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Physical and Chemical Principles > General Inorganic Chemistry > Flashcards

General Inorganic Chemistry Flashcards

1
Q

Elements are composed of tiny indivisible particles called

A

Atoms

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2
Q

Atoms of different elements are —

different; however, atoms of a given element are of the same size, —, — and chemical properties

A

Chemically
Shape
Mass

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3
Q

A chemical reaction only involves —, —, or — of atoms

A

Separation
Combination
Rearrangement

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4
Q

He said that elements are composed of tiny indivisible particles called atoms.

A

John Dalton

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5
Q

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

A

Law of Definite Proportions

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6
Q

The Law of Definite Proportions is stated by

A

Joseph Louis Proust

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7
Q

The Cathode Ray Tube is also known as

A

The Geissler Tube

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8
Q

The Cathode Ray Tube or the Geissler Tube experiment is developed by

A

Sir William Crookes

Heinrich Geissler

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9
Q

It is a glass tube with two metal plates connected to a high-voltage source which emitted a ray drawn from the negative plate towards the positive plate. The ray emitted has the same nature regardless of material of construction of the glass tube, electrode and the gas used.

A

Cathode Ray Tube

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10
Q

He determined the ratio of the electric charge to the mass of an electron to be -1.76x10^8 coulomb/gram

A

Joseph John Thompson

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11
Q

He determined the charge of an electron to be -1.60x10^-19 coulomb

A

Robert Andrews Millikan

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12
Q

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

A

Wilhelm Konrad Roentgen

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13
Q

He d the radioactivity in Uranium

A

Antoine Henri Becquerel

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14
Q

She discovered radioactivity in uranium and polonium

A

Mary’s Slodowska Curie

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15
Q

He performed the gold foil experiment wherein a thin foil of gold was bombarded with alpha particles

A

Ernest Rutherford

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16
Q

He generalized that most of the atom is an empty space and the positive charge of an atom is concentrated in the nucleus

A

Ernest Rutherford

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17
Q

The positively charged particles in the nucleus that carried the same quantity of the charges as an electron

A

Proton

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18
Q

The mass of proton

A

1.6752x10^-24 grams

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19
Q

He discovered neutron by bombarding 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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20
Q

It is the number of portions in the nucleus of an atom. An atom is electrically neutral where the number of protons is equal to the number of electrons

A

Atomic number

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21
Q

It is the total number of protons and neutrons in the nucleus of an atom

A

Mass number

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22
Q

These are atoms that have the same atomic number but different mass number

A

Isotopes

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23
Q

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

A

Average atomic mass

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24
Q

(n) pertains to the average distance of the electron from the nucleus in a particular orbital

A

Principal Quantum Number

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25
Q

(l) It tells the shape of the orbital. It has values from 0 to n-1

A

Azimuthal or Angular Momentum Quantum Number

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26
Q

(ml) It describes the orientation of orbitals in space. It allowable values are -l to 0 to +l

A

Magnetic quantum number

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27
Q

It shows the spin of electrons.
+1/2 clockwise
-1/2 counter clockwise

A

Spin quantum number

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28
Q

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

A

Aufbau Principles

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29
Q

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

A

Paula’s Exclusion Principle

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30
Q

He developed the Pauli’s Exclusion Principle

A

Wolfgang Pauli

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31
Q

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

A

Hund’s Rule of Multiplicity

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32
Q

He arranged the elements in triads like LiNaKa, CaSrBa, ClBrI

A

John AR Newlands

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33
Q

They arranged the elements in the periodic table according to their recurring periodic properties

A

Dmitri Mendeleev

Julius Lothar Meyer

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34
Q

He discovered the relationship between the atomic number and the frequency of X-Rays generated by bombarding the element with high energy electrons

A

Henry Gwyn-Jeffreys Moseley

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35
Q

The properties of the elements are functions of their atomic numbers

A

Modern Periodic Law

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36
Q

It is the average distance between the nucleus and the valence electron

A

Atomic Size

Atomic Radius

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37
Q

It is the energy to removed an electron from a gaseous atom in its ground state. The lower the value, the easier for an atom to form a cation

A

Ionization a Energy

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38
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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39
Q

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

A

Electro negativity

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40
Q

It results from the attraction of the nucleus and the electron of two or more atoms and usually involves two non-metals

A

Covalent Bond

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41
Q

It results from the attraction of two opposite charged particles and involves a meta, and non-metal

A

Ionic bond

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42
Q

It is the amount of energy involved in the formation and breaking of a bond

A

Bond energy

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43
Q

It is the distance between the nuclei of the atoms forming the bond

A

Bond length

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44
Q

It pertains to single, double, and triple bonds and those intermediate between single and double bonds

A

Bond order

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45
Q

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

A

Valence Bond Theory

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46
Q

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

A

Molecular Orbital Theory

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47
Q

Metal and oxygen gas yields

A

Basic oxide or basic anhydride

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48
Q

Nonmetal and oxygen gas yields

A

Acidic oxide or acidic anhydride

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49
Q

Non-metal oxide and water yields

A

Acid

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50
Q

Metal oxide and water yields

A

Alkali or base

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51
Q

The decomposition of metal carbonates yields

A

Metal oxide and carbon dioxide

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52
Q

The decomposition of metal nitrates yields

A

Metal nitrites and oxygen

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53
Q

Metal bicarbonate decomposition yields

A

Metal carbonate, water and carbon dioxide

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54
Q

Metal oxyhalides decomposes to

A

Metal halide and oxygen gas

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55
Q

The reaction of an acid and a base forms

A

Salt and water

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56
Q

The reaction of acid and a base is also called

A

Neutralization Reaction

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57
Q

A reaction which results to the formation of an insoluble product is called a

A

Precipitation reaction

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58
Q

Cryoscopic and ebullioscopic constants of water

A
  1. 52

1. 86

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59
Q

Cryoscopic and ebullioscopic constants of benzene

A
  1. 57

5. 12

60
Q

Cryoscopic and ebullioscopic constants of acetic acid

A
  1. 07

3. 90

61
Q

Cryoscopic and ebullioscopic constants of camphor

A

-

37.7

62
Q

Cryoscopic and ebullioscopic constants of ethanol

A

1.20

-

63
Q

Cryoscopic and ebullioscopic constants of methanol

A

0.80

-

64
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

65
Q

Charge of a beta particle of electron

A

-1

66
Q

The charge of a positron

A

+1

67
Q

The charge of a proton or a hydrogen nucleus

A

+1

68
Q

The charge of a neutron

A

0

69
Q

Charge of a gamma ray

A

0

70
Q

The charge of an alpha particle or helium nucleus

A

+2

71
Q

A way of expressing quantity of radiation which the the number of nuclear dis integrations per second

A

Activity

72
Q

The SI unit for activity

A

By

73
Q

1 Ci (curie) is equal to how many Bq

A

3.7x10^10

74
Q

The rate of disintegration of 1 gram of Ra

A

Curie

75
Q

The SI Unit for the radiation absorbed dose

A

Gray (Gy)

76
Q

1 red (radiation absorbed dose) is equal to J/gram of tissue

A

10^-5

77
Q

The total number of protons plus neutrons in the products and in the reactants must be the same

A

Conservation of mass number

78
Q

The total number of nuclear charges in the products and in the reactants must be the same

A

Conservation of atomic number

79
Q

This particle is basically a helium nucleus

A

Alpha particle

80
Q

It is commonly found during radioactive decay from heavier nutlike

A

Alpha particle

81
Q

Its net result is to increase the neutron to proton ratio

A

Alpha particle

82
Q

It is basically an electron

A

Beta particle

83
Q

The symbol which represents an electron in or from an atomic orbital

A

0-1 e

84
Q

The symbol which represents an electron that, although physically identical to any other electron, comes from the nucleus and not from an atomic orbital

A

0-1 beta

85
Q

It is emitted when the neutron to proton ratio is higher that the zone of stability (a neutron is transformed to a proton and an electron)

A

Beta Particle

86
Q

It is also known apps high energy photon

A

Gamma ray

87
Q

It is usually a by product of an alpha particle decay

A

Gamma ray

88
Q

An antimatter of electron emitted when the neutron to proton ratio is lower the zone of stability (a proton is transformed to a neutron)

A

Positron

89
Q

The inner orbital electron is captured by the nucleus to increase neutron to proton ratio

A

Electron capture

90
Q

It is usually accompanied by emission of gamma ray

A

Electron capture

91
Q

A force of attraction present between nucleons (proton and neutrons) over and extreme toy short distance of about 10^-15 m

A

Strong nuclear force

92
Q

It overcomes electromagnetic forces over short distances

A

Strong nuclear force

93
Q

It serves as a nuclear binder of neighboring protons despite the electric repulsion of positive charges but only over short distances

A

Neutrons

94
Q

A smaller atomic nuclei usually have the same number of — and —

A

Protons as neutrons

95
Q

A single neutron is rather — and will convert itself to a — and a —

A

Unstable
Proton
Electron

96
Q

A process where heavier nucleus loses nucleons to yield smaller but more stable nucleus

A

Radioactive decay

97
Q

When a nuclei die has — or more protons, it tends to be unstable and undergo radioactive decay

A

84

98
Q

The amount for energy released during nuclear transformation and is a measure of the energy used to bind the nucleons in a parent nuclei die

A

Binding energy

E=mc^2

99
Q

The change in mass during a nuclear transformation

A

Mass defect

100
Q

The higher the binding energy per nucleon implies more mass in converted to — energy to bind the nucleons and hence the more stable the — is

A

Pure

Stable

101
Q

The most stable nuclei where nuclei with lesser mass number needs to break up to achieve maximum stability while those with greater mass number combine to achieve maximum stability

A

Fe-26

102
Q

The fundamental number of hydrogen

A

Balmer constant

3645.6 Angstrom

103
Q

These experiments led to the discovery of the charge of electrons

A

Oils drop experiments

104
Q

A reaction that is involved in the creation and destruction of atoms

A

Nuclear reaction

105
Q

A disturbance characterized by its wavelength, amplitude and frequency

A

Wave

106
Q

The vertical distance from the midline of wave to the peak or trough

A

Amplitude

107
Q

Number of waves that pas through a particular point in 1 second

A

Frequency

108
Q

Waves with electric and magnetic field component

A

Electromagnetic waves or electromagnetic radiation

109
Q

Waves that can propagate through vacuum

A

Electromagnetic waves or radiation

110
Q

Ejection of electrons from a metal plate when light falls on it

A

Photoelectric effect

111
Q

He developed a mathematical model explains the observed frequencies for hydrogen spectral lines

A

Johannes Balmer

112
Q

He proposed that particles could be described as a wave

A

Louis de Broigle

113
Q

Electron beams were diffracted by these crystals which proved de Broigle’s idea

A

Sodium chloride crystals

114
Q

It states that the position and the velocity of an object cannot both be measured exactly at the same time

A

Heisenberg Uncertainty Principle

115
Q

He developed a mathematical model for wave function, for particles exhibiting wave-like properties

A

Erwin schrodinger

116
Q

It can be used to describe electron’s energy and most probable location in space

A

Wave function

117
Q

It is the interaction of electron with the magnetic field

A

Spin quantum number

118
Q

It tells how the electrons are distributed among the various atomic orbitals in an atom

A

Electronic configuration

119
Q

Elements of the same number of neutrons

A

Isotone

120
Q

Elements of the same number of electrons

A

Isoelectronic elements

121
Q

Elements of the same mass number

A

Isobar

122
Q

The tendency of atoms to prefer to have eight electrons in the valence shells, making it similar to noble gas

A

Octet rule

123
Q

When there is more than one Lewis structure that can represent of molecule

A

Resonance

124
Q

Distribution of regions of high electron density around the central atom

A

Electronic geometry

125
Q

Arrangement of atoms around the central atom

A

Molecular geometry

126
Q

High electron density can be regarded as

A

Bonds or lone pairs

127
Q

Covalent compounds are also known as

A

Molecular compounds

128
Q

Acid that contain hydrogen, oxygen and other element

A

Oxoacid

129
Q

True or False

Most decomposition reactions require an input of energy in the form of heat, light or electricity

A

True

130
Q

A reaction which a substance reacts with oxygen gas, releasing energy in the form of light and heat

A

Combustion

131
Q

The rates of the forward and reverse reactions are equal

A

Chemical equilibrium

132
Q

The concentrations of the reactants and product remain constant

A

Chemical equilibrium

133
Q

True or False

The ratio of concentrations between product and reactants is constant regardless of initial concentrations

A

True

134
Q

If the equilibrium constant is greater than 1, then the equilibrium favors the

A

Product

135
Q

This equilibrium applies to reactions in which all reacting species are in the same phase

A

Homogenous equilibrium

136
Q

This type of equilibrium applies to reactions in which reactants and products are in different phases

A

Heterogeneous equilibrium

137
Q

It is calculated by substituting the initial concentrations of the reactants and products into the equilibrium constants expression

A

Reaction quotient

138
Q

A homogenous mixture consisting of a solute dissolved into a solvent

A

Solution

139
Q

This substance produces a solution that can conduct electricity when being dissolved in water

A

Electrolyte

140
Q

Substance that does not conduct electricity when dissolved in water

A

Nonelectrolyte

141
Q

Properties of solutions that depend on the number of particles dissolved in the solution

A

Colligative properties

142
Q

This law predicts lower vapor pressure, boiling temperature elevation is determined by the number of moles of solute dissolved in the solution

A

Raoult’s Law

143
Q

The selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated solution

A

Osmosis

144
Q

It allows the passage of solvent molecules but blocks the passage of solute molecules

A

Semipermeable membrane

145
Q

The pressure required to stop the osmosis

A

Osmotic pressure

146
Q

The spontaneous decay of an unstable nucleus I which a heavy nucleus of mass number greater than 89 splits into a lighter nuclei and energy is released

A

Spontaneous fission

Physical and Chemical Principles (6 decks)

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