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(a)
Interpretation:
The balanced net ionic equation has to be written for the given reaction.
Concept introduction:
Transition element is one which can form one or more stable ions with a partially occupied d-subshell. Most of the
Ionic equation is an equation in which ions are explicitly shown.
Spectator ions are the ion that appears unchanged on both sides of a reaction arrow.
Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.
To write the net ionic equation, steps mentioned below must be followed.
- 1. Write the balanced molecular equation
- 2. Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.
- 3. Cancel the spectator ions on both sides of the ionic equation.
- 4. Check that charges and number of atoms are balanced in the net ionic equation.
(b)
Interpretation:
The balanced net ionic equation has to be written for the given reaction.
Concept introduction:
Transition element is one which can form one or more stable ions with a partially occupied d-subshell. Most of the transition elements are metals and majority of elements exists in various oxidation states also.
Ionic equation is an equation in which ions are explicitly shown.
Spectator ions are the ion that appears unchanged on both sides of a reaction arrow.
Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.
To write the net ionic equation, steps mentioned below must be followed.
- 1. Write the balanced molecular equation
- 2. Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.
- 3. Cancel the spectator ions on both sides of the ionic equation.
- 4. Check that charges and number of atoms are balanced in the net ionic equation.
(c)
Interpretation:
The balanced net ionic equation has to be written for the given reaction.
Concept introduction:
Transition element is one which can form one or more stable ions with a partially occupied d-subshell. Most of the transition elements are metals and majority of elements exists in various oxidation states also.
Ionic equation is an equation in which ions are explicitly shown.
Spectator ions are the ion that appears unchanged on both sides of a reaction arrow.
Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.
To write the net ionic equation, steps mentioned below must be followed.
- 1. Write the balanced molecular equation
- 2. Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.
- 3. Cancel the spectator ions on both sides of the ionic equation.
- 4. Check that charges and number of atoms are balanced in the net ionic equation.
(d)
Interpretation:
The balanced net ionic equation has to be written for the given reaction.
Concept introduction:
Transition element is one which can form one or more stable ions with a partially occupied d-subshell. Most of the transition elements are metals and majority of elements exists in various oxidation states also.
Ionic equation is an equation in which ions are explicitly shown.
Spectator ions are the ion that appears unchanged on both sides of a reaction arrow.
Net ionic equation is the chemical equation for a reaction which lists only those species participating in the reaction.
To write the net ionic equation, steps mentioned below must be followed.
- 1. Write the balanced molecular equation
- 2. Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.
- 3. Cancel the spectator ions on both sides of the ionic equation.
- 4. Check that charges and number of atoms are balanced in the net ionic equation.
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Chapter 20 Solutions
General Chemistry: Atoms First
- What is the oxidation state of Iron (Fe) in K3[Fe(C2O4)3.3H2O?arrow_forward4. Name the compounds below or give it's structure (the missing one!) (a) Barium phosphate (d) Fe(NO3)3 (b) iodine heptafluoride (e) (c) ethyl 2-ethoxyethan-1-oatearrow_forwardWhat is the balanced net ionic equation of NH3 reacting with Fe(NO3)3 and reacting with CuSO4?arrow_forward
- Give the oxidation state of the metal for each of the following oxides of the first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than oneoxidation state. It is possible to write these compound formulas in the equivalent format MO∙M2O3, to permit estimation of the metal’s two oxidation states.)(a) Sc2O3(b) TiO2(c) V2O5(d) CrO3(e) MnO2(f) Fe3O4(g) Co3O4(h) NiO(i) Cu2Oarrow_forwardWhat is the mass percent of iron in each of the following iron ores: Fe₂O₃, Fe₃O₄, FeS₂?arrow_forwardWrite the overall balanced equation for cobalt (II) nitrate hexahydrate reacting with ammonium carbonate, conecntrated ammonia, hydrogen peroxide, and water to form [Co(NH3)4CO3]NO3.arrow_forward
- Please draw the structure of the possible product for the following reaction, and how does the oxidation state of metal ion formally change in this reaction? (a) trans-Ir(CO)C((PPH3)2 + H2 → (b) H3C-Mn(CO)5 + P(CH3)Ph2 → (no gas evolved)arrow_forwardsniparrow_forwardThe final step in the smelting of FeCuS₂ is Cu₂S(s) +2Cu₂O(s) →6Cu(l) +SO₂(g)(a) Give the oxidation states of copper in Cu₂S, Cu₂O, and Cu.(b) What are the oxidizing and reducing agents in this reaction?arrow_forward
- 1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe*2 and titrated with 36.30 mL of a 0.1052 N solution of K2Cr207. (a) Calculate the percentage of iron (Fe) in the sample. (b) Express the percentage as Fe,03 rather than Fe. Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.arrow_forwardWrite the expression for the equilibrium constant Kc for the following equation. FeO(s) + CO(g) ↔ Fe(s) + CO2(g)arrow_forwardWrite the electron configurations for each of the following elements and its ions:(a) Ti(b) Ti2+(c) Ti3+(d) Ti4+arrow_forward
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