1. Bonds
1.1. Octet Rule
1.1.1. Achieve Stability
1.1.1.1. 2 8 8
1.1.2. Valence Electrons
1.1.2.1. Electrons in Last Shell
1.1.2.2. Counted by Group Number
1.2. Types of Bonds
1.2.1. Covalent
1.2.1.1. Bonds between non-metals. This is when two atoms share electrons.
1.2.2. Ionic
1.2.2.1. Bonds between metals and non-metals. Metals donate valence electrons to non metals.
1.2.3. Metallic Bonding
1.2.3.1. 'Metallic bond' is a collective sharing of a sea of valence electrons between several positively charged metal ions.
1.2.3.1.1. Metallic Bonding is formed in a lattice structure. Lattice structure means there is a regular repeating pattern.
2. Atom
2.1. Proton
2.1.1. Positively charged
2.1.1.1. Nucleus
2.2. Electron
2.2.1. Negativly Charged
2.2.1.1. Electron Orbit
2.3. Neutron
2.3.1. Neutral charged
2.3.1.1. Nucleus
3. Periodic Table Trends
3.1. Atomic Radius
3.1.1. Bigger down
3.1.1.1. More shells
3.1.2. Smaller right
3.1.2.1. More protons
3.2. Electron Affinity
3.2.1. Adding electron
3.2.1.1. Stronger right
3.2.1.1.1. Smaller radius, stronger pull
3.2.1.2. Weaker down
3.2.1.2.1. More shells, weaker pull
3.3. Ionization energy
3.3.1. Removing electron
3.3.1.1. Stronger right
3.3.1.1.1. Smaller radius, stronger pull
3.3.1.2. Weaker down
3.3.1.2.1. More shells, weaker pull
3.4. Electronegativity
3.4.1. Stronger right
3.4.1.1. Radius is smaller
3.4.2. Weaker down
3.4.2.1. More shells
3.5. Atomic mass
3.5.1. Number of Protons + Number of Neutrons
4. Groups
4.1. 1-Alkali Metals
4.2. 2- Alkali earth metals
4.3. 13-Boron/Aluminum Group
4.4. 14- Carbon Group
4.5. 15- The Nitrogen Group
4.6. 16-The oxgen group
4.7. 17-Halogen
4.8. 18-Noble Gases
5. Diagrams
5.1. Lewis Structure
5.1.1. Lewis structures, shows the bonding relationship between atoms of a molecule. (Covalent)
5.2. Dot and Cross Diagram
5.2.1. The outer shell of each atom is drawn as a circle. circles overlap. Show only Valence Electrons (covalent)
5.2.2. Electrons from one atom are drawn as dots, and electrons from another atom as crosses. Must show all Electrons (Ionic)
5.3. Lewis Dot Noatation
5.3.1. Number of Valence Electrons
5.4. Lattice Structures
5.4.1. Metallic bonds form a lattice structure. It is not a diagram but we need to know how it works. Electrons flow freely between multiple protons and multiple bonds. Bonds can be broken or attached.
6. Arranged in periods and groups
6.1. Periods is horizontal rows
6.1.1. Signifies the amount of valence electrons (1-8)
6.2. Groups are the vertical rows
6.2.1. Signifies the amount of shells in an atom (1-7)
7. Metals, Non-metals and Metalloids
7.1. Metals loose electrons
7.1.1. High Luster
7.1.2. Ductile
7.1.3. High boiling point
7.1.4. Good conductors of electricity and heat
7.1.5. Malleble
7.1.6. Mostly solid
7.2. Non metals gain electrons
7.2.1. No luster
7.2.2. Not ductile
7.2.3. Not malleable
7.2.4. Poor conductors of heat and electricity
7.2.5. Mostly gases
7.3. Metaloids share characterists of metals and non metals
7.3.1. Staircase
7.3.2. Shiny or dull
7.3.3. better conductors compared to non metals
7.3.4. ducle and mallebale
8. Ions
8.1. Cannot change proton number
8.1.1. Changes element
8.2. Cannot change electron number
8.2.1. Changes charge
8.2.2. Can allow electron number but charge changes, and it becomes a positive or a negative ion
8.3. Must change neutron number
8.4. Types of Ions
8.4.1. Cation
8.4.1.1. Positive Charge (more protons than electrons)
8.4.2. Anion
8.4.2.1. Negativeley Charge (more electrons than protons)
8.4.3. Isotope
8.4.3.1. Isotopes are members of a family of an element that all have the same number of protons but different numbers of neutrons
9. History
9.1. Dmitri Mendeleev.
9.1.1. 1869
9.1.2. Russian
9.1.3. 63 elements bases on atomic weight