A crystal lattice made of identical atoms is sketched below, seen from directly above. Atoms in the top layer are colored red, atoms in the second layer are colored green, and atoms in the third layer are colored blue. By dragging the slider you can shrink the atoms in the top layer so that you can see past them to the second layer. By dragging the slider even more you can shrink the atoms in the second layer, too, so you can see past them to the third layer. Use this sketch to answer the questions in the following table. Is this a close-packed crystal lattice? If you answered yes, what is the name of this type of crystal lattice? Your answer should be a word, a standard abbreviation, or a very short phrase. O yes O no ☐

A crystal lattice made of identical atoms is sketched below, seen from directly above. Atoms in the top layer are colored red, atoms in the second layer are colored green, and atoms in the third layer are colored blue. By dragging the slider you can shrink the atoms in the top layer so that you can see past them to the second layer. By dragging the slider even more you can shrink the atoms in the second layer, too, so you can see past them to the third layer. Use this sketch to answer the questions in the following table. Is this a close-packed crystal lattice? If you answered yes, what is the name of this type of crystal lattice? Your answer should be a word, a standard abbreviation, or a very short phrase. O yes O no ☐

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 163CP: The compound hexaazaisowurtzitane is one of the highest-energy explosives known (C E News, Jan. 17,...

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7. Melting points of Br2 and ICl are - 7.2 and 27.2°C, respectively and their electrons are same. Explain.
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6. The density of sodium chloride is 2.165 g/cm³. Using only the density and crystal structure, calculate the distance between Na and Cl atoms in the structure. 7 TL 1 ef. D-21 U DEN 1.1.-1 TI..
Metals can be rolled into sheets and stamped into various forms. In contrast, diamond is very hard and brittle. Which explanation for these different properties is correct? Metals have semi-ionic bonds, whereas diamond has covalent bonds. The electrons of a metal are held more tightly to the parent atom than the electrons of carbon. Hence, the bonds in a metal are stronger than the bonds in diamond. Metals are made of metal atoms, whereas diamond is made of non-metal carbon atoms. The electrons that surround a metal atom are free to move through the metal. The bonding electron pairs in a diamond are held tightly between two carbon atoms in an overall tetrahedral pattern. Diamond has strong double bonds between carbon atoms. Metal bonds are normally single covalent bonds, which bend easily.
Compare the hardness of SCF3 O SCF3 to AIF3. Which will be harder? O AIF3 Explain your answer in terms of Coulomb's Law.
7) The reason why can ionic substances conduct electricity when in solution or molten, but not when they are in the solid state is- O a. The ions are free to move but not free to move in the solid state. O b. The neutrons are free to move but not free to move in the solid state. O c. The protons are free to move, but not free to move in the solid state. O d. The atoms are free to move, but not free to move in the solid state.
2. Molybdenum has a BCC crystal structure, an atomic radius of 0.1363 nm, and an atomic weight of 95.94 g/mol. Compute and compare its theoretical density with the experimental value (10.22g/cm³).
Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca2+ ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is 3460 kJ/mol; the lattice energy of K2O is 2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
The molecules NH3andBF3have the same general formula (AB3)but different shapes. Find the shape of each of the above molecules. Provide more examples of real molecules that have the same general formulas but different shapes.
Look in Appendix D and compare the electron configurations shown there with the fusion enthalpies for the metals shown in Table 9.7. Is there any correlation between these configurations and this property? Does strength of attraction among metal atoms correlate with number of valence electrons? Explain your answers.
The compound hexaazaisowurtzitane is one of the highest-energy explosives known (C E News, Jan. 17, 1994, p. 26). The compound, also known as CL-20, was first synthesized in 1987. The method of synthesis and detailed performance data are still classified because of CL-20s potential military application in rocket boosters and in warheads of smart weapons. The structure of CL-20 is In such shorthand structures, each point where lines meet represents a carbon atom. In addition, the hydrogens attached to the carbon atoms are omitted; each of the six carbon atoms has one hydrogen atom attached. Finally, assume that the two O atoms in the NO2 groups are attached to N with one single bond and one double bond. Three possible reactions for the explosive decomposition ofCL-20 are i. C6H6N12O12(s)6CO(g)+6N2(g)+3H2O(g)+32O2(g) ii. C6H6N12O12(s) 3CO(g) + 3CO2(g) + 6N2(g) + 3H2O(g) iii. C6H6N12O12(s) 6CO2(g) + 6N2(g) + 3H2 (g) a. Use bond energies to estimate E for these three reactions. b. Which of the above reactions releases the largest amount of energy per kilogram of CL-20?
Consider the ions Sc3+, Cl, K+, Ca2+, and S2. Match these ions to the following pictures that represent the relative sizes of the ions.