Mr Nelson. The Greek philosopher Democritus began the search for a description of matter more than...
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Transcript of Mr Nelson. The Greek philosopher Democritus began the search for a description of matter more than...
Mr Nelson
The Greek philosopher Democritus began the search for a description of matter more than 2400 years ago.◦ He asked: Could
matter be divided into smaller and smaller pieces forever, or was there a limit to the number of times a piece of matter could be divided?
400 BC
This piece would be indivisible.
He named the smallest piece of matter “atomos,” meaning “not to be cut.”
The eminent philosophers of the time, Aristotle and Plato, had a more respected, theory.
Aristotle and Plato favored the earth, fire, air and water approach to the nature of matter.
In the early 1800s, English Chemist John Dalton performed experiments that verified the existence of atoms.
1803
Dalton’s Model was that atoms are indivisible particles.
All matter is composed of atoms.
Atoms of the same element are exactly alike.◦ Atoms of different elements are different.
Atoms are indestructible and cannot be divided.
In 1897, the English scientist J.J. Thomson proved the atom is made of even smaller particles.
Thomson studied the Cathode Ray Tube.
As the current passed through the gas, it gave off rays of negatively charged particles.
the atoms of the gas were uncharged.
Where had the negative charges come from?
Where did they come from?
Thomson concluded that the negative charges came from within the atom.
Thomson called the negatively charged electrons.
Since the gas was known to be neutral, he reasoned that there must be positively charged particles in the atom.
But he could never find them.
“Plum Pudding” model.
Atoms were made from a positively charged substance with negatively charged electrons scattered around
In 1908
English physicist Ernest Rutherford, began work on his gold foil experiment.
Rutherford was trying to verify Thomson’s model.
He expected positively charged particles to go straight through a piece of very thin gold.
Most particles passed straight through the gold foil
A small percentage of particles were deflected at large angles or returned to the source
http://micro.magnet.fsu.edu/electromag/java/rutherford/
There are 2 reasons alpha particles deflected
◦Density of the nucleus
◦Repelling charges
An atom has ◦ a small, dense, positively charged center that
repelled the positively charged particles.
Named the center of the atom the “nucleus”
The nucleus is tiny compared to the atom as a whole.◦ The atom is mostly empty space
An atom’s positively charged particles were contained in the nucleus.
The negatively charged particles were scattered outside the nucleus around the atom’s edge.
Was a Jewish Scientist in Copenhagen during the onset of WWII
Hitler was interested in his research of the atom.
He was moved to the US to protect his knowledge.
Electrons travelled in a specific orbit at a certain distance from the nucleus called an energy level
Worked well for Hydrogen and Helium
In this unit we need to be familiar with this type of symbol
Includes an element name a ‘-’ and a number◦ Example: Sulfur – 32◦ This sulfur atom has an atomic mass of 32◦ Since Sulfur has ______ protons & electrons◦ It also has ______ neutrons
Particle Symbol Charge Mass (amu) Location
Proton
Neutron
Electron
Calculate the average atomic mass of magnesium given the following information:
Mg, mass = 23.98 amu; percent abundance = 78.99%
Mg, mass = 24.98 amu; percent abundance = 10.00%
Mg, mass = 25.98 amu; percent abundance = 11.01%
Electrons are a HUGE deal in chemistry
Responsible for light, color & chem reactions
Electrons in atoms:◦when an atom absorbs energy - electrons jump to higher energy levels.
◦An “EXCITED” electron jumps from its ground state to a higher energy level.
◦When the electron returns it releases the same amount of energy that it absorbed.
Light is released as photons as electrons return from different energy levels.
Some of the photons are visible light◦ Balmer Series
Wave
Particle
Hydrogen
Mercury
Argon
Helium
How many wavelengths are represented in each figure below?
Red Light
Violet Light
• Low frequency
• Long wavelength
• High frequency
•Short wavelength
nm = 1 x 10-9 m