This document discusses how researchers used chemical bonding theories and models to develop drugs that treat HIV/AIDS. It explains that:
1) In the 1980s, researchers discovered the structure of the HIV protease protein and used bonding models to simulate how potential drugs might interact with it.
2) This allowed drug companies to design protease inhibitor molecules that disable the protease protein, preventing HIV from spreading.
3) Clinical trials showed these protease inhibitors, taken in combination with other drugs, reduced viral levels in HIV patients to undetectable amounts. While not a cure, the drugs allow those treated to have near-normal lifespans.
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 discusses chemical bonding and different types of bonds and structures. It explains that ionic bonds form between metals and non-metals via the transfer of electrons, giving ionic compounds high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds form between non-metals by the sharing of electrons, resulting in molecular compounds with low melting points that do not conduct electricity. It also describes macromolecular and metallic bonding, noting that structures like diamond, graphite and metals have high melting points due to their extended lattice structures held together by strong bonds or interactions between particles.
This document discusses chemical bonding and molecular structure. It begins by describing ionic and covalent bonding, including how molecular orbitals form through the overlap of atomic orbitals. It then discusses how valence electron Lewis dot structures are used to represent electron distribution in molecules as bond pairs and lone pairs. Rules for constructing Lewis structures, such as the octet rule, are covered. Exceptions to the octet rule for certain elements are also explained. Finally, the concept of resonance structures and using formal charges to determine the most important Lewis structure are introduced.
The document discusses the formation of compounds through chemical bonding. It explains that compounds form when atoms bond through electron sharing or transfer between elements. Atoms can form ionic bonds when a metal reacts with a non-metal, with the metal atom donating electrons to form positive ions and the non-metal accepting electrons to form negative ions. Compounds of non-metals form molecular bonds through covalent bonding where atoms share electrons. Bonding determines a compound's properties which differ from the original elements. Formulas represent the atoms in a compound's molecules.
The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and dative covalent bonding. Ionic bonding involves electron transfer between metals and nonmetals to form ionic compounds with electrostatic attraction between cations and anions. Covalent bonding involves sharing of electron pairs between atoms. Sigma and pi bonds are discussed as well as dot-and-cross diagrams and Lewis structures. Dative covalent bonding occurs when both electrons in a covalent bond come from the same atom, such as in a coordinate bond where a donor atom provides both electrons.
Atoms form bonds to achieve stable electron configurations. Covalent bonds form when atoms share valence electrons to fill their outer shells. Different bonding structures lead to varied properties. Diamond has a giant covalent structure where each carbon atom bonds to four others in a 3D network, giving it properties like hardness. Graphite also contains carbon but its layers can slide due to weaker bonds between layers, making it soft.
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.
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 discusses chemical bonding and different types of bonds and structures. It explains that ionic bonds form between metals and non-metals via the transfer of electrons, giving ionic compounds high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds form between non-metals by the sharing of electrons, resulting in molecular compounds with low melting points that do not conduct electricity. It also describes macromolecular and metallic bonding, noting that structures like diamond, graphite and metals have high melting points due to their extended lattice structures held together by strong bonds or interactions between particles.
This document discusses chemical bonding and molecular structure. It begins by describing ionic and covalent bonding, including how molecular orbitals form through the overlap of atomic orbitals. It then discusses how valence electron Lewis dot structures are used to represent electron distribution in molecules as bond pairs and lone pairs. Rules for constructing Lewis structures, such as the octet rule, are covered. Exceptions to the octet rule for certain elements are also explained. Finally, the concept of resonance structures and using formal charges to determine the most important Lewis structure are introduced.
The document discusses the formation of compounds through chemical bonding. It explains that compounds form when atoms bond through electron sharing or transfer between elements. Atoms can form ionic bonds when a metal reacts with a non-metal, with the metal atom donating electrons to form positive ions and the non-metal accepting electrons to form negative ions. Compounds of non-metals form molecular bonds through covalent bonding where atoms share electrons. Bonding determines a compound's properties which differ from the original elements. Formulas represent the atoms in a compound's molecules.
The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and dative covalent bonding. Ionic bonding involves electron transfer between metals and nonmetals to form ionic compounds with electrostatic attraction between cations and anions. Covalent bonding involves sharing of electron pairs between atoms. Sigma and pi bonds are discussed as well as dot-and-cross diagrams and Lewis structures. Dative covalent bonding occurs when both electrons in a covalent bond come from the same atom, such as in a coordinate bond where a donor atom provides both electrons.
Atoms form bonds to achieve stable electron configurations. Covalent bonds form when atoms share valence electrons to fill their outer shells. Different bonding structures lead to varied properties. Diamond has a giant covalent structure where each carbon atom bonds to four others in a 3D network, giving it properties like hardness. Graphite also contains carbon but its layers can slide due to weaker bonds between layers, making it soft.
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.
For Chem 1:
Significanceof the ELectron in Bonding
The Octet Rule
Lewis Symbol/Structures
Formal Charge
Polyatomic Ions
Types of Bonds (Ionic, Covalent, Coordinate Covalent, Metallic Bonds, Multiple Bonds)
Exceptions to the Octet Rules
Oxidation Number is not included in the class discussion and exam. ;D
Interactive textbook ch. 13 chemical bondingtiffanysci
Ionic bonds form when valence electrons are transferred from metal atoms to nonmetal atoms, resulting in positively charged metal ions and negatively charged nonmetal ions that are attracted to each other. Metal atoms easily lose electrons to achieve stable full outer energy levels, while nonmetal atoms gain electrons for the same reason. The ions associate in repeating three-dimensional crystal lattices to form solid ionic compounds that are brittle with high melting points and often dissolve in water.
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.
The document summarizes different types of chemical bonding:
1. Ionic bonding results from the attraction between oppositely charged ions
2. Covalent bonding results from the sharing of electron pairs between atoms
3. Metallic bonding allows for electron delocalization and mobility in metal solids due to overlapping vacant orbitals, contributing to metals' electrical and thermal conductivity properties.
This document contains a chemistry worksheet with 17 activities about chemical bonds. The activities cover topics such as ion formation, Lewis structures, ionic compounds, molecular compounds, conductivity, valence electrons, and crystal structures. Students are tasked with identifying cations and anions, writing formulas, explaining differences in properties, and completing other exercises about chemical bonding concepts.
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.
The document discusses chemical bonding and different types of bonds that join atoms together to form compounds. It begins by explaining that atoms combine to attain stable noble gas configurations, often through gaining or losing electrons to achieve 8 electrons in their outer shell.
It then describes ionic bonding specifically, where atoms transfer electrons to attain stable configurations. Sodium loses an electron to form Na+ while chlorine gains an electron to form Cl-, and the oppositely charged ions are held together by electrostatic attraction to form NaCl. Ionic compounds have high melting points, conduct electricity when molten or dissolved, and are generally soluble in water but not organic solvents.
The document also provides examples of other ionic compounds formed by electron
A bond is formed when two or more atoms join together through sharing or exchanging electrons to achieve stability. A molecule is two or more bonded atoms, and a substance can be either a pure element or compound made of two or more elements. There are two main types of bonds: covalent bonds formed by sharing electrons between nonmetals and ionic bonds formed by a transfer of electrons between a metal and nonmetal. The periodic table arranges elements and can provide information about their valence electrons and reactivity through bonding properties.
This document defines key terms related to chemical bonds and discusses how atoms bond to achieve stable electron configurations. It explains that atoms form ions by gaining or losing electrons to achieve a full outer electron shell like noble gases. Metals typically lose electrons to form positive ions while nonmetals gain electrons to form negative ions. These oppositely charged ions then form ionic bonds. The document also describes how nonmetal atoms can form covalent bonds by sharing electrons to achieve full outer shells. Polyatomic ions, which are groups of bonded atoms that act as a single unit, are presented and examples are given of how they form ionic bonds with metals through electron transfer.
Metals form metallic bonds when their valence electrons are released and move freely around the positively charged metal ions, creating a "sea of electrons". This sea of delocalized electrons is what gives metals their characteristic properties like malleability, ductility, luster, and high electrical and thermal conductivity. Alloys are mixtures of metals that are generally stronger yet less reactive than their pure metal components due to the metallic bonding between different kinds of metal atoms and ions.
The document discusses theories of covalent bonding including valence shell electron pair repulsion theory, valence bond theory, orbital hybridization, and molecular orbital theory. It focuses on how orbitals overlap to form bonds between atoms and the different types of hybrid orbitals that can form based on electron domain geometry. Examples are provided to illustrate sp, sp2, sp3, and other hybrid orbitals as well as sigma and pi bonding including delocalized pi bonding in benzene.
Covalent bonds form when atoms share electrons to complete their outer electron shells. Covalent compounds are typically made of nonmetal atoms. Binary covalent compounds contain only two elements. Their names follow specific rules based on element position in the periodic table. Molecular shape is determined by VSEPR theory, which predicts the geometry that minimizes electron pair repulsions. Polar covalent bonds result from unequal electron sharing between atoms of different electronegativity. Molecular polarity depends on both bond polarity and molecular geometry.
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are measures used to describe solutions.
csonn t1 atoms, molecules and stoichiometrycheeshengonn
Here are the key steps to solve this problem:
1) Isotope 35Cl has a relative abundance of 75.8%
2) Isotope 37Cl has a relative abundance of 24.2%
3) The relative atomic mass of 35Cl is 35 amu
4) The relative atomic mass of 37Cl is 37 amu
5) Use the formula: Relative Atomic Mass = Σ (Relative Abundance of isotope x Atomic Mass of isotope)
6) For 35Cl: Relative Abundance = 75.8%, Atomic Mass = 35 amu. So, contribution is 75.8% of 35 = 26.43
7) For 37Cl: Relative Abundance = 24
The document summarizes Dalton's atomic theory and provides information about atomic structure and subatomic particles. It discusses Dalton's four main postulates, including that atoms are indivisible and atoms of different elements combine in whole number ratios. The document also outlines the discoveries of key subatomic particles like electrons, protons, and neutrons by scientists such as Thomson, Rutherford, and Chadwick. It describes Bohr's model of the atom and introduces concepts like orbitals, electron configuration, and quantum numbers.
This document discusses the electronic configuration of carbon and how it forms bonds. It explains that carbon normally forms four single bonds by undergoing sp3 hybridization, where one 2s orbital and three 2p orbitals combine to form four new hybrid orbitals oriented toward the corners of a tetrahedron. It also discusses sp2 and sp hybridization which allow carbon to form multiple and triple bonds. The document contrasts primary covalent, ionic, and coordinate covalent bonds from secondary bonds formed by hydrogen bonding and van der Waals forces.
This document provides an introduction to organic chemistry concepts. It discusses:
1. The history of organic chemistry and the distinction between organic and inorganic compounds.
2. Key concepts in atomic structure like atomic number, mass, isotopes and electronic configurations.
3. Bonding theories including ionic, covalent and molecular orbital theory. Concepts like sigma bonds, pi bonds and hybridization are explained.
4. Acid-base theories including Bronsted-Lowry definitions, pH, acid dissociation constants (Ka) and how structure affects acidity.
This document summarizes key concepts from Chapter 9 of Chemistry: A Molecular Approach, 2nd Ed. by Nivaldo Tro, including:
- Lewis bonding theory uses valence electrons to explain how atoms bond by transferring or sharing electrons to achieve stable electron configurations like noble gases.
- Ionic bonds form when a metal transfers valence electrons to a nonmetal, creating oppositely charged ions that are attracted in a crystal lattice.
- Covalent bonds form when nonmetals share valence electrons to achieve stable configurations.
- The octet rule and Lewis dot structures can predict molecular geometry and polarity.
- Lattice energy released in crystal formation explains why ionic compounds are more stable than separate ions.
Review of Bonding and Lewis Structures for Organic Chemistrypotterjf
This document provides an overview of bonding and Lewis structures in organic chemistry. It discusses the two main types of bonding - ionic and covalent - and how they are determined by an element's location on the periodic table. Covalent bonds form when atoms share electrons to achieve stable noble gas configurations. Lewis structures use electron dot diagrams to represent bonding in molecules according to three rules: valence electrons are drawn, no more than eight electrons around second row elements, and two electrons around hydrogen. Formal charge is used to track electron distribution and identify common bonding patterns for carbon, nitrogen, and oxygen. Exceptions to the octet rule include hydrogen and certain third period and later elements.
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.
For Chem 1:
Significanceof the ELectron in Bonding
The Octet Rule
Lewis Symbol/Structures
Formal Charge
Polyatomic Ions
Types of Bonds (Ionic, Covalent, Coordinate Covalent, Metallic Bonds, Multiple Bonds)
Exceptions to the Octet Rules
Oxidation Number is not included in the class discussion and exam. ;D
Interactive textbook ch. 13 chemical bondingtiffanysci
Ionic bonds form when valence electrons are transferred from metal atoms to nonmetal atoms, resulting in positively charged metal ions and negatively charged nonmetal ions that are attracted to each other. Metal atoms easily lose electrons to achieve stable full outer energy levels, while nonmetal atoms gain electrons for the same reason. The ions associate in repeating three-dimensional crystal lattices to form solid ionic compounds that are brittle with high melting points and often dissolve in water.
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.
The document summarizes different types of chemical bonding:
1. Ionic bonding results from the attraction between oppositely charged ions
2. Covalent bonding results from the sharing of electron pairs between atoms
3. Metallic bonding allows for electron delocalization and mobility in metal solids due to overlapping vacant orbitals, contributing to metals' electrical and thermal conductivity properties.
This document contains a chemistry worksheet with 17 activities about chemical bonds. The activities cover topics such as ion formation, Lewis structures, ionic compounds, molecular compounds, conductivity, valence electrons, and crystal structures. Students are tasked with identifying cations and anions, writing formulas, explaining differences in properties, and completing other exercises about chemical bonding concepts.
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.
The document discusses chemical bonding and different types of bonds that join atoms together to form compounds. It begins by explaining that atoms combine to attain stable noble gas configurations, often through gaining or losing electrons to achieve 8 electrons in their outer shell.
It then describes ionic bonding specifically, where atoms transfer electrons to attain stable configurations. Sodium loses an electron to form Na+ while chlorine gains an electron to form Cl-, and the oppositely charged ions are held together by electrostatic attraction to form NaCl. Ionic compounds have high melting points, conduct electricity when molten or dissolved, and are generally soluble in water but not organic solvents.
The document also provides examples of other ionic compounds formed by electron
A bond is formed when two or more atoms join together through sharing or exchanging electrons to achieve stability. A molecule is two or more bonded atoms, and a substance can be either a pure element or compound made of two or more elements. There are two main types of bonds: covalent bonds formed by sharing electrons between nonmetals and ionic bonds formed by a transfer of electrons between a metal and nonmetal. The periodic table arranges elements and can provide information about their valence electrons and reactivity through bonding properties.
This document defines key terms related to chemical bonds and discusses how atoms bond to achieve stable electron configurations. It explains that atoms form ions by gaining or losing electrons to achieve a full outer electron shell like noble gases. Metals typically lose electrons to form positive ions while nonmetals gain electrons to form negative ions. These oppositely charged ions then form ionic bonds. The document also describes how nonmetal atoms can form covalent bonds by sharing electrons to achieve full outer shells. Polyatomic ions, which are groups of bonded atoms that act as a single unit, are presented and examples are given of how they form ionic bonds with metals through electron transfer.
Metals form metallic bonds when their valence electrons are released and move freely around the positively charged metal ions, creating a "sea of electrons". This sea of delocalized electrons is what gives metals their characteristic properties like malleability, ductility, luster, and high electrical and thermal conductivity. Alloys are mixtures of metals that are generally stronger yet less reactive than their pure metal components due to the metallic bonding between different kinds of metal atoms and ions.
The document discusses theories of covalent bonding including valence shell electron pair repulsion theory, valence bond theory, orbital hybridization, and molecular orbital theory. It focuses on how orbitals overlap to form bonds between atoms and the different types of hybrid orbitals that can form based on electron domain geometry. Examples are provided to illustrate sp, sp2, sp3, and other hybrid orbitals as well as sigma and pi bonding including delocalized pi bonding in benzene.
Covalent bonds form when atoms share electrons to complete their outer electron shells. Covalent compounds are typically made of nonmetal atoms. Binary covalent compounds contain only two elements. Their names follow specific rules based on element position in the periodic table. Molecular shape is determined by VSEPR theory, which predicts the geometry that minimizes electron pair repulsions. Polar covalent bonds result from unequal electron sharing between atoms of different electronegativity. Molecular polarity depends on both bond polarity and molecular geometry.
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are measures used to describe solutions.
csonn t1 atoms, molecules and stoichiometrycheeshengonn
Here are the key steps to solve this problem:
1) Isotope 35Cl has a relative abundance of 75.8%
2) Isotope 37Cl has a relative abundance of 24.2%
3) The relative atomic mass of 35Cl is 35 amu
4) The relative atomic mass of 37Cl is 37 amu
5) Use the formula: Relative Atomic Mass = Σ (Relative Abundance of isotope x Atomic Mass of isotope)
6) For 35Cl: Relative Abundance = 75.8%, Atomic Mass = 35 amu. So, contribution is 75.8% of 35 = 26.43
7) For 37Cl: Relative Abundance = 24
The document summarizes Dalton's atomic theory and provides information about atomic structure and subatomic particles. It discusses Dalton's four main postulates, including that atoms are indivisible and atoms of different elements combine in whole number ratios. The document also outlines the discoveries of key subatomic particles like electrons, protons, and neutrons by scientists such as Thomson, Rutherford, and Chadwick. It describes Bohr's model of the atom and introduces concepts like orbitals, electron configuration, and quantum numbers.
This document discusses the electronic configuration of carbon and how it forms bonds. It explains that carbon normally forms four single bonds by undergoing sp3 hybridization, where one 2s orbital and three 2p orbitals combine to form four new hybrid orbitals oriented toward the corners of a tetrahedron. It also discusses sp2 and sp hybridization which allow carbon to form multiple and triple bonds. The document contrasts primary covalent, ionic, and coordinate covalent bonds from secondary bonds formed by hydrogen bonding and van der Waals forces.
This document provides an introduction to organic chemistry concepts. It discusses:
1. The history of organic chemistry and the distinction between organic and inorganic compounds.
2. Key concepts in atomic structure like atomic number, mass, isotopes and electronic configurations.
3. Bonding theories including ionic, covalent and molecular orbital theory. Concepts like sigma bonds, pi bonds and hybridization are explained.
4. Acid-base theories including Bronsted-Lowry definitions, pH, acid dissociation constants (Ka) and how structure affects acidity.
This document summarizes key concepts from Chapter 9 of Chemistry: A Molecular Approach, 2nd Ed. by Nivaldo Tro, including:
- Lewis bonding theory uses valence electrons to explain how atoms bond by transferring or sharing electrons to achieve stable electron configurations like noble gases.
- Ionic bonds form when a metal transfers valence electrons to a nonmetal, creating oppositely charged ions that are attracted in a crystal lattice.
- Covalent bonds form when nonmetals share valence electrons to achieve stable configurations.
- The octet rule and Lewis dot structures can predict molecular geometry and polarity.
- Lattice energy released in crystal formation explains why ionic compounds are more stable than separate ions.
Review of Bonding and Lewis Structures for Organic Chemistrypotterjf
This document provides an overview of bonding and Lewis structures in organic chemistry. It discusses the two main types of bonding - ionic and covalent - and how they are determined by an element's location on the periodic table. Covalent bonds form when atoms share electrons to achieve stable noble gas configurations. Lewis structures use electron dot diagrams to represent bonding in molecules according to three rules: valence electrons are drawn, no more than eight electrons around second row elements, and two electrons around hydrogen. Formal charge is used to track electron distribution and identify common bonding patterns for carbon, nitrogen, and oxygen. Exceptions to the octet rule include hydrogen and certain third period and later elements.
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 discusses different types of chemical bonds, including ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, forming oppositely charged ions that are attracted in a crystal lattice. Covalent bonds involve the sharing of electrons between nonmetal atoms. Lewis structures can represent electron and bond arrangements in molecules and ions using dots and lines. The octet rule describes atoms' tendency to bond so they have eight electrons in their valence shell, like noble gases. Exceptions include hydrogen following the duet rule and structures with underfilled or overfilled octets.
Everyone seeks stability, which refers to resistance to change. Atoms also seek stability by obtaining a noble gas electron configuration with 8 outer electrons through bonding. The Lewis bonding theory states that atoms bond by transferring or sharing electrons to achieve stable configurations. There are different types of bonds including ionic bonds between metals and nonmetals formed by electron transfer, and covalent bonds between nonmetals formed by electron sharing to obtain octets.
Class 11 Chemistry Revision Notes Chemical Bonding and Molecular Structure.pdfNadishaFathima
This document discusses chemical bonding and molecular structure. It begins by introducing atoms, molecules, and the forces that hold atoms together in molecules. It then defines chemical bonding and describes the main types of bonds: ionic, covalent, hydrogen, and polar bonds. The remainder of the document discusses these bond types in more detail, including how to represent bonds using Lewis structures, the characteristics of ionic compounds, factors that influence ionic bond formation, and more. It also introduces concepts like formal charge, valence shell electron pair repulsion theory (VSEPR) for predicting molecular geometry, and hybridization.
This document discusses chemical bonding and molecular structure. It begins by explaining that atoms combine through chemical bonds to form molecules and different theories have sought to explain why certain combinations are possible and what determines molecular shapes. It then summarizes Kössel-Lewis approach to chemical bonding, which proposed that atoms achieve stability by gaining or sharing electrons to attain a full outer shell of 8 electrons. Covalent bonds are formed by shared pairs of electrons between atoms. Lewis structures use dots to represent valence electrons and predict molecular geometry.
The document discusses Lewis structures and covalent bonding. It provides steps for writing Lewis structures, including determining the molecular formula and connectivity, counting valence electrons, connecting atoms with bonds, adding electron pairs, checking for octets, and calculating formal charges. Constitutional isomers are described as isomers that differ in the order atoms are connected. Resonance structures are also discussed, where multiple Lewis structures can be written that differ in electron positions but have the same atomic positions.
Lewis symbols represent elements and their valence electrons using dots placed around the element's symbol. Elements form stable electron configurations by gaining, losing, or sharing electrons to match the configuration of the nearest noble gas. Ions are formed when elements gain or lose electrons during bonding to achieve stability. Anions are negatively charged ions formed when nonmetals gain electrons, while cations are positively charged ions formed when metals lose electrons. The type of bond (ionic, polar covalent, or nonpolar covalent) depends on the electronegativity difference between the elements.
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.
This document provides an introduction to biochemistry by discussing basic chemical principles like atomic structure, subatomic particles, isotopes, ionic bonds, covalent bonds, and molecular properties of water. It explains that biochemistry relies on an understanding of the chemistry of living systems, which are composed of chemical elements consisting of protons, neutrons, and electrons. The chemical properties of elements, including their ability to form ionic and covalent bonds, are determined by their electron configuration and electronegativity.
chap8lect_2015, perteneciente a fiisca del estado solido.pptJorgespw
The document summarizes key concepts in chemical bonding, including the three main types of bonds (ionic, covalent, and metallic), ionic bonding between metals and nonmetals, energetics of ionic bonding involving ionization energy, electron affinity, and lattice energy, properties of covalent bonding including polar covalent bonds and electronegativity, Lewis structures for representing covalent bonding including exceptions to the octet rule, and resonance structures.
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
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.
This document summarizes key concepts about ions, ionic bonding, and covalent bonding from chemistry. It defines ions as atoms that have gained or lost electrons, and discusses how ions bond to form ionic compounds like sodium chloride. It also explains how atoms can bond by sharing electrons in covalent bonds, including how bond polarity and molecular shape are determined. Chemical formulas and naming conventions for ionic and covalent compounds are presented.
The document discusses Lewis dot structures and how they are used to represent valence electrons in atoms and molecules. It provides examples of writing Lewis dot structures according to the octet rule, which states that atoms are most stable when their valence shells are filled with eight electrons. It also discusses how covalent bonds are formed by the sharing of valence electrons between atoms to achieve stable octet configurations. Key points covered include how to draw Lewis dot structures, count valence electrons, and distribute electrons to atoms following the octet rule.
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.
This document discusses different types of chemical bonds including ionic, covalent, and metallic bonds. It describes the formation of ionic bonds between metals and nonmetals and how ionization energy, electron affinity, and lattice energy contribute to the energetics of ionic bonding. Covalent bonding is explained as the sharing of electrons between nonmetals. Factors that determine bond polarity like electronegativity are also covered. The document provides details on writing Lewis structures, accounting for valence electrons and formal charges. Exceptions to the octet rule for molecules with odd numbers of electrons, incomplete octets, and expanded octets are explained.
Similar to 10lecture 150602233114-lva1-app6891 (20)
This document discusses suffixes and terminology used in medicine. It begins by listing common combining forms used to build medical terms and their meanings. It then defines several noun, adjective, and shorter suffixes and provides their meanings. Examples are given of medical terms built using combining forms and suffixes. The document also examines specific medical concepts in more depth, such as hernias, blood cells, acromegaly, splenomegaly, and laparoscopy.
The document is a chapter from a medical textbook that discusses anatomical terminology pertaining to the body as a whole. It defines the structural organization of the body from cells to tissues to organs to systems. It also describes the body cavities and identifies the major organs contained within each cavity, as well as anatomical divisions of the abdomen and back.
This document is from a textbook on medical terminology. It discusses the basic structure of medical words and how they are built from prefixes, suffixes, and combining forms. Some key points:
- Medical terms are made up of elements including roots, suffixes, prefixes, and combining vowels. Understanding these elements is important for analyzing terms.
- Common prefixes include hypo-, epi-, and cis-. Common suffixes include -itis, -algia, and -ectomy.
- Dozens of combining forms are provided, such as gastro- meaning stomach, cardi- meaning heart, and aden- meaning gland.
- Rules are provided for analyzing terms, such as reading from the suffix backward and dropping combining vowels before suffixes starting with vowels
This document is the copyright information for Chapter 25 on Cancer from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by a team that includes Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 24 on Immunology from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
Nerve cells, also known as neurons, are highly specialized cells that process and transmit information through electrical and chemical signals. This chapter discusses the structure and function of neurons, how they communicate with each other via synapses, and how signals are propagated along neurons through changes in their membrane potentials. Neurons play a vital role in the nervous system by allowing organisms to process information and coordinate their responses.
This document is the copyright information for Chapter 22 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "The Molecular Cell Biology of Development" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 21 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cell Birth, Lineage, and Death" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright page for Chapter 20 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Regulating the Eukaryotic Cell Cycle" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 19 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Integrating Cells into Tissues" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses microtubules and intermediate filaments, which are types of cytoskeletal filaments that help organize and move cellular components. Microtubules are involved in processes like cell division and intracellular transport, while intermediate filaments provide mechanical strength and help integrate the nucleus with the cytoplasm. Together, these filaments play important structural and functional roles in eukaryotic cells.
This chapter discusses microfilaments, which are one of the three main types of cytoskeletal filaments found in eukaryotic cells. Microfilaments are composed of actin filaments and play important roles in cell motility, structure, and intracellular transport. They allow cells to change shape and to move by contracting or extending parts of the cell surface.
This document is the copyright page for Chapter 16 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Signaling Pathways that Control Gene Activity" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright page for Chapter 15 of the 6th edition textbook "Molecular Cell Biology" by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira. It provides the chapter title "Cell Signaling I: Signal Transduction and Short-Term Cellular Responses" and notes the copyright is held by W. H. Freeman and Company in 2008.
This document is the copyright page for Chapter 14 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Vesicular Traffic, Secretion, and Endocytosis" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This chapter discusses how proteins are transported into membranes and organelles within cells. Proteins destined for membranes or organelles have targeting signals that are recognized by transport systems. The transport systems then direct the proteins to their proper destinations, such as inserting membrane proteins into membranes or delivering soluble proteins into organelles.
This document is the copyright information for Chapter 12 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cellular Energetics" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses the transmembrane transport of ions and small molecules across cell membranes. It covers topics such as passive transport through membrane channels and pumps, as well as active transport using ATP. The chapter is from the 6th edition of the textbook Molecular Cell Biology and is copyrighted by W. H. Freeman and Company in 2008.
This document is the copyright information for Chapter 10, titled "Biomembrane Structure", from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter was written by a team of authors including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright information for Chapter 9 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Visualizing, Fractionating, and Culturing Cells" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
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How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
The simplified electron and muon model, Oscillating Spacetime: The Foundation...RitikBhardwaj56
Discover the Simplified Electron and Muon Model: A New Wave-Based Approach to Understanding Particles delves into a groundbreaking theory that presents electrons and muons as rotating soliton waves within oscillating spacetime. Geared towards students, researchers, and science buffs, this book breaks down complex ideas into simple explanations. It covers topics such as electron waves, temporal dynamics, and the implications of this model on particle physics. With clear illustrations and easy-to-follow explanations, readers will gain a new outlook on the universe's fundamental nature.
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
Main Java[All of the Base Concepts}.docxadhitya5119
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM