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Day 1

Day 1. Naming Compounds Writing Formulas. SWBAT. Write and name binary and tertinary ionic compounds Write and name covalent compounds. Systematic Naming. There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms.

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Day 1

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  1. Day 1 Naming Compounds Writing Formulas

  2. SWBAT Write and name binary and tertinary ionic compounds Write and name covalent compounds

  3. Systematic Naming • There are too many compounds to remember the names of them all. • Compound is made of two or more elements. • Put together atoms. • Name should tell us how many and what type of atoms.

  4. Periodic Table • More than a list of elements. • Put in columns because of similar properties. • Each column is called a group.

  5. Metals

  6. Transition metals • The Group B elements

  7. Non-metals • Dull • Brittle • Nonconductors- insulators

  8. Metalloids or Semimetals • Properties of both • Semiconductors

  9. 5 Types of Chemical Compounds • Binary ionic - metal ion – nonmetal ion • Ternary ionic - at least one ion is a polyatomic ion • Binary molecular - two nonmetals • Binary acid - H – nonmetal • Ternary acid - H – Polyatomic ion

  10. Atoms and ions • Atoms are electrically neutral. • Same number of protons and electrons. • Ions are atoms, or groups of atoms, with a charge. • Different numbers of protons and electrons. • Only electrons can move. • Gain or lose electrons.

  11. Anion • Anegative ion. • Has gained electrons. • Non metals can gain electrons. • Charge is written as a superscript on the right. F1- Has gained one electron O2- Has gained two electrons

  12. Cations • Positive ions. • Formed by losing electrons. • More protons than electrons. • Metals form cations. K1+ Has lost one electron Ca2+ Has lost two electrons

  13. Charge in groups 1A, 2A and 3A is the group number 1+ in 5A, 6A and 7A is the group number - 8 2+ 3+ 3- 2- 1-

  14. Naming Cations Just Write the name K1+ Potassium ion

  15. Naming Anions • Anions are always the same. • Change the element ending to – ide • F1- Fluorin

  16. Naming Anions • Anions are always the same. • Change the element ending to – ide • F1- Fluorine

  17. Naming Anions • Anions are always the same • Change the element ending to – ide • F1- Fluori

  18. Naming Anions • Anions are always the same • Change the element ending to – ide • F1- Fluor

  19. Naming Anions • Anions are always the same • Change the element ending to – ide • F1- Fluori

  20. Naming Anions • Anions are always the same • Change the element ending to – ide • F1- Fluorid

  21. Naming Anions • Anions are always the same • Change the element ending to – ide • F1- Fluoride

  22. Naming Binary Ionic Compounds • Binary Compounds - 2 elements. • Ionic - a cation and an anion. • The name is just the names of the ions. • Cation first anion second • Easy with Group A elements. • NaCl = Na+ Cl- = sodium chloride • MgBr2 = Mg2+ Br- = magnesium bromide • Na2S

  23. Naming Binary Ionic Compounds • The problem comes with the transition metals. • Cation name includes the charge. • The compound must be neutral. • same number of + and – charges. • Use the negative charge to find the charge on the positive ion.

  24. Naming Binary Ionic Compounds • Write the name of CuO • Need the charge of Cu • O is 2- • copper must be 2+ • Copper(II) oxide • Name CoCl3 • Cl is 1- and there are three of them = 3- • Co must be 3+ • Cobalt(III) chloride

  25. Naming Binary Ionic Compounds • Write the names of the following • KCl • Na3N • CrN • Sc3P2 • PbO • PbO2 • Na2Se

  26. Polyatomic ions • Groups of atoms that stay together and have a charge. • Covalently bonded • You must memorize these.

  27. A Few Polyatomic Rules: PA ions which contain Oxygen contain endings of -ite ( the least amount of Oxygen )and –ate ( the greater amount). For ex. Sulfite SO32- and Sulfate SO42- Nitrite NO21- and Nitrate NO31-

  28. Polyatomic Rules cont. Hydrogen is often indicated by an ions name when present. For ex.: Hydrogen sulfate HSO41- The prefixes mono- and di- are sometimes used. For ex.: Dihydrogen phosphate H2PO41- The prefix thio- means, replace an Oxygen with a Sulfur.

  29. 1- ions • Acetate C2H3O21- • Nitrate NO31- • Nitrite NO21- • Hydroxide OH1- • Permanganate MnO41- • Cyanide CN1-

  30. 1- ions • Perchlorate ClO41- • Chlorate ClO31- • Chlorite ClO21- • Hypochlorite1-

  31. Sulfate SO42- Sulfite SO32- Carbonate CO32- Chromate CrO42- Dichromate Cr2O72- Silicate SiO32- 2- ions

  32. Phosphate PO43- Phosphite PO33- 3- ions 1+ ion • AmmoniumNH41+

  33. Adding Hydrogen to Polyatomics • Hydrogen ions are 1+ • Attach to other polyatomic ions- changes charge by one • Sulfate SO42- • Hydrogen sulfate HSO41- • Phosphate PO43- • Hydrogen phosphate HPO42- • Dihydrogen phosphate H2PO41-

  34. Ternary Ionic Compounds • Will have polyatomic ions • At least three elements (3 capital letters) • Still just name the ions • NaNO3 • CaSO4 • CuSO3

  35. Ternary Ionic Compounds • (NH4)2O • Fe(OH)3 • LiCN • (NH4)2CO3 • NiPO4

  36. Writing Formulas • The charges have to add up to zero. • Get charges on pieces. • Cations from name or periodic table. • Anions from periodic table or polyatomic. • Balance the charges by adding subscripts. • Put polyatomics in parenthesis if there is more than one of them

  37. Writing Formulas • Write the formula for calcium chloride. • Calcium is Ca2+ • Chloride is Cl1- • Ca2+Cl1- would have a 1+ charge. • Need another Cl1- • Ca2+Cl21-

  38. Crisscross • Switch the numerical value of the charges Ba2+ N3- 3 2 Ba3 N2 • Reduce ratio if possible

  39. Write the formulas for these • Lithium sulfide • tin (II) oxide • tin (IV) oxide • Copper (II) sulfate • Iron (III) phosphide • gallium nitrate • Iron (III) sulfide • ammonium sulfide

  40. Write the formulas for these • Ammonium chloride • barium nitrate

  41. Roman Numeral? Polyatomic? Yes No Yes No Charge from name Charge from table Formula and charge from memory Charge from table M+X Nm-Y MYNmX Ionic

  42. Things to look for • If cations have (), the number is their charge. Not how many. • If anions end in -ide they are probably off the periodic table (Monoatomic) • If anion ends in -ate or -ite it is polyatomic • The positive piece always gets written first • Hydrogen- it depends on where it’s at • If it is second, it’s a nonmetal -hydride

  43. Molecular Compounds Writing names and Formulas

  44. Molecular compounds • made of just nonmetals • smallest piece is a molecule • can’t be held together because of opposite charges. • can’t use charges to figure out how many of each atom

  45. Easier • Ionic compounds use charges to determine how many of each. • Have to figure out charges. • Have to figure out numbers. • Molecular compounds name tells you the number of atoms. • Uses prefixes to tell you the number

  46. Prefixes • 1 mono- • 2 di- • 3 tri- • 4 tetra- • 5 penta- • 6 hexa- • 7 hepta- • 8 octa- • 9 nona- • 10 deca-

  47. Naming • To write the name write two words • Exception - we don’t write mono- if there is only one of the first element. • No ao oo double vowels when writing name, io, oi, and ai are okay. Prefix name Prefix name -ide

  48. Name These • N2O • NO2 • Cl2O7 • CBr4 • CO2 • BaCl2

  49. Write formulas for these • diphosphorus pentoxide • tetraiodine nonoxide • sulfur hexaflouride • nitrogen trioxide • Carbon tetrahydride • phosphorus trifluoride • aluminum chloride • diagram

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