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Ch.5 (Types of compound ) Section 1( Ionic Compound)

Ch.5 (Types of compound ) Section 1( Ionic Compound). Gr.10 / Chemistry/LC3 Nagham Hussam Chemistry Teacher. Ionic compounds. Ionic compounds are:

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Ch.5 (Types of compound ) Section 1( Ionic Compound)

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  1. Ch.5 (Types of compound )Section 1(Ionic Compound) Gr.10 /Chemistry/LC3 Nagham Hussam Chemistry Teacher

  2. Ionic compounds • Ionic compounds are: 1. Made up of oppositely charged ions held together strongly in well-organized units. 2. Hard solids at room temperature and are difficult to melt. Look at the structure of magnesium oxide.

  3. The smallest part of compounds • Molecule: the smallest unit of the compound in a covalent compound. • Formula unit The simplest ratio of ions in a compound.

  4. Binary Ionic Compounds You will learn how to name and write formulas for ionic compounds. • Binary compound: a compound that contains only two elements. • Ex: Sodium chloride (NaCl), potassium iodide (KI) and (CaF2) calcium florid (contain more than one ion of each element)

  5. Predicting Charge on Ions • Metals have few outer-level electrons so they tend to lose them and become positive ions. • Sodium must lose just one electron, becoming a Na+ ion. • Calcium must lose two electrons, becoming a Ca2+ ion. • The charge on the ion is known as the oxidation number of the atom. • The oxidation numbers for many elements in the main groups are arranged by group number.

  6. Predicting Charge on Ions • Oxidation numbers for elements in Groups 3 through 12, the transition elements, cannot be predicted by group number. • Aluminum is in Group 13, so it loses its three outer electrons to become an Al3+ ion; oxygen is in Group 16 and has six valence electrons, so it gains two electrons to become an O2– ion.

  7. How to name a binary ionic compound • To name a binary ionic compound, first write the name of the positively charged ion, usually a metal, and then add the name of the nonmetal or negatively charged ion, whose name has been modified to end in -ide. • Magnesium combines with oxygen to form a compound called magnesium oxide (MgO).

  8. How to write the formula • Sodium chloride contains sodium ions that have a 1+ charge and chloride ions that have a 1– charge. • the sum of the charges in an ionic compound must always equal zero.

  9. Learning Check Write the correct formula for the compounds containing the following ions: A. Na+, S2- 1) NaS 2) Na2S 3) NaS2 B. Al3+, Cl- 1) AlCl3 2) AlCl 3) Al3Cl C. Mg2+, N3- 1) MgN 2) Mg2N3 3) Mg3N2

  10. Solution A. Na+, S2- 2) Na2S B. Al3+, Cl- 1) AlCl3 C. Mg2+, N3- 3) Mg3N2

  11. Naming Binary Ionic Compounds • Contain 2 different elements • Name the metal first, then the nonmetal as -ide. Examples: NaCl sodium chloride ZnI2 zinc iodide Al2O3 aluminum oxide

  12. Learning Check Complete the names of the following binary compounds: Na3N sodium ________________ KBr potassium ________________ Al2O3 aluminum ________________ MgS _________________________

  13. Solution Complete the names of the following binary compounds: Na3N sodium nitride KBr potassium bromide Al2O3 aluminum oxide MgS magnesium sulfide

  14. Learning Check A. The formula for the ionic compound of Na+ and O2- is 1) NaO 2) Na2O 3) NaO2 B. The formula of a compound of aluminum and chlorine is 1) Al3Cl 2) AlCl2 3) AlCl3 C. The formula of Fe3+ and O2- is 1) Fe3O2 2) FeO3 3) Fe2O3

  15. Solution A. The formula for the ionic compound of Na+ and O2- is 2) Na2O B. The formula of a compound of aluminum and chlorine is 3) AlCl3 C. The formula of Fe3+ and O2- is 3) Fe2O3

  16. Transition Metals Many form 2 or more positive ions 1+ 2+ 1+ or 2+ 2+ or 3+ Ag+ Cd2+ Cu+,Cu2+ Fe2+, Fe3+ silver cadmium copper(I) ion iron(II) ion ion copper (II) ion iron(III) ion Zn2+ zinc ion

  17. Names of Variable Ions Use a roman number after the name of a metal that forms two or more ions Transition metals and the metals in groups 4A and 5A FeCl3(Fe3+) iron (III) chloride CuCl (Cu+ ) copper (I) chloride SnF4 (Sn4+) tin (IV) fluoride PbCl2 (Pb2+) lead (II) chloride Fe2S3 (Fe3+) iron (III) sulfide

  18. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron (_____) bromide Cu2O copper (_____) oxide SnCl4 ___(_____ ) ______________ Fe2O3 ________________________ CuS ________________________

  19. Solution Complete the names of the following binary compounds with variable metal ions: FeBr2 iron ( II ) bromide Cu2O copper ( I ) oxide SnCl4tin (IV) chloride Fe2O3iron (III) oxide CuS copper (II) sulfide

  20. Learning Check Name the following compounds: A. CaO 1) calcium oxide 2) calcium(I) oxide 3) calcium (II) oxide B. SnCl4 1) tin tetrachloride 2) tin(II) chloride 3) tin(IV) chloride C. Co2O3 1) cobalt oxide 2) cobalt (III) oxide 3) cobalt trioxide

  21. Solution Name the following compounds: A. CaO 1) calcium oxide B. SnCl43) tin(IV) chloride C. Co2O32) cobalt (III) oxide

  22. Compounds Containing Polyatomic Ions • Polyatomic ion: An ion that has two or more different elements.

  23. Compounds Containing Polyatomic Ions

  24. Compounds Containing Polyatomic Ions Ionic compounds may contain: 1. positive metal ions bonded to negative polyatomic ions, such as in NaOH . 2. negative nonmetal ions bonded to positive polyatomic ions, such as in NH4I. 3. or positive polyatomic ions bonded to negative polyatomic ions, such as in NH4NO3.

  25. How to write formula of Compounds Containing Polyatomic Ions • Remember that the sumof the positive and negative charges must equal zero. • Write a subscript outside the parentheses to show the number of polyatomic ions in the compound. • The formula for the compound that contains one magnesium ion and two nitrate ions is Mg (NO3)2.

  26. How to name a compound containing a polyatomic ion • To name a compound containing a polyatomic ion, follow the same rules as used in naming binary compounds. • The name of the compound composed of calcium and the carbonate ion is calcium carbonate. • To form a neutral compound, one Ca2+ ion must combine with one CO32– ion to give the formula CaCO3.

  27. Hydrates • Hydrate:A compound in which there is a specific ratio of water to ionic compound. For example CaSO4 • 2H2O is calcium sulfate dihydrate. • Hygroscopic:compounds can easily become hydrates by absorbing water molecules from water vapor in the air. Example is Sodium Carbonate (Na2CO3).

  28. Hydrates • Deliquescent: Substances those are so hygroscopic that they take up enough water from the air to dissolve completely and form a liquid solution.

  29. Hydrates • The dot in the formula represents a ratioof compound formula units to water molecules. • For example, CaSO4 • 2H20 is the formula for a hydrate of calcium sulfate that contains two moleculesof water for each formula unit of calcium sulfate.

  30. How To name hydrates • To name hydrates, follow the regular name for the compound with the word hydrate, to which a prefix has been added to indicate the number of water molecules present. • The name of the compound with the formula CaSO4 • 2H2O is calcium sulfate dihydrate.

  31. Anhydrous compound • Heating hydrates can drive off the water. • This results in the formation of an anhydrous compound—one in which all of the water has been removed. • In some cases, an anhydrous compound may have different color from that of its hydrate. For example: CuSO4.5H2O is (blue) while anhydrousof CuSO4 is (white)

  32. Good luck

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