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SEM 1 > Gen Chem > Flashcards

Gen Chem Flashcards

1
Q

It is anything that occupies space and has mass

A

Matter

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2
Q

It refers to the amount of matter present in the material

A

Mass

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3
Q

Classifications of Matter

A

Element
Compound
Mixture

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4
Q

It is the simplest form of matter, 1 kind of material or atom

A

Element

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5
Q

Refers to substances composed of two or more elements united chemically in definite proportion

A

Compound

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6
Q

It is composed of 2 or more substances that are not chemicallv combined

A

Mixture

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7
Q

Colorless fluid part of blood, lymph, or milk in which corpuscles or fat globules are suspended

A

Plasma

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8
Q
  • Amber- colored protein-rich liquid that separates out wen blood coagulates
  • used to provide immunity
  • Diagnostic agent
A

Serum

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9
Q

Classification of Mixture According to the Nature of Particles

A

Homogenous
Heterogenous

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10
Q

Classification of Mixture According to the Size of Particles

A

Solution
Suspension
Colloid

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11
Q

uniform mixture (homogenous), composed of solute and solvent where solute is soluble

A

Solution

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12
Q

Coarse Mixture, finely divided solid materials distributed in a liquid where solid is insol.

A

Suspension

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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

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14
Q

difference in specific gravity or density

A

Decantation

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15
Q

evaporation and then condensation

A

Distillation

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16
Q

speeding up of settling process of a precipitate

A

Centrifugation

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17
Q

lowering of temp so that the more insoluble comp crystallizes out first

A

Fractional Crystallization

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18
Q

difference in solvent affinity

A

Chromatography

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19
Q

Properties of Matter

A

Intrinsic/Intensive
Extrinsic/Extensive

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20
Q

INDEPENDENT of mass or amount (density, specific gravity, melting point)

A

Intrinsic/Intensive

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21
Q
  • DEPENDENT on mass (weight, volume, pressure, heat content)
A

Extrinsic/Extensive

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22
Q

change in phase

A

Physical Change

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23
Q

change in both intrinsic and extrinsic properties

A

Chemical Change

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24
Q

splitting of a heavy atom

A

Nuclear Fission

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25
Q

union of 2 light atoms to form a bigger molecule

A

Nuclear Fusion

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26
Q

the number of protons + the number of neutrons

A

Mass Number

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27
Q

the number of protons

A

Atomic Number

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28
Q

Mass number – Atomic number

A

Neutrons

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29
Q

Protons - Charge

A

Electrons

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30
Q
  • Matter is made up of small indivisible particles
  • Coined “atomos”
A

Democritus

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31
Q

“Billiard Ball Model”

A

John Dalton

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32
Q

atom is a hard indestructible sphere

A

Billiard Ball Model

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33
Q

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

A

Dalton’s Atomic Theory

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34
Q

“Raisin Bread” model

A

JJ Thompson

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35
Q

Proton; Gold Film Experiment: Atom is mostly an empty space (99% passed)

A

Ernest Rutherford

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36
Q

Planetary model

A

Niel Bohr Model

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37
Q

Quantum Mechanic Model; “Electron Cloud”

A

Erwin Schrodinger

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38
Q

electrons move in 3D structure (Orbitals)

A

Electron cloud

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39
Q

Neutron

A

James Chadwick

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40
Q

It refers to charged atoms

A

Ions

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41
Q

atoms of different elements can link together in different ways to form substances with dift properties

A

Allotrope

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42
Q

Allotropes of Carbon

A

Diamond and Graphite

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43
Q

Allotropes of Oxygen

A

O - nascent
O2 - molecular
O3 - ozone

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44
Q

region in space where the probability of finding an electron is greatest

A

Orbitals

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45
Q

Determine the size of the particle

A

Principal Quantum Number

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46
Q

Subshell or sublevel, determines the shape (s, p, d, f)

A

Azimuthal or Angular Momentum

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47
Q

Orbitals, determine the orientation

A

Magnetic Quantum Number

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48
Q

Direction of the spin or rotation

A

Spin Quantum Number

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49
Q

The total mass of all products of a chemical reaction is equal to the total mass of all reactants of that reaction

A

Law of Conservation of Mass

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50
Q
  • Inorganic compounds
  • A chemical compound always contains exactly the same proportion of elements by mass
A

Law of Definite Proportions/Proust’s Law

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51
Q
  • Organic compounds
  • When chemical elements combine, they do so in a ratio of small whole numbers
A

Law of Multiple Proportion

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52
Q

No two electrons can have the same set of 4 quantum numbers.

Each atomic orbital can only accommodate 2 electrons (Ex: 1s2)

A

Pauli’s Exclusion Principle

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53
Q

Impossible to determine simultaneously the e- momentum & position

A

Heisenberg’s Uncertainty Principle

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54
Q

Lower energy levels are filled up first

A

Aufbau Building Up Principle

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55
Q

Orbitals are filled up singly before pairing up

A

Hund’s Rule of Maximun Multiplicity

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56
Q

He recognized Hydrogen as an element

First true periodic table

A

Antoine-Laurent Lavoisier

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57
Q

He discovered Triads (Li, Na, K | Ba, Ca, Sr | S, Se, Te | Cl, Br, I)

A

Johann Dobereiner

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58
Q

Octaves

A

John Newlands

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59
Q

Physical and chemical properties are periodic functions of their atomic weights

A

Meyer and Mendeleev

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60
Q

Elements are arranged based on atomic numbers (present)

A

Henry Mosley

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61
Q

It explains phases of matter based on movement (exclu. direction) of molecules/ions/atoms

A

Kinematic Molecular Theory

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62
Q
  • definite shape and size, definite volume
A

SOLID

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63
Q
  • follows the shape of container, definite volume
A

LIQUID

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64
Q
  • indefinite shape and volume
A

GAS

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65
Q

homogenous mixture single phase system of two of more substances

A

Solutions

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66
Q

maximum amount of solute

A

Saturated Solution

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67
Q

less solute

A

Unsaturated Solution

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68
Q

more solute than the solvent can dissolve

A

Supersaturated Solution

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69
Q

maximum amount of solute expressed in grams that can be dissolved in 100 g of water

A

Solubility

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70
Q

ability of one substance to mix with another substance

A

Miscibility

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71
Q

solubility decreases with increase in temp (Mg citrate)

A

Exothermic

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72
Q

solubility increases with increase in temp

A

Endothermic

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73
Q

↑ temperature = ↓ solubility of a gas

A
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74
Q

the solubility of a gas increases as pressure increases

A

Henry’s Law

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75
Q

Decreased particle size = Increased surface area = Increased solubility

A
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76
Q

presence of salt decreases solubility

A

Salting Out

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77
Q

presence of salt increases solubility

A

Salting In

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78
Q

force of attraction within molecules

A

Intramolecular Forces

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79
Q

Ex of Intra Forces

A

Covalent Bond - sharing
- polar (unequal)
- nonpolar (equal)
Ionic Bond - transfer

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80
Q

forces of attraction between molecules; physical attraction

A

Intermolecular Forces

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81
Q

mass per unit volume (M/V)

A

Density

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82
Q

density of sample/density of standard

A

Specific Gravity

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83
Q

reciprocal of specific gravity, opposite of density

A

Specific Volume

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84
Q

property of solution depend on the number of solute particles dissolved in a solvent

A

Colligative Property

85
Q

movement of water across a semipermeable membrane from low to high concentration

A

Osmosis

86
Q

causes crenation

A

Hypertonic

87
Q

causes swelling/lysis

A

Hypotonic

88
Q

0.9% (w/v) NaCl

A

Isotonic

89
Q

gradual mixing of molecules of one gas with molecules of another gas by virtue of kinetic properties

A

Diffusion

90
Q

passage of a gas under pressure through a small opening

A

effusion

91
Q

Acid yields H and H2O
Base yields OH

A

Arrhenius Theory

92
Q

Acid - proton donor
Base - proton acceptor

A

Bronsted-Lowry Theory

93
Q

Acid - E acceptor
Base - E donor

A

Lewis Theory

94
Q

progressive addition of a sol’n of known concentration to a substance of unknown conc

A

Titration

95
Q

Substance that changes color at the end point

A

Indicator

96
Q

point when equal amounts of acid and base have reacted; non-observable

A

Neutralization point (Stoichiometric point/Equivalence Point/Theoretical Point)

97
Q

Experimental approximate of neutralization point; observable

A

Endpoint

98
Q

the negative logarithm of the H+ concentration

A

pH

99
Q

Sorensen’s pH scale
Neutral = 7
Acidic < 7
Basic > 7

A
100
Q

Solutions that have the property of resisting changes in pH when acids or bases are added to them

A

Buffers

101
Q

 Ability of a buffer solution to resist changes in pH

A

Buffer Capacity (Buffer action/Buffer efficiency/Buffer index/Buffer value)

102
Q

an energy transfer due to temperature difference

A

Heat (q)

103
Q

form of energy transfer between a system and its surroundings in the form of compression or expansion of gas

A

Work

104
Q

total energy attributed to the particles of matter and their interactions within a system, composed of thermal energy and chemical energy

A

Internal Energy (U)

105
Q

degree of disorderliness

A

entropy

106
Q

energy of a reaction

A

enthalpy

107
Q

amount of heat required to raise the temperature of an object or substance by 1 degree

A

Heat Capacity

108
Q

amount of heat required to raise the temperature of an object per gram

A

Specific Heat

109
Q

reaction wherein heat is absorbed by the system, indicated by a (+) change in enthalpy

A

Endothermic Process

110
Q

reaction wherein heat is released by the system, indicated by a (-) change in enthalpy

A

Exothermic Process

111
Q

This law states that energy cannot be created or destroyed; it can only be redistributed or changed from one form to another.

A

Law of Conservation of Energy

112
Q

 Most reactive metals
 Valence = 1

A

Group IA - Alkali Metals

113
Q

Lightest and most reactive element

A

Hydrogen (Inflammable air)

114
Q

Isotopes of Hydrogen

A

Protium
Deuterium
Tritium

115
Q

o Lightest metal
o Depressant and Diuretic (SE: hyponatremia)

A

Lithium (Earth)

116
Q

Depressant

A

Lithium bromide

117
Q

DOC for Mania

A

Lithium Carbonate (Lithase®, Eskalith®)

118
Q

o Primary extracellular fluid cation
o Action: fluid retention

A

Sodium (Natrium)

119
Q

o Most abundant and predominant intracellular cation
o Deficiency: hypokalemia
o Manifestation: muscle paralysis (Barker’s syndrome)
o Diuretic, Important in muscle contraction

A

Potassium (Kalium)

120
Q

Never employed in medicine because it is the most toxic metal

A

Beryllium

121
Q

o Lightest of all structurally important metal
o 2nd most abundant intracellular cation

A

Magnesium

122
Q

Most malleable and ductile, Best conductor of electricity

A

Gold

123
Q

o Only reddish metal, 3rd most malleable, 3rd best conductor
o Protein precipitant, Enhances physiological utilization of iron

A

COPPER (Cuprum)

124
Q

Catalyst in polymerization of resin forming material

A

Cesium

125
Q

Hypothetical alkali metal

A

Ammonia

126
Q

contains 10% NH4; is known as 16° ammonia

A

Household ammonia

127
Q

o 2nd most abundant cation in extracellular fluid
o Vit. D is needed for its maximum absorption

A

Calcium

128
Q

Temperature desensitizing agent (Sensodyne®)

A

SrCl2

129
Q

Radioactive element used for cancer radiotherapy & diagnostic purpose

A

Radium

130
Q

o Present in inZulin and carbonic anhydraZe
o Parakeratosis

A

Zinc

131
Q

Astringent, manufacture of stink bomb

A

Cadmium

132
Q

It is used as anti sebborheic

A

CdS

133
Q

Industrial use: In vulcanizing rubber

A

Boron

134
Q

o Most abundant metal

o 3rd most abundant element

A

Aluminum

135
Q

o Pcol use: treatment of cancer-related hypercalcemia by binding with transferring

o Nonpharma: substitute for mercury in manufacture of arc lamps; Galvanized iron

A

Gallium

136
Q

Crystalline form of Carbon

A

Diamond (purest native form)
Graphite (lead pencil)

137
Q

Amorphous form of Carbon

A

Coal
Anthracite

138
Q

2nd most abundant element, Component of glass

A

Silicon

139
Q

Powerful reducing agent

A

Titanium

140
Q

Opacifying agent (Ocusert®) and UV ray protectant

A

TiO2

141
Q

antiperspirant but banned due to granuloma formation

A

Zirconium

142
Q

Most abundant gas in air

A

Nitrogen 71%

143
Q

White/yellow (poisonous), Red (non-poisonous)

A

Phosphorus

144
Q

o Protoplasmic poison
o Insecticide: Copper Aceto Arsenate (Paris green)

A

Arsenic

145
Q

First anti-syphilis (Paul Ehrlich)

A

Salvarsan/Magic Bullet/Compound 606/Arsphenamine

146
Q

Astringent, Antiseptic, Internal protective for ulcer, Used in silvering of mirror

A

Bismuth

147
Q

Not affected by any body fluid, Sheet form used in repair of bones, nerve and tissue

A

Tantalum

148
Q

Most abundant element, discovered by Scheele

A

Oxygen

149
Q

Antifungal, Parasiticide, Scabicide, Depilatory agent

A

Sulfur

150
Q

Promotes Vit. E absorption, Antioxidant (SeS2 /Selsun blue – anti-dandruff)

A

Selenium

151
Q

Becquerel, Atomic bombs

A

Uranium

152
Q

Co-factor enzyme

A

Molybdenum

153
Q

Strongest oxidizing agent

A

Fluorine

154
Q

o Most abundant extracellular anion, green gas

o Used as water disinfectant

A

Chlorine

155
Q

Used as bleaching agent

A

Hyporchlorite

156
Q

Used in treatment of achlorydria

A

HCl

157
Q

Dark reddish brown fuming liquid with suffocating odor

A

Bromine

158
Q

o Oldest known germicide
o Expectorant, Antifungal
o Preparation of T3 and T4
o Deficiency: Goiter

A

Iodine

159
Q

o Only metallic
o Only synthetic halogen
o Only radioactive halogen

A

Astatine

160
Q

o 1st element produced artificially
o Used in preparation of radiopharmaceuticals

A

Technecium

161
Q

o 2nd lightest gas
o Donald-duck-like sound

A

Helium

162
Q

o Least abundant of all noble gases
o Have inhalational anesthetic activity

A

Krypton

163
Q

Most abundant noble gas

A

Argon

164
Q

o Synthetic noble gas
o Used for treatment of CA (cervical CA)

A

Radon

165
Q

electron carrier in respiration chain; responsible for transport of molecular oxygen

A

iron

166
Q

alkaline bases used to neutralize the excess gastric HCl associated with gastritis and peptic ulcers

A

antacids

167
Q

persistent golden yellow in flame test

A

Sodium

168
Q

violet in flame test

A

Potassium

169
Q

Carmine red/Pink in flame test

A

Lithium

170
Q

Brick red in flame test

A

Calcium

171
Q

Blue in flame test

A

Pb, As, Sb, Bi, Cu

172
Q

Colorless in flame test

A

Ammonium

173
Q

branch of chemistry that deals with carbon-containing compounds with: H, O, P, N, S, X

A

Organic Chemistry

174
Q

 Contains 4 binding sites for other atoms to attach to it
 These four binding sites, when bonded with other atoms/molecules form a tetrahedron

A

Carbon

175
Q

deals with the physicochemical properties of drugs that affect its biological action

A

ORGANIC MEDICINAL CHEMISTRY

176
Q

introduced phenol (carbolic acid)

A

Joseph Lister

177
Q

Who discovered Salvarsan (compound 606), Selective toxicity

A

Paul Ehrlich

178
Q

for sleeping sickness

A

Atoxyl

179
Q

anti-infective agents that are used locally

A

germicides

180
Q

Fe + S -> FeS (all sulfides are BLACK)

A

Direct Union

181
Q

Na2CO3 -> Na2O + CO2

A

Decomposition/Analysis

182
Q

Na + HCl -> NaCl + H2

A

Single Replacement

183
Q

NaCl + AgNO3 -> NaNO3 + AgCl

A

Double Displacement

184
Q

Constant in Boyle’s/Mariotte Law

A

Temperature

185
Q

Constant in Charles Law

A

Pressure

186
Q

Constant in Gay-Lussac’s Law

A

Volume

187
Q

Constant in Avogadro’s Law

A

6.022 x 10^23

188
Q

Most systematic nomenclature

A

IUPAC

189
Q

Carbon valence

A

4

190
Q

Carbon Atomic Number

A

6

191
Q

It contains added methanol (wood alcohol) and benzene

A

Denatured Alcohol

192
Q

Astringent, rubefacient, refrigerant, mild local anesthetic

A

Rubbing Alcohol (70%)

193
Q

nlt 99% ethanol; obtained by azeotropic distillation

A

Dehydrated/Absolute Alcohol

194
Q

Rapidly bactericidal (50% to 95%), 40% equal antiseptic power to a 60% ethanol

A

Isopropyl Alcohol

195
Q

Used to sterilize temp-sensitive medical equipment and those that could not be autoclaved

A

Ethylene Oxide

196
Q

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

A

Phenol coefficient

197
Q

Introduced as surgical antiseptic by Joseph Lister; its use is now obsolete

A

Phenol

198
Q

Phenol with 10% water

A

Liquefied Phenol

199
Q

2% (shampoo), for athlete’s foot and jock itch

A

p-chloro-m-xylenol

200
Q

mixture of three isomeric methylphenols; obtained from coal tar or petroleum

A

Cresol

201
Q

Preservative more effective against molds

A

Methylparaben

202
Q

Preservative more effective against yeast, more oil soluble so it is preffered for oils and fats

A

Propylparaben

203
Q

common in vials of injectables with 1%to 4% concentrations in water or saline

A

Benzyl alcohol

204
Q

preservatives in foods and pharmaceuticals at low pH

A

Benzoic acid

205
Q

DOC for scabies; from Peru balsam and other resins

A

Benzyl benzoate

206
Q

Beta-lactam Antibiotics

A

Penicillin
Beta-lactamase Inhibitors
Cephalosporins
Carbapenem
Monobactam

207
Q

Binds to 30s

A

Aminoglycosides
Tetracyclines

208
Q

Binds to 50s

A

Macrolides
Lincosamides
Chloramphenicol

SEM 1 (8 decks)

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