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Anat/Phys1 > Chp. 2: Chemistry Comes Alive > Flashcards

Chp. 2: Chemistry Comes Alive Flashcards

Understanding the chemistry in the body

1
Q

Matter

A

anything that occupies space and has mass.
- all living and nonliving things contain matter

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2
Q

Mass

A

the actual amount of matter an object contains

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3
Q

Weight

A

measure of the force of gravity on a mass

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4
Q

Energy

A

the capacity to do work

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5
Q

Kinetic energy

A

energy of motion/ movement

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6
Q

Potential

A

Energy that has been stored

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7
Q

Forms of energy

A

chemical, mechanical, electrical, and radiant

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8
Q

Energy conversion is _______, with waste heat always _____.

A

inefficient; lost

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9
Q

Element

A

a substance that cannot be split into simpler substances by ordinary chem. reactions

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10
Q

How many elements are there?

A

112 to 118

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11
Q

How many elements occur in nature, and in the body?

A

A. 92
B. 24
- Carbon, Oxygen, Hydrogen, and nitrogen make up about 96% of body weight.

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12
Q

Atom is the ______ part of an elemental substance.

A

Smallest

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13
Q

Protons

A

+, in nucleus

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14
Q

Neutrons

A

neutral, in nucleus

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15
Q

Electrons

A

-, orbit nucleus in valence shell

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16
Q

What does it mean if protons, and electrons are equal?

A

Atom is electrically neutral.

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17
Q

Elements atomic #

A

A. its the # of protons
B. Large # on periodic table

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17
Q

What makes atoms differ from one another?

A

The # of protons in the nucleus

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18
Q

Isotope

A

A. Different atomic forms of the same element
B. Diff. # of neutrons
C. Same # of protons
D. Same chemical characteristics

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19
Q

Mass Number

A

the # of protons and neutrons

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20
Q

radioactive isotopes

A

unstable and decay into other isotopes, or other elements

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21
Q

atomic weight

A

avg. of mass # of all the isotopes

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22
Q

Molecule

A

particle of 2 or more atoms held together by a chemical bond

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23
Q

Compound

A

Substance composed of 2 or more different elements held together by chemical bonds

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24
mixture
substance composed of 2 or more components physically intermixed
25
Solutions
homogenous mixture of 2 or more components
26
Solvent
dissolving medium in which the other material are mixed in
27
Solute
Substance that is dissolved in a solution
28
Concentration
measure of the amount of solute dissolved in a solvent
29
Milligrams/ Deciliter
Mg/ Dl; measure of the blood concentration of glucose, cholesterol
30
molarity
Moles/ liter; element/ compound is = to its atomic weight or molecular weight measured in grams.
31
Colloids
heterogenous mixtures like jell-o; milky appearance; smaller particles scatter light; undergoes sol-gel transformation---> reversible change of a colloid from a fluid (sol) to a more solid (gel) state
32
Suspensions
Heterogenous mixture w/ large, visible solutes; blood -will settle out due to gravity
33
Chemical Bond
energy relationship holding atoms together, interaction of electrons
34
Role of Electrons
- they form clouds called shells - first 3 shells hold 2, 8, and 18 electrons, outer shell is the valence shell.
35
When are atoms considered stable?
Atoms are stable when the valence shell is full of electrons
36
Atoms are chemically reactive if what?
If the valence shell is not full of electrons
37
Covalent
A. sharing pairs of electrons B. May be polar (shared un=), or non-polar (= shared)
38
Nonpolar
A. type of covalent bond B. If electrons are shared =
39
Polar
A. type of covalent bond B. if electrons are shared un=
40
Ionic
Electrons sorted and are transferred from one atom to another; forming + and - ions - attraction btwn 2 oppositely charged ions
41
Cation
electron donors that have a positive charge (think cat and paws)
42
Anion
electron acceptors that have a negative charge
43
hydrogen
weakest attractions btwn different molecules which contain polar covalent bonds - covalently bound hydrogens attract other charged atoms
44
Water
forms many H-bonds; surface tension; important to waters properties that support life
45
Chemical reaction
Energy is transferred, waste heat is lost
46
Chem. equation
written in the form of the chemical reactions involved - A+B--> C
47
Synthesis
anabolic; atoms/ molecules combine to form larger, more complex molecules - always involves some type of chemical bond formation/ input of chemical energy - A+B--> AB ex: amino Acids to proteins
48
Decomposition
A. Catabolic B. Large molecule is broken down into smaller molecules - broken chemical bonds - chem. energy is released; may or may not be useful for another purpose
49
Chemical Exchange
A. Displacement B. bonds are both made and broken; atoms are combined w/ different atoms -AB+CD <---> AD+CB
50
Exergonic
A. releases energy (catabolic)
51
Endergonic
A. Absorbs energy (anabolic)
52
True or false: all chemical reactions are theoretically reversible?
TRUE!!! - more difficult when energy is released - energy MUST be added back to reverse the reaction
53
All chemical reactions tend toward a what state?
A. State of equilibrium
54
What 4 factors influence rate of reaction?
1. Temperature 2. Particle size 3. Concentration 4. Catalysts
55
Inorganic Compound
A. lack carbon B. smaller in size C. Various ions=electrolytes (salts, acids, bases)
56
High heat capacity
A. kinetic energy must be +/- to change the temp. of water by a degree B. contributes to body temp. stability
57
High heat of vaporization
A. change from liquid to a gas, breaks MANY hydrogen bonds B. energy used in boiling water
58
Polarity/ solvent properties
A. Polar covalent bonds, good solvent, brings solute molecules into close proximity; makes reactions more likely
59
Reactivity
A. participates in chemical reactions B. +/- from molec. in breakdown or synthesis reactions
60
Lubrication/ Cushioning
A. serous/ mucous fluid in many body locations lubricate the movement of various parts B. cerebrospinal fluid cushions the brain/ spinal chord C. Amniotic fluid cushions the fetus
61
Salts
A. Ionic compound contains cations other than [H+)/ [OH-] B. Dissociate (ionize) into component ions when dissolved in water C. Ions called electrolytes
62
Acids
A. release hydrogen ions when in solution B. proton donors C. dissociate to release hydrogen ions
63
Bases
A. proton acceptors B. generally dissociate in hydroxyl ions/ one or more cations
64
PH Scale
A. concentration of hydrogen ions is measure in pH units - ranges from 0-14
65
What is a neutral pH
7
66
What is an acidic pH
below pH 7
67
What is a basic pH
above pH 7
68
Acid-Base Balance
A. important for homeostasis, keep balanced in body fluid B. biochemical reactions very sensitive to pH
69
What are 3 homeostatic mechanisms to regulate acid base balance?
1. buffers 2. respiratory system 3. renal system
70
Buffers
minimize changes in ph by releasing/ binding hydrogen ions
71
Respiratory and renal
regulate buffer concentrations
72
bicarbonate system
helps maintain ph homeostasis of blood
73
neutralization
acid+base=salts
74
organic compounds
any compound composed of atoms held together by a covalent bond - proteins, lipids, carbs, nucleic acids - ALWAYS has C, H, and generally O - polar oc. dissolves in water, nonpolar doesn't - may be large, good structural components
75
Carbon
can form 4 covalent bonds
76
simple molecules
monomers are joined to form macromolecules - polymers
77
dehydration synthesis
large molc. in synthesis
78
hydrolysis
water is used to split a substance into smaller parts

Anat/Phys1 (2 decks)

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