Bohr Model of the Hydrogen Atom
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PHXII12:ATOMS

356447 For the ground state the electron in the \(H\)-atom has an angular momentum \(h\), according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true,

1 Because angular momentum must be in the direction of spin of electron
2 Because Bohr model gives incorrect values of angular momentum
3 Because only one of these would have a minimum energy
4 Because electrons go around only in circular orbits
NCERT Exemplar
PHXII12:ATOMS

356448 The main defect of Bohr’s atomic model is

1 Can’t explain Zeeman effect
2 Can’t explain spectra of more complex atoms
3 Can’t explain fine structure of spectral lines
4 All of the above
PHXII12:ATOMS

356449 The energy of an electron in excited hydrogen atom is \( - 3.4\,eV\). Then, according to Bohr's theory, the angular momentum of the electron is

1 \(2.1 \times {10^{ - 34}}\;J - s\)
2 \(3 \times {10^{ - 34}}\;J - s\)
3 \(2 \times {10^{ - 34}}\;J - s\)
4 \(0.5 \times {10^{ - 34}}\;J - s\)
PHXII12:ATOMS

356450 For atomic model of hydrogen atom given by Niels Bohr, match the following proportionalities.
Column I
Column II
A
Angular momentum
P
\(1/n\)
B
Velocity of electron
Q
\({n^2}\)
C
Radius of electron
R
\(1/{n^2}\)
D
Energy of electron
S
\(n\)

1 A-P, B-Q, C-R, D-S
2 A-S, B-R, C-Q, D-P
3 A-S, B-P, C-R, D-Q
4 A-S, B-P, C-Q, D-R
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PHXII12:ATOMS

356447 For the ground state the electron in the \(H\)-atom has an angular momentum \(h\), according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true,

1 Because angular momentum must be in the direction of spin of electron
2 Because Bohr model gives incorrect values of angular momentum
3 Because only one of these would have a minimum energy
4 Because electrons go around only in circular orbits
NCERT Exemplar
PHXII12:ATOMS

356448 The main defect of Bohr’s atomic model is

1 Can’t explain Zeeman effect
2 Can’t explain spectra of more complex atoms
3 Can’t explain fine structure of spectral lines
4 All of the above
PHXII12:ATOMS

356449 The energy of an electron in excited hydrogen atom is \( - 3.4\,eV\). Then, according to Bohr's theory, the angular momentum of the electron is

1 \(2.1 \times {10^{ - 34}}\;J - s\)
2 \(3 \times {10^{ - 34}}\;J - s\)
3 \(2 \times {10^{ - 34}}\;J - s\)
4 \(0.5 \times {10^{ - 34}}\;J - s\)
PHXII12:ATOMS

356450 For atomic model of hydrogen atom given by Niels Bohr, match the following proportionalities.
Column I
Column II
A
Angular momentum
P
\(1/n\)
B
Velocity of electron
Q
\({n^2}\)
C
Radius of electron
R
\(1/{n^2}\)
D
Energy of electron
S
\(n\)

1 A-P, B-Q, C-R, D-S
2 A-S, B-R, C-Q, D-P
3 A-S, B-P, C-R, D-Q
4 A-S, B-P, C-Q, D-R
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PHXII12:ATOMS

356447 For the ground state the electron in the \(H\)-atom has an angular momentum \(h\), according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true,

1 Because angular momentum must be in the direction of spin of electron
2 Because Bohr model gives incorrect values of angular momentum
3 Because only one of these would have a minimum energy
4 Because electrons go around only in circular orbits
NCERT Exemplar
PHXII12:ATOMS

356448 The main defect of Bohr’s atomic model is

1 Can’t explain Zeeman effect
2 Can’t explain spectra of more complex atoms
3 Can’t explain fine structure of spectral lines
4 All of the above
PHXII12:ATOMS

356449 The energy of an electron in excited hydrogen atom is \( - 3.4\,eV\). Then, according to Bohr's theory, the angular momentum of the electron is

1 \(2.1 \times {10^{ - 34}}\;J - s\)
2 \(3 \times {10^{ - 34}}\;J - s\)
3 \(2 \times {10^{ - 34}}\;J - s\)
4 \(0.5 \times {10^{ - 34}}\;J - s\)
PHXII12:ATOMS

356450 For atomic model of hydrogen atom given by Niels Bohr, match the following proportionalities.
Column I
Column II
A
Angular momentum
P
\(1/n\)
B
Velocity of electron
Q
\({n^2}\)
C
Radius of electron
R
\(1/{n^2}\)
D
Energy of electron
S
\(n\)

1 A-P, B-Q, C-R, D-S
2 A-S, B-R, C-Q, D-P
3 A-S, B-P, C-R, D-Q
4 A-S, B-P, C-Q, D-R
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PHXII12:ATOMS

356447 For the ground state the electron in the \(H\)-atom has an angular momentum \(h\), according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true,

1 Because angular momentum must be in the direction of spin of electron
2 Because Bohr model gives incorrect values of angular momentum
3 Because only one of these would have a minimum energy
4 Because electrons go around only in circular orbits
NCERT Exemplar
PHXII12:ATOMS

356448 The main defect of Bohr’s atomic model is

1 Can’t explain Zeeman effect
2 Can’t explain spectra of more complex atoms
3 Can’t explain fine structure of spectral lines
4 All of the above
PHXII12:ATOMS

356449 The energy of an electron in excited hydrogen atom is \( - 3.4\,eV\). Then, according to Bohr's theory, the angular momentum of the electron is

1 \(2.1 \times {10^{ - 34}}\;J - s\)
2 \(3 \times {10^{ - 34}}\;J - s\)
3 \(2 \times {10^{ - 34}}\;J - s\)
4 \(0.5 \times {10^{ - 34}}\;J - s\)
PHXII12:ATOMS

356450 For atomic model of hydrogen atom given by Niels Bohr, match the following proportionalities.
Column I
Column II
A
Angular momentum
P
\(1/n\)
B
Velocity of electron
Q
\({n^2}\)
C
Radius of electron
R
\(1/{n^2}\)
D
Energy of electron
S
\(n\)

1 A-P, B-Q, C-R, D-S
2 A-S, B-R, C-Q, D-P
3 A-S, B-P, C-R, D-Q
4 A-S, B-P, C-Q, D-R
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