The document summarizes key aspects of the periodic table, including its structure, historical development, and trends in elemental properties. It explains that the periodic table arranges elements in rows and columns based on atomic number and properties. Mendeleev and Moseley helped develop the modern periodic table by arranging elements based on atomic mass and charge. Elements are classified as metals, nonmetals, and metalloids based on their physical and chemical properties, which vary predictably within and between groups and periods.
The document provides information about the periodic table, including its organization into periods and families. It describes the properties and composition of different types of elements such as metals, non-metals, and metalloids. Key figures who developed the periodic table, like Dmitri Mendeleev, are mentioned. Different areas of the periodic table are also summarized, including the alkali metals, transition metals, and noble gases. Basic chemistry concepts such as elements, compounds, and mixtures are defined.
The periodic table arranges the elements based on atomic number and chemical properties. It is divided into metals, nonmetals, and metalloids. The periodic table predicts chemical behavior, trends, and element properties. It organizes elements by atomic structure, number, and physical/chemical traits.
The periodic table organizes 118 known elements and displays their symbols and names. It arranges elements in rows called periods and columns called groups based on their atomic structure and properties. Elements in the same group have the same number of outer electrons and similar chemical properties, while properties vary greatly across each period from very reactive solids to inactive gases. The periodic table provides a way to classify and compare elements according to their atomic number and mass.
The document provides an overview of key concepts related to the periodic table including periods and groups, trends across the table, families of elements, and properties of metals, nonmetals, noble gases, and other groups. It defines elements and ions, and discusses oxidation numbers, trends in properties, and the organization and discoveries of early periodic tables.
The periodic table organizes the elements based on their atomic structure, especially the number of protons and electrons. Elements in the same column usually have similar properties because they have the same number of valence electrons. The periodic table can be used to predict an element's identity, properties, and reactivity based on its location on the table.
The document discusses key aspects of the periodic table, including its structure, properties of different groups of elements, and how position on the table relates to electron configuration and chemical properties. It provides details on the alkali metals, halogens, and noble gases groups, describing their physical and chemical characteristics. Examples are given of elements in each group to illustrate trends in properties.
The document discusses the periodic table of elements, which organizes the 118 known elements. Elements are organized according to their atomic number and have unique symbols and properties. The periodic table provides information about each element's atomic structure and how they react and bond with other elements. Elements are grouped into families based on their valence electrons and similar chemical properties.
The document provides information about the periodic table, including its organization into periods and families. It describes the properties and composition of different types of elements such as metals, non-metals, and metalloids. Key figures who developed the periodic table, like Dmitri Mendeleev, are mentioned. Different areas of the periodic table are also summarized, including the alkali metals, transition metals, and noble gases. Basic chemistry concepts such as elements, compounds, and mixtures are defined.
The periodic table arranges the elements based on atomic number and chemical properties. It is divided into metals, nonmetals, and metalloids. The periodic table predicts chemical behavior, trends, and element properties. It organizes elements by atomic structure, number, and physical/chemical traits.
The periodic table organizes 118 known elements and displays their symbols and names. It arranges elements in rows called periods and columns called groups based on their atomic structure and properties. Elements in the same group have the same number of outer electrons and similar chemical properties, while properties vary greatly across each period from very reactive solids to inactive gases. The periodic table provides a way to classify and compare elements according to their atomic number and mass.
The document provides an overview of key concepts related to the periodic table including periods and groups, trends across the table, families of elements, and properties of metals, nonmetals, noble gases, and other groups. It defines elements and ions, and discusses oxidation numbers, trends in properties, and the organization and discoveries of early periodic tables.
The periodic table organizes the elements based on their atomic structure, especially the number of protons and electrons. Elements in the same column usually have similar properties because they have the same number of valence electrons. The periodic table can be used to predict an element's identity, properties, and reactivity based on its location on the table.
The document discusses key aspects of the periodic table, including its structure, properties of different groups of elements, and how position on the table relates to electron configuration and chemical properties. It provides details on the alkali metals, halogens, and noble gases groups, describing their physical and chemical characteristics. Examples are given of elements in each group to illustrate trends in properties.
The document discusses the periodic table of elements, which organizes the 118 known elements. Elements are organized according to their atomic number and have unique symbols and properties. The periodic table provides information about each element's atomic structure and how they react and bond with other elements. Elements are grouped into families based on their valence electrons and similar chemical properties.
The periodic table arranges the known chemical elements in order of their atomic number, with elements in the same group (vertical column) having similar properties. Elements are classified into periods (horizontal rows) and groups based on their atomic structure and electron configuration, with elements in the same group having the same number of electrons in their outer shell and exhibiting similar chemical behaviors. The periodic table summarizes periodic trends in properties of the elements and how an element's position determines its chemical properties.
The document discusses elements and the periodic table, including the properties of protons, neutrons, and electrons; atomic structure; atomic number; valence electrons; periodic trends; electron configurations; and groups on the periodic table. It asks questions about the location of mass in an atom, gold's atomic number and protons/electrons, bromine's protons, why scientists don't create a periodic table of compounds, hydrogen and lithium's valence electrons, which group elements belong to, how electrons fill energy levels, electron dot diagrams for vanadium, periods and rows on the periodic table, and what element is represented by an atom cookie. It also reviews distinguishing chemical and physical properties/changes, conservation of mass, and experimental variables.
The document provides an overview of the modern periodic table, including how elements are arranged and classified. It discusses the atomic number and mass, groups and periods, and the three main classifications of elements as metals, nonmetals, and metalloids. Key groups like the alkali metals, alkaline earth metals, transition metals, and noble gases are described based on their physical and chemical properties.
This is a revised PowerPoint on five families of the periodic table I put together for my HS chemistry 9 class after taking a course on visual literacy, inclusive of effective PowerPoint presentations. It could still be much better but I hope some improvement between the two PowerPoints is evident.
The document discusses the periodic table and its development. It explains that John Newlands first arranged elements by properties in 1865. Dmitri Mendeleev arranged the known 63 elements by atomic mass in 1869 and left gaps for undiscovered elements. Henry Moseley rearranged the table in order of increasing atomic number in 1914. The periodic table is organized into groups and periods that show similar properties recurring periodically. Main groups include alkali metals, alkaline earth metals, halogens and noble gases. Transition metals include lanthanides and actinides. The document also describes trends in ionization energy, atomic radius, electronegativity and electron affinity across the periodic table.
The periodic table organizes the chemical elements and provides information about their properties and reactions. Elements are arranged in order of increasing atomic number and are grouped together based on similar chemical properties. The position of an element in the periodic table can reveal whether it is a metal, nonmetal, or noble gas, as well as provide details about its reactivity and physical state. Element symbols represent the elements concisely and are typically derived from each element's name.
This document provides information about the periodic table and its development over time. It discusses how Dmitry Mendeleev discovered a pattern among the elements when arranged by atomic mass in 1869, creating the first periodic table. Later, Henry Moseley arranged the elements by atomic number, producing the modern periodic table. The document then describes the key components and organization of the periodic table, including periods, groups, and the properties of metals, nonmetals, and metalloids.
This document is a lesson on groups and periods in the periodic table. It defines periods as rows from left to right, and groups as columns from top to bottom. Elements in the same group have similar properties because they have the same number of valence electrons. The lesson discusses special metal and nonmetal groups, including alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. It provides examples of elements in each group and their properties. The document concludes with practice questions for students.
Periodic Classification of Elements and PeriodicityNEHANEHA67
The document discusses the history and development of the periodic table. It explains that early scientists like Dobereiner and Newlands began classifying elements based on their properties, but that Dmitri Mendeleev created the first recognizable periodic table in 1871. His table arranged elements in order of atomic mass and predicted properties of undiscovered elements. Later, Moseley's discovery of atomic number allowed the modern periodic table to arrange elements by atomic number instead of mass. The document also discusses trends in properties within the periodic table.
This document provides information about the periodic table and periodic trends. It discusses the organization of the periodic table into rows (periods) and columns (groups/families) and explains how elements in the same group have similar properties based on their electron configuration. Periodic trends are covered, including how atomic radius decreases across a period as effective nuclear charge increases, and how ionization energy and electron affinity vary periodically. Metals, nonmetals, and metalloids are defined based on their characteristic properties.
The document discusses the organization and classification of elements in the periodic table. It describes how Mendeleev organized the elements based on increasing atomic mass and similar properties. The modern periodic table is organized by increasing atomic number. Elements are classified into metals, nonmetals, and metalloids, which are grouped based on their location on the periodic table. Each group of elements has a characteristic number of valence electrons that determine their chemical properties.
The document discusses the periodic table, its history, organization, and the trends in various elemental properties that can be predicted from it. The periodic table was developed by Mendeleev in 1869 and organizes elements by atomic number. It allows prediction of trends in properties like atomic radius, ionization energy, and electronegativity across periods and down groups. The periodic table classifies elements as metals, nonmetals, metalloids and noble gases and notes important families like alkali metals, alkaline earth metals, and halogens.
Glenn Seaborg, who had an element named after him while still alive, played a key role in the development of the modern periodic table. The periodic table organizes elements according to their atomic number and similar chemical properties. Elements are made of protons, neutrons, and electrons, and their atomic structure helps explain their placement in the periodic table and their chemical behaviors.
The document discusses the periodic table, including its organization into periods and families. It describes the electron configuration of elements in different families, showing how the outer electron shells determine an element's chemical properties and reactivity. Examples are given of elements from families such as alkali metals, halogens, and noble gases along with their electron configurations.
This document discusses periodicity and trends in properties across and down periods of the periodic table. It explains that atomic radius generally decreases across periods as nuclear charge increases, outweighing constant screening effects. Atomic radius increases down groups as nuclear charge rises but screening effects also increase. Ionic radius follows similar trends as atomic radius but is smaller for cations and larger for anions. Melting and boiling points are influenced by type and strength of bonding. Metallic bonding results in higher melting points for metals with more delocalized electrons. Network covalent bonding in nonmetals produces high melting points due to needing to overcome many bonds. Molecular nonmetals have weaker van der Waals forces between molecules. First ionization energies also follow trends
Ch 6 The Periodic Table And Periodic Law Short2frhsd
The periodic table organizes elements based on repeating patterns of their chemical and physical properties.
1) Mendeleev organized the elements based on properties and predicted new elements before discovery.
2) Elements are arranged in periods and groups, with similar properties repeating vertically in groups.
3) Periodic trends like atomic size, ionization energy, and electronegativity can be explained by the attraction of electrons to the atomic nucleus and how electrons fill energy levels.
The document summarizes key aspects of the periodic table, including its discovery by Dmitri Mendeleev who predicted undiscovered elements, and the periodic law stating elements' properties repeat periodically with their atomic number. It describes the main categories of elements as metals, nonmetals, and metalloids, and explains parts of the periodic table including periods and groups. It provides details on each group's properties including electron configuration, reactivity, and shared physical traits.
The periodic table is arranged based on atomic number and properties repeat periodically. Early forms grouped elements based on atomic mass but Moseley found atomic number was key. The table is divided into periods and groups with trends in properties like atomic size decreasing left to right across periods and ionization energy increasing. Metallic character increases down groups and nonmetallic character increases right across periods. The periodic table organizes the elements and allows prediction of properties.
For educational purposes only. No copyright intended to use the material. Credited the owner of the ppt. This is only for reference for the topic of Grade 8 Science in TNHS 2023-2024
periodic table of elements for grade 8 learnersAceReyes9
The document provides an overview of the periodic table of elements and key concepts related to elements and their organization. It discusses how elements are organized according to their atomic number and properties that can be determined from an element's position on the periodic table. Examples of different families of elements are provided, including their typical properties and valence electron configuration. Key terms like atomic number, atomic mass, and symbols are defined.
The periodic table arranges the known chemical elements in order of their atomic number, with elements in the same group (vertical column) having similar properties. Elements are classified into periods (horizontal rows) and groups based on their atomic structure and electron configuration, with elements in the same group having the same number of electrons in their outer shell and exhibiting similar chemical behaviors. The periodic table summarizes periodic trends in properties of the elements and how an element's position determines its chemical properties.
The document discusses elements and the periodic table, including the properties of protons, neutrons, and electrons; atomic structure; atomic number; valence electrons; periodic trends; electron configurations; and groups on the periodic table. It asks questions about the location of mass in an atom, gold's atomic number and protons/electrons, bromine's protons, why scientists don't create a periodic table of compounds, hydrogen and lithium's valence electrons, which group elements belong to, how electrons fill energy levels, electron dot diagrams for vanadium, periods and rows on the periodic table, and what element is represented by an atom cookie. It also reviews distinguishing chemical and physical properties/changes, conservation of mass, and experimental variables.
The document provides an overview of the modern periodic table, including how elements are arranged and classified. It discusses the atomic number and mass, groups and periods, and the three main classifications of elements as metals, nonmetals, and metalloids. Key groups like the alkali metals, alkaline earth metals, transition metals, and noble gases are described based on their physical and chemical properties.
This is a revised PowerPoint on five families of the periodic table I put together for my HS chemistry 9 class after taking a course on visual literacy, inclusive of effective PowerPoint presentations. It could still be much better but I hope some improvement between the two PowerPoints is evident.
The document discusses the periodic table and its development. It explains that John Newlands first arranged elements by properties in 1865. Dmitri Mendeleev arranged the known 63 elements by atomic mass in 1869 and left gaps for undiscovered elements. Henry Moseley rearranged the table in order of increasing atomic number in 1914. The periodic table is organized into groups and periods that show similar properties recurring periodically. Main groups include alkali metals, alkaline earth metals, halogens and noble gases. Transition metals include lanthanides and actinides. The document also describes trends in ionization energy, atomic radius, electronegativity and electron affinity across the periodic table.
The periodic table organizes the chemical elements and provides information about their properties and reactions. Elements are arranged in order of increasing atomic number and are grouped together based on similar chemical properties. The position of an element in the periodic table can reveal whether it is a metal, nonmetal, or noble gas, as well as provide details about its reactivity and physical state. Element symbols represent the elements concisely and are typically derived from each element's name.
This document provides information about the periodic table and its development over time. It discusses how Dmitry Mendeleev discovered a pattern among the elements when arranged by atomic mass in 1869, creating the first periodic table. Later, Henry Moseley arranged the elements by atomic number, producing the modern periodic table. The document then describes the key components and organization of the periodic table, including periods, groups, and the properties of metals, nonmetals, and metalloids.
This document is a lesson on groups and periods in the periodic table. It defines periods as rows from left to right, and groups as columns from top to bottom. Elements in the same group have similar properties because they have the same number of valence electrons. The lesson discusses special metal and nonmetal groups, including alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. It provides examples of elements in each group and their properties. The document concludes with practice questions for students.
Periodic Classification of Elements and PeriodicityNEHANEHA67
The document discusses the history and development of the periodic table. It explains that early scientists like Dobereiner and Newlands began classifying elements based on their properties, but that Dmitri Mendeleev created the first recognizable periodic table in 1871. His table arranged elements in order of atomic mass and predicted properties of undiscovered elements. Later, Moseley's discovery of atomic number allowed the modern periodic table to arrange elements by atomic number instead of mass. The document also discusses trends in properties within the periodic table.
This document provides information about the periodic table and periodic trends. It discusses the organization of the periodic table into rows (periods) and columns (groups/families) and explains how elements in the same group have similar properties based on their electron configuration. Periodic trends are covered, including how atomic radius decreases across a period as effective nuclear charge increases, and how ionization energy and electron affinity vary periodically. Metals, nonmetals, and metalloids are defined based on their characteristic properties.
The document discusses the organization and classification of elements in the periodic table. It describes how Mendeleev organized the elements based on increasing atomic mass and similar properties. The modern periodic table is organized by increasing atomic number. Elements are classified into metals, nonmetals, and metalloids, which are grouped based on their location on the periodic table. Each group of elements has a characteristic number of valence electrons that determine their chemical properties.
The document discusses the periodic table, its history, organization, and the trends in various elemental properties that can be predicted from it. The periodic table was developed by Mendeleev in 1869 and organizes elements by atomic number. It allows prediction of trends in properties like atomic radius, ionization energy, and electronegativity across periods and down groups. The periodic table classifies elements as metals, nonmetals, metalloids and noble gases and notes important families like alkali metals, alkaline earth metals, and halogens.
Glenn Seaborg, who had an element named after him while still alive, played a key role in the development of the modern periodic table. The periodic table organizes elements according to their atomic number and similar chemical properties. Elements are made of protons, neutrons, and electrons, and their atomic structure helps explain their placement in the periodic table and their chemical behaviors.
The document discusses the periodic table, including its organization into periods and families. It describes the electron configuration of elements in different families, showing how the outer electron shells determine an element's chemical properties and reactivity. Examples are given of elements from families such as alkali metals, halogens, and noble gases along with their electron configurations.
This document discusses periodicity and trends in properties across and down periods of the periodic table. It explains that atomic radius generally decreases across periods as nuclear charge increases, outweighing constant screening effects. Atomic radius increases down groups as nuclear charge rises but screening effects also increase. Ionic radius follows similar trends as atomic radius but is smaller for cations and larger for anions. Melting and boiling points are influenced by type and strength of bonding. Metallic bonding results in higher melting points for metals with more delocalized electrons. Network covalent bonding in nonmetals produces high melting points due to needing to overcome many bonds. Molecular nonmetals have weaker van der Waals forces between molecules. First ionization energies also follow trends
Ch 6 The Periodic Table And Periodic Law Short2frhsd
The periodic table organizes elements based on repeating patterns of their chemical and physical properties.
1) Mendeleev organized the elements based on properties and predicted new elements before discovery.
2) Elements are arranged in periods and groups, with similar properties repeating vertically in groups.
3) Periodic trends like atomic size, ionization energy, and electronegativity can be explained by the attraction of electrons to the atomic nucleus and how electrons fill energy levels.
The document summarizes key aspects of the periodic table, including its discovery by Dmitri Mendeleev who predicted undiscovered elements, and the periodic law stating elements' properties repeat periodically with their atomic number. It describes the main categories of elements as metals, nonmetals, and metalloids, and explains parts of the periodic table including periods and groups. It provides details on each group's properties including electron configuration, reactivity, and shared physical traits.
The periodic table is arranged based on atomic number and properties repeat periodically. Early forms grouped elements based on atomic mass but Moseley found atomic number was key. The table is divided into periods and groups with trends in properties like atomic size decreasing left to right across periods and ionization energy increasing. Metallic character increases down groups and nonmetallic character increases right across periods. The periodic table organizes the elements and allows prediction of properties.
For educational purposes only. No copyright intended to use the material. Credited the owner of the ppt. This is only for reference for the topic of Grade 8 Science in TNHS 2023-2024
periodic table of elements for grade 8 learnersAceReyes9
The document provides an overview of the periodic table of elements and key concepts related to elements and their organization. It discusses how elements are organized according to their atomic number and properties that can be determined from an element's position on the periodic table. Examples of different families of elements are provided, including their typical properties and valence electron configuration. Key terms like atomic number, atomic mass, and symbols are defined.
The document provides information about the periodic table of elements. It explains that the periodic table organizes the 118 known elements according to properties like atomic number and mass. Elements are grouped into families that have similar chemical behaviors, and periods that show how properties change across rows. Key aspects like reactivity, metallic and non-metallic properties, and the discoveries of scientists like Mendeleev who developed the periodic table are summarized.
The document provides information about the periodic table of elements, including how it organizes the 118 known elements according to their atomic structure and properties. Elements are arranged based on their atomic number and can be grouped into families that show similar traits. The periodic table provides a way to predict chemical behaviors and allows scientists to identify unknown elements based on trends in atomic structure.
The document provides information about the periodic table of elements, including that it organizes elements according to their atomic number and properties. Key aspects of the periodic table include the atomic number, atomic mass, symbols, and position of elements which can provide insight into their properties. The document also summarizes common elements, families of elements, and properties of metals, non-metals, and metalloids.
The document summarizes key information about the periodic table of elements, including its organization of elements according to atomic number and properties. Elements are grouped into families with similar properties, and the periodic table can be used to predict chemical reactions and properties of elements. Different areas of the periodic table are described, including alkali metals, transition metals, noble gases, and more.
The periodic table organizes the 118 known chemical elements according to their atomic structure. Elements are arranged by atomic number, symbols, atomic mass, and other properties like valence electrons. This allows scientists to predict elements' chemical and physical behaviors, as elements in the same families on the periodic table have similar properties. The periodic table is a useful tool for understanding the building blocks of all matter in the universe.
The periodic table organizes the 118 known chemical elements according to their atomic structure. Elements are arranged by atomic number, protons, and electrons, which determine their chemical and physical properties. The periodic table provides information on each element including symbol, atomic mass, number of protons and electrons, and whether they are metals, nonmetals, or metalloids.
The document summarizes key concepts about the periodic table of elements, including how it organizes the 118 known elements according to their atomic structure and properties. Elements are classified into families based on their valence electrons and include metals, non-metals, metalloids and noble gases. The periodic table provides a way to predict an element's properties and reactivity.
The document discusses the periodic table of elements, explaining how the elements are organized according to properties like atomic number and mass and describing important groups of elements including metals, non-metals, noble gases, and families like alkali metals and halogens. It provides details on the development of the periodic table and key aspects of classifying and understanding the elements.
The history of the periodic table's development, the arrangement of the elements, and the reactivity of each group of elements will all be covered in this lecture.
Periodic table of elements by Muhammad Fahad Ansari 12IEEM14fahadansari131
The document provides information about the periodic table of elements:
- The periodic table organizes the 118 known elements according to their atomic structure and properties. It allows one to predict chemical and physical properties of elements.
- Elements are organized by atomic number and grouped into families with similar properties. The position of an element provides information about its atomic mass, number of protons/electrons, and whether it is a metal, nonmetal, or metalloid.
- Families include the alkali metals, alkaline earth metals, halogens, noble gases, and more. The periodic table is a useful tool for understanding elemental properties and chemical behavior.
periodic_table element chemistry pptx jjcriandyputra3
The document provides information about the periodic table of elements, including:
1) It describes how the periodic table organizes 118 known elements according to their atomic structure and properties.
2) Key aspects that are organized in the table include the element's atomic number, symbol, atomic mass, number of valence electrons, and state of matter.
3) Understanding the periodic table allows one to predict an element's physical and chemical properties and reactions.
The document provides information about the periodic table of elements, including:
1) It describes how the periodic table organizes 118 known elements according to their atomic structure and properties.
2) Key aspects that are organized in the table include the element's atomic number, symbol, atomic mass, number of valence electrons, and state of matter.
3) Understanding the periodic table allows one to predict an element's physical and chemical properties and reactions.
The document provides information about the periodic table of elements, including:
1) It describes how the periodic table organizes 118 known elements according to their atomic structure and properties.
2) Key aspects that are organized in the table include the element's atomic number, symbol, atomic mass, number of valence electrons, and state of matter.
3) Understanding the periodic table allows one to predict an element's physical and chemical properties and reactions.
periodic table of elements power point presentationLEOPOLDOMALAAY1
The document provides information about the periodic table of elements, including:
1) It describes how the periodic table organizes 118 known elements according to their atomic structure and properties.
2) Key aspects that are organized include the element's atomic number, symbol, atomic mass, number of valence electrons, and state of matter.
3) Understanding the periodic table allows one to predict an element's physical and chemical properties and reactions.
The periodic table organizes the chemical elements. It displays elements in columns and rows, with elements in the same column having similar properties. The number of protons, neutrons, and electrons in an atom determine its placement on the periodic table. Elements are classified as metals, non-metals, and metalloids based on their physical and chemical properties. Metals are good conductors of heat and electricity, while non-metals are brittle and poor conductors. The position and number of valence electrons allow prediction of an element's reactivity and bonding abilities.
The document provides information about the periodic table of elements, including:
1) It describes the organization of the periodic table and the properties that can be determined from an element's position.
2) Key information included in each element square is discussed, such as atomic number, symbol, atomic mass, and valence electrons.
3) The properties of metals, non-metals, and metalloids are outlined.
4) The document explains the patterns in the periodic table, including periods and families (groups).
The periodic table organizes the 118 known chemical elements according to their atomic structure and properties, with elements in the same columns having similar traits. Elements can exist individually, combine to form compounds with distinct properties, or be mixed together without bonding. The periodic table provides a framework for understanding elements and predicting how they will react and combine.
The document provides information about the periodic table of elements. It defines key terms like elements, compounds, mixtures and discusses the organization and properties of different groups of elements on the periodic table. The periodic table organizes 118 known elements according to their atomic structure and properties. Elements are grouped into blocks like alkali metals, halogens, noble gases etc. based on their valence electrons and reactivity. The positions of elements in the periodic table can reveal information about their chemical and physical properties.
This document provides an overview of atomic structure and bonding. It discusses subatomic particles like protons, neutrons, and electrons and their properties. It explains how atomic number and mass are determined. Electron arrangement in energy levels is covered, along with ionic and covalent bonding processes. Ionic bonding occurs through the transfer of electrons between atoms, while covalent bonding involves the sharing of electrons between atoms. Common ionic and covalent compounds are listed as examples.
This document discusses the structure and properties of matter at the atomic level. It begins by defining matter as anything that occupies space and has mass, and is composed of tiny discrete particles. It then discusses the kinetic molecular theory and how it relates to the behavior of solids, liquids, and gases. Next, it introduces the atomic structure of elements, including subatomic particles like protons, neutrons, and electrons. It provides properties of these particles and explains how electrons are arranged in shells in an atom. The document concludes by discussing electron configuration and how the arrangement of electrons determines an element's properties.
Mendeleev arranged the elements in order of increasing atomic mass in a periodic table. He noticed that elements with similar properties fell into recurring patterns, allowing him to predict properties of undiscovered elements. Later, Moseley arranged elements by atomic number, better reflecting their properties. The periodic table organizes elements into metals, nonmetals, and metalloids, which have characteristic physical and chemical properties depending on their group and period.
The atomic model has changed significantly over time as scientists have conducted experiments and gained new insights. Democritus first proposed the idea of indivisible "atomos" over 2000 years ago, but this was largely ignored. John Dalton's atomic theory in the 1800s that elements are made of atoms helped establish modern chemistry. J.J. Thomson's experiments led to the discovery of electrons within atoms. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus. Niels Bohr incorporated electrons in specific energy levels around the nucleus. Today's atomic model is based on wave mechanics and electrons having probable locations rather than definite paths.
This document discusses the structure and properties of matter at the atomic level. It begins by defining matter as anything that occupies space and has mass, and is composed of tiny discrete particles. It then discusses the kinetic molecular theory and how it relates to the behavior of solids, liquids, and gases. The rest of the document covers atomic structure, including the historical development of atomic models, the subatomic particles (proton, neutron, electron), electron configuration, and examples of writing out configurations for various elements.
Atoms are the basic building blocks of all matter and are made up of a nucleus containing protons and neutrons surrounded by electrons. John Dalton's atomic theory established that atoms are indivisible and that different elements are composed of different types of atoms. Rutherford discovered that the nucleus is small and dense at the center of the atom, surrounded by electrons. Niels Bohr's model represented electrons orbiting the nucleus in fixed energy levels or shells.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
Thinking of getting a dog? Be aware that breeds like Pit Bulls, Rottweilers, and German Shepherds can be loyal and dangerous. Proper training and socialization are crucial to preventing aggressive behaviors. Ensure safety by understanding their needs and always supervising interactions. Stay safe, and enjoy your furry friends!
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
Physiology and chemistry of skin and pigmentation, hairs, scalp, lips and nail, Cleansing cream, Lotions, Face powders, Face packs, Lipsticks, Bath products, soaps and baby product,
Preparation and standardization of the following : Tonic, Bleaches, Dentifrices and Mouth washes & Tooth Pastes, Cosmetics for Nails.
A Strategic Approach: GenAI in EducationPeter Windle
Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
2. • Introduction
– The periodic table is made up of rows of elements
and columns.
– An element is identified by its chemical symbol.
– The number above the symbol is the atomic number
– The number below the symbol is the rounded
atomic weight of the element.
– A row is called a period
– A column is called a group
3. Organizing the Elements
• Chemists used the properties of
elements to sort them into groups.
• JW. Dobreiner grouped elements into
triads.
• A triad is a set of three elements with
similar properties.
4. Mendeleev’s Periodic Table
• In 1869, a Russian
chemist and
teacher published a
table of the
elements.
• Mendeleev arranged
the elements in the
periodic table in
order of increasing
atomic mass.
5. Henry Moseley
1887 - 1915
In 1913, through his work with X-rays, he
determined the actual nuclear charge
(atomic number) of the elements*. He
rearranged the elements in order of
increasing atomic number.
*“There is in the atom a fundamental
quantity which increases by regular
steps as we pass from each element to
the next. This quantity can only be the
charge on the central positive nucleus.”
6. The Periodic Law
In the modern periodic
table elements are
arranged in order of
increasing atom ic
num ber.
Periodic Law states:
When elements are
arranged in order of
increasing atomic
number, there is a
periodic repetition
of their physical and
chemical properties.
7. • The elements can be grouped into
three broad classes based on their
general properties.
• Three classes of elements are Metals,
Nonmetals, and Metalloids.
• Across a period, the properties of
elements become less metallic and
more nonmetallic.
8. Properties of Metals
• Metals are good conductors
of heat and electricity.
• Metals are shiny.
• Metals are ductile (can be
stretched into thin wires).
• Metals are malleable (can be
pounded into thin sheets).
• A chemical property of metal
is its reaction with water
which results in corrosion.
• Solid at room temperature
except Hg.
9. Properties of Non-Metals
• Non-metals are poor
conductors of heat and
electricity.
• Non-metals are not ductile
or malleable.
• Solid non-metals are
brittle and break easily.
• They are dull.
• Many non-metals are
gases.
Sulfur
10. Properties of Metalloids
• Metalloids (metal-like) have
properties of both metals and
non-metals.
• They are solids that can be
shiny or dull.
• They conduct heat and
electricity better than non-
metals but not as well as
metals.
• They are ductile and
malleable.
Silicon
11. Groups PeriodsGroups Periods
Columns of elements areColumns of elements are
called groups or families.called groups or families.
Elements in each groupElements in each group
have similar but nothave similar but not
identical properties.identical properties.
For example, lithium (Li),For example, lithium (Li),
sodium (Na), potassiumsodium (Na), potassium
(K), and other members of(K), and other members of
group IA are all soft, white,group IA are all soft, white,
shiny metals.shiny metals.
All elements in a groupAll elements in a group
have the same number ofhave the same number of
valence electrons.valence electrons.
Each horizontal row ofEach horizontal row of
elements is called a period.elements is called a period.
The elements in a periodThe elements in a period
are not alike in properties.are not alike in properties.
In fact, the propertiesIn fact, the properties
change greatly across evenchange greatly across even
given row.given row.
The first element in a periodThe first element in a period
is always an extremelyis always an extremely
active solid. The lastactive solid. The last
element in a period, iselement in a period, is
always an inactive gas.always an inactive gas.
12. HydrogenHydrogen
The hydrogen square sits atop group AI, butThe hydrogen square sits atop group AI, but
it is not a member of that group. Hydrogen isit is not a member of that group. Hydrogen is
in a class of its own.in a class of its own.
It’s a gas at room temperature.It’s a gas at room temperature.
It has one proton and one electron in its oneIt has one proton and one electron in its one
and only energy level.and only energy level.
Hydrogen only needs 2 electrons to fill up itsHydrogen only needs 2 electrons to fill up its
valence shell.valence shell.
13. 6.2 Classifying the Elements6.2 Classifying the Elements
The periodic tableThe periodic table
displays the symbolsdisplays the symbols
and names of theand names of the
elements along withelements along with
information about theinformation about the
structure of theirstructure of their
atoms.atoms.
14. Four chemical groupsFour chemical groups
of the periodic table:of the periodic table:
2.2. alkali metals (IA)alkali metals (IA)
3.3. alkaline earth metalsalkaline earth metals
(IIA),(IIA),
4.4. Halogens (VII),Halogens (VII),
5.5. NobleNoble gasesgases (VIIIA).(VIIIA).
15. Alkali MetalsAlkali Metals
The alkali family is found inThe alkali family is found in
the first column of thethe first column of the
periodic table.periodic table.
Atoms of the alkali metalsAtoms of the alkali metals
have a single electron in theirhave a single electron in their
outermost level, in otheroutermost level, in other
words, 1 valence electron.words, 1 valence electron.
They are shiny, have theThey are shiny, have the
consistency of clay, and areconsistency of clay, and are
easily cut with a knife.easily cut with a knife.
16. Alkali MetalsAlkali Metals
They are the mostThey are the most
reactive metals.reactive metals.
They react violentlyThey react violently
with water.with water.
Alkali metals areAlkali metals are
never found as freenever found as free
elements in nature.elements in nature.
They are alwaysThey are always
bonded with anotherbonded with another
element.element.
17. Alkaline Earth MetalsAlkaline Earth Metals
They are never found uncombined in nature.They are never found uncombined in nature.
They have two valence electrons.They have two valence electrons.
Alkaline earth metals include magnesium andAlkaline earth metals include magnesium and
calcium, among others.calcium, among others.
18. Transition MetalsTransition Metals
Transition ElementsTransition Elements
include those elements ininclude those elements in
the B groups.the B groups.
These are the metals youThese are the metals you
are probably mostare probably most
familiar: copper, tin, zinc,familiar: copper, tin, zinc,
iron, nickel, gold, andiron, nickel, gold, and
silver.silver.
They are good conductorsThey are good conductors
of heat and electricity.of heat and electricity.
19. Transition MetalsTransition Metals
The compounds of transition metals are usually brightlyThe compounds of transition metals are usually brightly
colored and are often used to color paints.colored and are often used to color paints.
Transition elements have 1 or 2 valence electrons, whichTransition elements have 1 or 2 valence electrons, which
they lose when they form bonds with other atoms. Somethey lose when they form bonds with other atoms. Some
transition elements can lose electrons in their next-to-transition elements can lose electrons in their next-to-
outermost level.outermost level.
20. Transition ElementsTransition Elements
Transition elementsTransition elements have propertieshave properties
similar to one another and to other metals,similar to one another and to other metals,
but their properties do not fit in with thosebut their properties do not fit in with those
of any other group.of any other group.
Many transition metals combineMany transition metals combine
chemically with oxygen to formchemically with oxygen to form
compounds called oxides.compounds called oxides.
21. Representative ElementsRepresentative Elements
Groups 1A – 7A.Groups 1A – 7A.
Elements are refered to as representativeElements are refered to as representative
elements because they display a wideelements because they display a wide
range of physical and chemical properties.range of physical and chemical properties.
For any representative element, its groupFor any representative element, its group
number equals the number of electrons innumber equals the number of electrons in
the highest occupied energy level.the highest occupied energy level.
22. Trends in the periodicTrends in the periodic
table:table:
Ionization EnergyIonization Energy
Atomic RadiusAtomic Radius
Electron AffinityElectron Affinity
ElectronegativityElectronegativity
23. Sizes of AtomsSizes of Atoms
The bonding atomicThe bonding atomic
radius is defined asradius is defined as
one-half of theone-half of the
distance betweendistance between
covalently bondedcovalently bonded
nuclei.nuclei.
24. Atomic Radius TrendAtomic Radius Trend
Group Trend – As you goGroup Trend – As you go down a columndown a column,,
atomic radius increases.atomic radius increases.
As you go down, eAs you go down, e--
are filled into orbitals that areare filled into orbitals that are
farther away from the nucleus (attraction notfarther away from the nucleus (attraction not
as strong).as strong).
Periodic Trend – As you goPeriodic Trend – As you go across a periodacross a period (L(L
to R),to R), atomic radius decreases.atomic radius decreases.
As you go L to R, eAs you go L to R, e--
are put into the same orbital,are put into the same orbital,
but more pbut more p++
and eand e--
total (more attraction =total (more attraction =
smaller size).smaller size).
27. Ionic Radius TrendIonic Radius Trend
MetalsMetals – lose e– lose e--
, which means more p, which means more p++
than ethan e--
(more attraction) SO…(more attraction) SO…
Ionic RadiusIonic Radius << Neutral Atomic RadiusNeutral Atomic Radius
NonmetalsNonmetals – gain e– gain e--
, which means more e, which means more e--
than pthan p++
(not as much attraction) SO…(not as much attraction) SO…
Ionic RadiusIonic Radius >> Neutral Atomic RadiusNeutral Atomic Radius
28. Sizes of IonsSizes of Ions
Ionic size dependsIonic size depends
upon:upon:
Nuclear charge.Nuclear charge.
Number ofNumber of
electrons.electrons.
Orbitals in whichOrbitals in which
electrons reside.electrons reside.
29. Sizes of IonsSizes of Ions
Cations areCations are
smaller than theirsmaller than their
parent atoms.parent atoms.
The outermostThe outermost
electron iselectron is
removed andremoved and
repulsions arerepulsions are
reduced.reduced.
30. Sizes of IonsSizes of Ions
Anions are largerAnions are larger
than their parentthan their parent
atoms.atoms.
Electrons areElectrons are
added andadded and
repulsions arerepulsions are
increased.increased.
31. Sizes of IonsSizes of Ions
Ions increase in sizeIons increase in size
as you go down aas you go down a
column.column.
Due to increasingDue to increasing
value ofvalue of nn..
32. Metals versus NonmetalsMetals versus Nonmetals
Metals tend to form cations.Metals tend to form cations.
Nonmetals tend to form anions.Nonmetals tend to form anions.
33. BackgroundBackground
Electrons can jump between shells (Bohr’sElectrons can jump between shells (Bohr’s
model supported by line spectra)model supported by line spectra)
The electrons can be pushed so far thatThe electrons can be pushed so far that
they escape the attraction of the nucleusthey escape the attraction of the nucleus
Losing an electron is called ionizationLosing an electron is called ionization
An ion is an atom that has either a netAn ion is an atom that has either a net
positive or net negative chargepositive or net negative charge
Q: what would the charge be on an atomQ: what would the charge be on an atom
that lost an electron? Gained two electrons?that lost an electron? Gained two electrons?
A: +1 (because yourA: +1 (because your losinglosing a -ve electron)a -ve electron)
A: -2 (because you gain 2 -ve electrons)A: -2 (because you gain 2 -ve electrons)
34. Ionization EnergyIonization Energy
Amount of energy required to remove anAmount of energy required to remove an
electron from the ground state of aelectron from the ground state of a
gaseous atom or ion.gaseous atom or ion.
First ionization energy is that energy requiredFirst ionization energy is that energy required
to remove first electron.to remove first electron.
Second ionization energy is that energySecond ionization energy is that energy
required to remove second electron, etc.required to remove second electron, etc.
35. Ionization EnergyIonization Energy
Group Trend – As you goGroup Trend – As you go down a columndown a column,,
ionization energy decreases.ionization energy decreases.
As you go down, atomic size is increasing (lessAs you go down, atomic size is increasing (less
attraction), so easier to remove an eattraction), so easier to remove an e--
..
Periodic Trend – As you goPeriodic Trend – As you go across a periodacross a period (L to(L to
R),R), ionization energy increases.ionization energy increases.
As you go L to R, atomic size is decreasing (moreAs you go L to R, atomic size is decreasing (more
attraction), so more difficult to remove an eattraction), so more difficult to remove an e--
(also, metals want to lose e(also, metals want to lose e--
, but nonmetals do, but nonmetals do
not).not).
36. Ionization EnergyIonization Energy
It requires more energy to remove eachIt requires more energy to remove each
successive electron.successive electron.
When all valence electrons have been removed,When all valence electrons have been removed,
the ionization energy takes a quantum leap.the ionization energy takes a quantum leap.
37. Trends in First IonizationTrends in First Ionization
EnergiesEnergies
As one goes down aAs one goes down a
column, less energycolumn, less energy
is required to removeis required to remove
the first electron.the first electron.
For atoms in the sameFor atoms in the same
group,group, ZZeffeff is essentiallyis essentially
the same, but thethe same, but the
valence electrons arevalence electrons are
farther from thefarther from the
nucleus.nucleus.
39. Electronegativity TrendElectronegativity Trend
Group Trend – As you goGroup Trend – As you go down a columndown a column,,
electronegativity decreases.electronegativity decreases.
As you go down, atomic size is increasing, so lessAs you go down, atomic size is increasing, so less
attraction to its own eattraction to its own e--
and other atom’s eand other atom’s e--
..
Periodic Trend – As you goPeriodic Trend – As you go across a periodacross a period (L to R),(L to R),
electronegativity increases.electronegativity increases.
As you go L to R, atomic size is decreasing, so there isAs you go L to R, atomic size is decreasing, so there is
more attraction to its own emore attraction to its own e--
and other atom’s eand other atom’s e--
..