To determine which of the given compounds is a binary ionic compound, we need to understand what a binary ionic compound is.
A binary ionic compound is composed of two different elements: one metal and one non-metal. The metal donates electrons to the non-metal, forming positive and negative ions that attract each other due to electrostatic forces.
Let's analyze each option to determine if it fits this definition:
A. \( \mathrm{MgCl_2} \):
- Magnesium (Mg) is a metal.
- Chlorine (Cl) is a non-metal.
- The compound consists of magnesium ions (Mg²⁺) and chloride ions (Cl⁻).
- This combination makes \( \mathrm{MgCl_2} \) a binary ionic compound.
B. \( \mathrm{C_6H_{12}O_6} \):
- This compound contains carbon (C), hydrogen (H), and oxygen (O).
- It is not composed of only two different elements.
- It is a covalent compound, not an ionic one.
C. \( \mathrm{CO_2} \):
- This compound consists of carbon (C) and oxygen (O).
- It is composed of two non-metals.
- It forms covalent bonds, not ionic bonds.
D. \( \mathrm{PO_4^{3-}} \):
- This is a polyatomic ion, not a compound by itself.
- It consists of phosphorus (P) and oxygen (O).
- It does not qualify as a binary ionic compound.
E. \( \mathrm{CH_4} \):
- This compound consists of carbon (C) and hydrogen (H).
- It is composed of two non-metals.
- It forms covalent bonds, not ionic bonds.
After examining each option, we can conclude that the correct answer is:
A. \(\mathrm{MgCl_2}\)
This compound is a binary ionic compound because it consists of magnesium ions and chloride ions.
