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The document discusses the atomic structure and models proposed by scientists over time. It explains that the atom consists of a nucleus and electrons. Rutherford proposed that the nucleus is at the center of the atom and contains protons and neutrons, while electrons orbit the nucleus. Bohr's atomic model built on Planck's quantum theory by postulating that electrons orbit in fixed energy levels and can only absorb or emit photons of energy equal to the difference between orbit levels. The model helped explain atomic stability and emission spectra but had limitations for multi-electron atoms.
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4. Nuclear physics including structure of the nucleus, radioactive decay, nuclear stability, fission and fusion processes, and applications of nuclear technology.
Electrons in atoms
The document discusses the historical development of atomic models from Dalton to Bohr and beyond. It introduces John Dalton's early model of atoms as indivisible particles with no internal structure in 1863. Later models incorporated the discoveries of the electron by J.J. Thomson in 1897 and the nuclear structure of atoms by Ernest Rutherford in 1911. Niels Bohr's 1913 model proposed that electrons orbit the nucleus in fixed, quantized energy levels. This laid the foundations for understanding atomic emission spectra and the quantum mechanical model that later replaced Bohr's model.
BE UNIT-1 basic electronics unit one.pptx
1. The document discusses the atomic structure of matter, which is made up of protons, electrons, and neutrons. Atoms contain protons and neutrons in their nucleus, surrounded by electrons.
2. Atoms of different elements have different atomic structures because they contain different numbers of protons and electrons. Neutral atoms have equal numbers of protons and electrons, but atoms can gain or lose electrons to become ions.
3. The document then discusses subatomic particles like protons, neutrons, and electrons in more detail, including their relative masses and charges. It also discusses isotopes and how they have the same number of protons but different numbers of neutrons.
Atoms Class 12 NCERT chapter 12
Ernest Rutherford's alpha ray scattering experiment led him to propose the nuclear model of the atom. The key findings were:
1) Most alpha particles passed through the thin gold foil with little deflection, but a small percentage were deflected by large angles, including backwards.
2) This could only be explained if the positive charge of the atom was concentrated into a very small, dense nucleus.
3) Rutherford concluded atoms have a small, dense nucleus containing its positive charge and mass, with electrons orbiting the nucleus.
This nuclear model replaced the plum pudding model, but had its own limitations that were later addressed by Niels Bohr's model of electron orbits and quantization
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This document discusses Rutherford's atomic model and Bohr's model of the atom. It provides details of Rutherford's alpha particle scattering experiment which showed that atoms have a small, dense nucleus. This led Rutherford to propose a planetary model of the atom with electrons orbiting the nucleus. The document then discusses limitations of Rutherford's model and how Bohr proposed quantized electron orbits to explain atomic stability. It provides Bohr's key postulates and formulas for the hydrogen atom spectrum and energy levels.
Class 11 . ATOMIC STRUCTURE.pptx
1. The document discusses the historical development of atomic structure theories from Dalton's atomic theory to Bohr's atomic model.
2. Dalton's atomic theory proposed that all matter is composed of indivisible atoms that combine in fixed ratios, but it did not account for subatomic particles.
3. Rutherford's gold foil experiment led to the discovery of the nucleus and nuclear model of the atom, with electrons in orbits around the nucleus, though this model could not explain the stability of atoms.
Quantum theory and the atom
This document provides an overview of Bohr's model of the atom and the development of the quantum mechanical model. It discusses key aspects of Bohr's model including discrete energy levels and allowed electron orbits. It then describes limitations of Bohr's model and the proposal of the quantum mechanical model treating electrons as waves. The quantum mechanical model uses wave functions and orbitals to describe electron location probabilities rather than defined orbits. It introduces the concepts of principal and subenergy levels characterized by quantum numbers that specify allowed electron configurations.
7.1
This document discusses atomic, nuclear and particle physics concepts including:
1. Discrete energy levels in atoms lead to line spectra fingerprints of elements. Electrons can only have certain quantized energy levels and jump between them, emitting photons of specific wavelengths.
2. The Bohr model of the atom helped explain line spectra by proposing electrons orbit nuclei in fixed, quantized energy levels. Electron transitions between levels emit or absorb photons of specific energies.
3. Atoms are composed of a nucleus containing protons and neutrons. Isotopes are atoms of the same element with different numbers of neutrons. Evidence for neutrons comes from isotopes having the same number of protons but different masses.
4. Radio
Structure of atom
This document discusses the structure of the atom. It begins by describing Bohr's model of the atom and its limitations. It then introduces shells and subshells, as well as quantum numbers and the shapes of atomic orbitals. Rules for filling electrons into orbitals, such as the Aufbau principle and Pauli exclusion principle, are also covered. The document discusses atomic spectra, photoelectric effect, and the dual wave-particle nature of light and matter. It provides an overview of concepts like de Broglie wavelength, Heisenberg uncertainty principle, and atomic electron configuration.
Chem chapt 5
The document discusses electrons in atoms and their arrangement. It begins by explaining the wave-particle duality of light and electrons. It then discusses the historical atomic models of Rutherford, Bohr, and the quantum mechanical model. The quantum mechanical model treats electrons as waves and describes their location in terms of probability distributions within orbitals. The document concludes by explaining the rules that determine electron configuration, including the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Atomic structure.pdf
Atomic structure is composed of protons, neutrons, and electrons. Rutherford's gold foil experiment showed that atoms are mostly empty space with a small, dense nucleus at the center containing protons and neutrons. Electrons orbit the nucleus in specific energy levels. The Bohr model explained electrons in hydrogen having discrete energy levels. Atoms bond via ionic bonds between metals and nonmetals by transferring electrons, covalent bonds between nonmetals by sharing electrons, and metallic bonds between metals by delocalized electrons.
Characterizing the Electrons
The presentation can be a remedial lesson on the topic "electronic structure of matter" grade 9, science second quarter
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Test
- 5. QUANTUM THEORY OF RADIATION In 1901 Max Plank proposed Quantum theory of Radiation from hot (black) body studies. A hot body radiates (emits) energy not in continuous waves but in small units of waves. When atoms or molecules absorb or emit radiant energy in quanta (a small packet of energy) or photons.