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SgPrWAuIs the electron configuration for Zn2+and Ni the same? Explain.A transition metal ion has one electron removed from the 5s orbital. Giving it a completely empty 5s shell and a completely filled 4d orbital. What is the ion?Based on what you know about electron configurations explain why Sb would form +3 and 5+ ions? Write out their electron configurations.
For the quantum number n=3. What is the possible l values? What orbitals do they correspond with? How many total electrons can you have with the quantum number l =1?Lewis Structures and VSEPR ModelLewis Structures•The electrons involved in bonding are the valence shell electrons•Number of electrons in the valence shell is determine by row # excluding the transition metals•Count the number of electron each atom brings in…..That is the total number of electrons you are allowed to have in the molecule.•Put the least electronegative element in the middle of the structure•Nature likes symmetry•Terminal atoms (atoms at the end of the Lewis structure) always satisfy the octet rule•Fluorine and Hydrogen (Hydrogen can only have 2 electrons) alwaysonly make one bond•N, O, and F always obey the octet rule •Atom in the second row of the periodic table cannot have more than 8 electrons surrounding it because no d prbitals are close enough in energy to useFormal charge1.Sum of all the formal charges is equal to the overall charge on the molecule2.Minimize the number of atoms with a formal charge3.Minimize the magnitude of the formal charge (we don’t like #’s >1)4.A more electronegative element is more likelyto have a negative formal charge (there are exceptions)ProblemsDraw the Lewis structures of the following compoundsSF4 NO2NO3-IO3-PO43-
Draw 3 possible Lewis structures for COS. Assign Formal charges. Which structure is the best and why?VSEPR ModelBasic Geometry0 lone pair(shape)1 lone pair(shape)2 lone pair(shape)3 lone pairs(shape)HybridizationTrigonal PlanarTrigonal PlanarbentlinearSp2TetrahedralTetrahedraltrigonal planarbentlinearSp3Trigonal BipyramidTrigonal Bipyramidsee-sawT-shapelinearSp3dOctahedralOctahedralsquare pyramidsquare planarSp3d2Problem
Draw the VSEPR models of the following molecules. What are their geometries, shapes, approximate bond angles, hybridization, and state whether they are polar or nonpolar?a.SbF4-b. BiBr3c.IOF4-d.GeCl4e.SO3MO Theory To the left of NitrogenTo the right of Nitrogen
Notes:-The column containing nitrogen can use either MO structure- for heteronuclear diatomic (two different atoms) use the side that the atoms lay on, if they lay on opposite side of nitrogen use the structure for the right of nitrogen-paramagnetic: magnetic, unpaired electrons- diamagnetic: all the electrons are paired-bonding orbitals: overlap of the electron density of the orbitals-antibonding orbitals: no overlap, signified by a star (*)- bond order = ½ (bonding electrons – antibonding electrons)