Exam #1 Flashcards
(80 cards)
1
Q
carbon in biology
A
the framework of biological molecules consists primarily of carbon bonded to:
* another carbon
* O, N, S, P, and H
can form 4 covalent bonds
2
Q
hydrocarbons
A
- molecule consisting only of carbon and hydrogen
- HYDROCARBONS ARE NONPOLAR
3
Q
Isomers and the 2 types
A
- molecules with the same molecular/empirical formula (which means that they have the same # of atoms)
1. structural isomers
2. stereoisomers: differ in how groups are attached
4
Q
enantiomers
A
mirror image molecules = chiral
example: D-sugars
5
Q
define polymer
A
built by linking monomers
6
Q
define monomer
A
small, similar chemical subunits
7
Q
monomer for carbohydrates
A
monosaccharide
8
Q
monomer for nucleic acid
A
nucleotide
9
Q
monomer for protein
A
amino acid
10
Q
dehydration synthesis
A
- formation of large molecules by the removal of water
- monomers are joined to form polymers
11
Q
hydrolysis
A
- breakdown of large molecules by the addition of water
- polymers are broken down to monomers
12
Q
carbohydrates
A
- molecules with a 1:2:1 ratio of C, H, O
- CH2O
- C-H hold much energy
- Carbs are good energy storage
- example: sugars, starch
13
Q
Monosaccharides
A
- simplest carbohydrate
- 6 carbon sugars are important
14
Q
glucose
A
C6H12O6
* fructose is a structural isomer of glucose
* galactose is a stereoisomer of glucose
15
Q
Disaccharides
A
- 2 monosaccharides linked together by dehydration synthesis
- used for sugar transport or energy storage
- sucrose, lactose, maltose
16
Q
polysaccharides
A
- long chains of monosaccharides (linked thru dehydration synthesis)
- energy storage (plants use starch)
- structural support (plants use cellulose)
17
Q
nucleic acids
name polymer and monomer
A
polymer: nucleic acids
monomers: nucleotides
* nucleotides are connected by phosphodiester bonds
18
Q
nitrogenous bases include:
A
purines: adenine and guanine
pyrimidines: thymine, cytosine and uracil
19
Q
deoxyribonucleic acid (DNA)
A
- encodes information for amino acid sequence of proteins
- base-pairing rules:
A with T (or U in RNA)
C with G
20
Q
define double helix
A
2 polynucleotide strands connected by hydrogen bonds
21
Q
ATP
A
adenosine triphosphate
- primary energy currency of the cell
21
Q
ribonucleic acid (RNA)
A
- single polynucleotide strand
- RNA uses info in DNA to specify sequence of amino acids in proteins
21
Q
DNA vs RNA
A
DNA
* contains deoxyribose
* contains thymine
* double stranded sugar phosphate
RNA
* contains ribose
* contains uracil
* sigle stranded sugar phosphate
22
Q
NAD+ and FAD+
A
- nicotinamide adenine dinucleotide
- flavin adenine dinucleotide
- electron carriers for many cellular rxns
23
the 7 protein functions:
1. enzyme catalysis
2. defense
3. transport
4. support
5. motion
6. regulation
7. storage
24
protein
* proteins are polymers
- composed of 1 or more long, unbranched chains
* amino acids are monomers
* amino acids are joined by dehydration synthesis
- peptide bond
25
1st and 2nd levels of protein structure
shape of protein = its function
1. primary: sequence of AA
2. secondary: interaction of groups in the peptide backbone
* alpha helix
* beta helix
26
3rd and 4th levels of protein structure
3. tertiary: final folded shape of a globular protein
- stabilized by a number of forces
- final level of structure IF protein only consists of a single polypeptide chain
4. quaternary: arrangement of individual chains (subunits) in a protein with 2 or more polypeptide chains
27
motifs
| additional structural characteristics
- common elements of secondary structure seen in many polypeptides
- useful in determining the function of unknown proteins
28
domains
| additional structural characteristics
* functional units within a larger structure
* most proteins made of multiple domains that perform different parts of the protein's function
29
chaperone proteins
* chaperone proteins help protein fold correctly
* deficiencies in chaperone proteins implicated in certain diseases
- cystic fibrosis (protein fails to fold)
30
define matter
* matter has mass and occupies space
* all matter is composed of atoms
31
atomic structure
atoms are composed of:
Protons: (+) located in the nucleus
Neutrons: neutral charge, located in the nucleus
Electrons: (-) located in orbitals surrounding the nucleus
32
atomic number
atomic number = number of protons
number of protons = number of electrons
33
define element
any substance that cannot be broken down to any other substance by ordinary chemcial means
34
mass vs weight
mass: refers to the amount of substance
weight: refers to force gravity exerts on substance
35
atomic mass
atomic mass = sum of protons and neutrons
* each proton and neutron has a mass of 1 dalton
36
ions
charged particles, means that they are unbalanced
N3-
37
cation
(+ charge), more protons than electrons
38
anion
(- charge), more electrons than protons
39
isotopes
* atoms of a single element that possess different numbers of neutrons
* radioactive isotopes are unstable and emit radiaion as the nucleus breaks up
* Half-life: time it takes for one-half of the atoms in a sample to decay
40
electron arrangement
* chemical behavior is due to the number and arrangemnet of its electrons
* Bohr: electrons in discrete orbitals
**no orbital can contain more than 2 electrons**
41
electron energy trends
electrons farther from the nucleus have more energy
42
redox
in some rxns, electrons can be transferred from one atom to another
43
oxidation
loss of an electron
44
reduction
gain of an electron
| OIL RIG
45
valence electrons
number of electrons in outermost energy level
46
define inert
(nonreactive) elements have all eight electrons
47
define molecules
groups of atoms held together in a stable association
48
define compounds
are molecules containing more than one type of element
49
ionic bonding
* formed by the attraction of oppositely charged ions
* gain or loss of electrons forms ions Na+
* electrical attraction of water molecules can disrupt the forces that hold ions together
50
covalent bonding
when atoms share 2 or more valence electrons
51
electronegativity
* atoms affinity for electrons
* most electronegative element is F
* nonpolar covalent bonds = equal sharing of electrons
* polar covalent bonds = unequal sharing of electrons
the more electronegative atom wants the electrons more
52
chemical rxn
involve the formation or breaking of chemical bonds
reactants = orginal molecules
products = molecules resulitng from rxn
53
3 things that influence chemical rxns
1. temperature
2. concentration of reactants and products
3. catalysts
54
polarity of water
* within the water molecule, the bonds between oxygen and hydrogen are highly polar
- O is much more electronegative than H
* partial electrical charges develop
- Oxygen is partially negative δ-
- Hydrogen is partially positive δ+
55
cohesion
polarity of water allows water molecules to be atteached to one another
(water molecules stick to each other due to hydrogen bonds)
56
adhesion
water molecules stick to other polar molecules by hydrogen bonding
57
6 properties of water
1. water has a high specifc heat
2. water has a high heat of vaporization
3. solid water is less dense than liquid water
4. water is a good solvent
5. water organizes nonpolar molecules
6. water can form ions
58
pH
pH is the negative logarithm of hydrogen ion concentration of solution
59
define acid
* any substance that dissociates in water to increase the [H+] and lower pH
* the stronger the acid the more hydrogen ions it produces
60
define base
* any substance that combines with H+ dissolved in water, and thus lowers the [H+]
61
Buffers
* a substance that resists changes in pH
* they **release** hydrogen ions when a **base** is added
* **absorbing** hydrogen ions when **acid** is added
62
7 characteristics of all living organisms
1. Composed of cells
2. Complex and ordered
3. Respond to their environment
4. Can grow, develop, and reproduce
5. Obtain and use energy
6. Maintain internal balance
7. Allow for evolutionary adaptation
63
hypothesis
tentative educated guess
64
theory
description of the world that covers a relatively large number of phenomena and has met many observations and experimental test
65
"law of nature"
an overarching statement of how the universe works
66
scientific method
1. Make an observation/identify a pattern
2. Create a hypothesis
3. Device an experiment to test the prediction of the hypothesis
4. Test the prediction by running the experiment
5. Evaluate the results of the experiment against your hypothesis
6.Repeat
67
deductive and inductive reasoning
- Deductive reasoning uses general principles to make specific predictions
- Inductive reasoning uses specific observations to develop general conclusions
68
define reductionism (philosophical approach)
to break a complex process down into its simpler parts
69
define systems biology (philosophical approach)
focus on emergent properties that can’t be understood by looking at simpler parts
70
cell theory
- All organisms composed of cells
- Cells are basic units of life
- All cells come from preexisting cells
71
define gene
discrete unit of information
72
genome
entire set of DNA instructions
73
bacteria
single-celled prokaryote
74
archaea
single-celled prokaryote
75
eukarya
single-celled or multicelled eukaryote
76
evolutionary conservation
all organisms today descended from a simple creature 3.5 billion years aog
77
nonequilibrium state
* living systems are open systems
* constant supply of energy needed
78
Darwin and Evolution Book
on the origin of species by means of natural selection
