Atoms are the fundamental units that make up elements. John Dalton proposed the atomic theory which states that elements are made of atoms and atoms of the same element are identical. Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The discovery of the electron, proton, neutron, and development of quantum theory led to modern atomic structure and periodic table. The periodic table organizes elements based on atomic structure including atomic number and trends in properties.
The document discusses the history of atomic theory from ancient Greek philosophers to modern atomic structure. It begins with Democritus proposing atoms in 460 BC, though Aristotle disagreed. In the early 1800s, John Dalton revived atomic theory and proposed atoms combine in whole number ratios, explaining conservation of mass. In the early 1900s, J.J. Thomson, Ernest Rutherford, and Niels Bohr contributed atomic models. Atoms are made of electrons, protons, and neutrons. Isotopes have the same number of protons but different neutrons. Unstable nuclei undergo radioactive decay through alpha, beta, or gamma radiation.
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.
The document discusses the atomic theory of matter and the development of atomic structure models. It describes John Dalton's atomic theory which stated that elements are composed of atoms that are unique and atoms are neither created nor destroyed in chemical reactions. The discovery of the electron by J.J. Thompson and experiments by Robert Millikan and Ernest Rutherford helped develop the modern atomic structure model of a small, dense nucleus surrounded by electrons. The document also discusses isotopes, atomic numbers, mass numbers, and how the periodic table is arranged based on atomic structure.
- John Dalton developed the first modern atomic theory in the early 1800s based on experiments observing chemical reactions. He proposed that all matter is composed of tiny, indivisible particles called atoms.
- Atoms consist of a small, dense nucleus containing protons and neutrons, surrounded by electrons. The number of protons defines the identity of the atom as a particular chemical element.
- Atoms of the same element can differ in the number of neutrons, forming isotopes. Unstable isotopes decay through emission of radiation like alpha or beta particles to become stable.
This document summarizes key concepts about atomic structure from Chapter 4. It discusses early atomic models proposed by Democritus and Dalton. Dalton's atomic theory stated that all matter is made of atoms that cannot be divided further. The document then explains discoveries of subatomic particles like electrons, protons, and neutrons. It describes Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus. Finally, it defines atomic number, mass number, isotopes, and how average atomic masses are calculated based on isotope abundances.
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
Atoms are the fundamental units that make up elements. John Dalton proposed the atomic theory which states that elements are made of atoms and atoms of the same element are identical. Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The discovery of the electron, proton, neutron, and development of quantum theory led to modern atomic structure and periodic table. The periodic table organizes elements based on atomic structure including atomic number and trends in properties.
The document discusses the history of atomic theory from ancient Greek philosophers to modern atomic structure. It begins with Democritus proposing atoms in 460 BC, though Aristotle disagreed. In the early 1800s, John Dalton revived atomic theory and proposed atoms combine in whole number ratios, explaining conservation of mass. In the early 1900s, J.J. Thomson, Ernest Rutherford, and Niels Bohr contributed atomic models. Atoms are made of electrons, protons, and neutrons. Isotopes have the same number of protons but different neutrons. Unstable nuclei undergo radioactive decay through alpha, beta, or gamma radiation.
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.
The document discusses the atomic theory of matter and the development of atomic structure models. It describes John Dalton's atomic theory which stated that elements are composed of atoms that are unique and atoms are neither created nor destroyed in chemical reactions. The discovery of the electron by J.J. Thompson and experiments by Robert Millikan and Ernest Rutherford helped develop the modern atomic structure model of a small, dense nucleus surrounded by electrons. The document also discusses isotopes, atomic numbers, mass numbers, and how the periodic table is arranged based on atomic structure.
- John Dalton developed the first modern atomic theory in the early 1800s based on experiments observing chemical reactions. He proposed that all matter is composed of tiny, indivisible particles called atoms.
- Atoms consist of a small, dense nucleus containing protons and neutrons, surrounded by electrons. The number of protons defines the identity of the atom as a particular chemical element.
- Atoms of the same element can differ in the number of neutrons, forming isotopes. Unstable isotopes decay through emission of radiation like alpha or beta particles to become stable.
This document summarizes key concepts about atomic structure from Chapter 4. It discusses early atomic models proposed by Democritus and Dalton. Dalton's atomic theory stated that all matter is made of atoms that cannot be divided further. The document then explains discoveries of subatomic particles like electrons, protons, and neutrons. It describes Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus. Finally, it defines atomic number, mass number, isotopes, and how average atomic masses are calculated based on isotope abundances.
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
This document provides an overview of atomic structure and properties. It discusses John Dalton's atomic theory, early atomic models including Thomson's plum pudding model and Rutherford's nuclear model. Later, it describes Bohr's model of electron orbits and different atomic orbitals. The document also defines key atomic properties including atomic number, mass number, and isotopes.
The document provides an overview of atomic structure and models of the atom over time. It discusses:
1) Early atomic models including Thomson's model of a positively charged sphere with electrons inside and Rutherford's discovery of the nucleus at the atom's center.
2) Modern atomic structure with a dense nucleus surrounded by an electron cloud, and that protons and neutrons are made of quarks.
3) Differences between atoms including atomic number, isotopes having different neutron numbers, and ions forming when atoms gain or lose electrons.
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.
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.
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.
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.
CBSE Class 9 Science Chapter 4- structure of atomAarthiSam
This document discusses the structure of atoms and the development of atomic models over time. It covers John Dalton's early atomic theory that atoms are indivisible and different for each element. J.J. Thomson's plum pudding model described atoms as electrically neutral spheres. Rutherford determined atoms have a small, dense nucleus through alpha particle scattering experiments. Niels Bohr incorporated quantum theory, proposing electrons orbit in discrete energy levels. The document also discusses atomic number, mass number, isotopes, electron configuration, and valency.
The document summarizes key concepts in atomic theory and structure:
- Early atomic theory proposed atoms as indivisible particles, but experiments showed atoms have internal structure including a small, dense nucleus and orbiting electrons.
- Atoms are composed of protons, neutrons, and electrons. The number of protons defines an element and is its atomic number. Isotopes differ in their number of neutrons.
- The periodic table organizes elements based on atomic structure, with elements in the same group having similar properties. Metals are on the left, nonmetals on the right, and metalloids in between.
- Compounds are formed by the combination of elements. Molecular compounds contain molecules
1) The document discusses Dalton's atomic theory and the key discoveries that led to the modern understanding of atomic structure.
2) It describes J.J. Thomson's discovery of electrons in cathode rays and Millikan's oil drop experiment which determined the charge of an electron.
3) Rutherford's gold foil experiment revealed that atoms have a small, dense nucleus containing most of their mass, with electrons in the space around the nucleus.
The document discusses the fundamental particles and forces that make up atoms. It describes how atoms were discovered to be made up of even smaller particles, including electrons discovered by J.J. Thomson and the nuclear model developed by Rutherford based on experiments by Rutherford, Geiger, and Marsden. The document also discusses the three main subatomic particles (protons, neutrons, and electrons), isotopes, radioactive decay, and the four main forces (electromagnetic, strong nuclear, weak, and gravity) that act inside atoms.
1) An atom is made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus.
2) Rutherford's gold foil experiment showed that the mass and positive charge of an atom are concentrated in a small nucleus.
3) Bohr's model improved upon Rutherford's by proposing that electrons can only orbit in discrete, fixed energy levels rather than any path, resolving the issue of electrons radiating energy in orbits.
The document summarizes the development of atomic theory from ancient Greek philosophers to modern quantum mechanics. It describes early atomic models including Dalton's theory that atoms are indivisible particles that combine in whole number ratios, as well as Thomson's plum pudding model and Rutherford's nuclear model developed from his gold foil experiment. Later, Bohr incorporated quantized energy levels to explain atomic spectra, while quantum mechanics describes electrons as probabilistic clouds within orbitals and energy levels.
The document summarizes the development of atomic theory over time. It describes the early ideas of Democritus and Dalton's contributions, including defining atoms and the key points of his atomic theory. Later discoveries included the electron by Thomson, the nuclear model from Rutherford's gold foil experiment, discovery of the proton, neutron discovered by Chadwick, and development of quantum mechanics to better explain atomic structure.
This document provides an overview of the structure of an atom according to different atomic models over time. It begins with Dalton's atomic theory from 1807 that atoms are fundamental units of matter. Later models include Thomson's "plum pudding" model from 1897, Rutherford's discovery of the nucleus from experiments in 1908, and Bohr's model from 1913 which proposed electrons orbit in distinct energy levels. The document then discusses the subatomic particles of protons, neutrons, and electrons and their roles. It concludes with definitions of related atomic concepts such as atomic number, mass number, isotopes, and isobars.
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
Structure of matter atoms and moleculesSuman Tiwari
- An atom is the smallest particle of an element that retains the chemical properties of that element. All atoms of the same element are identical.
- Atoms are very small, not visible even under a powerful microscope. Models like the ball-and-stick model are used to represent atoms and molecules.
- Atoms consist of even smaller subatomic particles - protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The number of protons determines the element.
This document summarizes the history and development of the atomic theory and periodic table. It discusses early Greek philosophers' ideas about atoms, John Dalton's atomic theory in the early 1800s, J.J. Thomson's discovery of electrons in the late 1800s, Ernest Rutherford's discovery of the nucleus in 1909, and the discovery of neutrons in 1930 which completed the modern atomic model. It also explains how atoms are composed of protons, neutrons and electrons, how atomic and mass numbers are used to identify elements and isotopes, and how average atomic masses are calculated based on the relative abundances of isotopes in nature.
CHM021 5 GROSS STRUCTURE OF ATOM (model).pptxYaySandoval1
1. The document discusses the early theories of matter composition from the Greeks to Dalton's atomic theory. It then summarizes evidence from experiments in the late 19th to early 20th century that led to discoveries of the internal structure of atoms, including discovery of the electron, proton, and neutron.
2. Key experiments and scientists discussed include Thomson's discovery of the electron, Millikan's measurement of the electron's charge, Rutherford's nuclear model of the atom based on radioactive experiments, discovery of the proton by Goldstein and Chadwick's discovery of the neutron.
3. These discoveries revealed that atoms are mostly empty space with a small, dense nucleus containing protons and neutrons, and electrons in orbits around
This document provides an overview of models of the atom from ancient Greek philosophers to modern scientific theories. It discusses early ideas that matter was made of indivisible particles called atoms. John Dalton proposed the first modern atomic model with atoms as hard spheres. J.J. Thomson's discovery of electrons led to a "plum pudding" model of atoms. Rutherford's gold foil experiment showed atoms had a small, dense nucleus. Later, the discovery of neutrons completed the nuclear model of the atom. Modern quantum models describe electron distribution as "clouds" rather than definite orbits.
This document provides an overview of atomic structure and properties. It discusses John Dalton's atomic theory, early atomic models including Thomson's plum pudding model and Rutherford's nuclear model. Later, it describes Bohr's model of electron orbits and different atomic orbitals. The document also defines key atomic properties including atomic number, mass number, and isotopes.
The document provides an overview of atomic structure and models of the atom over time. It discusses:
1) Early atomic models including Thomson's model of a positively charged sphere with electrons inside and Rutherford's discovery of the nucleus at the atom's center.
2) Modern atomic structure with a dense nucleus surrounded by an electron cloud, and that protons and neutrons are made of quarks.
3) Differences between atoms including atomic number, isotopes having different neutron numbers, and ions forming when atoms gain or lose electrons.
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.
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.
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.
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.
CBSE Class 9 Science Chapter 4- structure of atomAarthiSam
This document discusses the structure of atoms and the development of atomic models over time. It covers John Dalton's early atomic theory that atoms are indivisible and different for each element. J.J. Thomson's plum pudding model described atoms as electrically neutral spheres. Rutherford determined atoms have a small, dense nucleus through alpha particle scattering experiments. Niels Bohr incorporated quantum theory, proposing electrons orbit in discrete energy levels. The document also discusses atomic number, mass number, isotopes, electron configuration, and valency.
The document summarizes key concepts in atomic theory and structure:
- Early atomic theory proposed atoms as indivisible particles, but experiments showed atoms have internal structure including a small, dense nucleus and orbiting electrons.
- Atoms are composed of protons, neutrons, and electrons. The number of protons defines an element and is its atomic number. Isotopes differ in their number of neutrons.
- The periodic table organizes elements based on atomic structure, with elements in the same group having similar properties. Metals are on the left, nonmetals on the right, and metalloids in between.
- Compounds are formed by the combination of elements. Molecular compounds contain molecules
1) The document discusses Dalton's atomic theory and the key discoveries that led to the modern understanding of atomic structure.
2) It describes J.J. Thomson's discovery of electrons in cathode rays and Millikan's oil drop experiment which determined the charge of an electron.
3) Rutherford's gold foil experiment revealed that atoms have a small, dense nucleus containing most of their mass, with electrons in the space around the nucleus.
The document discusses the fundamental particles and forces that make up atoms. It describes how atoms were discovered to be made up of even smaller particles, including electrons discovered by J.J. Thomson and the nuclear model developed by Rutherford based on experiments by Rutherford, Geiger, and Marsden. The document also discusses the three main subatomic particles (protons, neutrons, and electrons), isotopes, radioactive decay, and the four main forces (electromagnetic, strong nuclear, weak, and gravity) that act inside atoms.
1) An atom is made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus.
2) Rutherford's gold foil experiment showed that the mass and positive charge of an atom are concentrated in a small nucleus.
3) Bohr's model improved upon Rutherford's by proposing that electrons can only orbit in discrete, fixed energy levels rather than any path, resolving the issue of electrons radiating energy in orbits.
The document summarizes the development of atomic theory from ancient Greek philosophers to modern quantum mechanics. It describes early atomic models including Dalton's theory that atoms are indivisible particles that combine in whole number ratios, as well as Thomson's plum pudding model and Rutherford's nuclear model developed from his gold foil experiment. Later, Bohr incorporated quantized energy levels to explain atomic spectra, while quantum mechanics describes electrons as probabilistic clouds within orbitals and energy levels.
The document summarizes the development of atomic theory over time. It describes the early ideas of Democritus and Dalton's contributions, including defining atoms and the key points of his atomic theory. Later discoveries included the electron by Thomson, the nuclear model from Rutherford's gold foil experiment, discovery of the proton, neutron discovered by Chadwick, and development of quantum mechanics to better explain atomic structure.
This document provides an overview of the structure of an atom according to different atomic models over time. It begins with Dalton's atomic theory from 1807 that atoms are fundamental units of matter. Later models include Thomson's "plum pudding" model from 1897, Rutherford's discovery of the nucleus from experiments in 1908, and Bohr's model from 1913 which proposed electrons orbit in distinct energy levels. The document then discusses the subatomic particles of protons, neutrons, and electrons and their roles. It concludes with definitions of related atomic concepts such as atomic number, mass number, isotopes, and isobars.
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
Structure of matter atoms and moleculesSuman Tiwari
- An atom is the smallest particle of an element that retains the chemical properties of that element. All atoms of the same element are identical.
- Atoms are very small, not visible even under a powerful microscope. Models like the ball-and-stick model are used to represent atoms and molecules.
- Atoms consist of even smaller subatomic particles - protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The number of protons determines the element.
This document summarizes the history and development of the atomic theory and periodic table. It discusses early Greek philosophers' ideas about atoms, John Dalton's atomic theory in the early 1800s, J.J. Thomson's discovery of electrons in the late 1800s, Ernest Rutherford's discovery of the nucleus in 1909, and the discovery of neutrons in 1930 which completed the modern atomic model. It also explains how atoms are composed of protons, neutrons and electrons, how atomic and mass numbers are used to identify elements and isotopes, and how average atomic masses are calculated based on the relative abundances of isotopes in nature.
CHM021 5 GROSS STRUCTURE OF ATOM (model).pptxYaySandoval1
1. The document discusses the early theories of matter composition from the Greeks to Dalton's atomic theory. It then summarizes evidence from experiments in the late 19th to early 20th century that led to discoveries of the internal structure of atoms, including discovery of the electron, proton, and neutron.
2. Key experiments and scientists discussed include Thomson's discovery of the electron, Millikan's measurement of the electron's charge, Rutherford's nuclear model of the atom based on radioactive experiments, discovery of the proton by Goldstein and Chadwick's discovery of the neutron.
3. These discoveries revealed that atoms are mostly empty space with a small, dense nucleus containing protons and neutrons, and electrons in orbits around
This document provides an overview of models of the atom from ancient Greek philosophers to modern scientific theories. It discusses early ideas that matter was made of indivisible particles called atoms. John Dalton proposed the first modern atomic model with atoms as hard spheres. J.J. Thomson's discovery of electrons led to a "plum pudding" model of atoms. Rutherford's gold foil experiment showed atoms had a small, dense nucleus. Later, the discovery of neutrons completed the nuclear model of the atom. Modern quantum models describe electron distribution as "clouds" rather than definite orbits.
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
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
2. Early Models of Atoms
• Democritus (460-400B.C.) first suggested the existence of
these particles, which he called “atoms” for the Greek word
for “uncuttable”. They lacked experimental support due to the
lack of scientific testing at the time.
• John Dalton (1766-1844) performed experiments to study the
ratios in which elements combine in chemical reactions.
Formulate hypotheses and theories to explain his
observations, which became Dalton’s Atomic Theory.
– All elements are composed of tiny indivisible particles called
atoms.
– Atoms of the same element are identical. The atoms of any one
element are different from those of any other element.
– Atoms of different elements can physically mix together or
combine in simple, whole number ratios to form compounds.
– Chemical reactions occur when atoms are separated, joined or
rearranged. Atoms of one element, however, are never changed
into atoms of another element as a result of a chemical reaction.
3. Size of an Atom
• Imagine grinding a copper coin (penny) into fine
dust. Each speck in the small pile of shiny red
dust would still have the properties of copper. If
by some means you could still make the dust
particles smaller you would eventually come upon
a particle known as an atom.
• An atom is the smallest particle of an element
that retains the properties of that element.
• A pure copper penny contains about 2.4 X 1022
atoms, compared to the Earth’s population of 6 X
106 people.
• If you lined 100,000,000 copper atoms up side by
side they would produce a line 1 cm long.
4. Atomic Structure
• Atoms are now known to be divisible as they can be broken
down to even smaller particles by atom smashers.
• J.J. Thomson (1856-1940) discovered electrons using
cathode ray tubes.
• Robert Millikan (1868-1953) carried out experiments to
determine the charge of an electron (-). He also determined
the ratio of the charge to the mass of an electron.
• In 1886, E. Goldstein observed a cathode ray tube and
found rays traveling in the opposite direction to that of the
cathode rays. He called these rays canal rays and
concluded that they must be positive particles, which are
now called protons.
• In 1932, James Chadwick confirmed the existence of yet
another subatomic particle: the neutron. Neutrons are
subatomic particles with no charge but with a mass nearly
equal to that of a proton. See simulation
5. • After discovering these subatomic particles,
scientists wondered how they were put together.
• JJ Thomson thought since the electrons
contributed such a small fraction of the atoms
mass, they were probably an equal fraction of it
size so it was like “Plum Pudding”.
• In 1911, Ernest Rutherford and his coworkers
performed the Gold Foil Experiment to further
study the phenomenon.
• Concluded that most of the mass of each atom
and all of its positive charge reside in a very
small, extremely dense region which is called
the nucleus. The rest of the atom is mostly
empty space.
6. Modern View of Atomic Structure
• Since the time of Rutherford, physicists have learned much
about the nucleus. Although many other parts have been
discovered, chemists tend to only work with three main
particles since they determine chemical behavior: Electron,
Neutron and Proton
• Electron has a charge of -1.602 X 10-19 C and a proton has a
charge of 1.602 X 10-19 C so this quantity of Coulombs is
known as one electronic charge and atomic and subatomic
particles usually have a charge that is multiples of this.
Neutrons have no charge and are electrically neutral.
• Atoms have extremely small masses so instead of using
the real numbers, atomic mass units (amus) are used.
Protons and neutrons are very similar in mass but it would
take 1836 electrons to equal 1 proton so most of an atoms
mass is in the nucleus.
• Atoms are also extremely small with diameters between 1
X 10-10 and 5 X 10-10 so they are usually expressed with
angstroms, which is 10-10.
7. Atomic Number
• The number of protons in the nucleus
of an atom of that element
• For an atom with no charge, this is also
the number of electrons since the
positive charge of the protons cancels
the negative charge of the electrons.
• Practice problems #7-8 pg 115
8. Mass Number
• Most of the mass of an atom is found in the
nucleus so the total number of protons and
neutrons equals the mass number.
• If you know the atomic umber and mass number
you can determine the composition of that atom.
• The composition can be represented by the
shorthand notation using the element symbol,
atomic number and mass number.
• For gold, Au is the symbol for the element and
the atomic number is subscript and mass
number is superscript on the left side.
Au
79
197
• Practice problems 9-11 pg 116
9. Isotopes
• Atoms that have the same number of
protons but different number of
neutrons.
• Affects the shorthand notation of the
element.
• Practice problems 12-13 on pg 117
10. Atomic Mass
• Today we can determine the masses of
individual atoms with a relative high degree of
accuracy but since they are so small atomic
mass units are used with hydrogen being 1
amu.
• The average atomic mass for an element due
to the different isotopes, the mass of those
isotopes and the natural percent abundance.
• Add up the different atomic mass of each atom
and then divide by the number of atoms.
• Or, multiply mass by % and then determine
average mass.
• Practice problems 14-15 pg 120 and 16-17 pg
121.
11. Mass Spectrometer
• The most direct and accurate means for
determining atomic and molecular
weights. See pg 48
12. Periodic Table
• The arrangement of elements in order of
increasing atomic number, with elements
having similar properties placed in vertical
column.
• Atomic number, symbol, name, atomic
weight are found in each square for each
element. Some tables have additional
information as well. Example
• Can be arranged according to metals, non-
metals and metalloids, solid liquid and
gases, and by family. Example