In solid KCI, which has the same solid state structure as NacI (simplecubic unit cell), the distance between the ions is 314 pm. Calculate thelength of the edge of the unit cell.

Answered: n solid KCI, which has the same solid…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Many elements crystallize with a unit cell that is hexagonally shaped (6 sided). The calculations of the unit cell dimension are not significantly more complicated than those for cubic unit cells. A hexagonal unit cell is shown below. 3/3 a²c Volume 6 atoms per unit cell The cell dimension "a" is twice the radius (r) of the atom. 2r=a. For most elements the dimension "c" is approximately 1.633x"a". The element cerium (Ce) crystallizes with a Simple Hexagonal unit cell. The density of a cerium is 6.689 g/cm³. Use this information to calculate the metallic radius of cerium in picometers (pm). 1 pm = 1×10-12 meters. You can assume that the dimension c=1.633-a [Note: The theoretical value for the radius may be different from the experimentally determined value. Simply Googling the radius may not yield the correct result] Radius = pm
BeO has a face-centered cubic unit cell in which the O2- anions occupy corners and face centers, while the cations fit into the hole between adjacent anions. What is its density if the ionic radii of Be2+, O2- ions are 6.385 pm and 184.0 pm, respectively?
Consider the unit cell of a face-centred cubic structure of platinum (Pt) atoms, each with radius 139 pm. The unit cell and arrangement of atoms centred on a plane within the unit cell are shown below.
Sample Exercise 6: Empirical Formula and Density: Ionic Solid The unit cell of a binary compound of copper and oxygen is shown here. Given this image and the ionic radii rcut = 0.74 Å and ro² = 1.26 Å, (a) determine the empirical formula of this compound, (b) determine the coordination numbers of copper and oxygen, (c) estimate the length of the edge of the cubic unit cell, and (d) estimate the density of the compound. Solution (a) To determine the empirical formula we need to determine how many of each type of ion there are per unit cell. O: 8(1/8) + 1 = 2 0²-ions in the unit cell. Cu: 4(1) = 4 Cut ions in the unit cell. Empirical Formula: Cu₂O (b) If we can visually determine the coordination number of one of the ions, we can use Equation 12.1 to determine the coordination number of the other ion. Number of cations per formula unit Number of anions per formula unit anion coordination number cation coordination number Cation coordination number = anion coordination number Copper…
Metallic uranium crystallizes in a body-centered cubic lattice, with one U atom per lattice point. If the metallic radius of U is 148.5 pm, what is the volume of the unit cell?
Iron forms a body-centered cubic crystal structure. (a) How many Fe atoms are in a unit cell? (b) What is the mass of a unit cell in grams? (c) If the density of iron is 7.86 g/cm', calculate the volume of unit cell, the edge length of the unit cell in pm, and the atomic radius of iron in pm. (Atomic mass of iron = 55.85 amu; 1 amu = 1.6605 x 10 24 g; 1 pm = 10-10 cm)
Manganese has a body-centered cubic unit cell and has a density of7.88g/cm 3 . From this information, determine the length of the edge of thecubic.
Assume some metal X that has a body- centered cubic lattice with all atoms at lattice points. Its density is 3.11 g/cm3 and its atomic weight is 157.3 amu. From these data, calculate the edge length of a unit cell. Edge length = %3D pm

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

n solid KCI, which has the same solid state structure as NaCI (simple cubic unit cell), the distance between the ions is 314 pm. Calculate the ength of the edge of the unit cell.