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A&P I Lecture > Chapter 2 (I) > Flashcards

Chapter 2 (I) Flashcards

(69 cards)

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1
Q

what cannot be broken down into simpler substances by ordinary chemical methods?

A

elements

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2
Q

what are the unique building blocks for each element and give each element its physical and chemical properties?

A

atoms

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3
Q

what 4 elements make up 96.1% of body mass?

A

carbon, hydrogen, oxygen, and nitrogen

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4
Q

what is the purpose of carbon, hydrogen, oxygen, and nitrogen?

A

they are the structure of biomolecules

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5
Q

what 9 elements make up 3.9% of body mass?

A

calcium, chlorine, magnesium, sulfur, iodine, potassium, sodium, iron, and phosphorous

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6
Q

what elements generate electric potentials of cells?

A

sodium and potassium

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7
Q

what element is involved in cell signaling, muscle contraction, and bone mineralization?

A

calcium

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8
Q

what element stores chemical energy for cell processes?

A

phosphorous

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9
Q

the 11 elements that make up less than 0.01% of body mass are part of/activate what?

A

enzymes

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10
Q

what is composed of subatomic particles?

A

atoms

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11
Q

where are protons and neutrons found?

A

nucleus

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12
Q

where are electrons found?

A

orbiting the nucleus

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13
Q

the number of protons and electrons are always ______.

A

equal

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14
Q

what model is simplified/outdated and incorrectly depicts fixed circular electron paths around the nucleus?

A

planetary model

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15
Q

what model is current/used by chemists, depicts probable regions of greater electrons density, and predicts chemical behavior of atoms?

A

orbital model

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16
Q

atomic number

A

number of protons in nucleus

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17
Q

mass number

A

total number of protons and neutrons in nucleus

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18
Q

what has structural variations of atoms and differ in the number of neutrons they contain?

A

isotopes

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19
Q

atomic weight

A

average of mass numbers of all isotopes of an atom

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20
Q

radioisotopes

A

heavy isotopes decompose to more stable forms

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21
Q

spontaneous decay is called what?

A

radioactivity

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22
Q

what can be detected with a scanner (PET scan)?

A

radioisotopes

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23
Q

why are radioisotopes valuable tools?

A

for biological research and medicine and diagnosis

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24
Q

what damages living tissue and can destroy localized cancers?

A

radioisotopes

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25
molecule vs compound
molecule: made up of 2/more atoms bonded together compound: 2/more different kinds of atoms bonded
26
most matter exists as
mixtures
27
what are the 3 types of mixtures?
solutions, colloids, and suspensions
28
solutions
homogeneous gas, liquid, solid dissolved in water transparent
29
concentration of solutions can be expressed as what?
percent of solute in total solution milligrams per deciliter molarity (mol/L)
30
colloids
heterogeneous large solute particles that do not settle out sol-gel transformations
31
suspensions
heterogeneous | large, visible solutes settle out
32
what has no chemical bonding between components, can be separated by physical means, and is either homogeneous or heterogeneous?
mixture
33
what has chemical bonding between components, can be separated only by breaking bonds, and are all homogeneous?
compounds
34
chemical bonds
energy relationships between electrons
35
what type of electrons have the most potential energy and are all chemically reactive?
valence electrons
36
what elements are stable, un-reactive, have a fully occupied valence shell, and are noble gases?
chemically inert elements
37
what elements have an unfilled valence shell and tend to gain, lose, or share electrons with other atoms to achieve stability?
chemically reactive elements
38
what are true bonds? what are not true bonds?
true bonds: ionic and covalent bonds | not true bonds: hydrogen bonds
39
what is an atom that gains or loses electrons and becomes charged?
ions
40
ionic bonds
transfer valence shell electrons from 1 atom to another to form ions attraction of opposite charges result in a bond
41
in an ionic bond the metal gives to the nonmetal, making the metal a _______ and nonmetal a ______.
``` metal= cation nonmetal= anion ```
42
most ionic compounds are ______.
salts
43
dry salts form ______ instead of individual molecules.
crystals
44
covalent bonds
share 2 or more valence shell electrons | deals mostly with nonmetals
45
20 amino acids are similar except in their "R" group. what does this mean in an organic chemistry context?
always know what these atoms are going to do
46
amino acids are linked together by what kind of reaction and form what type of bonds?
linked together by dehydration synthesis | form peptide bonds
47
nonpolar covalent bonds
electrons shared equally | electrically balanced
48
how do you breathe out carbon dioxide?
carbon dioxide cannot dissolve in the blood so it converts to its ionic form (bicarbonate) to get it dissolved in the blood and return to the lungs
49
polar covalent bonds
unequal sharing of electrons | produce dipole molecules
50
small atoms with 6 or 7 valence shell electrons are _______ and atoms with 1 or 2 valence shell electrons are _______.
6/7 valence shell electrons = electronegative | 1/2 valence shell electrons = electropositive
51
hydrogen bonds
attractive force between electropositive hydrogens and electronegative atoms
52
hydrogen bonds act as ______ bonds, holding a large molecule in a 3D shape.
intramolecular
53
what bond results in high surface tension of water?
hydrogen bonds
54
chemical reactions occur when chemical bonds are ______, ______, or ______.
formed, rearranged, or broken
55
what reactions combine to form larger, more complex molecule and always involve bond formation?
synthesis reactions
56
amino acids are joined together to form a protein molecule is an example of what reaction?
synthesis
57
what reactions break down into smaller molecules?
decomposition reactions
58
glycogen breaking down to release glucose units is an example of what reaction?
decomposition
59
what reactions are also called displacement reactions and involve both synthesis and decomposition?
exchange reactions
60
ATP transferring its terminal phosphate group to glucose to form glucose phosphate is an example of what reaction?
exchange
61
what reactions are both decomposition reactions and exchange reactions?
redox reactions
62
glucose being oxidized and oxygen being reduced in glycolysis is an example of what reaction?
redox
63
what reaction has a net release of energy, with products that have less potential energy than reactants, and are catabolic/oxidative reactions?
exergonic reactions
64
what reaction has a net absorption of energy, with products that have more potential energy than reactants, and are anabolic reactions?
endergonic reactions
65
how do you speed up an endergonic reaction? how do you speed up an exergonic reaction?
endergonic: give reaction heat exergonic: take away heat (ice bath)
66
all chemical reactions are theoretically ______ and many biological reactions are essentially ______.
chem rxns: reversible | bio rxns: irreversible
67
why are biological reactions irreversible?
energy requirements and removal of products
68
how do you increase rate of reaction?
increased temperature and concentration decreased particle size catalysts
69
what are catalysts?
increase rate without being chemically changed/part of product

A&P I Lecture (8 decks)

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