Portfolio_Group_01

=__//Chapter 1- The Nature of Matter // __= = =

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//**__Electrons__-** Electrons were discovered by Professor James Chadwick. He had discovered that electrons are negatively charged sub-atomic particles which can move from one atom to another to form compounds.//======

- //Electrons also have very low mass compared to its neighbor sub-atomic particles.//
- //Electrons revolve around the nucleus in different orbits, and every orbit has a different size and number of electrons depending on its energy. - Number of electrons increase from one energy level to another as the size of orbits increase in ascending order.//

__//**Protons and Nucleus**//__//**-** Protons were discovered by Rudherford who concluded that protons were positively charged sub-atomic particles which were present inside a central spherical ball like shape called nucleus.The nucleus has the highest mass compared to the sub-atomic particles.//

[[image:http://www.radartutorial.eu/21.semiconductors/pic/helium.big.en.jpg width="313" height="266" caption="The Structure of an Atom"]]
//__**Drawbacks of Bohr's Model**__//
 * Goes against Heisenberg's Principal of uncertainity
 * Cannot explain the fine spectra of elements

//__**Quantum Mechanic Model**__// The most recent model of the atom. It's based on the theory that the energy levels within an atom are further divided into subshell (s,p,d,f) and that eletrons fill up these subshells before moving on to the successive energy level. This model also supports Heisenberg's principle because according to this model there's only a high probablility of finding electron within the energy levels. The exact location of the electron are difficult to pinpoint.

The three dimensional space around the nucleus within an atom where there is a high probablity of locating electrons. They are also known as subshells and they are labelled s,p,d and f and they are placed in the order of increasing energy.
 * //__Orbitals__//**



These are four numbers that are used to locate electrons within an atom. According to Pauli's Exclusion Principle, no two electrons in an atom have all 4 of the same quantum numbers. The quantum numbers are the following:
 * //__Quantum Numbers__//**

It specifies the location and energy of an electron, it is a measure of the effective volume or size of the electron cloud denoted by ‘n’ and can have values 1,2,3,4....
 * //__Principal Quantum Number 'n'__//** **:**

**//__Angular Momentum Quantum Number 'l'__//** **:** It determines the shape of the orbital. It takes integral values from 0 to (n-1) where 'n' is the principal quantum number. Whn 'l' = 1 it means the p-orbital of an energy level.

It gives the orientation of the orbitals in space. When m= -1...0...1 it signifies the p-orbital which has 3 orientations and that it can hold 6 eletrons.
 * //__Magnetic Moment Quantum Number 'm'__//** **:**

It indicates the direction in which the electron rotates on its own axis. It's represented by the letter 's' and s= +1/2 or -1/2.
 * //__Spin Quantum Number 's'__//** **:**

=__//** Chapter 2 - **// __=

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//**__Ionic Bonds:__** Ionic bonds are formed when a metal loses its electron(s) to a non-metal and they both become oppositely charged.Sodium and Chlorine together form an ionic bond when they react and the resulting compound is known as Sodium Chloride. Sodium and Chlorine are very harmful elements in their elemental state however safe when they form into a compound. The common name for Sodium Chloride is salt which is added in food.//======

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//- During this bond Sodium looses one electron from its outermost shell and gives it to Chlorine to complete its outer shell. Transfer of electron happens in order to form a stable compound ( NaCl).//======

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 * //__Sodium and Chlorine forming an ionic bond.__//**

Covalent bonds are formed when two non-metals react with each and share the electrons in their outer shell to acheive a full outer shell. For example hydrogen and chlorine form a covalent bond [H - Cl] which results in the molecular compound hydrochloric acid.
 * //__Covalent bonds__ :

__Shapes of molecules__://**
 * **//Molecules//** || **//'VESPR' Shape//** || **//Bond Angle//** || **//Example//** ||
 * **//HX//** || **//Linear//** || **//-//** || **//H - Cl, H - F//** ||
 * **//AX//**₂ || **//Linear//** || **//180º//** || **//CO//**₂ ||
 * **//AX//**₃ || **//Trigonal//** || **//120º//** || **//BF//**₃ ||
 * **//AX//**₃ **//E//** || **//Pyramidal//** || **//107º//** || **:NH**₃ ||
 * **//AX//**₂ **//E//**₂ || **//V-shape or Bent//** || **//104.5º//** || **//H//**₂:O: ||
 * **//AX//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₄ || **//Tetrahedral//** || **//109.5º//** || **//CH//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₄ ||
 * **//AX//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₅ || **//Trigonal bipyramidal//** || **//120º and 90º//** || **//PCL//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₅ ||
 * **//AX//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₆ || **//Octahedral//** || **//90º//** || **//SF//**<span style="FONT-SIZE: 11pt; LINE-HEIGHT: 115%; FONT-FAMILY: 'Calibri','sans-serif'; mso-fareast-font-family: Calibri; mso-fareast-language: EN-US; mso-ascii-theme-font: minor-latin; mso-fareast-theme-font: minor-latin; mso-hansi-theme-font: minor-latin; mso-bidi-font-family: 'Times New Roman'; mso-bidi-theme-font: minor-bidi; mso-ansi-language: EN-CA; mso-bidi-language: AR-SA">₆ ||


 * //__Polar Covalent Bonds__//:**
 * //If a covalent bond is formed between two atoms with a significant difference in electronegativety (greater than 0.7) they are considered to have formed a polar covalent.//**
 * __Chapter 3__**