Lesson: Tuesday 9/1
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Two quantities that define matter are volume and mass. Volume can be measured using units like liters, cubic centimeters. Mass is measured using standard units like grams. The document discusses the history of atomic theory. Ancient Greek philosophers proposed the idea of atoms as the smallest indivisible units of matter. In the 1800s, John Dalton further developed atomic theory, proposing that atoms are the building blocks of all matter and composed of even smaller subatomic particles like protons, neutrons and electrons. The size of an atom is incredibly small. For example, about 10 trillion atoms could fit in a single centimeter. Despite their small size, atoms are not truly indivisible as originally proposed, as they can be broken
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The document traces the development of atomic theory from ancient Greek philosophers to modern quantum mechanics. It describes early particle theories proposed by Democritus and Dalton, Thomson's "plum pudding" model, Rutherford's gold foil experiment which established the nucleus, Bohr's model of electron orbits, and the current wave model of electron clouds. The atomic model has changed significantly over time as new evidence challenged earlier conceptions and led scientists to develop more accurate representations of atoms and their structure.
ATOMS_ppt.pptx
1) Almost 2500 years ago, Leucippus and his student Democritus believed that all matter was made of tiny, indivisible particles called atoms.
2) A little over two centuries ago, John Dalton expanded on this idea and theorized that all matter is made of very small particles called atoms, and that atoms are the smallest particles that have the properties of each element.
3) Today we know that atoms combine to form molecules, which are the smallest particles of elements or compounds that can exist independently. Molecules consist of two or more atoms arranged in a specific structure.
the atom
Atoms are the smallest and most basic building blocks that make up all matter in our world. Atoms themselves are composed of even smaller particles, including a nucleus containing protons and neutrons at the center, and electrons that orbit around the nucleus. Everything visible in our daily lives, from the smallest molecules to large objects, are comprised of combinations of these tiny atoms.
Structure of atoms10
Scientists have been studying atoms since the 1800s using models to understand their structure and behavior. Early philosophers proposed the idea of atoms, while scientists like Dalton, Thomson, Rutherford, and Bohr developed atomic models through experiments. They discovered that atoms are mostly empty space with a small, dense nucleus at the center containing protons and neutrons, and electrons orbiting the nucleus. The number of protons determines the element, while isotopes of an element have different numbers of neutrons.
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The document traces the development of atomic theory from ancient Greek philosophers to modern quantum mechanics. It describes early particle theories proposed by Democritus and Dalton, Thomson's "plum pudding" model, Rutherford's gold foil experiment which established the nucleus, Bohr's model of electron orbits, and the current wave model of electron clouds. The atomic model has changed significantly over time as new evidence challenged earlier conceptions and led scientists to develop more accurate representations of atoms and their structure.
ATOMS_ppt.pptx
1) Almost 2500 years ago, Leucippus and his student Democritus believed that all matter was made of tiny, indivisible particles called atoms.
2) A little over two centuries ago, John Dalton expanded on this idea and theorized that all matter is made of very small particles called atoms, and that atoms are the smallest particles that have the properties of each element.
3) Today we know that atoms combine to form molecules, which are the smallest particles of elements or compounds that can exist independently. Molecules consist of two or more atoms arranged in a specific structure.
the atom
Atoms are the smallest and most basic building blocks that make up all matter in our world. Atoms themselves are composed of even smaller particles, including a nucleus containing protons and neutrons at the center, and electrons that orbit around the nucleus. Everything visible in our daily lives, from the smallest molecules to large objects, are comprised of combinations of these tiny atoms.
Structure of atoms10
Scientists have been studying atoms since the 1800s using models to understand their structure and behavior. Early philosophers proposed the idea of atoms, while scientists like Dalton, Thomson, Rutherford, and Bohr developed atomic models through experiments. They discovered that atoms are mostly empty space with a small, dense nucleus at the center containing protons and neutrons, and electrons orbiting the nucleus. The number of protons determines the element, while isotopes of an element have different numbers of neutrons.
Intro to Atoms
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DEVELOPMENT OF THE ATOM MODEL.pptx
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Lesson 2 Scale of Objects Student Materials .docx
Lesson 2:
Scale of Objects
Student Materials
Contents
• Visualizing the Nanoscale: Student Reading
• Scale Diagram: Dominant Objects, Tools, Models, and Forces at Various
Different Scales
• Number Line/Card Sort Activity: Student Instructions & Worksheet
• Cards for Number Line/Card Sort Activity: Objects & Units
• Cutting it Down Activity: Student Instructions & Worksheet
• Scale of Objects Activity: Student Instructions & Worksheet
• Scale of Small Objects: Student Quiz
2-S1
Visualizing the Nanoscale: Student Reading
How Small is a Nanometer?
The meter (m) is the basic unit of length in the metric system, and a nanometer is one
billionth of a meter. It's easy for us to visualize a meter; that’s about 3 feet. But a
billionth of that? It’s a scale so different from what we're used to that it's difficult to
imagine.
What Are Common Size Units, and Where is the Nanoscale Relative to Them?
Table 1 below shows some common size units and their various notations (exponential,
number, English) and examples of objects that illustrate about how big each unit is.
Table 1. Common size units and examples.
Unit Magnitude as an
exponent (m)
Magnitude as a
number (m)
English
Expression
About how
big?
Meter 100 1 One A bit bigger
than a yardstick
Centimeter 10-2 0.01 One Hundredth Width of a
fingernail
Millimeter 10-3 0.001 One
Thousandth
Thickness of a
dime
Micrometer 10-6 0.000001 One Millionth A single cell
Nanometer 10-9 0.000000001 One Billionth 10 hydrogen
atoms lined up
Angstrom 10-10 0.0000000001 A large atom
Nanoscience is the study and development of materials and structures in the range of 1
nm (10-9 m) to 100 nanometers (100 x 10-9 = 10-7 m) and the unique properties that arise
at that scale. That is small! At the nanoscale, we are manipulating objects that are more
than one-millionth the size of the period at the end of this sentence.
What if We Measured the Size of Various Objects in Terms of Nanometers?
A typical atom is anywhere from 0.1 to 0.5 nanometers in diameter. DNA molecules are
about 2.5 nanometers wide. Most proteins are about 10 nanometers wide, and a typical
virus is about 100 nanometers wide. A bacterium is about 1000 nanometers. Human
cells, such as red blood cells, are about 10,000 nanometers across. At 100,000
nanometers, the width of a human hair seems gigantic. The head of a pin is about a
million nanometers wide. An adult man who is 2 meters tall (6 feet 5 inches) is about 2
billion nanometers tall!
2-S2
So is That What Nanoscience is All About––Smallness?
No, smallness alone doesn’t account for all the interest in the nanoscale. Nanoscale
structures push the envelope of physics, moving into the strange world of quantum
mechanics. For nanoparticles, gravity hardly matters due to their small mass. However,
the Brownian motion of these particles now becomes important. Nanosized particles of
any given substance exhibit differen ...
The building blocks_of_matter_-_atoms
Atoms are the smallest particles of matter that retain the chemical properties of an element. They are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit around the nucleus. The number of protons determines the element, while the number of neutrons determines the isotope. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Electromagnetic force attracts opposite charges, while strong force holds the nucleus together against electromagnetic repulsion between protons.
Basic-Atomic-Structure.9248797.powerpoint.pptx
This document summarizes early theories of atomic structure from the 5th century BC through the early 20th century. It discusses the Greek philosophers Leucippus and Democritus who proposed that matter is made of indivisible atoms. John Dalton's atomic theory from 1803 stated that matter is composed of atoms that combine in whole number ratios. Experiments by J.J. Thomson, Rutherford, and others led to the discoveries of subatomic particles like electrons and discovery of the nucleus. Rutherford's gold foil experiment showed that atoms have a small, dense positively charged nucleus occupying a tiny fraction of the atom's volume.
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.
Nuclear and Atomic Physics
Nuclear physics involves understanding atoms through experiments like Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus surrounded by empty space. Radiation like alpha, beta, and gamma rays is used in applications such as cancer treatment, electricity generation, and radiocarbon dating which relies on the radioactive decay of carbon-14 to determine the age of ancient materials.
Chapter 4 - The Atom
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.
Atomic Structure
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.
Chapter 3
The document discusses the history of atomic theory from ancient Greek philosophers to modern atomic structure. It introduces key figures like Democritus, Dalton, Thomson, and Rutherford and their contributions to understanding that all matter is made of tiny indivisible particles called atoms. The document also describes the discovery of subatomic particles like protons, neutrons, and electrons, and how electrons occupy distinct energy levels around the nucleus in an atom.
3.-Atoms-Molecules-and-Ions.pdf
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
Of Atoms and of Radioactivity
The document provides information about radioactivity and the structure of atoms. It discusses that atoms are made up of protons, neutrons and electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. It describes that there are three main types of radiation: alpha, beta and gamma. Alpha particles consist of two protons and two neutrons, beta particles are high speed electrons, and gamma radiation is a high energy wave. It explains that radioactive atoms are unstable and emit these types of radiation to become stable. Each type of radiation has different properties in terms of what they are made of, how far they can travel in air, and what can stop them. The document seeks to educate about radioactivity and radiation.
Atomic models Dr. vijender singh
The atomic model has changed significantly over time based on new evidence and experiments. Early philosophers proposed that atoms were indivisible spheres, while later scientists like Thomson and Rutherford provided evidence that atoms have internal structure, including a small, dense nucleus surrounded by electrons. The current wave model depicts electrons as existing in probabilistic electron clouds rather than definite orbits, representing our most accurate understanding of atomic structure to date.
Of Atoms and of Radioactivity
The document provides information about radioactivity and radiation. It begins by explaining the structure of atoms and the three main types of radiation: alpha, beta, and gamma. Alpha radiation is emitted as high-speed helium nuclei, beta as high-speed electrons, and gamma is a high-energy electromagnetic wave released after alpha or beta decay. It then discusses that radioactive atoms are unstable and emit radiation to become stable. The properties of the three types of radiation are explained, including what distance they can travel in air and what materials can stop them. Examples of radioactive materials and a quiz conclude the document.
The Atom
The document discusses the history and development of atomic theory from ancient Greek philosophers to modern atomic structure. Some key points covered include:
- Democritus first proposed the idea of atoms in ancient Greece but lacked evidence.
- In the 1800s, Dalton proposed his atomic theory that elements are made of atoms that combine in simple whole number ratios.
- Advances revealed atoms have internal structure including a tiny dense nucleus and orbiting electrons.
- Atoms are identified by their atomic number and mass number, which indicate protons, neutrons, and isotopes.
- The mole, molar mass, and Avogadro's number allow relating masses to numbers of atoms and particles.
Atomos
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
Atomos[1]
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
Atomos
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's model of atoms as indivisible spheres, Thomson's "plum pudding" model with electrons scattered in a positively charged substance, Rutherford's gold foil experiment showing atoms are mostly empty space with a dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus like planets, and the modern wave model where electrons exist as probability clouds rather than definite orbits.
3 2 What Is Heat
The document outlines a science lesson on heat and phase changes. It provides objectives for defining heat and classifying phase changes as endothermic or exothermic. Examples of endothermic and exothermic processes like melting, evaporation, condensation and freezing are discussed. Students complete exit slips to assess their understanding.
2 24 Unit #7 Jeopardy
The document provides an agenda and materials for a chemistry class review session in preparation for an exam on Unit 7. The session will include reviewing practice questions from the previous day, going over the objectives for the day which is a review, and participating in a jeopardy game to further review the material in a fun way. The calendar shows that today is the review session and tomorrow will be the exam.
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Similar to Lesson: Tuesday 9/1
Intro to Atoms
The document discusses the history of the concept of atoms from ancient Greek philosophers to modern quantum physics. It explains that atoms are the smallest particles of an element that retain the element's chemical properties, and are made up of protons, neutrons, and electrons. The protons and neutrons are packed tightly together in the nucleus, while electrons orbit the nucleus in electron clouds. Cutting a gold bar in half repeatedly would result in smaller pieces of gold until individual atoms were reached, which cannot be further divided while retaining gold's chemical identity.
Chem m10 what's inside the atom
The document provides information about Module 10 of an alternative secondary education chemistry course. It discusses the evolution of atomic theory from ancient Greek philosophers' idea of atoms as indivisible particles, to John Dalton's atomic theory in the early 1800s. It also describes the discovery of subatomic particles like electrons, protons, and neutrons using instruments like the cathode ray tube. The module aims to teach students about atomic structure and composition, isotopes, radioactivity, and the development of modern atomic models. It includes lessons, learning objectives, and guidance for self-study.
DEVELOPMENT OF THE ATOM MODEL.pptx
1. The document describes the development of atomic models over time from Democritus' idea of indivisible atoms to modern particle models.
2. Key contributors mentioned include Dalton with his billiard ball model, Thomson and his plum pudding model, Rutherford and his discovery of the nucleus through gold foil experiments, Bohr and his planetary model with electron shells, and Chadwick's discovery of the neutron.
3. The progression of models incorporated new evidence about the internal structure of atoms and location of the electron, from Thomson first showing atoms have internal parts to Rutherford locating a small, dense nucleus to Bohr adding electron shells.
Lesson 2 Scale of Objects Student Materials .docx
Lesson 2:
Scale of Objects
Student Materials
Contents
• Visualizing the Nanoscale: Student Reading
• Scale Diagram: Dominant Objects, Tools, Models, and Forces at Various
Different Scales
• Number Line/Card Sort Activity: Student Instructions & Worksheet
• Cards for Number Line/Card Sort Activity: Objects & Units
• Cutting it Down Activity: Student Instructions & Worksheet
• Scale of Objects Activity: Student Instructions & Worksheet
• Scale of Small Objects: Student Quiz
2-S1
Visualizing the Nanoscale: Student Reading
How Small is a Nanometer?
The meter (m) is the basic unit of length in the metric system, and a nanometer is one
billionth of a meter. It's easy for us to visualize a meter; that’s about 3 feet. But a
billionth of that? It’s a scale so different from what we're used to that it's difficult to
imagine.
What Are Common Size Units, and Where is the Nanoscale Relative to Them?
Table 1 below shows some common size units and their various notations (exponential,
number, English) and examples of objects that illustrate about how big each unit is.
Table 1. Common size units and examples.
Unit Magnitude as an
exponent (m)
Magnitude as a
number (m)
English
Expression
About how
big?
Meter 100 1 One A bit bigger
than a yardstick
Centimeter 10-2 0.01 One Hundredth Width of a
fingernail
Millimeter 10-3 0.001 One
Thousandth
Thickness of a
dime
Micrometer 10-6 0.000001 One Millionth A single cell
Nanometer 10-9 0.000000001 One Billionth 10 hydrogen
atoms lined up
Angstrom 10-10 0.0000000001 A large atom
Nanoscience is the study and development of materials and structures in the range of 1
nm (10-9 m) to 100 nanometers (100 x 10-9 = 10-7 m) and the unique properties that arise
at that scale. That is small! At the nanoscale, we are manipulating objects that are more
than one-millionth the size of the period at the end of this sentence.
What if We Measured the Size of Various Objects in Terms of Nanometers?
A typical atom is anywhere from 0.1 to 0.5 nanometers in diameter. DNA molecules are
about 2.5 nanometers wide. Most proteins are about 10 nanometers wide, and a typical
virus is about 100 nanometers wide. A bacterium is about 1000 nanometers. Human
cells, such as red blood cells, are about 10,000 nanometers across. At 100,000
nanometers, the width of a human hair seems gigantic. The head of a pin is about a
million nanometers wide. An adult man who is 2 meters tall (6 feet 5 inches) is about 2
billion nanometers tall!
2-S2
So is That What Nanoscience is All About––Smallness?
No, smallness alone doesn’t account for all the interest in the nanoscale. Nanoscale
structures push the envelope of physics, moving into the strange world of quantum
mechanics. For nanoparticles, gravity hardly matters due to their small mass. However,
the Brownian motion of these particles now becomes important. Nanosized particles of
any given substance exhibit differen ...
The building blocks_of_matter_-_atoms
Atoms are the smallest particles of matter that retain the chemical properties of an element. They are made up of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons orbit around the nucleus. The number of protons determines the element, while the number of neutrons determines the isotope. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Electromagnetic force attracts opposite charges, while strong force holds the nucleus together against electromagnetic repulsion between protons.
Basic-Atomic-Structure.9248797.powerpoint.pptx
This document summarizes early theories of atomic structure from the 5th century BC through the early 20th century. It discusses the Greek philosophers Leucippus and Democritus who proposed that matter is made of indivisible atoms. John Dalton's atomic theory from 1803 stated that matter is composed of atoms that combine in whole number ratios. Experiments by J.J. Thomson, Rutherford, and others led to the discoveries of subatomic particles like electrons and discovery of the nucleus. Rutherford's gold foil experiment showed that atoms have a small, dense positively charged nucleus occupying a tiny fraction of the atom's volume.
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.
Nuclear and Atomic Physics
Nuclear physics involves understanding atoms through experiments like Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus surrounded by empty space. Radiation like alpha, beta, and gamma rays is used in applications such as cancer treatment, electricity generation, and radiocarbon dating which relies on the radioactive decay of carbon-14 to determine the age of ancient materials.
Chapter 4 - The Atom
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.
Atomic Structure
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.
Chapter 3
The document discusses the history of atomic theory from ancient Greek philosophers to modern atomic structure. It introduces key figures like Democritus, Dalton, Thomson, and Rutherford and their contributions to understanding that all matter is made of tiny indivisible particles called atoms. The document also describes the discovery of subatomic particles like protons, neutrons, and electrons, and how electrons occupy distinct energy levels around the nucleus in an atom.
3.-Atoms-Molecules-and-Ions.pdf
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
Of Atoms and of Radioactivity
The document provides information about radioactivity and the structure of atoms. It discusses that atoms are made up of protons, neutrons and electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. It describes that there are three main types of radiation: alpha, beta and gamma. Alpha particles consist of two protons and two neutrons, beta particles are high speed electrons, and gamma radiation is a high energy wave. It explains that radioactive atoms are unstable and emit these types of radiation to become stable. Each type of radiation has different properties in terms of what they are made of, how far they can travel in air, and what can stop them. The document seeks to educate about radioactivity and radiation.
Atomic models Dr. vijender singh
The atomic model has changed significantly over time based on new evidence and experiments. Early philosophers proposed that atoms were indivisible spheres, while later scientists like Thomson and Rutherford provided evidence that atoms have internal structure, including a small, dense nucleus surrounded by electrons. The current wave model depicts electrons as existing in probabilistic electron clouds rather than definite orbits, representing our most accurate understanding of atomic structure to date.
Of Atoms and of Radioactivity
The document provides information about radioactivity and radiation. It begins by explaining the structure of atoms and the three main types of radiation: alpha, beta, and gamma. Alpha radiation is emitted as high-speed helium nuclei, beta as high-speed electrons, and gamma is a high-energy electromagnetic wave released after alpha or beta decay. It then discusses that radioactive atoms are unstable and emit radiation to become stable. The properties of the three types of radiation are explained, including what distance they can travel in air and what materials can stop them. Examples of radioactive materials and a quiz conclude the document.
The Atom
The document discusses the history and development of atomic theory from ancient Greek philosophers to modern atomic structure. Some key points covered include:
- Democritus first proposed the idea of atoms in ancient Greece but lacked evidence.
- In the 1800s, Dalton proposed his atomic theory that elements are made of atoms that combine in simple whole number ratios.
- Advances revealed atoms have internal structure including a tiny dense nucleus and orbiting electrons.
- Atoms are identified by their atomic number and mass number, which indicate protons, neutrons, and isotopes.
- The mole, molar mass, and Avogadro's number allow relating masses to numbers of atoms and particles.
Atomos
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
Atomos[1]
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's atomic theory of elements composed of atoms, J.J. Thomson's "plum pudding" model showing atoms contain smaller particles, Rutherford's gold foil experiment proving atoms have a small, dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus, and the modern wave model showing electrons as probability clouds rather than definite orbits.
Atomos
The document traces the development of atomic theory over time from ancient Greek philosophers to modern models. It describes Democritus' idea that matter is made of indivisible particles called "atomos", Dalton's model of atoms as indivisible spheres, Thomson's "plum pudding" model with electrons scattered in a positively charged substance, Rutherford's gold foil experiment showing atoms are mostly empty space with a dense nucleus, Bohr's model of electrons in specific energy levels orbiting the nucleus like planets, and the modern wave model where electrons exist as probability clouds rather than definite orbits.
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Lesson: Tuesday 9/1
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