Question

Identify the compound that contains ionic bonds
• \( \mathrm{MgF_2} \)
• \( \mathrm{CH_2Cl_2} \)
• \( \mathrm{CH_2FCOOH} \)
• \( \mathrm{SiCl_4} \)

• A. \( \mathrm{MgF_2} \)
• B. \( \mathrm{CH_2Cl_2} \)
• C. \( \mathrm{CH_2FCOOH} \)
• D. \( \mathrm{SiCl_4} \)

Hint:

A quick way to identify ionic compounds:
• Metal + Non-metal \(\Rightarrow\) Usually ionic
• Non-metal + Non-metal \(\Rightarrow\) Usually covalent Fluorides of metals are commonly ionic because fluorine is highly electronegative.

Answer 1

The Correct Option is A

Concept: Chemical bonds are mainly classified into:
• Ionic bonds
• Covalent bonds An ionic bond is formed by the complete transfer of electrons from one atom to another. Generally:
• Metals lose electrons and form positive ions (cations).
• Non-metals gain electrons and form negative ions (anions). The electrostatic attraction between oppositely charged ions forms an ionic bond. On the other hand, covalent bonds are formed by sharing of electrons between atoms, usually between non-metals. Thus, compounds formed between a metal and a highly electronegative non-metal are generally ionic.

Step 1: Analyze Option (1): \( \mathrm{MgF_2} \) Magnesium (\(\mathrm{Mg}\)) is a metal belonging to Group 2 of the periodic table. Fluorine (\(\mathrm{F}\)) is a highly electronegative non-metal belonging to Group 17. Magnesium loses two electrons: \[ \mathrm{Mg \rightarrow Mg^{2+} + 2e^-} \] Each fluorine atom gains one electron: \[ \mathrm{F + e^- \rightarrow F^-} \] Thus: \[ \mathrm{Mg^{2+} + 2F^- \rightarrow MgF_2} \] The bond formed here is due to electrostatic attraction between ions. Hence, \( \mathrm{MgF_2} \) is an ionic compound. Therefore, Option (1) is correct.

Step 2: Analyze Option (2): \( \mathrm{CH_2Cl_2} \) This compound contains:
• Carbon
• Hydrogen
• Chlorine All these elements are non-metals. Non-metals generally form covalent bonds by sharing electrons. Therefore, \( \mathrm{CH_2Cl_2} \) contains covalent bonds, not ionic bonds. Hence, Option (2) is incorrect.

Step 3: Analyze Option (3): \( \mathrm{CH_2FCOOH} \) This is an organic compound containing:
• Carbon
• Hydrogen
• Oxygen
• Fluorine All these are non-metals. The bonding occurs through sharing of electrons. Thus, the compound is covalent in nature. Hence, Option (3) is incorrect.

Step 4: Analyze Option (4): \( \mathrm{SiCl_4} \) Silicon tetrachloride consists of silicon and chlorine atoms. Even though chlorine is highly electronegative, silicon forms covalent bonds with chlorine through electron sharing. Therefore, \( \mathrm{SiCl_4} \) is covalent. Hence, Option (4) is incorrect. Final Conclusion: Among the given compounds, the one containing ionic bonds is: \[ \boxed{\mathrm{MgF_2}} \] Hence, the correct answer is: \[ \boxed{(1)} \]