7B

• Orbital hybridization is the process by which new kinds of orbitals with equal energies are formed by a combination of orbitals with different energies
• Diatomic elements have no polarity because they have the same electronegativity, meaning their electrons are equally shared when bonded
• Polar bonds

  The the greater the difference in EN the more unequal the attraction is, which causes the ends to be partially charged
• Poles


  The charged ends of polar bonds
• Dipole moment

  A measure of polarity
• The larger the dipole moment, the more polar the molecule is
• Dipole moment is the vector sum of all bond polarities that exist within the molecule
• Non-polar molecules have no dipole moment
• VSEPR theory

  • Valence Shell Electron Pair Repulsion
  • focuses on the highest electron density surrounding the central atom of a molecule
• in the VSEPR model, the areas of negative charges repel each other until they are as far away from each other as possible
• electrons repel each other, bonded or not
• Charge Repulsion determines the shape of molecules held together by covalent bonds.
• The VSEPR theory was created because the repulsion of lone and bonded electrons in a molecule limits the possible arrangements of covalent bonds around the central atom
• diatomic elements have no polarities because they have same electronegativities, which means their electrons are equally shared when bonding
• covalent bonds are polar because their electronegativities are different, electrons are unequally shared
• poles


  charged ends of polar bonds
• if the difference is electronegativites are high enough it is polar enough to be an ionic bonds
• all bonds formed between atoms of different elements are polar to some extent
• polar covalent bonds can be nonpolar depending on its geometrical symmetry of its molecule
• polarities of bonds may be high, but if arranged symmetrically, they balance out each other, becoming non polar
• if all outer electronegativities are the same, they are non polar