This document discusses aldehydes and ketones. It defines aldehydes as carbonyl compounds containing at least one hydrogen atom bonded to the carbonyl carbon, while ketones contain two carbon groups bonded to the carbonyl carbon. The document covers nomenclature rules for naming aldehydes and ketones based on IUPAC conventions, examples of common aldehydes and ketones, and different types of isomerism exhibited by these compound classes. Physical and chemical properties of aldehydes and ketones are also outlined.
[DOCUMENT] discusses inorganic chains, rings, cages, and clusters. It provides examples of:
- Silicate chains including different types of silicates based on their structure.
- Borazine and phosphazenes which are cyclic like benzene.
- Cages including white phosphorus, boranes, and carboranes.
- Polymeric sulfur nitride ((SN)x) which is a superconductor.
- Cluster valence electron theory and Wade's rule for classifying boranes and carboranes.
Aromatic compounds contain benzene rings and have delocalized pi bonds between carbon atoms in the ring. Common aromatic hydrocarbons include benzene, methylbenzene, and ethylbenzene which are liquids insoluble in water but soluble in non-polar solvents. Aromatic compounds have a wide range of uses including pharmaceuticals, herbicides, detergents, dyes, and acid-base indicators. Some aromatics like benzene are carcinogenic but not all are, such as aspirin.
This document describes a laboratory experiment on Cannizzaro's reaction of benzaldehyde. Benzaldehyde undergoes a solvent-free disproportionation reaction in the presence of sodium hydroxide to produce benzoic acid and benzyl alcohol. The reaction is carried out by grinding benzaldehyde and sodium hydroxide together for 30 minutes. Benzoic acid precipitates out and is collected by filtration. Benzyl alcohol is extracted from the filtrate using ethyl acetate. The yields of benzoic acid and benzyl alcohol are calculated and their melting points determined and compared to theoretical values.
Complexometric titrations involve the formation of a soluble, stoichiometric complex during the titration of a sample solution. EDTA titrations are commonly used for complexometric titrations. EDTA forms stable complexes with metal ions and produces a sharp color change at the equivalence point. The stability and selectivity of metal-EDTA complexes can be increased through factors like pH, ligand properties, and use of metallochromic indicators that form colored complexes with metal ions.
Atomic spectroscopy plays a major role as the basis of a wide range of analytical techniques that contribute data on elemental concentrations and isotope ratios .These analytical data provide the raw material on which progress in geochemistry depends.
The main advantages of AAS & AES are that it is relatively inexpensive and easy to use, while still offering high throughput, quantitative analysis of the metal content of solids or liquids. This makes it suitable for use in a wide range of applications.
This document summarizes key concepts in organometallic chemistry. It discusses the definition of organometallic compounds as those containing metal-carbon bonds. It outlines different types of ligands that can bind to metals, including carbonyl, carbene, and cyclic π systems. It also describes principles for understanding bonding interactions between ligands and metals, such as the 18-electron rule and molecular orbital theory. Spectroscopic techniques for analyzing organometallic compounds are also summarized.
This document discusses aldehydes and ketones. It defines aldehydes as carbonyl compounds containing at least one hydrogen atom bonded to the carbonyl carbon, while ketones contain two carbon groups bonded to the carbonyl carbon. The document covers nomenclature rules for naming aldehydes and ketones based on IUPAC conventions, examples of common aldehydes and ketones, and different types of isomerism exhibited by these compound classes. Physical and chemical properties of aldehydes and ketones are also outlined.
[DOCUMENT] discusses inorganic chains, rings, cages, and clusters. It provides examples of:
- Silicate chains including different types of silicates based on their structure.
- Borazine and phosphazenes which are cyclic like benzene.
- Cages including white phosphorus, boranes, and carboranes.
- Polymeric sulfur nitride ((SN)x) which is a superconductor.
- Cluster valence electron theory and Wade's rule for classifying boranes and carboranes.
Aromatic compounds contain benzene rings and have delocalized pi bonds between carbon atoms in the ring. Common aromatic hydrocarbons include benzene, methylbenzene, and ethylbenzene which are liquids insoluble in water but soluble in non-polar solvents. Aromatic compounds have a wide range of uses including pharmaceuticals, herbicides, detergents, dyes, and acid-base indicators. Some aromatics like benzene are carcinogenic but not all are, such as aspirin.
This document describes a laboratory experiment on Cannizzaro's reaction of benzaldehyde. Benzaldehyde undergoes a solvent-free disproportionation reaction in the presence of sodium hydroxide to produce benzoic acid and benzyl alcohol. The reaction is carried out by grinding benzaldehyde and sodium hydroxide together for 30 minutes. Benzoic acid precipitates out and is collected by filtration. Benzyl alcohol is extracted from the filtrate using ethyl acetate. The yields of benzoic acid and benzyl alcohol are calculated and their melting points determined and compared to theoretical values.
Complexometric titrations involve the formation of a soluble, stoichiometric complex during the titration of a sample solution. EDTA titrations are commonly used for complexometric titrations. EDTA forms stable complexes with metal ions and produces a sharp color change at the equivalence point. The stability and selectivity of metal-EDTA complexes can be increased through factors like pH, ligand properties, and use of metallochromic indicators that form colored complexes with metal ions.
Atomic spectroscopy plays a major role as the basis of a wide range of analytical techniques that contribute data on elemental concentrations and isotope ratios .These analytical data provide the raw material on which progress in geochemistry depends.
The main advantages of AAS & AES are that it is relatively inexpensive and easy to use, while still offering high throughput, quantitative analysis of the metal content of solids or liquids. This makes it suitable for use in a wide range of applications.
This document summarizes key concepts in organometallic chemistry. It discusses the definition of organometallic compounds as those containing metal-carbon bonds. It outlines different types of ligands that can bind to metals, including carbonyl, carbene, and cyclic π systems. It also describes principles for understanding bonding interactions between ligands and metals, such as the 18-electron rule and molecular orbital theory. Spectroscopic techniques for analyzing organometallic compounds are also summarized.
The document discusses various methods of classifying and naming organic compounds according to IUPAC rules. It outlines main types of classifications including aromatic vs aliphatic, saturated vs unsaturated, and classification based on functional groups. It then explains general rules for naming compounds including writing the parent name, naming substituents, and combining all parts of the name. Specific examples are provided for naming alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, carboxylic acids and their derivatives, amines, cycloalkanes and more. Naming of isomers and handling of multiple functional groups are also covered.
This document discusses organometallic chemistry and is presented by Dr. Manju Sebastian. It describes the classification of organometallic compounds based on the type of metal-carbon bond formed. The classifications include ionic compounds, compounds with sigma bonds, compounds with pi bonds, and compounds with multicenter bonds. Examples are provided for each classification. Additional topics covered include carbonyl complexes, ferrocene, applications of organometallics as catalysts including the Ziegler-Natta and Wilkinson catalysts.
Aldehydes and ketones are the carbonyl compounds with general formula CnH2nO. Aldehydes have at least one hydrogen atom bonded to the carbonyl group and other group is either hydrogen or an alkyl or aryl group (i.e. Aldehyde has one alkyl or aryl group and one of the hydrogen bonded to the carbonyl carbon) with characteristics functional group -CHO.
In organic chemistry, a carbonyl group is a functional group composed of a carbon atom double-bonded to an oxygen atom: C=O. It is common to several classes of organic compounds, as part of many larger functional groups. A compound containing a carbonyl group is often referred to as a carbonyl compound.
This document discusses gravimetric analysis, which is a quantitative chemical analysis method to determine the amount of a substance by directly measuring its mass. It involves converting the substance into a pure chemical compound, then weighing it. There are several techniques used for this conversion, such as precipitation, volatilization by ignition, and electrogravimetry. Gravimetric analysis is accurate, precise, and involves direct measurement of the substance. The key steps involve isolating and weighing the pure compound, which is typically done through precipitation, filtration, washing, drying, and weighing.
The document discusses carbonyl compounds, which contain a carbonyl group (C=O). This includes aldehydes, ketones, carboxylic acids, amides, and acid chlorides. It describes the structure of the carbonyl group and how the C=O double bond is polarized towards oxygen. This polarization allows carbonyl compounds to undergo nucleophilic addition reactions. Aldehydes are generally more reactive than ketones for electronic and steric reasons. Examples of reactions include hydration, cyanohydrin formation, imine formation, acetal formation, oxidation, reduction, and Friedel-Crafts acylation. Qualitative tests and important carbonyl compounds and their uses are also outlined.
Coulometry is an electroanalytical technique where the amount of electricity (in coulombs) required to complete an electrochemical reaction is measured. There are two main types - potentiostatic coulometry, where the potential is held constant, and coulometric titration with a constant current. The quantity of electricity is directly proportional to the amount of analyte and can be used to determine concentrations. Coulometry has applications in inorganic analysis, analysis of radioactive materials, microanalysis, and determination of organic compounds.
The document provides information about aliphatic hydrocarbons, specifically alkanes. It begins with learning outcomes which state that students will understand organic compound families, explain alkane structure and properties, name organic compounds using IUPAC rules, describe alkane isomers and synthesis reactions. The document then covers classes of organic compounds including hydrocarbons, alkane properties such as physical states and solubility, IUPAC nomenclature rules, cyclic alkane naming, and alkane reaction and synthesis methods like hydrogenation of alkenes.
This chapter discusses alcohols, which are organic compounds containing a hydroxyl (-OH) functional group. It covers the IUPAC nomenclature rules for naming alcohols, including cyclic alcohols, alcohols containing multiple functional groups, diols, and phenols. The chapter also discusses the classification, physical properties, acidity, and preparation of alcohols. Alcohols can be prepared through Grignard synthesis or hydrolysis of alkyl halides. Common alcohols include ethanol, used in alcoholic beverages, and methanol, an important industrial solvent.
Lecture 06; atomization by Dr. Salma Amirsalmaamir2
This document discusses different techniques for atomizing samples in atomic spectroscopy, including flame atomization and electrothermal atomization. Flame atomization involves aspirating a sample solution into a flame where it is converted to a fine mist and heated to evaporate, volatilize, and atomize the analyte. Electrothermal atomization uses a graphite furnace to precisely heat samples through drying, pyrolysis, and atomization steps. Key factors that influence the atomization process, such as droplet size, flame temperature, and chemical properties of the analyte, are also outlined.
The document discusses the IUPAC system of nomenclature for naming organic compounds. It explains the key concepts of word roots, prefixes, suffixes, functional groups and rules for naming compounds. The longest carbon chain is identified and numbered from the end closest to the first branch or substituent. Functional groups and multiple bonds are given priority in numbering over substituents.
Gravimetric analysis is a quantitative analytical technique used to determine the purity of a sample by measuring its mass. It involves selectively converting the analyte into an insoluble precipitate, filtering to separate the precipitate, drying, igniting, and weighing the precipitate. Key steps include precipitation, digestion or ripening to form larger crystals, filtration, washing to remove impurities, drying and igniting the precipitate, and final weighing and calculations. Accuracy depends on quantitative precipitation and removal of impurities through careful control of parameters like pH, temperature, supersaturation levels, and multiple washings.
The document provides information about electroanalytical methods of analysis. It defines electroanalytical methods as techniques that study analytes by measuring potentials or currents in an electrochemical cell containing the analyte. It discusses various types of electroanalytical techniques including potentiometry, voltammetry, and Karl Fischer titration. It provides details on the principles, instrumentation, applications, and advantages of these analytical methods.
1. The chapter introduces organic chemistry and the different functional groups that classify organic compounds.
2. It describes IUPAC nomenclature rules for systematically naming organic structures and explains how to identify substituents.
3. The chapter covers different types of isomerism including structural, stereoisomers, and optical isomers that can exist.
This document discusses ionic liquids and their advantages over conventional organic solvents. Ionic liquids are salts that are liquid at ambient temperatures, have a stable liquid range over 300K, and very low vapor pressure. They have selective solubility of water and organics. Ionic liquids can replace volatile organic solvents used in industrial processes. Common cations include 1-alkyl-3-methylimidazolium and common anions include [PF6]-, [BF4]-, and [AlCl4]-. Ionic liquids offer advantages like easy separation, low volatility, non-flammability, high thermal and chemical stability, low toxicity, and non-volatility. They have applications as solvents in Frie
Alkynes are unsaturated hydrocarbons containing a carbon-carbon triple bond. They are more unsaturated than alkenes. Alkynes undergo characteristic reactions including addition reactions, oxidation, hydration, and polymerization. They can be prepared through methods such as the dehydrogenation of tetrahalides, dehydrohalogenation of vicinal dihalides, and the reaction of sodium acetylides with primary alkyl halides.
The factors that affect the stability of complexes Ernest Opoku
The stability of metal complexes is affected by various ligand and metal factors. Ligand factors that increase stability include small size, high charge, chelation which forms multiple bonds to the metal, and high basicity. Steric effects from bulky ligands decrease stability. For the metal, higher charge and smaller size increase stability, as do behaviors defined by the Ahrland-Chatt classification like class A metals forming more stable complexes with lighter donor atoms. The Irving-Williams series and crystal field theory show transition metal complex stability follows trends based on ionic radius, crystal field splitting, and effects like Jahn-Teller distortion.
Qualitative analysis is used to identify the cations and anions present in an unknown chemical substance. Cations such as sodium, calcium, and ammonium can be identified using sodium hydroxide and ammonia solutions. Anions like chloride, nitrate, and sulfate can be identified through chemical tests involving silver nitrate, sodium hydroxide with aluminum foil, and barium chloride solutions respectively. These tests produce characteristic precipitates or gas emissions to reveal the ions present. Dilute nitric acid is first added to remove any interfering carbonate ions.
The document discusses various methods of classifying and naming organic compounds according to IUPAC rules. It outlines main types of classifications including aromatic vs aliphatic, saturated vs unsaturated, and classification based on functional groups. It then explains general rules for naming compounds including writing the parent name, naming substituents, and combining all parts of the name. Specific examples are provided for naming alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, carboxylic acids and their derivatives, amines, cycloalkanes and more. Naming of isomers and handling of multiple functional groups are also covered.
This document discusses organometallic chemistry and is presented by Dr. Manju Sebastian. It describes the classification of organometallic compounds based on the type of metal-carbon bond formed. The classifications include ionic compounds, compounds with sigma bonds, compounds with pi bonds, and compounds with multicenter bonds. Examples are provided for each classification. Additional topics covered include carbonyl complexes, ferrocene, applications of organometallics as catalysts including the Ziegler-Natta and Wilkinson catalysts.
Aldehydes and ketones are the carbonyl compounds with general formula CnH2nO. Aldehydes have at least one hydrogen atom bonded to the carbonyl group and other group is either hydrogen or an alkyl or aryl group (i.e. Aldehyde has one alkyl or aryl group and one of the hydrogen bonded to the carbonyl carbon) with characteristics functional group -CHO.
In organic chemistry, a carbonyl group is a functional group composed of a carbon atom double-bonded to an oxygen atom: C=O. It is common to several classes of organic compounds, as part of many larger functional groups. A compound containing a carbonyl group is often referred to as a carbonyl compound.
This document discusses gravimetric analysis, which is a quantitative chemical analysis method to determine the amount of a substance by directly measuring its mass. It involves converting the substance into a pure chemical compound, then weighing it. There are several techniques used for this conversion, such as precipitation, volatilization by ignition, and electrogravimetry. Gravimetric analysis is accurate, precise, and involves direct measurement of the substance. The key steps involve isolating and weighing the pure compound, which is typically done through precipitation, filtration, washing, drying, and weighing.
The document discusses carbonyl compounds, which contain a carbonyl group (C=O). This includes aldehydes, ketones, carboxylic acids, amides, and acid chlorides. It describes the structure of the carbonyl group and how the C=O double bond is polarized towards oxygen. This polarization allows carbonyl compounds to undergo nucleophilic addition reactions. Aldehydes are generally more reactive than ketones for electronic and steric reasons. Examples of reactions include hydration, cyanohydrin formation, imine formation, acetal formation, oxidation, reduction, and Friedel-Crafts acylation. Qualitative tests and important carbonyl compounds and their uses are also outlined.
Coulometry is an electroanalytical technique where the amount of electricity (in coulombs) required to complete an electrochemical reaction is measured. There are two main types - potentiostatic coulometry, where the potential is held constant, and coulometric titration with a constant current. The quantity of electricity is directly proportional to the amount of analyte and can be used to determine concentrations. Coulometry has applications in inorganic analysis, analysis of radioactive materials, microanalysis, and determination of organic compounds.
The document provides information about aliphatic hydrocarbons, specifically alkanes. It begins with learning outcomes which state that students will understand organic compound families, explain alkane structure and properties, name organic compounds using IUPAC rules, describe alkane isomers and synthesis reactions. The document then covers classes of organic compounds including hydrocarbons, alkane properties such as physical states and solubility, IUPAC nomenclature rules, cyclic alkane naming, and alkane reaction and synthesis methods like hydrogenation of alkenes.
This chapter discusses alcohols, which are organic compounds containing a hydroxyl (-OH) functional group. It covers the IUPAC nomenclature rules for naming alcohols, including cyclic alcohols, alcohols containing multiple functional groups, diols, and phenols. The chapter also discusses the classification, physical properties, acidity, and preparation of alcohols. Alcohols can be prepared through Grignard synthesis or hydrolysis of alkyl halides. Common alcohols include ethanol, used in alcoholic beverages, and methanol, an important industrial solvent.
Lecture 06; atomization by Dr. Salma Amirsalmaamir2
This document discusses different techniques for atomizing samples in atomic spectroscopy, including flame atomization and electrothermal atomization. Flame atomization involves aspirating a sample solution into a flame where it is converted to a fine mist and heated to evaporate, volatilize, and atomize the analyte. Electrothermal atomization uses a graphite furnace to precisely heat samples through drying, pyrolysis, and atomization steps. Key factors that influence the atomization process, such as droplet size, flame temperature, and chemical properties of the analyte, are also outlined.
The document discusses the IUPAC system of nomenclature for naming organic compounds. It explains the key concepts of word roots, prefixes, suffixes, functional groups and rules for naming compounds. The longest carbon chain is identified and numbered from the end closest to the first branch or substituent. Functional groups and multiple bonds are given priority in numbering over substituents.
Gravimetric analysis is a quantitative analytical technique used to determine the purity of a sample by measuring its mass. It involves selectively converting the analyte into an insoluble precipitate, filtering to separate the precipitate, drying, igniting, and weighing the precipitate. Key steps include precipitation, digestion or ripening to form larger crystals, filtration, washing to remove impurities, drying and igniting the precipitate, and final weighing and calculations. Accuracy depends on quantitative precipitation and removal of impurities through careful control of parameters like pH, temperature, supersaturation levels, and multiple washings.
The document provides information about electroanalytical methods of analysis. It defines electroanalytical methods as techniques that study analytes by measuring potentials or currents in an electrochemical cell containing the analyte. It discusses various types of electroanalytical techniques including potentiometry, voltammetry, and Karl Fischer titration. It provides details on the principles, instrumentation, applications, and advantages of these analytical methods.
1. The chapter introduces organic chemistry and the different functional groups that classify organic compounds.
2. It describes IUPAC nomenclature rules for systematically naming organic structures and explains how to identify substituents.
3. The chapter covers different types of isomerism including structural, stereoisomers, and optical isomers that can exist.
This document discusses ionic liquids and their advantages over conventional organic solvents. Ionic liquids are salts that are liquid at ambient temperatures, have a stable liquid range over 300K, and very low vapor pressure. They have selective solubility of water and organics. Ionic liquids can replace volatile organic solvents used in industrial processes. Common cations include 1-alkyl-3-methylimidazolium and common anions include [PF6]-, [BF4]-, and [AlCl4]-. Ionic liquids offer advantages like easy separation, low volatility, non-flammability, high thermal and chemical stability, low toxicity, and non-volatility. They have applications as solvents in Frie
Alkynes are unsaturated hydrocarbons containing a carbon-carbon triple bond. They are more unsaturated than alkenes. Alkynes undergo characteristic reactions including addition reactions, oxidation, hydration, and polymerization. They can be prepared through methods such as the dehydrogenation of tetrahalides, dehydrohalogenation of vicinal dihalides, and the reaction of sodium acetylides with primary alkyl halides.
The factors that affect the stability of complexes Ernest Opoku
The stability of metal complexes is affected by various ligand and metal factors. Ligand factors that increase stability include small size, high charge, chelation which forms multiple bonds to the metal, and high basicity. Steric effects from bulky ligands decrease stability. For the metal, higher charge and smaller size increase stability, as do behaviors defined by the Ahrland-Chatt classification like class A metals forming more stable complexes with lighter donor atoms. The Irving-Williams series and crystal field theory show transition metal complex stability follows trends based on ionic radius, crystal field splitting, and effects like Jahn-Teller distortion.
Qualitative analysis is used to identify the cations and anions present in an unknown chemical substance. Cations such as sodium, calcium, and ammonium can be identified using sodium hydroxide and ammonia solutions. Anions like chloride, nitrate, and sulfate can be identified through chemical tests involving silver nitrate, sodium hydroxide with aluminum foil, and barium chloride solutions respectively. These tests produce characteristic precipitates or gas emissions to reveal the ions present. Dilute nitric acid is first added to remove any interfering carbonate ions.
Qualitative analysis of salts involves conducting a series of tests on an unknown chemical substance to identify the cation and anion present. Common tests include observing the color of the salt, its solubility in water, the effect of heating, and flame tests to determine ions like sodium or calcium. Additional confirmatory tests help identify the specific cation and anion through observing reactions with gases or changes from heating different salt types.
The document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes the general characteristics, properties, reactions and tests to identify these anions. Carbonates and bicarbonates are identified through reactions with acids that produce carbon dioxide gas. Sulfur-containing anions like sulfides, sulfites and thiosulfates can be identified through reactions that produce hydrogen sulfide gas, sulfur dioxide gas or sulfur precipitates.
CVB222 UV-vis Absorption and Fluorescence LectureMark Selby
- The document discusses absorption and fluorescence spectroscopy techniques. It covers fundamental concepts like Beer's law, deviations from Beer's law, instrumentation for absorption and fluorescence measurements, and applications like drug and pollutant analysis.
- Key concepts covered include energy level diagrams to explain fluorescence and phosphorescence, factors that influence fluorescence intensity, and examples of fluorescent molecules and how their structure impacts fluorescence properties.
- Applications discussed are determination of carcinogenic polyaromatic hydrocarbons like benzo(a)pyrene and fluorimetric analysis of drugs like quinine and LSD.
The document summarizes various chemical tests that can be used to identify different ions in solution. It provides tables showing the observed colour changes or precipitates formed when aqueous solutions of different ions are treated with sodium hydroxide solution, aqueous ammonia solution, or other reagents like silver nitrate, barium chloride and concentrated sulfuric acid. The tables also indicate what ion can be inferred from each observation and provide additional comments and explanations for some reactions.
The document discusses qualitative analytical chemistry techniques for separating and identifying cations and anions in aqueous solutions. It provides examples of separation schemes based on differences in solubility rules of metal hydroxides and oxides. Confirmatory tests are described to verify the presence of specific cations like Fe3+, Al3+, Pb2+, and Ni2+ after separation. The document also discusses approaches for distinguishing between common anions using chemical reactions.
Gravimetric analysis is a quantitative analytical technique where the concentration of an analyte is determined by precipitating it from solution, isolating the precipitate, and weighing it. Some key aspects of gravimetric analysis are that the precipitate must be insoluble, of known composition, and pure to minimize errors from impurities. Conditions like precipitation temperature, reagent concentrations, and digestion can be adjusted to increase particle size and purity for accurate weighing and analysis.
The document describes tests to identify common halide ions and other anions. Chloride, bromide, and iodide ions were tested with silver nitrate and ammonia to observe solubility. Sulphite ions were detected by the production of sulfur dioxide gas detected by dichromate paper. Carbonate and hydrogen carbonate ions were detected through gas production and barium chloride precipitate formation with hydrochloric acid. Nitrate ions were identified by the production of ammonia gas on addition of aluminum and sodium hydroxide.
This document provides instructions for identifying cations through qualitative analysis using sodium hydroxide (NaOH) and ammonium hydroxide (NH3) solutions. Precipitates formed when salts are reacted with these reagents can indicate the present metal ions. Observations of solubility in excess reagent and reactions with other substances like hydrochloric acid help distinguish between ions. Proper technique like warming solutions gently and testing gas evolution with litmus paper is emphasized.
Carbon exists in several allotropes with unique properties. Graphite has layered structures that allow for easy sliding of layers and is used as lubricant. Diamond has a tetrahedral structure and is the hardest material. Fullerenes like buckminsterfullerene have soccer ball geometries. Carbon also forms many inorganic compounds including carbon monoxide, carbon dioxide, carbonates, bicarbonates, carbides and cyanides with various applications.
The document summarizes common cation and anion analysis methods using precipitation reactions. Group I cations like lead Pb2+ form white precipitates with hydrochloric acid. Group II cations like copper Cu2+ form colored precipitates - copper forms light green with sodium hydroxide and ammonia. Common anion tests involve adding reagents to induce color changes - nitrates form a brown gas with concentrated sulfuric acid and heat, while chlorides form a white precipitate with silver nitrate.
Qualitative analysis of group 4 cationsJessa Arino
The Group IV cations are Ba2+, Sr2+, Ca2+.
These metals form chlorides, sulfides and hydroxides that are soluble under that prevail in the precipitations of Group I, II, and III.
This document lists various anions and their identifying chemical properties. It groups the anions based on which precipitation agent can be used to identify them. For each anion, the symbol, identifying reagent, and expected color change or precipitate are provided. This allows for the identification of anions based on their reactions with specific reagents.
Quantitive Time Series Analysis of Malware and Vulnerability Trendsamiable_indian
The document presents the results of a quantitative time series analysis of malware and vulnerability trend data. Three datasets were analyzed: reported monthly virus incidents, incidents attributed to the most prevalent malware, and a dataset of malware reported "in the wild". ARIMA models were fitted to each dataset and found to accurately model and forecast short-term trends. The analysis found that threats are increasing in a non-linear manner and individual malware variants are having a greater impact over time.
The document discusses different types of titrations including acid-base, oxidation-reduction, complex formation, and precipitation reactions. It defines key terms like indicator, equivalence point, and endpoint. Examples are provided for calculating concentration using titration data from reactions like acid-base titrations for chloride in urine and carbon monoxide determination. Steps are outlined for the Kjeldahl method to determine nitrogen content through acid digestion and titration.
Quantitative Analysis (Language and Literature Assessment)Joy Labrador
Share the documents you have :) Learning Assessment this covers all the following:
-Criteria of A Good Test
-Validity
-Sub-classification of Validity
-Reliability
-Factors affecting Reliability
- Correlations
ENJOY READING!!!
Nellie Deutsch will be discussing Qualitative and Quantitative Analysis for Action Research in today's webinar July 30, 2015 at 12 PM EST on WizIQ: http://www.wiziq.com/online-class/2866384-ar-qualitative-and-quantitative-data-analysis Recordings will be available to those who join the class.
This document provides information on naming ionic and covalent compounds. It discusses how to name ionic compounds based on their cation and anion. It also discusses naming transition metal ions based on their charge. For covalent compounds, it describes naming binary molecular compounds and compounds containing hydrogen or carbon. It provides examples of naming ionic compounds, transition metal compounds, and molecular compounds systematically. It also discusses writing chemical formulas, identifying common polyatomic ions, and recognizing ionic versus covalent character.
Lecture 9.3 through 9.5- Naming molecules & acidsMary Beth Smith
The document discusses naming binary molecular compounds and acids and bases. It provides guidelines for naming compounds based on their formulas or vice versa. The key points are:
- Binary molecular compounds are named with prefixes to indicate the number of atoms and the suffix "-ide" for the second element.
- Acids are named after their anions and have formulas starting with hydrogen and ending with the anion formula. Their names indicate the anion stem.
- Bases are named by the cation name followed by the hydroxide anion name and have the hydroxide formula.
- The laws of definite and multiple proportions describe the consistent element ratios in compounds.
This document provides information on naming and writing formulas for different types of chemical compounds including:
1. Ionic compounds consisting of monatomic and polyatomic ions are named by writing the cation first followed by the anion. Transition metal ions have stock and classical naming systems.
2. Molecular compounds consisting of two nonmetals are named using prefixes to indicate the number of atoms of each element followed by the "-ide" suffix.
3. Acids are named based on the anion present, using prefixes like "hydro-", "-ous", or "-ic" depending on the anion suffix. Their formulas are written with hydrogen and the anion.
4. Bases are named by writing the cation
This document discusses stoichiometry, which includes naming chemical compounds and writing balanced chemical equations. It begins by explaining the systematic naming of elements based on their symbols. Rules are provided for naming binary compounds of nonmetals, compounds of metals and nonmetals, compounds of metal ions and polyatomic ions, and naming oxides, acids, and bases. Balanced chemical equations are described as representing chemical changes where reactants on the left produce products on the right while obeying the law of conservation of mass. Examples of several types of chemical names and balanced equations are also provided.
This document provides information on naming and writing formulas for different types of compounds:
- Binary molecular compounds contain two nonmetal elements joined by a covalent bond. Prefixes are used to name them and indicate the number of atoms in the formula.
- Binary acids contain hydrogen and one nonmetal element. They follow a consistent naming pattern of "hydro-" plus the nonmetal root plus "-ic acid".
- Ternary acids contain hydrogen and a polyatomic ion. Their names indicate whether the polyatomic ion ends in "-ate", "-ite" or another suffix. Formulas are written by balancing hydrogen's +1 charge with the charges of the other elements/ions.
This document provides information about chemical compounds and their nomenclature. It defines a chemical compound as a pure substance formed by two or more elements combined in fixed proportions. Examples of common compounds and their chemical formulas are provided. The document then discusses different systems for naming compounds, including classical nomenclature, nomenclature using Roman numerals to indicate elemental valence, and nomenclature using Greek prefixes to indicate the number of atoms present. Specific rules and examples are provided for naming oxides, hydroxides, and peroxides. A series of exercises are included to have the reader practice writing formulas and names according to the various nomenclature systems.
Chemistry is the science and study of matter, including its properties, composition as well as reactivity. Chemistry relates to everything that can be sensed from the minute elements to complex structures. The atom and molecules are the basic unit or components of Chemistry.
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 6
Common and Systematic Names
• Chemical nomenclature is the systematic naming of chemical compounds
• Common names are historical names of compounds which are not based
on systematic rules
• Common names are often used because systematic names are too long
and technical for everyday use
• Chemists prefer systematic names that precisely identify the chemical
composition of compounds.
• Example CaO
• Common name: lime
• Systematic name: calcium oxide
Naming
Flowchart
We will focus on nomenclature of inorganic compounds
Elements and Ions
• The formula for most elements is the symbol of the element off of
the periodic table.
• Diatomic molecules are an exception:
• Two other elements also exist in polyatomic arrangements:
Naming Anions
•Remember from Chapter 5
that any neutral atom that
gains an electron is called
an anion
•When naming anions,
change the element ending
to -ide
Symbols
of the
Elements
•Each element has an
abbreviation called a symbol.
•The first letter of a symbol
must always be capitalized.
•If a second letter is needed, it
should be lowercase.
Predicting Ion
Charge from
Periodic Table
•Metals form cations
•The positive charge is equal
to the group number
Predicting Ion
Charge from
Periodic Table
•Nonmetals form anions
•The negative charge is equal
to 8 – the group number
Writing Formulas from Names of Ionic Compounds
•Ionic compounds contain both a cation and
an anion.
•Ionic compounds must have a net charge of
0
•The sum of charges of the cations and
anions in an ionic compound equal 0
•Rules for writing formulas for ionic
compounds:
• Write the metal ion followed by the
nonmetal ion formula
• Combine the smallest whole numbers
of each ion to provide an overall
charge equal to zero
• Write the compound formula for the
metal and nonmetal, using subscripts
determined from Step 2 for each ion
Naming Ionic
Binary
Compounds
•Binary compounds containing
a metal which forms only one
cation
•By convention, the cation is
written/named first followed
by the anion
•Rules for naming binary ionic
compounds:
• Name the cation
• Write the anion root and
add the –ide suffix
Naming
Compounds
Containing
Metals with
Multiple
Charges
•Rules for Naming Compounds Involving Metals that Could Form
Multiple Charges
• Write the cation name.
• Write the cation charge in Roman numerals in parentheses.
• Write the root of the anion and use the –ide suffix.
•Exception: for metals that only form two cations, a Latin root with
either an –ous or –ic suffix can also be used.
Formula Name Classical Name Formula Name Classical Name
Cu+ Copper(I) cuprous Sn2+ Tin(II) stannous
Cu2+ Copper(II) cupric Sn4+ Tin(IV) stannic
Fe2+ Iron(II) ferrous Pb2+ Lead(II) plumbous
Fe3+ Iron(III) ferric Pb4+ Lead(IV) plumbic
Naming Molecular
Compounds
•Molecular compounds contain two nonmetals
•Rules for ...
Chemical nomenclature is the system used to name chemical compounds. It allows chemists to communicate effectively. The name of a compound provides information about its structure. There are currently 114 known elements, some of which are gases while most are solids. In the early 1800s, Berzelius established the modern system of using the first letter of the element's name as its symbol. Chemical formulas represent the elements in a compound along with subscript numbers indicating mole ratios. Empirical formulas provide the simplest whole number ratio of atoms in a compound, while molecular formulas give the exact number of atoms in a molecule.
The document provides information about atoms, molecules, and ions. It discusses:
- Atomic number and mass number
- Isotopes and examples of isotopes of hydrogen
- Molecular and empirical formulas
- Ionic compounds and how their formulas are determined
- Naming common compounds and ions
- Acids, bases, and naming acid anions and hydrate compounds
Chemistry is involved with various and diverse interactions of matter either around us or simply inside the laboratory. These are described using the language of chemistry which consists of symbols, formulas and equations.
This document provides an overview of inorganic chemical nomenclature. It discusses the naming of elements, ions, binary compounds including hydrides, oxides, peroxides, halides, hydroxides, oxoacids and oxosalts. Different naming systems are covered, including compositional, stoichiometric, oxidation number, traditional and IUPAC nomenclature. Key concepts covered include oxidation numbers, types of ions, writing formulas for binary compounds, and distinguishing features of different compound classes.
The document provides information on naming ionic compounds, cations, anions, and polyatomic ions. It discusses how to name monatomic and transition metal cations by adding "-ion" or the charge in Roman numerals after the element name. Anions are named by adding "-ide" after the element root. Ionic compounds are formed by writing the cation first followed by the anion. Polyatomic ions are also included.
This document discusses nomenclature rules for binary compounds, binary bases and acids, and oxoacids. It explains that binary compounds contain two elements, binary bases contain OH- or have hydroxide in their name, and binary acids form when a hydrogen atom bonds to another element and dissolves in water. Rules are provided for naming binary acids based on the elements present. Oxoacids contain oxygen, hydrogen, and another element, and have suffixes that indicate the number of oxygen atoms such as -ous, -ic, and -ic. Examples are given for common oxoacid ions and their names.
1. The document provides rules for systematically naming coordination compounds, including naming cations, anions, ligands and indicating metal oxidation states.
2. It discusses different types of isomerism that can occur in coordination compounds, including coordination isomers, linkage isomers, geometric isomers and optical isomers.
3. Geometric isomers occur when ligands can be arranged on the same or opposite sides of the central metal ion, such as cis and trans isomers of octahedral complexes.
This document provides information about a module on chemical nomenclature. It begins with an introduction that names are used to identify and distinguish between people and compounds. It then outlines the lessons contained in the module, which are on chemical symbols, formulas, empirical formulas, molecular formulas, and nomenclature. The document concludes by explaining how students should approach learning from the module, including taking pre- and post-tests.
Applied Chapter 5.3 : Names and Formulas of CompoundsChris Foltz
This document discusses naming and writing formulas for ionic compounds and compounds containing polyatomic ions. It explains that ionic compounds are made up of positive and negative ions in the simplest ratio to achieve neutral charge. Formulas show the types and numbers of ions present. Names specify the cation first followed by the anion. Polyatomic ions are named and treated as a single unit. Examples are provided to illustrate naming and writing formulas for various ionic compounds and those containing common polyatomic ions.
Chapter 7.1 : Chemical Names and FormulasChris Foltz
Chemical formulas indicate the relative number and type of atoms in a chemical compound or molecule. A chemical formula for an ionic compound represents one formula unit and uses the simplest whole number ratio of ions present. Binary ionic compounds are composed of two elements and the total positive charges must equal the total negative charges. Molecular compounds use a prefix system to indicate the number of atoms of the less electronegative element present. Polyatomic ions are named as units within chemical formulas.
This document discusses chemical concepts related to combustion analysis, oxidation states, assigning oxidation states, naming inorganic compounds, binary compounds, polyatomic ions, and oxoacids. It provides examples and rules for determining oxidation states, naming inorganic compounds based on their formulas, and identifying common polyatomic ions and their names. Key points include that combustion analysis can be used to analyze chemical substances, oxidation states are related to electrons gained or lost by atoms, and there are systematic rules for naming inorganic compounds and identifying polyatomic ions based on their structures and formulas.
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Reimagining Your Library Space: How to Increase the Vibes in Your Library No ...Diana Rendina
Librarians are leading the way in creating future-ready citizens – now we need to update our spaces to match. In this session, attendees will get inspiration for transforming their library spaces. You’ll learn how to survey students and patrons, create a focus group, and use design thinking to brainstorm ideas for your space. We’ll discuss budget friendly ways to change your space as well as how to find funding. No matter where you’re at, you’ll find ideas for reimagining your space in this session.
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
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.
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.
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.
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Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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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.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
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Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
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Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
2. Increasing chemical literacy
Developing skills and knowledge that are relevant to
chemical industry and research.
Achieving this:
Practical skills through the laboratory program
Developing chemical concepts (mental models) through
simulations --- a work in progress
Alignment of fundamental principles taught in lectures
with practical work in the laboratory (where possible)
Objectives
3. Literacy, in its most common usage, is defined as the ability to
read and write. These are basic skills and the absence of one or
both is considered to be a handicap in an industrialized society.
Chemical Literacy
4. See information on pages 12 – 17 of the Practical Manual and the
notes under the heading “Review” in these PowerPoint slides.
Handwritten reports are acceptable and will not result in any
reduction in grades.
Over the course of the semester in this unit you should be
developing your skills in writing reports that will meet a standard
acceptable to industry or research.
Improvement in writing reports is to be judged by the structuring of
the report, the standard of written communication, quality of
recorded observations and discussion of results, and the use of
chemical equations.
The mechanics of writing your report (i.e., handwritten versus word-
processing) is of secondary importance (but word processing may be
expected in Industry or research).
Writing chemical equations
5. Tools for writing reports
The nuts and bolts of word processing for chemistry
6. The RSC font:
The Royal Society of Chemistry
font is a specialist chemistry font
that may be downloaded free and
used on PCs and Macs. This font
allows chemical symbols to be
introduced easily into Word
documents.
http://www.rsc.org/Education/Teachers/Re
sources/Font.asp
Fonts for Chemistry
Chem97 Font:
ChemFont97 is a Windows font package that simplifies the entry of chemical equations
and notation. The font includes all upper and lower case Greek characters, superscripts,
subscripts, many chemistry-specific symbols like reaction arrows. ChemFont97 comes in
two styles: serif, which is like Times New Roman, and sans-serif, which is like Arial.
8. Wolfram Alpha
Wolfram Alpha solves
chemical equations and
provides comprehensive
chemical data.
Apps for Android and
iPad.
Handy for Mol. Wt.
9. Collaborate but don’t plagiarise. Make sure you understand
the difference!
See for instance:
http://www4.caes.hku.hk/writing_turbocharger/collaborating/
default_answers.htm
Collaborate but don’t Plagiarise
10. 1. Single atom anions are named with an -ide suffix: for
example, F− is fluoride.
2. Compounds with a positive ion (cation), the name of the
compound is simply the cation's name, followed by the
anion. For example, CaF2 is calcium fluoride.
3. Cations able to take on more than one positive charge
are labeled with Roman numerals in parentheses. For
example, Cu+ is copper(I), Cu2+ is copper(II).
An older, out-dated notation is to append -ous or -ic to the
root of the Latin name to name ions with a lesser or greater
charge. Under this naming convention, Cu+ is cuprous and
Cu2+ is cupric.
IUPAC nomenclature
12. 4. Oxyanions (polyatomic anions containing oxygen) are named with -ite
or -ate, for a lesser or greater quantity of oxygen. For example, NO2
− is
nitrite, while NO3
− is nitrate. If four oxyanions are possible, the
prefixes hypo- and per- are used: hypochlorite is ClO−, perchlorate is
ClO4
−.
5. The prefix bi- is an out-dated way of indicating the presence of a single
hydrogen ion, as in "sodium bicarbonate" (NaHCO3). The preferred
method specifically names the hydrogen atom. Thus, NaHCO3 would
be called "sodium hydrogen carbonate".
6. The prefix thio indicates the substitution of oxygen by sulfur, so that
thiosulfate ion is a sulfate ion SO4
2- with one oxygen replaced by a
sulfur as in S2O3
2-.
The preferred IUPAC name for the protonated species H2S2O3 is thiosulfuric
acid.
IUPAC nomenclature
14. Hydrates are ionic compounds that have absorbed water. They
are named as the ionic compound followed by a numerical prefix
and -hydrate. The numerical prefixes used are listed below:
For example, CuSO4 · 5H2O is "copper(II) sulfate pentahydrate".
Naming hydrates
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
15. Acids are named by the anion they form when dissolved in water. If
an acid forms an anion ending in ide, then its name is formed by
adding the prefix hydro to the anion's name and replacing the ide
with ic. Finally the word acid is appended.
For example, hydrochloric acid forms a chloride anion. With sulfur,
however, the whole word is kept instead of the root: i.e.:
hydrosulfuric acid.
Secondly, anions with an -ate suffix are formed when acids with an -
ic suffix are dissolved, e.g. chloric acid (HClO3) dissociates into
chlorate anions to form salts such as sodium chlorate (NaClO3);
anions with an -ite suffix are formed when acids with an -ous suffix
are dissolved in water, e.g. chlorous acid (HClO2) disassociates into
chlorite anions to form salts such as sodium chlorite (NaClO2).
Naming acids
16. The four oxyacids of chlorine are called hypochlorous acid
(HClO), chlorous acid (HClO2), chloric acid (HClO3) and
perchloric acid (HClO4).
Their respective conjugate bases are the hypochlorite
(ClO-), chlorite (ClO2
-), chlorate (ClO3
-) and perchlorate
(ClO4
-) ions.
The corresponding potassium salts are potassium
hypochlorite (KClO), potassium chlorite (KClO2), potassium
chlorate (KClO3) and potassium perchlorate (KClO4).
Oxyacids of chlorine
17. Acid Formula Anions Notes
Sulfuric acid H2SO4 sulfate ,SO4
2- and hydrogen
sulfate, HSO4
-
Thiosulfuric acid H2S2O3 thiosulfate, S2O3
2− Aqueous solutions
decompose:
{write equation}†
Sulfurous acid H2SO3
Sulfite, SO3
2- and hydrogen
sulfite, HSO3
-
Aqueous solutions
decompose:
{write equation}†
Oxyacids of sulfur
Only the most common oxyacids are shown in the table below:
† Hint: see Prac. Manual pages 25 and 26
18. When the metal has more than one possible ionic charge or
oxidation number the name becomes ambiguous.
In these cases the oxidation number (the same as the charge) of
the metal ion is represented by a Roman numeral in parentheses
immediately following the metal ion name.
For example in uranium(VI) fluoride the oxidation number of
uranium is 6. Another example is the iron oxides. FeO is iron(II)
oxide and Fe2O3 is iron(III) oxide.
An older system used prefixes and suffixes to indicate the
oxidation number, according to the following scheme (next
page):
Traditional naming
19. This system has partially fallen out of use, but survives in the
common names of many chemical compounds: e.g., "ferric chloride"
(instead calling it "iron(III) chloride") and "potassium
permanganate" (instead of "potassium manganate(VII)").
Traditional naming
Oxidation state Cations and acids Anions
Lowest hypo- -ous hypo- -ite
-ous -ite
-ic -ate
per- -ic per- -ate
Highest hyper- -ic hyper- -ate
20. When naming a complex ion, the ligands are named before the
metal ion.
Write the names of the ligands in alphabetical order (numerical
prefixes do not affect the order.)
Multiple occurring monodentate ligands receive a prefix according to the
number of occurrences: di-, tri-, tetra-, penta-, or hexa. Polydentate
ligands (e.g., ethylenediamine, oxalate) receive bis-, tris-, tetrakis-, etc.
Anions end in ido. This replaces the final 'e' when the anion ends with
'-ate', e.g. sulfate becomes sulfato. It replaces 'ide': cyanide becomes
cyanido.
Neutral ligands are given their usual name, with some exceptions: NH3
becomes ammine; H2O becomes aqua or aquo; CO becomes carbonyl; NO
becomes nitrosyl.
Naming complexes
21. Write the name of the central atom/ion. If the complex is an
anion, the central atom's name will end in -ate, and its Latin
name will be used if available (except for mercury).
If the central atom's oxidation state needs to be specified, write
it as a Roman numeral in parentheses.
Name cation then anion as separate words.
Examples:
[NiCl4]2− tetrachloridonickelate(II) ion
[CuNH3Cl5]3− amminepentachloridocuprate(II) ion
[Cd(en)2(CN)2] dicyanidobis(ethylenediamine)cadmium(II)
[Co(NH3)5Cl]SO4 pentaamminechloridocobalt(III) sulfate
Naming complexes
22. Soluble Insoluble
Group I and NH4
+ compounds
Carbonates (Except Group I, NH4
+ and
uranyl compounds)
Nitrates, chlorates (all are highly soluble)
Sulfites (Except Group I and NH4
+
compounds)
Acetates (Ethanoates) (Except Ag+
compounds)
Phosphates (Except Group I and NH4
+
compounds)
Chlorides, bromides and iodides (Except
Ag+, Pb2+, Cu+ and Hg2
2+)
Hydroxides and oxides (Except Group I,
NH4
+, Ba2+, Sr2+ and Tl+)
Sulfates (Except Ag+, Pb2+, Ba2+, Sr2+ and
Ca2+)
Sulfides (Except Group I, Group II and
NH4
+ compounds)
Chromates (Except Na2CrO4, K2CrO4,
(NH4)2CrO4, and MgCrO4)
Solubility Rules
25. Safe Handling of Acids and Bases
There are a number of proper procedures for the safe handling of acids and bases
that you need to know because you’ll be working with them quite a bit. (These
guidelines are also listed in your Practical Manual.)
Both acids and bases can be corrosive to human tissue. When concentrated, they can
react with tissue and break it down. In general, the more concentrated the acid or
base happens to be, the more hazardous it is. Although the more concentrated acids
and bases are the most dangerous ones, don't ignore the dilute ones.
You must be particularly careful about getting them in your eyes. It is compulsory to
wear safety glasses when handling either acids or bases. But if you do get any in your
eyes, let the demonstrator know and flush it out immediately with lots of water,
several minutes worth. There are eye washes in the lab. You will learn where they are,
and how to use them, in the online induction.
Precautions
26. Safe Handling of Acids and Bases
Suppose you get some acid or base on you, other than in your eyes. The procedure is
the essentially the same: flush that area immediately for several minutes with water
and consult the demonstrator for further advice. If you should be unfortunate
enough to spill it all over you, use the safety shower in the lab.
If you spill acid or base on the lab bench top or on the floor, treat it immediately. If it
is an acid, first neutralize it with sufficient sodium hydrogen carbonate, (commonly
known as baking soda). We have spill kits for use with extensive spills available in the
lab or in the adjoining prep room (check with demonstrator or technical staff).
The quantities and concentrations of acids and bases used in the exercises at QUT are
permissible to flush down the drain. However, the quantity involved in a spill should
be neutralized before disposal (see technical staff).
Precautions
27. Remember the triple AAA:
Always add acids to water: never the other way around
Hazard warning symbols
29. Also known as inorganic acids or mineral acids and include: Hydrochloric
acid: Nitric acid (dilute), Phosphoric acid, Sulfuric acid (dilute), Boric acid,
Hydrofluoric acid and Hydrobromic acid.
Inorganic acids are generally soluble in water with the release of hydrogen
ions. The resulting solutions have pHs of less than 7.0.
Acids neutralize chemical bases (for example: amines and inorganic
hydroxides) to form salts. Neutralization occurs as the base accepts
hydrogen ions that the acid donates.
Neutralization can generate dangerously large amounts of heat in small
spaces. The dissolution of acids in water or the dilution of their
concentrated solutions with additional water may generate significant heat;
the addition of water often generates sufficient heat in the small region of
mixing to cause some of the water to boil explosively. The resulting
"bumping" spatters the acid.
These materials react with active metals, including such structural metals as
aluminum and iron, to release hydrogen, a flammable gas.
Non-oxidising acids
30. Test for Test method Observations Equations
H2(g) lighted splint “pop” {write equation}
O2(g) Glowing splint Re-ignites {write equation}
CO2(g) limewater White ppt {write equation}
HCl(g) Moist blue litmus paper Turns red {write equation}
NH3(g) Moist red litmus paper Turns blue {write equation}
SO2(g) Moist dichromate paper Turns green {write equation}
Cl2(g) Pungent gas - Drop of AgNO3 White ppt {write equation}
Br2(g) Orange-brown gas - Drop of AgNO3 Cream ppt {write equation}
NO2(g) Orange-brown gas No simple test {write equation}
NO(g) Colourless → orange brown gas Colourless in the
absence of air
{write equation}
H2S(g) moist lead ethanoate (acetate) paper Turns black {write equation}
Qualitative tests for gases
31. A basic oxide is an oxide that shows basic properties (in
opposition to acidic oxides) and that either:
reacts with water to form a base; or
reacts with an acid to form a salt.
Examples include:
Sodium oxide which reacts with water to produce sodium hydroxide
Magnesium oxide, which reacts with hydrochloric acid to form
magnesium chloride
Copper oxide, which reacts with nitric acid to form copper nitrate
Basic oxides are oxides mostly of metals, especially alkali and alkaline
earth (Group I and II) metals.
Basic oxides (and hydroxides)
32. An amphoteric substance is a compound that can react as an acid as
well as a base. The word is derived from the Greek word amphoteroi
(ἀμφότεροι) meaning "both".
Many metals (such as zinc, tin, lead, aluminium, and beryllium) and most
metalloids have amphoteric oxides or hydroxides. Amphoteric
substances can either donate or accept a proton.
Zinc oxide (ZnO) reacts differently depending on the pH of the solution:
In acids: ZnO + 2H+ → {write products}
In bases: ZnO + H2O + 2OH- → {write products}
This effect can be used to separate different cations, such as zinc from
manganese (next week: separation schemes).
Amphoteric oxides and hydroxides
33. Aluminium hydroxide is as well:
Base (neutralizing an acid): Al(OH)3 + 3HCl → {write products}
Acid (neutralizing a base): Al(OH)3 + NaOH → {write products}
Some other examples include:
Aluminium oxide
with acid: Al2O3 + 3H2O + 6H3O+(aq) →) {write products}
with base: Al2O3 + 3H2O + 2OH-(aq) → 2 {write products}
Lead oxide
with acid: PbO + 2HCl → {write products}
with base: PbO + Ca(OH)2 +H2O → {write products}
Question: see if you can write ionic chemical equations that illustrate the
amphoteric nature of Beryllium hydroxide?
Amphoteric oxides and hydroxides
34. An oxidizing acid is a Brønsted acid that is also a strong oxidizing agent.
All Brønsted acids can act as moderately strong oxidizing agents, because
the acidic proton can be reduced to hydrogen gas.
However, some acids contain other structures that act as stronger
oxidizing agents than hydrogen. Generally, they contain oxygen in the
anionic structure.
These include nitric acid, perchloric acid, chloric acid, chromic acid, and
concentrated sulfuric acid, among others.
For example, copper metal cannot be oxidized by and dissolved in a non-
oxidizing acid, because it is lower on the reactivity series than acidic
hydrogen. However, an oxidizing acid such as nitric acid can oxidize the
copper, and allow it to dissolve.
Oxidizing acids
35. Strongly electropositive metals, such as magnesium react with nitric acid as with other acids,
reducing the hydrogen ion.
Mg + 2 H+ → {write products}
With less electropositive metals the products depend on temperature and the acid concentration.
For example, copper reacts with dilute nitric acid at ambient temperatures with a 3:8 stoichiometry.
3Cu + 8 HNO3 → {write products}
The nitric oxide produced may react with atmospheric oxygen to give nitrogen dioxide.
With more concentrated nitric acid, nitrogen dioxide is produced directly in a reaction with 1:4
stoichiometry.
Cu + 4H+ + 2 NO3
− → {write products}
Passivation
Although chromium (Cr), iron (Fe) and aluminium (Al) readily dissolve in dilute nitric acid, the
concentrated acid forms a metal oxide layer that protects the metal from further oxidation, which is
called passivation.
Nitric Acid
36. Sulfuric acid reacts with most bases to give the corresponding sulfate. For example, the blue copper
salt copper(II) sulfate is prepared by the reaction of copper(II) oxide with sulfuric acid:
CuO(s) + H2SO4 (aq) → {write products}
Sulfuric acid can also be used to displace weaker acids from their salts. Reaction with sodium
acetate, for example, displaces acetic acid, CH3COOH, and forms sodium hydrogen sulfate:
H2SO4 + CH3COONa → {write products}
Similarly, reacting sulfuric acid with potassium nitrate can be used to produce nitric acid and
potassium hydrogen sulfate.
Concentrated sulfuric acid reacts with sodium chloride, and gives hydrogen chloride gas and sodium
hydrogen sulfate:
NaCl + H2SO4 → {write products}
Similarly with other halide salts
Sulfuric Acid
37. Sulfuric acid reacts with most metals via a single displacement reaction to produce hydrogen gas
and the metal sulfate. Dilute H2SO4 attacks iron, aluminium, zinc, manganese, magnesium and nickel,
but reactions with tin and copper require the acid to be hot and concentrated.
Lead and tungsten, however, are resistant to sulfuric acid. The reaction with iron shown below is
typical for most of these metals, but the reaction with tin produces sulfur dioxide rather than
hydrogen.
Fe(s) + H2SO4(aq) → {write products}
Sn (s) + 2H2SO4(aq) → {write products}
These reactions may be taken as typical: the hot concentrated acid generally acts as an oxidizing
agent whereas the dilute acid acts as a typical acid. Hence hot concentrated acid reacts with tin,
zinc and copper to produce the salt, water and sulfur dioxide, whereas the dilute acid reacts with
metals high in the reactivity series (such as Zn) to produce a salt and hydrogen.
Sulfuric Acid