Sg Pr W Au Is the electron configuration for Zn 2 and Ni the same Explain A

Sg pr w au is the electron configuration for zn 2 and

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Sg Pr W Au Is the electron configuration for Zn 2+ 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.
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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 Model Lewis 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) always only 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 use Formal charge 1. Sum of all the formal charges is equal to the overall charge on the molecule 2. Minimize the number of atoms with a formal charge 3. Minimize the magnitude of the formal charge (we don’t like #’s >1) 4. A more electronegative element is more likely to have a negative formal charge (there are exceptions) Problems Draw the Lewis structures of the following compounds SF 4 NO 2 NO 3 - IO 3 - PO 4 3-
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Draw 3 possible Lewis structures for COS. Assign Formal charges. Which structure is the best and why? VSEPR Model Basic Geometry 0 lone pair (shape) 1 lone pair (shape) 2 lone pair (shape) 3 lone pairs (shape) Hybridizatio n Trigonal Planar Trigonal Planar bent linear Sp2 Tetrahedral Tetrahedral trigonal planar bent linear Sp3 Trigonal Bipyramid Trigonal Bipyramid see-saw T- shape linea r Sp3d Octahedral Octahedral square pyramid square planar Sp3d2 Problem
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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. SbF 4 - b. BiBr 3 c. IOF 4 - d. GeCl 4 e. SO 3 MO Theory To the left of Nitrogen To the right of Nitrogen
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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)
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