1. Unit 6 – Naming Chemical Compounds
Ch. 7 – Chemical Formulas and Chemical Compounds

2. Opener 1/8/
Choose two of the following elements that would make an ionic compound. Write the formula K, He, H, F, Ca, O
Choose two of the following elements that would make a covalent compound. Write the formula K, He, H, F, Ca, O
What is the formula of a compound made between Mg+2 and Cl-1 ?
What is the name of the compound you made in question #3?

3. Opener 1/6/16
Choose two of the following elements that would make an ionic compound K, He, H, F, Ca, O
Choose two of the following elements that would make a covalent compound K, He, H, F, Ca, O
What is the formula of a compound made between Na+1 and O-2 ?
What is the name of the compound you made in question #3?

4. Opener 1/7/16
Choose the correct formula for the compounds containing the following ions:
1. Na+, S2-
NaS Na2S NaS2
2. Al3+, Cl-
AlCl3 AlCl Al3Cl
3. Mg2+, N3-
MgN Mg2N3 Mg3N2

5. Learning Targets Explain the significance of a chemical formula.
Describe the naming of binary ionic and covalent compounds.

6. Chemical Names and Formulas
What information can be gained from a chemical formula?
Chemical formula – indicates the number of atoms of each kind of element in a chemical compound

7. Chemical Names and Formulas
3 main types of chemical bonding Metallic Bonding – bonding of at least 2 metals between a sea of electrons Ionic Bonding – bonding of at least 1 metal and 1 nonmetal created by the transfer of electrons between a cation and an anion. Covalent Bonding – bonding by the sharing of electrons between at least 2 nonmetals

8. Chemical Names and Formulas
What are monatomic ions?
Monatomic ions – ions formed from a single atom
Examples: Mg2+ , H+ , Cl-, O2-

9. Chemical Names and Formulas
Naming monatomic ions
Monatomic cations are identified simply by the element’s name
Monatomic anion – the ending of the element’s name is dropped and –ide is added to the root name.
Examples: Mg (Magnesium) Mg2+ (Magnesium)
F (Fluorine) F- (Fluoride)
N (Nitrogen) N3- (Nitride)

10. Monatomic Ions

11. Chemical Names and Formulas
What is a binary compound?
Binary Compound – Compounds composed of only 2 different elements
Examples: MgBr2, HCl, LiF

12. Predicting Charges on Monatomic Ions
KNOW THESE !!!!
Cd+2

13. 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

14. Chemical Names and Formulas
Balancing an ionic compound
a) Write the symbols for the ions side by side. Write the cations 1st.
Al 3+ O2-
b) Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion.
Al3+2 O2-3
c) Check the subscripts and divide them by their largest common factor to give the smallest possible whole # ratio of ions. Then write the formula.
Al2O3

15. Chemical Names and Formulas
Rules for naming a binary ionic compound
a) The name of the cation (metal) is given first.
b) This is followed by the name of the anion.
Example: MgBr2 = Magnesium Bromide

16. Practice!!! zinc (II) iodide aluminum oxide
Write the chemical formula for the following:
sodium chloride
zinc (II) iodide
aluminum oxide
2. Complete the names of the following binary compounds with transition metal ions:
FeBr2 iron (_____) bromide
CuCl copper (_____) chloride
SnO2 ___(_____ ) ______________
Fe2O3 ________________________
Hg2S ________________________

17. Polyatomic Ions
NO3-
nitrate ion
NO2-
nitrite ion

18. Polyatomic Ions
You can make additional polyatomic ions by adding a H+ to the ion!
CO3 -2 is carbonate
HCO3– is hydrogen carbonate
H2PO4– is dihydrogen phosphate
HSO4– is hydrogen sulfate
**See list**

19. Chemical Names and Formulas
Rules for naming compounds that contain polyatomic ions
Compounds containing polyatomic ions are named in a similar manner as binary ionic compounds. The name of the cation is given 1st and followed by the name of the anion.
Ex. NH4Cl = Ammonium chloride
LiOH = Lithium hydroxide

20. Ternary Ionic Naming 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 to indicate the ion’s charge when needed (stock system)

21. Chemical Names and Formulas
Rules for naming compounds that contain transition metals
Roman numerals are used to indicate an ion’s charge. The numeral is enclosed in parentheses and placed immediately after the metal name.
Ex. Fe2+ = Iron (II) Fe3+ = Iron (III)

22. Examples: Ternary Ionic Naming
Sodium Sulfate
Na+ and SO4 -2
Na2SO4
Iron (III) hydroxide
Fe+3 and OH-
Fe(OH)3
Ammonium carbonate
NH4+ and CO3 –2
(NH4)2CO3

23. Opener 1/13/15 1. aluminum nitrate 2. copper(II) nitrate
3. Iron (III) hydroxide
4. Tin(IV) hydroxide

24. Opener 1/13/15 1. aluminum nitrate Al(NO3)3 2. copper(II) nitrate
Cu(NO3)2
3. Iron (III) hydroxide
Fe(OH)3
4. Tin(IV) hydroxide
Sn(OH)4

25. Opener 1/14/14 Match each set with the correct name:
Na2CO3 magnesium sulfite
MgSO3 magnesium sulfate
MgSO4 sodium carbonate
2 . Ca(HCO3)2 calcium carbonate
CaCO3 calcium phosphate
Ca3(PO4)2 calcium bicarbonate

26. Opener 1/7/16 Write formula: 1. Sodium carbonate 2. Magnesium sulfate
3. Iron(III) sulfite
Write name:
4. Ca(HCO3)2
CuSO4
Co3(PO4)2

27. Naming Molecular (Covalent) Compounds
All are formed from two or more nonmetals.
CO2 Carbon dioxide
Ionic compounds generally involve a metal and nonmetal
(NaCl)
BCl3 boron trichloride
CH4 methane

28. Chemical Names and Formulas
Rules for naming binary covalent compounds
a) The less electronegative element is given 1st. It is given a prefix only if it contributes more than 1 atom to the molecule of the compound.
b) The 2nd element is named by combining (1) a prefix indicating the # of atoms contributed by the element, (2) the root of the name of the 2nd element, and (3) the ending –ide
c) The “o” or “a” at the end of a prefix is usually dropped when the word following the prefix begins with another vowel

29. Chemical Names and Formulas
Prefixes for binary covalent compounds
Number of atoms
Prefix 1
Mono- 2
Di- 3
Tri- 4
Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8
Octa- 9
Nona- 10
Deca-

30. Molecular Naming: Examples
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride

31. More Molecular Examples
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10

32. Common Names
A lot of chemicals have common names as well as the proper IUPAC name.
Chemicals that should always be named by common name and never named by the IUPAC method are:
H2O water, not dihydrogen monoxide
NH3 ammonia, not nitrogen trihydride

33. Learning Check Name the follow covalent compounds. CO CO2 PCl3 CCl4
N2O

34. Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO2 carbon _______________
PCl3 phosphorus _______chloride
CCl4 carbon ________chloride
N2O _____nitrogen _____oxide

35. Opener 1/13/15
1. P2O5
2. Cl2O7
Sn(SO4)2 * 5 (H2O)
Cl2

36. Opener 1/14/15
1. P2O5
2. Cl2O7
Sn(SO4)2
Cl2

37. Opener 1/14/15 1. P2O5 Diphosphorus pentoxide 2. Cl2O7
Dichlorine heptoxide
Sn(SO4)2
Cl2 Chlorine

38. Overall strategy for naming chemical compounds.

39. A flow chart for naming binary compounds.
Fig. 4-1

40. Review of Chemical Formulas
Recall that in a chemical formula, the subscript indicates the number of atoms of each element present in a compound.
C12H22O11
12 carbon atoms
22 hydrogen atoms
11 oxygen atoms

41. Review of Chemical Formulas
When parentheses are used in a formula, each element inside must be multiplied by the subscript outside the ( ).
Ca(C2H3O2)2
1 Calcium
4 Carbon
6 Hydrogen
4 Oxygen

42. Molar Mass/GFM
Molar Mass or Gram Formula Mass (GFM) is the sum of all the masses of each element for one mole of a compound.
Water (H2O) has a GFM of 18 g for every mole:
2 hydrogen = 2(1 g) = g
1 oxygen = 1(16 g) = +16 g
total mass = 18 g/mole

43. Molar Mass/GFM Find the molar mass of the following compounds:
Sugar C12H22O11
Mg(NO3)2

44. Molar Mass/GFM Sugar, C12H22O11 12 carbon 12(12 g) = 144 g
22 hydrogen 22(1 g) = 22 g
11 oxygen 11(16 g) = 176 g
total g/mole

45. Molar Mass/GFM Mg(NO3)2 1 magnesium 1(24.3 g) = 24.3 g
2 nitrogen (14 g) = 28 g
6 oxygen (16 g)= 96 g
total g/mole

46. Percent Composition Percent (%) = (part/whole) x 100
To determine the percent composition by mass of a compound, you must know its Molar Mass/GFM.
For example, NaOH
1 Na = g %Na = (23/40) x 100 =57.5%
1 O = g %O = (16/40) x 100= 40.0%
1H = g %H = (1/40) x 100 = 2.5%
Total = g/mol

47. Percent Composition ?’s
Name, molar mass (GFM), % composition
C12H22O11
Fe2(SO4)3

48. Percent Composition ?’s
Name, molar mass (GFM), % composition
MgCl2
FeSO4

49. Lab: Percent Composition of Sugar in bubble gum
Learning Targets
I can define percent composition.
I can accurately calculate the percent composition of a compound.

50. Lab: Percent Composition of Sugar in bubble gum
When bubble gum is chewed, the sugar from the gum is dissolved in your saliva and removed from the gum.
We want to find out how much sugar is contained in one piece of gum!... Will use mass to determine this!

51. Lab: Percent Composition of Sugar in gum
Read lab handout thoroughly!
Answer Pre-Lab questions
Write Hypothesis, Materials list and Procedure
Obtain Gum, complete experiment and data tables
Calculations!!
Graphs!!
Conclusion!!
Post Lab Questions

52. Molar Mass/GFM Sugar, C12H22O11 12 carbon 12(12 g) = 144 g
22 hydrogen 22(1 g) = 22 g
11 oxygen 11(16 g) = 176 g
total g/mole

53. Percent Composition Percent (%) = (part/whole) x 100
To determine the percent composition by mass of a compound, you must know its Molar Mass/GFM.
For example, NaOH
1 Na = g %Na = (23/40) x 100 =57.5%
1 O = g %O = (16/40) x 100= 40.0%
1H = g %H = (1/40) x 100 = 2.5%
Total = g

54. Percent Composition ?’s
Name, molar mass (GFM), % composition
MgCl2
FeSO4

55. Percent Composition ?’s
Name, molar mass (GFM), % composition
C12H22O11
Fe2(SO4)3

56. [( )/6.4] *100=

57. Lab: Percent Composition of Sugar in gum
Read lab handout thoroughly!
Answer Pre-Lab questions
Write Hypothesis, Materials list and Procedure
Obtain Gum, complete experiment and data tables
Calculations!!
Graphs!!
Conclusion!!
Post Lab Questions

58. Opener 1//16
Name, molar mass (GFM), % composition
C12H22O11
Fe2(SO4)3

59. Molar Mass/GFM Sugar (sucrose), C12H22O11 12 carbon 12(12 g) = 144 g
22 hydrogen 22(1 g) = 22 g
11 oxygen 11(16 g) = 176 g
total g/mole

60. Molar Mass/GFM Iron (III) sulfate, Fe2(SO4)3
2 iron 2(55.8 g) = g
3 sulfur 3(32.1 g) = g
12 oxygen 12(16 g) = 192 g
total g/mole

61. Mole Conversions Find how many grams of NaCl are in 10 moles of NaCl.
10 moles g = 585 g
1 mole

62. Molar Mass- Conversions
Find how many grams of MgO are in 50 moles of MgO.

63. Opener 1// What is the formula for calcium acetate?
How many oxygen atoms does it contain?
Name the following compounds: S4O Na2O Mg3(PO4)2
What is the molar mass of each compound above?

64. Moles Mole Road Mass in Grams Atoms or molecules 6.02 x 1023
Multiply by
6.02 x 1023
Multiply by MM
Divide by MM
Divide by
6.02 x 1023
Moles

65. Molar Mass- Conversions
Find how many grams of MgO are in 4.68 moles of MgO.

66. Molar Mass- Conversions
Find how many moles of CaCl2 are in 350 grams of CaCl2

67. Quiz Review/Study Guide Questions
Review misconceptions on Quiz
Study Guide Questions

68. Organic Compound Naming
See other PP

69. Opener 1//16
Name, molar mass (GFM), % composition
K3N
C3F7

70. Name, molar mass (GFM), % composition
disilicon pentoxide
sodium carbonate

71. Name, molar mass (GFM), % composition
Magnesium Iodide
Fe2(SO4)3

72. UNIT TEST
What you can use for test: Periodic tables, Survival Sheet and a calculator
Please do not write on the test!!!
TEST ID