Sulfur tetrafluoride (SF 4 ) reacts slowly with O 2 to form sulfur tetrafluoride monoxide (OSF 4 ) according to the following unbalanced reaction: SF 4 (g) + O 2 (g) → OSF 4 (g) The O atom and the four F atoms in OSF 4 are bonded to a central S atom. (b) Write a Lewis structure of OSF 4 in which the formal charges of all atoms are zero.

hey everyone, we're asked to predict the lewis structure of the following compound. And we need to make sure that all of our atoms have zero formal charges first. Let's go ahead and determine the total number of valence electrons will have for our compound. Looking at our oxygen, we have one of oxygen and we're going to multiply this by six valence electrons since oxygen is in our group six a. This will get us the sticks. Next looking at our selenium, we have one of selenium and we're going to multiply this by six as well since it's also in our group six A. This will get assistance valence electrons And lastly looking at our chlorine we have four of chlorine and we're going to multiply this by seven since it's in our group seven A. This will get us to 28 valence electrons. When we add these three values up, we get a total of 40 valence electrons. Now to draw our lewis structure, we were told that selenium was our central atom and we have our four chlorine and our oxygen attached to it as well To complete our chlorine octet we will add three lone pairs onto each chlorine And to get 40 valence electrons, we can go ahead and create a double bond between selenium and oxygen and add two lone pairs to calculate the formal charge of each atom. We can go ahead and take our group number and subtract the sum of our bonds plus our non bonding electrons. Starting off with the formal charge of oxygen. We're going to take our group number of six and subtract the sum of two plus four. Since we have two bonds and four non bonding electrons, this will get us so formal charge of zero, calculating the former charge of selenium. We're going to take our group number of six and subtract the sum of six plus zero, which will also get us to zero. And lastly calculating the formal charge of chlorine. We're going to take our group number of seven and subtract The sum of 1-plus 6, which will also get us to a formal charge of zero. So each atom has a formal charge of zero and this will be our final lewis structure for our compound. Now, I hope that made sense. And let us know if you have any questions.

Ch.9 - Molecular Geometry and Bonding Theories

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Brown 15th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 111b

Chapter 9, Problem 111b

Sulfur tetrafluoride (SF₄) reacts slowly with O₂ to form sulfur tetrafluoride monoxide (OSF₄) according to the following unbalanced reaction: SF₄(g) + O₂(g) → OSF₄(g) The O atom and the four F atoms in OSF₄ are bonded to a central S atom. (b) Write a Lewis structure of OSF₄ in which the formal charges of all atoms are zero.

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Identify the total number of valence electrons in OSF_4. Sulfur (S) has 6 valence electrons, oxygen (O) has 6, and each fluorine (F) has 7. Therefore, the total is 6 (S) + 6 (O) + 4 * 7 (F) = 40 valence electrons.

Place the sulfur (S) atom in the center, as it is the least electronegative element, and arrange the oxygen (O) and four fluorine (F) atoms around it.

Draw single bonds between the central sulfur atom and each of the surrounding atoms (O and F). This uses up 5 bonds * 2 electrons/bond = 10 electrons.

Distribute the remaining 30 electrons to satisfy the octet rule for the surrounding atoms, starting with the more electronegative atoms (O and F). Each F atom should have 6 more electrons to complete its octet, using 24 electrons in total.

Assign the remaining electrons to the central sulfur atom. Check the formal charges: S should have 0 formal charge with 6 electrons around it, O should have 0 formal charge with 8 electrons around it, and each F should have 0 formal charge with 8 electrons around it.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 constructing a Lewis structure, one must account for the total number of valence electrons and ensure that each atom achieves a stable electron configuration, typically resembling that of noble gases.

Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule. It is calculated by taking the number of valence electrons in an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. A formal charge of zero on all atoms in a molecule is often desirable, as it indicates a more stable structure. Understanding formal charges is crucial for drawing accurate Lewis structures and predicting molecular stability.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom, which can affect the molecule's shape and properties. The VSEPR (Valence Shell Electron Pair Repulsion) theory is commonly used to predict molecular geometry, helping to understand how the arrangement of atoms can impact reactivity and interactions with other molecules.

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Textbook Question

The energy-level diagram in Figure 9.40 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the to the molecular orbital. c. Is the bond in ethylene stronger or weaker in the excited state than in the ground state? Why?

Textbook Question

Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur tetrafluoride monoxide 1OSF42 according to the following unbalanced reaction: SF41g2 + O21g2¡OSF41g2 The O atom and the four F atoms in OSF4 are bonded to a central S atom. (a) Balance the equation.

Textbook Question

Sulfur tetrafluoride (SF₄) reacts slowly with O₂ to form sulfur tetrafluoride monoxide (OSF₄) according to the following unbalanced reaction: SF₄(g) + O₂(g) → OSF₄(g) The O atom and the four F atoms in OSF₄ are bonded to a central S atom. (c) Use average bond enthalpies (Table 8.3) to estimate the enthalpy of the reaction. Is it endothermic or exothermic?

Textbook Question

Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur

tetrafluoride monoxide 1OSF42 according to the following

unbalanced reaction:

SF41g2 + O21g2¡OSF41g2

The O atom and the four F atoms in OSF4 are bonded to a

central S atom.

(e) For each of the molecules you drew in part (d), state how many

fluorines are equatorial and how many are axial.

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Textbook Question

Methyl isocyanate, CH₃NCO, was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate.