Lecture II: Basic Chemistry Flashcards
1
Q
is a pure substance that is distinguished from all other matter by the fact that it cannot be created or broken down by ordinary chemical means.
A
Elements
2
Q
5 elements which are essential for human survival
A
oxygen, carbon, hydrogen, nitrogen, and sulfur
3
Q
is a substance composed of two or more elements joined by chemical bonds.
A
Compound
4
Q
is a substance composed of two or more elements joined by chemical bonds.
A
Compound
5
Q
is the number of protons (also electrons) in the nucleus of an atom which identifies the element.
A
Atomic number
6
Q
is the sum of the number of protons and neutrons in its nucleus.
A
Mass number
7
Q
is one of the different forms of an element, distinguished from one another by different numbers of neutron.
A
Isotope
8
Q
have more than the usual number of neutrons and are unstable:
A
Heavy isotopes
9
Q
differ in their half - life, the time it takes for half of any size sample of an isotope to decay.
A
Radioisotopes
10
Q
There is a layer of electrons that encircle the nucleus at a distinct energy level called the.
A
ELECTRON SHELL
11
Q
an atom’s outermost electron shell and the number of electrons in it determines the tendency of an atom to participate in chemical reactions.
A
Valence shell
12
Q
is a weak or strong electrical attraction that holds atoms the same vicinity.
A
Bond
13
Q
is grouping of two or more atoms held together by chemical bonds.
A
Molecule
14
Q
Is a molecule made up of two or more atoms of different elements.
A
Chemical compound
15
Q
3 types of chemical bonds important in human physiology:
A
ionic bonds, covalent bonds and hydrogen bonds.
16
Q
These are ions that play roles in transmitting nerve signals.
A
Sodium, potassium, and calcium ions.
17
Q
___ ions regulate fluid in and out of cells. The body uses ___ to make hormones that regulate metabolism.
A
Chloride and Iodine
18
Q
Respiration produces ___ , a molecular energy source for our cells.
A
Adenosine Triphosphate or ATP
19
Q
Bones and teeth are mainly ___.
A
calcium phosphate
20
Q
Without ___ , bones are spongier and break more easily.
A
Manganese
21
Q
So far, ___ is the number of elements that have been identified with certainty. ___ occur in nature.
A
118, 92
22
Q
It comes from the Greek word meaning “incapable of being divided.”
A
Atoms
23
Q
TRUE or FALSE. The electric charge of a particle is a measure of its ability to attract or repel other charged particles.
A
TRUE
24
Q
A neutral atom must have an equal number of what?
A
protons and electrons
25
Atoms that have gained or lost electrons are called?
Ions
26
In this ___ model of an atom, the electrons move around the nucleus in fixed orbits.
Planetary model
27
In this model of an atom, electrons are shown as a cloud of negative charge.
Orbital model
28
What is the simplest arom?
Hydrogen
29
TRUE OR FALSE. The atomic number indirectly tells us the number of electrons that atom contains.
TRUE
30
They have the same number of protons and electrons but vary in the number of neutrons they contain. Same atomic number but different atomic masses.
Isotopes
31
This kind of bond is formed when electrons are completely transferred from one atom to another.
Ionic bond
32
This kind of bond forms when atoms share valence electrons.
Covalent bond
33
Give an example of a nonpolar covalent molecule.
CO2 or Carbon dioxide
O=C=O
34
Give an example of a polar covalent molecule.
H2O or water
35
result when electrons are unequally shared between atoms
Polar covalent bonds
36
result when electrons are more equally shared between atoms.
Nonpolar covalent bond
37
Are extremely weak bonds formed when a hydrogen atom bound to one “electron-hungry” nitrogen or oxygen atom is attracted by another such atom, and the hydrogen atom forms a “bridge” between them.
Hydrogen bonds
38
Is the kind of bond responsible for water’s surface tension.
Hydrogen bond
39
Three patterns of chemical reactions.
Synthesis reactions, decomposition reactions, exchange reactions.
40
The formation of protein molecules is what pattern of chemical reaction?
Synthesis reactions
41
Digestion of food and breakdown of glycogen to release glucose when the blood sugar level starts to decline is what pattern of chemical reaction?
Decomposition reactions
42
Involve simultaneous synthesis and decomposition reactions.
Exchange reactions
43
What pattern of chemical reaction happens when ATP transfers its terminal phosphate group to glucose to form glucose-phosphate?
Exchange reactions
44
What are the factors that affect the rate of chemical reactions?
Temperature, concentration of reacting particles, particle size, presence of catalysts
45
TRUE OR FALSE. Smaller particles have lower kinetic energy and move slower than larger ones, hence they don’t take part in more collisions.
FALSE. It has more kinetic energy and moves faster. They also take part in more collisions.
46
TRUE OR FALSE. Carbon dioxide and carbon monoxide are organic compounds.
FALSE
47
Examples of inorganic compounds found in the body.
Water, salts, some acids and bases
48
The most abundant inorganic compound in the body. It accounts 2/3 of body weight.
Water
49
The liquid part of blood that is mostly made up of water.
Blood plasma
50
It is a common form of a chemical reaction where water is mostly used to break down the chemical bonds that exists between a particular substance.
Hydrolysis
51
The fluid that surrounds a developing fetus within the mother’s body.
Amniotic fluid
52
Translucent mixtures with solute particles of intermediate size are called?
Colloids
53
If the particles of the mixture are visible to the naked eye and settle down under the influence of gravity, it is a _____.
suspension
54
What are the water properties that make it so vital?
High heat capacity
Polarity/solvent properties
Chemical reactivity
Cushioning
55
Why salt disassociate in water?
Because of its polarity
56
Substances that conduct an electrical current in solution.
Electrolytes
57
List the 3 examples of electrolytes and why they are called such?
Acids, bases, and salts
-they ionize, dissociate in water, and can then conduct an electrical current
58
It is a substance that can release hydrogen ions (H+) in detectable amounts. They are defined as proton (H+) donors. Puts protons “in the game.”
Acids
59
An acid produced by stomach cells that aids digestion.
Hydrochloric acid
60
Acids that ionize completely and liberate all their protons are called ____ ____. An example is ____.
Strong acids, hydrochloric acid
HCI —> H+(proton) + CI-(anion)
61
Give examples of weak acids that don’t ionize completely.
Carbonic acid - found in soft drinks and wines
Acetic acid - acidic component of vinegar
62
The proton (H+) acceptors. Puts protons “out of the game.”
Bases
63
When acids are dissolved in water, they release hydrogen ions and some ____.
Anions
64
When bases ionize and dissociate in water, the hydroxide ion (OH-) and some ____ are released.
Cations
65
Example of a strong base. It is a common ingredient in cleaners and soaps.
Sodium hydroxide or lye
66
An important base in blood which is a fairly weak base.
Bicarbonate ion or HCO3-
67
This type fo exchange reaction, in which an acid and a base interact, is more specifically called a _______ reaction.
neutralization
68
Determine what type of reaction is happening below.
HCI + NAOH —> H2O + NACI
Neutralization
69
The ____, which was devised in 1909 by a Danish Biochemist (and part-time beer brewer) named ____, is based on the number of protons in solution.
pH scale
Sørensen
70
Solutions with a pH lower than 7 are what?
Acidic solutions
71
Solutions with a pH number higher than 7 are what?
Basic or alkaline solutions
72
A ____ is a solution or chemicals that can resist pH change upon the addition of an acidic or basic components.
buffer
73
A solution with a pH of 7 is a ______.
Neutral solution
74
Biological molecules are formed from their monomers (units) by _____ _____ and broken down to their monomers by ____.
dehydration synthesis
hydrolysis
75
Normal blood pH
7.35-7.45
76
It is the protein contained in red blood cells that is responsible for delivery of oxygen to the tissues.
Hemoglobin
77
The process of combination of two molecules with the elimination of water molecules is called _____ _____.
dehydration synthesis
78
Carbohydrates means ____ according to scientists.
Hydrates of carbon
79
carbohydrates are classified according to what?
Solubility and size
80
monosaccharides are also referred to as?
simple sugars
81
these are carbohydrates that contain 3-7 carbon atoms
Monosaccharides
82
most important monosaccharides
glucose
fructose
galactose
ribose
deoxyribose
83
also called blood sugar, universal cellular fuel
Glucose
84
The liver then converts both ____ and ____ into glucose, so that dissolved glucose, known as blood sugar, is the only monosaccharide present in circulating blood.
fructose and galactose
85
These are formed when two simple sugars are joined by dehydration synthesis.
Disaccharides
86
Sucrose monomers
glucose-fructose
87
table sugar found in fruits, vegetables, and nuts
Sucrose
88
lactose monomers
glucose and galactose
89
maltose monomers
glucose-glucose
90
long, branching chains of linked simple sugars
ideal storage products because they are large, insoluble molecules
lack sweetness
Polysaccharides
91
Storage polysaccharide formed by plants
Starch
92
It is the stored form of glucose in animals and humans (largely in muscles and liver).
Glycogen
93
energy currency of body cells
ATP
94
If not immediately needed for ATP synthesis, dietary carbohydrates are converted to ____ or ____ and stored.
glycogen or fat
95
Most abundant lipids in the body
Triglycerides, steroids, phospholipids
96
Egg yolks, meats, dairy products, and oils are examples of what macromolecule?
Lipid or fat
97
among the CHO element, what is abundant in lipid molecules?
Carbon and hydrogen
98
neutral fats
Triglycerides
99
Building blocks of triglycerides
Fatty acids and glycerol
100
Monomers of lipids
Fatty acids and glycerol
101
What makes the different kinds of neutral fats?
The variation of fatty acid chains.
102
It determines how solid the molecule of triglyceride is at a given temperature.
The length of a triglyceride’s fatty acid chains and their type of C=C bonds.
103
Fatty acid chains with only single covalent bonds between carbon atoms are referred to as ____ fats. Their fatty acid chains are straight, and, at room temperature, the molecules pack closely together, forming a solid; butter is an example.
saturated
104
Fatty acids that contain one or more double bonds between carbon atoms are said to be ____. The double and triple bonds cause the fatty acid chains to kink so that they cannot pack closely enough to solidify.
unsaturated fats (monounsaturated and polyunsaturated, respectively).
105
_____ fats (including a type called trans fat) tend to stay solid at room temperature and can cause fatty deposits in blood vessels, leading to atherosclerosis ("hardening of the arteries").
Saturated
106
____ fats stay liquid at room temperature and are less likely to clog your arteries.
Unsaturated
107
____ fats are common in many margarines and baked products, are oils that have been solidified by the addition of hydrogen atoms at sites of double carbon bonds, which reduces those bonds to single carbon bonds. They increase the risk of heart disease by raising “bad” cholesterol and decreasing “good” cholesterol.
Trans fats
108
The ____ fatty acids, found naturally in cold-water fish, appear to decrease the risk of heart disease and some inflammatory diseases.
omega-3
109
When they are oxidized, they yield large amounts of energy. They are stored chiefly in fat deposits beneath the skin and around body organs, where they help insulate the body and protect deeper body tissues from heat loss and injury.
Triglycerides
110
What’s the difference between phospholipids and triglycerides?
The major difference is that a phosphorus-containing group is always part of the molecule and takes the place of one of the fatty acid chains. Thus, phospholipids have two instead of three attached fatty acids.
111
They are basically flat molecules formed of four interlocking carbon rings. However, like fats, they are made largely of hydrogen and carbon atoms and are fat-soluble.
Steroids
112
The single most important steroid molecule is ____.
cholesterol
113
____ is found in cell membranes and is the raw material used to make vitamin D.
Cholesterol
114
The basis of all body steroids.
Cholesterol
115
A breakdown product of cholesterol; released by the liver into the digestive tract, where they aid in fat digestion and absorption.
Bile salts
116
A fat-soluble vitamin produced in the skin on exposure to UV (ultraviolet) radiation (sunshine); necessary for calcium absorption and normal bone growth and function.
Vitamin D
117
Female hormones
Estrogen and progesterone
118
Male hormone
Testosterone
119
Is a glucocorticoid, is a long-term antistress hormone that is necessary for life
Cortisol
120
What is the structure of an amino acid?
An amino acid's structure consists of a central carbon atom attached to a hydrogen, an acidic carboxyl group (−COOH), an amino group (−NH2) and an organic side chain (also called an R group).
121
Simplest amino acids
Glycine
122
Amino acids differ in what group?
Amino acids differ from each other with respect to their side chains, which are referred to as R groups.
123
Building blocks of carbohydrates
Monosaccharides
124
most abundant biomolecule in the human body
proteins
125
Elements of proteins
CHONS
126
Building blocks of protein
Amino acids
127
amino acid group that provides basic properties
-NH2 or amine group
128
Acid group formula
-COOH
129
Also called functional proteins with at least a tertiary structure
Globular proteins
130
Also called structural proteins.
Fibrous proteins
131
Example of fibrous protein
Collagen
132
Example of globular protein
Hemoglobin
133
Elements of nucleic acids
CHONSP
134
3 basic parts of a nucleotide
(1) nitrogen-containing base
(2) pentose or the 5-carbon sugar
(3) phosphate group
135
2 major kinds of nucleic acids
Deoxyribonucleic acid or DNA
Ribonucleic acid or RNA
136
Approximately equal to the mass number of the most abundant isotope.
Atomic weight
137
TRUE OR FALSE. Hydrogen bonds involve electrons.
FALSE
138
Important bases that act as buffers (resist changes in pH).
Bicarbonate ions
139
Examples of polysaccharides
Starch and glycogen
140
Type of fat that provides insulation in fat tissue and reserve body fuel.
Triglycerides
141
Determine the level of protein structure: amino acid sequence
Primary structure
142
Determine the level of protein structure: the alpha-helix and beta-pleated sheet
Secondary structure
143
Determine the level of protein structure: a three dimensional structure formed by secondary structures folding on one another.
Tertiary structure
144
Determine the level of protein structure: a globular structure formed by two or more polypeptide chains.
Quaternary
145
are functional proteins such as enzymes, peptide hormones, and hemoglobin
Globular proteins
146
These proteins unfold (denature and inactivate) when their hydrogen bonds are disrupted by heat or pH changes.
Globular or functional proteins
147
Speed the rates of chemical reactions by binding temporarily and specifically with reactants and holding them in the proper position to interact.
Enzymes
148
TRUE OR FALSE. Enzymes are reusable biological catalysts.
TRUE
149
Monomers of nucleic acid
Nucleotides
150
The element essential for normal thyroid function.
Iodine
