Gen Chem Flashcards
(208 cards)
1
Q
It is anything that occupies space and has mass
A
Matter
2
Q
It refers to the amount of matter present in the material
A
Mass
3
Q
Classifications of Matter
A
Element
Compound
Mixture
4
Q
It is the simplest form of matter, 1 kind of material or atom
A
Element
5
Q
Refers to substances composed of two or more elements united chemically in definite proportion
A
Compound
6
Q
It is composed of 2 or more substances that are not chemicallv combined
A
Mixture
7
Q
Colorless fluid part of blood, lymph, or milk in which corpuscles or fat globules are suspended
A
Plasma
8
Q
- Amber- colored protein-rich liquid that separates out wen blood coagulates
- used to provide immunity
- Diagnostic agent
A
Serum
9
Q
Classification of Mixture According to the Nature of Particles
A
Homogenous
Heterogenous
10
Q
Classification of Mixture According to the Size of Particles
A
Solution
Suspension
Colloid
11
Q
uniform mixture (homogenous), composed of solute and solvent where solute is soluble
A
Solution
12
Q
Coarse Mixture, finely divided solid materials distributed in a liquid where solid is insol.
A
Suspension
13
Q
particles of solute not broken down to the size of the molecules but are small enough to remain suspended and evenly dispersed throughout the medium
A
Colloid
14
Q
difference in specific gravity or density
A
Decantation
15
Q
evaporation and then condensation
A
Distillation
16
Q
speeding up of settling process of a precipitate
A
Centrifugation
17
Q
lowering of temp so that the more insoluble comp crystallizes out first
A
Fractional Crystallization
18
Q
difference in solvent affinity
A
Chromatography
19
Q
Properties of Matter
A
Intrinsic/Intensive
Extrinsic/Extensive
20
Q
INDEPENDENT of mass or amount (density, specific gravity, melting point)
A
Intrinsic/Intensive
21
Q
- DEPENDENT on mass (weight, volume, pressure, heat content)
A
Extrinsic/Extensive
22
Q
change in phase
A
Physical Change
23
Q
change in both intrinsic and extrinsic properties
A
Chemical Change
24
Q
splitting of a heavy atom
A
Nuclear Fission
25
union of 2 light atoms to form a bigger molecule
Nuclear Fusion
26
the number of protons + the number of neutrons
Mass Number
27
the number of protons
Atomic Number
28
Mass number – Atomic number
Neutrons
29
Protons - Charge
Electrons
30
- Matter is made up of small indivisible particles
- Coined "atomos"
Democritus
31
"Billiard Ball Model"
John Dalton
32
atom is a hard indestructible sphere
Billiard Ball Model
33
Matter is made up of atoms
All atoms of a given element are alike
Atoms enter into a combination with other atoms to form compounds but remain unchanged during ordinary chemical rn
Dalton’s Atomic Theory
34
"Raisin Bread" model
JJ Thompson
35
Proton; Gold Film Experiment: Atom is mostly an empty space (99% passed)
Ernest Rutherford
36
Planetary model
Niel Bohr Model
37
Quantum Mechanic Model; “Electron Cloud”
Erwin Schrodinger
38
electrons move in 3D structure (Orbitals)
Electron cloud
39
Neutron
James Chadwick
40
It refers to charged atoms
Ions
41
atoms of different elements can link together in different ways to form substances with dift properties
Allotrope
42
Allotropes of Carbon
Diamond and Graphite
43
Allotropes of Oxygen
O - nascent
O2 - molecular
O3 - ozone
44
region in space where the probability of finding an electron is greatest
Orbitals
45
Determine the size of the particle
Principal Quantum Number
46
Subshell or sublevel, determines the shape (s, p, d, f)
Azimuthal or Angular Momentum
47
Orbitals, determine the orientation
Magnetic Quantum Number
48
Direction of the spin or rotation
Spin Quantum Number
49
The total mass of all products of a chemical reaction is equal to the total mass of all reactants of that reaction
Law of Conservation of Mass
50
- Inorganic compounds
- A chemical compound always contains exactly the same proportion of elements by mass
Law of Definite Proportions/Proust’s Law
51
- Organic compounds
- When chemical elements combine, they do so in a ratio of small whole numbers
Law of Multiple Proportion
52
No two electrons can have the same set of 4 quantum numbers.
Each atomic orbital can only accommodate 2 electrons (Ex: 1s2)
Pauli’s Exclusion Principle
53
Impossible to determine simultaneously the e- momentum & position
Heisenberg’s Uncertainty Principle
54
Lower energy levels are filled up first
Aufbau Building Up Principle
55
Orbitals are filled up singly before pairing up
Hund’s Rule of Maximun Multiplicity
56
He recognized Hydrogen as an element
First true periodic table
Antoine-Laurent Lavoisier
57
He discovered Triads (Li, Na, K | Ba, Ca, Sr | S, Se, Te | Cl, Br, I)
Johann Dobereiner
58
Octaves
John Newlands
59
Physical and chemical properties are periodic functions of their atomic weights
Meyer and Mendeleev
60
Elements are arranged based on atomic numbers (present)
Henry Mosley
61
It explains phases of matter based on movement (exclu. direction) of molecules/ions/atoms
Kinematic Molecular Theory
62
- definite shape and size, definite volume
SOLID
63
- follows the shape of container, definite volume
LIQUID
64
- indefinite shape and volume
GAS
65
homogenous mixture single phase system of two of more substances
Solutions
66
maximum amount of solute
Saturated Solution
67
less solute
Unsaturated Solution
68
more solute than the solvent can dissolve
Supersaturated Solution
69
maximum amount of solute expressed in grams that can be dissolved in 100 g of water
Solubility
70
ability of one substance to mix with another substance
Miscibility
71
solubility decreases with increase in temp (Mg citrate)
Exothermic
72
solubility increases with increase in temp
Endothermic
73
↑ temperature = ↓ solubility of a gas
74
the solubility of a gas increases as pressure increases
Henry’s Law
75
Decreased particle size = Increased surface area = Increased solubility
76
presence of salt decreases solubility
Salting Out
77
presence of salt increases solubility
Salting In
78
force of attraction within molecules
Intramolecular Forces
79
Ex of Intra Forces
Covalent Bond - sharing
- polar (unequal)
- nonpolar (equal)
Ionic Bond - transfer
80
forces of attraction between molecules; physical attraction
Intermolecular Forces
81
mass per unit volume (M/V)
Density
82
density of sample/density of standard
Specific Gravity
83
reciprocal of specific gravity, opposite of density
Specific Volume
84
property of solution depend on the number of solute particles dissolved in a solvent
Colligative Property
85
movement of water across a semipermeable membrane from low to high concentration
Osmosis
86
causes crenation
Hypertonic
87
causes swelling/lysis
Hypotonic
88
0.9% (w/v) NaCl
Isotonic
89
gradual mixing of molecules of one gas with molecules of another gas by virtue of kinetic properties
Diffusion
90
passage of a gas under pressure through a small opening
effusion
91
Acid yields H and H2O
Base yields OH
Arrhenius Theory
92
Acid - proton donor
Base - proton acceptor
Bronsted-Lowry Theory
93
Acid - E acceptor
Base - E donor
Lewis Theory
94
progressive addition of a sol’n of known concentration to a substance of unknown conc
Titration
95
Substance that changes color at the end point
Indicator
96
point when equal amounts of acid and base have reacted; non-observable
Neutralization point (Stoichiometric point/Equivalence Point/Theoretical Point)
97
Experimental approximate of neutralization point; observable
Endpoint
98
the negative logarithm of the H+ concentration
pH
99
Sorensen’s pH scale
Neutral = 7
Acidic < 7
Basic > 7
100
Solutions that have the property of resisting changes in pH when acids or bases are added to them
Buffers
101
Ability of a buffer solution to resist changes in pH
Buffer Capacity (Buffer action/Buffer efficiency/Buffer index/Buffer value)
102
an energy transfer due to temperature difference
Heat (q)
103
form of energy transfer between a system and its surroundings in the form of compression or expansion of gas
Work
104
total energy attributed to the particles of matter and their interactions within a system, composed of thermal energy and chemical energy
Internal Energy (U)
105
degree of disorderliness
entropy
106
energy of a reaction
enthalpy
107
amount of heat required to raise the temperature of an object or substance by 1 degree
Heat Capacity
108
amount of heat required to raise the temperature of an object per gram
Specific Heat
109
reaction wherein heat is absorbed by the system, indicated by a (+) change in enthalpy
Endothermic Process
110
reaction wherein heat is released by the system, indicated by a (-) change in enthalpy
Exothermic Process
111
This law states that energy cannot be created or destroyed; it can only be redistributed or changed from one form to another.
Law of Conservation of Energy
112
Most reactive metals
Valence = 1
Group IA - Alkali Metals
113
Lightest and most reactive element
Hydrogen (Inflammable air)
114
Isotopes of Hydrogen
Protium
Deuterium
Tritium
115
o Lightest metal
o Depressant and Diuretic (SE: hyponatremia)
Lithium (Earth)
116
Depressant
Lithium bromide
117
DOC for Mania
Lithium Carbonate (Lithase®, Eskalith®)
118
o Primary extracellular fluid cation
o Action: fluid retention
Sodium (Natrium)
119
o Most abundant and predominant intracellular cation
o Deficiency: hypokalemia
o Manifestation: muscle paralysis (Barker’s syndrome)
o Diuretic, Important in muscle contraction
Potassium (Kalium)
120
Never employed in medicine because it is the most toxic metal
Beryllium
121
o Lightest of all structurally important metal
o 2nd most abundant intracellular cation
Magnesium
122
Most malleable and ductile, Best conductor of electricity
Gold
123
o Only reddish metal, 3rd most malleable, 3rd best conductor
o Protein precipitant, Enhances physiological utilization of iron
COPPER (Cuprum)
124
Catalyst in polymerization of resin forming material
Cesium
125
Hypothetical alkali metal
Ammonia
126
contains 10% NH4; is known as 16° ammonia
Household ammonia
127
o 2nd most abundant cation in extracellular fluid
o Vit. D is needed for its maximum absorption
Calcium
128
Temperature desensitizing agent (Sensodyne®)
SrCl2
129
Radioactive element used for cancer radiotherapy & diagnostic purpose
Radium
130
o Present in inZulin and carbonic anhydraZe
o Parakeratosis
Zinc
131
Astringent, manufacture of stink bomb
Cadmium
132
It is used as anti sebborheic
CdS
133
Industrial use: In vulcanizing rubber
Boron
134
o Most abundant metal
o 3rd most abundant element
Aluminum
135
o Pcol use: treatment of cancer-related hypercalcemia by binding with transferring
o Nonpharma: substitute for mercury in manufacture of arc lamps; Galvanized iron
Gallium
136
Crystalline form of Carbon
Diamond (purest native form)
Graphite (lead pencil)
137
Amorphous form of Carbon
Coal
Anthracite
138
2nd most abundant element, Component of glass
Silicon
139
Powerful reducing agent
Titanium
140
Opacifying agent (Ocusert®) and UV ray protectant
TiO2
141
antiperspirant but banned due to granuloma formation
Zirconium
142
Most abundant gas in air
Nitrogen 71%
143
White/yellow (poisonous), Red (non-poisonous)
Phosphorus
144
o Protoplasmic poison
o Insecticide: Copper Aceto Arsenate (Paris green)
Arsenic
145
First anti-syphilis (Paul Ehrlich)
Salvarsan/Magic Bullet/Compound 606/Arsphenamine
146
Astringent, Antiseptic, Internal protective for ulcer, Used in silvering of mirror
Bismuth
147
Not affected by any body fluid, Sheet form used in repair of bones, nerve and tissue
Tantalum
148
Most abundant element, discovered by Scheele
Oxygen
149
Antifungal, Parasiticide, Scabicide, Depilatory agent
Sulfur
150
Promotes Vit. E absorption, Antioxidant (SeS2 /Selsun blue – anti-dandruff)
Selenium
151
Becquerel, Atomic bombs
Uranium
152
Co-factor enzyme
Molybdenum
153
Strongest oxidizing agent
Fluorine
154
o Most abundant extracellular anion, green gas
o Used as water disinfectant
Chlorine
155
Used as bleaching agent
Hyporchlorite
156
Used in treatment of achlorydria
HCl
157
Dark reddish brown fuming liquid with suffocating odor
Bromine
158
o Oldest known germicide
o Expectorant, Antifungal
o Preparation of T3 and T4
o Deficiency: Goiter
Iodine
159
o Only metallic
o Only synthetic halogen
o Only radioactive halogen
Astatine
160
o 1st element produced artificially
o Used in preparation of radiopharmaceuticals
Technecium
161
o 2nd lightest gas
o Donald-duck-like sound
Helium
162
o Least abundant of all noble gases
o Have inhalational anesthetic activity
Krypton
163
Most abundant noble gas
Argon
164
o Synthetic noble gas
o Used for treatment of CA (cervical CA)
Radon
165
electron carrier in respiration chain; responsible for transport of molecular oxygen
iron
166
alkaline bases used to neutralize the excess gastric HCl associated with gastritis and peptic ulcers
antacids
167
persistent golden yellow in flame test
Sodium
168
violet in flame test
Potassium
169
Carmine red/Pink in flame test
Lithium
170
Brick red in flame test
Calcium
171
Blue in flame test
Pb, As, Sb, Bi, Cu
172
Colorless in flame test
Ammonium
173
branch of chemistry that deals with carbon-containing compounds with: H, O, P, N, S, X
Organic Chemistry
174
Contains 4 binding sites for other atoms to attach to it
These four binding sites, when bonded with other atoms/molecules form a tetrahedron
Carbon
175
deals with the physicochemical properties of drugs that affect its biological action
ORGANIC MEDICINAL CHEMISTRY
176
introduced phenol (carbolic acid)
Joseph Lister
177
Who discovered Salvarsan (compound 606), Selective toxicity
Paul Ehrlich
178
for sleeping sickness
Atoxyl
179
anti-infective agents that are used locally
germicides
180
Fe + S -> FeS (all sulfides are BLACK)
Direct Union
181
Na2CO3 -> Na2O + CO2
Decomposition/Analysis
182
Na + HCl -> NaCl + H2
Single Replacement
183
NaCl + AgNO3 -> NaNO3 + AgCl
Double Displacement
184
Constant in Boyle’s/Mariotte Law
Temperature
185
Constant in Charles Law
Pressure
186
Constant in Gay-Lussac’s Law
Volume
187
Constant in Avogadro’s Law
6.022 x 10^23
188
Most systematic nomenclature
IUPAC
189
Carbon valence
4
190
Carbon Atomic Number
6
191
It contains added methanol (wood alcohol) and benzene
Denatured Alcohol
192
Astringent, rubefacient, refrigerant, mild local anesthetic
Rubbing Alcohol (70%)
193
nlt 99% ethanol; obtained by azeotropic distillation
Dehydrated/Absolute Alcohol
194
Rapidly bactericidal (50% to 95%), 40% equal antiseptic power to a 60% ethanol
Isopropyl Alcohol
195
Used to sterilize temp-sensitive medical equipment and those that could not be autoclaved
Ethylene Oxide
196
ratio of a dilution of a given test disinfectant to the solution of phenol that is required to kill a
strain of S.typhi under carefully controlled time and temperature
Phenol coefficient
197
Introduced as surgical antiseptic by Joseph Lister; its use is now obsolete
Phenol
198
Phenol with 10% water
Liquefied Phenol
199
2% (shampoo), for athlete’s foot and jock itch
p-chloro-m-xylenol
200
mixture of three isomeric methylphenols; obtained from coal tar or petroleum
Cresol
201
Preservative more effective against molds
Methylparaben
202
Preservative more effective against yeast, more oil soluble so it is preffered for oils and fats
Propylparaben
203
common in vials of injectables with 1%to 4% concentrations in water or saline
Benzyl alcohol
204
preservatives in foods and pharmaceuticals at low pH
Benzoic acid
205
DOC for scabies; from Peru balsam and other resins
Benzyl benzoate
206
Beta-lactam Antibiotics
Penicillin
Beta-lactamase Inhibitors
Cephalosporins
Carbapenem
Monobactam
207
Binds to 30s
Aminoglycosides
Tetracyclines
208
Binds to 50s
Macrolides
Lincosamides
Chloramphenicol
