Chapter 02 periodic table and atomic periodicity or properties

Chapter 02
periodic table and atomic periodicity or properties:

Modern periodic table: the table in which elements are arrange in order of increasing atomic number.

Modern periodic law: physical and chemical properties of elements are periodic function of their atomic number.

periodic function: repelition of properties after certain interval of time.

periodicity of elements: the repelition of properties after certain interval of time.

the elements repeats their properties because their valence shell electron configuration repeats.

eg. li 2 1
Na 2 8 1
k 2 8 8 1

114 elements are known today. for their systematic study they have been classified into group and period.

Group :vertical column are called group there are 18 vertical column. so their are 18 groups.

Periods: horizontal rows are called periods there are 7 horizontal rows. so their are 7 periods .

A/c to periods no. of elements

1 period 2 elements
2 period 8 elements
3 period 8 elements
4 period 18 elements
5 period 18 elements
6 period 32 elements
7 period 32 elements

the elements constituent groups 1,2,13,14,15,16,17,18 are called normal elements or representation elements.

the elements of 3,4,5,6,7,8,9,10,11,12 are called transistion elements. because they show transistion (change) in property.

# from highly +ve s block to least + ve P block

Two rows of elements which are placed at the bottom of periodic table are called lanthanoids and actinoids.

Comments

Physical significance of sie and sie^2

Physical significance of sie and sie^2 The wave function sie has no physical significance, it simply represents amplitude of wave while square of amplitude sie^2 represent intensity of electron. i. e sie ^2 gives probability of finding the electron in space .p the space is called atomic orbital A zero value of sie^2 means probability of finding the electron is zero and high value of sie^2 means greater chances of finding the electron . the value of sie^2 lies between 0&1. if sie^2 =1 100℅ sie^2=0 0℅

Radial probability distribution for p and d orbital, radial wave functions

Radial probability distribution for p and d orbital Radial and Angular wave function: the radial part of wave function depends upon quantum no. n and l and gives the distribution of electron w. r. t distance .it is governed mainly exponential term e^-Zr/na°(a not) here e based on natural log. Z Atomic number r distance from nucleus n principal quantum no. or radial quantum no. a° 0.529A° for hydrogen ( Bohr radii) the exact mathematical expression for radial part of wave function for 1s or 2s and 2p orbitals. n= 1 ,l=0 s orbital R(r) =2× (z/a°) ^3/2 ×(2-zr/a°) ×e^-zr/2a° n= 2 ,l=0 2s orbital R(r) = (z/a°) ^3/2 ×(2-zr/a°) ×e^-zr/2a° n= 2 ,l=1 2p orbital R(r) = 1√3×(z/2a°) ^3/2 ×(zr/a°) ×e^-zr/2a ° the radial wave function can be represented by plotting radial function R(r) apart distance(r)

Linear combination of atomic orbital, Molecular orbital theory, Difference between bonding & anti bonding moleculer orbital.

Linea combination of atomic orbital molecular orbital are formed by combination of atomic orbital if ꌏ(A) andꌏ(B) are the wave function of atomic orbital of two combining atomic A and B then according to Linea combination of atomic orbital, these two wave function can be added or can be substracted .that means there are two modes of interaction (symmetric and antisymmetric) We know ꌏ(s) = ꌏ(A) +ꌏ(B) ꌏ(a) = ꌏ(A)- ꌏ(B) ꌏ(s) and ꌏ(a) represent wave function of bonding and antibonding moleculer orbital. the formation of moleculer orbital ꌏ(s) and ꌏ(a) from two atomic orbital ꌏ(A) and ꌏ(B) is represented as Molecular orbital theory (MO) theory: main points of mo theory are: 1.whwn atomic orbital combine they formed molecular orbital. 2.Number of molecular orbital formed is equal to number of atomic orbital combine. 3.atomic orbital are uninuclear while molecular orbital are polynuclear. 4.The various molecular orbital are arranged in order of in increas

Chemistry

Search This Blog