The document discusses atomic structure and the periodic table. It describes how atoms are made up of subatomic particles including protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit in energy shells around the nucleus. The atomic number is the number of protons, and the mass number is the total number of protons and neutrons. Elements are arranged in the periodic table based on their atomic structure and properties. Metals are located on the left side and are generally solids, while non-metals are on the right side and can be solids or gases.
An ion is an atom or molecule which has lost or gained one or more valence electrons, giving it a positive or negative electrical charge
Ions are formed by the loss or gain of electrons by single atoms or groups of atoms.
This presentation was put together by Ivan Ukiwah.
The document provides information about the four fundamental forces and particles that make up everything in the universe:
1) Gravity and magnetism are the two forces that act on matter and charged particles respectively. Gravity always pulls while magnetism can pull or push.
2) All matter is made up of fundamental particles called protons, neutrons, and electrons that combine to form atoms. Protons and neutrons are found in the nucleus while electrons orbit around the nucleus.
3) Atoms can combine to form molecules, and everything in the universe from people to planets are made up of these fundamental forces and particles.
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
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 document summarizes key concepts about the periodic table, including:
1) The periodic table organizes elements horizontally by period and vertically by group, with elements in the same group having similar properties.
2) Elements are classified as metals, nonmetals, and metalloids based on their properties, with metals generally conducting heat/electricity and nonmetals not.
3) Periodic trends show atomic radius decreases but ionization energy, electronegativity, and ionic size increase moving left to right across a period.
The document discusses the key concepts of elements, atoms, ions, and the periodic table. It covers early atomic theories proposed by scientists like Dalton, Thomson, and Rutherford. Key discoveries included that atoms are made up of a tiny, dense nucleus surrounded by electrons. The periodic table organizes elements by increasing atomic number and groups elements with similar properties together. Elements can form ions by gaining or losing electrons to become charged particles like cations and anions. Ionic compounds are formed from the attraction between oppositely charged ions.
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
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
An ion is an atom or molecule which has lost or gained one or more valence electrons, giving it a positive or negative electrical charge
Ions are formed by the loss or gain of electrons by single atoms or groups of atoms.
This presentation was put together by Ivan Ukiwah.
The document provides information about the four fundamental forces and particles that make up everything in the universe:
1) Gravity and magnetism are the two forces that act on matter and charged particles respectively. Gravity always pulls while magnetism can pull or push.
2) All matter is made up of fundamental particles called protons, neutrons, and electrons that combine to form atoms. Protons and neutrons are found in the nucleus while electrons orbit around the nucleus.
3) Atoms can combine to form molecules, and everything in the universe from people to planets are made up of these fundamental forces and particles.
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
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 document summarizes key concepts about the periodic table, including:
1) The periodic table organizes elements horizontally by period and vertically by group, with elements in the same group having similar properties.
2) Elements are classified as metals, nonmetals, and metalloids based on their properties, with metals generally conducting heat/electricity and nonmetals not.
3) Periodic trends show atomic radius decreases but ionization energy, electronegativity, and ionic size increase moving left to right across a period.
The document discusses the key concepts of elements, atoms, ions, and the periodic table. It covers early atomic theories proposed by scientists like Dalton, Thomson, and Rutherford. Key discoveries included that atoms are made up of a tiny, dense nucleus surrounded by electrons. The periodic table organizes elements by increasing atomic number and groups elements with similar properties together. Elements can form ions by gaining or losing electrons to become charged particles like cations and anions. Ionic compounds are formed from the attraction between oppositely charged ions.
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
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
Isotopes are atoms of the same element that have different numbers of neutrons, while ions are atoms or groups of atoms that have gained or lost electrons, giving them a positive or negative charge. Ions are formed by gaining or losing electrons, not protons. Cations are positively charged ions formed when atoms lose electrons, such as metals, while anions are negatively charged ions formed when nonmetals gain electrons. The periodic table can be used to predict which elements will form cations or anions based on their group.
1. Atomic radius increases down and to the left on the periodic table due to increasing nuclear charge pulling electrons closer to the nucleus. Silicon has a larger atomic radius than sulfur. Sodium has a larger atomic radius than potassium.
2. Ionization energy increases up and to the right on the periodic table due to increasing nuclear charge holding electrons more tightly. Francium has the lowest ionization energy while helium has the highest. Phosphorus has a higher ionization energy than aluminum. Calcium has a lower ionization energy than strontium.
3. Electronegativity increases up and to the right on the periodic table. Fluorine has the highest electronegativity while francium has
The document describes different structures of pure substances and how their structure determines physical properties. Ionic substances form crystal structures of positively and negatively charged ions with strong bonds, giving them high melting points and ability to conduct electricity when molten or dissolved. Metallic substances have strong atomic bonds and free electrons, making them conductors. Giant molecular and simple molecular substances have covalent bonds that result in high and low melting points respectively. Graphite has strong in-plane bonds but weak between-plane bonds, making it soft and able to conduct. Structure determines properties like melting point, strength, and conductivity.
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.
This document summarizes key concepts from Chapter 7 on ionic and metallic bonding. It discusses how valence electrons determine an element's chemical properties. Ions form when atoms gain or lose electrons to achieve stable noble gas configurations. Ionic compounds consist of cation and anion ions with opposite charges that are attracted via ionic bonds. Metals form crystalline structures with mobile valence electrons that provide conductivity and malleability. Alloys combine elements to produce superior properties.
This document summarizes key concepts about atomic structure from Chapter 4. It discusses early atomic models proposed by Democritus and Dalton. Dalton's atomic theory stated that all matter is made of atoms that cannot be divided further. The document then explains discoveries of subatomic particles like electrons, protons, and neutrons. It describes Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus. Finally, it defines atomic number, mass number, isotopes, and how average atomic masses are calculated based on isotope abundances.
Hello everyone, I am Dr. Ujwalkumar Trivedi, Head of Biotechnology Department at Marwadi University Rajkot. I teach Molecular Biology to the students of M.Sc. Microbiology and Biotechnology.
The current presentation is about the historical perspectives of the discovery of atoms and subatomic particles. The later part of the presentation describes various atomic models and the properties of subatomic particles with a description of commonly used terms like molecules, ions and compounds.
The periodic table organizes elements by atomic number and recurring chemical properties. Elements are grouped into rows called periods and columns called groups based on their atomic structure and how they gain, lose or share electrons to form bonds. The location of an element on the periodic table can provide information about its physical and chemical properties.
This document provides an overview of physical science concepts related to subatomic particles, the periodic table, oxidation numbers, and Lewis dot diagrams. The key points are:
1) It reviews subatomic particles, periods and groups of the periodic table, and electron configurations.
2) The objective is to predict oxidation numbers and draw Lewis dot diagrams by understanding valence electrons.
3) It defines valence electrons, oxidation numbers, and ionic bonds in chemical compounds.
4) Examples are given of writing chemical symbols, determining valence electrons, and drawing Lewis dot diagrams using the cross method.
This document discusses ion formation and naming ions. It explains that atoms become ions by gaining or losing electrons to obtain a full outer electron shell of 8 electrons. It gives examples of common monatomic cations such as K+, Ca2+, and Al3+ and anions such as S2-, O2-, Br-, and N3-. The document also provides guidelines for naming ions, indicating that positive ions are called cations and named after the element, while negative ions are called anions and named by taking the element root and adding -ide.
Transition metals have electrons in their incomplete d-subshells that allow them to form stable ions. They exhibit several key properties including variable oxidation states due to similar energy levels of the 4s and 3d orbitals, paramagnetism from unpaired electrons, colored compounds from d-d transitions of electrons between orbitals split by ligands, and the ability to act as catalysts by changing oxidation states. Transition metals can form various types of complexes with ligands that bond through dative covalent bonds, including monodentate, bidentate, and polydentate ligands, which determine the coordination number and shape of the complex ion.
The document discusses the atomic theory of matter and the development of atomic structure models. It describes John Dalton's atomic theory which stated that elements are composed of atoms that are unique and atoms are neither created nor destroyed in chemical reactions. The discovery of the electron by J.J. Thompson and experiments by Robert Millikan and Ernest Rutherford helped develop the modern atomic structure model of a small, dense nucleus surrounded by electrons. The document also discusses isotopes, atomic numbers, mass numbers, and how the periodic table is arranged based on atomic structure.
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 organizes elements by their atomic number and properties. Elements are grouped together based on their proton number and electron configuration. Groups are columns that elements fall into from left to right, with elements in the same group having similar properties. Periods run from top to bottom, with elements in the same period having the same number of electron shells. Most elements to the left of the zigzag line are metals that are shiny, good conductors with high melting points; nonmetals are to the right and have opposite properties. Transition metals between groups 3-12 have properties of both metals and nonmetals.
Grade 8 Chemistry Structure of Matter : Atoms, Molecules and IonsSaraChehab
- The atom is the basic building block of all matter and is composed of subatomic particles like protons, neutrons and electrons.
- Atoms of different elements are distinguished by their number of protons.
- Molecules are formed when atoms bond together and can be made of two or more atoms of the same or different elements.
- Ions are formed when atoms gain or lose electrons, resulting in a positive or negative charge. Cations are positively charged while anions are negatively charged.
The document introduces the periodic table and discusses how it is organized. It explains that elements are arranged by atomic number vertically into groups and horizontally into periods. [The document] instructs the reader to draw electron configuration diagrams for the first 20 elements and observe that elements in the same group have the same number of valence electrons. It also notes that elements in the same period have the same number of electron shells. In conclusion, [the document] emphasizes that the number and arrangement of valence electrons determines how an element bonds and reacts chemically.
The periodic table arranges elements in order of increasing atomic number. Elements are placed in blocks based on their outer electron configurations (s, p, d, f). Elements in the same group have similar properties due to their outer shell electrons. Properties trend periodically across periods and groups due to changing nuclear charge and electron shielding. Metals generally have high melting points due to delocalized electrons, while nonmetals have covalent or weak van der Waals bonding and lower melting points. Ionization energy increases down groups and across periods as it is harder to remove electrons.
Portfolio containing creative copy writing by Sohailسہیل احمد صدیقی
I've only shortlisted samples of my Creative writing, done for my present agency, Ogilvy & Mather Pakistan, Karachi and my previous agency, VAMS+ some freelance.
The document provides 10 reasons for wanting an iPhone for Christmas. It argues that the requester will do chores, volunteer work, rub feet or backs without pay, and only order water at restaurants. It also notes the current phone has problems and an iPhone would be easier to contact and care for. Finally, it suggests selling an iPod Nano to help pay and this could serve as multiple gift occasions.
Isotopes are atoms of the same element that have different numbers of neutrons, while ions are atoms or groups of atoms that have gained or lost electrons, giving them a positive or negative charge. Ions are formed by gaining or losing electrons, not protons. Cations are positively charged ions formed when atoms lose electrons, such as metals, while anions are negatively charged ions formed when nonmetals gain electrons. The periodic table can be used to predict which elements will form cations or anions based on their group.
1. Atomic radius increases down and to the left on the periodic table due to increasing nuclear charge pulling electrons closer to the nucleus. Silicon has a larger atomic radius than sulfur. Sodium has a larger atomic radius than potassium.
2. Ionization energy increases up and to the right on the periodic table due to increasing nuclear charge holding electrons more tightly. Francium has the lowest ionization energy while helium has the highest. Phosphorus has a higher ionization energy than aluminum. Calcium has a lower ionization energy than strontium.
3. Electronegativity increases up and to the right on the periodic table. Fluorine has the highest electronegativity while francium has
The document describes different structures of pure substances and how their structure determines physical properties. Ionic substances form crystal structures of positively and negatively charged ions with strong bonds, giving them high melting points and ability to conduct electricity when molten or dissolved. Metallic substances have strong atomic bonds and free electrons, making them conductors. Giant molecular and simple molecular substances have covalent bonds that result in high and low melting points respectively. Graphite has strong in-plane bonds but weak between-plane bonds, making it soft and able to conduct. Structure determines properties like melting point, strength, and conductivity.
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.
This document summarizes key concepts from Chapter 7 on ionic and metallic bonding. It discusses how valence electrons determine an element's chemical properties. Ions form when atoms gain or lose electrons to achieve stable noble gas configurations. Ionic compounds consist of cation and anion ions with opposite charges that are attracted via ionic bonds. Metals form crystalline structures with mobile valence electrons that provide conductivity and malleability. Alloys combine elements to produce superior properties.
This document summarizes key concepts about atomic structure from Chapter 4. It discusses early atomic models proposed by Democritus and Dalton. Dalton's atomic theory stated that all matter is made of atoms that cannot be divided further. The document then explains discoveries of subatomic particles like electrons, protons, and neutrons. It describes Rutherford's gold foil experiment which showed that atoms have a small, dense nucleus. Finally, it defines atomic number, mass number, isotopes, and how average atomic masses are calculated based on isotope abundances.
Hello everyone, I am Dr. Ujwalkumar Trivedi, Head of Biotechnology Department at Marwadi University Rajkot. I teach Molecular Biology to the students of M.Sc. Microbiology and Biotechnology.
The current presentation is about the historical perspectives of the discovery of atoms and subatomic particles. The later part of the presentation describes various atomic models and the properties of subatomic particles with a description of commonly used terms like molecules, ions and compounds.
The periodic table organizes elements by atomic number and recurring chemical properties. Elements are grouped into rows called periods and columns called groups based on their atomic structure and how they gain, lose or share electrons to form bonds. The location of an element on the periodic table can provide information about its physical and chemical properties.
This document provides an overview of physical science concepts related to subatomic particles, the periodic table, oxidation numbers, and Lewis dot diagrams. The key points are:
1) It reviews subatomic particles, periods and groups of the periodic table, and electron configurations.
2) The objective is to predict oxidation numbers and draw Lewis dot diagrams by understanding valence electrons.
3) It defines valence electrons, oxidation numbers, and ionic bonds in chemical compounds.
4) Examples are given of writing chemical symbols, determining valence electrons, and drawing Lewis dot diagrams using the cross method.
This document discusses ion formation and naming ions. It explains that atoms become ions by gaining or losing electrons to obtain a full outer electron shell of 8 electrons. It gives examples of common monatomic cations such as K+, Ca2+, and Al3+ and anions such as S2-, O2-, Br-, and N3-. The document also provides guidelines for naming ions, indicating that positive ions are called cations and named after the element, while negative ions are called anions and named by taking the element root and adding -ide.
Transition metals have electrons in their incomplete d-subshells that allow them to form stable ions. They exhibit several key properties including variable oxidation states due to similar energy levels of the 4s and 3d orbitals, paramagnetism from unpaired electrons, colored compounds from d-d transitions of electrons between orbitals split by ligands, and the ability to act as catalysts by changing oxidation states. Transition metals can form various types of complexes with ligands that bond through dative covalent bonds, including monodentate, bidentate, and polydentate ligands, which determine the coordination number and shape of the complex ion.
The document discusses the atomic theory of matter and the development of atomic structure models. It describes John Dalton's atomic theory which stated that elements are composed of atoms that are unique and atoms are neither created nor destroyed in chemical reactions. The discovery of the electron by J.J. Thompson and experiments by Robert Millikan and Ernest Rutherford helped develop the modern atomic structure model of a small, dense nucleus surrounded by electrons. The document also discusses isotopes, atomic numbers, mass numbers, and how the periodic table is arranged based on atomic structure.
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 organizes elements by their atomic number and properties. Elements are grouped together based on their proton number and electron configuration. Groups are columns that elements fall into from left to right, with elements in the same group having similar properties. Periods run from top to bottom, with elements in the same period having the same number of electron shells. Most elements to the left of the zigzag line are metals that are shiny, good conductors with high melting points; nonmetals are to the right and have opposite properties. Transition metals between groups 3-12 have properties of both metals and nonmetals.
Grade 8 Chemistry Structure of Matter : Atoms, Molecules and IonsSaraChehab
- The atom is the basic building block of all matter and is composed of subatomic particles like protons, neutrons and electrons.
- Atoms of different elements are distinguished by their number of protons.
- Molecules are formed when atoms bond together and can be made of two or more atoms of the same or different elements.
- Ions are formed when atoms gain or lose electrons, resulting in a positive or negative charge. Cations are positively charged while anions are negatively charged.
The document introduces the periodic table and discusses how it is organized. It explains that elements are arranged by atomic number vertically into groups and horizontally into periods. [The document] instructs the reader to draw electron configuration diagrams for the first 20 elements and observe that elements in the same group have the same number of valence electrons. It also notes that elements in the same period have the same number of electron shells. In conclusion, [the document] emphasizes that the number and arrangement of valence electrons determines how an element bonds and reacts chemically.
The periodic table arranges elements in order of increasing atomic number. Elements are placed in blocks based on their outer electron configurations (s, p, d, f). Elements in the same group have similar properties due to their outer shell electrons. Properties trend periodically across periods and groups due to changing nuclear charge and electron shielding. Metals generally have high melting points due to delocalized electrons, while nonmetals have covalent or weak van der Waals bonding and lower melting points. Ionization energy increases down groups and across periods as it is harder to remove electrons.
Portfolio containing creative copy writing by Sohailسہیل احمد صدیقی
I've only shortlisted samples of my Creative writing, done for my present agency, Ogilvy & Mather Pakistan, Karachi and my previous agency, VAMS+ some freelance.
The document provides 10 reasons for wanting an iPhone for Christmas. It argues that the requester will do chores, volunteer work, rub feet or backs without pay, and only order water at restaurants. It also notes the current phone has problems and an iPhone would be easier to contact and care for. Finally, it suggests selling an iPod Nano to help pay and this could serve as multiple gift occasions.
Atomic structure consists of subatomic particles including protons, neutrons, and electrons. Atoms have a nucleus composed of protons and neutrons surrounded by electrons in energy shells. The number of protons determines the element, while the number of neutrons distinguishes isotopes of that element. Elements exhibit trends in properties across periods and down groups in the periodic table due to their atomic structure and configuration of electrons.
Alternative Housing Pilot Program Expansion AlternativesJorge Quintero
Following Hurricane Katrina, the State of Mississippi was awarded a grant from the FEMA-funded Alternative Housing Pilot Program (AHPP) to develop a prototype alternative disaster housing unit. In my role as a Housing Recovery Specialist for FEMA in Mississippi, I designed a number expansion options to those units to allow them to function as permanent housing and promote greater acceptance by the local community. Several of these expansion designs where successfully built by local Habitat for Humanity affiliates. For more information, go to www.association.net
The document provides an overview of mutual funds in India, including:
1) It defines mutual funds as pooled investment funds that allow investors to invest in a diversified portfolio managed by fund managers.
2) It describes the structure of mutual funds in India including sponsors, trustees, asset management companies, custodians, and SEBI regulations.
3) It outlines different types of mutual fund schemes according to structure, investment objectives, and maturity periods.
El documento ofrece consejos para mejorar la autoconfianza, incluyendo arreglar la apariencia, conocerse a sí mismo, vestirse bien, pensar y actuar de manera positiva, prepararse para las tareas, hablar lento y pararse derecho. La autoconfianza se define como creer en la propia capacidad para lograr metas y actuar de forma adecuada.
Here you could find the complete Wordpress's localhost technical installation for Windows and Mac's users
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O documento é sobre um evento chamado "Dia da Biblioteca" que ocorreu em 24 de outubro de 2013, mas não fornece mais detalhes sobre o que aconteceu nesse dia ou quais atividades foram realizadas.
Organo Gold is a network marketing company that sells coffee, tea, and other beverage products. The company promotes its products as using ganoderma lucidum, a mushroom claimed to have health benefits. This document is a website that appears to promote joining the Organo Gold business opportunity and selling its products.
This document provides an overview of Organo Gold Philippines and its multi-level marketing business opportunity. In 3 sentences:
Organo Gold is an MLM company founded in 2008 that sells wellness products enhanced with ganoderma lucidum mushrooms. It has a global network in over 35 countries and offers a lucrative compensation plan with 7 ways to earn including retail profits, bonuses, and incentives like cars for high-ranking distributors. The company provides regular training and support for distributors to help them succeed with the business opportunity.
The document summarizes key aspects of the periodic table, including its organization into periods and groups based on atomic number and electron configuration. Elements within the same group share similar chemical properties due to having the same number of valence electrons. Metals are divided into groups such as alkali metals, alkaline earth metals, and transition metals based on their properties. Nonmetals are poor conductors of heat and electricity, while metalloids have some properties of metals and nonmetals.
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.
The document summarizes key concepts about the periodic table, including:
(1) Elements are arranged vertically in groups based on their outer electron configuration and horizontally in periods based on the number of electron shells.
(2) Chemical groups such as the alkali metals (Group IA), alkaline earth metals (Group IIA), halogens (Group VII), and noble gases (Group VIIIA) have characteristic properties due to their outer electron configuration.
(3) Atoms consist of a nucleus of protons and neutrons surrounded by electrons arranged in shells. The number of protons determines the element. Isotopes are atoms of the same element with different numbers of neutrons.
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.
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 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.
This document discusses the organization and properties of elements in the periodic table. It describes how elements are organized into periods and groups based on their electron configuration. Elements within the same group have similar chemical properties because they have the same number of valence electrons. It also distinguishes between metals, nonmetals, and metalloids, and discusses some representative properties and common elements in various groups of the periodic table.
- The periodic table arranges elements vertically into groups and horizontally into periods based on their atomic structure.
- Elements in the same group have similar properties because they have the same number of electrons in their outer shell. Elements in the same period have the same number of electron shells.
- The periodic table is divided into metals, nonmetals, and metalloids. Metals are usually solids and conduct electricity well. Nonmetals are usually brittle and do not conduct electricity well.
- Atoms can form ions by gaining or losing electrons to fill their outer shell. Cations are positively charged ions formed when atoms lose electrons. Anions are negatively charged ions formed when atoms gain electrons.
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 discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
The document discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
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 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 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.
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.
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This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
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إضغ بين إيديكم من أقوى الملازم التي صممتها
ملزمة تشريح الجهاز الهيكلي (نظري 3)
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تتميز هذهِ الملزمة بعِدة مُميزات :
1- مُترجمة ترجمة تُناسب جميع المستويات
2- تحتوي على 78 رسم توضيحي لكل كلمة موجودة بالملزمة (لكل كلمة !!!!)
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3- دقة الكتابة والصور عالية جداً جداً جداً
4- هُنالك بعض المعلومات تم توضيحها بشكل تفصيلي جداً (تُعتبر لدى الطالب أو الطالبة بإنها معلومات مُبهمة ومع ذلك تم توضيح هذهِ المعلومات المُبهمة بشكل تفصيلي جداً
5- الملزمة تشرح نفسها ب نفسها بس تكلك تعال اقراني
6- تحتوي الملزمة في اول سلايد على خارطة تتضمن جميع تفرُعات معلومات الجهاز الهيكلي المذكورة في هذهِ الملزمة
واخيراً هذهِ الملزمة حلالٌ عليكم وإتمنى منكم إن تدعولي بالخير والصحة والعافية فقط
كل التوفيق زملائي وزميلاتي ، زميلكم محمد الذهبي 💊💊
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How Barcodes Can Be Leveraged Within Odoo 17Celine George
In this presentation, we will explore how barcodes can be leveraged within Odoo 17 to streamline our manufacturing processes. We will cover the configuration steps, how to utilize barcodes in different manufacturing scenarios, and the overall benefits of implementing this technology.
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Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...indexPub
The recent surge in pro-Palestine student activism has prompted significant responses from universities, ranging from negotiations and divestment commitments to increased transparency about investments in companies supporting the war on Gaza. This activism has led to the cessation of student encampments but also highlighted the substantial sacrifices made by students, including academic disruptions and personal risks. The primary drivers of these protests are poor university administration, lack of transparency, and inadequate communication between officials and students. This study examines the profound emotional, psychological, and professional impacts on students engaged in pro-Palestine protests, focusing on Generation Z's (Gen-Z) activism dynamics. This paper explores the significant sacrifices made by these students and even the professors supporting the pro-Palestine movement, with a focus on recent global movements. Through an in-depth analysis of printed and electronic media, the study examines the impacts of these sacrifices on the academic and personal lives of those involved. The paper highlights examples from various universities, demonstrating student activism's long-term and short-term effects, including disciplinary actions, social backlash, and career implications. The researchers also explore the broader implications of student sacrifices. The findings reveal that these sacrifices are driven by a profound commitment to justice and human rights, and are influenced by the increasing availability of information, peer interactions, and personal convictions. The study also discusses the broader implications of this activism, comparing it to historical precedents and assessing its potential to influence policy and public opinion. The emotional and psychological toll on student activists is significant, but their sense of purpose and community support mitigates some of these challenges. However, the researchers call for acknowledging the broader Impact of these sacrifices on the future global movement of FreePalestine.
THE SACRIFICE HOW PRO-PALESTINE PROTESTS STUDENTS ARE SACRIFICING TO CHANGE T...
Atomic structure
1. :Atomic structure:
Atomic Structure and Periodic Table Earlier, we’ve studied that elements are the purest substances
of all. And each element has its own type of atoms. When scientists first discovered the atom, they
believed it was a spherical structure like marbles. Later on other scientists discovered that there
the
Atom is made up of even smaller sub-atomic particles.
It was discovered that an atom is made up of three types of sub-atomic particles; these are
protons, neutrons and electrons.
It was also discovered that in the center of an atom, there is a Nucleus which is made up of protons
and neutrons.
Around the nucleus there are energy shells in which electrons are. Electrons are always orbiting the
nucleus in the energy shells.
Protons and Neutrons are said to be Nucleons because together they make the nucleus. Each type
of these sub-atomic particles has its own physical properties which are explained in this table:
Particle Symbol Mass Charge
Proton p 1 +1
Neutron n 1 no charge
Electron e 1/2000 (Negligible) -1
These physical properties tell us several factors:
The mass of the atom is concentrated in the nucleus; this is because the mass of an electron is
negligible,
A neutron has no charge, it is neutral, an atom is also neutral; this is because it always contains
as much positive protons as negative electrons.
The mass of the sub-atomic particles is in atomic mass unit (AMU). This is because they are so
light that they can’t be measured in grams.
There are two numbers given to each type of atoms:
2. Atomic/Proton Number: it is the number of protons in an atom. And since an atom has an equal
number of protons and electrons, it is the number of electrons in the atom too.
Mass/Nucleon Number: it is the number of protons + number of nucleons in the nucleus of an
atom. It is called mass number because its value is also mass of the atom.
The atomic number is the number of protons, and the mass number is the number of protons
and neutrons.
No. of neutrons =Atomic no. – Mass no. (A-Z)
Mass no. =A & Atomic no. =Z
The mass number goes above the symbol and the atomic number goes below the symbol.
For example:
This represents the sodium Atom,
Its symbol is Na,
Its mass number is 24,
Its atomic number is 11,
It has 11 protons, 13 neutrons (24 - 11 = 13), and 11 electrons.
Always remember that:
An atom has an equal number of positive protons and negative electrons which makes it neutral
in charge
The Electronic Configuration of Atoms:
Electrons are arranged in energy shells or energy levels. But each energy shell can hold up to a
certain amount of electrons.
1st energy shell holds up to 2e,
2nd energy shell holds up to 8e,
3. 3rd energy shell holds up to 18e, but stable with only 8e.
If an atom has its 3rd energy shell holding 8e, if it receives 2 more they go to the 4th energy
shell. If further 10e are received, they go to the 3rd energy shell making it saturated with 18e.
Valency electrons are the electrons in the outer most energy shell.
Electronic arrangements in some elements:
Carbon Lithium
The Ion:
During chemical reactions involving two or more atoms, some types of atoms lose one or more
electron turning into a positive ion. It is called a positive ion because when it loses electrons, the
number of positive protons becomes larger than the number of negative electrons, so the overall
charge of the particle is positive. If it loses two electrons its charge will be +2. If it loses 3, its charge
will be +3 and so on.
Other types of atoms gain the electrons lost by the positive ions. In this case they become negative
ions. This is because the number of negative electrons becomes larger than the number of positive
protons, making the overall charge of the ion negative. If it gains two electrons its charge becomes
-2. If it gains 3 electrons its charge becomes -3, and so on.
The Isotope:
Only that they have a different number of neutrons. Chlorine for example has two isotopes,
Chlorine-35 and Chlorine-37. Isotopes of the same elements do not differ in Behavior or anything,
only their masses differ, as a result of having a different number of neutrons.
There are two kinds of isotopes, stable ones and unstable ones. Unstable ones have a lot of
neutrons, and they are radioactive. They are called radioisotopes.
4. Calculating the Relative Atomic Mass (Ar):
The relative atomic mass of an element is the average mass of all its isotopes compared to one-
twelfth the mass of an atom of Carbon-12.
The rule of calculating the Ar of an element is:
M is the mass number
If we have two isotopes of Chlorine; Chlorine-35 and Chlorine 37. The percentage of abundance of
these two isotopes in the world is 75% and 25% respectively. We could calculate the Ar by:
:The Periodic Table of Elements:
The periodic table is a table containing all elements arranged in ascending order from the one with
lowest atomic number to the one with highest atomic number.
There are there are 8 vertical groups (Columns) in the periodic table. The group number is equal to
the number of electrons in the outer most energy shell of the atoms of the elements in the
group. This is why elements of the same group share the same chemical properties.
There are seven horizontal periods (rows) in the periodic table. The period number is also the
number of occupied energy shells in the atoms of the elements in the period.
So if an element has 3 valence electrons, it will be in group 3. And if it has 4 occupied energy
shells, it will be in period 4.
We have two types of elements in the periodic table. These are Metals and Non-metals. As we
move in the periodic table from the left to the right, the metallic properties of elements decrease.
Metals include Magnesium, Calcium, and Sodium. Non-metals include Carbon, Oxygen and
Chlorine. All metals are solid. All non-metals are either solid or gas, except for bromine which is
liquid.
5. Silver appears as a lustrous white metal Bromine is a non-metal
Metals and non-metals have different Physical properties:
Physical Property: Metals Non-Metals
State In Room temperature Solid (Except Mercury, Liquid) Solid-Gas (Except Bromine, liquid)
Density Very Dense (Except Group 1) Low Density
Appearance Shiny, Most Are Grey Except Most Are Dull (Except Diamond)
Copper And Gold
Melting Point High (Except Groups 1 & 2) Low (Except Diamond-Graphite)
Boiling Point High (Except Groups 1 & 2) Low (Except Diamond-Graphite)
Malleability Hard and Malleable Soft and Brittle
Ductility Ductile Not Ductile
Electrical Conductivity Conductors Poor Conductors (Except Graphite-Silicon)
Heat Conductivity Good Very Poor
Sonority Sonorous Non-Sonorous
Malleability: If a metal is malleable it means it can be hammered into shapes without being broken.
Ductility: If a metal is Ductile it means it can be pulled into wires.
Sonority: If a metal is sonorous, it means it makes a pleasant sound when struck.
Metals and non-metals also differ in chemical properties:
6. Metals Non-Metals
They have either 1,2 or 3 valence electrons They have either 4,5,6,7 or 8 valence electrons.
Except helium which has 2.
They lose electrons forming positive ions They gain electrons forming negative ions
They are reducing agents They are oxidizing agentsThey form basic or
amphoteric compounds They form acidic or neutral compounds
Forms ionic compounds with non-metals Form either ionic compounds with metals, or covalent
compounds with other non-metals
Special Elements:
Alkali Metals:
These elements lie in group 1 of the periodic table. They are Lithium, Sodium, Potassium,
Rubidium, Cesium and Francium (radioactive). We will study the properties of the first three;
Lithium, Sodium and Potassium. Like any metals they are all good conductors of heat and
electricity. They are however, soft. Lithium is the hardest of them and potassium is the softest.
They are extremely reactive; they have to be stored away from any air or water. They have low
densities and melting points.
For this group, the further you go down the more reactive the metals become, this is the most
reactive group
They react with oxygen or air forming a metal oxide:
4Li(Lithium) + O2(Oxygen) → 2Li2O(Lithium Oxide)
Their oxides can dissolve in water forming an alkaline solution of the metal hydroxide:
Li2O(Lithium Oxide) + H2O(Water) → 2LiOH(Lithium Hydroxide)
They react with water vigorously forming metal hydroxide and hydrogen gas:
2K(Potassium) + 2H2O(Water) → 2KOH(Potassium Hydroxide) + H2(Hydrogen)
They React with Halogens forming a metal halide:
2Na(Sodium) + Cl2(Chlorine) → 2NaCl(Sodium Chloride)
The Halogens:
These are elements of group 7; Fluorine, Chlorine, Bromine, Iodine and Astatine.
7. We will study only properties of chlorine, bromine & iodine. They are colored and the color gets
darker as we go down the group. They exist as diatomic molecules (Cl2, Br2, and I2). As you go
down, they gradually change from gas to solid (chlorine is gas, bromine is liquid and iodine is solid).
They react with hydrogen forming hydrogen halide, which is an acid if dissolved in water:
H2(Hydrogen) + Cl2(Chlorine) → 2HCl(Hydrochloric Acid)
They react with metals forming metal halide:
2Fe(Iron) + 3Cl2(Chlorine) → 2FeCl3(Iron Chloride)
The reactivity also decreases as we do down, chlorine is most reactive, followed by bromine then
iodine.
If you bubble chlorine gas through a solution of potassium bromide, chlorine will take bromine’s
place because it more reactive. This is a displacement reaction.
2KBr(Potassium Bromide) + Cl2(Chlorine) → 2KCl(Potassium Chloride) + Br2(Bromine)
Transition Elements:
These are metals. They form a big part of the periodic table. Some of them are very common like
copper, zinc and iron.
They have the following properties:
1. They are harder and stronger than metals of groups 1 & 2.
2. They have much higher densities than metals other metals.
3. They have high melting points except for mercury.
4. They are less reactive than metals of group 1 & 2.
5. Excellent conductors of heat and electricity.
6. They show catalytic activity (act as catalysts)
7. They react slowly with oxygen and water
8. They form simple ions with several oxidation states and complicated ions with high oxidation states.
Noble Gases:
These are elements in group 8 of the periodic table. They are colorless gases. They are extremely
unreactive; this is because they have their outer energy shell full with electrons. So they are
stable, this is why they exist as single atoms. They have some uses however, for example argon is
used in light bulbs to prevent the tungsten filament from reacting with air, making the bulb last
longer. Neon is also used in the advertising and laser beams. These gases are Helium, Neon,
Argon, Krypton, Xenon and Radon (radioactive).