Naming Ionic Compounds
CsI
Cesium Iodide
What's the difference between a cation and anion?
Cation - pawsitive
anion - negative
Potassium Sulfide
K2S
Why are metals good conductors?
delocalized/free moving electrons
How many atoms are present in acetate CH2O2
5
Hg2O
Mercury (I) oxide
Ionic structures are typically held together by
Lattice structure
Silicon Bromide
SiBr4
Oxidation number of carbon
+ or - 4
The electron sea model refers to what?
The bonding of metallic bonds with delocalized electrons
Rb3P
Rubidium Phosphide
A compound (X4Y3) with Y's oxidation number of -4 means the oxidation of X must be what?
+3
Iron (III) Oxide
Fe2O3
Define ductile
Ability to create thin sheets of a material -- still retains it's properties when being hit with a hammer for example (doesn't break/crumble)
A compound (2 or more elements) with an overall charge
Polyatomic Ion
FePO4
Iron (III) Phosphate
Why do we use roman numerals?
Transition metals oxidation numbers change depending on what they're bonded to! So roman numerals show the oxidation number of a transition metal in a given compound
Be(CH3COO)2
Beryllium acetate
What kinds of bonds allow electricity to flow through them in the liquid phase?
BOTH metallic and ionic
A shorthand method used to represent one atom of a specific element is a
Chemical symbol
Manganese (I) Nitride
There are many distinctive and shared properties between metallic and ionic compounds. Name 1 similarity and 1 difference.
Similarity: Both conduct electricity in the liquid phase
Difference:
- Metallic has delocalized electrons, while ionic doesn't, metallic things are shiny, ionic things are brittle, etc.
Ammonium Hydroxide
NH4OH
What's wrong with Si2Ra4
Cation goes first! Should be Ra4Si2
Define delocalized electrons
Electrons which are able to move freely