- 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?
(a) The electronic configuration of Sodium: 2,8,1 and of Oxygen: 2,6. Hence 2 atoms of sodium donate one electron each to oxygen to get stable 2 [Na+] and The oxygen, in turn, get stable by gaining two electrons and form O2-.
The formation of Na2O by the transfer of electrons between the combining atoms is given below:
(b) Ionic compounds are usually hard because they have oppositely charged ions that attract each other strongly and forms a crystal structure.
(c) Solid ionic compounds are made up of ions but do not conduct electricity because they are held together by a strong electrostatic force of attraction that restricts movement. In the molten state, the crystal structure is broken and ions move freely. Therefore, it conducts electricity.
(d) 4 covalent bonds are present in carbon tetrachloride (CCl4).
(e) Ionic bonds are present in MgCl
2 where one Mg atom donates 2 electrons to 2 chlorine atoms and become stable.
Related Articles
- What are ionic compounds? Why do ionic compounds not conduct electricity in the solid-state?
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- What type of chemical bonds are present in a solid compound which has a high melting point, does not conduct electricity in the solid state but becomes a good conductor in the molten state?
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- Why do ionic compounds have high melting points?(iii) What are ions present in these compounds?
- What type of bonds are present in hydrogen chloride and oxygen?
- (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.
- State one major difference between covalent and ionic bonds and give one example each of covalent and ionic compounds.
- What are (i) ionic compounds, and (ii) molecular compounds? Give two examples of each type of compounds.
- (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?
- What are ionic compounds? List two properties of these compounds.
- What type of bonds are present in water molecule? Draw the electron-dot structure of water (H2O).
- (a) Give the electron configuration of magnesium and chlorine.(b) Write the electron-dot structures of magnesium and chlorine atoms. (c) Describe the formation of magnesium chloride from magnesium and chlorine by the transfer of electrons. (d) What type of chemical bonds are present in the magnesium chloride formed? (e) Why do such compounds have high melting points?
- 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?
- (a) Write the electron arrangement in (i) a magnesium atom, and (ii) an oxygen atom.(b) How many electrons are there in the valence shell of (i) a magnesium atom, and (ii) an oxygen atom. (c) Show on a diagram the transfer of electrons between the atoms in the formation of MgO. (d) Name the solvent in which ionic compounds are generally soluble. (e) Why are aqueous solutions of ionic compounds able to conduct electricity?
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