Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl_2 when constructing its Lewis dot structure?

• A. Because BeCl_2 is an ionic compound and does not have covalent bonds.
• B. Because chlorine cannot form double bonds with any element.
• C. Because double bonds would violate the octet rule for chlorine.
• D. Because beryllium does not have enough valence electrons to form double bonds with chlorine.

Answer: (D)

Verified step by step guidance

1. Recall that Lewis structures represent the valence electrons involved in bonding and lone pairs around atoms in a molecule.
2. Identify the valence electrons for beryllium (Be) and chlorine (Cl). Beryllium has 2 valence electrons, and each chlorine has 7 valence electrons.
3. Understand that beryllium tends to form only two single bonds because it has only 2 valence electrons to share, which limits its bonding capacity.
4. Recognize that chlorine atoms typically form one single bond to complete their octet, and forming double bonds with beryllium would require beryllium to share more electrons than it has available.
5. Conclude that double bonds are not drawn between Be and Cl because beryllium cannot expand its valence shell or provide enough electrons to form double bonds, so only single bonds are shown in the Lewis structure.