chapter 2.2

• molecules: a substance made up of two or more atoms
• chemical bond: any form of attraction between atoms that holds them together
• valence electrons: an electron in the outer shell of atom, which can participate in the formation of a chemical bond, highest energy level of the atom
• molecular orbital: a merged orbital that contains electrons from two or more atoms (hybrid orbital)
• covalent bond: a chemical bond that forms between two non-metal atoms by sharing electrons, sharing of electrons, shown with a straight line, electrons are often shared unequally
• double bond: a type of covalent bond that occurs when two pairs of electrons are shared between two atoms
• molecules tend to be more stable when they have a higher electronegativity
• a polar covalent bond is a bond between two atoms with a difference in electronegativity
• in many bonds the electrons are not shared equally, this is called a bonding pair
• electronegativity: the ability to attract electrons
• ionic bonds: formed when electrons are transfered from one atom to another with opposite charges, dotted lines
• electrostatic attraction: the attraction between oppositely charged ions in a solution
• d-: negative charge
• d+: postive charge
• non-polar covalent bonds: equal sharing of electrons
• whenever the difference is greater than 0.5 it is considered significant
• dipoles: a pair of electrons that are attracted to the positive and negative ends of a molecule
• onchps: levels of electronegativity, nonpolar covalent bonds
• vander waals interactions: weak intermolecular forces between molecules that are not covalently bonded