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

Chapter 2 (I) Flashcards

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what model is simplified/outdated and incorrectly depicts fixed circular electron paths around the nucleus?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

molecule vs compound

A

molecule: made up of 2/more atoms bonded together
compound: 2/more different kinds of atoms bonded

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26
Q

most matter exists as

A

mixtures

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27
Q

what are the 3 types of mixtures?

A

solutions, colloids, and suspensions

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28
Q

solutions

A

homogeneous
gas, liquid, solid dissolved in water
transparent

29
Q

concentration of solutions can be expressed as what?

A

percent of solute in total solution
milligrams per deciliter
molarity (mol/L)

30
Q

colloids

A

heterogeneous
large solute particles that do not settle out
sol-gel transformations

31
Q

suspensions

A

heterogeneous

large, visible solutes settle out

32
Q

what has no chemical bonding between components, can be separated by physical means, and is either homogeneous or heterogeneous?

A

mixture

33
Q

what has chemical bonding between components, can be separated only by breaking bonds, and are all homogeneous?

A

compounds

34
Q

chemical bonds

A

energy relationships between electrons

35
Q

what type of electrons have the most potential energy and are all chemically reactive?

A

valence electrons

36
Q

what elements are stable, un-reactive, have a fully occupied valence shell, and are noble gases?

A

chemically inert elements

37
Q

what elements have an unfilled valence shell and tend to gain, lose, or share electrons with other atoms to achieve stability?

A

chemically reactive elements

38
Q

what are true bonds? what are not true bonds?

A

true bonds: ionic and covalent bonds

not true bonds: hydrogen bonds

39
Q

what is an atom that gains or loses electrons and becomes charged?

A

ions

40
Q

ionic bonds

A

transfer valence shell electrons from 1 atom to another to form ions
attraction of opposite charges result in a bond

41
Q

in an ionic bond the metal gives to the nonmetal, making the metal a _______ and nonmetal a ______.

A 
metal= cation
nonmetal= anion
42
Q

most ionic compounds are ______.

A

salts

43
Q

dry salts form ______ instead of individual molecules.

A

crystals

44
Q

covalent bonds

A

share 2 or more valence shell electrons

deals mostly with nonmetals

45
Q

20 amino acids are similar except in their “R” group. what does this mean in an organic chemistry context?

A

always know what these atoms are going to do

46
Q

amino acids are linked together by what kind of reaction and form what type of bonds?

A

linked together by dehydration synthesis

form peptide bonds

47
Q

nonpolar covalent bonds

A

electrons shared equally

electrically balanced

48
Q

how do you breathe out carbon dioxide?

A

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
Q

polar covalent bonds

A

unequal sharing of electrons

produce dipole molecules

50
Q

small atoms with 6 or 7 valence shell electrons are _______ and atoms with 1 or 2 valence shell electrons are _______.

A

6/7 valence shell electrons = electronegative

1/2 valence shell electrons = electropositive

51
Q

hydrogen bonds

A

attractive force between electropositive hydrogens and electronegative atoms

52
Q

hydrogen bonds act as ______ bonds, holding a large molecule in a 3D shape.

A

intramolecular

53
Q

what bond results in high surface tension of water?

A

hydrogen bonds

54
Q

chemical reactions occur when chemical bonds are ______, ______, or ______.

A

formed, rearranged, or broken

55
Q

what reactions combine to form larger, more complex molecule and always involve bond formation?

A

synthesis reactions

56
Q

amino acids are joined together to form a protein molecule is an example of what reaction?

A

synthesis

57
Q

what reactions break down into smaller molecules?

A

decomposition reactions

58
Q

glycogen breaking down to release glucose units is an example of what reaction?

A

decomposition

59
Q

what reactions are also called displacement reactions and involve both synthesis and decomposition?

A

exchange reactions

60
Q

ATP transferring its terminal phosphate group to glucose to form glucose phosphate is an example of what reaction?

A

exchange

61
Q

what reactions are both decomposition reactions and exchange reactions?

A

redox reactions

62
Q

glucose being oxidized and oxygen being reduced in glycolysis is an example of what reaction?

A

redox

63
Q

what reaction has a net release of energy, with products that have less potential energy than reactants, and are catabolic/oxidative reactions?

A

exergonic reactions

64
Q

what reaction has a net absorption of energy, with products that have more potential energy than reactants, and are anabolic reactions?

A

endergonic reactions

65
Q

how do you speed up an endergonic reaction? how do you speed up an exergonic reaction?

A

endergonic: give reaction heat
exergonic: take away heat (ice bath)

66
Q

all chemical reactions are theoretically ______ and many biological reactions are essentially ______.

A

chem rxns: reversible

bio rxns: irreversible

67
Q

why are biological reactions irreversible?

A

energy requirements and removal of products

68
Q

how do you increase rate of reaction?

A

increased temperature and concentration
decreased particle size
catalysts

69
Q

what are catalysts?

A

increase rate without being chemically changed/part of product

A&P I Lecture (8 decks)

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