Agenda Nov 28, Slip quiz 1. Naming Ionic Compounds Pogil - Part 2 corrections and overview. Notes - properties of ionic compounds
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1 Agenda Nov 28, 2016 Slip quiz 1 Naming Ionic Compounds Pogil - Part 2 corrections and overview Notes - properties of ionic compounds Notes - Covalent compounds - models
2 Slip Quiz: Name the following ionic compounds. Na 2 O CaF 2 Al 2 S 3 Li 3 N NaCl
3 Slip Quiz: Name the following ionic compounds. Na 2 O Sodium oxide CaF 2 Al 2 S 3 Li 3 N NaCl Calcium fluoride Aluminum sulfide Lithium nitride Sodium chloride
4 Naming Ionic Compounds Part 2 Model 3 - Ionic Compound Names (Metals that form multiple ions)
5 Read This! When the metal in an ionic compound always forms an ion with the same charge, you need not indicate that charge as part of the compound name. However, some atoms have the ability to from more than one type of ion. This can make naming confusing. You can t simply refer to a compound of copper and oxygen as copper oxide. People won t know which compound you are referring to - CuO or Cu 2 O.
6 Model 3 - Ionic compound names - metals that form multiple ions. Cu 2 O Copper(I) oxide CuO Copper(II) oxide SnF 2 Tin(II) fluoride SnF 4 Tin(IV) fluoride PbO Lead(II) oxide PbO 2 Lead(IV) oxide FeCl 2 Iron(II) chloride FeCl 3 Iron(III) chloride
7 16. Model 3 - what other metals could be included in the table? See Model 1 - Ion Charges for Selected Element
8 16. Model 3 - what other metals could be included in the table? See Model 1 - Ion Charges for Selected Element Mercury and nickel
9 17. Describe the most obvious difference between names in Model 2 and those in Model 2.
10 17. Describe the most obvious difference between names in Model 2 and those in Model 2. The names now have roman numerals in them.
11 18. Do the Roman numerals in names in Model 3 relate to the number of cations or the number of anions in the formula unit?
12 18. Do the Roman numerals in names in Model 3 relate to the number of cations or the number of anions in the formula unit? No, the roman numerals do not appear to relate to the number of anions or cations in the formula unit.
13 Support for answer? No, the roman numerals do not appear to relate to the number of anions or cations in the formula unit. In PbO the name is is Lead(II) oxide but there is only one lead cation and only one oxide anion in the formula unit.
14 Support for answer? No, the roman numerals do not appear to relate to the number of anions or cations in the formula unit. In PbO 2 the name is is Lead(IV) oxide but there is only one lead cation and two oxide anions in the formula unit, nothing to do with a 4.
15 19. Sum of the charges in an ionic compound must equal zero. a) Identify the charge on the copper cations in Copper(I) oxide and Copper(II) oxide, respectively.
16 19. Sum of the charges in an ionic compound must equal zero. a) Identify the charge on the copper cations in Copper(I) oxide and Copper(II) oxide, respectively. Cu 2 O CuO Cu + Cu 2+ O2- O2- Cu +
17 19. Sum of the charges in an ionic compound must equal zero. b) Identify the charge on the iron cations in Iron(II) chloride and Iron(III) chloride, respectively. FeCl 2 FeCl 3 Fe 2+ Fe 3+ Cl - Cl - Cl - Cl - Cl -
18 20. What do the Roman Numerals in the compounds described in question 19 indicate?
19 20. What do the Roman Numerals in the compounds described in question 19 indicate? The Roman numerals always indicate the charge of the cation in the compound. Copper(I) Cu + Copper(II) Cu 2+ Iron(II) Fe 2+ Iron(III) Fe 3+ Lead(II) Pb 2+ * Lead(IV) Pb 4+ *oxidation state
20 21. Fill in the table below. Compound Charge on Cation Name of the compound PbCl 4 Pb 4+ Lead(IV) chloride Fe 2 O 3 SnO CuBr 2
21 21. Fill in the table below. Compound Charge on Cation Name of the compound PbCl 4 Pb 4+ Lead(IV) chloride Fe 2 O 3 SnO Sn 2+ Tin(II) oxide CuBr 2
22 21. Fill in the table below. Compound Charge on Cation Name of the compound PbCl 4 Pb 4+ Lead(IV) chloride Fe 2 O 3 SnO Sn 2+ Tin(II) oxide CuBr 2 Cu 2+ Copper(II) bromide
23 21. Fill in the table below. Compound Charge on Cation Name of the compound PbCl 4 Pb 4+ Lead(IV) chloride Fe 2 O 3 Fe 3+ Iron(III) oxide SnO Sn 2+ Tin(II) oxide CuBr 2 Cu 2+ Copper(II) bromide
24 22. Determine the type of metal and name the compound. Formula unit Metal forms only one ion Metal forms multiple ions Name of the compound CaBr 2 MgO Ag 3 N SnCl 2
25 22. Determine the type of metal and name the compound. Formula unit Metal forms only one ion Metal forms multiple ions Name of the compound CaBr 2 MgO Ag 3 N yes yes yes SnCl 2 yes
26 22. Determine the type of metal and name the compound. Formula unit Metal forms only one ion Metal forms multiple ions Name of the compound CaBr 2 yes Calcium bromide MgO yes Magnesium oxide Ag 3 N yes Silver nitride SnCl 2 yes Tin(II) chloride
27 22. Determine the type of metal and name the compound. Formula unit Metal forms only one ion Metal forms multiple ions Name of the compound CuF 2 yes Copper(II) fluoride K 3 P yes potassium phosphide Zn 3 N 2 yes Zinc nitride HgO yes Mercury(II) oxide
28 23. Write the chemical formula for each ionic compound. Name of compound Formula unit Al 3+ Br 1- Aluminum bromide Tin(IV) chloride Iron(II) chloride Lithium oxide Lead(II) oxide Sn 4+ Fe 2+ Li 1+ Pb 2+ Cl 1- O 2-
29 23. Write the chemical formula for each ionic compound. Name of compound Formula unit Aluminum bromide AlBr 3 Tin(IV) chloride SnCl 4 Iron(II) chloride FeCl 2 Lithium oxide Lead(II) oxide Li 2 O PbO
30 Notes Properties of Ionic Compounds Page reference?
31 No single unit consisting of only one ion attracting one other ion is formed. Large numbers of positive ions (usually metal cations) and negative ions (often non-metal anions) exist together in a ratio determined by the number of electrons transferred from the metal to the non-metal. Notes Properties of Ionic Compounds Page reference- p. 217
32 Properties of ionic compounds cont. Strong attraction of positive ions and negative ions result in a crystal lattice (a 3D geometric arrangement of particles, each +ve ion is surrounded by -ve ions and each -ve ion is surrounded by +ve ions). Ionic crystals will vary in shape based on the sizes and relative numbers of the ions bonded.
33 Properties of ionic compounds cont. Physical properties: Mpt - high Bpt - high Large amounts of energy are required to break the ions apart; If an external force is large enough to move the ions in a crystal, the crystal cracks as like-charged ions next to each other will provide a repulsive force large enough to crack the crystal. Hardness - hard, rigid and brittle solids All as a result of the strong and numerous attractions between the ions in the compound.
34 Properties of ionic compounds cont. Physical properties: Solid ionic compounds do not conduct electricity (ions cannot move). Liquid state or when dissolved in water, ionic compounds conduct electricity (ions free to move) - called electrolytes (chemical changes occur).
35 Properties of ionic compounds cont. Lattice Energy: defined as the heat of formation for ions of opposite charge in the gas phase to combine into an ionic solid. As an example, the lattice energy of sodium chloride, NaCl, is the energy released when gaseous Na + and Cl - ions come together to form a lattice of alternating ions in the NaCl crystal. The more negative the lattice energy the stronger the force of attraction between those ions. Smaller cations tend to have more negative values for lattice energy than larger cations bonded to the same anions. Ions with larger positive or negative charge generally have more negative lattice energy. See Table 8-3 p 220
36 Bonding - Using the building blocks on the periodic table - when atoms interact with each other
37 Which group of elements do we know are chemically unreactive? What do we know about how many valence electrons they all have? What phase do they exist in at room temperature and 1 atmosphere pressure? (RTP)
38 8 Valence electrons are electrons in outermost (outer) energy level
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41 For two elements with large differences in electronegativity we see transfer of electrons from metal to non-metal and ionic compounds result
42 For two elements with roughly the same electronegativity values, the valence electrons are going to be shared through a covalent bond
43 p p
44 This is a molecule of an element since it is only made up of hydrogen atoms. We can make hydrogen molecules by reacting acid with Mg
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46 This is a molecule of an element since it is only made up of chlorine atoms. We saw green chlorine gas react with sodium to make salt in a video clip
47 I
48 STP Standard temperature and pressure 0.00 C and 1 atmosphere pressure Kinetic energy = ½ mv 2 All gases at STP lscience.co.uk/bama/ 14-16/aerosch2pg1.ht ml
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50 Boiling point is the temperature at which the vapor pressure of a liquid equals the external atmospheric pressure, at this temperature all molecules in a liquid have enough energy to vaporize
51 What about Bromine (Br 2 ) and iodine (I 2 )? Notice some of the molecules have enough energy to escape into vapor phase below the boiling point of the liquid Intermolecular like an interview between two people With this much mass the molecules just don t have enough energy to all be vapor at STP or even room temperature; intermolecular forces become significant here
52 What about Bromine (Br 2 ) and iodine (I 2 )?
53 This is the crystal lattice for iodine high mass of the iodine molecules not moving as quickly as lower mass molecules intermolecular forces are sufficient to hold the molecules close together in an organized way a crystal lattice
54 One of hardest known materials used to cut granite, concrete, glass Colorless Shiny Does not conduct electricity Each carbon atom shares an electron with 4 other carbon atoms to form 4 covalent bonds - in a tetrahedral arrangement in space Macromolecular solid Giant covalent structure
55 One of softest known materials slippery (used as a lubricant) grey Shiny Does conduct electricity Each carbon atom shares an electron with 3 other carbon atoms to form 3 covalent bonds - in a flat layer. The fourth electron from each atom gets delocalized between the layers, hold layers together loosely Macromolecular solid giant covalent structure
56 For two atoms with a small difference in electronegativity values, the valence electrons are likely to be shared, but unequally through the covalent bond - polar molecules
57 nonmetals have tightly held valence electrons OK to share to get full outer energy level
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(b) Formation of calcium chloride:
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