In which type of bond does an element with only one electron in its outer shell lose that electron?

The correct response is based on the nature of ionic bonds. An ionic bond typically forms when an element has one electron in its outer shell and loses that electron to achieve a more stable electronic configuration. This process often involves a metal atom losing its outermost electron and becoming positively charged, known as a cation. The atom that gains this electron, often a non-metal, becomes negatively charged (anion).

This transfer of electrons leads to the formation of an electrostatic attraction between the positively and negatively charged ions, resulting in a strong ionic bond. The stability achieved by losing or gaining electrons is a key characteristic of ionic bonding, making it a fundamental concept in chemistry.

In contrast, covalent bonds involve the sharing of electron pairs between atoms, hydrogen bonds are weak interactions between molecules containing hydrogen, and polar bonds arise from unequal sharing of electrons between atoms due to differences in electronegativity, but they do not involve the complete transfer of an electron as seen in ionic bonds.