1. Chapter 2 Nomenclature

2. Periodic Table

3. Metals
Conductors
Lose electrons
Malleable and ductile

4. Nonmetals
Brittle
Gain electrons
Covalent bonds

5. Semi-metals or Metalloids

6. Alkali Metals

7. Alkaline Earth Metals

8. Halogens

9. Transition metals

10. Noble Gases

11. Inner Transition Metals

12. +1 +2 -3 -2 -1

13. Periodic Table
Periodic table is organized based on the properties that elements have in common with one another.
Groups: Elements in the same vertical columns are in the same group have similar chemical properties.
Group 1A: Alkali metals: Li, Na, K, Rb, Cs, Fr
Group 2A: Alkaline earth metals: Be, Mg, Ca, Sr, Ba, Ra
Group 7A: Halogens: F, Cl, Br, I, At (astatine)
Group 8A: Noble gases: He, Ne, Ar, Kr, Xe, Rn (radon)

14. Periodic Table
Periods: The horizontal rows of elements in the periodic table are called periods.
First period: horizontal row one contains H and He
Second period: row two contains Li through Ne
Letters in the boxes are the symbols for the elements
Abbreviations are based on the current element names or the original names.
The number above each symbol is the atomic number (number of protons)

15. Periodic Table Most of the elements are metals in the periodic table.
Metals: Conduction of heat and electricity, malleability, ductility, lustrous, form positive ions
Nonmetals: appear in the upper right hand corner of the periodic table except hydrogen. Nonmetals lack the physical properties that characterize the metal, gain electrons in chemical reaction and form negative ions, form covalent bond to each other.

16. Naming Compounds Binary Compounds: Compounds composed of two elements
Binary Ionic Compounds (Type I): contains a positive ion (cation) always written first in the formula and a negative ion (anion)
Rules:
The cation is always named first and the anion second
A monatomic (meaning one atom) cation takes its name from the name of the element
A monatomic anion is named by taking the root of the element name and adding –ide

17. Naming compounds Two types Ionic - metal and non metal or polyatomics.
Covalent- non-metals.

18. Ionic compounds
If the cation is monoatomic- Name the metal (cation) just write the name.
If the cation is polyatomic- name it.
If the anion is monoatomic- name it but change the ending to –ide.
If the anion is poly atomic- just name it.

19. Covalent compounds Two words, with prefixes.
Prefixes tell you how many.
mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
First element whole name with the appropriate prefix, except mono.
Second element, -ide ending with appropriate prefix.

20. Ionic compounds
If the cation is monoatomic- Name the metal (cation) just write the name.
If the cation is polyatomic- name it
If the anion is monoatomic- name it but change the ending to -ide
If the anion is poly atomic- just name it from a table.

21. Ionic Compounds Have to know what ions they form CaS K2S AlPO4 K2SO4
FeS
CoI3

22. Some Polyatomic Ions (Table 2.3)
2.7

23. Naming compounds
Binary Ionic Compounds (Type II): Metals that form more than one type of positive ion. Fe2+ and Fe3+
Transition metals form several positive oxidation states
Charge on the metal ion must be specified
Roman numeral indicates the charge of the cation. Iron (II) chloride and iron (III) chloride
The ion with the higher charge has a name ending in –ic and the one with the lower charge has a name ending in –ous; ferrous chloride and ferric chloride

24. Naming Compounds Ionic Compounds with Polyatomic Ions:
Need to know the names of the polyatomic ions (Table 2.5).
NH4+  ammonium, SO42-  sulfate
Na2SO4 Sodium sulfate
KH2PO4 Potassium dihydrogen phosphate
Fe(NO3)3 Iron(III) nitrate
CsClO4 Cesium perchlorate
NaOCl sodium hypochlorite
Al2(Cr2O7)3 Aluminum dichromate
Sr(CN)2 Strontium cyanide

25. Naming compounds Binary Covalent Compounds (Type III):
Formed between two nonmetals
Rules:
The first element in the formula is named first, using the full element’s name
Second element is name as if it were an anion
Use prefixes to denote the number of atoms present
Never use mono – prefix for naming the first element

26. Molecular compounds nonmetals OR nonmetals + metalloids common names
H2O, NH3, CH4, C60
element further left in periodic table is 1st
element closest to bottom of group is 1st
if more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom
last element ends in ide
2.7

27. P2O5 ==> diphosphorus pentoxide S2Cl4 ==> disulfur tetrachloride
CO ==> carbon monoxide, not monocarbon monoxide
P2O5 ==> diphosphorus pentoxide
S2Cl4 ==> disulfur tetrachloride
NO2 ==> nitrogen dioxide
N2O5 ==> dinitrogen penoxide

28. Chemical Nomenclature
Ionic Compounds
often a metal + nonmetal
anion (nonmetal), add “ide” to element name
BaCl2
barium chloride
K2O
potassium oxide
Mg(OH)2
magnesium hydroxide
KNO3
potassium nitrate
2.7

29. Transition metal ionic compounds
indicate charge on metal with Roman numerals
FeCl2
iron(II) chloride
2 Cl- -2 so Fe is +2
FeCl3
3 Cl- -3 so Fe is +3
iron(III) chloride
Cr2S3
3 S-2 -6 so Cr is +3 (6/2)
chromium(III) sulfide
2.7

30. Molecular Compounds HI hydrogen iodide NF3 nitrogen trifluoride SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
TOXIC!
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
Laughing Gas
2.7

31. An acid can be defined as a substance that yields
hydrogen ions (H+) when dissolved in water.
HCl
Pure substance, hydrogen chloride
Dissolved in water (H+ Cl-), hydrochloric acid
An oxoacid is an acid that contains hydrogen, oxygen, and another element.
HNO3
nitric acid
H2CO3
carbonic acid
H2SO4
sulfuric acid
2.7

32. A base can be defined as a substance that yields
hydroxide ions (OH-) when dissolved in water.
NaOH
sodium hydroxide
KOH
potassium hydroxide
Ba(OH)2
barium hydroxide
2.7

33. Common Cations and Anions

34. Formulas from Names Name Chemical Formula Diphosphorus pentasulfide
P2S5 (two non metals)
Cesium peroxide
Cs2O2 (Cs1+, O22-)
Aluminum fluoride
AlF3 (Al3+, F-1)
Vanadium (v) fluoride
VF5 (V5+, F-1)
Dioxygen difluoride
O2F2 (two non metals)
Gallium oxide
Ga2O3 (Ga3+, O2-)
Ammonium dichromate
(NH4)2Cr2O7 (NH4+, Cr2O72-)
Cupric phosphate
Cu3(PO4)2 (Cu2+, PO43-)

35. Flowchart for Naming Binary Compounds

36. Acids
When dissolved in water produce a solution containing free H+ ions (protons)
An acid is a molecule with one or more H+ ions attached to an anion
If the anion does not contain oxygen, the acid is named with the prefix hydro – and the suffix –ic
HCl Hydrochloric acid
HCN Hydrocyanic acid

37. Acids
If the anion contains oxygen, the acidic name is formed from the root name of the anion with the suffix of –ic or –ous depending on the anion
HNO3 Nitric acid (Nitrate anion)
H2SO4 Sulfuric acid (Sulfate anion)
H3PO4 Phosphoric acid (Phosphate anion)
HC2H3O2 Acetic acid (Acetate anion)
H2SO3 Sulfurous acid (sulfite anion)
HNO2 Nitrous acid (nitrite anion)