COVALENT COMPOUNDS

Ionic vs. Covalent Compound Ionic Compounds Between a metal and a non-metal Transfers electrons Covalent Compounds Between a non-metal and a non-metal Electrons are shared

Covalent Compound Nitrogen = non-metal Oxygen = non-metal

Covalent Compounds Hydrogen = non-metal Carbon = non-metal Look at the first element listed in the compound… notice that it is a NON-METAL If both elements are non-metals, then it is a covalent bond. This means that rather than transferring electrons (like ionic compounds do), the two elements share their valence electrons

Naming Covalent Compounds Prefixes are used to indicate how many of each atom are in the compound. Prefixes are written in front of each element Prefixes Prefixes 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca

CO2 Naming Example Oxygen = non-metal Carbon = non-metal Have 2 oxygens CO2 2 = di Name (in the order they appear) Carbon dioxide Change to “ide”

P4O10 Naming Example Oxygen = non-metal Phosphorus = non-metal Have 10 oxygens P4O10 10 = deca Have 4 phosphorus’ 4 = tetra Name (in the order they appear) Tetraphosphorus decaoxide Change to “ide”

Formula Example CS2 Carbon disulfide C  only have 1 S  have 2 because it is “di” Carbon disulfide Formula (put them together in the order) CS2

Formula Example C2Cl4 Dicarbon tetrachloride C  have 2 (di) Cl  have 4 (tetra) Dicarbon tetrachloride Formula (put them together in the order) C2Cl4

Diatomics These are a type of covalent bond between two atoms of the same element Example: two chlorine atoms bond together to form Cl2 “Gens” rule Diatomics go by the GEN rule HydroGEN, oxyGEN, nitroGEN, haloGEN O2, N2, F2, Br2, Cl2, I2, H2