Cations have a positive charge and anions have a negative charge. 3. Complete the following table.
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1 Name Pre-AP Chemistry: Ionic Bonding and Nomenclature Period Homework #1: Ionic Bonding 1. Use Lewis Dot Diagrams to predict the ionic compound formed between each of the following atoms. Use arrows to show the electrons being transferred. Write the resulting chemical formula and name the compounds formed. a. Li and Cl d. Na and O LiCl; Lithium Chloride Na 2 O, Sodium Oxide b. Ca and Cl e. Ba and S Sulfide c. Al and Cl f. Ca and P 2. What type of charge does a cation have? What type of charge does an anion have? Cations have a positive charge and anions have a negative charge. 3. Complete the following table. Formula Lewis Structure (or Structural Formula) Name of Shape Molecular Polarity Intermolecular Forces of Attraction Present NI 3 Polar H 2 O Polar HF Polar CH 3 Cl Nonpolar CO 2 nonpolar BH 3 Planar Nonpolar
2 Name Pre-AP Chemistry: Ionic Bonding and Nomenclature Period Homework #2: Naming and Writing Formulas for Ionic Compounds 1. Complete the following table. Ion Name of Ion No. of e - lost or gained a. Pb 2+ loses 2e - b. O 2- c. Sodium Ion loses 1e - d. Fluoride Ion e. SO 4 2- gains 2e - f. Potassium Ion g. Barium Ion h. N 3- i. Iron(III) Ion 2. When is it necessary to use a Roman numeral when naming a compound? What does the Roman numeral indicate? A Roma n numeral must be used when the cation has more than one common oxidation number. The Roman numeral indicates 3. Chromium atoms can take a charge of 2+, 3+ or 6+. Write the names and formulas for all of the possible oxides of chromium. CrO Chromium(II) oxide Cr 2 O 3 Chromium(III) oxide CrO 3 Chromium(VI) oxide 4. Copper forms two different compounds with chlorine, CuCl and CuCl 2. In writing their names, how do we distinguish them? We use a Roman numeral. CuCl is copper(i) chloride. CuCl 2 is copper(ii)
3 5. Write the formula and name the compound formed from each of the following pairs of ions. a. Na +, S 2- b. Sn 4+, S 2- c. Mg 2+, P 3- d. Li +, Cl - e. K +, Cl - f. Sr 2+, Cl - g. Mg 2+, Br - h. Al 3+, F - i. Fe 3+, O 2- j. Mn 4+, O 2- k. Ca 2+, F - l. Be 2+, S 2- m. Al 3+, O 2- n. Ca 2+, O 2- o. Cu +1, O 2- p. Pb 2+, Cl - q. Li +, N 3- r. Ca 2+, I - s. Sr 2+, N 3- t. Ca 2+, P 3-6. Why is it necessary to use parentheses in writing the formula for calcium nitrate? The parentheses indicate that two nitrate polyatomic ions are needed to Balance out the char ge of one calcium ion. 7. What is the difference between (OH) 2 and OH 2 in a chemical formula? there are two hydroxide groups. The
4 8. Write the formula for the following compounds. a. tin(iv) chloride b. calcium sulfide c. nickel(ii) bromide d. lithium fluoride e. copper(i) nitride f. iron(ii) oxide g. sodium bromide h. sodium chloride i. tin(ii) bromide j. mercury(ii) nitride k. manganese(ii) oxide l. tin(iv) oxide m. potassium bromide n. lithium iodide o. magnesium chloride p. calcium bromide q. potassium sulfide 9. Write the formula and name the compound formed from each of the following pairs of ions. a. Na + 2-, SO 4 b. Sn 4+ 2-, CO 3 c. Mg 2+ 3-, PO 4 d. Li + -, ClO 3 e. NH + 4, Cl - f. Ba 2+ -, HCO 3 g. Ca 2+, ClO - h. NH + 2-4, SO 4 i. Al 3+ -, NO 3
5 10. Write the formula for the following compounds. a. potassium sulfate b. sodium nitrate c. copper(i) sulfate d. magnesium phosphate e. sodium hydrogen sulfate f. strontium hydrogen carbonate g. ammonium phosphate h. lead(ii) hydrogen carbonate i. ammonium dichromate j. sodium cyanide 11. An ionic compound made up of elements X and Y has the formula X 3 Y 2. What does this tell you about the probable charges of X and Y? The probable charge of X is +2. The probable charge of Y is In each of the following examples, assume that an element, X, forms an ionic compound of the formula shown. What is the charge on the X ion in each compound? a. XBr d. X 2 CO 3 b. XSO 3 e. (NH 4 ) 2 X c. Mg 3 X 2 f. X 3 (PO 4 ) 2
6 Name Pre-AP Chemistry: Ionic Bonding and Nomenclature Period Homework #5: Naming and Writing Formulas for Acids and Bases 1. Write names for each of the following acids and bases. a. HBr b. HNO 2 c. KOH d. Ca(OH) 2 e. H 2 SO 3 f. NH 3 g. H 3 PO 4 h. H 2 CO 3 i. HCl j. Sn(OH) 2 k. H 2 SO 4 l. HIO 3 m. Fe(OH) 3 2. Write the formulas for each of the following acids and bases. a. Barium hydroxide b. Magnesium hydroxide c. Phosphorous acid d. Hydroiodic acid e. Nitric acid f. Hydrosulfuric acid g. Hypochlorous acid h. Sodium hydroxide i. Perchloric acid j. Acetic acid k. Carbonous acid l. Bromous acid m. Periodic acid
7 3. Write formulas for each of the following compounds. a. lithium cyanide b. sodium hypochlorite c. bromic acid d. boron trichloride e. chromium(iii) chloride f. sulfur trioxide g. calcium bicarbonate h. barium bromide i. hydroiodic acid j. nitrous acid k. strontium nitrate l. potassium cyanide m. cobalt(ii) carbonate n. sodium sulfite o. mercury(ii) nitrite p. dichlorine monoxide 4. Determine if each of the following name/formula combinations is correct or not. If a combination is correct write C in the blank at the right. If it is not correct, write the correct name or formula in the blank at the right. a. Barium carbonate BaCO 3 b. Chromium(II) nitride CrN 2 c. Hydrosulfuric acid H 2 SO 4 d. Sodium hydride NaOH e. Silicon tetrachloride SiCl 4 f. Periodic acid HIO 4 g. Copper chloride CuCl 2 h. Calcium(II) phosphate Ca 3 (PO 4 ) 2 i. Dinitrogen trioxide N 3 O 2
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