Bond formation (l3)
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This document discusses different types of bonds: ionic bonds, covalent bonds, and the structures that represent them. Ionic bonds are electrostatic attractions between oppositely charged ions, formed when a metal transfers electrons to a nonmetal. Covalent bonds involve the sharing of electron pairs between atoms. Lewis structures use dots to represent valence electrons and show how atoms are arranged and bonded in molecules through single, double or triple bonds to achieve stable octets. Resonance structures depict alternative but equally valid Lewis structures for some molecules.
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bonding
This document discusses several topics related to chemical bonding:
Covalent bonding occurs when atoms share valence electrons to form stable molecular structures. Lewis structures use dots to represent these shared and unshared electron pairs, following the octet rule which states that atoms seek a full outer shell of 8 electrons. Exceptions exist for some atoms. Polar covalent bonds form when electrons are unequally shared between atoms, resulting in a partial positive and negative charge.
Ionic bond
Ionic bonds form between oppositely charged ions. They result from the transfer of electrons from one atom to another. Ionic bonding typically occurs between metals and nonmetals. Metals tend to lose electrons to fill their outer shell, becoming positively charged ions, while nonmetals gain electrons to fill their outer shell, becoming negatively charged ions. The electrostatic attraction between the opposite charges of the ions forms the ionic bond.
Covalent bond
This document defines covalent bonding and discusses different types of covalent bonds. It provides examples of covalent bonds in molecules like H2O and H2. The types of covalent bonds covered are single, double, and triple bonds. Covalent bonds are also classified as polar or nonpolar depending on differences in electronegativity. Key properties of covalent compounds discussed are low melting and boiling points, poor electrical conductivity, flammability for those containing carbon and hydrogen, and soft or brittle solid forms.
Chemical bonding
Chemical bonding is the force of attraction between atoms that allows for the formation of molecules. There are two main types of chemical bonds: covalent bonds, which involve the sharing of valence electrons between atoms, and ionic bonds, which involve the transfer of electrons from one atom to another. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Lewis dot structures use dots to represent valence electrons and show atomic configurations.
Types Of Chemical Bonds- Ionic Bond,Covalent Bonds,Coordinate Bonds, Basic In...
The document discusses different types of chemical bonds formed by atoms to achieve stable inert gas electronic configurations:
1) Ionic bonds occur through complete electron transfer between atoms, making one positively charged and one negatively charged. The ions are then held together by electrostatic attraction.
2) Covalent bonds involve sharing of electrons between atoms of similar electronegativity to attain stable configurations.
3) Coordinate bonds are a type of covalent bond where both shared electrons are donated by one atom to an acceptor atom in need of electrons.
covalent bond
This document discusses properties and uses of covalent compounds. It states that covalent compounds generally have lower melting and boiling points than ionic compounds. They are also more flexible, flammable, and less soluble in water than ionic compounds. The document notes that many fuels, medicines, clothes, and foods contain covalent bonds. It provides examples such as fuels powering daily life and clothes made from covalent materials. Covalent compounds share electrons between nonmetal atoms rather than transferring electrons.
Covalent Bonds
This document describes different types of covalent bonding, including:
1) Covalent bonds form when electron pairs are shared between two atoms, attracting their nuclei together.
2) Covalent compounds are usually composed of nonmetals and include many familiar substances like water and methane.
3) Dot and cross diagrams can represent covalent bonds, showing shared electron pairs between atoms.
Chemical bonding
This document discusses different types of chemical bonding: ionic bonding which involves the transfer of electrons between metals and non-metals and results in charged atoms attracting each other; covalent bonding which involves the sharing of electron pairs between atoms and can result in simple molecular or giant molecular structures; and metallic bonding which occurs between delocalized electrons in metal ions and positively charged metal ions. Each type of bonding is described along with examples and properties such as conductivity, melting/boiling points, and solubility.
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bonding
This document discusses several topics related to chemical bonding:
Covalent bonding occurs when atoms share valence electrons to form stable molecular structures. Lewis structures use dots to represent these shared and unshared electron pairs, following the octet rule which states that atoms seek a full outer shell of 8 electrons. Exceptions exist for some atoms. Polar covalent bonds form when electrons are unequally shared between atoms, resulting in a partial positive and negative charge.
Ionic bond
Ionic bonds form between oppositely charged ions. They result from the transfer of electrons from one atom to another. Ionic bonding typically occurs between metals and nonmetals. Metals tend to lose electrons to fill their outer shell, becoming positively charged ions, while nonmetals gain electrons to fill their outer shell, becoming negatively charged ions. The electrostatic attraction between the opposite charges of the ions forms the ionic bond.
Covalent bond
This document defines covalent bonding and discusses different types of covalent bonds. It provides examples of covalent bonds in molecules like H2O and H2. The types of covalent bonds covered are single, double, and triple bonds. Covalent bonds are also classified as polar or nonpolar depending on differences in electronegativity. Key properties of covalent compounds discussed are low melting and boiling points, poor electrical conductivity, flammability for those containing carbon and hydrogen, and soft or brittle solid forms.
Chemical bonding
Chemical bonding is the force of attraction between atoms that allows for the formation of molecules. There are two main types of chemical bonds: covalent bonds, which involve the sharing of valence electrons between atoms, and ionic bonds, which involve the transfer of electrons from one atom to another. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Lewis dot structures use dots to represent valence electrons and show atomic configurations.
Types Of Chemical Bonds- Ionic Bond,Covalent Bonds,Coordinate Bonds, Basic In...
The document discusses different types of chemical bonds formed by atoms to achieve stable inert gas electronic configurations:
1) Ionic bonds occur through complete electron transfer between atoms, making one positively charged and one negatively charged. The ions are then held together by electrostatic attraction.
2) Covalent bonds involve sharing of electrons between atoms of similar electronegativity to attain stable configurations.
3) Coordinate bonds are a type of covalent bond where both shared electrons are donated by one atom to an acceptor atom in need of electrons.
covalent bond
This document discusses properties and uses of covalent compounds. It states that covalent compounds generally have lower melting and boiling points than ionic compounds. They are also more flexible, flammable, and less soluble in water than ionic compounds. The document notes that many fuels, medicines, clothes, and foods contain covalent bonds. It provides examples such as fuels powering daily life and clothes made from covalent materials. Covalent compounds share electrons between nonmetal atoms rather than transferring electrons.
Covalent Bonds
This document describes different types of covalent bonding, including:
1) Covalent bonds form when electron pairs are shared between two atoms, attracting their nuclei together.
2) Covalent compounds are usually composed of nonmetals and include many familiar substances like water and methane.
3) Dot and cross diagrams can represent covalent bonds, showing shared electron pairs between atoms.
Chemical bonding
This document discusses different types of chemical bonding: ionic bonding which involves the transfer of electrons between metals and non-metals and results in charged atoms attracting each other; covalent bonding which involves the sharing of electron pairs between atoms and can result in simple molecular or giant molecular structures; and metallic bonding which occurs between delocalized electrons in metal ions and positively charged metal ions. Each type of bonding is described along with examples and properties such as conductivity, melting/boiling points, and solubility.
Bonding and Structure
The document discusses different types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between metals and non-metals to form ions. Covalent bonding involves the sharing of electron pairs between non-metals. Metallic bonding involves a sea of delocalized electrons that are attracted to cationic metal ions arranged in a lattice. Each type of bonding results in different material properties depending on whether electrons are transferred, shared, or free to move.
Covalent bonds
Covalent bonds result from the sharing of valence electrons between two nonmetallic atoms. A single covalent bond forms when one pair of electrons is shared, while double and triple bonds share two or three pairs of electrons, respectively. Molecular structure and bond angles are determined by the VSEPR model, which predicts molecular geometry based on electron pair repulsion. Hybridization occurs when atomic orbitals mix to form new hybrid orbitals and explain molecular bonding orientations.
Bond Formation (Ionic, Covalent, and Metallic Bonding)
Chemical bonds form between atoms to stabilize their outer electron shells. There are three main types of bonds: ionic bonds form when electrons are transferred between atoms, covalent bonds form when electrons are shared between atoms, and metallic bonds form from the delocalized "sea" of electrons in metal atoms. Ionic bonds result in oppositely charged ions, covalent bonds can be single, double or triple depending on electron pairs shared, and metallic bonding gives metals their conductivity. Compounds are classified as ionic, covalent or metallic based on the type of bonding between their atoms.
Covalent bond
This document defines and provides examples of covalent bonds. It discusses the history of the term being coined by Irving Langmuir in 1919. A covalent bond is defined as a chemical link where electrons are shared between two atoms. Examples given are the covalent bonds between oxygen and hydrogen in H2O and between hydrogen atoms in H2. The document also describes the different types of covalent bonds - single, double, and triple - based on the number of electron pairs shared between the bonded atoms.
Ionic Bond
Ionic bonds form when oppositely charged ions attract each other. They are strong but non-directional bonds. Ionic bonds form when there is a large difference in electronegativity between atoms. Cations form when atoms lose electrons and anions form when atoms gain electrons. Ionic solids have high melting points and are insoluble in non-polar solvents due to their strong electrostatic attractions.
Bonding and structure powerpoint
This document provides information on ionic and covalent bonding. It discusses how ionic bonding occurs through the transfer of electrons from metal to non-metal atoms, giving each atom a stable electron configuration. Ions are held together by electrostatic attraction in a lattice structure. Covalent bonding occurs through the sharing of electrons between non-metal atoms to achieve a stable electron configuration. Covalent structures can be either simple molecules or giant molecular structures held together by strong covalent bonds. The document also discusses allotropes such as diamond and graphite which are different structural forms of the same element.
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The document discusses covalent bonding, which involves the sharing of electron pairs between atoms. It defines covalent bonding and explains that it usually forms between non-metals and can result in sigma or pi bonds depending on orbital overlapping. The document also describes different types of covalent bonds including single, double, triple, polar, non-polar, and dative bonds. Examples are provided for each bond type.
Chemical bonds
This document discusses chemical bonds, specifically ionic and covalent bonds. It explains that ionic bonds are formed through the transfer of electrons between metal and non-metal atoms, resulting in oppositely charged ions that are attracted to one another. Covalent bonds are formed through the sharing of electron pairs between non-metal atoms. Key differences between ionic and covalent compounds are discussed, such as ionic compounds existing as solids and conducting electricity when molten or dissolved, while covalent compounds can be solids, liquids or gases and do not conduct electricity.
Covalent bonds
Covalent bonds occur when atoms share pairs of electrons to form molecules. Atoms form covalent bonds by sharing unpaired valence electrons, with examples being water (H2O) forming two covalent bonds and molecular oxygen (O2) forming a double covalent bond by sharing two pairs of electrons. Properties of covalent bonds include low melting and boiling points with poor conductivity.
Covalent bond
A covalent bond involves the sharing of electron pairs between atoms. There are two types of covalent bonding: non-polar, with equal sharing, and polar, with unequal sharing. A non-polar bond forms between like atoms that share electrons equally, while a polar bond forms between different atoms where one atom attracts the electrons more than the other due to differing electronegativity. Examples of non-polar molecules are H2, Cl2, and O2, where the atoms share electrons equally. Examples of polar molecules are HCl and H2O, where the more electronegative atom (Cl or O) attracts the electrons slightly more, giving it a partial negative charge and leaving the other atom with
Chemical Bonding
The atoms of molecules are linked together through a reaction known as chemical bonding. A chemical bond is a force that holds atoms together.
Chemical Bonding
There are three main types of chemical bonding:
1) Ionic bonding results from the electrostatic attraction between oppositely charged ions. It is characteristic of bonds between metals and nonmetals.
2) Covalent bonding involves the sharing of electron pairs between atoms. It can be polar, nonpolar, single, double or triple.
3) Metallic bonding occurs between metal atoms and involves delocalized valence electrons that are free to move throughout the structure.
Types of bond by KK Sahu sir
Definition
What constitute a chemical bond?
Types of bond
1. Strong bond
Covalent bond
Glycosidic bond
Peptide bond
Disulfide bond
2. Weak bond
Hydrogen bond
Van der waals bond
Hydrophobic bond
Ionic bond
Conclusion
References
Polar Covalent Bond
A polar covalent bond forms when electrons in a covalent bond are not shared equally between the two atoms due to differences in electronegativity. Atoms with large differences in electronegativity will form polar covalent bonds, causing the electrons to be attracted more to the atom with higher electronegativity, such as chlorine in a hydrogen-chlorine bond. Polar covalent bonds result in the atoms having partial positive and negative charges.
Chemical bonding
This document discusses the three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals when the metal transfers electrons to the nonmetal. Covalent bonds form when atoms share electrons in either single, double or triple bonds. Metallic bonds form when metal atoms contribute electrons to form a "sea of electrons" that are shared between all the atoms.
Chemical bonding
The document summarizes different types of chemical bonds including ionic bonds, covalent bonds, metallic bonds, hydrogen bonds, and Van der Waals interactions. It describes how each type of bond forms and provides examples. Ionic bonds form through electrostatic attraction between oppositely charged ions. Covalent bonds form when atoms share one or more pairs of electrons. Metallic bonds result from delocalized electrons within metal structures. Hydrogen bonds are electrostatic attractions between hydrogen and electronegative atoms. Van der Waals interactions arise from correlations in polarizations between particles.
Unit 11 - Covalent Bonding
This document discusses covalent bonds and how they differ from ionic bonds. Covalent bonds involve sharing electrons between atoms rather than transferring electrons. Chlorine atoms form a covalent bond by each atom sharing an electron pair, allowing both atoms to achieve a full outer shell or octet of electrons. Covalent bonds typically form between nonmetal atoms in groups 3-6 of the periodic table, which have incomplete outer shells and can share electrons to achieve full shells. Carbon is particularly important for life because it can form up to four covalent bonds, allowing for complex carbon chains and structures like DNA and proteins.
Covalent Bond
Covalent bonding occurs when two non-metal atoms share electrons in their outer shells to gain a stable electron configuration. Chlorine exists as Cl2 molecules where each chlorine atom shares one electron with the other to fill its outer shell. Oxygen also exists as O2 molecules where each oxygen atom shares two electrons in a double bond to fill its outer shell. Covalent compounds have strong bonds within their molecules but weak intermolecular forces, which explains their low melting points and why many exist as gases.
Types of chemical bonds
Chemical bonds form when atoms share or transfer electrons. There are several main types of bonds:
- Ionic bonds form when metals transfer electrons to nonmetals to form positive and negative ions that are attracted to each other. Ionic compounds are crystalline and dissolve in water.
- Covalent bonds form when atoms share two or more valence electrons to achieve stability. Covalent bond strength depends on the number of electron pairs shared. Covalent compounds exist as discrete molecules.
- Metallic bonds result from the attraction between positively charged metal ions and delocalized electrons in the "sea of electrons" in the solid metal. Metallic bonding explains the properties of metals like conductivity.
Covalent bonds
Covalent (molecular) bonds are bonds formed between non-metals. In this show, you'll see some examples of covalent bonds.
Chemical Bonds
This document discusses different types of chemical bonds including ionic bonding, covalent bonding, and metallic bonding. Ionic bonding involves the electrostatic attraction between oppositely charged ions when atoms gain or lose electrons. Covalent bonding occurs when atoms share pairs of electrons to gain stability. Metallic bonding results from the attraction between positively charged atomic nuclei and delocalized electrons in metals that act as the binding medium. The importance of chemical bonding is that it allows atoms to join together to form molecules and structures with unique physical and chemical properties essential for life.
Class 11 Chapter 4 Chemical Bonding and Molecular Structure.pptx
This document provides an overview of chemical bonding and molecular structure. It discusses topics such as octet rule, covalent bonds, limitations of the octet rule, ionic or electrovalent bonds, lattice enthalpy, bond parameters including bond length, bond angle, bond enthalpy and bond order. It also covers concepts of resonance, polar covalent bonds, dipole moment and covalent character in ionic bonds based on Fajans' rule. The document is presented as part of a Class XI chemistry curriculum on this unit.
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Bonding and Structure
The document discusses different types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between metals and non-metals to form ions. Covalent bonding involves the sharing of electron pairs between non-metals. Metallic bonding involves a sea of delocalized electrons that are attracted to cationic metal ions arranged in a lattice. Each type of bonding results in different material properties depending on whether electrons are transferred, shared, or free to move.
Covalent bonds
Covalent bonds result from the sharing of valence electrons between two nonmetallic atoms. A single covalent bond forms when one pair of electrons is shared, while double and triple bonds share two or three pairs of electrons, respectively. Molecular structure and bond angles are determined by the VSEPR model, which predicts molecular geometry based on electron pair repulsion. Hybridization occurs when atomic orbitals mix to form new hybrid orbitals and explain molecular bonding orientations.
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Chemical bonds form between atoms to stabilize their outer electron shells. There are three main types of bonds: ionic bonds form when electrons are transferred between atoms, covalent bonds form when electrons are shared between atoms, and metallic bonds form from the delocalized "sea" of electrons in metal atoms. Ionic bonds result in oppositely charged ions, covalent bonds can be single, double or triple depending on electron pairs shared, and metallic bonding gives metals their conductivity. Compounds are classified as ionic, covalent or metallic based on the type of bonding between their atoms.
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This document defines and provides examples of covalent bonds. It discusses the history of the term being coined by Irving Langmuir in 1919. A covalent bond is defined as a chemical link where electrons are shared between two atoms. Examples given are the covalent bonds between oxygen and hydrogen in H2O and between hydrogen atoms in H2. The document also describes the different types of covalent bonds - single, double, and triple - based on the number of electron pairs shared between the bonded atoms.
Ionic Bond
Ionic bonds form when oppositely charged ions attract each other. They are strong but non-directional bonds. Ionic bonds form when there is a large difference in electronegativity between atoms. Cations form when atoms lose electrons and anions form when atoms gain electrons. Ionic solids have high melting points and are insoluble in non-polar solvents due to their strong electrostatic attractions.
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This document provides information on ionic and covalent bonding. It discusses how ionic bonding occurs through the transfer of electrons from metal to non-metal atoms, giving each atom a stable electron configuration. Ions are held together by electrostatic attraction in a lattice structure. Covalent bonding occurs through the sharing of electrons between non-metal atoms to achieve a stable electron configuration. Covalent structures can be either simple molecules or giant molecular structures held together by strong covalent bonds. The document also discusses allotropes such as diamond and graphite which are different structural forms of the same element.
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This document discusses chemical bonds, specifically ionic and covalent bonds. It explains that ionic bonds are formed through the transfer of electrons between metal and non-metal atoms, resulting in oppositely charged ions that are attracted to one another. Covalent bonds are formed through the sharing of electron pairs between non-metal atoms. Key differences between ionic and covalent compounds are discussed, such as ionic compounds existing as solids and conducting electricity when molten or dissolved, while covalent compounds can be solids, liquids or gases and do not conduct electricity.
Covalent bonds
Covalent bonds occur when atoms share pairs of electrons to form molecules. Atoms form covalent bonds by sharing unpaired valence electrons, with examples being water (H2O) forming two covalent bonds and molecular oxygen (O2) forming a double covalent bond by sharing two pairs of electrons. Properties of covalent bonds include low melting and boiling points with poor conductivity.
Covalent bond
A covalent bond involves the sharing of electron pairs between atoms. There are two types of covalent bonding: non-polar, with equal sharing, and polar, with unequal sharing. A non-polar bond forms between like atoms that share electrons equally, while a polar bond forms between different atoms where one atom attracts the electrons more than the other due to differing electronegativity. Examples of non-polar molecules are H2, Cl2, and O2, where the atoms share electrons equally. Examples of polar molecules are HCl and H2O, where the more electronegative atom (Cl or O) attracts the electrons slightly more, giving it a partial negative charge and leaving the other atom with
Chemical Bonding
The atoms of molecules are linked together through a reaction known as chemical bonding. A chemical bond is a force that holds atoms together.
Chemical Bonding
There are three main types of chemical bonding:
1) Ionic bonding results from the electrostatic attraction between oppositely charged ions. It is characteristic of bonds between metals and nonmetals.
2) Covalent bonding involves the sharing of electron pairs between atoms. It can be polar, nonpolar, single, double or triple.
3) Metallic bonding occurs between metal atoms and involves delocalized valence electrons that are free to move throughout the structure.
Types of bond by KK Sahu sir
Definition
What constitute a chemical bond?
Types of bond
1. Strong bond
Covalent bond
Glycosidic bond
Peptide bond
Disulfide bond
2. Weak bond
Hydrogen bond
Van der waals bond
Hydrophobic bond
Ionic bond
Conclusion
References
Polar Covalent Bond
A polar covalent bond forms when electrons in a covalent bond are not shared equally between the two atoms due to differences in electronegativity. Atoms with large differences in electronegativity will form polar covalent bonds, causing the electrons to be attracted more to the atom with higher electronegativity, such as chlorine in a hydrogen-chlorine bond. Polar covalent bonds result in the atoms having partial positive and negative charges.
Chemical bonding
This document discusses the three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals when the metal transfers electrons to the nonmetal. Covalent bonds form when atoms share electrons in either single, double or triple bonds. Metallic bonds form when metal atoms contribute electrons to form a "sea of electrons" that are shared between all the atoms.
Chemical bonding
The document summarizes different types of chemical bonds including ionic bonds, covalent bonds, metallic bonds, hydrogen bonds, and Van der Waals interactions. It describes how each type of bond forms and provides examples. Ionic bonds form through electrostatic attraction between oppositely charged ions. Covalent bonds form when atoms share one or more pairs of electrons. Metallic bonds result from delocalized electrons within metal structures. Hydrogen bonds are electrostatic attractions between hydrogen and electronegative atoms. Van der Waals interactions arise from correlations in polarizations between particles.
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This document discusses covalent bonds and how they differ from ionic bonds. Covalent bonds involve sharing electrons between atoms rather than transferring electrons. Chlorine atoms form a covalent bond by each atom sharing an electron pair, allowing both atoms to achieve a full outer shell or octet of electrons. Covalent bonds typically form between nonmetal atoms in groups 3-6 of the periodic table, which have incomplete outer shells and can share electrons to achieve full shells. Carbon is particularly important for life because it can form up to four covalent bonds, allowing for complex carbon chains and structures like DNA and proteins.
Covalent Bond
Covalent bonding occurs when two non-metal atoms share electrons in their outer shells to gain a stable electron configuration. Chlorine exists as Cl2 molecules where each chlorine atom shares one electron with the other to fill its outer shell. Oxygen also exists as O2 molecules where each oxygen atom shares two electrons in a double bond to fill its outer shell. Covalent compounds have strong bonds within their molecules but weak intermolecular forces, which explains their low melting points and why many exist as gases.
Types of chemical bonds
Chemical bonds form when atoms share or transfer electrons. There are several main types of bonds:
- Ionic bonds form when metals transfer electrons to nonmetals to form positive and negative ions that are attracted to each other. Ionic compounds are crystalline and dissolve in water.
- Covalent bonds form when atoms share two or more valence electrons to achieve stability. Covalent bond strength depends on the number of electron pairs shared. Covalent compounds exist as discrete molecules.
- Metallic bonds result from the attraction between positively charged metal ions and delocalized electrons in the "sea of electrons" in the solid metal. Metallic bonding explains the properties of metals like conductivity.
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Chemical bonds 2020
Chemical bonds are the forces that hold atoms together in molecules and compounds. There are several types of bonds including ionic bonds, covalent bonds, hydrogen bonds, metallic bonds, and coordinate bonds. Ionic bonds form between metals and nonmetals when electrons are transferred. Covalent bonds form when atoms share electrons. Hydrogen bonds occur between polar molecules containing hydrogen. Metallic bonds are electrostatic attractions between positively charged metal ions and delocalized electrons. Coordinate bonds form when both electrons in a bond come from the same atom. Each bond type influences the properties of the resulting compounds.
Mecchapter3 120815080608-phpapp01
This document provides an overview of chemical bonding, naming ionic and covalent compounds, and the properties of ionic and covalent compounds. It discusses the different types of chemical bonds including ionic bonds formed by electron transfer between metals and nonmetals, covalent bonds formed by electron sharing between nonmetals, and polar covalent bonds where electron sharing is unequal. It also describes how to name ionic and covalent compounds and write their chemical formulas, and compares the physical properties of ionic and covalent compounds.
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Class 11 Chapter 4 Chemical Bonding and Molecular Structure.pptx
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The document discusses soil resources and composition. Soil is a complex mixture of minerals, organic matter, water, and air. Organic matter like humus improves soil quality by enhancing moisture retention and providing nutrients. Soil texture depends on mineral particle size. The layers of soil include the O horizon of decomposing plant matter, the A horizon containing humus and minerals, the B horizon receiving materials from the A, the C horizon of weathered bedrock, and the R horizon of unweathered bedrock.
The environment of the philippines.pptx
This document discusses different coordinate systems including the Cartesian coordinate system, one-dimensional system, and three-dimensional system. It then focuses on two coordinate systems used for locating places on Earth: the Universal Transverse Mercator (UTM) system and the geographic coordinate system. The geographic coordinate system uses latitude and longitude measured in degrees relative to the equator and prime meridian to specify locations.
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The document discusses the location of the Philippines and the different continents. It notes that a long time ago, all the continents were joined together in a landmass called Pangaea, surrounded by water called Panthalassa. It provides details about the seven continents, with Asia being the largest and Australia the smallest. The document specifies that the Philippines is located in Asia as one of the 11 Southeast Asian nations, and gives more information about the country's geography as an archipelago composed of over 7,000 islands grouped into Luzon, Visayas, and Mindanao, surrounded by various seas and oceans.
Atmosphere
This document discusses key concepts about the atmosphere including:
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Breezes
This document discusses several key concepts related to physics. It defines breeze as wind near bodies of water. It then explains specific heat capacity as the amount of heat required to raise the temperature of a material by one degree Celsius. Specific heat is described as how slowly an object heats up and cools down. The document also defines pressure as the ratio of force per unit area. Density is explained as the ratio of mass to volume, with denser materials sinking and less dense materials floating. Finally, it outlines the three mechanisms of heat transfer: conduction through physical contact, radiation through electromagnetic waves, and convection through fluid movement.
Learning about the moon(lunar eclipse)
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The document discusses the day/night cycle and seasons on Earth. It explains that Earth's rotation on its axis causes day and night, and its revolution around the sun takes 365 days. The tilt of Earth's axis relative to its orbit causes the seasons as different parts receive more/less sunlight over the course of a year. The seasons are distinguished by equinoxes when day and night are equal and solstices when one hemisphere receives more sunlight. The Philippines experiences 2-4 seasons depending on location, with hot/rainy/cool seasons in most areas.
The basics of solar eclipse
An eclipse occurs when one celestial body passes in front of another, blocking its light. A solar eclipse happens when the moon passes between Earth and the sun, casting its shadow on Earth. There are several types of solar eclipses depending on how much of the sun is obscured by the moon, including total, annular, partial, and hybrid eclipses. The moon's shadow during an eclipse consists of the umbra, penumbra, and antumbra regions. Historical beliefs about eclipses included that they were caused by evil spirits or were omens of tragedy.
Weather instruments
The document describes various weather instruments and their uses, including anemometers, barometers, hygrometers, radars, radiosondes, weather balloons, weather satellites, wind vanes, and thermometers. It also discusses different weather disturbances like drizzles, typhoons, tropical cyclones, and hurricanes. Monsoons, trade winds, and the intertropical convergence zone are explained. Public storm warning signals issued by PAGASA are outlined. Greenhouse gases, the greenhouse effect, and global warming are briefly covered.
Biomes
There are eight major terrestrial biomes: tropical forest, temperate forest, taiga, tundra, desert, grassland, savanna, and shrubland. Aquatic biomes include freshwater biomes like lakes, rivers, and wetlands, as well as marine biomes like estuaries, mangrove forests, coral reefs, and different ocean zones. Biomes are characterized by their climate, plants, and animals that are adapted to that environment.
Separation techniques
This document describes several methods for separating mixtures: mechanical or manual separation uses hands or tools to separate solids; filtration uses a sieve or filter to separate insoluble particles from liquids; decantation relies on differences in density to separate solids from liquids; a separating funnel partitions liquid mixtures into immiscible phases; dissolution separates insoluble solids from soluble ones using a solvent; and distillation separates liquid solvents from solutions by boiling and condensing vapors.
Substances and mixtures(1st)
This document discusses substances and mixtures. It defines a pure substance as matter that has consistent properties and composition that does not vary between samples and cannot be separated into other substances using physical or mechanical means. A mixture is defined as the physical combination of two or more substances where the composition varies between samples. The document also notes that chemistry is the study of matter, its composition, and changes it undergoes. It categorizes mixtures as either homogeneous, with a uniform phase and appearance, or heterogeneous, with no uniform phase or appearance.
Sci method(gr.7)
Measurement is the skill of using the proper measuring tool for a given situation, such as using a ruler to measure length or a thermometer to measure temperature. Prediction is the ability to forecast a future outcome based on evidence of a pattern. Some common quantities that are measured include mass, length, temperature, time, and volume.
Volcanoes
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Stars are huge balls of gases that emit their own light through nuclear fusion. A star's magnitude describes its brightness, with apparent magnitude referring to brightness as seen from Earth and absolute magnitude referring to the amount of light it intrinsically emits. Stars are classified according to their color, from hottest to coolest, and shown on the Hertzsprung-Russell diagram, which plots stars' temperatures and luminosities. Stars are born in nebulae, where increasing temperatures from hydrogen collisions eventually lead to nuclear fusion, the birth of a protostar.
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Major climate zones on earth
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Constellations
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This document discusses carbon compounds and their classes. It introduces carbon catenation, which allows carbon to form chains through covalent bonds. The main classes of carbon compounds discussed are hydrocarbons, which are composed of carbon and hydrogen. Hydrocarbons can be saturated, containing only single bonds, or unsaturated, containing double or triple bonds. Specific types of saturated hydrocarbons discussed include alkanes, which are saturated hydrocarbons with only single carbon-carbon bonds. Unsaturated hydrocarbons include alkenes with double bonds and alkynes with triple bonds. The document also discusses cyclic and aromatic hydrocarbons. It introduces molecular and structural formulas for writing formulas of organic compounds.
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This is a short talk that I gave at the Banff International Research Station workshop on Modeling and Theory in Population Biology. The idea is to try to understand how the burden of natural selection relates to the amount of information that selection puts into the genome.
It's based on the first part of this research paper:
The cost of information acquisition by natural selection
Ryan Seamus McGee, Olivia Kosterlitz, Artem Kaznatcheev, Benjamin Kerr, Carl T. Bergstrom
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Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
Anti-Universe And Emergent Gravity and the Dark Universe
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Context. The observation of several L-band emission sources in the S cluster has led to a rich discussion of their nature. However, a definitive answer to the classification of the dusty objects requires an explanation for the detection of compact Doppler-shifted Brγ emission. The ionized hydrogen in combination with the observation of mid-infrared L-band continuum emission suggests that most of these sources are embedded in a dusty envelope. These embedded sources are part of the S-cluster, and their relationship to the S-stars is still under debate. To date, the question of the origin of these two populations has been vague, although all explanations favor migration processes for the individual cluster members. Aims. This work revisits the S-cluster and its dusty members orbiting the supermassive black hole SgrA* on bound Keplerian orbits from a kinematic perspective. The aim is to explore the Keplerian parameters for patterns that might imply a nonrandom distribution of the sample. Additionally, various analytical aspects are considered to address the nature of the dusty sources. Methods. Based on the photometric analysis, we estimated the individual H−K and K−L colors for the source sample and compared the results to known cluster members. The classification revealed a noticeable contrast between the S-stars and the dusty sources. To fit the flux-density distribution, we utilized the radiative transfer code HYPERION and implemented a young stellar object Class I model. We obtained the position angle from the Keplerian fit results; additionally, we analyzed the distribution of the inclinations and the longitudes of the ascending node. Results. The colors of the dusty sources suggest a stellar nature consistent with the spectral energy distribution in the near and midinfrared domains. Furthermore, the evaporation timescales of dusty and gaseous clumps in the vicinity of SgrA* are much shorter ( 2yr) than the epochs covered by the observations (≈15yr). In addition to the strong evidence for the stellar classification of the D-sources, we also find a clear disk-like pattern following the arrangements of S-stars proposed in the literature. Furthermore, we find a global intrinsic inclination for all dusty sources of 60 ± 20◦, implying a common formation process. Conclusions. The pattern of the dusty sources manifested in the distribution of the position angles, inclinations, and longitudes of the ascending node strongly suggests two different scenarios: the main-sequence stars and the dusty stellar S-cluster sources share a common formation history or migrated with a similar formation channel in the vicinity of SgrA*. Alternatively, the gravitational influence of SgrA* in combination with a massive perturber, such as a putative intermediate mass black hole in the IRS 13 cluster, forces the dusty objects and S-stars to follow a particular orbital arrangement. Key words. stars: black holes– stars: formation– Galaxy: center– galaxies: star formation
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Slides from talk:
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https://ashpc.eu/
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Ahota Beel, nestled in Sootea Biswanath Assam , is celebrated for its extraordinary diversity of bird species. This wetland sanctuary supports a myriad of avian residents and migrants alike. Visitors can admire the elegant flights of migratory species such as the Northern Pintail and Eurasian Wigeon, alongside resident birds including the Asian Openbill and Pheasant-tailed Jacana. With its tranquil scenery and varied habitats, Ahota Beel offers a perfect haven for birdwatchers to appreciate and study the vibrant birdlife that thrives in this natural refuge.
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...ABHISHEK SONI NIMT INSTITUTE OF MEDICAL AND PARAMEDCIAL SCIENCES , GOVT PG COLLEGE NOIDA
Microbial interaction
Microorganisms interacts with each other and can be physically associated with another organisms in a variety of ways.
One organism can be located on the surface of another organism as an ectobiont or located within another organism as endobiont.
Microbial interaction may be positive such as mutualism, proto-cooperation, commensalism or may be negative such as parasitism, predation or competition
Types of microbial interaction
Positive interaction: mutualism, proto-cooperation, commensalism
Negative interaction: Ammensalism (antagonism), parasitism, predation, competition
I. Mutualism:
It is defined as the relationship in which each organism in interaction gets benefits from association. It is an obligatory relationship in which mutualist and host are metabolically dependent on each other.
Mutualistic relationship is very specific where one member of association cannot be replaced by another species.
Mutualism require close physical contact between interacting organisms.
Relationship of mutualism allows organisms to exist in habitat that could not occupied by either species alone.
Mutualistic relationship between organisms allows them to act as a single organism.
Examples of mutualism:
i. Lichens:
Lichens are excellent example of mutualism.
They are the association of specific fungi and certain genus of algae. In lichen, fungal partner is called mycobiont and algal partner is called
II. Syntrophism:
It is an association in which the growth of one organism either depends on or improved by the substrate provided by another organism.
In syntrophism both organism in association gets benefits.
Compound A
Utilized by population 1
Compound B
Utilized by population 2
Compound C
utilized by both Population 1+2
Products
In this theoretical example of syntrophism, population 1 is able to utilize and metabolize compound A, forming compound B but cannot metabolize beyond compound B without co-operation of population 2. Population 2is unable to utilize compound A but it can metabolize compound B forming compound C. Then both population 1 and 2 are able to carry out metabolic reaction which leads to formation of end product that neither population could produce alone.
Examples of syntrophism:
i. Methanogenic ecosystem in sludge digester
Methane produced by methanogenic bacteria depends upon interspecies hydrogen transfer by other fermentative bacteria.
Anaerobic fermentative bacteria generate CO2 and H2 utilizing carbohydrates which is then utilized by methanogenic bacteria (Methanobacter) to produce methane.
ii. Lactobacillus arobinosus and Enterococcus faecalis:
In the minimal media, Lactobacillus arobinosus and Enterococcus faecalis are able to grow together but not alone.
The synergistic relationship between E. faecalis and L. arobinosus occurs in which E. faecalis require folic acid
快速办理(UAM毕业证书)马德里自治大学毕业证学位证一模一样
学校原件一模一样【微信：741003700 】《(UAM毕业证书)马德里自治大学毕业证学位证》【微信：741003700 】学位证，留信认证（真实可查，永久存档）原件一模一样纸张工艺/offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
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CLASS 12th CHEMISTRY SOLID STATE ppt (Animated)
Description:
Dive into the fascinating realm of solid-state physics with our meticulously crafted online PowerPoint presentation. This immersive educational resource offers a comprehensive exploration of the fundamental concepts, theories, and applications within the realm of solid-state physics.
From crystalline structures to semiconductor devices, this presentation delves into the intricate principles governing the behavior of solids, providing clear explanations and illustrative examples to enhance understanding. Whether you're a student delving into the subject for the first time or a seasoned researcher seeking to deepen your knowledge, our presentation offers valuable insights and in-depth analyses to cater to various levels of expertise.
Key topics covered include:
Crystal Structures: Unravel the mysteries of crystalline arrangements and their significance in determining material properties.
Band Theory: Explore the electronic band structure of solids and understand how it influences their conductive properties.
Semiconductor Physics: Delve into the behavior of semiconductors, including doping, carrier transport, and device applications.
Magnetic Properties: Investigate the magnetic behavior of solids, including ferromagnetism, antiferromagnetism, and ferrimagnetism.
Optical Properties: Examine the interaction of light with solids, including absorption, reflection, and transmission phenomena.
With visually engaging slides, informative content, and interactive elements, our online PowerPoint presentation serves as a valuable resource for students, educators, and enthusiasts alike, facilitating a deeper understanding of the captivating world of solid-state physics. Explore the intricacies of solid-state materials and unlock the secrets behind their remarkable properties with our comprehensive presentation.
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Bond formation (l3)
- 3. A chemical bond is the force of attraction between and among atoms to form molecules and compounds.
- 4. Valence electrons are electrons found in the highest energy level of an atom.
- 6. ENERGY IONIZATION is the energy required to remove an electron from a gaseous atom
- 7. Electron Dot Structure In 1916, Gilbert N. Lewis developed a system of dots to represent valence electrons and to keep track on them during bond formation.
- 10. IONIC BOND • Ionic Bond is the electrostatic force of attraction that holds ions together in an ionic compound. • Metallic atoms conform to the octet rule by losing electrons while nonmetallic atoms obey the rule by gaining electrons.
- 11. Classifications of Ionic Compound • Binary compounds • Ternary compounds
- 12. BINARY COOPOUNDS Binary compounds are compounds composed of only two elements. Ex. NaCl – Sodium chloride TERNARY COMPOUNDS Ternary compounds are compounds composed of three or more elements. Ex. 𝐻2 𝑆𝑂4 - Sulfuric acid
- 13. Steps in writing formulas in Ionic Compounds: 1. Determine the charge of the ion above the symbol. 2. Balance the charges of the ions (you can also use the criss-cross method) whereas: 𝑀 𝐴 + 𝑁 𝐵 = 𝑀 𝐵 𝑁𝐴 Note: When there is more than one of a polyatomic ion in the formula, we use parenthesis.
- 14. Shortquiz: #4 1. Sodium bicarbonate 2. Sodium flouride 3. Iron (lll) chloride 4. Sodium carbonate 5. Copper (ll) sulfate 6. Magnesium hydroxide 7. Barium nitrate 8. Lithium sulfate 9. Magnesium oxide 10.Silver nitrate Write the formula for the following ionic compounds.
- 15. Steps in writing the chemical names of the ionic compounds 1. Write the cation name first, then name the anion. • Monoatomic anions use the “ide” suffix • Do not change the suffix to “ide” with polyatomic ions. 2. If the cation is one of the transition metals with various charges, write the charge using parenthesis and Roman numerals after the metal name. Ex. Copper (ll) flouride
- 16. Write the chemical names of the following compounds: 1. NaCl 2. F𝑒2(C𝑂3)3 3. Cu(OH)2 4. (N𝐻4)2S𝑂4 5. LiN𝑂3 6. BaS𝑂4 7. Mg(N𝑂3)2 8. AgCl 9. Al(OH)3 10. CaS𝑂4
- 17. Covalent Bond • Covalent bond is an attractive force that holds atoms together due to sharing of electrons. • Atoms that tend to form covalent bonds are the nonmetals. • Nonmetals have higher ionization energy and higher electronegativities, these type of atoms have higher tendency to attract electrons toward themselves.
- 18. Covalent Bond • A covalent bond consists of shared electrons.
- 19. Covalent Bond • One pair of electrons shared between two atoms constitutes a single covalent bond, commonly referred to as single bond.
- 20. Covalent Bond • When there are two pairs of shared electrons, the covalent is a double bond.
- 21. Covalent Bond • When three pairs of electrons are shared, the covalent bond is called a triple bond.
- 22. Covalent Bond • STRUCTURAL FORMULA - is a chemical formula that shows the arrangement of 3 atoms in molecules or polyatomic ions.
- 23. Covalent Bond • ELECTRON DOT STRUCTURE - is a chemical formula that shows the arrangement of 3 atoms in molecules or polyatomic ions. • COVALENCE NUMBER - refers to the number of possible bonds the atom can form
- 24. ELECTRON DOT STRUCTURE • Steps for Drawing a Lewis Diagram: 1. Count all the valence electrons 2. Determine the central atom (the element that there is only one of) 3. Draw single bonds to the central atom 4. Put all remaining valence electrons on atoms as lone pairs 5. Turn lone pairs into double or triple bonds to give every atom an octet
- 25. • RESONANCE FORMS or STRUCTURES - are two or more equally valid Lewis structures or electron dot formulas that can be drawn from the molecule