Explain close packing in one dimension. Explain close packing in two dimensions.

Vedclass pdf generator app on play store
Vedclass iOS app on app store
(N/A) The spheres in one dimension can be arranged only in one way,that is,to arrange them in a row and touching each other.
Close packing of spheres in one dimension:
In this arrangement,each sphere is in contact with two of its neighbours. The number of nearest neighbours of a particle is called the coordination number. Thus,in a one-dimensional arrangement,the coordination number is $2$.
The close packing in two dimensions can be done in two ways by stacking the rows of closed-packed spheres: $(i)$ Square Close Packing,$(ii)$ Hexagonal Close Packing $(HCP)$.
$(i)$ Square Close Packing: In square close packing,the spheres of the second row are placed exactly above the spheres of the first row such that the spheres of these two rows are aligned horizontally as well as vertically.
If the first row of spheres is called $A$ type row,the second row being exactly the same as the first one is also of $A$ type and hence by placing more rows,$AAAA...$ type of arrangement is obtained.
In this arrangement,each sphere is in contact with four of its neighbours and hence the coordination number of a sphere is $4$.
If the centres of the four immediate neighbours are joined,a square is formed and hence it is named Square Close Packing.
$(ii)$ Hexagonal Close Packing $(HCP)$:
In hexagonal close packing,the spheres of the second row are fit in the depressions of the spheres of the first row.
If the spheres of the first row are called $A$ type,the ones in the second row may be called $B$ type. The spheres of the third row are placed in the depressions of the spheres of the second row such that the spheres of the first row and third row are in the same alignment horizontally and vertically.
As the third row is exactly the same as that of the first row,it is called $A$ type. Hence,we get $ABABAB...$ type of arrangement.
In this arrangement,each sphere is in contact with six of its neighbours and thus in two dimensions,the coordination number is $6$. The centres of these six spheres are at the corners of a regular hexagon,hence this packing is called two-dimensional hexagonal close packing.

Explore More

Similar Questions

The molecular formula of a compound is $AB_2O_4$. Atoms of $O$ form a $ccp$ lattice. Atoms of $A$ (cation) occupy $\frac{1}{8}$ of the tetrahedral voids. Atoms of $B$ (cation) occupy a fraction of the octahedral voids. What is the fraction of vacant octahedral voids?

In a cubic close-packed $(ccp)$ structure,if there are $N$ spheres,what is the number of octahedral voids?

In a compound,nitrogen atoms $(N)$ make a cubic close-packed lattice and metal atoms $(M)$ occupy one-third of the tetrahedral voids present. Determine the formula of the compound formed by $M$ and $N$.

$A$ compound made up of elements $A$ and $B$ (with a general formula $A_x B_y$),where $B$ forms an $hcp$ lattice and $A$ occupies $2/3$ of the tetrahedral voids. The formula of the compound is

The ratio of densities if the same element undergoes $FCC$ and $HCP$ close packing is:

Difficult
View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial
For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free
For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo