chapter 6.1 atoms & their interactions units of matter ….. l atoms l elements l compounds...
TRANSCRIPT
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Chapter 6.1
Atoms & their interactions
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Units of Matter …..
Atoms
Elements
Compounds & Molecules
C, O, H, N, S
CO2, H20, C6H1206
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Common Molecules
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Atoms of the same Element:
Same number of protons, electrons & neutrons
Same atomic structure
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Atoms
Germanium Ge Tunneling
Microscope Computer
enhancement
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Atomic Models
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Rules for Bohr model:
Atomic number = # electrons = # protons
1st shell = 2 paired electrons
2nd shell up to 83rd shell up to 8
(-, outer shell) (+, nucleus)
Nucleus
+2P,N
ee
He
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Ions
Atoms that Loose orGain Electrons
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Ionic Bonds =
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Covalent BONDS
Share electrons
Stronger than ionic that
Donate or Gain electrons
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pH? pH? pH scale?affect us?pH balanced shampoo
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WATER:H2 O
How many atoms??Types of bonds??Strong or Weak? Break
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Water molecule…...
Covalent bonds Polar + charge at O
end - charge at H
end Pull apart ions
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H2O-->H+ & OH-
H+ = Hydrogen ionin excess= acidOH- = Hydroxide ionin excess= base
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How frequently do they break apart?
(10)-7 concentration of H+
.00000011 for every 10 million water molecules!
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pH=measurement
-log of the {H+}
for water= (10)-7 pH = 7
pH 2 pH4 pH8 pH10 pH12
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?H20 a neutral pH
#hydrogen ions = #hydroxide ions.
H+ = (10)-7OH- = (10)-7
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?Makes an acid
Increase the relative amount of H+
adding a weak acid= {H+}= 10-5 ? pH pH = 5
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?Base
{H+} lower than 10-7 tips the balance of H+ to
OH- = more OH- than H+. = base with pH 8 =alkaline
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?strong or weak
The more acid the __________the pH number.
(lower) (1-5) The more alkaline, the
________________ the pH (higher, above 7) (8-12)
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Examples
Lemons Vinegar Aspirin Battery acid“sour”
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Bases
Ammonia Lye Sodium
hydroxide Baking soda“slippery”
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? living systems & pH challenges?
? is low body pH ?extreme pH’s & cells ?spills of strong acids or
bases on your hand?
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?BUFFERS
?buffered asprin buffers “take up” excess H+
or OH- ions maintain constant pH blood Homeostasis: CO2 + H2O = H2CO3