The document discusses the lanthanides and actinides, which are groups of elements found below the main periodic table. There are a total of 30 elements between the lanthanides (elements 57-71) and actinides (elements 89-103). The lanthanides and actinides are often referred to as the "inner transition metals" and exhibit similar chemical properties to lanthanum and actinium, respectively.
This chapter discusses the periodic table, explaining that elements are arranged in order of atomic number and grouped into periods and groups based on their electron configuration, with groups having similar properties and periods showing trends down the table. Properties of elements in groups I, VII, and 0 are described, including their physical states, reactivity, and chemical properties.
Redox Reaction and Electrochemical Cell (Reaksi Redoks dan Sel Elektrokimia)DindaKamaliya
An electrochemical cell converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells separated by a salt bridge. In the cathode half-cell, reduction occurs as oxidized species gain electrons. In the anode half-cell, oxidation occurs as reduced species lose electrons. Electrons flow through an external circuit from the anode to the cathode. The standard electrode potential of each half-reaction predicts the cell's voltage under standard conditions.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
This document summarizes the effective atomic number concept and the 18 electron rule for metal carbonyl compounds.
The effective atomic number (EAN) of a metal atom is calculated by adding the atomic number of the metal to twice the number of carbon monoxide ligands. This takes into account the electrons donated by CO to the metal center. Two examples of calculating EAN for mononuclear carbonyls are given.
The 18 electron rule states that the sum of the outer shell electrons of the metal atom and the electrons donated by carbon monoxide ligands should equal 18 for stable configurations. Two examples are provided to illustrate this rule.
This document presents information on reactive intermediates. It discusses four main types of reactive intermediates: carbocations, carbanions, free radicals, and carbenes. For each type, it describes examples, structures, factors that influence their stability, and common methods of generation. The document contains 19 slides covering an introduction, the four types of intermediates, conclusions, references, and acknowledgments.
This document provides an overview of metal clusters presented by Joel M. Smith at a Baran Group meeting. It begins with definitions of "cluster" and "metal cluster". The document then discusses the history of metal clusters, including important discoveries of polyoxometallates and metal carbonyl clusters. Preparation methods for metal clusters such as solution synthesis, hydrothermal synthesis, and reductive methods under CO atmosphere are described. Examples of reactions catalyzed by metal carbonyl clusters and polyoxometallate clusters are provided, including carbonylation, C-H oxidation, and dehydrogenation reactions.
1. A sigmatropic reaction is a rearrangement where a σ bond migrates within a conjugated π system, either suprafacially (same face) or antarafacially (opposite faces).
2. [3,3]-sigmatropic rearrangements include Cope and oxy-Cope rearrangements, where two π systems interact, as well as Claisen and Claisen-Cope rearrangements, where a π system interacts with an oxygen π system.
3. Cope, oxy-Cope and Claisen rearrangements can proceed with stereochemical inversion or retention, depending on the order and conditions, while Claisen-Cope rearrange
The document discusses the lanthanides and actinides, which are groups of elements found below the main periodic table. There are a total of 30 elements between the lanthanides (elements 57-71) and actinides (elements 89-103). The lanthanides and actinides are often referred to as the "inner transition metals" and exhibit similar chemical properties to lanthanum and actinium, respectively.
This chapter discusses the periodic table, explaining that elements are arranged in order of atomic number and grouped into periods and groups based on their electron configuration, with groups having similar properties and periods showing trends down the table. Properties of elements in groups I, VII, and 0 are described, including their physical states, reactivity, and chemical properties.
Redox Reaction and Electrochemical Cell (Reaksi Redoks dan Sel Elektrokimia)DindaKamaliya
An electrochemical cell converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells separated by a salt bridge. In the cathode half-cell, reduction occurs as oxidized species gain electrons. In the anode half-cell, oxidation occurs as reduced species lose electrons. Electrons flow through an external circuit from the anode to the cathode. The standard electrode potential of each half-reaction predicts the cell's voltage under standard conditions.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
This document summarizes the effective atomic number concept and the 18 electron rule for metal carbonyl compounds.
The effective atomic number (EAN) of a metal atom is calculated by adding the atomic number of the metal to twice the number of carbon monoxide ligands. This takes into account the electrons donated by CO to the metal center. Two examples of calculating EAN for mononuclear carbonyls are given.
The 18 electron rule states that the sum of the outer shell electrons of the metal atom and the electrons donated by carbon monoxide ligands should equal 18 for stable configurations. Two examples are provided to illustrate this rule.
This document presents information on reactive intermediates. It discusses four main types of reactive intermediates: carbocations, carbanions, free radicals, and carbenes. For each type, it describes examples, structures, factors that influence their stability, and common methods of generation. The document contains 19 slides covering an introduction, the four types of intermediates, conclusions, references, and acknowledgments.
This document provides an overview of metal clusters presented by Joel M. Smith at a Baran Group meeting. It begins with definitions of "cluster" and "metal cluster". The document then discusses the history of metal clusters, including important discoveries of polyoxometallates and metal carbonyl clusters. Preparation methods for metal clusters such as solution synthesis, hydrothermal synthesis, and reductive methods under CO atmosphere are described. Examples of reactions catalyzed by metal carbonyl clusters and polyoxometallate clusters are provided, including carbonylation, C-H oxidation, and dehydrogenation reactions.
1. A sigmatropic reaction is a rearrangement where a σ bond migrates within a conjugated π system, either suprafacially (same face) or antarafacially (opposite faces).
2. [3,3]-sigmatropic rearrangements include Cope and oxy-Cope rearrangements, where two π systems interact, as well as Claisen and Claisen-Cope rearrangements, where a π system interacts with an oxygen π system.
3. Cope, oxy-Cope and Claisen rearrangements can proceed with stereochemical inversion or retention, depending on the order and conditions, while Claisen-Cope rearrange
Percent Composition, Empirical and Molecular FormulaEllebasy Tranna
This document provides examples and explanations for calculating percent composition, empirical formulas, and molecular formulas. It begins with examples of calculating percent composition of elements in compounds and mixtures. It then defines empirical and molecular formulas, and provides steps for calculating empirical formulas from mass percentages of elements or experimental data. Several examples are worked through. The document emphasizes that empirical formulas show the simplest whole number ratio of elements in a compound, while molecular formulas indicate the actual number of each type of atom in a molecule.
This document provides an outline for 8 lessons on chemical kinetics for an IB Chemistry class. It includes objectives, content, and activities for each lesson. Lesson 1 reviews topic 6. Lessons 2-4 cover rate equations, determining rate experimentally, and evaluating reaction mechanisms. Lesson 5 discusses the rate-determining step. Lessons 6-7 focus on the Arrhenius equation and determining activation energy experimentally. Lesson 8 reviews the topic with exam questions. The lessons provide definitions, examples, and practice problems to help students understand reaction rates, orders, rate laws, mechanisms, and the temperature dependence of reaction rates.
Biological Applications & Environmental aspects of Organometallic CompoundsRudreshMr
It is the descriptive approach on Applicational aspects of Organometallic Compounds with a higly Interactive e-Content with appropriate links, references....
This document discusses coordination chemistry and transition metals. It begins by explaining why transition metals are important to study, as they are found in nature and have many applications. It then discusses the electronic configurations of transition metals and how they can exist in multiple oxidation states. The focus is on coordination complexes formed when transition metals act as Lewis acids and bond to other ligands. Different types of ligands are described along with common coordination geometries. Rules for naming coordination compounds according to IUPAC nomenclature are also provided.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
The document discusses various electrolytic processes including electrolysis of molten aluminum and electroplating of gold, silver, and lead. It explains that electrolysis uses electricity to drive chemical reactions like the reduction of aluminum ions to produce aluminum metal at the cathode. Impure metals can also be refined through electrorefining which uses electrolysis to oxidize impurities at the anode while reducing the desired metal at the cathode.
This document discusses thermometric titration, where the endpoint of a titration reaction is determined by measuring the temperature change. Key points:
- Titrant is added continuously and the temperature change is measured, with the endpoint identified by an inflection point on the temperature curve.
- The temperature change observed is directly related to the enthalpy change of the reaction.
- Factors like heat losses, temperature differences between titrant and analyte, and stirring must be controlled for accurate results.
- Automated systems use burets for precise titrant addition, a thermistor probe for temperature measurement, and software for data collection and endpoint determination.
- Parameters like mixing, probe placement,
IB Chemistry on Ionization energy and electron configurationLawrence kok
The document provides information on electron configuration and the organization of the periodic table. It discusses the s, p, d, and f "blocks" that elements are grouped into based on which orbitals are being filled with electrons. The s block has s orbitals partially filled, the p block has p orbitals partially filled, the d block has d orbitals partially filled and consists of transition elements, and the f block has f orbitals partially filled. It then provides examples of the electron configurations of various elements that exemplify these blocks and orbitals. It also discusses principles that govern the filling of electrons, such as the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
This document discusses the stereochemistry of allenes, spiranes, and biphenyls. It explains that allenes with different substituents on the terminal carbons can exhibit chirality and enantiomers. Spiranes can also show chirality and optical isomerism if they have different substituents. Biphenyls become chiral when large substituents in the ortho position prevent free rotation of the phenyl rings, leading to atropisomerism with a chiral axis and restricted rotation.
This document provides an introduction to nuclear chemistry. It discusses the basic components of atoms and how nuclear reactions differ from chemical reactions. It describes the three types of nuclear radiation (alpha, beta, gamma) and their properties. The document also covers radioactive decay and concepts such as decay constant, half-life, and average life. Additional topics include nuclear stability factors, mass defect and binding energy, and the application of radioisotopes as tracers and in radiotherapy, mutation breeding, and carbon dating.
The document discusses halogens and their medicinal uses. It covers the five halogens found in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine) and their physical properties like density and electronegativity decreasing from fluorine to iodine. Halogens and halogenides have medical importance, with chlorinated lime, iodine solutions, and salts like sodium chloride being used. Hypochlorites are also discussed as unstable compounds containing hypochlorite ion, used for bleaching, disinfection and water treatment when in aqueous solution.
The Zimmerman-Traxler model is invoked to rationalize the unexpected stereochemical outcomes of certain aldol reactions, such as the Reformatsky and Ivanov reactions. It models the stereochemistry of the products, based on the steric hindrance in the possible six-membered transition states in the aldol condensation reactions.
Created by Alexis Johnson (Undergraduate)
Edited by Margaret Hilton
Honors Organic Chemistry
CHEM 2321 (Sigman), 2013, University of Utah
Contains information about various crystal types in solid state chemistry like Rock Salt, Wurtzite, Nickel Arsenide, Zinc Blende etc. It also gives a brief description of lattice energy and Born Haber cycle.
Factors that determine the properties of a hydrocarbon are: The number of carbon atoms.
How the atoms are arranged: Straight chain, Branched chain, and Ring
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
This document discusses atomic structure and masses of atoms. It explains that the mass number of an atom equals the number of protons plus neutrons. Isotopes are atoms of the same element that have different mass numbers. The relative atomic mass of an atom is calculated relative to 1/12 the mass of a carbon-12 atom. To calculate the average atomic mass of an element, the percentage and atomic mass of each isotope is determined and a weighted average is calculated.
This document discusses the properties of various p-block elements, including boron, carbon, silicon, and aluminum. It provides general information on electron configurations, atomic radii, ionization energies, and trends within groups. Specific compounds are also examined, such as borax, boronic acid, diamond, graphite, fullerenes, silicon polymers, zeolites, and aluminum alloys. Common uses of carbon, silicon, and aluminum compounds/alloys in materials and applications are described. Global warming due to excessive carbon dioxide emissions is also briefly mentioned.
1. The document discusses calculating percent composition and determining empirical and molecular formulas.
2. To calculate percent composition, the formula mass is determined and the mass of each element is calculated as a percentage of the total mass.
3. An empirical formula shows the lowest whole number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms. Molecular formulas for ionic compounds are always empirical, while molecular formulas for molecular compounds may or may not be empirical.
This document discusses relative atomic mass and relative molecular mass. It provides examples to calculate these values.
The key points are:
1. Relative atomic mass (Ar) is the average mass of a single atom of an element compared to 1/12 the mass of one carbon-12 atom.
2. The relative molecular mass (Mr) of a molecule is the sum of the relative atomic masses of all the atoms in the molecule.
3. Examples are provided to calculate relative atomic masses and relative molecular masses using atomic mass values and molecular formulas. Formulas, atomic masses, and molecular masses are compared to calculate unknown values.
This document provides an overview of basic chemistry concepts and calculations. It begins by explaining that chemistry is involved in everyday life through materials like polymers, drugs, and alloys. Matter can be classified based on physical state as solid, liquid, or gas, and chemically as pure substances or mixtures. Elements are composed of single atom types, while compounds contain two or more different atom types bonded together. The mole concept allows chemists to quantify amounts of substances down to the molecular level. Chemical calculations can be performed based on molar mass, stoichiometry from balanced equations, and other relationships between amounts of reactants and products.
This document provides an overview of basic chemistry concepts and calculations. It begins by explaining that chemistry is involved in everyday life through materials like polymers, drugs, and alloys. Matter can be classified based on physical state as solid, liquid, or gas, and chemically as pure substances or mixtures. Elements are composed of single atom types that can be monatomic or polyatomic. Compounds contain two or more elements. The mole concept is introduced to quantify atoms and molecules using Avogadro's number. Empirical and molecular formulas are distinguished. Methods for determining formulas from elemental analysis or molar mass are presented. Equivalent mass and stoichiometric calculations are also covered.
Percent Composition, Empirical and Molecular FormulaEllebasy Tranna
This document provides examples and explanations for calculating percent composition, empirical formulas, and molecular formulas. It begins with examples of calculating percent composition of elements in compounds and mixtures. It then defines empirical and molecular formulas, and provides steps for calculating empirical formulas from mass percentages of elements or experimental data. Several examples are worked through. The document emphasizes that empirical formulas show the simplest whole number ratio of elements in a compound, while molecular formulas indicate the actual number of each type of atom in a molecule.
This document provides an outline for 8 lessons on chemical kinetics for an IB Chemistry class. It includes objectives, content, and activities for each lesson. Lesson 1 reviews topic 6. Lessons 2-4 cover rate equations, determining rate experimentally, and evaluating reaction mechanisms. Lesson 5 discusses the rate-determining step. Lessons 6-7 focus on the Arrhenius equation and determining activation energy experimentally. Lesson 8 reviews the topic with exam questions. The lessons provide definitions, examples, and practice problems to help students understand reaction rates, orders, rate laws, mechanisms, and the temperature dependence of reaction rates.
Biological Applications & Environmental aspects of Organometallic CompoundsRudreshMr
It is the descriptive approach on Applicational aspects of Organometallic Compounds with a higly Interactive e-Content with appropriate links, references....
This document discusses coordination chemistry and transition metals. It begins by explaining why transition metals are important to study, as they are found in nature and have many applications. It then discusses the electronic configurations of transition metals and how they can exist in multiple oxidation states. The focus is on coordination complexes formed when transition metals act as Lewis acids and bond to other ligands. Different types of ligands are described along with common coordination geometries. Rules for naming coordination compounds according to IUPAC nomenclature are also provided.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
The document discusses various electrolytic processes including electrolysis of molten aluminum and electroplating of gold, silver, and lead. It explains that electrolysis uses electricity to drive chemical reactions like the reduction of aluminum ions to produce aluminum metal at the cathode. Impure metals can also be refined through electrorefining which uses electrolysis to oxidize impurities at the anode while reducing the desired metal at the cathode.
This document discusses thermometric titration, where the endpoint of a titration reaction is determined by measuring the temperature change. Key points:
- Titrant is added continuously and the temperature change is measured, with the endpoint identified by an inflection point on the temperature curve.
- The temperature change observed is directly related to the enthalpy change of the reaction.
- Factors like heat losses, temperature differences between titrant and analyte, and stirring must be controlled for accurate results.
- Automated systems use burets for precise titrant addition, a thermistor probe for temperature measurement, and software for data collection and endpoint determination.
- Parameters like mixing, probe placement,
IB Chemistry on Ionization energy and electron configurationLawrence kok
The document provides information on electron configuration and the organization of the periodic table. It discusses the s, p, d, and f "blocks" that elements are grouped into based on which orbitals are being filled with electrons. The s block has s orbitals partially filled, the p block has p orbitals partially filled, the d block has d orbitals partially filled and consists of transition elements, and the f block has f orbitals partially filled. It then provides examples of the electron configurations of various elements that exemplify these blocks and orbitals. It also discusses principles that govern the filling of electrons, such as the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
This document discusses the stereochemistry of allenes, spiranes, and biphenyls. It explains that allenes with different substituents on the terminal carbons can exhibit chirality and enantiomers. Spiranes can also show chirality and optical isomerism if they have different substituents. Biphenyls become chiral when large substituents in the ortho position prevent free rotation of the phenyl rings, leading to atropisomerism with a chiral axis and restricted rotation.
This document provides an introduction to nuclear chemistry. It discusses the basic components of atoms and how nuclear reactions differ from chemical reactions. It describes the three types of nuclear radiation (alpha, beta, gamma) and their properties. The document also covers radioactive decay and concepts such as decay constant, half-life, and average life. Additional topics include nuclear stability factors, mass defect and binding energy, and the application of radioisotopes as tracers and in radiotherapy, mutation breeding, and carbon dating.
The document discusses halogens and their medicinal uses. It covers the five halogens found in group 17 of the periodic table (fluorine, chlorine, bromine, iodine, astatine) and their physical properties like density and electronegativity decreasing from fluorine to iodine. Halogens and halogenides have medical importance, with chlorinated lime, iodine solutions, and salts like sodium chloride being used. Hypochlorites are also discussed as unstable compounds containing hypochlorite ion, used for bleaching, disinfection and water treatment when in aqueous solution.
The Zimmerman-Traxler model is invoked to rationalize the unexpected stereochemical outcomes of certain aldol reactions, such as the Reformatsky and Ivanov reactions. It models the stereochemistry of the products, based on the steric hindrance in the possible six-membered transition states in the aldol condensation reactions.
Created by Alexis Johnson (Undergraduate)
Edited by Margaret Hilton
Honors Organic Chemistry
CHEM 2321 (Sigman), 2013, University of Utah
Contains information about various crystal types in solid state chemistry like Rock Salt, Wurtzite, Nickel Arsenide, Zinc Blende etc. It also gives a brief description of lattice energy and Born Haber cycle.
Factors that determine the properties of a hydrocarbon are: The number of carbon atoms.
How the atoms are arranged: Straight chain, Branched chain, and Ring
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
This document discusses atomic structure and masses of atoms. It explains that the mass number of an atom equals the number of protons plus neutrons. Isotopes are atoms of the same element that have different mass numbers. The relative atomic mass of an atom is calculated relative to 1/12 the mass of a carbon-12 atom. To calculate the average atomic mass of an element, the percentage and atomic mass of each isotope is determined and a weighted average is calculated.
This document discusses the properties of various p-block elements, including boron, carbon, silicon, and aluminum. It provides general information on electron configurations, atomic radii, ionization energies, and trends within groups. Specific compounds are also examined, such as borax, boronic acid, diamond, graphite, fullerenes, silicon polymers, zeolites, and aluminum alloys. Common uses of carbon, silicon, and aluminum compounds/alloys in materials and applications are described. Global warming due to excessive carbon dioxide emissions is also briefly mentioned.
1. The document discusses calculating percent composition and determining empirical and molecular formulas.
2. To calculate percent composition, the formula mass is determined and the mass of each element is calculated as a percentage of the total mass.
3. An empirical formula shows the lowest whole number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms. Molecular formulas for ionic compounds are always empirical, while molecular formulas for molecular compounds may or may not be empirical.
This document discusses relative atomic mass and relative molecular mass. It provides examples to calculate these values.
The key points are:
1. Relative atomic mass (Ar) is the average mass of a single atom of an element compared to 1/12 the mass of one carbon-12 atom.
2. The relative molecular mass (Mr) of a molecule is the sum of the relative atomic masses of all the atoms in the molecule.
3. Examples are provided to calculate relative atomic masses and relative molecular masses using atomic mass values and molecular formulas. Formulas, atomic masses, and molecular masses are compared to calculate unknown values.
This document provides an overview of basic chemistry concepts and calculations. It begins by explaining that chemistry is involved in everyday life through materials like polymers, drugs, and alloys. Matter can be classified based on physical state as solid, liquid, or gas, and chemically as pure substances or mixtures. Elements are composed of single atom types, while compounds contain two or more different atom types bonded together. The mole concept allows chemists to quantify amounts of substances down to the molecular level. Chemical calculations can be performed based on molar mass, stoichiometry from balanced equations, and other relationships between amounts of reactants and products.
This document provides an overview of basic chemistry concepts and calculations. It begins by explaining that chemistry is involved in everyday life through materials like polymers, drugs, and alloys. Matter can be classified based on physical state as solid, liquid, or gas, and chemically as pure substances or mixtures. Elements are composed of single atom types that can be monatomic or polyatomic. Compounds contain two or more elements. The mole concept is introduced to quantify atoms and molecules using Avogadro's number. Empirical and molecular formulas are distinguished. Methods for determining formulas from elemental analysis or molar mass are presented. Equivalent mass and stoichiometric calculations are also covered.
This document provides an overview of basic chemistry concepts and calculations. It begins by explaining that chemistry is involved in everyday life through materials like polymers, drugs, and alloys. Matter can be classified based on physical state as solid, liquid, or gas, and chemically as pure substances or mixtures. Elements are composed of single atom types that can be monatomic or polyatomic. Compounds contain two or more elements. The mole concept is introduced to quantify atoms and molecules using Avogadro's number of 6.022x1023 particles. Empirical and molecular formulas are distinguished. Methods are described for determining empirical formulas from elemental analysis data and calculating molecular formulas. Stoichiometry allows determining quantitative relationships between reactants and products in chemical equations
- Relative atomic mass (RAM) is a weighted average mass of a chemical element's atoms as compared to 1/12 the mass of one carbon-12 atom and is expressed in atomic mass units.
- RAM is calculated by determining the atomic mass and natural abundance of each isotope of an element, then taking a weighted average of these values.
- The mole is the standard unit used to express the amount of a substance and refers to Avogadro's number of atoms, molecules, or other particles. It allows for direct calculation of mass from molar mass and vice versa.
John Dalton proposed the first scientific atomic theory, which stated that each chemical element is composed of atoms of a single, unique type that can combine to form chemical compounds. An atom is the fundamental unit of matter and consists of a nucleus containing protons and neutrons surrounded by electrons. Atoms of the same element contain the same number of protons but can vary in the number of neutrons, resulting in different isotopes of that element. Molecules are the smallest fundamental units of compounds made of two or more atoms bonded together.
This document discusses relative atomic mass (Ar) and relative molecular mass (Mr). It defines these terms and provides examples of calculating them.
Ar is a ratio of the average mass of a given atom to 1/12 the mass of one carbon-12 atom. It allows easy comparison of atomic masses. Mr is the sum of Ar values for all atoms in a molecule or polyatomic ion. Examples are given for calculating Mr of common substances like CO2, glucose, and ionic compounds. The document also addresses why some Ar values are not whole numbers due to isotope mixtures.
Atoms combine to form molecules, and molecules combine to form compounds. Mass spectrometry can determine the relative masses of atoms and molecules. It works by converting samples into ion beams, which are then deflected by electric and magnetic fields based on their mass-to-charge ratio. This allows scientists to determine molecular formulas by identifying molecular fragments and isotope abundances. Stoichiometry uses this information to calculate quantities of materials involved in chemical reactions.
This document defines key terms related to atomic structure and isotopes. It explains that atoms are made up of protons and neutrons in the nucleus surrounded by electrons. The atomic number (Z) represents the number of protons, while the mass number (A) is the total number of protons and neutrons. Isotopes are atoms of the same element with different numbers of neutrons. Isotopes have similar chemical properties but different physical properties like mass and density due to varying numbers of neutrons. The relative atomic mass (Ar) takes into account the natural abundance of isotopes and represents the average mass of atoms of an element.
Relative masses of atoms and moleculesericseow1997
The document discusses relative atomic and molecular masses. It explains that relative atomic mass is used to compare the mass of atoms to hydrogen, with hydrogen defined as 1. Molecular mass is the average mass of a molecule compared to 1/12 the mass of a carbon-12 atom. Molecular mass can be calculated by adding the relative atomic masses of the elements in a compound. Knowing the relative masses allows calculating the mass of elements in samples of compounds. Hydrated compounds contain water that is included in their chemical formula for mass calculations.
Organic compounds are almost 60% of all compounds. because of carbons tendency to form a compound as it has more than1 electron(4electrons) to form covallent compounds. SO a wide range of everything we eat is formed from carbon and hydrogen, which is the second important element to form organic compounds.
Relative molecular mass and percentage compositionyizeng
The relative molecular mass (Mr) of a molecule is calculated by adding the relative atomic masses of all the atoms in the molecule. It is a ratio comparing the average mass of a molecule to 1/12 the mass of one atom of carbon-12 or one hydrogen atom. Some examples are given of calculating the Mr of carbon dioxide (CO2), sugar (C12H22O11), and sulfuric acid (H2SO4). The percentage composition of elements in compounds can be calculated from the formula and relative atomic masses. The mass of an element in a sample can then be determined from the percentage composition and total mass of the compound. Empirical formulas can be determined from the masses of elements that combine or from percentage
The document discusses several important laws and concepts in chemistry:
1) The Law of Constant Composition states that a chemical compound always contains the same elements in the same proportions by mass.
2) The Law of Conservation of Mass says that mass is neither created nor destroyed in chemical reactions.
3) The Law of Multiple Proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element are ratios of small whole numbers.
4) Concepts like molar mass, the mole, and stoichiometry provide quantitative relationships between substances in chemical equations and reactions.
This document provides information about relative atomic masses and how they are determined. It discusses how chemists use a relative scale rather than actual atomic masses, which are too small to measure. On this scale, carbon-12 is assigned a mass of 12. Isotopes of each element have different relative isotopic masses. A mass spectrometer is used to separate isotopes and determine their relative abundances. The average relative atomic mass (Ar) of an element is calculated based on the relative isotopic masses and abundances of its isotopes. Molecular and formula masses can also be determined by adding the relative atomic masses of each atom in a molecule or compound unit.
For more such informative content, go to https://scifitechify.blogspot.com/. This video will introduce you to the world of ATOMS & MOLECULES. HOPE YOU ENJOY IT. NEXT POST ON: WHY DO WE WEIGH LESS ON THE MOON ?
This lecture covers the basics of matter including the three phases of matter, classification of matter as pure substances or mixtures, and the key differences between elements, compounds, and mixtures. It also discusses atomic structure including atoms, ions, isotopes, and the atomic mass scale. The lecture defines important terms like atomic number, mass number, relative atomic mass. It describes how to name ionic and molecular compounds using common nomenclature rules. Key topics covered include Dalton's atomic theory, the mass spectrometer, and different families of ions like oxoanions.
This document provides an overview of organic chemistry and organic medicinal chemistry. It discusses general chemistry topics including the definition of chemistry, classification of matter, physical and chemical properties, and acid-base properties. It also covers organic chemistry topics such as the difference between inorganic and organic chemistry, functional groups, isomerism, and reactions. The document is intended to serve as a refresher course on these fundamental concepts.
This document provides an overview of organic chemistry and organic medicinal chemistry concepts. It discusses the definition of chemistry and its role in modern life, including biological molecules, biochemical processes, and drug discovery. It covers classification of matter into elements, compounds, mixtures and pure substances. It also describes physical and chemical properties and changes, as well as measurement units, temperature, volume, mass, precision, accuracy, and significant figures. The document serves as a refresher for these fundamental chemistry concepts relevant to organic chemistry and drug development.
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This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
How to Make a Field Mandatory in Odoo 17Celine George
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In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
11. Relative Molecular Mass
The ratio of the average mass of one molecule of an element or
compound to one twelfth of the mass of an atom of carbon-12.
Formula:
13. Relative Formula Mass
The relative formula mass of an ionic molecule is the ratio of sum of the
atomic weights of the atoms in the formula of the ionic compound and
1/12th of the mass of one atom of C-12.
Formula:
15. Summery
• We did Atomic, Isotopic, Molecular and Formula masses.
• Which are relative to s standard “ 1/12th of mass of one
atom of C-12”.
16. Try it out
• Calculate the molecular masses of : HNO3, H2SO4,
AgNO3.
• List out the atomic masses of: Zn, V , Mn , Fe.
• Give three examples of elements having isotopes.
Mention them with their isotopic masses.