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This document discusses different types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals when electrons are transferred from the metal atom to the nonmetal atom. Covalent bonds form between nonmetal atoms through the sharing of electron pairs. Metallic bonds form between metal atoms when electrons are delocalized and pooled throughout the structure. Examples of ionic bonding forming between sodium and chlorine atoms and covalent bonding forming between oxygen and hydrogen atoms are provided. Single, double, and triple covalent bonds are also defined based on the number of electron pairs shared.
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Minvya
A chemical bond is an attraction between atoms that allows the formation of substances containing two or more atoms. The bond is caused by electrostatic forces of attraction, either between electrons and nuclei or due to dipole attraction. When metals bond to nonmetals, electrons from the metal atoms are transferred to the nonmetal atoms, resulting in the metal atoms becoming positively charged ions and the nonmetal atoms becoming negatively charged ions.
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:
➡➡➡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
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between oppositely charged ions, such as between sodium and chlorine atoms where sodium loses an electron to become positively charged and chlorine gains an electron to become negatively charged. Covalent bonds form when atoms share electrons, such as in water where oxygen and hydrogen share electron pairs. Metallic bonds form by the attraction of free-floating electrons within a lattice of positive metal ions.
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.
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.
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.
9/25 What is the trend for electronegativity?
The document is a chemistry class lecture on trends in the periodic table, specifically electronegativity. It defines electronegativity as an atom's ability to attract electrons in a chemical bond. It then explains that electronegativity increases from left to right across periods due to more protons, but decreases down groups because more electron shells shield the nucleus from outer electrons. Practice problems are assigned for students to study these trends.
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A chemical bond is an attraction between atoms that allows the formation of substances containing two or more atoms. The bond is caused by electrostatic forces of attraction, either between electrons and nuclei or due to dipole attraction. When metals bond to nonmetals, electrons from the metal atoms are transferred to the nonmetal atoms, resulting in the metal atoms becoming positively charged ions and the nonmetal atoms becoming negatively charged ions.
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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
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between oppositely charged ions, such as between sodium and chlorine atoms where sodium loses an electron to become positively charged and chlorine gains an electron to become negatively charged. Covalent bonds form when atoms share electrons, such as in water where oxygen and hydrogen share electron pairs. Metallic bonds form by the attraction of free-floating electrons within a lattice of positive metal ions.
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.
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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.
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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Metallic bonding occurs when metal atoms bond through delocalized electrons. Metals form a lattice structure with positive metal ions surrounded by a sea of delocalized electrons that are attracted to the positive ions. This bonding allows metals to have distinctive physical and chemical properties including malleability, conductivity, and high melting points. Metallic bonding is important for creating alloys and is found in many materials used in daily life.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
Ionic compound
Ionic bonding occurs when valence electrons are transferred from metal atoms to non-metal atoms, resulting in positively charged cation and negatively charged anion ions that are attracted via electrostatic forces. Ionic compounds form when a metal donates its valence electrons to a nonmetal. The electrostatic attraction between opposite charges holds the ions together. Common ionic compounds include sodium chloride, formed from sodium cations and chloride anions, and magnesium oxide, formed from magnesium cations and oxide anions.
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Ch 6 4 Metallic Bonds Others
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.
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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.
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There are 4 main types of chemical bonds: nonpolar covalent bonds form between identical atoms and share electrons equally. Polar covalent bonds form between different atoms and electrons are closer to the more electronegative atom. Ionic bonds form when atoms gain or lose electrons to become ions with opposite charges that are attracted to each other. Hydrogen bonds occur when a hydrogen atom bonded to an electronegative atom is attracted to another electronegative atom, and can occur between or within molecules like water and DNA.
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Diamonsters !!! If you like to study in advance about our report, just save this file! :D
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
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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.
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Electronegativity is an element's ability to attract bonding electron pairs in a covalent bond. It depends on an element's atomic radius and number of protons - larger atomic radius and fewer protons result in lower electronegativity as electrons are farther from the nucleus and protons have less attraction. However, full electron shells provide shielding that reduces the effect of more protons on electronegativity.
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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.
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The document discusses how to determine if a bond is ionic, polar covalent, or covalent. It explains that electronegativity values are used to calculate the difference between two bonded atoms. A difference of 0 means the bond is covalent. A difference greater than 0 but less than 1.9 means the bond is polar covalent. A difference greater than or equal to 1.9, where one atom is a metal and the other is non-metal, means the bond is ionic. Examples of calculating electronegativity differences and classifying bond types are provided.
Chemicalbonding
There are three main types of chemical bonds: ionic bonds, covalent bonds, and hydrogen bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, resulting in oppositely charged ions that are attracted to each other. Covalent bonds involve the sharing of electrons between two atoms. Hydrogen bonds are attractive forces between a hydrogen atom covalently bonded to an electronegative atom, like oxygen or nitrogen, and another electronegative atom.
Lecture of chemistry of secondary bonding
Secondary bonding includes dipole forces, induction forces, van der Waals forces, and hydrogen bonding. These weaker intermolecular forces influence the properties of organic compounds. Dipole forces are caused by partial charges on polar bonds and affect properties like melting point. Hydrogen bonding is the strongest secondary bond and significantly increases boiling points, as seen when comparing methanol, ethanol, and water. Hydrogen bonding also improves the mechanical properties of materials like nylon.
The chemical bonds
There are 4 main types of chemical bonds: nonpolar covalent bonds form between identical atoms and share electrons equally. Polar covalent bonds form between different atoms and electrons are closer to the more electronegative atom. Ionic bonds form when atoms gain or lose electrons to become ions with opposite charges that are attracted to each other. Hydrogen bonds occur when a hydrogen atom bonded to an electronegative atom is attracted to another electronegative atom, and can occur between or within molecules like water and DNA.
Chemical bonding
Report for Chem III :)
Diamonsters !!! If you like to study in advance about our report, just save this file! :D
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
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.
Chapter 6.1 : Introduction to Chemical Bonding
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.
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.
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Chemical Bonding and it's Types 001.pptx
Chemical bonding occurs when atoms form compounds, with the strength of the bond depending on the atoms involved. There are four main types of bonds: ionic bonds form between metals and nonmetals via the transfer of electrons; covalent bonds involve the sharing of electrons between two atoms, which can be single, double or triple; hydrogen bonds are electrostatic attractions between hydrogen and electronegative atoms like nitrogen, oxygen or fluorine; and metallic bonds form when metal atoms bond together via delocalized electrons among positively charged metal ions.
Primary bonding in organic compound
Ionic bonding involves the transfer of valence electrons from metal to nonmetal atoms, creating positively charged cations and negatively charged anions that are attracted in a crystal lattice. Covalent bonding is the sharing of valence electrons between atoms. Metallic bonding delocalizes valence electrons among the positively charged metal ions in a crystal structure.
Ionic bond,covalent bond and hydrogen bond
Ionic bond,covalent bond and hydrogen bond . we can see from this slide the definition and mechanism of those chemical bonding eaily
Types-of-Chemical-Bonding.pdf
Chemical bonding occurs through the attraction between positively charged protons and negatively charged electrons, forming stable compounds. There are three main types of chemical bonds: covalent bonds form when atoms share electron pairs to attain stable electron configurations, ionic bonds form when electrons are transferred between metals and nonmetals creating positively and negatively charged ions that are attracted, and metallic bonds form when metal atoms share their outer electrons in a "sea of electrons" allowing for conductivity and malleability. Chemical bonds are crucial as they allow for the formation of all substances including living things, materials, and objects through lowering energy and achieving stability.
Lecture on atomic structure.pptx
1. The document discusses various topics related to atomic structure including classical theories of atomic structure, discovery of the proton and nucleus, electron shells, and electron dot structures.
2. It also discusses different types of chemical bonds including ionic bonds formed by electron transfer, covalent bonds formed by electron sharing, hydrogen bonds, and metallic bonds.
3. Additional topics covered include electromagnetic radiations, radioactivity, nuclear decay processes, medical and other applications of radioisotopes, and uses of radiation in agriculture and food preservation.
There are two types of atomic bonds - ionic bonds and covalent bonds.pdf
There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their
structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and
bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 -
200 kcal/mol). Whether two atoms can form a covalent bond depends upon their
electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two
atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the
atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and
negatively charged ion (anion). The bond between these two ions is called an ionic bond.
Covalent BondsIonic Bonds
Polarity:LowHigh
Formation:A covalent bond is formed between two non-metals that have similar
electronegativities. Neither atom is \"strong\" enough to attract electrons from the other. For
stabilization, they share their electrons from outer molecular orbit with othersAn ionic bond is
formed between a metal and a non-metal. Non-metals(-ve ion) are \"stronger\" than the
metal(+ve ion) and can get electrons very easily from the metal. These two opposite ions attract
each other and form the ionic bond.
Shape:Definite shapeNo definite shape
What is it?:Covalent bonding is a form of chemical bonding between two non metallic atoms
which is characterized by the sharing of pairs of electrons between atoms and other covalent
bonds.Ionic bond, also known as electrovalent bond is a type of bond formed from the
electrostatic attraction between oppositely charged ions in a chemical compound. These kinds of
bonds occur mainly between a metallic and a non metallic atom.
Melting point:lowHigh
Examples:Methane (CH4), Hydro Chloric acid (HCl)Sodium chloride (NaCl), Sulphuric Acid
(H2SO4 )
Occurs between:Two non-metalsOne metal and one non-metal
Boiling point:LowHigh
State at room temperature:Liquid or gaseousSolid
Ability to conduct electricity in molten/aqueous state:
Yes
Ability to conduct electricity in solid state:
Solution
There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their
structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and
bind the atoms in a fixed orientation. Relatively high energies are required to break them (50 -
200 kcal/mol). Whether two atoms can form a covalent bond depends upon their
electronegativity i.e. the power of an atom in a molecule to attract electrons to itself. If two
atoms differ considerably in their electronegativity - as sodium and chloride do - then one of the
atoms will lose its electron to the other atom. This results in a positively charged ion (cation) and
negatively charged ion (anion). The bond between these two ions is called an ionic bond.
Covalent BondsIonic Bonds
Polarity:LowHigh
Formation:A covalent bond is formed between two non-metals that have similar
electronegativities. .
Chemical bonding
The document summarizes different types of chemical bonds including ionic bonds, covalent bonds, metallic bonds, hydrogen bonds, and Van der Waals interactions. It describes how each type of bond forms and provides examples. Ionic bonds form through electrostatic attraction between oppositely charged ions. Covalent bonds form when atoms share one or more pairs of electrons. Metallic bonds result from delocalized electrons within metal structures. Hydrogen bonds are electrostatic attractions between hydrogen and electronegative atoms. Van der Waals interactions arise from correlations in polarizations between particles.
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
.
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.
Chemical bonding theories, 10(1)
Theories about how chemical bonds are formed. Covalent bond, multi covalent bonds. How to write Lewis Structures
BONDING.pptx
The atomic mass of an element can vary because the number of neutrons in the nucleus may be variable, even though the number of protons remains the same for a given element. There are four main types of atomic bonding - ionic, covalent, metallic, and van der Waals - which determine key material properties like hardness, melting point, and whether a material is a metal, polymer, or ceramic based on electron configuration and bonding forces between atoms. These bonding types arise from atoms seeking stable electron configurations through gaining, losing, or sharing valence electrons.
Enlace quimico
This document summarizes key concepts from Chapter 8 of a chemistry textbook, including:
- The three main types of chemical bonds are covalent, ionic, and metallic bonds. Covalent bonds result from shared electron pairs, ionic bonds from electron transfers, and metallic bonds hold pure metals together.
- Lewis structures represent electron arrangements and bonding using dots around atom symbols. The octet rule states atoms seek full outer shells of 8 electrons.
- Ionic bonds form when metals donate electrons to nonmetals, giving stable noble gas configurations. They form crystalline lattices with strong attractions.
- Covalent bonds share electron pairs so atoms both attain full outer shells. Polarity arises from differing electronegativities.
2016 topic 4.2 bonding - covalent
This document provides an overview of ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged ion and another atom gains those electrons to become a negatively charged ion. For example, in sodium chloride, sodium atoms lose electrons to form Na+ ions and chloride atoms gain electrons to form Cl- ions. The oppositely charged ions are then held together by electrostatic forces in a repeating crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity in solid form but do conduct when molten or dissolved in water as the ions become mobile.
Chemical bonding 1
1) Chemical bonds form when atoms overlap their orbitals to achieve stable noble gas configurations. This increases stability as atoms form ionic or covalent bonds.
2) Metallic bonding occurs via a "sea of electrons" model where mobile electrons are shared between rigid positive ions. This explains properties like conductivity and malleability.
3) There are various types of bonds including ionic formed between metals and nonmetals, and covalent including polar, nonpolar, and coordinate bonds formed by electron sharing or donation.
Chemical bonding 1
Chemical bonding 1 is the first of two presentations on Chemical Bonding by Aditya Abeysinghe.This presentation mainly focuses on the basic/principle bonds formed between two or more elements.
Chemical bonding
There are three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form when electrons transfer from a metal to a non-metal, resulting in oppositely charged ions. Covalent bonds form when atoms share one or more pairs of electrons to achieve an octet. Metallic bonds form through delocalized electrons that are free to move throughout the metal lattice, allowing metals to conduct electricity and have high melting points.
Chemical bonding
There are four main types of chemical bonds: ionic bonds, covalent bonds, metallic bonds, and hydrogen bonds. Ionic bonds form through the transfer of electrons from one atom to another, creating oppositely charged ions. Covalent bonds form through the sharing of electron pairs between atoms. Metallic bonds arise from the electrostatic attraction between positively charged metal ions and delocalized electrons. Hydrogen bonds result from the attraction between hydrogen atoms covalently bonded to electronegative atoms like nitrogen or oxygen, and another electronegative atom. Chemical bonds form through these interactions to hold groups of atoms together in molecules, ions, crystals and other stable species.
Chemical bonding-I
This document discusses chemical bonding, including ionic bonds, covalent bonds, and molecular orbital theory. It covers the factors that influence ionic bond formation, such as ionization energy and lattice energy. Born-Haber cycles are used to calculate the lattice energy of ionic compounds like NaCl. The document also discusses polar covalent bonds and how electronegativity differences between atoms determine bond polarity. Hybridization of atomic orbitals and VSEPR theory are introduced.
Forces Of Attraction
Forces of attraction include intramolecular and intermolecular forces. Intramolecular forces like ionic bonds and covalent bonds hold atoms together in molecules through electrostatic attraction or electron sharing. Intermolecular forces between molecules include hydrogen bonding, dipole-dipole interactions, and induced dipole forces from electron motion. These weaker forces influence melting/boiling points and physical states. Polar molecules form stronger intermolecular attractions than nonpolar molecules through orientations of their charge distributions.
Chemical bonding
This document discusses different types of chemical bonds:
1) Metallic bonds form when valence electrons are delocalized and shared between all metal atoms in a lattice, holding the positive ions together.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions that are attracted to each other.
3) Covalent bonds form when two nonmetals share valence electrons in a molecule through electron pairs. Lewis structures are used to represent electron sharing in covalent bonds.
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Sethu.ppt.
- 3. Submitted By, SETHULEKSHMI K R PHYSICAL SCIENCE REG NO: 18214383019 Submitted To, MRS.LINI MOL.K.S Faculty in Physical science department SNTC Poochakkal
- 5. A chemical bond is an attraction between atoms that allows the formation chemical substances that contain two or more atoms . The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction
- 7. Types of Atoms Type of Bond Bond Characteristic metals to nonmetals Ionic electrons transferred nonmetals to nonmetals Covalent electrons shared metal to metal Metallic electrons pooled
- 8. 8
- 9. Tro, Chemistry: A Molecular Approach When metals bond to nonmetals, some electrons from the metal atoms are transferred to the nonmetal atoms –Metals have low ionization energy, relatively easy to remove an electron from –Nonmetals have high electron affinities, relatively good to add electrons to
- 10. Electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.
- 12. “Bond formed by the sharing of electrons” Tro, Chemistry: A Molecular Approach 12 Nonmetals have relatively high ionization energies, so it is difficult to remove electrons from them When nonmetals bond together, it is better in terms of potential energy for the atoms to share valence electrons Potential energy lowest when the electrons are between the nuclei Shared electrons hold the atoms together by attracting nuclei of both atoms
- 13. Two atoms share one or more pairs of outer-shell electrons Oxygen Atom Oxygen Atom Oxygen Molecule (O2)
- 14. Tro, Chemistry: A Molecular Approach 14 1. Single Covalent Bonds Two atoms share a pair of electrons 2 electrons One atom may have more than one single bond F •• •• •• • F •• •• • •• F •• •• •• •• •• F •• •• HH O •• •• •• •• H•H• O •• • • •• F F
- 15. Tro, Chemistry: A Molecular Approach 15 2.Double Covalent Bond Two atoms sharing two pairs of electrons 4 electrons O O•••• O •• • ••• O •• • • •• O O···· ·· ··
- 16. Tro, Chemistry: A Molecular Approach 16 3.Triple Covalent Bond Two atoms sharing 3 pairs of electrons 6 electrons N •• • • • N •• • • • N •••••• N N N····