This document discusses key concepts in atomic structure and bonding:
1. It describes John Dalton's atomic theory and the discoveries of J.J. Thomson, Ernest Rutherford, and other scientists that led to developing the modern atomic model.
2. Key aspects of the modern atomic model are explained, including that atoms are composed of protons, neutrons, and electrons, with the nucleus at the center containing protons and neutrons.
3. The document also introduces concepts such as isotopes, ions, and how elements are arranged on the periodic table based on their atomic structure.
The document summarizes the structure of an atom in 3 paragraphs:
1) It describes the three main subatomic particles - electrons, protons, and neutrons - and their relative masses and charges.
2) It outlines the historical discoveries of these particles, including Thomson discovering electrons in 1900, discoveries of positively charged particles (protons) in the late 1800s, and Chadwick discovering neutrons in 1932.
3) It discusses several historical models of the atom, including Thomson's "plum pudding" model, Rutherford's discovery of the nucleus from alpha scattering experiments, and Bohr's improvement adding discrete electron orbits that explained atomic stability.
Chemical Structure: Structure of Matter. Atoms – the building blocks of matterulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
J.J. Thomson proposed the plum pudding model where electrons were embedded in a uniform sphere of positive charge, making the atom electrically neutral. However, Rutherford's gold foil experiment found that most alpha particles passed through, but some were deflected at very large angles. This led Rutherford to propose that the positive charge and mass of an atom are concentrated in a very small nucleus, with electrons orbiting the outside. This nuclear model of the atom replaced Thomson's plum pudding model.
This document provides information about atomic structure. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like J.J. Thomson, E. Goldstein, and Chadwick. Models of the atom proposed by scientists like Thomson, Rutherford, and Bohr are explained. The distribution of electrons in different shells is given according to Bohr's model. Information about isotopes, isobars, and valency is also provided.
- Atoms contain positively charged protons, uncharged neutrons, and negatively charged electrons. Electrons orbit the small, dense nucleus that contains protons and neutrons.
- Rutherford's gold foil experiment showed that the atom consists mostly of empty space, with a small, dense nucleus at the center containing most of the atom's mass.
- Electrons orbit the nucleus in distinct energy levels or shells, allowing atoms to be stable without electrons losing energy through radiation.
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
Here are cutouts of magnesium and chlorine atoms:
Mg-24 atom:
Nucleus: 12 protons, 12 neutrons
Electrons: 12
Cl-35 atom:
Nucleus: 17 protons, 18 neutrons
Electrons: 17
To form an ionic bond:
- Mg loses 2 electrons to have a full outer shell of 8
- Cl gains 1 electron to have a full outer shell of 8
The ratio of Mg to Cl atoms that would result in a neutral compound is 1:1.
The name of the ionic compound is magnesium chloride.
The chemical symbol is MgCl2.
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 summarizes the structure of an atom in 3 paragraphs:
1) It describes the three main subatomic particles - electrons, protons, and neutrons - and their relative masses and charges.
2) It outlines the historical discoveries of these particles, including Thomson discovering electrons in 1900, discoveries of positively charged particles (protons) in the late 1800s, and Chadwick discovering neutrons in 1932.
3) It discusses several historical models of the atom, including Thomson's "plum pudding" model, Rutherford's discovery of the nucleus from alpha scattering experiments, and Bohr's improvement adding discrete electron orbits that explained atomic stability.
Chemical Structure: Structure of Matter. Atoms – the building blocks of matterulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
J.J. Thomson proposed the plum pudding model where electrons were embedded in a uniform sphere of positive charge, making the atom electrically neutral. However, Rutherford's gold foil experiment found that most alpha particles passed through, but some were deflected at very large angles. This led Rutherford to propose that the positive charge and mass of an atom are concentrated in a very small nucleus, with electrons orbiting the outside. This nuclear model of the atom replaced Thomson's plum pudding model.
This document provides information about atomic structure. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like J.J. Thomson, E. Goldstein, and Chadwick. Models of the atom proposed by scientists like Thomson, Rutherford, and Bohr are explained. The distribution of electrons in different shells is given according to Bohr's model. Information about isotopes, isobars, and valency is also provided.
- Atoms contain positively charged protons, uncharged neutrons, and negatively charged electrons. Electrons orbit the small, dense nucleus that contains protons and neutrons.
- Rutherford's gold foil experiment showed that the atom consists mostly of empty space, with a small, dense nucleus at the center containing most of the atom's mass.
- Electrons orbit the nucleus in distinct energy levels or shells, allowing atoms to be stable without electrons losing energy through radiation.
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
Here are cutouts of magnesium and chlorine atoms:
Mg-24 atom:
Nucleus: 12 protons, 12 neutrons
Electrons: 12
Cl-35 atom:
Nucleus: 17 protons, 18 neutrons
Electrons: 17
To form an ionic bond:
- Mg loses 2 electrons to have a full outer shell of 8
- Cl gains 1 electron to have a full outer shell of 8
The ratio of Mg to Cl atoms that would result in a neutral compound is 1:1.
The name of the ionic compound is magnesium chloride.
The chemical symbol is MgCl2.
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 various properties of metals such as aluminium being the most abundant metal, platinum being the most precious metal, and iron being the most usable metal. It also discusses properties of specific metals like lithium being the lightest metal and lead being the poorest conductor of heat.
- Metals are elements that form cations by losing electrons and exist as electropositive elements, except for hydrogen. Mercury is an example of a metal that exists in liquid form. Metal oxides are generally basic in nature.
- Alkali metals are the most reactive group of metals due to their large size and low ionization energy values. Properties like malleability, ductility and reactivity can also vary between
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPointMr. Walajtys
This document covers naming and writing formulas for ions, ionic compounds, molecular compounds, acids, and bases. It provides objectives and definitions for each section, examples of naming and writing formulas, and explanations of naming conventions and rules including prefixes, charges, and endings for different types of compounds.
Magnesium and calcium atoms form ions with a charge of +2 because they are in the same group on the periodic table. Atoms in the same group have the same electron configuration in their outer shell. Magnesium and calcium atoms lose two electrons each to achieve a full outer shell, giving them a 2+ charge as an ion. Forming ions with a charge allows atoms to gain or lose electrons to achieve stability.
this ppt is all about basic working of most basic unit atom. and could enrich your knowledge about atom. and follow me at my instagram
https://www.instagram.com/shantanu_stark/?hl=en
This document summarizes key concepts from a chemistry textbook chapter on the periodic table. It discusses how elements are organized in the periodic table based on their atomic structure and properties. Early sections describe the historical development of periodic tables and how elements are classified into groups based on electron configuration. Later sections summarize periodic trends in atomic size, ionization energy, and ion size based on an element's position in the periodic table and how its electron configuration is filled.
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.
Grade 9 chemistry, ions and writing chemical formulaeNellexo
This document provides information on writing chemical formulas for ionic compounds. It discusses how ions are formed by elements gaining or losing electrons to achieve stability like the nearest noble gas. The charge on simple ions relates to the number of electrons gained or lost. Polyatomic ions contain two or more combined atoms and usually have a negative charge except for ammonium. To write formulas for ionic compounds, the numbers of positive and negative ions must balance to give an electrically neutral compound. The names of ionic compounds consist of the cation name followed by the anion name changed to end in "-ide".
It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
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.
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 summarizes key concepts from a chapter on the periodic table, including:
1) It traces the historical development of the periodic table from early classifications of elements by their properties to Dobereiner's discovery of triads of elements and eventual development of the modern periodic table by Mendeleev and Moseley's organization by atomic number.
2) It explains how to read information from the periodic table such as the atomic number, name, and mass of elements as well as trends in various properties that are illustrated in the organization of the table.
3) It describes periodic trends in properties including atomic radius, ionization energy, electron affinity, and electronegativity that help explain elements' chemical behaviors
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.
Ionic compounds are formed when ions combine. During formation, atoms transfer electrons to form cations (positively charged ions) and anions (negatively charged ions). Ionic compounds have high melting points and dissolve in water to form conductive solutions. They are named by writing the name of the metal cation followed by the non-metal anion or polyatomic ion.
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
The document discusses the periodic table of elements and its development over time. It explains how elements are arranged based on their proton number and how this arrangement allows prediction of element properties based on periodic trends. Examples are given of common elements and their uses to illustrate the practical importance of the periodic table.
This document provides information about the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like Thomson, Goldstein, and Chadwick. The document then explains four major atomic models - Thomson's model, Rutherford's model, Bohr's model, and the distribution of electrons in shells. It also discusses concepts like atomic number, mass number, isotopes, isobars, and valency.
There are several misconceptions about the valence shell of the atom. The key questions that arise in the minds of the learners are:
Is valence shell really the outermost shell?
2. Are there only seven shells in an atom?
3. When shells are supposed to be made up of subshells, why can we not represent the subshells in the valence shell structure of the atom?
4. When electrons are said to occur in orbitals, why can we not indicate the orbitals in the valence shell structure?
4. How can we represent the origins for valance band and conduction band in the atomic structure?
5. What are some good metaphors for the core of the atom and the rest of the atom?
Here is a lesson created by Chemistry teachers to address these misconceptions.
The document discusses chemical bonding and formula writing. It explains that there are two main types of bonds: ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between atoms to form ions, while covalent bonds involve the sharing of electrons between atoms. It provides examples of common ionic compounds and their formulas, such as NaCl, as well as explaining how to write formulas for compounds containing polyatomic ions like OH-. Covalent bonding is demonstrated through the example of methane, CH4, where carbon shares electrons with four hydrogen atoms to fill their outer energy levels.
A nearly-comprehensive list of vocabulary terms needed for introductory chemistry in grade 9 science, including a variety of source websites for reference.
This document discusses chemical bonding and intramolecular bonding. It begins by introducing ionic and covalent bonds as the two major types of intramolecular bonding that hold atoms together to form molecules. Ionic bonds form between ions through the transfer of electrons from metals to nonmetals. Covalent bonds form between nonmetals by the sharing of electrons. The document then goes into further detail about the formation of ions, ionic compounds through electron transfers, and the naming of ionic compounds according to IUPAC nomenclature rules.
The document discusses the structure of atoms. It explains that atoms contain protons, neutrons and electrons. The atomic model has evolved over time from Thomson's "plum pudding" model to Rutherford's discovery of the nucleus at the center of the atom, to Bohr's model of electrons in discrete orbits. It further discusses the distribution of electrons in different shells, an element's valency which is determined by its outer shell electrons, atomic and mass numbers, isotopes and isobars.
The document summarizes key concepts about the structure of the atom:
1) Atoms contain positively charged protons, neutral neutrons, and negatively charged electrons. Rutherford discovered the nucleus and that atoms are mostly empty space.
2) Bohr's model improved on Rutherford's by proposing electrons orbit in discrete energy levels.
3) Elements are defined by their atomic number, or number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
- The document discusses various properties of metals such as aluminium being the most abundant metal, platinum being the most precious metal, and iron being the most usable metal. It also discusses properties of specific metals like lithium being the lightest metal and lead being the poorest conductor of heat.
- Metals are elements that form cations by losing electrons and exist as electropositive elements, except for hydrogen. Mercury is an example of a metal that exists in liquid form. Metal oxides are generally basic in nature.
- Alkali metals are the most reactive group of metals due to their large size and low ionization energy values. Properties like malleability, ductility and reactivity can also vary between
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPointMr. Walajtys
This document covers naming and writing formulas for ions, ionic compounds, molecular compounds, acids, and bases. It provides objectives and definitions for each section, examples of naming and writing formulas, and explanations of naming conventions and rules including prefixes, charges, and endings for different types of compounds.
Magnesium and calcium atoms form ions with a charge of +2 because they are in the same group on the periodic table. Atoms in the same group have the same electron configuration in their outer shell. Magnesium and calcium atoms lose two electrons each to achieve a full outer shell, giving them a 2+ charge as an ion. Forming ions with a charge allows atoms to gain or lose electrons to achieve stability.
this ppt is all about basic working of most basic unit atom. and could enrich your knowledge about atom. and follow me at my instagram
https://www.instagram.com/shantanu_stark/?hl=en
This document summarizes key concepts from a chemistry textbook chapter on the periodic table. It discusses how elements are organized in the periodic table based on their atomic structure and properties. Early sections describe the historical development of periodic tables and how elements are classified into groups based on electron configuration. Later sections summarize periodic trends in atomic size, ionization energy, and ion size based on an element's position in the periodic table and how its electron configuration is filled.
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.
Grade 9 chemistry, ions and writing chemical formulaeNellexo
This document provides information on writing chemical formulas for ionic compounds. It discusses how ions are formed by elements gaining or losing electrons to achieve stability like the nearest noble gas. The charge on simple ions relates to the number of electrons gained or lost. Polyatomic ions contain two or more combined atoms and usually have a negative charge except for ammonium. To write formulas for ionic compounds, the numbers of positive and negative ions must balance to give an electrically neutral compound. The names of ionic compounds consist of the cation name followed by the anion name changed to end in "-ide".
It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
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.
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 summarizes key concepts from a chapter on the periodic table, including:
1) It traces the historical development of the periodic table from early classifications of elements by their properties to Dobereiner's discovery of triads of elements and eventual development of the modern periodic table by Mendeleev and Moseley's organization by atomic number.
2) It explains how to read information from the periodic table such as the atomic number, name, and mass of elements as well as trends in various properties that are illustrated in the organization of the table.
3) It describes periodic trends in properties including atomic radius, ionization energy, electron affinity, and electronegativity that help explain elements' chemical behaviors
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.
Ionic compounds are formed when ions combine. During formation, atoms transfer electrons to form cations (positively charged ions) and anions (negatively charged ions). Ionic compounds have high melting points and dissolve in water to form conductive solutions. They are named by writing the name of the metal cation followed by the non-metal anion or polyatomic ion.
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
The document discusses the periodic table of elements and its development over time. It explains how elements are arranged based on their proton number and how this arrangement allows prediction of element properties based on periodic trends. Examples are given of common elements and their uses to illustrate the practical importance of the periodic table.
This document provides information about the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like Thomson, Goldstein, and Chadwick. The document then explains four major atomic models - Thomson's model, Rutherford's model, Bohr's model, and the distribution of electrons in shells. It also discusses concepts like atomic number, mass number, isotopes, isobars, and valency.
There are several misconceptions about the valence shell of the atom. The key questions that arise in the minds of the learners are:
Is valence shell really the outermost shell?
2. Are there only seven shells in an atom?
3. When shells are supposed to be made up of subshells, why can we not represent the subshells in the valence shell structure of the atom?
4. When electrons are said to occur in orbitals, why can we not indicate the orbitals in the valence shell structure?
4. How can we represent the origins for valance band and conduction band in the atomic structure?
5. What are some good metaphors for the core of the atom and the rest of the atom?
Here is a lesson created by Chemistry teachers to address these misconceptions.
The document discusses chemical bonding and formula writing. It explains that there are two main types of bonds: ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between atoms to form ions, while covalent bonds involve the sharing of electrons between atoms. It provides examples of common ionic compounds and their formulas, such as NaCl, as well as explaining how to write formulas for compounds containing polyatomic ions like OH-. Covalent bonding is demonstrated through the example of methane, CH4, where carbon shares electrons with four hydrogen atoms to fill their outer energy levels.
A nearly-comprehensive list of vocabulary terms needed for introductory chemistry in grade 9 science, including a variety of source websites for reference.
This document discusses chemical bonding and intramolecular bonding. It begins by introducing ionic and covalent bonds as the two major types of intramolecular bonding that hold atoms together to form molecules. Ionic bonds form between ions through the transfer of electrons from metals to nonmetals. Covalent bonds form between nonmetals by the sharing of electrons. The document then goes into further detail about the formation of ions, ionic compounds through electron transfers, and the naming of ionic compounds according to IUPAC nomenclature rules.
The document discusses the structure of atoms. It explains that atoms contain protons, neutrons and electrons. The atomic model has evolved over time from Thomson's "plum pudding" model to Rutherford's discovery of the nucleus at the center of the atom, to Bohr's model of electrons in discrete orbits. It further discusses the distribution of electrons in different shells, an element's valency which is determined by its outer shell electrons, atomic and mass numbers, isotopes and isobars.
The document summarizes key concepts about the structure of the atom:
1) Atoms contain positively charged protons, neutral neutrons, and negatively charged electrons. Rutherford discovered the nucleus and that atoms are mostly empty space.
2) Bohr's model improved on Rutherford's by proposing electrons orbit in discrete energy levels.
3) Elements are defined by their atomic number, or number of protons. Isotopes are atoms of the same element with different numbers of neutrons.
1) Atoms contain positively charged protons, neutral neutrons, and negatively charged electrons. Electrons orbit the dense, positively charged nucleus at the center of the atom.
2) Rutherford discovered the nucleus through alpha particle scattering experiments. His model showed electrons orbiting the tiny, dense nucleus. Bohr added that electrons can only orbit in discrete energy levels.
3) Elements are defined by their atomic number, or number of protons. Isotopes are atoms of the same element with different numbers of neutrons, giving them different mass numbers.
This document summarizes the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like Thomson, Goldstein, and Chadwick. The document then summarizes four major atomic models - Thomson's model, Rutherford's model, Bohr's model, and the distribution of electrons in shells. It also discusses concepts like atomic number, mass number, isotopes, isobars, and valency.
The document outlines key learning outcomes and concepts about atomic structure, including describing the structure of atoms with atomic numbers 1 to 20, defining terms like atomic number and mass number, explaining electron configuration and outer electrons, and distinguishing between isotopes, ions, and molecules of elements and compounds. It also provides illustrations of atomic structure and examples of applying atomic structure concepts.
This document provides a summary of the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It then describes the historical models of the atom including Thomson's plum pudding model, Rutherford's nuclear model, and Bohr's orbital model. Key topics covered include the distribution of electrons in shells, atomic number, mass number, isotopes, isobars, and valency.
The document outlines key concepts about atomic structure including the structure of atoms with protons, neutrons and electrons, atomic number and mass number, electron configuration, isotopes, ions, and molecules of elements and compounds. It also provides learning outcomes for describing atomic structure and properties as well as interpreting atomic symbols and notations.
This document outlines key concepts about atomic structure including:
1) The structure of atoms including protons, neutrons, and electrons that make up the nucleus and electron cloud.
2) Atomic properties such as atomic number, mass number, and relative atomic mass.
3) Electron configuration, isotopes, ions, and molecules of elements and compounds.
4) Learning objectives are to describe atomic structure, state particle properties, define related terms, list uses of isotopes, and predict bonding based on structure.
Atomos, Teorías Atómicas, Teoría Cuántica, Masa Atómica e Isotoposfernandogc
The document provides information about atoms and their subatomic particles. It defines the atom as the smallest particle of an element that retains its characteristics. It describes atoms as consisting of protons, neutrons, and electrons. The number of protons defines the element and its atomic number, while the total of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons. Electron configuration diagrams show how electrons are arranged in an atom's energy levels.
This document outlines key concepts about atomic structure including:
1) The structure of atoms consists of a nucleus containing protons and neutrons surrounded by electrons. Protons are positively charged, neutrons have no charge, and electrons are negatively charged.
2) Atomic number refers to the number of protons in an atom. Mass number refers to the total number of protons and neutrons. Atomic symbols represent these numbers.
3) Electrons surround the nucleus in fixed shells. The number of electrons in each shell is limited. The arrangement of electrons is known as the electronic structure or electron configuration.
1. Atoms are the smallest particles that make up elements, consisting of a nucleus surrounded by electrons. John Dalton established the first atomic theory in 1808.
2. In the early 20th century, experiments by Thomson, Rutherford, and Chadwick led to discoveries about the internal structure of atoms, including the identification of protons, electrons, and neutrons within the nucleus.
3. Isotopes are atoms of the same element that differ in their number of neutrons. Molecules, ions, and compounds are formed through combinations and interactions between atoms.
This document discusses ionic and metallic bonding. It explains that ions are formed when atoms gain or lose electrons to achieve stable noble gas electron configurations. Metals form cations by losing electrons while nonmetals form anions by gaining electrons. Ionic compounds contain cations and anions in ratios represented by chemical formulas. Metallic bonding occurs via delocalized valence electrons that are shared between metal atoms.
1) Atoms are made up of electrons, protons and neutrons. Electrons occupy different energy levels called electron shells.
2) There are three main types of chemical bonds: ionic bonds form between metals and nonmetals via electron transfer, covalent bonds form between nonmetals by electron sharing, and metallic bonds involve delocalized electrons binding metal atoms.
3) Electron configuration determines an element's chemical properties. Chemical bonds form as elements try to achieve stable electron configurations, such as the octet rule where atoms gain, lose or share electrons to have eight electrons in their outer shell.
This document discusses the structure of atoms and the types of chemical bonds. It begins by defining the atom and its components like protons, neutrons, and electrons. It describes the organization of electrons into shells and how this determines an element's properties. There are three main types of bonds: ionic bonds form when electrons are transferred between atoms, covalent bonds form when electrons are shared between atoms, and metallic bonds involve delocalized electrons between metal atoms. The document provides examples of each bond type and explains how ions are formed.
This document discusses the structure of atoms and different types of chemical bonds. It begins by defining the atom and electron shells. It then explains ionic bonds which form when a metal transfers electrons to a nonmetal, covalent bonds which form when atoms share electrons, and metallic bonds which hold metal atoms together. Examples of each bond type are given. The document also discusses electron dot structures, chemical formulas, and formula weights.
The document provides information on writing chemical formulas and naming compounds. It begins by defining oxidation numbers and discussing how they are used to write formulas for binary ionic compounds and polyatomic ionic compounds. Cationic elements are written first, followed by anionic elements or polyatomic ions in parentheses. Naming conventions are also outlined, with binary ionic compounds taking the cation name followed by "-ide" and polyatomic compounds taking the cation name followed by the name of the polyatomic ion. Lewis structures, molecular shapes, and intermolecular forces are also summarized.
The document provides information about the structure of atoms. It discusses that atoms are made up of protons, neutrons and electrons. The protons and neutrons are located in the nucleus at the center, while the electrons move around the nucleus. It explains different atomic models proposed by scientists like Thomson, Rutherford and Bohr. It also discusses the distribution of electrons in shells, valency, atomic number and mass number. Isotopes and isobars are defined. In summary, the document outlines the key particles that make up an atom and the various atomic structure models developed over time.
The document summarizes key concepts about the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes early atomic models proposed by Thomson, Rutherford, and Bohr. Key points of each model are provided. The document also discusses concepts like the distribution of electrons in shells, valency, atomic number, mass number, isotopes, and isobars. In summary, it provides an overview of the historical development of atomic structure and defines important atomic terms.
This chapter introduces fundamental concepts in chemistry including atoms, molecules, ions and chemical formulas. It discusses atomic theory and how experiments led to the discovery that atoms consist of electrons, protons and neutrons. The chapter also introduces the periodic table and explains how elements are arranged based on atomic structure and properties. It describes how atoms can form ions and molecules, and how ionic and molecular compounds are named using chemical formulas.
This document provides an overview of several key chemistry concepts across multiple chapters:
Chapter 1 introduces fundamental concepts like the three states of matter, elements and compounds, and physical and chemical properties.
Chapter 2 discusses atomic structure, including Dalton's atomic theory, early experiments that led to modern atomic models, and the organization of the periodic table. It also introduces molecules, ions, and chemical bonding.
Chapter 3 covers stoichiometry, including atomic masses, the mole concept, and percent composition of compounds.
The document defines important terms and provides examples to illustrate concepts like the periodic table, naming simple ionic and covalent compounds, and acid naming conventions. Diagrams and figures are included to summarize key ideas.
STATATHON: Unleashing the Power of Statistics in a 48-Hour Knowledge Extravag...sameer shah
"Join us for STATATHON, a dynamic 2-day event dedicated to exploring statistical knowledge and its real-world applications. From theory to practice, participants engage in intensive learning sessions, workshops, and challenges, fostering a deeper understanding of statistical methodologies and their significance in various fields."
Codeless Generative AI Pipelines
(GenAI with Milvus)
https://ml.dssconf.pl/user.html#!/lecture/DSSML24-041a/rate
Discover the potential of real-time streaming in the context of GenAI as we delve into the intricacies of Apache NiFi and its capabilities. Learn how this tool can significantly simplify the data engineering workflow for GenAI applications, allowing you to focus on the creative aspects rather than the technical complexities. I will guide you through practical examples and use cases, showing the impact of automation on prompt building. From data ingestion to transformation and delivery, witness how Apache NiFi streamlines the entire pipeline, ensuring a smooth and hassle-free experience.
Timothy Spann
https://www.youtube.com/@FLaNK-Stack
https://medium.com/@tspann
https://www.datainmotion.dev/
milvus, unstructured data, vector database, zilliz, cloud, vectors, python, deep learning, generative ai, genai, nifi, kafka, flink, streaming, iot, edge
Analysis insight about a Flyball dog competition team's performanceroli9797
Insight of my analysis about a Flyball dog competition team's last year performance. Find more: https://github.com/rolandnagy-ds/flyball_race_analysis/tree/main
End-to-end pipeline agility - Berlin Buzzwords 2024Lars Albertsson
We describe how we achieve high change agility in data engineering by eliminating the fear of breaking downstream data pipelines through end-to-end pipeline testing, and by using schema metaprogramming to safely eliminate boilerplate involved in changes that affect whole pipelines.
A quick poll on agility in changing pipelines from end to end indicated a huge span in capabilities. For the question "How long time does it take for all downstream pipelines to be adapted to an upstream change," the median response was 6 months, but some respondents could do it in less than a day. When quantitative data engineering differences between the best and worst are measured, the span is often 100x-1000x, sometimes even more.
A long time ago, we suffered at Spotify from fear of changing pipelines due to not knowing what the impact might be downstream. We made plans for a technical solution to test pipelines end-to-end to mitigate that fear, but the effort failed for cultural reasons. We eventually solved this challenge, but in a different context. In this presentation we will describe how we test full pipelines effectively by manipulating workflow orchestration, which enables us to make changes in pipelines without fear of breaking downstream.
Making schema changes that affect many jobs also involves a lot of toil and boilerplate. Using schema-on-read mitigates some of it, but has drawbacks since it makes it more difficult to detect errors early. We will describe how we have rejected this tradeoff by applying schema metaprogramming, eliminating boilerplate but keeping the protection of static typing, thereby further improving agility to quickly modify data pipelines without fear.
Learn SQL from basic queries to Advance queriesmanishkhaire30
Dive into the world of data analysis with our comprehensive guide on mastering SQL! This presentation offers a practical approach to learning SQL, focusing on real-world applications and hands-on practice. Whether you're a beginner or looking to sharpen your skills, this guide provides the tools you need to extract, analyze, and interpret data effectively.
Key Highlights:
Foundations of SQL: Understand the basics of SQL, including data retrieval, filtering, and aggregation.
Advanced Queries: Learn to craft complex queries to uncover deep insights from your data.
Data Trends and Patterns: Discover how to identify and interpret trends and patterns in your datasets.
Practical Examples: Follow step-by-step examples to apply SQL techniques in real-world scenarios.
Actionable Insights: Gain the skills to derive actionable insights that drive informed decision-making.
Join us on this journey to enhance your data analysis capabilities and unlock the full potential of SQL. Perfect for data enthusiasts, analysts, and anyone eager to harness the power of data!
#DataAnalysis #SQL #LearningSQL #DataInsights #DataScience #Analytics
ViewShift: Hassle-free Dynamic Policy Enforcement for Every Data LakeWalaa Eldin Moustafa
Dynamic policy enforcement is becoming an increasingly important topic in today’s world where data privacy and compliance is a top priority for companies, individuals, and regulators alike. In these slides, we discuss how LinkedIn implements a powerful dynamic policy enforcement engine, called ViewShift, and integrates it within its data lake. We show the query engine architecture and how catalog implementations can automatically route table resolutions to compliance-enforcing SQL views. Such views have a set of very interesting properties: (1) They are auto-generated from declarative data annotations. (2) They respect user-level consent and preferences (3) They are context-aware, encoding a different set of transformations for different use cases (4) They are portable; while the SQL logic is only implemented in one SQL dialect, it is accessible in all engines.
#SQL #Views #Privacy #Compliance #DataLake
1. 21
Chapter 4 Atoms and Elements
John Dalton’s Atomic Theory
1. Each element is composed of tiny indestructible particles called atoms.
2. All atoms of a given element have the same mass and other properties that distinguish them from the
atoms of other elements.
3. Atoms combine in simple, whole-number ratios to form compounds.
J.J. Thomson (1856 - 1940)
•Discovered electrons
Electron
• negatively charged (-1 charge)
• much smaller and lighter than atoms (1/1836th the mass of a hydrogen atom
• uniformly present in many different substances.
*Thomson proposes plum pudding model to explain the structure of the atom
Plum Pudding Model
• Replaces Daltons first statement - the atom is breakable
• The structure of the atom:
• Electrons suspended in a positively charged electric field.
• Positive charge necessary to balance negative electrons.
• There was no experimental evidece of positive matter, so Thomson assumed there must be
positive energy.
• The mass of the atom is due to the mass of the electrons
• Electrons in the atom repel each other; there must be a lot of empty space in the atom.
electron
sphere of positive energy
2. 22
Earnest Rutherford (1871- 1937)
Goal: prove the atom has a lot of empty space
Did he prove this?________________
Nuclear Theory of the Atom (Rutherford)
• Most of mass in nucleus. Positive charge (protons) in nucleus.
• Most of volume is empty space occupied by electrons outside nucleus.
• Number of electrons equals protons.
Neutrons – neutral particles contained in nucleus
The Modern Atom
• We know atoms are composed of three main pieces - protons, neutrons and electrons
• The nucleus contains protons and neutrons
• The nucleus is only about 10-13
cm in diameter
• The electrons move outside the nucleus with an average distance of about 10-8
cm
à the radius of the atom is about 100,000 times larger than the radius of the nucleus
• Atoms are neutral in charge, so the number of protons = the number of electrons
Atomic Number = Z = number of protons
Ex:
element Z # p # e-
C
Fe
Cu
3. 23
Periodic Table Workshop
1. What is the atomic number of boron, B?
2. What is the atomic mass of silicon, Si?
3. How many protons does a chlorine atom have? How many electrons?
4. How many electrons does a neutral neon atom have?
5. Will an atom with 6 protons, 6 neutrons and 6 electrons be electrically neutral?
6. Will an atom with 27 protons, 32 neutrons and 27 electrons be electrically neutral?
7. Will a Na atom with 10 electrons be electrically neutral?
8. What is the charge of a Lithium atom with two electrons?
4. 24
Dmitri Mendeleev
• order elements by atomic mass
• noticed a repeating pattern of properties
• Periodic Law – When the elements are arranged in order of increasing relative mass, certain sets
of properties recur periodically
• used pattern to predict properties of undiscovered elements
Element Classification
Metals: Shiny, ductile, malleable, conductors of heat and electricity
ex:
Non-metals: dull, poor conductors of heat and electricity
ex:
Metalloids (semiconductors): properties of metals and non-metals
ex:
5. 25
Ions: Atoms with a charge
Cations:
• Ions with a positive charge
• Metals lose one or more electron to form a cation
K à K+
+ 1 e-
potassium
atom
potassium
cation
1 e-
no charge +1 charge
19 p 19 p
19 e-
18 e-
Mg à Mg2+
+ 2 e-
magnesium
atom
magnesium cation
___ e-
___ charge ___ charge
___ p ___ p
___ e-
___ e-
Anions:
• Ions with a negative charge
• Non-metals gain one or more electron to form a anion
F + 1 e- à F-
fluorine atom
1 e-
fluoride anion
no charge - 1 charge
9 p 9 p
9 e-
10 e-
S + 2 e- à S2-
________atom __________anion
____charge ______ charge
____ p ____ p
____e-
____ e-
____ e-
6. 26
Preferred Charge of Monatomic Ions:
• IA = Alkali Metals:_________
• IIA = Alkali Earth Metals: _________
• VIIA = Halogens: _________
• VIIIA = Noble Gases: _________
• Others?
What charge do the following atoms prefer to form? Do they form cations or anions?
Element Charge Cation or Anion?
1. Na
2. Be
3. Cl
4. F
5. N
6. O
7. Al
8. Zn
9. Ag
10. In
7. 27
Isotopes = Atoms with the same number of protons, but different number of neutrons.
•Most elements have isotopes, with own unique percent natural abundance.
Mass Number (A)
The number of protons plus neutrons
A = p + n
Isotopes have different mass numbers
Isotope Symbol: X-A (i.e. Ne-20, Ne-21, Ne-22) OR
What is the mass number of an atom with 12 protons, 12 electrons, and 13 neutrons? Write the isotope
symbol.
A = ____ Isotope Symbol = __________ OR _____________
(Electrons are not included in the mass number.)
Practice Problem: Cobalt-60 (for cancer radiation treatment)
How many protons and neutrons does Co-60 have?
Z
A
X
8. 28
ATOMIC MASS
The weighted average of the masses of the naturally occurring isotopes of that element.
Atomic Mass = (abundance 1)(mass 1) + (abundance 2)(mass 2) + …
Express abundance in decimal form à 72.11% = 0.7211
Example 1:
Calculate the atomic mass of copper given the following:
Isotope % Abundance Exact Atomic Mass
Cu-63 69.17% 62.9395 amu
Cu-65 30.83% 64.9278 amu
Example 2:
(a) Silver has two naturally occurring isotopes (Ag-107 and Ag-109). If the natural abundance of Ag-107
is 51.84 %, what is the natural abundance of Ag-109?
(b) If the mass of Ag-107 is 106.905, what is the mass of Ag-109?
9. 29
Chapter 4 Workshop
1.What is the charge on an electron? _____________
2.What is the charge on a pronon? _____________
3.What is the charge on a neutron? _____________
4.Which has the greatest mass? e-
, p, or n? _____________
5.How many protons are in a silver atom? _____________
6.Which of the following is a metalloid?
aluminum silicon tin phosphorus iodine
7.What family does strontium belong? _____________
8.How many electrons are in a bromine ion? _____________
9.How many e-
, p, and n are in an iron (III) ion, 56
Fe3+
?
10.What is the symbol for an ion having 15 protons and 18 electrons? _____________
11.The nucleus of a flourine–19 atom contains how many protons and neutrons?
12.Which element would have a similar reaction in water as potassium?
calcium argon iron sodium carbon
10. 30
Chapter 5 Molecules and Compounds
atomic elements = elements whose particles are single atoms
molecular elements = elements whose particles are multi-atom molecules
There are 7 common diatomic elements; H2, N2, O2, F2, Cl2, Br2, I2
molecular compounds = compounds whose particles are molecules made of only nonmetals
2 or more non-metals, smallest unit is a molecule
ionic compounds = compounds whose particles are cations and anions
Metals + nonmetals
No individual molecular units, instead have a 3-dimensional array of cations and anions
mad of formula units
Molecular View of Elements and Compounds
Practice Problem: Classifying the following
1. aluminum, Al =
2. aluminum chloride, AlCl3 =
3. chlorine, Cl2 =
4. acetone, C3H6O =
5. carbon monoxide, CO =
6. cobalt, Co
!
Pure
substances
Elements
Atomic Molecular
Compounds
Molecular
2 or more
nonmetals
Ionic
metal +
nonmetal
Ex: Ex:
Ex: Ex:
Fe
Al
Zn
Hg
H2, N2, F2, O2
I2, Cl2, Br2,
S8
P4
one chemical symbol
= 2 or more elements co
CO2
H2O
CH4
NH3
NaCl
MgBr
Fe(NO3)2
element, atomic
compound, ionic
elements (Cl2)
molecular element
compound, molecular
compound, molecular
atomic element
11. Formula-to-Name Flow Chart
Examples Chemical Formula Name
Ionic Type 1
Ionic Type 1I
Molecular
Binary Acid
Oxyacid
Ionic
metal + nonmetal
Molecular
2 or more
nonmetals
Acids
H + one or more
nonmetal
Type 1
metal forms one
type of ion only
Type 2
metal forms more
than one type of ion
name of
cation
(metal)
base name of
anion* (nonmetal)
+ -ide
name of
cation
(metal)
base name of
anion* (nonmetal)
+ -ide
charge of cation (metal)
in roman numerals in
parentheses
prefix name of
1st
element
prefix Base name
of 2nd
element +
ide
element
Binary
2 element
Oxyacid
Contains oxygen
-ate -ite
base name
of oxyanion
+ -ic
acid
base name
of oxyanion
+ - ous
acid
base name
of nonmetal
+ - ic
acid
hydro
Subscript Prefixes for
Molecular Compounds
1 = mono-;
not used on first nonmetal
2 = di-
3 = tri-
4 = tetra-
5 = penta-
6 = hexa-
7 = hepta-
8 = octa-
drop last “a” if name begins
with vowel
Common Names
H2O = water, steam, ice
NH3 = ammonia
CH4 = methane
NaCl = table salt
C12H22O11 = table sugar
*Polyatomic ions. Write the entire
name. Do not change anything!
Zn 2+
Al3+
Cu+
Cu2+
A2+, Na +,
Mg+
K2S
Zn(C2H3O2)2
potassium sulfide K+ S-
Zinc acetate. Zn2+ C2H3O2-
C2H32O-
CrO
Ni2SO4
Chromium(II) oxide Cr 2+O2-
nickle (I) sulfate Ni+ SO4^2-
CO2
Co
P2Cl5
Carbon dioxide
carbon monoxide
diphosphorus pentachloride
HCl(aq)
HF(aq)
Hydrochloric acid
Hydrofluoric acid
NHO3(aq)
HNO2(aq)
hitric acid
hitrous acid
Fe2+
Fe3+
ex:NaCl= sodium chloride
MgBr2= Magnesium bromide
Text
ex: FeCl3 = iron(III)chloride
CuF2= copper (II) fluoride
k+ S2-
K+
K2S
Cr^3+ O2-
Cr2O3 = chromiuum (III) oxiide
hitric acid=HNO3 NO3- = nitrate
hitrous acid =HNO2 NO2- = hirtite
12. 32
MONATOMIC IONS TO MEMORIZE
Common Monotomic Anions
Nonmetal Symbol
Base
Name
Anion
Name
Fluorine F-
fluor fluoride
Chlorine Cl-
chlor chloride
Bromine Br-
brom bromide
Iodine I-
iod iodide
Oxygen O2-
ox oxide
Sulfur S2-
sulf sulfide
Nitrogen N3-
nitr nitride
Phosphorus P3-
phosph phosphide
Common Metals that Form Cations with
Different Charges
Metal Ion Name
*Older
Name (you
are not
responsible
for
memorizing
these)
Chromium Cr2+
chromium(II) chromous
Cr3+
chromium(III) chromic
Iron Fe2+
iron(II) ferrous
Fe3+
iron(III) ferric
Cobalt Co2+
cobalt(II) cobaltous
Co3+
cobalt(III) cobaltic
Copper Cu+
copper(I) cuprous
Cu2+
copper(II) cupric
Tin Sn2+
tin(II) stannous
Sn4+
tin(IV) stannic
Mercury Hg2
2+ mercury(I) mercurous
Hg2+
mercury(II) mercuric
Lead Pb2+
lead(II) plumbous
Pb4+
lead(IV) plumbic
Type 1 Metals
Ion Name
Li+
lithium
Na+ sodium
K+
potassium
Rb+
rubidium
Cs+
cesium
Be2+
beryllium
Mg2+
magnesium
Ca2+
calcium
Sr2+
strontium
Ba2+
barium
Al3+
aluminum
Zn2+
zinc
Ag+
silver
Ga3+
gallium
In3+
indium
14. 34
Ionic Compound Formula Writing Workshop
Write the ionic compound formed from the following ions
Li+
Mg2+
NH4
+
Al3+
Na+
Ba2+
K+
Ca2+
Br-
Ex:
LiBr
SO4
2-
OH-
F-
O2-
NO3
-
Ex:
Mg(NO3)2
PO4
3-
Cl-
S2-
I-
CO3
2-
Text Text Text Text Text Text Text
Text Text Text Text Text Text Text Text
Text Text Text Text Text Text Text Text
15. 35
Ionic Compounds Nomenclature Workshop
Compound Cation
symbol
Type I or
II metal?
Cation name Anion
symbol
Anion Name Compound Name
NaCl Na+
I sodium Cl-
chloride Sodium chloride
Fe(NO3)2 Fe2+
II iron (II) NO3
-
nitrate iron (II) nitrate
AlCl3
Be2C
Sn(C2H3O2)2
MgO2
CaHPO4
K2SO4
NiS
Au2S
CrPO4
Ca3N2
CaCO3