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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 114a
Capitolo 9, Problema 114a

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.

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Step 1: Identify the reactants and products in the chemical reaction. In this case, the reactants are sulfur tetrafluoride (SF4) and oxygen (O2), and the product is sulfur tetrafluoride monoxide (OSF4).
Step 2: Start by balancing the atoms that appear in the most complex molecules first. In this case, we start with sulfur (S) and fluorine (F). Since there is one S atom in both the reactants and products, it is already balanced. For F, there are 4 atoms in both the reactants and products, so it is also balanced.
Step 3: Next, balance the oxygen (O) atoms. There are 2 O atoms in the reactant (O2) and 1 O atom in the product (OSF4). To balance this, we need to put a coefficient of 1/2 in front of O2 in the reactants.
Step 4: However, in chemical equations, we avoid fractional coefficients. Therefore, to get rid of the 1/2, we multiply all the coefficients by 2. This gives us 2SF4 + O2 → 2OSF4.
Step 5: Finally, check to make sure that the equation is balanced by counting the atoms of each element on both sides of the equation. There should be the same number of each type of atom on the reactant side as there is on the product side.

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Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is achieved by adjusting the coefficients in front of the chemical formulas. The law of conservation of mass dictates that matter cannot be created or destroyed in a chemical reaction, thus requiring balanced equations to accurately represent the reaction.
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Molecular Structure and Bonding

Understanding molecular structure and bonding is crucial for predicting how molecules interact during a reaction. In the case of sulfur tetrafluoride monoxide (OSF4), the central sulfur atom is bonded to one oxygen atom and four fluorine atoms, which influences the molecule's reactivity and the overall reaction mechanism. Knowledge of molecular geometry can also aid in visualizing how these atoms are arranged.
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Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced, based on the balanced equation. In this context, stoichiometry will help determine the correct coefficients needed to balance the reaction between sulfur tetrafluoride and oxygen, ensuring that the proportions of reactants and products are accurately represented.
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Domanda del libro di testo

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?

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Domanda del libro di testo

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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Domanda del libro di testo

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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Domanda del libro di testo

The energy-level diagram in Figure 9.36 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 π 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 p2p to the p*2p molecular orbital. (c) Is the C¬C bond in ethylene stronger or weaker in the excited state than in the ground state? Why?

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