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BIOL 1A > Unit 1 > Flashcards

Unit 1 Flashcards

1
Q

logical, rational, problem-solving way to investigate the world

A

Scientific Method

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2
Q

A suggested explanation for a test that one can test

A

Hypothesis

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3
Q

tested and confirmed explanation for observations and phenomena

A

Theory

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4
Q

any part of the experiment that can vary or change during the experiment

A

Variable

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5
Q

contains every feature of the experimental group except it is not given the manipulation that the researcher hypothesizes

A

Control Group

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6
Q

A suggested explanation for a test that one can test

A

Hypothesis

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7
Q

Necessary qualifications for a hypothesis

A

It has to be testable

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8
Q

aims to answer fundamental questions about biology

A

Basic Science

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9
Q

uses the information from basic science to solve real-world problems

A

Applied Science

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10
Q

Form of logical thinking that uses related observations to arrive at a general conclusion

A

Inductive Reasoning
Ex - I get tired if I don’t drink coffee. Coffee is addictive, I’m addicted to coffee.

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11
Q

form of logical thinking that uses a general principle or law to predict specific results

A

Deductive Reasoning
Ex - All dogs have ears; golden retrievers are dogs, therefore they have ears.

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12
Q

scientific papers that a scientist’s colleagues or peer reviews

A

Peer-Reviewed Manuscripts

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13
Q

Process of Peer Review

A

They share their findings in order for other research to expand and build upon their discoveries.

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14
Q

reports of original research that follow Introduction, Methods, Results, and Discussions format. Also have an abstract (quick summary) along with references and acknowledgements.

A

Primary Sources

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15
Q

summary and compile many primary sources, most common in literature reviews.

A

Secondary Sources

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16
Q

unique forms of matter with specific chemical and physical properties that cannot break down into smaller substances by ordinary chemical reactions

A

Elements

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17
Q

Elements of Highest Abundance

A

Oxygen, Carbon, Hydrogen, Nitrogen

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18
Q

positively charges

A

Proton

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19
Q

uncharged

A

Neutron

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20
Q

negatively charged

A

Electron

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21
Q

different forms of an element that have the same number of protons but a different number of neutrons

A

Isotopes

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22
Q

Some isotopes emit neutrons, protons, and electrons and attain a more stable atomic configuration. Radioactive decay then occurs which explains this process of the energy loss that occurs when an unstable atom’s nucleus releases radiation.

A

Radioisotopes

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23
Q

use process to backtrack on normal human decay of the body to see how old something is and by seeing how much carbon converted into nitrogen

A

Carbon Dating

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24
Q

Carbon-14 Half life

A

5,730 years

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25
Q

Periodic Table (Atomic number and mass)

A

The elements are organized and displayed according to their atomic number and are arranged in a series of rows and columns based on shared chemical and physical properties, In addition it provides the atomic number for each element, and the elements atomic mass.

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26
Q

the sharing of electrons between two molecules/atoms

A

Covalent Bonds

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27
Q

some atoms are more stable when they gain or lose an electron and form ions. So when an ion is given to another ion and it isn’t shared.

A

Ionic Bonds

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28
Q

negative ions that form by gaining electrons

A

Anion

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29
Q

positive ions that form by losing electrons

A

Cation

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30
Q

electrons are shared unequally between two atoms because of their electronegativity, so the electron will spend more time circling the oxygen atom in H20 then the hydrogen atom.

A

polar covalent bond

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31
Q

form between two atoms of the same elements or between different elements that share the electrons equally, AKA they have the same electronegativity.

A

Non-Polar Covalent Bonds

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32
Q

weak interactions between (example) when a hydrogen is bonded to an electronegative atom and another one

A

Hydrogen Bonds

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33
Q

In water what atoms are positively charged and which are negatively charged.

A

Hydrogen - slightly positive
Oxygen - slightly negative

34
Q

What type of bond dorms between different water molecules?

A

Hydrogen Bond

35
Q

4 Properties of water that make it an ideal medium for life.

A
  • Water is the Solvent for Life - It’s a polar solvent so it dissolves polar substances or Hydrophilic (water-loving)
  • Ice Floats on Water - The hydrogen bonds between ice is less dense than the water so the ice floats to the top, if ice sank lakes would freeze
  • Moderation of Temperature by Water - water has the highest specific heat capacity of any liquid and it takes it a lot longer to heat up or cool down than lets say land so animals may use it to regulate their temperature
  • Cohesion and Adhesion by Water Molecules - Cohesion (water molecules attracted to each other) and adhesion (attraction between water molecules and other molecules) is important for examples water uptake into trees from roots, and surface tension for some animals
36
Q

Relationship between concentration of hydrogen ions, hydroxide ions, and pH.

A

Hydrogen ions spontaneously generate in pure water by the ionization of a small percentage of water molecules into equal numbers of hydrogen ions and hydroxide ions. Hydroxide are kept in solution by their hydrogen atoms bonding with other water molecules, the hydrogen ions attract to un-ionized water molecules forming hydronium ions.

37
Q

When the pH is acidic..

A

increase in hydrogen ions

38
Q

When the pH is basic…

A

increase in hydroxide ions

39
Q

readily absorb excess Hydrogen or Hydroxide keep the body’s pH in a narrow range for survival

A

Buffer

40
Q

How buffers work

A
  • When bicarbonate ions combine with free hydrogen ions and become carbonic acid it removes the hydrogen ions, and moderates pH
  • Carbonic acid can convert to carbon dioxide gas which we then exhale through the lungs that prevent hydrogen ions from building up in the blood.
  • OR if too much hydroxide enters the system carbonic acid will combine with it to create bicarbonate, lowering the pH.
  • WITHOUT BUFFER SYSTEM BODY’S PH WOULD FLUCTUATION ENOUGH TO PUT SURVIVAL IN JEOPARDY.
41
Q

Why is carbon a versatile element?

A

because it can form covalent bonds to as many as four different atoms, making it a good “backbone” for macromolecules.

42
Q

molecules that share the same chemical formula but differ in the placement of their atoms or chemical bonds

A

Isomers

43
Q

differ in placement of their covalent bonds

A

Structural Isomers

44
Q

similar placements of covalent bonds but differ if how these bonds are made to the surrounding atoms

A

Geometric Isomers

45
Q

share the same chemical structure and chemical bonds but differ in the three-dimensional placement of atoms so that they are non-superimposable mirror images

A

Enantiomers

46
Q

the combination of monomers using covalent bonds to form larger molecules

A

Polymer

47
Q

single subunits most macromolecules are made from

A

Monomer

48
Q

breaks down big complex molecules into smaller, easier to absorb molecules

A

Catabolic

49
Q

builds molecules required for the body’s function

A

Anabolic

50
Q

When monomers form the polymers they release water molecules as a byproduct

A

Dehydration Reaction

51
Q

when polymers break down during hydrolysis, when inserting water molecules across the bond it breaks the covalent bonds and the polymer breaks into into monomers, one getting the hydrogen atom and the other the hydroxyl molecule

A

Hydrolysis

52
Q

simple sugars (mono = one, sacchar = sweet), number of carbons ranges from 3-7

A

Monosaccharides

53
Q

on the end

A

Aldose

54
Q

in the middle

A

Ketose

55
Q

two sugars covalently joined at a glycosidic bond, related because monosaccharides are one sugar molecules while this to two of those joined

A

Disaccharides

56
Q

the hydroxyl group of one monosaccharides joins with the hydrogen of another monosaccharides forming a covalent bond and dehydration synthesis

A

Glycosidic Linkage

57
Q

long polymers of monosaccharides

A

Polysaccharides

58
Q

polymers of alpha-glucose used to store energy (starch)
Found in nature from sugars in plants and amylose and amylopectin. Glycogen is a storage polysaccharide in animals

A

Polysaccharide (Energy Storage)

59
Q

polymers of beta-glucose (cellulose)
Cellulose - polymer of beta-glucose, found in nature in plant cell walls

A

Polysaccharides (Structural)

60
Q

store energy (formed by the joining of three fatty acids to a glycerol backbone in a dehydration reaction, three molecules of water are released in this process)

A

Triglycerides

61
Q

Types of Triglycerides

A

Saturant, Monounsaturated, Polyunsaturated

62
Q

major plasma membrane constituents that comprise cells outermost layer

A

Phospholipids

63
Q

Phospholipids in water

A

The Phospholipid has a hydrophilic head and a hydrophobic tail.

64
Q

fused ring structure, it’s necessary for the production of cholesterol which is necessary for the body to properly function.

A

Steroids

65
Q

monomers that comprise proteins

A

Amino Acids

66
Q

The functional groups present in every amino acid are,

A

amine and carboxyl

67
Q

Amino acids are classified by..

A

chiral or alpha carbon, amino group, hydrogen atom, carboxyl group, and a side chain (R group)

68
Q

covalent bond

A

Peptide Bond

69
Q

Polypeptide functional groups…

A

amino acids carboxyl group and the incoming amino acids group combining releasing a water molecule. The products that form the linkages are peptides and as more amino acids join to the growing chain the result is a polypeptide chain. Grows from the amino acid to the carboxyl end

70
Q

amino acids unique sequence in a polypeptide chain.

A

Primary structure of a protein

71
Q

local folding of the polypeptide in some regions (a-helix and b-pleated sheets)

A

Secondary Structure of a Protein

72
Q

polypeptides unique three-dimensional structure

A

Tertiary Structure of a Protein

73
Q

the interactions of proteins when they form from several polypeptides

A

Quaternary Structure of a Protein

74
Q

What happen to a protein in unfavorable conditions

A

the protein structure may change, losing its shape without losing its primary sequence which we call Denaturation.

75
Q

carry the cells genetic blueprint and carry instructions for its functioning

A

Nucleic Acid

76
Q

genetic material in all living organisms, in the nucleus of eukaryotes and in organelles, chloroplasts and mitochondria.

A

DNA

77
Q

mostly involved in protein synthesis

A

RNA

78
Q

cytosine, thymine and uracil, single-cell carbon-nitrogen rings as their primary structures

A

Pyrimidine

79
Q

3 Parts of a Nucletioide

A

nitrogen base, pentose (five-carbon) sugar, and phosphate group
These carbons are important because it distinguishes these residues from those in the base

80
Q

adenine and guanine, primary structure is two-carbon nitrogen rings

A

Purine

81
Q

Carbons in a Nucleotide

A

5C’ phosphate group
3C’ hydroxyl group important for synthesis of new DNA and RNA
2C’ Hydroxyl in RNA and hydroxyl in DNA

82
Q
A

BIOL 1A (3 decks)

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