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Principles of Chemistry - Coggle Diagram

- - - - Alkali metals - 1A give up electrons easily
      - Alkali Earth Metals - 2A
      - Nobel Gas - 8A
  - - - Shell 1: 2
      - Shell 2: 8
      - Shell 3: 18
      - Shell 4: 32
      - Electrons in the first shall are hard to remove because they are close to the positively charged nucleus. Electrons in higher numbered shell are father from nucleus and are held less strongly, making them easier to remove.
      - Shells are divided into sub-shells designated by the letters (s, p, d, and f). In the sub-shells electrons are grouped into orbitals. An orbital is a region of space that can hold 2 e-.
    - - ground state: lowest possible energy level
      - The further the e- is from the nucleus the more reactive.
    - - Rule 1: orbitals fill in the order of increasing energy from lowest to highest. (1s, 2s, 2p, 3s, 3p, 3d)
      - Rule 2: Each orbital can hold up to two electrons with opposite spins.
      - Rule 3: when there is a set of orbitals of equal energy, each orbital becomes half full before any of them becomes completely filled.
  - - - Monatomic Cations: forms when a metal loses one or more valence e-. elements of groups 1A, 2A, and 3A form only one type of cation. Therefore, there is no need to specify with roman numerals.
        
        Examples:
        
        H+: Hydrogen ion
        
        K+: Potassium ion
        
        Li+: Lithium ion
      - Monatomic Anions: named by adding "ide" to the stem part of the name.
        
        Examples:
        
        H-: Hydride
        
        F-: Fluoride
        
        Cl-: Chloride
  - - - Examples:
        
        AlCl3: Aluminum Chloride
        
        LiBr: Lithium Bromide
        
        NaF: Sodium Fluoride
        
        Binary Ionic compounds of metals that form more than one positive ion:
        
        CuO: Copper (II) Oxide
        
        Cu2O: Copper (I) Oxide
        
        Fe2O3: Iron (III) Oxide
    - - first name the less electronegative element, normally the first atom
      - then name the more electronegative element. To name it add -ide to the stem name of the element.
      - use the prefixes di, tri, tetra to show the number of atoms of each element. Prefix mono is omitted when it refers to the first atom named and is rarley used with the second atom.
      - Examples:
        
        NO: Nitrogen oxide
        
        SF2: Sulfur Difluoride
        
        N2O: Dinitrogen Oxide