Alkenes and Alkynes

There are unsaturated hydrocarbon compounds that are either connected by double bond or triple bond.  Alkenes are the ones bonded by a double bond and alkynes are the ones bonded by a triple bond.  For alkenes the root names give the number of carbons in the longest continuous chain. Alkene names are formed by dropping the "ane" and replacing it with "ene".  It is written with this formula: C_nH_2n.  For alkynes the root names give the number of carbons in the longest continuous chain. Alkyne names are formed by dropping the "ane" and replacing it with "yne".  It is written with this formula: C_nH_2n-2.

A table for alkenes:

No. of Carbons	Root Name	Formula CnH2n	Structure
2	ethene	C2H4	CH2=CH2
3	propene	C3H6	CH2=CHCH3
4	1-butene	C4H8	CH2=CHCH2CH3
5	1-pentene	C5H10	CH2=CHCH2CH2CH3

A table for alkynes:

No. of Carbons	Root Name	Formula CnH2n-2	Structure
2	ethene	C2H2	CH=CH
3	propene	C3H4	CH=CHCH3
4	1-butene	C4H6	CH=CCH2CH3
5	1-pentene	C5H8	CH=CCH2CH2CH3

Here is a video explaining name both alkenes and alkynes:

Alkanes

Alkanes are chemical compounds composing of only carbon and hydrogen atoms by single bonds.  The image above is the most simple alkane, methane.  This means that the compound contains 1 carbon atom and 4 hydrogen atoms.  The trend for the other compounds is increasing the number of carbon atoms.  Since the first one is methane with 1 carbon and 4 hydrogen, the next compound would be ethane which contains 2 carbon and 6 hydrogen.  As you gain more carbons, the number of hydrogen is 2 more. 
Here is a table of the simple alkanes:

# Carbon

Name

Molecular Formula

Structural Formula

1

Methane

CH4

CH4

2

Ethane

C2H6

CH3CH3

3

Propane

C3H8

CH3CH2CH3

4

Butane

C4H10

CH3CH2CH2CH3

5

Pentane

C5H12

CH3CH2CH2CH2CH3

6

Hexane

C6H14

CH3(CH2)4CH3

7

Heptane

C7H16

CH3(CH2)5CH3

8

Octane

C8H18

CH3(CH2)6CH3

9

Nonane

C9H20

CH3(CH2)7CH3

10

Decane

C10H22

CH3(CH2)8CH3

Here is a video:

Bohr Model

The image above is the picture of the bohr model for Cl.  The bohr model shows the electron levels of the element that you want to draw.  Just find out how many electrons are in the element and then fill in the number of electrons in the proper shell.  There are limits for each shell.  They follow as:
1st shell : 2 electrons max
2nd shell : 8 electrons max
3rd shell and all others : 8 max

For example carbon has 6 protons and since we are drawing a carbon atom without a charge it has a overall charge of 0.  This means that there are 6 electrons.  The bohr diagram will look like:

Here is a video:

Lewis Diagrams

What is that picture? That is the lewis structure model of H2O, water.  This diagram shows the bonding between atoms of a molecule and the pairs of electrons that exist within the molecule.  This diagram is used to for showing covalently bonded molecules and compounds. 

To draw this, you have to follow these steps:
Step 1: Count up the number of valence electrons for each atom, and total them up to give the total number of electrons for the molecule

Step 2: Determine which atom is the central atom and join all the atoms using only single bonds. Sometimes which atom is the central atom is hard to determine

Step 3: Add lone pairs to each atom as necessary so that each atom has an octet (except H which can only have 2 electrons total) when you count all the atom's lone pairs and two electrons for each of its bonds.

Step 4: If the total you got in Step 1 is the same as in Step 3, you're done! If it doesn't you'll need to make some changes. If the number of electrons in Step 3 is larger than in Step 1, you must add double bonds as necessary between atoms. Then adjust the number of lone pairs again so that each atom has an octet. **Remember no double bonds to H or with any of the halogens!** If the total electron count with only single bonds is smaller than in Step 1, you probably made a mistake somewhere. Go back and double check.

Step 5: Continue adjusting the arrangement of single and double bonds and lone pairs (and also triple bonds if necessary) until the total electron count matches what you got in Step 1.

Here is a video: 

April. 20 Electron Configuration

HOLY Angelina JOLIE! Look at that diagram!  That is how we write the electron configuration of any element.  You write then how the arrows go down.  So you start with 1s then 2s then 2p then 3s then 3p then 4s and so on.  Remember this: the maximum amount of electrons in each shell are 2 for s, 6 for p, 10 for d, and 14 for f. 

April 18 Atomic Mass and Isotopes

When you look at the periodic table of elements, you see that each element is in a box with numbers and a symbol.  It goes from top to bottom as element name, atomic number, symbol, and atomic mass.  The atomic number is the amount of protons that the element has and the atomic number is the mass of the atom.  In order to get the mass, you add the amount of protons and neutrons.  The reason why you add these two is because the nucleus of the atom contains only of protons and neutrons.  You don't add electrons because they only orbit the atom.  The protons are already given to you from the atomic number so all you need to do is subtract the atomic mass with the atomic number to get the number of neutrons.  The atomic mass is usually shown as a decimal number in periodic tables because that the average mass of the atom.  From the picture above, you can just say that Helium has an atomic mass of 4. That means it has 2 neutrons because it has 2 protons from the atomic number.
 

 In Copper, its atomic number is 29.  This means that there is 29 protons.  The atomic mass is 63.5.  You can make it 64.  We then subtract 64 and 29.  The result is 35 neutrons.  From Titanium, its atomic number is 22.  That means there are 22 protons.  With a atomic mass of 48, we subtract the two numbers and get 26 neutrons.

What does the word isotope mean? An isotope is a variation of an atom with more or less neutrons.  Isotopes are atoms that have lost/gain neutrons and also electrons.  For example, Krypton has an atomic mass of 84.   It can also be called Krypton-84.  Sometimes you might see it written as Krypton-83 or Krypton-85.  This means it lost and gained an electron.  From Krypton-84 to Krypton-83 it lost a neutron.  And from Krypton-84 to Krypton-85 it gained an electron.  Sometimes you might see a number and a positive or negative symbol beside the atomic mass number.  If there is no number or symbol beside the atomic mass number, this means the isotope is neutral.  If you see a positive symbol and a number beside it, it means it has lost the number of electrons from the isotope making it positive by the number of charge because it lost that number of electrons.  This means the isotope has more protons than electrons.  And same goes for a negative number beside the atomic mass number.  It means that the isotope gained the amount of electrons making the isotope negative because it has more electrons than protons.  If there is just a negative or positive symbol, it means it has 1 less/more electron.

Examples:
How many electrons are in Ca²⁺?
For Ca, there is 20 protons.  Since it is 2+, this means that the isotope is positively charged.  The amount of electrons would be 18.

How many protons and electrons are in Cl^-

^{Cl has 17 protons.  This isotope is negatively charged.  Remember that if it just has a negative sign, it means it lost 1 proton.  That means there is 16 electrons in this isotope.}

This is pretty much straight forward.  No need to video... After doing the worksheets you should be fine with the stuff. 

April. 14 The Atomic Theory

*LONG POST!!, IF DONT WANT TO READ, WATCH THE VIDEO AT THE BOTTOM OF THE PAGE :)*
How did we get from this:

To this:

The very first person to come up with the concept of the atomic theory was Democritus (460 BC - 370 BC).  He came up with the thought that everything was made up of matter which was composed of atoms and they looked like tiny spheres.  He thought it looked liked this:

Next Aristotle (384 BC - 322 BC) thought up that everything was made up of elements.  They were fire, earth, air, water, and aether. 

Antoine Lavoisier (Aug.26 1743 - May 8 1794) discovered that water is made of oxygen and hydrogen.  He also discovered that chemical elements were neither destroyed or created, but just combined in different compounds in chemical reactions.

John Dalton (Sept. 6 1766 - July. 27 1844) proposed an atomic theory with five major important points.  They were 1. Elements are made of tiny particles called atoms, 2. The atoms of a given elements are different from those of any other element, 3. All atoms of a given element are identical, 4. Atoms of one element can combine with atoms of other elements to form chemical compounds, 5. Atoms cannot be created, divided into smaller particles, nor destroyed in the chemical process.

 

Henri Becquerel (Dec. 15 1852 - Aug. 25 1908), Marie Curie ( Nov. 7 1867 - July 4 1934) and Pierre Currie (May 15 1859 - Apr. 19 1906) were three physicist who all three won the 1903 Nobel Prize in Physics for their discoveries of radioactivity.  In 1911, Marie Currie won the 1911 Nobel Prize in Chemistry for her discovery of the elements Radium and Polonium. 

J.J. Thompson (Dec. 18 1856 - Aug. 30 1940) was a physicist who is credited for the discovery of the electron and of isotopes and is the inventor of the mass spectrometer.  In 1906, he won the Nobel Prize in Physics for the discovery of the electron and for his work on the conduction of electricity in gases.

Robert Millikan (Mar. 22 1868 - Dec. 19 1953) was an American physicist who discovered the charge on the electron which is negative.  He measured the charge with his oil-drop experiment and confirmed that the charges were calculated to be 1.5924(17) x 10^-19.

Ernest Rutherford ( Aug. 30 1871 - Oct. 19 1937) was a New-Zealand born British chemist and physicist who became known as the father of nuclear physics.  He discovered the concept of radioactive half life.  He directed the Geiger-Marsden experiment in 1909 which proved J.J. Thompson's plum pudding model of the atom was incorrect.  His model had the features of a high central charge concentrated in a very small volume in comparison to the rest of the atom and containing the bulk of the atomic mass which would be know as the atomic nucleus.  He would also go on to discover the proton in 1919.

Niels Bohr (Oct. 7 1885 - Nov. 18 1962) was a Danish physicist who made contributions of understanding the atomic structure.  He created the famous "Bohr Model" which shows the electrons and their orbits around the atom's nucleus. 

Henry Moseley (Nov. 23 1887 - Aug. 10 1915) was an English physicist who contributed to concept of the atomic number.  He also developed a law called Moseley's Law which also justified many concepts in chemistry by sorting the chemical elements of the Periodic Table of the Elements in a logical order based on physics.

James Chadwick (Oct. 20 1891 - July 24 1974) is known for his discovery of the neutron in 1932.  His discovery of the neutron was crucial for the fission of uranium 235.  He was later awarded the Nobel Prize in Physics in 1935 for his discovery of the neutron.

NOW FOR A VIDEO!! BONUS: SLIDESHOW OF THE ATOMIC THEORY WITH MILEY CYRUS'S PARTY IN THE USA... just instrumental though :( (Defiantly on the subject of Atomic Theory and Chemistry)TEHE