STRUCTURE OF THE ATOM.pptx
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This document discusses the history and structure of the atom. It explains that ancient Greek philosophers first proposed that all matter is made of tiny indivisible particles called atoms. Over time, scientists discovered subatomic particles like electrons, protons, and neutrons that make up the nucleus of the atom. The document defines key terms like atomic number, mass number, isotopes, and provides examples of subatomic particles for some common elements.
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The document traces the history and development of atomic models from ancient Greek philosophers to modern quantum theory. It describes Democritus's early idea of indivisible atoms, followed by John Dalton formalizing the first atomic theory in the early 1800s. J.J. Thomson later discovered the electron and proposed that atoms are like "plum puddings" with positive matter and embedded electrons. Ernest Rutherford's gold foil experiment revealed that atoms have a small, dense positive nucleus, leading Niels Bohr to model electrons orbiting the nucleus in fixed shells. Modern quantum theory describes electrons as occupying probability clouds or orbitals around the nucleus.
Atoms
1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom has a small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in energy levels or an electron cloud. Atoms of the same element can have different numbers of neutrons, known as isotopes.
Chapter 3 - Atoms
1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom's small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in regions of probable location called electron clouds.
Atomic Theory Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental indivisible units of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing positive charge.
3. Later models like Bohr's incorporated the idea that electrons orbit the nucleus in fixed energy levels, accounting for the emission and absorption of photons.
A T O M I C T H E O R Y Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental building blocks of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing most of its mass.
3. Later discoveries found that the nucleus contains protons and neutrons, while electrons orbit the nucleus, leading to the modern understanding of atomic structure.
Ch 4 power point 08 09
This document provides a summary of chapter 4 on atomic structure:
1. It discusses early atomic theories from Democritus and Dalton, including Dalton's four postulates that atoms are indivisible, identical for a given element, combine in fixed ratios, and reactions involve rearrangement not destruction of atoms.
2. It describes the discovery of subatomic particles including electrons, protons, and neutrons. The nuclear model places the protons and neutrons in the nucleus with electrons orbiting.
3. Key terms are defined including atomic number, mass number, and isotopes. Isotopes are varieties of the same element that differ in neutron number.
102730464 the-atom
The document discusses the history of atomic theory from ancient Greek philosophers' ideas of "primal matter" to modern atomic structure. It describes early atomic models including Thomson's "plum pudding" model and Rutherford's gold foil experiment. Key developments included Dalton's atomic theory, the discovery of subatomic particles like the electron, proton, and neutron, and the modern nuclear model with electrons orbiting a small, dense, positively-charged nucleus.
giant presentation on model of an atom
it explains the model of an atom along with all necesary details
it contains all the theorems orbitals etc
complete giant slide file of and on atoms
Recommended
Mod+13,+History+Of+Atom+Part+A
The document traces the history and development of atomic models from ancient Greek philosophers to modern quantum theory. It describes Democritus's early idea of indivisible atoms, followed by John Dalton formalizing the first atomic theory in the early 1800s. J.J. Thomson later discovered the electron and proposed that atoms are like "plum puddings" with positive matter and embedded electrons. Ernest Rutherford's gold foil experiment revealed that atoms have a small, dense positive nucleus, leading Niels Bohr to model electrons orbiting the nucleus in fixed shells. Modern quantum theory describes electrons as occupying probability clouds or orbitals around the nucleus.
Atoms
1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom has a small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in energy levels or an electron cloud. Atoms of the same element can have different numbers of neutrons, known as isotopes.
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1. The document discusses the historical development of atomic theory from Democritus' idea of indivisible atoms to the modern atomic model.
2. Key contributors included Dalton who proposed atoms of different elements have different properties, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed the atom's small, dense nucleus.
3. The modern atomic model consists of a small, positively charged nucleus surrounded by electrons in regions of probable location called electron clouds.
Atomic Theory Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental indivisible units of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing positive charge.
3. Later models like Bohr's incorporated the idea that electrons orbit the nucleus in fixed energy levels, accounting for the emission and absorption of photons.
A T O M I C T H E O R Y Reg
1. Early atomic models proposed by philosophers like Democritus and Dalton proposed that atoms were the fundamental building blocks of matter.
2. Rutherford's gold foil experiment in the early 1900s showed that the atom has a small, dense nucleus at its center containing most of its mass.
3. Later discoveries found that the nucleus contains protons and neutrons, while electrons orbit the nucleus, leading to the modern understanding of atomic structure.
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This document provides a summary of chapter 4 on atomic structure:
1. It discusses early atomic theories from Democritus and Dalton, including Dalton's four postulates that atoms are indivisible, identical for a given element, combine in fixed ratios, and reactions involve rearrangement not destruction of atoms.
2. It describes the discovery of subatomic particles including electrons, protons, and neutrons. The nuclear model places the protons and neutrons in the nucleus with electrons orbiting.
3. Key terms are defined including atomic number, mass number, and isotopes. Isotopes are varieties of the same element that differ in neutron number.
102730464 the-atom
The document discusses the history of atomic theory from ancient Greek philosophers' ideas of "primal matter" to modern atomic structure. It describes early atomic models including Thomson's "plum pudding" model and Rutherford's gold foil experiment. Key developments included Dalton's atomic theory, the discovery of subatomic particles like the electron, proton, and neutron, and the modern nuclear model with electrons orbiting a small, dense, positively-charged nucleus.
giant presentation on model of an atom
it explains the model of an atom along with all necesary details
it contains all the theorems orbitals etc
complete giant slide file of and on atoms
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The document discusses the history and development of atomic theory from ancient Greek philosophers to modern scientists like Dalton, Thomson, Rutherford, and Bohr. It explains key concepts like atoms being the smallest particle of an element that retains its properties, atomic number representing the number of protons, isotopes being variants of the same element with different numbers of neutrons, and the discovery of subatomic particles like protons, neutrons, and electrons that make up the tiny nuclear structure of atoms.
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This document summarizes key concepts from Chapter 4 on atomic structure:
1) It describes early atomic theories from Democritus and Dalton, including defining atoms as indivisible particles and Dalton's atomic theory.
2) It outlines the discovery of subatomic particles like electrons, protons, and neutrons through experiments by Thomson, Rutherford, and Chadwick.
3) It explains how atoms are distinguished based on their number of protons (atomic number) and total nuclear particles (mass number), including definitions of isotopes.
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- Matter is composed of particles called atoms and molecules. Atoms are the smallest particles of elements, while molecules contain two or more bonded atoms.
- The kinetic theory of matter describes the states of matter based on particle motion. Solids have fixed shapes, liquids have mobile particles that follow container shapes, and gases have freely moving particles.
- The atomic structure has been discovered through the work of scientists like Dalton, Thomson, Rutherford, Bohr, and Chadwick. Modern atomic theory includes electrons orbiting a nucleus of protons and neutrons.
- Isotopes are atoms of the same element with different numbers of neutrons. Isotopes have identical chemical properties but different physical properties and masses
Chapter 2 form 4
- Matter is composed of particles called atoms and molecules. Atoms are the smallest particles that make up elements, and molecules are made of two or more bonded atoms.
- The structure of the atom has been discovered over time by scientists like Dalton, Thomson, Rutherford, Bohr, and Chadwick. We now know atoms have a tiny, dense nucleus containing protons and neutrons, surrounded by electrons.
- Isotopes are atoms of the same element with different numbers of neutrons. Some isotopes are unstable and radioactive, while others are stable. Radioactive isotopes have important applications in medicine, agriculture, and industry.
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The document discusses the history and development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes John Dalton's atomic theory from the late 1700s that all matter is made of tiny indivisible particles called atoms. It then discusses J.J. Thomson's 1897 discovery of the electron using cathode ray tubes and Ernest Rutherford's experiments in the early 1900s that revealed the atom's small, dense nucleus. The modern atomic model views atoms as mostly empty space with a tiny nucleus at the center containing protons and neutrons, surrounded by electrons.
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The document discusses the structure of atoms. It defines an atom as the smallest particle of an element that retains its identity in chemical reactions. It describes how atoms are composed of subatomic particles including protons, neutrons, and electrons. It discusses how the number of protons determines the element, the number of electrons usually equals the number of protons, and the mass number is the total of protons and neutrons. Isotopes are defined as atoms of the same element with different numbers of neutrons. The document also discusses electron shells and valence electrons.
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atomic models
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The document traces the development of atomic models from ancient Greek philosophers to modern quantum mechanics. It discusses early concepts of atoms proposed by Democritus and Aristotle. John Dalton later proposed atoms as basic indivisible units that combine in fixed ratios. J.J. Thomson's experiments led to the "plum pudding" model of atoms with a positive nucleus and negative electrons. Rutherford's gold foil experiment showed the nucleus is dense and positively charged at the center. Niels Bohr incorporated orbits and quantized energy levels. Later discoveries of the neutron, electron probability clouds, and electron configurations further refined atomic structure models.
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The document summarizes key ideas from a chemistry chapter on the structure of the atom. It discusses how ancient Greek philosophers like Democritus and Aristotle attempted to explain matter. John Dalton later revived the idea of atoms in the early 1800s based on his scientific experiments. The document also outlines the discovery of subatomic particles like protons, neutrons, and electrons, and how this led to models of the structure of the atom. It describes how atoms can be unstable and undergo radioactive decay by emitting radiation like alpha, beta, or gamma particles.
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The document discusses the history and development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes John Dalton's atomic theory from the late 1700s that all matter is made of tiny indivisible particles called atoms. It then discusses J.J. Thomson's 1897 discovery of the electron using cathode ray tubes and Ernest Rutherford's experiments in the early 1900s that revealed the atom's small, dense nucleus. The modern atomic model views atoms as mostly empty space with a tiny nucleus at the center containing protons and neutrons, surrounded by electrons.
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This document summarizes key concepts from Chapter 4 on atomic structure:
1) It describes early atomic theories from Democritus and Dalton, including Dalton's postulates that atoms are indivisible and atoms of different elements have different properties.
2) Modern research has shown atoms are composed of subatomic particles like electrons, protons, and neutrons. Experiments by Thomson, Millikan, Rutherford and others led to discoveries about these particles and the nuclear model of the atom.
3) Isotopes are atoms of the same element that differ in number of neutrons. Atomic mass is an average that takes isotopic abundance into account. The periodic table organizes elements based on repeating atomic properties.
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The document outlines key concepts in atomic structure including Democritus and Dalton's early atomic theories, the discovery of subatomic particles like electrons, protons, and neutrons, and how Rutherford's gold foil experiment led to the development of the nuclear model of the atom with a small, dense nucleus surrounded by electrons. It also discusses how atoms of the same element can differ in the number of neutrons to form isotopes, and how atomic number and mass are used to identify and characterize different atoms and isotopes.
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1. John Dalton developed the first modern atomic theory in the early 1800s based on experiments showing atoms combine and separate in whole number ratios during chemical reactions.
2. Atoms are made up of a tiny, positively charged nucleus surrounded by electrons. The nucleus contains protons and neutrons.
3. Unstable atoms emit radiation like alpha, beta, or gamma particles to become stable. This process is called radioactive decay.
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The document discusses the structure of atoms. It defines an atom as the smallest particle of an element that retains its identity in chemical reactions. It describes how atoms are composed of subatomic particles including protons, neutrons, and electrons. It discusses how the number of protons determines the element, the number of electrons usually equals the number of protons, and the mass number is the total of protons and neutrons. Isotopes are defined as atoms of the same element with different numbers of neutrons. The document also discusses electron shells and valence electrons.
3.2 structure of atoms
- Thompson discovered electrons using cathode ray tubes. Rutherford discovered the nucleus and that it is positively charged through gold foil experiments.
- Chadwick discovered neutrons by observing particles in a beam that were not deflected by a magnetic field.
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit the nucleus. The number of protons defines the element.
atomic models
- Maharishi Kanad proposed that matter is made of tiny indivisible particles called "paramanu" and "anu", which may be composed of even smaller particles. (Sentence 1)
- Atoms are the smallest units of matter that take part in chemical reactions and combine in small whole numbers to form molecules. Atoms themselves are made up of electrons, protons, and neutrons. (Sentence 2)
- J.J. Thomson's "plum pudding" model depicted the atom as a positively charged sphere with electrons embedded in it, while Rutherford's gold foil experiment showed that the mass and positive charge of an atom are concentrated in a tiny nucleus at the center. (Sentence 3
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The document traces the development of atomic models from ancient Greek philosophers to modern quantum mechanics. It discusses early concepts of atoms proposed by Democritus and Aristotle. John Dalton later proposed atoms as basic indivisible units that combine in fixed ratios. J.J. Thomson's experiments led to the "plum pudding" model of atoms with a positive nucleus and negative electrons. Rutherford's gold foil experiment showed the nucleus is dense and positively charged at the center. Niels Bohr incorporated orbits and quantized energy levels. Later discoveries of the neutron, electron probability clouds, and electron configurations further refined atomic structure models.
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The document summarizes key ideas from a chemistry chapter on the structure of the atom. It discusses how ancient Greek philosophers like Democritus and Aristotle attempted to explain matter. John Dalton later revived the idea of atoms in the early 1800s based on his scientific experiments. The document also outlines the discovery of subatomic particles like protons, neutrons, and electrons, and how this led to models of the structure of the atom. It describes how atoms can be unstable and undergo radioactive decay by emitting radiation like alpha, beta, or gamma particles.
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- 1. STRUCTURE OF THE ATOM
- 2. Thales of Miletus - discovered that a piece of amber, after rubbing it with fur, attracts bits of hair and feathers and other light objects. He suggested that this mysterious force came from the amber. Thales, however, did not connect this force with any atomic particle. Democritus – (460 – 370 B.C.) a Greek philosopher proposed that all matter is composed of tiny indivisible particles. - He called this particles atomos, which meant indivisible or indestructible. History of the Atom
- 3. Plato (427 – 347 B.C.) and Aristotle (384 – 322 B.C.) - They were of the opinion that all materials could be broken down into smaller parts and smaller parts without end. Atomism – was the notion that all matter was composed of very tiny, individual, finite, and indivisible particles. John Dalton (1766 – 1844) – an English schoolmaster concluded that the properties of matter could be explained in terms of atoms.
- 4. Matter consists of tiny particles called atoms. Atoms are indestructible. In chemical reactions, the atoms rearrange but no new atoms are created and atoms themselves do not break apart. The atoms of one particular element are all identical in mass and other properties. The atoms of different elements differ in mass and other properties. When atoms of different elements combine into a compound, the constituent atoms are always present in the same fixed numerical ratio. DALTON’S ATOMIC THEORY
- 5. MODELS OF THE ATOM
- 6. 1. Electrons – negatively charged particles Discovered by Sir joseph John Thomson 2. Protons – positively charged particles Discovered by Eugen Goldstein 3. Neutrons – neutral charged Discovered by James Chadwick SUBATOMIC PARTICLES
- 7. Nucleus – central part of the atom - It is where the neutrons and protons are found - Discovered by Ernest Rutherford
- 8. A Summary of the Subatomic Particles of an Atom Mass Number – the whole number which is closest to the atomic mass Mass number = number of protons + number of neutrons Atomic number (Z) = no of proton = no. of electron Name Symbol Electrical Charge Mass (amu) Mass (g) Electron e- -1 0.000549 9.1093 x 10-28 Proton p+ +1 1.00728 or 1 1.673 x 10-24 Neutron no 0 1.00867 or 1 1.675 x 10-24
- 9. Eelement Atomic number No. of Protons No. of Electrons No. of neutrons Atomic Mass (amu) Mass number Carbon 6 6 6 6 12.011 12 Sodium 11 11 11 12 22.991 23 Sulfur 16 16 16 16 32.06 32 Calcium 20 20 40.08 Silver 47 107.88 108 Gold 118 197.00 197 Lead 82 125 207.21 Subatomic Particles of Some Elements
- 10. Isotopes – are atoms of the same element having the same atomic number but different atomic masses Protium Deuterium Tritium Isotopes can be classified as natural (found in nature) or man made (artificial or synthetic) Isotopes can be classified as stable or unstable