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The document appears to be a PowerPoint presentation submitted by Rakhi Babu for her B.Ed program at Kerala University. The presentation summarizes Rutherford's gold foil experiment, which provided evidence for the nuclear model of the atom by showing that alpha particles could be deflected by the small, dense nucleus at the center of the atom. The experiment led Rutherford to conclude that atoms have a small, dense, positively charged nucleus surrounded by electrons.
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Rutherford gold foil experiment
Rutherford performed an experiment in 1911 where he bombarded a thin gold foil with alpha particles. He observed that:
1) Most alpha particles passed through the foil without deflection.
2) A few particles were deflected by small angles.
3) Very few were deflected back at 180 degrees.
From these observations, Rutherford concluded that:
1) Atoms are mostly empty space.
2) A small, dense nucleus explains the few particles being deflected.
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1) Rutherford performed an experiment where he bombarded a thin gold foil with alpha particles and observed that most passed through without deflection, some were deflected by small angles, and a few were deflected back.
2) This led Rutherford to propose an atomic model where the atom has a small, dense nucleus containing its mass and positive charge, surrounded by electrons in orbits.
3) This was a major departure from the previous "plum pudding" model where charge and mass were thought to be uniformly distributed. However, Rutherford's model failed to explain the stability of electron orbits.
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Luminescence
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Rutherford gold foil experiment
Rutherford performed an experiment in 1911 where he bombarded a thin gold foil with alpha particles. He observed that:
1) Most alpha particles passed through the foil without deflection.
2) A few particles were deflected by small angles.
3) Very few were deflected back at 180 degrees.
From these observations, Rutherford concluded that:
1) Atoms are mostly empty space.
2) A small, dense nucleus explains the few particles being deflected.
3) The nucleus is much smaller than the atom.
Star
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- The model's main postulates include electrons revolving in fixed orbits with discrete energies and angular momenta that are whole number multiples of a fundamental constant.
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1) Rutherford performed an experiment where he bombarded a thin gold foil with alpha particles and observed that most passed through without deflection, some were deflected by small angles, and a few were deflected back.
2) This led Rutherford to propose an atomic model where the atom has a small, dense nucleus containing its mass and positive charge, surrounded by electrons in orbits.
3) This was a major departure from the previous "plum pudding" model where charge and mass were thought to be uniformly distributed. However, Rutherford's model failed to explain the stability of electron orbits.
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2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
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This presentation is presented by a physics Scholar Ayat Ullah
Department of Physics
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Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
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Thermionic emission occurs when thermal energy causes charge carriers like electrons or ions to flow from a heated surface. Thomas Edison discovered the Edison effect in 1880, where charge could flow in one direction from a heated filament to a cooler metal plate inside an incandescent light bulb. A cathode ray tube uses an electron gun to produce an electron beam that is accelerated and deflected to strike a fluorescent screen, displaying images. It finds uses in oscilloscopes, TVs, and computer monitors. Radioactivity involves the emission of alpha, beta, or gamma radiation from unstable atomic nuclei. While it has uses like power generation and medical imaging, radiation exposure can also cause cell damage and increase cancer risks.
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The document discusses the Bohr model of the hydrogen atom. It explains that the electron can only orbit the nucleus in fixed energy levels called orbits. The lowest energy level is the ground state, with higher levels being excited states. When an electron moves to a higher level, energy is absorbed, and when it moves to a lower level, a photon of energy is released. The wavelength and frequency of light are related to the energy of photons by Planck's constant and the speed of light. Quantum numbers describe the properties of atomic orbitals and electrons, including principal, orbital, and spin quantum numbers. Electron configurations show how electrons are arranged in orbitals according to Aufbau principle, Hund's rule, and Pauli exclusion
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The document is the notes from an atomic spectrum class that include the agenda, objectives, and content about atomic spectra. The key points are:
1. Atoms emit and absorb specific frequencies of light that make up their atomic spectrum, which acts as a fingerprint to identify elements.
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1) Effective nuclear charge (Zeff) is the nuclear charge actually experienced by an electron of an atom, which depends on the orbital and is less than the actual nuclear charge due to shielding by inner shell electrons.
2) Zeff is calculated using the formula Zeff = Z - σ, where Z is the actual nuclear charge and σ is the shielding constant which accounts for screening of the nuclear charge by inner electrons.
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The document discusses quantum theory and the atomic model. It introduces Nicholas Bohr's quantum model of the hydrogen atom, which explained why atomic emission spectra are discontinuous rather than continuous. Bohr's model proposed that electrons can only orbit the nucleus at certain distances, corresponding to discrete energy levels. Later models improved on this by describing the electron's probable location using 3D regions called atomic orbitals, within which the electron spends most of its time near the positively charged nucleus.
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The teacher will be preparing spectroscopes and gas tubes to revisit atomic structure with students. The document discusses how light and atomic structure are related, including that electrons move between discrete energy levels and absorb or emit photons of specific wavelengths when changing levels. Different elements have unique emission spectra due to variations in electron configuration.
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- Electronegativity, ionization energy, and electron affinity all generally increase from left to right across a period as the effective nuclear charge increases. Electronegativity also increases up a group as the distance from valence electrons to the nucleus decreases.
- Ionization energy increases from top to bottom within a group as it is easier to remove an electron from an atom with fewer energy levels. Electron affinity generally increases from left to right across a period and decreases
RUTHERFORD ATOM MODEL
Rutherford conducted an experiment where he fired alpha particles at a thin gold foil. Most alpha particles passed straight through the foil, but some were deflected at small angles and a few were deflected at large angles. This showed that the positive charge and mass of an atom must be concentrated in a small nucleus at the center, with electrons orbiting the outside. The Rutherford model concluded that (1) the positive charge of an atom is contained in a nucleus at its center, (2) there is mostly empty space between the nucleus and electrons, and (3) electrons revolve around the positively charged nucleus.
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(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
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𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
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Power point english
- 2. SNTC SREEKANDESWARAM POOCHACKAL B.Ed 2013-14 KERALA UNIVERSITY
- 3. SUBMITTED BY RAKHI BABU PHYSICAL SCIENCE REG.NO:13383017
- 4. SUBMITTED TO LINIMOL K S
- 5. POWERPOINT PRESENTATION ON gold foil experiment
- 7. PICTURE OF GOLD FOIL EXPERIMENT
- 8. The deviation of alpha rays through gold foil us experimentally proved by Rutherford. When the alpha rays collided very fastly on the gold foil, then he found a deviation in the path of some rays.
- 9. RUTHERFORD ARRIVES AT THESE CONCLUSIONS • Nucleus is the centre of an atom • Nucleus has a positive charge
- 10. Compared to the total volums of atom, the volume of nucleus is very small The whole mass of atom is concentrated its nucleus. The electrons are distributed around the nucleus.