Chemical bond 2.ppt
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This document discusses different types of intermolecular forces: 1) Dipole-dipole forces occur between polar molecules due to the attraction between opposite charges. 2) Ion-dipole forces occur between ions and polar molecules. 3) Dispersion forces, the weakest intermolecular forces, arise from temporary dipoles induced in nonpolar molecules. 4) Hydrogen bonding, a stronger intermolecular force, occurs between a hydrogen covalently bonded to F, O or N and another electronegative atom.
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Ionic bonding occurs when there is a difference in electronegativity between two atoms. The atom with higher electronegativity attracts the electrons in the bond, becoming negatively charged (δ-), while the other atom loses electrons, becoming positively charged (δ+). This ionic attraction forms ionic compounds of cations and anions. Intermolecular forces include dipole-dipole interactions between polar molecules, ion-dipole interactions between ions and polar molecules, and hydrogen bonding between molecules containing hydrogen bonded to fluorine, oxygen, or nitrogen.
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Chemical bonds form between atoms to achieve more stable arrangements with lower potential energy. The main types of bonds are ionic, covalent, and metallic. Ionic bonds form between oppositely charged ions, covalent bonds form when atoms share electrons, and metallic bonds result from delocalized electrons being shared among many atoms in a metal. The degree of ionic or covalent character in a bond depends on the electronegativity difference between the atoms. Molecular compounds are made of molecules held together by covalent bonds, while ionic compounds are made of ionic bonds between cations and anions.
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Chemical bonds form between atoms to achieve more stable arrangements with lower potential energy. The type of bonding depends on differences in electronegativity between atoms. Ionic bonds form between ions, covalent bonds involve shared electron pairs, and metallic bonds result from delocalized electrons shared among many atoms in a lattice. Molecular geometry and intermolecular forces also influence molecular properties.
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Ionic bonds form when electrons are transferred between metals and nonmetals, resulting in oppositely charged ions. Covalent bonds form when nonmetals share electrons in order to achieve a stable electron configuration. Ionic compounds have high melting points and conduct electricity well when melted but not solid, while covalent compounds have low melting points and generally do not conduct electricity or dissolve in water well.
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Polarity and Intermolecular Forces.ppt
This document discusses polarity and intermolecular forces. It defines electronegativity and explains how differences in electronegativity between atoms result in polar covalent bonds. Dipole moments are used to represent bond polarity. Intermolecular forces, including dipole-dipole interactions, hydrogen bonding, and London dispersion forces are described. These intermolecular forces influence important properties like melting and boiling points.
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9
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structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
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Chemical bond 2.ppt
- 1. Intermolecular Forces Intermolecular forces are forces between molecules. Intramolecular forces hold atoms together in a molecule. Example: ionic, covalent, and metallic.
- 2. Electronegativity is the ability of an atom to attract toward itself the electrons in a chemical bond. Electronegativity - relative, F is highest H F electron poor region electron rich region
- 3. H F d+ d-
- 4. e- e- δ - δ + 2 + e- e- 2 + e- e- 2 + e- e- δ - δ + 2 + e- e- δ - δ + 2 + e- e- δ - δ + 2 + repel attract e- e- 2 +
- 5. Types of Intermolecular Forces Dipole-Dipole Forces Attractive forces between polar molecules Orientation of Polar Molecules in a Solid
- 6. Dipole – Dipole Forces d+ d- d+ d- d+ d- d+ d- d+ d-
- 7. Types of Intermolecular Forces Ion-Dipole Forces Attractive forces between an ion and a polar molecule Ion-Dipole Interaction
- 8. Ion – Dipole Forces Exist when we dissolve an ionic compound in a polar solvent, like H2O. The d- end of H2O is attracted to a cation (+). The d+ end of H2O is attracted to an anion (-).
- 9. Types of Intermolecular Forces Dispersion Forces – van der Walls forces/London forces (weakest) Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules ion-induced dipole interaction dipole-induced dipole interaction
- 10. Hydrogen Bonding Hydrogen Bond = an attraction between a slightly positive hydrogen atom and a slightly negative atom, often oxygen or nitrogen
- 11. Hydrogen Bonding
- 12. O H H δ + δ + δ- O H H δ + δ + δ- O H H δ + δ + δ- O H H δ + δ + δ- O H H δ δ + δ- hydrogen bonds
- 13. • A hydrogen bond is an intermolecular bond. F—H O—H N—H • A hydrogen bond is formed between polar molecules that contain hydrogen covalently bonded to a small, highly electronegative atom: F, O, N.
- 14. hydrogen bond covalent bond covalent bond A dipole-dipole bond bond will be formed between the two molecules which is called a hydrogen bond.
- 15. Remember, you need: A hydrogen atom covalently bonded to an electronegative atom … N, O or F. If only one of these conditions is met, you don’t get hydrogen bonding. A lone pair of electrons on the electronegative atom.
- 16. Coordinate Covalent Bond • A coordinate bond (also called a dative covalent bond) is a covalent bond (a shared pair of electrons) in which both electrons come from the same atom. • A coordinate covalent bond is usually shown with an arrow.
- 17. Amino-Borane N has a full octet an a lone pair of electrons. NH3 is an uncharged molecule. B only has 6 electrons, it is deficient. BH3 is an uncharged molecule. N can “donate” its lone pair to B forming a co-ordinate bond.
- 18. Amino-Borane Now we have a new molecule with a covalent bond between N and B. While there are formal charges on N and B, the overall charge on the molecule is neutral. The bond formed between N and B is just as strong as any covalent bond.
- 19. ammonium ion