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![Page 1: Www.cengage.com/chemistry/brown Albia Dugger Miami Dade College Cecie Starr Christine Evers Lisa Starr Chapter 1 Invitation to Biology.](https://reader035.fdocuments.net/reader035/viewer/2022062314/56649de65503460f94adf3b2/html5/thumbnails/1.jpg)
www.cengage.com/chemistry/brown
Albia Dugger • Miami Dade College
Cecie StarrChristine EversLisa Starr
Chapter 1Invitation to Biology
![Page 2: Www.cengage.com/chemistry/brown Albia Dugger Miami Dade College Cecie Starr Christine Evers Lisa Starr Chapter 1 Invitation to Biology.](https://reader035.fdocuments.net/reader035/viewer/2022062314/56649de65503460f94adf3b2/html5/thumbnails/2.jpg)
Space fish
Milk fish
Hagfish
Puffer
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• Life defies a simple, one-sentence definition• Life is recognized by what living things do
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
LIFE
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Order
Evolutionary adaptation
Responseto theenvironment
Reproduction
Growth anddevelopment
Energyprocessing
Regulation
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Biology The scientific and systematic study of life
Biologists think about life at different levels of organization
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The biosphere
Communities
Populations
Organisms
Ecosystems
Organs and organ systems
Cells
Cell
Organelles
Atoms
MoleculesTissues
10 µm
1 µm
50 µm
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The biosphere
Communities
Populations
Organisms
Ecosystems
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Organs and organ systems
Cells
Cell
Organelles
Atoms
MoleculesTissues
10 µm
1 µm
50 µm
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• atom – Fundamental building block of all matter
• molecule – An association of two or more atoms
• organelle– Functional components that make up cells
• cell – Smallest unit of life
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• tissue – In multicelled organisms, specialized cells organized in
a pattern that allows them to perform a collective function
• organ – In multicelled organisms, a grouping of tissues that
perform a collective function
• organ system – In multicelled organisms, set of tissues and cells
engaged in a collective function that keeps the body functioning properly
• organism – Individual that consists of one or more cells
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• A population is a group of individuals of a species in a given area
• A community is all populations of all species in a given area
• An ecosystem is a community interacting with its environment
• The biosphere includes all regions of Earth that hold life
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Species Genus Family Order Class Phylum Kingdom Domain
Ursus americanus(American black bear)
Ursus
Ursidae
Carnivora
Mammalia
Chordata
Animalia
Eukarya
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1 µmOrganelles
Nucleus (contains DNA)
Cytoplasm
Membrane
DNA(no nucleus)
Membrane
Eukaryotic cellProkaryotic cell
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Nucleus DNA
Cell
Nucleotide
(a) DNA double helix (b) Single strand of DNA
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NucleicontainingDNA
Sperm cell
Egg cell
Fertilized eggwith DNA fromboth parents
Embryo’s cells withcopies of inherited DNA
Offspring with traitsinherited fromboth parents
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• DNA contains information that guides all of an organism’s metabolic activities, including growth, development, and reproduction
• Small variations in DNA structure give rise to differences between species and individuals
• The passage of DNA from parents to offspring is inheritance
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• DNA – Deoxyribonucleic acid; carries hereditary information
that guides growth and development
• growth – In multicelled species, an increase in the number, size,
and volume of cells
• development – Multistep process by which the first cell of a new
individual becomes a multicelled adult
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• reproduction – Processes by which parents produce offspring
• inheritance – Transmission of DNA from parents to offspring
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Outer membraneand cell surface
Cytoplasm
Nucleus
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Negativefeedback
Excess Dblocks a step
D
D D
A
B
C
Enzyme 1
Enzyme 2
Enzyme 3
D
(a) Negative feedback
W
Enzyme 4
XPositivefeedback
Enzyme 5
Y
+
Enzyme 6
Excess Zstimulates astep
ZZ
Z
Z
(b) Positive feedback
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Charles Darwin
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Populationwith variedinherited traits.
Eliminationof individualswith certaintraits.
Reproductionof survivors.
Increasingfrequencyof traits that enhance survival and reproductive success.
4321
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www.cengage.com/chemistry/brown
Albia Dugger • Miami Dade College
Cecie StarrChristine EversLisa Starr
Chapter 2Life’s Chemical Basis
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Start With Atoms
• At life’s first level of organization, atoms interact with other atoms to form molecules
• The properties of molecules depend on, but differ from, those of their atomic components
• The behavior of elements, which make up all living things, depends on the structure of individual atoms
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• nucleus – Core of an atom; occupied by protons and neutrons
• proton – Positively charged subatomic particle that occurs in
the nucleus of all atoms
• neutron – Uncharged subatomic particle in the atomic
nucleus
• electron – Negatively charged subatomic particle that
occupies orbitals around an atomic nucleus
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• Isotopes are atoms of an element that differ in mass number
• isotopes – Forms of an element that differ in the
number of neutrons their atoms carry
• mass number – Total number of protons and neutrons in the
nucleus of an element’s atoms
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• radioisotope – Isotope with an unstable nucleus that
spontaneously emit subatomic particles or energy by the process of radioactive decay
• radioactive decay – Process by which atoms of a radioisotope
emit energy and/or subatomic particles when their nucleus spontaneously disintegrates, which can transform one element onto another
• tracer – Molecule labeled with a detectable
substance that track biological processes inside living organisms
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Cancerousthroattissue
PET, positron-emission tomography
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(a) A ball bouncing down a flight of stairs provides an analogy for energy levels of electrons
Third shell (highest energylevel)
Second shell (higherenergy level)
Energyabsorbed
First shell (lowest energylevel)
Atomicnucleus
(b)
Energylost
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Periodic table
Hydrogen
1H
Lithium
3LiBeryllium
4BeBoron
5BCarbon
6CNitrogen
7NOxygen
8OFluorine
9FNeon
10Ne
Helium
2HeAtomic number
Element symbol
Electron-distributiondiagram
Atomic mass
2He
4.00Firstshell
Secondshell
Thirdshell
Sodium
11NaMagnesium
12MgAluminum
13AlSilicon
14SiPhosphorus
15PSulfur
16SChlorine
17ClArgon
18Ar
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• shell model – Model of electron distribution in an atom that help
us visualize how electrons populate atoms from the innermost shell outward
• Concentric circles represent successive energy levels– 1st shell: up to 2 electrons– 2nd shell: up to 8 electrons– 3rd shell: up to 8 electrons
• ion – Charged atom
• electronegativity – Measure of the ability of an atom to pull electrons
away from other atoms
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Why Atoms Interact
• The characteristics of a bond arise from the properties of atoms that take part in it
• Atoms form different types of bonds depending on their electronegativity– Ionic bonds– Covalent bonds– Hydrogen bonds– Van der Waals interaction
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Ionic Bonds
• An ionic bond is a strong association between oppositely charged ions that arises from the mutual attraction of opposite charges
• ionic bond – Type of chemical bond in which a strong
mutual attraction forms between ions of opposite charge
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Covalent Bonds
• Atoms share a pair of electrons in a covalent bond, which is nonpolar if the sharing is equal, and polar if it is not
• covalent bond – Chemical bond in which two atoms share a pair of
electrons
• polarity – Any separation of charge into distinct positive and
negative regions
2, 3, or 4 covalent bonds may form between two atoms when they share multiple electrons
Molecular oxygen: O=OMolecular nitrogen: (N=N)
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Hydrogen Bonds
• Hydrogen bonds collectively stabilize the structures of large molecules
• hydrogen bond – Attraction that forms between a covalently
bonded hydrogen atom and another atom taking part in a separate covalent bond
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Water’s Life-Giving Properties• Water is essential to life because of its
unique properties:– Solvent for salts and other polar solutes– Resists temperature changes– Cohesion
• Unique properties of water result from extensive hydrogen bonding among water molecules
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Water Is an Excellent Solvent• Water is a solvent that easily dissolves
salts, sugars, and other polar substances
• solvent – Liquid that can dissolve other substances
• solute – A dissolved substance
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Hydrophilic and Hydrophobic
• Hydrophilic substances dissolve easily in water; hydrophobic substances do not
• hydrophilic – Substance that dissolves easily in water,
such as salt
• hydrophobic – Substance that resists dissolving in water,
such as oil
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• Ice forms below about 0°C (32°F) floats because the molecules pack less densely than in water
• evaporation – Transition of a liquid to a gas – Requires energy (removes heat from liquid)
Water resists changing its temperature because of its high specific heat
• High specific heat
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Cohesion• Hydrogen bonds cause water molecules to resist
separating from each other
• Cohesion
– Tendency of molecules to stick together – Pulls water upward in plants– Causes surface tension
• Adhesionan attraction between different substances, for example, between water and plant cell walls
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Neutral solution
Acidic solution
Basic solution
OH–
OH–
OH–
OH–
OH–OH–OH–
H+
H+
H+
OH–
H+ H+
H+ H+
OH–
OH–
OH–OH–
H+
OH–
H+
H+
H+
H+
H+
H+
H+
OH–
Neutral [H+] = [OH–]
Incr
easi
ngly
Aci
dic
[H+ ]
> [O
H– ]
Incr
easi
ngly
Bas
ic [H
+ ] <
[OH
– ]
pH Scale0
1
2
3
4
5
6
7
8
Battery acid
Gastric juice,lemon juice
Vinegar, beer,wine, cola
Tomato juice
Black coffee
RainwaterUrine
SalivaPure waterHuman blood, tears
Seawater
9
10Milk of magnesia
Household ammonia
Householdbleach
Oven cleaner
11
12
13
14
Acids and Bases
• Most biological processes occur within a narrow range of pH, typically around pH 7
• pH – Measure of
concentration of hydrogen ions (H+) in a fluid
• concentration – Number of molecules
or ions of a solute per unit volume of a solution
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Buffers• A buffer keeps a solution within a
consistent range of pH
• Most cell and body fluids are buffered because most molecules of life work only within a narrow range of pH
• buffer – Set of chemicals that stabilize pH of a
solution by alternately donating and accepting ions that contribute to pH
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The Bicarbonate Buffer System• Carbon dioxide gas becomes a weak acid when it
dissolves in the fluid portion of human blood:
H2O + CO2 (carbon dioxide) → H2CO3 (carbonic acid)
• Carbonic acid separates into hydrogen ions and bicarbonate ions, which can separate into hydrogen ions and carbonate ions :
H2CO3 (carbonic acid) ↔ H+ + HCO3-
(bicarbonate) ↔ H+ + H+ + CO3 -
2
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Bicarbonate Buffer System (cont.)
• Exchange of ions between carbonic acid and bicarbonate keeps blood pH between 7.3 and 7.5 – up to a point
• Buffer failure can be catastrophic in a biological system
• Example: Too much carbonic acid forms in blood when breathing is impaired suddenly – the resulting decline in blood pH may cause coma
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Fig. 3-10
Moreacidic
0
AcidrainAcidrain
Normalrain
Morebasic
123456789
1011121314
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Fig. 3-11
EXPERIMENT
RESULTS
Calc
ifica
tion
rate
(mm
ol C
aCO
3pe
r m2 p
er d
ay)
[CO32–] (µmol/kg)
150 200 250 3000
20
40
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Water vapor
H 2NH
3
“Atmosphere”
Electrode
Condenser
Coldwater
Cooled watercontainingorganicmolecules
Sample forchemical analysis
H2O“sea”
EXPERIMENT
CH4
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Long Nose Butterfly
Flatfish