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 S4Cl2 SF6 Subscripts (2). In the formulas the less electronegative atom is written first
Compounds Covalent (Molecular) Ionic I-Cl NaCl
Na2O N2O
NaCl CO CO2 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.
Nomenclature of Binary Compounds
Nomenclature of Binary Compounds Covalent (molecular) compounds
Root Root Root Root O oxygen ox Br Bromine Cl chlorine chlor As Arsenic N nitrogen nitr Te Tellurium I iodine Se selenium P phosphorus F fluorine S sulfur C carbon
Numerical Prefixes 1 mono 8 octa 2 di 9 nona 3 tri 10 deca 4 tetra 11 undeca 5 penta 12 dodeca 6 hexa 13 trideca 7 hepta 14 tetradeca
As2S3 Na2S Mo2Cl8 (name as a covalent compound) Al4C3 Cl2O7 B3N3 ICl RbCl MgI2 SF6 KF
Name the following binary compounds 1. NaCl 13. SO3 2. ICl 14. P2S5 3. Al2O3 4. C2O3 15. SF6 5. Al4C3 16. XeF4 6. CS2 7. CO 8. AlP 17. S4Cl2 9. SO3 10. NI3 11. Ba3N2 12. OF2
Name the following binary compounds (name the following metal - containing compounds as covalent compounds) 18. CrO3 19. TiCl4 20. W2Cl8 21. PbO2
The Formation and Nomenclature of Monatomic Ions
Representative Elements that may form only 1 cation
1A 4A 5A 6A 7A H C N O F Si P S Cl As Se Br Te I 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.
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.
Nomenclature of Monatomic Anions Root + ide identifies the element identifies the ion as a
Representative Elements that may form only 1 cation
Non metals and metalloids Forming Monatomic Anions
The reaction of the elements Li and F
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.
Following the outline given on the previous slide determine the formula of the following combinations of elements Following the outline given on the previous slide determine the formula of the following combinations of elements Al and O Ba and Se
Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements)
Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements)
Metals that form more than 1 cation: Transition and Post-Transition Metals Transition Metals Post Transition Metals 3B 4B 5B 6B 7B 8B 1B 2B 3A 4B 5A
Metals that form more than 1 cation: Transiton Metals 3B 4B 5B 6B 7B 8B 1B 2B 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)
Metals that form more than 1 cation: Transiton Metals 3B 4B 5B 6B 7B 8B 1B 2B 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)
I. 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
II. 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
Fe iron ferrum Cu copper cuprum Sn tin stannum Pb lead plumbum Ag silver argentenum Au gold aurum
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