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Anatomy & Physiology > Chemical Level of Organization > Flashcards

Chemical Level of Organization Flashcards

(90 cards)

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1
Q

Biochemistry

A

The field of chemistry that deals with living organisms and life processes

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2
Q

Matter

A

Anything that has mass and occupies space

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3
Q

Element

A

A simple form of matter, a substance that cannot be broken down into two or more different substances

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4
Q

How many elements are in the human body?

A

26 Elements

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5
Q

How many of the 26 elements in the human body are major?

A

11 Elements- Carbon Oxygen Hydrogen and Nitrogen

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6
Q

How many trace elements are in the body?

A

15 trace elements

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7
Q

Compound

A

An atom of two or more elements joined to form chemical combinations

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8
Q

Atomic Number

A

Number of Protons

Identifies Type of Element

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9
Q

Large letter/Large and small letter

A

Chemical Symbol

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10
Q

Atomic Mass Number

A

Number of protons plus average number of neutrons

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11
Q

Major Elements in the Cytoplasm

A

Oxygen
Hydrogen
Carbon

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12
Q

Minor Elements in the Cytoplasm

A

Iron
Manganese
Silicon

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13
Q

Atomic structure

A

Atoms contain several different kinds of subatomic particles

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14
Q

The concept of an atom was proposed by…….?

A

English Chemist John Dalton

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15
Q

Greek word atomos

A

Indivisible

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16
Q

Everything, whether liquid, gas, or solid, is made up of…….?

A

Atoms

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17
Q

Protons

A

The positively charged subatomic particles found in the nucleus

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18
Q

Neutrons

A

The neutral subatomic particles found in the nucleus

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19
Q

Electrons

A

The negatively charged subatomic particles found in the electron cloud formed around the nucleus

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20
Q

The total number of ……. in an atom equals the number of ………. in the nucleus in a stable atom

A

Electrons and Protons

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21
Q

Probability Distribution

A

The cloud model suggests that any one electron cannot be exactly located at a specific point at any particular time

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22
Q

The Octet Rule

A

States that atoms with fewer than or more than eight electrons in the outer energy levels will attempt to lose, gain, or share electrons with other atoms to achieve stability.

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23
Q

Bohr Model

A

Exhibits electrons in concentric circles, showing the relative distances of electrons from the nucleus
Number and arrangement of electrons determine whether an atom is chemically stable
An atom with eight electrons, or four pairs of electrons, in the outermost energy level is chemically stable

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24
Q

Hydrogen is……?

A

Reactive

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25
Isotopes
Have the same atomic number, and therefore have the same basic chemical propertied, as any other atom of the same element, but they have a different mass number.
26
Atomic Weight
The average mass number of isotopes typically found among atoms in nature.
27
Radioactive Isotope
An unstable isotope that undergoes nuclear breakdown and emits nuclear particles and radiation
28
H
Hydrogen
29
H^2
Deuterium
30
H^3
Tritium
31
Chemical bonds
Two types unite atoms into groupings, such as crystals and molecules
32
A Chemical Reaction
Is the interaction between two or more atoms that occurs as a result of activity between electrons in their outermost energy levels
33
Molecule
Is made up of two or more atoms covalently joined
34
A Compound
Consists of groupings of atoms of two or more elements
35
A Ionic Bond
Formed by the transfer of electrons; it is a strong electrostatic force that binds positively and negatively charged ions together
36
A Covalent Bond
Formed by sharing of electron pairs between atoms
37
Hydrogen Bonds
Result from unequal charge distribution on molecules Are much weaker than ionic or covalent bonds Areas of different partial charges attract one another and form
38
Polar Molecules
have regions with partial electrical charges that result from unequal sharing of electrons among atoms
39
Chemical Reactions
Involve the formation or breaking of chemical bonds
40
A Synthesis Reaction
Results from combining two or more substances to form a more complex substance A + B  AB
41
A Decomposition Reaction
Results from breaking down a substance into two or more simpler substances AB  A + B
42
An Exchange Reaction
The decomposition of two substances and, in exchange, synthesis of two new compounds from them AB + CD  AD + CB
43
Reversible Reactions
Occur in both directions
44
Metabolism
Describes all of the chemical reactions that occur in body cells
45
Catabolism
Chemical reactions that break down complex compounds into simpler ones and release energy Some of the energy released is transferred to adenosine triphosphate (ATP), Ultimately, the end products of catabolism are carbon dioxide, water, and other waste products ex. Hydrolysis
46
Anabolism
A chemical reaction that joins simple molecules to form more complex molecules Ex. dehydration synthesis (condensation)
47
ATP
molecules provide the energy needed to join monosaccharide units to form larger carbohydrates, fuse amino acids into peptide chains, and form fat molecules from glycerol and fatty acid subunits
48
Inorganic Compounds
Few have carbon atoms and none have C—C or C—H bonds
49
Organic Molecules
Have at least one carbon atom and at least one C—C or C—H bond in each molecule Often have functional groups attached to the carbon-containing core of the molecule
50
Polarity
Allows water to act as an effective solvent in the body | Ionizes substances in solution, allows transportation of essential materials throughout the body
51
High Specific Heat
Enables the body to maintain a relatively constant temperature, water can lose and gain large amounts of heat with little change in its own temperature
52
High Heat of Vaporization
Allows the body to dissipate excess heat, water requires the absorption of significant amounts of heat to change it from a liquid to a gas
53
The most abundant and most important compound in the body is.......?
Water, % of Body weight that is water is 70%.
54
Oxygen
Required to complete the decomposition reactions necessary for the release of energy in the body
55
Carbon Dioxide
Produced as a waste product and also helps maintain the appropriate acid-base balance in the body
56
Electrolytes
Substances that dissociate in solution to form ions; the resulting ions are also sometimes called electrolytes, are a large group of inorganic compounds that include acids, bases, and salts
57
Acids
Substances that release a hydrogen ion (H+) when in solution – proton donors, taste sour
58
Bases
Electrolytes that dissociate to yield hydroxide ions (OH–) or other electrolytes that combine with hydrogen ions (H+) Bases accept hydrogen ions Proton Acceptors
59
Cations
Positively charged ions
60
Anions
Negatively charged ions
61
pH 7
neutrality (equal amounts of H+ and OH–)
62
pH less than 7
Indicates acidity
63
A pH higher than 7
Indicates alkalinity
64
Hydrochloric Acid | pH 0
Acidic
65
Gastric Fluid | pH 1
Acidic
66
Lemon Juice | pH 2
Acidic
67
Vinegar | pH 3
Acidic
68
Wine | pH 3
Acidic
69
Beer | pH 4
Acidic
70
Coffee | pH 5
Acidic
71
Skin Film | pH 5
Acidic
72
Milk | pH 6
Acidic
73
Distilled Water | pH 7
Neutral
74
Blood pH 7
Neutral
75
Egg White | pH 8
Alkaline
76
Urine | pH 6
Acidic
77
Baking Soda | pH 8
Alkaline
78
Pancreatic Juice | pH 8
Alkaline
79
Borax pH 9
Alkaline
80
Great Salt Lake | pH 10
Alkaline
81
Milk of Magnesia | pH 10
Alkaline
82
Household Ammonia | pH 11
Alkaline
83
Oven Cleaner pH 13
Alkaline
84
Lye pH 13
Alkaline
85
Caustic Soda | pH 13
Alkaline
86
Sodium Hydroxide | pH 14
Alkaline
87
Tomatoes | pH 4
Acidic
88
Orange Juice | pH 3
Acidic
89
Buffers
Minimize changes in the concentrations of H+ and OH– ions | Act as a reservoir for hydrogen ions
90
Salts
Reaction between an acid and a base to form a salt and water is called a neutralization reaction

Anatomy & Physiology (5 decks)

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