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Molecular Bonding . Shapes and VSEPR Theory. Lesson Frame. I will be able to predict the shape of a molecule if given the formula or Lewis dot structure . I will do this by practicing on 2D and 3D virtual models . I will show mastery by being able to predict the shape based on the formula.
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Molecular Bonding Shapes and VSEPR Theory
Lesson Frame • I will be able to predict the shape of a molecule if given the formula or Lewis dot structure. • I will do this by practicing on 2D and 3D virtual models. • I will show mastery by being able to predict the shape based on the formula.
VSEPR • VSEPR stands for Valence Shell Electron Pair Repulsion • Electrons are negative and same charge particles repel each other. Electrons are either shared or transferred between atoms • Shared pairs have a greater repulsion than single electrons. • Unshared pairs have a greater repulsion than shared pairs • Electrons involved in bonding and not involved in bonding will affect the shape of a molecules.
Polar Bond • Ionic Bonds are polar because they are a transfer of electrons and have an electronegativity difference of 1.7 or greater. • Polar covalent bonds are formed when there is a electronegativity difference of between 0.3 and 1.7 . • Nonpolar covalent bonds are formed when the electronegativity difference is less than 0.3.
Polar Molecule • Polar Molecules: • must contain at least one polarbond • are shaped so that there is a positive and a negative end • example of a polar molecule:
Nonpolar Molecule • Non-polar Molecule: • contains only _non-polar_bonds -or- • contains polar bonds, but has no _charged_ _ends___ • example of a non-polar molecule:
Intermolecular Forces • Intermolecular Forces • __Force_ of attraction __between___molecules • are __weaker___than covalent and ionic bonds • 3 types: • 1. Dipole-dipole forces: • force of attraction between the positive_ end of one _molecule_ and the _ negative _ end of another molecule • the __strongest_ of all the intermolecular forces • 2. Hydrogen Bonding: • occurs in molecules with H -_N_ , H - _F_ , and H - _O_ bonds • large __positive__ charge on H is attracted to an _unshared__pair of electrons on a neighboring _molecule______ • 3. London Dispersion Forces: • _____weak____ intermolecular forces resulting from constant ____motion_____ of _______electrons______ • the only type of intermolecular force between nonpolar molecules
1. What type of bond exist between magnesium and chloride? • ionic bond • polar covalent bond • nonpolar covalent bond • metallic bond [Default] [MC Any] [MC All]
2. When two atoms share three pairs of electrons, the bond is called a _______. • single bond • double bond • triple bond • quadruple bond [Default] [MC Any] [MC All]
3. A molecule containing only two atoms has which of the following shapes? • linear • trigonal planar • tetrahedral • pyramidal [Default] [MC Any] [MC All]
4. A molecule in which the central atom is bonded to four other atoms has which of the following shapes? • linear • trigonal planar • tetrahedral • pyramidal [Default] [MC Any] [MC All]
5. A molecule is considered non-polar if which of the following is true? • A. all bond with in the molecule are non-polar • B. bonds are polar and positive ends exist • C. bonds are polar but no positive ends exist • D. both a and c are true [Default] [MC Any] [MC All]
6. What is the strongest intermolecular force that exists in polar molecules? • dipole-dipole • ionic bonding • London-dispersion forces • None of the above. [Default] [MC Any] [MC All]
7. What is the intermolecular force that exists in all molecules called? • dipole-dipole • ionic bonding • London-dispersion forces • None of the above. [Default] [MC Any] [MC All]
