atomic theory. first person to purpose that matter was not infinitely divisible “atomos”
TRANSCRIPT
ARISTOTLE•Rejected atomic theory• did not believe in “nothingness” of space
JOHN DALTON (1766-1844) Modern atomic theory –
19th century Conservation of mass –
separation, combination, or rearrangement of atoms
Was all of his theory accurate? NO!!
Dalton’s Atomic Theory (1808)
Atoms cannot be subdivided, created, or destroyed Atoms of different elements combine in simple whole-number ratios to form chemical compounds In chemical reactions, atoms are combined, separated, or rearranged
All matter is composed of extremely small particles called atoms Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties
DEFINING THE ATOM The smallest particle of an element that
still retains the properties of the element
How small is an atom?World population: 6300000000Atoms in a penny:
29000000000000000000000 Scanning tunneling microscope – allows
individual atoms to be seen
CATHODE RAY TUBE
William Crookes
Discovered Cathode Ray Tube
JJ Thomson
Used Cathode Ray tube to discover Electron
Discovery of the Electron1897: J.J. Thomson used a cathode ray tube to deduce the presence of a negatively charged particle.
Cathode ray tubes pass electricity through a gas that is contained at a very low pressure.
CATHODE RAY RESULTS Cathode ray deflected in a magnetic
field, indicated charged particles Deflected towards positively charged
plate, indicating particles must have negative charge
Altering gas, altering material had no effect on results, so particles must be in all matter
Called…. ELECTRONS!!!! First subatomic particles! Meant Dalton was… wrong!!!
MASS AND CHARGE OF THE ELECTRON 1909 – Robert Millikan determines the
mass of the electron. Mass of the electron was much smaller
than that of the hydrogen atom, the smallest known atom
Meant atoms were divisible into subatomic particles
Mass = 9.1 x 10-28 = 1/1840 mass of hydrogen
Charge = -1
Conclusions from the Study of the Electron
Electrons are negative. Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons. Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons Electrons have so little mass that atoms must contain other particles that account for most of the mass
THOMSON’S PLUM PUDDING MODEL Atom breakable!! Atom has structure Electrons suspended in a positively charged
electric field must have positive charge to balance negative
charge of electrons and make the atom neutral mass of atom due to electrons atom mostly “empty” space
compared size of electron to size of atom Cookie dough model
Rutherford’s Gold Foil Experiment
Alpha particles are positively charged Particles were fired at a thin sheet of gold foil Particle hits on the detecting screen (film) are recorded
Rutherford’s Findings Most of the particles passed right through
A few particles were deflected
GREATLY Deflected particles were repulsed by positive charge of nucleus
Conclusions: Nuclear Model
RUTHERFORD’S NUCLEAR MODEL
The atom contains a tiny dense center called the nucleus the volume is about 1/10 trillionth the volume
of the atom The nucleus is essentially the entire
mass of the atom The nucleus is positively charged
the amount of positive charge of the nucleus balances the negative charge of the electrons
The electrons move around in the empty space of the atom surrounding the nucleus
PROTONS AND NEUTRONS Rutherford - Protons
Subatomic particle in nucleus protons :+1 charge (equal, opposite of
electrons) Chadwick – Neutrons
Subatomic particle in nucleusMass nearly equal to a proton, but carries
no electrical charge
Atoms are indivisible!
Actually, Mr. Dalton, we have proved that part of your theory
wrong.
What!?!Atoms can be divided into electrons,
protons, and neutrons.
Atom – electrically neutral particle composed of protons, neutrons, electronsSpherical shape
Atoms consist of two regionsNucleus – 99.7% of mass
Very small, dense region in the center. Contains protons & neutrons.
Electrons Cloud Mainly empty space surrounding nucleus Very large compared to the nucleus. Contains electrons.
Subatomic particlesProtons, neutrons, and electrons
THE STRUCTURE OF THE ATOM
Atomic Particles
Particle
Charge
Mass (kg) Location
Electron
-1 9.109 x 10-
31
Electron cloud
Proton +1 1.673 x 10-
27
Nucleus
Neutron
0 1.675 x 10-
27
Nucleus
Atomic NumberAtomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. Identifies the atom.Element # of
protonsAtomic #
(Z)
Carbon 6 6
Phosphorus
15 15
Gold 79 79
Isotopes
Elements occur in nature as mixtures of isotopes.
Isotopes are atoms of the same element that differ in the number of neutrons
Isotopes…Again (must be on the test)
Isotopes are atoms of the same element having different masses due to varying numbers of neutrons.Isotope Proto
nsElectron
sNeutron
sNucleus
Hydrogen–1 (protium)
1 1 0
Hydrogen-2
(deuterium)
1 1 1
Hydrogen-3 (tritium)
1 1 2
Mass NumberMass number is the number of protons and neutrons in the nucleus of an isotope.
Mass # = p+ + n0
Nuclide p+ n0 e- Mass #
Oxygen - 10
- 33 42
- 31 15
8 8 1818
Arsenic 75 33 75
Phosphorus 15 3116
Atomic Masses
Isotope Symbol
nucleus % in nature
Carbon-12
12C 6 protons 6 neutrons
98.89%
Carbon-13
13C 6 protons 7 neutrons
1.11%
Carbon-14
14C 6 protons 8 neutrons
<0.01%
Atomic mass is the average of all the naturally isotopes of that element. Carbon = 12.0125
amuOn Periodic Table
WRITING NUCLEAR SYMBOLS
He3
2
Mass #
Atomic #
Atomic Symbol
How many protons, electrons, and neutrons?
2 protons, 2 electrons, 1 neutron
Mass # - Atomic # = # Neutrons
WRITING ISOTOPES USING HYPHEN NOTATION
Uranium-235, Helium-3, or Carbon-14
Name of atom
Mass #
How many proton, electrons, neutrons?92 protons, 143
neutrons, 92 electrons