WS 6.4 Ionic and Covalent Formula Writing
Name:______________________________p.______
1a. Covalent compounds most typically contain:
both metals and nonmetals
only metals
only nonmetals
Examples of covalent compounds include CO2, CO, H2O, CCl4, SO3, SO2, OF2, PCl5, NI3, C6H12O6,
In covalent molecules, electrons are shared in “covalent bonds.”
b. Ionic compounds most typically contain:
both metals and nonmetals
only metals
only nonmetals
Examples of ionic compounds include MgCl2, NaNO3, K2SO4, Li2CO3, AlPO4, Cu2SO4, NH4Cl
The _____________ loses electrons to form a/an _____________ ion,
and the ________________ gains electrons to form a/an ________________ ion.
These ions “stick” together in an “ionic bond”, due to the attractive force between the opposite charges.
Latin Prefixes... for COVALENT compounds only!!!!!:
1 = mono
2 = di
3 = tri
4 = tetra
8 = octa
9 = nona
10 = deca
5 = penta
6 = hexa
7 = hepta
2a. Fill in the missing name or formula for these covalent compounds:
NO2 ______________________________
carbon tetraiodide____________________
NO ______________________________
CBr2I2 ______________________________
P2O5 ______________________________
2b. Fill in the missing name or formula for these ionic compounds:
BaCl2 ______________________________
Al2S3 ______________________________
PbO ______________________________
Fe2S3 ______________________________
ammonium sulfate _______________________
Tin (IV) carbonate ______________________
3. For each compound below, classify it as ionic or covalent, and then fill in the missing name or formula.
NCl3 ____
_______________________
SF6
AlCl3 ____
_______________________
gold (III) sulfide
____
_______________________
____
__________________
CO ____
_______________________
XeF4 ____
CO2 ____
_______________________
Li2O
____
________________________
N2 O4
____
_______________________
NiBr2 ____
_______________________
____________________________
SO2 ____
_______________________
sulfur trioxide
NI3 ____
_______________________
Iron (III) phosphide
____
______________
Calcium phosphate
____
________________
B2O3 ____
_______________________
potassium peroxide
PCl5
____
____
_______________
_______________________
Calcium hydride
____
disilicon hexahydride
____________________
____
______________
____
___________________
Si3N4
____
___________________________
Pb3N4
____
________________________
disulfur decafluoride ____
silver sulfate
____
________________
_____________________
Each chemical equation below shows two elements reacting to form a compound. For each reaction:
a) classify the compound that forms as ionic or covalent.
b) name the compound that forms.
c) state whether the each reacting element will need to gain, lose, or share electrons to bond in the compound.
d) If electrons are lost or gained, indicate which element will gain electrons and which will lose electrons.
4.
S(s)
+
O2(g)
-------> SO2 (g)
+ energy
c/d:
a. __________________
b. ___________________________
5.
2 Na(s) + Cl2(g)
-------> 2 NaCl (s) + energy
c/d:
a. __________________
b. ___________________________
6.
C(s)
+ 2 Cl2(g) ----> CCl4
+ energy
c/d:
a. __________________
b. ___________________________
7.
4 P(s) + 5 O2 (g) -------> P4O10(s) + energy
c/d:
a. __________________
b. ___________________________
8. (Demo!)
3 Br2 + 2 Al(s) -------> 2 AlBr3 (s) + energy
c/d:
a. __________________
b. ___________________________
9.
F2 + S(s)
------> SF4(g) + S2F4(g) + SF6(g)
+ energy
c/d:
a. __________________
b. ________________________
10.
________________________
3 F2 + 2 Fe(s) ------> 2 FeF3 (s) + energy
________________________
c/d:
a. __________________
b. ___________________________
11.
6 Na(s) + N2(g)
-------> 2 Na3N(s) + energy
c/d:
a. __________________
b. ___________________________
12.
O2(g)
+ 2 Sn(s)
-------> 2 SnO(s) + energy
a. __________________
b. ___________________________
c/d: