Test #1 Flashcards

1
Q

Define matter (& three types):

A

Anything that has mass and takes up space; all matter is composed of elements and all elements are composed of atoms
1) Solid (definite shape & volume)
2) Liquid (indefinite shape, definite volume
3) Gas (indefinite shape & volume)

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2
Q

Define atomic number:

A

The number of protons an atom has (equal to the number of electrons); written as subscript to the left: “3Li”

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3
Q

Define atomic mass:

A

Protons & neutrons combined; written as superscript to the left: “7Li”

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4
Q

Define isotope:

A

An element that has a different number of neutrons than the same base element

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5
Q

Define molecule:

A

General terms for two or more atoms chemically bonded together (H2)

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6
Q

Define compound:

A

A specific molecule that has two or more different kinds of atoms bonded together (e.g., H2 doesn’t count, C6H12O6 does)

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7
Q

Define mixture (& 3 types):

A

Matter that is intermixed are not chemically bonded
1) solution (air; doesn’t scatter light, doesn’t settle)
2) colloid (jell-o; scatters light, doesn’t settle)
3) suspension (blood; scatters light, settles)

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8
Q

Define ion:

A

An atom that has lost or gained an electron (electron no longer matches the protons)

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9
Q

Define anion:

A

Negatively charge ion (has gained an electron)

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10
Q

Define cation:

A

Positively charged ion (has lost an electron)

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11
Q

Define pH:

A

The measurement of H+ ions; more H+ the more acidic; logarithmic

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12
Q

Define neutralization reaction:

A

When a base neutralizes an acid; salt is the result; this is an exchange/displacement chemical reaction

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13
Q

Define buffer:

A

Something that prevents swings in pH; converts strong acids or bases to weak ones; releases H+ if pH rises, binds H+ if pH falls

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14
Q

Cell drawing

A

1) membrane
2) nucleus
3) cytoplasm
a) organelles (little organs)
b) cytosol (the fluid that holds everything together)
c) inclusions (e.g., melanin)
4)Electrochemical gradient (- - - inside. +++ outside)
a) inside K+, AA- -, PO4 -2
b) outside Na+, Cl-

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15
Q

Structural organization of the body

A

1) chemicals, 2) cells, 3) tissue, 4) organs, 5) organ systems, 6) organism

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16
Q

Requirements for life/necessary life functions

A

1) maintaining boundaries
2) movement - skeletal muscle (s.n.s), cardiac muscle, smooth muscle (a.n.s.)
3) responsiveness
4) digestion
5) metabolism - sums up all chemical reactions (catabolism - breaking down molecules; anabolism - synthesis of molecules)
6) excretion
7) reproduction
8) growth

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17
Q

Five survival needs

A

1) nutrients
2) oxygen
3) water
4) normal body temp
5) appropriate atmospheric pressure

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18
Q

Homeostasis

A

Maintaining a relatively stable internal environment despite a changing external environment

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19
Q

Homeostatic control diagram

A

1) stimulus (change in variable), 2) receptor (detects the change), 3) input, 4) output, 5) response

1) receptor, control center, effector

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20
Q

Effector organs

A

1) skeletal muscle (s.n.s), 2) cardiac muscle, 3) smooth muscle, glands (a.n.s.)

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21
Q

Anatomical position

A

Feet slightly apart, erect spine, hands at side with thumbs pointing away from body

22
Q

Regions of the body

A

Posterior:

23
Q

Regions of the body

A

Anterior:

24
Q

Directional words

A

Superior/cranal vs inferior/caudal, anterior/ventral vs posterior/dorsal, medial vs lateral vs intermediate, proximal vs distal, superficial vs deep

25
Q

Planes

A

Sagittal (L/R), frontal/coronal (F/B), transverse/horizontal (superior/inferior), oblique (non 90 degree)

26
Q

Two main body cavities

A

Dorsal (cranial, spinal/vertebral), ventral (thoracic [pleural, pericardial], abdominopelvic [abdominal, pelvic])

27
Q

Membranes

A

1) mucous (opens to external), 2) cutaneous (skin), serous (ventral cavity): visceral/parietal pleural, visceral/parietal pericardial, visceral/parietal peritoneum, falciform ligament, omentum, mesentry

28
Q

Four abdomial reigons

A

ULQ, URQ, LLQ, LRQ (appendix)

29
Q

Nine abdomen reigons

A

R. hypochondriac, epigastric, L. hypochondriac
R. lumbar, umbilical, L. lumbar
R. illiac, hypogastric, L. illiac

30
Q

Organ systems

A

1) integumentary (vit. D synth), 2) skeletal (stores calcium/other minerals, produces blood cells), 3) muscular (creates heat), 4) digestive, 5) urinary/renal, 6) cardiovascular, 7) respiratory, 8) endocrine, 9) lymphatic (immunity, picks up fluid), 10) reproductive, 11) nervous (fast-acting)

31
Q

Four major elements

A

ONCH - oxygen, nitrogen, carbon, hydrogen; make up 96% of body

32
Q

Atom & subdivision characteristics

A

Nucleus - protons (+; 1amu) & neutrons (~; 1 amu; Shell - electrons (-; 0 amu)

33
Q

Define energy

A

The capability to do work

34
Q

Types & forms of energy

A

Types: 1) kinetic (energy in action), 2) potential (inactive/stored)
Forms: 1) chemical, 2) electrical, 3) mechanical, 4) radiant/electromagnetic

35
Q

Chemical bonds (& three types)

A

Energy relationships between electrons

1) ionic (give/take electrons; e.g., acids, bases, salts)
2) covalent (sharing electrons; strongest)
2a) share equally = non-polar/electrically balanced (DOES NOT dissolve in water)
2b) share unequally = polar/electrically imbalanced (dissolves in water)
3) hydrogen (weakest; e.g., water strider walking on water because of the high surface tension of water)

36
Q

Significance of electrons

A

Involved in all chemical reactions

37
Q

Octet rule

A

Atoms want a complete valence shell (eight electrons; inert valence vs reactive valence)

38
Q

Chemical reactions (& three types)

A

When chemical bonds are made, broken, or rearranged

1) synthesis (anabolic reaction, endergonic [absorption of energy], dehydration synthesis; products have MORE potential energy than reactants)
2) decomposition (catabolic & oxidative reactions, exergonic [release of energy], hydrolysis; products have LESS potential energy than reactants)
3) exchange/displacement

39
Q

Speed of reactions (three things)

A

1) the size of the particle (smaller particles increase rate)
2) temperature (higher temp usually increases rate of reaction)
3) concentration of reactants (increased concentration increases rate of reaction)

40
Q

Organic/inorganic compounds?

A

Anything with C is organic (exception: CO and CO2)

41
Q

Four main organic compounds, what are they composed of?

A

Carbs, proteins, lipids, nucleic acids

Polymers & monomers - broken down by hydrolysis, built by dehydration synthesis

Polymer/monomer examples - glycogen (polysaccharide in animals) breaks down to glucose; starch (polysaccharide in plants) breaks down to glucose; protein breaks down to amino acids

42
Q

Properties of water

A

60-80% of all living cells (most abundant)

1) High heat capacity - ability to absorb and release heat with little temperature change; prevents sudden temperature changes
2) High heat vaporization - evaporation requires large amounts of heat; useful as a cooling mechanism
3) Polar solvent properties - dissolves and dissociates ionic substances (but not the ions themselves); body’s major transport medium
4) Reactivity - necessary part of hydrolysis and dehydration synthesis reactions
5) Cushioning

43
Q

Electrolytes

A

Conduct electricity in water (e.g., acid, base, salt)

44
Q

Effector organ response

A

Negative feedback (decreases the stimulus), positive feedback (increases the stimulus (only found in labor contractions, suckling, blood clotting)

45
Q

ATP

A

Adenosine triphosphate - main energy currency of the body; energy from broken down glucose stored here; three phosphate bonds can be hydrolyzed for energy (ATP -> ADP -> AMP)

46
Q

Four main organic compounds: carbohydrates

A

Saccharides

Monosaccharides (hexagonal/pentagonal)
Hexose
1) glucose
2) fructose (pentose)
3) galactose
Pentose
4) ribose
5) deoxyribose

Disaccharides (dual monosaccharides)
GF (glucose, fructose) - sucrose
GG - (glucose, galactose) - lactose
GG (glucose, glucose) - maltose

Polysaccharides (chain shape)
E.g., glycogen, starch, etc.

47
Q

Four main organic compounds: proteins

A

Polymers of amino acid monomers held together by covalent bonds called peptide bonds, can act as acid or base, 20-30% cell mass, most varied functions of any molecules (1. structural [e.g. collagen - most abundant protein in body], 2. enzyme, 3. transport [e.g., hemoglobin, transports oxygen in blood], 4. contractile, 5. communication, 6. defense), fibrous (strand-like, water insoluble and stable) vs globular (compact, spherical, water soluble, sensitive to environmental changes [denaturation - unfold from 3D, active sites become inactive])

Structure levels
1) primary - sequence of amino acids form the polypeptide chain
2) secondary - primary chains form a-helices or b-sheets
3) tertiary - helices or chains fold into compact globular molecules
4) quaternary - two or more polypeptide chains, each with its own tertiary structure, combine to form functional proteins

48
Q

Four main organic compounds: lipids (& four types)

A

Insoluble in water

1) triglycerides - main function to store energy; three fatty acids to one glycerol; saturated has no double bond, unsaturated has double bond and a kink
2) phospholipids - one glycerol and two fatty acids, one w/double bond and kink, plus a phosphorus containing head (head is hydrophilic, tail is hydrophobic)
3) steroids - most important is cholesterol, made in the liver; shape of four interlocking rings
4) eicosanoids - e.g., prostaglandins (blood clotting, blood pressure, inflammation, labor contractions)

49
Q

Four main organic compounds: nucleic acids (& three types of RNA)

A

Made up of the monomer nucleotide joined at the phosphate bases, RNA (single strand, ribose carb, A-U pair, caries out order for protein synthesis), DNA (double stranded, deoxyribose carb, A-T pair, hydrogen bonds occur between nitrogenous bases)

Types of RNA
1) messenger
2) transfer
3) ribosomal

50
Q

Chemical bonding essay question

A

Energy relationships between electrons (electrons involved in all chemical reactions)

1) Ionic bonding - give/take electrons, i.e. salts, acids, bases; atoms that give up electron become +ve cations, atoms that give up electron become -ve anions; cations and anions may bind together in ionic bonds

2) Covalent bonding - can happen when both atoms need electrons; allows each atom to fill its valence shell at least part of the time; single/double/triple covalent bonds (2/4/6 electrons shared); may share equally or unequally as determined by electronegativity (if EN is same then they share equally/if different they share unequally) - equal is non-polar: does not dissolve in water, electrically balanced; unequal is polar, dissolves in water, electrically imbalanced
C=0=C (CO2; carbon dioxide is non-polar)
0 (-)/H(+)\H(+) (H20; water is polar and dipole)

3) Hydrogen - individually weak, collectively strong; combine to support the structure of complex molecules (DNA, proteins, etc.) but does don’t bind atoms into molecules; forms between polar molecules; common between dipoles; influences how water molecules behave

51
Q

Define energy conversion

A

Energy results in lost energy, in the form of heat, which is unusable.

52
Q

Define catalyst

A

Catalysts increase rate of reaction without becoming part of the product; e.g., enzymes are biological catalysts (lowers the activation energy needed to start a reaction)