An element X reacts with oxygen to form XO 2 and with chlorine to form XCl 4 . XO 2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl 4 is a colorless liquid with a boiling point of 58 °C. (a) XCl 4 reacts with water to form XO 2 and another product. What is the likely identity of the other product?

Hey everyone in this example we have X. O. And X. P. R. Two as products of element X. From its reaction with oxygen and bromine respectively. The reaction XpR two with water produces X. O. And an unknown. We need to identify what the unknown would be. So we're going to write the reaction out x. b. r. two reacting with water. And according to the prompt we produce X. O. And an unknown second product. So we need to determine what this unknown product is and based on our first product being given as X. O. In the product that means we have our X atom here that is bonded to the oxygen. So these two combined with one another and so all that leaves is for women to combine with our hydrogen atom here. So what we would have is H. B. R. As our product. And we need to make sure that this equation is balanced. So we're going to go ahead and place a two in front of our hbr or hydroponic acid so that everything is balanced in our equation. So based on how our products formed, we had the combination of these two atoms and then the combination of these two atoms here to form our products X. O. And H. B. R. And we want to recall that this type of reaction is a double displacement reaction or double replacement reaction. So for our final answer, we would say that the unknown product is HbR and this would be our final answer to complete this example. So I hope that everything I went through is clear. If you have any questions, please leave them down below, and I will see everyone in the next practice video.

Ch.7 - Periodic Properties of the Elements

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Brown 14th Edition

Ch.7 - Periodic Properties of the Elements

Problem 64a

Chapter 7, Problem 64a

An element X reacts with oxygen to form XO₂ and with chlorine to form XCl₄. XO₂ is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl₄ is a colorless liquid with a boiling point of 58 °C. (a) XCl₄ reacts with water to form XO₂ and another product. What is the likely identity of the other product?

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Identify the reaction between XCl4 and water. The given information states that XO2 and another product are formed.

Write the chemical equation for the reaction of XCl4 with water. Since XO2 is one of the products and XCl4 contains chlorine, hypothesize that the other product involves chlorine.

Consider the common reactions of chlorine in compounds when they react with water. Typically, chlorine can form hydrochloric acid (HCl).

Propose a balanced chemical equation: XCl4 + H2O → XO2 + 4 HCl. This equation suggests that hydrochloric acid (HCl) is the other product formed.

Verify the stoichiometry of the proposed reaction to ensure mass and charge are balanced, confirming that all atoms on the reactants side are accounted for in the products.

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Key Concepts

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

Chemical Reactions

Chemical reactions involve the transformation of reactants into products through the breaking and forming of chemical bonds. In this case, the reaction of XCl4 with water illustrates a hydrolysis reaction, where water reacts with a compound to produce new substances, including an oxide and an acid or another product.

Oxides and Halides

Oxides are compounds formed by the reaction of an element with oxygen, while halides are compounds formed with halogens like chlorine. The question indicates that X forms XO2 (an oxide) and XCl4 (a halide), which suggests that X is likely a non-metal that can form stable compounds with both oxygen and chlorine.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In the context of the reaction between XCl4 and water, the likely other product is an acid formed from the chlorine component, such as hydrochloric acid (HCl), indicating that XCl4 acts as a Lewis acid in this reaction.

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Chlorine reacts with oxygen to form Cl2O7. (b) Write a balanced equation for the formation of Cl2O71l2 from the elements.

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Textbook Question

Chlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?

Chlorine reacts with oxygen to form Cl₂O₇ . (d) If the oxygen in Cl₂O₇ is considered to have the -2 oxidation state, what is the oxidation state of the Cl? What is the electron configuration of Cl in this oxidation state?

Textbook Question

An element X reacts with oxygen to form XO₂ and with chlorine to form XCl₄. XO₂ is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl₄ is a colorless liquid with a boiling point of 58 °C. (b) Do you think that element X is a metal, nonmetal, or metalloid?

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Textbook Question

An element X reacts with oxygen to form XO₂ and with chlorine to form XCl₄. XO₂ is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl₄ is a colorless liquid with a boiling point of 58 °C. (c) By using a sourcebook such as the CRC Handbook of Chemistry and Physics, try to determine the identity of element X.

Textbook Question

Write balanced equations for the following reactions: (a) boron trichloride with water (b) cobalt (II) oxide with nitric acid (d) carbon dioxide with aqueous barium hydroxide.

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