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- Part A) Consider the structural changes that occur in the following molecules. Begin by drawing the best Lewis Structure for each of the following molecules. BH3 CH4 NH3 H2O HF Part B)What are the ideal bond angles for each structure, and which are expected to be distorted? For the ones that are distorted look up on the internet and record their experimental values here: Part C)According to Lewis and VSEPR theory, why do these changes occur?A.) What is the electron-pair geometry for I in ICl4-? ____There are _____ lone pair(s) around the central atom, so the geometry of ICl4- is _____.B.) What is the electron-pair geometry for I in ICl5? ______There are _____ lone pair(s) around the central atom, so the geometry of ICl5 is _______.A. What is the electron-pair geometry for Al in AlBr3? _______There are _____ lone pair(s) around the central atom, so the geometry of AlBr3 is ________.B. What is the electron-pair geometry for P in PCl6-? _______There are ______ lone pair(s) around the central atom, so the geometry of PCl6- is _________.
- TeS2 the electron pair geometry is? the molecular geometry is? how many double bonds does it havePropylene, C3H6,C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule? (b) How many valence electrons are used to make σσ bonds in the molecule? (c) How many valence electrons are used to make ππ bonds in the molecule? (d) How many valence electrons remain in nonbonding pairs in the molecule? (e) What is the hybridization at each carbon atom in the molecule?Is it possible to draw a resonance structure with the lone pair? What is the hybridization of the heteroatom? Draw a valence bond orbital diagram to show the location of the lone pair (you do not need to draw any orbitals to show s bonds). In what orbital are the electron pairs located?
- How many ?σ and ?π bonds are in this molecule?How many ? and ? bonds are in this molecule?Which is true about valence bond theory? Select the correct answer below: Describes how the direction of overlap of s orbitals influences bond energy. Describes how two atoms can never overlap and share electrons. Describes how s orbitals are dumbbell shaped, they can only overlap end to end. Describes how the overlap of half-filled atomic orbitals yields a pair of shared electrons.
- Define the dipole moment for the molecule?The electronic geometry of PF3 is while the molecular geometry due to the presence of a lone pair. The F-P-F bond angle is is than 109.5 degrees found in the electronic geometry.How can sigma bonds in molecules be source of electrons? (Include a drawing in the explanation as needed)