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Unit 1: Structure and Properties - Coggle Diagram
Unit 1: Structure and Properties
Early Atomic Theories
Bohr Model
Based off the planetary Rutherford Model
Rather than all electrons in 1 orbit. They exist in energy level orbits
Electrons can move in the orbits without losing energy
Electrons can move between the orbits by accepting or radiating energy. If accepts, it moves higher, if it radiates it moves to a lower energy
the amount of energy gained or lost by an electron moving between orbits corresponds to a frequency of electromagnetic radiation.
Problems
The calculations that are made for this theory only work with atoms of 1 electron
And the transition to different energy levels can be split with a magnetic or electric fields
Rutherford Model
Work is based off the Thompson's model
Gold foil experiment, electrons shot at a thin gold foil, expected results were that all electrons fly through with no issues. But a very small percentage went flying in a completely different direction. proved that there is a positive nucleus
1914: Rutherford concluded there was a positive particle called the Proton
1932: with the help of Chadwick, there was also the discovery of the neutron, a neutral charged particle
The model was presented as a planetary system, with a nucleus and electrons orbiting around it
Problems
According to Classical Physics, electrons that orbit should lose energy through light and crash to the nucleus.
Electrons gives off/ absorbs very specifics wave lengths depending on what is the atom
Thompson's model
With a CRT, Thompson discovered that there was a mass of negative particles.
This led to the discover of the electron
The Thompson "pudding" model consisted of a positively charged spherical area with electrons inside of it, like raisins in pudding
Dalton Theory
All Matter is compromised of small indivisible particles called atoms
Quantum Mechanical Model
Uncertainty Principle: You can never know what the momentum and the exact position of an electron
Orbitals
4 Main Types: S(Max 2) P(Max 6) D(Max 10) F (Max 14)
S Orbital
P Orbital
D Orbital
F orbital
Each orbital can hold 2 electrons
Orbitals are a region of space where there is a %95 of an electron
Electron Configurations + Energy level Diagrams
Aufbau's Principle
2 electrons per Orbital
Hund's Rule
Pauli Exclusion Principle
Magnetism
Para magnetism relies on the number of unpaired electrons, as the number increases, para magnetism increases
Diamagnetism is when there are no unpaired electrons
Trends in the periodic Table
Factors affecting Properties:
1.The number of occupied energy levels
2.The number of protons in the Nucleus
Trends in Atomic Radius
1.The radius increases as you go down the group
2.The radius decreases as you go across the period
First Ionization Energy.
1.Energy required to remove the first electron
2.Decreases as you go down a group
3.Increases as you across the period
Electron Affinity
1.Energy released when an electron is added
2.Decreases as you go down a group
3.Increases as you across the period
4.Noble Gases have the lowest Electron affinity
Exceptions to the Trends.
1.Group 2/13, new p orbital causes a decrease in Ionization energy
2.Group 15/16, all p orbitals in group 15 filled, decrease in Ionization energy
Bonding Theories + Vsper
Bonding Theories
Lewis Bonding Theory
Reaching stable octets through electron transfer
Valence Bond Theory
VB Theory is the quantum theory for bonding
Covalent bonds form when a when 2 orbitals with 1 electrons overlap to form a new hybrid orbitals
Bonded orbitals contain 2 electrons with opposite spin.
Vsper Theory is the theory used to predict the shape of compounds. Electron pairs will always take on the furthest angles from each other in 3D due to repulsion force
Properties of Solids
Solids have different melting points based on the types of intermolecular bonds they have. The order from lowest melting point to highest is
Atomic molecules
Non-polar, polar
Hydrogen bonding
Metallic
Ionic
Network compounds
Connection to Organic Chemistry. In Organic chemistry there is the exploration of the properties of Organic compounds. The main properties are boiling point and solubility which use the intermolecular bonds we learned in unit 1 to determine this.
Connection to Equilibrium theory. In equilibrium we learned about the Haber process. We also learned that in the process lowering the temperature in the system allows us to yield more ammonia, this is because ammonia has Non-Polar bonds versus the Atomic Molecules Nitrogen and Hydrogen, this means it turns to liquid at a higher temperature which means you can yield more NH3 and allow the reaction to occur faster in the products direction
