General Inorganic Chemistry Flashcards
1
Q
Elements are composed of tiny indivisible particles called
A
Atoms
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
3
Q
A chemical reaction only involves —, —, or — of atoms
A
Separation
Combination
Rearrangement
4
Q
He said that elements are composed of tiny indivisible particles called atoms.
A
John Dalton
5
Q
It states that a pure compound is made up of elements in the same proportion by mass
A
Law of Definite Proportions
6
Q
The Law of Definite Proportions is stated by
A
Joseph Louis Proust
7
Q
The Cathode Ray Tube is also known as
A
The Geissler Tube
8
Q
The Cathode Ray Tube or the Geissler Tube experiment is developed by
A
Sir William Crookes
Heinrich Geissler
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
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
11
Q
He determined the charge of an electron to be -1.60x10^-19 coulomb
A
Robert Andrews Millikan
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
13
Q
He d the radioactivity in Uranium
A
Antoine Henri Becquerel
14
Q
She discovered radioactivity in uranium and polonium
A
Mary’s Slodowska Curie
15
Q
He performed the gold foil experiment wherein a thin foil of gold was bombarded with alpha particles
A
Ernest Rutherford
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
17
Q
The positively charged particles in the nucleus that carried the same quantity of the charges as an electron
A
Proton
18
Q
The mass of proton
A
1.6752x10^-24 grams
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
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
21
Q
It is the total number of protons and neutrons in the nucleus of an atom
A
Mass number
22
Q
These are atoms that have the same atomic number but different mass number
A
Isotopes
23
Q
The weighted average of the atomic masses of the isotopes based on their percentage abundance
A
Average atomic mass
24
Q
(n) pertains to the average distance of the electron from the nucleus in a particular orbital
A
Principal Quantum Number
25
(l) It tells the shape of the orbital. It has values from 0 to n-1
Azimuthal or Angular Momentum Quantum Number
26
(ml) It describes the orientation of orbitals in space. It allowable values are -l to 0 to +l
Magnetic quantum number
27
It shows the spin of electrons.
+1/2 clockwise
-1/2 counter clockwise
Spin quantum number
28
The orbitals of an atom must be filled up in increasing energy levels
Aufbau Principles
29
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
Paula's Exclusion Principle
30
He developed the Pauli's Exclusion Principle
Wolfgang Pauli
31
The most stable arrangement of electrons in subs hells is the one with more parallel spins
Hund's Rule of Multiplicity
32
He arranged the elements in triads like LiNaKa, CaSrBa, ClBrI
John AR Newlands
33
They arranged the elements in the periodic table according to their recurring periodic properties
Dmitri Mendeleev
| Julius Lothar Meyer
34
He discovered the relationship between the atomic number and the frequency of X-Rays generated by bombarding the element with high energy electrons
Henry Gwyn-Jeffreys Moseley
35
The properties of the elements are functions of their atomic numbers
Modern Periodic Law
36
It is the average distance between the nucleus and the valence electron
Atomic Size
| Atomic Radius
37
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
Ionization a Energy
38
The change in energy when an electron is accepted by a gaseous atom to form an anion
Electron affinity
39
It is the measure of the ability of an atom to attract towards itself a bonding electron
Electro negativity
40
It results from the attraction of the nucleus and the electron of two or more atoms and usually involves two non-metals
Covalent Bond
41
It results from the attraction of two opposite charged particles and involves a meta, and non-metal
Ionic bond
42
It is the amount of energy involved in the formation and breaking of a bond
Bond energy
43
It is the distance between the nuclei of the atoms forming the bond
Bond length
44
It pertains to single, double, and triple bonds and those intermediate between single and double bonds
Bond order
45
The formation of bond is due to the overlap of two atomic orbitals
Valence Bond Theory
46
A bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-bonding molecular orbital
Molecular Orbital Theory
47
Metal and oxygen gas yields
Basic oxide or basic anhydride
48
Nonmetal and oxygen gas yields
Acidic oxide or acidic anhydride
49
Non-metal oxide and water yields
Acid
50
Metal oxide and water yields
Alkali or base
51
The decomposition of metal carbonates yields
Metal oxide and carbon dioxide
52
The decomposition of metal nitrates yields
Metal nitrites and oxygen
53
Metal bicarbonate decomposition yields
Metal carbonate, water and carbon dioxide
54
Metal oxyhalides decomposes to
Metal halide and oxygen gas
55
The reaction of an acid and a base forms
Salt and water
56
The reaction of acid and a base is also called
Neutralization Reaction
57
A reaction which results to the formation of an insoluble product is called a
Precipitation reaction
58
Cryoscopic and ebullioscopic constants of water
0. 52
| 1. 86
59
Cryoscopic and ebullioscopic constants of benzene
2. 57
| 5. 12
60
Cryoscopic and ebullioscopic constants of acetic acid
3. 07
| 3. 90
61
Cryoscopic and ebullioscopic constants of camphor
-
| 37.7
62
Cryoscopic and ebullioscopic constants of ethanol
1.20
| -
63
Cryoscopic and ebullioscopic constants of methanol
0.80
| -
64
A system in equilibrium when subjected to a stress will act in such a way to relieve the stress
Le Chatelier's Principle
65
Charge of a beta particle of electron
-1
66
The charge of a positron
+1
67
The charge of a proton or a hydrogen nucleus
+1
68
The charge of a neutron
0
69
Charge of a gamma ray
0
70
The charge of an alpha particle or helium nucleus
+2
71
A way of expressing quantity of radiation which the the number of nuclear dis integrations per second
Activity
72
The SI unit for activity
By
73
1 Ci (curie) is equal to how many Bq
3.7x10^10
74
The rate of disintegration of 1 gram of Ra
Curie
75
The SI Unit for the radiation absorbed dose
Gray (Gy)
76
1 red (radiation absorbed dose) is equal to J/gram of tissue
10^-5
77
The total number of protons plus neutrons in the products and in the reactants must be the same
Conservation of mass number
78
The total number of nuclear charges in the products and in the reactants must be the same
Conservation of atomic number
79
This particle is basically a helium nucleus
Alpha particle
80
It is commonly found during radioactive decay from heavier nutlike
Alpha particle
81
Its net result is to increase the neutron to proton ratio
Alpha particle
82
It is basically an electron
Beta particle
83
The symbol which represents an electron in or from an atomic orbital
0-1 e
84
The symbol which represents an electron that, although physically identical to any other electron, comes from the nucleus and not from an atomic orbital
0-1 beta
85
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)
Beta Particle
86
It is also known apps high energy photon
Gamma ray
87
It is usually a by product of an alpha particle decay
Gamma ray
88
An antimatter of electron emitted when the neutron to proton ratio is lower the zone of stability (a proton is transformed to a neutron)
Positron
89
The inner orbital electron is captured by the nucleus to increase neutron to proton ratio
Electron capture
90
It is usually accompanied by emission of gamma ray
Electron capture
91
A force of attraction present between nucleons (proton and neutrons) over and extreme toy short distance of about 10^-15 m
Strong nuclear force
92
It overcomes electromagnetic forces over short distances
Strong nuclear force
93
It serves as a nuclear binder of neighboring protons despite the electric repulsion of positive charges but only over short distances
Neutrons
94
A smaller atomic nuclei usually have the same number of --- and ---
Protons as neutrons
95
A single neutron is rather --- and will convert itself to a --- and a ---
Unstable
Proton
Electron
96
A process where heavier nucleus loses nucleons to yield smaller but more stable nucleus
Radioactive decay
97
When a nuclei die has --- or more protons, it tends to be unstable and undergo radioactive decay
84
98
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
Binding energy
| E=mc^2
99
The change in mass during a nuclear transformation
Mass defect
100
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
Pure
| Stable
101
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
Fe-26
102
The fundamental number of hydrogen
Balmer constant
| 3645.6 Angstrom
103
These experiments led to the discovery of the charge of electrons
Oils drop experiments
104
A reaction that is involved in the creation and destruction of atoms
Nuclear reaction
105
A disturbance characterized by its wavelength, amplitude and frequency
Wave
106
The vertical distance from the midline of wave to the peak or trough
Amplitude
107
Number of waves that pas through a particular point in 1 second
Frequency
108
Waves with electric and magnetic field component
Electromagnetic waves or electromagnetic radiation
109
Waves that can propagate through vacuum
Electromagnetic waves or radiation
110
Ejection of electrons from a metal plate when light falls on it
Photoelectric effect
111
He developed a mathematical model explains the observed frequencies for hydrogen spectral lines
Johannes Balmer
112
He proposed that particles could be described as a wave
Louis de Broigle
113
Electron beams were diffracted by these crystals which proved de Broigle's idea
Sodium chloride crystals
114
It states that the position and the velocity of an object cannot both be measured exactly at the same time
Heisenberg Uncertainty Principle
115
He developed a mathematical model for wave function, for particles exhibiting wave-like properties
Erwin schrodinger
116
It can be used to describe electron's energy and most probable location in space
Wave function
117
It is the interaction of electron with the magnetic field
Spin quantum number
118
It tells how the electrons are distributed among the various atomic orbitals in an atom
Electronic configuration
119
Elements of the same number of neutrons
Isotone
120
Elements of the same number of electrons
Isoelectronic elements
121
Elements of the same mass number
Isobar
122
The tendency of atoms to prefer to have eight electrons in the valence shells, making it similar to noble gas
Octet rule
123
When there is more than one Lewis structure that can represent of molecule
Resonance
124
Distribution of regions of high electron density around the central atom
Electronic geometry
125
Arrangement of atoms around the central atom
Molecular geometry
126
High electron density can be regarded as
Bonds or lone pairs
127
Covalent compounds are also known as
Molecular compounds
128
Acid that contain hydrogen, oxygen and other element
Oxoacid
129
True or False
| Most decomposition reactions require an input of energy in the form of heat, light or electricity
True
130
A reaction which a substance reacts with oxygen gas, releasing energy in the form of light and heat
Combustion
131
The rates of the forward and reverse reactions are equal
Chemical equilibrium
132
The concentrations of the reactants and product remain constant
Chemical equilibrium
133
True or False
| The ratio of concentrations between product and reactants is constant regardless of initial concentrations
True
134
If the equilibrium constant is greater than 1, then the equilibrium favors the
Product
135
This equilibrium applies to reactions in which all reacting species are in the same phase
Homogenous equilibrium
136
This type of equilibrium applies to reactions in which reactants and products are in different phases
Heterogeneous equilibrium
137
It is calculated by substituting the initial concentrations of the reactants and products into the equilibrium constants expression
Reaction quotient
138
A homogenous mixture consisting of a solute dissolved into a solvent
Solution
139
This substance produces a solution that can conduct electricity when being dissolved in water
Electrolyte
140
Substance that does not conduct electricity when dissolved in water
Nonelectrolyte
141
Properties of solutions that depend on the number of particles dissolved in the solution
Colligative properties
142
This law predicts lower vapor pressure, boiling temperature elevation is determined by the number of moles of solute dissolved in the solution
Raoult's Law
143
The selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated solution
Osmosis
144
It allows the passage of solvent molecules but blocks the passage of solute molecules
Semipermeable membrane
145
The pressure required to stop the osmosis
Osmotic pressure
146
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
Spontaneous fission
