... Quantum Mechanics, Isotopes and Atoms, Trends on the Periodic Table, Electron Structure and Naming Compunds (Part 2)

....where was I? ......OH YEAH. 

Trends on the Periodic Table
We learned that elements that are close to each other display similar characteristics. On the periodic table, there are 7 different trends:

1. Reactivity
2. Ion Charge
3. Melting Point
4. Atomic Radium
5. Ionization Energy
6. Electronegativity
7. Density*

*Density was taught into full context during this lesson.

Reactivity:
The main information we needed to know was that metals and non-metals show different trends, the most reactive metal is Francium and the most reactive non-metal is Flourine.

Ion Charge
Elements' ion charges depend on their group (Alkali Metals, Alkali Earth Metals, Halogens, Noble Gases, etc...)

Melting Point
With the melting point, elements in the center of the table have the highest melting points and the noble gases have the lowest. Also, starting from left to right, melting point increases (until the middle on the table)
Note: Although a non-metal, Carbon has one of the highest melting points on the periodic table.

Atomic Radium
The radium increases to the top and to the right. Helium has the smallest radius and Francium has the largest radius

Ionization Energy:
Ionization energy is the energy needed to completely remove an electron from an atom. Energy increases going up to the right. Noble Gases have the highest energy, Helium is the highest, Francium is the lowest.

Electronegativity

Electronegativity refers to how much atoms want to gain electrons. The trend is the same as that of ionization energy; increasing up and to the right 

Electron Structure

Here are some things to know when drawing Electron Dot Diagrams. The nucleus is represented by the atomic symbol, for the elements, you need to determine the number of valence electrons, electrons are represented by dots around the symbol, there are four orbitals, each orbital gets 2 and each orbital gets 1 electron before getting paired up. Look to the left for an example.

When drawing Lewis Diagrams for Compounds and Ions, you need to determine the number of valence electrons for each atom and place atoms so that the valence electrons are shared to fill each orbital. To the right, you will see an example of Nitrogen Tri Chloride:

When drawing Lewis Dot Diagrams for Ionic Compounds, you first have to determine the number of valence electrons on the cation. Move these electrons to the anion. Draw square brackets ( [ ] ) around the metal and non metal. Write the charge outside of the bracket. To the right is an example of Sodium Chlorate:


Naming Compounds:
Today, the most common system is IUPAC for most chemicals
-ions
-binary ionic
-polyatomic ions
-molecular compounds
-hydrates
-acids/bases 

Chemical Formulas
Be aware of the difference between ion and compound formulas 

Multivalent Ions

Some elements can form more than 1 ion. For example, Copper has a plus 2 AND plus 1 charge. Usually the top number on the periodic table is more common. IUPAC uses roman numerals in brackets to show the charge. Classic systems were latin names of elements and suffixes -ic and -ous (larger charge and smaller charge respectively)

*Note: there are other classic names for different elements:

ferr - iron

cupp - copper 

mercur - mercury

stann - tin

aunn - gold

plumb - lead

Hydrates

Some compounds can form lattices that bod to water molecules, these crystals contain water inside them which can be released by heating. To name hydrates you: 1) write the name of the chemical formula, 2) add a prefix indicating the number of water molecules (mono-1, di-2, tri-3) and 3) add hydrate after the prefix