Ncert Solutions Chemistry Class 11th
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Give the number of electrons in the species: H2+, H2 and O2+.
Give the number of electrons in the species: H2+, H2 and O2+.
Number of electrons in:
(i) H2+ = 1
(ii) H2 = 2
(iii) O2+ = 15
Upvote 
An atom of an element contains 29 electrons and 35 neutrons. Deduce
(i) The number of protons and
(ii) The electronic configuration of the element.
An atom of an element contains 29 electrons and 35 neutrons. Deduce
(i) The number of protons and
(ii) The electronic configuration of the element.
(i) No. of protons in a neutral atom = No. of electrons = 29
(ii) Electronic configuration = 1s2 2s2 2p6 3s2 3p6 3d10 4s1
Upvote An electron is in one of the 3d orbitals. Give the possible values of n, l and nil for the electron.
An electron is in one of the 3d orbitals. Give the possible values of n, l and nil for the electron.
For electron in 3d orbital, n = 3, l = 2, mi = -2, -1, 0, +1, +2.
Upvote What is the lowest value of n which allows ‘g’ orbital to exist?
What is the lowest value of n which allows ‘g’ orbital to exist?
The lowest value of l where ‘g’ orbital can be present = 4
As for any value ‘n’ of principal quantum number, the Azimuthal quantum number (l) can have a value from zero to (n – 1).
∴ For l = 4, the minimum of n where ‘g’ orbital can be present = 4+1=5.
Upvote (i) Write the electronic configuration of the following ions :
(a) H (b) Na+ (c) O2- (d) F–.
(ii) What are the atomic numbers of the elements whose outermost electronic configurations are represented by:
(a) 3s1 (b) 2p3 and (c) 3p5?
(iii) Which atoms are indicated by the following configurations?
(a) [He]2s1 (b) [Ne] 3s2 3p3 (c) [Ar] 4s2 3d1.
(i) Write the electronic configuration of the following ions :
(a) H (b) Na+ (c) O2- (d) F–.
(ii) What are the atomic numbers of the elements whose outermost electronic configurations are represented by:
(a) 3s1 (b) 2p3 and (c) 3p5?
(iii) Which atoms are indicated by the following configurations?
(a) [He]2s1 (b) [Ne] 3s2 3p3 (c) [Ar] 4s2 3d1.
(i) (a) 1s2 (b) 1s2 2s2 2p6 (c) 1s22s22p6 (d) 1s22s22p6.
(ii) (a) Na (Z = 11) has outermost electronic configuration = 3s1
(b) N (Z = 7) has outermost electronic configuration = 2p3
(c) Cl (Z = 17) has outermost electronic con
Upvote Which of the following are iso-electronic species i.e., those having the same number of electrons?
Na+, K+, Mg2+, Ca2+, S2-, Ar.
Which of the following are iso-electronic species i.e., those having the same number of electrons?
Na+, K+, Mg2+, Ca2+, S2-, Ar.
Na+ and Mg2+ are iso-electronic species having 10 electrons each. K+, Ca2+, S2- are iso-electronic species having 18 electrons each.
Upvote The mass of an electron is 9.1 × 10-31 kg. If its kinetic energy is 3.0 × 10-25 J, calculate its wavelength.
The mass of an electron is 9.1 × 10-31 kg. If its kinetic energy is 3.0 × 10-25 J, calculate its wavelength.
Kinetic energy. K.E. = ½ mv2
=> v2 = (2 x K.E.) / m
Given, K.E. = 3 x 10-25 J = 3 x 10-25 kg m2 s-2
Therefore, v2 = [2 x (3 x 10-25 kg m2 s-2)] / 9.1 x 10-31 kg
=> v2= 65.9 x 104 m2 s-2
=>v = 8.12 x 102 m s-1
To calculate the wavelength of the electron
According to de Broglie’s equation,
λ=h/mv = (6
Upvote Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 m s-1.
Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 m s-1.
We know that the mass of an electron, me = 9.1 x 10-31 kg,
Velocity of electron, v = 2.05 × 107 m s-1
We know that Planck’s constant, h = 6.626 x 10-34 kg m2 s-1
As per de Broglie’s equation, λ=h/mv
= (6.626 x 10-34 kg m2 s-1) / (9.1 x 10-31 kg) x (2.05 x 107 m s-1) = 3.55 x 10-11 m
Upvote The electronic energy in hydrogen atom is given by En = -2.18 × 10-18 / n2J. Calculate the energy required to remove an electron completely from the n = 2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?
The electronic energy in hydrogen atom is given by En = -2.18 × 10-18 / n2J. Calculate the energy required to remove an electron completely from the n = 2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?
Step I: Calculation of energy required
ΔE = E∞– E2
= 0 – (–2.18 × 10-18 J) / 4 = 5.45 x 10-19 J
Step II: Calculation of the longest wavelength of light in cm used to cause the transition
λ = hc / ΔE = (6.626 x 10-34 J s) x (3 x 108 ms-1) / (5.45 x 10-19 J)
= 3.644 x 10-7 x 102 = 3.645 x 10-5 cm.
Upvote What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of light emitted when the electron returns to the ground state? The ground state electronic energy is – 2.18 × 11-11 ergs.
What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of light emitted when the electron returns to the ground state? The ground state electronic energy is – 2.18 × 11-11 ergs.
Step I: calculation of energy required
Energy of electron (En) = (- 2.18 x 10-11ergs) / n2= (- 2.18 x 10-18 J) / n2
Energy in Bohr’s 1st orbit (E1) = (- 2.18 x 10-18 J) / 12
Energy in Bohr’s 5th orbit (E1) = (- 2.18 x 10-18 J) / 52
Therefore, energy required (ΔE) = E5 – E1 = [ (- 2.18 x 10-18 J) / 25] –
Upvote