Answered: C60 fullerenes crystallizes into a…

C60 fullerenes crystallizes into a cubic close-packed structure known as fullerite, with a lattice constant of a=14.17 Å. Calculate the density of fullerite in units of g/cm³.

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

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 124SCQ

See similar textbooks

Related questions

Q: The cell dimension "a" is twice the radius (r) of the atom. 2r=a. For most elements the dimension…

Q: An element has hcp packing with a hexagonal unit cell. Its density is 21000 kg/m3 and the unit cell…

A: The density of HCP molecule can be shown as:Where, d is density of cellM is molar mass of elementA3…

Q: VC (polyvinyl chloride) has the formula C2H3Cl. (Cl=35.45 g/mol). If there are 1565 repeat units in…

A: Polymers are formed by the combination of the monomers unit.1g/mole=1 amu

Q: To form an addition polymer, what structural feature must the monomer possess?

A: Polymer can be defined as the chemical compound that is formed by the combination of one or more…

Q: The element technetium (Tc) crystallizes with a Simple Hexagonal unit cell. The density of a…

A: The density is defined as mass per volume occupied. Density = MassVolume

Q: please help? make the answer clear

A: Density of aluminum = 2698 kg/m3Cell volume = 6.643×10-23 cm3

Q: The density of an unknown metal is 2.64 g/cm3 and its atomic radius is 0.215 nm. It has a…

A: Given density = 2.64g/cm3 r= 0.215nm = 0.215 x 10-7cm a = 4r/2 a = The cube has face centered…

Q: Three molecular requirements for crystallinity in polymers

A: POLYMERS: Polymer is a macromolecule which is made up of small monomer molecules that are…

Q: When silver crystallizes, it forms face- centered cubic cells. The unit cell edge length is 4.087 A.…

Q: An element has ccp packing with a face-centered cubic unit cell. Its density is 12400 kg/m^3 and the…

A: Given that the unit cell volume is 5.50×10-29 cubic meters. The equation which is used to calculate…

Q: Determine the lattice constant, a (in nm), of a metal conforming to the FCC structure having an…

A: For a FCC lattice the relation between lattice constant (a) and radius of atom (r) is 4r=2a Here…

Q: Suppose that a crystal lattice is composed of a structure where anions, X, occupy all o the corners…

A: Given, a crystal lattice is composed of a structure where anions, X, occupy all of the corners in…

Q: The heat of fusion of polyethylene is approximately 7.7 kJ/mol, and the corresponding entropy is 19…

A: Given Heat of fusion ( ∆Hfusion ) = 7.7 KJ/mol = 7700…

Q: lattice structure of CsCl is shown below. What

A: We have to tell which option is correct from given choices of options by telling which type of unit…

Q: Silicon (Si) and germanium (Ge) can be used as semiconducting materials. The band gap between the…

A: Each metal or metalloid is capable of conducting current when the valence electrons of the atom can…

Q: A certain element exists in a face-centered cubic structure. The atomic radius of an atom of this…

Q: Calculate the density (g/cm³) of Rb if it crystallizes in body center cubic (bcc) and has a radius…

A: Given the radius of Rb is 272 pm. The density of Rb has to be calculated.

Q: Which substance has the highest melting point? Kr Cl 2 Mg SiO 2 (silica) C…

A: Melting point:

Q: CaF2 crystallizes is shown below: What is the arrangement of the Ca2+ ions (white spheres)? FCC…

Concept explainers

Crystal Lattices and Unit Cell

Consider a crystal. The regular and repeating pattern of constituent particles is the most distinguishing feature of crystalline solids. A crystal lattice is formed when these particles are replaced with representative points. The three-dimensional arrangement of constituent particles is known as a crystal lattice. Unit cell is that the smallest portion of a space lattice which when repeated in several directions, generate the whole lattice. Unit cell is a building block of a lattice. It is the smallest unit of cell.

Question

C60 fullerenes crystallizes into a cubic close-packed structure known as
fullerite, with a lattice constant of a=14.17 Å.
Calculate the density of fullerite in units of g/cm³.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Why is the C 60form of carbon called buckminsterfullerene?
Phase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions. (a) How many triple points are present and what phases are in equilibrium for each? (b) Is there a single point where all four phases are in equilibrium? (c) Which is more stable at high pressures, diamond or graphite? (d) Which is the stable phase of carbon at room temperature and 1 atmosphere pressure?
A metal crystallizes in the face-centered cubic (FCC) lattice. The density of the metal is 10500 kg/m', and the length of a unit cell edge, a, is 408.6 pm. Calculate the mass of one metal atom. mass: Identify the metal. O nickel O rhodium O copper O silver
Silicon has a face-centred cubic structure with two atoms per lattice point, just like diamond. At 25°C, a = 543.1 pm. What is the density of silicon? What is the Si-Si bond length?
8. An element with atomic mass 106.3amu crystallizes in a face–centered cubic unit cell. Its density is 12.9 g/cm3 at 27°C. Calculate the atomic radius of an atom of the element in centimeters.
At room temperature, the edge length of the cubic unit cell in elemental silicon is 5.431 Å, and the density of silicon at the same temperature is 2.328 g cm-3 . Each cubic unit cell contains eight silicon atoms. Using only these facts, perform the following operations.(a) Calculate the volume (in cubic centimeters) of one unit cell.(b) Calculate the mass (in grams) of silicon present in a unit cell.(c) Calculate the mass (in grams) of an atom of silicon.(d) The mass of an atom of silicon is 28.0855 u. Estimate Avogadro’s number to four significant figures.
The density of platinum is 21.45 g/cm3. It crystallizes in a fcc lattice. Calculate its metallic radius.
An element has ccp packing with a face-centered cubic unit cell. Its density is 12400 kg/m^3 and the unit cell volume is 5.50×10^-29 cubic meters. Calculate the molar mass (g·mol^–1) of the element to three significant figures.
The accompanying figure shows three different crystallographic planes for a unit cell of a hypothetical metal. The circles represent atoms. Draw its unit cell and show the atoms’ positions. To what crystal system does the unit cell belong and what would this crystal structure be called?
An alloy structure (element: Co, Y, Si) adopts the cubic crystal structure with lattice constant a = 5.19 Å. Please determine (1) the bond length between Co-Y, Co-Si, Y-Si. (2) the density of the alloy. (Hint: atomic weight for Co: 58.9 g/mol; Y: 88.9 g/mol; Si: 28 g/mol; Avogadro constant: NA = 6.022 ×10²³ mol-1).
6. A compound consists of A-atoms and B-atoms, and its solid crystal forms a cubic unit cell structure, as shown below. A-atoms occupy corners and faces of the cube. B-atoms are inside the cube and are not shared by adjacent cubic unit cells. Based on the information here, we can conclude that (a) A-atoms form an FCC structure; the empirical formula of the compound is A,B2. (b) A-atoms form an FCC structure; the empirical formula of the compound is AB. (c) A-atoms form a BCC structure; the empirical formula of the compound is A¬B2. (d) A-atoms form a BCC structure; the empirical formula of the compound is AB. (e) None of the above. A-atoms (corners and faces) B-atoms (inside, not shared) a m n T OF THE FL EMENTS
An element has a density of 10.25 g/cm3 and a metallic radius of 136.3 pm. The metal crystallizes in a bcc lattice. Identify the element.