The Chemical Level Of Organization

Front 1

Chemistry

Back 1

the science of the structure and interactions of matter.

Front 2

Matter

Back 2

anything that occupies space and has mass.

Front 3

Mass

Back 3

The amount of matter in any object which does not change.

Front 4

Weight

Back 4

The force of gravity acting on matter, does change.

Front 5

Major Elements in the body

Back 5

CHON

Oxygen (O)

Carbon (C)

Hydrogen (H)

Nitrogen (N)

Front 6

Lesser Elements in the body

iMCCPPSS

Back 6

Iron (Fe)

Magnesium (Mg)

Calcium (Ca)

Chlorine (Cl)

Potassium (K)

Phosphorus (P)

Sulfur (S)

Sodium (Na)

Front 7

Atomic Number

Back 7

Number of protons in the nucleus

upper left of tile

Front 8

Mass Number

Back 8

Sum of its protons and neutrons

bottom of tile

Front 9

Element

Back 9

A substance that cannot be split into a simpler substance

Front 10

Atoms

Back 10

Smallest units of matter thatretain the properties and characteristics ofan element. Atoms are composedof subatomic particles: protons (+), neutrons and electrons (-).

Protons and neutrons make up the nucleus

Front 11

Chemical Symbol

Back 11

Letter in the center of tile

Front 12

Isitopes

Back 12

Atoms of an element that have different numbers ofneutrons

Front 13

Radioactive Isitopes

Back 13

are unstable. They give offparticles or energy in the form of radiation as theydecay into a more stable form.

Front 14

Tracers - Name one used in medicine

Back 14

Useful radioactive isotopes that follow moment of certain substance through the body.

Iodine-131 is used to detect cancer of the thyroid gland and to asses its size and activity, and may also be used to destroy part of an overactive thyroid gland.

Front 15

When an atom is in a neutral state

Back 15

the # of protons = the # ofelectrons

Front 16

Atomic Mass

Back 16

theaverage mass of all of an element’s isotopes – measured in Daltons

Front 17

Ion

Back 17

an atom that has lost or gained an electron

Front 18

Molecule

Back 18

formed when two or more atoms join together – ex. H2

Front 19

Compound

Back 19

a type of molecule that contains atoms of two or more different elements – ex. H20, but not H2

Front 20

A chemical bond occurs

Back 20

when atoms are held together by forces of attraction

- The number of electrons in the valence shell (outermost) determines the likelihood that an atom will form a chemical bond with another atom

Front 21

Families

Back 21

vertical rows of elements with similar traits

Front 22

Free Radical

Back 22

An atom with an unpaired electron in the outermost shell, which makes it unstable, highly reactive, and destructive to nearby cells.

Front 23

Ionic Bond

Back 23

The force of attraction that holds ions with opposite charges together:

Front 24

Cation and Anion

Back 24

Cation = positive ion (lost e-)

Anion = negative ion (gained e-)

Front 25

Covalent bond

Back 25

When two or more atoms share their electrons. Can be single, double, or triple

Front 26

Nonpolar Covalent

Back 26

atoms share e- equally; ex. CH4, O2, H2 (bonds between two identical atoms are always nonpolar)

Front 27

Polar Covalent

Back 27

atoms share e- unevenly; ex. H2O

creates a slightly neg or pos charge at one "pole" of the molecule

Front 28

Hydrogen bond

Back 28

A bond between two or more polar molecules that contain hydrogen. H-bonds create cohesion between molecules

– the tendency of molecules to stay together. This gives water a high surface tension

Front 29

Antioxidants

Back 29

Thought to slow the pace of damage causing free radicals.

Important dietary antioxidants include:

Selenium Zinc

Beta-carotene Vitamins C and E

Red, Blue, or purple fruits and vegetables contain high levels of antioxidants.

Front 30

Periodic Tile

Back 30

Name of Element

Atomic Number

Chemical Symbol

Atomic Mass

Front 31

Chemical Bond

Back 31

occurs when atoms are held together by forces of attraction

Front 32

Properties of Water

Back 32

Good solvent

hydrolysis -break down molecules

Dehydration synthesis

High capacity for heat and a high heat of vaporization

Good lubricant.

Front 33

Chemical Reactions

Back 33

occurs when new bonds are formed or old bonds are broken

Reactants – starting substances

Products – ending substances

Front 34

Law of Conservation of Energy

Back 34

Energy can be neither created or destroyed, but it can be converted from one form to another

Other forms of energy include chemical, mechanical, and electrical

Front 35

Exergonic vs Endergonic reactions

Back 35

Exergonic reactions – release more energy than they absorb

Endergonic reactions – absorb more energy than they release

Front 36

Activation energy

Back 36

the amount of energy needed to get a reaction started; influenced by: Concentration Temperature

Front 37

Catalyst

Back 37

Chemical compounds that speed up chemical reactions by lowering the activation energy

The most important catalysts in the human body are enzymes.

Front 38

Types of Chemical Reactions

Back 38

-Synthesis (anabolism) A + B AB

-Decomposition (catabolism) AB A + B

-Exchange (both) AB + CD AD + BC

-Reversible AB A + B

-Oxidation-reduction (Ch. 25)

Front 39

Inorganic vs. Organic Compounds

Back 39

Inorganic compounds usually lack carbon and are simple moleculesH2O is the most important and abundant inorganic compound in all living things

– makes up 55-60% of adult body The most common inorganic compound w/carbon is CO2

Organic compounds always contain C, usually contain H, and always have covalent bonds

Front 40

Acid, Base, and Salt

Back 40

Acid – dissociates into hydrogen ions

Base – dissociates into hydroxide ions

Acids and bases react with each other to form salts

Salt – dissociates into cations and anions, neither of which is H+ or OH-

Front 41

The pH Scale

Back 41

A change in one whole number represents a 10x change in value

Front 42

Ph value of blood

Back 42

7.35-7.45

slightly basic

Front 43

carbonic acid-bicarbonate buffer system

Back 43

carbonic acid-bicarbonate buffer system is an important system in the body. Because this reaction is reversible the same reaction can buffer either strong bases or strong acids.

Front 44

Carbon (Organic) Properties

Back 44

Carbon can from bonds with thousands of other carbon atoms to produce large molecules with many different shapes. It can bond with a variety of other atoms.Organic compounds do not dissolve easily in water.Organic compounds are held together by stable covalent bonds

Front 45

Functional Groups of Carbon

Back 45

Carbon Skeleton – The chain of carbon atoms that make up an organic molecule

Hydrocarbon – an organic molecule in which many of the carbon atoms are bonded to hydrogen atoms

Functional group – specific arrangements of other atoms or molecules that give an organic molecule a specific function.

Front 46

Carbohydrates

Back 46

Carbohydrates provide most of the energy needed for life

C6H12O6 - Chemical formula for glucose, fructose, and galactose

Front 47

Lipids

Back 47

Eicosanoids

Other Lipids

Carotenes

Vitamin E

Vitamin K

Lipoproteins

Front 48

Fatty Acids

Back 48

Saturated = only single bonds between carbon atoms

Unsaturated = one or more double bonds between carbon atoms

Front 49

Triglycerides

Back 49

lipids made up of a glycerol and 3 fatty acids; provide protection, insulation, and energy

Front 50

Phospholipids

Back 50

lipids made up of a glycerol, 2 fatty acids, and a phosphate group; important component of plasma membranes

Front 51

Proteins

Back 51

Large organic molecules that contain carbon, hydrogen, oxygen, and a nitrogen functional group called amines. Proteins are formed by combining various amino acids.Proteins give structure to the body, regulate processes, provide protection, assist in muscle contraction, transport substances, and serve as enzymes

Front 52

Nucleic Acids

Back 52

Contain C, H, O (sugars), N-bases and a phosphate group

Front 53

Adenosine Triphosphate (ATP)

Back 53

Three phosphate groups attached to an adenosine group; the principal energy-storing molecule in the body