Chapter7:ionic compounds Flashcards
Chemical Bond
The force that holds atoms together
Ionic Compound
Formed by metal and nonmetal
Forms a formula unit(formula unit is a ratio)
Form a crystal lattice
The negative are surrounded at all times by a positive and vise verce.
The strength of the bond is related to: latice energy. magnitude of charge, and size
latice Energy
energy needed to break up 1 mole
Cations and their charges
Group 1- 1+
Group 2- 2+
Most 2 block metals can form several cations
vanadium= 2+ 3+ 4+
Silver is always 1+
Cadmium is always 2+
Fe charge
1-
I charge
1-
ClO2-
Chlorite
1-
ClO3-
Chlorite
1-
CN-
Cyanide 1-
CO3 2-
Carbonate
2-
SO3 2-
Sulfite 2-
SO4 2-
Sulfate 2-
PO4 3-
Phosphate 3-
Inorganic Nomenclature
Name of cation
write anion
if cation can have multiple charges add roman numeral
Patterns in Oxyanion Nomenclature
- when there are two oxyanions involving the same element the one with fewer oxygens ends in ‘ite’ and the one with more ends in ‘ate’
- the one with the fewest ends in ‘hypo’ and ends in ‘ite’
- the one with the most starts with ‘per’ and ends in ‘ate’
Metalic bond
Metal cations are surrounded by a sea of delocalized valence electrons
Metals are not covalently bonded, but the attractions between atoms are too strong to be van de waals forces
in metals valence electrons are delocalized throughout the solid.
Alloys
mixture of elements that have metalic properties
Substitutional Alloy
something about the same size substitutes out an atom in a crystal
Interstitial Alloy
tiny atoms fill the spaces inbetween atoms and makes it stronger.
