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Chapter 2: Q.46E (page 67)

Using the periodic table, predict whether the following chlorides are ionic or covalent:\(SiC{l_4},PC{l_3},CaC{l_2},CsCl,CuC{l_2}{\rm{ and }}CrC{l_3}.\)

Short Answer

Expert verified

\(\begin{aligned}{}SiC{l_4} \to Covalent\\PC{l_3} \to Covalent\\CaC{l_2} \to Ionic\\CsCl \to Ionic\\CuC{l_2}{\rm{ }} \to Ionic\\CrC{l_3} \to Ionic\end{aligned}\)

Step by step solution

01

Step 1. Understanding which elements can make ionic and covalent compound

We know that,

  1. Metals with Non-metals makes ionic compound
  2. Non-metals with Non-metals makes covalent compound
  3. Metalloids with Non-metals also makes covalent compound
02

Step 2.  Analyzing given compounds one by one

\(SiC{l_4} \to \)Consists a metalloid and a non-metal. So, it is covalent.

\(PC{l_3} \to \)Consists only non-metals. So, it is covalent.

\(CaC{l_2} \to \)Consists a metal and a non-metal. So, it is ionic.

\(CsCl \to \)Contains one metal and a non-metal. So, it is ionic.

\(CuC{l_2}{\rm{ }} \to \)Consists a metal and a non-metal. So, it is ionic.

\(CrC{l_3} \to \)Consists a metal and a non-metal. So, it is ionic.

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