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The document summarizes the development of atomic theory from Dalton's billiard ball model to the modern quantum mechanical model. John Dalton proposed the first atomic theory in 1808, modeling atoms as solid spheres. J.J. Thomson's plum pudding model viewed atoms as positive spheres with electrons spread throughout. Ernest Rutherford's gold foil experiment in 1911 revealed the atom's small, dense nucleus. Niels Bohr incorporated orbits for electrons around the nucleus. The modern atomic model describes electrons as existing in probabilistic electron clouds rather than definite orbits.
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The document discusses the structure of atoms. It describes how early scientists like Dalton, Thomson, Rutherford, and Bohr contributed to developing models of the atom through experiments. Thomson's "plum pudding" model depicted electrons distributed uniformly in a positively charged sphere, but it could not explain atomic stability. Rutherford's gold foil experiment showed that the positive charge and mass of atoms are concentrated in a tiny nucleus, leading to his nuclear model. Bohr's model incorporated discrete electron orbits to explain atomic stability. The document also discusses subatomic particles like protons, neutrons, isotopes, isobars, and how electrons are arranged in shells according to their quantum numbers.
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Atoms are composed of electrons, protons, and neutrons. Electrons orbit around a small, dense nucleus composed of protons and neutrons. Over time, scientists have developed models of the atom based on new discoveries. Democritus first proposed atoms could not be further divided in 450 BC. In the 19th and 20th centuries, physicists discovered subatomic particles within atoms like electrons, proving atoms could still be divided. Now atoms are understood to have a nucleus surrounded by electron clouds.
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The atomic nucleus is at the center of atoms and is composed of protons and neutrons. It was discovered in 1911 by Ernest Rutherford based on experiments showing that atoms have small, dense, positively charged nuclei. The nucleus contains nearly all of an atom's mass. Protons and neutrons are bound together in the nucleus by the strong nuclear force. Nuclear chemistry deals with the composition, properties, and reactions of atomic nuclei. Key discoveries included the neutron by Chadwick in 1932 and the development of nuclear models showing electrons orbiting the positively charged nucleus.
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Structure Of The Atom.pdf notes important
The document provides information on the structure of atoms, including key experiments and models that helped reveal the internal structure of atoms. It discusses J.J. Thomson's cathode ray experiment that discovered electrons, Rutherford's alpha particle scattering experiment that showed atoms have a small, dense nucleus, and Bohr's model of electron orbits around the nucleus. It also covers topics like isotopes, mass number, atomic number, electron configuration, and valency.
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The document discusses the structure of atoms. It describes how early scientists like Dalton, Thomson, Rutherford, and Bohr contributed to developing models of the atom through experiments. Thomson's "plum pudding" model depicted electrons distributed uniformly in a positively charged sphere, but it could not explain atomic stability. Rutherford's gold foil experiment showed that the positive charge and mass of atoms are concentrated in a tiny nucleus, leading to his nuclear model. Bohr's model incorporated discrete electron orbits to explain atomic stability. The document also discusses subatomic particles like protons, neutrons, isotopes, isobars, and how electrons are arranged in shells according to their quantum numbers.
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Atoms are composed of electrons, protons, and neutrons. Electrons orbit around a small, dense nucleus composed of protons and neutrons. Over time, scientists have developed models of the atom based on new discoveries. Democritus first proposed atoms could not be further divided in 450 BC. In the 19th and 20th centuries, physicists discovered subatomic particles within atoms like electrons, proving atoms could still be divided. Now atoms are understood to have a nucleus surrounded by electron clouds.
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Rutherford conducted a gold foil experiment where he bombarded a thin gold foil with alpha particles. He discovered that some alpha particles bounced back, indicating there was a small, dense nucleus at the center of the atom. This led Rutherford to propose an atomic model where a small, positively charged nucleus is surrounded by electrons. Later, Bohr added to this model by suggesting electrons can only orbit the nucleus in certain fixed energy levels. The Rutherford-Bohr model helped explain the stability of atoms and how electrons can move between energy levels by absorbing or emitting photons.
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electronic properties of atoms 1.pptx
- 1. DEVELOPMENT OF THE ATOMIC THEORY WSU CHY15M0 - electronic properties of an atom
- 2. PURPOSE OF ATOMIC MODELS The models of the atom do not provide a complete understanding of the atom. The models help us to make useful predictions about how matter will behave. WSU CHY15M0 - electronic properties of an atom
- 3. Dalton Thomson Rutherford Bohr Schrodinger WSU CHY15M0 - electronic properties of an atom
- 4. JOHN DALTON (1766-1844), ❑Proposed the first atomic theory in 1808. WSU CHY15M0 - electronic properties of an atom
- 5. JOHN DALTON (1766-1844), ❑The atom is a solid sphere – billiard ball model. ⮚All matter consists of tiny particles called atoms, which cannot be broken up. ⮚All the atoms of a particular element are the same. Atoms of different elements are different. WSU CHY15M0 - electronic properties of an atom
- 6. JOHN DALTON (1766-1844), ❑The atom is a solid sphere – billiard ball model. ⮚When atoms combine, they form compounds. ⮚Atoms cannot be created or destroyed in a chemical reaction WSU CHY15M0 - electronic properties of an atom
- 7. Thomson WSU CHY15M0 - electronic properties of an atom
- 8. Thomson WSU CHY15M0 - electronic properties of an atom
- 9. JOSEPH J THOMSON ❑JJ Thomson discovered electrons in 1897. ❑The atom is a positive sphere where the electrons were randomly spread out inside the atom. ❑This model was known as the “plum- pudding” model. WSU CHY15M0 - electronic properties of an atom
- 10. Rutherford WSU CHY15M0 - electronic properties of an atom
- 11. Ruther- ford WSU CHY15M0 - electronic properties of an atom
- 12. ERNEST RUTHERFORD ❖In 1911 Ernest Rutherford used the discovery of an alpha particle to do further experiments on the atom. ❖The alpha(α) particle has the same mass as a helium atom but as a positive charge. ❖Rutherford directed a beam of alpha particles at a thin gold foil so that he could explore the inside of the atom. ❖The alpha particle scattering experiment. WSU CHY15M0 - electronic properties of an atom
- 13. ERNEST RUTHERFORD p38 ❖Almost all the mass of the atom is found in a very small positively charged nucleus in the centre of the atom. He later found the positive charge comes from protons. ❖The space around the nucleus is empty for the negatively charged electrons to be found there. ❖Rutherford’s nuclear atomic model. ❖One drawback: Opposite charges must attract each other and electrons should lose energy and spiral inward. WSU CHY15M0 - electronic properties of an atom
- 14. Bohr WSU CHY15M0 - electronic properties of an atom
- 15. NIELS BOHR ❖Electrons move in orbits(or energy levels) around the nucleus. ❖Electrons with the same energy move around in the same orbit. ❖Electrons in orbits that are further away from the nucleus have a higher energy than the orbits closer to the nucleus. WSU CHY15M0 - electronic properties of an atom
- 16. MODERN ATOMIC MODEL ❖The quantum mechanical model or electron cloud model ❖An atom consists of a nucleus and electrons spinning around the nucleus. ❖The electrons move in a cloud around the nucleus. ❖We cannot tell exactly where the electrons are at any given time. ❖We do know that electrons exist more frequently in certain regions around the nucleus than others. WSU CHY15M0 - electronic properties of an atom
- 17. MODERN ATOMIC MODEL p39 WSU CHY15M0 - electronic properties of an atom
- 18. WSU CHY15M0 - electronic properties of an atom