Quizzes about: Atomic emission spectra, Bohr s atomic model and Rutherford atomic model

Quizzes about: Atomic emission spectra, Bohr s atomic model and Rutherford atomic model

Explore the key differences between Bohr’s atomic model and Rutherford’s atomic model, their historical context, and their implications for our understanding of atomic structure

This article provides a detailed comparison of two significant atomic models: Bohr’s atomic model and Rutherford’s atomic model. These models, developed in the early 20th century, marked significant advances in our understanding of atomic structure. We will explore their differences, their historical context, and how they contributed to the development of modern atomic theory.

Quiz 1 :atomic emission spectra to test your knowledge:

1-What is an atomic emission spectrum?

a) A spectrum of light emitted by excited atoms

b) A spectrum of light absorbed by atoms

c) A spectrum of light reflected by atoms

d) A spectrum of light scattered by atoms

2-Which scientist is credited with the discovery of atomic emission spectra and the development of the Bohr model of the atom?

a) Albert Einstein

b) Niels Bohr

c) Max Planck

d) Ernest Rutherford

3-Why do atoms emit light in the form of discrete lines in their emission spectra?

a) Because electrons move randomly in the atom

b) Because electrons transition between quantized energy levels

c) Because electrons orbit the nucleus continuously

d) Because electrons combine with protons to emit light

4-Which element is often used as a reference in atomic emission spectroscopy to calibrate instruments?

a) Helium

b) Neon

c) Hydrogen

d) Oxygen

5-In an atomic emission spectrum, each line represents a specific:

a) Atomic weight

b) Atomic number

c) Wavelength of emitted light

d) Number of electrons in the atom

6-Which of the following statements is true about the relationship between the energy of emitted photons and the energy levels of electrons in an atom?

a) The energy of emitted photons is not related to the energy levels of electrons.

b) The energy of emitted photons is proportional to the square of the energy levels of electrons.

c) The energy of emitted photons is equal to the energy difference between two electron energy levels.

d) The energy of emitted photons is inversely proportional to the energy levels of electrons.

7-When an electron transitions from a higher energy level to a lower energy level, is energy absorbed or emitted, and what type of spectrum is produced?

a) Energy is absorbed, and an absorption spectrum is produced.

b) Energy is emitted, and an absorption spectrum is produced.

c) Energy is absorbed, and an emission spectrum is produced.

d) Energy is emitted, and an emission spectrum is produced.

8-Which of the following factors can affect the positions of spectral lines in an atomic emission spectrum?

a) Temperature

b) Pressure

c) Atomic mass

d) All of the above

9-What do the intensity or brightness of the lines in an atomic emission spectrum represent?

a) The number of electrons in the atom

b) The probability of electron transitions

c) The energy of emitted photons

d) The concentration of atoms in the sample

10-In a flame test, which metal ion is often responsible for producing a bright green flame?

a) Sodium

b) Copper

c) Potassium

d) Barium

Answers:

1. a) A spectrum of light emitted by excited atoms
2. b) Niels Bohr
3. b) Because electrons transition between quantized energy levels
4. c) Hydrogen
5. c) Wavelength of emitted light
6. c) The energy of emitted photons is equal to the energy difference between two electron energy levels.
7. d) Energy is emitted, and an emission spectrum is produced.
8. a) Temperature
9. d) The concentration of atoms in the sample
10. c) Potassium

Quiz 2 :The line spectrum of hydrogen atom

Here’s a quiz about the line spectrum of the hydrogen atom:

1-Who is credited with the discovery and explanation of the line spectrum of the hydrogen atom?

a) Niels Bohr

b) Ernest Rutherford

c) Max Planck

d) Albert Einstein

2-What is the primary reason for the line spectrum of the hydrogen atom having discrete lines?

a) The electron’s random motion in the atom

b) The continuous variation in energy levels of the electron

c) The quantized energy levels in the hydrogen atom

d) The interaction of electrons with the nucleus

3-The Lyman series in the hydrogen spectrum consists of lines in which region of the electromagnetic spectrum?

a) Ultraviolet

b) Visible

c) Infrared

d) X-ray

4-Which quantum number is primarily responsible for defining the energy levels of electrons in the hydrogen atom?

a) Principal quantum number (n)

b) Angular momentum quantum number (l)

c) Magnetic quantum number (ml)

d) Spin quantum number (ms)

5-Which transition in the hydrogen atom results in the emission of the longest wavelength (lowest energy) photon in the visible spectrum?

a) n = 1 to n = 2

b) n = 2 to n = 3

c) n = 3 to n = 4

d) n = 4 to n = 5

6-The Balmer series in the hydrogen spectrum consists of lines in which region of the electromagnetic spectrum?

a) Ultraviolet

b) Visible

c) Infrared

d) Microwave

7-Which of the following spectral lines corresponds to the transition of an electron from the third energy level (n = 3) to the second energy level (n = 2) in the hydrogen atom?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

8-How is the intensity of the lines in the hydrogen spectrum related to the energy difference between energy levels?

a) The intensity is directly proportional to the energy difference.

b) The intensity is inversely proportional to the energy difference.

c) The intensity is unrelated to the energy difference.

d) The intensity is determined by the electron’s speed.

9-Which line in the hydrogen spectrum corresponds to the electron transitioning from the first energy level (n = 1) to the third energy level (n = 3)?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

10-In the hydrogen spectrum, what does the “n” value represent in the electron’s energy level?

a) The electron’s spin

b) The electron’s angular momentum

c) The electron’s principal quantum number

d) The electron’s magnetic quantum number

Answers:

1. a) Niels Bohr
2. c) The quantized energy levels in the hydrogen atom
3. a) Ultraviolet
4. a) Principal quantum number (n)
5. a) n = 1 to n = 2
6. b) Visible
7. b) Balmer series
8. b) The intensity is inversely proportional to the energy difference.
9. c) Paschen series
10. c) The electron’s principal quantum number

11-What is the significance of the Rydberg formula in the context of the hydrogen spectrum?

a) It describes the quantization of angular momentum in the hydrogen atom.

b) It calculates the wavelength of spectral lines in the hydrogen spectrum.

c) It explains the magnetic properties of hydrogen atoms.

d) It defines the energy levels of electrons in the hydrogen atom.

12-Which of the following spectral series in the hydrogen spectrum involves transitions to the fifth energy level (n = 5)?

a) Lyman series

b) Balmer series

c) Paschen series

d) Pfund series

13-What is the value of the principal quantum number (n) for the first energy level in the hydrogen atom?

a) n = 0

b) n = 1

c) n = 2

d) n = 3

14-When an electron in the hydrogen atom transitions from a higher energy level to a lower energy level, is energy absorbed or emitted, and what type of spectrum is produced?

a) Energy is absorbed, and an absorption spectrum is produced.

b) Energy is emitted, and an absorption spectrum is produced.

c) Energy is absorbed, and an emission spectrum is produced.

d) Energy is emitted, and an emission spectrum is produced.

15-The spectral lines in the hydrogen spectrum are often named after the scientists who contributed to their discovery. Which scientist is associated with the “Lyman” series of lines?

a) Max Planck

b) Niels Bohr

c) Theodore Lyman

d) Albert Einstein

Answers:

11. b) It calculates the wavelength of spectral lines in the hydrogen spectrum.
12. d) Pfund series
13. b) n = 1
14. d) Energy is emitted, and an emission spectrum is produced.
15. c) Theodore Lyman

Quiz 3: Bohr s postulates of atomic model

Here’s a quiz about Niels Bohr’s postulates of the atomic model:

1-Niels Bohr’s atomic model was primarily developed for which element?

a) Hydrogen

b) Helium

c) Oxygen

d) Carbon

2-According to Bohr’s first postulate, electrons in an atom revolve around the nucleus in specific orbits. What is the term for these allowed orbits?

a) Energy bands

b) Energy shells

c) Energy levels

d) Energy paths

3-Bohr’s second postulate states that electrons in these orbits have quantized values of what physical quantity?

a) Charge

b) Mass

c) Energy

d) Spin

4-According to Bohr’s third postulate, what happens when an electron transitions from one energy level to another within an atom?

a) It emits or absorbs a photon of energy

b) It combines with a proton

c) It changes its mass

d) It gains or loses electrons

5-Which of the following statements accurately describes the relationship between the energy levels in Bohr’s atomic model?

a) The energy levels are equally spaced.

b) The energy levels are inversely proportional to the principal quantum number.

c) The energy levels are directly proportional to the principal quantum number.

d) The energy levels are unrelated to the principal quantum number.

6-According to Bohr’s fourth postulate, in which situation does an electron not emit or absorb radiation?

a) When it transitions to a higher energy level

b) When it transitions to a lower energy level

c) When it remains in a stationary orbit

d) When it changes its spin direction

7-Bohr’s fifth postulate explains that the angular momentum of an electron in a particular orbit is quantized. Which formula represents the quantization of angular momentum in Bohr’s model?

a) L = mvr

b) E = mc^2

c) F = ma

d) E = hf

8-According to Bohr’s sixth postulate, when an electron moves to a higher energy level, it absorbs energy and moves to a lower energy level, it emits energy. What type of electromagnetic radiation does it emit or absorb?

a) Gamma rays

b) Infrared radiation

c) Ultraviolet radiation

d) X-rays

9-Bohr’s seventh postulate introduces a concept that explains why electrons in certain orbits do not lose energy and spiral into the nucleus. What is this concept called?

a) Quantum spin

b) Quantum tunneling

c) Quantum leap

d) Quantum stability

10-In Bohr’s atomic model, what happens when an electron transitions from a higher energy level to a lower energy level and emits a photon?

a) The electron’s speed increases

b) The electron’s angular momentum decreases

c) The electron’s charge changes

d) The electron’s energy increases

Answers:

1. a) Hydrogen
2. c) Energy levels
3. c) Energy
4. a) It emits or absorbs a photon of energy
5. c) The energy levels are directly proportional to the principal quantum number.
6. c) When it remains in a stationary orbit
7. a) L = mvr
8. c) Ultraviolet radiation
9. d) Quantum stability
10. b) The electron’s angular momentum decreases

11-Bohr’s atomic model was a significant improvement over the earlier Rutherford model. What was the major shortcoming of Rutherford’s model that Bohr’s model addressed?

a) It couldn’t explain the stability of the atom.

b) It couldn’t account for the quantization of energy levels.

c) It couldn’t describe the behavior of electrons.

d) It couldn’t explain the presence of a nucleus.

12-According to Bohr’s model, what happens to an electron when it is in its lowest energy level (n = 1)?

a) It is in its most stable state and cannot absorb or emit energy.

b) It is in its most excited state.

c) It emits energy continuously.

d) It is not bound to the nucleus.

13-Bohr’s model successfully explained the line spectrum of which element, providing strong support for his postulates?

a) Helium

b) Oxygen

c) Hydrogen

d) Carbon

14-Bohr’s model was later replaced by the quantum mechanical model, which provided a  accurate description of atomic behavior. What is the key difference between Bohr’s model and the quantum mechanical model?

a) Bohr’s model describes the wave-like behavior of electrons.

b) Bohr’s model is based on classical physics, while the quantum mechanical model incorporates wave-particle duality.

c) Bohr’s model accurately predicts the position and momentum of electrons.

d) Bohr’s model does not consider energy quantization.

15-What did Bohr’s atomic model contribute to our understanding of atomic structure and behavior, even though it was eventually replaced by the quantum mechanical model?

a) It explained the chemical properties of elements.

b) It provided a foundation for understanding energy quantization in atoms.

c) It accurately described the behavior of electrons.

d) It introduced the concept of atomic mass.

Answers:

11. a) It couldn’t explain the stability of the atom.
12. a) It is in its most stable state and cannot absorb or emit energy.
13. c) Hydrogen
14. b) Bohr’s model is based on classical physics, while the quantum mechanical model incorporates wave-particle duality.
15. b) It provided a foundation for understanding energy quantization in atoms.

Quiz 4: points that Bohr agree with Rutherford postulates

 Niels Bohr’s atomic model built upon Ernest Rutherford’s nuclear model of the atom while introducing some key modifications. Here’s a quiz about the points on which Bohr’s model agreed with Rutherford’s postulates:

1-Rutherford’s model proposed that the atom consists of a central nucleus. What aspect of this postulate did Bohr agree with?

a) The nucleus is positively charged.

b) Electrons revolve around the nucleus.

c) The nucleus contains most of the atom’s mass.

d) Electrons are evenly distributed within the nucleus.

2-Rutherford’s model suggested that electrons orbit the nucleus. Which aspect of this orbital motion did Bohr accept in his model?

a) Electrons can move in any random path.

b) Electrons move in quantized, circular orbits.

c) Electrons move in continuous, spiral paths.

d) Electrons move with constant velocity.

3-Rutherford’s model described the central nucleus as positively charged. What did Bohr agree with regarding the charge of the nucleus?

a) The nucleus contains both positive and negative charges.

b) The nucleus is negatively charged.

c) The nucleus is electrically neutral.

d) The nucleus is positively charged.

4-Rutherford’s model stated that electrons move freely in space within their allowed orbits. What did Bohr agree with concerning the motion of electrons within orbits?

a) Electrons move in spiral paths.

b) Electrons can occupy any energy level.

c) Electrons have quantized angular momentum.

d) Electrons emit continuous radiation.

5-Rutherford’s model suggested that electrons experience electrostatic attraction to the nucleus. What did Bohr agree with regarding this interaction?

a) Electrons experience a constant force from the nucleus.

b) Electrons experience quantized energy levels.

c) Electrons experience repulsion from the nucleus.

d) Electrons can exist without any interaction with the nucleus.

Answers:

1. c) The nucleus contains most of the atom’s mass.
2. b) Electrons move in quantized, circular orbits.
3. d) The nucleus is positively charged.
4. b) Electrons can occupy any energy level.
5. a) Electrons experience a constant force from the nucleus.

Bohr’s model improved upon Rutherford’s model by introducing the concept of quantized energy levels for electrons, but it retained the central nucleus and the electrostatic attraction between electrons and the nucleus.

Quiz 5 :New postulates of Bohr

Niels Bohr’s atomic model introduced several new postulates to explain the behavior of electrons in atoms. Here’s a quiz about Bohr’s new postulates:

1-Bohr introduced the idea that electrons in atoms can only exist in certain quantized energy levels. What is this principal quantum number, denoted by “n,” used to represent?

a) The electron’s charge

b) The electron’s mass

c) The electron’s energy level or shell

d) The electron’s angular momentum

2-Bohr’s model introduced the concept of angular momentum quantization. What formula is used to express the quantization of angular momentum in Bohr’s model?

a) L = n^2h/2π

b) E = mc^2

c) F = ma

d) E = hf

3-Bohr’s model postulated that when an electron is in a stable orbit, it does not emit or absorb radiation. What term is used to describe such stable orbits?

a) Stationary orbits

b) Quantum jumps

c) Spiral orbits

d) Circular paths

4-Bohr’s model suggested that when an electron transitions from a higher energy level to a lower energy level, it emits a photon. What equation relates the energy of a photon to this transition?

a) E = hf

b) L = n^2h/2π

c) F = ma

d) E = mc^2

5-According to Bohr’s model, which type of electromagnetic radiation is emitted when an electron transitions to a lower energy level within the atom?

a) Gamma rays

b) X-rays

c) Ultraviolet radiation

d) Infrared radiation

6-Bohr’s postulates included the idea that electrons in atoms are restricted to specific, quantized orbits. What term describes the allowed energy levels in his model?

a) Energy bands

b) Energy shells

c) Energy continuum

d) Energy valleys

7-One of Bohr’s postulates was that the angular momentum of an electron in a particular orbit is an integer multiple of h/2π, where “h” is Planck’s constant. Which quantum number is used to define these orbits?

a) Principal quantum number (n)

b) Angular momentum quantum number (l)

c) Magnetic quantum number (ml)

d) Spin quantum number (ms)

8-Bohr’s model successfully explained the spectral lines of which element, providing strong support for his new postulates?

a) Helium

b) Oxygen

c) Hydrogen

d) Carbon

Answers:

1. c) The electron’s energy level or shell
2. a) L = n^2h/2π
3. a) Stationary orbits
4. a) E = hf
5. c) Ultraviolet radiation
6. b) Energy shells
7. b) Angular momentum quantum number (l)
8. c) Hydrogen

9-Bohr’s atomic model postulated that electrons do not emit radiation while they are in stable orbits. What happens when an electron transitions from one stable orbit to another?

a) It emits a photon.

b) It absorbs a photon.

c) It changes its charge.

d) It remains in the same orbit.

10-Bohr introduced the concept of quantized energy levels, but his model was limited to which type of atoms?

a) Only hydrogen atoms

b) All elements in the periodic table

c) Only noble gases

d) Only transition metals

11-Bohr’s model accounted for the line spectrum of the hydrogen atom. What is the name of the series of lines that correspond to transitions from higher energy levels to the second energy level (n = 2)?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

12-According to Bohr’s model, what happens when an electron absorbs energy and transitions to a higher energy level?

a) It emits a photon.

b) It emits an electron.

c) It moves closer to the nucleus.

d) It gains energy and changes its principal quantum number.

Answers:

9. a) It emits a photon.
10. a) Only hydrogen atoms
11. b) Balmer series
12. d) It gains energy and changes its principal quantum number.

Bohr’s model was specifically developed to describe the hydrogen atom and its line spectrum, and its postulates were not applicable to  complex atoms or ions.

Quiz 6 :The visible line spectrum of hydrogen atom

Here’s a quiz about the visible line spectrum of the hydrogen atom:

1-In the visible line spectrum of the hydrogen atom, which spectral series corresponds to transitions of electrons from higher energy levels to the second energy level (n = 2)?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

2-What is the spectral series in the hydrogen atom that corresponds to transitions to the first energy level (n = 1) and is found in the ultraviolet region of the electromagnetic spectrum?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

3-Which spectral series in the hydrogen atom involves transitions to the third energy level (n = 3) and is found in the infrared region of the electromagnetic spectrum?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

4-What is the principle quantum number (n) for the spectral lines in the Balmer series of the hydrogen atom’s visible line spectrum?

a) n = 1

b) n = 2

c) n = 3

d) n = 4

5-Which spectral series in the hydrogen atom results from transitions to the fourth energy level (n = 4)?

a) Lyman series

b) Balmer series

c) Paschen series

d) Brackett series

6-The Balmer series of the hydrogen atom’s visible line spectrum primarily consists of which type of lines?

a) Ultraviolet lines

b) Infrared lines

c) Visible lines

d) X-ray lines

7-When an electron in the hydrogen atom transitions from a higher energy level to a lower energy level, is energy absorbed or emitted, and what type of spectrum is produced?

a) Energy is absorbed, and an absorption spectrum is produced.

b) Energy is emitted, and an absorption spectrum is produced.

c) Energy is absorbed, and an emission spectrum is produced.

d) Energy is emitted, and an emission spectrum is produced.

Answers:

1. b) Balmer series
2. a) Lyman series
3. c) Paschen series
4. d) n = 4
5. d) Brackett series
6. c) Visible lines
7. d) Energy is emitted, and an emission spectrum is produced.

Quiz  7: The advantages of Bohr s atomic model

Here’s a quiz about the advantages of Bohr’s atomic model:

1-What was one significant advantage of Bohr’s atomic model over the earlier Rutherford model?

a) It accurately described the wave-particle duality of electrons.

b) It successfully explained the stability of atoms.

c) It provided a complete mathematical framework for atomic behavior.

d) It accounted for the existence of the nucleus.

2-Bohr’s atomic model was the first to introduce quantization of energy levels for electrons. What is the advantage of this quantization concept?

a) It allows electrons to move freely within the atom.

b) It explains the continuous spectrum of atomic emission.

c) It provides a basis for explaining atomic spectra and the allowed transitions.

d) It describes the random motion of electrons in atoms.

3-Bohr’s model explained the line spectrum of the hydrogen atom. What advantage did this model provide in understanding atomic behavior?

a) It accurately predicted the precise positions of electrons.

b) It successfully described the behavior of electrons in all elements.

c) It showed that electrons could exist in any energy level.

d) It offered a quantitative explanation for the observed spectral lines.

4-Bohr’s model introduced the concept of quantized angular momentum for electrons in specific orbits. What was one advantage of this concept?

a) It explained the distribution of electrons in the atom.

b) It accounted for the electron’s spiral motion around the nucleus.

c) It allowed for continuous transitions between energy levels.

d) It described the stability of electrons in specific orbits.

5-Bohr’s model was a crucial stepping stone in the development of quantum mechanics. What advantage did it provide in this context?

a) It completely replaced quantum mechanics.

b) It laid the foundation for understanding wave-particle duality.

c) It demonstrated the invalidity of quantization.

d) It introduced the concept of atomic mass.

Answers:

1. b) It successfully explained the stability of atoms.
2. c) It provides a basis for explaining atomic spectra and the allowed transitions.
3. d) It offered a quantitative explanation for the observed spectral lines.
4. d) It described the stability of electrons in specific orbits.
5. b) It laid the foundation for understanding wave-particle duality.

Bohr’s atomic model had several advantages, including explaining the stability of atoms, quantized energy levels, and the spectral lines of hydrogen. However, it was later replaced by the  comprehensive quantum mechanical model.

Quiz 8: inadequacies of Bohr s atomic model

Here’s a quiz about the inadequacies of Bohr’s atomic model:

1-One of the major inadequacies of Bohr’s atomic model was its inability to explain the behavior of atoms with  than one electron. What was the specific issue?

a) It could not account for the quantization of energy levels.

b) It failed to predict the existence of the nucleus.

c) It could not accurately describe the spectrum of helium.

d) It lacked a mathematical framework for multi-electron atoms.

2-Bohr’s model suggested that electrons move in circular orbits. What inadequacy does this assumption have when applied to electrons in reality?

a) Electrons move in non-circular orbits.

b) Electrons do not move in quantized orbits.

c) Electrons do not experience electrostatic attraction.

d) Electrons move with constant velocity.

3-One inadequacy of Bohr’s model was its inability to explain the fine structure of spectral lines, especially in heavy atoms. What concept did it lack to address this issue?

a) Quantization of energy levels

b) Wave-particle duality

c) Relativity

d) Electromagnetic radiation

4-Bohr’s model successfully explained the line spectrum of hydrogen but failed to provide a general framework for all elements. What was the main limitation in this regard?

a) It couldn’t describe quantized energy levels.

b) It couldn’t explain the structure of the nucleus.

c) It didn’t account for the electrostatic attraction between electrons and the nucleus.

d) It lacked a generalization to accommodate multi-electron atoms.

5-What inadequacy in Bohr’s model led to the development of the quantum mechanical model of the atom?

a) It couldn’t describe electron orbits.

b) It couldn’t explain quantization.

c) It couldn’t account for the emission and absorption of radiation.

d) It couldn’t explain wave-particle duality.

Answers:

1. d) It lacked a mathematical framework for multi-electron atoms.
2. a) Electrons move in non-circular orbits.
3. c) Relativity
4. d) It lacked a generalization to accommodate multi-electron atoms.
5. b) It couldn’t explain quantization.

Bohr’s model was a significant advancement but had inadequacies, particularly when applied to atoms with  than one electron. These limitations led to the development of the quantum mechanical model to address these issues.

6-One of the inadequacies of Bohr’s model was its inability to explain the splitting of spectral lines in the presence of a magnetic field. What phenomenon did it fail to account for?

a) Absorption of radiation

b) Zeeman effect

c) Photoelectric effect

d) Diffraction

7-Bohr’s model assumed that electrons moved in fixed orbits, which violated Heisenberg’s Uncertainty Principle. What inadequacy does this violate?

a) It contradicts the quantization of energy levels.

b) It ignores the probabilistic nature of electron behavior.

c) It fails to explain the wave-particle duality of electrons.

d) It violates the concept of relativity.

8-Bohr’s model was unable to provide a comprehensive explanation for the chemical properties and behavior of atoms. What concept was missing to address this inadequacy?

a) Quantization of energy levels

b) Wave-particle duality

c) Quantum numbers

d) Electron probability distribution

9-Bohr’s model assumed that electrons moved in stable, quantized orbits, which could not account for the continuous and variable transitions of electrons within atoms. What inadequacy did this assumption have?

a) It failed to predict the existence of the nucleus.

b) It contradicted the principle of electrostatic attraction.

c) It ignored the quantization of angular momentum.

d) It couldn’t explain the observed emission and absorption spectra.

10-One of the key inadequacies of Bohr’s model was its inability to explain the fine structure of spectral lines, especially for heavy elements. What was the primary cause of this inadequacy?

a) Failure to account for the quantization of energy levels

b) Lack of a complete mathematical framework

c) Neglect of wave-particle duality

d) Absence of the concept of quantization of angular momentum

Answers:

6. b) Zeeman effect
7. b) It ignores the probabilistic nature of electron behavior.
8. d) Electron probability distribution
9. d) It couldn’t explain the observed emission and absorption spectra.
10. c) Neglect of wave-particle duality.

Bohr’s atomic model had several inadequacies, particularly when applied to  complex atoms and elements, which were addressed by the development of the quantum mechanical model.

compare between :Bohr s atomic model and Rutherford atomic model in tabular format