What do you remember? Classifying Compounds Section 1.5 pg

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1 What do you remember? Classifying Compounds Section 1.5 pg

2 Pre-test What is the name for the following combinations of atoms? What state are they at SATP? Metal and Non-metal? Non-metal and Non-metal? Metal and Metal? What is a polyatomic ion? Give one example? What are multivalent ions? What is a hydrate? How would you name the following? NaCl (s) CaCO 3(s) NiF 2(s)

3 THREE TYPES OF COMPOUNDS From the two classes of elements (metals and non-metals) there can be three classes of compounds: A) Ionic Compounds = Metal and Non-Metal e.g. NaCl, MgO, CaCO 3 B) Molecular Compounds = Non-Metal Non-Metal e.g. H 2 O, C 12 H 22 O 11, P 4 O 10 C) Intermetallic (Metallic) Compounds or Alloys Metal metal combinations e.g. Brass (Cu + Zn), Loonie (Cu + Sn)

4 IONIC COMPOUNDS Composed of cations (+) and anions (-) Form a crystal lattice of ionic bonds An ionic bond is a strong attraction of opposite charges Relatively high m.p. and b.p. (because bonds are so strong) Crystalline solids at SATP (these DO NOT conduct electricity) May dissolve in water (soluble) or not (insoluble) Soluble has an (aq) subscript; use solubility table to determine Will only conduct electricity if soluble in water because the ions are separated and electrons can move (dissociation)

5 MOLECULAR COMPOUNDS Consists of covalently bonded non-metal atoms Molecular (covalent) bonds are the result of sharing electrons Relatively low m.p. and b.p. (because covalent bonds are weaker) Solid, liquid or gas at SATP (will NOT conduct electricity in any state because there are no ions present) May be soluble or insoluble in water Will not conduct electricity if soluble (aq)

6 INTERMETALLIC COMPOUNDS The simultaneous attraction between positive nuclei and mobile valence electrons in a metal In a metallic bond, electrons flow freely around atomic nuclei Alloys solutions of a metal with other metals; don t combine in definite proportions Ex. Sterling silver (Ag + Cu); Loonie (Cu + Sn) Intermetallic compounds metal-metal combinations in definite proportions Ex. CuZn, Cu 5 Zn 8, CuZn 3 in brass at certain temperatures This model shows a continuous (grey) area occupied by mobile valence electrons, attracting all the positive metal ions at once, to hold them together in a regular structure with a net (overall) charge of zero

7 STATES OF MATTER Ionic compounds are always (s) at SATP Molecular compounds are (s), (l), or (g) at SATP States are known through memorization, tables, experience, etc Metallic compounds are always (s) at SATP (except Hg (l) ) Diagnostic Test a procedure to identify or classify chemicals Ex. Ionic compounds conduct electricity in an aqueous state Empirical Definition defines a class of compounds based on empirical (observeable) properties Ex. Solubility, state, ph, conductivity

8 Monatomic Ions single atom that has gained or lost electrons You must be able to predict charges for ions formed from atoms in groups 1, (representative elements) Draw with a element symbol and a superscript + or Cl (has 17 p + and 17 e - ) Cl - (has 17 p + and 18 e - ) Naming Monatomic Ions: Cations: (name) ion ex. Na + = sodium ion Anions: (name)ide ion ex. F - = fluoride ion Transition Elements (Groups 3-12) cannot be predicted - so charges are listed on the periodic table - always use the most common charge unless otherwise indicated Boron, Silicon, and Carbon rarely form ions (supported by empirical evidence) Hydrogen atoms usually lose 1 e - to become a positive ion =H + (hydrogen ion) - Although unusual, hydrogen can gain 1 e - and form a negative ion = H - (hydride ion) Binary Ionic Compounds composed of 2 monatomic ions Ex. NaCl, BaCl 2, CaO, Al 2 O 3, etc.

9 Polyatomic Ions a group of atoms covalently bonded (thus a molecular compound) that carries a net charge This group always stays together and acts as a unit. Ex. PO 4 3-, CH 3 COO -, NO 3-, SO 4 2- Naming Polyatomic Ions refer to the Polyatomic Ion Table (do not change the names at all)

10 Multivalent Ions metals that can form more than one stable ion charge (can be determined from the anion it is joined with) Ex. Fe has a Fe 2+ and a Fe 3+ ion (Looking at the periodic table, which is more common?) FeO (s) oxygen has a 2 - charge so Fe must be the 2 + charge CHECK: 1(-2) + 1(+2) = 0 the net charge is zero so Fe 2+ is the correct ion Fe 2 O 3(s) there are 3 oxygen s with the 2- charge = -6 so to be balanced by 2 iron ions, we must be using the Fe 3+ ion CHECK: 3 (-2) + 2 (+3) = 0 the net charge is zero so Fe 3+ is the correct ion Naming Multivalent Ions: Roman numeral numbers are used so that the reader knows which ion to use Ex. Fe 2+ is the iron(ii) ion (no space) Fe 3+ is the iron(iii) ion (no space)

11 Hydrates ionic compounds that have water held loosely to the compound Decompose at relatively low temp. to produce water and the ionic compound Water within an ionic crystal is called the water of hydration Anhydrous a compound that is usually a hydrate but the water of hydration has been removed Writing the chemical formula for hydrates: A large dot is use in the formula to connect the ionic compound formula unit with the number of water molecules present Ex. CuSO 4 5H 2 O (s) Naming Hydrates: Name the ionic compound first then: a) add -#- water (no spaces) IUPAC NAME b) add mono, di, tri, etc. hydrate Traditional NAME Ex. CuSO 4 5H 2 O (s) IUPAC = copper(ii) sulfate-5-water Traditional = copper(ii) sulfate pentahydrate See Figure 7 pg. 31

12 Naming Ionic Compounds 1. If your compound is ionic and you have the formula: Practice: a) the name of the metallic element appears first b) the name of the non-metallic element appears last *Its ending is changed to ide, except if it comes from the polyatomic ion table c) always use lowercase letters d) if you re dealing with a transition metal (multivalent element) that can form more than one stable ion, use Roman Numerals, in brackets, to indicate the charge 1) CaCl 2 = calcium chloride change non-metallic ending to ide 2) Mg 3 (PO 4 ) 2 = magnesium phosphate from polyatomic ion table don t change ending 3) SnO 2 = tin(iv) oxide tin has a +2 or +4 ion possible; had to use roman numerals to show we were dealing with Sn 4+

13 Writing Ionic Formulas 2) If your compound is ionic and you have the name: a) the symbol for the metallic element comes first b) the symbol for the non-metallic element comes last c) you need a net charge of zero, so subscripts are used to indicate the ratio of ions in the compound. d) if using polyatomic ions, make sure to put brackets around the ion if there are multiples of it present e) all ionic compounds are solid at SATP so add a (s) subscript Practice: 1) barium phosphide = Ba 2+ P 3- = Ba 3 P 2 (s) check: 3 (+2) + 2 (-3) = 0 net charge 2) nickel(ii) oxide = Ni 2+ O 2- = NiO (s) check: (+2) + (-2) = 0 net charge 3) copper(ii) phosphate = Cu 2+ PO = Cu 3 (PO 4 ) 2 (s) check: 3 (+2) + 2 (-3) = 0 net charge

14 Post-test Describe the three combinations of atoms possible. What state are they at SATP? Give two examples of polyatomic ions. Give two examples of multivalent ions write all ions possible and circle the most common one. What is the difference between a hydrate and an anhydrous compound? Name the following: Write the formula for the following: KCl (s) strontium phosphide NaNO 3(s) calcium phosphate NiF 3(s) cobalt(iii) chloride

15 Homework Read Ionic Compounds Summary pg. 31 Naming Ionic Compounds Worksheet Section 1.5 pg.32 #5, 8-11, 14 Read pg

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