Chapter 2

Front 1

Chemistry

Back 1

Science that deals with the structure or matter

Front 2

Matter

Back 2

Made up of atoms, takes up space, and has mass

Front 3

Mass

Back 3

The amount of material in matter, which determines weight. The mass of your body is the sum of the masses of all your atoms.

*Mass does not always equal weight!

Front 4

Atoms

Back 4

Smallest stable units of matter that retain the properties and characteristics of an element.

Front 5

Subatomic particles

Back 5

Proton, neutrons, electrons

Front 6

Nucleus

Back 6

Center of an atom. Contains protons and neutrons

Front 7

Atomic number

Back 7

Number of protons in an atom

Front 8

Element

Back 8

Pure substance made of just one kind of atom

Front 9

Isotopes

Back 9

Versions of the same element which have nuclei containing different mubrrs of neutrons

Front 10

Radioisotope

Back 10

An isotope who nucleus readily decays, giving off subatomic particles and electromagnetic energy

Front 11

Atomic weight

Back 11

An average of all the atomic masses of an element's different isotopes

Front 12

Mole

Back 12

A mole (mol) is the amount of a substance that contains 6.022 X 10^23 representative particles of that substance.

Front 13

Energy level

Back 13

The shell where an electronic lives; counted by how far from the nucleus

Front 14

Valence shell

Back 14

Outermost energy shell of an atom. Furthest from the nucleus

Front 15

Reactive

Back 15

Elements (atoms) with unfilled valence shells. Become stable by gaining or losing e- and filling valence shell

Front 16

Inert

Back 16

Elements without active chemical properties due to already having full valence shells

Front 17

Molecule

Back 17

Two or more atoms of same kind or different kind (O2 or H2O) but they share electrons

Front 18

Molecular formula

Back 18

Ex: CO2 means there is 1 carbon atom bonded to 2 oxygen atoms

Front 19

Compound

Back 19

Two or more different atoms bonded together, and it does not matter if they share or swap electrons

Front 20

Molecular weight

Back 20

Sum of all the atomic weights of its component atoms

Front 21

Chemical bond

Back 21

A weak or strong electrical attraction that holds atoms in the same vicinity

Front 22

Ionic bonds

Back 22

Form after a complete transfer of electrons from one atom to another

Front 23

Cation

Back 23

Atom that lost and electron (+ charge)

Front 24

Anion

Back 24

Atom that gained an electronic (- charge)

Front 25

Covalent bonds

Back 25

Sharing of electron pairs to complete a valence shell. Shared pairs or bonding pairs. Much more common than ionic bonds

Front 26

Nonpolar covalent bonds

Back 26

Equal sharing of electrons between atoms that have equal pull on the electrons

Front 27

Polar covalent bonds

Back 27

Unequal sharing of electrons because one atomhas a disproportionately strong pull on the electrons

Front 28

Free radicals

Back 28

Result when an atom, ion, or molecule contains unpaired electrons in its valence shell. Goes hunting for the missing electron, stripping it off anything it can. Can damage vital proteins (enzymes!)

Front 29

Surface tension

Back 29

How difficult it is to stretch or break the attraction of H+ bonds. The tendency of liquid surfaces to shrink into the minimum surface area possible.

Front 30

Solid

Back 30

Constant volume and shape

Front 31

Liquid

Back 31

Constant volume but changes shape

Front 32

Gas

Back 32

Changes volume and shape

Front 33

Chemical reaction

Back 33

New chemical bonds form between atoms OR existing bonds are broken

Front 34

Reactants

Back 34

Starting substances

Front 35

Products

Back 35

Ending substances

Front 36

Metabolism

Back 36

All chemical reactions taking place in cells or tissues at any given moment

Front 37

Energy

Back 37

The capacity to do work

Front 38

Work

Back 38

Movement of an object or change in matter

Front 39

Kinetic energy

Back 39

Energy of motion; transferred to object

Front 40

Potential energy

Back 40

Stored energy; converted back to kinetic

Front 41

Chemical energy

Back 41

Potential energy stored in chemical bonds

Front 42

Law of conservation

Back 42

Can neither be created nor destroyed but converted from one form of energy to another

Front 43

Concentration

Back 43

The more particles present, the more likely they are to collide (think of a crowded elevator or party).

Front 44

Temperature

Back 44

Particles move faster when heated up, causing them to collide with enough force to disrupt the valence shell e-

Front 45

Types of chemical reactions

Back 45

1. Decomposition (catabolism)

2. Synthesis (anabolism)

3.Exchange

4. Reversible

5. Oxidation-Reduction (OIL RIG)A

Front 46

Reversible reaction

Back 46

Decomposition and synthesis occurs at same time. Equation can go either way; depends on what is needed.

Front 47

Equilibrium

Back 47

When rate for conversion back and forth is the same

Front 48

Decomposition

Back 48

Breaks chemical bonds. Breaks a molecule into smaller fragments

Front 49

Catabolism

Back 49

Breaking covalent bonds to release kinetic E to do work in cells

Front 50

Hydrolysis reaction

Back 50

Breaking bonds by adding water

Front 51

Synthesis

Back 51

Makes chemical bonds. Assembling smaller molecules into new, larger ones

Front 52

Anabolism

Back 52

Synthesis of new products in the body. Uphill (energy required)

Front 53

Dehydration synthesis (condensation)

Back 53

Creating bonds by removing water

Front 54

Exchange

Back 54

Parts of the rwactants are shuffled to produce new products l. Involves decomposition first, then synthesis. No new components are added or rwmoved; just a new combination!

Front 55

Oxidation-Reduction

Back 55

The transfer of electrons

Front 56

OIL RIG

Back 56

Oxidation is loss, reduction is gained

Front 57

Reactivity

Back 57

Water serves as a relaxant in some reactions and chemical reactions in our bodies take place in water

Front 58

Specific heat capacity

Back 58

Heat capacity is the heat required to raise the temperature of a unit mass of a substance 1°C

Front 59

Lubrication

Back 59

Effective lubricant because so little friction between water molecules

Front 60

Solvent

Back 60

Dissolves another substance

Front 61

Solute

Back 61

The thing being dissolved

Front 62

Solution

Back 62

Uniform mixture of solvent and solute

Front 63

Dissociation

Back 63

Ionic compounds (salt, acids, bases) break apart in water

Front 64

Ionization

Back 64

Cations and anion result when dissociation occurs

Front 65

Hydration sphere

Back 65

Water isolates each cation and anion; they cannot form ionic bonds. This solution will conduct electricity!

Front 66

Electrolytes

Back 66

Inorganic ions that conduct electricity when dissolved in water

Front 67

Hydrophilic

Back 67

Water-loving. Includes ions and polar molecules. Interact with water

Front 68

Hydrophobic

Back 68

Includes nonpolar molecules, fats, and oils. Do not interact with water.

Front 69

Colloid

Front 70

Suspension

Back 70

Contains large particles that settle out of solution. Particles will precipitate; can measure a sedimentation rate (set rate).Ex: whole blood components will eventually fall to bottom of a beaker

Contains large particles that settle out of solution. Particles will precipitate; can measure a sedimentation rate (set rate).Ex: whole blood components will eventually fall to bottom of a beaker

Front 71

PH

Back 71

Measure of the hydrogen ions (H+) concentration of a solution. pH decreases as H+ concentration increases. The pH of water is Neutral 7

Front 72

Acidic

Back 72

pH lower then 7.0. High H+ concentration. Low OH- concentration

Front 73

Basic (or alkaline)

Back 73

pH lower than 7.0. Low H+ concentration. High OH- concetration

Front 74

Acid (proton donor)

Back 74

A solute that adds hydrogen ions to a solution. Dissociates into an H+ and anion

Front 75

Base (proton acceptor)

Back 75

A solute that removes hydrogen ions from a solution. Dissociated into an OH- and a cation

Front 76

Weak acids and weak bases

Back 76

Do NOT dissociate completely. Functions as buffer to balance the pH

Front 77

Salt

Back 77

Ionic compound containing any cation except H+ and any anion except OH-. Dissociate unto cations and anion in solution, as neutral solutes

Front 78

Buffers

Back 78

Stabilize pH of a solution by removing or replacing H+. Weak acids and its related slat, which functions as weak base

Front 79

Inorganic compound

Back 79

A substance that does not contain carbon bonded to hydrogen as their primary structure

Front 80

Organic compounds

Back 80

Molecules containing carbon and hydrogen

Front 81

Nutrients

Back 81

Essential molecules obtained from food

Front 82

Metabolites

Back 82

Molecules made or broken down in the body

Front 83

Monomer

Back 83

Single molecule that can be bonded to other identical molecules to form a polymer

Front 84

Polymer

Back 84

Repeating monomers joined together

Front 85

Proteins

Back 85

Organic molecule composed of amino acids linked by peptide bonds

Front 86

Primary structure

Back 86

The sequence of amino acids along a polypeptide - straight chain

Front 87

Secondary structure

Back 87

For to hydrogen bonding.

Aloha-helix (simple spiral) or beta-pleated sheets (flat sheet)

Front 88

Tertiary structure

Back 88

Coiling and folding produce three-dimensional shape

Front 89

Quarter nary structure

Back 89

Final protein complex produced by interacting polypeptide chains