Help me please 6. The table below lists some properties of three carbon allotropes. Explain, from amolecular viewpoint, why these materials have such different properties.GeneralHeatElectricalAllotropeStructureStrengthResistivityConductivityGraphiteLowVery lowVery highDiamondVery highModerateNoneBucky BallsModerateHighLow

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The table below lists some properties of three carbon allotropes. Explain, from a molecular viewpoint, why these materials have such different properties. General Нeat Electrical Allotrope Structure Strength Resistivity Conductivity Graphite Low Very low Very high Diamond Very high Moderate None Bucky Balls Moderate High Low

The table below lists some properties of three carbon allotropes. Explain, from a molecular viewpoint, why these materials have such different properties. General Нeat Electrical Allotrope Structure Strength Resistivity Conductivity Graphite Low Very low Very high Diamond Very high Moderate None Bucky Balls Moderate High Low

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter12: The Solid State

Section: Chapter Questions

Problem 23PS

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The coordination number for the Al3+ ion is typically betweenfour and six. Use the anion coordination number todetermine the Al3 + coordination number in the followingcompounds: (a) AlF3 where the fluoride ions are two coordinate,(b) Al2O3 where the oxygen ions are six coordinate, (c)AlN where the nitride ions are four coordinate.
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8.97 The doping of semiconductors can be done with enough precision to tune the size of the band gap in the material. Generally, in order to have a larger band gap, the dopant should be smaller than the main material. If you are a materials engineer and need a semiconductor that has lower conductivity thin pure silicon, what clement or elements could you use as your dopant? (You do not want either an n- or a p- type material) Explain your reasoning.
Consider the lattice energies of the following Group 2Acompounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol;CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol.(a) What is the oxidation number of H in these compounds?(b) Assuming that all of these compounds have the samethree-dimensional arrangement of ions in the solid, whichof these compounds has the shortest cation–anion distance?(c) Consider BeH2. Does it require 3205 kJ of energyto break one mole of the solid into its ions, or does breakingup one mole of solid into its ions release 3205 kJ of energy?(d) The lattice energy of ZnH2 is 2870 kJ/mol. Consideringthe trend in lattice enthalpies in the Group 2A compounds,predict which Group 2A element is most similar in ionic radiusto the Zn2+ ion.
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(a) Why does Li Cl acquire pink colour when heated in Li vapours? (b) A solid with cubic crystal is made of two elements ‘P’ and ‘Q’ Atoms of ‘Q’ are at the comers of the cube and ‘P’ at body centre. What is the formula of compound?
The table below shows some physical properties of halogenatedliquids. Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole-dipole interactions. (c) The trend in electronegativityis F > Cl > Br; therefore, the most ionic compound (CH2F2)has the lowest boiling point, and the most covalent compound(CH2Br2) has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.
The table below shows some physical properties of halogenatedliquids.Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole–dipole interactions. (c) The trend in electronegativityis F 7 Cl 7 Br; therefore, the most ionic compound 1CH2F22has the lowest boiling point, and the most covalent compound1CH2Br22 has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.

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