Bio Ch.2

Front 1

electromagnetically

Back 1

ability of an atom to form electrons

Front 2

negative charged subatomic particles outside the nucleus

Back 2

electron

Front 3

___ of an atom will pull electrons towards it

Back 3

nucleus

Front 4

stronger or weaker electron have more electrons around it more often

Back 4

stronger

Front 5

Atoms sharing electrons drift apart or stay together?

Back 5

stay together

Front 6

biology is based on the principles of __ and __

Back 6

Chemistry and physics

Front 7

All living organisms are a collection of __ and __

Back 7

Atoms and molecules

Front 8

Multiple forms of an element that differ in the number of neutrons

Back 8

Isotopes

Front 9

C12 contains __ protons and __ neutrons

Back 9

6

6

Front 10

C14 contains __ protons and __ neutrons

Back 10

6

8

Front 11

Averages of the weights of different isotopes of an element

Back 11

Average masses

Front 12

Make up 95% of the atoms in a living organism (4 elements)

Back 12

Carbon

Hydrogen

Oxygen

Nitrogen

Front 13

Hydrogen and oxygen are found primarily in this element

Back 13

Water

Front 14

Nitrogen is mainly found in what?

Back 14

protein

Front 15

Building block of all living matter

Back 15

Carbon

Front 16

Mineral elements make up what percent of living things?

Back 16

Less than 1%

Front 17

Trace elements make up what percent of living things?

Back 17

0.01%

Front 18

Trace elements are crucial for normal __ and __

Back 18

Growth

Function

Front 19

Two or more atoms bonded together

Back 19

Molecule

Front 20

Contains chemical symbols of elements found in a molecule

Back 20

Molecular formula

Front 21

What in the molecular formula indicates how many of each atom are present

Back 21

Subscript

Front 22

Molecule composed of two or more elements

Back 22

Compounds

Front 23

Three types of bonding

Back 23

Covalent

- polar and nonpolar

Hydrogen

Ionic

Front 24

Type of bonding where atoms share two electrons

Back 24

covalent

Front 25

bonding that occurs between two atoms whose outer electron shells are not full

Back 25

covalent

Front 26

Say the Octet rule

Back 26

Atoms are stable when their outer shell is full

Front 27

For many atoms, their outer shell is filled with how many electrons?

Back 27

8

Front 28

How many electrons can hydrogen hold in it's outer shell

Back 28

2

Front 29

Water is the classic example of what kind of bonding

Back 29

Polar covalent bonding

Front 30

what type of bonding occurs between molecules having polar covalent bonds (between polar molecules)?

Back 30

Hydrogen bonds

Front 31

Bonding represented on diagrams by dashed/ dotted lines

Back 31

Hydrogen bonds

Front 32

This generally weak bond when it is individual can form a strong bond overall

Back 32

hydrogen bonds

Front 33

What type of bonds hold two DNA strands together

Back 33

Hydrogen bonds

Front 34

Substrate and enzyme bonding is what kind of bonding?

Back 34

Hydrogen

Front 35

An atom or molecule that has gained or lost one or more electrons

Back 35

Ion

Front 36

What kind of net charge does an ion have?

Back 36

electric

Front 37

Cations have a net _ charge

Back 37

+

Front 38

Anions have a net _ charge

Back 38

-

Front 39

Bonding that occurs when a cation binds to an anion

Back 39

Ionic

Front 40

Occurs when one or more substances are changed into other substances

Back 40

Chemical reactions

Front 41

Chemical reactions

Reactants ---> ____

Back 41

products

Front 42

All chemical reactions require a source of _

Back 42

Energy

Front 43

All chemical reactions with living organisms often require a..

Back 43

Catalyst

Front 44

Catalyst

Back 44

Enzymes

Front 45

Tend to proceed in a particular direction and will eventually reach equilibrium

Back 45

Chemical reactions

Front 46

Chemical reactions occur in what kind of environment?

Back 46

Liquid environment

Front 47

Solvent

Back 47

Liquid

Front 48

Which two subatomic particles are nearly equal in size?

Protons

Electons

Neutrons

Back 48

Protons

Neutrons

Front 49

Term stating an atom's mass relative to the mass of other atoms

Back 49

Atomic Mass

Front 50

Atomic mass of hydrogen

Back 50

1

Front 51

Atomic mass of magnesium

Back 51

24

Front 52

When 2 atoms with difference electronegatives form a covalent bond, will more shared electrons be in the outer shell of the more electronegative one or the less?

Back 52

More

Front 53

This bond occurs because the distribution of electrons around the atoms creates a polarity in electric charge across the molecules

Back 53

Polar covalent bonds

Front 54

Polarity

Back 54

Difference in electric charges

Front 55

In water, which atom do more electrons share with?

Hydrogen or oxygen

Back 55

Oxygen

It is more electronegative

Front 56

2 regions of molecules in a polar covalent bond

Back 56

(partially) negative

(partially) positive

Front 57

Solutes

Back 57

Substances that dissolve in water

Front 58

In an aqueous solution, is water or the other solution's element the solvent

Back 58

water

Front 59

Ions and polar molecules will do what in water?

Why?

Back 59

dissolve

Ions and polar molecules are the solutes of the solution

Front 60

Hydrophilic

Back 60

water loving

Front 61

Are ion and polar molecules hydrophobic or hydrphilic?

Back 61

hydrophilic

Front 62

hydrophobic

Back 62

water fearing

Front 63

Which one doesn't readily dissolve in water?

Hydrophobic

Hydrophilic

Back 63

hydrophobic

Front 64

Are nonpolar molecules like hydrocarbon hydrophobic or hydrophilic?

Back 64

Hydrophobic

Front 65

Molecules having both polar or ionized regions at one or more sites and nonpolar regions at the other sites

Back 65

amphipathic molecules

Front 66

amount of a solute dissolved in a unit volume of solution

Back 66

concentration

Front 67

The concentration of

1gram of NaCl dissolved in a 1L of water =

Back 67

1g/L

Front 68

Number of moles of a solute dissolved in 1L of water

Back 68

Molarity

Front 69

1mol of a substance =

Back 69

atomic mass and also molecular mass

Front 70

Molarity equation

Back 70

Mols of solute
Liters of solution

Front 71

changes in state involve an input or output of

Back 71

energy

Front 72

is water stable?

Back 72

very

Front 73

Four important functions of water

Back 73

Participates in chemical reaction

removes toxic waste components

evaporative cooling

provides support of force

also cohesion and adhesion

hydrolysis and dehydration

Front 74

acids are molecules that release _ ions into a solution

Back 74

hydrogen

Front 75

Will a stronger of weaker acid release more H+?

Back 75

Stronger

Front 76

What lowers the H+ concentration of an acid

Back 76

bases

Front 77

bases lower the hydrogen concentration by sometimes releasing _ and other times binding _

Back 77

OH-

H+

Front 78

OH-

Back 78

hydroxide

Front 79

pH=

Back 79

Front 80

acidic solutions on the pH scale

Back 80

pH 6 or below

Front 81

neutral pH

Back 81

7

Front 82

When a solution is above 7 pH, it is called a _ solution

Back 82

alkaline

Front 83

Pure water ionizes slightly into what

Back 83

H and OH-

[H+] = 10 to the -7

Front 84

There is a lake and a cup.

Tell me about their heat capacity

Back 84

Lake has higher heat capactiy

Front 85

There is a lake and a cup

Tell me about their specific heat

Back 85

Specific heat doesn't change

Front 86

Hydrophilic

What kind of bond(s)?

Dissolves in what?

Loves or no?

Back 86

Polar and ionic

Water

loves

Front 87

Hydrophobic

What kind of bond(s)?

Dissolves in what?

Loves or no?

Back 87

Nonpolar

NOT water; nonpolar solvents

Hates

Front 88

heat of fusion

Back 88

heat needed to change the temperature by 1 unit

Front 89

effects shapes and functions of molecules, rates of many chemical reactions, ability of two molecules to bind together, and the ability of ions or molecules to dissolve in water

Back 89

pH

Front 90

Organisms tolerate (large, small) changes in pH

Back 90

small

Front 91

helps pH to keep constant

Back 91

buffer

Front 92

an acid-based __ system can shift to generate or remove H+ to adjust for changes in pH

Back 92

buffer

Front 93

In a(n) __ reaction, water is used to break apart another molecule

Back 93

Hydrolysis

Front 94

If pH rises too high in the blood, carbonic acid will release _ and form bicarbonate. This bicarbonate does what to the pH

Back 94

H+

Lowers it

Front 95

pH buffers do what to the pH of a solution?

Back 95

minimize flucuations

Front 96

pH buffers are usually what?

Back 96

weak acids and weak bases

Front 97

Will take up H+ when acids are added to them

Back 97

pH buffers

Front 98

Will release H+ when bases are added to them

Back 98

pH buffers

Front 99

If an atom looses or gains electrons, it acquires what? What does it become?

Back 99

Net charge; ion

Front 100

Acidic solutions contain more _ ions than _ ions

Back 100

H+ ions than OH- ions

Front 101

study of the nature of atoms and molecules with the exception of those that contain rings or chains of carbon

Back 101

inorganic chemisty

Front 102

Study of carbon containing molecules

Back 102

organic chemistry

Front 103

Physical region of space where an electron may be found

Back 103

orbital

Front 104

orbitals are found in these "energy levels" in a cell

Back 104

electron shells

Front 105

the capacity to do work or cause a change

Back 105

energy

Front 106

3 orbitals from closest to the nucleus to furthest away

Back 106

1s, 2s, 2p

Front 107

indicates an atom's mass relative to the mass of other atoms

Back 107

atomic mass

Front 108

a _ of any substance contains the same number of particles as there are atoms in exactly 12 g of carbon.

Back 108

mol

Front 109

measure for one half the mass of a carbon atoms, or about the mass of a hydrogen atom

Back 109

Dalton (or atm)

Front 110

different forms of the same element that differ only in the number of neutrons they contain

Back 110

isotopes

Front 111

unstable isotopes that emit radiation to try to convert themselves into stability

Back 111

radiosotopes

Front 112

all living organisms require these. They are present in extremely small qualities and necessary for normal growth and function

Back 112

trace elements

Front 113

pH buffers will do what when bases are added to them

Back 113

Release H

Front 114

occurs when atoms share 2 pairs of electrons rather than one pair

Back 114

double bond

Front 115

weak force that occurs because electrons are located within the orbitals in a random way. At any moment they could be distributed

Back 115

van der Waals dispersion force

Front 116

when mixed with water, long amphipathic molecules aggregate into spheres called

Back 116

micelles

Front 117

heat requires to vaporize 1 mol of any substance at its boiling point

Back 117

heat of vaporization

Front 118

amount of heat needed to be withdrawn or released from a substance to cause it to chance from the liquid to the solid state

Back 118

heat of fusion

Front 119

properties defined as those that depend strictly on the total number of dissolved solutes and not the specific type of solute

Back 119

colligitive properties

Front 120

water molecules attracting to each other

Back 120

cohesion

Front 121

ability of water to be attracted to and adhere to a surface that is not electrically neutral

Back 121

adhesion

Front 122

attraction between molecules at the surface of a liquid

Back 122

surface tension

Front 123

Molecule containing an atom with a single unpaired electron

Back 123

Free radical

Front 124

(Polar, nonpolar) region of micelle is located at the surface of the micelle

Back 124

Polar

Front 125

The tail region on amphapathic molecule will always be polar or nonpolar

Back 125

Nonpolar

Front 126

Concentration is defined as what

Back 126

Amount of solute (dissolved in)

Liter of solution

Front 127

Isotopes are multiple forms of an element that differ in the number of what

Back 127

Neutrons

Front 128

If pH in blood gets too low, bicarbonate will bind _ to form carbonic acid

Back 128

H+

Front 129

atomic mass =

atomic number =

Back 129

Atoms mass relative to the mass of another atom

number of protons in an atom

Front 130

what atom can only hold 2 electron in outer shell?

what atom can only hold 4 electron in outer shell?

Back 130

hydrogen has two

carbon has four

Front 131

atom with higher electronegativity has electrons orbiting _ to the nucleus

Back 131

closer

Front 132

sum of the atomic masses of all the atoms in a molecule

Back 132

molecular mass

Front 133

regarding the pH types of solutions, which has the lowest proton concentration

Back 133

alkaline - neutral - acidid

Front 134

water is so important to all living things because of it's

Back 134

stucture and polarity

Front 135

2 examples of pH buffers

Back 135

Carbonic acid and bicarbonate