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UNIT IV Naming Inorganic Compounds Lesson 1 Slide 2 INORGANIC NOMENCLATURE Nomenclature refers to naming In organic = Non Carbon compounds & Elements. Organic chemistry= study of carbon compounds. The periodic table organizes the elements by vertical columns (___________) and horizontal rows (______________). The elements are arranged depending on the chemical and physical properties of elements in repeated patterns and increasing atomic masses. Slide 3 IV.1 THE CHEMICAL ELEMENTS Element symbol: The first letter is always in upper case and the second letter (if present) is always lower case. Ex: Sodium (Na), Nitrogen (N) 3 Major classifications: pg. 67 Non-MetalsMetalsMetalloids or Semi Metals Clustered elements around the staircase between metals and non-metals. Slide 4 P ERIODIC TABLE http://www.colgurchemistry.com/2008PeriodicTable.pdf Slide 5 IV.2 NAMING INORGANIC COMPOUNDS METALS: Found on left side in periodic table Form _________ ions Cation: an ion with a positive charge NON-METALS : Found on right side in periodic table form __________ ions (H is generally an exception) Anion: an ion with a negative charge Slide 6 N AMING INORGANIC COMPOUNDS Some other definitions Monoatomic Diatomic Triatomic Polyatomic Slide 7 NAMING MONATOMIC METAL IONS Simply use the name of the metal and add the word ion Element Name Ion Name Sodium Metal(Na) Aluminum (Al) Write the names of the following ions: Ca +2 Ag + Slide 8 NAMING MONATOMIC METAL IONS If a metal has more than one possible charge, the charge has to be indicated by a Roman numeral, in parenthesis, immediately following the name. Ex: Fe +3 Fe +2 Roman numerals are: I 1 V 5 IX 9 II 2 VI 6 X 10 III 3 VII 7 IV 4 VIII 8 Slide 9 NAMING MONATOMIC METAL IONS Write the formula of the following ions to show their charges: Uranium (VI) ion = __________ Iron (II) ion = __________ Nickel (II) ion = __________ Slide 10 NAMING MONATOMIC NON-METAL IONS Take off the original ending and add an ide ending. Element Name Ion Name Florine (F) Sulphur (S) Write the names of the following ions: a) Br - = __________________________ b) Cl - = __________________________ c) I - = __________________________ d) O -2 = __________________________ e) N -3 = __________________________ Slide 11 Naming Polyatomic Ions: Rules for naming are more complicated (we wont learn them). But we will need to KNOW some common polyatomic ions (names, formula, charge). * Know table on page 69. Slide 12 How to write the formula and how to write the name of Ionic Compounds Slide 13 H OW TO WRITE THE FORMULA OF IONIC COMPOUNDS An ionic compound A compound made up of ions ( usually a metal + non-metal ) The ions have charges but the compound is a neutral molecule. remember in ionic compounds, one ion loses and one ion gains electrons). The chemical name of an ionic compound always gives the positive ion (cation) first and the negative ion (anion) second. Ex: Sodium Chloride Slide 14 3 SIMPLE RULES Slide 15 C ALCIUM C HLORIDE & M AGNESIUM O XIDE Slide 16 W RITING FORMULA OF I ONIC COMPOUNDS Slide 17 M ORE EXAMPLES Potassium oxide: Tin (IV) oxide: Calcium phosphide Iron (II) sulphate: We do not change the endings of polyatomic ions because they already have special endings that end in ate or ite Slide 18 How to Write the Name of an IONIC COMPOUND Check your periodic table to see if the positive ion has more than one ion charge. Slide 19 How to Write the Name of an IONIC COMPOUND A) If the first ion has only one possible ion charge: write the names of the ions (not elements) one after the other omit the word ion ZnCl 2 Ag 2 SO 4 Slide 20 B) If the first ion has more than one possible charge: Slide 21 De-swap and de-drop the subscripts (to find out the real charge) check the charge on negative ion (if it is not as what it should be, you probably need to double or triple it) write the charge of the positive ion with roman numerals Write the charge of the negative ion with ide Slide 22 T RY THESE ON YOUR OWN FeS Fe 2 (SO 4 ) 3 Slide 23 Note: you must memorize the common name of 2 compounds: H 2 O = water NH 3 = ammonia be careful of Ammonium NH 4 +1 Slide 24 Naming Hydrates Hydrates are ionic compounds that include water molecules in their crystal structures. Naming hydrates is pretty straightforward and relies on using prefixes to tell how many water molecules are attached. The # of water molecules is shown after a centered dot Example of a hydrate: CuSO 4 5H 2 O see table on page 72 for prefixes Slide 25 Naming Hydrates see table of page 72 for prefixes CuSO 4.5H 2 O= copper (II) sulphate pentahydrate Ca(NO 3 ) 2 4H 2 O= Slide 26 P RACTICE T IME ! Self-test on page66 All of it Ex#1 on page 68 Ex#4 on page 71 Ex# 5 on page 72 Page 73 Ex#6: a, c, d, f, g, I Page 73 Ex#7: a, b, c, d, e, f Slide 27 UNIT IV: LESSON 2 How to write the formula and how to write the name of Covalent Compounds Slide 28 Naming COVALENT COMPOUNDS Using the Prefix-Naming System Remember covalent compounds SHARE their electrons ( usually two non-metals together). Binary Compound : a compound made of two different types of atoms (usually two non-metals) SO 2, Na 2 S, NaCl Tertiary Compound : a compound made of three different types of atoms. H 2 SO 4 KOH KMnO 4 Slide 29 Naming COVALENT COMPOUNDS Using the Prefix-Naming System We use the prefix-naming system 1- Each compound name is made of words, each with a suitable prefix see p. 73 Slide 30 Naming COVALENT COMPOUNDS Using the Prefix-Naming System Prefix-system naming continued First word is the name of element(not ion) with a prefix to indicate the # of atoms Second word is the name of the element with an ide ending and a prefix to indicate the # of atoms P 2 S 3 = di phosphorus tri sulphide Exception: if there is only ONE atom of the first element, dont use the prefix mono. Ex: CO 2 = Slide 31 T RY ON YOUR OWN Examples: P 2 S 3 = CO = BrCl 3 = S 2 Cl 2 = Slide 32 PREFIX NAMING SYSTEM Basically used when you have two different Non- Metals. Non-metals are usually found on the right side of the periodic table. Remember the prefixes. Slide 33 W RITING FORMULAS FOR COVALENT COMPOUNDS Steps: Write down the symbol for each element Use the prefix to determine the number of atoms of each element. Example: dinitrogen tetroxide carbon dioxide Do NOT reduce ! Slide 34 Some Common Acids A compound is called an acid when the chemical formula starts with H ex: HCl, H 2 SO 4 see common acids on p. 74 KNOW THESE Slide 35 S UMMARY Naming First identify if it is ionic or covalent Ionic compounds Metal and non-metal Positive ion first then negative ion Use roman numerals to indicate the ions with more than one possible charge For the negative ions(non-metals) change the ending to ide. Covalent compounds Non-metal and non-metal For both, we use the prefix-naming system (mono, di, tri, tetra, etc) First one, you just write the elements original name with prefix You change the second elements name to ide with prefix. Slide 36 S UMMARY Writing Formulas First identify if it is ionic or covalent Ionic compounds Write formula for positive ion first then negative ion Swap and drop charges as subscripts Reduce if you need to. Covalent compounds Write down the symbol for each element Use the prefix to determine the number of atoms of each element. Do NOT reduce ! Slide 37 P RACTICE TIME ! Page 74 Ex8 and Ex9. Page 75 writing the names question ( only odd numbers ) 15 89 ( only odds) Page 76 writing the formulas question ( only even numbers) 90 162 (only evens) Slide 38