Which of the following is a molecular solid

The correct option is B Solid SO 2 To answer this question, first we need to know about the types of crystalline solids. Molecular solids → In these solids, the constituent particles are molecules. Metallic solids → In such solids, the constituent particles are orderly arranged positively charged metal ions (called kernels) surrounded by a sea of free electrons. These electrons are mobile and are evenly spread out throughout the crystal and flow throughout the metal crystal such as water in the sea. These are produced from metal atoms having low ionization energy and can easily lose their valence electrons to leave behind positively charged ions (kernels). Each metal atom contributes one or more electrons towards this sea of mobile electrons. Hence, it is called electrons sea model. Ionic Solids → In ionic solids, the constituent particles are positive and negative ions. Such solids are formed by the three-dimensional arrangement of positive (cations) and negative (anions)( ions held by strong electrostatic (coulombic) force of attraction. Covalent solid → In covalent solids, the constituent particles are non-metal atoms linked to the adjacent atoms by covalent bonds throughout the crystal. As a result, a network of covalent bond is formed. Hence, they form giant molecules. So, here Diamond → Giant 3-d network with covalent bonds between carbon. So, covalent solid Iron (Fe) → Metallic solid C a F 2 → Ionic solid Constituent particles are C a 2 + and F − ions Solid S O 2 → ...

Q. Which of the following statements is/are correct? 1.0 g mixture of C a C O 3 ( s ) and glass beads liberate 0.22 g of C O 2 upon treatment with excess of H C l. Glass does not react with H C l. C a C O 3 + 2 H C l → C O 2 + H 2 O + C a C l 2 [Molecular weight of C a C O 3 = 100 g/mol, C O 2 = 44 g/mol and atomic weight of C a = 40 g]

• • • • Question:6. Which of the following statements is true? a. Metallic solids have a dull appearance. b. Molecular solids have a low density. c. Covalent solids have low melting points. d. lonic solids are soft. 7. If you wanted to synthesize a compound that had a fairly low melting point and a low density, you would want to synthesize a. a metallic solid. b. a covalent 6. Which of the following statements is true? a. Metallic solids have a dull appearance. b. Molecular solids have a low density. c. Covalent solids have low melting points. d. lonic solids are soft. 7. If you wanted to synthesize a compound that had a fairly low melting point and a low density, you would want to synthesize a. a metallic solid. b. a covalent solid. C. an ionic solid d. a molecular solid. 8. The radius of silicon and lithium are quite different. What type of impurity will lithium be? a. common substitutional impurity b. Frenkel defect C. interstitial impurity d. Schottky defect 9. Which of the following statements is true? a. Molecular solids have a low density. b. lonic solids are soft. c. Covalent solids have low melting points. d. Metallic solids have a dull appearance. 10. Which of the following statements is true? a. Metallic solids are easily deformed. b. Ionic solids have a low density. c. Covalent solids are good conductors of heat and electricity. d. Molecular solids have substantial luster. Previous question Next question

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:Which of the following will be a molecular solid when it solidifies. Select all that apply. NaCl methanol (CH3OH) Water (H2O) Silica dioxide (SiO2) Iodine (I2)

now the most fundamental distinction between solids is that they can be classified as either crystalline or amorphous solids. Now we say crystal and solid, we're going to say here that atoms ions or molecules that have highly ordered uh arrangements throughout. And amorphous solids are particles that are randomly arranged throughout with no discernible pattern. Now when we say crystalline solids we're referring to as ionic solids, molecular solids, co violent network solids and metals. Now here we're going to say for ionic solids, the smallest unit is the ionic part and that's because it's electric electrostatic forces is the attraction between a positive ion and a negative ion. Remember we know the definition of ionic compounds is a cat eye on connected to an an eye on that. Can I um can be a metal or ammonium ion, that an ion is just some non metals. Now we can say here also their properties is that ionic solids tend to be brittle and yet hard and we're gonna stay here that they have high melting points. A good example is if we're looking at solid sodium chloride for Ariana compound, molecular solids, not molecular solids. Their smallest student is the molecule. Their electrostatic force are the inter molecular forces. We're gonna stay here that they have soft textures to them we're going to say they have low to moderate melting points. Good example of a molecular solids or molecular solid that we can think of. We could think of ice which is just hte tool solid Covalin n...

MCQ Questions Based On Class 12 Chemistry Term 1 Syllabus • • • • • MCQs based on class 12 chemistry chapter 1 solid state Q.1. Which of the following statements about amorphous solids is incorrect ? (a) They melt over a range of temperature (b) They are anisotropic (c) There is no orderly arrangement of particles (d) They are rigid and incompressible Answer Ans. (b) Amorphous solids are isotropic, because these substances show same properties in all directions. Q.2. Which of the following statement is not true about amorphous solids ? (a) On heating they may become crystalline at certain temperature. (b) They may become crystalline on keeping for long time. (c) Amorphous solids can be moulded by heating. (d) They are anisotropic in nature. Answer Ans. (d) Q.3. Which of the following is not a characteristic property of solids? (a) Intermolecular distances are short. (b) Intermolecular forces are weak. (c) Constituent particles have fixed positions. (d) Solids oscillate about their mean positions. Answer Ans. (b) Intermolecular forces are strong in solids. Q.4. Most crystals show good cleavage because their atoms, ions or molecules are (a) weakly bonded together (b) strongly bonded together (c) spherically symmetrical (d) arranged in planes Answer Ans. (d) Crystals show good cleavage because their constituent particles are arranged in planes. Q.5. The coordination number of Y will be in the XY types of crystal: (a) 6 (b) 8 (c) 12 (d) 4 Answer Ans. (a) 6 Q.6. Which of the fo...

1.Which of the following properties DOES NOT describe metallic crystalline solids? A. brittle B. ductile C. malleable D. good conductor of heat 2.Which of the following properties characterizes covalent network crystalline solids? A. brittle B. high melting point C. poor conductor of electricity D. with cations and anions very 3.Which of the following phrases about molecular crystalline solid is FALSE? A. fairly soft B. poor thermal conduction C. made up of atoms or molecules D. very high electrical conduction 4.Which of the following phrases about ionic crystalline solid is TRUE? A. very hard B. good thermal conduction C. high melting point D. very high electrical conduction 5.Why is metallic crystalline solid a good conductor of electricity? A. Atoms are packed close together. B. Particles can move through the crystal. C. The charged particles move through the crystal. Rubidium chloride has the sodium chloride structure at normal pressures but assumes the cesium chloride structure at high pressures. (See Exercise 69.) What ratio of densities is expected for these two forms? Does this change in structure make sense on the basis of simple models? The ionic radius is 148 pm for Rb+ and 181 pm for CI.