Forming Compounds - Homework Package SNC2D1 Grade 10 Academic Science

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1 Forming Compounds - Homework Package SNC2D1 Grade 10 Academic Science Name: Date: 1. The Formation of Ions complete the following table. Group Example & Bohr-Rutherford diagram # of valence electrons Lose or gain electrons? 1 Li 2 Be Ionic charge Conclusion: The atoms of the elements in each GROUP (i.e. column) share a common property they all have the same number of 2. What is the charge of each of the following common elements? Element Charge Element Charge Potassium +1 Calcium Sulphur Magnesium Mercury Bromine Phosphorus Barium Iodine Rubidium 13 (3) 14 (4) 15 (5) 16 (6) 17 (7) 18 (8) B C N O F He 3. Types of chemical bonds is it ionic or molecular? Put a checkmark ( ) in the appropriate column. Ionic Molecular Ionic Molecular CaCl 2 Silver bromide CaO Dinitrogen monoxide CuCl 2 Aluminum bromide CO Lead (II) oxide Cu 2O Sodium chloride SO 2 Carbon dioxide SnF 2 Copper (II) chloride MgCl 2 dihydrogen monoxide Li 2O Carbon monoxide Na 2O Zinc oxide PbI 2 Aluminum oxide CO 2 Copper (II) oxide FeCl 2 Calcium chloride NaCl Potassium chloride SO 3 Tin (II) chloride NaI Nitrogen dioxide KCl Sodium fluoride PbCl 2 Sulphur trioxide K 2O Lithium oxide N 2O 5 Zinc chloride

2 IONIC BONDING Ionic bonding occurs when a transfers one or more electrons to a in an effort to attain a stable of electrons. 1. Show the transfer of electrons using Bohr-Rutherford diagrams in the following combinations. K + F For example, the transfer of one electron from a sodium to chlorine atom can be depicted by the Bohr-Rutherford diagram below: Mg + I The attraction between the newly formed cation and anion is called the ionic bond. Be + S Example 2: Al and Cl Aluminum would need three chlorine atoms to get rid of its 3 valence electrons. The concept: The total positive charge and the total negative charge needs to equal ZERO in order to form a stable ionic compound. So Al 3+ is a stable cation, and Cl - is a stable anion. But there are more positive charges than negative charges if there is only one of each. So there needs to be a total of 3 negative charges to balance out the 3 positive charges that Al 3+ has. Therefore, three chlorine ions are needed for every aluminum ion present. Na + O Al + Br

3 Forming Ionic Compounds 2. Complete the following tables: Example 1: Lithium + Iodine Li + I - Li1 I1 LiI Lithium iodide Calcium + Bromine Aluminum + Chlorine Magnesium + Sulphur Potassium + Fluorine Beryllium + oxygen Calcium + nitrogen Magnesium + phosphorus Aluminum + oxygen

4 Elements with Multiple Ionic Charges 1. Complete the following tables. Example 1: Cation Anion Tin (II) iodide Sn 2+ I - Sn1 I2 SnI2 Cation Anion Copper (I) bromide Cation Anion Iron (III) chloride Cation Anion Tin(IV) fluoride Cation Anion Iron (II) oxide 2. Write the chemical names for the following compounds. a. CuCl 2 Copper (II) chloride b. FeBr 3 c. PbS d. SnO 2 e. FeP f. CuI g. PbI 2 h. FeCl 2 i. SnF 2 j. PbCl 2 k. Cu 2O 3. More practice! PART A: Write the chemical formula for the following compounds a. Copper (II) oxide b. Silver chloride c. Tin (II) chloride d. Cobalt (II) phosphide e. Sodium fluoride f. Lithium oxide g. Lead (II) oxide h. Iron (III) oxide i. Magnesium bromide j. Zinc oxide k. Chromium (II) bromide l. Nickel (III) oxide m. Lead (IV) oxide n. Aluminum nitride o. Lithium iodide p. Copper (II) chloride PART B: Write the chemical names for the following compounds a. NaCl b. MgCl 2 c. FeCl 3 d. FeO e. Mg 3N 2 f. Cu 3N g. SnS 2 h. AuCl 3 i. Fe 2O 3 j. Cu 3P 2 k. CuF 2 l. LiBr m. K 3P

5 Polyatomic Ions 1. Complete the following tables. Example 1: Cation Anion Sodium phosphate Na + (PO4) 3- Na3 (PO4)1 Na3PO4 Cation Anion Calcium sulphate Cation Anion Copper (I) carbonate Cation Anion Tin (II) hydroxide Cation Anion Sodium chlorate 2. Write the chemical names for the following compounds. a. KNO 3 (found in gun powder) Potassium nitrate b. Ca(OH) 2 (an ingredient in plaster) c. CaCO 3 (in chalk) d. CuSO 4 (a fungicide) e. KOH (used to make soap) f. Fe(NO 3) 3 (used in water treatment) g. Cu(ClO 3) 2 (used to colour fireworks) h. (NH 4) 3PO 4 (ingredient in bread dough) 3. Write the chemical formula for each of the following compounds. a. Potassium nitrate (used to colour fireworks purple) b. Barium sulphate (given prior to an X-ray of the intestine) c. Ammonium nitrate (common ingredient in fertilizer) d. Aluminum sulphate (used in preparing pickles) e. Potassium chlorate (an explosive) f. Copper (II) nitrate (used to colour ceramics) g. Lead (II) sulphate (found in car batteries) h. Tin (II) phosphate (used in the dyeing of silk) 4. More Practice! PART A: Write the chemical names for the following compounds. a. Li 2CO 3 b. Mg 3(PO 4) 2 c. K 2SO 4 d. NaNO 3 e. Al(OH) 3 f. Pb 3(PO 4) 2 g. Sn(ClO 3) 2 h. NaOH i. FeSO 4 j. K 3PO 4 PART B: Write the chemical formulas for the following compounds. a. Magnesium sulphate b. Copper (I) chlorate c. Sodium chlorate d. Magnesium hydroxide e. Aluminum nitrate f. Lead (II) nitrate g. Sodium bicarbonate h. Aluminum carbonate i. Copper (II) hydroxide j. Ammonium sulphate k. Iron (II) phosphate l. Cobalt (II) phosphate m. Beryllium sulphate n. Barium nitrate

6 Ionic Compounds Review Write the chemical formulas and chemical names of the compounds produced from the listed ion in the grid below. Cl - CO3 2- OH - SO4 2- PO4 3- NO3 - Na + Example: NaCl Sodium chloride NH4 + K + Ca 2+ Mg 2+ Zn 2+ Fe 2+ Al 3+ Co 3+ Fe 3+ H +

7 Molecular compounds - Covalent bonds Covalent bonding occurs when two more SHARE electrons, attempting to attain a stable octet of electrons at least part of the time. (Note: Hydrogen is stable with 2 electrons, not 8!) 1. Using Bohr-Rutherford diagrams, show how covalent bonding occurs in each of the following pairs of atoms. Atoms may share one, two, or three pairs of electrons (i.e. there can be a single bond, double bond, or triple bond between atoms). a. H + H (H 2) b. F + F (F 2) c. O + O (O 2) d. N + N (N 2) e. C + O (CO 2) f. H + O (H 2O) RULES for Naming molecular compounds using the PREFIX METHOD: Prefix 1* mono- or mon *MONO is only used with the 2 nd non-metal! 2. Write the chemical formula for the following molecular compounds. a. Carbon dioxide CO 2 b. Silicon dioxide c. Carbon disulfide d. Sulphur trioxide e. Carbon tetrachloride f. Diphosphorus trioxide g. Dinitrogen monoxide h. Arsenic tribromide i. Phosphorus pentrabromide j. Dinitrogen tetroxide k. Silicon monocarbide l. Sulphur dioxide m. Dinitrogen monoxide n. Sulphur difluoride 3. Write the chemical name for the following molecular compounds. a. CF 4 Carbon tetrafluoride b. PBr 3 c. CS 2 d. N 2O 2 e. H 2O 2 f. CO g. N 2O 3 h. SiC i. P 2O 5 j. SO 3 k. SiO 2 l. PCl 5 m. N 2O 5

8 4. Ionic or Covalent For each of the following compounds, place a checkmark ( ) under the appropriate column to state if it is IONIC or COVALENT and name the compound. Compound Ionic Covalent Chemical Name Example: BaS Barium sulphide a. Rb 3N b. N 2S 5 c. BeO d. HI e. SrCl 2 f. FeCl 3 g. P 2S 5 h. SCl 2 i. Ag(NO 3) j. As 2S 3 k. Cu(HCO 3) 2 l. SnO 2 m. K 3(PO 4) n. NaCl o. CCl 4 p. NO q. Na 2(SO 4) r. CaCl 2 s. CO 2 t. H 2O u. BaSO 4 v. K 2O w. NaF x. Na 2CO 3 y. NH 4Cl Naming & writing chemical formulas for ionic & molecular compounds. 5. Write the chemical formula for the following compounds. Lithium bromide Carbon monoxide Arsenic trifluoride Barium hydride Calcium phosphate Tin (IV) iodide Sodium sulfide Iodine monobromide Lead (II) carbonate Selenium tribromide Barium nitrate Ammonium sulfide Barium iodate Sodium hydroxide Ammonium sulfate Chromium (III) oxide Dihydrogen monosulfide Mercury (II) sulfate Cobalt (III) chloride Phosphorus pentachloride Copper (I) oxide Dinitrogen trisulfide Beryllium bromide Lead (IV) oxide Potassium chlorate Chromium (II) nitrate Calcium bicarbonate Manganese (II) fluoride Calcium hydroxide Tricarbon tetraphosphide Iron (III) carbonate Magnesium nitride 2. Write the correct name for each of the following compounds NF 3 Ag 3N K 2SO 4 CrCl 3 Na 3P Au 2O 3 Co(NO 3) 3 KOH Fe 2S 3 Co(ClO 3) 2 P 2S 5 Li(NO 3) Ca 3(PO 4) 2 Mg 3(PO 4) 2 CBr 4 Si 3N 2 SO 2 Fe(ClO 3) 2