Science 10 Ms. Yu. How do we know if something is organic or inorganic in chemistry?

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Presentation transcript:

Science 10 Ms. Yu

How do we know if something is organic or inorganic in chemistry?

ORGANIC  Contains mainly Carbon & Hydrogen (sometimes also N and O)  COVALENT!  E.g. CH 4 (methane)  C 6 H 12 O 6 (glucose) INORGANIC  Contain little or no carbon  Contain carbon but no Hydrogen  IONIC OR COVALENT  E.g. H 2 O, NH 3, CO 2, N 2 O, NaHCO 3

ACID  A solution with more H+ ions than OH- ions Properties:  pH 0-less than 7 (7= neutral)  Contains “H” in formula  Releases H+ ions in solutions  Conducts electric current  Taste sour  Touch: will burn your skin  Reacts with metals to form Hydrogen gas (H 2 )  Can be neutralized by a base

BASE  A solution with more OH- ions than H+ ions Properties:  pH greater than >7  Contains “OH” in formula  Releases OH- ions in solutions  Conducts electric current  Taste bitter  Feels slippery  DOES NOT Reacts with metals  Can be neutralized by an acid

 Acids and Base are Always in SOLUTIONS  dissolved in water  aqueous (aq)

ACID OR BASE?

ACID

BASE

ACID

BASE

ACID

BASE

BASE

 A solution with the same concentration of H+ and OH- ions  pH= 7

 Measures Acidity (Amount of H+ ions)  Normal range is 0-14  pH 7 is basic  Neutral pH=7  pH scale is Logarithmic (change in 1= 10 times more e.g. pH4 solution has 10 times more H+ ions than pH5 solution  Power of Hydrogen

What is the difference in acidity (H+ ion concentration) between pH 4 and 6? 100 times!! Normal Rain pH=6

Acid rain (pH=4)

What is the difference in H+ ion concentration between a pH 1 solution and a pH 4 solution? ppH1  pH4 Difference of 3 So pH1 solution has 1000 times more H+ than pH 4 solution!!

 Chemicals that change colour depending on the pH of solution

SUFFIXOxygen?Name of AcidExample -ateYes 1.Drop Hydrogen and -ate 2.Add –ic acid H 2 CO 3 Hydrogen carbonate  Carbonic acid -iteYes 1.Drop Hydrogen and –ite 2.Add –ous acid H 2 SO 3 Hydrogen sulphite  Sulphurous acid -ideNo 1.Drop Hydrogen and –ide 2.Add Hydro-----ic acid HCl Hydrogen chloride  Hydrochloric acid

 METAL OXIDES dissolves in water to form a BASE e.g. Na 2 O + H 2 O  NaOH BASE CaO + H 2 O  Ca(OH) 2 BASE

 NON-METAL OXIDES dissolve in water to form ACIDS e.g. SO 2 + H 2 O  H 2 SO 3 ACID SO 3 + H 2 O  H 2 SO 4 ACID 2 NO 2 + H 2 O  HNO 2 + HNO 3 ACID CO 2 + H 2 O  H 2 CO 3 ACID

 Taste (you’ve guessed it!) Salty!  Conduct electricity when dissolved in water e.g. NaCl (aq)  Does not react with metals  Does not change colour of indicators  Form from acid & base neutralization

ACID + BASE  SALT + WATER E.g. HCl + NaOH  NaCl + H 2 O Hydrocholric Acid + sodium hydroxide  Sodium chloride + Water E.g. 3H 2 SO 4 + 2Al(OH) 3  Al 2 (SO 4 ) 3 + 6H 2 O