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BIO > Ch 1-3 > Flashcards

Ch 1-3 Flashcards

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Biology 101 flashcards
1
Q
A

the study of life; “bios” = life

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2
Q

characteristics of life

A
  1. living organisms reproduce
  2. living organisms grow and develop
  3. organisms process energy
  4. regulation
  5. organisms interact
  6. composed of cells
  7. evolutionary adaptation
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3
Q

Living organisms reproduce

A

they produce copies of themselves; pass on genetic information to the future

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4
Q

Living organisms grow and develop

A

growth and development

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5
Q

growth

A

increase in size and number

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6
Q

development

A

change during life cycle (infant-child-adolescent-adult)

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7
Q

organisms process energy

A

allliving organisms live at the expense of their environment; they must extract energy and materials from the environment; convert energy from another source (ex: plants from sun and animals from food they eat)

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8
Q

regulation

A

organisms maintain their interval environment within limits that sustain life; ex: sweating, jackrabbit has blood vessel in ears to maintain body temp.; have to eat right food, balanced pH

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9
Q

organisms interact

A

interact with one another and their environment, responding to stimuli (ex: venus fly trap)

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10
Q

composed of cells

A

order; all living things exhibit complex organization

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11
Q

evolutionary adaptaino

A

over many generations, individuals with inheritied traits best suited to their local environment tend to pass these traits on to their offspring

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12
Q
A

“to know”; science is a way of knowing (one way, not the only way)

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13
Q
A

is to better understand the natural world; looking for empirical evidence; supernatural is outside of the realm of science

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14
Q

to approaches to science

A
  1. discovery science

2. scientific method

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15
Q

discovery science

A
  • verifiable observations and measurements
  • describe life in a variety of ways
  • aka “descriptive science”
  • looks at physical characteristics (what we see, hear, smell, taste, and feel)
  • observe behaviors
  • dissections
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16
Q

scientific method

A
  • formal process of inquiry
  • series of steps
  • begins with observations (discovery science)
  • asks questions and seek answers (forms hypothesis)
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17
Q

scientific hypothesis

A
  • a proposition that can be tested by careful observation or experiment (more than an educated guess)
  • “if ___ occurs, then ___ will result”
  • has to be potentially falsifiable which means it has to be able to be proven false
  • controlled experiment
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18
Q
A

with a control group, only one variable changed in each ofthe experimental groups; not always possible for practical and ethical reasons (es: global warming and testing drugs on children)

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19
Q

results of the scientific method

A
  • scientists do not tend to prove hypothesis, but support hypothesis with evidence
  • lots of evidence in support is considered “proof”
  • if the tests supports the hypothesis, move on to another question
  • if test does not support the thesis go back and provide another hypothesis to explain it
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20
Q

scientific fact

A

an observation that has been repeatedly confirmed and for all practical purposes is accepted as true (ex: cells have membranes, egg and sperm contain DNA)

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21
Q

Scientific Theory

A

a well substantiated explanation for some aspect of the natural that can incorporate facts, laws, inferences and tested hypothesis (ex: theory of evolution); lot of evidence behind it;

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22
Q

science is not set in stone

A
  • understandings can change as we learn more
  • the body of knowledge grows and science adapts to this new knowledge
  • science can change (# of planets changes, we can’t entirely stop disease with antibiotics because bacteria evolves extremely fast)
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23
Q

science tends to be self-correcting

A
  • scientists publish their findings in “peer-reviewed” journals and conferences
  • other scientists repeat their procedures to see if they get the same results and come to the same conclusions
  • over time, incorrect conclusions will usually be corrected
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24
Q

strengths of science

A
  • scientists strive to be free of bias and coercion in order to obtain objective answers and results
  • use controlled experiments when possible]
  • findings are reported in peer-reviewed journals with methods and results (helps for replication and self-correcting)
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25
Q

limitations of science

A
  • it isn’t always possible to do controlled experiments for practical and ethical reasons (climate change, testing drugs on kids)
  • science is reductive (looks at ever smaller parts, separate from the whole so it may not give an accurate picture of how the parts function within the whole)
  • the objective, value-free approach of good science cannot determine if something is good/bad, ethical/unethical, and cannot answers about the spiritual/supernatural (basically, it is only one facet of knowledge)
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26
Q

binomial nomenclature

A
  • scientific names (2 names)
  • italicized
  • genus and species
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27
Q

genus

A

begins with a capital letter (first word)

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28
Q

species

A

begins with a lower case letter (second word)

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29
Q

common name

A

both names are capitalized

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30
Q

three domains

A

domain bacteria
domain archaea
domain eukarya

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31
Q

domain bacteria

A
  • prokaryotic
  • unicelular
  • no nucleus
  • some (not all) cause disease
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32
Q

domain archaea

A
  • prokaryotic
  • unicellular
  • do not cause disease
  • some can do photosythesis
  • some can live in extreme environments (hot, salty, acidic…)
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33
Q

Domain eukarya

A
  • eukaryotic
  • some multi and some unicellular
  • 4 kingdoms
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34
Q

Domain Eukarya Kingdoms

A

kingdoms…Protista, plantae, fungi, and animalia

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35
Q

Kingdom protista

A
  • protists
  • eukaryotic
  • unicellular
  • more complex and larger than bacteria and archaea
  • some are photsynthetic
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36
Q

Kindom Plantae

A
  • plants
  • eukaryotic
  • multicellular
  • photosynthetic
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37
Q

Kingdom Fungi

A
  • eukaryotic
  • most are multicellular
  • do not photosynthesis
  • decomposers (live off dead things)
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38
Q

Kingdom Animalia

A
  • animals
  • eukaryotic
  • multicellular
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39
Q

energy flows

A
  • almost all energy on the earth comes from the sun
  • some energy can be used to do work but much of the rest is lost as heat
  • energy has to be continually brought into a system
  • slows in and out of a system
  • once you use it, its gone (reason we have to eat everyday)
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40
Q

chemicals cycle`

A
  • chemicals are used over and over again

- nature recycles (to be sustainable on this planet we need to learn how to recycle almost everything)

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41
Q

elements that make up 96.3% of our body weight

A
  1. oxygen
  2. carbon
  3. hydrogen
  4. nitrogen
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42
Q

fifith element need in molecules of life

A
  1. phosphorus
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43
Q

molecules of life

A
  1. water (O & H)
  2. carbohydrates (O,H,C)
  3. lipids or fats (O,H,C)
  4. Proteins (O,H,C,N)
  5. nucleic acids or DNA (O,H, C,N, P)
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44
Q
A

submicroscopic units of matter, smalles unit of all physical materials; molecules are made up of atoms

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45
Q

Proton

A
  • located in nucleus

- one unit positive charge (+)

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46
Q

Neutrons

A
  • located in nucleus

- no charge

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47
Q

electrons

A
  • revolve around nucleus in shells (shells are energy levels)
  • one unit negative charge
  • shell closest to nucleus holds 2 electrons; second and third shells hold 8 electrons
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48
Q

atomic number

A

determined by the number of protons (whereas mass number is the combined number of protons and neutrons)

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49
Q

what does the atomic number tell us?

A

of protons

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50
Q

what does the mass number tells us?

A

of protons and neutrons

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51
Q

isotopes

A

have the same number of protons and electrons but different number of neutrons; can be dangerous because some are radio active (nucleus decays, giving off particles and energy); living cells cannot distinguish between radioactive and non-radioactive elements so they take up both and use them (used in carbon dating and medicine)

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52
Q

Danger of isotopes

A
  • uncontrolled exposure to large doses can damage molecules, especially DNA
  • it does this by breaking chemical bonds and reforming abnormal bonds
  • can cause cancer and other diseases
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53
Q

outer electron shell

A

number of electrons in outermost shell determines the chemical properties of atom; atoms are considered reactive when their outermost shell is incomplete (these openings are the place where bonds form); atoms bond to fill up their outer shell

54
Q

unfilled spaces in atoms?

A

they are the places where atoms can bond to fill up the outer shells; the place where bonds form

55
Q

ionic bonds

A

form ionic compounds; ions are atoms or molecules with a positive or negative charge; attractions between ions of opposite charges (ex: NaCl); ionic compounds are held together by attraction of opposite charges

56
Q

covalent bonds

A

form molecules; share electrons; share one or more electrons to complete their outermost shell; ability to single bond (H2) and double bond (02); ex: water, carbohydrates, lipids, proteins, nucleic acid

57
Q

ions

A

atoms/molecules with a positive or negative charge

58
Q

what causes the attraction of ions?

A

the attractions between ions of opposite charge (one negative and one positive)

59
Q

% of earth’s water is freshwater

A

less than 3%

60
Q

% of freshwater available to us

A

0.5%

61
Q

what causes water to be a polar molecule?

A
  • water is held together by covalent bonds
  • oxygen atoms pulls the 10 electrons much more strongly than the hydrogen atoms so they don’t share the electrons equally
  • the electrons spend more time around the oxygen nucleus than around the hydrogen nucleus
  • since electrons have a negative charge, the oxygen side pole is slightly negative and the hydrogen side is slightly positive
62
Q

hydrogen bonds

A

form between water molecules as they align themselves by opposite charges (oxygen pole which is negative aligns up with the hydrogen pole which is positive of another molecule

63
Q

hydrogen bond vs. ionic and covalent bond

A
  • hydrogen bonds form a weak bond that is not as strong as ionic bonds, they are much less than a unit of charge
  • water stays bonded for only a fraction of a second, but at any given moment, many are bonded
64
Q

four qualities of water that make it unique

A

water reacts differently than most other molecules

  1. liquid water is cohesive
  2. ice floats
  3. water moderates temperatures
  4. water is the universal solvent
65
Q

liquid water is cohesive

A
  • cohesion- stick together
  • hydrogen bonds cause water molecules to stick together and pull each other along
  • ex: moving water up trees and other plants
    ex: surface tension; water bug on top of water
66
Q

ice floats

A
  • ice is less dense than liquid water
  • when water freezes, hydrogen bonds form between 100% of the molecules, pushing the molecules apart so there is more space between molecules
  • lattice like structure
  • becomes less dense and thus lighter than liquid water
  • vary rare (most substances become more dense as they get cold)
  • less dense b/c water molecules are farther apart
67
Q

water moderates temperatures

A
  • water gains and loses heat slowly***
  • the hydrogen bonds must first be broken in order for water to evaporate when heated causing water to heat up slowly
  • when water cools the opposite happens; hydrogen bonds have to reform causing water to cool down slowly
  • favorable for aquatic life in coastal areas and lakes because the water changes temperature slowly giving organisms time to adapt
  • water moderates temp. changes in cells
  • evaporative cooling (sweat)
68
Q

water is the universal solvent

A
  • many materials dissolve in water
  • helps materials to move around in cells
  • breaks materials down to their components
69
Q

acids

A

chemicals that increase the concentration (relative number) of H+ ions; ex - hydrochloric acid in our stomachs

70
Q

bases

A

chemicals that increase the concentration of OH- ions; ex - ammonia, household bleach

71
Q

pH represents…

A
  • each pH unit represents a 10fold change in concentration

- you multiply by 10 (from 1-2,2-3…)

72
Q

acid precipitation

A

when water has a pH below 5.6

73
Q

at what temperature is water most dense?

A

4 degrees celsius/ 39.2 degrees F

74
Q

pH biological range

A
  • 7 = neutral

- 6.5 to 8.2 = biological range

75
Q

pH of pure water

A

7

76
Q

Cause of acid precipitation

A

sulfur and nitrogen oxides, mostly from burning fossil fuels (coal, oil, gasoline)

77
Q

electron shells

A

energy levels

78
Q

nucleus

A

contains the protons and neutrons; center of atom

79
Q

bohrs model

A

know carbon has 4 openings, nitrogen has 3 openings, and oxygen has 2 openings; count the openings in the outer shell and that will give you the answer

80
Q

similarity b/t ionic and covalent bonds

A

they bond atoms together

81
Q

hydrogen bond

A

bond between water molecules

82
Q

Where is most of the energy stored in hydrocarbons, carbohydrates and fats

A
  • between the carbon and the hydrogen
  • much of the energy stored in organic molecules is stored in these carbon-hydrogen bonds
  • this energy is released when the bonds are broken (much of the energy is released as heats)
83
Q

what is the monosaccharide in fruit

A

fructose

84
Q

what are two differences between hydro carbons and carbohydrates?

A
  • all carbohydrates have oxygen in them; hydrocarbons do not

- difference in use, carbohydrates are used for power fuel;

85
Q

protein structures

A

primary structure (unique sequence of amino acids, different for each protein); secondary structure (interactions caused by hydrogen bonds); tertiary structure (proteins automatically go into its three dimensional shape as they are being formed in water, no additional energy needed) – 3d shape determines the function of the protein

86
Q

how many monomers

A

20 different possibilities

87
Q

what are two forces that causes proteins to self construct into their three dimensional shape?

A

hydrogen bonds; hydrophobic/hydrophilic interactions

88
Q

why is carbon so important for building these organic molecules?

A

-it can bond in all four directions; you can make all different structures and complexities

89
Q

what is the difference b/t saturated and unsaturated fats?

A
  • saturated fat is the fatty acids filled with the maximum number of hydrogen atoms on the carbon chain; packs tightly
  • unsaturated fat is the fatty acid with less than the maximum of hydrogen atoms on the carbon chain (b/c of double bond) (healthier than saturated)
90
Q

at room temperature, ___ is ___

A

saturated fat; solid

91
Q

polyunsaturated fat

A

can’t pack tightly together; become liquids at room temperature

92
Q

“partially hydrogenated oils”

A

trans fats are present in that food

93
Q

components of nucleic acids

A

sugar, phosphate group, nitrogenous base

94
Q

what forms the backbone of DNA

A

sugar and phosphate; bases form the bond across

95
Q

monomers

A

monosaccharides (carbohydrates), amino acids (protein), nucleotides (nucleic acids)

96
Q

polymers

A

polysaccharides (carbohydrates), proteins, nucleic acids

97
Q

organic molecules that are essential to life

A
  1. carbohydrates
  2. lipids
  3. proteins
    4 nucleic acid
98
Q

importance of carbon

A
  • carbon can form bonds in four directions
  • forms the backbone for all the macromolecules of life
  • present in each of the four organic molecules/all have carbon backbones
99
Q

hydrocarbon

A

the most simple carbon molecules; made up of hydrogen and carbon only

100
Q

macromolecules =

A

organic molecules

101
Q

polymers

A

molecules built by linking together a large number of subunits

102
Q

monomers

A

the subunits

103
Q

carbohydrates

A
  • range from small sugars to large polysaccharides
  • CHO
  • fuel for our bodies (our primary source of energy)
  • saccharide
  • polar like water
  • hydrophilic
104
Q

monosaccharide

A
  • carbohydrate
  • single sugar (monomer)
  • glucose
  • 3 to 7 carbons long
105
Q

names of sugars end in ___

A

ose

106
Q

disaccharide

A
  • carbohydrate

- two sugar monomers bound together

107
Q

disaccharide examples

A

sucrose (sugar), lactose (milk),maltose (beer)

108
Q

monosaccharide examples

A

-glucose (plants), fructose (fruit), galactose

109
Q

polysaccharide

A

polymers of a few hundred to a few thousand monosaccharides long

110
Q

polysaccharide examples

A

starch (food, grains, potatos), glycogen (muscle cells), cellulose (wood, plant cell walls)

111
Q

hydrophilic molecules

A

attracted to water

112
Q

carbohydrates are hydrophilic

A
  • small molecules will dissolve in water (sugar, flour, corn starch)
  • large molecules do not dissolve but attract water (wood and cotton)
113
Q

lipids

A

diverse compounds that consist mainly of carbon and hydrogen with some oxygen

  • no monomers or polymers
  • nonpolar
  • do not mix with water
  • hydrophobic
  • ex: fats and oils
114
Q

hydrophobic

A

wants to get away from water

115
Q

fats are made up of…

A

fatty acid

s

116
Q

triglceride

A

three fatty acids linked to glycerol (another name for fat)

117
Q

fatty acidd

A

C=O group plus a hydrocarbon

118
Q

with what are saturated fats saturated with?

A

hydrogen

119
Q

why are some fats solid at room temperature adn other liquid?

A

saturated fats pack tightly and are therefore solid whereas polyunsaturated fats can’t pack tightly so the become liquid at room temperature

120
Q

trans fats

A

unsaturated fats that have been partially hydrogenated (hydrogen atoms added)
no kink
look for the line “partially hydrogenated oils”
very unhealthy for you

121
Q

Protein

A
  • made up of COHN
  • the polymers are called proteins
  • monomers = amino acids
  • unique 3d structure
122
Q

protein stuctures

A

primary, secondary, tertiary

123
Q

primary structure

A
  • unique sequence of amino acids

- different for each protein

124
Q

secondary structure

A

-interactions caused by hydrogen bonds

125
Q

tertiary structure

A

-proteins automatically go into its 3d shape as they are being formed in water; shape determines function of proteins; happens by itself in water solution

126
Q

reasoning behind tertiary structure

A
  1. hydrogen bonds
  2. hydrophobic/philic interactinos
  3. other reactions.
127
Q

nucleic acids

A

information storage in cells, COHNP; DNA; RNA

128
Q

monomers of nucleic acid

A

nucleotide

129
Q

components of nucleotide

A

sugar, phosphate group, nitrogenous base (sugar and phospate bond to form backbone and nitrogenous base extends out from backbone)

130
Q

major classes of protein

A
  • contractile (muscles)
  • structural (hair, tendons)
  • signaling (messages within cells)
  • enzymes (increase rate of reaction in cells)
131
Q

how many monomers are in protein?

A

proteins are made up of 20 amino acid monomers

BIO (18 decks)

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