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AP Chemistry summer assignment: Nitya Marepally Per.5 (Chemical…

- - - - Product favored equilibrium: A large K value signifies a product favored equilibrium in which equilibrium is achieved when most reactant is converted into product.
      - Reactant favored equilibrium: A small K value signifies a reactant favored equilibrium in which equilibrium is achieved when very little reactant is converted into product.
    - - If Q = K, the reaction will
      - If Q < K, the reaction will move forward to get to K
      - If Q > K, the reaction will reverse to get to K
  - - - Change in surface area: more/less area for particles to collide, which causes more/less collisions so the reaction takes place quicker/slower
      - Change in concentration: usually an increase in concentration means more reacting particles so the reaction happens faster
      - Change in temperature: the particles move faster/slower, therefore more collisions occur and the reaction happens faster/slower
      - Catalysts: find an alternate pathway with a lower activation energy, which causes the reaction to speed up
    - - Activation Energy: the minimum amount of energy required to transform reactants into the active complex and produce an effective collision
        
        Exothermic reaction: have a low activation energy, release heat, and tend to be spontaneous
        
        Endothermic reactions: have a high activation energy and absorb heat
  - - - Empirical Formula: is the simplified/ base chemical formula for a compound (for ex. the empirical formula for H4O2 is H2O. The way to find the empirical formula of a substance is to assume 100g, then go from the percent of each element to the mass, then convert the mass of each element to moles, then divide each element by the smallest number of moles, then multiply till all values are whole numbers or very close to whole number. To go from the empirical formula to the regular formula, you can scale the subscripts based on the given molar mass.
- - - - Ionization Energy: is defined as the energy required to remove an electron from an atom in the gaseous state. The ionization energy tends to increase across a period because, as the radius decreases, the electron being removed in closer to the nucleus, so it has a stronger attraction and requires more energy. The ionization energy tends to decrease down a group because the outer electrons are further away from the nucleus, making it easier to remove
      - Electronegativity: is defined as the measure of the ability of a n atom in a chemical compound to attract electrons. The electronegativity tends to increase across a period because, as the radius decreases, the electrons get closer to the bonding atoms nucleus. Electronegativity tends to decrease down a group because as the radius increases, electrons get farther away from the bonding atoms nucleus.
      - Atomic Radius: is defined as half the distance between nuclei in covalently bonded diatomic molecules. The atomic radius decreases across a period because of the increased effective nuclear charge due to decreased shielding. The atomic radius increases down a group because each row on the periodic table adds a shell or energy level of electrons, making it bigger and increasing the amount of shielding.
      - Ionic Radius: is defined when positively charged ions form when an atom of a metal loses one or more electrons. The ionic radius is always small for cations compared to their corresponding neutral atom, and larger for anions compared to their corresponding neutral atom.
      - Shielding and Effective Nuclear charge: Each electron in a multi electron atom experiences both attraction to the nucleus and repulsion by other electrons in the atom. These repulsion cause the electrons to have a net reduced attraction to the nucleus (it is shielded from the nucleus). The total amount of attraction that an electron feels for the nucleus is called the effective nuclear charge or the Zeff of the electron.
    - - Anions: negative ions, columns VA, VIA, VIIA
      - Monatomic Ions: Ions that consist of only one element
      - Cations: positive ions, columns IA, IIA, IIIA
      - Polyatomic ions: Ions that consist of two or more elements
  - - - Polar: these types of covalent bonds occur when there is an unequal sharing of electrons and the electronegativity difference is between 0.3 and1.7.
      - Non Polar: these types of covalent bonds occur when there is equal sharing, or the bond is diatomic