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A&P 1 - Chap 1 - 4 (1st test) > Chapter 2 - Intro to Chemistry > Flashcards

Chapter 2 - Intro to Chemistry Flashcards

1
Q

Compound

A

substance composed of 2 or more elements in a fixed ratio

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2
Q

Mixture

A

substance composed of 2 or more components physically blended together; not a fixed ratio

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3
Q

Solution

A

homogeneous (evenly mixed) mixture of gases, liquids or solids

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4
Q

Solvent

A

dissolving medium, substance present in the greatest amount

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5
Q

Solute

A

substance that is dissolved, substance present in a smaller amount

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6
Q

Colloid or Emulsion

A

heterogeneous (unevenly mixed) mixture

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7
Q

Suspension

A

heterogeneous mixture, solutes tend to settle out and are visible

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8
Q

Organic compounds

A

CARBON-based compounds that are usually LARGE and COMPLEX

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9
Q

Inorganic compounds

A

compounds that usually LACK CARBON and are SIMPLE

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10
Q

Base

A

a substance that removes H+ ions from a solution

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11
Q

Acid

A

a substance that releases H+ ions into solution

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12
Q

Buffers

A

weak acids or bases that help minimize changes in pH

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13
Q

Dehydration synthesis

A

a synthesis reaction in which water is removed and a covalent bond is formed; results in something bigger

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14
Q

Hydrolysis

A

a decomposition reaction in which water is added and a covalent bond is broken

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15
Q

Exchange reaction

A

reactions in with both synthesis and decomposition occur

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16
Q

Catalyst

A

a substance that increases the rate of a chemical reactions

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17
Q

Enzyme

A

biological catalyst: a protein that speeds up chemical reactions

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18
Q

Isomers

A

substances with the same molecular formula but different arrangement of atoms (so slightly different properties)

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19
Q

Functional groups

A

groups of atoms that participate in chemical reactions; groups of organic compounds attached to carbon skeleton that allow it to participate in chemical reactions.

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20
Q

Metabolism

A

the sum of all the chemical reactions that take place in the body; all synthesis, decomposition & exchange reactions taking place in body

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21
Q

Atomic #

A

of protons in nucleus

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22
Q

Mass #

A

sum of its protons and neutrons

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23
Q

of Electrons

A

of protons

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24
Q

Major elements that make up over 96% of the human body:

A
  1. Oxygen - O
  2. Carbon - C
  3. Hydrogen - H
  4. Nitrogen - N
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25
Q

Lesser elements - Make up about 3.9% of the body:

A
  1. Calcium - Ca
  2. Phosphorous - P
  3. Sulfur - S
  4. Potassium - K
  5. Sodium - Na
  6. Chlorine - Cl
  7. Magnesium - Mg
  8. Iodine - I
  9. Iron - Fe
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26
Q

3 Chemical bonds:

A
  1. Ionic bonds - transfer of electrons
  2. Covalent bonds - can form molecules
  3. Hydrogen bonds - weak attraction that exists between polar molecules
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27
Q

2 Kinds of Molecules

A
  1. Polar molecule - electrons not shared equally; the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom.
  2. Nonpolar molecules - electrons are evenly distributed; one atom does not attract the shared electrons more strongly than the other atom
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28
Q

3 Kinds of Mixtures:

A
  1. Solution - homogeneous (evenly mixed); dissolves in solution completely; clear & transparent
  2. Colloid - particles are large enough to scatter light; cloudy, translucent or opaque; somewhere between liquid & solid
  3. Suspension - particles so large they fall out of the solution & sink to the bottom
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29
Q

Examples of Solution

A
  • Salt (solute) dissolved in water (solvent);
  • sugar dissolved in water;
  • air - mixture of forming gases - N, H2O, O
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30
Q

Examples of Colloid

A
  • Jello (dissolves in water, but cloudy, proteins scatter light;
  • cytosol - fluid inside cells (water, proteins - consistency of jello)
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31
Q

Biological example of Suspension

A

blood - blood settles when it sits, red blood cells sink to the bottom, & plasma floats on top & white blood cells & platelets are in the middle

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32
Q

Chemical Reactions

A

rearrangements of matter (mass); these rearrangements make new substances; matter is not destroyed or created, it’s just rearranged

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33
Q

Reactant

A

Starting material before reaction occurs

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34
Q

Product

A

what is formed as a result of chemical reaction

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35
Q

3 Kinds of Chemical Reactions

A
  1. Synthesis reactions - chemical bonds are formed, larger molecule results
  2. Decomposition reactions - chemical bonds are broken, small molecules or atoms result
  3. Exchange reaction - chemical bonds are formed & broken & something bigger & smaller results; both synthesis & decomposition occur
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36
Q

Example of Syntheses reactions

A

Amino acids (link many together) — Protein molecule (larger molecule)

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37
Q

Example of Decomposition reactions

A

Glycogen — Glucose molecules

38
Q

Example of Exchange reactions

A

Glucose + ATP — Glucose Phosphate + ADP:
Synthesis happens when Glucose forms into Glucose Phosphate;
Decomposition happens when ATP forms into ADP

39
Q

Most important Synthesis reaction taking place in body

A

Dehydration Synthesis - involves loss of water; removal of water causes a covalent bond–how we build large molecules in body

40
Q

Most important Decomposition reaction taking place in body

A

Hydrolysis - add water to break down things in the body; main way we break down things in body; digestive system

41
Q

Things to speed up chemical reactions:

A
  1. Temperature - if temp increases, atoms & molecules move faster
  2. Concentration - of reactants; add more particles–increase concentration; more likely to bump into each other
  3. Particle size - small particles move faster, large particles sluggish; decrease particle size
  4. Catalysts - introduce a catalyst to increase chemical reaction (i.e enzymes)
42
Q

Biological Catalyst

A

Enzymes - proteins (made inside our cells); specific–target 1 specific chemical reaction; can be reused; presence & absence of enzymes determine whether chemical reactions take place in the body

43
Q

Biochemistry

A

study of chemical reactions & chemical composition of living things

44
Q

Chemical composition of living things

A

chemicals in body reactive–combine with other elements in body to form compounds

45
Q

Examples of organic compounds

A

Mainly food molecules–proteins, carbs, lipids (fats), DNA (hold nucleic acids

46
Q

Examples of inorganic compounds

A

Water, salts, acids & bases

47
Q

Examples of organic compounds

A

Mainly food molecules–proteins, carbs, lipids (fats), DNA (hold nucleic acids) & ATP

48
Q

Examples of inorganic compounds

A

Water, salts, acids & bases

49
Q

Properties of Water (Inorganic compound):

A
  1. High heat capacity
  2. High heat of vaporization
  3. Universal solvent
  4. Reactant
  5. Cushioning
50
Q

High heat of vaporization (property of water)

A

takes a lot of heat to change water into gas; affects how our body is cooled down

51
Q

High heat capacity (property of water)

A

can hold a lot of heat without changing temp; body temp fairly constant

52
Q

Universal solvent (property of water)

A

dissolving medium; water dissolves a lot of substances in body bc most of molecules in body are polar: polar molecules dissolve other polar molecules; why chemical reactions take place in body

53
Q

Reactant (property of water)

A

water PARTICIPATES in chemical reactions

54
Q

Cushioning (property of water)

A

fluid that surrounds brain & spinal cord (CSF-cerebrospinal fluid)–mostly water

55
Q

O

A

selfish; holds electrons tightly; when electrons are shared, pulled more to O side–negatively charged

56
Q

H

A

partial positive;

57
Q

Hydrogen bonds

A

weak attractions between polar molecules such as water

58
Q

Salts (inorganic compound)

A

ionic compound when dissolved in water, doesn’t release H; are electrolytes

59
Q

Ionic bonds

A

electrons transferred from one atom to another which causes resulting atoms to be charged; always forms compounds

60
Q

electrolytes

A

substance that conducts electricity in water; release charged particles

61
Q

Na+

A

important for water balance; most abundant ion in body; water attracted to ions; the more sodium in body, the more water; too much Na+ = too much water in body

62
Q

Na+ and K+

A

important in generating electrical systems & running of nervous system; how we control our body

63
Q

Ca++

A

important for skeletal system; essential for muscle contractions; plays role in blood clotting

64
Q

Acid

A

always releases H+ ions; electrolytes

65
Q

Bases

A
  • usually releases OH- (hydroxyl ion) solution

- removes H+ ions that are already in the solution

66
Q

pH scale

A

way we measure amounts of H+ ions in solutions; can only be measured if dissolved in a liquid (H2O); scale that tell us if a solution is acidic or basic (alkaline)

67
Q

’s below pH7

A

acidic solution; H+ (more hydrogen ions)

68
Q

’s above pH7

A

basic solutions; H+ (less hydrogen ions)

69
Q

decrease pH

A

more acidic; more H+ in solution

70
Q

increase pH

A

more basic; fewer H+ in solution

71
Q

pH6

A

10x more H+ than pH7; one pH unit lower means 10x more H+ ions

72
Q

pH5

A

100x more H+ than pH7; one pH unit higher means 1/10 less H+ ions

73
Q

buffer

A

substances that keep pH fairly constant in body

74
Q

pH affects proteins & enzymes are proteins so it affects chemical reactions

A

k

75
Q

Blood buffer =

A

carbonic acid (weak acid)-bicarbinate buffer (weak base)

76
Q

when pH increases

A

carbonic acid brings it down–adds H+

77
Q

when pH decreases (too many H+)

A

bicarbinate removes H+

78
Q

pH7

A

neutral; concentration of H+ and OH- are equal (10 to the -7 mol/liter) = .0000001; (ex. pure water–distilled water)

79
Q

Carbon

A

has 4 unpaired electrons in its outermost valence shell; can form variety of bonds

80
Q

Carbon skeleton

A

framework; chain of carbons or ring of carbons that service framework for organic compounds

81
Q

Hydroxyl

A

OH

82
Q

Carbonyl

A

C=O

83
Q

Carboxyl

A

COOH

84
Q

Amino

A

NH2

85
Q

Sulfhydryl

A

SH

86
Q

Phosphate

A

PO4-2

87
Q

Hydrogen bond

A

forms when a hydrogen atom w/a partial positive charge attracts the partial negative charge of neighboring electronegative atom, most ofter larger oxygen or nitrogen atoms. Result from attraction of oppositely charged parts of molecules rather than from sharing of electrons (covalent bonds) or loss/gain of electrons (ionic bonds)

88
Q

Ionic bonds form

A

compounds

89
Q

Covalent bonds result in

A

molecules

90
Q

H2O

A

compound, molecule, polar molecule–slightly lopsided; electrons not shared equally

A&P 1 - Chap 1 - 4 (1st test) (7 decks)

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