Periodic Trends
•Download as PPT, PDF•
3 likes•737 views
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity. 2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right. 3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Report
Share
Report
Share
![Periodic Law ,[object Object]](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
Recommended
CHM 101OL - Lecture
This document discusses periodic trends, including how atomic and ionic size, ionization energy, and electron affinity vary across the periodic table. It explains that atomic size increases down a group as more electron shells are added, but increases across a period from left to right as the nuclear charge felt by valence electrons increases. Ionization energy and electron affinity also increase as atomic size decreases, as it is harder to remove or add electrons to smaller atoms. The octet rule is introduced, where main group elements seek to obtain full s and p subshells of eight electrons to achieve stable electronic configurations.
Ionization energy
Ionization energy is the minimum amount of energy required to remove an electron from an atom or ion. It increases with each successive ionization as the electron removed is closer to the nucleus. Generally, first ionization energy increases from left to right across a period as atomic radius decreases, making electrons more tightly bound. It decreases from top to bottom in a group as atomic radius increases, meaning electrons are farther from the nucleus. The second ionization energy is always higher than the first as removal of the second electron requires overcoming a stronger force of attraction to the positively charged ion.
Ionization energy
- Ionization energy is the amount of energy required to remove an electron from an atom. The first ionization energy is the amount required to remove the outermost electron.
- More energy is required to remove the second electron compared to the first, and even more for the third electron.
- Ionization energy decreases down a group as the atomic number increases since electrons are farther from the nucleus and more shielded.
- There is a general trend of increasing ionization energy when moving left to right across a period as protons are added making electrons more tightly bound.
Periodic trends
Here are the answers to your questions:
1. Shielding of nuclear charge remains constant as you move across a period or down a group since the number of electron shells remains the same.
2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
Periodic trends cca
This document discusses trends in atomic properties across the periodic table, including atomic radius, ionization energy, and electronegativity. It explains that atomic radius generally increases down groups and decreases across periods. Ionization energy follows the opposite trend, increasing across periods as the number of protons increases but decreasing down groups. Electronegativity tends to decrease down groups but increase left to right across periods, with metals having low values and nonmetals having high values.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
Periodic trends
This document defines and discusses several periodic properties including atomic and ionic radii, ionization energy, electron affinity, and electronegativity. It states that atomic radii decrease across a period and increase down a group due to the increasing nuclear charge and electron cloud size. Ionization energies increase across a period as it is harder to remove electrons that are closer to the nucleus, and decrease down a group as the electrons are farther away. Electron affinity and electronegativity generally increase across periods and decrease down groups due to the effective nuclear charge and electron distance from the nucleus. Valence electrons are the outermost electrons involved in bonding, with atoms seeking to obtain a full outer shell of 8 electrons.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
Recommended
CHM 101OL - Lecture
This document discusses periodic trends, including how atomic and ionic size, ionization energy, and electron affinity vary across the periodic table. It explains that atomic size increases down a group as more electron shells are added, but increases across a period from left to right as the nuclear charge felt by valence electrons increases. Ionization energy and electron affinity also increase as atomic size decreases, as it is harder to remove or add electrons to smaller atoms. The octet rule is introduced, where main group elements seek to obtain full s and p subshells of eight electrons to achieve stable electronic configurations.
Ionization energy
Ionization energy is the minimum amount of energy required to remove an electron from an atom or ion. It increases with each successive ionization as the electron removed is closer to the nucleus. Generally, first ionization energy increases from left to right across a period as atomic radius decreases, making electrons more tightly bound. It decreases from top to bottom in a group as atomic radius increases, meaning electrons are farther from the nucleus. The second ionization energy is always higher than the first as removal of the second electron requires overcoming a stronger force of attraction to the positively charged ion.
Ionization energy
- Ionization energy is the amount of energy required to remove an electron from an atom. The first ionization energy is the amount required to remove the outermost electron.
- More energy is required to remove the second electron compared to the first, and even more for the third electron.
- Ionization energy decreases down a group as the atomic number increases since electrons are farther from the nucleus and more shielded.
- There is a general trend of increasing ionization energy when moving left to right across a period as protons are added making electrons more tightly bound.
Periodic trends
Here are the answers to your questions:
1. Shielding of nuclear charge remains constant as you move across a period or down a group since the number of electron shells remains the same.
2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
Periodic trends cca
This document discusses trends in atomic properties across the periodic table, including atomic radius, ionization energy, and electronegativity. It explains that atomic radius generally increases down groups and decreases across periods. Ionization energy follows the opposite trend, increasing across periods as the number of protons increases but decreasing down groups. Electronegativity tends to decrease down groups but increase left to right across periods, with metals having low values and nonmetals having high values.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
Periodic trends
This document defines and discusses several periodic properties including atomic and ionic radii, ionization energy, electron affinity, and electronegativity. It states that atomic radii decrease across a period and increase down a group due to the increasing nuclear charge and electron cloud size. Ionization energies increase across a period as it is harder to remove electrons that are closer to the nucleus, and decrease down a group as the electrons are farther away. Electron affinity and electronegativity generally increase across periods and decrease down groups due to the effective nuclear charge and electron distance from the nucleus. Valence electrons are the outermost electrons involved in bonding, with atoms seeking to obtain a full outer shell of 8 electrons.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
The periodic table & periodic law
The document summarizes the development and key features of the periodic table. It discusses how early chemists like Newlands, Meyer, and Mendeleev arranged elements in order of atomic mass and properties, recognizing repeating patterns. Mendeleev predicted new elements and Moseley later arranged elements by atomic number. The periodic table is organized into blocks by electron configuration and periods and groups that demonstrate trends in properties. Metals are on the left, nonmetals on the right, and metalloids border the stair-step line between them.
Periodic trends
The document discusses periodic trends in elemental properties. It explains that Dmitri Mendeleev was the first to organize elements in a periodic table based on their properties. Elements in the same group have similar properties due to their valence electrons. Atomic radius generally decreases moving left to right across a period and increases moving down a group due to electron shielding. Ionization energy increases as atomic radius decreases. Electron affinity is exothermic when gaining electrons fills an orbital. Metallic character decreases and electronegativity increases moving from left to right. Cations are smaller than their parent atoms while anions are larger.
Trends in the periodic table
Specifically designed for Leaving Cert Chemistry students. A simplified explanation of all the trends in the periodic Table. It includes details such as atomic radius, electronegativity and ionisation energy
periodic table trends
The Periodic Table and Periodic Law SECTION 3 Periodic Trends
ionization energy
atomic radius
electronegativity
Periodic trends
The document discusses periodic trends in atomic properties according to the periodic table. It explains that atomic radius decreases across a period as effective nuclear charge increases due to shielding effects, while radius increases down a group as each row adds a new shell. Ionization energy tends to increase across a period as removal of electrons becomes more difficult, and decreases down a group as outer electrons are farther from the nucleus. Electronegativity also increases across a period but decreases or stays the same down a group as distance from the nucleus increases. Positively charged cations are smaller than their parent atoms, while negatively charged anions are larger.
Trends of periodic atomic properties
1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
3) Electronegativity increases across a period for the same reasons as ionization energy, and decreases down a group as shielding increases and attraction decreases.
Presentation of periodic trends - STAGE 3
Periodic trends are patterns in the periodic table that illustrate properties of elements, including size and those relating to electrons. The main periodic trends are electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. These trends show how each property changes when moving left to right within a period or up and down within a group. For example, electronegativity increases left to right within a period but decreases up and down within a group. The document then discusses each trend in more detail and provides examples.
Periodic trends lecture notes a.k
The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
[2] Ionic radius follows the same trends as atomic radius, decreasing across periods and increasing down groups.
[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
Chem chapt 6
The document summarizes the development and key features of the periodic table. It traces how early scientists like Newlands and Mendeleev organized the elements and developed periodic trends. The modern periodic table is arranged by atomic number and contains metals, nonmetals, and metalloids organized into blocks and groups. Elements in the same group have similar properties due to their electron configurations, and properties vary periodically according to trends like atomic radius and ionization energy.
Periodic Trends KC
This slideshow was created by a student in a high school chemistry class to summarize trends in the periodic table for a class assignment.
Trends on the periodic table0809
The document discusses trends in atomic radii and ionization energies across the periodic table. It explains that atomic radius generally decreases moving left to right within a period, as the nuclear charge increases and pulls electrons closer. Radius generally increases moving down a group, as additional electron shells provide more screening from the nucleus. Ionization energy generally increases left to right within a period as it becomes more difficult to remove electrons. However, there are some anomalies where ionization energy decreases due to electronic configuration changes.
Periodic Trends
This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Introduction to electricity
Electricity is caused by the movement of electrons between atoms. Atoms are made up of protons which have a positive charge and electrons which have a negative charge. When atoms gain or lose electrons, they become positively or negatively charged which allows electric forces to act between them. Charged objects can either attract or repel depending on whether they have the same or opposite charges. Materials that allow electrons to move through them easily are conductors, while insulators do not, which is why electrical wires have plastic coatings to prevent electric currents from flowing through the human body.
Electricity introduction
The document provides information about electricity, including what it is, how it is produced and distributed, and safety features in homes. It explains that electricity is generated through burning fossil fuels or renewable sources in power plants, then transmitted through power lines and transformers before reaching homes. Homes have circuit breakers and fuses to control electricity flow and wall outlets have safety features like polarized plugs and ground fault circuit interrupters (GFCIs) to prevent electric shocks.
Trends of The Periodic Table
The document discusses trends in atomic size, ionization energy, and electronegativity across Groups 17 and 18 of the periodic table. Atomic size increases and ionization energy decreases down each group as the atomic number increases. Electronegativity decreases down Group 17 but does not follow trends in Group 18 due to noble gases having full valence shells. The reactivity of Groups 17 and 18 with water and air is also examined, with halogens generally being reactive while noble gases are not reactive due to closed electron shells.
Electromagnetism, electricity and digital electronics
This document provides an outline for a course on electromagnetism, electricity, and digital electronics. It covers topics such as the theory of electrons and electricity, resistors, Ohm's law, electric circuits, the theory of magnetism, diodes, logic gates, and flip-flops. It lists several textbooks that will be used as references. It then delves into some of the topics in more detail, including the structure of atoms, types of insulators and conductors, direct and alternating current, voltage, current, resistance, and Ohm's law. It also discusses magnetism, electromagnetism, and provides examples of devices that use magnets.
Chapter 5.3 : Electron Configuration and the Periodic Table
This document defines and compares various periodic properties including atomic radii, ionization energy, electron affinity, ionic radii, valence electrons, and electronegativity. It states that atomic radii decreases left to right and increases down a group. Ionization energy generally increases across a period and decreases down a group. Electron affinity is the energy released or absorbed when an atom gains or loses an electron. Ionic radii are smaller for cations and larger for anions. Valence electrons are those involved in bonding and their number varies by main group element. Electronegativity generally increases across a period and decreases down a group.
Electrical circuits
Electricity is a flow of electrons that can pass through conductors like metals but not insulators like plastics. Circuits allow electricity to flow through a closed loop using components like cells, batteries, bulbs, switches, and fuses. Current is measured in amps and is affected by the resistance in the circuit, with higher resistance resulting in lower current. Electricity can heat wires and power appliances, while fuses provide safety by melting with too much current. Circuits can be connected in series or parallel configurations.
Electronegativity and electropositivity trends in periodic table
Electronegativity and electropositivity trends in periodic table
Video link:
https://youtu.be/_ojmwCHhuJM
Paper E Sign La Firma Digitale Su Carta Seminario Epa
Paper e-Sign la firma digitale su carta come sistema di anticontraffazione dei documenti di identità
Paper E Sign
Paper e-Sign, a technology that has been developed by Secure Edge to protect documents from falsification.
It is a graphic seal that, when used on printed documents, makes them impossible to alter in any way
Based on 2D-Plus™ is the 2D graphic codification process itself, which, unlike other codes, allows the encryption of enough information to create an unalterable file of any kind of data; for example: biometric, retinal, and photographic data as well as digital fingerprints and address and birth data.
More Related Content
What's hot
The periodic table & periodic law
The document summarizes the development and key features of the periodic table. It discusses how early chemists like Newlands, Meyer, and Mendeleev arranged elements in order of atomic mass and properties, recognizing repeating patterns. Mendeleev predicted new elements and Moseley later arranged elements by atomic number. The periodic table is organized into blocks by electron configuration and periods and groups that demonstrate trends in properties. Metals are on the left, nonmetals on the right, and metalloids border the stair-step line between them.
Periodic trends
The document discusses periodic trends in elemental properties. It explains that Dmitri Mendeleev was the first to organize elements in a periodic table based on their properties. Elements in the same group have similar properties due to their valence electrons. Atomic radius generally decreases moving left to right across a period and increases moving down a group due to electron shielding. Ionization energy increases as atomic radius decreases. Electron affinity is exothermic when gaining electrons fills an orbital. Metallic character decreases and electronegativity increases moving from left to right. Cations are smaller than their parent atoms while anions are larger.
Trends in the periodic table
Specifically designed for Leaving Cert Chemistry students. A simplified explanation of all the trends in the periodic Table. It includes details such as atomic radius, electronegativity and ionisation energy
periodic table trends
The Periodic Table and Periodic Law SECTION 3 Periodic Trends
ionization energy
atomic radius
electronegativity
Periodic trends
The document discusses periodic trends in atomic properties according to the periodic table. It explains that atomic radius decreases across a period as effective nuclear charge increases due to shielding effects, while radius increases down a group as each row adds a new shell. Ionization energy tends to increase across a period as removal of electrons becomes more difficult, and decreases down a group as outer electrons are farther from the nucleus. Electronegativity also increases across a period but decreases or stays the same down a group as distance from the nucleus increases. Positively charged cations are smaller than their parent atoms, while negatively charged anions are larger.
Trends of periodic atomic properties
1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
3) Electronegativity increases across a period for the same reasons as ionization energy, and decreases down a group as shielding increases and attraction decreases.
Presentation of periodic trends - STAGE 3
Periodic trends are patterns in the periodic table that illustrate properties of elements, including size and those relating to electrons. The main periodic trends are electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. These trends show how each property changes when moving left to right within a period or up and down within a group. For example, electronegativity increases left to right within a period but decreases up and down within a group. The document then discusses each trend in more detail and provides examples.
Periodic trends lecture notes a.k
The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
[2] Ionic radius follows the same trends as atomic radius, decreasing across periods and increasing down groups.
[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
Chem chapt 6
The document summarizes the development and key features of the periodic table. It traces how early scientists like Newlands and Mendeleev organized the elements and developed periodic trends. The modern periodic table is arranged by atomic number and contains metals, nonmetals, and metalloids organized into blocks and groups. Elements in the same group have similar properties due to their electron configurations, and properties vary periodically according to trends like atomic radius and ionization energy.
Periodic Trends KC
This slideshow was created by a student in a high school chemistry class to summarize trends in the periodic table for a class assignment.
Trends on the periodic table0809
The document discusses trends in atomic radii and ionization energies across the periodic table. It explains that atomic radius generally decreases moving left to right within a period, as the nuclear charge increases and pulls electrons closer. Radius generally increases moving down a group, as additional electron shells provide more screening from the nucleus. Ionization energy generally increases left to right within a period as it becomes more difficult to remove electrons. However, there are some anomalies where ionization energy decreases due to electronic configuration changes.
Periodic Trends
This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Introduction to electricity
Electricity is caused by the movement of electrons between atoms. Atoms are made up of protons which have a positive charge and electrons which have a negative charge. When atoms gain or lose electrons, they become positively or negatively charged which allows electric forces to act between them. Charged objects can either attract or repel depending on whether they have the same or opposite charges. Materials that allow electrons to move through them easily are conductors, while insulators do not, which is why electrical wires have plastic coatings to prevent electric currents from flowing through the human body.
Electricity introduction
The document provides information about electricity, including what it is, how it is produced and distributed, and safety features in homes. It explains that electricity is generated through burning fossil fuels or renewable sources in power plants, then transmitted through power lines and transformers before reaching homes. Homes have circuit breakers and fuses to control electricity flow and wall outlets have safety features like polarized plugs and ground fault circuit interrupters (GFCIs) to prevent electric shocks.
Trends of The Periodic Table
The document discusses trends in atomic size, ionization energy, and electronegativity across Groups 17 and 18 of the periodic table. Atomic size increases and ionization energy decreases down each group as the atomic number increases. Electronegativity decreases down Group 17 but does not follow trends in Group 18 due to noble gases having full valence shells. The reactivity of Groups 17 and 18 with water and air is also examined, with halogens generally being reactive while noble gases are not reactive due to closed electron shells.
Electromagnetism, electricity and digital electronics
This document provides an outline for a course on electromagnetism, electricity, and digital electronics. It covers topics such as the theory of electrons and electricity, resistors, Ohm's law, electric circuits, the theory of magnetism, diodes, logic gates, and flip-flops. It lists several textbooks that will be used as references. It then delves into some of the topics in more detail, including the structure of atoms, types of insulators and conductors, direct and alternating current, voltage, current, resistance, and Ohm's law. It also discusses magnetism, electromagnetism, and provides examples of devices that use magnets.
Chapter 5.3 : Electron Configuration and the Periodic Table
This document defines and compares various periodic properties including atomic radii, ionization energy, electron affinity, ionic radii, valence electrons, and electronegativity. It states that atomic radii decreases left to right and increases down a group. Ionization energy generally increases across a period and decreases down a group. Electron affinity is the energy released or absorbed when an atom gains or loses an electron. Ionic radii are smaller for cations and larger for anions. Valence electrons are those involved in bonding and their number varies by main group element. Electronegativity generally increases across a period and decreases down a group.
Electrical circuits
Electricity is a flow of electrons that can pass through conductors like metals but not insulators like plastics. Circuits allow electricity to flow through a closed loop using components like cells, batteries, bulbs, switches, and fuses. Current is measured in amps and is affected by the resistance in the circuit, with higher resistance resulting in lower current. Electricity can heat wires and power appliances, while fuses provide safety by melting with too much current. Circuits can be connected in series or parallel configurations.
Electronegativity and electropositivity trends in periodic table
Electronegativity and electropositivity trends in periodic table
Video link:
https://youtu.be/_ojmwCHhuJM
What's hot (20)
Electromagnetism, electricity and digital electronics
Electromagnetism, electricity and digital electronics
Chapter 5.3 : Electron Configuration and the Periodic Table
Chapter 5.3 : Electron Configuration and the Periodic Table
Electronegativity and electropositivity trends in periodic table
Electronegativity and electropositivity trends in periodic table
Viewers also liked
Paper E Sign La Firma Digitale Su Carta Seminario Epa
Paper e-Sign la firma digitale su carta come sistema di anticontraffazione dei documenti di identità
Paper E Sign
Paper e-Sign, a technology that has been developed by Secure Edge to protect documents from falsification.
It is a graphic seal that, when used on printed documents, makes them impossible to alter in any way
Based on 2D-Plus™ is the 2D graphic codification process itself, which, unlike other codes, allows the encryption of enough information to create an unalterable file of any kind of data; for example: biometric, retinal, and photographic data as well as digital fingerprints and address and birth data.
SLC Process for Software Development & Quality Control
- Software Lifecycle Models
- SLC Process in the Industry
- Software Quality Control
- Q&A Session
Beisbol
El beisbol es un deporte de equipo jugado con bate y pelota entre dos equipos de nueve jugadores cada uno en un campo con cuatro bases formando un cuadrado. Cada equipo intenta anotar carreras completando una vuelta alrededor de las bases, impulsados por batazos de sus compañeros de equipo o por errores del equipo contrario. El equipo con más carreras anotadas al final del juego gana.
Crowdsourcing
The new innovation model
For more white papers and webinars, go to http://www.sldesignlounge.com
Or visit us at http://www.sld.com
CAD & GIS-Connecting the Two Worlds
See how to perform more sophisticated CAD-GIS transformations with FME 2016. We’ll look at topics like attribute validation, automated cell placement in dgn and so on
Trusted Experience
The document discusses how insurance companies can build brand loyalty like hotels do. It argues that while online sales are growing, physical stores excel at building trust and relationships. Leading insurance companies are realizing bricks-and-mortar locations complement online channels. Examples include RBC Insurance Centers colocated in banks and Belair Direct combining sales offices with a retail space offering insurance packages. The conclusion advocates a multi-channel approach including physical locations to avoid commoditization and build affinity through trusted, personal experiences.
Current Resistance & Power
The document discusses electrical current, resistance, and power. It defines current as the rate of flow of electrical charge and discusses its units. It defines power as the rate at which work is done or energy is transferred, and discusses its relationship to current and voltage. It also defines resistance as the opposition to current flow and discusses how it depends on various material properties and how it relates to current and voltage using Ohm's Law.
Global IGNITE Newcastle 2011
This document contains 20 unknown bookmarks on a variety of topics including LEGO computers, creepy places on earth, tips for upgrading your morning routine, reasons to celebrate mistakes at work, dropped food etiquette, and focusing on your strengths. The bookmarks cover technology, travel, self-improvement, and general interest subjects without providing more context for each link.
Metric System Scientific Notation
The document discusses the metric system and scientific notation. It provides the following key points:
1) The metric system is based on units of meters, liters, and grams, with prefixes like kilo and centi to denote multiples or fractions of the base units.
2) Conversions within the metric system involve moving the decimal point a consistent number of places to the right or left based on the prefix in use.
3) Scientific notation expresses very large or small numbers in a standardized form of a number between 1 and 10, multiplied by a power of 10. Conversions between scientific and standard notation involve moving the decimal accordingly.
Data is Power
Understand how data plays a key role in any GIS, how to rise above file format barriers and achieve true data interoperability
Periodic Table E Config
The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added as elements exhibit repeating properties in each column. It then discusses various models that describe the structure of atoms, including the Bohr model, quantum mechanical model, electron shells, orbitals, and electron configurations.
Wacky Definitions
This document contains humorous definitions of various words and concepts. Some key definitions include:
- School is a place where the father pays and the son plays.
- Life insurance keeps you poor during your life so you can die rich.
- A nurse wakes you up to give you sleeping pills.
- Marriage is when a man loses his bachelor's degree and a woman gains her master's.
- A lecture is when information is transferred from the lecturer's notes to the student's notes without passing through the minds of either.
Universal Gravitation
This document discusses Newton's law of universal gravitation and provides examples of calculating gravitational force. It begins by defining gravitational force as a mutual attraction between particles of matter that exists regardless of the medium or masses involved. It then provides Newton's equation for gravitational force as being dependent on the masses of the objects and the distance between them. Examples are given of calculating gravitational force and distance between objects based on their masses and the measured force. Homework questions at the end involve calculating escape velocity from Earth and questions about black holes.
Covalent Nomenclature
This document outlines the rules for naming binary covalent compounds composed of two non-metal elements. The first element is named first using its full name, and the second element name has the suffix -ide added after dropping the ending. Prefixes are used to indicate the number of atoms present of the second element, with mono- only used for the second element and not the first. Example prefixes and their corresponding numbers are also provided, as well as examples of names for several binary covalent compounds.
Toolkit: The Creative Process
Learn how to manage the creative process, and how to work with agencies. Briefs, Brainstorming, Concept/Mood Boards, Creative Presentation
Viewers also liked (20)
Paper E Sign La Firma Digitale Su Carta Seminario Epa
Paper E Sign La Firma Digitale Su Carta Seminario Epa
SLC Process for Software Development & Quality Control
SLC Process for Software Development & Quality Control
Similar to Periodic Trends
Periodic trends
Atomic radius decreases and ionization energy increases when moving from left to right across a period. The nuclear charge increases while shielding remains constant, strengthening the attraction between electrons and the nucleus. Atomic radius increases and ionization energy decreases when moving down a group, as the valence electrons are farther from the nucleus due to additional electron shells providing shielding.
Periodic trends detailed edit
Periodic Trends
This document discusses several periodic trends including ionization energy, electronegativity, atomic radius, and ionic radius. It notes that ionization energy generally decreases down a group and increases left to right in a period as the nuclear charge increases. Electronegativity also typically increases left to right and decreases down a group. Atomic radius decreases left to right in a period as the nuclear charge increases but increases down a group as the principal energy level increases. Ionic radius trends are similar, with positive ion size decreasing left to right and both positive and negative ion size increasing down a group.
Periodic properties of the elements
periodic properties of the elements for class 11th and 12th science students..go and copy all the stuff
Ionization Energy...
The document discusses ionization energy and atomic and ionic radii. It defines an ion as a charged atom or molecule resulting from an imbalance of protons and electrons. The first ionization energy is the amount of energy required to remove an electron from the outermost shell of an atom. Each subsequent ionization energy is greater than the preceding one. Atomic radius decreases left to right on the periodic table as nuclear charge increases, while it increases down a group as electron shells expand. Positive ions have smaller radii than their parent atoms due to their increased nuclear charge.
Trends in the periodic table
The document summarizes trends in properties of elements as you move through the periodic table, including atomic radius, ionic radii, ionization energy, electron affinity, and electronegativity. It explains that atomic radius increases down a family due to increasing energy levels, while decreasing left to right due to more protons. Ionic radii decrease when gaining electrons and increase when losing electrons. Ionization energy increases when removing electrons due to stronger nuclear attraction and decreases down a family and increases left to right. Electron affinity and electronegativity both increase left to right and decrease top to bottom.
Periodic Trends
1. The document discusses several periodic trends including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases left to right within a period and increases down a group. Ionization energy generally increases left to right within a period and decreases down a group. Electronegativity increases left to right within a period and decreases down a group.
2. The document also discusses ionic radius trends, explaining that the size of positive ions decreases left to right within a period while the size of negative ions increases. Ionic radius increases down a group for both positive and negative ions.
3. The octet rule is mentioned as determining what types of ions atoms will form in order to acquire
Periodic classification
The document discusses periodic trends in elemental properties according to the periodic table. It explains that atomic radius generally increases moving left to right within a period and increases moving down within a family. Ionization energy decreases moving left to right within a period and decreases moving down within a family, while electron affinity shows the opposite trends. Metallic character decreases and electronegativity increases moving from left to right across the periodic table. Overall reactivity of metals increases with increasing size while reactivity of nonmetals increases with decreasing size. The document also discusses ion formation and how cations are smaller than the original atom while anions are larger.
PT IRE
The document discusses periodic trends in atomic properties including atomic radius, ionization energy, and electronegativity. It explains that as you move down a group in the periodic table, atomic radius increases while ionization energy and electronegativity decrease due to increased electron shielding. However, as you move across a period, atomic radius decreases while ionization energy and electronegativity increase due to the stronger effective nuclear charge pulling electrons in more tightly.
Ionic Trends
The document discusses ionic trends in atomic radius, ionization energy, and electronegativity across the periodic table. It explains that atomic radius generally decreases from left to right as more protons are added to the nucleus, attracting the electrons closer. Ionization energy decreases from right to left as the right side has more full valence shells, making them less likely to lose electrons. Electronegativity increases from left to right and decreases down groups as the distance from the valence electrons to the nucleus changes.
3b. The periodic table and trends.pptx 11
1. This document provides an overview of trends in the periodic table, including atomic size, ionization energy, electronegativity, and metallic/non-metallic character. It explains that these properties trend both across periods, from left to right as atomic number increases, and down groups as additional shells are filled.
2. Specifically, it notes that atomic size decreases across periods as nuclear charge increases, while increasing down groups as additional shells are added. Ionization energy and electronegativity both increase from left to right as nuclear charge increases, while decreasing down groups as electrons are farther from the nucleus. Metallic character increases down groups and decreases across periods.
3. The document aims to explain these
Semiconductors
This document provides an introduction to semiconductors. It discusses that semiconductors have conductivity between conductors and insulators. Intrinsic semiconductors are pure, while extrinsic semiconductors are doped with impurities. N-type semiconductors are doped with donors, making electrons the majority carriers. P-type semiconductors are doped with acceptors, making holes the majority carriers. When a P-type and N-type semiconductor are joined, a PN junction is formed with a depletion region between them. Forward biasing the junction lowers the barrier for current to flow.
Periodic Table 5
The document discusses several periodic properties of elements including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases across a period as nuclear charge increases but increases down a group as electron shielding increases. Ionization energy generally increases across a period as it becomes harder to remove electrons but decreases down a group as electrons are farther from the nucleus. Electronegativity also increases across a period as nuclear attraction increases.
Forces Of Attraction
Forces of attraction include intramolecular and intermolecular forces. Intramolecular forces like ionic bonds and covalent bonds hold atoms together in molecules through electrostatic attraction or electron sharing. Intermolecular forces between molecules include hydrogen bonding, dipole-dipole interactions, and induced dipole forces from electron motion. These weaker forces influence melting/boiling points and physical states. Polar molecules form stronger intermolecular attractions than nonpolar molecules through orientations of their charge distributions.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
CHEMISTRY: SLIDES FOR MIDDLE SCHOOL TEACHERS.pptx
This document provides an overview of chemistry concepts including the structure of atoms, chemical bonding, states of matter, and reading chemical formulas. It discusses key ideas such as:
- Atoms are composed of protons, neutrons, and electrons. The number of protons determines the element.
- Chemical bonds form through the transfer or sharing of electrons between atoms. Ionic bonds form between oppositely charged ions, and covalent bonds form through shared pairs of electrons.
- Matter exists in solid, liquid, gas, or plasma states depending on the strength of interactions between particles and temperature. Changes between these states involve heat.
- Chemical formulas represent the elements and ratios present in a compound. Formulas indicate physical state and
Chapter 6.3
This document summarizes periodic trends among elements. It describes how nuclear charge shielding increases down groups but is constant across periods. Atomic radius decreases across periods as more protons attract electrons closer, but increases down groups as electrons are farther from the nucleus. Ionization energy increases across periods as more protons hold onto electrons, but decreases down groups as outer electrons are easier to remove. Electronegativity generally increases across periods as additional protons pull electrons closer, but decreases down groups due to increased shielding blocking the proton pull.
Trends in the periodic table
Trends in the periodic table: Atomic radius, ionization energy, electronegativity, metallic character
Chem 101 week 9 ch8
The document summarizes periodic trends among elements including atomic and ionic sizes, ionization energies, and electron affinities. It explains that atomic size decreases left to right across a period as effective nuclear charge increases, while size increases down a group as principal quantum number increases. Ionization energy generally increases left to right as effective nuclear charge increases, with exceptions between groups IIA-IIIA and VA-VIA. Electron affinity becomes more exothermic left to right with exceptions between groups IA-IIA and IVA-VA. The document also describes trends and properties of representative elements and families including alkali metals, alkaline earth metals, halogens, and noble gases.
APChem- Chapter 7 Lecture- Periodic Trends
The document discusses trends in the properties of elements in the periodic table. It describes how elements in the same group generally have similar chemical properties, though properties are not identical. It discusses how Mendeleev and Meyer independently organized the elements into the first periodic tables based on recurring trends in properties. Elements in the inner transition metals block were later added.
B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry ...
The document discusses several periodic trends:
1. Atomic radius generally increases moving down a group and decreases moving across a period, due to shielding and nuclear charge effects.
2. Ionization energy increases moving across a period as the effective nuclear charge increases, and decreases moving down a group as the distance from the nucleus increases.
3. Electronegativity increases moving across a period as it is easier to gain than lose electrons, and decreases moving down a group with increased atomic radius.
Similar to Periodic Trends (20)
B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry ...
B.sc(microbiology and biotechnology and biochemistry) ii inorganic chemistry ...
More from Regis Komperda
Ionic Nomenclature & Compounds
Ionic compounds are named by writing the cation first followed by the anion. Transition metals that can form multiple cations use Roman numerals in parentheses in the name to indicate the charge on the cation. The Roman numeral is not included in the chemical formula. Ionic compounds form crystalline structures where the cations and anions are packed tightly together.
Periodic Trends
This document discusses polyatomic ions and how to name and write formulas for compounds containing them. Polyatomic ions are ions made of more than one element that stay together as a unit in chemical reactions. To write formulas, identify the cation and anion present and determine the necessary subscripts to make the total charge neutral. Example formulas given are sodium phosphate (Na3PO4) and magnesium phosphate (Mg3(PO4)2) to illustrate this process.
Covalent Nomenclature
This document contains the chemical formulas or names of various substances that could be used in a chemistry bingo game. There are over 30 different chemicals listed, ranging from common salts and oxides to more complex compounds involving metals, nonmetals, and transition metals. The variety of substances mentioned provide many options for calling out formulas and properties as part of a bingo game focused on chemical compounds.
Polyatomic Nomenclature
The document discusses the metric system and scientific notation. It provides details on:
- The metric system is based on units of meters, liters, and grams with prefixes like kilo and centi to denote multiples or fractions of the base units.
- Scientific notation expresses very large or small numbers as a number between 1 and 10 with an exponent of 10. This makes concise expressions like 2.898 x 108 for 289,800,000.
- Conversions within the metric system move the decimal point left or right based on moving to a larger or smaller unit, following powers of 10 denoted by the prefixes.
Polyatomic Nomenclature
The document discusses the metric system and scientific notation. It provides details on:
- The metric system is based on units of meters, liters, and grams with prefixes like kilo and centi to denote multiples or fractions of the base units.
- Scientific notation expresses very large or small numbers as a number between 1 and 10 with an exponent of 10. This makes concise expressions like 2.898 x 108 for 289,800,000.
- Conversions within the metric system move the decimal point left or right based on moving to a larger or smaller unit, following powers of 10.
Periodic Table E Config
The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added as elements exhibit repeating properties in each column. It then discusses various models that were developed to explain the organization and placement of electrons in atoms, including the Bohr model, quantum mechanical model, electron orbitals, and electron configurations.
Nuclear Decay
The document discusses various types of nuclear decay:
- Alpha decay involves emitting an alpha particle (helium nucleus), decreasing the atomic number by 2 and mass number by 4.
- Beta decay involves changing a neutron to a proton and emitting an electron, increasing the atomic number by 1 while keeping the same mass number.
- Electron capture involves capturing an electron by a proton to form a neutron, decreasing the atomic number by 1 while keeping the same mass number.
- Positron emission involves changing a proton to a neutron and emitting a positron, decreasing the atomic number by 1 while keeping the same mass number.
- Gamma decay involves emitting a high-energy gamma ray without changing mass or atomic number
Semester 1 Review Jeopardy
This document contains a chemistry jeopardy game covering topics from 5 units:
1) Measurement and calculations
2) States of matter and properties
3) Atomic structure
4) Radioactivity
5) Periodic trends
The questions cover concepts such as significant figures, conversions, physical and chemical properties, atomic structure, radioactive decay, electron configurations, and trends in atomic radius and ionization energy across the periodic table.
Bingo
This document contains the chemical formulas or names of various substances that could be used in a chemistry bingo game. There are over 30 different chemicals listed, ranging from common salts and oxides to more complex compounds containing transition metals, nonmetals, and organic molecules. The variety of substances mentioned provide many options for calling out squares in a bingo game focused on chemical formulas and names.
Metric System Scientific Notation
The document discusses the metric system and scientific notation. It provides details on:
- The metric system is based on units of meters, liters, and grams with prefixes like kilo and centi to denote multiples or fractions of the base units.
- Scientific notation expresses very large or small numbers as a number between 1 and 10 with an exponent of 10. This makes concise expressions like 2.898 x 108 for 289,800,000.
- Conversions within the metric system move the decimal point left or right based on moving to a larger or smaller unit, following powers of 10.
Periodic Trends
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity.
2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right.
3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Periodic Table E Config
The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added to accommodate elements with repeating properties in each column. It also discusses the patterns in the periodic table including groups/families defined by their number of outer shell electrons and typical ion charges.
Semester 1 Review Jeopardy
This document contains a chemistry jeopardy game covering topics from 5 units:
1. Measurements and calculations
2. States of matter and properties
3. Atomic structure
4. Radioactivity
5. Periodic trends
The questions test knowledge of concepts like significant figures, conversions, physical and chemical properties, atomic structure, radioactive decay, electron configurations, and trends in atomic radius and ionization energy across the periodic table.
Metric System Scientific Notation
The document discusses the metric system and scientific notation. It provides the following key points:
1) The metric system is based on units of meters, liters, and grams, with prefixes like kilo and centi to denote multiples or fractions of the base units.
2) Conversions within the metric system involve moving the decimal point a consistent number of places to the right or left based on the prefix in use.
3) Scientific notation expresses very large or small numbers in a standardized form of a number between 1 and 10, multiplied by a power of 10. Conversions between scientific and standard notation involve moving the decimal accordingly.
Nuclear Decay
The document discusses various types of nuclear decay:
- Alpha decay involves emitting an alpha particle (helium nucleus), decreasing the atomic number by 2 and mass number by 4.
- Beta decay involves changing a neutron to a proton and emitting an electron, increasing the atomic number by 1 while keeping the same mass number.
- Electron capture involves capturing an electron by a proton to form a neutron, decreasing the atomic number by 1 while keeping the same mass number.
- Positron emission involves changing a proton to a neutron and emitting a positron, decreasing the atomic number by 1 while keeping the same mass number.
- Gamma decay involves emitting high energy gamma rays without changing mass or atomic number.
Periodic Table E Config
The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added to accommodate elements with repeating properties in each column. It then discusses various models that describe the structure of atoms, including the Bohr model, quantum mechanical model, electron shells, orbitals, and electron configurations.
Periodic Table E Config
The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added to accommodate elements with repeating properties in each column. It then discusses various models that describe the organization and location of electrons in atoms, including the Bohr model, quantum mechanical model, electron orbitals, and electron configurations.
Nomenclature Bingo
This document contains the chemical formulas or names of various substances that could be used in a chemistry bingo game. There are over 30 different chemicals listed, ranging from common salts and oxides to more complex compounds involving metals, nonmetals, and transition metals. The variety of substances mentioned provide many options for calling out formulas and getting bingo in a game focused on chemical names and formulas.
Chemical Bonding Part 1
A chemical bond is a force that holds atoms together, causing them to function as a single unit. There are three main types of bonds: ionic bonds, polar covalent bonds, and covalent bonds. Ionic bonds form between a metal and nonmetal when electrons are transferred from one atom to the other, creating oppositely charged ions. Polar covalent bonds involve the unequal sharing of electrons between two nonmetals. Covalent bonds equally share electrons between two nonmetals. Bonds are important because they determine how atoms interact and undergo chemical reactions.
Ions & Isotopes
Ion - an atom or group of atoms that has a positive or negative charge. Ions are formed by gaining or losing electrons, not protons. Cations have a positive charge and are formed by losing electrons. Anions have a negative charge and are formed by gaining electrons. The periodic table shows which elements tend to form which ions based on their group, with groups 1, 2, 6 and 7 typically forming cations or anions.
More from Regis Komperda (20)
Recently uploaded
Chapter wise All Notes of First year Basic Civil Engineering.pptx
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
Bossa N’ Roll Records by Ismael Vazquez.
Bossa N Roll Records presentation by Izzy Vazquez for Music Retail and Distribution class at Full Sail University
Temple of Asclepius in Thrace. Excavation results
The temple and the sanctuary around were dedicated to Asklepios Zmidrenus. This name has been known since 1875 when an inscription dedicated to him was discovered in Rome. The inscription is dated in 227 AD and was left by soldiers originating from the city of Philippopolis (modern Plovdiv).
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"National Information Standards Organization (NISO)
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.Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as discipline
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...Nguyen Thanh Tu Collection
https://app.box.com/s/tacvl9ekroe9hqupdnjruiypvm9rdaneBIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
Practical manual for National Examination Council, Nigeria.
Contains guides on answering questions on the specimens provided
A Visual Guide to 1 Samuel | A Tale of Two Hearts
These slides walk through the story of 1 Samuel. Samuel is the last judge of Israel. The people reject God and want a king. Saul is anointed as the first king, but he is not a good king. David, the shepherd boy is anointed and Saul is envious of him. David shows honor while Saul continues to self destruct.
Leveraging Generative AI to Drive Nonprofit Innovation
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.)
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Aberdeen
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
- Understand the goals and objectives of the Edukasyong Pantahanan at Pangkabuhayan (EPP) curriculum, recognizing its importance in fostering practical life skills and values among students. Students will also be able to identify the key components and subjects covered, such as agriculture, home economics, industrial arts, and information and communication technology.
𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...
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.
Recently uploaded (20)
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
SWOT analysis in the project Keeping the Memory @live.pptx
SWOT analysis in the project Keeping the Memory @live.pptx
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
Leveraging Generative AI to Drive Nonprofit Innovation
Leveraging Generative AI to Drive Nonprofit Innovation
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...
Periodic Trends
- 1. November 18 th & 19 th , 2009 Periodic Trends