Download - Bellwork 10/19/15 Tell me about one or more of your family traditions. Minimum 5 sentences
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Bellwork 10/19/15
• Tell me about one or more of your family traditions.
• Minimum 5 sentences.
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P. Sci.Unit 8
Chapter 4
Atoms
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Atomic Structure – timeline
• Ancient Greece - Democritus proposed the atom – a tiny solid particle that could not be subdivided.
• 1904 – J.J. Thomson – discovered that atoms contained small, negatively charged particles called electrons.
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• 1911 – Ernest Rutherford – proposed that the atom had two parts – the nucleus in the center (most of the mass) surrounded by the electrons.
• 1913 – Niels Bohr –
hypothesized that
electrons traveled in fixed
orbits around the atom’s nucleus.
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• 1913 – James Chadwick – concluded that the nucleus contained positive protons and neutral neutrons.
• 1926 – Erwin Schrodinger – developed the quantum mechanical model – which is based on the wavelike properties of the electron. (not a particle – leads to quantum physics)
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• 1927 – Werner Heisenberg – (the Heisenberg uncertainty Principle) described that it is impossible to know precisely both an electron’s position and path at a given time. Led to the electron cloud theory.
electron
neutron
proton
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Atoms
• The smallest particle that has the properties of an element.
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Dalton’s Atomic Theory• Every element is made of tiny,
unique, particles called atoms that cannot be subdivided.
• Atoms of the same element are exactly alike.
• Atoms of different elements can join to form molecules or compunds
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Parts of an Atom• Nucleus – small, dense center of
an atom made up of 2 subatomic particles that are identical in size and mass.
–Protons – have a
positive charge
–Neutrons – have no charge
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Parts of an Atom cont.• Electrons – are tiny subatomic
particles that have very little mass that moves around the outside of the nucleus. These particles are negatively charged and form a
“cloud” around
the nucleus.
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• The number of protons and electrons an atom has is unique for each element.
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Atomic Charge• Atoms have no overall charge
because the protons (+) cancel out the electrons (-).
Helium 2 protons - +2 2 neutrons - 0 2 electrons - -2 total charge 0
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Protons• positive (+) charge
• Found in the nucleus
• # of protons = atomic # • The number of protons identify
the element (atomic #)
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Neutrons• no charge
• Found in the nucleus
• Along with protons makes up atomic mass
• Atomic Mass – atomic number = # of neutrons (rounded to whole #)
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Electrons• negative (–) charge • travel in orbitals (or energy levels)
around the nucleus. (electron cloud) • Equals atomic number in neutral
atoms• valence electrons - the # of electrons
in the outer shell and relates to the oxidation #
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• Unit of measure for atomic particles is Atomic mass unit (amu) protons and neutrons = about 1 amu (electrons are about 1/2000 of the size of protons and neutrons))
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Chemical symbols• The one or two letter abbreviation of the element name.• Some are based on Latin name• ALL 1st letter is upper case• ALL 2nd letter is lower case
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Mass Number or Atomic Mass• the sum of the number of protons
and the number of neutrons in the nucleus of an atom.
• # of neutrons =
mass # - atomic #Protons
+
Neutrons
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Atom Summary• Atomic Number = protons = electrons• Atomic Mass = Protons + Neutrons
• Neutrons = atomic mass – atomic number• Atomic symbols
– First letter is ALWAYS upper case– Second letter is ALWAYS lower case
• Example:
Oxygen element 6 with mass 16
P = 8
E = 8
N = 16-8 = 8
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Isotopes• Atoms of the same element that have
a different # of neutrons and a different atomic mass. (identified by the element name followed by the mass # )
• ex. C-12, C-14, B-10, B-11)
6 electrons6 protonsCarbon 12 = 6 neutrons
Carbon 14 = 8 neutrons6 protons
6 electrons
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Average atomic mass• the weighted - average mass of the
mixture of all an atoms isotopes. The average atomic mass is close to the mass of its most abundant isotope.
• This is the number found on the periodic table