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Metallic Bonding
Metallic bonding occurs when metal atoms lose valence electrons to become positively charged ions embedded in a "sea" of delocalized electrons. This electron sea model explains several properties of metals, including their ability to conduct electricity and heat, as well as their malleability, ductility, lustrous appearance, and high melting and boiling points. The mobile electrons allow for heat and charge conduction, while the metallic lattice structure enables atoms to slide past one another under pressure.
Metallic bonding
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.
Chemical bonding
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.
Electronegativity
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
covalent bond
This document discusses properties and uses of covalent compounds. It states that covalent compounds generally have lower melting and boiling points than ionic compounds. They are also more flexible, flammable, and less soluble in water than ionic compounds. The document notes that many fuels, medicines, clothes, and foods contain covalent bonds. It provides examples such as fuels powering daily life and clothes made from covalent materials. Covalent compounds share electrons between nonmetal atoms rather than transferring electrons.
Types Of Chemical Bonds- Ionic Bond,Covalent Bonds,Coordinate Bonds, Basic In...
The document discusses different types of chemical bonds formed by atoms to achieve stable inert gas electronic configurations:
1) Ionic bonds occur through complete electron transfer between atoms, making one positively charged and one negatively charged. The ions are then held together by electrostatic attraction.
2) Covalent bonds involve sharing of electrons between atoms of similar electronegativity to attain stable configurations.
3) Coordinate bonds are a type of covalent bond where both shared electrons are donated by one atom to an acceptor atom in need of electrons.
Atomic Structure and Bonding
The document discusses atomic structure and bonding. It covers subatomic particles like protons, neutrons and electrons. It defines atomic number and atomic mass. Electrons orbit the nucleus in energy levels. Ionic bonding occurs when atoms gain or lose electrons to achieve full outer shells, forming ions. Covalent bonding occurs when atoms share electrons. Ionic bonds are usually strong solids while covalent bonds are weaker liquids or gases.
Metallic bonds and the properties of metals
This document describes metallic bonding and the properties of metals and alloys. It explains that metallic bonding results from the delocalization of valence electrons among metal atoms, forming a "sea" of electrons. Metals are good conductors of heat and electricity due to the mobility of these electrons. The properties of a metal, such as its hardness and melting point, depend on the number of delocalized electrons. Alloys are mixtures of elements that are substitutional, with one metal replacing atoms of another, or interstitial, with smaller atoms filling holes in the metallic crystal structure.
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Metallic Bonding
Metallic bonding occurs when metal atoms lose valence electrons to become positively charged ions embedded in a "sea" of delocalized electrons. This electron sea model explains several properties of metals, including their ability to conduct electricity and heat, as well as their malleability, ductility, lustrous appearance, and high melting and boiling points. The mobile electrons allow for heat and charge conduction, while the metallic lattice structure enables atoms to slide past one another under pressure.
Metallic bonding
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.
Chemical bonding
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.
Electronegativity
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
covalent bond
This document discusses properties and uses of covalent compounds. It states that covalent compounds generally have lower melting and boiling points than ionic compounds. They are also more flexible, flammable, and less soluble in water than ionic compounds. The document notes that many fuels, medicines, clothes, and foods contain covalent bonds. It provides examples such as fuels powering daily life and clothes made from covalent materials. Covalent compounds share electrons between nonmetal atoms rather than transferring electrons.
Types Of Chemical Bonds- Ionic Bond,Covalent Bonds,Coordinate Bonds, Basic In...
The document discusses different types of chemical bonds formed by atoms to achieve stable inert gas electronic configurations:
1) Ionic bonds occur through complete electron transfer between atoms, making one positively charged and one negatively charged. The ions are then held together by electrostatic attraction.
2) Covalent bonds involve sharing of electrons between atoms of similar electronegativity to attain stable configurations.
3) Coordinate bonds are a type of covalent bond where both shared electrons are donated by one atom to an acceptor atom in need of electrons.
Atomic Structure and Bonding
The document discusses atomic structure and bonding. It covers subatomic particles like protons, neutrons and electrons. It defines atomic number and atomic mass. Electrons orbit the nucleus in energy levels. Ionic bonding occurs when atoms gain or lose electrons to achieve full outer shells, forming ions. Covalent bonding occurs when atoms share electrons. Ionic bonds are usually strong solids while covalent bonds are weaker liquids or gases.
Metallic bonds and the properties of metals
This document describes metallic bonding and the properties of metals and alloys. It explains that metallic bonding results from the delocalization of valence electrons among metal atoms, forming a "sea" of electrons. Metals are good conductors of heat and electricity due to the mobility of these electrons. The properties of a metal, such as its hardness and melting point, depend on the number of delocalized electrons. Alloys are mixtures of elements that are substitutional, with one metal replacing atoms of another, or interstitial, with smaller atoms filling holes in the metallic crystal structure.
Ionic bonding
The document discusses the determination of lattice energy of ionic compounds using the Born-Haber cycle. It explains that the lattice energy of sodium chloride can be determined experimentally by considering its formation through two different methods. Method 1 is the direct combination of solid sodium and gaseous chlorine to form solid sodium chloride. Method 2 involves 5 steps including sublimation, dissociation, ionization, and combining to form ions and the ionic solid. Using Hess's law, the lattice energy is calculated by equating the enthalpy change between the two methods. For sodium chloride, the calculated lattice energy is -773.95 kJ/mol.
Chemical Bond MANIK
The chemical Bond: Electronic concept of valency. Different types of chemical bond e.g. ionic, covalent, coordinate covalent metallic, dipole, hydrogen bond etc. Theories of covalent bonding and hybridization.
Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
Chemical bonding and molecular structure grade 11
this is a pure CBSE chapter powerpoint made by me..any quiries please contact me on deepika.jonnes@gmail.com
Chap 1-1 intra and intermolecular forces
Chromatography is a separation technique that exploits differences in how compounds partition between a stationary and mobile phase. Separation occurs based on differences in each compound's distribution constant (KD), which describes how much distributes into each phase. Key intermolecular forces like dipole-dipole interactions, hydrogen bonding, and dispersion forces affect KD values and thus chromatographic separation by influencing compound solubility and interactions. These same intermolecular forces also impact physical properties like boiling point.
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Periodic Trends
This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Chemical Bonding
This document discusses the four main types of chemical bonds: ionic bonds, covalent bonds, hydrogen bonds, and metallic bonds. Ionic bonds involve the transfer of electrons between atoms. Covalent bonds involve the sharing of electrons between two atoms. Hydrogen bonds are electrostatic attractions between hydrogen atoms covalently bonded to electronegative atoms and another electronegative atom. Metallic bonds are electrostatic attractions between positively charged metal ions and delocalized electrons in metals. Examples of each type of bond are provided.
Valence bond teory
Valence bond theory describes the formation of covalent bonds between atoms through the overlap of atomic orbitals and the sharing of electron pairs. There are two types of orbital overlaps - sigma bonds form from head-on overlap along the internuclear axis, while pi bonds form from side-by-side overlap perpendicular to the axis. The extent of orbital overlap determines the bond strength. Valence bond theory also explains the directional properties of bonds in molecules and the octet rule by which atoms seek to attain the stable electron configuration of the nearest noble gas.
Covalent bond
This document defines covalent bonding and discusses different types of covalent bonds. It provides examples of covalent bonds in molecules like H2O and H2. The types of covalent bonds covered are single, double, and triple bonds. Covalent bonds are also classified as polar or nonpolar depending on differences in electronegativity. Key properties of covalent compounds discussed are low melting and boiling points, poor electrical conductivity, flammability for those containing carbon and hydrogen, and soft or brittle solid forms.
2.1.3.1 octet rule
The octet rule states that atoms are most stable when their outer electron shells contain 8 electrons. Atoms attain this stable electron configuration by gaining, losing, or sharing electrons with other atoms so that their outer shells match the noble gas configuration. The rule applies mainly to nonmetals like carbon, nitrogen, oxygen, and halogens, and also some metals such as sodium and magnesium.
Resonance
A brief description of resonance, resonance structures and drawing rules, with examples acetone and 2,4-pentanedione.
Lattice energy
Lattice energy refers to the energy released when separate ions in the gas phase form an ionic crystal lattice. It can be calculated theoretically using the Born-Landé equation or experimentally using the Born-Haber cycle. The Born-Landé equation considers the electrostatic attraction and repulsive forces between ions, while the Born-Haber cycle uses standard enthalpy data and Hess's law. Lattice energy depends on factors like ion charge and size - higher charge or smaller ions lead to stronger electrostatic forces and higher lattice energy. Lattice energy is an important concept for understanding the properties and stability of ionic compounds.
Types of chemical bonds
Chemical bonds form when atoms share or transfer electrons. There are several main types of bonds:
- Ionic bonds form when metals transfer electrons to nonmetals to form positive and negative ions that are attracted to each other. Ionic compounds are crystalline and dissolve in water.
- Covalent bonds form when atoms share two or more valence electrons to achieve stability. Covalent bond strength depends on the number of electron pairs shared. Covalent compounds exist as discrete molecules.
- Metallic bonds result from the attraction between positively charged metal ions and delocalized electrons in the "sea of electrons" in the solid metal. Metallic bonding explains the properties of metals like conductivity.
Ionic Radius & its Trends
Ionic radius is calculated by measuring the distance between two ion nuclei according to their sizes. Cations have a smaller radius than their parent atoms due to electron loss increasing the effective nuclear charge. Anions have a larger radius than their parent atoms due to electron gain decreasing the effective nuclear charge. Ionic radius decreases across a period as proton number and effective nuclear charge increase, making the nucleus attract electrons more strongly. Ionic radius increases down a group as the energy level and shielding effect increase, weakening nuclear attraction.
VSEPR Theory and molecular geometries
VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry based on the repulsion of electron pairs in the valence shell of an atom. It states that electron pairs will adopt a geometry that minimizes repulsion by maximizing distance between electron pairs. The number and type of electron pairs (lone pairs or bond pairs) determines the molecular shape. Lone pairs occupy more space than bond pairs due to greater repulsion from the single nucleus. Molecular geometry can be distorted from ideal shapes by the presence of lone pairs.
Chemical bonding
This document discusses the three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals when the metal transfers electrons to the nonmetal. Covalent bonds form when atoms share electrons in either single, double or triple bonds. Metallic bonds form when metal atoms contribute electrons to form a "sea of electrons" that are shared between all the atoms.
Types of Chemical Bonds
This document discusses different types of chemical bonds including covalent bonds, ionic bonds, metallic bonds, and hydrogen bonds. It explains that a chemical bond is an attraction between atoms that allows the formation of compounds. Covalent bonds involve the sharing of electron pairs between atoms, while ionic bonds involve the complete transfer of electrons from one atom to another, resulting in positively and negatively charged ions. The document also discusses electronegativity and how differences in electronegativity between bonded atoms determine whether a bond is polar or nonpolar. Polar bonds result in partial charges on atoms and a dipole moment, while nonpolar bonds do not.
Chemical Bonds 1.ppt
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.
Electronegativity
Linus Pauling introduced the concept of electronegativity in 1932 to help explain the nature of chemical bonds. Electronegativity is a property that reflects an atom's ability to attract electrons in a bond. Atoms with high electronegativity strongly attract electrons, while atoms with low electronegativity attract electrons weakly. Whether a bond is ionic or covalent depends on the difference in electronegativity between the bonded atoms - a large difference leads to ionic bonds where one atom takes the electrons, while a small difference leads to covalent bonds where electrons are shared. Electronegativity values help predict bond type based on this principle.
Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Metallic Bond
Presentation on Metallic Bond and its nature, presented by Engineer S.M. Wahid Mahmud from Daffodil International University from the department of Electronics & Telecommunication, Faculty of Science & IT.
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Ionic bonding
The document discusses the determination of lattice energy of ionic compounds using the Born-Haber cycle. It explains that the lattice energy of sodium chloride can be determined experimentally by considering its formation through two different methods. Method 1 is the direct combination of solid sodium and gaseous chlorine to form solid sodium chloride. Method 2 involves 5 steps including sublimation, dissociation, ionization, and combining to form ions and the ionic solid. Using Hess's law, the lattice energy is calculated by equating the enthalpy change between the two methods. For sodium chloride, the calculated lattice energy is -773.95 kJ/mol.
Chemical Bond MANIK
The chemical Bond: Electronic concept of valency. Different types of chemical bond e.g. ionic, covalent, coordinate covalent metallic, dipole, hydrogen bond etc. Theories of covalent bonding and hybridization.
Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
Chemical bonding and molecular structure grade 11
this is a pure CBSE chapter powerpoint made by me..any quiries please contact me on deepika.jonnes@gmail.com
Chap 1-1 intra and intermolecular forces
Chromatography is a separation technique that exploits differences in how compounds partition between a stationary and mobile phase. Separation occurs based on differences in each compound's distribution constant (KD), which describes how much distributes into each phase. Key intermolecular forces like dipole-dipole interactions, hydrogen bonding, and dispersion forces affect KD values and thus chromatographic separation by influencing compound solubility and interactions. These same intermolecular forces also impact physical properties like boiling point.
Chemical bonding (UPDATED)
Chemical bonding
valence electrons
electronegativity
ionization energy
Lewis Dot
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Metallic Bond
Periodic Trends
This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Chemical Bonding
This document discusses the four main types of chemical bonds: ionic bonds, covalent bonds, hydrogen bonds, and metallic bonds. Ionic bonds involve the transfer of electrons between atoms. Covalent bonds involve the sharing of electrons between two atoms. Hydrogen bonds are electrostatic attractions between hydrogen atoms covalently bonded to electronegative atoms and another electronegative atom. Metallic bonds are electrostatic attractions between positively charged metal ions and delocalized electrons in metals. Examples of each type of bond are provided.
Valence bond teory
Valence bond theory describes the formation of covalent bonds between atoms through the overlap of atomic orbitals and the sharing of electron pairs. There are two types of orbital overlaps - sigma bonds form from head-on overlap along the internuclear axis, while pi bonds form from side-by-side overlap perpendicular to the axis. The extent of orbital overlap determines the bond strength. Valence bond theory also explains the directional properties of bonds in molecules and the octet rule by which atoms seek to attain the stable electron configuration of the nearest noble gas.
Covalent bond
This document defines covalent bonding and discusses different types of covalent bonds. It provides examples of covalent bonds in molecules like H2O and H2. The types of covalent bonds covered are single, double, and triple bonds. Covalent bonds are also classified as polar or nonpolar depending on differences in electronegativity. Key properties of covalent compounds discussed are low melting and boiling points, poor electrical conductivity, flammability for those containing carbon and hydrogen, and soft or brittle solid forms.
2.1.3.1 octet rule
The octet rule states that atoms are most stable when their outer electron shells contain 8 electrons. Atoms attain this stable electron configuration by gaining, losing, or sharing electrons with other atoms so that their outer shells match the noble gas configuration. The rule applies mainly to nonmetals like carbon, nitrogen, oxygen, and halogens, and also some metals such as sodium and magnesium.
Resonance
A brief description of resonance, resonance structures and drawing rules, with examples acetone and 2,4-pentanedione.
Lattice energy
Lattice energy refers to the energy released when separate ions in the gas phase form an ionic crystal lattice. It can be calculated theoretically using the Born-Landé equation or experimentally using the Born-Haber cycle. The Born-Landé equation considers the electrostatic attraction and repulsive forces between ions, while the Born-Haber cycle uses standard enthalpy data and Hess's law. Lattice energy depends on factors like ion charge and size - higher charge or smaller ions lead to stronger electrostatic forces and higher lattice energy. Lattice energy is an important concept for understanding the properties and stability of ionic compounds.
Types of chemical bonds
Chemical bonds form when atoms share or transfer electrons. There are several main types of bonds:
- Ionic bonds form when metals transfer electrons to nonmetals to form positive and negative ions that are attracted to each other. Ionic compounds are crystalline and dissolve in water.
- Covalent bonds form when atoms share two or more valence electrons to achieve stability. Covalent bond strength depends on the number of electron pairs shared. Covalent compounds exist as discrete molecules.
- Metallic bonds result from the attraction between positively charged metal ions and delocalized electrons in the "sea of electrons" in the solid metal. Metallic bonding explains the properties of metals like conductivity.
Ionic Radius & its Trends
Ionic radius is calculated by measuring the distance between two ion nuclei according to their sizes. Cations have a smaller radius than their parent atoms due to electron loss increasing the effective nuclear charge. Anions have a larger radius than their parent atoms due to electron gain decreasing the effective nuclear charge. Ionic radius decreases across a period as proton number and effective nuclear charge increase, making the nucleus attract electrons more strongly. Ionic radius increases down a group as the energy level and shielding effect increase, weakening nuclear attraction.
VSEPR Theory and molecular geometries
VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry based on the repulsion of electron pairs in the valence shell of an atom. It states that electron pairs will adopt a geometry that minimizes repulsion by maximizing distance between electron pairs. The number and type of electron pairs (lone pairs or bond pairs) determines the molecular shape. Lone pairs occupy more space than bond pairs due to greater repulsion from the single nucleus. Molecular geometry can be distorted from ideal shapes by the presence of lone pairs.
Chemical bonding
This document discusses the three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals when the metal transfers electrons to the nonmetal. Covalent bonds form when atoms share electrons in either single, double or triple bonds. Metallic bonds form when metal atoms contribute electrons to form a "sea of electrons" that are shared between all the atoms.
Types of Chemical Bonds
This document discusses different types of chemical bonds including covalent bonds, ionic bonds, metallic bonds, and hydrogen bonds. It explains that a chemical bond is an attraction between atoms that allows the formation of compounds. Covalent bonds involve the sharing of electron pairs between atoms, while ionic bonds involve the complete transfer of electrons from one atom to another, resulting in positively and negatively charged ions. The document also discusses electronegativity and how differences in electronegativity between bonded atoms determine whether a bond is polar or nonpolar. Polar bonds result in partial charges on atoms and a dipole moment, while nonpolar bonds do not.
Chemical Bonds 1.ppt
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.
Electronegativity
Linus Pauling introduced the concept of electronegativity in 1932 to help explain the nature of chemical bonds. Electronegativity is a property that reflects an atom's ability to attract electrons in a bond. Atoms with high electronegativity strongly attract electrons, while atoms with low electronegativity attract electrons weakly. Whether a bond is ionic or covalent depends on the difference in electronegativity between the bonded atoms - a large difference leads to ionic bonds where one atom takes the electrons, while a small difference leads to covalent bonds where electrons are shared. Electronegativity values help predict bond type based on this principle.
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Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Metallic Bond
Presentation on Metallic Bond and its nature, presented by Engineer S.M. Wahid Mahmud from Daffodil International University from the department of Electronics & Telecommunication, Faculty of Science & IT.
Chemical bonding Powerpoint
Chemical bonds form when atoms attract each other and bind together. There are three main types of bonds: ionic bonds form when a metal transfers electrons to a non-metal, metallic bonds involve delocalized electrons that move freely between metal atoms, and covalent bonds occur when two non-metals share pairs of electrons. Ionic bonds are strong but brittle, metallic bonds allow metals to conduct heat and electricity, and covalent bonds can be single, double or triple depending on how many electron pairs are shared.
Metallic bonds
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.
4-2 Ionic & Covalent Bonding
The document summarizes the key differences between ionic and covalent bonding. Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions. Covalent bonds form when nonmetals share electrons to obtain a full outer shell. Ionic compounds have high melting points, are brittle solids, and dissolve well in water, while covalent compounds have lower melting points, are soft and pliable, and are generally insoluble in water.
Properties of covalent substances, metals and ionic compounds
This document discusses the properties of three classes of substances: molecular substances, ionic compounds, and metallic solids. Molecular substances exist as gases, liquids, or solids depending on the strength of intermolecular forces between molecules. Ionic compounds form crystalline structures with positive and negative ions in repeating patterns, making them hard and brittle solids with high melting points. Metallic solids consist of layers of metal atoms that share delocalized valence electrons, giving metals properties like conductivity and malleability.
Lecture 7.3- Metallic Bonds
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.
Intermolecular Forces
1. Molecular polarity depends on whether the bonds within a molecule are polar and the overall molecular geometry.
2. CO2 is nonpolar because its linear geometry causes the polar bonds between carbon and oxygen to cancel out. H2O is polar because its bent shape does not allow bond dipoles to cancel out.
3. Forces that hold substances together include ionic bonds, covalent networks, and intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London forces.
Chemical bonds.ppt
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.
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole Attractions
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole AttractionsShaina Mavreen Villaroza
Intermolecular Forces
Van der Waals Forces (Johannes van der Waals)
Dipole-Dipole Attractions (Polar)
Dispersion Forces (Nonpolar and Polar, induced dipole)
- Dipole-induced (London Dispersion)
- Ion-inducedChemical bonding and molecular structure
This slides describes the different concepts of topic that come under chemical bonding and molecular structure
Hydrogen bonding
1. Hydrogen bonding occurs between hydrogen atoms attached to electronegative atoms like oxygen, fluorine, and nitrogen of one molecule and an electronegative atom of another molecule.
2. Water is able to form extensive hydrogen bonding networks between molecules due to each water molecule having two hydrogen atoms and two lone pairs of electrons on the oxygen atom.
3. The hydrogen bonding network in liquid water is responsible for its unique properties, while hydrogen bonding in ice forms its crystalline lattice structure.
types of chemical bonding
This document discusses three main types of chemical bonding: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between metals and nonmetals through the transfer of electrons from one atom to another, producing charged ions. Covalent bonds form between nonmetals of similar electronegativity through the sharing of electron pairs. Metallic bonds form between metallic elements through a shared "electron cloud" that holds the atoms together strongly.
Intermolecular forces
The document discusses different types of intermolecular forces including London dispersion forces, dipole-dipole forces, dipole-induced dipole forces, ion-dipole interactions, and hydrogen bonding. It provides examples of how these forces influence the properties of substances such as their melting and boiling points. Hydrogen bonding specifically is described as being an important intermolecular force that influences the properties of water, alcohols, and other polar molecules.
Tang 06 bond energy
- Chemical reactions involve breaking old bonds and forming new ones. Bond breaking requires energy and is endothermic, while bond formation releases energy and is exothermic.
- The bond energies table lists the average energy required to break common types of bonds. However, bond energies can vary depending on neighboring bonds.
- Reaction enthalpy change (ΔH) can be calculated by adding the bond energies of reactants and subtracting the bond energies of products. This was demonstrated for combustion reactions of ethanol and methoxymethane.
Metallic bonds
Metallic bonds form when metal atoms come together and their valence electrons move freely around the atomic nuclei, creating a "sea of electrons" that positively charged metal ions are suspended within. This bond structure allows metals to be malleable, ductile, shiny, electrically conductive, and thermally conductive. Alloys are mixtures of metals that are generally stronger than their pure metal components due to metallic bonding between different kinds of metal atoms.
interatomic bonds
Interatomic bonds determine the macroscopic properties of materials. Ionic bonds in ceramics result in high melting temperatures, elastic moduli, and low thermal expansion. Metallic bonds produce intermediate properties due to varying bond strengths. Covalent and secondary bonds in polymers lead to low melting points, moduli and high thermal expansion, with secondary bonds dominating behavior. Bonding energy correlates with melting temperature, while curvature relates to thermal expansion and initial elastic response.
Shape of molecules
To draw molecular structures, one should:
1. Draw the Lewis structures of components and make the most electronegative atoms outer atoms, except for hydrogen.
2. Ensure outer atoms have a full outer shell of 8 electrons using single, double, or triple bonds and charges.
3. Central atoms in period 2 can have up to 8 outer electrons, and period 3 atoms can have up to 18.
The VSEPR theory then predicts 3D structure by minimizing electron pair repulsion between outer shell electron pairs and lone pairs.
Bonding and Structure
The document discusses different types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between metals and non-metals to form ions. Covalent bonding involves the sharing of electron pairs between non-metals. Metallic bonding involves a sea of delocalized electrons that are attracted to cationic metal ions arranged in a lattice. Each type of bonding results in different material properties depending on whether electrons are transferred, shared, or free to move.
Chemistry - Chp 7 - Ionic and Metallic Bonding - Study Guide
This study guide covers topics about ionic and metallic bonding including:
- The definitions of valence and core electrons
- How to determine the number of valence electrons from the periodic table
- Writing electron dot diagrams for elements and ions
- The octet rule and gaining/losing electrons to satisfy it
- What kinds of ions metals form and how
- Comparing ion configurations to noble gases
- What forms ionic bonds and which elements can form them
- Writing formula units for ionic compounds and their overall charge
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