Draw the Lewis structures and determine which of these molecules is least likely to exist. (A) SF; (B) SeF4 (C) PF3 (D) OF4 (E) SF4 Draw all 5 structures with 1 central atom. All of the other atoms are attached to the central atom.

An elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.

Draw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+

Which pair of elements has the most similar Lewis structures?(a) N and S (b) F and Ar(c) Cl and Ar (d) O and S

Write resonance forms that describe the distribution of electrons in each of these molecules or ions. (a) selenium dioxide, OSeo (b) nitrate ion, NO3 (c) nitric acid, HNO3 (N is bonded to an OH group and two O atoms) (d) benzene, CGH5: H (e) the formate ion:

Draw Lewis structures for HFO4, HFO3, HC0O4, HC0O3, HCO2. (These molecules have the halogen atom as the central atom. All O atoms are attached to the halogen. The hydrogen atom is bonded to one of the O atoms.) Use formal charges to determine which molecule is least likely to occur in nature. (A) HFO4 (B) HC(O2 (C) HC!O3 (D) HFO3 (E) HC\O4 DO000

Which two species have the same number of lone electron pairs in their Lewis structures?(a) H2O and H3O+(b) NH3 and H3O+(c) NH3 and CH4(d) NH3 and NH4+

Write Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) BrF3 (b) AsF5 (c) BI3 (d) AsF6−

In the Lewis structure of which molecule the central atom has an incomplete octet?          (A) GeF2          (B) KrF2          (C) SeF2          (D) All of them

Draw the Lewis Dot Structures for the following molecules. (Make sure to show the bonds and lone pairs clearly) (a) Formaldehyde (H2CO) (b) Ammonia (NH3)