Module 1 - Inorganic Chemistry Flashcards
Democritus Era
460-370 BC
ELECTRONS
Discovered by:
Mass:
Coulumb:
Charge:
Joseph John Thomson
9.10938 x 10-28
-1.6022 x 10 -19
-1
PROTONS
Discovered by:
Mass:
Coulumb:
Charge:
Eugene Goldstein
1.67262 x 10-24
+1.6022 x 10 -19
+1
NEUTRONS
Discovered by:
Mass:
Coulumb:
Charge:
James Chadwick 1932
1.67493 x 10-24
0
0
In 1897, J.J. Thomson discovered electrons which he named ______
corpuscles
- It shows the atom as composed of electrons scattered throughout a spherical cloud of positive charge
-Recognize electrons as components of atoms
-No nucleus, didn’t explain
Plum Pudding Model
Joseph John Thomson
1904
-His theory stated that atoms are indivisible, those of a given
Elements are identical, and compounds are combinations of different types of atoms
- Recognized atoms of a particular element differ from to other
-Atoms are not indivisible, composed of subatomic particles
SOLID SPHERE MODEL
(JOHN DALTON 1803)
-Fired positively charged alpha particles at a thin sheet of gold foil. Most passed through with a little deflection, but some
deflected at large angles
-This was only possible if the atom was mostly empty space, with
a positive charge concentrated in the center: the nucleus
-Realize positive charge was localized in the nucleus of an atom
-Did not explain why electrons remain in orbit around the nucleus
NUCLEAR MODEL (ERNEST RUTHERFORD 1911)
-Modified rutherford’s model of the atom by stating that electrons move around the nucleus in orbits of fixed sizes and
energies.
-Electron energy in this model was quantized; electrons
could not occupy values of energy between the fixed energy
levels
-Proposed stable electron orbits explain the emission spectra of some elements
-Moving electrons should emit energy and collapse into the nucleus, model did not work well for heavier atoms
PLANETARY MODEL
(Neils Bohr 1913)
Proponent stated that electrons do not move in set paths around the nucleus, but in waves. It is impossible to know the
exact location of the electrons; instead, you have clouds of probability called orbitals, in which we are more likely to find an electron
Shows electrons didn’t move around the nucleus in orbits but in clouds where their position is uncertain
Still widely accepted as most accurate model of the atom
QUANTUM MODEL (ERWIN SCHRODINGER 1926)
Clouds of probability is called
Orbitals
ATOMIC STRUCTURE
Atoms is a spherical mass containing electrons and that this spherical mass is positive but is made neutral by the electrons embedded in it.
Aka Plum Pudding Model
THOMSON MODEL
ATOMIC STRUCTURE
In this model, protons are in the nucleus and the electrons are in
the orbital motion around the nucleus Electrons may be found in any several definite orbits around the
nucleus
BOHR MODEL OF AN ATOM
ATOMIC STRUCTURE
Atoms are elliptical orbits of increasing number
RUTHERFORD-BOHR MODEL
This principle states that simultaneous determination of the exact position and exact momentum of electron is impossible
HEISENBURG UNCERTAINTY PRINCIPLE
Aka Electron Cloud Model
In this model, the nucleus is a single cluster of particles at the center of the atom while the electrons are everywhere
Has dense positive charge nucleus at the center and electrons still have a distinct amount of energy which are usually place outside the nucleus
The electrons are not orbiting the nucelus in definite or fixed pathways. Instead of orbiting, the electrons are placed in orbitals outside the nucleus (electrons are still orbiting the nucelus but not in fixed pathways)
WAVE MECHANICAL ATOM
This theory makes the assertion that electromagnetic radiation like X-rays, gamma rays, radio waves and light rays are made up of small bits of energy
SCHRODINGER “QUANTUM MODEL”
states that no two electrons can have the same set of quantum numbers
Pauli’s Exclusion Principle
○ corresponds to main energy levels
○ described the size of the orbital
Principal Quantum Number (n)
or angular momentum quantum number (can give and measure angular momentum of an electron and its motion around the nucleus)
○described the shape of orbital
Azithmuthal Quantum Number (l)
○indicate the behavior of electrons in the magentic field
○described the orientation in space of a particular orbital
Magnetic Quantum Number (m)
○indicate the spin of an electron about its own axis in clockwise or counterclockwise
Spin Quantum Number (s)
ATOMIC STRUCTURE
This theory states that the number of orbital types in a given shell is equal to the shell number
Orbitals have a three-dimensional region in space where the probability of finding the electron is greatest
ORBITAL THEORY
○orbitals with the same electron of same energy level must be filled in singly before pairing
Hund’s Rule of Maximum Multiplicity
ATOMIC STRUCTURE
According to this theory:
1st - 4th main energy level
ELECTRON CONFIGURATION THEORY
states that atoms may be built by progressively filling the main energy levels, sub levels and orbitals with electrons according to increasing level
*** levels of lower energy level are occupied first
AUFBAU PRINCIPLE
○the values are from 0 to n - 1
Azithmuthal QN
the value range from -1 to +1
Magnetic Quantum Number
1-4th Energy Level = Maximum number of electrons
1st = 2e
2nd = 8e
3rd = 18e
4th = 32e
equal to the number of protons and electrons
ATOMIC NUMBER (Z)
total number of protons and neutrons on the nucleus of nucleons,
MASS NUMBER (A)
Nuclear notation
A (Mass number)
N (Neutrons)
Z (Atomic number)
X (Element)
in other words, they have the same number of protons and electrons but different number of neutrons
ISOTOPES
__ isotopes is usually present in greater abundance than another isotopes
one
atoms of different elements having the same number of neutrons
ISOTONES
atoms of different elements having the same atomic mass
ISOBARS
it is a charged species, an atom or a molecule, that has lost or gained one or more electrons
IONS
it is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances
MOLECULES
aggregates of at least two atoms in a definite arrangement and held together by chemical forces
MOLECULES
a conductor that is used to make contact with non-metallic part of a circuit
commonly used in electrochemical cells, semi-conductors such as diodes and other medical devices
ELECTRODES
o positively charged electrodes
Anode
can also be zero
WEIGHT
when travelled to the moon, the weight of an object will only be ___ of its weight on earth
1/6
are made up only of one kind of matter possessing a definite, fixed and unvarying compositions
has unique set of properties
PURE SUBSTANCES
○ simplest form of substance that cannot be decomposed by chemical means; building blocks of matter
- Elements
○ possess the characteristics of metals and non-metals
1.3 Metalloids
EARTH’S CRUST COMPONENTS & %
Oxygen - 45.5%
Silicon - 27.2%
Aluminum - 8.3%
Iron - 6.2%
Others - 5.3%
Calcium 4.7%
Magnesium 2.8%
HUMAN BODY COMPONENTS AND %
Oxygen - 65%
Carbon - 18%
Hydrogen - 10%
Nitrogen - 3%
Calcium - 1.6%
Phosphorus - 1.2%
Others - 1.2%
○ are substances whose molecules are made up of two or more kinds of atoms
○ combined in definite proportion
COMPOUNDS
○ formed when there is a transfer of e-
2.1 Ionic compound
○ formed when e- are shared
2.2 Covalent compound
○ formed by interaction between elements which are usually metallic but the resulting compound behaves just like an ordinary metal
2.3 Metallic compound
○ any of the large class of chemical compounds in which one or more atoms of carbons are covalently linked to the atoms of another elements
○ carbon-containing compounds (such as H, O, N) except carbides, carbonates, and cyanides
2.4 Organic compound
○ these are combined with definite proportions of two elements
○ do not contain carbon
○ eg. graphites, carbon dioxide, and carbon monoxide
2.5 Inorganic compound
ACID-BASE THEORY
(Proponent + Theory)
Arrhenius
Bronsted-Lowry
Lewis
Water when it loses a proton forms ____
hydroxide ion
Water when it accepts a protn forms ____
hydronium ion
based on electrolytes nature; an equation that will provide the starting point for modern treatments of non- ideality of electrolytes solution
++ proponents
DEBYE-HUCKEL THEORY | by Peter Debye and Erich Huckel
substances that are resistant to pH; apply the theory of Henderson-Hasselbach equation
BUFFERS
maximum amount of either the strong acid or the strong base that can be added before a significant change in the pH will occur; apply the Van Slyke Equation
BUFFER CAPACITY
○ combination of any positive ion and negative ion except for OH; formed by the combination of acids and bases
2.5.3 Salts
acid and bases with a product of salt and water
○ NEUTRALIZATION
○ substances that consists oxygen and other elements
2.5.4 Oxides
blue litmus paper to red
ACID
red litmus paper to blue
BASE
Define the pH levels of:
Strong acids
Weak acids
Neutral
Weak bases
Strong bases
pH 1-3 pH 4-6 pH 7 pH 8-10 pH above 11
Solution particle size
< 10 ^(-7)cm
Colloid particle size is
10-7 cm and 10-5 cm
Suspension particle size is
> 10 ^(-5) cm
the liquids are colloidally suspended in another liquid samples
EMULSIONS
The particle size of ____ are much larger than solution but smaller than suspensions
colloids
- is the scattering of light by particles in a colloid or suspension
TYNDALL EFFECT
-aka Proust’s Law
-a given chemical compound will always contains the same elements in the same proportion by mass
LAW OF DEFINITE PROPORTIONS
-when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of a small whole numbers
LAW OF MULTIPLE PROPORTIONS
elements combine in the ratio of their combining weights or chemical equivalents; or in some simple multiple or sub-multiple of that ratio.
LAW OF COMBINING WEIGHTS
aka Proust’s Law
LAW OF DEFINITE PROPORTIONS
also called the Law of Reciprocal Proportions or Law of Equivalents
LAW OF COMBINING WEIGHTS
