. Inside its fully enclosed nuclear membrane, it contains the majority of the cell's genetic material. This material is organized as DNA molecules, along with a variety of proteins, to form chromosomes.

Front 12

Atomic number

Back 12

indicates how many protons are in each atom of that element.

Front 13

Ion

Back 13

defined as an atom or molecule that has gained or lost one or more of its valence electrons, giving it a net positive or negative electrical charge.

Front 14

Mass number/ atomic mass

Back 14

An atom’s mass number is the total number of protons and neutrons in its nucleus.

The mass number of the carbon atom shown below is 12.

Front 15

Isotope

Back 15

any of these different forms of the element.

Front 16

Atomic weight

Back 16

the mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes

Front 17

Radioactive

Back 17

the spontaneous emission of radiation in the form of particles or high energy photons resulting from a nuclear reaction. ... A substance that contains unstable atomic nuclei is considered to be

Front 18

Molecule

Back 18

a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction

Front 19

Compound

Back 19

substance formed when two or more chemical elements are chemically bonded together.

Front 20

Orbital

Back 20

describes properties characteristic of no more than two electrons in the vicinity of an atomic nucleus or of a system of nuclei as in a molecule.

Front 21

Energy shells

Back 21

Energy shells, or orbitals, contain the atom’s electrons.Shells exist at various distances from the atom’s nucleus. The shell farthest from the nucleus is important for bonding.

Front 22

Valence shells

Back 22

an electron of an atom, located in the outermost shell (valence shell) of the atom, that can be transferred to or shared with another atom.

Front 23

Electronegativity

Back 23

measure of how strongly atoms attract bonding electrons to themselves.

Front 24

Chemical bond

Back 24

physical phenomenon of chemical substances being held together by attraction of atoms to each other through sharing, as well as exchanging, of electrons -or electrostatic forces.

Front 25

Ionic bond

Back 25

the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions

Front 26

Covalent bond

Back 26

When atoms share electrons, as in this methane molecule

Front 27

Polar covalent bond

Back 27

a pair of electrons is unequally shared between two atoms.

Front 28

Non- polar covalent bond

Back 28

where two atoms share a pair of electrons with each other.

Front 29

Hydrogen bond

Back 29

attraction between the positive and negative poles of charged atoms.

Front 30

Cohesive

Back 30

the tendency of water molecules to stick to one another.Cohesion between molecules on the surface of liquid water give it high surface tension.

Front 31

Adhesive

Back 31

Water molecules also form hydrogen bonds with other molecules,

Front 32

Solvent

Back 32

able to dissolve other substances.

Ex. Water is a excellent solvent

Front 33

Solute

Back 33

the minor component in a solution, dissolved in the solvent.

Front 34

Solution

Back 34

homogeneous mixture of two or more substances.

For example, in a saline solution, salt is the solute dissolved in water as the solvent

Front 35

Hydrophilic

Back 35

having a tendency to mix with, dissolve in, or be wetted by water.

Front 36

Hydrophobic

Back 36

tending to repel or fail to mix with water.

Front 37

Evaporation

Back 37

the process of a substance in a liquid state changing to a gaseous state due to an increase in temperature and/or pressure.

Front 38

Density

Back 38

measure of mass per unit of volume.

Front 39

Chemical reactions

Back 39

a process in which one or more substances, the reactants, are converted to one or more different substances, the products.

Front 40

Reactants

Back 40

Water is a reactant in reactions that build and break down all classes of biological molecules

Front 41

Products

Back 41

a substance that is formed as the result of a chemical reaction

Front 42

Neutral

Back 42

when it is not positively or negatively charged. All atoms are neutral. This is because all atoms have equal numbers of positively charged protons and negatively charged electrons, leading to overall neutral charge.

Front 43

Acid

Back 43

a chemical species that donates protons or hydrogen ions and/or accepts electrons. Most acids contain a hydrogen atom bonded that can release (dissociate) to yield a cation and anion in water.

Front 44

Base

Back 44

a chemical species that donates electrons, accepts protons, or releases hydroxide (OH-) ions in aqueous solution.

Front 45

Ph scale

Back 45

shows the amount of H^+ ions in solutions

Front 46

Alkaline

Back 46

defined as a base that dissolves in water. A solution of a soluble base has a pH greater than 7.0.

Front 47

Buffers

Back 47

help maintain a constant pH by absorbing or releasing "H" ^+ into a solution.

Front 48

Organic molecules

Back 48

contains both carbon and hydrogen. Methane is a simple organic molecule.

Front 49

Monomers

Back 49

a single unit of a carbohydrate, protein, or nucleic acid. Monomers join to form polymers.

Front 50

Polymers

Back 50

is a molecule, made from joining together many small molecules called monomers.

Front 51

Dehydration synthesis

Back 51

a type of chemical reaction. joins monomers together

Front 52

Hydrolysis

Back 52

breaks polymers apart

a type of chemical reaction.

Front 53

Carbohydrates

Back 53

include simple sugars and polysaccharides

synthesis and breakdown

Front 54

Monosaccharides

Back 54

simple sugars; they are the monomersthat make up larger carbohydrates.

Front 55

Disaccharides

Back 55

a carbohydrate that is formed when two monosaccharides are joined together and a molecule of water is removed from the structure.

Front 56

Oligosaccharide

Back 56

A carbohydrate consisting of a relatively small and specifiable number of monosaccharides joined together.

Ex. Lactose, maltose, and sucrose are oligosaccharides consisting of two simple sugars.

Front 57

Polysaccharide

Back 57

long chains of carbohydrates.

Front 58

Protein

Back 58

the “workers” of cells; they do almost everything.

Proteins like collagen create cellular structures.

Proteins like actin and myosin produce muscle contractions.

Front 59

Amino Acid

Back 59

The monomers of proteins

There are 20 different amino acids in nature.

All amino acids have the same general structure.

Front 60

R Group

Back 60

The 20 different amino acids have 20 different R-groups.

Some are polar, some are nonpolar, some are charged.

Some are small, some are medium, some are bulky.

Front 61

Peptide Bond

Back 61

a chemical bond formed between two molecules when the carboxyl group of one molecule reacts with the amino group of the other molecule, releasing a molecule of water

Front 62

Polypeptide

Back 62

a string or linear chain of amino acids linked together. Amino acids are the basic building blocks of proteins.

Fold up into protein

Front 63

Primary Structure

Back 63

Amino acid (sequence) of a polypeptide

Front 64

Secondary Structure

Back 64

Substructure

Localized areas of coils, sheets, and loops within a polypeptide

Front 65

Tertiary Structure

Back 65

Overall shape of one (polypeptide shape)

Front 66

Quaternary Structure

Back 66

Overall (protein shape), arising from interaction between the multiple polypeptides that make up the functional protein. Only proteins with multiple polypeptides have quaternary structure.

Front 67

Denature

Back 67

Lose their shape

Front 68

Nucleic Acid

Back 68

include DNA and RNA.

The primary structure of each protein in a cell is determined by the nucleic acids.

Front 69

Deoxyribonucleic Acid

Back 69

a molecule that encodes an organism's genetic blueprint. In other words, DNA contains all of the information required to build and maintain an organism.

Front 70

Ribonucleic Acid

Back 70

which is a long, single-stranded chain of cells that processes protein. An example of RNA

Front 71

Nucleotide

Back 71

any of several compounds that consist of a ribose or deoxyribose sugar joined to a purine or pyrimidine base and to a phosphate group and that are the basic structural units of nucleic acids (such as RNA and DNA) — compare nucleoside.

Front 72

Lipids

Back 72

a collection of different hydrophobic molecules

Front 73

Triglyceride

Back 73

(fats and oils), are energy-rich. We need them for long-term energy storage.

Front 74

Fatty Acids

Back 74

a carboxylic acid (-C(=O)OH), with a long unbranched hydrocarbon tail. It is studied in organic chemistry and biochemistry. Fatty acids are important sources of body fuel.

Front 75

Glycerol

Back 75

Triglycerides are formed by covalently attaching three fatty acid molecules to a glycerol molecule.

Front 76

Saturated Fatty Acid

Back 76

bonded to four other atoms. This makes the fatty acid have a straight shape.

Front 77

Unsaturated Fatty Acid

Back 77

acid contains at least one double bond, which gives the fatty acid a bent shape.

Front 78

Trans Fat

Back 78

Trans fat (solid at room temperature)

Front 79

Steroids

Back 79

another group of lipids. They have a 4-ring structure.

Front 80

Waxes

Back 80

composed of fatty acids combined with alcohols.

This class of lipid is particularly hydrophobic.

In nature, waxes form waterproof seals, such as the cuticle that stops leaves from drying out.