Final answer:
Covalent bonds involve the sharing of electrons between nonmetals, are strong, and produce compounds with low melting points and poor electrical conductivity. Ionic bonds arise from the transfer of electrons between metals and nonmetals, creating charged ions that form compounds with high melting points and conductivity in solution.
Step-by-step explanation:
In chemical bonding, covalent bonds and ionic bonds represent two major types of atomic connections that form molecules and compounds. Covalent bonds involve the sharing of electrons between nonmetal elements. This sharing can be equal, leading to non-polar covalent bonds, or unequal, resulting in polar covalent bonds. Notable characteristics of covalent compounds include low melting and boiling points compared to ionic compounds and the fact that they are poor conductors of electricity.
Ionic bonds, on the other hand, form between a metal and a nonmetal and involve the transfer of electrons, creating charged ions. These ions exhibit electrostatic attractions that hold the compound together. Ionic compounds typically have higher melting and boiling points and can conduct electricity when dissolved in water.
Therefore, option a) 'Covalent bonds - Share; Ionic bonds - Steal' and option c) 'Covalent bonds - Nonmetals; Ionic bonds - Metals and nonmetals' are correct. Examples of each type of bond include hydrogen gas (H₂) for covalent bonds, where electrons are shared equally between hydrogen atoms, and sodium chloride (NaCl) for ionic bonds, where electrons are transferred from sodium to chlorine.