1. THERMOCHEMISTRY
   1. Important terms
      1. enthalpy of reaction
      2. calorimeter
      3. heat capacity
      4. system
      5. surroundings
      6. endothermic process
      7. enthalpy
      8. heat
      9. heat of reaction
      10. exothermic process
      11. Hess's law of heat summation
      12. standard state
      13. standard enthalpies (heat) of formation
      14. THERMOCHEMISTRY - Important terms.pdf
   2. Key equations
      1. Thermochemistry - key equations.pdf
2. ATOMIC STRUCTURE
   1. what is light?
      1. it's a kind of energy
      2. each color of light have different energy
      3. האור מאטום מימן (מהשמיים) אינו רציף
      4. מכאן שהאור מורכב משני מרכיבים, חשמלי ומגנטי, ולכן נקרא אלקטרומגנטי
      5. אורך הגל ג
      6. הגודל שעולה ויורד הוא המרכיב החשמלי E
      7. V=c/ג
         1. c=3X10^10
         2. c=speed of light (constant)
         3. v = frequency of light
      8. E=hv=hc/ג
         1. h=6.63X10^-34 J/sec
      9. when ג is greater, E is smaller; opposely proportional :)
         1. but when v is greater E is also greater
   2. רמות אנרגיה
      1. n = 1,2,3...
         1. מס' הקוונטום הראשי
      2. l = 0,1,2... n-1
         1. מסי הקווטום האורביטלי
      3. m= +1, -1... +1
         1. מסי הקוונטם המגנטי
   3. Electron afinity
      1. is the energy change for the process of adding an electron to a neutral atom in the gaseous state to form a negative ion.
      2. The negative value actually means the energy released by the atom when it gains an electron
      3. large negative number indicates a very stable negative ion is formed
      4. higher electron affinity means smaller negative value
   4. Electronegativity
      1. ability of an atom in a molecule to draw bonding electrons to itself
         1. low ionization energy and low electron affinity means it has tendency to become CATION
         2. high ionization energy and high electron affinity means it has tendency to become ANION
      2. general electonegativity INCREASES FROM LEFT TO RIGHT and DECREASES FROM TOP TO BOTTOM in the periodic table
   5. mass of electron = 1/1840 x mass of proton
   6. Ionization Energy
      1. האנרגיה הדרושה לעקור אלקטרון מאטום נקראת אנרגית יוניזציה
         1. האנרגיה הדרושה להפוך אטום ליון
         2. ionized atom loses its electron
         3. FIRST IONIZATION POTENTIAL of an atom is the minimum energy needed to remove the highest-energy (outermost) electron from the neutral atom in the gaseous state
3. MOLECULAR GEOMETRY AND CHEMICAL BONDING THEORY
   1. heteronuclear diatomic molecules
      1. molecules composed of two different nuclei
   2. VSEPR (valence-shell electron-pair repulsion model)
      1. linear 2
         1. 180 degree
      2. trigonal planar 3
         1. 120 degree
      3. Tetrahedral 4
         1. Tetrahedral 4
            1. 109 degree
         2. trigonal pyramidal 3 1
            1. 107 degree
         3. bent 2 2
            1. 105 degree
      4. trigonal bipyramidal 5
         1. trigonal bipyramidal 5
            1. 120 and 90 degree
         2. seesaw 4 1
         3. t-shaped 3 2
         4. linear 2 3
      5. octahedral 6
         1. octahedral 6
            1. 90 degree
         2. square pyramidal 5 1
         3. square planar 4 2
   3. dipole moment
      1. atoms with dipole movement have ל+ and ל- charges
      2. the movement is tend to move from weak electronegative atom to the strong atom
      3. Linear in AX2, Trigonal planar, Tetrahedral, Square planar, Trigonal bipyramidal, Octahedral have zero dipole movement
      4. Think then what kinds of molecules have dipole movements and how strong are they
   4. valence bond theory
      1. A bond forms when the following conditions are met
      2. 1. An orbital on one atom comes to occupy a portion of the same region of space as an orbital on the other. The two orbitals are said to overlap.
      3. 2. The total number of electrons in both orbitals is no more than two.
   5. hybrid orbitals
   6. I must write definitions in my own words!!
   7. VSEPR (valence-shell electron-pair repulsion model
      1. a model for predicting the shapes of molecules and ions in which valence-shell electron pairs are arranged about each atom so that electron pairs are kept as far away from one another as possible, thus minimizing electron-pair repulsions.
   8. dipole moment
      1. a quantitative measure of the degree of charge separation in a molecule
   9. valence bond theory
      1. an approximate theory to explain the electron-pair or covalent bond by quantum mechanics
   10. hybrid orbitals
       1. orbitals used to describe bonding that are obtained by taking combinations of atomic orbitals used to describe the isolated atoms
   11. sigma bond
       1. a bond that has a cylindrical shape about the bond axis
   12. Definitions
       1. VSEPR (valence-shell electron-pair repulsion model
          1. a model for predicting the shapes of molecules and ions in which valence-shell electron pairs are arranged about each atom so that electron pairs are kept as far away from one another as possible, thus minimizing electron-pair repulsions.
       2. dipole moment
          1. a quantitative measure of the degree of charge separation in a molecule
       3. valence bond theory
          1. an approximate theory to explain the electron-pair or covalent bond by quantum mechanics
       4. hybrid orbitals
          1. orbitals used to describe bonding that are obtained by taking combinations of atomic orbitals used to describe the isolated atoms
       5. sigma bond
          1. a bond that has a cylindrical shape about the bond axis
       6. pi bond
          1. a bond that has an electron distribution above and below the bond axis
       7. molecular orbital theory
          1. a theory of the electron structure of molecules in terms of molecular orbitals, which may spread over several atoms or the entire molecule
       8. bonding orbitals
          1. Molecular orbitals that are concentrated in regions between nuclei
       9. antibonding orbitals
          1. Molecular orbitals that are concentrated in regions other than between two nuclei
       10. homonuclear diatomic molecules
           1. molecules composed of two like nuclei
       11. heteronuclear diatomic molecules
           1. molecules composed of two different nuclei
   13. pi bond
       1. a bond that has an electron distribution above and below the bond axis
   14. molecular orbital theory
       1. a theory of the electron structure of molecules in terms of molecular orbitals, which may spread over several atoms or the entire molecule
   15. bonding orbitals
       1. Molecular orbitals that are concentrated in regions between nuclei
   16. antibonding orbitals
       1. Molecular orbitals that are concentrated in regions other than between two nuclei
   17. homonuclear diatomic molecules
       1. molecules composed of two like nuclei