1) Hess's law states that the overall enthalpy change of a chemical reaction is independent of the pathway taken, meaning you can find the enthalpy change of a reaction by adding the individual enthalpy changes of consecutive steps.
2) For the reaction of dissolving sodium hydroxide and reacting it with hydrochloric acid, Hess's law is demonstrated by showing that the enthalpy change of dissolving NaOH then reacting it with HCl equals the direct reaction of solid NaOH with HCl.
3) Bond enthalpies can be used to calculate the enthalpy change of a reaction by adding the bond energies needed to break bonds of reactants and subtracting the bond energies
Macromolecules are large molecules built from small repeating units joined by covalent bonds. There are two main types: synthetic polymers made from monomers linked through addition or condensation polymerization, and natural macromolecules like proteins, fats, and carbohydrates composed of amino acids, fatty acids, and sugars. Synthetic polymers have various uses but can pollute as they are non-biodegradable, while natural macromolecules are the main constituents of living things.
Nature of Bonding in Organic Molecules - Sahana KamathBebeto G
The document discusses the nature of bonding in organic molecules. It describes the different types of hybridization that carbon undergoes, including sp3, sp2, and sp hybridization, and how this allows carbon to form single, double, and triple bonds. It also discusses sigma and pi bonds, bond length, bond angle, bond energy, localized and delocalized bonds, and hydrogen bonding. In summary:
1) Carbon can undergo sp3, sp2, and sp hybridization to form tetrahedral, trigonal planar, and linear geometries respectively and allow carbon to form single, double, and triple bonds.
2) Sigma bonds are formed by head-on overlap of orbitals while pi bonds involve side
In this slide you can get about ,what are oxides and how they classify. In this slides I classify the oxides with respect to nature of oxides as well as the oxygen content in it.
1. Hemerythrin and hemocyanin are metalloproteins that transport oxygen in invertebrates. Hemerythrin contains iron centers while hemocyanin contains copper centers that reversibly bind oxygen.
2. Hemerythrin exists as an octamer with subunits containing two iron centers bridged by carboxylate groups. In the oxygenated form, it contains a high spin diiron(III) core with an oxo bridge. Hemocyanin exists as suspended in hemolymph and its subunits undergo a significant structural change upon oxygenation.
3. Both proteins show antiferromagnetic coupling between their metal centers in the oxygenated state. However, oxy-hemery
The document discusses epoxides, including their structure, nomenclature, preparation methods, and reactions. Epoxides contain an oxygen atom as part of a three-membered ring and have angle strain, making them reactive. They can be prepared by epoxidation of alkenes using peroxy acids or from vicinal halohydrins using an intramolecular nucleophilic substitution reaction. Epoxides undergo ring-opening reactions with strong nucleophiles or acids via SN2-like mechanisms at one carbon, controlled by substituent effects.
Gases are composed of tiny particles that are in constant, random motion. Three properties of gases are pressure, volume, and temperature. The kinetic molecular theory and gas laws describe the relationships between these properties. The ideal gas law combines earlier gas laws relating pressure, volume, amount of gas, and temperature into a single equation.
1) Hess's law states that the overall enthalpy change of a chemical reaction is independent of the pathway taken, meaning you can find the enthalpy change of a reaction by adding the individual enthalpy changes of consecutive steps.
2) For the reaction of dissolving sodium hydroxide and reacting it with hydrochloric acid, Hess's law is demonstrated by showing that the enthalpy change of dissolving NaOH then reacting it with HCl equals the direct reaction of solid NaOH with HCl.
3) Bond enthalpies can be used to calculate the enthalpy change of a reaction by adding the bond energies needed to break bonds of reactants and subtracting the bond energies
Macromolecules are large molecules built from small repeating units joined by covalent bonds. There are two main types: synthetic polymers made from monomers linked through addition or condensation polymerization, and natural macromolecules like proteins, fats, and carbohydrates composed of amino acids, fatty acids, and sugars. Synthetic polymers have various uses but can pollute as they are non-biodegradable, while natural macromolecules are the main constituents of living things.
Nature of Bonding in Organic Molecules - Sahana KamathBebeto G
The document discusses the nature of bonding in organic molecules. It describes the different types of hybridization that carbon undergoes, including sp3, sp2, and sp hybridization, and how this allows carbon to form single, double, and triple bonds. It also discusses sigma and pi bonds, bond length, bond angle, bond energy, localized and delocalized bonds, and hydrogen bonding. In summary:
1) Carbon can undergo sp3, sp2, and sp hybridization to form tetrahedral, trigonal planar, and linear geometries respectively and allow carbon to form single, double, and triple bonds.
2) Sigma bonds are formed by head-on overlap of orbitals while pi bonds involve side
In this slide you can get about ,what are oxides and how they classify. In this slides I classify the oxides with respect to nature of oxides as well as the oxygen content in it.
1. Hemerythrin and hemocyanin are metalloproteins that transport oxygen in invertebrates. Hemerythrin contains iron centers while hemocyanin contains copper centers that reversibly bind oxygen.
2. Hemerythrin exists as an octamer with subunits containing two iron centers bridged by carboxylate groups. In the oxygenated form, it contains a high spin diiron(III) core with an oxo bridge. Hemocyanin exists as suspended in hemolymph and its subunits undergo a significant structural change upon oxygenation.
3. Both proteins show antiferromagnetic coupling between their metal centers in the oxygenated state. However, oxy-hemery
The document discusses epoxides, including their structure, nomenclature, preparation methods, and reactions. Epoxides contain an oxygen atom as part of a three-membered ring and have angle strain, making them reactive. They can be prepared by epoxidation of alkenes using peroxy acids or from vicinal halohydrins using an intramolecular nucleophilic substitution reaction. Epoxides undergo ring-opening reactions with strong nucleophiles or acids via SN2-like mechanisms at one carbon, controlled by substituent effects.
Gases are composed of tiny particles that are in constant, random motion. Three properties of gases are pressure, volume, and temperature. The kinetic molecular theory and gas laws describe the relationships between these properties. The ideal gas law combines earlier gas laws relating pressure, volume, amount of gas, and temperature into a single equation.
1) Various chemical reactions and analyses showed that glucose has the molecular formula C6H12O6 and consists of a six-carbon chain with one aldehyde group, one primary alcohol group, and four other hydroxyl groups.
2) Determining the configurations of D-glucose involved studying its relationship to D-arabinose and other sugars. This indicated that D-glucose has the D configuration shown by structure VII.
3) Further evidence that structure VII represents D-glucose came from comparing it to L-gulose, which upon oxidation produces the same diacid product as D-glucose.
Benzene is an organic compound with the formula C6H6 that is a colorless, flammable liquid. It is a natural constituent of crude oil and is produced industrially from petroleum as well as through catalytic reforming, toluene hydrodealkylation, toluene disproportionation, and steam cracking. Benzene's structure involves delocalized pi bonding that contributes to its stability and defines its chemical properties. It is used mainly to produce other chemicals including styrene, phenol, cyclohexane, and naphthalene.
This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.
This document discusses stoichiometric calculations for combustion reactions. It begins by outlining applications of the combustion equation for determining correct air supply rates and combustion product composition. It then provides detailed explanations and examples of calculating air requirements and combustion products for gaseous, solid, and liquid fuels using elemental analyses and accounting for excess air. Specific topics covered include determining stoichiometric air-to-fuel ratios, calculating flue gas composition, and the relationship between carbon-hydrogen ratio in fuels and carbon dioxide concentration in flue gases. Worked examples are provided to demonstrate the stoichiometric calculation methods.
This document provides information on chemistry topics including shapes of molecules, carbon structures, polar bonds, intermolecular forces, solubility, redox reactions, group 2 elements, flame tests, the halogens, indicators, kinetics, chemical equilibria, alcohols, oxidation of alcohols, haloalkanes, and nucleophilic substitution reactions. Key concepts covered include VSEPR theory, the three allotropes of carbon, electronegativity, types of intermolecular forces, factors affecting solubility, rules for oxidation numbers, reactions of group 2 elements, uses of flame tests, properties of the halogens and halides, common acid-base indicators, Maxwell-Boltzmann distribution
Explain chemical properties of alcohols by various chemical reactions
Define and explain preparation of ethers from alcohols by using chemical equations
This document describes different types of covalent bonding, including:
1) Covalent bonds form when electron pairs are shared between two atoms, attracting their nuclei together.
2) Covalent compounds are usually composed of nonmetals and include many familiar substances like water and methane.
3) Dot and cross diagrams can represent covalent bonds, showing shared electron pairs between atoms.
The document discusses the determination of dipole moments of polar molecules in non-polar solvents. It defines the dipole moment as the separation of positive and negative charges in a molecule. The dipole moment is determined by measuring the relative permittivity and refractive index of solutions, which relate to molecular polarization from an applied electric field. The Debye equation describes this relationship and can be used to calculate dipole moments from experimental data.
This document discusses the octet rule for chemical bonding. It states that the octet rule describes the tendency of atoms to attain noble gas configurations by gaining, losing or sharing electrons to acquire eight electrons in their outer shell. There are exceptions when the octet is not complete, such as with boron trifluoride (BF3), or when it is expanded as in phosphorus pentachloride (PCl5) which has 10 electrons around the phosphorus atom. The limitations of the octet rule are also outlined.
Alkanes are saturated hydrocarbons with only carbon-carbon single bonds. Their general formula is CnH2n+2. Alkanes have low reactivity due to strong C-C and C-H bonds. They undergo combustion, producing carbon dioxide and water. In the presence of light, alkanes undergo substitution reactions with halogens like chlorine. Alkanes find many uses depending on their carbon number, such as fuels, solvents, polymers, and paraffin wax. Natural gas and petroleum contain alkanes that are crucial energy resources.
Hyperconjugation occurs when a σ bond and adjacent π bond become involved in resonance. This delocalization stabilizes molecules like carbocations, free radicals, alkenes, and alkynes. Specifically, hyperconjugation in carbocations involves overlap between the carbocation's empty p-orbital and the σ orbitals of alpha hydrogens. In free radicals, it is the overlap between the odd electron's p-orbital and the σ orbital of an alkyl group. For alkenes and alkynes, stability arises from partial overlap between sp3 σ orbitals and the π orbitals of the multiple bonds. This document discusses the hyperconjugation resonance structure effects in different organic molecules.
Group 15 of the periodic table consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements can be non-metals, metalloids, or metals. They have the general electronic configuration of ns2np3 and can form compounds with oxidation states of -3, +3, and +5. The reactivity and properties of the elements change as one goes down the group due to an increase in atomic size and metallic character.
The document summarizes key information about carboxylic acids from their general formula of RCOOH to their characteristic properties and reactions. It discusses (1) the nomenclature and structures of carboxylic acids, (2) their higher boiling points and water solubility compared to similar molecules due to hydrogen bonding, (3) their acidity stemming from ionization of the carboxyl group, and (4) several important reactions including preparation by oxidation, esterification, and formation of derivatives like acid chlorides, anhydrides, salts, and amides.
Tang 06 valence bond theory and hybridizationmrtangextrahelp
The document discusses valence bond theory and hybridization. Valence bond theory explains how covalent bonds form through the overlapping of atomic orbitals. Hybridization occurs when atomic orbitals combine to form new hybrid orbitals. This allows atoms to form more bonds than their valence shell configuration suggests. Carbon can form 4 bonds through sp3 hybridization where one 2s and three 2p orbitals combine. Hybridization also explains bonding in molecules such as methane (CH4), ethene (C2H4), ethyne (C2H2), and benzene (C6H6). It further discusses how hybridization allows atoms like boron, beryllium, sulfur, and phosphorus to attain unusual bonding configurations
Valence shell electron pair repulsion theory (VSEPR THEORY)Altamash Ali
Designed in a very easy manner so that u all are able to understand each and everything easily.
Gillespie & Nyholm proposed this theory ion 1957 and its is based on the direction of bonds in a polyatomic molecule.
Based on this there are several postulate that are very necessary to know before any molecule to study.
Alcohols contain an -OH group bonded to a carbon atom. They are classified based on the carbon the OH group is attached to as primary, secondary, or tertiary alcohols. Alcohols have higher boiling points than similar hydrocarbons due to hydrogen bonding. Common alcohols include methanol, ethanol, and isopropyl alcohol. Alcohols are used in drinks, fuels, solvents, and to synthesize other organic compounds. Phenol contains an OH group bonded directly to a benzene ring. It is used as an antiseptic and in making resins, plastics, and pharmaceuticals. Phenol undergoes electrophilic aromatic substitution reactions more readily than benz
Alkynes are hydrocarbons with a triple bond between two carbon atoms. Common alkynes include acetylene (C2H2), propyne, butyne, pentyne, etc. Their molecular formulas follow the pattern of CnH2n-2. Alkynes are named based on the number of carbons and whether the chain is straight or branched. They are generally reactive due to the triple bond. Alkynes undergo addition, polymerization, substitution, and combustion reactions. They can also form isomers based on chain structure or carbon position.
This document provides information and examples for calculating percent composition, empirical formulas, and molecular formulas of compounds. It defines key terms like percent composition and empirical formula. It then works through examples of calculating the percent composition of magnesium and oxygen that form a compound, the percent composition and mass of carbon in propane, and determining empirical formulas from elemental percentages or mole ratios. The document explains how to calculate molecular formulas from empirical formulas and molar masses. Finally, it provides practice problems for the reader to work through.
This document discusses different types of chemical formulas used to represent compounds:
- A chemical compound is made of two or more elements that are combined in fixed ratios.
- The chemical formula uses symbols of the elements and subscripts to show the relative proportions.
- The empirical formula shows the lowest whole number ratio of atoms in a compound, while the molecular formula gives the exact number of each atom.
- The structural formula depicts the specific bonding arrangement of the atoms in a compound.
1) Various chemical reactions and analyses showed that glucose has the molecular formula C6H12O6 and consists of a six-carbon chain with one aldehyde group, one primary alcohol group, and four other hydroxyl groups.
2) Determining the configurations of D-glucose involved studying its relationship to D-arabinose and other sugars. This indicated that D-glucose has the D configuration shown by structure VII.
3) Further evidence that structure VII represents D-glucose came from comparing it to L-gulose, which upon oxidation produces the same diacid product as D-glucose.
Benzene is an organic compound with the formula C6H6 that is a colorless, flammable liquid. It is a natural constituent of crude oil and is produced industrially from petroleum as well as through catalytic reforming, toluene hydrodealkylation, toluene disproportionation, and steam cracking. Benzene's structure involves delocalized pi bonding that contributes to its stability and defines its chemical properties. It is used mainly to produce other chemicals including styrene, phenol, cyclohexane, and naphthalene.
This chapter discusses the evolution of atomic models and the arrangement of electrons in atoms. It covers difficult concepts such as electrons occupying specific energy levels and orbitals. Students are advised to do all assigned homework and bring their textbook to class to fully understand these abstract ideas. Key models discussed include the Rutherford model, the planetary model, Bohr's model linking electrons and photon emission, and the modern quantum mechanical model based on probability.
This document discusses stoichiometric calculations for combustion reactions. It begins by outlining applications of the combustion equation for determining correct air supply rates and combustion product composition. It then provides detailed explanations and examples of calculating air requirements and combustion products for gaseous, solid, and liquid fuels using elemental analyses and accounting for excess air. Specific topics covered include determining stoichiometric air-to-fuel ratios, calculating flue gas composition, and the relationship between carbon-hydrogen ratio in fuels and carbon dioxide concentration in flue gases. Worked examples are provided to demonstrate the stoichiometric calculation methods.
This document provides information on chemistry topics including shapes of molecules, carbon structures, polar bonds, intermolecular forces, solubility, redox reactions, group 2 elements, flame tests, the halogens, indicators, kinetics, chemical equilibria, alcohols, oxidation of alcohols, haloalkanes, and nucleophilic substitution reactions. Key concepts covered include VSEPR theory, the three allotropes of carbon, electronegativity, types of intermolecular forces, factors affecting solubility, rules for oxidation numbers, reactions of group 2 elements, uses of flame tests, properties of the halogens and halides, common acid-base indicators, Maxwell-Boltzmann distribution
Explain chemical properties of alcohols by various chemical reactions
Define and explain preparation of ethers from alcohols by using chemical equations
This document describes different types of covalent bonding, including:
1) Covalent bonds form when electron pairs are shared between two atoms, attracting their nuclei together.
2) Covalent compounds are usually composed of nonmetals and include many familiar substances like water and methane.
3) Dot and cross diagrams can represent covalent bonds, showing shared electron pairs between atoms.
The document discusses the determination of dipole moments of polar molecules in non-polar solvents. It defines the dipole moment as the separation of positive and negative charges in a molecule. The dipole moment is determined by measuring the relative permittivity and refractive index of solutions, which relate to molecular polarization from an applied electric field. The Debye equation describes this relationship and can be used to calculate dipole moments from experimental data.
This document discusses the octet rule for chemical bonding. It states that the octet rule describes the tendency of atoms to attain noble gas configurations by gaining, losing or sharing electrons to acquire eight electrons in their outer shell. There are exceptions when the octet is not complete, such as with boron trifluoride (BF3), or when it is expanded as in phosphorus pentachloride (PCl5) which has 10 electrons around the phosphorus atom. The limitations of the octet rule are also outlined.
Alkanes are saturated hydrocarbons with only carbon-carbon single bonds. Their general formula is CnH2n+2. Alkanes have low reactivity due to strong C-C and C-H bonds. They undergo combustion, producing carbon dioxide and water. In the presence of light, alkanes undergo substitution reactions with halogens like chlorine. Alkanes find many uses depending on their carbon number, such as fuels, solvents, polymers, and paraffin wax. Natural gas and petroleum contain alkanes that are crucial energy resources.
Hyperconjugation occurs when a σ bond and adjacent π bond become involved in resonance. This delocalization stabilizes molecules like carbocations, free radicals, alkenes, and alkynes. Specifically, hyperconjugation in carbocations involves overlap between the carbocation's empty p-orbital and the σ orbitals of alpha hydrogens. In free radicals, it is the overlap between the odd electron's p-orbital and the σ orbital of an alkyl group. For alkenes and alkynes, stability arises from partial overlap between sp3 σ orbitals and the π orbitals of the multiple bonds. This document discusses the hyperconjugation resonance structure effects in different organic molecules.
Group 15 of the periodic table consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements can be non-metals, metalloids, or metals. They have the general electronic configuration of ns2np3 and can form compounds with oxidation states of -3, +3, and +5. The reactivity and properties of the elements change as one goes down the group due to an increase in atomic size and metallic character.
The document summarizes key information about carboxylic acids from their general formula of RCOOH to their characteristic properties and reactions. It discusses (1) the nomenclature and structures of carboxylic acids, (2) their higher boiling points and water solubility compared to similar molecules due to hydrogen bonding, (3) their acidity stemming from ionization of the carboxyl group, and (4) several important reactions including preparation by oxidation, esterification, and formation of derivatives like acid chlorides, anhydrides, salts, and amides.
Tang 06 valence bond theory and hybridizationmrtangextrahelp
The document discusses valence bond theory and hybridization. Valence bond theory explains how covalent bonds form through the overlapping of atomic orbitals. Hybridization occurs when atomic orbitals combine to form new hybrid orbitals. This allows atoms to form more bonds than their valence shell configuration suggests. Carbon can form 4 bonds through sp3 hybridization where one 2s and three 2p orbitals combine. Hybridization also explains bonding in molecules such as methane (CH4), ethene (C2H4), ethyne (C2H2), and benzene (C6H6). It further discusses how hybridization allows atoms like boron, beryllium, sulfur, and phosphorus to attain unusual bonding configurations
Valence shell electron pair repulsion theory (VSEPR THEORY)Altamash Ali
Designed in a very easy manner so that u all are able to understand each and everything easily.
Gillespie & Nyholm proposed this theory ion 1957 and its is based on the direction of bonds in a polyatomic molecule.
Based on this there are several postulate that are very necessary to know before any molecule to study.
Alcohols contain an -OH group bonded to a carbon atom. They are classified based on the carbon the OH group is attached to as primary, secondary, or tertiary alcohols. Alcohols have higher boiling points than similar hydrocarbons due to hydrogen bonding. Common alcohols include methanol, ethanol, and isopropyl alcohol. Alcohols are used in drinks, fuels, solvents, and to synthesize other organic compounds. Phenol contains an OH group bonded directly to a benzene ring. It is used as an antiseptic and in making resins, plastics, and pharmaceuticals. Phenol undergoes electrophilic aromatic substitution reactions more readily than benz
Alkynes are hydrocarbons with a triple bond between two carbon atoms. Common alkynes include acetylene (C2H2), propyne, butyne, pentyne, etc. Their molecular formulas follow the pattern of CnH2n-2. Alkynes are named based on the number of carbons and whether the chain is straight or branched. They are generally reactive due to the triple bond. Alkynes undergo addition, polymerization, substitution, and combustion reactions. They can also form isomers based on chain structure or carbon position.
This document provides information and examples for calculating percent composition, empirical formulas, and molecular formulas of compounds. It defines key terms like percent composition and empirical formula. It then works through examples of calculating the percent composition of magnesium and oxygen that form a compound, the percent composition and mass of carbon in propane, and determining empirical formulas from elemental percentages or mole ratios. The document explains how to calculate molecular formulas from empirical formulas and molar masses. Finally, it provides practice problems for the reader to work through.
This document discusses different types of chemical formulas used to represent compounds:
- A chemical compound is made of two or more elements that are combined in fixed ratios.
- The chemical formula uses symbols of the elements and subscripts to show the relative proportions.
- The empirical formula shows the lowest whole number ratio of atoms in a compound, while the molecular formula gives the exact number of each atom.
- The structural formula depicts the specific bonding arrangement of the atoms in a compound.
Stoichiometry is the study of quantitative relationships between amounts of substances involved in chemical reactions. It allows chemists to determine mole and particle quantities. The mole is the standard unit for measuring amounts of substances and refers to 6.022x1023 elementary entities. Molar mass is the mass of one mole of a substance and is calculated differently for elements versus compounds. Percent composition by mass can be determined by dividing the mass of each element by the total molar mass. Empirical and molecular formulas relate the simplest and actual ratios of elements in a compound.
This document discusses stoichiometry, which is the quantitative study of chemical reactions. It provides definitions of key terms used in stoichiometry such as mole, molar mass, and molar volume. Examples are given to demonstrate how to calculate the percent composition of compounds and determine empirical formulas from elemental analysis data. The three main stoichiometric laws - the law of conservation of mass, the law of definite proportions, and the law of multiple proportions - are also summarized. Overall, the document outlines fundamental concepts and principles of stoichiometry used in quantitative chemical calculations.
This document discusses stoichiometry, which is the quantitative study of chemical reactions. It provides definitions of key stoichiometric concepts such as mole, molar mass, and empirical formula. It also outlines three important stoichiometric laws: the law of conservation of mass proposed by Lavoisier, the law of definite proportions proposed by Proust, and the law of multiple proportions proposed by Dalton. These laws helped establish stoichiometry as a fundamental tool in chemistry. The document provides examples of stoichiometric calculations including determining empirical formulas and percent composition.
This document discusses chemical formulas and percent composition. It provides examples of calculating the percent composition of different compounds from their chemical formulas, such as NaCl, glucose, and Mg(OH)2. Empirical formulas can be determined from percent composition data by assuming 100 grams of the compound and calculating the moles of each element. Chemical equations are used to represent chemical reactions, and examples are given for writing and balancing equations. Common types of chemical reactions are also outlined.
Chemistry zimsec chapter 2 atoms, molecules and stoichiometryalproelearning
This document provides an overview of Chapter 2 in a chemistry textbook, which covers topics including:
- The mass of atoms and molecules, including relative atomic mass and molecular mass
- Using a mass spectrometer to determine relative isotopic masses and abundances
- The mole concept and amount of substance in relation to mass, volume of gases, and concentration of solutions
- Calculating empirical formulas from combustion data or elemental composition by mass and deducing molecular formulas
- Stoichiometry, including writing balanced chemical equations and ionic equations
The mole concept and chemical compounds.
Ethyl mercaptan, C2H6S, is added to natural gas to make gas leaks detectable.
The colorless, volatile liquid halothane has been used as a fire extinguisher and also as an inhalation anesthetic.
Dibutyl succinate is an insect repellent used against household ants and roaches.
This document discusses atomic mass and isotopes. It begins by explaining that an atomic mass unit (amu) is used to discuss the mass of atoms, where 1 amu is 1/12 the mass of a carbon-12 atom. Atomic masses listed in the periodic table are in amu. Isotopes have different atomic masses that result in the average atomic mass not being a whole number. Examples are provided to demonstrate calculating average atomic masses from the masses and abundances of isotopes.
New chm-151-unit-3-power-points-sp13-140227172226-phpapp01Cleophas Rwemera
This document provides an overview of stoichiometry concepts including:
- Balancing chemical equations by ensuring equal numbers of each type of atom on both sides of the equation.
- Determining empirical formulas, which show the simplest whole number ratio of elements in a compound, and molecular formulas, which show the actual numbers of atoms in a molecule of a compound.
- Relating the mole ratios in a balanced chemical equation to calculations involving amounts of reactants and products.
- Distinguishing between theoretical and actual yields in chemical reactions.
The document lists learning objectives and skills students should master related to these stoichiometry concepts and provides example problems demonstrating how to apply the concepts.
This document provides an overview of stoichiometry concepts covered in a George Mason University general chemistry course. It defines key terms like mole, molar mass, molecular weight, and formula weight. Examples are given for calculating the number of atoms or molecules in a given mass of a substance. The document also discusses mole-to-mole conversions in chemical equations, limiting reagents, and theoretical yield.
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 contains the table of contents for a chemistry textbook, outlining topics such as gases, liquids, atomic structure, chemical bonding, and organic chemistry. It provides an overview of the fundamental concepts covered in each chapter from introduction to chemistry through macromolecules and chemical formulas. The table of contents serves as a high-level outline of the essential information presented in the textbook.
This document provides an introduction to organic chemistry. It discusses the definition of organic compounds as those containing carbon, with some exceptions. It also covers nomenclature rules for naming organic compounds based on functional groups and carbon chain length. Additionally, it explains the concepts of isomerism, including structural, stereoisomers (geometric and optical), and hybridization of carbon orbitals. Hydrocarbons are introduced, specifically discussing alkanes as saturated hydrocarbons and their properties.
The document discusses chemical formulae and how they are used to represent elements and compounds. It provides examples of how to determine the empirical and molecular formula of substances based on experimental data like mass percentages and ratios of elements. Empirical formulae show the simplest whole number ratio of atoms in a compound, while molecular formulae show the actual number of each atom in a molecule of a substance. Percentage composition can also be calculated from the relative atomic masses and molecular formula.
The document provides information about chemical formulas and equations. It defines empirical and molecular formulas, and explains how to determine them through calculation of moles and mass ratios of elements in a compound. It also describes writing and balancing chemical equations, naming ionic compounds based on their constituent ions, and using formulas and equations to solve stoichiometric problems. Key topics covered include determining formulas from experimental data, relating formulas to molecular structure and mass, and representing chemical reactions systematically.
This document discusses concepts related to atomic masses and moles. It defines key terms like:
- Atomic mass unit (amu)
- Molar mass, which is the mass in grams of one mole of a compound
- Moles, which provide a way to count particles using Avogadro's number of 6.022x1023 particles per mole
- How to use atomic masses, molar masses, and moles to convert between masses and numbers of atoms/molecules in examples.
Stoichiometry is the quantitative study of chemical reactions and their mole-based ratios. It allows one to calculate amounts of substances involved in reactions based on molar masses, moles, and balanced chemical equations. Key concepts include empirical and molecular formulas, molarity, dilution calculations, spectrophotometry using Beer's Law, colorimetry, and determining limiting reactants.
Similar to Assignment: Empirical formula and typical question related mathematical problem. (20)
This document discusses ways to make polybags more sustainable. It proposes using biodegradable materials instead of traditional plastic to make bags. Other recommendations include reducing bag thickness, adding seeds to bags so they can grow plants when disposed, making bags from food waste, and using recycled materials and natural dyes. The conclusion emphasizes that while polythene is cheap and convenient, it is hazardous to the environment. A clean environment is necessary for health, so harmful materials like polythene should be replaced with natural elements to ensure sustainability.
Fundamental study on woven fabric Lab Report.Proshanto Saha
The document discusses the benefits of exercise for both physical and mental health. It notes that regular exercise can reduce the risk of diseases like heart disease and diabetes, improve mood, and reduce feelings of stress and anxiety. Exercise is also credited with boosting brain health and improving cognitive function as we age.
Assignment: Comparative Study on Various Types of Garment Production System.Proshanto Saha
Straight line system
Conventional Bundle System
Progressive Bundle System -Batch System
Unit Production System (UPS)
Modular Production System
Technology-enabled Manufacturing Systems
Apparel Production Process and Details
Department of Apparel Manufacturing & Technology
BGMEA University of Fashion & Technology
1. The document provides details about Fakir Fashion Limited, a vertically integrated knit composite factory in Bangladesh. It discusses the company's history, facilities, production processes, quality control measures, certifications and commitment to employees.
2. Key details include Fakir Fashion having over 6000 employees and producing 25 tons of knit fabric and 150,000 garments per day. It has facilities for knitting, dyeing, finishing, cutting, sewing, washing and quality inspection.
3. The company prioritizes sustainability, occupational health and safety. It has received several certifications and its annual sales have grown to over $130 million USD in 2020.
The simplified electron and muon model, Oscillating Spacetime: The Foundation...RitikBhardwaj56
Discover the Simplified Electron and Muon Model: A New Wave-Based Approach to Understanding Particles delves into a groundbreaking theory that presents electrons and muons as rotating soliton waves within oscillating spacetime. Geared towards students, researchers, and science buffs, this book breaks down complex ideas into simple explanations. It covers topics such as electron waves, temporal dynamics, and the implications of this model on particle physics. With clear illustrations and easy-to-follow explanations, readers will gain a new outlook on the universe's fundamental nature.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
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Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
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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.
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
Physiology and chemistry of skin and pigmentation, hairs, scalp, lips and nail, Cleansing cream, Lotions, Face powders, Face packs, Lipsticks, Bath products, soaps and baby product,
Preparation and standardization of the following : Tonic, Bleaches, Dentifrices and Mouth washes & Tooth Pastes, Cosmetics for Nails.
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Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
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RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
Assignment: Empirical formula and typical question related mathematical problem.
1. BGMEA University of Fashion & Technology
Department of Apparel Manufacturing & Technology
Course Code: CHEM-1101
Course Title: Chemistry
Assignment
Assignment Name: Empirical formula and typical
question related mathematical problem.
Submitted To: Submitted By:
Dr. Md. Mohibul Islam Khan Prosanto Saha
Assistant Professor ID: 201-120-101
BUFT Batch:201, AMT-3
2. 1. Benzoic acid is a white, crystalline powder used as a food
preservative. The compound contains 68.8% C, 5.0% H, and
26.2% O, by mass. What is its empirical formula?
Lat’s consider the total weeight of the gass composition is 100
The molar amount of, C=
.
= 5.7333
The molar amount of, H=
.
= 5.0
The molar amount of, O=
.
= 1.63
The molar ratio of, C=
.
.
= 3.501≅ 3.5
The molar ratio of, H=
.
= 3.053~3
The molar ratio of, O=
.
.
= 1
Thus, the empirical formula benzoic acid is C3.5H3O
= (C3.5H3O)2
=C7H6O2
3. 2. We found the percentage composition of acetic acid to be 39.9%
C, 6.7% H, and 53.4% O. Determine the empirical formula. The
molecular mass of acetic acid was determined by experiment to
be 60.0 amu. What is its molecular formula?
Given that,
Lat’s consider the total weeight of the gass composition is 100
The molar amount of, C=
.
= 3.32
The molar amount of, H=
.
= 6.7
The molar amount of, O=
.
= 3.33
The molar ratio of, C=
.
.
= 1
The molar ratio of, H=
.
.
= 2.02 ≅ 2
The molar ratio of, O=
.
.
= 1
The empirical formula of the composition is= 𝐶𝐻2O
The molecular mass of acetic acid is 60.0 amu
Since, the empirical formula is CH2O the molecular formula will be
(CH2O)n= CnH2nOn
The mass of empirical formula of the compound
stands=(12+1×2+16)=30 and molecular mass 60.
4. Therefore, n=
n= = 2
Thus, the molecular formula the compound is C2H4O2
3. The percentage composition of acetaldehyde is 54.5% C, 9.2% H,
and 36.3% O, and its molecular mass is 44 amu. Obtain the
molecular formula of acetaldehyde.
Lat’s consider the total weeight of the gass composition is 100
The molar amount of, C=
.
= 4.54
The molar amount of, H=
.
= 9.2
The molar amount of, O=
.
= 2.26
The molar ratio of, C=
.
.
= 2
The molar ratio of, H=
.
.
= 4
The molar ratio of, O=
.
.
= 1
The empirical formula of the composition is=C2H4O
The molecular mass of acetic acid is 44 amu
5. Since, the empirical formula is C2H4O the molecular formula will be
(C2H4O)n
The mass of empirical formula of the compound
stands=(12×2+1× 4 +16)=44 and molecular mass 44.
Therefore, n=
n= = 1
Thus, the molecular formula the compound is C2H4O
4. Oxalic acid is a toxic substance used by laundries to remove rust
stains. Its composition is 26.7% C, 2.2% H, and 71.1% O (by
mass), and its molecular mass is 90 amu. What is its molecular
formula?
Lat’s consider the total weeight of the gass composition is 100
The molar amount of, C=
.
= 2.225
The molar amount of, H=
.
= 2.2
The molar amount of, O=
.
= 4.44
6. The molar ratio of, C=
.
.
= 1
The molar ratio of, H=
.
.
= 1
The molar ratio of, O=
.
.
= 2
The empirical formula of the composition is= 𝐶𝐻O2
The molecular mass of the compound is 90 amu
Since, the empirical formula is CHO2 the molecular formula will be
(CHO2)n= CnH2nOn
The mass of empirical formula of the compound
stands=(12+1+16× 2)=45 and molecular mass 90.
Therefore, n=
n= = 2
Thus, the molecular formula the compound is C2H2O4
7. 5. Give examples of an element,a compound,a heterogeneous
mixture, and a homogeneous mixture.
Element: Element are the pure substances containing only one kind
of atoms.
Example: Iron is made of iron atoms so iron can be defined as
elements.
Compound: Any substance composed of identical molecules
consisting of atoms of two or more chemical elements can be called
compound.
Example: Water is a compound because it is made up of more than
one element-hydrogen and oxygen.
Example of Heterogeneous Mixture:
i. Concrete is heterogeneous mixture of an aggregate cement &
water.
ii. Ice cubes in cola from a heterogeneous mixture.
Example of Homogeneous Mixture:
Homogeneous mixture can be defined as solid mixture,liquid
mixture,gaseous mixture.
Such like: sugar water,sodas,bronze,blood plasma,dishwashwashing
detergents.
8. 6. What distinguishes an element from a compound? Can a
compound also be an element?
Elements are pure substances and they are composed of only one
type of atom and compounds are formed by two or more different
types of elements that are united chemically in fixed proprotions and
it is the main way to distinguish elements from compound.
A pure element cannot be a compound.
7. What is meant by the precision of a measurement? How is it
indicated?
The precision of a measurement system is refers to how close the
agreement is between to how close the agreements is between
repeated measurements which are repeated measurements which
are repeated under the same conditions.
One way to analyze the precision of the measurement would be to
determine the range or difference between the lowest and highest
measured values. In that case, the lowest value is 10.9 in and the
highest value is 11.2 in.
9. 8. Two rules are used to decide how to round the result of a
calculation to the correct number of significant figures. Use a
calculation to illustrate each rule.Explain how you obtained the
number of significant figures in the answers?
•Procedure to determine significant figures after multiplication or
division:
1. Multiply or divide the numbers using our calculator.
2. Round the result to have the same number of significant figures
as the measured value with the least number of significant figures.
• Below are two examples.
A) Write the product of 2.10 × 0.5896 with the correct number of
significant figures.
Step 1) 2.10 × 0.5896 = 1.23816
Step 2) 1.23816 = 1.24 (three sig. figs because 2.10 has three)
The answer is 1.24
B) Write the quotient of 16.15/2.7 with the correct number of
significant figures.
Step 1) 16.15 / 2.7 = 5.98148148
Step 2) 5.98148148 = 6.0 (two sig. figs because 2.7 has two)
The answer is 6.0
10. 9. Consider three masses that you wish to add together: 3 g,1.4 g,
and 3.3 g.These numbers represent measured values.Add the
numbers together and report your answer to the correct number
of significant figures?
The three given masses are 3.0g,1.4g, and 3.3g
Add the together and we get= (3.0+1.4+3.3)g
=7.7g
After adding the mass values the result value 7.7
Contain two significant numbers.
10. How many significant figures are there in each of the
following measurements?
a. 73.0000 g b. 0.0503 kg c. 6.300 cm d. 0.80090 m e. 2.010 s
a) 7.30000- significant figures -6
b) 0.0503- significant figures -3
c) 6.300- significant figures -4
d) 0.80090- significant figures -5
e) 2.010- significant figures -4