Aula #03 · Aula #03. Dalton’s Atomic Theory 2. 16 X + 8 Y 8 X 2 Y Proportion /relation between...
Transcript of Aula #03 · Aula #03. Dalton’s Atomic Theory 2. 16 X + 8 Y 8 X 2 Y Proportion /relation between...
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Aula #03
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Dalton’s Atomic Theory
2
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8 X2Y16 X 8 Y+Proportion /relation between matter
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atomic radius ~ 100 pm = 1 x 10-10 m
nuclear radius ~ 5 x 10-3 pm = 5 x 10-15 m
Rutherford’s Model of the Atom
What made by Rutherford and his
assistants Geiger and Marsden is perhaps one of the most important experiments of nuclear physics.
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1. atoms positive charge is concentrated in the nucleus
2. proton (p) has opposite (+) charge of electron (-)
3. mass of p is 1840 x mass of e- (1.67 x 10-24 g)
particle velocity ~ 1.4 x 107 m/s(~5% speed of light)
(1908 Nobel Prize in Chemistry)
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Alfa -particlehelium-4 nucleus
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- Neutron, n - Protons, He2+
- Electrons, e
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Atomic number, Mass number and Isotopes
Atomic number (Z) = number of protons in nucleus
Mass number (A) = number of protons + number of neutrons
= atomic number (Z) + number of neutrons
Isotopes are atoms of the same element (X) with
different numbers of neutrons in their nuclei
XA
Z
H1
1H (D)
2
1H (T)
3
1
U235
92U238
92
Mass Number
Atomic NumberElement Symbol
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Isotopes are atoms of the same element (X)
with different numbers of neutrons in their nuclei
XA
Z
Mass Number
Atomic NumberElement Symbol
U235
92
92 protons, 92 electrons
143 (235 - 92) neutrons,
Atomic number, Mass number and Isotopes
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Mass Relationships in Chemical Reactions
Atomic/Nano/Micro Worldatoms & molecules
Macro WorldGrams; tons
The mole (mol) is the amount of a substance that contains as many elementary entities as there
6.022140857 × 1023
are atoms in exactly 12.00 grams of 12C
Avogadro’s number (NA) 6.022 140 76 × 1023
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Mass Relationships in Chemical Reactions
The mole (mol) is the amount of a substance that contains as many elementary entities as 6.022 140 76 × 1023
there are atoms in exactly 12.00 grams of 12C …IUPAC 2018
http://physics.nist.gov/cgi-bin/cuu/Value?na
Lorenzo Romano Amedeo Carlo Avogadro
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On this scale
1H = 1.008 amu
16O = 16.00 amu
Atomic mass is the mass of an atom in atomic mass units (amu)
Natural abundance of lithium:
6Li (6.015 amu) 7.42%
7Li (7.016 amu) 92.58%
Average atomic mass of lithium:
7.42 x 6.015 + 92.58 x 7.016
100= 6.941 amu
Li
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Average atomic mass (6.941)
= 6.941 amu
Li
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Mass Relationships in Chemical Reactions
Atomic/Nano/Micro Worldatoms & molecules
Macro WorldGrams; tons
Avogadro’s number (NA) 6.022140857 × 1023 mol-1
1 mole (mol) Li MW=6.941 g/mol 6.941 gram
1 mole (mol) C MW=12.0107 g/mol 12.0107 gram
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Mass Relationships in Chemical Reactions
Carbon 12.0107 gSulfur 32.065 gMercury 200.59 gCopper 63.546 gIron 55.845 g
One Mole of:
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Mass Relationships in Chemical Reactions
6x (12.0107) + 12x(1.00794) + 6x(15.9994)
180.1559 gmol-1
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Mass Relationships in Chemical Reactions
How many molecules are in 5.0 g of Saccharose ?
342.2965 gmol-1
Formula: C12H22O11
Molar mass: 342.2965 g/mol
5.0 g
Avogadro’s number (NA)
x 6.022140857 × 1023 mol-1
mol
= 12 x 8.8 × 1021 atoms of C
= 8.8 × 1021 molecules of Saccharose
= 22 x 8.8 × 1021 atoms of H
= 11 x 8.8 × 1021 atoms of O
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Mass Relationships in Chemical Reactions
5.0 g of Saccharose ?
Formula: C12H22O11
Molar mass: 342.2965 g/mol
Avogadro’s number (NA)
6.022140857 × 1023 mol-1
20 milhões x 20 milhões x 20 milhões
= 8.8 × 1021 molecules of Saccharose
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Mass Relationships in Chemical Reactions
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Mass Relationships in Chemical Reactions
%C =2 x (12.01 g)
46.07 gx 100% = 52.14%
%H =6 x (1.008 g)
46.07 gx 100% = 13.13%
%O =1 x (16.00 g)
46.07 gx 100% = 34.73%
52.14% + 13.13% + 34.73% = 100.0%
C2H6O
Ethanol
Percent composition of an element in a compound =
n x molar mass of element
molar mass of compoundx 100%
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Mass Relationships in Chemical Reactions
nK = 24.75 g K x = 0.6330 mol K1 mol K
39.10 g K
nMn = 34.77 g Mn x = 0.6329 mol Mn1 mol Mn
54.94 g Mn
nO = 40.51 g O x = 2.532 mol O1 mol O
16.00 g O
Empirical formula of a compound that has the following percent composition by mass:
K= 24.75% , Mn= 34.77%, O= 40.51%
Base ..100 g
K : ~~ 1.00.6330
0.6329
Mn : 0.6329
0.6329= 1.0
O : ~~ 4.02.532
0.6329
nK = 0.6330, nMn = 0.6329, nO = 2.532
KMnO4
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Mass Relationships in Chemical Reactions
Combustion 11.5 g ethanol
Collect 22.0 g CO2 and 13.5 g H2O
g CO2 mol CO2 mol C g C
g H2O mol H2O mol H g H
g of O = g of sample – (g of C + g of H)
6.0 g C = 0.5 mol C
1.5 g H = 1.5 mol H
4.0 g O = 0.25 mol O
C0.5H1.5O0.25
Divide by smallest subscript (0.25)
Empirical formula C2H6O
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Ethane reacts with oxygen to form carbon dioxide and water
C2H6 + O2 2 CO2 + 3 H2O
Balancing Chemical Equations
C2H6 + O2 CO2 + H2O
multiply O2 by 72
C2H6 + 7/2O2 2 CO2 + 3 H2O
2C2H6 + 7O2 4CO2 + 6H2O
Balancing, C & H
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Mass Relationships in Chemical Reactions
2NO + 2O2 2NO2
NO is the limiting reagent
O2 is the excess reagent
limiting reagent
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Mass Relationships in Chemical Reactions
In one process, 124 g of Al are reacted with 601 g of Fe2O3
2Al + Fe2O3 Al2O3 + 2Fe
Calculate the mass of Al2O3 formed.
g Al mol Al mol Fe2O3 needed g Fe2O3 needed
OR
g Fe2O3 mol Fe2O3 mol Al needed g Al needed
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Mass Relationships in Chemical Reactions
In one process, 124 g of Al are reacted with 601 g of Fe2O3
2Al + Fe2O3 Al2O3 + 2Fe
Calculate the mass of Al2O3 formed.
g Al mol Al mol Fe2O3 needed g Fe2O3 needed
OR
g Fe2O3 mol Fe2O3 mol Al needed g Al needed
124 g /26.98 gmol-1
= 4.60 mol
601 g /159.688 gmol-1
= 3.76 mol
4.60/2 = 2.30 mol
3.76x2 = 7.52 mol
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Mass Relationships in Chemical Reactions
Theoretical Yield is the amount of product that wouldresult if all the limiting reagent reacted.
Actual Yield is the amount of product actually obtainedfrom a reaction.
% Yield = Actual Yield
Theoretical Yield
x 100
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Glass transition
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Liquid Nitrogen
Liquid nitrogen is
nitrogen in a liquid state at an extremely low temperature.
It is a colorless liquid with a density of 0.807 g/ml at
its boiling point (−195.79 °C (77 K; −320 °F))
Liquid nitrogen
liquid nitrogen can be stored and transported,
for example in vacuum flasks.