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Chemical Engineering Licensure Exam Oct. 2023 > General Inorganic Chemistry (Done) > Flashcards

General Inorganic Chemistry (Done) Flashcards

1
Q

Dalton’s Atomic theory states that? (5)

A
  1. Elements are composed of tiny indivisible particles called atoms.
  2. Atoms of a given element are identical in size, mass, and other properties. Atoms of different elements differ in size, mass, and other properties.
  3. Atoms cannot be subdivided, created, or destroyed.
  4. Atoms of different elements can combine in simple whole number ratios to form chemical compounds.
  5. In chemical reactions, atoms are combined, separated, or rearranged.
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2
Q

This law states that if 2 elements combine to form one compound, the ratio of the mass of an element to a fixed mass of the other element is a whole number or a simple fraction.

A

Law of Multiple Proportions

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3
Q

This law states that a chemical reaction only involves separation, combination or rearrangement of atoms.

A

Law of Conservation of Mass

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4
Q

This person pioneered the atomic theory.

A

John Dalton

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5
Q

Father of Chemistry; discovered the law of conservation of mass

A

Antoine Lavoisier

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6
Q

This law states that a pure compound is made up of elements in the same proportion by mass, regardless of its quantity or source.

A

Law of definite proportions

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7
Q

Discovered the law of definite proportions

A

Joseph Louis Proust

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8
Q

Invented the cathode ray tube

A

Sir William Crookes

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9
Q

The cathode ray tube was derived from _ by _.

A

Geissler Tube, Heinrich Geissler

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10
Q

Discovered the electron through the cathode ray tube experiment

A

Joseph John (JJ) Thomson

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11
Q

Ratio of electric charge to mass of electron

A

-1.76 x 10 ^ 8 C/g

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12
Q

_ discovered the definite charge of electron (and proton) through the _ (experiment)

A

Robert Andrews Millikan, Oil Drop Experiment

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13
Q

Definite charge of proton and electron

A

+- 1.6 x 10 ^ -19

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14
Q

Discovered x-rays

A

Wilhelm Konrad Roentgen

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15
Q

First to discovered evidence of radioactivity

A

Antoine Henri Becquerel

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16
Q

Discovered radioactivity in Uranium and Polonium and coined the term radioactivity

A

Maria Skolowdowska (Marie) Curie

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17
Q

_ discovered proton through _

A

Ernest Rutherford, gold foil experiment

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18
Q

Discoveries of Ernest Rutherford in the Gold Foil Experiment (2)

A
  1. Most of the atom is empty space.
  2. Positive charge of an atom is concentrated at the nucleus.
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19
Q

Mass of proton is _ and it is _ x mass of electron

A

1.6726 x 10 ^ 24 g

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20
Q

Discovered neutron and its mass

A

James Chadwick

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21
Q

Refers to the # of protons in the nucleus

A

Atomic number (Z)

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22
Q

Atom is _ when # of protons = # of electrons

A

Electrically neutral

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23
Q

This refers to the sum of the number of protons and neutrons

A

Mass number (A)

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24
Q

Elements of the same atomic number but different mass numbers; same number of protons but different number of neutrons

A

Isotopes

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25
Q

Molecules of the same charge or same # of electrons

A

Isoelectronic

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26
Q

Elements of different atomic number but same mass number

A

Isobar

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27
Q

Elements of the same number of neutrons but different number of protons

A

Isotone

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28
Q

Weighted average of atomic masses of isotopes based on percent abundance

A

Average atomic mass

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29
Q

What are the four quantum numbers?

A

Principal, azimuthal/angular momentum, magnetic and spin quantum number

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30
Q

This quantum number refers to the average distance of electrons from nucleus in a particular orbital; determines the size of the orbital

A

Principal quantum number (n)

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31
Q

This quantum number refers to the shape of the orbital

A

Azimuthal/angular momentum quantum number (ℓ)

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32
Q

This quantum number refers to the orientation of orbitals in space

A

Magnetic quantum number (m_ℓ)

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33
Q

This quantum number refers to the spin of the electrons

A

Spin quantum number (m_s)

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34
Q

Principal quantum number (n) has values of?

A

Natural/counting numbers or 1, 2, 3, 4, …

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35
Q

Azimuthal/angular momentum quantum number (ℓ) has values of

A

n - 1 or 0, 1, 2, 3, …

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36
Q

Magnetic quantum number (m_ℓ) has values of

A

-ℓ to ℓ or …,-3, 2, 1, 0, 1, 2, 3, …

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37
Q

Spin quantum number (m_s) has values of

A

+1/2 (CW) or -1/2 (CCW)

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38
Q

This principle states that orbitals must be filled up in increasing energy levels

A

Aufbau Principle

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39
Q

Principle that states no two electrons can have the same set of quantum numbers and an atomic orbital must contain maximum of 2 electrons with opposite spins

A

Pauli Exclusion Principle by Wolfgang Pauli

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40
Q

Arranged the elements in triads

A

Dobereiner

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41
Q

Arranged elements in atomic mass and fund that every 8th element has similar properties

A

Newlands

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42
Q

He is the father of the modern periodic table and together with _, they arranged the elements according to their recurring periodic properties and increasing atomic mass

A

Dmitri Mendeleev, Lothar Meyer

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43
Q

Discovered the relationship between element’s atomic number and frequency of x-rays generated when bombarded with high energy electrons

A

Moseley

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44
Q

Atomic property that refers to the distance between nucleus and valence electrons

A

Atomic size/radius

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45
Q

Electrons on the outermost shell

A

Valence electron

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46
Q

Electrons closer to the nucleus and have no participating in chemical bonding

A

Core electrons

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47
Q

Atomic property that refers to the energy required to remove an electron from a gaseous atom in its ground (lowest energy) state

A

Ionization energy

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48
Q

Atomic property that refers to the change in energy when an electron is accepted by a gaseous atom to form an anion

A

Electron affinity

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49
Q

Atomic property that refers to the measure of ability of atom to attract towards itself a bonding electron

A

Electronegativity

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50
Q

Atomic property that refers to the actual charge plus the repulsive effect due to shielding approximated by the difference between atomic number and the number of shielding/core electrons

A

Effective nuclear charge

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51
Q

True or False: Valence electrons shield core electrons better than core electrons shield each other.

A

False. Core electrons shield valence electrons better than valence electrons shield each other.

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52
Q

Atomic properties that decrease from left to right (or across the periodic table) and increase from top to bottom (or down the group)

A

Atomic size, metallic property, reactivity

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53
Q

Atomic properties that increase from left to right (or across the periodic table) and decrease from top to bottom (or down the group)

A

Ionization energy, electron affinity, electronegativity

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54
Q

Trend of effective nuclear charge

A

Increasing from left to right and top to bottom

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55
Q

Chemical bond that refers to the attraction of the nucleus and the electron of 2 or more atoms which usually occurs between 2 non-metals

A

Covalent bond

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56
Q

Chemical bond that refers to the attraction of 2 opposite charged particles (metal and non-metal)

A

Ionic bond

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57
Q

Property of chemical bond that refers to the energy released when a bond is formed

A

Bond energy

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58
Q

Property of chemical bond that refers to the distance between nuclei of the atoms forming the bond

A

Bond length

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59
Q

Property of chemical bond that refers to the number of bonding//shared pairs of electrons between two atoms

A

Bond order

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60
Q

Theory of bonding that assumes that electrons occupy atomic orbitals of the invidual atoms and states that bonds are formed due to overlap of 2 atomic orbitals.

A

Valence bond theory

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61
Q

Theory of bonding that states that electrons in the bonding molecular orbital are greater than the electrons in the non-bonding

A

Molecular orbital theory

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62
Q

This refers to chemical elements that is found naturally on Earth essentially as a single nuclide (which may, or may not, be a stable nuclide).

A

Monotopic/mononuclidic

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63
Q

How many elements are there that are monotopic?

A

21 elements (Be, F, Na, Al, P, Sc, Mn, Co, As, Y, Nb, Rh, I, Cs, Pr, Tb, Ho, Tm, Au, Bi, Pa)

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64
Q

Name this type of chemical reaction: A + B => AB

A

Combination/Synthesis

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65
Q

Name this type of chemical reaction: AB => A+B

A

Decomposition

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66
Q

Name this type of chemical reaction: AB + C => A + BC

A

Single displacement/replacement

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67
Q

Name this type of chemical reaction: AB + CD => AC + BD

A

Double displacement/decomposition

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68
Q

Combination of metal and oxygen forms

A

Basic oxide/anhydride

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69
Q

Combination of non-metal and oxygen forms

A

Acidic oxide/anhydride

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70
Q

Combination of non-metal oxide and water forms

A

Acid

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71
Q

Combination of metal oxide and water forms

A

Alkali/base

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72
Q

Decomposition of metal carbonate forms

A

Metal oxide and CO2

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73
Q

Decomposition of metal nitrates forms

A

Metal nitrites and O2

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74
Q

Decomposition of metal bicarbonate forms

A

Metal bicarbonate, water and CO2

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75
Q

Decomposition of oxyhalides form

A

Metal halides and oxygen

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76
Q

Activity series of halogens

A

F2 > Cl2 > Br2 > I2

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77
Q

Property that depends on the ratio of solute to solvent

A

Colligative properties

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78
Q

What are the four colligative properties?

A

Boiling point elevation
Freezing point depression
Vapor pressure lowering
Osmotic Pressure

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79
Q

Formula of boiling point elevation?

A

T_B,solution - T_B,solvent =K_b (m)
where T_B refers to boiling point temperature, K_b refers to the ebulliouscopic constant and m refers to the molality

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80
Q

Formula of freezing point depression

A

T_F,solution - T_F,solvent =K_F (m)
where T_F refers to freezing point temperature, K_F refers to the cryoscopic constant and m refers to the molality

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81
Q

Formula of vapor pressure lowering/Raoult’s law

A

P_solvent,initial - P_solution = X_solute P_solvent,initial
where P refers to the pressure and X refers to the mole fraction

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82
Q

Formula of osmotic pressure (π)

A

π = MRT
where M is molarity, R is the ideal gas constant and T is the temperature in [K]

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83
Q

Molality is approximately the same as molarity IF _.

A

Solution is diluted.

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84
Q

Solutions of the same osmotic pressure (equal concentration) are considered to be _.

A

Isotonic

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85
Q

What are the ebullioscopic and cryoscopic constants of water?

A

Ebullioscopic - 0.52
Cryoscopic - 1.86

86
Q

Relation between equilibrium constants Kp and Kc

A

Kp = Kc (RT) ^(Δn)

where n is the change in moles of gaseous products and reactants

87
Q

This principle states that a system in equilibrium when subjected to a stress will act in such a way to relieve the stress (or shift back to equilibrium).

A

Le Chatelier’s Principle

88
Q

Increase in concentration of reactant results in

A

Forward reaction

89
Q

Increase in concentration of product results in

A

Backward reaction

90
Q

Increasing the pressure of the reaction results in

A

Shifting towards less gaseous molecules

91
Q

Increasing the temperature when the reaction is endothermic results in

A

Forward reaction

92
Q

Increasing the temperature when the reaction is exothermic results in

A

Backward reaction

93
Q

Increasing the catalyst results in

A

No change in equilibrium

94
Q

True or false: Catalyst affects the rate of reaction but not the equilibrium of the reaction.

A

True

95
Q

SI unit of activity

A

Becquerel

96
Q

The unit Curie refers to _.

A

Rate of disintegration of 1 g of Ra

97
Q

SI unit of radiation absorbed dose

A

Gray

98
Q

Effect of beta particle on (a) mass number (b) atomic number

A

(a) no effect
(b) decrease by 1

99
Q

Effect of positron on (a) mass number (b) atomic number

A

(a) no effect
(b) increase by 1

100
Q

Effect of proton or a H nucleus on (a) mass number (b) atomic number

A

(a) and (b) increase by 1

101
Q

Effect of neutron on (a) mass number (b) atomic number

A

(a) increase by 1
(b) no effect

102
Q

Effect of gamma ray on (a) mass number (b) atomic number

A

None

103
Q

Effect of alpha particle or He nucleus on (a) mass number (b) atomic number

A

(a) increase by 4
(b) increase by 2

104
Q

Nuclear reactions are balanced by:

A
  1. Conservation of mass #
  2. Conversation of atomic #
105
Q

Alpha particle is essentially

A

He nucleus

106
Q

Beta particle is essentially

A

Electron

107
Q

Beta particle is emitted when _.

A

n/p is higher than the zone of stability

108
Q

It is a by product of alpha particle decay and it is a high energy proton

A

Gamma ray

109
Q

It is the antimatter of electron emitted when n/p is less than zone of stability

A

Positron

110
Q

Inner orbital is captured by the nucleus to increase n/p

A

Electron capture

111
Q

This is the force of attraction between nucleons over a distance (~ 1 x 10 ^ (-15) m) which overcomes the electromagnetic forces over short distances

A

Strong nuclear force

112
Q

What does nucleon refer to?

A

Proton and neutrons

113
Q

Value of n/p of stable nuclide

A

1

114
Q

Value of n/p of unstable nuclides

A

> 1

115
Q

Magic numbers of number of protons or neutrons

A

2, 8, 20, 50, 82, 126

116
Q

This refers to the loss of mass that shows up as amount of energy released during nuclear transformation

A

Nuclear binding energy (change in E) = (change in mass) x (speed of light)^2

117
Q

This refers to the change in mass during a nuclear transformation and it is computed through:

A

Mass defect (Δm) is computed by taking the difference between the mass of the products and the mass of the reactants.

118
Q

True or false: a lower binding energy per nucleon implies more mass is converted to pure energy to bind the nucleons, hence indicating that the nuclei is more stable.

A

False. A /higher/ binding energy per nucleon implies more mass is converted to pure energy to bind the nucleons, hence indicating that the nuclei is more stable.

119
Q

Coined “atomism”

A

Leucippus and Democritus

120
Q

Coined atomos

A

Democritus

121
Q

Proposed the law of multiple proportions

A

John Dalton

122
Q

Region in space where an electron is most likely to be found is called

A

Orbital

123
Q

Substances with unpaired electrons are called

A

Paramagnetic

124
Q

Substances with paired electrons are called

A

Diamagnetic

125
Q

Quantum Theory is proposed by _

A

Max Planck

126
Q

Quantum Theory states that

A

“When solids are heated, they emit electromagnetic radiation over a wide range of wavelengths.”

127
Q

True or false: the amount of radiant energy emitted by an object at a certain temperature depends on its wavelength.

A

True

128
Q

Max Planch assumed that atoms and molecules could emit or absorb energy in discrete quantities called _

A

quanta/quantum

129
Q

Proposed the photoelectric effect

A

Albert Einstein

130
Q

Albert Einstein proposed the _

A

Photoelectric effect

131
Q

_ explains that electrons are ejected from the surface of certain metals exposed to a light of at least a certain minimum frequency called _.

A

Photoelectric effect, threshold frequency

132
Q

Albert Einstein suggested that a beam of light is really a stream of particles called _

A

Photons

133
Q

Dual nature of light states that

A

Light is both a particle and a wave

134
Q

True or false: Photons cannot knock off electrons from surfaces of metals.

A

False. Photons can knock off electrons from surfaces of metals provided they have sufficient energy, i.e. energy is greater than the energy that binds the electrons to the metal (arising from attractive forces).

135
Q

Force binding the electron to the metal is called _

A

Work function

136
Q

Excess energy when electron is removed from the metal is converted into _ of the electrons that broke free.

A

Kinetic energy

137
Q

Emission spectra of atoms is attributed to

A

Bohr

138
Q

Bohr is attributed to

A

The emission spectra of atoms

139
Q

Emission spectra are shown either as _ or _.

A

Continuous spectra or line spectra of radiation emitted by substances.

140
Q

True or false: The emission spectra of atoms in the gas phase show a continuous spread of wavelength in the visible region.

A

False. It is not continuous.

141
Q

Hydrogen spectral series that starts with the first orbital

A

Lyman: UV

142
Q

Hydrogen spectral series that starts with the second orbital

A

Balmer: UV-Vis

143
Q

Hydrogen spectral series that starts with the third orbital

A

Paschen: IR

144
Q

Hydrogen spectral series that starts with the fourth orbital

A

Brackett

145
Q

Describes the distribution of electrons in hydrogen and other atoms (address)

A

Quantum numbers

146
Q

The Quantum numbers were derived from the mathematical solution of the _ for the hydrogen atom

A

Schrodinger equation

147
Q

These are the wave functions of electrons in an atom; solutions to the Schrodinger equation

A

Atomic orbitals

148
Q

This states that the square of the wave function determines the probability distribution of an electron in space.

A

Born interpretation

149
Q

This principle states that the most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins

A

Hund’s Rule of Maximum Multiplicity

150
Q

How to compute for an estimate of the effective nuclear charge?

A

{# of protons} - {# of electrons inside}

151
Q

_ devised a method for calculating relative electronegativities of most elements.

A

Linus Pauling

152
Q

Representation of covalent bonding in which shared electron pairs are shown either as lines or pairs of dots between two atoms and lone pairs are shown as pairs of dots on individual atoms

A

Lewis Structure

153
Q

True or false: Both core and valence electrons are shown in Lewis structures.

A

False. Only valence electrons are shown in Lewis structures.

154
Q

An atom other than hydrogen tneds to form bonds until it is surrounded by _ valence electrons and this is described by the _.

A

eight, octet rule

155
Q

Fajan’s rule states that:

A
  1. Small positive ion favors covalency.
  2. Large negative ion favors covalency.
  3. Large changers on either ion or on both ions favor covalency.
  4. If the positive ion does not have a noble gas configuration, polarization/covalency is favored.
156
Q

This has lower energy, which means greater stability than the atomic orbitals from which it was formed.

A

Bonding molecular orbital

157
Q

This has higher energy, which means lower stability than the atomic orbitals from which it was formed.

A

Antibonding molecular orbital

158
Q

This accounts for the geometric arrangements of electron pairs around a central atom in terms of the electrostatic repulsion between electron pair.

A

Valance-shell electron repulsion (VSEPR) model

159
Q

Arrange in terms of strength: LP-BP repulsion, BP-BP repulsion, LP-LP repulsion (LP = lone pair, BP = bonding pair)

A

LP-LP > LP-BP > BP-BP

160
Q

It is a quantitative measure of the polarity of a bond

A

Dipole moment

161
Q

These are diatomic molecules containing atoms of different elements that have dipole moments

A

Polar molecules

162
Q

These are diatomic molecules containing atoms of the same element that do not have dipole moments

A

Nonpolar molecules

163
Q

Colligative properties talk about solutions that are _, with concentrations that are _.

A

(relatively) dilute, <0.2 M

164
Q

Due to _, the vapor pressure of the solution of a nonvolatile solute is always _ than that of the pure solvent.

A

Vapor pressure lowering, less

165
Q

Temperature at which the vapor pressure of a liquid is equal to the external atmospheric pressure.

A

Boiling point

166
Q

Presence of a non-volatile solute _ the boiling point.

A

increases/elevates

167
Q

A solution with nonvolatile solute has a _ boiling point than that of the pure solvent.

A

Higher

168
Q

A solution with non-volatile solute has a _ freezing point that than of the pure solvent.

A

Lower

169
Q

Selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated on.

A

Osmosis

170
Q

This is the pressure required to stop osmosis

A

Osmotic Pressure

171
Q

If two solutions have unequal osmotic pressures, the more concentrated solution is called

A

Hypertonic

172
Q

If two solutions have unequal osmotic pressures, the less concentrated solution is called

A

Hypotonic

173
Q

True or false: The total number of solute particles determine the colligative properties of a solution

A

True

174
Q

This refers to the ratio of actual number of particles in a solution after disassociation and the number of formula units initially dissolve in solution

A

Van’t Hoff factor (i)

175
Q

Van’t Hoff factor has a value of _ for organics and non-electrolytic solutions

A

1

176
Q

True or false: the colligative properties of electrolyte solutions are usually larger than anticipated.

A

False. Colligative properties are usually smaller than anticipated due to the formation of ion pairs at higher concentrations.

177
Q

Formula for degree of disassociation (α)

A

α = (i-1)/(v-1)

where v is the maximum number of particles and i is the van’t Hoff factor

178
Q

Instead of the equilibrium constant, the _ is obtained when the reaction has not reached equilibrium.

A

Reaction quotient (Qc)

179
Q

Direction of reaction when Qc < Kc

A

Forward

180
Q

Direction of reaction when Qc > Kc

A

Backward

181
Q

Direction of reaction when there is addition of inert gas at constant pressure

A

Towards the most mole of gas

182
Q

Direction of reaction when there is addition of inert gas at constant volume

A

No change in direction

183
Q

Equilibrium between the same substance of different phases

A

Physical equilibrium

184
Q

Equilibrium between different substances of similar phases

A

Homogeneous equilibrium

185
Q

State where rate of forward reaction = rate of backward reaction

A

Chemical equilibrium

186
Q

Equilibrium between different substances of different phases

A

Heterogeneous equilibrium

187
Q

This is the study of reactions involving changes in atomic nuclei

A

Nuclear chemistry

188
Q

Spontaneous emission of particles and/or radition

A

Radioactivity

189
Q

Any element that spontaneously emits radiation is said to be

A

Radioactive

190
Q

Three types of rays produced by radioactive decay

A

Alpha, beta and gamma rays

191
Q

True or false: Neutrons can be accelerated in a particle accelerator.

A

False

192
Q

Densest element

A

Osmium

193
Q

The nucleus disintegrates and emits particles and/or radition when _.

A

repulsion > attraction

194
Q

The nucleus is stable when

A

Repulsion < attraction

195
Q

This is the principal factor that determines the stability of nucleus.

A

Neutron to proton ratio (n/p)

196
Q

n/p value becomes _ than 1 as atomic number increases

A

greater (since more neutrons are needed to counteract the stronger coulombic repulsion from protons)

197
Q

All isotopes of the elements with atomic numbers greater than _, as well as the elements _ and _ are radioactive.

A

83, technetium, promethium

198
Q

Stable nuclei are located within the _

A

Belt of stability

199
Q

True or false: most radioactive nuclei liu outside the belt of stability

A

True

200
Q

Binding energies per nucleon are greatest for group _ elements

A

8B (iron, cobalt and nickel region)

201
Q

It is more meaningful to use the _ when comparing stability of any two nuclei

A

Nuclear binding energy per nucleon (due to the fact that they have different numbers of nucleons)

202
Q

Formula for binding energy per nucleon

A

B = {[# of neutrons x mass of protons] + [# of neutrons x mass of neutrons] - [mass of atom]} x 931.49 MeV

203
Q

All radioactive decay obey _ order of kinetics.

A

First

204
Q

Formula for rate of decay at time t

A

t = λN

where λ is the rate constant and N is the number of radioactive nuclei present at time t

205
Q

Formula for half-life of radioactive decay is

A

t_(1/2) = ln(2) / λ

206
Q

It is the measure of the activity of the source of radioactivity

A

Disintegration rate

207
Q

It is the measure of the energy deposited in a medium by ionizing radiation. It is used in the calculation of dose uptake in living tissue in both radiation protection and radiology.

A

Absorbed dose.

208
Q

of proton, neutron and electron of Deuterium

A

1,1,1

209
Q

Most common radioactive trace used in SPECT?

A

Tc-99

210
Q

Most commonly used radioactive tracer in medicine?

A

Mo-99

211
Q

Radioisotope used in liver

A

Fe-59

212
Q

Radioisotope in carbon dating

A

C-14

Chemical Engineering Licensure Exam Oct. 2023 (3 decks)

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