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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
Anion
* negative ion | * gains electrons
26
Cation
* loses electrons | * positive charge
27
Ionization
•electrons transferring between atoms
28
Electrolytes
* substances that ionize in water & form solutions able to conduct electricity * acids, bases, salts
29
Free radicals
* 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)
30
Antioxidant
•chemical that neutralizes free radicals
31
Molecules
* chemical particles made of 2+ atoms (United by chemical bonds) * atoms can be identical or different
32
Compounds
•molecules made of 2+ elements
33
Isomers
•molecules w/identical molecular formulae but different arrangement of atoms
34
Molecular weight (MW)
(for compounds at least) | •sum of atomic weights & atoms
35
Chemical bonds
•holds molecules together
36
Ionic bond
* attraction between anion & cation * weak bonds * easily disrupted in water (like salt, it dissolves)
37
Covalent bonds
* 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
Hydrogen bond
•weak attraction between slightly positive hydrogen atom & slightly negative oxygen or nitrogen atom
39
Van set Waals forces
* important in protein folding (binding of proteins together & to molecules) * weak * brief attractions between neutral atoms
40
Why is the biological half-life of a radioisotope shorter than physical half-life?
* biological is leaving the body through excretion & decay * physical is just decay
41
How is the body protected from free radicals?
•antioxidants are produced to neutralize them
42
What’s the difference between ionic & covalent bond?
* covalent shares electrons | * ionic attracts elements based on opposite charge
43
Mixture
•physically blended substances but NOT chemically combined
44
Hydrophilic
•substances that dissolve in water Ex: sugar
45
Hydrophobic
•substances that don’t dissolve in water Ex: fats
46
Calorie
•bass unit of heat
47
Adhesion
•1 substance to clinging to another
48
Cohesion
•molecules of same substance clinging
49
Chemical reactivity
•ability to participate in chemical reactions
50
Solution
•solute mixed w/solvent
51
Solute
•particles of matter
52
Solvent
•abundant substance (usually water)
53
Colloids
* 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
Suspension
* particles exceed 100 nm * cloudy or opaque * can’t penetrated selectively permeable membranes * too heavy to remain suspended, mixture separates
55
Emulsion
•suspension of 1 liquid in another Ex: •oil & vinegar •day in breast milk
56
Acid
•proton donor (molecule that releases protons in water)
57
Base
•proton acceptor
58
pH
* term to express acidity | * measure from molarity if H^+
59
Neutral pH
7.0
60
Acidic pH
•below 7.0
61
Basic (alkaline) pH
•above 7.0
62
Buffers
•chemical solutions that resist changes in pH
63
What are 4 ways to express concentration?
* weight per volume * percentage * molarity * milliequivalents per liter
64
Weight per volume
•solute weight (g/grams/mg/milligrams) in given volume of solution (liters/L/deciliter/dL) Ex: 200 mg/dL
65
Percentage
•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
Molarity
* 1 mole of chemical = number of grams equal to molecular weight * measure of number of moles of solute per liter of solution
67
Milliequivalents per liter
* mEq/L | * expresses electrolyte concentrations
68
Energy
•capacity to do work
69
Work
•to move something (muscle or molecule)
70
Free energy
•potential energy available to do useful work
71
Chemical reaction
•process where covalent or iconic bond is formed or broken
72
Chemical equation
* course of chemical reaction * reactants on left * arrow from left pointing to right (reactants to products) * products on right
73
Decomposition reactions
•large molecule breaks into 2(+) smaller molecules Ex: AB > A + B
74
Synthesis reactions
•2(+) small molecules combining to form large one Ex: A + B > AB
75
Exchange reactions
•2 molecules exchange atoms/groups of atoms Ex: AB + CD > AC + BD
76
Reversible reactions
•go either direction depending on circumstances Ex: CO2 + H2O > H2CO3 > HCO3 + H
77
Law of mass action
•reversible reactions process from reactants w/greater quantity to substances w/less quantity
78
Equilibrium
•stable
79
Concentration
•reaction rate increases when reactants are concentrated | molecules are crowded & collide more
80
Temperature
•reaction rate increases as temp rises | heat causes molecules to live faster & collide w/greater force & frequency
81
Catalysts
* 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
Metabolism
* every chemical resection in body | * catabolism & anabolism
83
Catabolism
•energy-releasing decomposition reactions * break covalent bonds * produces smaller molecules from bigger molecules * release energy for other physiological work
84
Exergonic reactions
•energy-releasing reactions
85
Anabolism
•energy-storing synesthesia reactions Ex: •production of protein or fat
86
Endergonic reactions
•reactions that require energy input
87
Oxidation
•any chemical reaction where molecule gives up electron & releases energy
88
Reduction
•chemical reaction where molecule gains electrons & energy

A&P (11 decks)

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