Atomic Structure

Chuleeporn Thanomsilp
Mind Map by , created over 5 years ago

Overview of atomic structure. Classical and Quantum view.

Chuleeporn Thanomsilp
Created by Chuleeporn Thanomsilp over 5 years ago
AQA (9-1) Topic 1
C4 Quiz
Leah Firmstone
P2 Radioactivity and Stars
The Great Gatsby: Chapter Summaries
GCSE Chemistry C1.1 - Fundamental Ideas in Chemistry
chemistry: c2
kristy baker
Atomic Structure
AQA GCSE Chemsitry Fudamental ideas
Olivia Phillips
Atomic structure and the periodic table
Brodie McMeowface
WHMIS and The Structure of Matter
Mariapaula AR
Atomic Structure
1 Classical atomic model
1.1 Dalton's atomic theory
1.1.1 Dalton's model : solid sphere
1.1.2 1. Matter consists of tiny particles called atom.
1.1.3 2. Atoms of one element are identical in mass.
1.1.4 3. Compounds are the combination of atoms with a specific ratio.
1.1.5 4.Chemical reactions involve reorganization of the atoms.
1.2 Thomson's atomic model
1.2.1 Raisin in the plum pudding
1.2.2 Experiment with cathode ray and conclude that matters consist of negatively charged particle called electron.
1.2.3 Calculate mass/charge ratio of electron = -5.686 * 10^12 kg/C
1.3 Rutherford's atomic model
1.3.1 Suggest the atomic nuclear model from the results of bombardment gold foil with alpha particles.
1.3.2 Atom consists of electrons which move around the positively charged center called nucleus.
1.3.3 atomic planetary model
1.3.4 Atom is mostly empty space. The size of nucleus is very small compare to the atom itself.
2 Quantum View of Atom
2.1 Bohr's model
2.1.1 Bohr proposed that atom has energy levels as circular orbits. Electrons move as wave in a specific energy levels. Electrons can transfer to different energy levels when they lose or gain energy.
2.1.2 Each energy level has specific quantum number (n) starts from 1,2,3...
2.2 Erwin Schrödinger used Quantum Mechanics to explain the energy state in the hydrogen atom.
2.2.1 The equation is called wave function. A specific wave function is often called an orbital. Quantum number and atomic orbitals the principal quantum number (n) n = 1,2,3... small n, small size, close to nucleus, low energy the orbital angular momentum quantum number (l) give different shape of orbital s p d f orbitals the magnetic quantum number (ml) give different orientation of orbital the spin quantum number (ms) represent spin of electron. Only two possible values : +1/2 and -1/2
2.3 Wave Particle Duality
2.3.1 In subatomic level, energy and matter cannot be distinguished. They have both light and particle properties. light consists of particles called photon. Photon travels as wave. Matter consists of atom and subatomic particles. Subatomic particles such as electrons travel or move as wave.