Bio 1 Exam 1

Front 1

biology is..

Back 1

the scientific Study of life

Front 2

What are the 5 unifying themes of biology

Back 2

organization, information, energy and matter, interactions and evolution

Front 3

list the 10 levels of organization

Back 3

1.biosphere

2. ecosystems

3. communities

4. populations

5. organisms

6. organs and organ systems

7. tissues

8. cells

9. organelles

10. molecules

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eukaryotic cell

Back 4

has a membrane, enclosed organelles and a nucleus

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Prokaryotic Cell

Back 5

simpler, does not contain nucleus or other membrane enclosed organelles

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Genes

Back 6

encode information for building molecules, units of inheritance

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gene expression

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converting information from gene to cellular product

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genome

Back 8

entire set of genetic instructions

Front 9

genomics

Back 9

the study of sets of genes within and between species

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Proteomics

Back 10

the study of whole sets of proteins encoded by the genome (known as proteomes)

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Bioinformatics

Back 11

the use of computational tools to process a large volume of data

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Name the 8 taxonomy classes (from not specific- specific)

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1. domain

2. Kingdom

3. phylum

4. class

5. order

6. family

7. genus

8. species

Front 13

Who is Charles Darwin?

Back 13

publisher of "on the origin of species"

came up with the idea of natural selection

and decent with modification

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What does the scientific process include?

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1. making observations

2. forming logical hypotheses

3. experiment

4. interpretation

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controlled experiment

Back 15

and experimental group is compared with a control group

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What is the unit of inheritance?

Back 16

DNA

Front 17

what is the unifying theory in biology?

Back 17

evolution

Front 18

What is natural selection?

Back 18

those individuals most suited for their environment produce the most offspring

Front 19

what is the scientific method

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rigorous study of natural phenomena

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All organisms are composed of...

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matter

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element

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substance that can not be broken down to other substances by chemical reactions

Front 22

compound

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a substance consisting of 2 or more elements in a fixed ratio

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what are the 4 essential elements to life? (96%)

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carbon, hydrogen, oxygen, nitrogen

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Trace elements and what are they? (4%)

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those required by an organism only in minute quantities

calcium, phosphorus, potassium, sulfur

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atom

Back 25

the smallest unit of matter that still retains the properties of an element

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atoms are composed of..

Back 26

protons(+)

neutrons

electrons(-)

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neutrons and protons form..

Back 27

atom nucleus

Front 28

neutrons and protons are measured in..

Back 28

daltons

Front 29

atomic number

Back 29

number of protons in the nucleus

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mass number

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sum of protons and neutrons in the nucleus (same as atomic mass)

Front 31

isotopes

Back 31

2 atoms of the same element that differ in the number of neutrons in the nucleus

Front 32

radioactive isotopes

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decay spontaneously, giving off energy

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Half-life

Back 33

a "parent" isotope decays into its daughter isotope at a fixed rate. this can be used for radiometric dating where scientist measure the ratio of different isotopes and calculate how many half lives have passed since the fossil or rock was created

they can vary from seconds, days, billions of years

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energy

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the capacity to cause change

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potential energy

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is the energy that matter has because of its location and structure

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electron shell

Back 36

an electrons state of potential energy or its energy level can be measured here

Front 37

the chemical behavior is mostly determined by...

Back 37

valence electrons

Front 38

orbital

Back 38

is the 3 dimentional space where an electron is found 90% of the time

Front 39

covalent bonds

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is the sharing of a pair of valence electrons by 2 atoms, these electrons count as part of each atoms valence shell

Front 40

molecule

Back 40

consists of 2 or more atoms held together by covalent bonds

Front 41

give a structural formula example

Back 41

H-H

Front 42

give a molecular formula example

Back 42

H2

Front 43

bonding capacity is called the atoms..

Back 43

valence

Front 44

electronegativity

Back 44

is an atoms attraction for the electrons in a covalent bond, the more electronegative and an atom the more strongly it pulls shared electrons toward itself

Front 45

nonpolar covalent bond and example

Back 45

atoms share the electron equally ex. oil

Front 46

polar covalent bond

Back 46

one atom is more electronegative and the atoms do not share the electrons equally, this causes a partical positive and negative charge to each atom or molecule ex. water

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ionic bond

Back 47

and attraction between a cation and anion, one atom gives its electron to another atom. creating on positive atom and one negative atom, this attraction between the positive and negative creates the ionic bond. Ex. NaCl

Front 48

cation

Back 48

a positively charged ion

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anion

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a negatively charged ion

Front 50

compounds formed by ionic bonds are called ionic compounds or...

Back 50

salts

Front 51

hydrogen bond

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a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom (can only create molecules)

Front 52

chemical reations

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the making and breaking of chemical bonds

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reactants

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starting molecule of a chemical reaction

Front 54

products

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the final molecule of a chemical reaction

Front 55

chemical equilibrium

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when forward and reverse reactions occur at the same time

Front 56

what does the atomic number tell you?

Back 56

electrons and protons

Front 57

how would 2 isotopes of oxygen differ?

Back 57

number of neutrons and atomic weight

Front 58

what is different about hydrogen bonds in comparison with covalent and ionic bonds?

Back 58

hydrogen bonds are forces that help shape the molecule. and they hold molecules together not atoms.

Front 59

what 4 properties make is so water can facilitate an environment for life?

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1. cohesive behavior

2. ability to moderate temperature

3. expansion upon freezing

4. versatility as a solvent

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cohesion

Back 60

hydrogen bonds hold water molecules together ex. the transport of water against gravity in plants

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adhesion

Back 61

is an attraction between different substances ex. water and plant cell walls

Front 62

surface tension

Back 62

a measure of how hard it is to break the surface of a liquid

Front 63

water absorbs ... from warmer air and releases .... to cooler air

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heat

stored heat

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kinetic energy

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energy in motion

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thermal energy

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kinetic energy associated with random motion of atoms or molecules

Front 66

temperature

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a measure of energy that represents the average kinetic energy of the molecules in a body of matter

Front 67

heat

Back 67

thermal energy in transfer from one body of matter to another

Front 68

calorie

Back 68

the amount of heat required to raise the temperature of 1 g of water by 1 degree C

Front 69

the "calories" on food packages are actually..

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kilocalories where 1 kcal= 1,000 cal

Front 70

joule is another unit of energy where..

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1 J=0.239 cal or 1 cal = 4.184 J

Front 71

specific heat

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the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degree c ex. water is 1cal/g/C (water has a high specific heat)

Front 72

heat of vaporization

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the heat a liquid must absorb for 1 g to be converted to gas

Front 73

evaporative cooling

Back 73

as the liquid evaporates its remaining surface cools

evaporative cooling helps water stabilize temperatures in organisms and bodies of water

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why does ice float?

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hydrogen bonds in ice are more "ordered" making ice less dense than water

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solution

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A liquid that is a completely homogenous mixture of substances

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solute

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the substance that is dissolved

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solvent

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the dissolving agent

Front 78

Aqueous solution

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one in which water was the solvent

Front 79

hydration shell

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when and ionic compound is dissolved in water, each ion is surrounded by a sphere of water molecules

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hydropilic

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substance is one that has an affinity with water

Front 81

hydrophobic

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substance is one that does not have and affinity for water(cell membranes and oil, tend to be nonpolar)

Front 82

molecular mass

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the sum of all masses of all atoms in a molecule. this is usually measured in moles where 1 mole=6.02 x 10 to the 23rd.

Front 83

molarity (M)

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the number of moles of solute per liter of solution

Front 84

hydrogen ion (H+)

Back 84

the hydrogen atom leaves its electron behind and is transferred as a proton

Front 85

Hydroxide ion (OH)-

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the molecule that lost the proton

Front 86

hydronium ion (H3O)+ also (H+)

Back 86

the molecule with the extra proton

Front 87

water is in a state of ........ in which water molecules dissociate at the same rate at which they are being reformed

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dynamic equilibrium

Front 88

acid

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any substance that increases the H+ concentration of a solution

Front 89

base

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any substance that reduces the H+ concentration of a solution, so in turn heavier in OH-

Front 90

pH scale

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used to describe whether a solution is basic or acidic

Front 91

the pH scale is a .... scale

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Logarithmic- meaning each "step" will be up or down x10, so add a 0 every step up or down

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0-7 is..

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acidic and higher in H+

Front 93

7-14 is...

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basic and decreasing in H+

Front 94

most biological fluids have pH values in the range of...

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6-8

Front 95

buffers

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substances that minimize changes in concentrations of H+ and OH- in a solution, most buffer solutions contain a weak acid and its corresponding base which combine reversibly with H+ ions

Front 96

ocean acidification

Back 96

CO2 is dissolved in sea water forms carbonic acid

Front 97

how is water transported from roots to leaves?

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cohesion, adhesion and transpiration

Front 98

organic chemestry

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the study of compounds that contain carbon

Front 99

hydrocarbons

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organic molecules consisting of only carbon and hydrogen

Front 100

isomers

Back 100

compounds with the same molecular formula but different structures and properties

Front 101

structural isomers

Back 101

have different covalent arrangements of their atoms

Front 102

cis trans isomers

Back 102

have the same covalent bonds but differ on spatial arrangments

x x H x

C=C C=C

H H x H

Front 103

enantiomer isomers

Back 103

mirror images of each other

Front 104

Functional groups

Back 104

the components of organic molecules that are most commonly involved in chemical reactions

Front 105

what are the 7 functional groups..

Back 105

1. Hydroxyl group (-OH) ex. ethanol

2. Carbonyl group (\/C=O) ex. acetone

3. Carboxyl group (-COOH) ex. acetic acid

4.Amino group (-NH2) ex. glycine

5. Sulfhydryl group (-SH) ex. cysteine

6.Phosphate group (-OPO32-) ex. glycerol phosphate)

7.Methyl group (-CH3) ex. methyl cytosine

Front 106

how many protons, electrons and neutrons does the most common carbon atom have?

Back 106

6,6,6

Front 107

how many bonds can carbon form?

Back 107

4

Front 108

What is meant by the "carbon skeleton"?

Back 108

forms the backbone of organic molecules

Front 109

ATP reacts with H2O and turns into..

Back 109

ADP and energy