Chemistry Practicals Class 10

Properties of Ionic Compounds

  • Teach science experiments in a gamified way
  • Boost conceptual clarity and knowledge retention
  • Aligned with National Education Policy 2020
  • Helpful in getting NAAC accreditation
  • CBSE, ICSE, and state boards aligned curricula
  • Engaging simulations with easy-to-teach instructions

About Simulation

  • Through this interactive simulation, you will have the opportunity to explore the properties of salts in a safe and engaging virtual environment.
  • You can identify the physical state of sodium chloride, potassium iodide, and barium chloride within the simulation.
  • You will be able to determine the melting points of the salts through direct heating as part of the simulation.
  • Throughout the simulation, you can investigate the solubility of the salts in different solvents such as water, petrol, and kerosene.
  • By engaging in the simulation, you can conduct flame tests to observe any characteristic colours emitted by the salts.

Chemistry Practical Class

  • Additionally, you can explore the conductivity of electricity in solutions of the salts using a simple circuit setup within the simulation.

Simulation Details

Duration – 30 Minutes
Easily Accessible
Languages – Odia & English
Platforms – Android & Windows


When two or more oppositely charged ions are held together due to the presence of electrostatic force, the resulting bond formed is termed an ionic bond. Simply, a chemical bond will be formed among two atoms by transferring one or more electrons from one atom to another.

In a reaction between metals and non-metals, metals generally lose electrons (form cations) to complete their octet, while non-metals gain electrons (form anions) to complete their octet. Metals and non-metals generally react to form ionic compounds.

Due to the presence of oppositely charged ions, ionic compounds are held strongly by the electrostatic force of attraction. Prominent properties of ionic compounds are:

  • Physical Appearance: There is a strong force of attraction between positive and negative ions, which makes ionic compounds solid and not easily breakable.
  • Melting and Boiling Points: Ionic compounds have a significant force of attraction between them. So, it requires a large amount of energy to break the ionic bonds between the atoms. That’s why ionic compounds have a higher melting and boiling point.
  • Solubility: Ionic compounds can dissolve in polar solvents. Water, methanol, and formamide are some examples of polar solvents. Also, ionic compounds are insoluble or barely soluble in non-polar solvents like chloroform, hydrocarbons, etc.
  • Electric Conductivity: Ionic compounds don’t conduct electricity in solid states, but they do conduct in the molten state. As you know, the conduction of electricity involves a transfer of charge from one point to another.
  • In solid-state, the movement of ions is not possible, and thus, ionic compounds can’t conduct electricity. However, ionic compounds in the molten state can conduct electricity because their electrostatic forces of attraction get overcome by the heat released.
  • They are brittle in nature.

Watch this video to learn more about chemistry.

Requirements for this Science Experiment

  • Sodium chloride
  • Potassium iodide
  • Barium chloride
  • Water
  • Kerosene oil
  • Bunsen burner
  • Spatula
  • Graphite electrodes
  • Bulb
  • Battery
  • Plug Key
  • Connecting wires

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