Test Objectives: Ionic & Metallic Bonding
o Know the definition of a chemical bond
o Recognize that the driving force of chemical bond formation is the formation of an octet
(stable valence electron configuration just like a noble gas)
o Know that the attraction of opposite charges is the force of attraction in an ionic bond
o Be able to describe ionic bond formation in terms of an electron transfer process
o Metals transferring electrons to non-metals
o Draw Lewis dot structures to show how electrons are transferred to form ionic
compounds
o Given two elements be able to determine the chemical formula of the ionic compound formed
when they react
o Be able to use oxidation numbers to help explain the formula
o Be able to show how electrons are transferred between all the atoms
o Be able to explain why energy is absorbed when a bond is broken & energy is released when a
bond is formed
o Ionic reactions are exothermic
o Bond breaking is endothermic
o Know that metals tend to form cations (+ ions) & non-metals tend to form anions
(- ions) & together they form ionic compounds
o Know that binary ionic compounds contain 2 different elements (but not necessarily only 2
atoms)
o Know that ionic compounds form crystal lattice structures and be able to explain in general
terms what these are
o Be able to calculate which of several compounds is more ionic than the others based on
electronegativity differences
o Know that bonds having an electronegativity difference greater than 1.7 are
considered to be ionic
o the higher the electronegativity difference the greater the ionic character
o less than 1.7 the compound is not considered to be ionic
o Be able to discuss the physical properties of ionic compounds
o Be able to explain why ionic compounds will not conduct electricity in the solid (crystalline)
phase but will conduct electricity in the molten state or in solution
o Be able to draw Lewis Dot structures for ions & ionic compounds
o Define the term oxidation number
o Know the typical oxidation numbers for elements in groups 1,2, 13-18
o Know the crisscross method for determining subscripts in binary ionic compound formulas
o Know how to name ionic compounds using the stock system when given the chemical formula
o Know how to write ionic compound formulas when given their stock system
o Example: Cr(NO3)3 = Chromium (III) nitrate
o Know that the names of binary ionic compounds end in –ide
o know polyatomic ions are groups of atoms covalently bonded that have a + or – charge that
enables them to form ionic compounds
o be able to recognize polyatomic ions
o be able to use Table E to determine names, formulas & charge of polyatomic ions
o know that the endings of ployatomic ions end in –ite, -ate & -ide
o know that polyatomic ions ending in –ate have more oxygen than those ending in –ite (ex:
SO4 = sulfate; SO3 = sulfite)
o be able to explain how metallic bonds are formed in terms of valence electrons & temporary
cations
o freely flowing valence electrons moving from one overlapping valence shell to the next
o be able to explain what is meant by the term “sea of mobile electrons”
o be able to discuss the physical properties of metals
o explain the properties of metals in terms of delocalized electrons
o know that the number of delocalized electrons  strength & hardness of the metal 
o know why metals are malleable & ductile while ionic compounds are not
o ionic compounds from crystals that will shatter if struck hard