Interpretation:
The oxidation states of all the atoms in CO3 2 - should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
Interpretation:
The oxidation states of all the atoms in NO3 - should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
Interpretation:
The oxidation states of all the atoms in PO4 3 - should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
Interpretation:
The oxidation states of all the atoms in SO4 2 - should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
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Introductory Chemistry: A Foundation
- A transition metal X forms an oxide of formula X2O3. It is found that only 50% of X atoms in this compound are in the +3 oxidation state. The only other stable oxidation states of X are +2 and +5. What percentage of X atoms are in the +2 oxidation state in this compound?arrow_forwardYou have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246% nitrogen by mass. The ionic compound in solution B consists of potassium, chromium, and oxygen; chromium has an oxidation state of + 6 and there are 2 potassiums and 1 chromium in the formula. The masses of the solutes in each of the solutions are the same. When the solutions are added together, a blood-red precipitate forms. After the reaction bas gone to completion, you dry the solid and find that it has a mass of 331.8 g. a. Identify the ionic compounds in solution A and solution B. b. Identify the blood-red precipitate. c. Calculate the concentration (molarity) of all ions in the original solutions. d. Calculate the concentration (molarity) of all ions in the final solution.arrow_forwardWhy is it that when something gains electrons, it is said to be reduced? What is being reduced?arrow_forward
- Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) Al(s)+F2(g) (b) Al(s)+CuBr2(aq) (single displacement) (c) P4(s)+O2(g) (d) Ca(s)+H2O(l) (products are a strong base and a diatomic gas)arrow_forwardCommercial cold packs and hot packs are available for treating athletic injuries. Both types contain a pouch of water and a dry chemical. When the pack is struck, the pouch of water breaks, dissolving the chemical, and the solution becomes either hot or cold. Many hot packs use magnesium sulfate, and many cold packs use ammonium nitrate. Write reactions to show how these strong electrolytes break apart when they dissolve in water.arrow_forwardChromium has been investigated as a coating for steel cans. The thickness of the chromium film is determined by dissolving a sample of a can in acid and oxidizing the resulting Cr3+ to Cr2O72 with the peroxydisulfate ion: S2O82(aq) + Cr3+(aq) + H2O(l) Cr2O72(aq) + SO42(aq) + H+(aq) (Unbalanced) After removal of unreacted S2O82 an excess of ferrous ammonium sulfate [Fe(NH4)2(SO4)26H2O] is added, reacting with Cr2O72 produced from the first reaction. The unreacted Fe2+ from the excess ferrous ammonium sulfate is titrated with a separate K2Cr2O7 solution. The reaction is: H+(aq) + Fe2+(aq) + Cr2O72(aq) Fe3+(aq) + Cr3+(aq) + H2O(l) (Unbalanced) a. Write balanced chemical equations for the two reactions. b. In one analysis, a 40.0-cm2 sample of a chromium-plated can was treated according to this procedure. After dissolution and removal of excess S2O82, 3.000 g of Fe(NH4)2(SO4)26H2O was added. It took 8.58 mL of 0.0520 M K2Cr2O7 solution to completely react with the excess Fe2+. Calculate the thickness of the chromium film on the can. (The density of chromium is 7.19 g/cm3)arrow_forward
- . For each of the following unbalanced oxidation-reduction chemical equations, balance the equation by inspection, and identify which species is the reducing agent. a.Fe(s)+O2(g)Fe2O3(s)b.Al(s)+Cl2(g)AlCl3(s)c.Mg(s)+P4(s)Mg3P2(s)arrow_forwardWrite the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction? a. b. c.arrow_forward5 items multiple choice 35. What is the oxidation number of chlorine in HClO4? A. +1 B. +6 C. +7 D. -8 36. How many electrons were lost/gained in the following redox reaction 2K2Cr2O7 + 2H2O + 3S 4KOH + 2Cr2O3 + 3SO2? A. 2 B. 3 C. 6 D. 12 37. In the reaction, Fe2+ + Cr2O72- Fe3+ + Cr3+, which is involved in oxidation? A. Fe B. Cr2O7 C. Cr D. O 38. Which of the following half reactions in CORRECT? A. I2 + 1e- I- B. Cu2+ + 2e- Cu+ C. Zn2+ + 2e- Zn D. 2H+ + 2e- H2- 39. The following are examples of spontaneous reactions EXCEPT A. Water freezes spontaneously below 0ᵒC, and ice melts spontaneously above 0ᵒC. B. Heat flows from a colder one but reverse happens spontaneously. C. A waterfall runs downhill, but never up spontaneously. D. A lump of sugar spontaneously dissolves in a cup of coffee, but dissolved sugar does not spontaneously reappear in its original form. 40. For an equilibrium process, the free-energy change ∆G is A. less than zero. B. greater than zero. C. equal to…arrow_forward
- In nitrous acid (HNO2) the oxidation state of N is. . 1. +3 2. -3 3. +5 4. +6 а. 1 O b. 2 O c. 3 O d. 4arrow_forwardassign oxidation states to the elements in the following compounds or ions: a. KNO3 b.AlH3 c.NH4^+ d. H2PO4^-arrow_forwardGive the oxidation number of an atom in the compound: a. Mn in Mn04- b. Cr in CrO2 2+ c. Fe in Fe304 d. K in KCIO3 e. B in Na2B407arrow_forward
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