GeCl 4 reacts with Cl - to give GeCl 6 2- , but CCl 4 does not react with excess Cl - . Explain.

Welcome back everybody. Our next question says, why does S IC L four react with CL minus to produce S IC L six? Whereas CCL four does not react with CL minus A because CL is more electron than C B because si has vacant P orbitals while C does not C because si has vacant D orbitals while C does not or D because C is more electron than SI. So lets think about these two elements because were comparing them silicon and carbon, both are group four A elements, meaning they have four valence electrons but silicon is in row three whereas carbon is in row two. So we think about bonds they can form. Well, both have this two S 22 P two arrangement but in row two with carbon carbon only has S and P orbitals since it always only has the one and two energy levels available, silicon has D orbitals as well. So we know that when an element has D orbitals available, it can have an expanded octet. So it can bond with more than four atoms, it can hybridize the S and P orbitals can hybridize with those D orbitals offering more orbitals to bind. Whereas if only S and P orbitals are available, sp three hybridization is the greatest number of orbitals available for bonding, which would be four bonds possible. So, carbon cannot form more than four bonds. And that's why it wouldn't react with chloride ions to produce anything different. Whereas silicon chloride could take on some additional chloride bonds. So let's look at our answer. Choices. We would see that choice C is our correct explanation because Si has vacant D orbitals. While C does not, when we look at our other answer, choices, choice B says si has vacant P orbitals while C is not, well, this is not correct, both have vacant P orbitals available. So that wouldn't be our explanation when we look at choice. A because chloride is more electron negative than carbon. Well, that's true, but it's not our explanation. It's also more electron than silicon. So it doesn't explain that difference. So I'll put also silicon and then finally choice D because C is more electron than si. Well, that is true as you go up the periodic table, electronegativity increases since the electrons are closer to the nucleus. But this is not the explanation of why carbon doesn't go on to form more than four bonds. So that's why trustee isn't correct. So once again, if we're looking for the reasoning, why S IC L four will react with chloride ions to produce S IC L six. But CCL four does not is choice C because si has vacant de orbitals while C does not see you in the next video.

Ch.22 - The Main Group Elements

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

All textbooks

McMurry 8th Edition

Ch.22 - The Main Group Elements

Problem 22.47

Chapter 22, Problem 22.47

GeCl₄ reacts with Cl^- to give GeCl₆^2-, but CCl₄ does not react with excess Cl^-. Explain.

Verified step by step guidance

Identify the central atoms in GeCl_4 and CCl_4, which are Ge (Germanium) and C (Carbon), respectively.

Consider the electronic configuration and oxidation states of Ge and C. Ge can expand its octet due to available d-orbitals, while C cannot because it lacks d-orbitals.

Understand that GeCl_4 can accept additional Cl^- ions to form GeCl_6^{2-} because Ge can accommodate more than 8 electrons in its valence shell.

Recognize that CCl_4 does not react with Cl^- because carbon cannot expand its octet beyond 8 electrons, as it only has s and p orbitals available.

Conclude that the ability of Ge to expand its octet allows GeCl_4 to react with Cl^-, while the lack of d-orbitals in carbon prevents CCl_4 from doing the same.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

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

Coordination Chemistry

Coordination chemistry involves the study of complex compounds formed between metal ions and ligands. In this context, GeCl4 acts as a Lewis acid, accepting electron pairs from Cl- ligands to form the stable complex GeCl62-. Understanding how ligands interact with metal centers is crucial for explaining the reactivity of these compounds.

Lewis Acids and Bases

Lewis acids are substances that can accept an electron pair, while Lewis bases donate an electron pair. GeCl4 is a Lewis acid that can react with Cl- ions, whereas CCl4 is a neutral molecule and does not exhibit Lewis acid behavior. This distinction is key to understanding why GeCl4 reacts while CCl4 does not.

Oxidation States and Stability

The oxidation state of an element in a compound can influence its reactivity and stability. In GeCl4, germanium is in the +4 oxidation state, which allows it to stabilize additional negative charges when reacting with Cl-. In contrast, CCl4 does not have a favorable oxidation state for further reaction with Cl-, leading to its inertness in this scenario.

GeCl4 reacts with Cl- to give GeCl62-, but CCl4 does not react with excess Cl-. Explain.