name each of the following ionic compounds by stock system... couldn't find these in the list.
a)NaCl
b) KF
c) CaS
d) Co(NO3)2
e)FePO4
f)Hg2SO4
g) Hg3(PO4)2
You couldn't find them, probably because there is no reason to get confused with the answers, at least for some of them. I would name them
sodium(I) chloride **see note
potassium(I) fluoride ** see note
calcium(II) sulfide **see note
cobalt(II) nitrate (could confuse)
iron(III) phosphate (could confuse)
mercury(II) sulfate (could confuse)
mercury(II) phosphate (could confuse)
**The I is not necessary because Na, K, and Ca are known only in the +1 or +2(for Ca) states. Frankly, I don't know if placing a I or II there is incorrect or not.
Kf ionic name
a) Sodium chloride (NaCl)
b) Potassium fluoride (KF)
c) Calcium sulfide (CaS)
d) Cobalt(II) nitrate (Co(NO3)2)
e) Iron(III) phosphate (FePO4)
f) Mercury(I) sulfate (Hg2SO4)
g) Mercury(II) phosphate (Hg3(PO4)2)
To name each of the ionic compounds by the Stock system, we need to determine the oxidation states (or charges) of the elements involved in each compound.
a) NaCl:
Na is a group 1 element, so it has an oxidation state of +1. Cl is a group 7 element, so it has an oxidation state of -1. Since Na and Cl have opposite charges, they balance each other out in a 1:1 ratio, giving us an ionic compound named Sodium chloride.
b) KF:
K is a group 1 element, so it has an oxidation state of +1. F is a group 7 element, so it has an oxidation state of -1. Similarly to NaCl, K and F balance each other out in a 1:1 ratio, resulting in an ionic compound named Potassium fluoride.
c) CaS:
Ca is a group 2 element, so it has an oxidation state of +2. S is a group 6 element, so it has an oxidation state of -2. Their charges balance each other out in a 1:1 ratio, giving us an ionic compound named Calcium sulfide.
d) Co(NO3)2:
To name this compound, we need to determine the oxidation state of each individual element. NO3 is a polyatomic ion, known as nitrate, with a charge of -1. Since there are two NO3 groups, their total charge is -2. With Co having an overall charge of +2 to balance the negatively charged nitrate ions, the compound is named Cobalt(II) nitrate.
e) FePO4:
Fe is a transition metal, and its oxidation state can vary. In this case, Fe has an oxidation state of +2. PO4 is a polyatomic ion, known as phosphate, with a charge of -3. To balance the charges, we need two phosphate ions to match the +2 charge of Fe, resulting in an ionic compound named Iron(II) phosphate.
f) Hg2SO4:
Hg is a transition metal, and in this compound, it has an oxidation state of +2. SO4 is a polyatomic ion, known as sulfate, with a charge of -2. Since Hg2 has a 2+ charge, we only need one sulfate ion to balance the charges, resulting in an ionic compound named Mercury(I) sulfate.
g) Hg3(PO4)2:
Similar to the previous compound, Hg is a transition metal with an oxidation state of +2. PO4 is a polyatomic ion, known as phosphate, with a charge of -3. To balance the charges of Hg2+ and PO4^3-, we need two phosphate ions and three mercury ions, resulting in an ionic compound named Mercury(II) phosphate.