1. Chemical Names & Formulas
Chapter 7

2. The Periodic Law
Dimitri Mendeleev was the first scientist to publish an organized periodic table of the known elements.
He placed the elements in order of increasing atomic mass and noticed chemical similarities between them at regular intervals.

3. The Periodic Law Mendeleev understood the ‘Periodic Law’ which states:
When arranged in order by increasing atomic #, elements with similar properties appear at regular intervals.

4. The Periodic Law
Mendeleev even predicted the existence and properties of 3 undiscovered elements at the time, using empty spaces to represent them in his table.

5. Periodic Groups
Elements with similar properties appear in “Groups” (vertical columns) on the periodic table.
They are similar because they all have the same number of Valence (outer shell) electrons, which governs their chemical behavior.

6. Valence Electrons

8. The Octet Rule

9. Metals & Nonmetals
Metals
Semi-Metals
Non-Metals

10. Ions
When an atom gains an electron, it becomes negatively charged (more e- than p+ ) and is called an anion.
When an atom loses an electron, it becomes positively charged (less e- than p+) and is called a cation.

11. She’s unhappy and negative.
Ions
Here is a simple way to remember which is the cation and which the anion:
This is Ann Ion.
This is a cat-ion.
She’s unhappy and negative.
He’s “paw-sitive”

12. Periodic Groups Alkali Metals Alkaline Earth Metals Transition Metals
Halogens
Noble Gases

13. Periodic Groups

14. Periodic Groups
Boron forms -3?

15. Periodic Groups

16. Periodic Groups

17. Periodic Groups
Polonium forms +2, +4 ions?

18. Periodic Groups

19. Periodic Groups Group 18: Noble Gases Have 8 valence electrons (s2 p6)
Unreactive
Never form Ions
All are nonmetals

20. Periodic Groups Group 18: Noble Gases Have 8 valence electrons (s2 p6)
Unreactive
Never form Ions
All are nonmetals

21. Charges on Ions
For ‘main group elements’ (grps 1, 2, 13-18), you can predict the charge an ion will form based on its location on the periodic table.

22. Charges on Ions
Metals
Semi-Metals
Non-Metals +1 +2 +3 -3 -2 -1

23. Naming Monatomic Ions
Monatomic Ions are ions formed from a single atom.
To name Monatomic Cations (grp 1, 2, 13) you just give the name of the atom:
Na+ is Sodium ion
Mg2+ is Magnesium ion
Ag+ is Silver ion
Al3+ is Aluminum ion 1 2 3

24. Naming Monatomic Ions ↓
To name monatomic Anions (grp 15-17) you change their ending to –ide
Oxygen becomes Oxide ion
Fluorine becomes Fluoride ion
Nitrogen becomes Nitride ion
Chlorine becomes Chloride ion 17 16 ↓ 15 ↓

25. Practice

26. Practice Write the formulas of the following Monatomic Ions:
Sulfide Ion
Iodide Ion
Phosphide Ion
Strontium Ion

27. Writing Formulas for Binary Ionic Compounds
Binary Compounds are composed of two elements - Metal + Nonmetal
Ex: NaCl
(+) charges and (-) charges must equal

28. Writing Formulas for Binary Ionic Compounds

29. Naming Binary Ionic Compounds
Rules for Main Group Metals:
Name the Cation (from groups 1, 2, or 13)
Name the Anion (from groups 15, 16, 0r 17), changing the ending to –ide.
Name of Cation
Name of Anion
aluminum
oxide

30. Practice

31. Practice Write formulas for the following Ionic Compounds:
Potassium Iodide
Magnesium Chloride
Sodium Sulfide
Aluminum Sulfide
Aluminum Nitride
Calcium Bromide

32. Naming Binary Ionic Compounds Containing Transition Metals
Transition Metals are those in Groups 3-12 of the periodic table.
They REQUIRE Roman Numerals because they can have more than one possible charge:
Other than that same rules apply
Al, Zn, Cd, and Ag ?

33. Naming Binary Ionic Compounds Containing Transition Medals
Rules for Transition Metals:
Name the Cation (from groups 1, 2, or 13)
Place metal’s charge in parentheses using Roman #’s
Name the Anion (from groups 3-12), changing the ending to –ide.
Al, Zn, Cd, and Ag ?
Roman # indicating charge
Name of Cation
Name of Anion +
Copper (II)
Chloride

34. Practice

35. Practice Write formulas for the following Ionic Compounds:
Copper (II) Bromide
Iron (II) Oxide
Lead (II) Chloride
Mercury (II) Sulfide
Tin (II) Flouride
Iron (III) Oxide

36. Polyatomic Ions
Polyatomic Ions are tightly bound groups of ions that behave as a unit.
Poly = more
Most polyatomic ions end in –ate.
The ending –ite means one less oxygen is present than in –ate.
Example: Nitrate versus Nitrite:
NO NO2-
NOTE: Only the number of O’s changed, NOT the charge.

37. Polyatomic Ions
The Prefix Hypo means two less oxygen’s are present than in –ate.
The Prefix Per- means one extra oxygen is present than in –ate.
Examples:
Perchlorate ClO4-
Chlorate ClO3-
Chlorite ClO2-
HypoChlorite ClO-

38. Polyatomic Ions
When more than one Polyatomic is present you surround it with ()
Lead (IV) Phosphate
Pb+4 PO4-3
Pb3(PO4)4
NOTE: The subscripts on Polyatomic ions NEVER change.

39. Practice

40. Practice Write formulas for the following Ionic Compounds:
Lithium Nitrate
Copper (II) Sulfate
Sodium Carbonate
Calcium Nitrite
Silver Nitrate
Aluminum Sulfate

41. Naming Binary Molecular Compounds
Molecular Compounds are composed of two or more Nonmetals SHARING electrons in bond.
Nonmetal + Nonmetal
These elements are attached
Prefixes are used to specify the number of atoms present

42. Naming Binary Molecular Compounds
Rules:
Element with the smaller Group # or larger Period # is given first.
Prefix is used on first element only if more than 1 atom is present.
Prefix is added to second element followed by –ide ending.
The o or a after a prefix is dropped when followed by a vowel.

43. Naming Binary Molecular Compounds
Ex:
Monoxide not Mono-oxide
Pentoxide not Penta-oxide
Al, Zn, Cd, and Ag ?
Name of first element
Name of second element + -ide
Prefix- if more than 1
Prefix +
Tetraphosphorus
Decoxide

44. Naming Binary Molecular Compounds
Prefixes:
Number
Prefix 1
Mono- 2
Di- 3
Tri- 4
Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8
Octa- 9
Nona- 10
Deca-

45. Practice Name the following Molecular Compounds: N2O NO2 Cl2O7 CBr4
BaCl2

46. Practice Write formulas for the following Molecular Compounds:
Carbon Tetraiodide
Phosphorus Trichloride
Dinitrogen Trioxide
Oxygen Diflouride
Dinitrogen tetroxide
Phosporus Pentabromide
Trisilicon Tetranitride

47. Naming Binary Acids

48. Naming Binary Acids Rules:
If the anion attached to Hydrogen ends in –ide, add the prefix Hydro- and change –ide to –ic Acid
HCl= Hydrochloric Acid
H2S= Hydrosulfuric Acid

49. Naming Binary Acids Rules Continued:
If the anion has oxygen in it, then it ends in -ate or –ite
Change the ending -ate to -ic acid
HNO3 = Nitric acid
Change the ending -ite to -ous acid
HNO2 = Nitrous acid
Anions that end in –ate or –ite have oxygen in them

50. Naming Binary Acids I –ate something –icky I m-ite be naus-ous
Here’s an easy way to remember the endings:
I –ate something –icky
I m-ite be naus-ous

51. Practice Name the following Acids: H2SO4 H2CO3 H3PO3 HBr HF
Sulfuric Acid
Carbonic Acid
Phosphorous Acid
Hydrobromic Acid
Hydroflouric Acid

52. Practice Write formulas for the following Acids: Sulfurous Acid
Chloric Acid
Chlorous Acid
Hydroiodic Acid
Phosphoric Acid
H2SO3
HClO3
HClO2 HI
H3PO4