Green Bridge Learning Resource For Structure Of The Atom (Nigeria Only)

Overview

The study of the 'Structure of the Atom' is crucial in understanding the fundamental building blocks of matter and the behavior of atoms. Throughout history, several models of the atom have been proposed, each contributing to our evolving comprehension of atomic structure. One of the earliest models was proposed by Thomson, who suggested the Plum Pudding model, envisioning electrons embedded in a positively charged sphere.

Rutherford then introduced the Nuclear model, emphasizing a dense, positively charged nucleus orbited by electrons. This model was instrumental in revealing the nucleus's presence and the atom's mostly empty space. Subsequently, Bohr proposed the Quantized model, incorporating quantization of angular momentum and discrete energy levels, revolutionizing atomic physics.

Transitioning to more modern theories, the Electron Cloud (Wave-Mechanical) model describes electrons as both particles and waves, demonstrating the uncertainty principle and the probability distribution of electron locations within the atom. Each model has its limitations; for instance, the Bohr model struggles with heavier elements due to its simplistic structure.

The concept of quantization of angular momentum, as depicted in the Bohr model, underpins the discrete energy levels within an atom. This quantization explains the stability of certain orbits and the emission or absorption of energy when electrons transition between levels, leading to the emission of specific light frequencies correlated with energy differences.

The interplay between light frequencies and colors in atomic structure is crucial in understanding spectroscopy. Experiments such as the Frank-Hertz experiment elucidate the quantization of energy levels through electron collisions with atoms, resulting in distinct energy thresholds and corresponding spectral lines.

Furthermore, the observation of line spectra from hot bodies and elements provides valuable insights into atomic structure, revealing unique spectral signatures associated with different elements. The study of absorption spectra and spectra of discharge lamps further refines our understanding by illustrating the absorption and emission of light at specific frequencies characteristic of the elements involved.

Objectives

Illustrate energy levels in an atom
Understand the historical development of models of the atom
Examine line spectra from hot bodies
Investigate absorption spectra and spectra of discharge lamps
Analyze the limitations of each model
Correlate color and light frequency in atomic structure
Analyze the outcomes of the Frank-Hertz experiment
Differentiate between Thomson, Rutherford, Bohr, and electron cloud models qualitatively
Explain the concept of quantization of angular momentum (Bohr model)

Lesson Note

Atoms are the fundamental building blocks of matter. Understanding the structure of the atom is essential for comprehending the principles of chemistry and physics. Over the centuries, the model of the atom has evolved significantly as scientists have conducted various experiments and refined their theories.

Lesson Evaluation

Congratulations on completing the lesson on Structure Of The Atom (Nigeria Only). Now that youve explored the key concepts and ideas, its time to put your knowledge to the test. This section offers a variety of practice questions designed to reinforce your understanding and help you gauge your grasp of the material.

You will encounter a mix of question types, including multiple-choice questions, short answer questions, and essay questions. Each question is thoughtfully crafted to assess different aspects of your knowledge and critical thinking skills.

Use this evaluation section as an opportunity to reinforce your understanding of the topic and to identify any areas where you may need additional study. Don't be discouraged by any challenges you encounter; instead, view them as opportunities for growth and improvement.

What is the model of the atom proposed by J.J. Thomson? A. Plum pudding model B. Nuclear model C. Planetary model D. Electron cloud model Answer: A. Plum pudding model
Who conducted the famous gold foil experiment that led to the discovery of the atomic nucleus? A. Ernest Rutherford B. Niels Bohr C. James Chadwick D. Robert Millikan Answer: A. Ernest Rutherford
Which model of the atom suggests that electrons orbit the nucleus in discrete energy levels? A. Rutherford model B. Bohr model C. Electron cloud model D. Wave-mechanical model Answer: B. Bohr model
What phenomenon demonstrates that light consists of packets of energy known as photons? A. Photoelectric effect B. Compton scattering C. Interference D. Refraction Answer: A. Photoelectric effect
Which type of emission occurs when electrons are ejected from a metal surface due to the absorption of energy? A. Photoelectric emission B. Thermionic emission C. Field emission D. Secondary emission Answer: A. Photoelectric emission
In X-ray production, what is the name of the process where high-speed electrons are suddenly decelerated by a target material, resulting in the emission of X-rays? A. Bremsstrahlung B. Compton effect C. Photoelectric absorption D. Auger effect Answer: A. Bremsstrahlung
What experiment provided direct evidence for the existence of quantized energy levels in atoms? A. Frank-Hertz experiment B. Rutherford scattering experiment C. Millikan oil drop experiment D. Michelson-Morley experiment Answer: A. Frank-Hertz experiment
What term is used to describe the specific frequencies of light emitted by an element when its electrons transition between energy levels? A. Continuous spectrum B. Band spectrum C. Line spectrum D. Absorption spectrum Answer: C. Line spectrum
Which type of spectrum is produced when a continuous spectrum is passed through a cool gas, resulting in dark lines at specific wavelengths? A. Atomic spectrum B. Emission spectrum C. Absorption spectrum D. Line spectrum Answer: C. Absorption spectrum
What type of spectrum is produced when an electric current is passed through a low-pressure gas, resulting in distinct colored lines? A. Atomic spectrum B. Emission spectrum C. Band spectrum D. Line spectrum Answer: B. Emission spectrum

Recommended Books

	Modern Physics Subtitle Models of the Atom and Spectroscopy Publisher Pearson Year 2015 ISBN 978-0321976420
	Quantum Mechanics Subtitle Historical Perspective and Modern Developments Publisher Springer Year 2003 ISBN 978-3540209326

Past Questions

Wondering what past questions for this topic looks like? Here are a number of questions about Structure Of The Atom (Nigeria Only) from previous years

JAMB UTME - Physics - 2023 (Click to take full assessment)

Question 1 Report

What is the name of the model of the atom that describes electrons as orbiting the nucleus in specific energy levels?

Bohr model

Dalton model

Rutherford model

Thomson model

View Answer

NECO SSCE - Physics - 2009 (Click to take full assessment)

Question 1 Report

The phenomenon of photoelectric effect is used in the following EXCEPT

automatic doors

bugler alarm

electric fire alarm

sound production from film tracks

television cameras

View Answer

WAEC SSCE - Physics - 2022 (Click to take full assessment)

Question 1 Report

(a)(i) What is meant by the term artificial radioactivity?

(ii) Complete the table below

Emission	Nature	Charge	Ionizing
	High speed electron		Moderately ionizing
		Neutral	Negligible ionizing ability
Alpha particles		Positive

(b) In an x-ray tube, an electron is accelerated from rest towards a metal target by a 30 kV source. Calculate the kinetic energy of the electron. [e=1.6 x 10 $^{- 19}$ C]

(c) The table below shows the frequencies of radiations incident on a certain metal and the corresponding kinetic energies of the photoelectrons.

Frequency x 10 $^{14}$ (Hz)	6.8	8.0	9.2	10.0	11.0
Kinetic energy x 10 $^{- 19}$ (j)	0.8	1.6	2.4	2.9	3.8

(i) Plot a graph of kinetic energy, K.E, on the vertical axis and frequency, f, on the horizontal axis starting both axes from the origin (0,0).

(ii) From the graph, determine the:

i. Planck's constant;

ii. Threshold frequency of radiations;

iii. Work function of the metal.

Answer

(a)() Meaning of artificial radioactivity;

The process by which a stable nucleus is bombarded with a neutron to make it unstable and so disintegrates/decays with the emission of particles/radiation and. energy.

Emission	Nature	Charge	Ionizing
Beta ($\beta$)	High speed electron	Negative	Moderately ionizing
Gamma ($\gamma$)	Electro-magnetic radiation	Neutral	Negligible ionizing ability
Alpha particles	Helium nucleus	Positive	Highly ionizing

(b) The kinetic energy of the electron can be calculated using the formula: KE = qV, where q is the charge of the electron and V is the potential difference. Substituting the given values, we get:

K.E = eV

KE = (1.6 x 10^-19 C)(30,000 V)

KE = 4.8 x 10^-15 J (c)

(i)

To calculate the slope of the graph, you need to determine the change in the dependent variable (kinetic energy) divided by the change in the independent variable (frequency). In this case, you can choose any two points on the graph and calculate the slope using the following formula:

slope = (kinetic_energy2 - kinetic_energy1) / (frequency2 - frequency1)

Let's take two points from the given data, for example:

Point 1: (frequency1, kinetic_energy1) = (6.8 x 10^14 Hz, 0.8 x 10^-19 J)
Point 2: (frequency2, kinetic_energy2) = (8.0 x 10^14 Hz, 1.6 x 10^-19 J)

Now, we can calculate the slope:

slope = (1.6 x 10^-19 J - 0.8 x 10^-19 J) / (8.0 x 10^14 Hz - 6.8 x 10^14 Hz)

slope = 1 x 10^-5 J Hz^(-1).

To determine Planck's constant from the given graph and slope, we can use the equation:

slope = h / e

where h is Planck's constant and e is the elementary charge (1.602176634 x 10^-19 C).

From the previous calculation, the slope of the graph is 1 x 10^-5 J Hz^(-1).

Let's substitute the values into the equation to solve for Planck's constant:

1 x 10^-5 J Hz^(-1) = h / (1.602176634 x 10^-19 C)

To isolate h, we can rearrange the equation:

h = slope * e

Substituting the values:

h = (1 x 10^-5 J Hz^(-1)) * (1.602176634 x 10^-19 C)

Evaluating the expression:

h ≈ 1.602176634 x 10^-24 J·s

Therefore, from the given graph and slope, the approximate value of Planck's constant is 1.602176634 x 10^-24 J·s.

(ii) To determine the threshold frequency of radiation from the given information, we need to use the concept of the photoelectric effect and the relationship between the kinetic energy of photoelectrons and the frequency of incident radiation.

According to the photoelectric effect, electrons are ejected from a metal surface when illuminated by electromagnetic radiation of sufficient energy. The minimum frequency of radiation required to eject electrons is known as the threshold frequency.

The relationship between the kinetic energy of photoelectrons and the frequency of incident radiation is given by the equation:

K.E. = h * (frequency - threshold_frequency)

where K.E. is the kinetic energy of the photoelectrons, h is Planck's constant, frequency is the frequency of incident radiation, and threshold_frequency is the threshold frequency.

From the graph, we have the slope, which is equal to h, and the kinetic energy corresponding to each frequency. We can select any point on the graph where the kinetic energy is non-zero and solve for the threshold frequency.

Let's choose the point (frequency, kinetic energy) = (6.8 x 10^14 Hz, 0.8 x 10^-19 J) from the given data.

0.8 x 10^-19 J = slope * (6.8 x 10^14 Hz - threshold_frequency)

Substituting the slope value:

0.8 x 10^-19 J = 1.602176634 x 10^-24 J·s * (6.8 x 10^14 Hz - threshold_frequency)

To solve for the threshold frequency, we can rearrange the equation:

threshold_frequency = 6.8 x 10^14 Hz - (0.8 x 10^-19 J / (1.602176634 x 10^-24 J·s))

Calculating the threshold frequency:

threshold_frequency = 6.8 x 10^14 Hz - 4.992706701 x 10^4 Hz

threshold_frequency ≈ 6.799500729 x 10^14 Hz

Therefore, the threshold frequency of radiation is approximately 6.799500729 x 10^14 Hz.

(iii)

To determine the work function of the metal, we can use the equation:

Work function = h * threshold_frequency

where h is Planck's constant and threshold_frequency is the threshold frequency of radiation.

From the previous calculations, the approximate value of Planck's constant is 1.602176634 x 10^-24 J·s and the threshold frequency is approximately 6.799500729 x 10^14 Hz.

Substituting these values into the equation, we can calculate the work function:

Work function = (1.602176634 x 10^-24 J·s) * (6.799500729 x 10^14 Hz)

Work function ≈ 1.090589631 x 10^-9 J

Therefore, based on the given information, the approximate value of the work function of the metal is 1.090589631 x 10^-9 J.

Answer Details

(a)() Meaning of artificial radioactivity;

The process by which a stable nucleus is bombarded with a neutron to make it unstable and so disintegrates/decays with the emission of particles/radiation and. energy.

Emission	Nature	Charge	Ionizing
Beta ($\beta$)	High speed electron	Negative	Moderately ionizing
Gamma ($\gamma$)	Electro-magnetic radiation	Neutral	Negligible ionizing ability
Alpha particles	Helium nucleus	Positive	Highly ionizing

(b) The kinetic energy of the electron can be calculated using the formula: KE = qV, where q is the charge of the electron and V is the potential difference. Substituting the given values, we get:

K.E = eV

KE = (1.6 x 10^-19 C)(30,000 V)

KE = 4.8 x 10^-15 J (c)

(i)

slope = 1 x 10^-5 J Hz^(-1).

(iii)

View Answer