introduction to chemical bonding
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This document discusses three main types of chemical bonds: covalent bonds, ionic bonds, and metallic bonds. Covalent bonds involve the sharing of electron pairs between atoms, and can be single, double, or triple bonds. Ionic bonds form when electrons are transferred from a metal to a non-metal. Metallic bonds form between atoms in metallic elements through delocalized valence electrons that move freely through the metal lattice.
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Chemical bonding
Chemical bonding is the force of attraction between atoms that allows for the formation of molecules. There are two main types of chemical bonds: covalent bonds, which involve the sharing of valence electrons between atoms, and ionic bonds, which involve the transfer of electrons from one atom to another. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Lewis dot structures use dots to represent valence electrons and show atomic configurations.
Chemical bonding
This document summarizes the different types of chemical bonding: ionic bonding occurs between oppositely charged ions and is electrostatic in nature; covalent bonding involves sharing electrons between atoms and can range from partially ionic to completely covalent; metallic bonding is characterized by positive ions floating in a "sea" of delocalized electrons allowing metals to conduct electricity; van der Waals bonding is the weakest type and only present between inert gases due to induced dipole interactions. The document also discusses the different arrangements of spheres to model ion packing in cubic close, body-centered cubic, and hexagonal close packing of metals.
Chemical Bonding
Chemical Bonding and their properties
Ionic Bonding and their properties
Covalent Bonding and their proerties
Metallic Bonding and their properties
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.
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.
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.
Chemical bonding
This document discusses different types of chemical bonding: ionic bonding which involves the transfer of electrons between metals and non-metals and results in charged atoms attracting each other; covalent bonding which involves the sharing of electron pairs between atoms and can result in simple molecular or giant molecular structures; and metallic bonding which occurs between delocalized electrons in metal ions and positively charged metal ions. Each type of bonding is described along with examples and properties such as conductivity, melting/boiling points, and solubility.
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Chemical bonding
Chemical bonding is the force of attraction between atoms that allows for the formation of molecules. There are two main types of chemical bonds: covalent bonds, which involve the sharing of valence electrons between atoms, and ionic bonds, which involve the transfer of electrons from one atom to another. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Lewis dot structures use dots to represent valence electrons and show atomic configurations.
Chemical bonding
This document summarizes the different types of chemical bonding: ionic bonding occurs between oppositely charged ions and is electrostatic in nature; covalent bonding involves sharing electrons between atoms and can range from partially ionic to completely covalent; metallic bonding is characterized by positive ions floating in a "sea" of delocalized electrons allowing metals to conduct electricity; van der Waals bonding is the weakest type and only present between inert gases due to induced dipole interactions. The document also discusses the different arrangements of spheres to model ion packing in cubic close, body-centered cubic, and hexagonal close packing of metals.
Chemical Bonding
Chemical Bonding and their properties
Ionic Bonding and their properties
Covalent Bonding and their proerties
Metallic Bonding and their properties
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.
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.
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.
Chemical bonding
This document discusses different types of chemical bonding: ionic bonding which involves the transfer of electrons between metals and non-metals and results in charged atoms attracting each other; covalent bonding which involves the sharing of electron pairs between atoms and can result in simple molecular or giant molecular structures; and metallic bonding which occurs between delocalized electrons in metal ions and positively charged metal ions. Each type of bonding is described along with examples and properties such as conductivity, melting/boiling points, and solubility.
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The document discusses covalent bonding, which involves the sharing of electron pairs between atoms. It defines covalent bonding and explains that it usually forms between non-metals and can result in sigma or pi bonds depending on orbital overlapping. The document also describes different types of covalent bonds including single, double, triple, polar, non-polar, and dative bonds. Examples are provided for each bond type.
Types of Chemical bonds
This document provides an overview of different types of chemical bonds: ionic bonds, covalent bonds, coordinate covalent bonds, and metallic bonds. It defines each bond type, provides examples, and notes some key properties. Ionic bonds form when a metal transfers an electron to a nonmetal. Covalent bonds form through the sharing of electrons between two nonmetals or between atoms of different elements. Coordinate covalent bonds involve the sharing of an electron pair donated by one atom. Metallic bonds form a "sea of electrons" that holds metallic cations together. The document aims to clarify the concept of chemical bonding.
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.
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.
ppt chemical bonding
This document discusses three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds.
1. Ionic bonds form between metals and nonmetals by the transfer of electrons from one atom to another, resulting in positively and negatively charged ions.
2. Covalent bonds form between nonmetals of similar electronegativity by the sharing of electron pairs between atoms.
3. Metallic bonds form between metallic elements and involve a sea of electrons that hold the metal atoms together strongly.
Ionic, covalent, and metallic bonds
✔Here is an introduction to the Chemistry of Life, where you will learn about Ionic, Covalent and Metallic bonds. This presentation touches briefly, but it covers the definition of three major types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form due to the transfer of an electron from one atom to another. Covalent bonds involve the sharing of electrons between two atoms. Metallic bonds are formed by the attraction between metal ions and delocalized, or "free" electrons.✔
Here is a YouTube of this presentation:
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Chemical bonding (1)
Chemical bonding can occur via three main types: covalent, metallic, and ionic bonds. Covalent bonds form when atoms share pairs of electrons to attain stable electron configurations. Metallic bonds result from the delocalized electrons within metal atoms. Ionic bonds form when atoms transfer electrons completely, resulting in oppositely charged ions that are attracted via electrostatic forces.
Different types of chemical bonds
This document discusses the three main types of chemical bonds: ionic bonds, which form between metals and nonmetals and involve the transfer of electrons; covalent bonds, which involve the sharing of electron pairs between atoms; and metallic bonds in metals. Ionic bonds form crystalline structures in solids that do not conduct electricity well, but can conduct when molten or dissolved as ions move more freely. Covalent bonds involve the sharing of electron pairs and form very strong bonds between atoms.
Bonding in solids
This document discusses the different types of bonding in solids. There are two main categories - primary bonds and secondary bonds. Primary bonds include ionic bonding, where positive and negative ions attract; covalent bonding, where atoms share electrons; and metallic bonding, where loosely held electrons bond atoms. Secondary bonds are weaker and include hydrogen bonding between polar molecules and van der Waals bonding from induced dipoles between neutral molecules. Examples are provided for each type of bonding.
Types of bonding in solids
Ionic, covalent, metallic, hydrogen, and Van Der Wall's bonding are the main types of bonding. Ionic bonding occurs between positive and negative ions, covalent bonding involves sharing electrons between atoms, and metallic bonding involves loosely bound electrons in metal atoms that form an electron cloud. Hydrogen bonding arises from electrostatic attraction between hydrogen atoms partially charged by covalent bonds. Van Der Wall's bonding involves weak, temporary bonds between molecules of the same substance.
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Metallic bonds form between metal cations and delocalized electrons, allowing metals to conduct electricity. Organic compounds contain carbon and form covalent bonds, while inorganic compounds lack carbon and usually form ionic bonds between metals and nonmetals. Ionic bonds occur when atoms transfer electrons, and covalent bonds form when nonmetals share electrons equally. Electronegativity determines whether atoms form ionic or covalent bonds based on their ability to attract bonding electron pairs.
Chemical bonding
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a metal transfers electrons to a nonmetal, creating positively charged ions and negatively charged ions. Covalent bonds form when atoms share electrons as either single, double or triple bonds. Metallic bonds form a "sea of electrons" that are shared between positive metal ions throughout a crystalline structure.
Ionic bond
Ionic bonds form between oppositely charged ions. They result from the transfer of electrons from one atom to another. Ionic bonding typically occurs between metals and nonmetals. Metals tend to lose electrons to fill their outer shell, becoming positively charged ions, while nonmetals gain electrons to fill their outer shell, becoming negatively charged ions. The electrostatic attraction between the opposite charges of the ions forms the ionic bond.
Covalent bonds
Covalent bonds result from the sharing of valence electrons between two nonmetallic atoms. A single covalent bond forms when one pair of electrons is shared, while double and triple bonds share two or three pairs of electrons, respectively. Molecular structure and bond angles are determined by the VSEPR model, which predicts molecular geometry based on electron pair repulsion. Hybridization occurs when atomic orbitals mix to form new hybrid orbitals and explain molecular bonding orientations.
Chemical bonding by Saliha Rais
Chemical bonds are the forces that hold atoms together in molecules and crystals. There are two main types of bonds: ionic and covalent. Ionic bonds involve a complete transfer of electrons between atoms, giving one atom a positive charge and the other a negative charge. Covalent bonds involve sharing of electron pairs between atoms. Covalent bonding can involve single, double or triple bonds with one, two or three shared pairs respectively. Ionic compounds are usually solids with high melting points, while covalent compounds have lower melting points due to weaker intermolecular forces.
Covalent bond
This document defines and provides examples of covalent bonds. It discusses the history of the term being coined by Irving Langmuir in 1919. A covalent bond is defined as a chemical link where electrons are shared between two atoms. Examples given are the covalent bonds between oxygen and hydrogen in H2O and between hydrogen atoms in H2. The document also describes the different types of covalent bonds - single, double, and triple - based on the number of electron pairs shared between the bonded atoms.
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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.
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This document discusses chemical bonding. It defines chemical bonds as how most atoms are joined together in nature. It describes the two main types of chemical bonds: ionic bonding which results from the transfer of electrons between ions, and covalent bonding which results from the sharing of electron pairs between atoms. Atoms form chemical bonds to decrease their potential energy and become more stable. Bonds are rarely purely ionic or covalent, but instead exist on a spectrum depending on the electronegativity difference between the atoms.
Chemical Bonds
This document discusses different types of chemical bonds including ionic bonding, covalent bonding, and metallic bonding. Ionic bonding involves the electrostatic attraction between oppositely charged ions when atoms gain or lose electrons. Covalent bonding occurs when atoms share pairs of electrons to gain stability. Metallic bonding results from the attraction between positively charged atomic nuclei and delocalized electrons in metals that act as the binding medium. The importance of chemical bonding is that it allows atoms to join together to form molecules and structures with unique physical and chemical properties essential for life.
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This document summarizes different types of chemical bonds:
Ionic bonds form through electrostatic attraction between oppositely charged ions. Ionic compounds conduct electricity and have high boiling points. Covalent bonds share pairs of electrons between atoms. Metallic bonds constitute electrostatic forces between delocalized electrons in a "sea" of positive metal ions, giving metals high melting points. Alloys are mixtures of metals with constituents measured by mass that can be substitutional or interstitial in atomic arrangement.
Chemical Bonding.pptx
The document discusses different types of chemical bonds including ionic bonds, covalent bonds, and metallic bonds. Ionic bonds involve the transfer of electrons from a metal to a nonmetal, forming ionic compounds. Covalent bonds are formed when two nonmetals share electron pairs. There are also polar and nonpolar covalent bonds depending on the electronegativity difference between the atoms. Metallic bonds involve the collective sharing of valence electrons between metal ions. The document then has students identify types of bonds in example compounds such as NaCl, NO2, and CaO.
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The document discusses covalent bonding, which involves the sharing of electron pairs between atoms. It defines covalent bonding and explains that it usually forms between non-metals and can result in sigma or pi bonds depending on orbital overlapping. The document also describes different types of covalent bonds including single, double, triple, polar, non-polar, and dative bonds. Examples are provided for each bond type.
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This document provides an overview of different types of chemical bonds: ionic bonds, covalent bonds, coordinate covalent bonds, and metallic bonds. It defines each bond type, provides examples, and notes some key properties. Ionic bonds form when a metal transfers an electron to a nonmetal. Covalent bonds form through the sharing of electrons between two nonmetals or between atoms of different elements. Coordinate covalent bonds involve the sharing of an electron pair donated by one atom. Metallic bonds form a "sea of electrons" that holds metallic cations together. The document aims to clarify the concept of chemical bonding.
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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.
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.
ppt chemical bonding
This document discusses three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds.
1. Ionic bonds form between metals and nonmetals by the transfer of electrons from one atom to another, resulting in positively and negatively charged ions.
2. Covalent bonds form between nonmetals of similar electronegativity by the sharing of electron pairs between atoms.
3. Metallic bonds form between metallic elements and involve a sea of electrons that hold the metal atoms together strongly.
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✔Here is an introduction to the Chemistry of Life, where you will learn about Ionic, Covalent and Metallic bonds. This presentation touches briefly, but it covers the definition of three major types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form due to the transfer of an electron from one atom to another. Covalent bonds involve the sharing of electrons between two atoms. Metallic bonds are formed by the attraction between metal ions and delocalized, or "free" electrons.✔
Here is a YouTube of this presentation:
➡➡➡https://www.youtube.com/watch?v=8cRQjClbeas&feature=youtu.be
Check out more interesting posts on LabGirl:
➡➡➡ https://www.facebook.com/labgirldzd
Thank you! :)
Chemical bonding (1)
Chemical bonding can occur via three main types: covalent, metallic, and ionic bonds. Covalent bonds form when atoms share pairs of electrons to attain stable electron configurations. Metallic bonds result from the delocalized electrons within metal atoms. Ionic bonds form when atoms transfer electrons completely, resulting in oppositely charged ions that are attracted via electrostatic forces.
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This document discusses the three main types of chemical bonds: ionic bonds, which form between metals and nonmetals and involve the transfer of electrons; covalent bonds, which involve the sharing of electron pairs between atoms; and metallic bonds in metals. Ionic bonds form crystalline structures in solids that do not conduct electricity well, but can conduct when molten or dissolved as ions move more freely. Covalent bonds involve the sharing of electron pairs and form very strong bonds between atoms.
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This document discusses the different types of bonding in solids. There are two main categories - primary bonds and secondary bonds. Primary bonds include ionic bonding, where positive and negative ions attract; covalent bonding, where atoms share electrons; and metallic bonding, where loosely held electrons bond atoms. Secondary bonds are weaker and include hydrogen bonding between polar molecules and van der Waals bonding from induced dipoles between neutral molecules. Examples are provided for each type of bonding.
Types of bonding in solids
Ionic, covalent, metallic, hydrogen, and Van Der Wall's bonding are the main types of bonding. Ionic bonding occurs between positive and negative ions, covalent bonding involves sharing electrons between atoms, and metallic bonding involves loosely bound electrons in metal atoms that form an electron cloud. Hydrogen bonding arises from electrostatic attraction between hydrogen atoms partially charged by covalent bonds. Van Der Wall's bonding involves weak, temporary bonds between molecules of the same substance.
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Metallic bonds form between metal cations and delocalized electrons, allowing metals to conduct electricity. Organic compounds contain carbon and form covalent bonds, while inorganic compounds lack carbon and usually form ionic bonds between metals and nonmetals. Ionic bonds occur when atoms transfer electrons, and covalent bonds form when nonmetals share electrons equally. Electronegativity determines whether atoms form ionic or covalent bonds based on their ability to attract bonding electron pairs.
Chemical bonding
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a metal transfers electrons to a nonmetal, creating positively charged ions and negatively charged ions. Covalent bonds form when atoms share electrons as either single, double or triple bonds. Metallic bonds form a "sea of electrons" that are shared between positive metal ions throughout a crystalline structure.
Ionic bond
Ionic bonds form between oppositely charged ions. They result from the transfer of electrons from one atom to another. Ionic bonding typically occurs between metals and nonmetals. Metals tend to lose electrons to fill their outer shell, becoming positively charged ions, while nonmetals gain electrons to fill their outer shell, becoming negatively charged ions. The electrostatic attraction between the opposite charges of the ions forms the ionic bond.
Covalent bonds
Covalent bonds result from the sharing of valence electrons between two nonmetallic atoms. A single covalent bond forms when one pair of electrons is shared, while double and triple bonds share two or three pairs of electrons, respectively. Molecular structure and bond angles are determined by the VSEPR model, which predicts molecular geometry based on electron pair repulsion. Hybridization occurs when atomic orbitals mix to form new hybrid orbitals and explain molecular bonding orientations.
Chemical bonding by Saliha Rais
Chemical bonds are the forces that hold atoms together in molecules and crystals. There are two main types of bonds: ionic and covalent. Ionic bonds involve a complete transfer of electrons between atoms, giving one atom a positive charge and the other a negative charge. Covalent bonds involve sharing of electron pairs between atoms. Covalent bonding can involve single, double or triple bonds with one, two or three shared pairs respectively. Ionic compounds are usually solids with high melting points, while covalent compounds have lower melting points due to weaker intermolecular forces.
Covalent bond
This document defines and provides examples of covalent bonds. It discusses the history of the term being coined by Irving Langmuir in 1919. A covalent bond is defined as a chemical link where electrons are shared between two atoms. Examples given are the covalent bonds between oxygen and hydrogen in H2O and between hydrogen atoms in H2. The document also describes the different types of covalent bonds - single, double, and triple - based on the number of electron pairs shared between the bonded atoms.
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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.
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This document discusses chemical bonding. It defines chemical bonds as how most atoms are joined together in nature. It describes the two main types of chemical bonds: ionic bonding which results from the transfer of electrons between ions, and covalent bonding which results from the sharing of electron pairs between atoms. Atoms form chemical bonds to decrease their potential energy and become more stable. Bonds are rarely purely ionic or covalent, but instead exist on a spectrum depending on the electronegativity difference between the atoms.
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Ionic bonds form through electrostatic attraction between oppositely charged ions. Ionic compounds conduct electricity and have high boiling points. Covalent bonds share pairs of electrons between atoms. Metallic bonds constitute electrostatic forces between delocalized electrons in a "sea" of positive metal ions, giving metals high melting points. Alloys are mixtures of metals with constituents measured by mass that can be substitutional or interstitial in atomic arrangement.
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Chemical bonds form when atoms share or transfer electrons. There are several main types of bonds:
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A chemical bond forms when atoms combine together. There are three main types of bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a cation and anion combine through electrostatic attraction. Covalent bonds form when atoms share one or more pairs of electrons to fill their outer electron shells. Metallic bonds form a sea of electrons that positively charged metal ions are dissolved within.
ionicandcovalentbond-200830005101.pdf
Chemical bonds form through ionic or covalent bonding. Ionic bonding occurs when an atom transfers an electron to another atom, forming oppositely charged ions that are attracted to each other. Covalent bonding occurs when atoms share electrons equally. Ionic bonds are generally stronger than covalent bonds due to the electrostatic forces of attraction between ions. Examples of ionic compounds include sodium chloride and magnesium fluoride, while examples of covalent compounds include phosphorus trichloride.
Ionic and Covalent bond
Chemical bonds form through different types of attractions between atoms. Ionic bonds form when electrons are transferred from one atom to another, creating oppositely charged ions that are attracted to each other. Covalent bonds form when atoms share electrons equally. Ionic bonds are generally stronger than covalent bonds because more energy is required to overcome the electrostatic forces between ions.
Explain covalent bond- Explain Metallic bond and what important proper.docx
Explain covalent bond?
Explain Metallic bond and what important property derives from it in metals?
Solution
Covalent bonding occurs when pairs of electrons are shared by atoms. Atoms will covalently bond with other atoms in order to gain more stability, which is gained by forming a full electron shell. By sharing their outer most (valence) electrons, atoms can fill up their outer electron shell and gain stability. Nonmetals will readily form covalent bonds with other nonmetals in order to obtain stability, and can form anywhere between one to three covalent bonds with other nonmetals depending on how many valence electrons they posses. Although it is said that atoms share electrons when they form covalent bonds, they do not usually share the electrons equally.
Link : http://chemwiki.ucdavis.edu/Theoretical_Chemistry/Chemical_Bonding/General_Principles/Covalent_Bonds
Metallic bond is the reaction between molecules within metals called alkali reactive force. It was first discovered by K. Manishekar. It is the sharing of a sea of delocalised electrons amongst a lattice of positive ions, where the electrons act as a \"glue\" giving the substance a definite structure.
The electrons and the positive ions in the metal have a strong attractive force between them. Therefore metals often have high melting or boiling points. The principle is similar to that of ionic bonds.
The metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, luster, conduction of heat and electricity.
Because the electrons move independently of the positive ions in a sea of negative charge, the metal gains some electrical conductivity. It allows the energy to pass quickly through the electrons generating a current. Heat conduction works on the same principle - the free electrons can transfer the energy at a faster rate than other substances such as those which are covalently bonded, as these have their electrons fixed into position. There also are few non-metals which conduct electricity: graphite (because, like metals, they have free electrons), and molten and aqueous ionic compounds which have free moving ions
Link : https://simple.wikipedia.org/wiki/Metallic_bond
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introduction to chemical bonding
- 1. INTRODUCTIONINTRODUCTION TOTO CHEMICAL BONDINGCHEMICAL BONDING Presented by: KOMANE JOSHUA
- 2. LESSON OBJECTIVES • To know the definition of chemical bonding. • Describe the different types of chemical bonding.
- 3. DEFINITIONS • Chemical Bond – mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together.
- 4. • Valence electrons – outermost electrons that are available to be lost, gained, or shared to form a chemical bond
- 6. COVALENT BONDS • #1. Single covalent bond - Formed by mutual sharing of only one electron pair between two atoms.
- 7. #2. DOUBLE COVALENT BOND • - Formed by the mutual sharing of two electron pairs between two atoms.
- 8. • #3. TRIPLE COVALENT BOND •Formed by the sharing of three electron pairs.
- 9. IONIC BOND • An ionic bond forms when one or more electrons from a metal transfers to a non-metal.
- 10. METALLIC BOND • Chemical bond between atoms in a metallic element. Formed by valance electrons that are moving freely through the metal lattice.
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