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60 Cards in this Set
- Front
- Back
2 0 2
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Linear/ Linear/ 180/ sp/ Ex: CO2
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2 0 2
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Linear/ Linear/ 180/ sp/ Ex: BeCl2
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1 1 2
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Linear/ Paired/ N/A / sp/ Ex: CO, N2
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3 0 3
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Trigonal Planar/ Trigonal Planar/ 120/ sp2/ Ex: AlCl3, SO3
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2 1 3
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Trigonal Planar/ Bent/ <120/sp2/ Ex: SO2, O3
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1 2 3
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Trigonal Planar/ Paired/ N/A / sp2/ Ex: O2
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4 0 4
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Tetrahedral/ Tetrahedral/ 109.5/ sp3/ Ex: CH4
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3 1 4
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Tetrahedral/ Pyramidal/ <109.5/ sp3/ Ex: NH3
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2 2 4
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Tetrahedral/ Bent/ <109.5/ sp3/ Ex: H2O
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1 3 4
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Tetrahedral/ Paired/ N/A / sp3/ Ex: HCl
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5 0 5
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Trigonal Bipyramidal/ Trigonal Bipyramidal/ 90 or 120/ sp3d/ Ex: PCl5
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6 0 6
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Octahedral/ Octahedral/ 90/ sp3d2/ Ex: SF6
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Lewis Structures
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Representation of bonding (valence)electrons. Noble Gas configuration = GOAL!!! (Octet Rule)
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Rules for Lewis Structures
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Hydrogen Follows Octet Rule. He is stable. Octet Rule- representative elements (end in s/p sublevels). Psuedo Noble Gas Configuration (end in d/f sublevels).
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Step 1 for Drawing Lewis Structure
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1. Add all valence electrons of all atoms.
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Step 2 for Drawing Lewis Structure
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2. Use one pair of electrons to form stable bonds between atoms.
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Step 3 for Drawing Lewis Structure
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3. Arrange the electrons in pairs around atoms to follow the Octet Rule(NBP of electrons).
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Step 4 for Drawing Lewis Structure
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4. Count electrons to follow the Octet Rule.
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Step 5 for Drawing Lewis Structure (Not always used)
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5. Use Two pairs of electrons to form bonds between atoms.
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Step 6 for Drawing Lewis Structure (Not always used)
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6. Use three pairs of electrons to form bonds between atoms.
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Molecular Structures' Properties
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1. Geometric Structure
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Molecular Structures' Properties
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2. Three-Dimensional Arrangement of Atoms
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Molecular Structures' Properties
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3. Dependent on the Central Atom(s)
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Molecular Structures' Properties
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4. Basic Structures: Linear, Trigonal Planar, Tetrahedral, Trigonal Bipyramidal, Octahedral. All Symmetrical (automatically non-polar b/c symmetrical).
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Molecular Structures' Properties
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5. Other Structures: Bent, Pyramidal, Paired* (Asymmetrical. B/c asymmetrical, they have polar bonds and therefore are polar molecules).
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VSEPR (Valence Shell Electron Pair Repulsion) Theory
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Minimizes the repulsion of electron pairs and results in an *approximate* molecular structure.
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Step 1 to VSEPR Theory
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1. Draw Lewis Structure
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Step 2 to VSEPR Theory
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2. Count Electron pairs and arrange them to minimalize repulsion
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Step 3 to VSEPR Theory
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3. Determine the position of atoms from how they are paired
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Step 4 to VSEPR Theory
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4. Determine the name of the molecular structure from how the atoms are arranged
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Rule 1 of the VSEPR Theory
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1. Two pairs of electrons on central atom are always 180 degrees apart (Linear)
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Rule 2 of the VSEPR Theory
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2. Three pairs of electrons are always 120 degrees apart (Trigonal Planar)
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Rule 3 of the VSEPR Theory
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3. Four Pairs of electrons are always 109.5 degrees apart (Tetrahedral)
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Rule 4 of the VSEPR Theory
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4. When all pairs of electrons on the central atom are shared with another atom, the molecular structure is the same as the arrangement of electrons. (Zero NBP)
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Rule 5 of the VSEPR Theory
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5. When one or more electron pairs on a central atom are unshared (NBP), then the name for the molecular structure is different from the central atom.
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methane
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CH4
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carbon tetrachloride
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CCl4
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water
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H2O
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ammonia
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NH3
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hydrogen sulfide
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H2S
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phosphane
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PH3
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hydrogen peroxide
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H2O2
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chlorine
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Cl2
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hydrogen chloride
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HCl
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oxygen
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O2
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nitrogen
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N2
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carbon dioxide
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CO2
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carbon monoxide
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CO
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hydrogen
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H2
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fluorine
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F2
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bromine
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B2
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iodine
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I2
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ethane
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C2H6
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ethene
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C2H4
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ethyne
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C2H2
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ozone
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O3
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phosphorus pentachloride
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PCl5
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sulfur hexafluoride
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SF6
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sulfur dioxide
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SO2
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sulfur trioxide
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SO3
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