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Chapter 20: Problem 46

Tin forms compounds in the \(+2\) and \(+4\) oxidation states. Therefore, when tin reacts with fluorine, two products are possible. Write balanced equations for the production of the two tin halide compounds and name them.

Short Answer

Expert verified
The balanced equations for the production of two tin halide compounds are: \(Sn + \frac{1}{2}F_2 \rightarrow SnF_2\) - Tin(II) fluoride \(Sn + 2F_2 \rightarrow SnF_4\) - Tin(IV) fluoride

Step by step solution

01

Identify the possible compounds

Since tin has two possible oxidation states, +2 and +4, it can form two different compounds with fluorine, which has an oxidation state of -1. These compounds are Tin(II) fluoride and Tin(IV) fluoride.
02

Write the unbalanced equation and balance for Tin(II) fluoride

To write the equation, combine the elements for tin (Sn) and fluorine (F): \[Sn + F_2 \rightarrow SnF_2\] Now, we need to balance the equation by ensuring an equal number of each element on both sides. Currently, there are 2 fluorine atoms on the left side of the equation and only 1 on the right side. To balance this, we can add a coefficient of 2 to the fluoride ion on the product side: \[ Sn + \frac{1}{2}F_2 \rightarrow SnF_2\]
03

Write the unbalanced equation and balance for Tin(IV) fluoride

Repeat the process for tin(IV) fluoride (SnF4): \[Sn + F_2 \rightarrow SnF_4\] To balance the equation, we can see that there is only 1 tin atom on both sides, but Fluorine needs 4 atoms on the product side to match Tin(IV)'s oxidation state, so we add a coefficient of 2 on both sides of the equation: \[ Sn + 2F_2 \rightarrow SnF_4\]
04

Write the names of both compounds

Both compounds are correctly named as Tin(II) fluoride for SnF2 and Tin(IV) fluoride for SnF4. So, the balanced equations for the production of two tin halide compounds are: \(Sn + \frac{1}{2}F_2 \rightarrow SnF_2\) - Tin(II) fluoride \(Sn + 2F_2 \rightarrow SnF_4\) - Tin(IV) fluoride

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Most popular questions from this chapter

Fluorine reacts with sulfur to form several different covalent compounds. Three of these compounds are \(\mathrm{SF}_{2}, \mathrm{SF}_{4},\) and \(\mathrm{SF}_{6} .\) Draw the Lewis structures for these compounds, and predict the molecular structures (including bond angles). Would you expect \(\mathrm{OF}_{4}\) to be a stable compound?

Although nitrogen trifluoride \(\left(\mathrm{NF}_{3}\right)\) is a thermally stable compound, nitrogen triiodide (NI \(_{3} )\) is known to be a highly explosive material. \(\mathrm{NI}_{3}\) can be synthesized according to the equation $$ \mathrm{BN}(s)+3 \mathrm{IF}(g) \longrightarrow \mathrm{BF}_{3}(g)+\mathrm{NI}_{3}(g) $$ a. What is the enthalpy of formation for \(\mathrm{NI}_{3}(s)\) given the enthalpy of reaction \((-307 \mathrm{kJ})\) and the enthalpies of formation for \(\mathrm{BN}(s)(-254 \mathrm{kJ} / \mathrm{mol}), \mathrm{IF}(g)(-96 \mathrm{kJ} / \mathrm{mol})\) and \(\mathrm{BF}_{3}(g)(-1136 \mathrm{kJ} / \mathrm{mol}) ?\) b. It is reported that when the synthesis of \(\mathrm{NI}_{3}\) is conducted using 4 moles of IF for every 1 mole of \(\mathrm{BN}\) , one of the by-products isolated is \(\left[\mathrm{IF}_{2}\right]^{+}\left[\mathrm{BF}_{4}\right]^{-} .\) What are the molecular geometries of the species in this by-product? What are the hybridizations of the central atoms in each species in the by-product?

There are three known xenon fluoride covalent compounds: \(\mathrm{XeF}_{2}, \mathrm{XeF}_{4},\) and \(\mathrm{XeF}_{6} .\) In general, the xenon fluoride compounds must be stored in an inert atmosphere, free of oxygen and water. Why is this the case?

Sodium tripolyphosphate \(\left(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\right)\) is used in many synthetic detergents. Its major effect is to soften the water by complexing \(\mathrm{Mg}^{2+}\) and \(\mathrm{Ca}^{2+}\) ions. It also increases the efficiency of surfactants, or wetting agents, that lower a liquid's surface tension. The pK value for the formation of \(\mathrm{MgP}_{3} \mathrm{O}_{10}^{3-}\) is \(-8.60 .\) The reaction is $$ \mathrm{Mg}^{2+}(a q)+\mathrm{P}_{3} \mathrm{O}_{10}^{5-}(a q) \rightleftharpoons \mathrm{MgP}_{3} \mathrm{O}_{10}^{3-}(a q) $$ Calculate the concentration of \(\mathrm{Mg}^{2+}\) in a solution that was originally \(50 . \mathrm{ppm} \mathrm{Mg}^{2+}(50 . \mathrm{mg} / \mathrm{L} \text { of solution) after } 40 . \mathrm{g} \text { of }\) \(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\) is added to 1.0 \(\mathrm{L}\) of the solution.

Calcium and magnesium are essential for human life. Explain their importance.
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