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Chapter 2: Q.45E (page 67)

Using the periodic table, predict whether the following chlorides are ionic or covalent: \(KCl,{\rm{ }}NC{l_3},{\rm{ }}ICl,{\rm{ }}MgC{l_2},{\rm{ }}PC{l_5},\)and \(CC{l_4}\).

Short Answer

Expert verified

\(\begin{aligned}{}KCl \to Ionic\\NC{l_3} \to Covalent\\ICl \to Covalent\\MgC{l_2} \to Ionic\\PC{l_5} \to Covalent\\CC{l_4} \to Covalent\end{aligned}\)

Step by step solution

01

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

We know that,

  • Metals with Non-metals makes ionic compound.
  • Non-metals with Non-metals make a covalent compound.
  • Metalloids with Non-metals also make a covalent compound.
02

Step 2: Analysing given compounds one by one

  • \(KCl \to \)Consists of a metal and a non-metal. So, it is ionic.
  • \(NC{l_3} \to \)Consists of only non-metals. So, it is covalent.
  • \(ICl \to \)Consists of only non-metals. So, it is covalent.
  • \(MgC{l_2} \to \)Consists of a metal and a non-metal. So, it is ionic.
  • \(PC{l_5} \to \)Consists of only non-metals. So, it is covalent.
  • \(CC{l_4} \to \)Consists of only non-metals. So, it is covalent.

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Most popular questions from this chapter

Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% 6Li and 92.5% 7Li, which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% 6Li (and the rest 7Li). Calculate the average atomic mass values for each of these two sources.

In the following drawing, the green spheres represent atoms of a certain element. The purple spheres represent atoms of another element. If the spheres of different elements touch, they are part of a single unit of a compound. The following chemical change represented by these spheres may violate one of the ideas of Dalton’s atomic theory. Which one?

Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes:\(\begin{aligned}{}\left( a \right){\rm{ }}{}_3^7Li{\rm{ }}\\\left( b \right){\rm{ }}{}_{52}^{125}Te{\rm{ }}\\\left( c \right){\rm{ }}{}_{47}^{109}Ag{\rm{ }}\\\left( d \right){\rm{ }}{}_7^{15}N{\rm{ }}\\\left( e \right){\rm{ }}{}_{15}^{31}P\end{aligned}\)

Using the periodic table, identify the lightest member of each of the following groups:

(a) noble gases

(b) alkaline earth metals

(c) alkali metals

(d) chalcogens

Using the periodic table, identify the heaviest member of each of the following groups:

(a) Alkali metals

(b) Chalcogens

(c) Noble gases

(d) Alkaline earth metals
See all solutions

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