The document discusses the structure of atoms. It explains that atoms have two main parts - a nucleus at the center made up of protons and neutrons, and electrons that orbit around the nucleus. The nucleus is positively charged due to the protons, while the electrons are negatively charged. Together, the positive and negative charges balance each other out, giving the overall atom a net neutral charge. Diagrams are provided showing different ways atoms can be drawn to represent these components.
All matter is made up of atoms, which are composed of subatomic particles including electrons, protons, and neutrons. Atoms are mostly empty space with a dense nucleus at the center containing protons and neutrons. Electrons orbit the nucleus in shells or orbitals. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Multiple atoms can bond together to form molecules or crystalline solids, and compounds are made of different types of atoms chemically bonded together.
This document provides an overview of the history and development of atomic structure theory. It discusses early Greek philosophers like Democritus who proposed that all matter is made of tiny indivisible particles called atoms. It then outlines key discoveries and models proposed by scientists like Lavoisier, Dalton, Thomson, Rutherford, Bohr, Schrodinger that helped develop our modern understanding of atomic structure. The basic structure of an atom is described including the subatomic particles (protons, neutrons, electrons), their properties, and location within the atom. The nucleus is identified as containing most of the atom's mass.
The document summarizes key developments in the atomic theory of matter:
1) Early Greek philosophers like Democritus proposed ideas of atoms as indivisible particles that make up all matter.
2) Scientists like Lavoisier, Dalton, and Thomson contributed experimental evidence and early atomic models, including Dalton's first modern atomic theory stating atoms are indestructible particles that combine in specific ratios.
3) Rutherford's gold foil experiment provided evidence that atoms are mostly empty space with a small, dense positively charged nucleus at the center, overturning the plum pudding model.
The document discusses the basic structure and composition of atoms. Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit around the nucleus. Though atoms are small, they are the fundamental unit that makes up all matter. The number of protons determines the element, while the number of neutrons can vary forming isotopes of that element. The periodic table organizes the known elements based on their chemical and physical properties.
Electricity and magnetism are explained through the movement of electrons. Atoms are made up of protons, neutrons, and electrons. Electrons can move along a wire due to positive and negative charges. Static electricity is created through friction that changes the number of electrons on objects. Magnets have magnetic fields and poles that attract or repel other magnets or metals. The Earth has a magnetic field created by its liquid iron core that protects us with its magnetosphere.
All isotopes of an element have the same number of protons. Isotopes are forms of an element that have different numbers of neutrons. Isotopes are named by writing the element name followed by the mass number, which is the number of protons plus neutrons. The average atomic mass shown for an element on the periodic table takes into account the relative abundance of all its isotopes.
What is Atom in Chemistry ?
Atom is basic building block of all matter.
Atom Have
1. Nucleus
Nucleus is very small and heavy part of the atom.
2. An Surrounding Electron Cloud
Surrounding electron cloud is large and lightweight part of the atom.
Nucleus of an Atom
Nucleus Contains
Protons
Protons have a positive charge.
All atoms are distinguished by the number of protons it has (atomic number).
Neutrons
Neutrons have no charge.
Neutrons have same mass as protons.
Electron Cloud of an Atom
An Electron Cloud of an Atom Contains
Electrons
Electron have a negative charge.
Electrons are contained within the shells of electron cloud.
Electrons have very small mass as compared to neutrons and protons.
Electron move in orbital motion around nucleus.
Electrons decides how bonds formed.
Atomic Structure
Atom is made up of Nucleus (Protons and Neutrons) and Electrons.
Prepared and Published by-
http://www.ChemistryNotesInfo.com
http://www.ChemistryNotesInfo.Blogspot.com
Read full article on what is Atom in chemistry at
https://chemistrynotesinfo.com/what-is-an-atom/
and view video of Atom at https://youtu.be/5Sdo7VKJ1uk
1) Bohr's atomic model successfully explained the hydrogen spectrum by postulating that electrons revolve in definite orbits called energy levels without radiating energy.
2) The radius, energy, and frequency of radiation emitted by electrons in different orbits were derived based on Bohr's model.
3) Bohr's model showed that electrons can jump between discrete energy levels, emitting or absorbing photons of specific frequencies corresponding to the energy differences between levels.
All matter is made up of atoms, which are composed of subatomic particles including electrons, protons, and neutrons. Atoms are mostly empty space with a dense nucleus at the center containing protons and neutrons. Electrons orbit the nucleus in shells or orbitals. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Multiple atoms can bond together to form molecules or crystalline solids, and compounds are made of different types of atoms chemically bonded together.
This document provides an overview of the history and development of atomic structure theory. It discusses early Greek philosophers like Democritus who proposed that all matter is made of tiny indivisible particles called atoms. It then outlines key discoveries and models proposed by scientists like Lavoisier, Dalton, Thomson, Rutherford, Bohr, Schrodinger that helped develop our modern understanding of atomic structure. The basic structure of an atom is described including the subatomic particles (protons, neutrons, electrons), their properties, and location within the atom. The nucleus is identified as containing most of the atom's mass.
The document summarizes key developments in the atomic theory of matter:
1) Early Greek philosophers like Democritus proposed ideas of atoms as indivisible particles that make up all matter.
2) Scientists like Lavoisier, Dalton, and Thomson contributed experimental evidence and early atomic models, including Dalton's first modern atomic theory stating atoms are indestructible particles that combine in specific ratios.
3) Rutherford's gold foil experiment provided evidence that atoms are mostly empty space with a small, dense positively charged nucleus at the center, overturning the plum pudding model.
The document discusses the basic structure and composition of atoms. Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit around the nucleus. Though atoms are small, they are the fundamental unit that makes up all matter. The number of protons determines the element, while the number of neutrons can vary forming isotopes of that element. The periodic table organizes the known elements based on their chemical and physical properties.
Electricity and magnetism are explained through the movement of electrons. Atoms are made up of protons, neutrons, and electrons. Electrons can move along a wire due to positive and negative charges. Static electricity is created through friction that changes the number of electrons on objects. Magnets have magnetic fields and poles that attract or repel other magnets or metals. The Earth has a magnetic field created by its liquid iron core that protects us with its magnetosphere.
All isotopes of an element have the same number of protons. Isotopes are forms of an element that have different numbers of neutrons. Isotopes are named by writing the element name followed by the mass number, which is the number of protons plus neutrons. The average atomic mass shown for an element on the periodic table takes into account the relative abundance of all its isotopes.
What is Atom in Chemistry ?
Atom is basic building block of all matter.
Atom Have
1. Nucleus
Nucleus is very small and heavy part of the atom.
2. An Surrounding Electron Cloud
Surrounding electron cloud is large and lightweight part of the atom.
Nucleus of an Atom
Nucleus Contains
Protons
Protons have a positive charge.
All atoms are distinguished by the number of protons it has (atomic number).
Neutrons
Neutrons have no charge.
Neutrons have same mass as protons.
Electron Cloud of an Atom
An Electron Cloud of an Atom Contains
Electrons
Electron have a negative charge.
Electrons are contained within the shells of electron cloud.
Electrons have very small mass as compared to neutrons and protons.
Electron move in orbital motion around nucleus.
Electrons decides how bonds formed.
Atomic Structure
Atom is made up of Nucleus (Protons and Neutrons) and Electrons.
Prepared and Published by-
http://www.ChemistryNotesInfo.com
http://www.ChemistryNotesInfo.Blogspot.com
Read full article on what is Atom in chemistry at
https://chemistrynotesinfo.com/what-is-an-atom/
and view video of Atom at https://youtu.be/5Sdo7VKJ1uk
1) Bohr's atomic model successfully explained the hydrogen spectrum by postulating that electrons revolve in definite orbits called energy levels without radiating energy.
2) The radius, energy, and frequency of radiation emitted by electrons in different orbits were derived based on Bohr's model.
3) Bohr's model showed that electrons can jump between discrete energy levels, emitting or absorbing photons of specific frequencies corresponding to the energy differences between levels.
This document discusses the development of atomic models from ancient Greek ideas to Rutherford's gold foil experiment and Bohr's model of the hydrogen atom. It introduces Dalton's atomic theory and developments like the plum pudding model, discovery of the electron, Rutherford's nuclear model, and Bohr's explanation of emission spectra. Key concepts covered include atomic structure, isotopes, atomic notation, and forces that hold the nucleus together.
The document discusses early theories of atoms and subatomic particles. It describes Dalton's atomic theory and discoveries by Thomson, Rutherford, and Millikan that led to the modern view of the atom. The atom is mostly empty space with a small, dense nucleus containing protons and neutrons. Radioactive decay occurs when unstable nuclei emit alpha, beta, or gamma radiation.
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) The document provides instructions and reminders for science class, including completing an atom booklet, turning in test corrections, and updating a log.
2) It reviews key people and theories in the development of atomic structure such as Dalton's atomic theory, Thomson's plum pudding model, Rutherford's gold foil experiment, and Bohr's planetary model.
3) It summarizes the basic atomic structure including the nucleus containing protons and neutrons, electrons orbiting in an electron cloud, and the properties and relative masses of protons, neutrons, and electrons.
- Atoms consist of a nucleus containing protons and neutrons surrounded by electrons in orbitals.
- The atomic number is the number of protons, which identifies the element. The mass number is the total number of protons and neutrons.
- Isotopes are atoms of the same element with different numbers of neutrons. The relative atomic mass takes into account the natural abundance of isotopes.
This chapter discusses atomic structure and is divided into four sections. Section 5.1 describes the components of an atom, including protons, neutrons, and electrons, and their relative masses and charges. Section 5.2 defines proton number and nucleon number, and how they relate to the number of protons, neutrons, and electrons in an atom. Section 5.3 explains that isotopes are atoms of the same element with different numbers of neutrons. Section 5.4 discusses how electrons are arranged in shells or energy levels around the atomic nucleus.
This document provides an overview of the history and development of atomic structure theories from ancient Greece to modern times. It discusses key contributors including:
- Democritus (400 BC) who first proposed the idea of atoms as tiny indivisible particles.
- Dalton (1817-1844) who developed the first modern atomic theory stating that all matter is composed of atoms that combine in specific ratios.
- Rutherford (1898) whose gold foil experiment showed that atoms are mostly empty space with a small, dense positively charged nucleus at the center.
- Bohr (1922) who proposed the planetary model of electrons orbiting the nucleus like planets around the sun.
- Schröding
The document discusses the atomic structure including protons, neutrons, and electrons. Protons and neutrons are found in the nucleus which contains over 99% of the atom's mass. Protons are positively charged while neutrons are neutral. Electrons are negatively charged and orbit the nucleus, balancing out the positive charge of the protons to give atoms a net neutral charge.
The document summarizes key developments in the atomic theory model over time from ancient Greece to the 20th century. It discusses early ideas from Democritus and Dalton's first atomic theory. Major discoveries include Thomson discovering the electron and proposing the plum pudding model, Rutherford using the gold foil experiment to show the atom's structure with a dense nucleus, and Bohr introducing the planetary atomic model. Later, Schrodinger introduced the wave mechanic model and quantum theory. The basic atomic structure is then explained, identifying the subatomic particles - protons, neutrons, and electrons - and their properties. Key terms like atomic number, isotopes, and ions are also defined.
This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons surround the nucleus in energy levels. The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Standard atomic notation uses the mass number as a superscript on the left of the element symbol and the atomic number as a subscript.
This document provides an overview of atoms and atomic structure through a self-guided computer activity. It discusses the atomic-molecular theory of matter and how scientists have gathered indirect evidence to develop models of atoms. It describes the subatomic particles that make up atoms, including protons, neutrons, and electrons. Atoms are electrically neutral due to having equal numbers of protons and electrons. The activity guides students to learn about atomic structure by visiting websites and completing a study guide.
This document provides information about atomic structure, including the three main subatomic particles - protons, neutrons, and electrons. It discusses the key properties of each particle, including their location within the atom, mass, and electrical charge. Protons determine the element and have a positive charge. Neutrons are neutral and have a similar mass to protons. The number of protons and neutrons gives an atom its identity and mass number.
This document provides information about atomic structure and the history of atomic theory. It discusses early Greek philosophers' ideas of atoms, followed by key scientists and their experiments and models that advanced our understanding:
1) Dalton established the first modern atomic theory, proposing that all matter is made of tiny indivisible particles called atoms.
2) Rutherford's gold foil experiment showed that the mass of an atom is concentrated in a small, positively charged nucleus at the center.
3) Bohr incorporated Rutherford's findings into his planetary model of electrons orbiting the nucleus.
4) Schrödinger introduced the wave mechanical model where electrons vibrate around the nucleus rather than following precise orbits.
This document provides an overview of atomic structure and the periodic table. It discusses how atoms are mostly empty space, with a dense nucleus surrounded by electrons. Electrons can exist in different energy levels around the nucleus. The periodic table is organized into periods and groups based on atomic structure. Elements in the same group have similar properties due to their outer electron configuration. Noble gases are very stable as their outer energy level is complete.
The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
The document discusses the periodic table and classification of elements. It explains that (1) elements are arranged in the periodic table based on their atomic structure and chemical properties, which repeat periodically. (2) Each element is identified by its atomic number and atomic mass. (3) Elements are classified as metals, nonmetals, and metalloids based on their location in the periodic table and tendency to gain or lose electrons.
Here are the steps:
1. Write the positive ion
2. Write the negative ion
3. The formula shows the charges are balanced by having the same number of each ion.
4. For -ides the negative ion ends in ide e.g. Cl-, S2-
5. For -ates the negative ion ends in -ate or -ite and has O in it e.g. CO32-, SO42-
Now you try:
+ ion - ion Formula + ion - ron Formula
Na+ CO3z- Na2C03 Fez+ SO4z- FeSO4
+ ion -
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.
Empathy map #1 Redesigning the school to work transitionCíntia Citton
Go to school, get your degree, get a job. Does this traditional path from education to employment make sense today for
the hundreds of millions of learners around the world? Let's find out using the design thinking process.
Weight training can increase metabolism by building muscle mass. Muscle tissue burns more calories than fat tissue, so even small increases in muscle from weight training can boost metabolism long-term. Building more muscle through weight training raises the body's resting metabolism, causing it to burn more calories regularly.
The document summarizes the agenda for the Oracle Hyderabad Toastmasters Meeting #9. The theme was "Boss is ALWAYS Right". It includes the word and idiom of the day, list of speakers and evaluators, and ground rules for the meeting emphasizing that the theme is meant in fun and the Toastmaster of the Day is in charge of the meeting.
This document discusses the development of atomic models from ancient Greek ideas to Rutherford's gold foil experiment and Bohr's model of the hydrogen atom. It introduces Dalton's atomic theory and developments like the plum pudding model, discovery of the electron, Rutherford's nuclear model, and Bohr's explanation of emission spectra. Key concepts covered include atomic structure, isotopes, atomic notation, and forces that hold the nucleus together.
The document discusses early theories of atoms and subatomic particles. It describes Dalton's atomic theory and discoveries by Thomson, Rutherford, and Millikan that led to the modern view of the atom. The atom is mostly empty space with a small, dense nucleus containing protons and neutrons. Radioactive decay occurs when unstable nuclei emit alpha, beta, or gamma radiation.
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) The document provides instructions and reminders for science class, including completing an atom booklet, turning in test corrections, and updating a log.
2) It reviews key people and theories in the development of atomic structure such as Dalton's atomic theory, Thomson's plum pudding model, Rutherford's gold foil experiment, and Bohr's planetary model.
3) It summarizes the basic atomic structure including the nucleus containing protons and neutrons, electrons orbiting in an electron cloud, and the properties and relative masses of protons, neutrons, and electrons.
- Atoms consist of a nucleus containing protons and neutrons surrounded by electrons in orbitals.
- The atomic number is the number of protons, which identifies the element. The mass number is the total number of protons and neutrons.
- Isotopes are atoms of the same element with different numbers of neutrons. The relative atomic mass takes into account the natural abundance of isotopes.
This chapter discusses atomic structure and is divided into four sections. Section 5.1 describes the components of an atom, including protons, neutrons, and electrons, and their relative masses and charges. Section 5.2 defines proton number and nucleon number, and how they relate to the number of protons, neutrons, and electrons in an atom. Section 5.3 explains that isotopes are atoms of the same element with different numbers of neutrons. Section 5.4 discusses how electrons are arranged in shells or energy levels around the atomic nucleus.
This document provides an overview of the history and development of atomic structure theories from ancient Greece to modern times. It discusses key contributors including:
- Democritus (400 BC) who first proposed the idea of atoms as tiny indivisible particles.
- Dalton (1817-1844) who developed the first modern atomic theory stating that all matter is composed of atoms that combine in specific ratios.
- Rutherford (1898) whose gold foil experiment showed that atoms are mostly empty space with a small, dense positively charged nucleus at the center.
- Bohr (1922) who proposed the planetary model of electrons orbiting the nucleus like planets around the sun.
- Schröding
The document discusses the atomic structure including protons, neutrons, and electrons. Protons and neutrons are found in the nucleus which contains over 99% of the atom's mass. Protons are positively charged while neutrons are neutral. Electrons are negatively charged and orbit the nucleus, balancing out the positive charge of the protons to give atoms a net neutral charge.
The document summarizes key developments in the atomic theory model over time from ancient Greece to the 20th century. It discusses early ideas from Democritus and Dalton's first atomic theory. Major discoveries include Thomson discovering the electron and proposing the plum pudding model, Rutherford using the gold foil experiment to show the atom's structure with a dense nucleus, and Bohr introducing the planetary atomic model. Later, Schrodinger introduced the wave mechanic model and quantum theory. The basic atomic structure is then explained, identifying the subatomic particles - protons, neutrons, and electrons - and their properties. Key terms like atomic number, isotopes, and ions are also defined.
This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons surround the nucleus in energy levels. The number of protons determines the element and is known as the atomic number. The total number of protons and neutrons is the mass number. Standard atomic notation uses the mass number as a superscript on the left of the element symbol and the atomic number as a subscript.
This document provides an overview of atoms and atomic structure through a self-guided computer activity. It discusses the atomic-molecular theory of matter and how scientists have gathered indirect evidence to develop models of atoms. It describes the subatomic particles that make up atoms, including protons, neutrons, and electrons. Atoms are electrically neutral due to having equal numbers of protons and electrons. The activity guides students to learn about atomic structure by visiting websites and completing a study guide.
This document provides information about atomic structure, including the three main subatomic particles - protons, neutrons, and electrons. It discusses the key properties of each particle, including their location within the atom, mass, and electrical charge. Protons determine the element and have a positive charge. Neutrons are neutral and have a similar mass to protons. The number of protons and neutrons gives an atom its identity and mass number.
This document provides information about atomic structure and the history of atomic theory. It discusses early Greek philosophers' ideas of atoms, followed by key scientists and their experiments and models that advanced our understanding:
1) Dalton established the first modern atomic theory, proposing that all matter is made of tiny indivisible particles called atoms.
2) Rutherford's gold foil experiment showed that the mass of an atom is concentrated in a small, positively charged nucleus at the center.
3) Bohr incorporated Rutherford's findings into his planetary model of electrons orbiting the nucleus.
4) Schrödinger introduced the wave mechanical model where electrons vibrate around the nucleus rather than following precise orbits.
This document provides an overview of atomic structure and the periodic table. It discusses how atoms are mostly empty space, with a dense nucleus surrounded by electrons. Electrons can exist in different energy levels around the nucleus. The periodic table is organized into periods and groups based on atomic structure. Elements in the same group have similar properties due to their outer electron configuration. Noble gases are very stable as their outer energy level is complete.
The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
The document discusses the periodic table and classification of elements. It explains that (1) elements are arranged in the periodic table based on their atomic structure and chemical properties, which repeat periodically. (2) Each element is identified by its atomic number and atomic mass. (3) Elements are classified as metals, nonmetals, and metalloids based on their location in the periodic table and tendency to gain or lose electrons.
Here are the steps:
1. Write the positive ion
2. Write the negative ion
3. The formula shows the charges are balanced by having the same number of each ion.
4. For -ides the negative ion ends in ide e.g. Cl-, S2-
5. For -ates the negative ion ends in -ate or -ite and has O in it e.g. CO32-, SO42-
Now you try:
+ ion - ion Formula + ion - ron Formula
Na+ CO3z- Na2C03 Fez+ SO4z- FeSO4
+ ion -
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.
Empathy map #1 Redesigning the school to work transitionCíntia Citton
Go to school, get your degree, get a job. Does this traditional path from education to employment make sense today for
the hundreds of millions of learners around the world? Let's find out using the design thinking process.
Weight training can increase metabolism by building muscle mass. Muscle tissue burns more calories than fat tissue, so even small increases in muscle from weight training can boost metabolism long-term. Building more muscle through weight training raises the body's resting metabolism, causing it to burn more calories regularly.
The document summarizes the agenda for the Oracle Hyderabad Toastmasters Meeting #9. The theme was "Boss is ALWAYS Right". It includes the word and idiom of the day, list of speakers and evaluators, and ground rules for the meeting emphasizing that the theme is meant in fun and the Toastmaster of the Day is in charge of the meeting.
To lose 1 pound, a 34 year old 155 pound mom would need to wash cars for 11 hours or iron for over 22 hours. Alternatively, she could avoid eating 14 bagels with cream cheese per week. Generally, to lose 1 pound per week a person must burn an extra 500 calories daily through exercise, eating less, or a combination of both methods.
This document outlines the process for conducting customer satisfaction surveys through questionnaires. It discusses three types of questionnaires, rules for launching a questionnaire including identifying objectives, target markets and developing questions. It also covers determining sample sizes, distribution methods, collecting responses, sorting answers and reporting conclusions. The goal is to gather customer feedback to identify areas for improvement and inform initiatives to enhance customer satisfaction and relationships.
Facebook provides tools and guidance for event organizers to promote their events on Facebook. The document outlines how to create high-quality Facebook events with optimized details like photos, names and descriptions. It also explains how to spread event awareness through sharing, invites, calendars and ads. Facebook events can be promoted to drive responses, ticket sales and reach through audience targeting.
7 c environment and feeding relationshipscpugh5345
This document discusses relationships between organisms and their environment. It explains how organisms are adapted to their habitats and how animals adapt to seasonal changes through processes like hibernation, migration, growing thicker fur. It also discusses predators and prey, including features of each. Food chains and webs are explained as the transfer of energy from producers to primary, secondary and tertiary consumers. The impacts of removing organisms from these chains and webs is also examined.
Electricity is related to the structure and properties of atoms. Atoms are the smallest particle that matter can be divided into, consisting of a nucleus with positively charged protons and neutral neutrons surrounded by negatively charged electrons in energy levels. The attraction between the positive nucleus and negative electrons holds the atom together in a neutral state. Static electricity and lightning occur when an imbalance of charges develops, such as rubbing objects together to transfer electrons or friction separating charges within storm clouds.
Lecture 1 medical Chemistry.pptxxfjxfjfjcfSriRam071
This document provides an overview of the topics covered in the first lecture of a Medical Chemistry course. The lecture introduced the electronic structure of atoms, including the dual nature of electrons and quantum mechanical descriptions of hydrogen atoms. It also covered quantum numbers, atomic orbitals, electron configuration, and shielding effects in multi-electron atoms. The accompanying seminar discussed principal, angular momentum, magnetic, and electron spin quantum numbers as well as s, p, d, and f orbitals and their energies.
The document discusses atomic models and nuclear physics. It provides information on:
1) Early atomic models including Dalton's billiard ball model, Thomson's plum pudding model, Rutherford's nuclear model, and Bohr's planetary model.
2) Experiments that led to discoveries about the structure of the atom including Thomson's cathode ray tube experiment, Rutherford's gold foil experiment, and Bohr's model of electron orbits.
3) Components of the nucleus including protons, neutrons, and isotopes.
4) Types of radiation including alpha, beta, gamma particles and their properties such as mass, charge, penetration and ionization.
5) Experiments that helped discover radiation and nuclear decay processes.
BE UNIT-1 basic electronics unit one.pptxharisbs369
1. The document discusses the atomic structure of matter, which is made up of protons, electrons, and neutrons. Atoms contain protons and neutrons in their nucleus, surrounded by electrons.
2. Atoms of different elements have different atomic structures because they contain different numbers of protons and electrons. Neutral atoms have equal numbers of protons and electrons, but atoms can gain or lose electrons to become ions.
3. The document then discusses subatomic particles like protons, neutrons, and electrons in more detail, including their relative masses and charges. It also discusses isotopes and how they have the same number of protons but different numbers of neutrons.
This document defines static electricity and electric charges. It explains that atoms become charged when they gain or lose electrons, making them more positive or negative. Electrons can be easily removed from atoms, while protons are very difficult to remove. Charging occurs through friction, contact, or induction as electrons are transferred between objects. Conductors allow charge to spread evenly, while insulators trap charges on their surface. Grounding neutralizes charged objects by allowing electrons to flow to or from the earth.
This represents two isotopes of carbon:
1. Carbon-12: Has 6 protons and 6 neutrons. Neutral charge.
2. Carbon-13: Has 6 protons and 7 neutrons. Also neutral charge.
Carbon-13 is a stable isotope of carbon. The increased neutron number makes it an isotope. Both have 6 protons so they are the element carbon.
This document provides an overview of basic chemistry concepts. It explains that all matter is made up of atoms, and atoms can combine to form either elements or compounds. The structure of the atom is described, including subatomic particles like protons, neutrons, and electrons. Electron configuration and chemical bonding via ionic and covalent bonds are also summarized. Key terms like isotopes, ions, the periodic table, and electronegativity are defined.
Contents
The Atom
Materials Used in Electronics
Current in Semiconductors
N-Type and P-Type Semiconductors
The PN Junctions
Diode Operation, Voltage-Current (V-I) Characteristics
Bipolar Junction Transistor (BJT) Structure, Operation, and Characteristics and Parameters
Junction Field Effect Transistors (JFETs) Structure, Characteristics and Parameters and Biasing
Metal Oxide Semiconductor FET (MOSFET) Structure, Characteristics and Parameters and Biasing
The ATOM: Learning Objectives
Describe the structure of an atom
Discuss the Bohr model of an atom
Define electron, proton, neutron, and nucleus
Define atomic number
Discuss electron shells and orbits
Explain energy levels
Define valence electron
Discuss ionization
Define free electron and ion
Discuss the basic concept of the quantum model of the atom
Discuss insulators, conductors, and semiconductors and how they differ
Define the core of an atom
Describe the carbon atom
Name two types each of semiconductors, conductors, and insulators
Explain the band gap
Define valence band and conduction band
Compare a semiconductor atom to a conductor atom
Discuss silicon and germanium atoms
Explain covalent bonds
Define crystal
Describe how current is produced in a semiconductor
Discuss conduction electrons and holes
Explain an electron-hole pair
Discuss recombination
Explain electron and hole current
Describe the properties of n-type and p-type semiconductors
Define doping
Explain how n-type semiconductors are formed
Describe a majority carrier and minority carrier in n-type material
Explain how p-type semiconductors are formed
Describe a majority carrier and minority carrier in p-type material
Describe how a pn junction is formed
Discuss diffusion across a pn junction
Explain the formation of the depletion region
Define barrier potential and discuss its significance
State the values of barrier potential in silicon and germanium
Discuss energy diagrams
Define energy hill
This document summarizes atomic structure and isotopes. It defines protons, neutrons, and electrons, and describes their relative masses and charges. It explains that the nucleus contains protons and neutrons, which make up most of an atom's mass. The document also discusses how subatomic particles behave in electric fields based on their charge. It defines nucleon number and proton number, and how they relate to the composition of atoms and ions. Finally, it defines isotopes as atoms of the same element with different numbers of neutrons, and notes they have similar chemical properties but different physical properties like mass.
The document provides instructions for students, including scheduling a test retake, collecting parent signatures on corrected tests, and completing assignments on atomic structure models and Lewis dot diagrams. Students are also assigned jobs like materials manager and oral presenter for an upcoming lesson. The document quizzes students on electron configuration, ionic and covalent bonding, and using the periodic table to draw Bohr models and Lewis dot diagrams.
The document discusses basic electrical circuit theory and components. It explains that atoms are composed of protons, neutrons, and electrons. Protons determine elemental identity, neutrons determine mass, and electrons allow for attraction. A circuit is formed when a closed conducting loop allows electrons to flow from the negative terminal of a battery or other power source back to the positive terminal. Key requirements for a circuit include a closed conducting path and connections made only of conductive materials capable of carrying electric charge. Current occurs as electrons bump from atom to atom along a conductor within the circuit.
Electronics I SEMI-CONDUCTOR THEORY0.pptSphumzo2012
This chapter introduces the physics behind semiconductor devices. It discusses how quantum physics led to new understandings of atomic structure that contradicted earlier classical models. In particular, it describes Niels Bohr's planetary model of the atom and introduces concepts like atomic number, valence, free electrons, energy levels, and the distinction between conductors, semiconductors, and insulators based on their band gaps. The chapter lays the groundwork for understanding how semiconductor devices function by explaining these foundational quantum physics principles.
All matter is composed of atoms. Atoms are composed of protons, neutrons, and electrons. Rutherford's gold foil experiment disproved the plum pudding model of the atom and led to the discovery of the nuclear atom, with a small, dense nucleus surrounded by electrons. Niels Bohr refined this model by suggesting that electrons orbit the nucleus in discrete energy levels. When electrons change orbits, electromagnetic radiation is emitted or absorbed at wavelengths specific to each element.
This document provides an overview of key concepts related to the chemical basis of life, including:
1) Elements are the fundamental forms of matter that cannot be broken down further through normal means. The most common elements in the human body are oxygen, hydrogen, carbon, nitrogen, and calcium.
2) Atoms are made up of subatomic particles including protons, neutrons, and electrons. The number of protons determines the element, while the number of neutrons can vary between isotopes of the same element.
3) Electrons play an important role in how atoms interact, forming ions by gaining or losing electrons or bonding through electron sharing. The organization of the periodic table is based on electron configurations.
Atomic Structure Powerpoint Presentation by Computer CareersYaman Singhania
Powerpoint Presentation on Atomic Structure by Computer Careers.What is an Atom?ATOMIC STRUCTURE,There are two ways to represent the atomic structure of n element or compound,DOT & CROSS DIAGRAMS and many more ....
This document provides information about atomic structure. It discusses the basic parts of an atom including protons, neutrons, and electrons. Early atomic models proposed by Rutherford and Bohr are described, noting their limitations in explaining experimental observations. The modern quantum mechanical model represents electrons using quantum numbers and wave functions or "fuzzy clouds" to describe atomic orbitals. Electrons occupy different energy levels and sublevels based on their quantum numbers.
This document discusses various topics in electrostatics including:
1) Electric charge can be positive or negative and like charges repel while unlike charges attract.
2) Charge is conserved meaning the total amount of charge in a system remains constant during interactions and transformations.
3) The coulomb is the SI unit for electric charge and small amounts are measured in microcoulombs. The elementary charge is the smallest unit of charge possible.
4) Materials can be conductors, insulators or semiconductors depending on how freely charge can flow through them.
1) The document provides reminders and information about upcoming assignments in science class, including corrections for Test #2 that are due today and signed by parents.
2) It summarizes key concepts from the Bohr and Schrodinger atomic models, including that Bohr believed electrons orbited the nucleus in fixed orbits like planets around the sun, while Schrodinger proposed that electrons vibrate around the nucleus and can only predict where they are most likely to be found.
3) The document reviews basic atomic structure, isotopes including examples for hydrogen, and how to identify metals, nonmetals and metalloids on the periodic table based on their location in the boxes.
Here are the answers:
1. Aluminum
2. Helium
3. Palladium
4. Gold
5. Oxygen
6. Calcium has 20 protons
7. Silver has 47 protons
8. Neon has 10 protons
9. Potassium has 19 protons
10. Iron has 26 protons
11. Nitrogen has 7 protons in its nucleus.
Here are the answers:
1. Aluminum
2. Helium
3. Palladium
4. Gold
5. Oxygen
6. Calcium has 20 protons
7. Silver has 47 protons
8. Neon has 10 protons
9. Potassium has 19 protons
10. Iron has 26 protons
11. (Draws a picture of a nitrogen nucleus with 7 protons)
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...indexPub
The recent surge in pro-Palestine student activism has prompted significant responses from universities, ranging from negotiations and divestment commitments to increased transparency about investments in companies supporting the war on Gaza. This activism has led to the cessation of student encampments but also highlighted the substantial sacrifices made by students, including academic disruptions and personal risks. The primary drivers of these protests are poor university administration, lack of transparency, and inadequate communication between officials and students. This study examines the profound emotional, psychological, and professional impacts on students engaged in pro-Palestine protests, focusing on Generation Z's (Gen-Z) activism dynamics. This paper explores the significant sacrifices made by these students and even the professors supporting the pro-Palestine movement, with a focus on recent global movements. Through an in-depth analysis of printed and electronic media, the study examines the impacts of these sacrifices on the academic and personal lives of those involved. The paper highlights examples from various universities, demonstrating student activism's long-term and short-term effects, including disciplinary actions, social backlash, and career implications. The researchers also explore the broader implications of student sacrifices. The findings reveal that these sacrifices are driven by a profound commitment to justice and human rights, and are influenced by the increasing availability of information, peer interactions, and personal convictions. The study also discusses the broader implications of this activism, comparing it to historical precedents and assessing its potential to influence policy and public opinion. The emotional and psychological toll on student activists is significant, but their sense of purpose and community support mitigates some of these challenges. However, the researchers call for acknowledging the broader Impact of these sacrifices on the future global movement of FreePalestine.
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...EduSkills OECD
Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
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
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.)
4. ATOM Overview
Review: What are the 3
kinds of matter?
Atoms = Small pieces
that make up matter http://www.fotosearch.com/photos-images/atom.html
5. ATOM Overview
Review: What are the 3
kinds of matter?
Atoms = Small pieces
that make up matter http://www.fotosearch.com/photos-images/atom.html
Have two parts
6. ATOM Overview
Review: What are the 3
kinds of matter?
Atoms = Small pieces
that make up matter http://www.fotosearch.com/photos-images/atom.html
Have two parts
The nucleus
7. ATOM Overview
Review: What are the 3
kinds of matter?
Atoms = Small pieces
that make up matter http://www.fotosearch.com/photos-images/atom.html
Have two parts
The nucleus
The electron cloud
8. Parts of an Atom
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
9. Parts of an Atom
Nucleus:
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
10. Parts of an Atom
Nucleus:
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
11. Parts of an Atom
Nucleus:
A center with a
positive charge
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
12. Parts of an Atom
Nucleus:
A center with a
positive charge +
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
13. Parts of an Atom
Electron Cloud:
Nucleus:
A center with a
positive charge +
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
14. Parts of an Atom
Electron Cloud:
Nucleus:
A center with a
positive charge +
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
15. Parts of an Atom
Electron Cloud:
Nucleus: Cloud of
Electrons that
A center with a have a negative
positive charge + charge
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
16. Parts of an Atom
Electron Cloud:
Nucleus: Cloud of
- Electrons that
A center with a have a negative
positive charge + charge
http://www.estrellamountain.edu/faculty/farabee/biobk/BioBookCHEM1.html
17. Confused about Charge?
•Atoms are like batteries they have
zero total charge.
•Think about charges on an atom
like charges on a battery!
On one end there is a positive (+)
charge on the other a negative (-)
charge, but the whole battery has www.diytrade.com/china/4/products/2196408/Pan...
zero charge because they balance
out.
18. A Closer Look at the Nucleus
•2 particles
http://www.fotosearch.com/photos-images/atom.html
19. A Closer Look at the Nucleus
•2 particles
Proton (p+): a positive
particle; weight 1
http://www.fotosearch.com/photos-images/atom.html
20. A Closer Look at the Nucleus
•2 particles
Proton (p+): a positive
particle; weight 1
http://www.fotosearch.com/photos-images/atom.html
21. A Closer Look at the Nucleus
•2 particles
Proton (p+): a positive
particle; weight 1
http://www.fotosearch.com/photos-images/atom.html
•Neutron (n): a neutral
particle, weight 1
22. A Closer Look at the Nucleus
•2 particles
Proton (p+): a positive
particle; weight 1
http://www.fotosearch.com/photos-images/atom.html
•Neutron (n): a neutral
particle, weight 1
31. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons?
32. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons?
• What is the weight of an atom with 5 protons, 5
neutrons, and 5 electrons?
33. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons?
• What is the weight of an atom with 5 protons, 5
neutrons, and 5 electrons?
•What is the charge of an atom with 9 protons, 9
neutrons, and 9 electrons?
34. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons? +2
• What is the weight of an atom with 5 protons, 5
neutrons, and 5 electrons?
•What is the charge of an atom with 9 protons, 9
neutrons, and 9 electrons?
35. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons? +2
• What is the weight of an atom with 5 protons, 5
neutrons, and 5 electrons? 10
•What is the charge of an atom with 9 protons, 9
neutrons, and 9 electrons?
36. Atomic Weight and Charge Practice Problems
•What is the charge of an atom that has 2 protons
and 2 neutrons? +2
• What is the weight of an atom with 5 protons, 5
neutrons, and 5 electrons? 10
•What is the charge of an atom with 9 protons, 9
neutrons, and 9 electrons? 0
37. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
38. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
39. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
40. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
41. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
42. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
43. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
44. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
45. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
46. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
47. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
48. Ways of drawing atoms
Even though
drawings are
different
represent same
things!!
Nucleus
Electrons
Orbitals
49. A Closer Look at the Electron Cloud
*Fill orbitals from inside to out
*Orbital 3 also holds 8
50. A Closer Look at the Electron Cloud
*Fill orbitals from inside to out
*Orbital 3 also holds 8
51. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
*Fill orbitals from inside to out
*Orbital 3 also holds 8
52. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
53. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1:
Can carry up to
2 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
54. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1:
Can carry up to
2 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
55. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1:
Can carry up to
2 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
56. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1: Orbital 2:
Can carry up to can carry up
2 electrons to 8 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
57. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1: Orbital 2:
Can carry up to can carry up
2 electrons to 8 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
58. A Closer Look at the Electron Cloud
•Electrons travel in orbitals
•Orbitals (circles around nucleus) can carry different
amount of electrons
Orbital 1: Orbital 2:
Can carry up to can carry up
2 electrons to 8 electrons
*Fill orbitals from inside to out
*Orbital 3 also holds 8
59. What is an element?
Atoms come in different types (because the
number of protons, neutrons, and electrons
change)
element- a substance that cannot be
broken down chemically and all atoms in it
are the same
Examples : Copper, Oxygen, Hydrogen