Why do ionic compounds have high melting points?
(iii) What are ions present in these compounds?

Academic Chemistry NCERT Class 10

The ionic compounds are made up of positive and negative ions. There is a strong force of attraction between the oppositely charged ions, so a lot of heat energy is required to break this force of attraction and melt the ionic compound. Due to this, ionic compounds have high melting points.

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Updated on: 13-Mar-2023

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Why do ionic compounds have higher melting points?
Explain why:(a) Covalent compounds have generally low melting points.(b) Ionic compounds have generally high melting points.
What are ionic compounds? Why do ionic compounds not conduct electricity in the solid-state?
What are ionic compounds? List two properties of these compounds.
Covalent compounds have low melting and boiling point. Why?
(a) Giving one example each, state what are (i) ionic compounds, and (ii) covalent compounds.(b) Compare the properties of ionic compounds and covalent compounds.
What are (i) ionic compounds, and (ii) molecular compounds? Give two examples of each type of compounds.
Why do metals have different melting and boiling points?
(i) Write the electron dot structures for sodium, oxygen, and magnesium.(ii) Show the formation of Na2O and MgO by the transfer of electrons.(iii) What are ions present in these compounds?
Show the formation of Na2O by the transfer of electrons between the combining atoms.Why are ionic compounds usually hard?How is it that ionic compounds in the solid state do not conduct electricity but they do so when in molten state?What type of chemical bonds are present in CCl4?What type of chemical bonds are present in MgCl2?
Giver Reason: Why Carbon can neither form C4+ cations nor C4- anions, but forms covalent compounds and are bad conductors of electricity and have low melting and boiling points?
What are elements and compounds?
Which one of the following property is generally not exhibited by ionic compounds?(a) Solubility in water (b) Electrical conductivity in solid state (c) High melting and boiling points (d) Electrical conductivity in molten state
i. Write the electron dot structures for sodium, oxygen, and magnesium.ii. Show the formation of MgO and Na2O by the transfer of electrons.iii. What are the ions present in these compounds?
Which one of the following properties is not generally exhibited by ionic compounds?(a) Solubility in water(b) Electrical conductivity in solid-state(c) High melting and boiling points(d) Electrical conductivity in a molten state

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