how can we represent sodium chloride (NaCl) in electron dot structure?
The correct answer and explanation is:
Sodium chloride (NaCl) is an ionic compound formed between sodium (Na) and chlorine (Cl). In electron dot notation, we represent the valence electrons of the atoms involved. Here’s how to represent NaCl in electron dot structure:
- Sodium (Na):
Sodium belongs to Group 1 of the periodic table, meaning it has one electron in its outermost shell. In the electron dot structure, sodium will be represented with a single dot around the symbol Na, indicating the one valence electron. Na: • (The dot represents the single electron in the outermost shell) - Chlorine (Cl):
Chlorine belongs to Group 17, which means it has seven valence electrons. In the electron dot structure, chlorine will have seven dots around the symbol Cl, representing its seven valence electrons. Cl: • • • • • • • - Ionic Bond Formation:
Sodium, being a metal, loses its single valence electron to achieve a stable configuration, typically similar to the noble gas neon (Ne). When sodium loses its electron, it becomes a positively charged ion (Na⁺). Chlorine, being a nonmetal, has a strong tendency to gain one electron to achieve the stable electron configuration of the noble gas argon (Ar). When chlorine gains an electron, it becomes a negatively charged ion (Cl⁻). - Representation of the Ionic Bond:
After the transfer of the electron from sodium to chlorine, the two ions are held together by electrostatic attraction, forming an ionic bond. The electron dot structure for NaCl shows sodium as Na⁺ (with no dots) and chlorine as Cl⁻ (with eight dots, representing its filled valence shell).
In summary, the electron dot structure for sodium chloride can be written as:
Na: • → Na⁺ and Cl: • • • • • • • → Cl⁻
This illustrates the transfer of the electron from sodium to chlorine, resulting in the formation of NaCl, with sodium becoming positively charged and chlorine negatively charged. The resulting ionic bond holds the two ions together.