Chemical Basis Of Life Flashcards
(128 cards)
1
Q
Science dealing with the atomic composition of
substances and the reaction they undergo
A
Chemistry
2
Q
anything that occupies space and has mass
A
Matter
3
Q
amount of matter of an object
A
Mass
4
Q
international unit of mass
A
kilogram (Kg)
5
Q
gravitational force acting on an object of a given mass
A
Weight
6
Q
Not constant, changing from place to place
A
Weight
7
Q
constant
A
mass
8
Q
Smallest type of matter having unique chemical properties
A
Element
9
Q
Smallest particle on an element; Indivisible
A
Atom
10
Q
to be an ______, it can only have ______ type of atom
A
element
one
11
Q
an element is often represented by a
A
symbol
12
Q
atoms are composed of
A
subatomic particles
13
Q
3 Major Types of Subatomic Particles
A
Neutron, Proton, Electron
14
Q
has no electric charge
A
Neutron
15
Q
Has one positive charge
A
Proton
16
Q
Has one negative charge
A
Electron
17
Q
tendency of particles to be attracted to each other or repulsed from each other.
A
Electrical Charge
18
Q
2 Types of Electrical Charge
A
Positive
Negative
19
Q
the number of protons in each atom
A
Atomic Number
20
Q
the quantity of matter contained in an atom of an element (# of protons + # of neutrons)
A
Atomic Mass
21
Q
Common Elements in the Human Body
A
Hydrogen, Carbon, Nitrogen, Oxygen, Sulfur, Sodium, Phosphorus, Chlorine, Potassium, Calcium, Iron, Iodine
22
Q
the interaction between atoms to form
molecules by either sharing or transferring
their outermost electrons
A
Chemical Bonds
23
Q
the outside part of an atom around
the atomic nucleus
A
Electron Shells
24
Q
outermost shell
A
Valence Shell
25
if an atom’s valence shell is not at its
maximum, it will form bonds with other
atoms to achieve a full valence shell.
Octet
26
tendency of atoms to combine with
other atoms until each has 8 electrons
Octet Rule
27
ability of the atom’s nucleus to pull electrons toward it
Electronegativity
28
2 Major Types of Chemical Bonds
Ionic Bond
Covalent Bond
29
forms when electrons are transferred between atoms, creating
oppositely charged ions
Ionic Bond
30
forms when atoms share one or more pairs of electrons
Covalent Bond
31
sharing of one pair of electrons by two atoms results in
Single Covalent Bond
32
results when two atoms share two pairs of electrons
Double Covalent Bond
33
Electrons can be shared unequally in _____ bond
Covalent
34
an unequal, asymmetrical sharing of electrons
Polar Covalent Bond
35
molecules that are electrically asymmetric
Polar Molecules
36
there is an equal sharing of electrons between atoms; electronegativities are the same
Nonpolar Covalent Bond
37
Molecules that are Electrically Symmetric
Nonpolar molecules
38
interaction involving a hydrogen
atom located between a pair of
other atoms having a high affinity
for electrons
Hydrogen Bond
39
Weakest bond
Hydrogen bond
40
formed when two or more atoms chemically combine
to form a structure that behaves as an independent unit
Molecules
41
substance resulting from the
chemical combination of two or more different types of atoms
Compounds
42
molecules, sharing of compounds are in distinct units
Covalent Compounds
43
not molecules, did not consist of distinct units
Ionic compounds
44
sodium chloride is a molecule or a compound?
A compound, not a molecule
Ionic bond
45
C6H12O6
Glucose
46
Molecules and compounds can be represented by the ________ of
the atoms forming the molecule or compound plus ________
denoting the quantity of each type of atom present.
symbols
subscripts
47
when molecules separate or split into other things
Dissociation
48
dissociated ions
Electrolytes
49
have the capacity to conduct an
electrical current
Electrolytes
50
the flow of charged particles
Electrical current
51
a recording of electrical
currents produced by the heart.
Electrocardiogram (ECG)
52
formation or
breaking of chemical bonds between
atoms, ions, molecules, are
compounds
Chemical Reaction
53
Chemical Reactions
Synthesis
Decomposition
Exchange
Reversible
54
when 2 or more reactants combine to form a larger, more complex product
Synthesis Reaction
55
all synthesis reactions that occur in the body are
anabolism
56
A t B -> AB
Synthesis Reactions
57
Synthesis reaction where water is also a product
Dehydration reactions
58
Reactants are broken down into smaller, less
complex products
Decomposition Reaction
59
AB ---> A + B
Decomposition Reaction
60
decomposition reactions that occur in the body
catabolism
61
Reactions that use water
Hydrolysis reactions
62
a combination of a decomposition reaction and a synthesis reaction
Exchange Reactions
63
AB + CD ---> AC + BD
Exchange Reactions
64
reaction can run in the opposite direction, so that the products are converted back to the original reactants
Reversible Reactions
65
When the rate of product formation is equal to the rate of
reactant formation, the reaction is said to be at
equilibrium
66
capacity to do work
Energy
67
stored energy; currently not doing work
Potential Energy
68
energy caused by movement of an object and actually does
work
Kinetic Energy
69
a form of potential energy
stored in chemical bonds
Chemical Energy
70
a form of potential energy
because of the charges and positions of the
subatomic particles bound together
Chemical Bonding
71
energy resulting from the
position or movement of objects
Mechanical Energy
72
rate at which a reaction proceeds is influenced by several
factors
Reactants
Concentration
Temperature
Catalysts
73
Reactants differ from one another in their ability to
undergo chemical reactions
74
The greater the ______ of the reactants, the greater the rate at
which a chemical reaction will occur
concentration
75
the rate of chemical reactions is partially dependent on _______
temperature
76
A ________ increases the rate of a chemical reaction
Catalyst
77
a proton donor, positively charged
Acids
78
a proton acceptor, negatively charged
Bases
79
a measure of the H+ concentration of a solution
pH scale
80
the pH scale ranges from
0 to 14
81
pH of 7.0
an equal number of H+ and OH−
Neutral Solution
82
pH less than 7.0
a greater concentration of H+ than of OH−
Acidic Solution
83
pH greater than 7.0
fewer H+ than OH−
Basic/Alkaline Solution
84
blood pH drops below 7.35
acidosis
85
In acidosis, the nervous system becomes _______ and the individual becomes ______ and probably ________.
depressed
disoriented
comatose
86
blood pH rises above 7.45
alkalosis
87
In alkalosis, the nervous system becomes _______ and the individual becomes ______ and have ________.
overexcitable
extremely nervous
convulsions
88
a compound consisting of a positive ion other than
H+ and a negative ion other than OH−.Salts are formed
by the reaction of an acid and a base
Salts
89
a chemical that resists changes in pH when either an
acid or a base is added to a solution
Buffer
90
deals with those
substances that do not contain carbon
Inorganic Chemistry
91
CO2 and CO are examples of _______ chemistry
inorganic
92
study of carbon-containing substances
Organic Chemistry
93
Two oxygen atoms
bound by a double
covalent bond
Oxygen (O2)
94
Without O2 to accept the H+ and electrons, the ______
and the ___________ cannot function.
citric acid cycle
electron-transport chain
95
One carbon atom bound to
two oxygen atoms by a
double covalent bond
Carbon Dioxide (CO2)
96
A metabolic by-product,
exhaled during respiration
CO2
97
Becomes toxic when
accumulated in the cells
CO2
98
consists of one atom of
oxygen joined by polar
covalent bonds to two atoms
of hydrogen
Water (H2O)
99
4 Properties of Water
1. Stabilizing body temperature
2. Providing Protection
3. Facilitating chemical reactions
4. Transporting substances
100
4 Organic Chemistry
1. Carbohydrates
2. Lipids
3. Proteins
4. Nucleic Acids
101
most abundant organic compound in
the biosphere
Carbohydrates
102
consists of CHO
serves as a major source of energy
and structural components for
living organisms
Carbohydrates
103
3 Classes of Carbohydrates
Monosaccharides
Disaccharides
Polysaccharides
104
3 Types of Monosaccharides
Glucose
Fructose
Galactose
105
3 Exampls of Disaccharides
Maltose
Sucrose
Lactose
106
Examples of Polysaccharides
Starch (Amylose, Amylopectin)
Cellulose
Glycogen
107
a long, unbranched, chain
of glucose subunits
Amylose
108
has a branched structure
Amylopectin
109
the storage form of
carbohydrate in animals
Glycogen
110
an important structural molecule
in plants, and provides fiber
that we need in our diets
Cellulose
111
composed of C,H,O (others: N, P)
examples are Fats, phospholipids, eicosanoids, steroids
Lipids
112
important energy-
storage molecules
pad and insulate
the body
Fats
113
Building blocks of fat
Glycerol
Fatty Acids
114
Types of Fat
Saturated
Unsaturated (Monounsaturated and Polyunsaturated)
Transfat
115
Healthiest type of Fat
Unsaturated
116
our cell membrane
made of / structural
component (phosphate head - hydrophilic; hydrophobic tail)
Phospholipid
117
group of important
chemicals derived
from fatty acids
made in most cells
and important in
regulatory molecules
role is into the
response of tissues to
injuries
Eicosanoids
118
composed of carbon
atoms bound together into
four ringlike structures
e.g., progesterone, estrogen, testosterone
Steroids
119
contains CHON (Most have sulfur)
Proteins
120
Building blocks of proteins
Amino acids
121
There are ____ types of basic amino acids where __ are synthesized while ___ are obtained in the diet
20
12
8
122
6 Functions of Proteins
growth and maintenance
causes biochemical reactions
acts as messenger (enzymes)
provides structure
immunity / defense
transport of nutrients
123
protein catalyst that increases the rate at which a
chemical reaction proceeds
Enzymes
124
large molecules composed of CHONP
DNA and RNA
nucleic acids
125
building blocks of nucleic acids
nucleotide
126
DNA is composed of
Adenine, Thymine, Cytosine, and Guanine
127
RNA is composed of
adenine, uracil, cytosine, and guanina
128
the energy currency of cells, capable of both storing and providing energy
Adenosine Triphosphate (ATP)
