This document provides an overview of carbon and organic chemistry topics. It discusses the structure and properties of carbon, including its ability to form covalent bonds and exist in different allotropes like diamond, graphite and buckminsterfullerene. Carbon's versatility is explained by its properties of catenation and tetravalency. The document outlines saturated and unsaturated hydrocarbons, and describes how carbon can form chains, branches and rings. Lewis structures are introduced as a way to represent bonding. Homologous series are defined as compounds with the same functional group substituting for hydrogen in a carbon chain.
Carbon has four electrons in its outer orbit giving it a valency of four. It is a non-metal that can form long chains by combining with itself, providing a backbone to which other atoms can attach in various ways. In nature, carbon exists as two allotropes, diamond and graphite, which differ physically in properties like appearance, hardness, and conductivity despite being chemically identical. Hydrocarbons are compounds of carbon and hydrogen that are the main component of petroleum, and include saturated compounds like alkanes as well as unsaturated compounds with double or triple bonds between carbons like alkenes and alkynes.
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in the vast number and variety of carbon compounds found in nature, including hydrocarbons.
This document discusses ionic theory and properties of salts. It recaps that salts consist of ions and ionic theory is used to explain properties like conductivity when molten or in solution. Atoms that prefer to lose electrons to become cations include metals like sodium, while atoms that prefer to gain electrons to become anions include nonmetals like chlorine. When sodium and chlorine react, sodium loses an electron to become Na+ while chlorine gains that electron to become Cl-, and the ions are held together by ionic bonds in solid sodium chloride.
This document provides an introduction to organic chemistry concepts. It discusses:
1. The history of organic chemistry and the distinction between organic and inorganic compounds.
2. Key concepts in atomic structure like atomic number, mass, isotopes and electronic configurations.
3. Bonding theories including ionic, covalent and molecular orbital theory. Concepts like sigma bonds, pi bonds and hybridization are explained.
4. Acid-base theories including Bronsted-Lowry definitions, pH, acid dissociation constants (Ka) and how structure affects acidity.
The document discusses the versatile nature of carbon. It notes that carbon can form various straight chain, branched chain, and ring structures due to its properties of catenation and tetravalency. This allows carbon to form a large variety of compounds that are exceptionally stable due to the strong carbon-carbon bond. Carbon can also form multiple bonds, leading to saturated and unsaturated compounds. Homologous series are discussed as are isomers that can result from carbon's catenation and tetravalency. The IUPAC nomenclature system for naming organic compounds is also summarized.
This document discusses hybrid orbital bonding theory. It explains that atomic orbitals alone cannot describe bonding in molecules like methane, where carbon forms four equivalent bonds arranged tetrahedrally. Carbon's atomic orbitals cannot account for this. The solution is that carbon's 2s and 3p orbitals hybridize to form four new equivalent sp3 hybrid orbitals oriented at 109.5 degrees, allowing carbon to form four sigma bonds to hydrogen in methane. Hybridization is determined by counting electron domains, with sp, sp2, and sp3 hybridization occurring for 2, 3, and 4 domains respectively. This model explains methane's bonding and tetrahedral structure.
This document provides an overview of carbon and organic chemistry topics. It discusses the structure and properties of carbon, including its ability to form covalent bonds and exist in different allotropes like diamond, graphite and buckminsterfullerene. Carbon's versatility is explained by its properties of catenation and tetravalency. The document outlines saturated and unsaturated hydrocarbons, and describes how carbon can form chains, branches and rings. Lewis structures are introduced as a way to represent bonding. Homologous series are defined as compounds with the same functional group substituting for hydrogen in a carbon chain.
Carbon has four electrons in its outer orbit giving it a valency of four. It is a non-metal that can form long chains by combining with itself, providing a backbone to which other atoms can attach in various ways. In nature, carbon exists as two allotropes, diamond and graphite, which differ physically in properties like appearance, hardness, and conductivity despite being chemically identical. Hydrocarbons are compounds of carbon and hydrogen that are the main component of petroleum, and include saturated compounds like alkanes as well as unsaturated compounds with double or triple bonds between carbons like alkenes and alkynes.
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in the vast number and variety of carbon compounds found in nature, including hydrocarbons.
This document discusses ionic theory and properties of salts. It recaps that salts consist of ions and ionic theory is used to explain properties like conductivity when molten or in solution. Atoms that prefer to lose electrons to become cations include metals like sodium, while atoms that prefer to gain electrons to become anions include nonmetals like chlorine. When sodium and chlorine react, sodium loses an electron to become Na+ while chlorine gains that electron to become Cl-, and the ions are held together by ionic bonds in solid sodium chloride.
This document provides an introduction to organic chemistry concepts. It discusses:
1. The history of organic chemistry and the distinction between organic and inorganic compounds.
2. Key concepts in atomic structure like atomic number, mass, isotopes and electronic configurations.
3. Bonding theories including ionic, covalent and molecular orbital theory. Concepts like sigma bonds, pi bonds and hybridization are explained.
4. Acid-base theories including Bronsted-Lowry definitions, pH, acid dissociation constants (Ka) and how structure affects acidity.
The document discusses the versatile nature of carbon. It notes that carbon can form various straight chain, branched chain, and ring structures due to its properties of catenation and tetravalency. This allows carbon to form a large variety of compounds that are exceptionally stable due to the strong carbon-carbon bond. Carbon can also form multiple bonds, leading to saturated and unsaturated compounds. Homologous series are discussed as are isomers that can result from carbon's catenation and tetravalency. The IUPAC nomenclature system for naming organic compounds is also summarized.
This document discusses hybrid orbital bonding theory. It explains that atomic orbitals alone cannot describe bonding in molecules like methane, where carbon forms four equivalent bonds arranged tetrahedrally. Carbon's atomic orbitals cannot account for this. The solution is that carbon's 2s and 3p orbitals hybridize to form four new equivalent sp3 hybrid orbitals oriented at 109.5 degrees, allowing carbon to form four sigma bonds to hydrogen in methane. Hybridization is determined by counting electron domains, with sp, sp2, and sp3 hybridization occurring for 2, 3, and 4 domains respectively. This model explains methane's bonding and tetrahedral structure.
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
This document discusses the formation of ionic bonds between ions. Ionic bonds are electrostatic attractions between oppositely charged ions. Cations are positively charged ions formed when metals lose electrons. Anions are negatively charged ions formed when nonmetals gain electrons. Ionic bonds generally form between metallic cations and nonmetallic anions. The document provides examples of common cations and anions and identifies metals, nonmetals, and metalloids on the periodic table.
This document provides an overview of chapters 8 and 9 which cover bonding and molecular structure, and orbital hybridization. It discusses how Lewis dot structures, molecular geometry, polarity, hybridization, and sigma/pi bonding will be taught through a PowerPoint presentation and learning module. Key points covered include how to draw Lewis dot structures, identify molecular geometry using VSEPR theory, determine polarity, and identify hybridization. Examples are provided for common molecular structures like methane, water, carbon dioxide and more. The document emphasizes that hybridization is needed to explain the uniform bond lengths and angles observed in methane.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
X chem ch4_carbon_anditscompounds_topconceptsAkshay Fegade
1. The document discusses carbon and its compounds, specifically covalent bonds and covalent compounds. It describes the conditions for covalent bond formation and properties of covalent compounds like physical states, solubility, and electrical conductivity.
2. Key concepts include that carbon forms covalent bonds and a large number of compounds due to its tetravalency and ability to catenate. Carbon can form single, double, or triple bonds. Lewis dot structures are used to represent covalent bonding.
3. Hydrocarbons are classified as aliphatic or aromatic. Nomenclature and isomerism of hydrocarbons are also covered. Homologous series have a general molecular formula where successive members differ by -CH
Carbon being the most versatile element on this earth is also the most important element for mankind. Carbon (from Latin: carbo "coal") is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Carbon makes up only about 0.025 percent of Earth's crust.
This document discusses covalent bonding and molecular structures. It defines covalent bonds as bonds formed by shared electron pairs between atoms. It explains that molecules are groups of atoms held together by covalent bonds in a specific ratio and shape. The document discusses drawing Lewis dot structures and molecular diagrams to represent molecules and the bonding between their atoms. It provides examples of drawing the Lewis dot structure for carbon tetrachloride and matching molecular diagrams to chemical formulas.
1) Alkenes are unsaturated hydrocarbons that contain carbon-carbon double bonds. They can be converted to alkanes by adding hydrogen.
2) The simplest alkene is ethylene (C2H4), which contains a carbon-carbon double bond. Its structure is similar to ethane.
3) Alkene reactions typically involve the breaking of the weaker carbon-carbon pi bond and formation of two new carbon-atom bonds through addition reactions like hydrogenation, halogenation, hydration, and dimerization.
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
Chlorine atoms each have 7 electrons and need 1 more to achieve a stable configuration of 8 electrons. When two chlorine atoms bond, they share one pair of electrons to each gain the 1 electron needed. This forms a chlorine molecule, Cl2, held together by a single covalent bond with each chlorine atom achieving stable electron configuration.
This document discusses covalent bonding and molecular structures. It defines covalent bonds as bonds formed by the sharing of electron pairs between atoms. It explains that molecules are groups of atoms held together by covalent bonds, and that their structures can be represented through chemical formulas, structural diagrams, and Lewis dot diagrams. It provides examples of how to determine the elements and numbers of each from a chemical formula, and how to draw Lewis dot diagrams of molecules by matching atoms to reach full valence shells.
1) Chemical bonds can be either ionic or covalent. Ionic bonds form when electrons are transferred between metals and non-metals to form ions. Covalent bonds form when electrons are shared between non-metals.
2) Sodium chloride forms when sodium donates an electron to chlorine to form ions that are attracted in an ionic bond. Hydrogen molecule forms when hydrogen atoms share an electron pair in a single covalent bond.
3) Ionic compounds have high melting points, conduct electricity when molten or dissolved, and dissolve in water but not organic solvents. Covalent compounds have lower melting points, do not conduct electricity, and dissolve in organic solvents but not water.
The document summarizes key concepts from a chapter on the periodic table, including:
1) It traces the historical development of the periodic table from early classifications of elements by their properties to Dobereiner's discovery of triads of elements and eventual development of the modern periodic table by Mendeleev and Moseley's organization by atomic number.
2) It explains how to read information from the periodic table such as the atomic number, name, and mass of elements as well as trends in various properties that are illustrated in the organization of the table.
3) It describes periodic trends in properties including atomic radius, ionization energy, electron affinity, and electronegativity that help explain elements' chemical behaviors
This document discusses how to determine if an atom is a metal or non-metal based on its valence electrons, and describes the formation of ionic and covalent bonds. Ionic bonds form between metal and non-metal atoms through the transfer of electrons from the metal to the non-metal. Covalent bonds form between non-metal atoms through the sharing of electrons. Examples of ionic bond formation in sodium chloride and covalent bond formation in carbon dioxide are provided, along with electron diagrams to illustrate bonding.
1. The document discusses atomic structure and bonding. It describes the structure of atoms in terms of electrons and the nucleus containing protons and neutrons. It also discusses the arrangement of electrons in shells and the significance of noble gas structures and valency electrons.
2. The document then covers the periodic table and periodic trends. It defines properties such as atomic number, mass number, and isotopes. It explains how the periodic table is arranged based on these properties and how elements in the same group have similar properties.
3. The types of bonding are described including ionic bonding between metals and non-metals which forms ionic lattices, and covalent bonding between non-metals which forms molecules by sharing electron
This document provides an introduction to carbon and its compounds. It discusses that carbon has the unique property of combining with itself and other elements, forming many compounds. It can form single, double, and triple covalent bonds. Based on their structure and bonding, hydrocarbons are classified as aliphatic or aromatic. Alkanes contain only single bonds, alkenes contain double bonds, and alkynes contain triple bonds. The document also mentions that homologous series of these compounds will be covered in the next class.
Chapter 6.3 : Ionic Bonding and Ionic CompoundsChris Foltz
Ionic compounds are composed of positive and negative ions in ratios that balance the charges. They form crystalline lattices with ions arranged in an orderly pattern. The ions are held together by strong electrostatic forces called lattice energy. Ionic compounds have high melting and boiling points, are hard and brittle, and conduct electricity when molten or dissolved but not in the solid state. Polyatomic ions are charged groups of covalently bonded atoms that behave as single ions in ionic compounds.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
1. Carbon exists in three allotropic forms: diamond, graphite, and fullerenes.
2. Diamond is extremely hard due to its rigid, three-dimensional covalent network structure where each carbon atom is bonded to four others in a tetrahedral shape. It is formed under high temperature and pressure deep in the Earth.
3. Diamond has many uses such as cutting, grinding, drilling, and jewelry due to its properties including hardness, high melting point, thermal conductivity, and brilliance when cut and polished. Synthetic diamonds are also produced for industrial applications.
Silicates are inorganic polymers formed through the catenation of chemical bonds. They are typically solids in the form of crystals, such as diamond, graphite, and materials where all atoms are connected by covalent bonds. Zeolites are aluminosilicates that incorporate cations like sodium or potassium to balance the negative charge from aluminium replacing some silicon atoms in the three-dimensional network structure. Silicates are widely used in industries like petrochemicals for cracking hydrocarbons and isomerization.
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in a huge number and variety of carbon compounds known as hydrocarbons.
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
This document discusses the formation of ionic bonds between ions. Ionic bonds are electrostatic attractions between oppositely charged ions. Cations are positively charged ions formed when metals lose electrons. Anions are negatively charged ions formed when nonmetals gain electrons. Ionic bonds generally form between metallic cations and nonmetallic anions. The document provides examples of common cations and anions and identifies metals, nonmetals, and metalloids on the periodic table.
This document provides an overview of chapters 8 and 9 which cover bonding and molecular structure, and orbital hybridization. It discusses how Lewis dot structures, molecular geometry, polarity, hybridization, and sigma/pi bonding will be taught through a PowerPoint presentation and learning module. Key points covered include how to draw Lewis dot structures, identify molecular geometry using VSEPR theory, determine polarity, and identify hybridization. Examples are provided for common molecular structures like methane, water, carbon dioxide and more. The document emphasizes that hybridization is needed to explain the uniform bond lengths and angles observed in methane.
The document summarizes key information about atomic structure:
- The nucleus is positively charged and contains nearly all an atom's mass, while electrons are much smaller and negatively charged, orbiting in shells outside the nucleus.
- Electrons are arranged in shells (also called energy levels) around the nucleus, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- Atoms can be represented using Bohr models that show the nucleus and electrons arranged in shells, with the number of protons and neutrons indicated in the nucleus.
X chem ch4_carbon_anditscompounds_topconceptsAkshay Fegade
1. The document discusses carbon and its compounds, specifically covalent bonds and covalent compounds. It describes the conditions for covalent bond formation and properties of covalent compounds like physical states, solubility, and electrical conductivity.
2. Key concepts include that carbon forms covalent bonds and a large number of compounds due to its tetravalency and ability to catenate. Carbon can form single, double, or triple bonds. Lewis dot structures are used to represent covalent bonding.
3. Hydrocarbons are classified as aliphatic or aromatic. Nomenclature and isomerism of hydrocarbons are also covered. Homologous series have a general molecular formula where successive members differ by -CH
Carbon being the most versatile element on this earth is also the most important element for mankind. Carbon (from Latin: carbo "coal") is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Carbon makes up only about 0.025 percent of Earth's crust.
This document discusses covalent bonding and molecular structures. It defines covalent bonds as bonds formed by shared electron pairs between atoms. It explains that molecules are groups of atoms held together by covalent bonds in a specific ratio and shape. The document discusses drawing Lewis dot structures and molecular diagrams to represent molecules and the bonding between their atoms. It provides examples of drawing the Lewis dot structure for carbon tetrachloride and matching molecular diagrams to chemical formulas.
1) Alkenes are unsaturated hydrocarbons that contain carbon-carbon double bonds. They can be converted to alkanes by adding hydrogen.
2) The simplest alkene is ethylene (C2H4), which contains a carbon-carbon double bond. Its structure is similar to ethane.
3) Alkene reactions typically involve the breaking of the weaker carbon-carbon pi bond and formation of two new carbon-atom bonds through addition reactions like hydrogenation, halogenation, hydration, and dimerization.
The document discusses ionic bonding between metals and non-metals. Ionic bonding occurs when metals give up electrons to form positive ions and non-metals gain electrons to form negative ions. The positive and negative ions are then attracted to each other, forming an ionic compound. Metals are usually found on the left side of the periodic table and easily give up valence electrons. Non-metals are usually on the right side and readily gain electrons to achieve a full valence shell. When ions form, they arrange in a crystalline lattice structure with positive and negative ions alternating. Ionic compounds have properties like being crystalline solids, having high melting points, and being able to conduct electricity when melted or
Chlorine atoms each have 7 electrons and need 1 more to achieve a stable configuration of 8 electrons. When two chlorine atoms bond, they share one pair of electrons to each gain the 1 electron needed. This forms a chlorine molecule, Cl2, held together by a single covalent bond with each chlorine atom achieving stable electron configuration.
This document discusses covalent bonding and molecular structures. It defines covalent bonds as bonds formed by the sharing of electron pairs between atoms. It explains that molecules are groups of atoms held together by covalent bonds, and that their structures can be represented through chemical formulas, structural diagrams, and Lewis dot diagrams. It provides examples of how to determine the elements and numbers of each from a chemical formula, and how to draw Lewis dot diagrams of molecules by matching atoms to reach full valence shells.
1) Chemical bonds can be either ionic or covalent. Ionic bonds form when electrons are transferred between metals and non-metals to form ions. Covalent bonds form when electrons are shared between non-metals.
2) Sodium chloride forms when sodium donates an electron to chlorine to form ions that are attracted in an ionic bond. Hydrogen molecule forms when hydrogen atoms share an electron pair in a single covalent bond.
3) Ionic compounds have high melting points, conduct electricity when molten or dissolved, and dissolve in water but not organic solvents. Covalent compounds have lower melting points, do not conduct electricity, and dissolve in organic solvents but not water.
The document summarizes key concepts from a chapter on the periodic table, including:
1) It traces the historical development of the periodic table from early classifications of elements by their properties to Dobereiner's discovery of triads of elements and eventual development of the modern periodic table by Mendeleev and Moseley's organization by atomic number.
2) It explains how to read information from the periodic table such as the atomic number, name, and mass of elements as well as trends in various properties that are illustrated in the organization of the table.
3) It describes periodic trends in properties including atomic radius, ionization energy, electron affinity, and electronegativity that help explain elements' chemical behaviors
This document discusses how to determine if an atom is a metal or non-metal based on its valence electrons, and describes the formation of ionic and covalent bonds. Ionic bonds form between metal and non-metal atoms through the transfer of electrons from the metal to the non-metal. Covalent bonds form between non-metal atoms through the sharing of electrons. Examples of ionic bond formation in sodium chloride and covalent bond formation in carbon dioxide are provided, along with electron diagrams to illustrate bonding.
1. The document discusses atomic structure and bonding. It describes the structure of atoms in terms of electrons and the nucleus containing protons and neutrons. It also discusses the arrangement of electrons in shells and the significance of noble gas structures and valency electrons.
2. The document then covers the periodic table and periodic trends. It defines properties such as atomic number, mass number, and isotopes. It explains how the periodic table is arranged based on these properties and how elements in the same group have similar properties.
3. The types of bonding are described including ionic bonding between metals and non-metals which forms ionic lattices, and covalent bonding between non-metals which forms molecules by sharing electron
This document provides an introduction to carbon and its compounds. It discusses that carbon has the unique property of combining with itself and other elements, forming many compounds. It can form single, double, and triple covalent bonds. Based on their structure and bonding, hydrocarbons are classified as aliphatic or aromatic. Alkanes contain only single bonds, alkenes contain double bonds, and alkynes contain triple bonds. The document also mentions that homologous series of these compounds will be covered in the next class.
Chapter 6.3 : Ionic Bonding and Ionic CompoundsChris Foltz
Ionic compounds are composed of positive and negative ions in ratios that balance the charges. They form crystalline lattices with ions arranged in an orderly pattern. The ions are held together by strong electrostatic forces called lattice energy. Ionic compounds have high melting and boiling points, are hard and brittle, and conduct electricity when molten or dissolved but not in the solid state. Polyatomic ions are charged groups of covalently bonded atoms that behave as single ions in ionic compounds.
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
1. Carbon exists in three allotropic forms: diamond, graphite, and fullerenes.
2. Diamond is extremely hard due to its rigid, three-dimensional covalent network structure where each carbon atom is bonded to four others in a tetrahedral shape. It is formed under high temperature and pressure deep in the Earth.
3. Diamond has many uses such as cutting, grinding, drilling, and jewelry due to its properties including hardness, high melting point, thermal conductivity, and brilliance when cut and polished. Synthetic diamonds are also produced for industrial applications.
Silicates are inorganic polymers formed through the catenation of chemical bonds. They are typically solids in the form of crystals, such as diamond, graphite, and materials where all atoms are connected by covalent bonds. Zeolites are aluminosilicates that incorporate cations like sodium or potassium to balance the negative charge from aluminium replacing some silicon atoms in the three-dimensional network structure. Silicates are widely used in industries like petrochemicals for cracking hydrocarbons and isomerization.
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in a huge number and variety of carbon compounds known as hydrocarbons.
Allotropes of carbon
Carbon is capable of forming many allotropes due to its valency. Well known forms of carbon include diamond and graphite. In recent decades many more allotropes and forms of carbon have been discovered and researched including ball shapes such as buckminsterfullerene and sheets such as graphene. Larger scale structures of carbon include nanotubes, nanobuds and nanoribbons. Other unusual forms of carbon exist at very high temperature or extreme pressures.
The document provides instructions for laboratory experiments and activities related to carbon chemistry and organic chemistry. In carbon chemistry, students will make models of carbon allotropes, describe the greenhouse effect, prepare carbon dioxide in the laboratory, and describe the carbon cycle. In organic chemistry, students will name and draw alkanes, explain trends in alkane melting and boiling points, describe fractional distillation of alkanes, and write combustion equations. Additional experiments include drawing and naming alkenes and writing polymerization equations.
Carbon is a nonmetal that is the fourth most abundant element in the human body and is essential to life. It has several allotropes including diamond, graphite, and buckminsterfullerene. Carbon forms covalent bonds and can bond to other carbon atoms to form chains, rings, and complex molecules. Many organic compounds are based on carbon chains and rings that may be saturated or unsaturated. Carbon undergoes many important reactions including combustion, oxidation, and substitution reactions.
Carbon is a fundamental building block of life and forms millions of known compounds due to its properties of catenation, tetravalency, and isomerism. Carbon has multiple allotropes including diamond, graphite, and buckministerfullerene that differ in how carbon atoms are bonded. Diamond has carbon atoms bonded in a rigid 3D structure while graphite has layers of hexagonal arrays with double and single bonds between carbon atoms in each layer.
Class 10 chemistry Carbon and its compounds.pdfankitrajak629
Carbon is a unique element that can form large numbers of compounds. It has four valence electrons and forms covalent bonds, allowing it to link together in chains, branches, and rings. There are three main allotropes of carbon: diamond, graphite, and fullerene. Diamond has a three-dimensional crystalline structure that makes it very hard, while graphite has stacked hexagonal layers that allow for conductivity. Carbon forms the basis of all known life and many important compounds like fuels, plastics, and organic chemicals.
This presentation is prepared in view of engineering chemistry syllabus. It is useful for Engineering, Sciences and their research to understand basics of chemistry.
Carbon belongs to the group IV of
the periodic table.
◼ It has four electrons in its
outermost orbit, so its valency is
four.
◼ Carbon is a non-metal.
Physical properties of Diamond and graphite, hydrocarbon, long chain carbon, bonds of carbon all details are provided in this file.
This document discusses carbon and its compounds. It notes that carbon has four valence electrons and can form long chains, allowing it to combine with many other elements. This results in a vast number of carbon compounds in nature. Specifically, it discusses the allotropes of carbon - diamond and graphite. While chemically identical, they have very different physical properties due to variations in atomic arrangement. Hydrocarbons, compounds of carbon and hydrogen, are also discussed. The simplest, methane, is examined as are saturated hydrocarbons called alkanes and unsaturated versions like alkenes and alkynes.
Coordinate covalent bonds involve one atom contributing both electrons to form a bond that cannot be distinguished from a regular covalent bond. Metallic bonds are depicted by the electron sea model where positive metal ions are immersed in a sea of delocalized and mobile electrons. Network covalent solids have atoms bonded covalently forming very hard, high melting point materials that are poor conductors such as diamond. Allotropes of carbon include diamond, graphite, amorphous carbon, fullerenes, carbon nanotubes, buckyballs, and lonsdaleite which each have different bonding structures and properties.
carbon and its compound by Gagan prasadGagan Prasad
Gagan Prasad completed a PowerPoint presentation about carbon and its compounds under the guidance of Miss Anshu. The presentation covered the basic properties of carbon, different allotropes of carbon including graphite and diamond, hydrocarbon classifications including saturated and unsaturated hydrocarbons, functional groups in organic chemistry, and examples of alkanes from methane to hexane. The document provided information on the fundamental chemistry concepts relating to carbon.
Carbon and its Compounds, Class 10 Overview:
In the realm of chemistry, carbon stands as a versatile and unparalleled element, forming the cornerstone of organic compounds. This branch of chemistry explores the structure, properties, and reactions of carbon-containing compounds. Here's a brief insight into the key aspects covered in Class 10:
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Carbon is a nonmetallic element that can form four covalent bonds. It exists in several allotropes including graphite, diamond, and fullerenes. Hydrocarbons are organic compounds made of only carbon and hydrogen. Saturated hydrocarbons have only single bonds between carbon atoms while unsaturated hydrocarbons have double or triple bonds. The structure and properties of hydrocarbons depend on the number of carbon atoms and their arrangement in chains, branches, or rings. Functional groups are specific atomic groups that determine a molecule's chemical reactivity.
Carbon exhibits the unique property of catenation, which is the ability to form long chains by bonding with other carbon atoms. Carbon forms tetravalent covalent bonds that allow it to link up with many other carbon atoms. This catenation property is responsible for the vast variety of organic compounds found in nature. Carbon's small size, high bond energy, tetravalency, and orbital structure promote strong bonding that results in its exceptional ability to form complex cyclic and chain structures through catenation.
Myself being as a class 10 CBSE student; I understand the difficulties faced by the students.
so refer this presentation to have a well understanding over a difficult chapter.
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Carbon is a non-metal that forms more compounds than any other element. It can form long chains and attach to other atoms due to its unique ability to bond with itself. Pure carbon exists in two allotropes, diamond and graphite, which have identical chemical composition but different physical properties due to variations in atomic structure. Hydrocarbons are compounds of carbon and hydrogen, including saturated alkanes and unsaturated alkenes and alkynes, with alkenes containing double bonds and alkynes containing triple bonds between carbon atoms.
This document is a PowerPoint presentation on carbon and its compounds submitted by a student group. It provides information on carbon including that it is a nonmetallic element with an atomic number of 6 that forms covalent bonds. It discusses the origin of carbon in nature, the reasons for its versatility including catenation and tetracovalency. The presentation also covers different forms of carbon including graphite, diamond and fullerenes as well as saturated and unsaturated compounds. It provides examples of functional groups and homologous series and discusses chemical properties and uses of carbon compounds.
Similar to Carbon and it's compounds - part 2 (20)
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
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.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
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.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
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.
Executive Directors Chat Leveraging AI for Diversity, Equity, and InclusionTechSoup
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
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Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
3. Now, are you ready
for class??
Rotate your wrist
slowly-slowly in
clockwise and
anticlockwise
directions.
Find your seat
Bell Ringer
As you come in and get settled, follow these
instructions:
6. In this topic the students will learn about the
allotropic forms of the carbon i.e. why does carbon
exist in different forms? Why does graphite has
planner structure? Why it has a special property
among all other elements present in periodic table?
7. Core Skills
Carbon is a special element of the periodic table. It forms a
large number of compound due to its special behaviour of
catenation. Mostly organic compound which are present in
plants and animals have carbon atom as a main constituent.
According to vial force theory the organic compound were
synthesized in plant and animals only.
10. Allotropy - The phenomenon in which the element exists in two
or more different physical states with similar chemical properties
and different physical properties are called allotropes and this
phenomenon is called allotropy.
Carbon has three main allotropes
*Diamond
*Graphite
*Fullerene
11. Diamond - In diamond, each carbon atom is bonded to
the four other atoms of carbon forming three-dimensional
structures. It is the hardest substance and an insulator. It
is used for drilling rocks and cutting of glass. It is also used
for making jewellery.
12. Graphite - In graphite, each carbon atom is bonded to three
other carbon atoms. Ach carbon atom in graphite has one free
electron due to which graphite acts as a good conductor of heat and
electricity. It exists in layered form. These layers are held together by
weak vander Waal’s forces. These forces are very facile so graphite
acts as lubricant in heavy machines. It is also used in Gas-masks,
Pencils, to make electrodes of dry cells, in metallurgical processes, as
a neutron moderator in nuclear reactors, electrical contacts etc.
14. Buckminster Fullerene – Fullerene are spherical in
shape or has a soccer ball like structure which is hollow
from inside. The first fullerene identified was C-60 with 60
carbon atoms arranged in a football like structure. C-60 has
20 hexagonal and 12 pentagonal rings. It was discovered by
Buckminster Fuller, hence these are also known as
Buckminster Fullerenes or Bucky Balls.
16. Differences between Diamond and Graphite
Diamond is the hardest substance whereas graphite is very soft.
Diamond is used for grinding and polishing of ‘hard materials
and graphite is used as a lubricant.
Diamond has a three-dimensional rigid structure but graphite
has a hexagonal sheet layer structure.
Diamond is a bad conductor of electricity but graphite is a very
good conductor of electricity.
17. Versatile Nature of Carbon: The existence of such a large
number of organic compounds is due to the following nature of
carbon,
Catenation
Tetravalency
(i)Catenation: The self-linking property of carbon atom through
covalent bonds to form long straight, branched and rings of
different sizes is called Catenation. This property is due to –
18. a.The small size of the carbon atom.
b.The great strength of the carbon-carbon bond.
c. Carbon can also form stable multiple bonds (double or triple)
with itself and with the atoms of other elements.
Straight chain
21. Tetravalent Nature: Carbon has valency of four. It is
capable of bonding with four other atoms of carbon or
some other heteroatoms with single covalent bond as well
as double or triple bond.
23. Mark the correct answer –
Which of the following is used as a fuel in cars
along with petrol?
A. Methane
B. Ethane
C. Butane
D. Ethanol
24. Mark the correct answer –
Cation is formed when:
a) Atom gains electrons
b) Atom loses electrons
c) Proton is lost by the atom
d) Atom shares electrons