Nomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion

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1 PO 4 3- phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 - acetate ion SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

2 CHEMICAL BONDS A chemical bond is an electrostatic (attractive) force that holds oppositely charged particles together in an ionic compound. Bonds are represented using lines.

3 FORMS OF CHEMICAL BONDS Most bonds are somewhere in between ionic and covalent. There are 3 forms bonding atoms: Ionic complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) between a metal and a nonmetal. Covalent some valence electrons shared between atoms of nonmetals. Metallic holds atoms of a metal together

4 PROPERTIES OF COMPOUNDS Ionic Compounds- high melting and boiling points due to strong bonds between ions. Ionic compounds in an aqueous (water) solution conduct an electric charge, this means they are good conductors of electricity. They gain or lose electrons. Covalent Compounds- low melting and boiling points and have weak bonds. They only share electrons. Metallic Compounds- have a sea of electrons, metal atoms do not share or lose their valence electrons with neighboring atoms. Instead they overlap their electrons. They are malleable, ductile, and good conductors of electricity. They tend to have high melting and boiling points.

(International Union of Pure and Applied Chemistry) Chemicals that should

5 COMMON NAMES A lot of chemicals have common names as well as the proper IUPAC name. (International Union of Pure and Applied Chemistry) Chemicals that should always be named by common name and never named by the IUPAC method are: H 2 O water, not dihydrogen monoxide NH 3 ammonia, not nitrogen trihydride

6 COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na + + Cl - --> NaCl A neutral compound requires equal number of + and - charges.

7 Predicting Charges on Monatomic Ions KNOW THESE!!!! Cd +2

8 PROPERTIES OF IONIC COMPOUNDS FORMING NACL FROM NA AND CL 2 A metal atom can transfer an electron to a nonmetal. The resulting cation and anion are attracted to each other by electrostatic forces.

9 ammonium chloride, NH 4 Cl IONIC COMPOUNDS NH 4 + Cl -

SOME IONIC COMPOUNDS Ca 2+ + 2 F - ---> CaF 2 Mg 2+ + N -3 ----> Mg 3 N 2

10 SOME IONIC COMPOUNDS Ca F - ---> CaF 2 Mg 2+ + N > Mg 3 N 2 magnesium nitride Sn 4+ + O > calcium fluoride SnO 2 Tin (IV) oxide

11 FORMULAS OF IONIC COMPOUNDS Formulas of ionic compounds are determined from the charges on the ions atoms ions Na + F : Na + : F : NaF sodium + fluorine sodium fluoride formula Charge balance: = 0

12 MONATOMIC IONS

13 WRITING A FORMULA Write the formula for the ionic compound that will form between Ba 2+ and Cl. Solution: 1. Balance charge with + and ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl Cl 3. Write the number of ions needed as subscripts BaCl 2 4. Keep all subscripts together for polyatomic ions (ex: CO 3-2 ) K + + CO 3-2 K 2 CO 3 NH CO 3-2 (NH 4 ) 2 CO 3

14 LEARNING CHECK Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 S c) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

15 SOLUTION 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

16 COMMON POLYATOMIC IONS Negative 1 Charge Negative 2 Charge Acetate C 2 H 3 O 2-1 Perchlorate ClO 4-1 Chlorate ClO 3-1 Chlorite ClO 2-1 Hypochlorite ClO -1 Cyanide CN -1 Hydrogen Carbonate or Bicarbonate HCO 3-1 Hydrogen Sulfate HSO 4-1 Hydroxide OH -1 Nitrate NO 3-1 Permanganate MnO 4-1 Nitrite NO 2-1 Carbonate CO -2 3 Chromate CrO -2 4 Dichromate Cr 2 O -2 7 Oxalate C 2 O -2 4 Sulfate SO -2 4 Sulfite SO -2 3 Selenate SeO -2 4 Negative 3 Charge Phosphate PO -3 4 Phosphite PO -3 3 Borate BO -3 3 Positive 1 Charge Ammonium NH +1

18 CRISS CROSS METHOD Positive Ion always written first If you have a polyatomic ion, you must put it in parentheses ( ) if you cross a number other than 1 to the bottom. Ex: Be +2 SO 4-3 Be 3 (SO 4 ) 2 You do not have to put Be in parentheses since it is a monatomic ion (just one atom).

19 COUNTING ATOMS How many atoms are in the following compounds? NaCl (NH 4 ) 3 PO 4 NaOH LiNO 3 Mg(OH) 2 BeSO 4 Ca 3 (PO 4 ) 2 NH 4 Cl SrSO 3 Cs 2 CO 3

20 NAMING COMPOUNDS Binary Ionic Compounds: 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl = chloride CaCl 2 = calcium chloride

21 NAMING BINARY IONIC COMPOUNDS Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

22 LEARNING CHECK Complete the names of the following binary compounds: Na 3 N sodium KBr Al 2 O 3 MgS potassium aluminum

23 TRANSITION METALS Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(i) ion iron(ii) ion copper (II) ion iron(iii) ion

24 NAMES OF VARIABLE IONS These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ ) lead (II) chloride Fe 2 S 3 (Fe 3+ ) iron (III) sulfide

25 EXAMPLES OF OLDER NAMES OF CATIONS FORMED FROM TRANSITION METALS (YOU DO NOT HAVE TO MEMORIZE THESE)

26 LEARNING CHECK Complete the names of the following binary compounds with variable metal ions: FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S iron ( ) bromide copper ( ) chloride ( )

27 NAMING COMPOUNDS Poly- many Bi- 2 Polyatomic ions- many (2 or more) atoms bonded together that have a charge (positive or negative charge). Binary-2 atoms or elements bonded together Ternary- 3 or more atoms bonded together Oxidation number- charge of the atom

28 NAMING IONIC COMPOUNDS

29 POLYATOMIC IONS NO 3 - nitrate ion NO 2 - nitrite ion

30 POLYATOMIC IONS You can make additional polyatomic ions by adding a H + to the ion! CO 3-2 is carbonate HCO 3 is hydrogen carbonate H 2 PO 4 is dihydrogen phosphate HSO 4 is hydrogen sulfate

31 TERNARY IONIC NOMENCLATURE Writing Formulas Write each ion, cation first. Don t show charges in the final formula. Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion s charge when needed (stock system)

32 TERNARY IONIC NOMENCLATURE Sodium Sulfate Na + and SO 4-2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 2 (NH 4 ) 2 CO 3

TYPES OF REACTIONS Endothermic reaction- a chemical reaction in which a greater amount of energy is required to break the bonds than is released.

Exothermic reaction- a chemical reaction in which more energy is released than is required to break the bonds.

Delocalized electron- the electrons involved in metallic bonding that are free to move easily from one atom to the next.

33 TYPES OF REACTIONS Endothermic reaction- a chemical reaction in which a greater amount of energy is required to break the bonds than is released. (energy in) These reactions are cool to the touch in a container. Exothermic reaction- a chemical reaction in which more energy is released than is required to break the bonds. (energy out) The formation of ionic compounds is exothermic. Burning something releases energy and is an exothermic reaction. Delocalized electron- the electrons involved in metallic bonding that are free to move easily from one atom to the next. Oxyanion- a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms. Ex: Sulfate SO -2 4 Sulfite SO -2 3 Nitrate NO - 3, Nitrite NO 2-, etc. Formula unit- the simplest ratio of ions represented in an ionic compound. Ex: Ba 2 O 2 can be simplified to BaO, Ca 2 (SO 4 ) 2 can be simplified to CaSO 4

34 LEARNING CHECK 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(ii) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOH b) Fe 3 OH c) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

35 NAMING TERNARY COMPOUNDS Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate

36 LEARNING CHECK Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2. Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

37 MIXED PRACTICE! Name the following: 1. Na 2 O 2. CaCO 3 3. PbS 2 4. Sn 3 N 2 5. Cu 3 PO 4 6. HgF 2

38 MIXED UP THE OTHER WAY Write the formula: 1. Copper (II) chlorate 2. Calcium nitride 3. Aluminum carbonate 4. Potassium bromide 5. Barium fluoride 6. Cesium hydroxide

39 NAMING MOLECULAR COMPOUNDS CO 2 Carbon dioxide All molecular/ covalent compounds formed from two or more nonmetals. CH 4 methane BCl 3 boron trichloride Ionic compounds generally involve a metal and nonmetal (NaCl)

Add prefixes to indicate # of atoms. Omit monoprefix on the FIRST element.

40 MOLECULAR (COVALENT) NOMENCLATURE FOR TWO NONMETALS Prefix System (binary compounds) 1. Less electronegative atom comes first. 2. Add prefixes to indicate # of atoms. Omit monoprefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it s NOT optional!). 3. Change the ending of the second element to -ide.

41 MOLECULAR NOMENCLATURE PREFIXES PREFIX monoditritetrapentahexaheptaoctanonadeca- NUMBER

42 MOLECULAR NOMENCLATURE: EXAMPLES CCl 4 carbon tetrachloride N 2 O SF 6 dinitrogen monoxide sulfur hexafluoride

43 MORE MOLECULAR EXAMPLES arsenic trichloride AsCl 3 dinitrogen pentoxide N 2 O 5 tetraphosphorus decoxide P 4 O 10

44 LEARNING CHECK Fill in the blanks to complete the following names of covalent compounds. CO carbon oxide CO 2 PCl 3 CCl 4 N 2 O carbon phosphorus chloride carbon chloride nitrogen oxide

45 LEARNING CHECK 1. P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

46 OVERALL STRATEGY FOR NAMING CHEMICAL COMPOUNDS.

47 A FLOW CHART FOR NAMING BINARY COMPOUNDS.

48 MIXED REVIEW Name the following compounds: 1. CaO a) calcium oxide b) calcium(i) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachloride b) tin(ii) chloride c) tin(iv) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

49 SOLUTION Name the following compounds: 1. CaO 2. SnCl 4 a) calcium oxide c) tin(iv) chloride 3. N 2 O 3 b) Dinitrogen trioxide

50 MIXED PRACTICE 1. Dinitrogen monoxide 2. Potassium sulfide 3. Copper (II) nitrate 4. Dichlorine heptoxide 5. Chromium (III) sulfate 6. Iron (III) sulfite 7. Calcium oxide 8. Barium carbonate 9. Iodine monochloride

51 MIXED PRACTICE 1. BaI 2 2. P 4 S 3 3. Ca(OH) 2 4. FeCO 3 5. Na 2 Cr 2 O 7 6. I 2 O 5 7. Cu(ClO 4 ) 2 8. CS 2 9. B 2 Cl 4

52 ACID NOMENCLATURE Acids Compounds that form H + in water. Formulas usually begin with H. In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) Ternary acids are ALL aqueous Examples: HCl (aq) hydrochloric acid HNO 3 nitric acid H 2 SO 4 sulfuric acid

53 ACID NOMENCLATURE REVIEW No Oxygen w/oxygen Anion Ending -ide -ate -ite Acid Name hydro-(stem)-ic acid (stem)-ic acid (stem)-ous acid An easy way to remember which goes with which In the cafeteria, you ATE something ICky

54 ACID NOMENCLATURE FLOWCHART ACIDS start with 'H' 2 elements 3 elements hydro- prefix -ic ending no hydro- prefix -ate ending becomes -ic ending -ite ending becomes -ous ending

55 ACID NOMENCLATURE HBr (aq) 2 elements, -ide hydrobromic acid H 2 CO 3 3 elements, -ate carbonic acid H 2 SO 3 3 elements, -ite sulfurous acid

56 ACID NOMENCLATURE hydrofluoric acid 2 elements sulfuric acid 3 elements, -ic nitrous acid 3 elements, -ous H + F- H + SO 4 2- H + NO 2 - HF (aq) H 2 SO 4 HNO 2

57 NAME EM! HI (aq) HCl H 2 SO 3 HNO 3 H 3 PO 4

58 WRITE THE FORMULA! Hydrobromic acid Nitrous acid Carbonic acid Phosphoric acid Hydrotelluric acid

59 Nomenclature Summary Flowchart

60 RAINBOW MATRIX GAME Link on Chemistry Geek.com on Chemistry I page Use [ ] to represent subscripts since you can t enter subscripts into the computer So H 2 O would be H[2]O And Al 2 (SO 4 ) 3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3-3 ; Silicate = SiO 4-4 ; Manganate = MnO 4-2 (permanganate is -1)

Nomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion. Chemistry 1 Honors: Chapter 7: pp

Nomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion. Chemistry 1 Honors: Chapter 7: pp Chemistry 1 Honors: Chapter 7: pp218-258 PO 4 3- phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 - acetate ion SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts"