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Chapter 10: Q72 E (page 592)

Identify the following substances as ionic, metallic, covalent network, or molecular solids: Substance A is malleable, ductile, conducts electricity well, and has a melting point of\({\rm{1135 ^\circ C}}\). Substance B is brittle, does not conduct electricity as a solid but does when molten, and has a melting point of\({\rm{2072 ^\circ C}}\). Substance C is very hard, does not conduct electricity, and has a melting point of\({\rm{3440 ^\circ C}}\). Substance D is soft, does not conduct electricity, and has a melting point of\({\rm{185 ^\circ C}}\).

Short Answer

Expert verified

The substances are:

A is metallic, B is ionic, C is covalent and D is molecular solid.

Step by step solution

01

To identify the following substances 

Metallic solid :-

(a) Electrical Conductivity :- Good conductors of heat and electricity

(b) Melting Point :- Melting point depends strongly on electronic configuration.

(c) Appearance :- Malleable, ductile and lustrous.

(d) Water solubility :- Insoluble

Covalent solid :-

(a) Electrical Conductivity :- Poor conductors of heat and electricity

(b) Melting Point :- High

(c) Appearance :- Hard, ductile and lustrous.

(d) Water solubility :- Insoluble

Molecular solid :-

(a) Electrical Conductivity :- Poor conductors of heat and electricity

(b) Melting Point :- Low

(c) Appearance :- Soft and dull surface.

(d) Water solubility :- Insoluble

Ionic solid :-

(a) Electrical Conductivity :- Poor conductors of heat and electricity

(b) Melting Point :- relatively high Melting point.

c) Appearance :- Hard, brittle and dull

d) Water solubility :- Soluble

Hence we can say that A is metallic, B is ionic, C is covalent and D is molecular solid.

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Most popular questions from this chapter

Identify the type of crystalline solid (metallic, network covalent, ionic, or molecular) formed by each of the following substances:

\(\begin{aligned}{\rm{(a)Si}}{{\rm{O}}_{\rm{2}}}\\{\rm{(b)KCl}}\\{\rm{(c)Cu}}\\{\rm{(d)C}}{{\rm{O}}_{\rm{2}}}\\{\rm{(e)C(diamond)}}\\{\rm{(f)BaS}}{{\rm{O}}_{\rm{4}}}\\{\rm{(g)N}}{{\rm{H}}_{\rm{3}}}\\{\rm{(h)N}}{{\rm{H}}_{\rm{4}}}{\rm{\;F}}\\{\rm{(i)}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{OH}}\end{aligned}\)

Elemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in the phase diagram

  1. On the phase diagram, label the gas and liquid regions.
  2. Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase.
  3. If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. Label the diamond phase.
  4. Circle each triple point on the phase diagram.
  5. In what phase does carbon exist at 5000 K and 108 Pa?
  6. If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 106 Pa, which phase transition occurs, if any?

The edge length of the unit cell for nickel is 0.3524 nm. The density of Ni is \(8.90\;{\rm{g}}/{\rm{c}}{{\rm{m}}^3}\). Does nickel crystallize in a simple cubic structure? Explain.

Cadmium sulfide, sometimes used as a yellow pigment by artists, crystallizes with cadmium, occupying one-half of the tetrahedral holes in a closest packed aligned of sulfide ions. What is the formula of cadmium sulfide? Explain your answer.

Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) to answer the following questions:

(a) Select the Solid, Liquid, Gas tab. Explore by selecting different substances, heating and cooling the systems, and changing the state. What similarities do you notice between the four substances for each phase (solid, liquid, gas)? What differences do you notice?

(b) For each substance, select each of the states and record the given temperatures. How do the given temperatures for each state correlate with the strengths of their intermolecular attractions? Explain.

(c) Select the Interaction Potential tab, and use the default neon atoms. Move the Ne atom to the right and observe how the potential energy changes. Select the Total Force button, and move the Ne atom as before. When is the total force on each atom attractive and large enough to matter? Then select the Component Forces button, and move the Ne atom. When do the attractive (van der Waals) and repulsive (electron overlap) forces balance? How does this relate to the potential energy versus the distance between atoms graph? Explain.
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