Chapter 3 : Ionic Bonding Flashcards
Common polyatomic ions
Carbonate - CO3^2- Sulfate SO4^2- Ammonium - NH4^+ Phosphate - PO4^3- Hydroxide - OH^- Nitrate - NO3^-
-ide
S^2-
N^3-
P^3-
-ite
SO3^2-
NO2^2-
PO3^3-
-ate
SO4^2-
NO3^-
PO4^3-
Ionic bonding
When metallic atoms combine with non metallic atoks to form an ionic lattice
The transfer of electrons from a metal to a non-metal
Why do elements lose gain or share electrons?
To acheive stability of noble gases
Cation
An atom that has lost electrons to become stable and therefore positively charged
Metals
Anion
An atom that has gained electrons to become stable and therefore negatively charged
Non - metals
General name for an ionic compound
Salt, the substance formed when a metal and a non metal react together
Ionic lattices
Form crystals, 3D arrangement of metals and non metals
Held together by electrostatic attraction
Neutrally charged and contains enough anions and cation to balance
Properties of ionic compounds
High melting/boiling points Do not conduct electricity in solid Hard Dissolve in water Conduct electricity in molten/aqueous state(electrolytes) Brittle
Why have ionic compounds got high melting/boiling points?
The electrostatic attraction is very strong and it takes a lot of energy to separate the ionic compounds
Why does an ionic compound conduct in a molten/aqueous state but not solid?
To conduct a substance must contain free floating charged particles to make an electrical current and when dissolved in water or molten the ions are free flowing
Why are ionic compounds hard?
Due to the electrostatic attractions which holds together strongly
Why are ionic compounds brittle?
When something hits an ionic substance the lattics is moved and alike charges line up and repel each other therefore shattering
