4.1.3

Electrolysis of a Binary Compound in Molten State

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Electrolysis of a Binary Compound in the Molten State

Electrolysis splits molten binary compounds using electricity. Positive ions go to the cathode (reduction), forming metal. Negative ions go to the anode (oxidation), forming non-metal.

Introduction to electrolysis of binary compounds

Introduction to electrolysis of binary compounds

  • Electrolysis splits molten binary compounds into elements using electricity.
    • Binary compounds contain two elements, often metal and non-metal.
    • Molten state means the compound is melted to allow ions to move.
  • Electricity causes positive ions to go to cathode, negative ions go to anode.
Movement of ions during electrolysis

Movement of ions during electrolysis

  • Positive ions (cations) move to the cathode (negative electrode).
  • Negative ions (anions) move to the anode (positive electrode).
  • Electrolysis requires ionic movement for chemical changes at electrodes.
    • This movement allows prediction of products formed at each electrode.
Predicting products at the electrodes

Predicting products at the electrodes

  • At the cathode, cations gain electrons (reduction) to become atoms or molecules.
  • At the anode, anions lose electrons (oxidation) to become atoms or molecules.
  • For a molten binary compound, expect metal at cathode and non-metal at anode.
    • Example: Electrolysis of molten sodium chloride produces sodium metal and chlorine gas.
Example of electrolysis of molten sodium chloride (NaCl)

Example of electrolysis of molten sodium chloride (NaCl)

  • Sodium ions (Na+) move to cathode, gain electrons, form sodium metal (Na).
  • Chloride ions (Cl-) move to anode, lose electrons, form chlorine gas (Cl2).
  • This method produces pure sodium and chlorine through molten NaCl electrolysis.
Summary and importance

Summary and importance

  • Electrolysis of molten binary compounds separates elements by electricity.
  • It is possible to predict products based on ion movement and charge at electrodes.
  • This technique is essential in metal extraction and chemical industries.
Jump to other topics
1

States of Matter

1.1

Solids, Liquids, & Gases

1.1.1States of Matter - Solids, Liquids & Gases1.1.2Structure of Solids, Liquids & Gases1.1.3Changes of State1.1.4The Effects of Temperature & Pressure1.1.5Kinetic Theory1.1.6Kinetic Theory - Effects of Temperature & Pressure
1.2

Diffusion

1.2.1Diffusion1.2.2The Effect of Relative Molecular Mass
2

Atoms, Elements & Compounds

2.1

Elements, Compounds & Mixtures

2.1.1Differences Between Elements, Compounds & Mixtures
2.2

Atomic Structure & the Periodic Table

2.2.1The Structure of the Atom2.2.2Relative Charge, Mass & Atomic Numbers2.2.3Electronic Configuration of Elements
2.3

Isotopes

2.3.1Isotopes2.3.2Electronic Configuration of Isotopes2.3.3Calculating Relative Atomic Mass
2.4

Ions & Ionic Bonds

2.4.1Properties of Ionic Compounds - Structure & Bond2.4.2Formation of Ions & Ionic Bonds2.4.3Formation of Ionic Bonds - Metals & Non-Metals2.4.4Ionic Bonds2.4.5Ionic Compounds2.4.6Giant Lattice Structure of Ionic Compounds
2.5

Simple Molecules & Covalent Bonds

2.5.1Covalent Bonds2.5.2Formation of Covalent Bonds2.5.3Structure & Properties of Simple Molecules2.5.4Covalent Bonds in Simple Molecules2.5.5Properties of Simple Molecular Compounds
2.6

Giant Covalent Structures

2.6.1Giant Covalent Structures - Graphite2.6.2Giant Covalent Structures - Diamond2.6.3Uses of Graphite & Diamonds2.6.4Giant Covalent Structures - Silicon Oxide2.6.5Similarity Between Diamond & Silicon Oxide
2.7

Metallic Bonding

2.7.1Metallic Bonding2.7.2The Properties of Metals
3

Stoichometry

3.1

Formulae

3.1.1Understanding Formulae3.1.2Empirical Formula3.1.3Stoichiometry - Formulae, Word & Symbol Equations3.1.4Deduce & Write Ionic Compound Formulas
3.2

Relative Masses of Atoms & Molecules

3.2.1Relative Atomic Mass3.2.2Relative Molecular Mass (Mr)3.2.3Calculating Reacting Masses
3.3

The Mole & the Avogadro Constant

3.3.1Introducing Moles3.3.2Amounts of Substances3.3.3Moles & Equations3.3.4Calculations Involving Gases3.3.5Calculating Stoichiometric Reacting Masses3.3.6Calculating the Moles of Solute3.3.7Calculating Empirical Formula3.3.8Chemical Equations3.3.9Percentage Yield3.3.10Calculating Yield3.3.11Percentage Purity
4

Electrochemistry

4.1

Electrolysis

4.1.1Electrolytic Process4.1.2Electrolysis Examples4.1.3Electrolysis of a Binary Compound in Molten State4.1.4Electroplating4.1.5Transfer of Charge During Electrolysis4.1.6Electrolysis of Aqueous Solutions4.1.7Electrolysis of Copper Sulfate4.1.8Electrolysis of Halide Compounds4.1.9Half-Equations4.1.10Combustion of Hydrocarbons
4.2

Hydrogen–Oxygen Fuel Cells

4.2.1Fuel Cells4.2.2Hydrogen Fuel Cells4.2.3Comparing Hydrogen-Oxygen Fuel Cells & Petrol
5

Chemical Energetics

5.1

Exothermic & Endothermic Reactions

5.1.1Energy Conservation5.1.2Exothermic Reactions5.1.3Endothermic Reactions5.1.4Energy Change of a Reaction5.1.5Reaction Pathway Diagrams5.1.6Calculating Enthalpy Change
6

Chemical Reactions

6.1

Physical & Chemical Changes

6.1.1Difference btwn Physical & Chemical Changes
6.2

Rate of Reaction

6.2.1Collision Theory & Rate of Reaction6.2.2Factors Affecting Rate of Reaction6.2.3Investigating Rate of Reaction by Change in Mass6.2.4Investigating Rate - Formation of a Gas6.2.5Evaluating Methods to Investigate Reaction Rates
6.3

Reversible Reactions & Equilibrium

6.3.1Reversible Reactions6.3.2Conditions & Equilibrium6.3.3Dynamic Equilibrium6.3.4Changing Conditions - Heat & Water Effects6.3.5Factors Affecting Equilibria - Temperature6.3.6Factors Affecting Equilibria - Pressure6.3.7Factors Affecting Equilibria - Concentration6.3.8The Haber Process6.3.9The Haber Process Equation
6.4

Redox

6.4.1Redox Reactions6.4.2Redox Reactions - OIL RIG6.4.3Examples of Redox Reactions6.4.4Identifying Redox Reactions6.4.5Identifying Redox Reactions by Colour Changes6.4.6Testing for Oxidising & Reducing Agents
7

Acids, Bases & Salts

7.1

The Characteristic Properties of Acids & Bases

7.1.1Acids & Alkali7.1.2Reactions of Metals with Acids7.1.3Reactions of Bases with Acids7.1.4Reactions of Carbonates with Acids7.1.5Identifying Acids7.1.6Properties & Effects of Acids7.1.7Properties of Bases - Reactions with Acids & Salts7.1.8Properties of Alkalis & Indicators7.1.9Strong vs Weak Acids7.1.10Strong vs Weak Bases7.1.11Understanding Universal Indicator Paper7.1.12Acids, Bases & the Neutralisation Reaction
7.2

Oxides

7.2.1Oxides7.2.2Amphoteric Oxides - Reacting with Acids & Bases
7.3

Preparation of Salts

7.3.1Soluble Salts7.3.2Preparing Soluble Salts7.3.3Solubility of Salts7.3.4Preparing Insoluble Salts & Crystallisation
8

The Periodic Table

8.1

Arrangement of Elements

8.1.1The Periodic Table8.1.2Metals & Non-Metals
8.2

Group I Properties

8.2.1Alkali Metals8.2.2Alkali Metals - Properties8.2.3Reactivity of Alkali Metals8.2.4Alkali Metals & Water
8.3

Group VII Properties

8.3.1The Halogens - Properties8.3.2The Halogens - Colours & States8.3.3The Halogen - Displacement 18.3.4The Halogen - Displacement 2
8.4

Transition Elements

8.4.1Transition Metals8.4.2Transition Metals - Special Properties
8.5

Noble Gases

8.5.1Noble Gases - Properties
9

Metals

9.1

Properties of Metals

9.1.1Physical Properties of Metals9.1.2Chemical Properties of Metals9.1.3Metal Oxides
9.2

Uses of Metals

9.2.1Uses of Metals: Aluminium & Copper
9.3

Alloys & Their Properties

9.3.1Alloys9.3.2Alloys 29.3.3Alloys & their Uses in Everyday Life9.3.4Structural Diagrams of Alloys9.3.5Structure of Alloys & Their Strength
9.4

Reactivity Series

9.4.1Metals - Reactivity Series & Reactivity9.4.2Order of Reactivity9.4.3Reactivity of Metals
9.5

Corrosion of Metals

9.5.1Corrosion9.5.2Preventing Corrosion
9.6

Extraction of Metals

9.6.1Extraction of Metals9.6.2Extracting Iron9.6.3Extracting Aluminium from Bauxite
10

Chemistry of the Environment

10.1

Water

10.1.1Testing & Treating Water10.1.2Testing Water Purity Using Melting Point10.1.3Water from Natural Sources10.1.4Potable Water
10.2

Fertilisers

10.2.1Nitrogen & Fertilisers
10.3

Air Quality & Climate

10.3.1Gases in the Atmosphere10.3.2Common Atmospheric Pollutants10.3.3Consequences of Atmospheric Pollutants10.3.4Strategies to Reduce Pollution Effects10.3.5Photochemical Reactions10.3.6Car Engines, Nitrogen Oxides, & Converters
11

Organic Chemistry

11.1

Formulae, Functional Groups & Terminology

11.1.1Formula of a Molecule11.1.2General Formulae of Organic Compounds11.1.3Functional Groups11.1.4Homologous Series11.1.5Saturated & Unsaturated Organic Compounds11.1.6Structural Formula11.1.7Structural Isomers
11.2

Naming Organic Compounds

11.2.1Drawing Displayed Formulae11.2.2Naming Organic Compounds - Unbranched11.2.3Naming Unbranched Esters from Alcohols & Acids11.2.4Naming Structural Formulae
11.3

Fuels

11.3.1Fossil Fuels11.3.2Methane as the Main Constituent of Natural Gas11.3.3Fuels & Hydrocarbons11.3.4Petroleum - A Mixture of Hydrocarbons11.3.5Fractional Distillation11.3.6Fractions11.3.7Uses of Fractions - Fuels
11.4

Alkanes

11.4.1Alkanes11.4.2Properties of Alkanes11.4.3Substitution Reactions of Alkanes with Chlorine
11.5

Alkenes

11.5.1Alkenes11.5.2Shortest Alkenes11.5.3Reactions of Alkenes11.5.4Types of Alkene Reactions11.5.5Cracking11.5.6Testing Saturated & Unsaturated Hydrocarbons11.5.7Properties of Alkenes - Addition Reactions
11.6

Alcohols

11.6.1Alcohols11.6.2Smallest Alcohols11.6.3Fermentation11.6.4Steam11.6.5Fermentation vs Hydration of Ethene11.6.6Manufacture of Ethanol: Fermentation & Hydration11.6.7Combustion of Ethanol11.6.8Uses of Ethanol - Solvent & Fuel11.6.9Advantages & Disadvantages of Ethanol Manufacture
11.7

Carboxylic Acids

11.7.1Carboxylic Acids11.7.2Smallest Carboxylic Acids11.7.3Reactions of Carboxylic Acids11.7.4Formation of Ethanoic Acid
11.8

Polymers

11.8.1Polymers11.8.2Problems With Polymers11.8.3Polymers & Plastics11.8.4Problems with Plastics11.8.5Condensation Polymerisation11.8.6Condensation Polymerisation Examples11.8.7Addition Polymerisation11.8.8Addition Polymerisation Examples11.8.9Structure of Polymers11.8.10Natural Polyamides - Proteins & Amino Acids
12

Experimental Techniques & Chemical Analysis

12.1

Experimental Design

12.1.1Measurement Tools12.1.2Mixtures12.1.3Understanding Solvents, Solutes, & Solutions12.1.4Separating Mixtures12.1.5Distillation12.1.6Advantages & Disadvantages of Experimental Methods
12.2

Acid-base Titrations

12.2.1Acid-base Titrations
12.3

Chromatography

12.3.1Chromatography12.3.2Paper Chromatography12.3.3Chromatogram
12.4

Separation & Purification

12.4.1Purity12.4.2Methods of Separation & Purification
12.5

Identification of Ions & Gases

12.5.1Testing Aqueous Cations 112.5.2Testing Aqueous Cations 212.5.3Testing Cations - Flame Tests12.5.4Testing Cations12.5.5Testing for Aqueous Cations12.5.6Testing Anions - Sulfates12.5.7Testing Anions - Nitrates12.5.8Testing Gases - Hydrogen12.5.9Testing Gases - Oxygen12.5.10Testing Gases - Carbon Dioxide12.5.11Testing Gases - Chlorine12.5.12Identifying Gases

Practice questions on Electrolysis of a Binary Compound in Molten State

Can you answer these? Test yourself with free interactive practice on Seneca — used by over 10 million students.

  1. 1
    Why must a binary compound be in a molten state for electrolysis to occur effectively?Multiple choice
  2. 2
    A scientist melts a binary compound made of metal X and non-metal Y for electrolysis. If metal X forms positive ions and non-metal Y forms negative ions, what is the expected product at the cathode?Multiple choice
  3. 3
    During the electrolysis of molten sodium chloride, sodium ions move to the cathode. What process happens at the cathode that forms sodium metal?Multiple choice
  4. 4
    In an industrial process, molten compound AB is electrolysed. The cathode produces pure metal A. Which statement best explains why metal A is found at the cathode?Multiple choice
  5. 5
    A chemist observes that at the anode during electrolysis of a molten binary compound, a gas forms. Which inference about this gas is most consistent with the principles of electrolysis?Multiple choice
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Electrolysis Examples

Electroplating