Chapter 2 - Chemical Basis of Life Flashcards
1
Q
Physiological processes are based on?
A
Chemistry
2
Q
Anatomical structures are composed of?
A
Chemicals
3
Q
Anything that has weight and takes up space
A
matter
4
Q
All matter is composed of fundamental substances called?
A
elements
5
Q
How many known elements are there?
A
118 as of 2011
6
Q
How many elements occur naturally?
A
92
7
Q
Chemical combinations of elements
A
compounds
8
Q
Elements required by the body in large amounts
A
bulk elements
9
Q
Examples of bulk elements
A
nitrogen, carbon, oxygen, hydrogen, and phosphorous
10
Q
Elements required only in small amounts
A
trace elements
11
Q
Elements required in extremely small amounts and may be toxic in larger quantities
A
ultratrace elements
12
Q
Trace elements are important parts of what?
A
enzymes
13
Q
Example of an ultratrace element
A
arsenic
14
Q
Smallest units of an element which have the chemical properties of that element
A
atoms
15
Q
How can atoms be chemically different from each other in each element?
A
weight, size, and ways they interact with each other
16
Q
Central portion of an atom
A
nucleus
17
Q
Particles that constantly move around the nucleus
A
electrons
18
Q
Nucleus contains?
A
neutrons and protons (roughly the same weight)
19
Q
List the charges for protons, neutrons, and electrons
A
P = positive N = no charge E = negative
20
Q
What is the cause for an atom to be electrically neutral?
A
Nucleus is always positive charged (protons) and the electrons are always negatively charged. This results in the atom have a net charge of zero.
21
Q
Number of protons an atom has is called its what?
A
atomic number
22
Q
What is the atomic weight equal to?
A
number of protons plus neutrons in the nucleus
23
Q
Atoms that have the same atomic numbers but different atomic weights
A
isotopes
24
Q
Unstable isotopes are?
A
radioactive
25
Energy or atomic fragments that unstable isotopes emit
atomic radiation
26
3 common forms of atomic radiation
* alpha
* beta
* gamma (similar to x-radiation)
27
Two or more atoms may combine to form this distinctive kind of particle
molecule
28
Shows the numbers and kinds of atoms in a molecule
molecular formula
29
When atoms of different elements combine, they form these molecules of substances.
compounds
30
Bonds formed between atoms involve what?
electrons
31
Regions of space around the nucleus where electrons are found.
electron shells (aka energy shells)
32
First electron shell can hold a maximum of X electrons
2
33
Second electron shell can hold a maximum of X electrons
8
34
Third electron shell can hold a maximum of X electrons
8, though some complex atoms may have as many as 18 in this shell
35
What determines whether or not an atom will react with another atom?
The number of electrons in the outer shell. Atoms react in such a way that the outer shell will be completely filled with electrons. (octet rule)
36
Atoms that have filled outer shells are said to be?
non-reactive or inert
37
Examples of inert atoms
He, Ne, Ar, Kr, Xe, Rn
38
Atoms that gain or lose electrons become electrically charged and are called?
ions
39
Positively charged ions
cations
40
Negatively charged ions
anions
41
Bond where electrons are given/received (not shared)
ionic bond (electrovalent)
42
Bond where electrons are shared (not taken/received)
covalent bond
43
Covalent bond where electrons are not shared equally
polar covalent bond
44
This occurs when an H atom shares its single electron with 2 other atoms
hydrogen bond
45
This bond is depicted by a single line - one pair of shared electrons
single covalent bond
46
This bond is depicted by two lines - two pairs of shared electrons
double covalent bond
47
This bond is depicted by three lines - three pairs of shared electrons
triple covalent bond
48
Breaks bonds or forms bonds between atoms, ions, or molecules
chemical reaction
49
Those changed by the chemical reaction are called?
reactants
50
Those formed at the reaction's conclusion are called?
products
51
Reaction where two or more reactants bond to form a more complex structure
synthesis reaction
52
Reaction where the bonds of a reactant molecule are broken to yield simpler structures
decomposition reaction
53
Reaction where parts of two different kinds of molecules trade places
exchange reaction
54
True or false: many reactions are reversible
true; the direction of the reaction depends on the relative proportions of reactant and product as well as the amount of energy available
55
Molecules that influence the rate of a reaction but not the direction
catalysts
56
The polar nature of water causes what?
ionically bound salts to dissociated from one another forming ions
57
Substances that release ions
electrolytes
58
Electrolytes that release hydrogen in water
acids
59
Electrolytes that release irons that react with H ions in water
bases
60
Acid and bases can react to form water and electrolytes called?
salts
61
Hydrogen ion concentration can be measured in grams of ions per liter of solution. What system was developed to keep track of this?
pH scale
62
pH of 1 has an H+ concentration of?
0.1 gm/liter
63
pH of 2 has an H+ concentration of?
0.01 gm/liter
64
Equal of number of H+ and OH- when water ionizes causes the solution to be called?
Neutral
65
Solutions w/ more H+ than OH-
acidic; pH values less than 7.0
66
Solutions w/ a pH value above 7.0
bases
67
What is the normal pH of blood?
7.35 - 7.45
68
What happens when the blood pH is 7.5 - 7.8?
alkalosis - makes one feel agitated/dizzy
69
What happens when the pH is 7.0 - 7.3?
acidosis - makes one feel fatigued and disoriented, with breathing becoming difficult
70
List the two large groups of chemicals involved in chemical reactions
organic (contain carbon and hydrogen atoms) and inorganic substances
71
Inorganic substances usually dissolve in what?
Water, therefore they are electrolytes.
72
List the 5 inorganic substance
Water, oxygen, carbon dioxide, other gases (NO and CO), and inorganic salts
73
Use of the inorganic substance water
* polar water molecules cause molecules of substances to break apart so that they are more likely to take part in metabolic reactions
* transports materials
* can absorb and transfer heat
74
Use of the inorganic substance oxygen
organelles use oxygen to release energy from nutrient molecules
75
Use of the inorganic substance carbon dioxide
waste product formed when energy is released from nutrients
76
Use of NO and CO
NO and CO can be harmful in large amounts.
NO is used in digestion, memory, immunity, circulation, and respiration
CO is used in the spleen and in parts of the brain where it is used for memory, smell, and other vital functions
77
List inorganic salts
Na+, Cl-, K+, Ca2+, Mg2+, PO42-, CO32-, HCO3-, SO42-
78
Use of inorganic salts
* helps maintain correct water concentration in cells
* blood clotting
* pH
* bone development
* muscle and nerve function
79
What is electrolyte balance?
The need for inorganic salts to be present in certain concentrations to maintain homeostasis.
80
Organic substances are more like to dissolve in what than water?
organic solvents
81
List the 4 organic substances
* carbohydrates
* lipids
* proteins
* nucleic acid
82
Use of carbohydrates
provide much of the energy that the cells require; supply material to build cell structures; stored as energy reserves
83
Describe carbohydrates
* water-soluble molecules that contain carbon, hydrogen, and oxygen
* usually twice as many hydrogen atoms as oxygen atoms
* classified according to size
84
Simple carbohydrates, or sugars, include what?
monosaccharides and disaccharides
85
Describe monosaccharides
may include 3-7 carbons in a straight chain; examples are glucose, fructose, galactose, ribose, and deoxyribose
86
Describe disaccharides
consist of 2 6-carbon unites; examples are lactose and sucrose
87
These are built of simple carbohydrates
Complex carbohydrates aka polysaccharides; examples are cellulose, plant starch, and glycogen
88
Describe lipids
* insoluble in water but soluble in organic solvents
* fats, phospholipids, steroids; fats are the most common
* composed of carbon, hydrogen, and oxygen; much smaller percentage of oxygen than carbohydrates
89
Building blocks of fats
fatty acids and glycerol
90
What can supply more energy gram for gram: fats or carbohydrates?
fats
91
What is at the end of a fatty acid?
Carboxyl group (-COOH)
92
If all the bonds between the carbon atoms in the carbon chain of a fatty acid, the chain is called?
saturated
93
If there are some double bonds between the carbon atoms in the carbon chain of a fatty acid, the chain is called?
unsaturated
94
What type of unsaturated fatty acid only has one double bond?
monounsaturated fatty acid
95
What type of unsaturated fatty acid has more than one double bond?
polyunsaturated fatty acid
96
How are triglycerides formed?
fatty acids and glycerol unite so that each glycerol molecule binds to three fatty acid chains
97
These types of lipids consist of a glycerol portion, two fatty acid chains, and a third portion that contains a phosphate group.
Phospholipids
98
Describe the "head" of a phospholipid molecule
Made up of the phosphate group; this portion is water soluble and said to be "hydrophilic"
99
Describe the "tail" of a phospholipid molecule
Made up of the fatty acid portion; this portion is insoluble in water and said to be "hydrophobic"
100
Complex structures that include interconnected rings of carbon atoms
Steroids
101
Steroid that is found in all body cells and is used to synthesize other steroids
cholesterol
