Please Wait... While Loading Full Video### `color{red} ✎` PROBLEM SOLVING TECHNIQUES

• Problems based on nuclear structure

• Problems based on Planck's quantum theory and photoelectric effect

• For Balmer series [ Rydberg formula ]

• Problems based on Bohr's model

• Problems based on De- broglie

• Problems based on Heisenberg's Uncertainty principle

• Problems based on electronic configuration

• Problems based on Planck's quantum theory and photoelectric effect

• For Balmer series [ Rydberg formula ]

• Problems based on Bohr's model

• Problems based on De- broglie

• Problems based on Heisenberg's Uncertainty principle

• Problems based on electronic configuration

Q 3166878775

Complete the following table :

Particle | Mass Number | Atomic Number | Protons | Neutrons | Electrons |
---|---|---|---|---|---|

Nitrogen atom | - | - | - | 7 | 7 |

Calcium ion | - | 20 | - | 20 | - |

Oxygen atom | 16 | 8 | - | - | - |

Bromide | - | - | - | 45 | 36 |

For nitrogen atom :

No. of electrons = 7 ( given )

No. of neutrons = 7 ( given)

`therefore` No. of protons `= Z = 7` ( `because` atom is electrically neutral).

Atomic number = `Z = 7`

Mass no. (A) = NO. of protons+ NO. of neutrons

` = 7+7 = 14`

For Calcium ion

No. of neutrons `= 20` ( given)

Atomic Number `(Z) = 20` ( given)

`therefore` No. of protons ` = Z = 20`

No. of electrons in calcium atom `= Z = 20`

But in the formation of calcium ion , two electrons are lost from the extranuclear part according to the equation `Ca → Ca^(2+) + 2e^(-)`

but the composition of the nucleus remains unchanged.

`therefore` No. of electrons in calcium ion `= 20-2 = 18`

Mass number(A) = No. of protons + No. of neutrons

` = 20+20= 40`

For oxygen atom :

Mass number (A) = No. of protons +No. of neutrons = 16 (given)

Atomic No. (Z) = 8.(given)

No. of protons `= Z = 8` (given)

No. of electrons `= Z = 8`

No. of neutrons `= A-Z = 16-8 = 8`

For bromide ion : In the formation of bromide ion one electron is added to the extra nuclear part of the bromine atom according to the equation `Br + e^(-) → Br^(-)` but the composition of the nucleus remains unchanged .

Since the no. of electrons in bromide ion = 36 (given)

No. of electrons in bromine atom ` = 36-1 = 35`

Further , since in the above reaction , nucleus of the bromine atom remains unchanged.

`therefore` No. of protons in the bromine ion = No. of protons in the bromine atom = 35.

Putting the values of the various vacant place as calculated above , in the table we have

Particle | Mass Number (A) | Atomic Number (Z) | No. of Protons(Z) | No. of Neutrons(A-Z) | No. of Electrons(Z) |
---|---|---|---|---|---|

Nitrogen atom | 7+7 = 14 | 7 | 7 | 7 | |

Calcium ion | 20+20= 40 | 20 | 20 | 20 | 20-2 = 18 |

Oxygen atom | 16 | 8 | 8 | 16-8 = 8 | 8 |

Bromide ion | 45+35 = 80 | 35 | 36-1 = 35 | 45 | 36 |

Q 3116180970

Calculate the kinetic energy of the electron ejected when yellow light of frequency `5.2xx10^(14) sec^(-1)` falls on the surface of potassium metal . Threshold frequency of potassium is `5xx10^(14) sec^(-1)`

K.E of the ejected electron is given by

`1/2 mv^2 = hv - hv_0 = h(v - v_0)`

` = 6.625xx10^(-34) xx (5.2xx10^(14) -5.0xx10^(14))`

` = 6.625xx10^(-34) xx 0.2 xx 10^(14)` Joules

`= 1.325 xx 10^(-20)` Joules

Q 3146191073

Calculate the frequency and the wavelength of the radiation in nanometers emitted when an electron in the hydrogen atom jumps from third orbit to the ground state. In which region of the electromagnetic spectrum will this line lie ? ( Rydberg constant = 109 , 677 cm `text()^(-1)` )

According to Rydberg formula

`barnu = R ( 1/n_1^2 - 1/n_2^2)`

Here `R = 109 , 677 cm^(-1)`

`n_2 = 3`

`n_1 = 1` ( for ground state)

`therefore barnu = 109, 677(1/1^2 - 1/3^2) cm^(-1)`

` = 109 , 677 xx 8/9 cm^(-1) = 97490.7 cm^(-1)`

`lamda = 1/(bar nu) = 1/(97490.7 cm^(-1))`

` = 103xx10^(-7) cm`

` = 103xx10^(-9) m = 103 nm`

`nu = c/lamda = (3xx10^8 m s^(-1))/(103xx10^(-9)m)`

` = 2.91xx10^(15) s^(-1)`

The wavelength as calculated above , lies in this ultraviolet region . Otherwise too , as the jump is on the 1st orbit , the line will belong to Lyman series and hence lie in the ultraviolet region

Q 3116191079

The wavelength of the first line in the Balmer series is `656 nm`. Calculate the wavelength of the second line and the limiting line in Barmer series .

According to Rydberg formula

`barnu = 1/lamda = R (1/n_1^2 - 1/n_2^2)`

For the balmer series `n_1 = 2` and for the 1st line .

`n_2 = 3`

`therefore 1/656 = R (1/2^2 -1/3^2) = R xx (1/4-1/9)`

`= R xx 5/36 = (5R)/(36)` .................(i)

For the second line , `n_1 = 2 , n_2 = 4`

`therefore 1/lamda = R (1/2^2-1/4^2) = R (1/4-1/16)`

` = R xx 3/16 = (3R)/(16)` ...........(ii)

Dividing (i) by (ii) we get

`lamda/(656) = 5/36xx16/3`

or `lamda = 485.9 nm`

For the limiting line `n_1 = 2`

`n_2 = oo`

`therefore 1/lamda = R (1/2^2-1/oo^2) = R/4` ......(iii)

Dividing (i) by (iii) we get

`lamda/(656) = 5/36 xx 4`

or `lamda = 364.4 nm`

Alternatively first calculate R from (i) and sub stitute in (ii) and (iii)

Q 3146191973

Calculate the wavelength of the radiation emitted when an electron in a hydrogen atom undergoes a transition from 4th energy level to the 2nd energy level. In which part of the electromagnetic spectrum does this line lie ?

`E_n = - (21.8xx10^(-19))/n^2 J` atom `text()^(-1)`

Energy emitted when the electron jumps from ` n= 4` to `n = 2` will be given by

`DeltaE = E_4 - E_2 = 21.8 xx 10^(-19) (1/2^2-1/4^2)`

` = 21.8xx10^(-19) xx3/16 = 4.0875xx10^(-19) J`

The wavelength corresponding to this energy can be calculate using the expression

`E = hnu = h . c/lamda \ \ \ \ ( because c = nu lamda )`

so that `lamda = ( hc)/E`

`= ((6.626xx10^(-34) Js) (3xx10^8 m s^(-1)))/((4.0875xx10^(-19) J))`

` = 4.863xx10^(-7) m`

`= 4863 overset(o)A `

or `486.3 nm`

It lies in the visible region

Q 3166491375

Two particles A and B are in motion. If the wavelength associated with particles A is `5xx10^(-8) m` calculate the wavelength associated with particle B if its momentum is half of A.

By de Broglie equation

`lamda_A = h/(P_A)` and `lamda_B = h/(p_B)`

`therefore = lamda_A/lamda_B = p_B/P_A`

But `p_B = 1/2 p_A` ( given)

`lamda_A/lamda_B = (1/2 p_A)/(p_A) = 1/2`

or `lamda_B = 2 xx lamda_A = 2xx5xx10^(-8) m`

`= 10^(-7) m`

Q 3106491378

The kinetic energy of a sub - atomic particle is `5.85xx10^(-25) J.` Calculate the frequency of the particle wave. ( Plank's constant , `h = 6.626xx10^(-34) kg m^2 s^(-1)`)

`K.E = 1/2 mv^2 = 5.85xx10^(-25) J`

By de- Broglie equation `lamda = h/(mv)`

But `lamda = v/nu`

`therefore v/nu = h/(mv)`

or `nu = (mv^2)/h = ( 2xx5.85xx10^(- 25) J)/(6.626xx10^(-34) J s)`

` = 1.77 xx 10^9 s^(-1)`

Q 3126591471

Calculate the uncertainty in the velocity of a wagon of mass `3000kg` whose position is known to an accuracy of `pm 10 p m` (Plank's constant = `6.63xx10^(-34) Js`)

Here we are given `m = 3000kg`

`Deltax = 10 p m = 10xx10^(-12) m = 10^(-11) m`

`therefore` By uncertainty principle

`Deltav = h/(4pi xx m xx Deltax)`

`= (6.63xx10^(-34) kg m^2 s^(-1))/(4xx22/7xx3000 kg xx10^(-11) m)`

`= 1.76xx10^(-27) m s^(-1)`

Q 3156691574

A neutral atom of elements has 2K , 8L and 5M electrons . Field out the following from the data : (a) Atomic No. (b) Total No. of `s` electrons .(c) Total No. of p- electrons . (d) No. of protons in the nucleus and (e) Valency of the element.

The electronic configuration of the element with 2K , 8L and 5M electronic will be

`1s^2 2s^2 2p_x^2 2p_y^2 2p_z^2 3s^2 3p_x^1 3p_y^1 3p_z^1`

(a) Total no. of electrons `= 2+8+5 = 15`

`therefore ` Atomic No. of the element =` 15`

(b) Total no. of s- electrons `= 2+2+2= 6`

(c) Total no. of p - electrons `= 6+3 = 9`

(d) Since the atom is neutral

`therefore ` No. of protons = No. of electrons = Atomic No. = 15

(e) Since the electron has only three half- filled atomic orbitals , therefore valency of the element = 3