Nomenclature Test Study Guide PDF

The Nomenclature Test Next Class Tuesday November 17th- Here is a Study Guide you may use to help you prepare for the assessment. Terms to know: - Ions ( Cation/Anion) - Monatomic Ion - Polyatomic Ion - Ionic Compound Covalent Compound ( Molecular Compound) What is an Ionic Compound? W...

The Nomenclature Test Next Class Tuesday November 17th- Here is a Study Guide you may use to help you prepare for the assessment. Terms to know: - Ions ( Cation/Anion) - Monatomic Ion - Polyatomic Ion - Ionic Compound Covalent Compound ( Molecular Compound) What is an Ionic Compound? What are the electrons doing? What kind of elements usually make up these compounds? What is a Covalent ( Molecular) Compound? What are the electrons doing? What kind of elements usually make up these compounds? Be able to do the following for the test on Tuesday: 1. Write the name of a neutral element. 2. Determine the chemical formula for a neutral element. 3. Write the chemical formula of a compound using the name. 4. Write the name of a compound using the chemical formula. 5. Write the name for monatomic and polyatomic ions. 6. Determine the chemical formula using the name of monatomic and polyatomic ions. 7. Predict the charge of an Ion based on its location on the Periodic Table ( PTE) 8. Predict the ratio needed between a cation and anion. Quick Study Guide: Naming and Writing Chemical Formulas for Ionic and Covalent Compounds I. Basics of Chemical Compounds 1. Ionic Compounds - Formed between metals (cations) and non-metals (anions). - Transfer of electrons results in positive and negative ions. 2. Covalent Compounds - Formed between non-metals. - Electrons are shared between atoms. II. Naming Ionic Compounds 1. Binary Ionic Compounds (Two Elements): - Name the cation (metal) first. - Name the anion (non-metal) second and change its ending to "-ide". - Example: NaCl = Sodium chloride 2. Transition Metals with Variable Charges: - Use Roman numerals to indicate the metal’s charge. - Example: FeCl₃ = Iron(III) chloride 3. Compounds with Polyatomic Ions: - Name the cation first, then the polyatomic ion (do not change its name). - Example: NaNO₃ = Sodium nitrate III. Writing Formulas for Ionic Compounds 1. Determine the Charges: - Use the periodic table or polyatomic ion chart. 2. Balance the Charges: - Adjust the ratio of cations to anions so that the total charge equals zero. - Example: Mg²⁺ and Cl⁻ form MgCl₂ 3. Write the Formula: - Cation first, anion second. IV. Naming Covalent Compounds 1. Use Prefixes for Subscripts: - Mono- (1), Di- (2), Tri- (3), Tetra- (4), Penta- (5), etc. - The prefix “mono-” is not used for the first element if there is only one atom. 2. Naming Order: - The less electronegative element is named first. - The second element’s name ends in "-ide". - Example: CO = Carbon monoxide 3. Common Prefix Examples: - CO₂ = Carbon dioxide - N₂O₄ = Dinitrogen tetroxide V. Writing Formulas for Covalent Compounds 1. Use the Prefixes: - Convert prefixes directly into subscripts for each element. - Example: Diphosphorus pentoxide = P₂O₅ 2. Do Not Balance Charges: - Covalent compounds do not involve ions, so charges are not balanced. VI. Key Tips 1. Memorize Common Polyatomic Ions ( The list will NOT be provided on the Test) - Example: NO₃⁻ (nitrate), SO₄²⁻ (sulfate), NH₄⁺ (ammonium). 2. Check the Periodic Table: - Group numbers can help predict charges for ions. 3. Practice! - Work through examples to solidify your understanding. Some Extra Practice Problems 1. Name the following ionic compounds: - KBr - Ca(NO₃)₂ - Fe₂O₃ 2. Write the formula for these ionic compounds: - Aluminum sulfate - Copper(I) oxide 3. Name the following covalent compounds: - PCl₃ - SF₆ 4. Write the formula for these covalent compounds: - Carbon tetrachloride - Dinitrogen pentoxide