When considering the formation of ionic compounds from the elements sodium, calcium, neon, phosphorus, and chlorine, we first need to identify which of these elements can form ions.
Sodium (Na) is an alkali metal and tends to lose one electron to form a positive ion, Na+.
Calcium (Ca) is an alkaline earth metal and typically loses two electrons, forming a positive ion, Ca2+.
Neon (Ne) is a noble gas and is generally unreactive under normal conditions, so it does not form ions.
Phosphorus (P) can gain or share electrons. In ionic compounds, it often gains three electrons to form a negative ion, P3-.
Chlorine (Cl) is a halogen and typically gains one electron to form a negative ion, Cl–.
Considering these ions:
- From sodium: Na+
- From calcium: Ca2+
- From phosphorus: P3-
- From chlorine: Cl–
We can now determine potential ionic compounds:
- Sodium Chloride: Na+ + Cl– → NaCl
- Calcium Chloride: Ca2+ + 2Cl– → CaCl2
- Calcium Phosphide: Ca2+ + P3- → Ca3P2
In conclusion, the primary ionic compounds formed from these elements are sodium chloride (NaCl), calcium chloride (CaCl2), and calcium phosphide (Ca3P2).