covalent bond
chemical bond that results from sharing valence electrons
molecule
forms when 2 or more atoms bond covalently
lewis structure
representation of the arrangements of electrons in a molecule
sigma bond
single covalent bonds; occurs when the pair of shared electrons is in an area centered between the two atoms
pi bond
forms when parallel orbitals overlap and share electrons
endothermic reaction
occurs when a greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the product
exothermic reaction
occurs when more energy is released during product bond formation than is required to break bonds in the reactants
oxyacid
any acid that contains hydrogen and an oxyanion
coordinate covalent bond
froms when one atom donates a pair of electrons to be shared with an atom or ion that needs two electrons to become stable
resonance
condition that occurs when more than one valid Lewis structure exists for the same molecule
structural formula
a molecular model that uses symbols and bonds to show relative positions of atoms; can be predicted for many molecules by drawing the Lewis structure
hybridization
a process in which atomic orbitals are mixed to form new, identical hybrid orbitals
VSEPR model
is based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom
polar covalent bond
type of bond that forms when electrons are not equally shared
VSEPR
Valence Shell Electron Pair Repulsion
tetrahedral
trigonal pyramidal
trigonal planar
linear
bent
lewis structure of NH3
lewis structure of CCl4
Lewis structure of H2O
chloric acid
chlorous acid
nitrous acid
nitric acid
Naming oxyacids
identitify the polyatomic ion, if ending is -ate then drop the ending and add -ic acid to its name. If ending is -ite then drop ending and add -ous acid.
Example : H2SO4 --> sulfate --> drop ending and add -ic acid ----->sulfuric acid
Hydrochloric acid
HCl
Hydrobromic Acid
HBr