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Chemistry (the mole and chemical reactions (5 types of chem rxns…

- - - - numbers, units
- - - - particles less compacted
    - - particles less compacted
    - - particles packed together tightly
- - - - looks like one but is made up of multiple
        
        example: yogurt
    - - when particles separate after they are mixed
        
        example: clay is water
  - - - def: look like homogenious
  - - - maximum amount of solute is in solvent without changing temperature or pressure
    - - less solute in solvent then a saturated solution without changing temp or pressure
    - - solution has more solute in a solvent then a saturated solution
    - - solvent
        
        typically h20
      - solute
  - - - distilation apparatus
    - - filters
        
        filter paper, heat, removing rocks froma glass of water
    - - magnets
      - manually
- - - - the amount of energy needed to move an electron from its present energy level to the next one
        
        energy levels
        
        less spaced thefarther form nucleus
        
        when e are excited (gain in kinetic energy) they move up an orbital
        
        when e lose kinetic energy, they fall back to original orbital
        
        releases light
  - - - hgher energy
      - higher freuqency
      - short wavelength
    - - lower energy
      - low frequency
      - long wavelength
  - - - (n=1, n=2, n=3, n=4)
        
        Correspond to the period in the periodic table
  - - - Pauli Exclusion Principle:
      - An atomic orbital at most can hold 2 electrons
      - Electron configuration box = 1 orbital
    - - 1 arrow = 1 electron
  - - - Definition of valence electrons: electrons in the highest energy level of an etom (outermost energy level)
        
        Example. Carbon = 6 electrons total (2 in 1st orbital, 4 in 2nd orbital)
        
        Carbon has 4 valence electrons
        
        The number of valence electrons tells us about chemical properties of element
        
        Electron dot structures: diagrams that show valence electrons as dots
    - - Definition: atom that has a positive or negative charge
        
        Example: C (6p+, 6e-)= 0
        
        See lab book
        
        Ions are formed when valence electrons are taken, given, or shared with other atoms bonding
      - cations
        
        An atom that has lost valence electrons
        Positively charged
      - anions
        
        An atom that has gained 1 or more valence electron
        Negatively charged
  - - - Components of the periodic table
      - Periods
      - Horizontal
      - 7 of them
      - Tell us the # orbitals
      - Groups
      - Verticals
      - 18 of them
      - Similar physical and chemical properties
      - Also called families
      - Starcase
      - Divides metals and nonmetals (with the exception of hydrogen)
      - Metals
      - 4 main families
      - Alkali (group 1)
      - Alkaline earth metals (group 2)
      - Transitions (group 3-12)
      - Inner transitions (bottom of table)
      - Properties
      - color-grey/silver (except Augold+Cucopper)
      - State of matter-solid (except Hg)
      - When exposed to air or water, they corrode (except Au+Pt)
      - Tend to be good conductors of heat + electricity
      - Tend to have higher densities
      - Tend to be malleable
      - Tend to have luster
      - High boiling point
      - Nonmetals
      - 3 main families
      - Halogens (Group 17)
      - Noble gas (Group 18)
      - Hydrogen (Group 1, period 1)
      - Properties
      - Pretty much opposite of metal
      - State of matter
      - Most gas, some solid, 1 liquid
      - Brittle (tend to be)
      - Tend to be colorless + odorless (gas)
      - Group 18 = Inert (non reactive)
      - Group 17 = disatomic molecules
      - Ex. CL2, I2, Br2
      - Not conductive
      - Tend to have low boiling point
      - Dull if solid
      - Metaloids
      - Properties of both metals and nonmetals
      - (dont perfectly fit into other catefories)
      - Elements that fall under
      - B
      - AL
      - GE
      - Po
      - As
      - At
      - Sb
      - Te
      - Si
      - All solids
      - Many useda semiconductors
      - More conductive as heated
- - - - Ions = Atom or groups of atoms that have a positive or negative charge
      - Ex. Na
      - visual in book, pg. 62
      - Ionic bond = when an electron is ‘snatched’ NOT SHARED
      - Positively charged ion is a cation
      - Negatively charged ion is a anion
  - - - Covalent bond = atoms that share electrons
      - Diatomic molecule = 2 atom molecule where the atoms are the same
      - Single covalent bond = when 2 atoms share a pair of electrons
      - Lone pairs (unshared pairs, non bonding pairs) = pairs of valence electrons that are not shared between
  - - - E- shared unevenly between two different atoms (someone is winning tug of war)
      - Depends on electronegativity(tendency of an atom to pull an e- from another atom) values of the atoms
      - Atoms have partial charges
  - - - Look at electronegativity values for each atom being bound
      - Find the diff between atoms being bound
      - Locate diff on table to find bond type
      - Include any partial charges (if polar covalent)
- - - - Def: Energy is never created nor destroyed, rather it just shifts from one form of energy to another
      - Exothermic reactions: reactions that release more energy than what was put in
      - Decomposition: AB → A+B + energy
      - Endothermic reactions: reactions where more energy is put into a reaction than what was produced
      - Combination: A+B + energy → AB
      - Bond that keeps molecules together involves chemical energy
      - Examples of endothermic rxn would be baking soda + vinegar → CO2 + sodium acetate
      - “A lot of energy is put into this rxn” →
  - - - Def: compound that produces Hydrogen ions (H+) when dissolved in water
      - Ex. HCL In notebook
      - Properties:
      - Tend to corrode other substances
      - Many acids burn body tissue
      - Tend to be sour in taste
      - Citrus fruit (citric acid)
      - Vinegar (Acetic acid)
      - Soda (Phosphoric acid)
    - - Def: the negative logarithm of hydrogen ion concentration
        
        [H+]
        
        If high [H+] concentration = strong acid
        
        If low [H+] concentration = strong base
        
        [H+] H2O [OH-]
        
        [H+]=[OH-]
        
        Strong acid Strong base
        
        Indicator - substance that changes color based on the pH scale
        
        Litmus paper turns red/orange when an acid
        
        Litmus paper turns green/blue with a base
        
        Base properties: slippery
      - Neutralization Reactions
        
        Occur when an acid (H+ containing) and a base (OH- containing) react
        
        Ex. HCL+NaOH→ H2O + NaCl
        
        Acid +Base → water + ‘salt’
        
        double replacement reactions
      - Dissociation
        
        When an acid or a base is mixed in H2O, it will dissociate into ions
        
        The more dissociation that occurs, the stronger the acid or base is
        
        The less dissociation that occurs, the weaker the acid or base is
        
        Ex. HCl→ H+, Cl-
  - - - Def: compound that produces hydroxide ions (OH-) when dissolved in water
      - Properties:
      - If strong enough, can burn body tissues
      - Tends to have a ‘bitter’ taste
      - Ex:
        
        baking soda (NaCO2OH) Sodium bicarbonate
      - Tums (Calcium Carbonate)
      - Drain and oven cleaner (sodium hydroxide)