Electronic Structure of Matter PDF

J U M B L E D L E T T E R S R A T M T E M A T T E R T R O N P S O P R O T O N S E M L E E N S T E L E M E N T S T M O A S A T O M S  ATOM The smallest unit of matter. ...

J U M B L E D L E T T E R S R A T M T E M A T T E R T R O N P S O P R O T O N S E M L E E N S T E L E M E N T S T M O A S A T O M S  ATOM The smallest unit of matter.  DEMOCRITUS He is a Greek Philosopher, who proposed the idea of indivisible particles called "atomos"  DEMOCRITUS He is a Greek Philosopher, who proposed the idea of indivisible particles called "atomos" DEMOCRITUS  ATOMIC THEORY TIMELINE 1803 1897 1911 1913 1920s Solid Sphere Plum Pudding Nuclear Planetary Quantum John J.J. Ernest Niels Erwin Dalton Thomson Rutherford Bohr Schrödinger Atoms are dense and Atoms are described as Atom consists of a small, Electrons move in Electrons do not have solid, with no internal uniform, positively dense, positively charged quantized, discrete definite orbits, but are structure or subatomic charged spheres with nucleus at the center, energy levels around the described by wave particles considered. electrons embedded with electrons orbiting nucleus and emit or functions that represent within them, similar to around it, similar to absorb energy when probability distributions raisins in a pudding. planets orbiting around transitioning between of their locations. the sun. levels. JOHN DALTON He formulated the first modern atomic theory, based on experimental observations. 1803  JOHN DALTON SOLID SPHERE THEORY All matter is made of atoms, which are indivisible and indestructible.  JOHN DALTON SOLID SPHERE THEORY Atoms of the same element are exactly alike Atoms of different elements are different Compounds are formed by the joining of atoms of two or more elements Chemical reactions involve the rearrangement of atoms.  J.J. THOMSON Atoms are made of even smaller particles ELECTRONS 1897 J.J. THOMSON He discovered electrons 1897  J.J. THOMSON CATHODE RAY TUBE EXPERIMENT  J.J. THOMSON PLUM PUDDING MODEL The electrons were embedded in a positively charged sphere.  J.J. THOMSON PLUM PUDDING MODEL  ERNEST RUTHERFORD He conducted the Gold Foil Experiment NUCLEUS 1911  RUTHERFORD GOLD FOIL EXPERIMENT  RUTHERFORD GOLD FOIL EXPERIMENT It showed that most of the atom's mass is concentrated in a small, positively charged nucleus He proposed the "nuclear model," with electrons orbiting the nucleus like planets around the sun.  RUTHERFORD NUCLEAR MODEL Atom consists of a small, dense, positively charged nucleus at the center, with electrons orbiting around it  NIELS BOHR He modified Rutherford's model by proposing that electrons occupy specific energy levels (orbits) around the nucleus. 1913  NIELS BOHR ATOMIC MODEL Electrons move and are found in specific orbit around the nucleus  NIELS BOHR ATOMIC MODEL He placed electron in an specific energy level NIELS BOHR NIELS BOHR  ERWIN SCHRODINGER Father of Quantum Mechanics He introduced the Quantum Mechanical Model  SCHRODINGER QUANTUM MECHANICAL MODEL Electrons as existing in probability clouds, called orbitals, around the nucleus  SCHRODINGER QUANTUM MECHANICAL MODEL This gives the information about the energy of the electron principal or main energy levels.  HEISENBERG’S UNCERTAINTY PRINCIPLE This states that it is not possible to determine the exact location and velocity of an electron in an orbital at the same time. But there is a probability that the electron will be in a certain region in an atom which is called as the electron cloud. PRINCIPAL ENERGY LEVELS AND SUBLEVELS OF ELECTRONS  QUANTUM NUMBERS The set of numbers that describe the properties of an electron in an atom, specifically its energy, shape, and spatial orientation. They are essential for understanding the behavior of electrons in atoms and how they interact with each other. KINDS OF QUANTUM NUMBERS 1. Principal quantum number (n) 2. Angular Momentum Quantum Number (l) 3. Magnetic Quantum Number (ml) 4. Spin Quantum Number (ms) Principal quantum number (N) The energy level or the shell number of the electron in an atom. Principal quantum number (N) Principal quantum number (N)  angular momentum quantum number (l) This determines the shape of the electron's orbital. It can take values from 0 to n - 1. magnetic quantum number (ml) This specifies the orientation of the orbital in space. This refers to the possible behavior of the electrons in a magnetic field It can take values from -l to +l, including 0.  spin quantum number (ms) The rotations or the spins on how the electrons move on their own axis as they move around the nucleus It can be either +1/2 or -1/2, representing spin up or spin down. spin quantum number (ms) pauli exclusion principle WOFLGANG PAULI This states that no two electrons in an atom can have the same set of four quantum numbers. ELECTRON CONFIGURATION The arrangement of electrons within an atom's energy levels and orbitals.  ELECTRON CONFIGURATION No. of electrons in the subshell Energy Level Subshell ELECTRON CONFIGURATION ELECTRON CONFIGURATION ELECTRON CONFIGURATION TWO METHODS USED IN WRITING ELECTRON CONFIGURATION LONGHAND METHOD TWO METHODS USED IN WRITING ELECTRON CONFIGURATION NOBLE GAS OR ABBREVIATED METHOD TWO METHODS USED IN WRITING ELECTRON CONFIGURATION let’s try: let’s try: let’s try: let’s try: let’s try: let’s try: let’s try: let’s try:  activity no.2 A. Write the electron configuration of the following elements. 1. Phosphorus (15) 2. Lithium (3) 3. Potassium (19)  activity no.2 B. What is the element of the following electric configuration? let’s try: let’s try: let’s try: let’s try: let’s try:  activity no. 2 Distribute the electrons in the main energy level using the given electron configuration 1) 2)  Aufbau Principle Electrons fill orbitals starting with the lowest energy level and moving upwards. PAULI’S EXCLUSION Principle No two electrons in an atom can have the same set of four quantum numbers. This means each orbital can hold a maximum of two electrons, with opposite spins.  hund’s Principle Electrons fill the orbitals in a sub level, one by one, before pairing the electrons in an orbitals spin in opposite direction. hund’s Principle hund’s Principle hund’s Principle hund’s Principle EXAMPLE EXAMPLE  activity no. 3 Write the Electron Orbitals of the following Elements. Neon Calcium Magnesium