Naming Compounds worksheet for chemistry practice, featuring exercises on naming from formulas and writing formulas from names.
A worksheet titled "Naming Compounds" with two sections: Part I asks to write names from chemical formulas, and Part II asks to write formulas from compound names.
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Step-by-step solution for: Naming Compounds Worksheet. - ppt download
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Show Answer Key & Explanations
Step-by-step solution for: Naming Compounds Worksheet. - ppt download
To solve this worksheet, we need to apply the rules of chemical nomenclature. This involves identifying the type of compound (ionic, covalent, or acid) and then naming it or writing its formula based on the charges of the ions or the prefixes used.
Part I: Names From Formulas
1. AgF₂: Silver is a metal that typically forms a +1 ion (Ag⁺). Fluorine is a halogen that forms a -1 ion (F⁻). To balance the charges in AgF₂, silver must have a +2 charge here? Wait, silver is almost always +1. Let's re-evaluate. Actually, Silver (Ag) is a transition metal but it is one of the exceptions that usually only forms +1. However, in AgF₂, if F is -1, then Ag must be +2. While rare, Silver(II) fluoride exists. But in standard high school chemistry, students often memorize Ag as +1. If Ag is +1, the formula would be AgF. Since the formula is AgF₂, the silver must be in the +2 oxidation state. So, Silver(II) fluoride.
*Self-Correction*: Actually, looking at standard curriculum, sometimes worksheets have trick questions or specific contexts. However, the most standard answer for AgF₂ is Silver(II) fluoride. Let's look at the other options. Maybe it's just a typo in the worksheet and they meant AgF? Or maybe they are treating Ag as a variable charge metal here. Let's assume standard rules: Ag is usually +1, but if the formula dictates +2, we name it Silver(II) fluoride.
*Alternative thought*: Is it possible the student is expected to know Ag is always +1 and this is a "trick" or error? No, let's stick to the strict rules. Charge of F is -1. Two F's = -2. So Ag must be +2. Name: Silver(II) fluoride.
2. AlBr₃: Aluminum (Al) is in Group 13 and forms a +3 ion (Al³⁺). Bromine (Br) is in Group 17 and forms a -1 ion (Br⁻). This is an ionic compound. Since Aluminum has a fixed charge, we don't need Roman numerals.
Name: Aluminum bromide.
3. AuI₃: Gold (Au) is a transition metal. Iodine (I) is a halogen with a -1 charge. Three Iodines = -3 total charge. Therefore, Gold must be +3. We need to use the Roman numeral (III).
Name: Gold(III) iodide.
4. FeO: Iron (Fe) is a transition metal. Oxygen (O) has a -2 charge. To balance the -2 from oxygen, Iron must be +2. We use the Roman numeral (II).
Name: Iron(II) oxide.
5. BaI₂: Barium (Ba) is an alkaline earth metal (Group 2) and forms a +2 ion. Iodine (I) forms a -1 ion. This is ionic. Barium has a fixed charge.
Name: Barium iodide.
6. BeO: Beryllium (Be) is in Group 2 and forms a +2 ion. Oxygen (O) forms a -2 ion. Charges balance (+2 and -2).
Name: Beryllium oxide.
7. Br₂O₅: This is composed of two non-metals (Bromine and Oxygen). This is a covalent compound. We use prefixes to indicate the number of atoms.
- 2 Bromines = "Di-"
- 5 Oxygens = "Penta-"
Name: Dibromine pentoxide.
8. ClF: Two non-metals (Chlorine and Fluorine). Covalent.
- 1 Chlorine = "Mono-" (usually omitted for the first element)
- 1 Fluorine = "Mono-"
Name: Chlorine monofluoride.
9. H₃PO₄: This starts with H, so it's an acid. It contains the polyatomic ion Phosphate (PO₄³⁻). Acids with "-ate" ions become "-ic" acids.
Name: Phosphoric acid.
10. Cu(NO₃)₂: Copper (Cu) is a transition metal. Nitrate (NO₃) is a polyatomic ion with a -1 charge. There are two nitrates, so total negative charge is -2. Copper must be +2.
Name: Copper(II) nitrate.
Part II: Formulas From Names
11. Aluminum oxide: Aluminum is Al³⁺. Oxide is O²⁻. To balance charges, we need 2 Al (+6) and 3 O (-6).
Formula: Al₂O₃.
12. Aluminum nitride: Aluminum is Al³⁺. Nitride is N³⁻. Charges are +3 and -3, so they balance 1:1.
Formula: AlN.
13. Gold (III) oxide: Gold (III) means Au³⁺. Oxide is O²⁻. To balance, we need 2 Au (+6) and 3 O (-6).
Formula: Au₂O₃.
14. Barium carbonate: Barium is Ba²⁺. Carbonate is CO₃²⁻. Charges are +2 and -2, so they balance 1:1.
Formula: BaCO₃.
15. Beryllium acetate: Beryllium is Be²⁺. Acetate is C₂H₃O₂⁻ (or CH₃COO⁻). We need two acetates to balance the +2 charge of Beryllium.
Formula: Be(C₂H₃O₂)₂ (or Be(CH₃COO)₂).
16. Dicarbon tetrafluoride: "Di-" means 2 Carbons. "Tetra-" means 4 Fluorines.
Formula: C₂F₄.
17. Carbonic acid: This is an acid derived from the carbonate ion (CO₃²⁻). Acids with "-ate" become "-ic". The formula for carbonate is CO₃. To make it an acid, we add H⁺. We need 2 H⁺ to balance the -2 charge of carbonate.
Formula: H₂CO₃.
18. Hypochlorous acid: This is an acid derived from the hypochlorite ion (ClO⁻). Acids with "-ite" become "-ous". We need one H⁺ to balance the -1 charge of hypochlorite.
Formula: HClO.
19. Calcium hydride: Calcium is Ca²⁺. Hydride is H⁻. We need two hydrides to balance the +2 charge of Calcium.
Formula: CaH₂.
20. Carbon dioxide: "Di-" means 2 Oxygens.
Formula: CO₂.
Final Answer:
Part I. Names From Formulas
1. Silver(II) fluoride
2. Aluminum bromide
3. Gold(III) iodide
4. Iron(II) oxide
5. Barium iodide
6. Beryllium oxide
7. Dibromine pentoxide
8. Chlorine monofluoride
9. Phosphoric acid
10. Copper(II) nitrate
Part II. Formulas From Names
11. Al₂O₃
12. AlN
13. Au₂O₃
14. BaCO₃
15. Be(C₂H₃O₂)₂
16. C₂F₄
17. H₂CO₃
18. HClO
19. CaH₂
20. CO₂
Part I: Names From Formulas
1. AgF₂: Silver is a metal that typically forms a +1 ion (Ag⁺). Fluorine is a halogen that forms a -1 ion (F⁻). To balance the charges in AgF₂, silver must have a +2 charge here? Wait, silver is almost always +1. Let's re-evaluate. Actually, Silver (Ag) is a transition metal but it is one of the exceptions that usually only forms +1. However, in AgF₂, if F is -1, then Ag must be +2. While rare, Silver(II) fluoride exists. But in standard high school chemistry, students often memorize Ag as +1. If Ag is +1, the formula would be AgF. Since the formula is AgF₂, the silver must be in the +2 oxidation state. So, Silver(II) fluoride.
*Self-Correction*: Actually, looking at standard curriculum, sometimes worksheets have trick questions or specific contexts. However, the most standard answer for AgF₂ is Silver(II) fluoride. Let's look at the other options. Maybe it's just a typo in the worksheet and they meant AgF? Or maybe they are treating Ag as a variable charge metal here. Let's assume standard rules: Ag is usually +1, but if the formula dictates +2, we name it Silver(II) fluoride.
*Alternative thought*: Is it possible the student is expected to know Ag is always +1 and this is a "trick" or error? No, let's stick to the strict rules. Charge of F is -1. Two F's = -2. So Ag must be +2. Name: Silver(II) fluoride.
2. AlBr₃: Aluminum (Al) is in Group 13 and forms a +3 ion (Al³⁺). Bromine (Br) is in Group 17 and forms a -1 ion (Br⁻). This is an ionic compound. Since Aluminum has a fixed charge, we don't need Roman numerals.
Name: Aluminum bromide.
3. AuI₃: Gold (Au) is a transition metal. Iodine (I) is a halogen with a -1 charge. Three Iodines = -3 total charge. Therefore, Gold must be +3. We need to use the Roman numeral (III).
Name: Gold(III) iodide.
4. FeO: Iron (Fe) is a transition metal. Oxygen (O) has a -2 charge. To balance the -2 from oxygen, Iron must be +2. We use the Roman numeral (II).
Name: Iron(II) oxide.
5. BaI₂: Barium (Ba) is an alkaline earth metal (Group 2) and forms a +2 ion. Iodine (I) forms a -1 ion. This is ionic. Barium has a fixed charge.
Name: Barium iodide.
6. BeO: Beryllium (Be) is in Group 2 and forms a +2 ion. Oxygen (O) forms a -2 ion. Charges balance (+2 and -2).
Name: Beryllium oxide.
7. Br₂O₅: This is composed of two non-metals (Bromine and Oxygen). This is a covalent compound. We use prefixes to indicate the number of atoms.
- 2 Bromines = "Di-"
- 5 Oxygens = "Penta-"
Name: Dibromine pentoxide.
8. ClF: Two non-metals (Chlorine and Fluorine). Covalent.
- 1 Chlorine = "Mono-" (usually omitted for the first element)
- 1 Fluorine = "Mono-"
Name: Chlorine monofluoride.
9. H₃PO₄: This starts with H, so it's an acid. It contains the polyatomic ion Phosphate (PO₄³⁻). Acids with "-ate" ions become "-ic" acids.
Name: Phosphoric acid.
10. Cu(NO₃)₂: Copper (Cu) is a transition metal. Nitrate (NO₃) is a polyatomic ion with a -1 charge. There are two nitrates, so total negative charge is -2. Copper must be +2.
Name: Copper(II) nitrate.
Part II: Formulas From Names
11. Aluminum oxide: Aluminum is Al³⁺. Oxide is O²⁻. To balance charges, we need 2 Al (+6) and 3 O (-6).
Formula: Al₂O₃.
12. Aluminum nitride: Aluminum is Al³⁺. Nitride is N³⁻. Charges are +3 and -3, so they balance 1:1.
Formula: AlN.
13. Gold (III) oxide: Gold (III) means Au³⁺. Oxide is O²⁻. To balance, we need 2 Au (+6) and 3 O (-6).
Formula: Au₂O₃.
14. Barium carbonate: Barium is Ba²⁺. Carbonate is CO₃²⁻. Charges are +2 and -2, so they balance 1:1.
Formula: BaCO₃.
15. Beryllium acetate: Beryllium is Be²⁺. Acetate is C₂H₃O₂⁻ (or CH₃COO⁻). We need two acetates to balance the +2 charge of Beryllium.
Formula: Be(C₂H₃O₂)₂ (or Be(CH₃COO)₂).
16. Dicarbon tetrafluoride: "Di-" means 2 Carbons. "Tetra-" means 4 Fluorines.
Formula: C₂F₄.
17. Carbonic acid: This is an acid derived from the carbonate ion (CO₃²⁻). Acids with "-ate" become "-ic". The formula for carbonate is CO₃. To make it an acid, we add H⁺. We need 2 H⁺ to balance the -2 charge of carbonate.
Formula: H₂CO₃.
18. Hypochlorous acid: This is an acid derived from the hypochlorite ion (ClO⁻). Acids with "-ite" become "-ous". We need one H⁺ to balance the -1 charge of hypochlorite.
Formula: HClO.
19. Calcium hydride: Calcium is Ca²⁺. Hydride is H⁻. We need two hydrides to balance the +2 charge of Calcium.
Formula: CaH₂.
20. Carbon dioxide: "Di-" means 2 Oxygens.
Formula: CO₂.
Final Answer:
Part I. Names From Formulas
1. Silver(II) fluoride
2. Aluminum bromide
3. Gold(III) iodide
4. Iron(II) oxide
5. Barium iodide
6. Beryllium oxide
7. Dibromine pentoxide
8. Chlorine monofluoride
9. Phosphoric acid
10. Copper(II) nitrate
Part II. Formulas From Names
11. Al₂O₃
12. AlN
13. Au₂O₃
14. BaCO₃
15. Be(C₂H₃O₂)₂
16. C₂F₄
17. H₂CO₃
18. HClO
19. CaH₂
20. CO₂
Parent Tip: Review the logic above to help your child master the concept of chemistry worksheet on naming and writing compounds.
