Naming Polyatomic Ions - Help!?
1. FeSO3 = Iron (III) sulfite
2. Cu(NO3)2 = Copper (II) nitrate
3. Hg2Cl2 = Mercury (II) chloride
4. AgBr = Silver bromide
Please indicate my mistakes and explain what I did wrong and what should I do to correct it. Thank you so much in advance.
Answer:
FeSO3 is Iron (II) sulfite. The charge on SO3 is -2, so the charge on iron should be +2.
Hg2Cl2 is probably mercury (I) chloride, the mercury (I) ion is a polyatomic ion and since your assignment is obviously over that subject, the correct answer is mercury (I), which is Hg2^2+, two mercury atoms, each with a +1 charge, to make the overall charge +2. The other two are correct.
KClO3 = Potassium chlorate (correct)
MgCO3 = Magnesium carbonate (correct)
BaO2 = Barium peroxide (correct)
KO2 = Potassium peroxide (potassium superoxide), the charge of the potassium ion is +1, so O2 should be -1, making it the superoxide, potassium peroxide is K2O2.
SnO2 = Tin (II) peroxide (possible, but better it will be tin (IV) oxide), Tin can have a +4 state, so two O2- ions, makes it the oxide.
Pb(OH2) = Lead (II) hydroxide (correct)
Ni3(PO4)2 = Nickel (II) phosphate (correct)
CuCH3COO = Copper (I) acetate (correct)
N2O4 = Dinitrogen tetraoxide (tetroxide, when a greek prefix ends in a vowel and the name of the ion starts with a vowel, the last letter of the prefix is dropped).
Rb3P = Rubidium phosphorus (III) (rubidium phosphide, the P3- ion is called phosphide)
S8 = Sulfur (correct)
Fe2O = Iron (II) oxide (Iron (I) oxide, which is rare, but as written I will have to name it that, since O in ionic compounds is always -2, so the iron has to be +1). Iron (II) oxide is FeO.
(NH4)2SO3 = Ammonium sulfite (correct)
Ca(MnO4)2 = Calcium manganate (MnO42- is permanganate, so it is potassium permanganate)
PF5 = Phosphorus (V) fluoride (phosphorus pentafluoride, when two nonmetals are combined, the result is a covalent compound, so the roman numeral is dropped and you name it by using the first element name and then using a greek prefix to indicate the number of the second type of element and change its ending from -ine to -ide).
LiH = Lithium hydride (correct)
Ti(HPO4)2 = Titanium (II) monohydrogen phosphate (Titanium (IV) hydrogen phosphate, you drop the mono, it is understood that there is only one hydrogen, and the charge of HPO42- is 2-, so makes the titatium +4.)
cerium (IV) benzoate = Ce(C6H5COO)4 (correct)
potassium hydrogen phthalate = (KH)2(C8H4O4)2 (K2(HC8H4O4)2, the hydrogen belongs to the phthalate, as you wrote it, you are indicating that the hydrogen is covalently bonded to the potassium, which is not possible).
1) It is iron II, not III. Because sulfite has a -2 charge.
2) Correct
3) Correct
4) Correct
See, you're smart. You got it, you just had a minor error that is easy to fix. As long as you understand the concept. Good luck :)
They all look correct, except the iron one.
1) Iron (II) sulfite (the charge of sulfite is 2-, so iron in that equation is 2+)
2) Copper (II) nitrate
3) Mercury chloride (the charge of Cl is 1-, so Hg has to be 1+)
3) Silver bromide
1. iron(II) sulphite [or strictly, iron(II) sulphate(IV)]
2. copper(II) nitrate [or strictly, copper(II) nitrate(V)]
3. mercury(I) chloride [contains (Hg2)2+ ions]
4. silver bromide [or strictly, silver(I) bromide - silver(II) bromide does not exist (as far as I know) but silver(II) fluoride and silver(II) chloride do]
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