Mr. Lindsay Unit 1 Exam Chapter 2

Front 1

Atom

Back 1

Smallest units of stable matter

Front 2

Matter

Back 2

Anything that has mass and takes up space

Front 3

Mass

Back 3

The amount of material in matter, determines weight on earth

Front 4

subatomic particles

Back 4

Atoms are composed of these; includes protons, neutrons and electrons

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protons

Back 5

p+, have a positive electrical charge

Front 6

Neutrons

Back 6

n or n0, are electrically neutral or uncharged

Front 7

electrons

Back 7

e-, are much lighter than protons

Front 8

nucleus

Back 8

the central region of an atom where the protons and neutrons are located

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atomic number

Back 9

number of protons in an atom

Front 10

electron cloud

Back 10

electrons traveling around the nucleus at a high speed, within a spherical area

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electron shell

Back 11

Electrons which occupy a circular shell around the nucleus. There are a certain number of electrons which occupy each shell. Example: the first shell holds two, second shell holds eight, third shell holds eight, etc.

Front 12

element

Back 12

a pure substance composed of atoms of only one kind

Front 13

isotopes

Back 13

atoms of the same element whose nuclei contain different numbers of neutrons

Front 14

mass number

Back 14

total number of protons plus neutrons in the nucleus, used to designate isotopes

Front 15

radioisotopes

Back 15

Isotopes with an unstable nucleus, meaning they spontaneously break down and give off subatomic particles or radiation in measurable amounts

Front 16

half-life

Back 16

the decay rate of a radioisotope

Front 17

atomic weight

Back 17

an average of the different atomic masses and proportions of an element's different isotopes

Front 18

mole

Back 18

a specific quantity with a weight in grams equal to that element's atomic weight

Front 19

valence shell

Back 19

the outermost energy level which forms the "surface" of the atom, or the amount of electrons in the outermost electron shell

Front 20

chemical bonds

Back 20

hold atoms, those which are reactive (atoms with unfilled outermost energy levels that readily interact or combine with other atoms) together once the reaction has ended

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molecule

Back 21

refers to any chemical structure consisting of atoms held together by shared electrons

Front 22

compound

Back 22

a pure chemical substance made up of atoms of two or more different elements in a fixed proportion, regardless of the type of chemical bond joining them

Front 23

molecular weight

Back 23

the molecular weight of a molecule or compound is the sum of the atomic weights of its component atoms

Front 24

ion

Back 24

is an atom or group of atoms that have a different electrical charge, either positive or negative

Front 25

cation

Back 25

ions with a positive charge, meaning they give up an electron(s) to another atom so they have less electrons than neutrons

Front 26

anion

Back 26

atoms with a negative charge, meaning they take on electron(s) from another atom so they have more electrons than neutrons

Front 27

ionic bonds

Back 27

are chemical bonds created by the electrical attraction between anions and cations

Front 28

single covalent bond

Back 28

The sharing of one pair of electrons. Example: Hydrogen (H2)

Front 29

double covalent bond

Back 29

The sharing of two pairs of electrons. Example: Oxygen (O2)

Front 30

nonpolar covalent bond

Back 30

covalent bonds which involve an equal sharing of electrons

Front 31

covalent bond

Back 31

very strong bonds between atoms because the shared electrons hold the atoms together

Front 32

polar covalent bonds

Back 32

covalent bonds which involve an unequal sharing of electrons. Example: In water (H2O) an oxygen atom forms covalent bonds with two hydrogen atoms. The oxygen nucleus (8 protons) has a much stronger attraction for the shared electrons than the hydrogen atoms (each with 1 proton). Thus the electrons spend more time orbiting the oxygen nucleus

Front 33

hydrogen bond

Back 33

Very weak bond. The attraction between a slight positive charge on the hydrogen atom of a polar covalent bond and a slight negative charge on the oxygen, nitrogen, or fluorine atom of another polar covalent bond. Example: hydrogen bonding occurs in water

Front 34

chemical reaction

Back 34

new chemical bonds form between atoms, or existing bonds between atoms are broken

Front 35

reactants

Back 35

The reacting substances of a chemical reaction which are rearranged to form different substances

Front 36

products

Back 36

the different substances which are formed as a result of a chemical reaction

Front 37

metabolism

Back 37

all the reactions under way in the cells and tissues of the body at any given moment

Front 38

work

Back 38

the movement of an object or a change in the physical structure of matter

Front 39

energy

Back 39

The capacity to do work, and movement or physical change cannot take place without energy. Two kinds: potential energy and kinetic energy

Front 40

Kinetic Energy

Back 40

The energy of motion, energy that can be transferred to another object and do work. Example: when you fall off of a ladder, it is kinetic energy that does the damage

Front 41

Potential Energy

Back 41

Stored energy; energy that has the potential to do work. It may derive from an object's position (you standing on the ladder) or from its physical or chemical structure (a stretched spring or a charged battery)

Front 42

Decomposition

Back 42

A decomposition reaction breaks a molecule into smaller fragments. Example: AB -> A+B

Front 43

Hydrolysis

Back 43

In hydrolysis, one of the bonds in a complex molecule is broken, and the components of a water molecule (H and OH) are added to the resulting fragments.

Example: A-B+H2O -> A-H+HO-B

Front 44

Catabolism

Back 44

The decomposition reactions of complex molecules within the body's cells and tissues

Front 45

Synthesis

Back 45

The opposite of decomposition. A synthesis reaction assembles smaller molecules into larger molecules. Example: A+B -> AB

Front 46

Dehydration Synthesis

Back 46

Or, condensation reaction, is the formation of a complex molecule by the removal of a water molecule. Example: A-H+HO-B -> A-B+H2O

Front 47

Exchange Reactions

Back 47

When parts of reacting molecules are shuffled around to produce new products. Example: AB+CD -> AD+CB

Front 48

Enzymes

Back 48

Promote chemical reactions by lowering the activation energy required. Belong to the catalyst class. Enzymes only affect the rate of the reaction, not its direction or the products formed

Front 49

Catalyst

Back 49

Compounds that speed up chemical reactions without themselves being permanently changed or consumes

Front 50

Exergonic

Back 50

Reactions that release energy.

Front 51

Endergonic

Back 51

Reactions where more energy is required to begin the reaction than is released as it proceeds; energy is absorbed.

Front 52

Inorganic Compounds

Back 52

Generally do not contain carbon and hydrogen atoms as their primary structural ingredients. Example: Carbon Dioxide, Oxygen, water, inorganic acids bases and salts

Front 53

Organic Compounds

Back 53

Carbon and hydrogen always for the basis for organic compounds.

Front 54

Activation Energy

Back 54

The amount of energy required to start a reaction

Front 55

Solution

Back 55

A uniform mixture of two or more substances. Example: salt dissolves in water making the solution of salt water

Front 56

Solutes

Back 56

The dissolved substances in a solution. Example: the salt in salt water

Front 57

Solvent

Back 57

The liquid in which other atoms, ions, or molecules are distributed in a solution. Example: the water in salt water

Front 58

Polar Molecule

Back 58

A molecule with positive and negative ends, or poles. Example: a water molecule

Front 59

Nonpolar Molecule

Back 59

A molecule with the same charge at both ends

Front 60

Ionization

Back 60

AKA dissociation. In this process, ionic bonds are broken as the individual ions interact with the positive or negative ends of polar water molecules. Example: Sodium Chloride is an ionic compound and when it is in water it dissociates as the polar water molecules break the ionic bonds in the large crystal structure. Each sodium chloride molecule is surrounded by water molecules, creating a hydrogen sphere

Front 61

Electrolytes

Back 61

Soluble inorganic substances whose ions will conduct an electrical charge. Example: Sodium Chloride in a solution is an electrolyte

Front 62

Hydrophilic

Back 62

Molecules that readily interact with water molecules. Example: glucose molecule

Front 63

Hydrophobic

Back 63

Molecules that do not readily interact with water. Example: fats and oils

Front 64

Colloid

Back 64

A solution containing dispersed proteins or other large molecules. Particles or molecules in a colloid will remain in a solution indefinitely

Front 65

Suspension

Back 65

Contains large particles in solutions, but if undisturbed, its particles will settle out of solution due to the force of gravity

Front 66

pH

Back 66

The pH of an atoms is defined as the negative logarithm of the hydrogen ion concentration in moles per liter

Front 67

Base

Back 67

A solute that removes hydrogen ions from a solution, raising the pH. If the pH is above 7, meaning it has more hydroxide ions than hydrogen ions, it is said to be basic or alkaline

Front 68

Acid

Back 68

Any solute that dissociates in solution and releases hydrogen ions, lowering pH. If the pH of a solution is lower than 7, meaning it contains more hydrogen ions than hydroxide ions, it is said to be acidic

Front 69

Salt

Back 69

An inorganic compound containing any cation except a hydrogen ion, and any anion except a hydroxide ion.

Front 70

Buffer

Back 70

A compound that stabilizes the pH of a solution by removing or replacing hydrogen ions. Example: Alka-Seltzer uses sodium bicarbonate to neutralize excess hydrochloric acid in the stomach

Front 71

Carbohydrate

Back 71

An organic molecule that contains carbon, hydrogen, and oxygen in a ratio near 1:2:1. Examples: sugar, starches; 3 classes: monosaccharides, disaccharides, and polysaccharides

Front 72

Monosaccharide

Back 72

AKA simple sugar, a carbohydrate with 3-7 carbon atoms, triose (3 carbon), tetrose (4 carbon), pentose (5 carbon), hexose (6 carbon), or hexose (7 carbon). Example: a hexose glucose, C6H12O6

Front 73

Disaccharide

Back 73

Two monosaccharides joined together. Example: sucrose, table sugar

Front 74

Polysaccharide

Back 74

When additional monosaccharides are added to disaccharides via dehydration synthesis. Example: cellulose, comes from plants, cannot be broken down by the body

Front 75

Sucrose

Back 75

A disaccharide

Front 76

Glucose

Back 76

A monosaccharide

Front 77

Glycogen

Back 77

Or animal starch, has many sided branches consisting of chains of glucose molecules; cannot be broken down by water

Front 78

Starches

Back 78

Large polysaccharides formed from glucose molecules, can be broken down into monosaccharides via hydrolysis

Front 79

Lipids

Back 79

Contain carbon, hydrogen and oxygen and the carbon-to-hydrogen ratio is near 1:2 with a small oxygen ration. Five classes: fatty acids, eicosanoids, glycerides, steroids, and phospholipids and glycolipids

Front 80

Fatty Acids

Back 80

long carbon chains with hydrogen atoms attached. One end of the carbon chain is always attached to a carboxyl group (COOH). Saturated or unsaturated

Front 81

Unsaturated

Back 81

Fatty acid where one or more of the single covalent bonds between the carbon atoms is replaced by a double covalent bond. As a result, carbon atoms will only bind with one hydrogen atom instead of two. Monounsaturated=single double bond in hydrocarbon tail. Polyunsaturated=two or more double bonds

Front 82

Saturated

Back 82

Fatty acid where each carbon atom in the tail has four single covalent bonds. Two bind adjacent carbon atoms and the other two bind hydrogen atoms

Front 83

Glycerol

Back 83

The modified simple sugar needed to string fatty acids together

Front 84

glyceride

Back 84

when a simple sugar called glycerol is combined with a fatty acid

Front 85

triglyceride

Back 85

glycerol + 3 fatty acids

Front 86

Steroids

Back 86

large lipid molecules that share a distinctive four-ring carbon framework. Individual steroids differ in the side chains attached to the carbon rings. Example: cholesterol, estrogen, testosterone.

Front 87

phospholipids

Back 87

When a phosphate group links a diglyceride to a non-lipid group

Front 88

Proteins

Back 88

The most abundant organic compounds in the body. There are 7 essential functions of a protein including: support, movement, transport, buffering, metabolic regulation, coordination and control, and defense

Front 89

Amino Acid

Back 89

Long chains of organic molecules in proteins. Each amino acid consists of 5 parts: a central carbon atom, a hydrogen atom, an amino group (-NH2), a carboxile group (-COOH), and an R group (a variable side chain of one or more atoms)

Front 90

Peptide Bond

Back 90

When dehydration synthesis is used to link two amino acids which creates a covalent bond between the carboxyl group of one amino acid and the amino group of another

Front 91

Tertiary Structure

Back 91

The complex coiling and folding that gives a protein its final 3d shape

Front 92

Quaternary Structure

Back 92

The interaction between individual polypeptide chains to form a protein complex

Front 93

Denaturation

Back 93

When a protein undergoes a change in tertiary or quaternary structure that makes it nonfunctional

Front 94

substrates

Back 94

the reactants in enzymatic reations

Front 95

active site

Back 95

the special region of the enzyme where substrates must bind before the substrates can yield specified products

Front 96

Nucleic Acids

Back 96

large organic molecules composed of carbon, hydrogen, oxygen, nitrogen, and phosphorus. They store and process information at the molecular level inside cells. Two classes: DNA and RNA

Front 97

DNA

Back 97

Deoxyribonucleic acid molecules encode the information needed to build proteins. Regulates not only protein synthesis, but also all aspects of cellular metabolism, including the creation and destruction of lipids, carbohydrates, and other vital molecules

Front 98

RNA

Back 98

Ribonucleic acid cooperates with DNA to build specific proteins by using the information provided by DNA.

Front 99

Adenine

Back 99

Double ringed molecule called purines, DNA only, combines with Thymine

Front 100

Thymine

Back 100

Single ringed molecule, combines with Adenine in DNA and Uracil in RNA

Front 101

Uracil

Back 101

Single ringed, combines with Thymine, RNA only

Front 102

Cytosine

Back 102

Combines with Guanine in DNA and RNA

Front 103

Guanine

Back 103

combines with cytosine in DNA and RNA

Front 104

Adenosine triphosphate

Back 104

ATP, adenosine (adenine + ribose) + 3 phosphates combine to create this high energy compound

Front 105

Complementary base pairs

Back 105

In DNA, (A-T) and (C-G)

Front 106

Double Helix

Back 106

consists of two complimentary strands which twist around one another