(a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?

Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO₄ (b) sulfurous acid, H₂SO₃ (c) strontium sulfide, SrS

Determine the oxidation number of sulfur in each of the following substances: (d) hydrogen sulfide, H₂S

Determine the oxidation number of sulfur in each of the following substances: (e) Locate sulfur in the periodic table in Exercise 4.47; what region is it in?

Determine the oxidation number of sulfur in each of the following substances: (f) Which region(s) of the periodic table contains elements that can adopt both positive and negative oxidation numbers?

Determine the oxidation number for the indicated element in each of the following substances: (a) S in SO₃ (b) Ti in TiCl₄

Determine the oxidation number for the indicated element in each of the following substances: (c) P in AgPF₆

Determine the oxidation number for the indicated element in each of the following substances: (d) N in HNO₃

Determine the oxidation number for the indicated element in each of the following substances: (e) Pt in PtCl₄ (f) O in OF₂.

Determine the oxidation number for the indicated element in each of the following substances: (f) Cl in NaClO4.

Which element is oxidized, and which is reduced in the following reactions? (a) N₂(g) + 3 H₂(g) → 2 NH₃(g)

Which element is oxidized, and which is reduced in the following reactions? (b) 3 Fe(NO₃)₂(aq) + 2 Al(s) → 3 Fe(s) + 2 Al(NO₃)₃(aq)

Which element is oxidized, and which is reduced in the following reactions? (c) Cl₂(aq) + 2 NaI(aq) → I₂(aq) + 2 NaCl(aq) (d) PbS(s) + 4 H₂O₂(aq) → PbSO₄(s) + 4 H₂O(l)

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P4(s) + 10 HClO(aq) + 6 H₂O(l) → 4 H₃PO₄(aq) + 10 HCl(aq) (b) Br₂(l) + 2 K(s)→ 2 KBr(s) (c) CH₃CH₂OH(l) + 3 O₂(g) → 3 H₂O(l) + 2 CO₂(g) (d) ZnCl₂(aq) + 2 NaOH(aq) → Zn(OH)₂(s) + 2 NaCl(aq)

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid (b) chromium with hydrobromic acid (c) tin with hydrochloric acid (d) aluminum with formic acid, HCOOH.

Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel (b) dilute sulfuric acid with iron

Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium (d) acetic acid, CH₃COOH, with zinc.

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate (b) zinc metal is added to a solution of magnesium sulfate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate (c) hydrochloric acid is added to gold metal

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) hydrogen gas is bubbled through a solution of silver nitrate.

The metal cadmium tends to form Cd²⁺ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl₂(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO₃)(aq), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations.

The metal cadmium tends to form Cd²⁺ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl₂(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO₃)(aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:

Br₂(aq) + 2 NaI(aq) → 2 NaBr(aq) + I₂(aq)

Cl₂(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br₂(aq)

(a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:

Br₂(aq) + 2 NaI(aq) → 2 NaBr(aq) + I₂(aq)

Cl₂(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br₂(aq)

(b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed.

(a) Is the number of moles of ions present in a solution an intensive or an extensive property?