Electronic Configuration and Iron Reactions

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Questions and Answers

Which process does not require a catalyst?

Conversion of SO2 into SO3

Hydrogenation of oils

Preparation of ammonia in industry

Detection of glucose using Fehling solution (correct)

Which of the following is not an alloy formed from metal elements?

Stainless steel

Ferro manganese

Cementite (correct)

Dure alumin

Which compounds change color to red upon heating due to thermal decomposition?

FeCl2 – Fe3O4 – FeCO3 (correct)

Fe2(SO4)3 – 2Fe2O3.3H2O – FeS

FeCl3 – Fe3O4 – FeCO3

Fe(OH)3 – FeO – FeSO4

Which acid reacts with iron to produce only iron II salt?

X and yields iron III and water Signup and view all the answers

Which element cannot form the compound XCl3?

Sc Signup and view all the answers

Which alloy is produced due to the substitution of an atom with another of the same size and chemical properties?

Al - Ni - Al - Cu Signup and view all the answers

Which electronic configuration represents a non-transition element?

ns2, (n-1)d10 Signup and view all the answers

What process aims to increase the iron percentage in the ore?

Concentration – crushing Signup and view all the answers

For the production of car springs, vanadium is added to iron in which type of furnace?

Electric or open hearth furnaces Signup and view all the answers

Which statement is true regarding the characteristics of transition elements?

They form alloys with steel used in car springs. Signup and view all the answers

What type of reaction occurs when hot iron combines with non-metals?

Direct and may produce iron II or III salts. Signup and view all the answers

How can you differentiate between the alloys Zn + Fe and Zn + Cu?

By diluted HCl, the first dissolves and copper precipitates in the second Signup and view all the answers

Which element in the fifth column of the periodic table has the maximum magnetic moment in its oxide?

X2O5 Signup and view all the answers

The product of a reaction between iron and acids depends primarily on what factor?

Type and concentration of the acid. Signup and view all the answers

Which of the following elements shows variable oxidation states?

Ag Signup and view all the answers

When heating mixed oxides in the presence of a reducing agent at 500 °C, which compound is formed?

Iron Signup and view all the answers

Which of the following processes produces two distinct gases?

Heating iron II oxalate in air. Signup and view all the answers

Which compound has all of its d-orbitals paired with electrons?

TiSO4 Signup and view all the answers

What is the important role of a catalyst in a chemical reaction?

Preparing a path with low energy for the reaction Signup and view all the answers

What indicates that an acid is dilute when added to iron filings with no explosion occurring upon ignition?

Diluted sulfuric acid. Signup and view all the answers

In the reactions Fe2O3 ← Fe3O4 → FeO, what do the reactions represent respectively?

Reduction - oxidation Signup and view all the answers

What is the result of adding diluted sulphuric acid to iron II oxide?

It dissolves and iron III oxide precipitates Signup and view all the answers

Which oxidation state is commonly seen in coinage metals?

+1 Signup and view all the answers

Which solution will appear blue?

CuCl2 Signup and view all the answers

What is the atomic number of an element with the electronic configuration ns, (n-1)d where x=6 and n=5?

44 Signup and view all the answers

How many single electrons are present in CoF6 ion?

3 Signup and view all the answers

Which element is more suitable for manufacturing aircraft bodies due to its properties?

Low density, high hardness, high corrosion resistance Signup and view all the answers

What is the correct sequence for converting siderite into iron II chloride?

Roasting – Reduction - adding conc.HCl Signup and view all the answers

What is the formula for the oxide formed when an element from the 1st transition series loses an equal number of electrons from (4s) and (3d)?

TiO Signup and view all the answers

Study Notes

Electronic Configuration and Transition Metals

Non-transition elements have an electronic configuration of ns², (n-1)d¹⁰.
Transition metals can form alloys with other metals, such as steel (iron alloy), bronze (copper alloy), and brass (copper and zinc alloy).
Transition metals can have variable oxidation states, which means they can lose different numbers of electrons to form ions. This property contributes to the formation of colored compounds and catalytic activity.

Iron Reactions and Compounds

Iron reacts directly with non-metals, such as oxygen, sulfur, and halogens.
Iron (II) salts and iron (III) salts can be produced depending on the reaction conditions and the type of acid used.
Iron oxides (FeO, Fe₂O₃, Fe₃O₄) can be reduced to iron by using a suitable reducing agent at high temperatures, such as in a blast furnace.
Iron oxides can exhibit different magnetic properties depending on their structure.
Iron reacts with acids, producing hydrogen gas. The type and concentration of acid used determines the product of the reaction, which can be iron (II) or iron (III) salts.
Iron (II) salts are often green in color, while iron (III) salts are often yellow or brown.
Iron (II) salts are readily oxidized to iron (III) salts in the presence of air or strong oxidizing agents.
Concentrated sulfuric acid is a strong dehydrating agent and can react with iron to produce iron (III) sulfate and sulfur dioxide gas.

Alloys

Alloys are mixtures of metals that are often designed to enhance the properties of the individual metals.
Steel is an alloy of iron and carbon, often with other elements such as chromium, nickel, and manganese.
Bronze is an alloy of copper and tin.
Brass is an alloy of copper and zinc.
Alloys for specific applications:
- Steel for car springs.
- Aluminum alloys for aircraft bodies.
- Nickel-chromium alloys for heating coils.

Oxidation and Reduction Reactions

Oxidation is the gain of oxygen or the loss of electrons.
Reduction is the loss of oxygen or the gain of electrons.
Iron can undergo oxidation to form iron oxides.
Iron oxides can be reduced to iron by using a reducing agent, such as carbon.
Oxidation and reduction occur simultaneously in a redox reaction, where one species is oxidized and another species is reduced.

Catalyst

A catalyst is a substance that speeds up a chemical reaction without being consumed in the process.
Catalysts work by providing an alternate pathway for the reaction with lower activation energy.
Catalysts can be used in several industrial processes, such as the Haber-Bosch process for ammonia production and the contact process for sulfuric acid production.

Identifying and Differentiating Iron Compounds

FeCl₂ is green and dissolves in dilute HCl.
FeCl₃ is yellow and dissolves in dilute HCl.
FeO is black and dissolves in dilute HCl, producing a green solution.
Fe₂O₃ is black and dissolves in dilute HCl, producing a yellow solution.
Fe₃O₄ is black and dissolves in dilute HCl, producing a mixture of green and yellow solutions.

Transition Metal Properties

Transition metals often have a variable oxidation state, meaning they can exist in more than one ionic form.
Transition metals can form colorful compounds.
Transition metals often have paramagnetism, meaning they are weakly attracted by a magnetic field.

Cobalt (Co) Compounds

Cobalt (II) ions (Co²⁺) have a d⁷ electronic configuration and exhibit varying colors depending on the ligand coordination environment.

Scandium (Sc)

Scandium (Sc) is a relatively unreactive metal. It does not form colored compounds.

Titanium (Ti)

Titanium (Ti) is a strong, lightweight metal that is often used in the aerospace industry.
Titanium is also biocompatible and is used in implants for joint replacements.

Manganese (Mn)

Manganese (Mn) is a transition metal that is used in the production of steel and other alloys.
Manganese is also used as a catalyst in several chemical reactions.

Siderite (FeCO₃)

Siderite is a mineral that contains iron carbonate. It is a relatively common mineral and is mined as a source of iron.

Iron Oxide Reduction

Iron oxides can be reduced to iron by using coke (carbon) as a reducing agent in a blast furnace.

Cobalt (Co) Compounds and their Properties

Cobalt (II) sulfide (CoS) is a black solid that is insoluble in water.
Cobalt (II) chloride (CoCl₂) is blue in color.
Cobalt (II) sulfate (CoSO₄) is red in color.

Iron Compounds and their Properties

Iron (II) chloride (FeCl₂) is a green-colored salt that is soluble in water.
Iron (III) chloride (FeCl₃) is a yellow-brown colored salt that is soluble in water.
Iron (II) oxide (FeO) is a black, insoluble solid. It is also known as ferrous oxide.
Iron (III) oxide (Fe₂O₃) is a red-brown, insoluble solid. It is also known as ferric oxide.
Iron (II) sulfate (FeSO₄) is a greenish-blue colored salt that is soluble in water.
Iron (III) sulfate (Fe₂(SO₄)₃) is a pale yellow-brown colored salt that is soluble in water.

Alloys with Special Properties

Stainless steel is an alloy of iron, chromium, and nickel. It is resistant to corrosion and is often used in kitchen utensils and appliances.
Duralumin is an alloy of aluminum, copper, and manganese. It is lightweight and strong and is often used in aircraft construction.
Ferro-manganese is an alloy of iron and manganese. It is used in the production of steel.

Metal Properties and uses

Aluminum is a light and reactive metal. It is often used in the manufacture of cans, foils, and other packaging materials.
Nickel is a hard and durable metal. It is used in various applications, such as coins, jewelry, and batteries.

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Description

Explore the principles of electronic configuration in transition metals and understand the various reactions and compounds of iron. This quiz delves into the properties of transition metals, their oxidation states, and how iron interacts with non-metals and acids. Test your knowledge on these vital concepts in chemistry.