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Experiment 10 Variations on AX5; AX4U (see-saw), AX3U2 (T-shaped), and AX2U3 (linear). Draw Lewis structures, make 3-D models, and name the molecular shape of PCl5. Show the location of atoms and any lone pairs of electrons. Name the molecular shape: PCl5 Lewis Structure: PCl5 3-D Model: Name of Molecular Shape: Trigonal Bipyramidal Draw the Lewis structure for PCl3 (below). Show the location of atoms and any lone pairs of electrons. In PCl3, the lone pair of electrons can be placed in either an equatorial or an axial position. Determine the total number of each type of 90° repulsive interaction for each placement: Equatorial Placement of Lone Pair: - LP-LP: 90° - LP-BP: 90° - BP-BP: 90° Axial Placement of Lone Pair: - LP-LP: 90° - LP-BP: 90° - BP-BP: 90° In terms of increasing repulsions between electron pairs, the trend is: BP-BP (least repulsive) < BP-LP < LP-LP (most repulsive). In order to minimize repulsions between electrons situated 90° apart, the lone pair of electrons should be placed in an equatorial position. Show below the correct 3-D model and molecular shape name for PCl3: PCl3 Lewis Structure: PCl3 3-D Model: Name of Molecular Shape: Trigonal Pyramidal Draw a Lewis structure of ClF3. Show the location of atoms and any lone pairs of electrons.
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Draw the Lewis structure for PCl5: The Lewis structure for PCl5 is: P surrounded by 5 Cl atoms, with single bonds between P and each Cl atom. P has 5 valence electrons and each Cl has 7 valence electrons, making a total of 40 valence electrons. The structure Show more…
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Part 1: Lewis structures, polarities, VSEPR geometries, and bond angles These species will be explored: NH3, SO3, CH2I2, C2H4. 1. For every species listed above, write one valid Lewis structure. Include the total number of valence electrons used in the structure. 2. For every species listed above, use the model kit to construct the species. 3. If any double or triple bonds are present, then examine the first Lewis structure to see if resonance may occur. If so, then write all other resonance Lewis structures too. 4. Using electronegativity values from a trusted resource, calculate ΔEN values for each bond. 5. Indicate any permanent bond polarity (see table above) by writing the special arrow along the bond line in all Lewis structures already written. 6. Examine all bond polarities in each species to determine if molecular polarity (MP) exists. Be sure to examine the 3D model. Label each species as "polar" or "nonpolar". 7. For each central atom in each species, name the electronic geometry (arrangement of electron regions around that central atom). When more than one central atom exists in the species, it may be necessary to label the different central atoms (e.g., C1 and C2). 8. For each central atom in each species, name the molecular geometry (arrangement of atoms around that central atom). When more than one central atom exists in the species, it may be necessary to label the different central atoms (e.g., C1 and C2). 9. For each central atom in each species, list the bond angles that exist around it. When more than one central atom exists in the species, label the different central atoms (e.g., C1 and C2). SOO **** numbers 7, 8, and 9 only
Adi S.
Consider the hydrogen cyanide molecule, HCN, and its Lewis formula: H-C≡N. (a) What is the total number of bonding and nonbonding electron pairs around the central atom (the C atom)? (b) What is its parent structure? (c) What is the H-C≡N bond angle? (d) Is the shape of the molecule the same or different from its parent structure? Consider the SF6 molecule and its Lewis formula: F-S-F. (a) What is the total number of atoms and nonbonding electron pairs around the central atom? (b) What is the parent structure? From the model kit, choose the connector piece (atom) that corresponds to the parent structure. Build a 3-D model of this molecule. (i) Use the "connecting sticks" to represent bonding electrons to another atom. Do not use "connecting sticks" when there is only a nonbonding electron in position. Instead, use a blue or green paddle. (iv) Draw a picture of your model here. (d) What is the F-S-F bond angle? (e) Is the shape of the molecule the same or different from its parent structure? Use one or two words to describe the shape of the molecule considering only the atoms, not the "invisible" nonbonding electron pairs.
Sri K.
In I3-, the three lone pairs of electrons can be placed all equatorial, one axial and two equatorial; or two axial and one equatorial. Determine the total number of each type of 90° repulsive interaction for each placement. Determine the total number of each type of 90° repulsive interactions for each placement: Placement of three lone pairs - equatorial one axial - two equatorial - two axial/ one equatorial What we need to do is determine the total number of each type of 90 degree repulsive interactions. The types of interactions are as follows: 90° LP-LP, 90° LP-BP, and 90° BP-BP. In terms of increasing repulsions between electron pairs, the trend is: BP-BP (least repulsive) < BP-LP < LP-LP (most repulsive). In order to minimize repulsions between electron pairs situated 90° apart, the three lone pairs of electrons should be placed. Draw a Lewis structure, the correct 3-D model, and name the molecular shape for I3-. Show the location of atoms and any lone pairs of electrons.
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