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Anatomy & Physiology I > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Matter

A

Anything that has mass (weight) and occupies space. It can be seen, smelled, and/or felt.
Wt = mass x gravity
Earth g= 1.0

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2
Q

Energy

A

Not physical, cannot be confined to a space and doesn’t have mass. It is the capacity to do work or put matter into motion.

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3
Q

Where in an atom are protons and neutrons found?

A

The nucleus

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4
Q

Where in an atom are electrons found?

A

They orbit around the nucleus (orbitals/shells).

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5
Q

Kinetic Energy

A

The energy of motion/movement.

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6
Q

Potential Energy

A

The energy of position or stored (inactive) energy. Can be converted into kinetic energy.

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7
Q

Temperature

A

A measure of the amount of kinetic energy in a substance. How fast molecules are moving.

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8
Q

Solid

A

Molecules fixed in space, relative to each other. Definite shape and volume.

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9
Q

Fluid

A

Molecules are in motion relative to each other. Both liquid and gas are both fluid.

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10
Q

Liquid

A

Molecules are in motion but are transiently (temporarily) bound to each other.

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11
Q

Gas

A

A substance with molecules in motion, but they are not bound to each other.

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12
Q

Chemical Energy

A

A form of potential energy. Energy is stored in bonds of chemical substances. Lipids, fats, carbohydrates, atp.

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13
Q

Electrical energy

A

Movement of molecules that have positive or negative charges on them.

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14
Q

Laws of thermodynamics

A

1.) energy cannot be created or destroyed in normal chemical reactions
2.) energy can be converted, but some is lost as heat

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15
Q

Protons

A

Carry a positive charge (+)
Weighs 1 atomic mass unit (amu)

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16
Q

Mass of motion=

A

= 1 amu

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17
Q

Neutrons

A

Has no electrical charge, and weighs 1 amu.

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18
Q

Electrons

A

Carries a negative charge (-)
Has very little weight, but not zero

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19
Q

Electrically neutral atoms (the same)

A

The number of positive protons is balanced by the number of negative neutrons which makes atoms electrically neutral.

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20
Q

Atomic Number

A

The number of protons in the nucleus.

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21
Q

Mass number

A

The total number of protons and neutrons in the nucleus.
Protons + Neutrons = Mass number

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22
Q

Solutions (definition)

A

A solute is dissolved in a solvent to form a solution. Solutions are homogeneous mixtures.

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23
Q

Solute

A

The substance being dissolved Ex.: Sugar

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24
Q

Solvent

A

The substance doing the dissolving. Ex.: tea
Water is the universal solvent

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25
Q

Solution

A

Solute + Solvent = Solution
Ex.: Sweet tea
(Sugar/Solute + Tea/Solvent = Sweet Tea/solution)

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26
Q

Avogadro’s Number

A

6.02 x 10^23

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27
Q

Molarity (M)

A

The number of moles of solute per liter of solvent (water).

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28
Q

Chemical Bonds

A

“energy relationships” between electrons of reacting atoms. Electrons are the subatomic particles involved in all chemical reactions. Protons and neutrons are NOT involved in chemical bonds.

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29
Q

Electron Shell #1

A

Can only hold 2 electrons

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30
Q

Electron Shell #2

A

Shell 2 holds a maximum of 8 electrons

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31
Q

Electron Shell #3

A

Shell 3 holds a maximum of 8 electrons.

32
Q

Valence Shell

A

The outermost electron shell. The electrons in this shell are the ones involved in determining chemical bonding.

33
Q

What are electrons in the valence shell called?

A

Valence electrons

34
Q

Octet rule (rule of eights)

A

Most atoms desire 8 electrons in their valence shell. Exceptions are smaller atoms such as H and He. The desire to have 8 electrons is the driving force behind chemical reactions.

35
Q

Inert

A

Doesn’t have to interact with other elements because it is already stable. Example are the noble gases.

36
Q

Nobility

A

Noble elements that only interact with themselves.

37
Q

Electronegativity

A

The measure of how selfish and greedy an atom is for electrons (e-).

38
Q

Ionic Bond

A

Electrons are completely exchanged or transferred.

39
Q

Covalent Bonds

A

Sharing 2 or more valence shell electrons between 2 atoms.

40
Q

What are the 2 types of covalent bonds?

A

Polar and nonpolar covalent bonds

41
Q

Exergonic

A

Reactions release or give off energy.

42
Q

Endergonic

A

Reactions absorb or use up energy.

43
Q

Hemoglobin F

A

Has a higher affinity for oxygen. “Fetal hemoglobin” is found in fetuses only.

44
Q

Hemoglobin A

A

Found in adults. We start developing hemoglobin A as we grow.

45
Q

Adenine (A) Links with?

A

Thymine (T)

46
Q

Thymine (T) links with?

A

Adenine (A)

47
Q

Cytosine (C) links with?

A

Guanine (G)

48
Q

Guanine (G) links with?

A

Cytosine (C)

49
Q

Which nucleotide is only found in DNA?

A

Thymine (T)

50
Q

Which nucleotide is only found in RNA?

A

Uracil (U)

51
Q

What did Erwin Chargaff discover?

A

%A = %T and %C = %G

52
Q

What does DNA stand for?

A

Deoxyribonucleic acid

53
Q

What does RNA stand for?

A

Ribonucleic Acid

54
Q

What are nucleic acid polymers made up of?

A

Monomers called nucleotides

55
Q

What are nucleotides composed of?

A

A nitrogenous base, a pentose sugar (either ribose for RNA or deoxyribose for DNA), and a phosphate group.

56
Q

ALL proteins are made from how many different types of amino acids?

A

20 types of amino acids

57
Q

If something ends in -ase it is a…

A

Enzyme

58
Q

If something ends in -ose it is a…

A

Carbohydrate

59
Q

What is a pentose?

A

5 carbon sugar

60
Q

What is triose?

A

3 carbon sugar

61
Q

Blood pH of a normal, healthy person

A

7.4

62
Q

Blood pH range

A

7.35 ——- 7.4 ——- 7.45
(Acidic) (Normal) (Alkaline)

63
Q

What are the polymers of glucose?

A

Starch and glycogen.

64
Q

pH measures what?

A

Hydrogen (H^+)

65
Q

Which molecule is used by all animals as long-term storage?

A

Triglycerides

66
Q

Which molecule is used by all animals as medium-term storage?

A

Glycogen

67
Q

Which molecule is used by all animals as short-term storage?

A

Glucose

68
Q

What do catalysts do?

A

Catalysts increase the rate of reaction without being chemically changed or becoming apart of the product.

69
Q

What is an example of a biological catalyst?

A

Enzymes

70
Q

What is an acid?

A

A substance that will donate a H+ (hydrogen ion) when placed in an aqueous solution.

71
Q

What is a base?

A

A substance that will take up a H+ (hydrogen ion) when placed in an aqueous solution.

72
Q

What are buffers?

A

They resist abrupt and large swings in pH.

73
Q

When pH rises (alkaline), what do buffers release?

A

They can release H+ (hydrogen ions)

74
Q

When pH falls (acidic), what do buffers do?

A

They can bind H+ (hydrogen ions)

75
Q

What is the difference between ionic bonds and covalent bonds?

A

Ionic bonds completely transfer electrons. Covalent bonds share electrons, either equally (non-polar) or unequally (polar).

76
Q

What do negative catalysts do?

A

They can slow down a reaction without being consumed or becoming apart of the product.

Anatomy & Physiology I (15 decks)

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