Ap Bio Test I

Front 1

The molecules of life

Back 1

carbon, hydrogen, oxygen, nitrogen, phosphorus, sulfur (chonps)

Front 2

Vitalism

Back 2

the old way of looking at orgchem, which said that life force allowed certain compounds to be made only in the body.

Front 3

Who made urea and what did he use?

Back 3

Friedrich Wöhler using inorganic compounds and a substance in animal blood.

Front 4

Whoo made the first organic compound from inorganic compounds and what did he make?

Back 4

Hermann Kolbe, acetic acid

Front 5

Who simulated primordial earth and used lelectrical charges in the atmosphere, creating organic compounds?

Back 5

Stanley Miller

Front 6

What did vitalism eventually change to?

Back 6

Mechanism

Front 7

having 4 valence electrons

Back 7

tetravalance

Front 8

Methane

Back 8

CH4, tetrahedron

Front 9

When two carbons double bond...

Back 9

2-D molecule

Front 10

Ethane

Back 10

overlapping Methane

Front 11

The molecules of life

Back 11

carbon, hydrogen, oxygen, nitrogen, phosphorus, sulfur (chonps)

Front 12

Vitalism

Back 12

the old way of looking at orgchem, which said that life force allowed certain compounds to be made only in the body.

Front 13

Who made urea and what did he use?

Back 13

Friedrich Wöhler using inorganic compounds and a substance in animal blood.

Front 14

Whoo made the first organic compound from inorganic compounds and what did he make?

Back 14

Hermann Kolbe, acetic acid

Front 15

Who simulated primordial earth and used lelectrical charges in the atmosphere, creating organic compounds?

Back 15

Stanley Miller

Front 16

What did vitalism eventually change to?

Back 16

Mechanism

Front 17

having 4 valence electrons

Back 17

tetravalance

Front 18

Methane

Back 18

CH4, tetrahedron

Front 19

When two carbons double bond...

Back 19

2-D molecule

Front 20

Ethane

Back 20

overlapping Methane, C2H6

Front 21

hydrocarbons, examples

Back 21

molecules made of only H and C, petroleum and tail of fats

Front 22

Isomers

Back 22

compounds with the same number of atoms of the same elements but different structures

Front 23

structural isomers

Back 23

differ in covalent arrangement of atoms and locations of double bonds

Front 24

geometric isomers

Back 24

same covalent partnerships but differ in spatial arrangements

Front 25

enantiomers

Back 25

mirror image isomers

Front 26

T/F: Functional groups behave the same from molecule to molecule

Back 26

true

Front 27

Hydroxyl group
-form?
-properties?
-aka?

Back 27

-OH
-electronegative due to O
-Attracts water molecules which dissolves sugars and some organic molecules
-alcohols

Front 28

Carbonyl Group
-form?
-aka?
-example?

Back 28

-( >C=O)
-kenotes:carbonyl group within carbon skeleton ex. acetone
-aldehydes: carbonyl group on the end of a carbon skeleton ex. propanal

Front 29

Carboxyl Group
-form?
-aka?
-example?
-properties?

Back 29

-C< =O OH
-carboxylic acids
-ex. acetic acid
--acidic properties because it is a source of H+ ions... breaks into H+ ions and carboxylate group (-)

Front 30

Amino Group
-form?
-aka?
-example?
-properties?

Back 30

--N<H2
-amines
-glycine
-acts as a base to pick up protons. Under cellular conditions, has +1 charge

Front 31

Sulfhydryl Group
-form?
-aka?
-example?
-properties?

Back 31

-SH or -HS
-thiols
-ethanethiol
-two sulfhydryl groups can interact to stabilize a protein

Front 32

Phosphate group
-form?
-aka?
-example?
-properties?

Back 32

O
II
O-P-(-O)
(-O)

-organic phosphates
-glycerol phosphate
-makes the molecule its attached to an anion. can transfer energy between organic molecules

Front 33

aka ATP

Back 33

Adenosine triphosphate

Front 34

aka ADP

Back 34

Adenine diphosphate

Front 35

How many hydrogen bonds form to one water molecule?

Back 35

4

Front 36

cohesion

Back 36

water to water bonding

Front 37

adhesion

Back 37

water to other bonding

Front 38

surface tension

Back 38

how hard it is to stretch or break the surface of a liquid

Front 39

kinetic energy

Back 39

energy of movement

Front 40

heat

Back 40

total amount of kinetic energy

Front 41

temperature

Back 41

average kinetic energy of molecules

Front 42

Calorie (not calorie, kcal)

Back 42

amnt of heat needed to raise 1 kg of water 1•C.

Front 43

specific heat

Back 43

the amount of heat that must be absorbed or lost for 1 g of a substance to change its temp by 1•C.

Front 44

Heat of vaporization

Back 44

quantity of heat a liquid must absorb for 1g of it to be converted to gas

Front 45

heat of vaporization of water at 25•C

Back 45

58 calories

Front 46

evaporative cooling

Back 46

as a liquid evaporates, the liquid that remains cools down because the hottest molecules evaporate

Front 47

At what temp is water most dense?

Back 47

4•C

Front 48

What percent less dense is ice than water?

Back 48

10%

Front 49

solution

Back 49

liquid that is a completely homogeneous mixture of two or more substances

Front 50

solvent

Back 50

dissolving agent

Front 51

solute

Back 51

dissolved thing

Front 52

hydration shell

Back 52

sphere of water molecules around each dissolved ion

Front 53

colloid

Back 53

a stable suspension of fine particles in a liquid... a molecule is attracted to water but does not dissolve.

Front 54

avagadro's number

Back 54

6.02x10^23

Front 55

mole

Back 55

the number of molecules in grams which equals the atomic weight of the molecule, equal to avagadro's number

Front 56

atomic mass measured in

Back 56

daltons

Front 57

molarity

Back 57

number of molecules per liter of solution

Front 58

OH-

Back 58

hydroxide ion

Front 59

H+

Back 59

hydrogen ion

Front 60

hydronium ion

Back 60

H3O+

Front 61

equilibrium that involves movement

Back 61

dynamic equilibrium

Front 62

Concentration of each ion in pure water is..

Back 62

10^-7 M

Front 63

acid

Back 63

increases H+

Front 64

base

Back 64

reduces H+ count

Front 65

strong base/acid

Back 65

a > b

Front 66

weak base/acid

Back 66

a<>b

Front 67

In an aqueous solution, H+ concentration and OH- concentration equals

Back 67

10^-14

Front 68

formula to find pH

Back 68

-log [H+]... ex. neutral [H+] is 10^-7... therefore -log 10^-7= 7

Front 69

Buffers are usually

Back 69

weak acids and its corresponding base

Front 70

ex buffer

Back 70

carbonic acid: HCO3<>HCO3- and H+

Front 71

acid percipitation

Back 71

pH<5.6

Front 72

What is acid rain caused by?

Back 72

sulfur oxides and nitrogen oxides

Front 73

how many natural elements?

Back 73

92

Front 74

how many of the natural elements are essential to life?

Back 74

25

Front 75

cation

Back 75

positive ion

Front 76

anion

Back 76

negative ion

Front 77

ionic compounds form -_____, not ____

Back 77

salts not molecules

Front 78

T/F cations and anions are equal in salts

Back 78

false

Front 79

Van Der Waals interactions

Back 79

"hot spots" when electrons randomly cluster here or there giving random poles

Front 80

a molecule with 2 atoms is always

Back 80

linear

Front 81

start with ___ in a chemical reaction, end with ___

Back 81

reactants>products

Front 82

photosynthesis

Back 82

6CO2 + 6H2O > C6H12O6 + 6O6

Front 83

Heirarchy of Biological organization

Back 83

biosphere-ecosystems-communities-populations-organisms-organs and organ systems-tissues-cells-organelles-molecules

Front 84

prokaryotic cells

Back 84

bacteria and archea. DNA not separated from cell

Front 85

eukaryotic

Back 85

internal membranes, organelles

Front 86

high-throughput technology

Back 86

methods that analyze biological materials quickly and give large output

Front 87

bioinformatics

Back 87

extracting useful bio info from the surplus of info

Front 88

Three domains of lfie

Back 88

bacteria archea eukarya

Front 89

eukarya kingdoms

Back 89

protists fungi plantae animalia