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Pauli Exclusion Principle

When electrons occupy orbitals, they spin on their axis. No two electrons in an atom can have the same set of all four quantum number.

Mass of Nucleus is equal to

Mass of Atoms

Energy levels are called

Quantum Numbers

Atomic Orbitals

A region o probability where an electron can be found.

A

Mass Number

N

Energy Levels

Mass Number

The total Number of protons and Neutrons in an atom.

Isotopes

Element with the same number of protons (Atomic Number) but different number of neutrons or mass number

Heisenberg Uncertainty Principle

Its impossible to simultaneously determine the exact location and momentum of an electron at a particular time

Schrödinger Wave Function

A wave produced by the electrons moving in a three dimensional space propagates over time.

Quantum Numbers

Atomic Orbital where electron might be

Principle Quantum Number (N)

Indicate the energy level or shell where an atomic orbital is found

Azimuthal Quantum Number (L)

Specifies the sub level within a particular principal energy level

Aufbau Principle

Building up. Used to determine the electronic configuration of an atom or ion.

Magnetic Quantum Numbers

Specific orbital within the sub level where the electron is found.

Spin Quantum Number

Intrinsic Sou if the electron in an orbital

Hands Rules of Maximum Multiplicity

The orbital of a given sub shell are first filled singly, then paurug of electrons in each orbital beans.

Electron Configuration

Distribution of electrons in an atom or molecule in atomic and molecular orbitals.

Law of Tridads

Johann Wolfgang Dobereiner

Lothar Meyer

Periodic Trends

John Newlands

Law od Octave

Henry Moseley

Arranged periodic table according to threat atomic numbers. With the use of electron gun,

Dmitri Mendeleev

Father of Modern Periodic Table, arranged the 63 elements by their atomic mass and grouped them by their physical and chemical properties.

Atomic Mass

is the weighted average of the atomic mass of the naturally isotopes of an elements

Atomic Radius

Distance from the center to the outermost.

Ionization energy

Energy needed to remove electron from the atom

Electron Affinity

Amount of energy that is released when an electron is added to an atom

Electronegativity

measure of the ability of an atom in a chemical compound to attract electrons