Download The Atom - dsapresents.org

The Atom
Dalton’s Atomic Theory
1. All elements are composed of tiny indivisible particles called atoms
2. Atoms of the same element are identical. The atoms of any one
element are different from those of any other element.
3. Atoms can physically mix together or can chemically combine in
simple whole number ratios.
4. Chemical reactions occur when atoms are separated , joined or
rearranged. Atoms of one element never change into atoms of another
element as a result of a chemical reaction.
Electrons
• Electrons are negatively charged particles in an atom
• JJ Thomson passed current through gases at low pressure and found
cathode rays were attracted to the metal plates which had a positive
charge. Plates with a negative charge repelled the rays, so a cathode
ray is a stream of negatively charged particles called electrons.
• Millikan found the quantity of charge carried by an electron and the
ratio of charge to mass determining the mass of an electron.
Protons and Neutrons
• Goldstein discovered the proton using the cathode ray, a particle with
a positive charge. The proton mass is calculated as 1840 times the
mass of an electron.
• Chadwick discovered a neutral particle called the neutron with the
same mass as a proton.
• Rutherford directed a narrow beam of alpha particle at a thin sheet of
gold foil. Most of the alpha particles went through the foil with only a
few being repelled because an atom has a very small positive nucleus.
He concluded an atom is made up of mostly empty space.
Atomic Number
• Protons and neutrons are in the middle of the atom and have the
most mass. Electrons surround the nucleus with little mass.
• The atomic number is the proton number and electron number in a
neutral atom.
• Neutrons must always be calculated. Neutrons + protons =Mass
• Mass – protons = neutrons
• On your periodic table Atomic weight = Mass (Average atomic mass,
atomic mass unit)
Mass
• Mass may be represented as……
• Hydrogen-1 or H-1, Gold-197 or Au-197, Carbon-12 or C-12
• Or 1H, 197Au or 12C
• Proton numbers can be represented as…..
• 0H, 79AU, 6C
Together superscript to the left is mass, subscript to the left is
atomic/proton number 10H, 197 79Au, 126C
Isotopes
• Protons remain the same, neutrons differ. H-1, H-2, H-3 is an example
• Average atomic mass/atomic mass is based on isotopes and is the
weighted average mass of an atom in a naturally occurring sample of
the element.
• Atomic mass unit is defined as 1/12 mass of the carbon-12 atom,
protons + neutrons = mass
• Average atomic mass considers abundance
How to calculate Average Atomic Mass
• Mass X percent abundance = percent abundance mass
• Add all of the percent abundance mass’ = overall percent abundance
mass
• Overall percent abundance mass / 100 = average atomic mass
• X = multiply
• / = divide