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Acids • any substance that produces H+ when
dissolved in water• 2 types
– Binary – hydrogen and one other element– Oxyacids – contains hydrogen and oxygen
P. 271 - 273.
Naming AcidsBinary 1. Use the prefix hydro for hydrogen2. Use the root of the 2nd element and add -ic3. Write the word acid
HF, HBr, HI, HCl
Note: If a polyatomic ion does not contain oxygen these rules apply. Use the root of the polyatomic.
HCN – hydrocyanic acid
P. 271 - 273.
Naming Acids - continued
• Oxyacids– Depends on the oxyanion (polyatomic ion
containing oxygen)
1. Use the root of the oxyanion
2. Add the suffix
3. Write the word acid
ate = ic ite = ous
P. 271 - 273. Questions – 26-32.
Naming Bases
• An ionic compound that produces hydroxide ions when dissolved in water
• Ca(OH)2 – calcium hydroxide
• NaOH – Sodium hydroxide
• Named like other ionic compounds.
Chemical Reactions• Rearrangement of atoms from one or
more substances to form new substances– Bonds must break and then reform
Indicators of a reaction– Temp– Smell– Color– Bubbles– Solid formation
Collision Theory P. 541-544
1.Reacting substances must collide.
2.Collisions must be in the correct orientation.
3.Reacting substances must collide with sufficient kinetic energy to form the activated complex.
Activated complex – unstable arrangement of atoms that forms momentarily at the peak of the activation energy barrier.
P. 581 Q 13, 14
Law of Conservation of Mass P. 324-326
the amount of matter in a reaction cannot change it must
be conserved
Reactants Products
Mass = Mass
# of atoms = # of atoms
Word vs. Skeleton Equations
Which contains more information?
Hint : Single atom gases are diatomic, Cl2 (g) not Cl (g) BrINClHOF’s
P.324 Q 1 and 2
Balancing Equations (p. 327)
• Write a skeleton equation.• Count the atoms of the reactants and
products.• Add coefficients • Write coefficients in the lowest whole
number ratios.– If fractions are used you must multiply every
group by the number that cancels the fraction
Synthesis/Combination Reactions P. 330
P. 331 Q 13 and 14
O2 (g) + 2 H2 (g) 2H2O (l)Would the formation of water release heat(exothermic) or absorb
heat(endothermic)? Use the bond enthalpy chart.
Decomposition Reactions P. 332
P. 332 Q 15 and 16
2HCl (g) H2 (g) + Cl2 (g) Would the formation of hydrogen gas and chlorine gas release heat
(exothermic) or absorb heat (endothermic)? Use the bond enthalpy chart.
Combustion Reactions P. 336
• Oxygen reacts with a substance and releases heat and light
P. 336 Q 20 and 21 P. 339 Q 22-27
Would this reaction release heat or absorb heat? Use the enthalpy chart.
When will reactions take place?
• The more reactive atom will replace the least reactive one.
P. 334 Q 17
Acids and Metals
– React with metals to produce H2 (g)
– 2HCl (aq) + 2Na (s) 2NaCl (aq) + H2 (g)
– React with metal carbonates to produce CO2
NaHCO3 (aq) + HC2H3O2 (aq) H2O (l) + CO2 (g) + NaC2H3O2 (aq)
Double Replacement Reaction P. 334
Precipitate
Precipitates that are formed are either a solid, gas or water. Water forms when an acid (Contains H+ ion) and a base(OH-
ion) react with each other
Reactions that form precipitates in aqueous solutions.
Complete ionic reaction – how it actually exists
Reactions in Aqueous Solutions P. 342
• Most reactions are water based• Aqueous solutions consist of separate ions
2NaOH(aq) + CuCl2(aq) Cu(OH)2(s) + 2NaCl(aq)
Write the complete ionic equation: