This document provides an overview of chemical bonding and the covalent bond model. It discusses the key differences between ionic and covalent bonding. Covalent bonds form when two atoms share one or more pairs of electrons. Lewis structures are used to represent electron sharing between atoms in covalent compounds using dots or dashes to indicate bonding and nonbonding electron pairs. Molecular geometry can be predicted using VSEPR (valence shell electron pair repulsion) theory, which considers the number of electron pairs around an atom to minimize repulsions between pairs. Electronegativity refers to an atom's ability to attract shared electrons in a bond.
This document provides an overview of key concepts in chemical calculations including:
1) Formula masses are calculated by adding atomic masses of elements in a chemical formula.
2) A mole is a unit used to count particles and relates to Avogadro's number.
3) Molar mass is the mass in grams of one mole of a substance.
4) Chemical formulas indicate the number of atoms present at both the microscopic and macroscopic scale.
5) Balanced chemical equations conserve atoms and can be used to interconvert moles of reactants and products.
The document is a chapter about gases, liquids, and solids that discusses their properties based on kinetic molecular theory. It introduces the kinetic molecular theory, which states that matter is composed of tiny particles in constant random motion that interact through attractions and repulsions. It then describes the distinguishing physical properties of the three states of matter. Solids have a regular structure with particles fixed in place, while liquids and gases have particles in random motion but liquids are more dense with particles still near each other.
The document is a chapter about solutions from a chemistry textbook. It begins with definitions of key terms related to solutions like solute, solvent, saturated solution, and concentration units. It then discusses characteristics of solutions, factors that influence solubility such as temperature and pressure, and solubility rules for ionic compounds in water. Solubility is explained as the maximum amount of solute that can dissolve in a given amount of solvent. The chapter also covers methods for expressing the concentration of a solution, including percent concentration and molarity.
This document provides an overview of chemical bonding and ionic compounds. It discusses how ionic bonds form through the transfer of electrons between atoms, resulting in positively and negatively charged ions that are attracted to one another. Polyatomic ions, which are groups of atoms that behave as single units with positive or negative charges, are also introduced. The key concepts covered include writing formulas for ionic compounds, naming binary ionic compounds, and recognizing common polyatomic ions.
Covalent bonds form when electrons are shared between two elements that have close electronegativity, so neither element takes or loses electrons. Ionic bonds form when a metal takes electrons from a nonmetal, giving the metal a positive charge and the nonmetal a negative charge so they are attracted. Covalent bonds form between nonmetals and have low melting points, while ionic bonds form between metals and nonmetals and have high melting points due to the strong electrostatic forces between the ions.
Metallic bonding results from the attraction between metal cations and delocalized electrons in the "sea" of electrons. This allows electrons to move freely throughout the metal and form metallic bonds between atoms. Metallic bonding gives metals properties like high melting points, conductivity of heat and electricity, and malleability.
This document provides a summary of key concepts about the periodic table. It defines important terms like period, group, atomic number, atomic mass, atomic radius, and others. It explains trends in atomic mass and atomic radius across periods and groups, with mass increasing and radius decreasing across periods but increasing across groups. Electronegativity, ionization energy, and electron affinity follow the same trends. It identifies important regions of the periodic table and provides a mnemonic for the first 20 elements. Finally, it discusses how ionic radii change depending on whether an atom forms a cation or anion.
This document provides an overview of key concepts in chemical calculations including:
1) Formula masses are calculated by adding atomic masses of elements in a chemical formula.
2) A mole is a unit used to count particles and relates to Avogadro's number.
3) Molar mass is the mass in grams of one mole of a substance.
4) Chemical formulas indicate the number of atoms present at both the microscopic and macroscopic scale.
5) Balanced chemical equations conserve atoms and can be used to interconvert moles of reactants and products.
The document is a chapter about gases, liquids, and solids that discusses their properties based on kinetic molecular theory. It introduces the kinetic molecular theory, which states that matter is composed of tiny particles in constant random motion that interact through attractions and repulsions. It then describes the distinguishing physical properties of the three states of matter. Solids have a regular structure with particles fixed in place, while liquids and gases have particles in random motion but liquids are more dense with particles still near each other.
The document is a chapter about solutions from a chemistry textbook. It begins with definitions of key terms related to solutions like solute, solvent, saturated solution, and concentration units. It then discusses characteristics of solutions, factors that influence solubility such as temperature and pressure, and solubility rules for ionic compounds in water. Solubility is explained as the maximum amount of solute that can dissolve in a given amount of solvent. The chapter also covers methods for expressing the concentration of a solution, including percent concentration and molarity.
This document provides an overview of chemical bonding and ionic compounds. It discusses how ionic bonds form through the transfer of electrons between atoms, resulting in positively and negatively charged ions that are attracted to one another. Polyatomic ions, which are groups of atoms that behave as single units with positive or negative charges, are also introduced. The key concepts covered include writing formulas for ionic compounds, naming binary ionic compounds, and recognizing common polyatomic ions.
Covalent bonds form when electrons are shared between two elements that have close electronegativity, so neither element takes or loses electrons. Ionic bonds form when a metal takes electrons from a nonmetal, giving the metal a positive charge and the nonmetal a negative charge so they are attracted. Covalent bonds form between nonmetals and have low melting points, while ionic bonds form between metals and nonmetals and have high melting points due to the strong electrostatic forces between the ions.
Metallic bonding results from the attraction between metal cations and delocalized electrons in the "sea" of electrons. This allows electrons to move freely throughout the metal and form metallic bonds between atoms. Metallic bonding gives metals properties like high melting points, conductivity of heat and electricity, and malleability.
This document provides a summary of key concepts about the periodic table. It defines important terms like period, group, atomic number, atomic mass, atomic radius, and others. It explains trends in atomic mass and atomic radius across periods and groups, with mass increasing and radius decreasing across periods but increasing across groups. Electronegativity, ionization energy, and electron affinity follow the same trends. It identifies important regions of the periodic table and provides a mnemonic for the first 20 elements. Finally, it discusses how ionic radii change depending on whether an atom forms a cation or anion.
This document provides a summary of key concepts for predicting products in chemical reactions on the AP Chemistry exam. It defines common reaction types like precipitation and acid-base reactions. It outlines the steps to take to determine the molecular, complete ionic, and net ionic equations for different reaction types. These include double replacement, acid-base, decomposition, combustion, redox, and complex ion formation reactions. Solubility rules are also summarized to predict if a compound will precipitate out of solution. The document concludes with guidance on how to convert word problems into balanced chemical equations.
This document provides an overview of key concepts in chemical bonding theories, including different types of bonds (ionic, covalent, polar covalent, metallic) and how they are formed. It also discusses bond polarity, electronegativity, isomers, resonance structures, sigma and pi bonds, and hybridization. Common characteristics of different bond types are outlined such as melting points, solubility, and conductivity. Examples are given to illustrate concepts like bond polarity, isomers, resonance structures, and counting sigma and pi bonds.
Polarity refers to a separation of electric charge within molecules that gives them an electric dipole moment. Electronegativity is an atom's ability to attract electrons in a chemical bond. There are two types of covalent bonds: nonpolar bonds between identical atoms that share electrons equally, and polar bonds between different atoms that unequally share electrons.
Chemical bonding and the lewis structureLily Kotze
This document discusses different types of chemical bonds including ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a metal transfers electrons to a non-metal. Covalent bonds form when two non-metals share electrons. Metallic bonds form through electrostatic attraction between positively charged metal ions and delocalized electrons. Examples of different bonds are also provided such as lithium fluoride forming an ionic bond through Li+ and F- ions and metallic bonding in metals occurring through interaction of positively charged atomic residues and free-flowing electrons.
This document discusses covalent bonding and molecular compounds. It defines a chemical bond as a force that holds atoms together, and describes covalent bonding as atoms sharing electrons. As two atoms approach each other to form a bond, their potential energy decreases to a minimum at the bond length. Bond length and bond energy vary between different bonded atoms. The octet rule states atoms want 8 electrons in their valence shell. Practice problems classify bonds and identify valence electrons.
This document provides a summary of key concepts and steps for drawing Lewis structures of molecules and ions. It defines important terms like valence electrons, octet rule, and bonding vs. lone pairs. It outlines a 6-step process for drawing Lewis structures, including determining the number of valence electrons and arranging atoms to achieve full valence shells. Exceptions to the octet rule are noted for small atoms and those in period 3 or below. Mnemonics are provided to help remember electron configurations.
This document provides an overview of molecular shapes and bonding theories. It discusses how the shape of a molecule is determined by electron pairs and bond angles. The Valence Shell Electron Pair Repulsion (VSEPR) theory is introduced to predict molecular geometries based on the number of electron domains around a central atom. Hybridization of atomic orbitals is described as a way to explain molecular geometries. Sigma and pi bonding are discussed in the context of valence bond theory. Delocalized electrons and resonance are also summarized.
The document discusses chemical bonding and molecular structures. It explains that chemical bonding occurs through ionic bonding via the transfer of electrons between atoms, or covalent bonding via the sharing of electron pairs between atoms. It also describes molecular geometry models including VSEPR theory, which predicts the three-dimensional arrangements of atoms in molecules based on electron pair repulsion. Common molecular shapes such as linear, trigonal planar, tetrahedral and octahedral are defined.
This document provides a summary of covalent bonding and molecular compounds in 3 paragraphs:
Covalent bonds result from the sharing of valence electrons between nonmetallic elements. Atoms joined by covalent bonds form molecules, the smallest units of a molecular substance. Molecules have a molecular formula showing the number and type of atoms, and may be represented by Lewis structures or structural formulas.
Multiple bonds can form when atoms share more than one pair of valence electrons. The octet rule describes how atoms bond to acquire a full outer shell of 8 electrons. Molecular shape is determined by VSEPR theory based on electron pair repulsion. Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals for bonding
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
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.
This document provides a summary of key concepts in chemical bonding:
1. It defines different types of bonds including ionic bonds formed between ions, covalent bonds formed by shared electrons between nonmetals, and metallic bonds formed by pooled electrons between metal atoms.
2. It describes characteristics used to identify bond types such as solubility in water and conductivity. Electronegativity is also defined as an atom's pull on shared electrons.
3. Bond polarity is discussed in relation to differences in electronegativity, with polar bonds having an unequal sharing of electrons between atoms.
Calcium ion and bromide ion would form Calcium bromide. Potassium ion and sulfide ion would form Potassium sulfide. Aluminum ion and selenide ion would form Aluminum selenide. Metallic bonds form between metal cations through a "sea of electrons" shared between all the metal atoms. Metals are ductile and good conductors of electricity due to the free movement of delocalized valence electrons between metal cations. Alloys can have superior properties to their component elements.
This document provides an overview of chemical bonding and ionic compounds. It discusses the ionic bond model, where ions are formed through the transfer of electrons between atoms. Metals tend to lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions. Ionic compounds are formed when cations and anions combine in ratios that result in an electrically neutral compound. The structures and names of ionic compounds are also covered.
1) Atoms form chemical bonds in order to attain a stable electron configuration with 8 valence electrons, known as an octet.
2) There are three main types of bonds: ionic bonds form when atoms transfer electrons to become ions, covalent bonds form when atoms share electrons, and metallic bonds involve delocalized electrons distributed among positively charged metal ions.
3) Whether a bond is ionic or covalent depends on the electronegativity of the atoms involved - ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals.
This document provides an overview of chemical bonding and the covalent bond model. It begins by defining a covalent bond and comparing it to ionic bonding. It then discusses Lewis structures and how they represent shared electron pairs in covalent bonds. The document outlines different types of covalent bonds (single, double, triple) and how many bonds an atom will form based on its valence electrons. It also discusses molecular geometry and the VSEPR model for predicting molecular shapes. Additional sections cover bond polarity, molecular polarity, and naming binary molecular compounds.
The document discusses the octet rule in covalent bonding. It states that in covalent bonds, electron sharing usually occurs so that atoms attain the electron configuration of noble gases, with eight electrons in their outer shell. Atoms can form single, double or triple bonds to reach an octet. Single bonds involve one shared pair of electrons, double bonds two shared pairs, and triple bonds three shared pairs. Examples like hydrogen gas, oxygen gas, carbon dioxide and nitrogen gas are provided to illustrate the different bond types. The octet rule explains the bonding in many covalent compounds composed of nonmetals.
This document provides a summary of key concepts for predicting products in chemical reactions on the AP Chemistry exam. It defines common reaction types like precipitation and acid-base reactions. It outlines the steps to take to determine the molecular, complete ionic, and net ionic equations for different reaction types. These include double replacement, acid-base, decomposition, combustion, redox, and complex ion formation reactions. Solubility rules are also summarized to predict if a compound will precipitate out of solution. The document concludes with guidance on how to convert word problems into balanced chemical equations.
This document provides an overview of key concepts in chemical bonding theories, including different types of bonds (ionic, covalent, polar covalent, metallic) and how they are formed. It also discusses bond polarity, electronegativity, isomers, resonance structures, sigma and pi bonds, and hybridization. Common characteristics of different bond types are outlined such as melting points, solubility, and conductivity. Examples are given to illustrate concepts like bond polarity, isomers, resonance structures, and counting sigma and pi bonds.
Polarity refers to a separation of electric charge within molecules that gives them an electric dipole moment. Electronegativity is an atom's ability to attract electrons in a chemical bond. There are two types of covalent bonds: nonpolar bonds between identical atoms that share electrons equally, and polar bonds between different atoms that unequally share electrons.
Chemical bonding and the lewis structureLily Kotze
This document discusses different types of chemical bonds including ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a metal transfers electrons to a non-metal. Covalent bonds form when two non-metals share electrons. Metallic bonds form through electrostatic attraction between positively charged metal ions and delocalized electrons. Examples of different bonds are also provided such as lithium fluoride forming an ionic bond through Li+ and F- ions and metallic bonding in metals occurring through interaction of positively charged atomic residues and free-flowing electrons.
This document discusses covalent bonding and molecular compounds. It defines a chemical bond as a force that holds atoms together, and describes covalent bonding as atoms sharing electrons. As two atoms approach each other to form a bond, their potential energy decreases to a minimum at the bond length. Bond length and bond energy vary between different bonded atoms. The octet rule states atoms want 8 electrons in their valence shell. Practice problems classify bonds and identify valence electrons.
This document provides a summary of key concepts and steps for drawing Lewis structures of molecules and ions. It defines important terms like valence electrons, octet rule, and bonding vs. lone pairs. It outlines a 6-step process for drawing Lewis structures, including determining the number of valence electrons and arranging atoms to achieve full valence shells. Exceptions to the octet rule are noted for small atoms and those in period 3 or below. Mnemonics are provided to help remember electron configurations.
This document provides an overview of molecular shapes and bonding theories. It discusses how the shape of a molecule is determined by electron pairs and bond angles. The Valence Shell Electron Pair Repulsion (VSEPR) theory is introduced to predict molecular geometries based on the number of electron domains around a central atom. Hybridization of atomic orbitals is described as a way to explain molecular geometries. Sigma and pi bonding are discussed in the context of valence bond theory. Delocalized electrons and resonance are also summarized.
The document discusses chemical bonding and molecular structures. It explains that chemical bonding occurs through ionic bonding via the transfer of electrons between atoms, or covalent bonding via the sharing of electron pairs between atoms. It also describes molecular geometry models including VSEPR theory, which predicts the three-dimensional arrangements of atoms in molecules based on electron pair repulsion. Common molecular shapes such as linear, trigonal planar, tetrahedral and octahedral are defined.
This document provides a summary of covalent bonding and molecular compounds in 3 paragraphs:
Covalent bonds result from the sharing of valence electrons between nonmetallic elements. Atoms joined by covalent bonds form molecules, the smallest units of a molecular substance. Molecules have a molecular formula showing the number and type of atoms, and may be represented by Lewis structures or structural formulas.
Multiple bonds can form when atoms share more than one pair of valence electrons. The octet rule describes how atoms bond to acquire a full outer shell of 8 electrons. Molecular shape is determined by VSEPR theory based on electron pair repulsion. Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals for bonding
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
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.
This document provides a summary of key concepts in chemical bonding:
1. It defines different types of bonds including ionic bonds formed between ions, covalent bonds formed by shared electrons between nonmetals, and metallic bonds formed by pooled electrons between metal atoms.
2. It describes characteristics used to identify bond types such as solubility in water and conductivity. Electronegativity is also defined as an atom's pull on shared electrons.
3. Bond polarity is discussed in relation to differences in electronegativity, with polar bonds having an unequal sharing of electrons between atoms.
Calcium ion and bromide ion would form Calcium bromide. Potassium ion and sulfide ion would form Potassium sulfide. Aluminum ion and selenide ion would form Aluminum selenide. Metallic bonds form between metal cations through a "sea of electrons" shared between all the metal atoms. Metals are ductile and good conductors of electricity due to the free movement of delocalized valence electrons between metal cations. Alloys can have superior properties to their component elements.
This document provides an overview of chemical bonding and ionic compounds. It discusses the ionic bond model, where ions are formed through the transfer of electrons between atoms. Metals tend to lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions. Ionic compounds are formed when cations and anions combine in ratios that result in an electrically neutral compound. The structures and names of ionic compounds are also covered.
1) Atoms form chemical bonds in order to attain a stable electron configuration with 8 valence electrons, known as an octet.
2) There are three main types of bonds: ionic bonds form when atoms transfer electrons to become ions, covalent bonds form when atoms share electrons, and metallic bonds involve delocalized electrons distributed among positively charged metal ions.
3) Whether a bond is ionic or covalent depends on the electronegativity of the atoms involved - ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals.
This document provides an overview of chemical bonding and the covalent bond model. It begins by defining a covalent bond and comparing it to ionic bonding. It then discusses Lewis structures and how they represent shared electron pairs in covalent bonds. The document outlines different types of covalent bonds (single, double, triple) and how many bonds an atom will form based on its valence electrons. It also discusses molecular geometry and the VSEPR model for predicting molecular shapes. Additional sections cover bond polarity, molecular polarity, and naming binary molecular compounds.
The document discusses the octet rule in covalent bonding. It states that in covalent bonds, electron sharing usually occurs so that atoms attain the electron configuration of noble gases, with eight electrons in their outer shell. Atoms can form single, double or triple bonds to reach an octet. Single bonds involve one shared pair of electrons, double bonds two shared pairs, and triple bonds three shared pairs. Examples like hydrogen gas, oxygen gas, carbon dioxide and nitrogen gas are provided to illustrate the different bond types. The octet rule explains the bonding in many covalent compounds composed of nonmetals.
The document discusses compounds, ions, and molecules. It explains that compounds form when elements bond together, and that bonding can occur through electron transfer (ionic bonds) or electron sharing (covalent bonds). Ionic bonding forms ionic compounds, while covalent bonding forms molecular compounds. The document also covers how to write chemical formulas for ionic and molecular compounds based on ion charge balances or molecular prefixes, respectively.
This document discusses different types of chemical bonds: ionic bonds form when electrons are transferred between atoms, while covalent bonds form when electrons are shared between atoms. Ionic bonds occur between oppositely charged ions and result in crystalline solids with high melting points that conduct electricity when melted. Covalent bonds share electron pairs to achieve stability, and can be nonpolar or polar depending on electron distribution. Compounds formed by covalent bonding exist as gases, liquids or solids with low melting points and poor conductivity. Coordinate covalent bonds involve electron sharing where both electrons come from the same atom. Chemical bonding occurs for atoms to achieve stable electron configurations.
There are three main types of bonds: ionic bonds formed by electron transfer, covalent bonds formed by electron sharing, and metallic bonds formed by delocalization of electrons over a large area. Ionic compounds are made of ions and are called salts or crystals, while covalent compounds form by atoms sharing electrons to attain a noble gas configuration. Covalent bonds can be polar, with unequal electron sharing, or nonpolar with equal sharing. Molecular structures are determined by following steps to connect atoms with single or multiple bonds to complete valence shells. Covalent compounds generally exist as liquids or gases with low electrical conductivity and solubility compared to ionic compounds.
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.
The document discusses different types of chemical bonds including intramolecular and intermolecular forces. It defines ionic bonds as occurring between metal and non-metal atoms through the transfer of electrons, and covalent bonds as occurring between non-metal atoms through the sharing of electrons. The document also discusses metallic bonding, the octet rule, and provides examples of different ionic compounds.
chemical bonding and molecular structure class 11sarunkumar31
hybridisation, bonding and antiboding, dipole moment, VSPER theory, Molecular orbital diagram, Phosphorous pentachloride, ionic bond, bond order, bond enthalpy, bond dissociation, sp and sp2hybridisation, hydrogen bonding,electron pair,lone pair repulsion, resonance structure of ozone, how to find electron pair and lone pair, sp3 hybridization of methane.
The document provides information about ionic and covalent (molecular) bonding:
- Ionic bonds occur between metals and non-metals and involve the transfer of electrons. Covalent bonds occur between two non-metals and involve the sharing of electrons.
- Ionic compounds have high melting and boiling points and conduct electricity when melted or dissolved. Molecular compounds have lower melting and boiling points and do not conduct electricity.
- Ionic compounds exist as crystal lattices of ions, while molecular compounds exist as distinct molecules made of two or more nonmetal atoms bonded together.
This document discusses the properties and uses of covalent compounds. Some key points:
1) Covalent compounds have lower melting and boiling points than ionic compounds. They are also soft, flexible, and their molecules can easily move around.
2) Covalent compounds tend to be more flammable and not conduct electricity in water. They also aren't usually very soluble.
3) Many important substances like fuels, medicines, foods, and clothes contain covalent bonds between their elements. Covalent bonding explains the nature of substances.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
This document provides information about molecular and ionic compounds, including:
- Molecular compounds are formed by covalent bonds between nonmetal atoms, while ionic compounds involve metal and nonmetal atoms bonded by ionic bonds.
- Molecular formulas show the actual number and type of atoms in a molecule, while ionic formulas use the lowest whole number ratio.
- Covalent bonds are represented by electron dot structures that show how atoms share electrons to achieve stable configurations. Multiple and coordinate covalent bonds are also discussed.
- Polarity arises in polar covalent bonds due to unequal electron sharing. Polar molecules have dipole moments while intermolecular forces include hydrogen bonding, dipole-dipole interactions, and
Formation of covalent bonds
Formulas of molecular compounds
LEWIS STRUCTURE
Molecules of Elements
Molecules of Compounds
Non-Polar Covalent Bond
Polar Covalent Bond
Uses of Covalent bonds Real life application
This document discusses chemical bonding and the different types of bonds that can form between atoms. It describes how ionic bonds are formed via electron transfer between atoms, and covalent bonds are formed through electron sharing. The octet rule, where atoms gain, lose, or share electrons to achieve a noble gas configuration, is an important concept. Ionic compounds involve the formation of cations and anions, while covalent compounds share electrons between nonmetals. Covalent bonds can be polar, involving unequal electron sharing, or nonpolar with equal sharing. Coordinate or dative bonds also involve electron sharing, but with both electrons coming from the same atom.
This document provides information about covalent bonding including:
- Covalent bonds result from the sharing of valence electrons between nonmetal atoms.
- Molecules form when two or more atoms are bonded covalently. Diatomic molecules like O2, N2, and F2 contain two atoms of the same element bonded together.
- Single covalent bonds involve the sharing of one pair of electrons, double bonds two pairs, and triple bonds three pairs. Lewis structures are used to represent electron arrangements in molecules.
This document provides an overview of different types of bonds between atoms including ionic bonds, covalent bonds, and metallic bonds. It discusses the characteristics of each type of bond such as ionic bonds being crystalline, having high melting points, and being able to conduct electricity when molten. Covalent bonds are described as having definite shapes and being very strong. Molecular substances, network solids, polar vs. nonpolar covalent bonds, and coordinate covalent bonds are also summarized. Polyatomic ions and the geometric arrangements of electron pairs in molecules are defined. The document concludes with a review of the material presented.
This document summarizes different types of chemical bonds: covalent bonds formed by shared electrons between similar atoms, ionic bonds formed by attractions between oppositely charged ions, and metallic bonds formed when atoms share a "sea of electrons". It also discusses polar covalent bonds that occur between atoms with some difference in electronegativity, and intermolecular forces like hydrogen bonding and London dispersion forces. Key terms like crystal lattice, formula unit, and lattice energy are defined in the context of ionic bonds.
Trusted Execution Environment for Decentralized Process MiningLucaBarbaro3
Presentation of the paper "Trusted Execution Environment for Decentralized Process Mining" given during the CAiSE 2024 Conference in Cyprus on June 7, 2024.
Your One-Stop Shop for Python Success: Top 10 US Python Development Providersakankshawande
Simplify your search for a reliable Python development partner! This list presents the top 10 trusted US providers offering comprehensive Python development services, ensuring your project's success from conception to completion.
Digital Banking in the Cloud: How Citizens Bank Unlocked Their MainframePrecisely
Inconsistent user experience and siloed data, high costs, and changing customer expectations – Citizens Bank was experiencing these challenges while it was attempting to deliver a superior digital banking experience for its clients. Its core banking applications run on the mainframe and Citizens was using legacy utilities to get the critical mainframe data to feed customer-facing channels, like call centers, web, and mobile. Ultimately, this led to higher operating costs (MIPS), delayed response times, and longer time to market.
Ever-changing customer expectations demand more modern digital experiences, and the bank needed to find a solution that could provide real-time data to its customer channels with low latency and operating costs. Join this session to learn how Citizens is leveraging Precisely to replicate mainframe data to its customer channels and deliver on their “modern digital bank” experiences.
HCL Notes und Domino Lizenzkostenreduzierung in der Welt von DLAUpanagenda
Webinar Recording: https://www.panagenda.com/webinars/hcl-notes-und-domino-lizenzkostenreduzierung-in-der-welt-von-dlau/
DLAU und die Lizenzen nach dem CCB- und CCX-Modell sind für viele in der HCL-Community seit letztem Jahr ein heißes Thema. Als Notes- oder Domino-Kunde haben Sie vielleicht mit unerwartet hohen Benutzerzahlen und Lizenzgebühren zu kämpfen. Sie fragen sich vielleicht, wie diese neue Art der Lizenzierung funktioniert und welchen Nutzen sie Ihnen bringt. Vor allem wollen Sie sicherlich Ihr Budget einhalten und Kosten sparen, wo immer möglich. Das verstehen wir und wir möchten Ihnen dabei helfen!
Wir erklären Ihnen, wie Sie häufige Konfigurationsprobleme lösen können, die dazu führen können, dass mehr Benutzer gezählt werden als nötig, und wie Sie überflüssige oder ungenutzte Konten identifizieren und entfernen können, um Geld zu sparen. Es gibt auch einige Ansätze, die zu unnötigen Ausgaben führen können, z. B. wenn ein Personendokument anstelle eines Mail-Ins für geteilte Mailboxen verwendet wird. Wir zeigen Ihnen solche Fälle und deren Lösungen. Und natürlich erklären wir Ihnen das neue Lizenzmodell.
Nehmen Sie an diesem Webinar teil, bei dem HCL-Ambassador Marc Thomas und Gastredner Franz Walder Ihnen diese neue Welt näherbringen. Es vermittelt Ihnen die Tools und das Know-how, um den Überblick zu bewahren. Sie werden in der Lage sein, Ihre Kosten durch eine optimierte Domino-Konfiguration zu reduzieren und auch in Zukunft gering zu halten.
Diese Themen werden behandelt
- Reduzierung der Lizenzkosten durch Auffinden und Beheben von Fehlkonfigurationen und überflüssigen Konten
- Wie funktionieren CCB- und CCX-Lizenzen wirklich?
- Verstehen des DLAU-Tools und wie man es am besten nutzt
- Tipps für häufige Problembereiche, wie z. B. Team-Postfächer, Funktions-/Testbenutzer usw.
- Praxisbeispiele und Best Practices zum sofortigen Umsetzen
In the realm of cybersecurity, offensive security practices act as a critical shield. By simulating real-world attacks in a controlled environment, these techniques expose vulnerabilities before malicious actors can exploit them. This proactive approach allows manufacturers to identify and fix weaknesses, significantly enhancing system security.
This presentation delves into the development of a system designed to mimic Galileo's Open Service signal using software-defined radio (SDR) technology. We'll begin with a foundational overview of both Global Navigation Satellite Systems (GNSS) and the intricacies of digital signal processing.
The presentation culminates in a live demonstration. We'll showcase the manipulation of Galileo's Open Service pilot signal, simulating an attack on various software and hardware systems. This practical demonstration serves to highlight the potential consequences of unaddressed vulnerabilities, emphasizing the importance of offensive security practices in safeguarding critical infrastructure.
leewayhertz.com-AI in predictive maintenance Use cases technologies benefits ...alexjohnson7307
Predictive maintenance is a proactive approach that anticipates equipment failures before they happen. At the forefront of this innovative strategy is Artificial Intelligence (AI), which brings unprecedented precision and efficiency. AI in predictive maintenance is transforming industries by reducing downtime, minimizing costs, and enhancing productivity.
Ivanti’s Patch Tuesday breakdown goes beyond patching your applications and brings you the intelligence and guidance needed to prioritize where to focus your attention first. Catch early analysis on our Ivanti blog, then join industry expert Chris Goettl for the Patch Tuesday Webinar Event. There we’ll do a deep dive into each of the bulletins and give guidance on the risks associated with the newly-identified vulnerabilities.
Skybuffer AI: Advanced Conversational and Generative AI Solution on SAP Busin...Tatiana Kojar
Skybuffer AI, built on the robust SAP Business Technology Platform (SAP BTP), is the latest and most advanced version of our AI development, reaffirming our commitment to delivering top-tier AI solutions. Skybuffer AI harnesses all the innovative capabilities of the SAP BTP in the AI domain, from Conversational AI to cutting-edge Generative AI and Retrieval-Augmented Generation (RAG). It also helps SAP customers safeguard their investments into SAP Conversational AI and ensure a seamless, one-click transition to SAP Business AI.
With Skybuffer AI, various AI models can be integrated into a single communication channel such as Microsoft Teams. This integration empowers business users with insights drawn from SAP backend systems, enterprise documents, and the expansive knowledge of Generative AI. And the best part of it is that it is all managed through our intuitive no-code Action Server interface, requiring no extensive coding knowledge and making the advanced AI accessible to more users.
Dandelion Hashtable: beyond billion requests per second on a commodity serverAntonios Katsarakis
This slide deck presents DLHT, a concurrent in-memory hashtable. Despite efforts to optimize hashtables, that go as far as sacrificing core functionality, state-of-the-art designs still incur multiple memory accesses per request and block request processing in three cases. First, most hashtables block while waiting for data to be retrieved from memory. Second, open-addressing designs, which represent the current state-of-the-art, either cannot free index slots on deletes or must block all requests to do so. Third, index resizes block every request until all objects are copied to the new index. Defying folklore wisdom, DLHT forgoes open-addressing and adopts a fully-featured and memory-aware closed-addressing design based on bounded cache-line-chaining. This design offers lock-free index operations and deletes that free slots instantly, (2) completes most requests with a single memory access, (3) utilizes software prefetching to hide memory latencies, and (4) employs a novel non-blocking and parallel resizing. In a commodity server and a memory-resident workload, DLHT surpasses 1.6B requests per second and provides 3.5x (12x) the throughput of the state-of-the-art closed-addressing (open-addressing) resizable hashtable on Gets (Deletes).
Introduction of Cybersecurity with OSS at Code Europe 2024Hiroshi SHIBATA
I develop the Ruby programming language, RubyGems, and Bundler, which are package managers for Ruby. Today, I will introduce how to enhance the security of your application using open-source software (OSS) examples from Ruby and RubyGems.
The first topic is CVE (Common Vulnerabilities and Exposures). I have published CVEs many times. But what exactly is a CVE? I'll provide a basic understanding of CVEs and explain how to detect and handle vulnerabilities in OSS.
Next, let's discuss package managers. Package managers play a critical role in the OSS ecosystem. I'll explain how to manage library dependencies in your application.
I'll share insights into how the Ruby and RubyGems core team works to keep our ecosystem safe. By the end of this talk, you'll have a better understanding of how to safeguard your code.
TrustArc Webinar - 2024 Global Privacy SurveyTrustArc
How does your privacy program stack up against your peers? What challenges are privacy teams tackling and prioritizing in 2024?
In the fifth annual Global Privacy Benchmarks Survey, we asked over 1,800 global privacy professionals and business executives to share their perspectives on the current state of privacy inside and outside of their organizations. This year’s report focused on emerging areas of importance for privacy and compliance professionals, including considerations and implications of Artificial Intelligence (AI) technologies, building brand trust, and different approaches for achieving higher privacy competence scores.
See how organizational priorities and strategic approaches to data security and privacy are evolving around the globe.
This webinar will review:
- The top 10 privacy insights from the fifth annual Global Privacy Benchmarks Survey
- The top challenges for privacy leaders, practitioners, and organizations in 2024
- Key themes to consider in developing and maintaining your privacy program
Skybuffer SAM4U tool for SAP license adoptionTatiana Kojar
Manage and optimize your license adoption and consumption with SAM4U, an SAP free customer software asset management tool.
SAM4U, an SAP complimentary software asset management tool for customers, delivers a detailed and well-structured overview of license inventory and usage with a user-friendly interface. We offer a hosted, cost-effective, and performance-optimized SAM4U setup in the Skybuffer Cloud environment. You retain ownership of the system and data, while we manage the ABAP 7.58 infrastructure, ensuring fixed Total Cost of Ownership (TCO) and exceptional services through the SAP Fiori interface.
HCN – linear, 180 o PH 3 – trigonal pyramid, 107 o O 3 – bent, 120 o
Generally speaking, the electronegativity increases in going from left to right across a period because the number of protons increases which increases the effective nuclear charge. The electronegativity decreases going down a group because the size of the atoms increases as you go down so when other electrons approach the larger atoms, the effective nuclear charge is not as great due to shielding from the current electrons present.
The fluorine has more attraction for an electron than does lithium. Both have valence electrons in the same principal energy level (the 2nd), but fluorine has a greater number of protons in the nucleus. Electrons are more attracted to a larger nucleus (if the principal energy level is the same). The fluorine also has more attraction for an electron than does iodine. In this case the nuclear charge of iodine is greater, but the valence electrons are at a much higher principal energy level (and the inner electrons shield the outer electrons).
The greater the electronegativity difference between the atoms, the more polar the bond. C-F, N-F, O-F Si-F, C-F, N-O B-Cl, S-Cl, Cl-Cl
The correct answer is N-O. To be considered polar covalent, unequal sharing of electrons must still occur. Choose the bond with the least difference in electronegativity yet there is still some unequal sharing of electrons.
The correct answer is Si-O. To not be considered ionic, generally the bond needs to be between two nonmetals. The most polar bond between the nonmetals occurs with the bond that has the greatest difference in electronegativity.
False, a molecule may have polar bonds (like CO 2 ) but the individual dipoles might cancel out so that the net dipole moment is zero.
HF, NH 3 , SO 2
The correct name for P 2 O 5 is diphosphorus pentoxide.