chemsitry

• intramolecular=bonds within a molecule; covalent, ionic, metallic
• Ionic;metal and non-metal
• covalent= nonmetal and nonmetal, share valence, physical bond
• metalic=metal and metal, atraction between +cation meals and -E hold togther
• intermolecular=between different molecules, wealer then bonds (vander walls forces). Types of intermolecular forces: LDF, dipole-dipole, H-bond, ion-dipole forces
• LDF=temprary/induced dipole,wealest, from valence movements fo electrons, only type in nonpolar covalend bonds, but all matter has them

  small atoms- lighter,tighter

  large atoms-bigger,easier

  more elctrons=greater LDF

  due to aymetrical elctron density

  looses energy/ change state towards solid particles slow down chance of LDF increases as more likely for electrons to spend time near each other
• Dipole-dipole; attraction between polar molecules, based on partial charges, more polar=stronger dipole=strongle DD IMF
• Hydrogen bond-type of DD, betweeen H and other molecule, strongest standard IMF, polar molecules between H and F,O, or N

  high energy+small size=strongest

  control waters properties-life depends on it
• Ion-dipole force=between ion and molecule/dipole (between ion and polar molecule)

  result of attraction between ion and a molecule that has a dipole

  higher charge,higher magnitude of polar molecule dipole=stronger force

  how ionic comps dissolve(only if stronger then ion-ion IMF)

  stronger then H bond
• ion-ion force=structure and solubility, crystal lattice structure of ionic compunds, strength of IMF determine ionic compounds soulubility
• Types of IMFs(weakest to strongest)

  1)lmf=all moleular atoms

  2)DD-polar molcules

  3)H-bonding-molecules of H bonded to F<O<N

  4)ion-dipole-mixtures of ionic compunds and polar compounds
• physical changes=making and breaking IMFs