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Chemistry 8.4

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Chemistry 8.4

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    1. Chemistry 8.4

    5. Bond Polarity The bonding pairs of electrons in covalent bonds are pulled by the nuclei. The nuclei of atoms pull on the shared electrons, much as the knot in the rope is pulled toward opposing sides in a tug-of-war. The nuclei of atoms pull on the shared electrons, much as the knot in the rope is pulled toward opposing sides in a tug-of-war.

    6. Bond Polarity The chlorine atom attracts the electron cloud more than the hydrogen atom does. This electron-cloud picture of hydrogen chloride shows that the chlorine atom attracts the electron cloud more than the hydrogen atom does. Inferring Which atom is more electronegative, a chlorine atom or a hydrogen atom? This electron-cloud picture of hydrogen chloride shows that the chlorine atom attracts the electron cloud more than the hydrogen atom does. Inferring Which atom is more electronegative, a chlorine atom or a hydrogen atom?

    12. When polar molecules, such as HCl, are placed in an electric field, the slightly negative ends of the molecules become oriented toward the positively charged plate and the slightly positive ends of the molecules become oriented toward the negatively charged plate. Predicting What would happen if, instead, carbon dioxide molecules were placed between the plates? Why? When polar molecules, such as HCl, are placed in an electric field, the slightly negative ends of the molecules become oriented toward the positively charged plate and the slightly positive ends of the molecules become oriented toward the negatively charged plate. Predicting What would happen if, instead, carbon dioxide molecules were placed between the plates? Why?

    17. Attractions Between Molecules Dipole interactions occur when polar molecules are attracted to one another. Polar molecules are attracted to one another by dipole interactions, a type of van der Waals force. Polar molecules are attracted to one another by dipole interactions, a type of van der Waals force.

    18. Attractions Between Molecules Dispersion forces, the weakest of all molecular interactions, are caused by the motion of electrons. The strength of dispersion forces generally increases as the number of electrons in a molecule increases.

    19. Attractions Between Molecules Hydrogen Bonds Hydrogen bonds are attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.

    20. Attractions Between Molecules Hydrogen Bonding in Water The strong hydrogen bonding between water molecules accounts for many properties of water, such as the fact that water is a liquid rather than a gas at room temperature. The strong hydrogen bonding between water molecules accounts for many properties of water, such as the fact that water is a liquid rather than a gas at room temperature.

    21. Attractions Between Molecules The relatively strong attractive forces between water molecules cause the water to form small drops on a waxy surface. The strong attractions between water molecules cause the water to pull together into small drops rather than spread over the surface of the flower. The strong attractions between water molecules cause the water to pull together into small drops rather than spread over the surface of the flower.

    25. Diamond is a network-solid form of carbon. Diamond has a three-dimensional structure, with each carbon at the center of a tetrahedron. Diamond is a network-solid form of carbon. Diamond has a three-dimensional structure, with each carbon at the center of a tetrahedron.

    26. Intermolecular Attractions and Molecular Properties Silicon Carbide is a network solid. It has a melting point of about 2700°C. Silicon carbide, a network solid, is so hard that it is used in this grindstone to wear down the end of a hardened steel cutting tool to form a sharp edge. Silicon carbide, a network solid, is so hard that it is used in this grindstone to wear down the end of a hardened steel cutting tool to form a sharp edge.

    32. 3. Which of the following bond types is the weakest? ionic bond Van der Waals force covalent bond hydrogen bond 8.4 Section Quiz.

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