Question

5. Determine the oxidation states the elements in the following compounds: a. Nal b. GdCi c. LINO, d. H.Se e. Mg.si f. RbO2, rubidium superoxide 9. HF 6. Complete and balance the following acid-base equations: a. A solution of HCIO, is added to a solution of LIOH b. Aqueous H2SO, reacts with NaOH c. Be(OH)2 reacts with HF gas. 7. Write the molecular, total ionic, and net ionic equations for the following reactions: a. Ca(OH)2(aq) + HC2H4O2(aq) → b. H3PO4(aq) +CaCl(aq) → 8. Write the balanced equation, then outline the step necessary to determine the information requested in each of the following: a. The number of moles and the mass of chlorine, Cla, required to react with 10.0g of sodium metal, Na, to produce sodium chloride, NaCl. b. Then number of moles and the mass of oxygen formed by the decomposition of 1.252g of mercury (II)oxide.

Answer 1

The oxidation state or number usually calculated from the valency of a given element or its ability to gain or lose number of electrons.

a. NaI

Na belongs to group 1 and it has one valence electron , so it has 1 valence electron. Hence, it will lose electrons to attain an oxidation state of +1

I belongs to group 17 and it has 7 valence electrons , hence its valency is also 1 (8-7=1), and it will gain one electron to attain an oxidation state of -1 .

b. GdCl3

Cl belongs to group 17 and it has 7 valence electrons , hence its valency is also 1 (8-7=1), and it will gain one electron to attain an oxidation state of -1

Now let the oxidation state of Gd is x then ,

x + 3 x (-1) = 0

x-3=0

x=+3

Gd has an oxidation state of +3.

c. LiNO3

Oxygen has an oxidation number -2

Li belongs to group 1 and it has one valence electron , so it has 1 valence electron. Hence, it will lose electrons to attain an oxidation state of +1

Let oxidation number of nitrogen is x

Then

+1 + x+ 3x(-2)=0

x+1-6=0

x=+5

Oxidation number of nitrogen is +5

d. H2Se

H belongs to group 1 and it has one valence electron , so it has 1 valence electron. Hence, it will lose electrons to attain an oxidation state of +1

Let oxidation number of Se is x

Then ,

2x(+1) + x =0

+2+x=0

x=-2

The oxidation number of Se is -2

e. Mg2Si

Mg belongs to group 2 and it has two valence electron , hence it has 2 valence electron. Hence, it will lose electrons to attain an oxidation state of +2 .

Let the oxidation number of Si is x

Then ,

2x (+2) + x =0

+4 + x = 0

x= -4

The oxidation state of Si is -4

f. RbO2

Superoxide ion is O₂^- and it has an oxidation state of -1

Let the oxidation state of Rb is x . Then ,

x-1 =0

x=+1

g. HF

Hydrogen loses one electron , hence it has oxidation state of +1

Fluorine gains one electron, hence, it has oxidation state of  -1

NOTE: Due to provided guidelines, I have solved first question for you. If you need more , please post question again.