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Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
Covalent bonds ch 9 2
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Covalent bonds ch 9 2

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  • 1. 9.2
  • 2.  Binary molecular compound  Covalently bonded compound containing only two different elements  Composed of 2 different nonmetals  No ions or metals
  • 3. 1. Name the 1st element first using complete name.2. Name the 2nd element using the root of the element and adding the suffix –ide3. Prefixes are used to indicate the number of atoms that are present in the compound 1. Exception: first element in formula never uses mono-4. Hydrogen bonded to 7A halogens (drop mono)
  • 4. Nonmetal roots H - hyd1 - mon(o)  C - carb 2 - di  N - nitr 3 - tri  P - phosph 4 - tetr(a)  As - arsen 5 - pent(a)  O - ox 6 - hex(a)  S - sulf 7 - hept(a)  Se - selen 8 - oct(a)  F - fluor 9 - non(a)  Cl - chlor 10 - dec(a)  Br - brom  I - iod
  • 5. 1. CO 1. Carbon monoxide2. P2O5 2. Diphosphorus pentoxide3. CCl4 3. Carbon tetrachloride4. As2O3 4. Diarsenic trioxide5. NF3 5. Nitrogen trifluoride6. SO2 6. Sulfur dioxide
  • 6. 1. H2O Di hydrogen monoxide2. NH3 Nitrogen trihydride3. N2H4 Dinitrogen tetrahydride4. N 2O Dinitrogen monoxide5. NO Nitrogen monoxide 1. Water 2. Ammonia 3. Hydrazine 4. Nitrous oxide 5. Nitric oxide
  • 7.  Molecules can be put in aqueous solution (water) and they make acids Compound classified as an ACID if it releases H+ ions when put in water solution Only name acids if molecule is put in water!!! Two types  Binary Acids  Oxyacids
  • 8.  Hydrogen & one other element Sometimes there are more than 2 elements To name hydrogen, use prefix Hydro- Second element use Root (or form of root) followed by suffix –ic  If there are more than 2 elements involved, use the root of the polyatomic ion that acid contains Add the word acid to the end Example: HCl  Hydrochloric acid Example: HCN  Hydrocyanic acid
  • 9.  Acidsthat contain OXYANION What is an oxyanion?  Polyatomic ion that contains oxygen First:Determine anion present Use a form of the root of the anion Add suffix  Anion suffix –ate….oxyacid suffix= -ic  Anion suffix –ite….oxyacid suffix= -ous Add the word acid Example:HNO3  Oxyanion: nitrate NO3-  Oxyacid name: nitric acid Example:HNO2  Oxyanion: nitrite NO2-  Oxyacid: nitrous acid
  • 10. Acids Binary Oxyacid Use root of ion Use Hydro Does NOT use ate ic acidRoot – ic acid hydro ite  ous acid
  • 11. 1. HI 1. Hydroiodic acid2. HClO3 2. Chloric acid3. H2SO4 3. Sulfuric acid4. H2S 4. Hydrosulfuric acid5. HClO2 5. Chlorous acid
  • 12.  Write the symbols for the elements in the order mentioned in the name. Write subscripts indicated by the prefixes. If the first part of the name has no prefix, assume it is mono. Prefixes tell you SUBSCRIPTS for each element Example  Carbon tetrachloride CCl4
  • 13. 1 mono 2 di nitrogen dioxide NO2 3 tri 4 tetra 5 penta diphosphorus pentoxide P2O5 6 hexa 7 hepta 8 octa xenon tetrafluoride XeF4 9 nona 10 deca sulfur hexafluoride SF6* Second element in ‘ide’ from* Drop –a & -o before ‘oxide’
  • 14. Formula of Name of Formula of Name of Pollutant Molecule Acid Acid Many common air pollutants form acids when SO2 dissolved in a water solution Complete the Carbonic following table acid NO2 HNO3

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