Calculate the formal charge of each atom by drawing the most probable (stable) Lewis structures of the molecules given below the molecular formulas and atomic numbers in parentheses. Also, determine the VESPR structures and names (tetrahedral, octahedral, etc.) of each molecule using the Lewis structures you have determined. a) XY2 (X:7, Y:8) b) XY4 (X:16, Y:9) c) XY6 (X:15, Y:9) d) XY4 (X:10, Y:17) e) XY32- (X:16, Y:8)

1. a) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula CBr4 b) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula NH3

Draw the structures and assign formal charges, if applicable, to these structures. BH3 and BH4 Draw I with three lone pairs and add formal charges, if applicable. Which atoms have a complete octet? a) The B in BH4 b) iodine c) The B in BH3

We can draw three inequivalent Lewis structures for the arsenite ion , AsO33- . The concepts of formal charge and electronegativity can help us choose the structure that is the best representation.1. Assign formal charges to the elements in each of the structures below.Note: Count oxygen atoms starting from the left for each structure.   A B C Formal ChargeAsO1O2O3 2. The best Lewis structure for AsO33- is (A,B, or C)

Determine the formal charge for the atom indicated in the structures below. ASSUME that the structures are drawn correctly and that you do not have to change them due to formal charge issues. The external atom in this structure. :O: :O! Ar 11 :0: The central atom in this structure. = :0: (1 Si = : 0: 2- 1. +1 2. +2 3. +3 4. 0 5. -3 6.-2 7. -1

Draw the following lewis structures and give the formal charges for the atoms as well as the number of valence electrons A)SF4 B)ICl3 C)CH3CN D)CCl4 E)BrF5

Draw all possible resonance structures for SO2, S0,, and SO. Use the resonance structures to solve the problems below. (a) Arrange these species in order of increasing S-O bond length (shortest bond first). O SO O SO O SO2 O SO2 O so;²- O SO O So3? O SO2 (b) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.) SO: -Select-v bonds between S and 0. -Select--- v bonds between S and O. SO2: Select-v bonds between S and O. (c) Match each species with the correct formal charge on the central S atom. SO: Select- charge on S. SO2: Select--v charge on S. SO32:-Select-vcharge on S. (d) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. so: -Select-vaverage charge on…

1. Write Lewis symbols for the following atoms. (1pt each) (a) Kr (b) Ge (c) N (d) Ga (e) As (f) Rb 2. Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (2 pts each) (а) FCI (b) I2 (c) SF2 (d) NF3 (е) Н-Те 3. By means of Lewis structures, represent bonding between the following pairs of elements (Your structures should show whether the bonding is essentially ionic or covalent): (2 pts each) (a) Cs and Br (b) H and Sb (c) B and Cl (d) Cs and Cl (e) Li and O (f) Cl and I 4. Assign formal charges to each of the atoms in the following structures. (3 pts each) (a) [H–C=C:]¯ (c) [CH3–CH-CH3]* (b) |2– :0: :0: 5. What is the formal charge of the indicated atom in each of the following structures? (2 pts each) (a) the central O atom in 03 (b) Al in AIH4- (c) Cl in Cl03 (d) Si in SiF62- (e) Cl in CIF3 6. Arrange the following elements in the order of decreasing electronegativity: fluorine, bromine, lithium, francium, silicon. (1 pt each per…

Please help me solve the following question, explain and make sure everything is correct, thanks!

A newly discovered element Lm has 3 valence electrons. How many total valence electrons are in LmF3 molecule, a molecule that Lm forms with fluorine?  Draw a valid Lewis Structure for the molecule LmF3 that Lm forms with fluorine and use your Lewis structure to determine the number of lone pairs of electrons around the central Lm atom in this molecule.  What is the formal charge of Lm in LmF3? (Number and sign of formal charge) What is the hybridization of Lm according to the hybrid orbital model?