Name each ionic compound. a. SnCl 4 b. PbI 2 c. Fe 2 O 3 d. CuI 2 e. HgBr 2 f. CrCl 2

Hey everyone, let's go ahead and practice naming these compounds. So starting off with a, we have a gcl. Now before we start naming these, let's go ahead and look at our cat eons and are an ions individually. And the reason why we want to do this is because the charge of our caddy on is going to affect the way we name it. And that's because silver is a transition metal. So silver can have more than one possible charge. So to figure out its charge, we need to look at our chlorine. So we know that chlorine has that -1 charge since it's in our group seven a. In order for this compound to be balanced, that must mean silver has a plus one charge. When we name this, it's going to be silver one chloride. So we did note our charge for silver With our Roman numeral one. And the way we name chlorine is that we keep it space name but we changed the ending into ID. Moving on to be, we have see us now we know that Sue is copper and copper again is a transition metal. So we have to look at our sulfur in order to determine its charge. And sulfur is in our group six A. So it has a minus to charge for this to be balanced. It looks like copper must have a plus two charge When we name this, it's going to follow the same naming system where we have copper to sulfide. Lastly looking at our third compound, we have F E B R three. Now we know that iron is also one of our transition metals. And so we need to look at grooming in order to determine its charge. So we know that bromine has that -1 charge since it's in our group seven a. But we can see right here that we have a subscript of three. So that means we needed three of grooming in order to balance out our iron. So to balance this out, it looks like iron must have a plus three charge. When we name this, it's going to be iron three bromide and this is going to be our final answers. So I hope this made sense. And let us know if you have any other questions.

Ch.3 - Molecules, Compounds & Chemical Equations

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Tro 4th Edition

Ch.3 - Molecules, Compounds & Chemical Equations

Problem 38a,b,c,d,e,f

Chapter 3, Problem 38a,b,c,d,e,f

Name each ionic compound. a. SnCl₄ b. PbI₂ c. Fe₂O₃ d. CuI₂ e. HgBr₂ f. CrCl₂

Verified step by step guidance

Identify the cation and the anion in the compound. In SnCl_4, Sn is the cation (tin) and Cl is the anion (chloride).

Determine the charge of the anion. Chloride (Cl) has a charge of -1.

Calculate the total negative charge from the anions. Since there are four chloride ions, the total negative charge is 4(-1) = -4.

Determine the charge of the cation. The total positive charge must balance the total negative charge. Therefore, the charge on Sn must be +4.

Name the compound by stating the name of the cation followed by the anion. Since tin can have multiple oxidation states, specify the charge of the tin cation using Roman numerals. The name of SnCl_4 is tin(IV) chloride.

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Key Concepts

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

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable compound. The properties of ionic compounds include high melting and boiling points, and they typically dissolve in water to form electrolytes.

Nomenclature of Ionic Compounds

The nomenclature of ionic compounds involves naming the cation first, followed by the anion. For cations derived from metals, the name remains the same as the element, while anions typically have their names modified to end in '-ide' for simple anions or use specific names for polyatomic ions. In the case of transition metals, the oxidation state is indicated using Roman numerals.

Tin (Sn) and its Oxidation States

Tin (Sn) can exhibit multiple oxidation states, commonly +2 and +4. In the compound SnCl4, tin is in the +4 oxidation state, as it forms four bonds with chloride ions (Cl-). Understanding the oxidation state is crucial for correctly naming the compound and recognizing its chemical behavior.