TOPIC 2- Chemical Bonding Flashcards
Force of attraction that binds atom together in a given molecule.
Chemical Bond
two non-metal atoms
covalent
metal and non-metal atom
Ionic
Metal atoms
metallic
indicates the relative sizes and relative orientation of atoms
Space filling model
three dimensional model using spheres and rods.
Ball and stick method
the more electronegative element becomes the partial negative and become the central atom
Polar-Covalent Bonds
atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons
Octet Rule
If elements involved are not from the same group, the central atom is determined by the
Greatest normal covalency
a bond formed when each atom donates an electron
Normal Covalent Bond
only one atom donates the electron pair to form a bond
Dative or Coordinate Covalent Bond
atoms bonded has almost the same electronegativities
Non-polar covalent bond
having different electronegativities
Polar Covalent Bond
The ability of the atom in a molecule to attract electrons itself
Electronegativity
Takes energy to convert elements to atom
Takes energy to create cation
Endothermic
Energy is released by making anion
The formation of the solid releases a huge amount of energy
Exothermic
The energy required to completely separate a mole of a solid ionic compound into its gaseous ions.
Lattice energy
the number of bonds formed by an atom in forming a molecule
Covalency
the number of electrons needed by an atom to have octet of electrons
Normal Covalency
used to determine the number of covalent bonds formed.
Langmuir Formula
When it is necessary to exceed the octet rule for one of several third-row (or higher) elements, assume that the extra electrons should be placed on the central atom
Expanded Octet
it is an indication of the charge an atom would carry if it shared the electrons in a covalent bond equally.
Formal Charge
single bonds
Localized Bonds
Delocalized Bonds
multiple bonds
