Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
This document provides information on electron configurations and quantum numbers:
- It defines the principal quantum number n, which describes the main energy level of an electron. It also defines the subsidiary quantum number l, which describes the shape of an orbital, and the magnetic quantum number m, which describes the orientation of an orbital in space.
- It discusses the four quantum numbers that describe each electron in an atom: n, l, m, and spin quantum number s.
- It provides examples of writing the four quantum numbers for the last electron in different atoms like Li, Cl, B, O, and Ar.
- It includes sample exam questions that test understanding of electron configurations, ion formations, bonding definitions
This document discusses ionic and metallic bonding. Ionic compounds form when a metal transfers electrons to a non-metal to achieve a noble gas configuration. They are held together by ionic bonds between positively charged cations and negatively charged anions. Metallic bonding occurs when electrons are delocalized and free to move throughout the metal, explaining properties like conductivity and malleability. Formulas for ionic compounds are written using the crisscross method and polyatomic ions are treated like single atoms.
The document provides an overview of key topics in chemical bonding covered in Chapter 4, including:
- Electron configurations and valence electrons and how they relate to chemical bonding and stability.
- Drawing electron-dot structures to represent atoms, ions, and molecules.
- The two main types of chemical bonds - ionic bonds formed between ions and covalent bonds formed by shared electron pairs.
- Nomenclature rules for naming ionic and covalent compounds from their formulas and writing formulas from compound names.
- Electronegativity and how it determines if bonds are nonpolar, polar, or ionic.
- The different molecular geometries that result from electron pair repulsion in covalent
The document discusses naming ions and ionic compounds. It explains that ions are formed when atoms gain or lose electrons to obtain full outer shells, becoming negatively or positively charged anions and cations. Cations are named after the metal element, while anions are named by adding -ide to the nonmetal element name. Examples are provided of naming common monatomic cations such as sodium (Na+) and calcium (Ca2+), and anions such as chloride (Cl-) and sulfate (SO42-). The document concludes by demonstrating how to name ionic compounds by combining the names of the respective ions.
The document is a guide to chemical bonding for GCSE students produced by Knockhardy Publishing. It provides an overview of the types of chemical bonds formed between atoms, including ionic bonds formed through electron transfer between atoms with configurations just short and just over a noble gas, and covalent bonds formed through electron pair sharing between atoms with configurations short of a noble gas. Examples of ionic compounds like sodium chloride and covalent compounds like water and methane are given to illustrate how bonding allows atoms to achieve stable noble gas configurations.
Ionic bonding occurs between metal and non-metal atoms when they form ions. Metals form positive ions by losing electrons, filling their outer electron shells. Non-metals form negative ions by gaining electrons. The oppositely charged ions are attracted in an ionic compound via electrostatic forces. Sodium chloride is an example where sodium atoms lose electrons to become Na+ ions and chloride atoms gain electrons to become Cl- ions. The ions are arranged in a crystal lattice structure held together by ionic bonds.
This document provides an overview of redox reactions and electrochemistry applications. It discusses oxidation-reduction concepts like oxidation states and the OIL RIG mnemonic. Examples of redox reactions and electrochemistry applications are given, including galvanic cells, corrosion, electrolysis, and batteries. Key concepts covered include cell potential, the Nernst equation, and how concentration affects cell potential. Diagrams illustrate galvanic cells and how they function.
This document discusses several key atomic and molecular properties including electron configurations, ionization energies, atomic and ionic radii, and electron affinity. It explains how atoms gain or lose electrons to form ions that have noble gas configurations. Cations are typically smaller than the parent atom, while anions are larger. Trends in various properties across the periodic table are also examined, such as how ionization energy generally increases moving left to right and up a group, and how atomic radius decreases with increasing nuclear charge. Diagonal relationships between elements are explained in terms of similar cation charge densities.
This document provides information on electron configurations and quantum numbers:
- It defines the principal quantum number n, which describes the main energy level of an electron. It also defines the subsidiary quantum number l, which describes the shape of an orbital, and the magnetic quantum number m, which describes the orientation of an orbital in space.
- It discusses the four quantum numbers that describe each electron in an atom: n, l, m, and spin quantum number s.
- It provides examples of writing the four quantum numbers for the last electron in different atoms like Li, Cl, B, O, and Ar.
- It includes sample exam questions that test understanding of electron configurations, ion formations, bonding definitions
This document discusses ionic and metallic bonding. Ionic compounds form when a metal transfers electrons to a non-metal to achieve a noble gas configuration. They are held together by ionic bonds between positively charged cations and negatively charged anions. Metallic bonding occurs when electrons are delocalized and free to move throughout the metal, explaining properties like conductivity and malleability. Formulas for ionic compounds are written using the crisscross method and polyatomic ions are treated like single atoms.
The document provides an overview of key topics in chemical bonding covered in Chapter 4, including:
- Electron configurations and valence electrons and how they relate to chemical bonding and stability.
- Drawing electron-dot structures to represent atoms, ions, and molecules.
- The two main types of chemical bonds - ionic bonds formed between ions and covalent bonds formed by shared electron pairs.
- Nomenclature rules for naming ionic and covalent compounds from their formulas and writing formulas from compound names.
- Electronegativity and how it determines if bonds are nonpolar, polar, or ionic.
- The different molecular geometries that result from electron pair repulsion in covalent
The document discusses naming ions and ionic compounds. It explains that ions are formed when atoms gain or lose electrons to obtain full outer shells, becoming negatively or positively charged anions and cations. Cations are named after the metal element, while anions are named by adding -ide to the nonmetal element name. Examples are provided of naming common monatomic cations such as sodium (Na+) and calcium (Ca2+), and anions such as chloride (Cl-) and sulfate (SO42-). The document concludes by demonstrating how to name ionic compounds by combining the names of the respective ions.
The document is a guide to chemical bonding for GCSE students produced by Knockhardy Publishing. It provides an overview of the types of chemical bonds formed between atoms, including ionic bonds formed through electron transfer between atoms with configurations just short and just over a noble gas, and covalent bonds formed through electron pair sharing between atoms with configurations short of a noble gas. Examples of ionic compounds like sodium chloride and covalent compounds like water and methane are given to illustrate how bonding allows atoms to achieve stable noble gas configurations.
Ionic bonding occurs between metal and non-metal atoms when they form ions. Metals form positive ions by losing electrons, filling their outer electron shells. Non-metals form negative ions by gaining electrons. The oppositely charged ions are attracted in an ionic compound via electrostatic forces. Sodium chloride is an example where sodium atoms lose electrons to become Na+ ions and chloride atoms gain electrons to become Cl- ions. The ions are arranged in a crystal lattice structure held together by ionic bonds.
This document provides an overview of redox reactions and electrochemistry applications. It discusses oxidation-reduction concepts like oxidation states and the OIL RIG mnemonic. Examples of redox reactions and electrochemistry applications are given, including galvanic cells, corrosion, electrolysis, and batteries. Key concepts covered include cell potential, the Nernst equation, and how concentration affects cell potential. Diagrams illustrate galvanic cells and how they function.
This document discusses several key atomic and molecular properties including electron configurations, ionization energies, atomic and ionic radii, and electron affinity. It explains how atoms gain or lose electrons to form ions that have noble gas configurations. Cations are typically smaller than the parent atom, while anions are larger. Trends in various properties across the periodic table are also examined, such as how ionization energy generally increases moving left to right and up a group, and how atomic radius decreases with increasing nuclear charge. Diagonal relationships between elements are explained in terms of similar cation charge densities.
1. The document discusses electrolysis and differentiates between conductors, electrolytes, and non-electrolytes based on their ability to conduct electricity and undergo chemical changes.
2. It describes the components of an electrolytic cell including the electrodes (anode and cathode) and explains that electrolysis is the process of decomposing an electrolyte into its constituent elements using an electric current.
3. The summary explains that during electrolysis, electric energy is converted to chemical energy as ions in the electrolyte migrate to the electrodes. At the anode, anions are discharged and at the cathode, cations are discharged.
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
The document contains sample exam questions from various years on topics related to atomic structure, the periodic table, ionization energies, atomic spectra, bonding, and the historical experiments that led to discoveries about atomic structure. It includes multiple choice and open response questions testing definitions, explanations of trends, interpretations of data, and descriptions of experiments. The questions would require a strong understanding of foundational atomic and molecular concepts as well as the ability to apply this knowledge to analyze new situations.
Chemical Structure: Chemical Nomenclature. Inorganic Compoundsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
The document discusses ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged cation and another atom gains those electrons to become a negatively charged anion. This transfer of electrons allows both atoms to achieve a stable noble gas electron configuration. The resulting ions are held together by electrostatic attraction in a crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity as solids since the ions are tightly bound. They dissolve in water, allowing the ions to separate and move, making the solutions electrically conductive.
IB Chemistry on Periodic Trends, Effective Nuclear Charge and Physical proper...Lawrence kok
The document summarizes key concepts about the periodic table including periods, groups, and blocks. It explains that periods are horizontal rows based on the same principal quantum number, while groups are vertical columns with the same number of valence electrons. Blocks refer to different regions (s, p, d, f) based on which orbitals are being filled with electrons. It provides examples of trends in ionization energy and atomic radius across periods and down groups.
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".
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
Ions are formed when atoms gain or lose electrons to achieve a stable electron configuration. There are two main types of ions: cations, which are positively charged and form when metals lose electrons, and anions, which are negatively charged and form when nonmetals gain electrons. Cations have fewer electrons than protons, while anions have more electrons than protons. Examples given are sodium forming the Na+ cation by losing one electron, and oxygen forming the O2- anion by gaining two electrons.
This document provides information on covalent bonding including:
1) Covalent bonds form when atoms share pairs of electrons, with each atom contributing one electron to the bond. This holds the atoms together due to attraction between the nuclei and shared electrons.
2) Covalent bonds can form between atoms of the same element or different elements. Exceptions include cases where atoms don't achieve a full octet or share all electrons to exceed the octet limit.
3) Multiple bonds are stronger and shorter than single bonds due to greater orbital overlap in the bonding region. Bond polarity increases with difference in electronegativity between atoms.
This document provides information about the periodic table, including the location and properties of metals, non-metals, and metalloids. It discusses periodic trends such as atomic radius and ionic charge. Various topics are covered, including oxidation-reduction reactions, ionic and covalent bonding, naming ionic and covalent compounds, and common polyatomic ions.
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.
Ionic bonding occurs when a metal atom transfers electrons to a non-metal atom to form ions. The ions have full outer electron shells, making them stable. The positively charged metal ions are attracted to the negatively charged non-metal ions, forming an ionic bond. To determine the formula of an ionic compound, you write the symbols of the elements, determine the charge of each ion, and balance the ions so the total charge is zero. This gives the ratio of ions used to write the chemical formula. For example, sodium oxide has a 2:1 ratio of sodium and oxide ions, so its formula is Na2O.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has important industrial applications such as electroplating, metal purification, and metal extraction.
1) Noble gases are unreactive because their outer electron shells are full, giving them a stable configuration.
2) Atoms form ions to achieve a full outer shell like noble gases. Metals form cations by losing electrons, and non-metals form anions by gaining electrons.
3) Ionic bonds form when oppositely charged ions are attracted to each other, such as sodium and chloride ions forming sodium chloride. The chemical formula shows the ratio of ions.
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 document discusses the formation and properties of ionic compounds. It explains that ionic compounds are formed from cations and anions, which are electrically neutral overall. Ionic compounds are typically crystalline solids with high melting points that can conduct electricity when molten or dissolved. The document provides examples of common ionic compounds like sodium chloride and discusses how their ionic bonds give rise to properties like high melting points and conductivity.
1) Noble gases do not form ions or bonds because they have a stable octet of electrons, matching the configuration of the nearest noble gas.
2) Atoms form ions to achieve a stable octet. Metals form cations by losing electrons, nonmetals form anions by gaining electrons.
3) Ionic compounds consist of positively and negatively charged ions with an overall neutral charge. The formula shows the ratio of cations to anions needed for charge balance.
The document discusses the rules for naming binary covalent (molecular) compounds. It explains that these compounds are made of two nonmetals bonded together with covalent bonds. The naming involves identifying the elements present and using prefixes to indicate the number of atoms of each element, with the first word naming the first element and the second using "-ide" to name the second element. Examples are provided and worked through step-by-step.
Ion - an atom or group of atoms that has a positive or negative charge. Ions are formed by gaining or losing electrons, not protons. Cations have a positive charge and are formed by losing electrons. Anions have a negative charge and are formed by gaining electrons. The periodic table shows which elements tend to form which ions based on their group, with groups 1, 2, 6 and 7 typically forming cations or anions.
Isotopes are variations of chemical elements that have the same number of protons but different numbers of neutrons. We identify isotopes based on their mass, which is the sum of protons and neutrons. Carbon has three main isotopes: 12C with 6 protons and 6 neutrons; 13C with 6 protons and 7 neutrons; and 14C with 6 protons and 8 neutrons. Isotopes are identified by their distinct masses, which are measured using an isotope ratio mass spectrometer.
Isotopes are variations of a chemical element that have the same number of protons but different numbers of neutrons. Isotopes are identified based on their mass, which is the sum of protons and neutrons. Examples of carbon isotopes are 12C, 13C, and 14C, which have 6 protons but 6, 7, and 8 neutrons respectively.
1. The document discusses electrolysis and differentiates between conductors, electrolytes, and non-electrolytes based on their ability to conduct electricity and undergo chemical changes.
2. It describes the components of an electrolytic cell including the electrodes (anode and cathode) and explains that electrolysis is the process of decomposing an electrolyte into its constituent elements using an electric current.
3. The summary explains that during electrolysis, electric energy is converted to chemical energy as ions in the electrolyte migrate to the electrodes. At the anode, anions are discharged and at the cathode, cations are discharged.
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
The document contains sample exam questions from various years on topics related to atomic structure, the periodic table, ionization energies, atomic spectra, bonding, and the historical experiments that led to discoveries about atomic structure. It includes multiple choice and open response questions testing definitions, explanations of trends, interpretations of data, and descriptions of experiments. The questions would require a strong understanding of foundational atomic and molecular concepts as well as the ability to apply this knowledge to analyze new situations.
Chemical Structure: Chemical Nomenclature. Inorganic Compoundsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
The document discusses ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged cation and another atom gains those electrons to become a negatively charged anion. This transfer of electrons allows both atoms to achieve a stable noble gas electron configuration. The resulting ions are held together by electrostatic attraction in a crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity as solids since the ions are tightly bound. They dissolve in water, allowing the ions to separate and move, making the solutions electrically conductive.
IB Chemistry on Periodic Trends, Effective Nuclear Charge and Physical proper...Lawrence kok
The document summarizes key concepts about the periodic table including periods, groups, and blocks. It explains that periods are horizontal rows based on the same principal quantum number, while groups are vertical columns with the same number of valence electrons. Blocks refer to different regions (s, p, d, f) based on which orbitals are being filled with electrons. It provides examples of trends in ionization energy and atomic radius across periods and down groups.
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".
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
Ions are formed when atoms gain or lose electrons to achieve a stable electron configuration. There are two main types of ions: cations, which are positively charged and form when metals lose electrons, and anions, which are negatively charged and form when nonmetals gain electrons. Cations have fewer electrons than protons, while anions have more electrons than protons. Examples given are sodium forming the Na+ cation by losing one electron, and oxygen forming the O2- anion by gaining two electrons.
This document provides information on covalent bonding including:
1) Covalent bonds form when atoms share pairs of electrons, with each atom contributing one electron to the bond. This holds the atoms together due to attraction between the nuclei and shared electrons.
2) Covalent bonds can form between atoms of the same element or different elements. Exceptions include cases where atoms don't achieve a full octet or share all electrons to exceed the octet limit.
3) Multiple bonds are stronger and shorter than single bonds due to greater orbital overlap in the bonding region. Bond polarity increases with difference in electronegativity between atoms.
This document provides information about the periodic table, including the location and properties of metals, non-metals, and metalloids. It discusses periodic trends such as atomic radius and ionic charge. Various topics are covered, including oxidation-reduction reactions, ionic and covalent bonding, naming ionic and covalent compounds, and common polyatomic ions.
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.
Ionic bonding occurs when a metal atom transfers electrons to a non-metal atom to form ions. The ions have full outer electron shells, making them stable. The positively charged metal ions are attracted to the negatively charged non-metal ions, forming an ionic bond. To determine the formula of an ionic compound, you write the symbols of the elements, determine the charge of each ion, and balance the ions so the total charge is zero. This gives the ratio of ions used to write the chemical formula. For example, sodium oxide has a 2:1 ratio of sodium and oxide ions, so its formula is Na2O.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has important industrial applications such as electroplating, metal purification, and metal extraction.
1) Noble gases are unreactive because their outer electron shells are full, giving them a stable configuration.
2) Atoms form ions to achieve a full outer shell like noble gases. Metals form cations by losing electrons, and non-metals form anions by gaining electrons.
3) Ionic bonds form when oppositely charged ions are attracted to each other, such as sodium and chloride ions forming sodium chloride. The chemical formula shows the ratio of ions.
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 document discusses the formation and properties of ionic compounds. It explains that ionic compounds are formed from cations and anions, which are electrically neutral overall. Ionic compounds are typically crystalline solids with high melting points that can conduct electricity when molten or dissolved. The document provides examples of common ionic compounds like sodium chloride and discusses how their ionic bonds give rise to properties like high melting points and conductivity.
1) Noble gases do not form ions or bonds because they have a stable octet of electrons, matching the configuration of the nearest noble gas.
2) Atoms form ions to achieve a stable octet. Metals form cations by losing electrons, nonmetals form anions by gaining electrons.
3) Ionic compounds consist of positively and negatively charged ions with an overall neutral charge. The formula shows the ratio of cations to anions needed for charge balance.
The document discusses the rules for naming binary covalent (molecular) compounds. It explains that these compounds are made of two nonmetals bonded together with covalent bonds. The naming involves identifying the elements present and using prefixes to indicate the number of atoms of each element, with the first word naming the first element and the second using "-ide" to name the second element. Examples are provided and worked through step-by-step.
Ion - an atom or group of atoms that has a positive or negative charge. Ions are formed by gaining or losing electrons, not protons. Cations have a positive charge and are formed by losing electrons. Anions have a negative charge and are formed by gaining electrons. The periodic table shows which elements tend to form which ions based on their group, with groups 1, 2, 6 and 7 typically forming cations or anions.
Isotopes are variations of chemical elements that have the same number of protons but different numbers of neutrons. We identify isotopes based on their mass, which is the sum of protons and neutrons. Carbon has three main isotopes: 12C with 6 protons and 6 neutrons; 13C with 6 protons and 7 neutrons; and 14C with 6 protons and 8 neutrons. Isotopes are identified by their distinct masses, which are measured using an isotope ratio mass spectrometer.
Isotopes are variations of a chemical element that have the same number of protons but different numbers of neutrons. Isotopes are identified based on their mass, which is the sum of protons and neutrons. Examples of carbon isotopes are 12C, 13C, and 14C, which have 6 protons but 6, 7, and 8 neutrons respectively.
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.
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
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.
Chemical Structure: Chemical Bonding. Ionic, Metallic & Coordinate Bondsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical Structure: Chemical Bonding. Molecular Orbitalsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical and Physical Properties: Radioactivity & Radioisotopes ulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical and Physical Properties: Isotopes and Forensic Scienceulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical Structure: Chemical Bonding. Properties of Coordination Compounds ulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
This document discusses particle theory and the structure of atoms. It begins by defining particles as the tiny discrete units that make up matter, including atoms, molecules, ions. It then discusses the historical development of atomic models from Dalton to Chadwick. Key points include: atoms consist of protons, neutrons, and electrons; protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Electron configuration and the filling of electron shells in the first 20 elements is also explained. Isotopes are defined as atoms of the same element with different numbers of neutrons.
1) The document discusses the history and modern structure of the atomic model, including the discovery of subatomic particles like protons, neutrons, and electrons. It describes the structure of the atom including the nucleus and electron cloud.
2) Quantum numbers are introduced to describe the allowed energy states of electrons. Electron configuration is used to write out the arrangement of electrons in atoms and relates to an element's position in the periodic table.
3) Different types of chemical bonds are described including ionic bonds formed by electron transfer, covalent bonds formed by electron sharing, and metallic bonds formed by delocalized electrons in metal crystals. Secondary bonds like hydrogen bonds are also introduced.
1) The document discusses atomic structure and bonding, covering the history of atomic theory from Dalton to Chadwick. It describes the structure of atoms including protons, neutrons and electrons.
2) Atomic number and mass are defined, and electron configuration is explained using quantum numbers. Different types of chemical bonds are covered - ionic formed by electron transfer, covalent by electron sharing, and metallic by delocalized electrons.
3) Secondary bonds such as hydrogen and van der Waals bonds are also summarized. The periodic table is shown organizing elements by electron configuration. Different classes of elements - metals, nonmetals and metalloids - are defined by their bonding properties.
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.
The document discusses radioactive decay and nuclear physics concepts. It describes the discovery of radioactivity by Henri Becquerel and the Curies. It defines key nuclear physics terms like isotopes, isobars, isotones. It explains the different types of radioactive decay including alpha, beta, positron decay and gamma emission. It discusses the penetration and ranges of different types of radiation. Finally, it covers the conservation of energy and mass in nuclear reactions based on Einstein's mass-energy equivalence formula.
This document discusses types of radioactivity and nuclear decay. It describes alpha, beta, gamma radiation and positron emission. It explains that alpha particles consist of two protons and two neutrons, beta particles are high energy electrons, and gamma rays are high energy electromagnetic radiation without mass or charge. Nuclear decay occurs through radioactive processes like alpha, beta, gamma or positron emission. The rate of radioactive decay is measured by half-life, which is the time for half of a radioactive sample to decay. Radioisotope dating uses half-lives of elements like carbon-14, potassium-40 and uranium-238 to determine the age of materials.
This document discusses the periodic table and periodic trends among the elements. It begins by outlining the ground state electron configurations of elements. It then classifies the elements and discusses how atomic and ionic radii vary periodically. The document also examines how other properties like ionization energy and electron affinity change across the periodic table. Specific trends in reactivity are described for representative main group elements in Groups 1A through 8A. In summary, the key periodic trends and relationships among atomic and physical properties of the elements are outlined.
The document discusses trends in the properties of elements in the periodic table. It describes how elements in the same group generally have similar chemical properties, though properties are not identical. It discusses how Mendeleev and Meyer independently organized the elements into the first periodic tables based on recurring trends in properties. Elements in the inner transition metals block were later added.
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 talks about the formation of chemical bonds. This presentation gives insight into the formation of Ionic Bonds, Covalent Bonds and Metallic Bonds with examples.
1. The document discusses atomic structure and properties of subatomic particles like electrons, protons, and neutrons.
2. It also covers terminology used in atomic structure like atomic number, mass number, and isotopes. Methods for calculating relative atomic mass and isotope percentages are presented.
3. The formation of ionic and covalent bonds is explained through examples of ionic compounds like NaCl and covalent compounds like H2O and CH4. Dot and cross diagrams are used to represent bonding.
This document provides an overview of basic chemistry concepts including:
- The law of multiple proportions and how it is illustrated by nitrogen and hydrogen oxides.
- Definitions of a mole and how it is used to calculate the number of hydrogen atoms in 1 mole of methane.
- How stoichiometry is used to calculate the amount of water formed from the combustion of a given amount of methane.
- The concept of a limiting reagent and how to calculate the mass of a product given specific amounts of reactants.
- A summary of the key observations and conclusions from Rutherford's gold foil experiment that led to the nuclear model of the atom.
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.
Chemical Structure: Chemical Bonding. Homonuclear Covalent Bondsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
This document summarizes key concepts from Chapter 7 on ionic and metallic bonding. It discusses how ions form as atoms gain or lose electrons to achieve stable noble gas electron configurations. Cations are positive ions that form when metals lose electrons, while anions are negative ions that form when nonmetals gain electrons. Ionic compounds consist of cations and anions bonded through electrostatic attraction. Their properties include being crystalline solids with high melting points that conduct electricity when molten or dissolved. Metallic bonding is described as a "sea of electrons" where metal atoms are positively charged cations floating in a sea of delocalized electrons that are free to move, explaining metals' malleability and conductivity. Alloys are mixtures of
Similar to Chemical Structure: Structure of Matter. Elements, Ions & Isotopes (20)
Analytics for http://forensicchemistry.lincoln.ac.uk, Feb/March 2011ulcerd
The document summarizes website analytics for the forensicchemistry.lincoln.ac.uk site from February 20, 2011 to March 21, 2011. It received 45 visits from 11 countries over this period. The majority of traffic came from search engines (53.33%) and referring sites (37.78%). The United Kingdom contributed the most visits (14) and had the highest average pages per visit (2.14) and average time on site (1 minute, 44 seconds). The overall bounce rate was 64.44% and 93.33% of visits were from new visitors.
EPrints Analytics - Forensic Chemistry OER Course site, Feb/March 2011ulcerd
This document summarizes webpage analytics for content from the Introductory Chemistry institutional repository from February 21 to March 21. It shows the number of pageviews and unique pageviews for each page, as well as average time on page, bounce rate, exit percentage, and cost index for the overall page and individual pages. The most visited page was /2366/ with 15 pageviews and 14 unique pageviews. The average time on page for all content was 53 seconds, with bounce and exit rates lower than the site average.
Organic Chemistry: Classification of Organic Compounds: Seminarulcerd
This document discusses various organic functional groups including alcohols, aldehydes, ketones, carboxylic acids, esters, ethers, amines, amides, halogenoalkanes, nitriles, nitro compounds, and thiols. It provides examples of each functional group and discusses their classifications. Primary, secondary, and tertiary alcohols and amines are defined. Common illegal and recreational drugs like amphetamines, aspirin, cannabis, LSD, cocaine, morphine, and codeine are analyzed in terms of their functional group components.
Chemical and Physical Properties: Practical Sessionulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
1. The document discusses moles, molar mass, molarity, and provides example calculations involving these concepts. Molarity is defined as the number of moles of solute per liter of solution.
2. The document then provides 21 practice problems calculating things like the number of moles or grams of various substances, the molarity of different solutions, and multi-step dilution problems.
3. Students are asked to use the concepts of moles, molar mass, and molarity to solve quantitative chemistry problems involving substances in solutions.
Calculations using standard enthalpies of formationulcerd
1. The document provides standard enthalpies of formation (ΔfH°) for various compounds and asks the reader to use these values to calculate the enthalpy change for 10 chemical reactions and processes.
2. It lists the standard enthalpies of formation for common compounds such as water, carbon dioxide, benzene, cyclohexane, calcium carbonate, quicklime, sulfur dioxide, sulfuric acid, ethanol, bromoethane and more.
3. The reader is to apply Hess's law and add or subtract the given standard enthalpies of formation to determine the enthalpy change for the 10 processes listed, such as the enthalpy of solution of hydrogen bromide gas and
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical and Physical Properties: Chemical vs. Physical Propertiesulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Organic Chemistry: Classification of Organic Compoundsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical Structure: Chemical Bonding. Polar Bondsulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
This document discusses various topics in thermochemistry including:
- Enthalpy changes in chemical reactions and how they are measured using calorimetry. Exothermic and endothermic reactions are explained.
- Hess's law, which states that the enthalpy change of a reaction is independent of the reaction pathway. It can be used to calculate enthalpy changes.
- Standard enthalpies of formation and how they allow calculation of enthalpy changes using Hess's law and bond dissociation enthalpies.
- Measuring enthalpy changes using bomb calorimetry and coffee cup calorimetry. Limitations of each method are discussed.
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
‘Pencils and Pixels’ is a learning resource aimed at helping you to improve your communication skills through drawing. An important part of the design process is to develop ideas from the imagination and share those ideas in the wider world. Whether you are having a conversation with yourself or with others, improving your drawing skills will help you to explain that most important of questions, ‘but what will it look like?
For more information and related videos, visit: http://pencilsandpixels.blogs.lincoln.ac.uk/lessons/lesson-1/
‘Pencils and Pixels’ is a learning resource aimed at helping you to improve your communication skills through drawing. An important part of the design process is to develop ideas from the imagination and share those ideas in the wider world. Whether you are having a conversation with yourself or with others, improving your drawing skills will help you to explain that most important of questions, ‘but what will it look like?
For more information and related videos, visit: http://pencilsandpixels.blogs.lincoln.ac.uk/lessons/lesson-1/
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.pptHenry Hollis
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
Richard Seddon, George Grey,
Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
How to Setup Warehouse & Location in Odoo 17 InventoryCeline George
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
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.
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptxEduSkills OECD
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 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.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
1. This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License Elements, Ions & Isotopes University of Lincoln presentation
2.
3. 1. Elements This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License
4.
5.
6.
7.
8.
9. For Example This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License 20 40 11 22 1 1 H Na Ca
10.
11. This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License H Be Li Na K Rb Cs Fr Mg Ca Sr Ba Ra Sc Y La Ac Ti V Cr Mn Fe Co Ni Cu Zn Zr Hf Ta W Re Os Ir Pt Au Hg Tl Nb Mo Tc Ru Rh Pd Ag Cd In Sn Pb Bi Po At Rn Xe Kr Ar Ne Sb Te I Ga Al Ge Si P S Cl As Se Br Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr He B C N O F Metals Semi-metals Non-Metals Classification of elements
12.
13. Allotropes of Carbon This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License C 60 fullerene structure Graphite layered structure Diamond structure
14.
15. 2. Ions This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License
16.
17. The Periodic Table This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License n=1 n=2 n=3 n=4 n=5 n=6 n=7 The Periodic Table consists of rows of 8 elements (s + p block only) Each row corresponds to a different quantum number (n=1–7) Each column has the same VALENCE CONFIGURATION ns 1 ns 2 ns 2 np 1 ns 2 np 2 ns 2 np 3 ns 2 np 4 ns 2 np 5 ns 2 np 6 f - block elements H Be Li Na K Rb Cs Fr Mg Ca Sr Ba Ra Sc Y La Ac Ti V Cr Mn Fe Co Ni Cu Zn Zr Hf Ta W Re Os Ir Pt Au Hg Tl Nb Mo Tc Ru Rh Pd Ag Cd In Sn Pb Bi Po At Rn Xe Kr Ar Ne Sb Te I Ga Al Ge Si P S Cl As Se Br Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr He B C N O F Lanthanoids Actinoids d – block elements Hydrogen and s – block elements p – block elements
18.
19.
20. Valence Electrons This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License [Ar] 4s 2 Ca 20 1s 2 2s 2 2p 6 Ne 10 [Ar] 4s 1 K 19 [He] 2s 2 2p 5 F 9 1s 2 2s 2 2p 6 3s 2 3p 6 Ar 18 [He] 2s 2 2p 4 O 8 [Ne] 3s 2 3p 5 Cl 17 [He] 2s 2 2p 3 N 7 [Ne] 3s 2 3p 4 S 16 [He] 2s 2 2p 2 C 6 [Ne] 3s 2 3p 3 P 15 [He] 2s 2 2p 1 B 5 [Ne] 3s 2 3p 2 Si 14 [He] 2s 2 Be 4 [Ne] 3s 2 3p 1 Al 13 [He] 2s 1 Li 3 [Ne] 3s 2 Mg 12 1s 2 He 2 [Ne] 3s 1 Na 11 1s 1 H 1 Electronic configuration Element Symbol Atomic number Electronic configuration Element Symbol Atomic number
21.
22.
23.
24. 3. Isotopes This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License
25.
26.
27. This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License Henri Becquerel Marie & Pierre Curie Radioactivity discovered in 1896
28. Stable v. Radioactive Isotopes This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License There are approximately 1,700 isotopes known to exist
29. Chart of the nuclides This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License
30. Chart of the nuclides This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License Black squares denote STABLE isotopes Z N
31.
32. Relative Atomic Mass, A r This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License Mg 24 78.7 Mg 25 10.1 Mg 26 11.2 % abundance The relative atomic mass of an element is the weighted mean of the atomic masses of all the stable isotopes for that element. For example: A r (Mg) = 24.3 Atomic mass