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The Atom and The Periodic Table (The Atom (Electrons (Valence Electrons …

- - - - Thought atoms were balls of positive energy with smaller balls of negatively charged electrons
    - - Electric current through gas at low pressure
      - Negatively charged particles go from negative to positive
        
        Cathode Rays
    - - The electrons in the highest occupied energy level of an element's atoms.
      - Number of Valence electrons largely determine the element's chemical properties
      - Octet Rule
        
        In forming compounds, atoms want to have 8 Ve-
    - - How attracted an element is to an electron
      - Generally increases as you move from left to right on the periodic table
      - Generally decreases as you move down a group of the periodic table.
  - - - Particles moved from positive to negative
        
        Canal Rays
  - - - Discovered by E. Rutherford
        
        Model he created had a nucleus but did not know about orbitals, knew nucleus was positive
      - The central core of the atom
  - - - Horizontal
      - Determines energy level
    - - Vertical
      - Determines Ve-
      - Determines physical and chemical properties
  - - - Adding neutrons to an atom creates different isotopes
      - Have the same number of protons
      - Are Chemically similar
      - Have different masses
      - Atoms of the same element that have the same atomic number but different atomic masses due to a different number of Neutrons
  - - - Energy levels are less spaced the farther they are from the nucleus
    - - Atoms need to be filled from the inside out to be stable
      - Electron configuration
        
        Aufbau Principle
        
        Electrons enter orbitals of lowest energy first
        
        Pauli Exclusion Principle
        
        An atomic orbital may hold a max of 2 electrons. 1 box equals 1 orbital.
        
        Hund's Rule
        
        When electrons occupy orbitals of equal energy, one electron enters each orbital until all orbitals contain one electron with parallel spins.
  - - - When element share electrons to form compounds
      - Monatonic
        
        1 atoms
        
        (stable) ex. Noble Gases
      - Diatomic
        
        2 of the same atoms
        
        ex. Halogens
      - Triatomic
        
        3 of the same atoms
        
        ex. Ozone
      - Molecule
        
        Smallest electrically neutral unit of a substance that still has the properties of the substance
        
        Molecular Compound
        
        Compounds composed of molecules ex. Deionized water
      - Ionic Bonds
        
        Properties
        
        Crystalline solids
        
        High MP/BP
        
        Good conductors
        
        Soluble in water
      - Covalent Bonding
        
        Single Covalent Bond
        
        When electrons are shared between two atoms
        
        Double Covalent Bond
        
        Bonds that involve two shared pairs of electrons
        
        Unshared Pairs (Lone Pairs)
        
        Pairs of Ve- that are not shared between atoms
        
        Triple Covalent Bond
        
        Bonds that involve three shared pairs of electrons
        
        Bond Polarity
        
        Non-polar Covalent Bonds
        
        A covalent bond where in electrons are shared equally
        
        The shared electron is equally distant from both atoms
        
        Polar Covalent Bonds
        
        A covalent bond where in electrons are not shared equally
        
        One atom has a stronger pull on the shared electron
        
        Atom with the stronger pull has a partially negative charge and the other atom has a partially negative charge
        
        (think back to electronegativity)
        
        Determining if a bond is polar of non-polar find the difference of each atoms electronegativity (subtract them) and if the difference is 0 than the bond is non-polar and if the difference is in not zero the shared electron will be closer to the atom with the larger electronegativity.
        
        Differences
        
        0.0-0.4
        
        Non-polar Covalent
        
        0.4-1.0
        
        Moderatley Polar Covalent
        
        1.0-2.0
        
        Very Polar Covalent
        
        ≥ 2.0
        
        Ionic
    - - The energy required to overcome the attraction of the nuclear charge and remove an electron from a gaseous atom.
        
        First Ionization Energy
        
        The energy needed to remove the first Valence Electron
        
        Second Ionization Energy
        
        The energy needed to remove the second Valence Electron
        
        As the number of Ve- decreases the energy required to remove a Ve- increases.
      - Generally decreases as you move down a group of the periodic table.
      - Increases as you move from left to right on the periodic table
    - - Positively charged ion
      - Metals
    - - Negatively charged ion
      - Nonmetals
  - - - The distance between the nuclei and the outer most orbital of an atom
      - As electrons decrease the Radius also decreases
      - Atomic Radius is always estimated
- - - - Ex. [Li + F] --> {LiF} = [Reactants] {Products}
      - "s" = An atom or molecule that is solid at room temp
      - "l" =An atom or molecule that is a liquid a room temp
      - "g" = An atom or molecule that is a gas at room temp
      - "aq" = A substance that is dissolved in water
      - Coefficant
        
        The number that appears before a atom or molecule
        
        Ex. 2Fe (2 is coefficient) there are 2 iron molecules
      - Subscript
        
        A number that appears in the bottom right position that tells how many atoms of that element there are (-)
    - - A Chem equation written with words
        
        "+" = reacts with
        
        "--->" = To Produce
    - - Mass in never created or destroyed
  - - - Either 2 elements or 2 combounds
    - - Always a combound
- - - - 1) Find molar mass of N-2 O-3 = 76.014g/mol
        
        2) 118 x (1mol/76.014)
        
        3) = 1.55mol N-2 O-3
- - - - The atoms first absorb energy then release energy as they emit light