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Determine the electron and molecular geometry of each molecule. For molecules with two central atoms. Indicate the geometry about each central atom.
a.
b.
c.
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Introductory Chemistry (5th Edition) (Standalone Book)
- As a general rule, MX molecules (where M represents a central atom and X represents terminal atoms; n = 2 5) are polar if there is one or more lone pairs of electrons on M. NH3 (M = N, X = H, n = 3) is an example. There are two molecular structures with lone pairs that are exceptions to this rule. What are they?arrow_forwardConsider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.arrow_forwardWhy is the geometric structure of a molecule important, especially for biological molecules?arrow_forward
- A. What is the electron-pair geometry for Xe in XeO3? There are lone pair(s) around the central atom, so the geometry of XeO3 is B. What is the electron-pair geometry for Se in SeH₂? There are lone pair(s) around the central atom, so the geometry of SeH₂ isarrow_forwardWhich molecule has polar bonds but is overall nonpolar? O A. H2S О В. Оз O C. SO3 O D. SO2arrow_forwardWrite the Lewis structure for each molecule.a. CH2O b. C2Cl4c. CH3NH2 d. CFCl3 (C central)arrow_forward
- 2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.arrow_forwardWrite an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds.a. Al2O3 b. ClF5c. MgI2 d. XeO4arrow_forwardConsider lewis structure of NH3. how many Ione pairs are on nitrogen: 1 2 4 0 3 When the predicted Lewis structure of ArO3, ^2+ is drawn correctly, how many lone pairs are on the central atom? O A.3 O B. 2 O C.o O D.4 O E.1 How many valence electrons would an AX4 molecule have if A was a group 6A atom and X was from group 7 A? O A. 32 О B. 36 O C. 30 O D. 28 O E. 34arrow_forward
- For each of the following molecular compounds, identify the atom that is most likely to be found in the center of its Lewis structure. a. CBr4b. SO2c. H2S d. NOF e. BI3f. SO3g. AsH3h. HCNarrow_forwardo=c=0 ö-s=ö 10. Lewis electron dot diagrams for CO2 and SO2 are given above. Which of the following is true regarding the molecular geometry and the polarity for both substances? A. they are both linear because they only have two non-central atoms B. they are both polar molecules due to the polar bonds between the central atom and oxygen C. the lone pair of electrons on the S atom in SO, make it a polar bent molecule D. they are both nonpolar because the formal charge on each atom is zero 150 to 140 130arrow_forward1. Determine the Lewis structure, shape, and polarity of the following molecules a. BrO2-, bromite ion b. BrO3-, bromate ion c, Cl207, dichlorine heptoxide 2. Write all the valid Lewis structures of bromate ion.arrow_forward
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