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Day 1 > Black Notes > Flashcards

Black Notes Flashcards

1
Q

Give the Hardness Acceptability level

A

Soft(<50mg/L as CaCO3)
Moderately hard (50-150 mg/l as CaCO3)
Hard(150-300mg/L as CaCO3)
Very hard (>300mg/L as CaCO3)

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2
Q

Give the formula for unseede dilution of BOD5

A

BOD5=(DOi-DOf)/P

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3
Q

BOD5 for seeded dilution

A

BOD5=((Doi-Dof)-(Bi-Bf)(f))/P

P=Volume of wastewater/300ml
f=(1-p)

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4
Q

Elements are composed of tiny indivisible particles called atoms

A

John Dalton

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5
Q

Law of conservation of mass

A

Antoine Lavoiser

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6
Q

States that a pure compound is made up of elements in the same proportion by mass

A

Law of definite Proportion by Joseph Louis Proust

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7
Q

Who discover Cathode Ray Tube or Geissler Tube

A

Sir William Crookes and Heinrich Geissler)

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8
Q

Determined the ratio of electric charge to the mass of an electron to be -1.76x10^8 coul/gram

A

Joseph John Thomson

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9
Q

Determined the charge of an electron to be -1.60x10^-19 coul

A

Robert Andrews Milikan

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10
Q

Discovered the X-rays, which penetrated matter, darkened unexposed photographic plates and caused metals to emit unusual rays

A

Wilhelm Konrad Rontgen

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11
Q

Discovered Radioactivity in uranium

A

Antoine Henri Becquerel

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12
Q

Discovered Radioactivity in uranium and Polonium

A

Marya Skolodowska Curie

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13
Q

He made the following generalizations:
1. Most of the atom is an empty space
2.The positive charge of an atom is concentrated in the nucleus

A

Ernest Rutherford

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14
Q

The positively charged particle in the nucleus is the

A

Proton

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15
Q

Discovered neutron by bombarding a beryllium atom with alpha particles producing an electrically neutral particle having a mass slightly greater than that of a proton

A

James Chadwick

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16
Q

The number of protons in the nucleus of an atom

A

Atomic number

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17
Q

The total number of protons and neutrons in the nucleus of an atom

A

Mass number

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18
Q

Are atoms that have the same atomic number but different mass number

A

Isotopes

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19
Q

The weighted average of the atomic masses of the isotopes based on their percentage abundance

A

Average atomic mass

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20
Q

Give the 4 quantum numbers

A
  1. Principal quantum number (n)
  2. Azimuthal/Angular Momentum Quantum Number (l)
  3. Magnetic Quantum Number (ml)
  4. Spin Quantum Number (ms)
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21
Q

Pertains to the average distance of the electron from the nucleus in a particular orbital. It has integral values 1, 2 etc.

A

Principal quantum number (n)

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22
Q

Tells the shape of the orbital. It has a value from to n-1

A

Azimuthal/Angular Momentum Quantum Number

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23
Q

Describe the orientation of orbitals in space. Its allowable values are -l to 0 +l

A

Magnetic Quantum Number

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24
Q

Shows the spin of electrons It’s values are +1/2 (clockwise) and -1/2(counter clockwise)

A

Spin Quantum Number

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25
Q

The orbitals of an atom must be filled up in increasing energy levels

A

Aufbau Principle

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26
Q

No two electrons in an atom can have the same set of quantum numbers and an atomic orbital must contain a maximum of two electrons with opposite spins

A

Pauli’s Exclusion Principle by Wolfgang Pauli

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27
Q

The most stable arrangement of electrons in subshells is the one with more parallel spins

A

Hund’s Rule of Multiplicity

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28
Q

German chemist, arranged the elements in triads like Li-Na-K, Ca-Sr-Ba, and Cl-Br-I

A

Johann Wolfgang Dobreiner

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29
Q

English chemist, arranged the elements in atomic mass and found out that every eight element has similar properties

A

John Ar Newlands

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30
Q

A Russian chemist and German chemist arranged the elements in the periodic table according to their recurring periodic properties

A

Dmitri Ivanovich Mendeleev and Julius Lothar Meyer

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31
Q

A young English physicist, discovered the relationship between the elements atomic number and the frequency of X-rays generated by bombarding the element with high energy electrons

A

Henry Gwyn-Jeffreys Mosely

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32
Q

The properties of the elements are functions of their atomic number

A

Modern periodic law

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33
Q

The average distance between the nucleus and the valence electrons

A

Atomic size (atomic radius)

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34
Q

The energy required to remove an electron from a gaseous atom in it’s ground state.

A

Ionization Energy

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35
Q

The change in energy when an electron is accepted by a gaseous atom to form an anion

A

Electron Affinity

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36
Q

The measure of the ability of an atom to attract towards itself a bonding electron

A

Electronegativity

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37
Q

Results from the amount of the nucleus and the electron of two or more atoms and usually involves two non-metals

A

Covalent Bond

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38
Q

Results from the attraction of two opposite charged particles and involves a metal and non-metal

A

Ionic bond

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39
Q

Is the amount of energy involved in the formation and breaking of a bond

A

Bond energy

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40
Q

The distance between the nuclei of the atoms forming the bond

A

Bond length

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41
Q

Pertains to single bond, double bond, triple bond and those intermediate between single and double bonds.

A

Bond Order

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42
Q

The formation of a bond is due to the overlap of two atomic orbitals

A

Valence bond theory

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43
Q

A bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-binding molecular orbital

A

Molecular Orbital Theory

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44
Q

Reaction of an Acid and a base forming salt and water

A

Neutralization Reaction

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45
Q

Reaction which results in the formation of an insoluble product

A

Precipitation Reaction

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46
Q

A system in equilibrium when subjected to a stress will act in such a way to relieve the stress.

A

Le Chatelier’s Principle

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47
Q

The rate of disintegration of 1 gram of Ra

A

Curie

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48
Q

Basically a helium nucleus

A

Alpha particles

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49
Q

Basically an electron

A

Beta particle

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50
Q

Also known as high energy photon

A

Gamma ray

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51
Q

Who discovered positron

A

Carl Anderson

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52
Q

An antimatter emitted when the neutron to proton ratio is lower than the zone of stability

A

Positron

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53
Q

A proton is transformed to a neutron is also known as

A

Positron

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54
Q

Branch of chemistry that deals with compounds of carbon

A

Organic Chemistry

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55
Q

Organic compounds originated from living materials, either plants or animals. Such materials posses vital force and compounds that are extremely difficult to synthesize in the laboratory

A

Vital Force Theory

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56
Q

He synthesize urea in the laboratory from the inorganic compound, ammonium cyanate

A

Friedrich Wohler

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57
Q

Component of urine, and thereby ending the concept of vitalism

A

Urea

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58
Q

Atoms in an organic compound have fixed number of bonds. This combining ability is termed as

A

Valence

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59
Q

Carbon can form bonds with another carbon atom accounting for high percentage of carbon in most organic compounds. This ability of carbon is called

A

Catenation

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60
Q

Atoms are being held by electrical attraction between species of opposite charge

A

Dualism (Berzelius)

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61
Q

Atoms with high ionization energy tend to lose electrons easily while atoms with low electron affinity tend to gain electrons easily

A

Ionic bond

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62
Q

A molecule or an ion represented in two or more Lewis structures that differ only in the positions of electrons exhibit the property of resonance.

A

Resonance Theory

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63
Q

Compounds containing carbon and hydrogen

A

Hydrocarbons

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64
Q

Compounds whose carbon atoms are arranged in chains whether straight or branched

A

Aliphatic

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65
Q

Formula of Alkanes

A

CnH2n+2 - contains single bonds

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66
Q

Formula of Alkenes

A

CnH2n -contain double bonds

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67
Q

Formula of Alkynes

A

CnH2n-2 - contain two double bonds

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68
Q

Compounds whose carbon atoms are arranged in chains whether straight or branched

A

Aliphatic

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69
Q

Compounds containing carbon atoms in a ring system

A

Alicyclic

70
Q

Alkanes arranged in the form of a closed chain

A

Cycloalkanes (CnH2n)

71
Q

Non-conjugated Alkenes in a ring system

A

Cycloalkanes (CnH2n-2)

72
Q

Compounds containing carbon atoms with conjugated double bonds in a ring system

A

Aromatic

73
Q

Hydrocarbons with one or more hydrogen atom replaced by -OH group

A

Alcohols (R-OH) and Phenols (Ar-OH)

74
Q

Hydrocarbon derivatives with two hydrocarbon groups attached to oxygen

A

Ethers (ROR)

75
Q

Cyclic ethers in which the oxygen is included in a three-membered ring

A

Epoxides

76
Q

Hydrocarbons with one or two alkyl groups attached to C=O

A

Aldehydes (RCHO) and Ketones (RCOR)

77
Q

Hydrocarbons with the carboxyl group-COOH

A

Carboxylic Acids (RCOOH)

78
Q

Carboxylic acid derivatives with the hydrogen atom replaced by an alkyl group

A

Ester (RCOOR)

79
Q

Carboxylic acid derivatives with the hydrogen atom replaced by RC=O

A

Acid Anhydride

80
Q

Hydrocarbons with the hydrogen atom replaced by one or more halogens

A

Alkyl Halides and Aryl Halides

81
Q

Hydrocarbon derivatives with hydrogen atom replaced with-SH

A

Thiols

82
Q

Hydrocarbon derivatives with general formula R-S-S-R

A

Disulfides

83
Q

Organic derivative of NH3

A

Amine

84
Q

Carboxylic acid derivatives with hydrogen atom replaced with-NH2

A

Amides

85
Q

Also called paraffins

A

Alkanes
-saturated and sp3 hybridized carbon

86
Q

Physical state at Room Temperature of Alkanes
C1-C4
C5-C17
C18-Cn

A

Gases
Liquids
Solids

87
Q

Solubility of Alkanes

A

Practically insoluble in water due to non-polar character and inability to form hydrogen bonds while soluble in benzene, chloroform and carbon tetrachloride

88
Q

Boiling point of alkane

A

Increases as length of carbon chain increases and decreases due to branching

89
Q

Also called olefins

A

Alkenes

90
Q

This rule said that the alkene formed is the one that is more alkyl substituted

A

Saitsev’s Rule

91
Q

This rule states that “The halogen attaches to the carbon that is more alkyl substituted thus producing a higher order alkyl halide

A

Markovnikoff’s Rule

92
Q

Addition of HBR in the presence of Organic Peroxides

A

Anti-Markovnikoffs

93
Q

Also called acetylenes

A

Alkynes-sp hybridized carbon

94
Q

Compounds that are planar, cyclic follows

A

Huckel’s rule

95
Q

4n+2=π electrons, where n must be a whole number

A

Huckel’s Rule

96
Q

Vinyl benzene is also known as

A

Styrene

97
Q

Ortho, meta and para also used to denote

A

1, 2, 1,3 and 1,4

98
Q

Presence of KMNO4 will always create an

A

Acid

99
Q

Two hydroxyl groups are called

A

Glycols

100
Q

Alcohols have higher boiling points compared to ethers True or false

A

True

101
Q

Named as Alkanal

A

Aldehydes

102
Q

Aldehydes and ketones are soluble in water. True or false

A

True

103
Q

Father of chemistry

A

Antoine Lavoisier

104
Q

Branch of chemistry that deals with the separation, identification and composition of matter

A

Analytical chemistry

105
Q

Type of analysis that reveals the components of the sample

A

Qualitative Analysis (what is present)

106
Q

Type of analysis the determines the amount of components present in a sample

A

Quantitative Analysis ( how much is present)

107
Q

Deals with the measurement of the mass of a substance that is chemically related to the analyte

A

Gravimetric method

108
Q

Measures the volume of sodium necessary to react completely with the analyte

A

Volumetric method

109
Q

Measures the electromagnetic radiation produced by the analyte or it’s interactions with it

A

Spectroscopicethod

110
Q

Measures the electromagnetic radiation produced by the analyte or its interactions with it

A

Spectroscopic Method

111
Q

Measures the electrical properties of the analyte such as current, potential,resistance and amount of charge

A

Electroanalytic Method

112
Q

Solution of known concentration

A

Standard solution

113
Q

Process of determining the concentration of an unknown solution

A

Standardization

114
Q

A substance of high purity used for standardization

A

Primary Standard

115
Q

Give the constant concentration of
HCl
NaOH
H2SO4

A

12.1M
19.4 M
18M

116
Q

The analyte reacts with the standard solution directly

A

Direct Titration

117
Q

An excess standard solution is added and the excess is determined by the addition of another standard solution

A

Back Titration

118
Q

The analyte is converted to a product chemically related to it and the product of such reaction is titrated with a standard solution

A

Replacement Titration

119
Q

Reaction involving formation of ions

A

Ionization Reaction

120
Q

Determination of Organic Nitrogen

A

Kjeldahl Method

121
Q

Percentage Protein in the sample
f=cereals
f= meat products
f=dairy products

A

5.70
6.25
6.38

122
Q

The presence of hydroxide, carbonate and bicarbonate in water is also referred to as

A

Alkalinity

123
Q

It is a measure of the acid-neutralizing capacity of water

A

Alkalinity

124
Q

M-Cresol purple can also be used to detect phenolphthalein alkalinity (P) while bromocresol green or_______for the total alkalinity(T)

A

Methyl orange

125
Q

Direct method for Halides and Cyanides

A

Mohr Method
Titrant:Silver nitrate, AgNo3
Titration Reaction:Ag+Cl=>AgCl(white)
Indicator:sodium chromate, Na2CrO4

126
Q

Direct method for silver-Indirect method for halide
Titrant:KSCN
Direct Titration Reaction:Ag+SCN=>AgSCN(white)
Indirect Titration reaction:Ag+Cl=>AgCl(white)
Indicator:ferric alum

A

Volhard method

127
Q

Indicator:dichlorofluorescein, best for determination of Halides and Cyanides
Titration is carried out between pH of 4-7. Dextrin is added to prevent excessive coagulation of the AgCl precipitate

A

Fajans Method

128
Q

What do we determined using Leibig Method?

A

Cyanide

129
Q

Involves an increase in the oxidation state of an element

A

Oxidation reaction

130
Q

Involves a decrease in the oxidation state

A

Reduction reaction

131
Q

Loss of Electrons,Oxidation substance oxidized is the

A

Reducing Agent

132
Q

Gain of Electrons, Reduction, substance reduced is the

A

Oxidizing Agent

133
Q

The potential of a cell with the hydrogen electrode as the anode.

A

Electrode potential

134
Q

Differentiate Electrochemical cells and galvanic or voltaic cell

A

Electrochemical cells have two electrodes, which are immersed in an electrolyte solution. Salt bridges are used to prevent the two

135
Q

Differentiate Electrochemical cells and galvanic or voltaic cell

A

Electrochemical cells have two electrodes, which are immersed in an electrolyte solution. Salt bridges are used to prevent the two

136
Q

Differentiate Electrochemical cells and galvanic or voltaic cell

A

Electrochemical cells have two electrodes, which are immersed in an electrolyte solution. Salt bridges are used to prevent the two

137
Q

The absorption of radiant energy by matter can be described using

A

Beer’s Law.

138
Q

Branch of chemistry that deals with the study of the structures and physical properties of matter with the laws of chemical interaction and the theories governing these interactions.

A

Physical Chemistry

139
Q

A state of matter results from a mixture of neutral atoms, free electrons and charged ions, usually a fluid but due to charged particles present, it responds to and generates electromagnetic forces

A

Plasma

140
Q

Special state of matter in which atoms in a confined gas act together like a single giant particle after being cooled cryogenically to a temperature near absolute zero.

A

Bose-Einstein Condensate

141
Q

Kinetic molecular theory states that gases are considered to be composed of minute discrete particles called

A

Molecules

142
Q

It states that the absolute temperature is a quantity proportional to the average kinetic energy of all molecules in a system

A

Kinetic Molecular Theory

143
Q

(V/T)=k

A

Charles law (P)
Isobaric

144
Q

(PV)=k

A

Boyle’s (T)
Isothermal

145
Q

(P/T)=k

A

Gay-Lussac’S Law(V)
Isochoric

146
Q

Vapor density method was developed by?

A

Jean Baptiste Andre Dumas

147
Q

For an ideal gas, Z=?

A

Z=1

148
Q

At high temperature, Z is what for all pressures

A

Z>1

149
Q

___ between molecules results to reduction in the value of Z while__ between molecules results to increase in the Value of Z

A

Attraction, Repulsion

150
Q

As soon as equilibrium is established between the liquid and vapor, the pressure exerted by the vapor is known as the

A

Saturated vapor pressure

151
Q

Defined as the resistance offered by a fluid to the flow of another fluid

A

Viscosity

152
Q

True or false
-for gases,viscosity increases with increasing temperature
-at low pressures, viscosity is affected by pressure

A

-True, False(not affected)

153
Q

This law is applicable when the radius of the falling body is greater than the distance between the molecules of the fluid

A

Stoke’s Law(Falling Sphere Viscometer)

154
Q

Amount of work required to increase the surface area of a liquid by one unit of area

A

Surface tension

155
Q

Du Nouy Ring Method

The device in this method is known as___, which was developed in Rockefeller Institute for Medical Research

A

Tensiometer

156
Q

-constituent structural units are arranged in a definite geometrical configuration characteristics of the substance
-melts sharply at a constant and definite temperature

A

Crystalline

157
Q

-does not show a definite configurational arrangement
-not considered as true solids but highly supercooled liquids with very high viscosity
-melts gradually over a temperature interval

A

Amorphous

158
Q

Amount of heat evolved during crystallization or solidification per mole of substance at a given temperature and pressure

A

Heat of Crystallization

159
Q

The reverse of heat of Crystallization which is the amount of heat that must be absorbed in the transition of one mole of solid to liquid

A

Heat of Fusion

160
Q

A study dealing with the geometry, properties and structure of crystals and crystalline substances

A

Crystallography

161
Q

-Existence of substance in more than one modification
-examples include carbon exists as diamond or graphite, calcium carbonate as calcite or aragonite

A

Polymorphism

162
Q

Transformation from one form to another takes place at a temperature known as transition temperature or transition point

A

Allotropy

163
Q

State at which the net rate of all chemical reactions is zero

A

Chemical Equilibrium

164
Q

Properties that depends on the number of solute particles and the nature of the solvent

A

Colligative Properties of solutions

165
Q

Produces electricity as a result of the spontaneous reactions occuring inside it where the cathode has a higher potential than the anode

A

Galvanic cell

166
Q

Non-spontaneous reaction is driven by an external source of current. They have a common electrolyte and no salt bridge

A

Electrolytic cell

167
Q

In electrolytic cells the anode is_ and the cathode is_ while in galvanic cells the anode is_and the cathode is __

A

Electrolytic cell cells the anode is positive and the cathode is negative.

Galvanic cells the anode is negative and the cathode is positive

168
Q

A redox reaction brought about by the passage of a direct current through a solution of an electrolyte is known as

A

Electrolysis

169
Q

It states that the mass of a substance involved in the reaction at the electrode is proportional to the quality of electricity passed through the solution

A

Faraday’s Law

170
Q

Used to estimate the molar enthalpy of vaporization of liquids

A

Trouton’s Rule

171
Q

governs the temperature dependence of pressure in a two-phase, one component system

A

Clapeyron Equation(dP/dT)/(∆Hm/T∆Vm)

172
Q

Gives the relationship between pressure and temperature for a two-phase, one component system assuming that the vapor phase is ideal and the molar volume of the condensed phase is negligible compared to that of the vapor phase

A

Clausius-Clapeyron Equation (dP/P)=(∆Hvap/sub/R)(dT/T^2)

Day 1 (4 decks)

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