atomic structure the idea of the atom early models greek philosophers – 450 b.c. what is the...
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Atomic Structure
The Idea of the Atom
Early Models Greek philosophers – 450 B.C. what is the
smallest particle? Democritus - Particles are atomos An atom is the smallest particle of an
element that retains the chemical identity of that element.
Aristotle Wins Greek society - slave based Beneath them to work with hands – no
experiments Settled disagreements by arguments Aristotle more famous than Democritus
Aristotle wins Didn’t believe or look into atoms until…
Late 1700s Chemists believed elements:
couldn’t be broken down by ordinary means Combine to form compounds
Advancements in balances better experiments
Laws Discovered Law of Conservation of mass: mass is neither
created nor destroyed during chemical or physical changes
Then discovered no matter where or how a compound is made it is made of fixed proportions of elements Law of Definite Proportions
Ex: Sodium Chloride, table salt, always has 39.34% Na and 60.66% Cl by mass
Laws Discovered Elements combine to form more than one
compound Ex: carbon monoxide, CO, and carbon dioxide CO2
Law of Multiple Proportions
John Dalton 1808 –DALTON’S ATOMIC THEORY
1. All matter is composed of small particles called atoms.
2. *All atoms of a given element are identical, but they differ from those of any other element.
Dalton’s Atomic Theory3. *Atoms cannot be subdivided, created, or
destroyed
4. Atoms of different elements combine in whole-# ratios to form compounds
5. In a chemical reaction, atoms are combined, separated, or rearranged.
1800s – The atom IS divisible Atom has two regions:
Nucleus: center of atom Protons: (+) charged Neutrons: no charge
Electron cloud: region around nucleus containing electrons, (-) charged
Subatomic particles: p+, no, and e-
Voltage source
+-
Moving electrical current (Cathode Ray) through glass tube with inert gas (Noble Gas)
J.J. Thomson’s ExperimentCathode - Ray Tube
Voltage source
J.J. Thomson’s ExperimentJ.J. Thomson’s Experiment
• By adding magnets, found the moving (-) particles By adding magnets, found the moving (-) particles
+
-
Thomson’s Model Same properties no
matter what element used
All atoms had ELECTRONS!!
Thomson’s Model Plum pudding: bunch of positive stuff, with the electrons able to be removed.
Ernest Rutherford - 1911 Atoms have e- = (-) charge Atoms are neutral need (+) to balance Must be other particles to account for mass
of atom… Rutherford used alpha particles to test.
Alpha particle: (+) charge, (2 p+ and 2 no) Experiment: beam of high speed alpha
particles into thin gold foil
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
Lead block
Uranium
Gold Foil
Florescent Screen
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
His prediction….
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
What he expected
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
What he happened
Results… Most particles passed through 1 in 8000 bounced back Some particles completely reversed path!!!
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
Plum-pudding is WRONG!
+
Atom is mostly empty Small dense,
positive pieceat center, nucleus
Alpha particlesare deflected by nucleus if they get close.
Mr. Green. Mr. Green’s Homepage. 10 Sept. 2003. http://www.tvgreen.com/index.htm. 21 Aug. 2004
+
Electron Cloud Model Current model of atom Nucleus surrounded by negative cloud
“electron cloud”
Size of Atom Atom = size of football stadium Nucleus = smaller than a dime in center Electron = each one smaller than
Roosevelt’s eye on the dime Atom is mostly empty space!
Composition of Atom Proton has (+) charge equal in magnitude to (-)
charge of electron Atoms neutral # p+ = # e-
p+ and no about same mass e- = 1836 times smaller than p+
Nucleus has majority of mass Nuclear Forces: short-range forces that hold
nucleus together p+-p+, p+-no, no-no
Counting Atoms Atomic Number (Z): number of p+ of
each atom of the element
Identifies Elements!!
Atomic Number What is the atomic number for… Hg What is the element with … 20 p+
Neutral atoms # p+ = # e-
In neutral atoms, atomic number = # e-
Isotopes Def: atoms of same element with different
# of no (different masses) 3 H isotopes:
Protium: 1 p+ 99.9885% Deuterium: 1 p+ 1 no 0.0115% Tritium: 1 p+ 2 no
Mass Number Use mass number to determine isotopes Mass #: # of p+ and n0
Atom with 17 p+ and 20 no has mass # of… Chlorine-37 – Hyphen Notation
Writing Isotopes Nuclear symbol:
Cl37
17Elemental symbol
Mass number
Atomic number
Finding # of Neutrons # of neutrons = mass # - atomic # How many p+, no and e- are in… Selenium – 79
27Al
Oxygen - 18
13
Isotopes Write the complete chemical/nuclear
symbol for the isotope with 21 protons, 24 neutrons, and 21 electrons.
Relative Mass of Atom Mass of Oxygen-16 = 2.656 x 10-23 g Use relative atomic masses Pick standard other masses are
expressed in relation to standard Standard: Carbon –12 atom
Carbon - 12 Has mass of 12 atomic mass units (amu) 1 amu: is exactly 1/12 the mass of a
carbon-12 atom Carbon-12: how many p+ and no? 1 p+ 1 amu (1.007276 amu) 1 no 1 amu (1.008665 amu) 1 e- 0 amu (0.005486 amu)
Carbon - 12 What element is 4 x mass of Carbon –12? What element is 1/3 mass of Carbon –12?
Average Atomic Masses Most elements are mixture of isotopes Mass of element is average mass of
isotopes We need the % of each isotope Average Atomic Mass: weighted average
of the atomic masses of the naturally occurring isotopes of an element.
Weighted Average Box with 100 marbles of 2 sizes:
25% have mass of 2.00g 75% have mass of 3.00g
What is the average mass of a marble? 2.75g (sig figs!!)
Average Atomic Mass Or (atomic weight) found on periodic table
(ROUND TO 2 DECIMAL PLACES!!) Average Atomic Mass =
(% Iso. #1)(Mass Iso.#1) + (%Iso.#2)(Mass Iso.#2) + …
100
Average Atomic Mass Find the atomic mass of Li if… 7.5% is Lithium – 6 = 6.015 amu 92.5% is Lithium – 7 = 7.016 amu
Example – AAM = 16.00 amuIsotope Fractional Abundance
Oxygen – 16 (15.99 amu) 99.757%
Oxygen – 17 (17.00 amu) .038%
Oxygen – x .235%
The Mole
Quantities 1 dozen =
12 1 gross =
144 1 ream of paper =
500 In chemistry: 1 mole = 6.022 x 1023
The Mole SI unit for amount of substance (mol) Def: the number of particles in exactly 12
g of carbon – 12. 12 g of carbon –12 has 6.022 x 1023 atoms Avogadro’s #, after Amadeo Avogadro The number is HUGE!!
Molar Mass Def: mass of 1 mole of a pure substance 1 mole Carbon –12 = 12 g 1 atom Carbon – 12 = 12 amu Mass of 1 mole of He atoms? 4.00g/mol Same as atomic mass from periodic table,
different units
Molar MassSo: 4.00g He, 6.94 g Li and 200.59 g Hg all
have 6.022 x 1023 atoms = 1 mole!!! Molar mass (g/mol) conversion factor!!
Gram/Mole Conversions
Mass, in g, of 3.6 mol of C? 43g
How many moles are in 23.5 g S? 0.733 mol
p. 85 problems
Conversions with Avogadro’s # Diatomic Molecules: elements that exist
as 2-atom molecules in natural state 7 diatomic molecules H2, O2, N2, F2, Cl2, Br2, I2
Remember!!! HONClBrIF
Conversions with Avogadro’s # How many moles of oxygen are in
2.00x1022 molecules of oxygen? How many atoms of sodium are in 3.80
mol of sodium?
Conversions with Avogadro’s # How many molecules of hydrogen are in
0.020 g of hydrogen? Mass of 5.0x109 atoms of neon? p.86 problems