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A&P > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Biochemistry

A

•study of molecules that make up living organisms

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2
Q

What are the elements of the human body?

A
  1. Oxygen (O)
  2. Carbon (C)
  3. Hydrogen (H)
  4. Nitrogen (N)
  5. Calcium (Ca)
  6. Phosphorus (P)
  7. Sulfur (S)
  8. Potassium (K)
  9. Sodium (Na)
  10. Chlorine (Cl)
  11. Magnesium (Mg)
  12. Iron (Fe)
  13. Chromium (Cr)
  14. Cobalt (Co)
  15. Copper (Cu)
  16. Fluorine (F)
  17. Iodine (I)
  18. Manganese (Mn)
  19. Molybdenum (Mo)
  20. Selenium (Se)
  21. Silicon (Si)
  22. Tin (Sn)
  23. Vanadium (V)
  24. Zinc (Zn)
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3
Q

What’s the difference between elements & compounds?

A

Elements:
•singular chemical properties

Compounds:
•combinations of 2+ elements

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4
Q

What are the functions of minerals in the body?

A
  • 4% of body weight
  • contribute to teeth & bones (make them stronger)
  • enable enzymes
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5
Q

How many types of chemical bonds are there? What are they?

A

•4

  • ionic
  • covalent
  • hydrogen
  • van set Waals
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6
Q

What are the hazards of ionizing radiation?

A
  • produces free radicals & ions in human tissues
  • possibly fatal or cause mutations
  • possibly carcinogenic (cause cancer)
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7
Q

Elements

A

•simplest form of matter w/unique chemical properties

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8
Q

Trace elements

A

•12 elements in body (none of them account for more than .02% of body weight)

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9
Q

Minerals

A

•inorganic elements extracted from soil by plants & passed up the food chain (to humans & other organisms)

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10
Q

Atoms

A
  • particles so small they can’t be cut

* imaginary particles

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11
Q

Protons

A
  • single positive charge

* center of atom/makes up nucleus w/neutrons

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12
Q

Neutrons

A
  • no charge

* center of atom/makes up nucleus w/protons

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13
Q

What is in the nucleus of an atom? What orbits the nucleus?

A
  • protons
  • neutrons

•electrons

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14
Q

Electrons

A
  • single negative charge
  • orbit/swarm nucleus
  • low mass (1,836 electrons = 1 proton)
  • determine atom’s chemical property
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15
Q

What do electrons & protons do to each other?

A
  • equal number of each

* cancel each other out making atoms electrically neutral

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16
Q

Valence electrons

A
  • outermost shell

* determine chemical bonding properties of atoms

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17
Q

What’s an electron shell?

A
  • energy level of an atom
  • concentric regions
  • more energy of an electron the farther it is from nucleus
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18
Q

Isotopes

A
  • varieties of elements

* differ only in number of neutrons & change atomic mass (no change in protons/electrons, that changes element)

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19
Q

Ionizing radiation

A
  • high energy radiation
  • ejects electrons from atoms (converting atoms to ions)
  • destroys molecules
  • produces free radicals & ions in human tissues
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20
Q

Radioisotopes

A

•unstable isotopes

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21
Q

Radioactivity

A

•process of decaying elements to reach stable levels

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22
Q

Physics half-life

A
  • characteristic of radioisotope
  • time required for 50% of atoms to decay to stable state
Ex:
•1 gram of 90^Sr would be...
     •1/2 gone in 28 years
     •.25 grams in 56 years 
     •.125 grams in 84 years
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23
Q

Biological half-life

A

•time required for 1/2 of radioisotope to disappear from body
(lost by radioactivity & excretion)

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24
Q

Ions

A

•charged particles w/unequal number of protons & electrons

can be…
•single atom w/positive or negative charge
•group of atoms
•molecule w/many charges

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25
Q

Anion

A
  • negative ion

* gains electrons

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26
Q

Cation

A
  • loses electrons

* positive charge

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27
Q

Ionization

A

•electrons transferring between atoms

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28
Q

Electrolytes

A
  • substances that ionize in water & form solutions able to conduct electricity
  • acids, bases, salts
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29
Q

Free radicals

A
  • chemical particles w/odd number of electrons
  • common
  • destructive
  • represented w/dot (symbolizes odd electron)

Ex:
•oxygen’s normally stable (2 oxygen atoms)
•add 1 electron & it forms superoxide anion (a free radical)

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30
Q

Antioxidant

A

•chemical that neutralizes free radicals

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31
Q

Molecules

A
  • chemical particles made of 2+ atoms (United by chemical bonds)
  • atoms can be identical or different
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32
Q

Compounds

A

•molecules made of 2+ elements

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33
Q

Isomers

A

•molecules w/identical molecular formulae but different arrangement of atoms

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34
Q

Molecular weight (MW)

A

(for compounds at least)

•sum of atomic weights & atoms

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35
Q

Chemical bonds

A

•holds molecules together

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36
Q

Ionic bond

A
  • attraction between anion & cation
  • weak bonds
  • easily disrupted in water (like salt, it dissolves)
37
Q

Covalent bonds

A
  • sharing electrons
  • single-share 1 pair of electrons
  • double-share 2 pairs of electrons
  • nonpolar-electrons equal time near each nucleus; strongest of chemical bonds
  • polar-electrons at 1 nucleus more than another (giving negative charge to nucleus they’re with the most)
38
Q

Hydrogen bond

A

•weak attraction between slightly positive hydrogen atom & slightly negative oxygen or nitrogen atom

39
Q

Van set Waals forces

A
  • important in protein folding (binding of proteins together & to molecules)
  • weak
  • brief attractions between neutral atoms
40
Q

Why is the biological half-life of a radioisotope shorter than physical half-life?

A
  • biological is leaving the body through excretion & decay
  • physical is just decay
41
Q

How is the body protected from free radicals?

A

•antioxidants are produced to neutralize them

42
Q

What’s the difference between ionic & covalent bond?

A
  • covalent shares electrons

* ionic attracts elements based on opposite charge

43
Q

Mixture

A

•physically blended substances but NOT chemically combined

44
Q

Hydrophilic

A

•substances that dissolve in water

Ex: sugar

45
Q

Hydrophobic

A

•substances that don’t dissolve in water

Ex: fats

46
Q

Calorie

A

•bass unit of heat

47
Q

Adhesion

A

•1 substance to clinging to another

48
Q

Cohesion

A

•molecules of same substance clinging

49
Q

Chemical reactivity

A

•ability to participate in chemical reactions

50
Q

Solution

A

•solute mixed w/solvent

51
Q

Solute

A

•particles of matter

52
Q

Solvent

A

•abundant substance (usually water)

53
Q

Colloids

A
  • particles range 1-100 nm
  • usually cloudy
  • can’t pass through (most) selectively permeable membranes
  • small enough to remain mixed
  • most common (in body) mixtures of protein & water
  • many can change: liquid to gel
54
Q

Suspension

A
  • particles exceed 100 nm
  • cloudy or opaque
  • can’t penetrated selectively permeable membranes
  • too heavy to remain suspended, mixture separates
55
Q

Emulsion

A

•suspension of 1 liquid in another

Ex:
•oil & vinegar
•day in breast milk

56
Q

Acid

A

•proton donor (molecule that releases protons in water)

57
Q

Base

A

•proton acceptor

58
Q

pH

A
  • term to express acidity

* measure from molarity if H^+

59
Q

Neutral pH

A

7.0

60
Q

Acidic pH

A

•below 7.0

61
Q

Basic (alkaline) pH

A

•above 7.0

62
Q

Buffers

A

•chemical solutions that resist changes in pH

63
Q

What are 4 ways to express concentration?

A
  • weight per volume
  • percentage
  • molarity
  • milliequivalents per liter
64
Q

Weight per volume

A

•solute weight (g/grams/mg/milligrams) in given volume of solution (liters/L/deciliter/dL)

Ex: 200 mg/dL

65
Q

Percentage

A

•solute weight as percentage of solution volume (weight per volume, w/v) or volume of liquid as percentage of total solution volume (volume per volume, v/v)

66
Q

Molarity

A
  • 1 mole of chemical = number of grams equal to molecular weight
  • measure of number of moles of solute per liter of solution
67
Q

Milliequivalents per liter

A
  • mEq/L

* expresses electrolyte concentrations

68
Q

Energy

A

•capacity to do work

69
Q

Work

A

•to move something (muscle or molecule)

70
Q

Free energy

A

•potential energy available to do useful work

71
Q

Chemical reaction

A

•process where covalent or iconic bond is formed or broken

72
Q

Chemical equation

A
  • course of chemical reaction
  • reactants on left
  • arrow from left pointing to right (reactants to products)
  • products on right
73
Q

Decomposition reactions

A

•large molecule breaks into 2(+) smaller molecules

Ex:
AB > A + B

74
Q

Synthesis reactions

A

•2(+) small molecules combining to form large one

Ex:
A + B > AB

75
Q

Exchange reactions

A

•2 molecules exchange atoms/groups of atoms

Ex:
AB + CD > AC + BD

76
Q

Reversible reactions

A

•go either direction depending on circumstances

Ex:
CO2 + H2O > H2CO3 > HCO3 + H

77
Q

Law of mass action

A

•reversible reactions process from reactants w/greater quantity to substances w/less quantity

78
Q

Equilibrium

A

•stable

79
Q

Concentration

A

•reaction rate increases when reactants are concentrated

molecules are crowded & collide more

80
Q

Temperature

A

•reaction rate increases as temp rises

heat causes molecules to live faster & collide w/greater force & frequency

81
Q

Catalysts

A
  • substances temporarily bind to reactants, hold in good position, may change shape of reactant to make it more likely to react
  • speeds up reaction
82
Q

Metabolism

A
  • every chemical resection in body

* catabolism & anabolism

83
Q

Catabolism

A

•energy-releasing decomposition reactions

  • break covalent bonds
  • produces smaller molecules from bigger molecules
  • release energy for other physiological work
84
Q

Exergonic reactions

A

•energy-releasing reactions

85
Q

Anabolism

A

•energy-storing synesthesia reactions

Ex:
•production of protein or fat

86
Q

Endergonic reactions

A

•reactions that require energy input

87
Q

Oxidation

A

•any chemical reaction where molecule gives up electron & releases energy

88
Q

Reduction

A

•chemical reaction where molecule gains electrons & energy

A&P (11 decks)

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