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2. Synthesis  two or more elements or compounds may combine to form a more complex compound.  Basic form: A + X → AX  EX. 2Mg (s) + O 2(g) → 2MgO (s) Decomposition  A single compound breaks down into its component parts or simpler compounds.  Basic form: AX → A + X  Ex. CaCO 3(s) → CaO (s) + CO 2(g)

3.  Single Replacement:  a more active element takes the place of another element in a compound and sets the less active one free  Basic form: A + BX → AX + B  EX. Fe (s) + CuSO 4(aq) → FeSO 4(aq) + Cu (s)  Double Replacement:  parts of two compounds switch places to form two new compounds. Two reactants yield two new products  EX. AB + XY ---> AY + XB  EX. NaCl + H 2 SO 4 ---> Na 2 SO 4 + HCl

4.  Acids are chemicals in which the positive ion is a hydrogen atom.  HCl or H 2 SO 4  When mixed with water they produce a free hydrogen ion that combines with a water molecule to produce a hydronium ion (H 3 O)  H +1 + H 2 O  H 3 O +1  An acid is a substance that releases hydrogen ions when it breaks apart in water.

5.  Taste sour  React with metals to produce hydrogen  2HCl + 2Na  2NaCl + H 2  Conduct electricity.

6.  Bases are substances in which the negative ion is an ion called hydroxide (OH) -1  For example; NaOH, or KOH  used to make soap, household cleaners, fertilizers, and explosives.

7.  Taste bitter  Feel slippery  Conduct electricity  Sometimes Caustic. That is they eat away at certain substances and they are irritating or damaging to skin.

8.  A salt is a compound formed from the positive metal ions of a base and a negative nonmetal ion of an acid.  NaCl, K 2 SO 4  Are the product of a reaction between an acid and a base, along with water.

9.  They form crystals when in solid form  They usually have a higher hardness because of their ionic bonding.  An acid plus a base yields a salt and water. HCl + NaOH  NaCl + HOH HCl + NaOH  NaCl + H 2 O

10.  A reaction between an acid and base.  The products of a neutralization reaction are a salt and water.

11.  The pH scale gives a measure of the concentration of positive hydrogen ions in a solution.  a way of describing the acidic or basic strength of a solution.  the acidity of a solution can be expressed by using the pH scale

12.  the scale ranges from 0 to 14  acids range from 0 to 6, with 0 being the strongest acid  bases range from 8 to 14, with 14 being the strongest base.  pure water, which is neither acid nor base, has a pH level of 7 or is neutral

13.  Indicators are substances that visibly show a change in the nature of a chemical system.  Universal indicator- an acid/base indicator that shows, by color, the pH of a substance.

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