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Understanding Copper Compounds: Key Differences and Naming Conventions

This chapter explores the essential differences between copper compounds, specifically Cu2O and CuO. It emphasizes the importance of precise naming in distinguishing similar compounds, as well as the characteristics and uses of each compound. Cu2O, a red powder, is known as a fungicide, while CuO, a black powder, is commonly used in batteries. Furthermore, the chapter delves into the fundamentals of naming ionic and covalent compounds, including the roles of cations and anions, and provides strategies for balancing charges in chemical formulas.

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Understanding Copper Compounds: Key Differences and Naming Conventions

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  1. Chapter 9 Chemical Names and Formulas

  2. Copper Compounds • What is the difference between Cu2O and CuO? Is there any difference? • You may think that there is very little difference between the two, but there is! Naming compounds very specifically is important in order to tell the difference between similar compounds? • Cu2O • Red powder • fungicide • CuO • Black powder • Used in batteries

  3. Remeber Naming Ions? • What is a cation? • Cations – positively charged ion • How many electrons does Group 1,2, and 3 lose? • Groups 1,2, and 3 lose electrons • Group 1 – lose 1 electron • Group 2 – lose 2 electrons • Group 3 – lose 3 electrons

  4. Remember Naming Ions? • Anion – negatively charged ion • Groups 5,6, and 7 generally gain electrons • Group 5 – gain 3 electrons • Group 6 – gain 2 electrons • Group 7 – gain 1 electron

  5. Naming Ions Transition metals usually lose electrons, how many electrons they lose depends on the element You should memorize these metal ions – Table 9.2!

  6. Naming Ions • If you actually think about it, it will make sense why some of the transition elements could have two different ions • Ex: Tin (Sn) forms both a +2 and a +4 cation • Why? (Hint: Use the periodic table and electron configuration.) • +2 cation: Sn= [Kr] 5s24d10 5p2– loses 2 from the 5psubshell • +4cation: Sn can lose both the 2 electron’s from the 5p subshell AND two electrons from the 5s subshell to achieve full stability

  7. Learning Objective of the Day: Writing and naming ionic compounds. Writing and naming covalent compounds.

  8. Polyatomic Ions Ions composed of more than 1 atom You just have to memorize these – Table 9.3 Most end in –ite or –ate -ite tells you there is 1 less oxygen atom than the –ate ending

  9. Naming and Writing Formulas for Ionic Compounds • what do ionic compounds contain? • Ionic compounds – contain a metal and a nonmetal • How do we name a binary ionic compound (binary means composed of 2 elements)? • Place the cation name first, then the anion name • Usually add –ide to the end of the anion name

  10. Naming and Writing Formulas for Ionic Compounds • What would Cs2O be? • Cesium oxide • NaF? • Sodium fluoride • Cu2O (hint: copper has two possible ions! Which one is it?) • Copper (I) oxide • SnS2 • Tin (IV) Sulfide • Mn2O3 • Manganese (III) oxide • LiCN • Lithium cyanide • (NH4)2C2O4 • Ammonium oxalate (the –ide ending is usually left out if the anion is a polyatomic ion)

  11. Naming and Writing Formulas for Ionic Compounds • To write a formula for a binary ionic compound, we need to go back to Ch. 7 and balance the charges • Ex: iron (III) oxide • Fe+3 O-2 • Fe2O3 • Ca+2 S-2 • Ca2S2….reduce to CaS • Remember crisscross the charge and reduce subscripts to the lowest whole number ratio

  12. Naming and Writing Formulas for Ionic Compounds • Another way…just think about how you would balance the charges out by finding the least common multiple • K+1 N-3 • We need a 3 to balance out the +1 on K (1 x 3 =3) and a 1 to balance out the -3 on N (1 x 3) = 3 • So K3N • Ba+2 S-2 • Both have a 2 charge, they balance each other out • BaS

  13. Naming and Writing Formulas for Ionic Compounds • For polyatomic ions, keep the ion together – balance the overall charge of the ion • Ex: Ca+2 (NO3)-1 • Ca(NO3)2 • Use parentheses to set off the polyatomic ion only if there is than one of the polyatomic ion • Ex: Li+1 (CO3)-2 • Li2CO3 – no parentheses because there is only one polyatomic ion • Ex: NH4+1 (SO3)-2 • (NH4)2SO3

  14. Naming and Writing Formulas for Molecular Compounds • What is a binary molecular compound? • A compound composed of 2 elements that are both nonmetals – NOT ions • Binary compounds can have 2 elements composed in various ways – ex: CO and CO2 or NO and N2O so we can’t name them like we did with ionic compounds • We need prefixes…prefixes tell us how many atoms of each element are present in each molecule

  15. Naming and Writing Formulas for Molecular Compounds • Here are a few hints: • If there is only 1 atom of the first element, omit the prefix mono- • You will usually add the –ide ending to the second element • Ex: CO • Carbon monoxide • Ex: N2O • Dinitrogen monoxide • Ex: Cl2O7 • Dichlorineheptoxide • Ex: BCl3 • Boron trichloride

  16. Naming and Writing Formulas for Molecular Compounds • Use the prefixes of each element to write the formula (hint: -mono is left out of the first element if there is only 1 atom) • Ex: carbon monoxide • CO • Ex: carbon tetrabromide • CBr4 • Ex: diphosphorus trioxide • P2O3 • Ex: iodine heptafluoride • IF7

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