Ionic and covalent bonds are two major types of chemical bonds that involve different ways of sharing electrons between atoms. Their structures and properties are distinct, which leads to different characteristics in the compounds they form.Ionic Bonds:Ionic bonds are formed when electrons are transferred from one atom to another, resulting in the formation of positively charged ions cations and negatively charged ions anions . These ions are attracted to each other due to their opposite charges, creating an ionic bond. Ionic bonds usually occur between metals and non-metals.Properties of Ionic Compounds:1. High melting and boiling points: Due to the strong electrostatic forces between the ions, ionic compounds have high melting and boiling points.2. Solubility in water: Ionic compounds are generally soluble in water because the polar water molecules can separate the ions.3. Conductivity: Ionic compounds conduct electricity when dissolved in water or in the molten state, as the ions are free to move and carry an electric charge.4. Brittle: Ionic compounds are brittle because when pressure is applied, the ions with similar charges may be forced close to each other, causing repulsion and breaking the crystal lattice.Example of an Ionic Compound: Sodium chloride NaCl is a common example of an ionic compound. It has a high melting point, is soluble in water, conducts electricity when dissolved or molten, and is brittle.Covalent Bonds:Covalent bonds are formed when atoms share electrons to achieve a stable electron configuration. This type of bond typically occurs between non-metal atoms. The shared electrons are attracted to the nuclei of both atoms, holding them together in a covalent bond.Properties of Covalent Compounds:1. Lower melting and boiling points: Covalent compounds have lower melting and boiling points compared to ionic compounds due to weaker intermolecular forces.2. Solubility: Covalent compounds can be soluble or insoluble in water, depending on their polarity.3. Conductivity: Covalent compounds generally do not conduct electricity because they do not have charged particles ions to carry an electric charge.4. Flexibility: Covalent compounds are often more flexible and softer than ionic compounds due to the weaker intermolecular forces.Example of a Covalent Compound: Water H2O is a common example of a covalent compound. It has a relatively low boiling point, is a polar molecule that dissolves many substances, does not conduct electricity in its pure form, and has a flexible structure.In summary, the main difference between ionic and covalent bonds lies in the way electrons are shared or transferred between atoms. This difference leads to distinct structures and properties in the compounds they form, such as differences in melting points, solubility, conductivity, and flexibility.