307556
If an electron is present in \({\rm{n = 6}}\) level. How many spectral lines would be observed in case of H atom?
1 \({\rm{10}}\)
2 \({\rm{15}}\)
3 \({\rm{20}}\)
4 \({\rm{25}}\)
Explanation:
The no. of special lines is given by \(\frac{{{\rm{n(n - 1)}}}}{{\rm{2}}}\) When \({\rm{n = 6,}}\) the no. of spectral lines \({\rm{ = }}\frac{{{\rm{6 \times (6 - 1)}}}}{{\rm{2}}}{\rm{ = }}\frac{{{\rm{6 \times 5}}}}{{\rm{2}}}{\rm{ = 15}}\)
CHXI02:STRUCTURE OF ATOM
307557
Which one of the following transitions have minimum wavelength?
1 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\)
2 \(\mathrm{n}_{2} \rightarrow \mathrm{n}_{1}\)
3 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{2}\)
4 \(\mathrm{n}_{3} \rightarrow \mathrm{n}_{1}\)
Explanation:
\({\rm{E}} = \frac{{{\rm{hc}}}}{{\rm{\lambda }}}\) \(\therefore \mathrm{E} \propto \dfrac{1}{\lambda}\) \(\therefore\) Decrease in wavelength, increases the energy. \(\because\) Energy difference in \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition is maximum. \(\therefore \mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition has minimum wavelength.
CHXI02:STRUCTURE OF ATOM
307558
When the electron of a hydrogen atom jumps from n=4 to n=1 state, the number of spectral lines emitted is
1 15
2 9
3 6
4 3
Explanation:
When an electron jumps from higher energy level n = 4 to ground state (i.e. n = 1 ), the number of spectral lines \(=\dfrac{\mathrm{n}(\mathrm{n}-1)}{2}\) \(\therefore\) When an electron jumps from \(\mathrm{n}=4\) level, number of spectral lines \(=\dfrac{4(4-1)}{2}\) \(=\dfrac{4 \times 3}{2}=6\)
CHXI02:STRUCTURE OF ATOM
307559
Suppose that a hypothetical atom gives a red, green, blue and violet line spectrum. Which jump according to the figure would give off the red spectral line?
1 \(3 \rightarrow 1\)
2 \(2 \rightarrow 1\)
3 \(4 \rightarrow 1\)
4 \(3 \rightarrow 2\)
Explanation:
\(\mathrm{E}=\dfrac{\mathrm{hc}}{\lambda} \Rightarrow \mathrm{E} \propto \dfrac{1}{\lambda}\) Red line has highest wavelength so, lowest energy difference and minimum energy difference is between \(3 \rightarrow 2\) transition.
307556
If an electron is present in \({\rm{n = 6}}\) level. How many spectral lines would be observed in case of H atom?
1 \({\rm{10}}\)
2 \({\rm{15}}\)
3 \({\rm{20}}\)
4 \({\rm{25}}\)
Explanation:
The no. of special lines is given by \(\frac{{{\rm{n(n - 1)}}}}{{\rm{2}}}\) When \({\rm{n = 6,}}\) the no. of spectral lines \({\rm{ = }}\frac{{{\rm{6 \times (6 - 1)}}}}{{\rm{2}}}{\rm{ = }}\frac{{{\rm{6 \times 5}}}}{{\rm{2}}}{\rm{ = 15}}\)
CHXI02:STRUCTURE OF ATOM
307557
Which one of the following transitions have minimum wavelength?
1 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\)
2 \(\mathrm{n}_{2} \rightarrow \mathrm{n}_{1}\)
3 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{2}\)
4 \(\mathrm{n}_{3} \rightarrow \mathrm{n}_{1}\)
Explanation:
\({\rm{E}} = \frac{{{\rm{hc}}}}{{\rm{\lambda }}}\) \(\therefore \mathrm{E} \propto \dfrac{1}{\lambda}\) \(\therefore\) Decrease in wavelength, increases the energy. \(\because\) Energy difference in \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition is maximum. \(\therefore \mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition has minimum wavelength.
CHXI02:STRUCTURE OF ATOM
307558
When the electron of a hydrogen atom jumps from n=4 to n=1 state, the number of spectral lines emitted is
1 15
2 9
3 6
4 3
Explanation:
When an electron jumps from higher energy level n = 4 to ground state (i.e. n = 1 ), the number of spectral lines \(=\dfrac{\mathrm{n}(\mathrm{n}-1)}{2}\) \(\therefore\) When an electron jumps from \(\mathrm{n}=4\) level, number of spectral lines \(=\dfrac{4(4-1)}{2}\) \(=\dfrac{4 \times 3}{2}=6\)
CHXI02:STRUCTURE OF ATOM
307559
Suppose that a hypothetical atom gives a red, green, blue and violet line spectrum. Which jump according to the figure would give off the red spectral line?
1 \(3 \rightarrow 1\)
2 \(2 \rightarrow 1\)
3 \(4 \rightarrow 1\)
4 \(3 \rightarrow 2\)
Explanation:
\(\mathrm{E}=\dfrac{\mathrm{hc}}{\lambda} \Rightarrow \mathrm{E} \propto \dfrac{1}{\lambda}\) Red line has highest wavelength so, lowest energy difference and minimum energy difference is between \(3 \rightarrow 2\) transition.
307556
If an electron is present in \({\rm{n = 6}}\) level. How many spectral lines would be observed in case of H atom?
1 \({\rm{10}}\)
2 \({\rm{15}}\)
3 \({\rm{20}}\)
4 \({\rm{25}}\)
Explanation:
The no. of special lines is given by \(\frac{{{\rm{n(n - 1)}}}}{{\rm{2}}}\) When \({\rm{n = 6,}}\) the no. of spectral lines \({\rm{ = }}\frac{{{\rm{6 \times (6 - 1)}}}}{{\rm{2}}}{\rm{ = }}\frac{{{\rm{6 \times 5}}}}{{\rm{2}}}{\rm{ = 15}}\)
CHXI02:STRUCTURE OF ATOM
307557
Which one of the following transitions have minimum wavelength?
1 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\)
2 \(\mathrm{n}_{2} \rightarrow \mathrm{n}_{1}\)
3 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{2}\)
4 \(\mathrm{n}_{3} \rightarrow \mathrm{n}_{1}\)
Explanation:
\({\rm{E}} = \frac{{{\rm{hc}}}}{{\rm{\lambda }}}\) \(\therefore \mathrm{E} \propto \dfrac{1}{\lambda}\) \(\therefore\) Decrease in wavelength, increases the energy. \(\because\) Energy difference in \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition is maximum. \(\therefore \mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition has minimum wavelength.
CHXI02:STRUCTURE OF ATOM
307558
When the electron of a hydrogen atom jumps from n=4 to n=1 state, the number of spectral lines emitted is
1 15
2 9
3 6
4 3
Explanation:
When an electron jumps from higher energy level n = 4 to ground state (i.e. n = 1 ), the number of spectral lines \(=\dfrac{\mathrm{n}(\mathrm{n}-1)}{2}\) \(\therefore\) When an electron jumps from \(\mathrm{n}=4\) level, number of spectral lines \(=\dfrac{4(4-1)}{2}\) \(=\dfrac{4 \times 3}{2}=6\)
CHXI02:STRUCTURE OF ATOM
307559
Suppose that a hypothetical atom gives a red, green, blue and violet line spectrum. Which jump according to the figure would give off the red spectral line?
1 \(3 \rightarrow 1\)
2 \(2 \rightarrow 1\)
3 \(4 \rightarrow 1\)
4 \(3 \rightarrow 2\)
Explanation:
\(\mathrm{E}=\dfrac{\mathrm{hc}}{\lambda} \Rightarrow \mathrm{E} \propto \dfrac{1}{\lambda}\) Red line has highest wavelength so, lowest energy difference and minimum energy difference is between \(3 \rightarrow 2\) transition.
307556
If an electron is present in \({\rm{n = 6}}\) level. How many spectral lines would be observed in case of H atom?
1 \({\rm{10}}\)
2 \({\rm{15}}\)
3 \({\rm{20}}\)
4 \({\rm{25}}\)
Explanation:
The no. of special lines is given by \(\frac{{{\rm{n(n - 1)}}}}{{\rm{2}}}\) When \({\rm{n = 6,}}\) the no. of spectral lines \({\rm{ = }}\frac{{{\rm{6 \times (6 - 1)}}}}{{\rm{2}}}{\rm{ = }}\frac{{{\rm{6 \times 5}}}}{{\rm{2}}}{\rm{ = 15}}\)
CHXI02:STRUCTURE OF ATOM
307557
Which one of the following transitions have minimum wavelength?
1 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\)
2 \(\mathrm{n}_{2} \rightarrow \mathrm{n}_{1}\)
3 \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{2}\)
4 \(\mathrm{n}_{3} \rightarrow \mathrm{n}_{1}\)
Explanation:
\({\rm{E}} = \frac{{{\rm{hc}}}}{{\rm{\lambda }}}\) \(\therefore \mathrm{E} \propto \dfrac{1}{\lambda}\) \(\therefore\) Decrease in wavelength, increases the energy. \(\because\) Energy difference in \(\mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition is maximum. \(\therefore \mathrm{n}_{4} \rightarrow \mathrm{n}_{1}\) transition has minimum wavelength.
CHXI02:STRUCTURE OF ATOM
307558
When the electron of a hydrogen atom jumps from n=4 to n=1 state, the number of spectral lines emitted is
1 15
2 9
3 6
4 3
Explanation:
When an electron jumps from higher energy level n = 4 to ground state (i.e. n = 1 ), the number of spectral lines \(=\dfrac{\mathrm{n}(\mathrm{n}-1)}{2}\) \(\therefore\) When an electron jumps from \(\mathrm{n}=4\) level, number of spectral lines \(=\dfrac{4(4-1)}{2}\) \(=\dfrac{4 \times 3}{2}=6\)
CHXI02:STRUCTURE OF ATOM
307559
Suppose that a hypothetical atom gives a red, green, blue and violet line spectrum. Which jump according to the figure would give off the red spectral line?
1 \(3 \rightarrow 1\)
2 \(2 \rightarrow 1\)
3 \(4 \rightarrow 1\)
4 \(3 \rightarrow 2\)
Explanation:
\(\mathrm{E}=\dfrac{\mathrm{hc}}{\lambda} \Rightarrow \mathrm{E} \propto \dfrac{1}{\lambda}\) Red line has highest wavelength so, lowest energy difference and minimum energy difference is between \(3 \rightarrow 2\) transition.
