Explanation Analyze and contrast the properties of crystalline and amorphous solids. Arrangement of components : Crystalline solids have a regular, compact and well-defined orderly arrangement of their components in a long range order whereas amorphous solids do not have such an orderly arrangement instead a random arrangement of components is observed. Intermolecular forces: Crystalline solids have relatively strong intermolecular forces than amorphous solids. Melting point: Crystalline solids melt at definite temperature whereas amorphous solids do not. Cleavage: Crystalline solids give clear cleavage when cut with a sharp object whereas amorphous solids give irregular cut. Rigidity and deformation : Crystalline solids are very rigid and not compressible and high force is needed to deform them. Amorphous solids are non-rigid and can be deformed by applying moderate force. Isotropy and anisotropy: Crystalline solids exhibit anisotropy whereas amorphous solids exhibit isotropy. Crystalline and amorphous solids do differ widely in the arrangement of their respective components. The structural variation results in the difference between their respective properties. Since the components are regularly and orderly stacked in a crystalline solid, the intermolecular forces are stronger and sustained. In amorphous solid the intermolecular forces are weaker due to disorderly arrangement. Each component in a crystalline solid is considered as a “unit cell” which is the simplest and basic unit of a crystal. The unit cell repeats itself orderly in a regular fashion and builds a plane known as lattice plane. A crystal has several lattice planes likes this arranged orderly. The strong intermolecular forces exist in the crystalline solids provides resistance to deform to a certain extent by mild forces. In case of amorphous solids, deformation occurs easily than in the crystalline solids. The evenly distributed intermolecular forces make crystalline solids to melt at definite temperature whereas in amorphous solids there is no such existence and hence melt over a varying range of temperature. For example, glass, being an amorphous solid melts gradually over a certain range of temperatures around 1400 o to 1500 o C but NaCl a crystalline solid has definite melting point of 801 o C . Crystalline solids when cut with a sharp object, the neatly stacked unit cells in the lattice plane gives clean cleavage to the crystal. Amorphous solids do lack such feature and gives irregular cleavage. Crystalline solids are generally anisotropic that mean their properties differ with respect to directions but amorphous solids are isotropic and exhibit same properties in all directions. Analyze and contrast the properties of ionic solids and molecular solids. Appearance: Ionic solids are hard and brittle. Molecular solids are soft to some extent. Intermolecular forces: The intermolecular force exist in ionic solids is known as “electrostatic force of attraction” whereas in molecular solids it is known as “Van der Waals forces”. Density: Ionic solids are denser than the molecular solids. Melting point: Melting point of ionic solids is high whereas that of molecular solids is low to moderately high. Mechanical strength: Ionic solids are rigid, brittle and cannot be deformed easily whereas molecular solids are not very rigid and can be deformed. Solubility: Ionic solids are soluble in polar solvents and insoluble in non-polar solvents. Molecular solids are soluble either in polar or non-polar solvents. Conductivity: Ionic solids have good conductivity but molecular solids have poor conductivity. Both ionic and molecular solids belong to the category of crystalline solids. Ionic solids have ions neatly stacked in an orderly fashion of a long range order. In molecular solids, molecules are regularly and orderly arranged in a long range order. Ionic solid consists of ions of opposite charges that are cation and anion. These two ions are held together as a compound by strong intermolecular force called electrostatic force of attraction. Molecular solids consists molecules as their components. The like molecules are held together by weak Van der Waals forces such as London dispersion forces, dipole-dipole forces and hydrogen bonding. Among these three, “hydrogen bonding” is the strongest. The strong intermolecular force is responsible for the rigidity, brittleness and high density of the ionic solids and such instance is not found in molecular solids so they are not hard, brittle and dense as ionic solids and deformed quite easily. Electrostatic attraction is the strongest known force. The ions in the unit cells must be held together so tightly and strongly that high energy is required to break the lattice points in the crystal of ionic solids. Hence, they melt under high temperature. But in case of molecular solids the weak Van der waals force does not make their lattice sites so strong that, low to moderate temperature is enough to break the lattice sites. Hence, they melt under low to moderate temperature itself. Ionic solids shows good conductivity because, when in dissolved and molten state they exist as individual ions of positive and negative charges which are highly mobile enough to exhibit conductivity. Many ionic solids in aqueous state are good electrolytes. But molecular solids are made of molecules which are almost neutral and unable to exhibit conductivity

Bundle: Chemistry, Loose-Leaf Version, 10th + OWLv2, 4 terms (24 months) Printed Access Card

10th Edition

ISBN: 9781337537933

Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

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Crystal Structures

Solids are present all around us. They have different properties and applications. Diamond and graphite are two well-known solids. Diamond is the hardest material in the world and is used in making jewelry. Graphite on the other hand is soft. The lead of…

Question

Chapter 10, Problem 4RQ

Interpretation Introduction

Interpretation:

Differences between crystalline solid and amorphous solid, ionic solid and molecular solid, molecular solid and network solid, metallic solid and network solid have to be explained.

Concept introduction:

Solids constitute the major part of the matter in the universe. Beneath the earth and above the sky in our Universe, as well as in our everyday life, solids can be found. Solids do have such a profound significance since the beginning of the Universe and human evolution.

A solid is anything that is firm and stable in shape. Physics and Chemistry do provide clear cut explanation for the structure of solids. The firm and dense nature of solids is due to the strong intermolecular forces between their components which are nothing but molecules or ions.

On the basis of the arrangement of the components of a solid, there are two distinct types of solids viz., crystalline solids and amorphous solids. These two types differ in the arrangement of their respective components and so in their properties.

Crystalline solids have their own sub-classification. The types of solids can be summarized as follows –

Crystalline solids have well-defined regular, compact, orderly arrangements of their components in a very long range order. They are termed as true solids. Amorphous solids lack such well defined arrangement of its components thus disordered or random arrangement does exist in them. They are termed as pseudo solids or super cooled liquids.

Ionic solids, molecular solids, covalent solids and metallic solids are the types of crystalline solids. The components that are found to be arranged in regular, compact, three dimensional patterns are ions, then it is an ionic solid.

If molecules are arranged in such a fashion, then it is molecular solid whereas metal atoms are arranged in such a manner, it is metallic solid. In Covalent solids the components are atoms bonded by covalent bond repetitively and thus forms huge network form of solid.

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Chapter 10 Solutions

Bundle: Chemistry, Loose-Leaf Version, 10th + OWLv2, 4 terms (24 months) Printed Access Card

Ch. 10 - What are intermolecular forces? How do they differ...Ch. 10 - Define the following terms and describe how each...Ch. 10 - Compare and contrast solids, liquids, and gases.Ch. 10 - Prob. 4RQ Ch. 10 - What is a lattice? What is a unit cell? Describe a...Ch. 10 - What is closest packing? What is the difference...Ch. 10 - Describe, in general, the structures of ionic...Ch. 10 - Prob. 9RQ Ch. 10 - Prob. 10RQ Ch. 10 - Compare and contrast the phase diagrams of water...

Ch. 10 - It is possible to balance a paper clip on the...Ch. 10 - Consider a sealed container half-filled with...Ch. 10 - Explain the following: You add 100 mL water to a...Ch. 10 - Prob. 4ALQ Ch. 10 - Prob. 5ALQ Ch. 10 - Why do liquids have a vapor pressure? Do all...Ch. 10 - Prob. 7ALQ Ch. 10 - What is the vapor pressure of water at 100C? How...Ch. 10 - Prob. 9ALQ Ch. 10 - Prob. 10ALQ Ch. 10 - Prob. 11ALQ Ch. 10 - Why is N2 a gas at room temperature? Explain why...Ch. 10 - Prob. 13ALQ Ch. 10 - In the diagram below, which lines represent the...Ch. 10 - Prob. 16Q Ch. 10 - Prob. 17Q Ch. 10 - The conductivity of silicon is enhanced by doping....Ch. 10 - Atoms are assumed to touch in closest packed...Ch. 10 - Define critical temperature and critical pressure....Ch. 10 - Prob. 21Q Ch. 10 - Describe what is meant by a dynamic equilibrium in...Ch. 10 - Prob. 23Q Ch. 10 - Prob. 24Q Ch. 10 - Prob. 25Q Ch. 10 - Prob. 26Q Ch. 10 - When wet laundry is hung on a clothesline on a...Ch. 10 - You have three covalent compounds with three very...Ch. 10 - Prob. 30Q Ch. 10 - Compare and contrast the structures of the...Ch. 10 - Silicon carbide (SiC) is an extremely hard...Ch. 10 - A common prank on college campuses is to switch...Ch. 10 - A plot of In (Pvap) versus 1/T (K) is linear with...Ch. 10 - Prob. 36Q Ch. 10 - Identify the most important types of interparticle...Ch. 10 - Prob. 38E Ch. 10 - Predict which substance in each of the following...Ch. 10 - Consider the compounds CI2, HCI. F2, NaF, and HF....Ch. 10 - Prob. 41E Ch. 10 - Consider the following electrostatic potential...Ch. 10 - In each of the following groups of substances,...Ch. 10 - Prob. 44E Ch. 10 - The shape of the meniscus of water in a glass tube...Ch. 10 - Prob. 46E Ch. 10 - Hydrogen peroxide (H2O2) is a syrupy liquid with a...Ch. 10 - Carbon diselenide (CSe2) is a liquid at room...Ch. 10 - X rays from a copper X-ray tube ( = 154 pm) were...Ch. 10 - The second-order diffraction (n = 2) for a gold...Ch. 10 - A topaz crystal has an interplanar spacing (d) of...Ch. 10 - X rays of wavelength 2.63 were used to analyze a...Ch. 10 - Calcium has a cubic closest packed structure as a...Ch. 10 - Nickel has a face-centered cubic unit cell. The...Ch. 10 - A certain form of lead has a cubic closest packed...Ch. 10 - The density of polonium metal is 9.2 g/cm3. 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The first...Ch. 10 - Prob. 121AE Ch. 10 - Argon has a cubic closest packed structure as a...Ch. 10 - Prob. 123AE Ch. 10 - A 20.0-g sample of ice at 10.0C is mixed with...Ch. 10 - Prob. 125AE Ch. 10 - Carbon tetrachloride. CCl4, has a vapor pressure...Ch. 10 - A special vessel (see Fig. 10.45) contains ice and...Ch. 10 - Prob. 128AE Ch. 10 - In regions with dry climates, evaporative coolers...Ch. 10 - Which of the following compound(s) exhibit only...Ch. 10 - Which of the following statements about...Ch. 10 - Prob. 133CWP Ch. 10 - Aluminum has an atomic radius of 143 pm and forms...Ch. 10 - Pyrolusite is a mineral containing manganese ions...Ch. 10 - The structure of the compound K2O is best...Ch. 10 - Prob. 137CWP Ch. 10 - Some ice cubes at 0c with a total mass of 403 g...Ch. 10 - The enthalpy of vaporization for acetone is 32.0...Ch. 10 - Prob. 140CWP Ch. 10 - When I mole of benzene is vaporized at a constant...Ch. 10 - You and a friend each synthesize a compound with...Ch. 10 - Prob. 143CP Ch. 10 - Prob. 144CP Ch. 10 - Consider two different organic compounds, each...Ch. 10 - Rationalize the differences in physical properties...Ch. 10 - Prob. 147CP Ch. 10 - Some ionic compounds contain a mixture of...Ch. 10 - Some ionic compounds contain a mixture of...Ch. 10 - Spinel is a mineral that contains 37.9% aluminum,...Ch. 10 - Mn crystallizes in the same type of cubic unit...Ch. 10 - You are asked to help set up a historical display...Ch. 10 - Some water is placed in a sealed glass container...Ch. 10 - The molar enthalpy of vaporization of water at 373...Ch. 10 - Prob. 155CP Ch. 10 - Rubidium chloride has the sodium chloride...Ch. 10 - Prob. 157IP Ch. 10 - A metal burns in air at 600c under high pressure...Ch. 10 - Prob. 159IP Ch. 10 - General Zod has sold Lex Luthor what Zod claims to...

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Solution Summary: The author explains the differences between crystalline and amorphous solids.

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Chapter 10 Solutions