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Chapters 1 & 2 Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

What is the core theme of biology?

A

Evolution

The process of change that has transformed life on Earth

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2
Q

7 Characteristics of Life

A
  1. Order (organization)
  2. Evolutionary adaptation
  3. Response to environment
  4. Reproduction
  5. Growth and development
  6. Energy processing
  7. Regulation
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3
Q

10 Levels of Biological Hierarchy (Biggest level to smallest level)

A
  1. Biosphere
  2. Ecosystem
  3. Community
  4. Population
  5. Organism
  6. Organs and Organ System
  7. Tissue
  8. Cell
  9. Organelles
  10. Molecule
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4
Q

Biosphere

A

all environments (everything) on Earth

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5
Q

Ecosystem

A

all living and nonliving things in a particular area

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6
Q

Community

A

all organisms (living things) in an ecosystem

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7
Q

Population

A

all individuals of a species in a particular area

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8
Q

Organism

A

an individual living thing (one single organism)

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9
Q

Organs and Organ Systems

A

specialized body parts made up of tissues. Ex: heart, stomach

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10
Q

Tissue

A

a group of similar cells

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11
Q

Cell

A

life’s fundamental unit of structure and function. (cells are alive)

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12
Q

Organelles

A

a structural component of a cell (building blocks of a cell)

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13
Q

Molecule

A

a chemical structure consisting of atoms

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14
Q

Emergent Properties

A

new properties that arise with each step upward in the hierarchy of life owing to the arrangement and interactions of parts as complexity increases.

Emergent properties characterize nonbiological entities as well.
Ex: Bike

Emergent Properties- put them/things together

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15
Q

Reductionism

A

is the reduction of complex systems to simpler components that are more manageable to study.
Ex: the molecular structure of DNA v. heredity

An understanding of biology balances reductionism with the study of emergent properties.

Reductionism- breaks things apart

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16
Q

Life requires energy transfer and transformation

A

Living organisms transform energy from one form to another

food (chemical energy)&raquo_space; motion (kinetic energy)

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17
Q

Two Rules of Ecosystem Dynamics (how they work)

The two major processes that the dynamics of an ecosystem include

A
  1. Chemical nutrients recycle (chemicals cycle)

2. Energy flows- usually enters as sunlight exits as heat

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18
Q

Structure and Function of living organisms

A

are closely related.

By looking at the structure we can figure out the function.

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19
Q

The fundamental unit of life

A

Cell

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20
Q

The lowest level of organization that can perform all activities required for life (Order, evolutionary adaptation, response to the environment, reproduction, growth and development, energy processing, regulation)

A

The Cell

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21
Q

All Cells

A
  • are enclosed by a membrane (outside part)

- use DNA as their genetic material (inside part)

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22
Q

Two main forms of cells are

A

Eukaryotic Cell and Prokaryotic Cell

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23
Q

Eukaryotic Cell

A

has membrane-enclosed organelles, the largest of which is usually the nucleus

(have internal membrane)

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24
Q

Prokaryotic Cell

A

is simpler and usually smaller, and does not contain a nucleus or other membrane-enclosed organelles

(doesn’t have internal membrane. normally much smaller)
(bacteria)

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25
Q

the ability of cells to divide is

A

the basis of all reproduction, growth, and repair of multicellular organisms

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26
Q

DNA is

A

a simple molecule.

Each DNA molecule is made up of two long chains arranged in a double helix

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27
Q

A, G, C, and T

A

each link of a chain is one of four kinds of chemical building blocks called nucleotides and nicknamed A, G, C, and T.

Its all about the order of things and order of the nucleotides

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28
Q

A gene codes for

A

protein

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29
Q

DNA&raquo_space; RNA» Protein

A

DNA is transcribed into RNA then translated into a protein

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30
Q

Negative Feedback

A

means that as more of a product accumulates, the process that creates it slows and less of the product is produced.

ATP generation

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31
Q

Positive Feedback

A

means that as more of a product accumulates, the process that creates it speeds up and more of the product is produced

Blood clotting

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32
Q

Taxonomy

A

is the branch of biology that names and classifies species into groups of increasing breadth

Domains followed by kingdoms are the broadest units of classification

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33
Q

Organisms are divided into three domains

the three domains of life

A 
Domain Bacteria (prokaryotic-unicellular)
Domain Archaea (prokaryotic-unicellular)
Domain Eukarya (eukaryotic)
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34
Q

Domain Bacteria

A

Prokaryotic-unicellular.
has no nucleus.
it is anything normal that lives on skin or in lungs or in normal areas or normal environments

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35
Q

Domain Archaea

A

Prokaryotic-unicellular.
has no nucleus.
it is anything weird that lives in like volcanoes or really cold environments or just weird environments

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36
Q

Domain Eukarya

A

Eukaryotic.
anything that has a nucleus.

It has four kingdoms that can be distinguished by how they get their food:

  1. Kingdom Plantae
  2. Kingdom Fungi
  3. Kingdom Animalia
  4. Protists.
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37
Q

Kingdom Plantae

A

photosynthetic

multicellular

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38
Q

Kingdom Fungi

A

absorb nutrients

multicellular

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39
Q

Kingdom Animalia

A

ingest their food

multicellular

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40
Q

Protists

A

unicellular

many kingdoms

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41
Q

DNA is the

A

universal genetic language common to all organisms.

Unity is evident in many features of cell structure

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42
Q

natural selection

A

results in the adaptation of organisms to their environment

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43
Q

Evolution occurs at

A

the population level

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44
Q

Inquiry

A

is the search for information and explanation

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45
Q

The scientific process includes

A

making observations, forming logical hypotheses, and testing them

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46
Q

Types of Data

A

Qualitative

Quantitative

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47
Q

Qualitative

A

descriptions rather than measurements.

Descriptive

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48
Q

Quantitative

A

recorded measurements, which are sometimes organized into tables and graphs (NUMBERS).

Numerical

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49
Q

Hypothesis

A

is a tentative answer to a well framed question (if … then)

They are NOT best guesses.
They are usually narrow in scope.

A scientific hypothesis leads to predictions that can be tested by observation or experimentation

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50
Q

Failure to falsify a hypothesis

A

does not prove that hypothesis.

Nothing “proves” a hypothesis beyond a shadow of a doubt

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51
Q

Inductive Reasoning

A

draws conclusions through the logical process of induction.

Repeat specific observations can lead to important generalizations.
Specific –> General

Observations and inductive reasoning can lead us to ask questions and propose hypothetical explanations called hypothesis

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52
Q

Deductive Reasoning

A

uses general premises to make specific predictions.
General –> Specific

Deductive Reasoning– If . . . Then . . .

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53
Q

A hypothesis must be

A

testable and falsifiable.

Supernatural and religious explanations are outside the bounds of science.

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54
Q

A theory is

A
  • broader in scope than a hypothesis.
  • general, and can lead to a new testable hypotheses.
  • supported by a large body of evidence in comparison to a hypothesis
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55
Q

A controlled experiment

A

compares an experimental group with a control group.

A controlled experiment means that control groups are used to cancel the effects of unwanted variables.

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56
Q

Dependent Variables

A

what is the outcome. what depends on the entire experiment before something happens. the end.

Goes on the Y axis

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57
Q

Independent Variables

A

what “I” ,the researcher, does. the thing that is manipulated. what changes. the beginning.

Goes on the X axis.

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58
Q

Science VS. Technology

A

the goal of science is to understand natural phenomena.

The goal of technology is to apply scientific knowledge for some specific purpose.

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59
Q

Organisms are composed of

A

matter.

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60
Q

Matter

A

anything that takes up space and has mass.

Matter is made up of elements.

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61
Q

Carbon, Hydrogen, Oxygen, and Nitrogen

A

make up about 96% of living matter.

CHON

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62
Q

Most of the remaining 4% of living matter consists of

A

calcium, phosphorus, potassium, and sulfur

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63
Q

Trace elements

A

are those required by an organism in minute quantities.
Iodine, goiter.

minute- teeny tiny

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64
Q

An Element

A

is a substance that cannot be broken down to other substances by chemical reactions.

C, N, Na

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65
Q

A Compound

A

is a substance consisting of two or more elements in a fixed ratio

NaCl, H2O

A compound has characteristics different from those of its elements

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66
Q

An element consists of

A

unique atoms

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67
Q

An Atom

A

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

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68
Q

Atoms are composed of

A

subatomic particles

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69
Q

Relevant subatomic particles inclue

A
  • Neutrons (no electrical charge) (found in nucleus)
  • Protons (positive charge)
  • Electrons (negative charge)
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70
Q

Protons

A

+ charge.

determine element.

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71
Q

Neutrons

A

no charge.

determine isotope.

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72
Q

Electrons

A
  • charge.

form negative cloud around the nucleus and determine chemical behavior

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73
Q

neutrons and protons form the

A

atomic nucleus.

74
Q

Neutron mass and proton mass are almost identical and measured in

A

Daltons.

Proton= about 1 dalton (Weight)

75
Q

Electrons do not

A

follow circular orbits around the nucleus.

instead they are constantly moving around the nucleus.

76
Q

Atoms of various elements differ in

A

number of subatomic particles

77
Q

An element’s atomic number is the

A

number of protons in its nucleus.

Atomic Number= # of protons

78
Q

An element’s atomic mass is the

A

sum of protons plus neutrons in the nucleus.

Atomic Mass= P + N

79
Q

Atomic mass

A

the atom’s total mass, can be approximated by the mass number

Atomic Mass= P + N + E

80
Q

The mass number is

A

written as a superscript to the left of an element’s symbol

Mass Number= # of Protons + # of Neutrons

81
Q

The atomic number is

A

written as a subscript to the left of an element’s symbol

Atomic Number= # of Protons

82
Q

All atoms of an element have the same number of protons but may differ

A

in number of neutrons

83
Q

Isotopes

A

are two atoms of an element that differ in number of neutrons

C12, C13, C14

84
Q

Radioactive isotopes

A

decay spontaneously giving off particles and energy

85
Q

Energy is

A

the capacity to cause change

86
Q

Potential energy is

A

the energy that matter has because of its location or structure

87
Q

The electrons of an atom differ in their amounts of

A

potential energy

88
Q

An electron’s state of potential energy is called its

A

energy level or electron shell

89
Q

First shell

A

can hold up to 2 electrons

90
Q

Second shell

A

can hold up to 8 electrons

91
Q

Third shell

A

can hold up to 8 electrons

92
Q

The chemical behavior of an atom is determined by

A

the distribution of electrons in electron shells.

the valence electrons (in the outer shell)

93
Q

Mostly always the number of protons will be the same as the

A

number of electrons, unless stated otherwise

94
Q

Valence electrons

A

are electrons in the outermost shell, or valence shell

95
Q

The Valence of an element

A

is how many electrons it still wants. the number of empty spots that need to be filled with electrons to fill the shell.

96
Q

Elements with a full valence shell are chemically

A

inert

97
Q

Valence tells you how many

A

bonds it’ll make and how many electrons are missing in the outer shell

98
Q

Oxygen

A

6 valence electrons

valence of 2

99
Q

Hydrogen

A

1 valence electron

Valence of 1

100
Q

Carbon

A

4 valence electrons

valence of 4

101
Q

Nitrogen

A

5 valence electrons

valence of 3

102
Q

Covalent Bonds

A

strongest bonds you can make that happen by sharing the electrons.

A covalent bond is the sharing of a pair of valence electrons by two atoms.

Covalent bond= Strong. Share.

In a covalent bond, the shared electrons count as a part of each atom’s valence shell.

103
Q

A Molecule consists of

A

two or more atoms held together by covalent bonds.

104
Q

A single covalent bond, or single bond, is the

A

sharing of one pair of valence electrons

105
Q

A double covalent bond, or double bond, is the

A

sharing of two pairs of valence electrons

106
Q

Covalent bonds can form between

A

atoms of the same element or atoms of different elements

107
Q

H20

A

a molecule and compound

108
Q

H2

A

a molecule

109
Q

Electronegativity

A

is an atom’s attraction for the electrons in a covalent bond

110
Q

The more electronegative an atom,

A

the more strongly it pulls shared electrons toward itself

111
Q

Two types of covalent bonds

A

Non-polar covalent bond and Polar Covalent Bond

112
Q

Non-Polar Covalent Bonds

A

share electrons equally

113
Q

Polar Covalent Bonds

A

share electrons UNequally.

One atom is more electronegative and the atoms do not share the electron equally.

114
Q

Unequal sharing of electrons causes a

A

partial positive or negative charge for each atom or molecule

115
Q

Ionic Bonds

A

weaker, and transfer electrons.

Atoms sometimes strip electrons from their bonding partners.
An example is the transfer of an electron from sodium to chlorine. NaCl
After the transfer of an electron, both atoms have charges.

116
Q

A charged atom (or molecule) is called an

A

ion

117
Q

NaCl

A

is an ionic bond.

118
Q

A cation

A

is a positively charged ion

119
Q

A anion

A

is a negatively charged ion

120
Q

An ionic bond is an attraction between an

A

anion and a cation

121
Q

Sodium loses an electron so it is a

A

cation

Na+

122
Q

Chloride gains an electron so it is an

A

anion

Cl-

123
Q

Most of the strongest bonds in organisms are

A

covalent bonds that form a cell’s molecules

124
Q

Weak chemical bonds are

A

ionic bonds and hydrogen bonds

125
Q

Weak chemical bonds reinforce

A

shapes of large molecules and help molecules adhere to each other

126
Q

Hydrogen Bonds

A

weak, and form between molecules.

A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom.

In living cells, the electronegative partners are usually oxygen or nitrogen atoms

127
Q

Van Der Waals Interactions

A

Weak and asymmetrical electrons.

Van Der Waals Interactions are attractions between molecules that are close together as a result of these chargers.
(Asymmetrical electron distribution).

Collectively, such interactions can be strong, as between molecules of gecko’s toe hairs and a wall surface.

If electrons are distributed asymmetrically in molecules or atoms, they can result in “hot spots” of positive or negative charge.

128
Q

All organisms on your campus make up

A

a community

129
Q

which of the following is a correct sequence of levels in life’s hierarchy, proceeding downward from an individual matter?

A

Nervous system, brain, nervous tissue, nerve cell

130
Q

Systems biology is mainly an attempt to

A

Understand the behavior of entire biological systems

131
Q

Which of the following are observations or interferences on which Darwin’s theory of natural selection is based?

A
  • There is heritable variation among individuals
  • Because of overproduction of offspring, there is competition for limited resources
  • Individuals whose inherited characteristics best fit them to the environment will generally produce more offspring
  • A population can become adapted to its environment over time
132
Q

Protists and bacteria are grouped into different domains because

A

Protists have a membrane-bounded nucleus, which bacteria cells lack

133
Q

Which of the following best demonstrates the unity among all organisms?

A

The structure and function of DNA

134
Q

A controlled experiment is one that

A

Tests experimental and control groups in parallel

135
Q

Which of the following statements best distinguishes hypotheses from theories in science?

A

Hypotheses usually are relatively narrow in scope; theories have broad explanatory power

136
Q

Which of the following is an example of qualitative data?

A

The fish swam in a zigzag motion

137
Q

Which of the following best describes the logic of scientific inquiry?

A

If my hypothesis is correct, I can expect certain test results

138
Q

in the term trace element, the adjective trace means that

A

the element is required in very small amounts

139
Q

compared with 31P, the radioactive isotope 32P has

A

one more neutron

140
Q

the reactivity of an atom arises from

A

the existence of unpaired electrons in the valence shell

141
Q

which statement is true of all atoms that are anions?

A

The atom has more electrons than protons

142
Q

Which of the following statements correctly describes any chemical reaction that has reached equilibrium?

A

The rates of the forward and reverse reactions are equal

143
Q

We can represent atoms by listing the number of protons, neutrons, and electrons—for example, 2p+, 2n0, 2e- for helium. Which of the following represents 18O isotope of oxygen?

A

8p+, 10n0, 8e-

144
Q

the atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound.

A

H2S

145
Q

What coefficients must be placed in the following blanks so that all atoms are accounted for in the products?
C6H12O6 →______ C2H6O + ______ CO2

A

2; 2

146
Q

A substance that cannot be broken down into other substances by ordinary chemical procedures is a(n) _____.

A

element

147
Q

Which of the following is a trace element required by most living organisms?

A

magnesium

148
Q

Which of the following subatomic particles always has a positive charge?

A

proton

149
Q

Changing the number of _____ would change an atom into an atom of a different element.

A

protons in an atom

150
Q

The atoms of different phosphorus isotopes _____.

A

have different numbers of neutrons

151
Q

The type of bonding and the numbers of covalent bonds an atom can form with other atoms is determined by _____.

A

the number of unpaired electrons in the valence shell

152
Q

A carbon atom and a hydrogen atom form what type of bond in a molecule?

A

nonpolar covalent bond

153
Q

An ionic bond is formed when _____.

A

one atom transfers an electron to another atom

154
Q

Hydrogen bonding is most often seen _____.

A

when hydrogen is covalently bonded to an electronegative atom

155
Q

Chemical equilibrium is reached when _____.

A

The forward and reverse reactions occur at the same rate so that the concentrations of reactants and products remain the same

156
Q

An organ, such as the liver, is composed of _____.

A

tissues

157
Q

Which of these is an organ system?

A

digestive

158
Q

What are the two main types of cells?

A

Prokaryotes and Eukaryotes

159
Q

Which of the following is true?

A

Bacteria can mutate within the human body

160
Q

The innermost electron shell of an atom can hold up to _____ electrons.

A

2

161
Q

Which of these relationships is true of an uncharged atom?

A

The number of protons is equal to the number of electrons

162
Q

What determines the types of chemical reactions that an atom participates in?

A

the number of electrons in the outermost electron shell

163
Q

`An atom is least likely to participate in a reaction when

A

its outermost shell is stable.

164
Q

What is the atomic number of an atom that has 6 protons, 6 neutrons, and 6 electrons?

A

6

165
Q

Which of these refers to atoms with the same atomic number but different atomic masses?

A

these atoms are isotopes

166
Q

Atoms with the same atomic number and different atomic masses are referred to as

A

isotopes.

167
Q

Fluorine’s atomic number is 9 and its atomic mass is 19. How many neutrons does fluorine have?

A

10

168
Q

Atomic mass is equal to

A

the number of protons plus the number of neutrons (19-9 = 10).

169
Q

the atomic number is equal to

A

the number of protons.

170
Q

The proton, neutron, and electron are

A

the three main subatomic particles that make up all the elements.

171
Q

Mass of ~1 amu=

A

neutron and proton

172
Q

Mass of ~1/2000 amu=

A

electron

173
Q

A covalent bond is one in which

A

electron pairs are shared

174
Q

A(n) _____ refers to two or more atoms held together by covalent bonds.

A

molecule

175
Q

A molecule is defined as

A

two or more atoms held together by covalent bonds

176
Q

A hydrogen atom with a net positive charge is attracted to

A

an oxygen atom with a net negative charge.

177
Q

What name is given to the bond between water molecules?

A

hydrogen

178
Q

Atoms with the same number of protons but with different electrical charges _____.

A

are different ions

179
Q

An ionic bond involves

A

an attraction between ions of opposite charge

180
Q

The tendency of an atom to pull electrons toward itself is referred to as its _____.

A

Electronegativity

► Biology (29 decks)

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