1. The Nomenclature of Binary Compounds

2. Formula of Binary Compounds (Compounds composed of two elements)
(1). Shows the number of atoms of each type that are found in the compound. These numbers are indicated by subscripts
Al2O3 NaCl S4Cl SF6
Subscripts
(2). In the formulas the less electronegative atom is written first

3. Compounds Covalent (Molecular) Ionic I-Cl NaCl Cl- Cl- Cl- Cl- Na+ Na+

4. Na2O N2O NO
NO2
N2O3
N2O5

5. NaCl CO CO2
Be able to summerize the nomenclature of binary ionic and binary covalent ( i.e. molecular) compounds contrasting differences in the way that the two classes of compounds are named.

6. Nomenclature of Binary Compounds
ionic compounds
(typically compounds of metallic and non-metallic elements)
Name the Name the
less electronegative element more electronegative element
Name of the
Element
Root + ide
Prefixes like di, or tri (indicating the number of atoms) are never used when naming ionic compounds

7. Nomenclature of Binary Compounds
Covalent (molecular) compounds
(typically compounds of non-metallic elements)
Name the Name the
less electronegative element more electronegative element
Name of the
Element
Prefix+
Root + ide
Prefix+
prefix: used to indicate the number of less electronegative atoms ( if more than one) and is always used to indicate the number of more electronegative atoms

8. Root Root O oxygen ox Br Bromine Cl chlorine chlor As Arsenic
N nitrogen nitr Te Tellurium
H hydrogen hydr
I iodine
Se selenium
P phosphorus
F fluorine
S sulfur
C carbon
Brom
Arsen
tellur
Iod
Selen
Phosph
fluor
sulf
carb

9. Numerical Prefixes 1 mono 8 octa 2 di 9 nona 3 tri 10 deca
4 tetra undeca
5 penta dodeca
6 hexa trideca
7 hepta tetradeca

10. Name the following binary compounds
As2S3
Na2S
Mo2Cl8 (name as a covalent compound)
Al4C3
Cl2O7
B3N3
ICl
RbCl
MgI2
SF6 KF
diarsenic trisulfide
Sodium sulfide
dimolydenum octachloride
Aluminum carbide
dichlorine heptoxide
Triboron trinitride
Iodine monochloride
rubidium chloride
magnesium iodide
Sulfur hexafluoride
potassium fluoride

11. Name the following binary compounds
1. NaCl SO3
2. ICl P2S5
3. Al2O3
4. C2O SF6
5. Al4C XeF4
6. CS2
7. CO
8. AlP S4Cl2
9. SO3
10. NI3
11. Ba3N2
12. OF2
Sulfur trioxide
Sodium chloride
Iodine monochloride
diphosphorus pentasulfide
Aluminum oxide
Dicarbon trioxide
Sulfur hexafluoride
Xenon tetrafluoride
Aluminum carbide
Carbon disulfide
Carbon monoxide
tetrasulfur dichloride
Aluminum phosphide
Sulfur trioxide
Nitrogen triiodide
Barium nitride
Oxygen difluoride

12. Name the following binary compounds
(name the following metal -
containing compounds as
covalent compounds)
18. CrO3
19. TiCl4
20. W2Cl8
21. PbO2
Chromium trioxide
Titanium tetrachloride
ditungsten octachloride
lead dioxide

13. The Formation and Nomenclature of Monatomic Ions

14. Representative Elements that may form only 1 cation1+ H
Named as: Element name+ ion 2+ 1+ Li Be 3+ Al 2+ 1+ Na Mg
(1). lose all electrons from the valence shell 2+ 1+ K Ca 1+
(2). form a cation, Mn+; where n is the number of electrons lost( designated by the Group Nb.) 2+ Rb Sr 1+ 2+ Cs Ba

15. Non metals and metalloids Forming Monatomic Anions
1A 4A 5A 6A 7A H
C N O F
Si P S Cl
As Se Br
Te I
These elements gain one or more electrons into the outer shell forming an anion, An-
The charge, n-, of the anion is the number of electrons gained
The nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb.

16. Non metals and metalloids Forming Monatomic Anions
1A 4A 5A 6A 7A
H1-
C4- N3- O2- F1-
Si4- P3- S2- Cl1-
As3- Se2- Br1-
Te2- I1-
These elements gain one or more electrons into the outer shell forming an anion, An-
The charge, n-, of the anion is the number of electrons gained
The nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb.

17. Nomenclature of Monatomic Anions
Root + ide
identifies the element identifies the
ion as a
monatomic anion

18. Representative Elements that may form only 1 cation1+ H
Named as: Element name+ ion 2+ 1+ Li Be 3+ Al 2+ 1+ Na Mg
(1). lose all electrons from the valence shell 2+ 1+ K Ca 1+
(2). form a cation, Mn+; where n is the number of electrons lost( designated by the Group Nb.) 2+ Rb Sr 1+ 2+ Cs Ba

19. Non metals and metalloids Forming Monatomic Anions
1A 4A 5A 6A 7A H
C N O F
Si P S Cl
As Se Br
Te I
H1-
C4- N3- O2- F1-
Si4- P3- S2- Cl1-
As3- Se2- Br1-
Te2- I1-
Names:
Root + ide
These elements gain one or more electrons into the outer shell forming an anion, An-
The charge, n-, of the anion is the number of electrons gained
The nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb.

20. The reaction of the elements Li and F
Li F 9+ 3+
Li F1-

21. Determine the stoichiometry of the formula unit for the compound.
Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements)
Determine the identity of the cation and the anion that the metal and non-metal would form.
Determine the stoichiometry of the
formula unit for the compound.

22. Following the outline given on the previous slide determine the formula of the following combinations of elements
Al and O
Ba and Se

23. Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements)
Al and O
Determine the identity of the cation and the anion that the metal and non-metal would form.
Al3+ O2-
Determine the stoichiometry of the formula unit for the compound.
Al O2-
Al2O3 2 3

24. Ba and Se Ba2+ Se2- Ba2Se2 Ba2+ O2- BaSe
Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements)
Ba and Se
Determine the identity of the cation and the anion that the metal and non-metal would form.
Ba2+ Se2-
Determine the stoichiometry of the formula unit for the compound.
Ba2Se2
Ba O2- 2 2
BaSe

25. Ca2+ Cl1- 1. Ca and Cl 2. C and Al 3. Na and F 4. Ba and O Al3+ C4-
Give formula for, and name, the binary ionic compounds that would be formed through the reaction of the following pairs of elements:
Formula
Ions Formed
CaCl2
1. Ca and Cl
Ca2+ Cl1-
Calcium chloride
2. C and Al
Al C4-
Al4C3
C Al3+
Aluminum carbide
3. Na and F
Na1+ F1-
NaF
Sodium fluoride
4. Ba and O
Ba O2-
BaO
Barium oxide

26. 5. N and Mg 6. Li and Se 7. Ga and As Mg3N2 Mg2+ N3- N3- Mg2- Li2Se
Give formula for, and name, the binary ionic compounds that would be formed through the reaction of the following pairs of elements:
Formula
Ions Formed
Mg3N2
Mg N3-
N Mg2-
5. N and Mg
6. Li and Se
7. Ga and As
Magnesium nitride
Li2Se
Li Se2-
Lithium selenide
GaAs
Ga As3-
Gallium arsenide

27. Metals that form more than 1 cation: Transition and Post-Transition Metals
Transition Metals Post Transition
Metals
3B 4B 5B 6B 7B 8B B 2B A 4B 5A Sc
Tii V Cr Mn Fe Co Ni Cu Zn Ga Ag Cd In Sn Au Hg Tl Pb Bi

28. Metals that form more than 1 cation: Transiton Metals
3B 4B 5B 6B 7B 8B 1B B
Sc2+ Ti2+ V2+ Cr2+ Mn2+ Fe2+ Co2+ Ni2+ Cu1+ Zn2+
Cation of Lower Charge: Formed by losing Ag1+ Cd2+
all electrons from the outermost electron shell
( 2 e- for all, except for Group 1B Au1+ Hg1+
where 1 e- is lost)

29. Metals that form more than 1 cation: Transiton Metals
3B 4B 5B 6B 7B 8B 1B B
Sc3+ Ti3+ V3+ Cr3+ Mn3+ Fe3+ Co3+ Ni3+ Cu2+ Zn3+
Ag2+ Cd3+
Cation of Higher Charge: Possesses a charge Au2+ Hg2+
1 higher than the cation of lower charge
(ions in red are uncommon)

30. Nomenclature of Transition and Post-Transition Metal Ions
Stock System
Name of Metal (Ionic Charge:Roman Numerals)
Fe2+ iron(II) ion Sn4+ tin(IV) ion
Cu1+ copper(I) ion Cr3+ chromium(III) ion

31. -ic (ion of higher charge) Root + endings
II.
Older Nomenclature
-ic (ion of higher charge)
Root endings
identifies the metal -ous (ion of lower charge)
Fe2+ ferrous ion Sn4+ stannic ion
Cu1+ cuprous ion Cr3+ chromic ion

32. Fe iron ferrum
Cu copper cuprum
Sn tin stannum
Pb lead plumbum
Ag silver argentenum
Au gold aurum

33. Fe2O3 CuCl PbCl4 SnO AgO Name the following compounds:
Iron(III) or ferric oxide
CuCl
Copper (1) or cuprous chloride
PbCl4
Lead (IV) or plumbic chloride
SnO
Tin (II) or stannous oxide
Iron (II) or ferrous sulfide
FeS
AgO
Silver (II) or argentenic oxide