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This document outlines Dalton's atomic theory from the early 19th century. It states that Dalton was the first to propose atomic theory in 1803. The theory included seven main postulates: 1) Elements are made of atoms, 2) Atoms are indivisible, 3) Atoms can neither be created nor destroyed, 4) Atoms of the same element are alike, 5) Atoms of different elements differ, 6) Atoms cannot be converted between elements, 7) Atoms combine in simple ratios. The document then asks three questions about Dalton's atomic theory and atoms.
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Dalton's Atomic Theory
John Dalton developed atomic theory in the early 1800s based on careful chemical measurements. The main postulates of Dalton's atomic theory were that matter is composed of very tiny indivisible particles called atoms, atoms of a given element are identical in mass and properties, and atoms of different elements have different properties and combine in small whole number ratios. While some aspects have been updated, Dalton's atomic theory of atoms as the basic building blocks of matter remains valid in modern chemistry.
Dalton Atomic Theory
John Dalton developed atomic theory in 1808, proposing six main postulates: 1) Matter is made of extremely small indivisible particles called atoms, 2) Atoms of a given element are identical in mass and properties, 3) Atoms of different elements differ in mass and properties, 4) Atoms combine in simple whole number ratios to form chemical compounds, 5) In compounds the relative number and type of atoms is fixed, and 6) Atoms cannot be created, destroyed, or divided in chemical reactions. Dalton's theory did not account for isotopes or allotropes which have atoms of varying masses or properties within an element.
Ananya shukla
John Dalton proposed the Dalton's Atomic Theory in 1808, which stated that matter is made of indivisible particles called atoms. The theory postulated that atoms of the same element have identical properties, while atoms of different elements have different properties and combine in fixed ratios to form compounds. The theory was limited in that it was later discovered atoms can be subdivided and isotopes exist with differing masses but the same element. It also failed to explain allotropes and complex organic compounds. While some aspects remain valid, Dalton's Atomic Theory formed the basis for modern atomic structure models.
Atomic structure in detailed
This document summarizes the history of atomic structure and the discovery of subatomic particles. It discusses:
1) Early ideas about atoms from Maharshi Kanada and Democritus.
2) John Dalton's atomic theory from 1808 that atoms are indivisible and combine to form molecules.
3) Discovery of the electron from cathode ray experiments by Crookes and Thomson, showing electrons are negatively charged and part of atoms.
4) Realization that atoms must also contain positively charged particles, leading to the discovery of the proton by Goldstein and verification by Thomson.
2 contribution of john dalton martin
John Dalton's atomic theory proposed that all matter is composed of extremely small indivisible particles called atoms. He hypothesized that atoms of the same element are identical, while atoms of different elements differ in their properties. Dalton also suggested that atoms combine in fixed ratios to form compounds. His atomic theory provided an explanation for laws such as the law of conservation of mass and the law of definite proportions. Dalton's experiments helped establish the idea that atoms are the basic building blocks of all matter.
Akash patel
John Dalton was an English chemist and physicist best known for his pioneering work in developing atomic theory. In 1808, Dalton presented his atomic theory, which proposed that (1) matter is made up of extremely small indivisible particles called atoms, (2) atoms of a given element are identical in mass and properties, and (3) atoms of different elements can combine to form compounds with fixed ratios of the constituent atoms. Dalton's atomic theory provided an explanation for laws of conservation of mass and definite proportions in chemical reactions.
Chapter 4 Pp
Defining the atom,structure of the atom, rutherfords gold foil experiment, distinguishing among atoms, mass number, atomic number, isotopes
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.
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Dalton's Atomic Theory
John Dalton developed atomic theory in the early 1800s based on careful chemical measurements. The main postulates of Dalton's atomic theory were that matter is composed of very tiny indivisible particles called atoms, atoms of a given element are identical in mass and properties, and atoms of different elements have different properties and combine in small whole number ratios. While some aspects have been updated, Dalton's atomic theory of atoms as the basic building blocks of matter remains valid in modern chemistry.
Dalton Atomic Theory
John Dalton developed atomic theory in 1808, proposing six main postulates: 1) Matter is made of extremely small indivisible particles called atoms, 2) Atoms of a given element are identical in mass and properties, 3) Atoms of different elements differ in mass and properties, 4) Atoms combine in simple whole number ratios to form chemical compounds, 5) In compounds the relative number and type of atoms is fixed, and 6) Atoms cannot be created, destroyed, or divided in chemical reactions. Dalton's theory did not account for isotopes or allotropes which have atoms of varying masses or properties within an element.
Ananya shukla
John Dalton proposed the Dalton's Atomic Theory in 1808, which stated that matter is made of indivisible particles called atoms. The theory postulated that atoms of the same element have identical properties, while atoms of different elements have different properties and combine in fixed ratios to form compounds. The theory was limited in that it was later discovered atoms can be subdivided and isotopes exist with differing masses but the same element. It also failed to explain allotropes and complex organic compounds. While some aspects remain valid, Dalton's Atomic Theory formed the basis for modern atomic structure models.
Atomic structure in detailed
This document summarizes the history of atomic structure and the discovery of subatomic particles. It discusses:
1) Early ideas about atoms from Maharshi Kanada and Democritus.
2) John Dalton's atomic theory from 1808 that atoms are indivisible and combine to form molecules.
3) Discovery of the electron from cathode ray experiments by Crookes and Thomson, showing electrons are negatively charged and part of atoms.
4) Realization that atoms must also contain positively charged particles, leading to the discovery of the proton by Goldstein and verification by Thomson.
2 contribution of john dalton martin
John Dalton's atomic theory proposed that all matter is composed of extremely small indivisible particles called atoms. He hypothesized that atoms of the same element are identical, while atoms of different elements differ in their properties. Dalton also suggested that atoms combine in fixed ratios to form compounds. His atomic theory provided an explanation for laws such as the law of conservation of mass and the law of definite proportions. Dalton's experiments helped establish the idea that atoms are the basic building blocks of all matter.
Akash patel
John Dalton was an English chemist and physicist best known for his pioneering work in developing atomic theory. In 1808, Dalton presented his atomic theory, which proposed that (1) matter is made up of extremely small indivisible particles called atoms, (2) atoms of a given element are identical in mass and properties, and (3) atoms of different elements can combine to form compounds with fixed ratios of the constituent atoms. Dalton's atomic theory provided an explanation for laws of conservation of mass and definite proportions in chemical reactions.
Chapter 4 Pp
Defining the atom,structure of the atom, rutherfords gold foil experiment, distinguishing among atoms, mass number, atomic number, isotopes
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.
Anurag Dhiwar
---Topic Dalton atomic Theory---
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Lesson-2.1-Daltons-Atomic-Theory-revised (1).ppt
This picture illustrates the Law of Definite Proportions. The law states that a given compound always contains the same elements in a fixed ratio by mass. Here, both samples of sulfur dioxide contain oxygen and sulfur in a 50:50 ratio by mass, regardless of whether it was manufactured in a lab or mined from the ground.
Lesson3_Theory of Atomic Structure Models.pptx
Greek philosophers first proposed the idea of atoms as the fundamental indivisible units that make up all matter. Democritus named these fundamental units "atoms", from the Greek word meaning "indivisible". He concluded through observation and questioning that matter cannot be divided infinitely into smaller pieces, but rather is made of discrete atoms. John Dalton further developed atomic theory in the early 19th century. He proposed that all matter is composed of tiny indivisible particles called atoms, that atoms of a given element are identical, and that atoms combine in whole number ratios to form compounds through chemical reactions.
Science Performance Task
John Dalton formulated his atomic theory in the early 1800s based on careful chemical measurements and observations. His theory proposed that (1) all matter is composed of tiny indivisible atoms, (2) atoms of the same element are identical in mass, (3) atoms of different elements have different masses, and (4) atoms combine in simple whole number ratios. Dalton's atomic theory provided the foundation for modern chemistry and physics by establishing that elements combine at the atomic level. While Dalton's model has been refined over time, it represented a revolutionary shift in understanding the basic nature of matter.
Supriya Kaushik
John Dalton presented his atomic theory in 1808 to explain the properties of matter. Dalton's atomic theory states that all matter is made up of very tiny indivisible particles called atoms. Atoms are identical in mass and chemical properties for a given element but differ between elements. Atoms combine in whole number ratios to form compounds, with the relative numbers and kinds of atoms remaining constant for a given compound. Dalton's atomic theory became a foundation of modern chemistry.
Hrishabh
John Dalton was born in England and began his career as a teacher at age 12, later becoming a school principal. In 1793, he began teaching mathematics, physics, and chemistry, focusing his research on the study of matter. Dalton presented his Atomic Theory in 1808, which established that all matter is made of tiny indivisible particles called atoms that combine in whole number ratios to form compounds. The theory marked a turning point in understanding the composition of matter.
HISTORY OF ATOMIC THEORY
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
Atomicnotes 7 And 8
The document discusses atomic structure and the periodic table. It explains that atoms are the basic unit of matter and are made up of protons, neutrons, and electrons. The number of protons determines the element. The periodic table organizes the elements and provides information about atomic structure like atomic number and mass. It also describes the historical models of the atom including those proposed by Dalton, Thomson, Rutherford, and Bohr.
Daltons atomic theory
Dalton's atomic theory proposed that:
1) Matter is made of extremely small indivisible particles called atoms.
2) Atoms of a given element are identical in size, mass and properties.
3) Atoms of different elements vary in size, mass and properties.
The theory had limitations such as not explaining Gay-Lussac's law of combining volumes or the nature of atomic bonding.
Modern atomic theory has updated that:
1) Atoms can be subdivided into smaller particles like electrons and protons.
2) Atoms are destructible through nuclear processes converting mass to energy.
3) Atoms of a given element can differ in mass and properties as
science.pptx
This presentation provides information about atoms and molecules. It defines an atom as the smallest particle of an element that cannot be created or destroyed in a chemical reaction. Atoms combine to form molecules, which are groups of two or more atoms held together by attractive forces. The document then discusses the symbols used to represent different elements, laws of chemical combination including conservation of mass and constant proportions, Dalton's atomic theory, and provides some biographical information about John Dalton.
John dalton[1]
John Dalton was an English chemist who developed modern atomic theory in the early 1800s. He proposed that all matter is made of extremely small indivisible particles called atoms, which are identical for a given element but differ between elements. Atoms of different elements combine in simple whole number ratios to form compounds, and chemical reactions involve atoms combining, separating, or rearranging. Dalton's atomic theory laid the foundation for understanding the composition and behavior of matter at the atomic scale.
Chapter 3.1 : The Atom: The Building Blocks of Matter
John Dalton developed the first atomic theory in 1808 based on experimental evidence from the laws of mass conservation, definite proportions, and multiple proportions. His theory proposed that all matter is composed of extremely small indivisible particles called atoms, atoms of a given element are identical, and atoms of different elements combine in simple whole number ratios to form compounds. Modern atomic theory has since modified Dalton's theory by showing atoms are divisible and some elements exist as different atomic masses.
Chemistry Class 11 sbcc part IV
John Dalton developed the first modern atomic theory in the early 1800s. He proposed that each chemical element is composed of unique atoms that cannot be created or destroyed through chemical reactions, but can combine to form compounds. Dalton hypothesized that differences in the masses of gas particles explained why water absorbed gases like carbon dioxide and nitrogen to different extents. His atomic theory marked the first truly scientific explanation of atoms. Dalton's concepts of atoms and molecules helped establish chemistry as a rigorous science.
History of atoms
Greek philosopher Democritus first proposed the idea of atoms in 460 BC, reasoning that matter must be divisible into indivisible particles. However, his idea was largely ignored. In the early 1800s, John Dalton performed experiments and developed an atomic theory, stating that elements are made of identical atoms that combine to form compounds. In 1897, Joseph John Thomson discovered the electron and proposed a early atomic model where electrons were embedded in a uniform sphere of positive charge, like raisins in pudding, known as the plum pudding model.
Science-8-week-5.pptx
1. The document discusses the early theories of the structure of atoms from ancient Greek philosophers to the modern atomic model.
2. It describes the discoveries of subatomic particles like the electron by J.J. Thomson and the nucleus by Ernest Rutherford through experiments.
3. Later scientists like Niels Bohr, James Chadwick, and Erwin Schrodinger further refined the model, with Bohr proposing electron shells and orbits, Chadwick discovering the neutron, and Schrodinger explaining electron probability clouds.
Chapter 4
This document discusses the structure of atoms. It begins by defining an atom and outlining Dalton's atomic theory. It then explains that atoms are composed of subatomic particles like electrons, protons, and neutrons. The nucleus contains protons and neutrons, while electrons orbit around the nucleus. Different elements are distinguished by their atomic number, which is the number of protons. Isotopes are atoms that have the same number of protons but different numbers of neutrons. The average atomic mass takes into account the relative abundances of isotopes in a naturally occurring sample of an element.
Physical science: Models of Atom
This document discusses the historical development of atomic models from Dalton to Bohr. It begins by explaining John Dalton's original model of atoms as indivisible, spherical particles. It then describes J.J. Thomson's "plum pudding" model which introduced electrons and viewed atoms as a soup of positive charge with electrons floating within. Rutherford's experiments led to his model of atoms with a small, dense nucleus surrounded by orbiting electrons. Bohr further refined this by proposing that electrons can only orbit in certain fixed energy levels. The document also notes Rutherford's prediction of a neutral particle in the nucleus, which was discovered by James Chadwick and named the neutron.
Lesson 3: Concepts About Chemical Elements
John Dalton's atomic theory proposed that all matter is composed of extremely small indivisible particles called atoms. Dalton theorized that elements are composed of atoms that are identical in mass and properties, and that compounds form when elements combine in whole number ratios. This led to laws like the law of definite proportions and law of multiple proportions. Later, Dmitri Mendeleev organized the known elements into the periodic table based on their atomic masses, and Henry Moseley rearranged the table based on atomic number, establishing it as a fundamental property of elements.
Minooka - Elements Part 2
Atoms are the smallest particles of elements that retain their chemical properties. Atoms consist of protons, neutrons, and electrons. John Dalton proposed his atomic theory in 1808, stating that all matter is made of indivisible atoms, atoms of the same element are identical, and atoms combine in simple whole number ratios. In the early 1900s, experiments showed that atoms have a small, dense nucleus surrounded by electrons, and electrons can exist in certain energy levels or orbits around the nucleus.
Chapter 4 pp (1)
This document summarizes key concepts about atomic structure:
1) It describes early atomic models including Democritus' idea of indivisible atoms and Dalton's atomic theory.
2) It explains the discovery of subatomic particles (electrons, protons, neutrons) and the nuclear model of the atom with electrons orbiting a nucleus.
3) It defines important atomic properties including atomic number, mass number, isotopes, and how to calculate atomic mass.
4) It provides an overview of how the periodic table organizes elements based on these atomic properties.
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Anurag Dhiwar
---Topic Dalton atomic Theory---
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This picture illustrates the Law of Definite Proportions. The law states that a given compound always contains the same elements in a fixed ratio by mass. Here, both samples of sulfur dioxide contain oxygen and sulfur in a 50:50 ratio by mass, regardless of whether it was manufactured in a lab or mined from the ground.
Lesson3_Theory of Atomic Structure Models.pptx
Greek philosophers first proposed the idea of atoms as the fundamental indivisible units that make up all matter. Democritus named these fundamental units "atoms", from the Greek word meaning "indivisible". He concluded through observation and questioning that matter cannot be divided infinitely into smaller pieces, but rather is made of discrete atoms. John Dalton further developed atomic theory in the early 19th century. He proposed that all matter is composed of tiny indivisible particles called atoms, that atoms of a given element are identical, and that atoms combine in whole number ratios to form compounds through chemical reactions.
Science Performance Task
John Dalton formulated his atomic theory in the early 1800s based on careful chemical measurements and observations. His theory proposed that (1) all matter is composed of tiny indivisible atoms, (2) atoms of the same element are identical in mass, (3) atoms of different elements have different masses, and (4) atoms combine in simple whole number ratios. Dalton's atomic theory provided the foundation for modern chemistry and physics by establishing that elements combine at the atomic level. While Dalton's model has been refined over time, it represented a revolutionary shift in understanding the basic nature of matter.
Supriya Kaushik
John Dalton presented his atomic theory in 1808 to explain the properties of matter. Dalton's atomic theory states that all matter is made up of very tiny indivisible particles called atoms. Atoms are identical in mass and chemical properties for a given element but differ between elements. Atoms combine in whole number ratios to form compounds, with the relative numbers and kinds of atoms remaining constant for a given compound. Dalton's atomic theory became a foundation of modern chemistry.
Hrishabh
John Dalton was born in England and began his career as a teacher at age 12, later becoming a school principal. In 1793, he began teaching mathematics, physics, and chemistry, focusing his research on the study of matter. Dalton presented his Atomic Theory in 1808, which established that all matter is made of tiny indivisible particles called atoms that combine in whole number ratios to form compounds. The theory marked a turning point in understanding the composition of matter.
HISTORY OF ATOMIC THEORY
John Dalton proposed the atomic theory in 1804, stating that all matter is composed of tiny, indivisible particles called atoms that cannot be divided further. Later discoveries found that atoms consist of even smaller subatomic particles, including electrons discovered by J.J. Thomson in 1897 and the nucleus discovered by Ernest Rutherford in 1910. The quantum mechanical model developed in 1926 by Schrodinger, Heisenberg and others proposed that electrons exist as waves of energy around the nucleus, rather than following fixed orbits as proposed by Niels Bohr's 1913 planetary model of the atom.
Atomicnotes 7 And 8
The document discusses atomic structure and the periodic table. It explains that atoms are the basic unit of matter and are made up of protons, neutrons, and electrons. The number of protons determines the element. The periodic table organizes the elements and provides information about atomic structure like atomic number and mass. It also describes the historical models of the atom including those proposed by Dalton, Thomson, Rutherford, and Bohr.
Daltons atomic theory
Dalton's atomic theory proposed that:
1) Matter is made of extremely small indivisible particles called atoms.
2) Atoms of a given element are identical in size, mass and properties.
3) Atoms of different elements vary in size, mass and properties.
The theory had limitations such as not explaining Gay-Lussac's law of combining volumes or the nature of atomic bonding.
Modern atomic theory has updated that:
1) Atoms can be subdivided into smaller particles like electrons and protons.
2) Atoms are destructible through nuclear processes converting mass to energy.
3) Atoms of a given element can differ in mass and properties as
science.pptx
This presentation provides information about atoms and molecules. It defines an atom as the smallest particle of an element that cannot be created or destroyed in a chemical reaction. Atoms combine to form molecules, which are groups of two or more atoms held together by attractive forces. The document then discusses the symbols used to represent different elements, laws of chemical combination including conservation of mass and constant proportions, Dalton's atomic theory, and provides some biographical information about John Dalton.
John dalton[1]
John Dalton was an English chemist who developed modern atomic theory in the early 1800s. He proposed that all matter is made of extremely small indivisible particles called atoms, which are identical for a given element but differ between elements. Atoms of different elements combine in simple whole number ratios to form compounds, and chemical reactions involve atoms combining, separating, or rearranging. Dalton's atomic theory laid the foundation for understanding the composition and behavior of matter at the atomic scale.
Chapter 3.1 : The Atom: The Building Blocks of Matter
John Dalton developed the first atomic theory in 1808 based on experimental evidence from the laws of mass conservation, definite proportions, and multiple proportions. His theory proposed that all matter is composed of extremely small indivisible particles called atoms, atoms of a given element are identical, and atoms of different elements combine in simple whole number ratios to form compounds. Modern atomic theory has since modified Dalton's theory by showing atoms are divisible and some elements exist as different atomic masses.
Chemistry Class 11 sbcc part IV
John Dalton developed the first modern atomic theory in the early 1800s. He proposed that each chemical element is composed of unique atoms that cannot be created or destroyed through chemical reactions, but can combine to form compounds. Dalton hypothesized that differences in the masses of gas particles explained why water absorbed gases like carbon dioxide and nitrogen to different extents. His atomic theory marked the first truly scientific explanation of atoms. Dalton's concepts of atoms and molecules helped establish chemistry as a rigorous science.
History of atoms
Greek philosopher Democritus first proposed the idea of atoms in 460 BC, reasoning that matter must be divisible into indivisible particles. However, his idea was largely ignored. In the early 1800s, John Dalton performed experiments and developed an atomic theory, stating that elements are made of identical atoms that combine to form compounds. In 1897, Joseph John Thomson discovered the electron and proposed a early atomic model where electrons were embedded in a uniform sphere of positive charge, like raisins in pudding, known as the plum pudding model.
Science-8-week-5.pptx
1. The document discusses the early theories of the structure of atoms from ancient Greek philosophers to the modern atomic model.
2. It describes the discoveries of subatomic particles like the electron by J.J. Thomson and the nucleus by Ernest Rutherford through experiments.
3. Later scientists like Niels Bohr, James Chadwick, and Erwin Schrodinger further refined the model, with Bohr proposing electron shells and orbits, Chadwick discovering the neutron, and Schrodinger explaining electron probability clouds.
Chapter 4
This document discusses the structure of atoms. It begins by defining an atom and outlining Dalton's atomic theory. It then explains that atoms are composed of subatomic particles like electrons, protons, and neutrons. The nucleus contains protons and neutrons, while electrons orbit around the nucleus. Different elements are distinguished by their atomic number, which is the number of protons. Isotopes are atoms that have the same number of protons but different numbers of neutrons. The average atomic mass takes into account the relative abundances of isotopes in a naturally occurring sample of an element.
Physical science: Models of Atom
This document discusses the historical development of atomic models from Dalton to Bohr. It begins by explaining John Dalton's original model of atoms as indivisible, spherical particles. It then describes J.J. Thomson's "plum pudding" model which introduced electrons and viewed atoms as a soup of positive charge with electrons floating within. Rutherford's experiments led to his model of atoms with a small, dense nucleus surrounded by orbiting electrons. Bohr further refined this by proposing that electrons can only orbit in certain fixed energy levels. The document also notes Rutherford's prediction of a neutral particle in the nucleus, which was discovered by James Chadwick and named the neutron.
Lesson 3: Concepts About Chemical Elements
John Dalton's atomic theory proposed that all matter is composed of extremely small indivisible particles called atoms. Dalton theorized that elements are composed of atoms that are identical in mass and properties, and that compounds form when elements combine in whole number ratios. This led to laws like the law of definite proportions and law of multiple proportions. Later, Dmitri Mendeleev organized the known elements into the periodic table based on their atomic masses, and Henry Moseley rearranged the table based on atomic number, establishing it as a fundamental property of elements.
Minooka - Elements Part 2
Atoms are the smallest particles of elements that retain their chemical properties. Atoms consist of protons, neutrons, and electrons. John Dalton proposed his atomic theory in 1808, stating that all matter is made of indivisible atoms, atoms of the same element are identical, and atoms combine in simple whole number ratios. In the early 1900s, experiments showed that atoms have a small, dense nucleus surrounded by electrons, and electrons can exist in certain energy levels or orbits around the nucleus.
Chapter 4 pp (1)
This document summarizes key concepts about atomic structure:
1) It describes early atomic models including Democritus' idea of indivisible atoms and Dalton's atomic theory.
2) It explains the discovery of subatomic particles (electrons, protons, neutrons) and the nuclear model of the atom with electrons orbiting a nucleus.
3) It defines important atomic properties including atomic number, mass number, isotopes, and how to calculate atomic mass.
4) It provides an overview of how the periodic table organizes elements based on these atomic properties.
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Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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- 2. MATTER ATOM
- 3. In the early nineteenth century, an English chemist Dalton stated clearly his ideas regarding atoms. He was the first person to give out atomic theory in 1803. This theory is known as Dalton's Atomic Theory.
- 6. DALTON'S ATOMIC THEORY 1. Elements are made up of tiny particles called “atoms”. 2. Atoms are indivisible. 3. Atoms can neither be created nor destroyed. 4. Atoms of the same element are alike in their mass and chemical properties.
- 7. DALTON'S ATOMIC THEORY [Con.] 5. Atoms of different element differ in their mass and chemical properties. 6. Atoms of one element cannot be converted into atoms of another element 7. Atoms of different elements always combine in simple, definite and integral ratios to form compound atoms.
- 8. According to Dalton atom is the smallest, indivisible particle of an element that takes part in a chemical reaction.
- 9. 1. According to Dalton ,what is an atom ? 2. What are the properties of an atom according to Dalton ? 3. What are the postulates of Dalton's atomic theory ?
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- 14. 10000V 0.01atm Cathode rays travel in straight line.
- 15. 10000V 0.01atm Pedle These rays consist of material particles.
- 16. 10000V 0.01atm Cathode rays originate from cathode
- 17. 10000V 0.01atm CATHODE Cathode rays are deflected by electric field.
- 18. 10000V 0.01atm CATHODE Cathode rays consist negatively charged particles called "electron".
- 19. 1) Cathode rays originate from cathode. 2) Cathode rays travel in straight line. 3) Cathode rays are deflected by electric field. 4) Cathode rays are deflected by magnetic field. 5) These rays consist of material particles. 6) Cathode rays consist negatively charged particles called "electron".
- 20. 11000V 0.01atm Eugene Goldstein Anode Ray Experiment Discovery of Positively charged particle - Proton