Answer: The first ten elements in modern periodic table are hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and ...for more reading click here,https://bidyashramodia.blogspot.com/2022/06/ncert-solutions-for-class-10-science_24.html
Assingment 2 rl no. 5209 e2 ene reaction.pptJabrilHaad
The document discusses several types of cycloaddition reactions including the Alder ene reaction, carbonyl ene reaction, Diels-Alder reaction, and thermal [2+2] cycloaddition. The Alder ene reaction involves an alkene reacting with an enophile to form one new C-C and C-H bond without ring formation. The Diels-Alder reaction is a concerted [4+2] cycloaddition that occurs between a conjugated diene and substituted alkene to form a cyclohexene ring system. The thermal [2+2] cycloaddition mainly involves ketene chemistry and forms a four-membered ring from an alkene and electrophilic al
Crown ethers are cyclic chemical compounds containing oxygen atoms separated by carbon atoms in their ring structure. They form stable complexes with metal ions through electrostatic attraction between the metal ion situated in the cavity of the ring and the surrounding oxygen atoms. Crown ethers are named based on the total number of atoms in the ring and the number of oxygen atoms. They are used to help dissolve ionic salts needed for organic reactions in organic solvents by forming soluble complexes with metal cations.
Periodic classification of elements by nandishShambu Nandish
1) The document discusses the periodic classification of elements, including early attempts by Dobereiner, Newlands, and Mendeleev.
2) Mendeleev organized the elements into a periodic table based on atomic mass and properties, leaving gaps for undiscovered elements.
3) Modern periodic law states that properties are a periodic function of atomic number, with elements in the same group having the same number of valence electrons.
The Barton reaction involves the photolysis of an alkyl nitrite to form a δ-nitroso alcohol which can dimerize or form an oxime. Sir Derek Barton discovered this reaction in 1960 and was awarded the Nobel Prize in Chemistry in 1969 for his work, including understanding the Barton Reaction. The reaction mechanism involves homolytic cleavage of the RO-NO bond, followed by δ-hydrogen abstraction, radical recombination, and tautomerization to form an oxime. An example provided is the Barton reaction of butyl nitrite to form a δ-nitroso butanol that can then dimerize or form an oxime. Applications include the synthesis of natural products like hormones and alkaloids.
An absorption spectrum occurs when a photon is absorbed, exciting an electron to a higher quantum energy state. Absorption spectra involve atoms increasing in energy level. An emission spectrum occurs when a photon is emitted as an electron drops to a lower quantum energy state, with emission spectra involving electrons decreasing their energy level. The document also provides a conversion between electronvolts (eV) and joules (J).
Essential and non-essential elements/types of essential elements-Bulk and trace elements/ Some important essential elements/their uses / role in biological processes.
Prepared for my college-Kanya Maha Vidyalaya,Jalandhar.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
Assingment 2 rl no. 5209 e2 ene reaction.pptJabrilHaad
The document discusses several types of cycloaddition reactions including the Alder ene reaction, carbonyl ene reaction, Diels-Alder reaction, and thermal [2+2] cycloaddition. The Alder ene reaction involves an alkene reacting with an enophile to form one new C-C and C-H bond without ring formation. The Diels-Alder reaction is a concerted [4+2] cycloaddition that occurs between a conjugated diene and substituted alkene to form a cyclohexene ring system. The thermal [2+2] cycloaddition mainly involves ketene chemistry and forms a four-membered ring from an alkene and electrophilic al
Crown ethers are cyclic chemical compounds containing oxygen atoms separated by carbon atoms in their ring structure. They form stable complexes with metal ions through electrostatic attraction between the metal ion situated in the cavity of the ring and the surrounding oxygen atoms. Crown ethers are named based on the total number of atoms in the ring and the number of oxygen atoms. They are used to help dissolve ionic salts needed for organic reactions in organic solvents by forming soluble complexes with metal cations.
Periodic classification of elements by nandishShambu Nandish
1) The document discusses the periodic classification of elements, including early attempts by Dobereiner, Newlands, and Mendeleev.
2) Mendeleev organized the elements into a periodic table based on atomic mass and properties, leaving gaps for undiscovered elements.
3) Modern periodic law states that properties are a periodic function of atomic number, with elements in the same group having the same number of valence electrons.
The Barton reaction involves the photolysis of an alkyl nitrite to form a δ-nitroso alcohol which can dimerize or form an oxime. Sir Derek Barton discovered this reaction in 1960 and was awarded the Nobel Prize in Chemistry in 1969 for his work, including understanding the Barton Reaction. The reaction mechanism involves homolytic cleavage of the RO-NO bond, followed by δ-hydrogen abstraction, radical recombination, and tautomerization to form an oxime. An example provided is the Barton reaction of butyl nitrite to form a δ-nitroso butanol that can then dimerize or form an oxime. Applications include the synthesis of natural products like hormones and alkaloids.
An absorption spectrum occurs when a photon is absorbed, exciting an electron to a higher quantum energy state. Absorption spectra involve atoms increasing in energy level. An emission spectrum occurs when a photon is emitted as an electron drops to a lower quantum energy state, with emission spectra involving electrons decreasing their energy level. The document also provides a conversion between electronvolts (eV) and joules (J).
Essential and non-essential elements/types of essential elements-Bulk and trace elements/ Some important essential elements/their uses / role in biological processes.
Prepared for my college-Kanya Maha Vidyalaya,Jalandhar.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
Dioxygen complexes, dioxygen as ligand Geeta Tewari
This presentation describes about the preparation, properties, bonding modes, classification and applications of metal Dinitrogen Complexes. Also explains the MO diagram of molecular nitrogen.
This document discusses elimination reactions where a small molecule is removed from a reactant. It describes the elimination of HBr from bromoalkanes using a dilute NaOH solution, which can cause either a substitution or elimination reaction depending on conditions. The two types of elimination reactions are E2, a bimolecular process without intermediates typical of primary/secondary halides, and E1, a unimolecular reaction with a carbocation intermediate typical of tertiary halides. Hydroxide acts as a base by accepting a proton from the alkyl halide, initiating electron movement that forms a C=C double bond and removes the halide.
Vinyl chloride is a colorless, flammable gas with a sweet odor that is used to make polyvinyl chloride (PVC) plastics and polymers. It has a chemical formula of C2H3Cl and molecular weight of 62.5 g/mol. Exposure can occur through factory emissions, evaporation from waste sites, or off-gassing from new plastic products. Vinyl chloride is carcinogenic and toxic, especially to the liver, kidneys, and central nervous system. A 2004 explosion at a Formosa Plastics plant in Texas released vinyl chloride, ignited an explosion, and caused fires that burned for days after the accident.
This is an effort to make ppt of p block elements , a topic in XII, chemistry(cbse) , whom as a tutor i have often felt students are horrified due to its large text size, long descriptipns, several information to be remembered and several reasonings to keep in mind.
Hope this ppt would solve thier problem of a thorough preparation of topic with all important aspects covered in the ppt.
Founder Dr Mona Srivastava
Masterchemclasses
Atomic radii decrease across a period as nuclear charge increases. Cations are smaller than their parent atoms. Among isoelectronic species, the one with the larger positive nuclear charge will have the smallest radius. Ionization energy generally increases across a period as it is more difficult to remove electrons, and decreases down a group as shielding increases. Electronegativity follows similar trends as ionization energy.
Polarizable & non polarizable ElectrodesTalha Liaqat
A polarizable electrode is characterized by charge separation at the electrode-electrolyte boundary and behaves like a capacitor. It does not allow faradic current to pass freely and the electrode reaction is very slow. In contrast, a non-polarizable electrode does not exhibit charge separation and allows faradic current to pass through without polarization. It has an infinitely fast electrode reaction and behaves like a resistor. Examples of polarizable electrodes include platinum while silver/silver chloride is an example of a non-polarizable electrode.
Hemerythrin is a non-heme iron containing protein found in invertebrates that contains 8 subunits with 2 iron active sites per subunit. It reversibly binds oxygen without cooperativity. Each iron site is coordinated by carbonyl groups from amino acids and hydroxyl ions. Deoxy-hemerythrin has antiferromagnetically coupled iron sites.
Hemocyanin is a copper containing protein that carries oxygen in invertebrates. Deoxyhemocyanin contains copper(I) which is colorless and non-coordinated, while oxygenated hemocyanin has copper(II) in a coordinated structure, removing strain.
Cytochromes are electron carrier proteins found
Giacomo Ciamician is considered the father of photochemistry, which is the study of chemical reactions caused by the absorption of light. Photochemistry includes reactions accompanied by the emission of energy as radiation. There are four types of electronic transitions that can occur when molecules absorb light: sigma-sigma*, sigma-pi*, pi-pi*, and n-pi*. These transitions differ in the amount of energy required, with sigma-sigma* requiring the most and n-pi* the least. Key laws in photochemistry include Grotthuss-Draper law which states only absorbed light can cause chemical changes, and Stark-Einstein law that one quantum of light is absorbed per reacting molecule. Photophysical processes like fluorescence
A chain reaction involves intermediates generated in one step leading to intermediates in subsequent steps. Radicals and ions can act as chain carriers that propagate the reaction. Initiation steps form the initial chain carriers. Propagation steps produce new carriers from reactants. Branching steps generate multiple carriers from a product. Termination and inhibition steps end the chain reaction. The rate law for the pyrolysis of ethanal follows the Rice-Herzfeld mechanism and is third order with respect to ethanal concentration.
Nonstoichiometric or Berthollide compounds have ratios of atoms that are not whole numbers as implied by the chemical formula. There are several types of defects that can occur in nonstoichiometric compounds including negative ions being absent, interstitial ions and electrons, positive ions being absent, and extra interstitial negative ions. These defects can cause the compounds to act as n-type or p-type semiconductors depending on whether there is a metal excess or deficiency.
The document discusses the modern periodic law and periodic trends in atomic properties. It can be summarized as follows:
1. The modern periodic law states that the properties of elements are periodic functions of their atomic numbers. Elements are arranged in the periodic table based on increasing atomic number and similar outer electron configurations that repeat at regular intervals.
2. The periodic table is divided into blocks based on orbital types. Elements show trends in properties within periods and down groups, including decreasing atomic radius and increasing ionization energy with increasing atomic number. Electron affinity also tends to decrease down groups.
3. Successive ionization energies increase as more energy is required to remove additional electrons. Stability of half-filled and fully-filled
This chapter discusses carbonyl compounds, including aldehydes and ketones. It covers nomenclature, reactivity, and reactions of carbonyl compounds. Specifically, it describes how aldehydes are more reactive than ketones due to increased partial positive charge and steric accessibility. It also summarizes key reactions such as addition, reduction, substitution involving nucleophiles, protecting groups, and stereochemistry of additions.
Alkali metals have a single outer electron, making them highly reactive and electropositive. They are never found naturally in their elemental forms, instead occurring as oxides, halides, borates, silicates, and nitrates. Alkali metals increase in size down the group and have low ionization energies, with lithium being the smallest and most reactive and cesium being the largest and least reactive. They react vigorously with air, water, halogens, and dihydrogen to form ionic compounds. Common uses include softening hard water, manufacturing glass, detergents, and as reducing agents.
Chemical reactions and equations 10 chm(1)VeenuGupta8
This presentation is based on the chapter 1 of chemistry .this presentation includes the basic informations related with the chemical Reactions and equations . it will help students and teachers in the teaching learning process
This document summarizes the synthesis and characterization of new Schiff base ligands and their metal complexes. It describes the synthesis of five Schiff base ligands derived from substituted benzaldehydes and anilines using the reflux method. Copper and nickel complexes were formed from two of the ligands. The ligands and complexes were characterized using infrared spectroscopy, which showed shifts in the C=N and C-O peaks upon complexation. The research aims to synthesize new Schiff bases and their Cu2+ and Ni2+ complexes and characterize them using IR spectroscopy to determine the coordination sites.
Borates are boron-containing compounds that contain borate anions. They are classified based on the number of boron atoms in the anion, ranging from orthoborates to hexaborates. Borates have many important uses such as increasing plant growth, preventing bacterial growth, and as flame retardants. They are found naturally occurring as minerals like ulexite and colemanite and have a variety of industrial applications.
Carbon is a key element that forms the basis of many important compounds due to its ability to bond with other carbon atoms and elements. It exists in several allotropes with varying properties, including diamond and graphite. Carbon can form single, double, and triple bonds with other atoms, allowing it to create large, complex molecules through catenation. Saturated carbon compounds contain only single bonds, while unsaturated compounds contain double or triple bonds. Functional groups and structural isomers give compounds unique reactivity and properties. Important carbon compounds discussed include ethanol, ethanoic acid, soaps, and detergents.
The document provides an introduction to organic photochemistry, including classifications of photochemical reactions and their application in organic synthesis. It discusses key concepts like Jablonski diagrams, excited state processes like fluorescence, phosphorescence, and intersystem crossing. Photochemistry is described as overcoming kinetic barriers quickly to form complex products and access reactivity not possible by other methods, though it can have low selectivity and conversion in some cases. Common photochemical reactions mentioned are α-cleavage and hydrogen abstraction.
The document summarizes the development of the periodic table of elements from early classifications by Dobereiner and Newlands to Mendeleev's and Meyer's published periodic tables to Moseley's establishment of the ordering by atomic number. It explains key periodic properties including atomic structure and trends in atomic size, and provides an overview of the layout and information contained in the modern periodic table.
This document summarizes several organic rearrangement reactions: the Cope rearrangement, Claisen rearrangement, and Curtius rearrangement. The Cope rearrangement involves the [3,3]-sigmatropic rearrangement of 1,5-dienes. The Claisen rearrangement is a carbon-carbon bond forming reaction that rearranges allyl vinyl ethers to γ,δ-unsaturated carbonyls. The Curtius rearrangement converts carboxylic acids to isocyanates through an acid azide intermediate. Mechanisms are provided for each reaction.
The document discusses periodic properties of elements including groups and periods in the periodic table. It provides explanations and examples of how properties such as valence electrons, valency, and molecular formulas vary between elements in the same period and group. It also answers questions about predicting electronic configurations, group numbers, metallic/non-metallic character, and other properties based on an element's atomic number.
1. The document provides a summary of the periodic classification of elements, including the theories of Dobereiner, Newlands, and Mendeleev, and the modern periodic law.
2. It describes the achievements and limitations of their classifications, and how the modern periodic table addresses the limitations by arranging elements by atomic number instead of atomic mass.
3. The document also summarizes key trends in the modern periodic table such as how properties change from period to period and group to group.
Dioxygen complexes, dioxygen as ligand Geeta Tewari
This presentation describes about the preparation, properties, bonding modes, classification and applications of metal Dinitrogen Complexes. Also explains the MO diagram of molecular nitrogen.
This document discusses elimination reactions where a small molecule is removed from a reactant. It describes the elimination of HBr from bromoalkanes using a dilute NaOH solution, which can cause either a substitution or elimination reaction depending on conditions. The two types of elimination reactions are E2, a bimolecular process without intermediates typical of primary/secondary halides, and E1, a unimolecular reaction with a carbocation intermediate typical of tertiary halides. Hydroxide acts as a base by accepting a proton from the alkyl halide, initiating electron movement that forms a C=C double bond and removes the halide.
Vinyl chloride is a colorless, flammable gas with a sweet odor that is used to make polyvinyl chloride (PVC) plastics and polymers. It has a chemical formula of C2H3Cl and molecular weight of 62.5 g/mol. Exposure can occur through factory emissions, evaporation from waste sites, or off-gassing from new plastic products. Vinyl chloride is carcinogenic and toxic, especially to the liver, kidneys, and central nervous system. A 2004 explosion at a Formosa Plastics plant in Texas released vinyl chloride, ignited an explosion, and caused fires that burned for days after the accident.
This is an effort to make ppt of p block elements , a topic in XII, chemistry(cbse) , whom as a tutor i have often felt students are horrified due to its large text size, long descriptipns, several information to be remembered and several reasonings to keep in mind.
Hope this ppt would solve thier problem of a thorough preparation of topic with all important aspects covered in the ppt.
Founder Dr Mona Srivastava
Masterchemclasses
Atomic radii decrease across a period as nuclear charge increases. Cations are smaller than their parent atoms. Among isoelectronic species, the one with the larger positive nuclear charge will have the smallest radius. Ionization energy generally increases across a period as it is more difficult to remove electrons, and decreases down a group as shielding increases. Electronegativity follows similar trends as ionization energy.
Polarizable & non polarizable ElectrodesTalha Liaqat
A polarizable electrode is characterized by charge separation at the electrode-electrolyte boundary and behaves like a capacitor. It does not allow faradic current to pass freely and the electrode reaction is very slow. In contrast, a non-polarizable electrode does not exhibit charge separation and allows faradic current to pass through without polarization. It has an infinitely fast electrode reaction and behaves like a resistor. Examples of polarizable electrodes include platinum while silver/silver chloride is an example of a non-polarizable electrode.
Hemerythrin is a non-heme iron containing protein found in invertebrates that contains 8 subunits with 2 iron active sites per subunit. It reversibly binds oxygen without cooperativity. Each iron site is coordinated by carbonyl groups from amino acids and hydroxyl ions. Deoxy-hemerythrin has antiferromagnetically coupled iron sites.
Hemocyanin is a copper containing protein that carries oxygen in invertebrates. Deoxyhemocyanin contains copper(I) which is colorless and non-coordinated, while oxygenated hemocyanin has copper(II) in a coordinated structure, removing strain.
Cytochromes are electron carrier proteins found
Giacomo Ciamician is considered the father of photochemistry, which is the study of chemical reactions caused by the absorption of light. Photochemistry includes reactions accompanied by the emission of energy as radiation. There are four types of electronic transitions that can occur when molecules absorb light: sigma-sigma*, sigma-pi*, pi-pi*, and n-pi*. These transitions differ in the amount of energy required, with sigma-sigma* requiring the most and n-pi* the least. Key laws in photochemistry include Grotthuss-Draper law which states only absorbed light can cause chemical changes, and Stark-Einstein law that one quantum of light is absorbed per reacting molecule. Photophysical processes like fluorescence
A chain reaction involves intermediates generated in one step leading to intermediates in subsequent steps. Radicals and ions can act as chain carriers that propagate the reaction. Initiation steps form the initial chain carriers. Propagation steps produce new carriers from reactants. Branching steps generate multiple carriers from a product. Termination and inhibition steps end the chain reaction. The rate law for the pyrolysis of ethanal follows the Rice-Herzfeld mechanism and is third order with respect to ethanal concentration.
Nonstoichiometric or Berthollide compounds have ratios of atoms that are not whole numbers as implied by the chemical formula. There are several types of defects that can occur in nonstoichiometric compounds including negative ions being absent, interstitial ions and electrons, positive ions being absent, and extra interstitial negative ions. These defects can cause the compounds to act as n-type or p-type semiconductors depending on whether there is a metal excess or deficiency.
The document discusses the modern periodic law and periodic trends in atomic properties. It can be summarized as follows:
1. The modern periodic law states that the properties of elements are periodic functions of their atomic numbers. Elements are arranged in the periodic table based on increasing atomic number and similar outer electron configurations that repeat at regular intervals.
2. The periodic table is divided into blocks based on orbital types. Elements show trends in properties within periods and down groups, including decreasing atomic radius and increasing ionization energy with increasing atomic number. Electron affinity also tends to decrease down groups.
3. Successive ionization energies increase as more energy is required to remove additional electrons. Stability of half-filled and fully-filled
This chapter discusses carbonyl compounds, including aldehydes and ketones. It covers nomenclature, reactivity, and reactions of carbonyl compounds. Specifically, it describes how aldehydes are more reactive than ketones due to increased partial positive charge and steric accessibility. It also summarizes key reactions such as addition, reduction, substitution involving nucleophiles, protecting groups, and stereochemistry of additions.
Alkali metals have a single outer electron, making them highly reactive and electropositive. They are never found naturally in their elemental forms, instead occurring as oxides, halides, borates, silicates, and nitrates. Alkali metals increase in size down the group and have low ionization energies, with lithium being the smallest and most reactive and cesium being the largest and least reactive. They react vigorously with air, water, halogens, and dihydrogen to form ionic compounds. Common uses include softening hard water, manufacturing glass, detergents, and as reducing agents.
Chemical reactions and equations 10 chm(1)VeenuGupta8
This presentation is based on the chapter 1 of chemistry .this presentation includes the basic informations related with the chemical Reactions and equations . it will help students and teachers in the teaching learning process
This document summarizes the synthesis and characterization of new Schiff base ligands and their metal complexes. It describes the synthesis of five Schiff base ligands derived from substituted benzaldehydes and anilines using the reflux method. Copper and nickel complexes were formed from two of the ligands. The ligands and complexes were characterized using infrared spectroscopy, which showed shifts in the C=N and C-O peaks upon complexation. The research aims to synthesize new Schiff bases and their Cu2+ and Ni2+ complexes and characterize them using IR spectroscopy to determine the coordination sites.
Borates are boron-containing compounds that contain borate anions. They are classified based on the number of boron atoms in the anion, ranging from orthoborates to hexaborates. Borates have many important uses such as increasing plant growth, preventing bacterial growth, and as flame retardants. They are found naturally occurring as minerals like ulexite and colemanite and have a variety of industrial applications.
Carbon is a key element that forms the basis of many important compounds due to its ability to bond with other carbon atoms and elements. It exists in several allotropes with varying properties, including diamond and graphite. Carbon can form single, double, and triple bonds with other atoms, allowing it to create large, complex molecules through catenation. Saturated carbon compounds contain only single bonds, while unsaturated compounds contain double or triple bonds. Functional groups and structural isomers give compounds unique reactivity and properties. Important carbon compounds discussed include ethanol, ethanoic acid, soaps, and detergents.
The document provides an introduction to organic photochemistry, including classifications of photochemical reactions and their application in organic synthesis. It discusses key concepts like Jablonski diagrams, excited state processes like fluorescence, phosphorescence, and intersystem crossing. Photochemistry is described as overcoming kinetic barriers quickly to form complex products and access reactivity not possible by other methods, though it can have low selectivity and conversion in some cases. Common photochemical reactions mentioned are α-cleavage and hydrogen abstraction.
The document summarizes the development of the periodic table of elements from early classifications by Dobereiner and Newlands to Mendeleev's and Meyer's published periodic tables to Moseley's establishment of the ordering by atomic number. It explains key periodic properties including atomic structure and trends in atomic size, and provides an overview of the layout and information contained in the modern periodic table.
This document summarizes several organic rearrangement reactions: the Cope rearrangement, Claisen rearrangement, and Curtius rearrangement. The Cope rearrangement involves the [3,3]-sigmatropic rearrangement of 1,5-dienes. The Claisen rearrangement is a carbon-carbon bond forming reaction that rearranges allyl vinyl ethers to γ,δ-unsaturated carbonyls. The Curtius rearrangement converts carboxylic acids to isocyanates through an acid azide intermediate. Mechanisms are provided for each reaction.
The document discusses periodic properties of elements including groups and periods in the periodic table. It provides explanations and examples of how properties such as valence electrons, valency, and molecular formulas vary between elements in the same period and group. It also answers questions about predicting electronic configurations, group numbers, metallic/non-metallic character, and other properties based on an element's atomic number.
1. The document provides a summary of the periodic classification of elements, including the theories of Dobereiner, Newlands, and Mendeleev, and the modern periodic law.
2. It describes the achievements and limitations of their classifications, and how the modern periodic table addresses the limitations by arranging elements by atomic number instead of atomic mass.
3. The document also summarizes key trends in the modern periodic table such as how properties change from period to period and group to group.
Science classification of elements chapter 5 pptanveshasupriya
Mendeleev's periodic table arranged elements in order of increasing atomic mass and grouped those with similar properties. It left gaps for undiscovered elements and accurately predicted some of their properties. The modern periodic table is based on atomic number instead of mass. It has 18 groups and 7 periods, with trends like atomic size decreasing left to right in a period and increasing down a group. Properties also periodically repeat based on atomic number. Mendeleev's table had limitations like isotopes and hydrogen positions but represented a major step forward in classifying the elements.
This document is a lesson on groups and periods in the periodic table. It defines periods as rows from left to right, and groups as columns from top to bottom. Elements in the same group have similar properties because they have the same number of valence electrons. The lesson discusses special metal and nonmetal groups, including alkali metals, alkaline earth metals, transition metals, halogens, and noble gases. It provides examples of elements in each group and their properties. The document concludes with practice questions for students.
This document contains the scheme of work and lesson plans for teaching chemistry to SS2 students. It covers topics on the periodic table over two weeks, including properties of elements, groups and periods. It then covers chemical reactions over one week, discussing concepts like reactants and products, and factors that affect reaction rates such as concentration, temperature, and catalysts. The lessons include content, examples, evaluations, and assignments.
1) Moseley showed that the atomic number of an element is equal to the number of protons in its nucleus. He suggested atomic number is a more fundamental property than atomic weight for classifying elements.
2) In the modern periodic table, elements are arranged in order of increasing atomic number in a more systematic way based on Moseley's work.
3) The electronic configuration of an element is directly related to its atomic number. The modern periodic law states that the properties of elements are periodic functions of their atomic numbers.
The document discusses the periodic classification of elements. It describes early attempts at classification including grouping elements as metals and non-metals. Dobereiner classified elements into triads based on atomic mass. Newlands arranged elements in order of increasing atomic mass in octaves but this classification had defects. Mendeleev arranged elements in order of atomic mass and predicted properties of undiscovered elements, establishing the basis of the modern periodic table. The modern periodic table arranges elements by atomic number and groups elements with similar properties and valence electrons.
This document provides information about groups, periods, and electrons on the periodic table. It discusses how elements in the same group have the same number of valence electrons and will therefore react similarly. It gives examples of sodium and potassium both having one valence electron. It also discusses how atoms gain or lose electrons to form ions, and how the periodic table is organized by increasing atomic number.
subject-chemistry,medium-english,chapter-periodic classification of elements,...PavithraT30
It is time, we stop wondering about students learning through devices. Online schooling is in practice right after the pandemic and online classes have brought students closer to technology than the conventional classroom.
https://v-learning.in/blogs/2
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
This document contains a question bank with multiple choice and short answer questions about chemical bonding. Some key topics covered include ionic and covalent bonding, oxidation-reduction reactions, electronegativity, and the structures of ions and molecules. Students are asked to define terms, identify examples, describe electron configurations and bonding patterns, and explain differences in properties between ionic and covalent compounds. Diagrams illustrate atomic structures and bonding arrangements. The question bank is intended to test students' understanding of fundamental concepts in chemical bonding.
Periodic Classification of Elements and PeriodicityNEHANEHA67
The document discusses the history and development of the periodic table. It explains that early scientists like Dobereiner and Newlands began classifying elements based on their properties, but that Dmitri Mendeleev created the first recognizable periodic table in 1871. His table arranged elements in order of atomic mass and predicted properties of undiscovered elements. Later, Moseley's discovery of atomic number allowed the modern periodic table to arrange elements by atomic number instead of mass. The document also discusses trends in properties within the periodic table.
1. Ionic compounds form when a metal reacts with a non-metal, resulting in positively charged metal ions and negatively charged non-metal ions that bond together in a crystalline lattice structure.
2. When ionic compounds dissolve in water or melt, the ions become free to move and conduct electricity. During electrolysis, positively charged metal ions move to the cathode and negatively charged non-metal ions move to the anode.
3. Common ionic compounds include sodium chloride, formed from sodium and chlorine ions, and copper chloride, used in electrolysis to extract copper metal from its ionic form.
The document summarizes key concepts about the periodic table, including its history and development by Mendeleev and Moseley. It discusses trends in various periodic properties, including atomic radius, ionization energy, electron affinity, and electronegativity. These properties follow predictable trends as one moves across or up/down the periodic table, which is explained by electron configurations and the organization of elements. The periodic table provides an organized framework for understanding similarities and differences among elements.
Periodic classification of elements 2
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The document discusses the periodic table and periodic trends in properties of elements. It defines key periodic table terms like groups, periods, atomic radius, ionization energy, and provides examples of how properties change within periods and groups. It also discusses Mendeleev's original periodic table and the modern periodic law.
- John Newlands proposed his Law of Octaves in 1863, noting that elements seemed to repeat properties every eighth element when arranged by atomic mass, but this law failed beyond calcium due to later discoveries.
- Mendeleev arranged the known 63 elements in his periodic table of 1869 based on increasing atomic mass, leaving gaps for undiscovered elements. He made accurate predictions that were later verified.
- Moseley determined in 1913 that atomic number, not mass, was fundamental to the ordering of elements, establishing the modern periodic law.
1. Early chemists attempted to classify elements based on similarities in their properties, including Dobereiner who grouped elements into triads and Newlands who arranged them in octaves based on increasing atomic mass. However, these classifications had limitations as they could not accommodate all known elements.
2. Mendeleev organized the periodic table with elements arranged in order of increasing atomic mass and proposed that elements with similar properties would fall into the same groups. His periodic table allowed for predictions of unknown elements and became widely accepted.
3. Modern periodic tables are based on atomic number rather than mass and include additional periodic trends like atomic size, metallic character, and valency that help explain elements' properties. The current 18-
1. Early chemists like Dobereiner and Newlands attempted to classify elements based on their properties, but their systems had limitations as they could not accommodate all known elements.
2. Mendeleev organized the known elements into the first periodic table based on their atomic masses and properties, allowing elements with similar properties to be grouped together. He also predicted new elements, and his table became the basis for modern classifications.
3. The modern periodic table is arranged by atomic number rather than atomic mass. Elements in the same group have the same number of valence electrons and similar properties, while periods correspond to the filling of electron shells as atomic number increases from left to right.
Similar to NCERT solutions for class 10 science chapter 5 (Periodic Classification of Elements) (20)
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NCERT solutions for class 10 science chapter 5 (Periodic Classification of Elements)
1. Science
(Chapter – 5) (Periodic Classification of Elements)
(Class – X)
6
Exercises
Question 1:
Which of the following statements is not a correct statement about the trends when going
from left to right across the periods of periodic Table.
(a) The elements become less metallic in nature.
(b) The number of valence electrons increases.
(c) The atoms lose their electrons more easily.
(d) The oxides become more acidic.
Answer 1:
(c) The atoms lose their electrons more easily.
(On moving from left to right across the periods of the periodic table, the non-metallic
character increases. Hence, the tendency to lose electrons decreases.)
Question 2:
Element X forms a chloride with the formula XCl2, which is a solid with a high melting
point. X would most likely be in the same group of the Periodic Table as
(a) Na (b) Mg (c) Al (d) Si
Answer 2:
(a)X would most likely be in the same group of the Periodic Table as magnesium (Mg).
Question 3:
Which element has
(a)two shells, both of which are completely filled with electrons?
(b)the electronic configuration 2, 8, 2?
(c) a total of three shells, with four electrons in its valence shell?
(d)a total of two shells, with three electrons in its valence shell?
(e)twice as many electrons in its second shell as in its first shell?
Answer 3:
(a)Neon has two shells, both of which are completely filled with electrons (2 electrons in
K shell and 8 electrons in L shell).
(b)Magnesium has the electronic configuration 2, 8, 2.
2. 7
(c) Silicon has a total of three shells, with four electrons in its valence shell (2 electrons
in K shell, 8 electrons in L shell and 4 electrons in M shell).
(d)Boron has a total of two shells, with three electrons in its valence shell (2 electrons in
K shell and 3 electrons in L shell).
(e)Carbon has twice as many electrons in its second shell as in its first shell (2 electrons
in K shell and 4 electrons in L shell).
Question 4:
(a)What property do all elements in the same column of the Periodic Table as boron
have in common?
(b)What property do all elements in the same column of the Periodic Table as fluorine
have in common?
Answer 4:
(a)All the elements in the same column as boron have the same number of valence
electrons (3). Hence, they all have valency equal to 3.
(b)All the elements in the same column as fluorine have the same number of valence
electrons (7). Hence, they all have valency equal to 1.
Question 5:
An atom has electronic configuration 2, 8, 7.
(a)What is the atomic number of this element?
(b)To which of the following elements would it be chemically similar? (Atomic
numbers are given in parentheses.)
N(7) F(9) P(15) Ar(18)
Answer 5:
(a)The atomic number of this element is 17.
(b)It would be chemically similar to F(9) with configuration as 2, 7.
3. 8
Question 6:
The position of three elements A, B and C in the Periodic Table are shown below −
Group 16 Group 17
− −
− A
− −
B C
(a)State whether A is a metal or non-metal.
(b)State whether C is more reactive or less reactive than A.
(c) Will C be larger or smaller in size than B?
(d)Which type of ion, cation or anion, will be formed by element A?
Answer 6:
(a)A is a non-metal.
(b)C is less reactive than A, as reactivity decreases down the group in halogens.
(c) C will be smaller in size than B as moving across a period, the nuclear charge
increases and therefore, electrons come closer to the nucleus.
(d) A will form an anion as it accepts an electron to complete its octet.
Question 7:
Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group 15 of
the Periodic Table. Write the electronic configuration of these two elements. Which of these
will be more electronegative? Why?
Answer 7:
Element K L M
Nitrogen
Phosphorus
2 5
2 8 5
Nitrogen is more electronegative than phosphorus. On moving down a group, the number
of shell increases. Therefore, the valence electrons move away from the nucleus and the
effective nuclear charge decreases. This causes the decrease in the tendency to attract
electron and hence electronegativity decreases.
4. 9
Question 8:
How does the electronic configuration of an atom relate to its position in the Modern
Periodic Table?
Answer 8:
In the modern periodic table, atoms with similar electronic configurations are placed in the
same column. In a group, the number of valence electrons remains the same. Elements
across a period show an increase in the number of valence electrons.
Question 9:
In the Modern Periodic Table, calcium (atomic number 20) is surrounded by elements with
atomic numbers 12, 19, 21, and 38. Which of these have physical and chemical properties
resembling calcium?
Answer 9:
The element with atomic number 12 has same chemical properties as that of calcium.
This is because both of them have same number of valence electrons (2).
Question 10:
Compare and contrast the arrangement of elements in Mendeleev’s periodic Table and
the Modern Periodic Table.
Answer 10:
Mendeleev’s periodic
table
Modern periodic table
1. Elements are arranged in
the increasing order of their
atomic masses.
1. Elements are arranged in the increasing order
of their atomic numbers.
2. There are a total of 7 groups
(columns) and 6 periods
(rows).
2. There are a total of 18 groups (columns) and 7
periods (rows).
3. Elements having similar
properties were placed
directly under one another.
3. Elements having the same valence shell are
present in the same period while elements
having the same number of valence electrons
are present in the same group.
4. The position of hydrogen
could not be explained.
4. Hydrogen is placed above alkali metals.
5. No distinguishing positions
for metals and non-metals.
5. Metals are present at the left hand side of the
periodic table whereas non-metals are present
at the right hand side.
5. 1
Page 81
Question 1:
Did Dobereiner’s triads also exist in the columns of Newlands’ Octaves? Compare and
find out.
Answer 1:
Only one triad of Dobereiner’s triads exists in the columns of Newlands’ octaves. The
triad formed by the elements Li, Na, and K of Dobereiner’s triads also occurred in the
columns of Newlands’ octaves.
Dobereiner’s triads
Li Ca Cl
Na Sr Br
K Ba I
Newlands’ octaves
H Li Be B C N O
F Na Mg Al Si P S
Cl K Ca Cr Ti Mn Fe
Co and Ni Cu Zn Y In As Se
Br Rb Sr Ce and La Zr − −
6. 2
Question 2:
What were the limitations of Dobereiner’s classification?
Answer 2:
Limitation of Dobereiner’s classification:
All known elements could not be classified into groups of triads on the basis of their
properties.
Question 3:
What were the limitations of Newlands’ Law of Octaves?
Answer 3:
Limitations of Newlands’ law of octaves:
a) It was not applicable throughout the arrangements. It was applicable up to calcium
only. The properties of the elements listed after calcium showed no resemblance
to the properties of the elements above them.
b) Those elements that were discovered after Newlands’ octaves did not follow the
law of octaves.
c) The position of cobalt and nickel in the group of the elements (F, Cl) of different
properties could not be explained.
d) Placing of iron far away from cobalt and nickel, which have similar properties as
iron, could also not be explained.
7. 3
Page 85
Question 1:
Use Mendeleev’s Periodic Table to predict the formulae for the oxides of the following
elements: K, C, Al, Si, Ba.
Answer 1:
K is in group 1. Therefore, the oxide will be K2O.
C is in group 4. Therefore, the oxide will be CO2.
Al is in group 3. Therefore, the oxide will be Al2O3.
Si is in group 4. Therefore, the oxide will be SiO2.
Ba is in group 2. Therefore, the oxide will be BaO.
Question 2:
Besides gallium, which other elements have since been discovered that were left by
Mendeleev in his Periodic Table? (any two)
Answer 2:
Scandium and germanium
Question 3:
What were the criteria used by Mendeleev in creating his Periodic Table?
Answer 3:
Mendeleev’s periodic table was based on the observation that the properties of elements
are a periodic function of their atomic masses. This means that if elements are arranged
in the increasing order of their atomic masses, then their properties get repeated after
regular intervals.
Question 4:
Why do you think the noble gases are placed in a separate group?
Answer 4:
Noble gases are inert elements. Their properties are different from the all other elements.
Therefore, the noble gases are placed in a separate group.
8. 4
Page 90
Question 1:
How could the Modern Periodic Table remove various anomalies of Mendeleev’s Periodic
Table?
Answer 1:
Mendeleev was unable to give fixed position to hydrogen and isotopes in the periodic table.
In Mendeleev’s periodic table, the increasing manner of atomic mass of the elements is
not always regular from one to its next. It was believed that a more fundamental property
than atomic mass could explain periodic properties in a better manner.
It was Henry Moseley who demonstrated that atomic number of an element could explain
periodic properties in a better way than atomic mass of an element and arranged the
elements in increasing order of their atomic numbers. Then it was found that the various
anomalies of Mendeleev’s periodic table were removed by the modern periodic table.
Question 2:
Name two elements you would expect to show chemical reactions similar to magnesium.
What is the basis for your choice?
Answer 2:
Calcium (Ca) and strontium (Sr) are expected to show chemical reactions similar to
magnesium (Mg). This is because the number of valence electrons (2) is same in all these
three elements. And since chemical properties are due to valence electrons, they show
same chemical reactions.
Question 3:
Name
(a)three elements that have a single electron in their outermost shells.
(b)two elements that have two electrons in their outermost shells.
(c) three elements with filled outermost shells.
Answer 3:
(a)Lithium (Li), sodium (Na), and potassium (K) have a single electron in their outermost
shells.
(b)Magnesium (Mg) and calcium (Ca) have two electrons in their outermost shells.
(c) Neon (Ne), argon (Ar), and xenon (Xe) have filled outermost shells.
9. 5
Question 4:
(a)Lithium, sodium, potassium are all metals that react with water to liberate
hydrogen gas. Is there any similarity in the atoms of these elements?
(b)Helium is an unreactive gas and neon is a gas of extremely low reactivity. What, if
anything, do their atoms have in common?
Answer 4:
(a)Yes. The atoms of all the three elements lithium, sodium, and potassium have one
electron in their outermost shells.
(b)Both helium (He) and neon (Ne) have filled outermost shells. Helium has a duplet
in its K shell, while neon has an octet in its L shell.
Question 5:
In the Modern Periodic Table, which are the metals among the first ten elements?
Answer 5:
Among the first ten elements, lithium (Li) and beryllium (Be) are metals.
Question 6:
By considering their position in the Periodic Table, which one of the following elements
would you expect to have maximum metallic characteristic?
Ga, Ge, As, Se, Be
Answer 6:
Since Be lies to the extreme left hand side of the periodic table, Be is the most metallic
among the given elements.