Which statement correctly contrasts ionic and covalent bonds?

Which statement correctly contrasts ionic and covalent bonds?

• A. Ionic bonds result from a complete transfer of electrons between atoms, forming ions that attract each other.
• B. Covalent bonds involve the transfer of electrons to form charged ions.
• C. Ionic bonds involve sharing electron pairs between atoms.
• D. Covalent bonds produce lattice structures with high melting points.

Answer: (A)

The main idea being tested is how electron arrangement distinguishes ionic and covalent bonds. Ionic bonds form when one atom donates electrons to another, creating ions that attract each other through electrostatic forces. This transfer and resulting charged particles are what hold ionic compounds together, and it’s why they often form crystalline solids with high melting points. This description directly contrasts with covalent bonds, where atoms share electron pairs rather than transfer electrons to form ions. In covalent bonds, electrons are shared to achieve stability, so the atoms stay as neutral entities rather than becoming ions. The bond strength comes from the shared electrons rather than an electrostatic attraction between ions. Because of this fundamental difference, covalent compounds can exist as discrete molecules or network structures with a range of melting points, not inherently defined by lattice formation and strong ionic attractions. The other statements mischaracterize the contrasts. Covalent bonds do not involve transferring electrons to form charged ions. Saying covalent bonds involve sharing electron pairs is correct for covalent bonds, but it doesn’t describe the contrasting idea with ionic bonds. And while some covalent networks have high melting points, lattice structures with high melting points are not the defining contrast between ionic and covalent bonding.

The main idea being tested is how electron arrangement distinguishes ionic and covalent bonds. Ionic bonds form when one atom donates electrons to another, creating ions that attract each other through electrostatic forces. This transfer and resulting charged particles are what hold ionic compounds together, and it’s why they often form crystalline solids with high melting points. This description directly contrasts with covalent bonds, where atoms share electron pairs rather than transfer electrons to form ions.

In covalent bonds, electrons are shared to achieve stability, so the atoms stay as neutral entities rather than becoming ions. The bond strength comes from the shared electrons rather than an electrostatic attraction between ions. Because of this fundamental difference, covalent compounds can exist as discrete molecules or network structures with a range of melting points, not inherently defined by lattice formation and strong ionic attractions.

The other statements mischaracterize the contrasts. Covalent bonds do not involve transferring electrons to form charged ions. Saying covalent bonds involve sharing electron pairs is correct for covalent bonds, but it doesn’t describe the contrasting idea with ionic bonds. And while some covalent networks have high melting points, lattice structures with high melting points are not the defining contrast between ionic and covalent bonding.