(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe¬O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

검증된 단계별 안내

insert step 1: Start by drawing the Lewis structure of XeO3 with zero double bonds. Place Xe in the center and connect it to three O atoms with single bonds. Complete the octet for each O atom by adding lone pairs.

insert step 2: Draw the Lewis structure of XeO3 with one double bond. Choose one Xe-O bond to convert into a double bond. Adjust the lone pairs on the involved O atom to maintain its octet.

insert step 3: Draw the Lewis structure of XeO3 with two double bonds. Select two Xe-O bonds to convert into double bonds. Adjust the lone pairs on the involved O atoms to maintain their octets.

insert step 4: Draw the Lewis structure of XeO3 with three double bonds. Convert all three Xe-O bonds into double bonds. Adjust the lone pairs on the O atoms accordingly.

insert step 5: Evaluate each structure for formal charges and the octet rule. Determine which structure has the most favorable formal charges and if any satisfy the octet rule for all atoms.

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Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, allowing chemists to predict molecular geometry and reactivity. In the case of xenon trioxide (XeO3), drawing different Lewis structures involves varying the number of double bonds between xenon and oxygen atoms.

Octet Rule

The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. In the context of XeO3, evaluating whether the resonance structures satisfy the octet rule involves checking if each atom, particularly xenon and oxygen, has a complete octet in the proposed Lewis structures.

Formal Charge

Formal charge is a concept used to determine the charge of an atom in a molecule based on its valence electrons and the electrons it owns in a Lewis structure. It is calculated using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). In the analysis of XeO3, identifying which Lewis structure yields the most favorable formal charges helps in determining the most stable resonance structure, as structures with lower formal charges are generally more favorable.