Gaseous iodine pentafluoride, IF 5 , can be prepared by the reaction of solid iodine and gaseous fluorine: I 2 (s) + 5 F 2 (g) → 2 IF 5 (g) A 5.00-L flask containing 10.0 g of I 2 is charged with 10.0 g of F 2 , and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (c) Draw the Lewis structure of IF 5 .

Hello. Everyone in this video we're going to draw out the lewis structure for Penta chloride which is PCL five. So first things first we're gonna go ahead and calculate for the total number of valence electrons. So for phosphorus that's going to be in group 58. That means that we have five electrons or valence electrons per atom. So in our compound or molecule we have one phosphorus atom and then we have five electrons per atom. So that will give us five electrons total for phosphorus. And then for chlorine here we have five atoms of chlorine and chlorine is in group 78. So there's going to be seven valence electrons per atom. So multiplied by seven giving us total 35 for the whole molecule. Then five plus 35 is going to be 40. So there should be 40 total valence electrons in this molecule. So now choosing the central atom we're comparing phosphorus with chlorine. Well if there's more than one of another atom, usually that's the indicator that that's not going to be the central atom. So phosphorus in our case will be our central atom and of course it's connected to five different chlorine atoms. So go ahead and draw those in. Alright. And to fulfill its octet, the chlorine has to have eight total electrons on it. Right now it's shared with the phosphorus. So that's considered to then we need six more. So we'll draw out three lone pairs per chlorine atom. Now we do this we can see that each chlorine will have eight toilet trans around it and we have five chlorine to five Or yes, five times are eight valence electrons will give us a total of 40 electrons in which we have used. And so this right here is going to be our LewiS structure for our pento chloride.

Ch.10 - Gases

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Brown 14th Edition

Ch.10 - Gases

Problem 126c

Chapter 10, Problem 126c

Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous fluorine: I₂(s) + 5 F₂(g) → 2 IF₅(g) A 5.00-L flask containing 10.0 g of I₂ is charged with 10.0 g of F₂, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (c) Draw the Lewis structure of IF₅.

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Identify the central atom in IF5, which is iodine (I), as it is less electronegative than fluorine (F).

Count the total number of valence electrons available. Iodine has 7 valence electrons, and each fluorine has 7 valence electrons. Since there are 5 fluorine atoms, the total is 7 + (5 * 7) = 42 valence electrons.

Place iodine in the center and arrange the 5 fluorine atoms around it, forming single bonds between iodine and each fluorine. This uses up 10 electrons (5 bonds * 2 electrons per bond).

Distribute the remaining 32 electrons to satisfy the octet rule for the fluorine atoms. Each fluorine needs 6 more electrons to complete its octet, using up 30 electrons (5 fluorines * 6 electrons).

Place the remaining 2 electrons as a lone pair on the iodine atom, completing the Lewis structure of IF5 with iodine having an expanded octet.

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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, which is crucial for understanding molecular geometry and reactivity. In the case of IF5, drawing its Lewis structure involves determining the total number of valence electrons and how they are distributed among the iodine and fluorine atoms.

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 polarity. For IF5, understanding its geometry is essential for predicting its physical and chemical properties, as well as its reactivity with other substances.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass and the mole concept. It allows chemists to predict how much of each reactant is needed and how much product will be formed. In the context of the reaction producing IF5, stoichiometry is used to determine the limiting reagent and the amounts of iodine and fluorine consumed during the reaction.

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Textbook Question

Natural gas is very abundant in many Middle Eastern oil fields. However, the costs of shipping the gas to markets in other parts of the world are high because it is necessary to liquefy the gas, which is mainly methane and has a boiling point at atmospheric pressure of -164 °C. One possible strategy is to oxidize the methane to methanol, CH₃OH, which has a boiling point of 65 °C and can therefore be shipped more readily. Suppose that 3.03×10⁸ m³ of methane at atmospheric pressure and 25 °C is oxidized to methanol. (a) What volume of methanol is formed if the density of CH₃OH is 0.791 g/mL?

Textbook Question

Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous fluorine: I₂(s) + 5 F₂(g) → 2 IF₅(g) A 5.00-L flask containing 10.0 g of I₂ is charged with 10.0 g of F₂, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (a) What is the partial pressure of IF5 in the flask?

Textbook Question

Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous fluorine: I₂(s) + 5 F₂(g) → 2 IF₅(g) A 5.00-L flask containing 10.0 g of I₂ is charged with 10.0 g of F₂, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (b) What is the mole fraction of IF₅ in the flask?

Textbook Question

Gaseous iodine pentafluoride, IF₅, can be prepared by the reaction of solid iodine and gaseous fluorine: I₂(s) + 5 F₂(g) → 2 IF₅(g) A 5.00-L flask containing 10.0 g of I₂ is charged with 10.0 g of F₂, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (d) What is the total mass of reactants and products in the flask?

Textbook Question

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28 °C and 99.06 kPa pressure. (a) Write balanced chemical equations for the reactions that occur between hydrochloric acid and each component of the mixture.

Textbook Question

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28 °C and 99.06 kPa pressure. (c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture.

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