Chapter 1 & 2 Campbell Biology (Ap)

Front 1

Hierarchy of Organization

Back 1

Atom, molecule, organelle, cell, tissue, organ, organism

Front 2

Examples of Organelles/ Functions

Back 2

Golgi - packages, Mitochondria - makes energy, cellular respiration, RER - membranous network in eukaryotic cells, Ribosomes - protein synthesis, Chlorophyll

Front 3

Atom vs. Molecule

Back 3

Atoms are the chemical building blocks of all matter, which are ordered into the more complex biological molecules

Front 4

Emergent Properties

Back 4

Order, Reproduction, Growth and Development, Energy Utilization (photosynthesis, ATP, cellular respiration), Responsiveness to environment, Homeostasis, Evolutionary Adaptation

Front 5

Reductionism

Back 5

Reducing complex system into simpler components

Front 6

Hooke

Back 6

(1665) first to describe and name cell (cork)

Front 7

Leeuwenhoek

Back 7

(1753) made microscope, discovered single-celled organisms (microorganisms)

Front 8

Schleiden & Schwann

Back 8

(1839) concluded that all living things consist of cells (leads to cell theory)

Front 9

Basics of DNA

Back 9

The substance of genes and the units of inheritance; made up of four kinds of nucleotides; double helix shape

Front 10

Ecosystem dynamics

Back 10

Nutrients cycle between abiotic and biotic components; energy from sun --> producers --> consumers --> lost as heat

Front 11

Enzymes

Back 11

Organic catalyst that speeds up chemical reactions, allows it to respond to changing conditions

Front 12

Regulatory Mechanisms

Back 12

positive and negative feedback; ensure dynamic balance in living systems

Front 13

Positive feedback

Back 13

Speeds up a process - blood clotting

Front 14

Negative Feedback

Back 14

slows or stops processes, body temperature increase -- why we sweat so that the body cools to set point

Front 15

Energy Conversion

Back 15

plants convert solar energy to chemical energy; work of cells relies on chemical energy which is converted to kinetic energy, which is dissipated as heat

Front 16

Homeostasis

Back 16

Maintaining an internal balance, uses positive and negative feedback

Front 17

Taxonomic Levels

Back 17

the grouping of species;
species, genus, family, order, class, phylum, kingdom

Front 18

Protista

Back 18

consists of unicellular eukaryotes and simple multicellular relatives

Front 19

Fungi

Back 19

multicellular eukaryotes, decomposers

Front 20

Animalia

Back 20

multicellular eukaryotes, obtain food by ingestion, motile

Front 21

Plantae

Back 21

Multicellular eukaryotes, produce own food through photosynthesis

Front 22

Monera

Back 22

all prokaryotes

Front 23

Archaea

Back 23

unicellular, prokaryotes; much like bacteria, but uses different chemicals for cellular respiration (?)

Front 24

Prokaryotes

Back 24

Have no nuclear membrane; bacteria and archaea

Front 25

Eukaryotes

Back 25

the membrane encloses the nucleus (nuclear membrane) and the organelles, DNA on chromosomes

Front 26

Domains

Back 26

3 Domains: Bacteria, Archaea, Eukarya (Eukaryotes)

Front 27

Kingdoms

Back 27

Protista, Animalia, Plantae, Fungi, Archaea, Monera

Front 28

Why Domains over Kingdoms?

Back 28

In kingdoms, all prokaryotes are recognized as members of Monera; while in the Domains, Bacteria and Archaea separates prokaryotes because Archaea may be more closely related to eukaryotes

Front 29

Evolution, Natural Selection, Darwin (Origin of Species), descent with modification

Back 29

connects all life by common ancestry, individuals in a population of species vary in many heritable traits; descent with modification - differences due to natural selection

Front 30

Scientific Method

Back 30

Observations, Question, Hypothesis, Prediction, Test. Must have a testable hypothesis, needs a control

Front 31

Inductive Reasoning

Back 31

Specific to generalized observations

Front 32

Deductive Reasoning

Back 32

Makes a general observation/ hypothesis to specific predictions

Front 33

Matter

Back 33

Anything that takes up space and has mass

Front 34

Mass

Back 34

The amount of matter in an object (like weight, except not affected by gravity)

Front 35

Element

Back 35

a substance that cannot be broken down by chemical reactions

Front 36

Compound

Back 36

a substance composed of 2 or more elements combined in a fixed ratio; organized matter having emergent properties

Front 37

Molecule

Back 37

two or more atoms held together by covalent bonds

Front 38

Atom

Back 38

smallest unit of matter that retains properties of an element

Front 39

Proton

Back 39

Subatomic Particle, positive charge, one Dalton

Front 40

Neutron

Back 40

subatomic particle, no charge, 1 Dalton

Front 41

Electron

Back 41

subatomic particle, negative charge, weight negligible

Front 42

Life's Essential Elements

Back 42

C, O, H, N, P, Ca, S, K

Front 43

Atomic number

Back 43

# of protons (and electrons), unique to element

Front 44

Atomic Weight

Back 44

Approximation of the total mass of atom

Front 45

Atomic mass

Back 45

the sum of protons and neutrons

Front 46

Isotopes

Back 46

Atoms of a given element have same number of protons, but some atoms have more neutrons than others

Front 47

Stable vs. Radioactive

Back 47

Stable - do not lose particles; radioactive decays spontaneously

Front 48

Radioactive uses

Back 48

Radioactive isotopes useful as tracers of atoms through metabolism, diagnostic tool to monitor chemical processes as they occur in the body (PET scans, Autoradiography)

Front 49

Energy levels of electrons

Back 49

only electrons enter into chemical reactions; electrons can change shell but only by absorbing or losing amt. of energy (move farther from nucleus = absorb energy; move to closer shell = release energy)

Front 50

Electron configuration

Back 50

2 electrons in first shell, maximum of 8 electrons in second shell

Front 51

Chemical Properties/ Behaviors (electrons)

Back 51

chemical behavior depends on # of e's in outermost shell (valence electrons in valence shell)

Front 52

Reactivity of atoms

Back 52

arises from the presence of unpaired electrons in one or more orbitals of their valence shells

Front 53

Covalent Bonds

Back 53

When two atoms share a pair of valence electrons

Front 54

Ionic Bonds

Back 54

If two atoms are very different in their attraction of shared electron, the more electronegative atom may completely transfer an electron from one atom to another

Front 55

Structural Formula

Back 55

H -- H

Front 56

Double Covalent Bond

Back 56

in oxygen molecule, two pairs of valences electrons are shared

Front 57

Polar covalent bond

Back 57

if one element is more electronegative - it pulls shared electrons closer to itself (more water-like ??) (slight positive/ negative charge)

Front 58

Nonpolar covalent bond

Back 58

if atoms have similar electronegativities, electrons remained equally shared

Front 59

Electronegativity

Back 59

the attraction of an atom for shared electrons

Front 60

Ions

Back 60

Complete transfer of an electron from another atom

Front 61

Cation

Back 61

Atom that loses an electron, results in a positive charge

Front 62

Anion

Back 62

Atom that gains an electron, negatively charged

Front 63

Hydrogen bonds

Back 63

weak bond, when H atom is covalently bonded with an electronegative atom, has partial positive charge

Front 64

Van der Waals interactions

Back 64

momentary uneven distributions produce changing positive and negative regions

Front 65

Chemical equilibrium

Back 65

the same number and kinds of atoms are present in both the reactants and the products

Front 66

Molecular shape

Back 66

atoms form covalent bonds, their s and 3 p orbital hybridize to form teardrop-shaped orbitals in tetrahedral arrangement

Front 67

Chemical Reactions

Back 67

involve the making or breaking of chemical bonds in transformation of matter into different forms (matter is conserved)