Ionic Bonding Flashcards
What is the charge of metals in group 1?
+1
What is the charge of metals in group 2?
+2
What is the charge of metals in group 3?
+3
What is the charge of non-metals in group 5?
-3
What is the charge of non-metals in group 6?
-2
What is the charge of non-metals in group 7?
-1
What is the charge of Ag?
+
What is the charge of Cu?
2+
What are the charges of Fe?
-Fe2+
-Fe3+
What is the charge of Pb?
2+
What is the charge of Zn?
2+
What is the charge of hydrogen?
+
(H+)
What is the charge of hydroxide?
- (OH-)
What is the charge of ammonium (NH4)?
+
(NH4+)
What is the charge of carbonate?
2-
(CO3 2-)
What is the charge of nitrate?
-
(NO3-)
What is the charge of sulfate?
2-
(SO4 2-)
Define ionic bonding:
Ionic bonding is the strong electrostatic attraction between positive and negative ions.
Do compounds with giant ionic lattices have high or low melting and boiling points?
Why?
High, because of the strong electrostatic forces between them which take a great deal of energy to seperate.
What is the difference between ‘ide’ and ‘ate’ at the ending of an ion?
‘ide’ means it contains those compounds only, ‘ate’ means there is oxygen (and possible other things) there as well.
What form do ionic compounds tend to be in?
Crystalline.
Why do ionic crystals tend to be brittle?
Any small distortion will bring ions with the same charge along side each other. Like charges repel so the crystalline splits itself.
Ionic substances are soluble in what?
Water.
Ionic compounds are insoluble in what?
Organic solvents.
Can ionic compounds conducts electricity?
Not when they are solid, but yes when they are liquid (molten or an aqueous solution). This happens because ions become free to move around, but are in fixed positions and not free to move around when they’re solid.
What word do you use instead of ‘electrons’ when explaining ionic conductivity?
Ions
