1. Atoms, Molecules, and Ions Nomenclature
Chemistry review
Atoms, Molecules, and Ions
Nomenclature

2. Modern View The atom is mostly empty space. Two regions
Nucleus- protons and neutrons.
Electron cloud- region where you might find an electron.

3. Sub-atomic Particles
Z - atomic number = number of protons determines type of atom.
A - mass number = number of protons + neutrons.
Number of protons = number of electrons if neutral.

4. Symbols A X Z 23 Na 11

5. Chemical Bonds
The forces that hold atoms together in molecules and polyatomic ions.
Covalent bonding - sharing electrons.
Chemical formula- the number and type of atoms in a molecule.
C2H6 - 2 carbon atoms, 6 hydrogen atoms,
Structural formula shows the connections, but not necessarily the shape.

6. H H H C C H H H
There are also other model that attempt to show three dimensional shape.

7. Ions Atoms or groups of atoms with a charge.
Cations- positive ions - get by losing electrons(s).
Anions- negative ions - get by gaining electron(s).
Ionic bonding- held together by the opposite charges.
Ionic solids are called salts.

8. Polyatomic Ions Groups of atoms that have a charge.
Yes, you have to memorize them.
List in appendix C, page 801

9. Periodic Table

10. Metals
Conductors
Lose electrons
Malleable and ductile

11. Nonmetals
Brittle
Gain electrons
Covalent bonds

12. Semi-metals or Metalloids

13. Alkali Metals

14. Alkaline Earth Metals

15. Halogens

16. Transition metals

17. Noble Gases

18. Inner Transition Metals

19. +1 +2 -3 -2 -1

20. Writing Formulas for compounds
Two sets of rules
Ionic Covalent
If first element is a metal If the first element or a polyatomic ion is a non-metal

21. Ionic compounds
If the cation is monoatomic- Name the metal (cation) just write the name. sodium ion, Na+
If the cation is polyatomic- name it. Ammonium, NH4+
If the anion is monoatomic- name it but change the ending to –ide. Chloride, Cl-
If the anion is poly atomic- just name it Sulfate SO42-

22. Classical vs Stock methods
Ionic compounds
What to do when the metal has more than one valence number?
Classical vs Stock methods
Classical uses original language to name metal
Higher valence # uses “ic” suffix
Eg: iron +3 is ferric
Lower valence # uses “ous” suffix
Eg: iron +2 is ferrous

23. Ionic compounds
Stock method uses roman numerals to represent the valence # of the metal.
Eg: iron (III) chloride or iron (II) chloride

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

25. More Naming

26. Ionic Compounds
Name these
CaS
K2S
AlPO4
K2SO4
FeS
CoI3

27. Ionic Compounds Name these CaS K2S AlPO4 K2SO4 FeS CoI3
calcium sulfide
potassium sulfide
aluminum phosphate
potassium sulfate
ferrous sulfide or iron (II) sulfide
cobalt (III) iodide

28. Ionic Compounds
Fe2(C2O4)3
MgO
MnO
KMnO4
NH4NO3
CuCl2
Cr2O3

29. Ionic Compounds Fe2(C2O4)3 MgO MnO KMnO4 NH4NO3 CuCl2 Cr2O3
iron (III) oxalate or ferric oxalate
magnesium oxide
manganese (II) oxide
potassium permanganate
ammonium nitrate
copper (II) chloride or cupric chloride
chromium (III) oxide

30. Ionic Compounds
KClO4
NaClO3
YBO3
Cr(ClO)6

31. Ionic Compounds KClO4 NaClO3 YBO3 Cr(ClO)6 potassium perchlorate
sodium chlorate
yttrium borate
chromium (VI) hypochlorite

32. Ionic Compounds sodium sulfite calcium iodide lead (II) oxide
lead (IV) oxide
mercury (I) sulfide
barium chromate
aluminum hydrogen sulfate
cerium (IV) nitrite

33. Ionic Compounds sodium sulfite calcium iodide lead (II) oxide
lead (IV) oxide
mercury (I) sulfide
barium chromate
aluminum hydrogen sulfate
cerium (IV) nitrite
Na2SO3
CaI2
PbO
PbO2
Hg2S
BaCrO4
Al(HSO4)3
Ce(NO2)4

34. Covalent compounds The name tells you how to write the formula
sulfur dioxide
difluorine monoxide
nitrogen trichloride
diphosphorus pentoxide

35. Covalent compounds The name tells you how to write the formula
sulfur dioxide
difluorine monoxide
nitrogen trichloride
diphosphorus pentoxide
SO2
F2 O
NCl3
P2 O5

36. Naming Covalent Compounds
CCl4
N2O4
XeF6
N4O4
P2O10

37. Naming Covalent Compounds
CCl4
N2O4
XeF6
N4O4
P2O10
carbon dioxide
carbon monoxide
carbon tetrachloride
dinitrogen tetroxide
xenon hexafluoride
tetranitrogen tetroxide
diphosphorus decoxide

38. More Names and formulas

39. Acids Substances that produce H+ ions when dissolved in water.
All acids begin with H.
Two types of acids:
Oxyacids Non-oxyacids

40. Naming oxyacids If the formula has oxygen in it
write the name of the anion, but change
ate to -ic acid
ite to -ous acid
Eg: sulfate becomes sulfuric acid (H2SO4aq) and sulfite becomes sulfurous acid (H2SO3aq)
H2CrO4 (aq)
HMnO4 (aq)
HNO2 (aq)

41. Naming oxyacids If the formula has oxygen in it
write the name of the anion, but change
ate to -ic acid
ite to -ous acid
Eg: sulfate becomes sulfuric acid (H2SO4aq) and sulfite becomes sulfurous acid (H2SO3aq)
H2CrO4 (aq)
HMnO4 (aq)
HNO2 (aq)
chromic acid
permanganic acid
nitrous acid

42. Naming non-oxyacids If the acid doesn’t have oxygen
add the prefix hydro-
change the suffix -ide to -ic acid
HCl (aq)
H2S (aq)
HCN (aq)

43. Naming non-oxyacids If the acid doesn’t have oxygen
add the prefix hydro-
change the suffix -ide to -ic acid
HCl (aq)
H2S (aq)
HCN (aq)
hydrochloric acid
hydrosulfuric acid
hydrocyanic acid

44. How to write formulas for acids
Backwards from names.
If it has hydro- in the name it has no oxygen
Anion ends in -ide
No hydro, anion ends in -ate or -ite
Write anion and add enough H to balance the charges.

45. Formulas for acids hydrofluoric acid dichromic acid carbonic acid
hydrophosphoric acid
hypofluorous acid
perchloric acid
phosphorous acid
HF (aq)
H2Cr2 O7 (aq)
H2CO3 (aq)
H3P (aq)
HFO (aq)
HClO4 (aq)
H3PO3 (aq)

46. Formulas for acids hydrofluoric acid dichromic acid carbonic acid
hydrophosphoric acid
hypofluorous acid
perchloric acid
phosphorous acid

47. Hydrates Some salts trap water crystals when they form crystals.
These are hydrates.
Both the name and the formula needs to indicate how many water molecules are trapped.
In the name we add the word hydrate with a prefix that tells us how many water molecules.

48. Hydrates
In the formula you put a dot and then write the number of molecules.
calcium chloride dihydrate = CaCl2·2H2O
chromium (III) nitrate hexahydrate = Cr(NO3)3· 6H2O