Chapter 2

Front 1

Matter

Back 1

All such tangible materials that occupy space and have mass.

Front 2

Atoms

Back 2

Tiny particle that cannot be subdivided into smaller substances without losing its properties. Building blocks.

Front 3

Elements vs isotopes

Back 3

Elements are a varied combinations of subatomic particles (electrons, protons, neutrons) form unique type of atoms-pure, structural and predictable behavior

Isotopes are unstable, various forms of the same element that differ in the number of neutrons and have different mass numbers.

Front 4

Protons

Back 4

Subatomic particles which are positively charged

Front 5

Electrons

Back 5

Subatomic particles which are negatively charged.

Front 6

Neutrons

Back 6

subatomic particles which have no charge, neutral.

Front 7

Element

Back 7

When subatomic particles come together in specific, varied combinations, unique types of atoms structural and predictable chemical behavior.

Front 8

Atomic Number

Back 8

Each element is assigned a atomic number (AN)based on the number of protons.

Front 9

Mass Number

Back 9

Useful measurement equal to the number of protons and neutrons.

*Subtract the mass number and the atomic number to determine the number of neutrons .

Front 10

Isotopes

Back 10

Variant forms of the same element that differ in the number of neutrons and thus have different mass numbers.

Front 11

Atomic Weight

Back 11

An important measurement of a element that gives the average mass numbers of all isotopic forms.

Front 12

Biological Important Elements

Back 12

the following elements comprise 97% of the dry mass in living cells.

47% Carbon

30% Oxygen

9% Hydrogen

8% Nitrogen

3% Phosphorous

2% Sulfur, Potassium, Calcium, Sodium,

Chlorine, Magnesium.

1% others.

Front 13

Abbreviations of Elements

Back 13

Ca Calcium I-131 Iodine*

C Carbon Fe Iron

C-14 Carbon* Mg Magnesium

Cl Chlorine Mn Magnese

Co Cobalt N Nitrogen

Cu Copper O Oxygen

H Hydrogen P Phosphorous

H-3 Hydrogen* P-32 Phosphorous*

K Potassium Na Sodium

S Sulfur Zn Zinc

I Iodine

Front 14

Isotopes of the same element

Back 14

If two atoms have the same number of protons and electrons but different numbers of neutrons.

Front 15

Electron Orbital Shells

Back 15

The number of electrons in the outer shells is an indicator of how reactive the atom will be.

Front 16

Molecule

Back 16

Chemical substance that results from the combination of two or more atoms.

ex. H20-cannot be accompanied.

Front 17

Compound

Back 17

Molecules that are combinations of two or more different elements. Can be a molecule.

Front 18

Formula/Mass weight

Back 18

Sum of all the atomic masses of the atoms a

molecule contains.

Front 19

Chemical bonds

Back 19

when 2 or more atoms share, donate, or accept electrons to form molecules and compounds.

3 basic types:

1) Covalent

2) Ionic

3) Hydrogen

Front 20

Covalent bonds

Back 20

Electrons are shared among atoms.

* Molecules are stable when outer shells are full. Example: Hydrogen bond, Methane gas.

Front 21

Polar covalent bonds

Back 21

Unequal sharing or distribution of charges-

it has positive and negative poles.

ex. H20. the oxygen atom is larger and has more protons than the hydrogen atoms, it will have a stronger attraction than the hydrogen atoms. Electrons spend more time with O2.

Front 22

Nonpolar covalent bonds

Back 22

Electrons are shared equally between two atoms. This balanced distribution, no part of the molecule has a greater attraction for the

electrons makes this molecule electrically

neutral.

Front 23

Polarity

Back 23

When covalent bonds occur between two atoms with different atomic masses, the electrons tend to spend more time toward the larger atom (more electronegativity)

Front 24

Ionic bonds

Back 24

Electrons are transferred to one atom forming positively charged cations, negatively charged anions.

If one atom is so charged that is pulls an electron from the other atom.

NaCl

Front 25

Hydrogen bonds

Back 25

Weak bonds between water molecules. Formed when more electronegative oxygen attracts the electrons.

Front 26

Oxidation

Back 26

The loss of electrons such as sodium loses its electron to chlorine and becomes more positively charged ion - cation

Front 27

Reducing agent (Na)

Back 27

When sodium donates a electron to chlorine it becomes the Reducing agent because it reduced another atom.

Front 28

Reduction

Back 28

The gaining of electrons and coverts to a anion.

Like chlorine does when it receives a electron from sodium.

Front 29

Oxidizing agent

Back 29

An atom that receives a extra electron oxidizes another molecule making more positively charged.

ex. chlorine in NaCl

Front 30

Redox reactions

Back 30

Oxidation-reduction reaction. When electrons are transferred from one atom or molecule to another.

Front 31

Reactants

Back 31

Molecules involved and starting a reaction and that are changed by the reaction.

Front 32

Products

Back 32

Substances left by the reactions

Front 33

Synthesis reaction

Back 33

The reactants bond together in a manner that produces an entirely new molecule.

S + O2 > SO2

Front 34

Decomposition Reaction

Back 34

The bonds on a single reactant molecule are broken to release two or more products

2H2O2 > 2H2O + O2

Front 35

Exchange Reaction

Back 35

The reactants trade portions between each other and release products that are a combination of two.

HCL + NaOH > NaCL + H2O

Front 36

Solution

Back 36

a mixture of one or more substances called solutes in solvent.

Front 37

Solutes

Back 37

one or more substances uniformly dispersed in a dissolving medium.

Front 38

Solvent

Back 38

a medium.

Front 39

Hydrophilic molecules

Back 39

dissolve in water

Front 40

Hydrophobic molecules

Back 40

repel water

Front 41

Amphipathic molecules

Back 41

have both hydrophilic and hydrophobic properties.

example: soap, or phospholipid.

Front 42

Acidity (acidic)

Back 42

Ionization of H2O releases excess hydrogen [H+].

PH below 7.

Front 43

Alkalinity (Basic)

Back 43

When a component releases excess hydroxide ions . Anything above pH of 7.

Front 44

pH scale

Back 44

0-14

example: pH 2 contains [0.01 moles H+/L]

pH 2 has an [H+] of 10-2

Front 45

Organic chemicals

Back 45

compounds containing carbon bonded hydrogens.

Front 46

Carbon

(backbone or organic compounds)

Back 46

*contains 4 atoms in its outer orbital.

*can form single, double, or triple covalent bonds.

*can form linear, branched, or ringed molecules.

Front 47

Inorganic

Back 47

a chemical that usually does not contain both carbon and hydrogen.

ex: H2O, O2, NaCl, Mg3(PO4)2

Front 48

Functional group

Back 48

Accessory molecules that bind to organic

compounds.

confer unique reactive properties on the whole

molecule.

Hydroxyl, Carboxyl, Amino, Ester, Sulfhydryl,

carbonyl, phosphate.

Front 49

Macromolecules

Back 49

Biochemicals are organic compounds produced by living things.

Large compounds assembled from smaller

subunits.

Front 50

Monomer

Back 50

a repeating unit or subunits except lipids are formed by polymerization.

Front 51

Polymer

Back 51

a chain of monomers bound into chains of various lengths.

Front 52

4 basic macromolecules

Back 52

1) carbohydrates

2) lipids

3) proteins

4) nucleic acids.

Front 53

Carbohydrates

Back 53

Monosaccharides -

3-7 carbon sugars. Glucose, fructose

Disaccharides-

two monosaccharides. Maltose, Lactose,

Sucrose.

Polysaccharides-

chain of monosaccharides. starch, cellulose,

Front 54

Lipids

Back 54

Triglycerides

fatty acids+glycerol - fats, oils, storage.

Phospholipids

fatty acids + glycerol + glycerol. Membranes

waxes

fatty acids + alcohols - mycolic acid

steroids

ringed structures - cholesterol, ergosterol

Front 55

Proteins

Back 55

polypeptides

amino acids in chain bound by peptide bonds -

enzymes.

Front 56

Nucleic acids

Back 56

Nucleotides - Purines.

Deoxyribonucleic acid (DNA) -

Front 57

Carbohydrates

Back 57

Saccharide- simple carbohydrates

-Monosaccharide: 3-7 carbons

-Disaccharide: two monosaccharides

-Polysaccharide: five or more monosaccharides.

Functions: cell structure, adhesion, metabolism and energy.

Front 58

Carbohydrates

Back 58

*subunits linked by glycosidic bonds of disaccharides, and polysaccharides.

Front 59

Dehydration synthesis

Back 59

loss of water in a polymerization reaction. Polymerization forms polymers.

Front 60

Lipids

Back 60

Diverse group: insoluble in water, hydrophobic.

-long or complex, phospholipid in membranes, steroids like cholesterol.

Functions:

Triglycerides-energy storage.

Phospholipid- major cell membrane

component

Steroids- cell membrane component.

Front 61

Triglycerides

Back 61

3 fatty acids bound to glycerol.

*triglycerides are used for energy storage-

no double bonds.

* could be saturated or unsaturated

saturated-no double bonds

unsaturated-a lot of double bonds.

Front 62

Phospholipid

Back 62

major cell membrane component- polar and

unipolar, phosphate group.

glycerol with 2 fatty acids and a phosphate group

*bilayers of phospholipids form membranes.

Front 63

Steroids

Back 63

cell membrane component- cholesterol.

Front 64

Proteins

Back 64

predominant molecules in cells

Monomer- amino acids- 20 different naturally

occurring forms make up protein, backbone carbon. Amino & carboxyl.

polymer-peptide, polypeptide, protein.

Functions: support enzymes, transport, defense and movement.

Front 65

Proteins

Back 65

* subunits linked by peptide bonds

* fold into very specific 3-D shapes

* Functions: support, enzymes, transport, defense, movement.

Front 66

Amino Acids

Back 66

Are the monomers that make up protein

polymer.

-are attached through peptide bonds to form

proteins.

Front 67

Nucleic Acids

Back 67

* DNA and RNA

* Nucleotide monomer

* DNA- deoxyribonucleic acid- A,T,C,G

double helix, function-heredity material

- deoxyribose.

* RNA- ribonucleic acid- A,U,C,G-nitrogen bases

function- organize protein synthesis, single

strand.

- ribose

Front 68

Nucleotide Components (heredity material)

Back 68

*DNA Nucleotides

Doxyribose

C,G,A, or T

Double helix

* RNA Nucleotides:

Ribose

C,G,A or U

single strand

Front 69

Double Helix of DNA

Back 69

*DNA is formed by two very long polynucleotide strands linked along their length by hydrogen bonds.

*each stand is copied.

* replication is guided by base pairing.

* End result is two separate double strands.

Front 70

ATP

Back 70

The energy molecule of cells

* adenosine triphosphate

-Nucleotide-adenine, ribose, three phospates

* Function- transfer and storage of energy.