Covalent & Ionic Bonding
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Covalent bonds involve sharing of electrons between non-metal atoms, which can be unequally shared (polar covalent) or equally shared (pure covalent). Ionic bonding occurs between a metal and non-metal and involves the transfer of electrons from the metal to the non-metal. Electronegativity is a property that determines an atom's ability to attract electrons, and differences in electronegativity between bonded atoms can be used to classify bonds as ionic, polar covalent, or pure covalent.
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Atoms form bonds by gaining, losing, or sharing electrons to attain a stable electron configuration with 8 valence electrons, known as an octet. Ionic bonds form when atoms transfer electrons to become ions with opposite charges that are attracted to each other. Covalent bonds form when atoms share electrons to attain a full outer shell. Common diatomic molecules that form through covalent bonding include hydrogen (H2), oxygen (O2), nitrogen (N2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2). Ionic bonds typically form between metals and nonmetals, while covalent bonds form between two nonmetals.
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1. Covalent bonding involves the sharing of electron pairs between two or more atoms. Examples include bonds in H2, F2, Br2, Cl2, HCl, and H2O.
2. Covalent bonds form when electrons are shared between two non-metal atoms to fill their outer electron shells. Ionic bonds only occur between a metal and non-metal.
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Check out more interesting posts on LabGirl:
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Here is a video link:
➡➡➡https://www.youtube.com/watch?v=hv4KAioR8aU
Check out more interesting posts on LabGirl:
➡➡➡ https://www.facebook.com/labgirldzd
Thank you! :)
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Atoms form bonds by gaining, losing, or sharing electrons to attain a stable electron configuration with 8 valence electrons, known as an octet. Ionic bonds form when atoms transfer electrons to become ions with opposite charges that are attracted to each other. Covalent bonds form when atoms share electrons to attain a full outer shell. Common diatomic molecules that form through covalent bonding include hydrogen (H2), oxygen (O2), nitrogen (N2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2). Ionic bonds typically form between metals and nonmetals, while covalent bonds form between two nonmetals.
Covalent bonding
1. Covalent bonding involves the sharing of electron pairs between two or more atoms. Examples include bonds in H2, F2, Br2, Cl2, HCl, and H2O.
2. Covalent bonds form when electrons are shared between two non-metal atoms to fill their outer electron shells. Ionic bonds only occur between a metal and non-metal.
3. Covalent bonds can be polar or non-polar depending on whether the electrons are shared equally or are attracted more strongly to one atom. Polar covalent bonds result in partial charges on the atoms.
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This document provides an overview of ionic and covalent bonding. It discusses the formation of ions through the loss or gain of valence electrons to achieve stable electron configurations. Ionic compounds are formed between metallic and nonmetallic elements and are held together by ionic bonds between cations and anions. Molecular compounds are formed by the sharing of valence electrons between nonmetallic elements to form covalent bonds. Polar and nonpolar covalent bonds are discussed based on differences in electronegativity between bonded atoms. Hydrogen bonds that occur between polar molecules like water are also summarized. Key terms related to ionic bonding, covalent bonding, and molecular structure are defined.
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chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
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Covalent bonding occurs when two non-metal atoms share electrons in their outer shells to gain a stable electron configuration. Chlorine exists as Cl2 molecules where each chlorine atom shares one electron with the other to fill its outer shell. Oxygen also exists as O2 molecules where each oxygen atom shares two electrons in a double bond to fill its outer shell. Covalent compounds have strong bonds within their molecules but weak intermolecular forces, which explains their low melting points and why many exist as gases.
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.
Covalent Bonding - Chapter 8
The document discusses different types of covalent bonds:
- Single covalent bonds involve one shared pair of electrons between two nonmetal atoms.
- Double and triple covalent bonds share two or three pairs of electrons respectively.
- Polar covalent bonds occur when electrons are shared unequally between atoms of different electronegativity, giving the atoms partial positive and negative charges. Polar molecules have regions of positive and negative charge.
Covalent bonds - Chemistry
Covalent bonds form between nonmetal atoms by sharing valence electrons. Atoms share electrons to attain stable electron configurations like noble gases. Lewis structures show how valence electrons are arranged between bonded atoms. To draw Lewis structures, count the total valence electrons and distribute them to form single or double bonds between atoms until each atom has an octet of electrons. Examples of molecules held by covalent bonds are hydrogen, oxygen, and chlorine.
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 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.
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
Chapter 8 Covalent Bonds
1. Covalent bonds form when two atoms share one or more pairs of valence electrons in order to achieve a stable octet of electrons.
2. Molecules are formed when atoms are bonded together by covalent bonds, and molecular compounds are composed of molecules.
3. Molecular compounds tend to have lower melting and boiling points than ionic compounds and many are gases or liquids at room temperature.
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.
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CHEMICAL BONDING.ppt
This document discusses chemical bonding and Lewis dot structures. It explains that atoms combine to achieve stable electron configurations, often those of noble gases. Ionic bonds form when electrons are transferred between atoms, creating ions. Covalent bonds form through electron sharing between nonmetals. Lewis dot structures represent valence electrons and can show electron transfers in ion formation. Different bond types - ionic, covalent, and metallic - depend on differences in electronegativity between atoms. Practice problems are provided to determine bond type based on electronegativity values.
johnvic098 chemical bonds inoin bond covalent bond metallic bond.pptx
Ionic bonds form when electrons are transferred permanently from one atom to another, resulting in oppositely charged ions that are attracted to each other. The atom that loses electrons becomes a positively charged cation, while the atom that gains electrons becomes a negatively charged anion. Ionic bonds form crystalline solids where the ions are arranged so that positive and negative charges alternate, balancing each other out and resulting in an overall neutral charge. Ionic crystals have considerable electrostatic forces, making them hard and nonvolatile.
chemistry module-3-ppt.pptx
Ionic compounds are formed between a metal and nonmetal where electrons are transferred, creating oppositely charged ions held together by ionic bonds. Covalent molecular compounds are formed between two or more nonmetals where atoms share electrons through covalent bonds to form electrically neutral molecules like table sugar. Both compound types exhibit distinct physical properties depending on their bonding such as ionic compounds having high melting points and being brittle while covalent compounds have low melting points and are soft and flexible.
Covalent Bonding Notes
Covalent bonding occurs when two or more nonmetals share electrons to attain a stable octet. The shared electron pairs may be distributed unequally between the atoms. The concept of electronegativity describes an atom's ability to attract shared electrons towards itself. Atoms with a large difference in electronegativity form ionic bonds, while smaller differences result in polar or nonpolar covalent bonds. Electronegativity values provide an estimate of bond polarity.
LEWIS SYMBOL.pptx
Lewis symbols represent elements and their valence electrons using dots placed around the element's symbol. Elements form stable electron configurations by gaining, losing, or sharing electrons to match the configuration of the nearest noble gas. Ions are formed when elements gain or lose electrons during bonding to achieve stability. Anions are negatively charged ions formed when nonmetals gain electrons, while cations are positively charged ions formed when metals lose electrons. The type of bond (ionic, polar covalent, or nonpolar covalent) depends on the electronegativity difference between the elements.
Chemical bonds
This document discusses three types of chemical bonds: metallic bonds, ionic bonds, and covalent bonds. It then describes different types of covalent bonds including nonpolar, polar, and coordinated covalent bonds. Finally, it discusses three types of intermolecular forces: dispersion forces, dipole-dipole forces, and hydrogen bonding. Dispersion forces exist between all molecules due to temporary dipoles, while dipole-dipole forces exist between polar molecules due to attraction of partial charges. Hydrogen bonding is a strong form of dipole-dipole force between a hydrogen atom covalently bonded to an electronegative atom like N, O, or F.
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.
Chemical bonds amro.pptx
This document discusses different types of chemical bonds. It begins by defining a chemical bond as the forces that hold groups of atoms together. There are three main types of bonds discussed: covalent bonds, which involve sharing electron pairs between atoms; ionic bonds, which involve the transfer of electrons from metal to nonmetal atoms; and dative covalent bonds, where one atom donates an electron pair to another atom. The document also discusses bond properties like bond length, bond energy, dipole moments, and electronegativity.
Me cchapter 3
This document provides an overview of chemical bonding and the properties of ionic and covalent compounds. It discusses the following key points:
1. Chemical bonds form due to the attraction between atoms and involve the transfer or sharing of valence electrons. Ionic bonds form through electron transfer between metals and nonmetals, while covalent bonds involve electron sharing.
2. Lewis symbols represent atoms and their valence electrons and are used to predict bonding patterns. Electronegativity determines bond polarity.
3. Ionic compounds have high melting and boiling points due to strong electrostatic attractions in the crystal lattice. Covalent compounds can be solids, liquids or gases.
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.
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.
Chapter 8 Powerpoint.pptx
This document provides information about molecular and ionic compounds, including:
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- Molecular formulas show the actual number and type of atoms in a molecule, while ionic formulas use the lowest whole number ratio.
- Covalent bonds are represented by electron dot structures that show how atoms share electrons to achieve stable configurations. Multiple and coordinate covalent bonds are also discussed.
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bonding_regents_chem.ppt
This document defines chemical bonding and describes the three main types of bonds: metallic, ionic, and covalent. Metallic bonds form a crystalline lattice structure with freely moving electrons. Ionic bonds form when ions with opposite charges are attracted to each other via electrostatic forces. Covalent bonds form when atoms share electrons to achieve stable electron configurations. The type of bonding determines various physical properties like melting point, hardness, and conductivity.
Chemical bonding (UPDATED)
Chemical bonding
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Octet Rule
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The document discusses different types of chemical bonds:
- Ionic bonds form when there is a large difference in electronegativity between two atoms, causing one atom to transfer an electron to the other.
- Covalent bonds form when there is a small difference in electronegativity between two non-metal atoms, causing them to share electrons. Covalent bonds can be nonpolar or polar.
- Water is an example of a polar covalent molecule, with the oxygen end being partially negative and the hydrogen ends being partially positive.
Chemical Bonds 2.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.
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.
Chemical bonding
This document discusses chemical bonding and the different types of bonds that can form between atoms. It describes how ionic bonds are formed via electron transfer between atoms, and covalent bonds are formed through electron sharing. The octet rule, where atoms gain, lose, or share electrons to achieve a noble gas configuration, is an important concept. Ionic compounds involve the formation of cations and anions, while covalent compounds share electrons between nonmetals. Covalent bonds can be polar, involving unequal electron sharing, or nonpolar with equal sharing. Coordinate or dative bonds also involve electron sharing, but with both electrons coming from the same atom.
Chemical bonds 2020
Chemical bonds are the forces that hold atoms together in molecules and compounds. There are several types of bonds including ionic bonds, covalent bonds, hydrogen bonds, metallic bonds, and coordinate bonds. Ionic bonds form between metals and nonmetals when electrons are transferred. Covalent bonds form when atoms share electrons. Hydrogen bonds occur between polar molecules containing hydrogen. Metallic bonds are electrostatic attractions between positively charged metal ions and delocalized electrons. Coordinate bonds form when both electrons in a bond come from the same atom. Each bond type influences the properties of the resulting compounds.
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This document discusses intermolecular forces and polarity. It defines intermolecular forces as the attractive or repulsive forces between molecules. The document then explains the different types of intermolecular forces and how they relate to a substance's properties. It also discusses how intermolecular forces are used in applications like medical implants and electronics. Next, it describes how polarity is determined by bond polarity and molecular geometry. Polar molecules interact through dipole-dipole interactions and hydrogen bonding, while non-polar molecules interact through London dispersion forces. The document provides several examples of applying concepts of electronegativity, bond polarity, and molecular geometry to determine if a substance is polar or non-polar.
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- 6. Using Lewis Structure and Orbital Diagrams to represent bonding
- 7. Electronegativity values can be used to determine whether bonds are: pure covalent, polar covalent, or ionic • EN differences that equal 1.7 mean that the bond between the two elements is 50% polar covalent/50% ionic. • EN differences of >1.7 means that the bond between the two elements is ionic (or very polar covalent i.e. HF). • EN differences that are <1.7 mean that the bond between the two elements is polar covalent • EN differences of 0 mean that the bond is pure covalent • Use EN values to determine the type of bond in each of the following o BN o KF o O2
Editor's Notes
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