Chapters 1-4 Flashcards
(165 cards)
1
Q
Seven characteristics of living things:
A
- cellular organization
- ordered complexity
- sensitivity
- growth development reproduction
- energy utilization
- homeostasis
- evolutionary adaption
2
Q
Living systems 3 hierarchical organizations:
A
- cellular level
- organism all level
- populational level
3
Q
Sub divisions of cellular level:
A
1- atoms 2-molecule 3-macromolecule 4-organelle 5- cell
4
Q
Sub division of organismal level:
A
1- tissue
2- organ
3- organ system
4- organism
5
Q
Sub divisions of populational level:
A
1-population 2- species 3- community 4- ecosystem 5-biosphere
6
Q
Cellular organization:
A
Organisms consist of one or more cells
•cells carry out basic activities of living
•bound by membrane that separates it from its surroundings
7
Q
Sensitivity:
A
All organisms respond to stimuli
•ex plants grow towards the light
8
Q
Energy utilization:
A
All organisms take in energy to do work
Ex: muscles powered by food
9
Q
Evolutionary adaptation:
A
All organisms interact with others and non living environment
Influence their survival
10
Q
Tissue:
A
Groups of similar cells that act as a functional unit
11
Q
Organs:
A
Groups of different tissues
12
Q
Population:
A
Group of same species living together
13
Q
Species
A
All populations of a particular type of organism together
14
Q
Community
A
Populations of All different species living together
15
Q
Deductive reasoning
A
General principles used
16
Q
Inductive reasoning
A
Logic reasoning
•using specific reasoning
17
Q
Hypothesis
A
Suggested explanation accounting for an observation
18
Q
Experiment
A
Test of hypothesis
19
Q
Variables
A
- test experiment
* control experiment
20
Q
Test experiment
A
One variable is altered
21
Q
Control experiment
A
No variable is altered
22
Q
Reductionism
A
Reduces complex systems to working parts to analyze
•focuses on a specific part
23
Q
Theory
A
Interconnected concepts collected by scientific reasoning and experimental evidence
24
Q
Basic research vs applied research
A
•basic: extend boundaries of what we know •at universities •applied: uses basic as a foundation •work in industry Ex: creation of new drugs
25
Darwin facts
* natural selection
* 19th century
* Galapagos islands
* eating different foods on different islands, finches beaks had changed during decent
* artificial selection
26
Thomas Malthus: an essay of the principle population.
People population increases geometrically (fast)
•food increases arithmetically (slower fixed rate)
•deaths limit population
27
The earth formed ____ years ago.
4.5 BYA
28
Darwin received criticism in area of heredity. What proved skeptics wrong?
When genetics was figured out
| -were able to understand laws if inheritance
29
Homologous
Same evolutionary origin
•different structure and function
•ex: human and car
30
Analogous
Same function
| •different evolutionary origins
31
Phylogenetic tree
Represents the evolutionary history of the gene, it's family tree
•shows pattern of decent
32
Cell theory
Conclude that all living organisms consist of cells
•cells come from preexisting cells
• proposed by Theodore Schwann and matthias Scheiden
33
DNA
* information that identifies what a cell is like
* formed from two long chains
* four nucleotides, wound around each other
34
Gene
Made of different nucleotides
35
Gnome
Entire set if DNA that specifies a cell
36
Domain: Bacteria
Single cell organisms
| •prokaryotes
37
Domain: archaea
Single cell organisms
• prokaryotes
•little internal structure
38
Domain: eukarya four kingdoms
```
•plantae
•fungi
•animalia
•protista
*complex organized cell or multiple complex cells
```
39
Domain eukarya: kingdom Protista
* unicellular eukaryotes
| * except yeasts
40
Kingdom animalia
* organisms that lack cells walls
| * obtain energy by ingesting other organisms then ingesting internally
41
Kingdom plantae
* have cell walls
| * photosynthesis
42
Kingdom fungi
* cell walls if chitin
| * take in energy by secreting enzymes then absorbing products from external environment
43
Scientists believe that organisms have ___ from simple cellular creatures from 3.5 BYA
Descended
44
Matter is made up of small particles called
Atoms
45
What did Bohr propose?
Every atom has an orbiting cloud of subatomic particles orbiting it called electrons
46
What makes up the center of an atom?
Protons and neutrons
47
Atomic number
Number of protons an atom contains
48
Neutral atom if:
If atom has one electron for every proton
| •considered electrical neutral
49
What does electron effect?
•chemicals behavior of an atom, due to configuration of electrons
50
Element
Atoms with the same atomic numbers and same chemical properties
51
Atomic mass
The sum of an atoms protons and neutrons
52
Neutral atoms
Have same number of protons and electrons
•have no net charge
•electrons are negative, protons positive, balancing out each other
53
Ions
* electrons does not equal number of protons
| * charged particles
54
Cation
More protons than electrons
| •positive charge
55
Anion
More electrons than protons
| •negative charge
56
Isotopes
•same element
•different number of neutrons
(Same #protons)
Ex: C12 C13 C14
57
Radioactive isotopes
* radioactive decay: atom tried to break down into smaller atomic numbers
* unstable
* isotopes with same characteristics are called radioactive
58
Half life
For any given isotope the rate of decay is constant
| •decay time is know as half life, how long it takes to break down half the atoms in a sample
59
Electrons determine
Chemical behavior of atoms
60
Orbital energy levels in atoms:
* closer to the nucleus, less energy
* gains energy as it climbs ladder
* electrons energy is determined by how far it is from nucleus NOT what orbital it's in
* energy levels is what is responsible for the chemical reactivity of elements
61
Oxidation
* occurs during chemical reaction when electron is transferred from one atom to another
* LOSS OF ELECTRON
* making atom more positive
62
Reduction
* GAIN OF ELECTRON (gaining a negative ion)
| * makes atom more negative
63
Redox reactions
When one atom is oxidized and one atom is reduced in same reaction
64
Dmitri Mendeleev
Creator of periodic table of elements
•based on electron interactions at their outermost energy level
•valence electrons
65
Valence electrons
Electrons in outermost energy levels
| •basis for elements differing properties
66
Octet rule
* mendeleevs period table based off this principle
* atoms tend to completely fill outer energy levels
* no more than 8 electrons
* one s orbital and three p orbitals
67
Organic compounds
Contain only CHON
68
Molecule
Group held together in a stable association
69
Compound
When molecule contains atoms of more than one element
70
Chemical bonds
Atoms in a molecule are joined by these
71
List bond times in decreasing order of strength:
```
1- covalent- strong
2-ionic
3- hydrogen
4- hydrophobic interaction
5- van der Waals attraction -weak
```
72
NaCl
Is an ionic compound
•electrically neutral
•Na+ Cl- (na loses ion to cl)
•When placed in water, breaks up into equal parts Na+ and Ca-
73
Covalent Bond qualities
```
1- had no net charge
2- the octet rule is satisfied
3- has no unpaired electrons
*strongest bonds are triple bonds
**ex: N2 triple
**ex: O2 double
**ex: H2 single
```
74
Electronegativity
* an atoms affinity for electrons
* increases left to right across the table
* decrease down column
* atoms that different greatly in electronegativity, the shared electrons are more Likely going to be closer to the atom with greater electro negativity
75
Nonpolar
When electrons are evenly shared
| •common in atoms identical to each other
76
Polar covalent
Unequal distribution of electrons resulting in partial negatives near more electromagnetic atom and partial positives near less electromagnetic atom
77
Chemical reaction
All involve shifting of atoms from one molecule or ionic compound to another without any change in number or identity if the atoms
78
What are chemical reactions influenced by?
* Temperature
* concentration of reactants and products
* catalysts
79
Catalysts
Substance that increase the rate of reaction
•doesn't alter the reactions equilibrium
•shortens the time needed to reach equilibrium
80
Hydrogen bonds
Formed by water molecules
• are important to DNA and protein structure
•between the H and O
•responsible for chemical organization in living systems
81
Water is highly what?
Polar
•electronegativity of O is much greater than H
•makes bonds highly polar
•this quality underlies waters chemistry and the chemistry of life
82
Explain the cohesiveness of water molecules:
* waters polarity causes attractions between molecules aka cohesion
* hydrogen holds water molecules together
* weak bonds but made up for because of high number of bonds
* ex: leaves pull water upward from roots
83
Explain waters surface tension:
All surface water molecules are hydrogen bonded to molecules below them
•creates surface for insects to walk on air water interface
84
Adhesion
Water also attracts other polar substances
| Ex: adhesion of water to glass surface, will climb up glass
85
Properties of water
```
Cohesion
•high specific heat
•high heat of vaporization
•lower density of ice
•solubility
```
86
Explain high specific heat in water:
Hydrogen bonds absorb heat when they break
•release heat when they form
•minimizing temperature changes
Ex: water stabilizes the temperature of organisms in the environment
**1g of substance must absorb to change in 1 degree Celsius
87
Explain the high heat of vaporization in water:
Many hydrogen bonds must be broken for water to evaporate
Ex: evaporation of water cools body surfaces
*energy required to change 1g of a substance from a liquid to a gas
88
Explain the lower density of ice relating to water:
Water molecules in an ice crystal are spaced relatively far apart because of hydrogen bonding
Ex: because ice is less dense, allows animals to live under the sea
89
Explain solubility in water:
Polar water molecules are attracted to ions in polar compounds, making. These compound soluble
Ex: permitting diverse chemical reactions because the molecules can move freely in cells
90
Hydrophobic
Water fearing
| •non polar molecules such as oils that shrink from contact of water
91
Hydrophilic
Polar molecules that readily form hydrogen bonds
92
Hydrophobic exclusion
Tendency of no polar molecules to aggregate in water
93
Ionization
When a proton dissociates from a molecule, leaving the rest of the molecule negative and the proton positive
•ex: H2O--> OH- (hydroxide ion)+ H+ (hydrogen ion)
94
pH scale
Expressed hydrogen ion concentration or a solution
•meaning partial hydrogen
• pH= -log[H+]
•is written 10 to the -7, would be 7 on the pH scale
•1 on the scale represent a 10 fold change
Ex: 4= 10 times more H+ than 5 and 100 times more than 5
95
Acids
* any substance that dissociates in water to increase the H+
| * and lower the pH
96
Pure waters pH would be
Neutral
| •neither acidic or basic
97
Bases
* a substance that combines with H+ in water
* thus lowering the H+
* pH values above 7
98
Buffer
* substance that resists change in pH
* release ions when a base is added
* absorbs hydrogen ions when acid is added
99
What is the equation for photosynthesis?
6H20+6CO2-->C6H12O2+6O2
100
Equation for disassociation of water
H2O--> OH- + H+
101
Explain buffers
Absorb or release hydrogen ions to create a stable pH
•ex: buffers in the blood stream, when becomes over saturated with CO2 body is signaled to breathe and release excess gas
102
Radioactive decay vs chemical reactions
Chemical reactions involve changes in the electronic configuration of atoms
• radioactive decay involves decay of nucleus producing another atom and emitting radiation
103
What distinguishes an atom of one element from an atom of another?
#of protons
104
Valence electrons are associated with what type of bonds?
Ionic
105
A molecule with polar covalent bonds would
Be soluble in water
106
Hydrogen is formed when
When hydrogen is part of a polar bond
107
Structural isomer
Identical chemical groups bonded to different carbon atoms
108
Stereoisomer
Has identical chemical groups bonded to same carbon, but in different orientation
109
Monosaccharide
Simplest carbs
•contain as few as three carbons
•6 carbon monosaccharides play key roll in energy storage
110
Disaccharides
Two monosaccharides bonded together
•transport forms of sugar
•harder to break down bond unless enzyme specific
111
5 carbon sugars
* Deoxyribose
| * ribose
112
6 carbon sugars aka monosaccharides
* glucose
* fructose (pentose)
* galactose
113
Disaccharides form by
Dehydration reaction
114
Glucose and fructose are made into sucrose by what reaction?
Dehydration reaction
115
How does alpha glucose and beta glucose differ?
-OH bond to carbon
116
Plants use sucrose to
Transport glucose
117
Sucrose is commonly _____ by humans and animals
Eaten
118
Polysaccharides
•longer polymers made of monosaccharides joined by dehydration synthesis
119
Starch
Storage polysaccharide
•made if alpha glucose linked in chains
•simplest structure starch is amylose
120
Cellulose
Structural polysaccharide
| •made of beta glucose linkages
121
The bonds between adjacent glucose molecules In cellulose are
Glycosidic linkages
122
Cellulose
* unbranched and form long strong fibers
* resistant to metabolic breakdown
* ex: why wood is used for building
* makes plant cell walls
123
Chitin
* structural material found in Arthropods and fungi
| * hard exoskeleton when formed with proteins
124
Hydroxyl group
-OH
125
Carbonyl group
O=C
126
Carboxyl
C=O
+
-OH
127
Amino
H-N-H
| Amino group
128
Sulfhydryl
-S-H
| In proteins
129
Phosphate
P surrounded by one double bonded O, one single bonded O and two -O's
130
Methyl
C surrounded by three H
| Found in proteins
131
Isomer
Have same empirical formula but exists in different forms
132
Four types of polymer macromolecules
Lipids
Proteins
Carbohydrates
Nucleic acids
133
Polymer
Long molecule made by linking together smaller units know as monomers
134
Two main nucleic acids
DNA
| RNA
135
Nucleotides
Nucleic acids are long polymers of repeating subunits called
136
Nucleic acid is
A chain of five carbon sugars
Linked by phosphodiester
With a nitrogenous base coming off each sugar
137
Purines
Large double ring molecules
Found in DNA and RNA
ex: guanine and adenine
138
Pyramidines
Smaller single ring molecules
Found only in DNA
Ex: thymine
139
DNA
* has four different types of nucleotides that can be arranged differently
* has hydrogen bonds between nitrogenous bases
* deoxyribose back bone
* double helix
* consists of two polynucleotide chains wrapped in double helix
140
RNA
Had a ribose phosphate back bone
•nitrogenous bases
•use uracil not thymine
•single stranded
141
Adenine is key component of the molecule____
ATP- the energy currency of cells
142
Main protein functions
* enzyme catalyst: facilitates chemical reactions
* defense: recognize cancer cells, dominates immune system
* transport:transport O2 in blood
* support:hair skin nails
* motion:muscle contraction by filaments
* regulation:hormones act as intercellular messengers
* storage: calcium and iron are stored in the body
143
Amino acids
Contain and amino group (-NH2)
And an acidic carboxyl groups (-COOH)
•order of amino acids determines proteins structure and function
144
Proteins
Linear polymers made with 20 different amino acids
145
20 amino acids grouped into 5 chemical classes based on R group. They are:
```
Nonpolar
Polar uncharged
Charged
Aromatic amino acids
Amino acids with unique qualities
```
146
Peptide bond
Covalent bond that links two amino acids
| -through dehydration synthesis
147
Polypeptide
A long unbranched chain, many make up proteins
148
Primary structure
It's amino sequence
149
Secondary structure
Alpha helix/beta sheet
•hydrogen bonding between r groups
•motifs made here
150
Tertiary structure
Final globular shape of a protein
•determined by the chemical nature if its side groups
•3D shape
•domains former here
151
Quaternary structure
Multiple polypeptides arranged together to form a functional protein
•two or more
152
Chaperone proteins
Help proteins fold correctly
153
Denaturation
When proteins environment is altered it may chance it's shape
154
Disassociation
Subunits that dissociate without losing their individual tertiary structure
155
Lipids
```
•insoluble in water
•fatty acids and glycerol
•stores energy in fat
•has high proportion of nonpolar C-H bonds
•nonpolar away from water, hydrophobic
•polar hydrophilic end towards the water
•
```
156
Fatty acids
Long chain hydrocarbons with carboxylic acid (COOH) at one end
157
Glycerol
Three carbon polyalcohol (three -OH) groups
158
Most lipids consist of
A glycerol molecule with three fatty acids attached, one to each carbon of the glycerol backbone
159
Triglyceride
Containing three fatty acids
160
Saturated
Having all hydrogen atoms possible
| •single bonds only
161
Unsaturated
Has double bonds between one it more pairs of carbons
162
Polyunsaturated
Fatty acids with one double bond are called monounsaturated while multiple double bonds are polyunsaturated
163
Phospholipids
* form membranes
| * a triglyceride with a phosphate replacing one of the fatty acids
164
Phospholipid sub units
Glycerol
Fatty acid chains
A phosphate group
- has a polar head and non polar tail
165
Micelles
When polar head goes towards the water and nonpolar tails away from the water
