how atoms differ section 4.3. what information can be used for one’s home address? atoms have...
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H O W AT O M S D I F F E R
SECTION 4.3
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• What information can be used for one’s home address?• Atoms have identifying information too.
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ATOMIC NUMBER
•Henry Moseley (1887-1915)• Discovered that atoms of
each element contain a unique positive charge in their nuclei
• The # of protons in an atom identifies it as an atom of a particular element.
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ATOMIC NUMBER
• The number of protons in an atom is referred to as the atomic number• The number of electrons in a NEUTRAL atom is also equal to the atomic number
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ATOMIC NUMBER
•DOES NOT ALWAYS EQUAL the number of neutrons!!!•So we cannot determine the number of neutrons from the atomic number
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MORE ON THE ATOMIC NUMBER
• All Atoms are neutral, so therefore, the number of electrons in an atom equals the atomic number.•When an atom has a charge, it is called an ion… not an atom.
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LET’S FILL IN A TABLE
Element Atomic # # of protons
# of electrons
F4
2935
1823
Cu
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ISOTOPES AND MASS NUMBER
•Atoms with the same # of protons but different numbers of neutrons are called isotopes.• Example: 3 types of potassium.• All 3 types contain 19 protons and 19
electrons• 1 contains 20 neutrons• another contains 21 neutrons• And another contains 22 neutrons
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MASS OF ISOTOPES
•When an isotope contains more neutrons, it has a greater mass than the isotopes that contain less neutrons.• Even with different masses, the isotopes have the same chemical behavior.
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ISOTOPE NOTATION
• Every isotope of an element is identified with a number called the mass number.
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• The mass number is the sum of the atomic number (or number of protons) and the number of neutrons in the nucleus.
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LET’S BREAK IT DOWN
• Mass number =
• So, then we can say….
• Number of neutrons =
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TIME FOR ANOTHER TABLE
Element
Atomic #
Mass #
# of p+
# of n0
# of e-
Cd36
107.86814 8
11 12
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ISOTOPE NOTATION
•We can write isotopes in 2 manners•One method is simply to write the element name followed by a hyphen and the atomic mass (Ex: carbon-14)•Or we could simply write in the format of , where A is the atomic mass and Z is the atomic number (Ex: )
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ISOTOPE NOTATION
•Given one isotope notation, write the other corresponding isotope notation:• Zinc-70
• Silicon-29• Silver-106
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ISOTOPE NOTATION
•Hydrogen has 3 isotopes: Hydrogen-1, Hydrogen-2, and Hydrogen-3. • Isotopes of hydrogen are special, because hydrogen-2 and hydrogen-3 have special names.•We simply call hydrogen-1 “hydrogen,” while we call hydrogen-2 “deuterium” and we call hydrogen-3 “tritium”
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• Atomic mass unit: arbitrary number chosen by scientists many years ago that is equal to the mass of 1/12 of a C-12 atom (most commonly written amu)
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•Most elements are found in nature as mixtures of isotopes.•Usually any sample of an element contains the same relative abundance of each isotope• So, if there is a different mass for each isotope, then why is there only 1 mass number for an element?
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AVERAGE ATOMIC MASS
• The mass number on the PT is the AVERAGE atomic mass, calculated by using the relative abundance of each isotope.
•How’s that calculated?(Mass of isotope)(% abundance) +(mass of isotope)(% abundance)+…
100
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EXAMPLE
• Element X has 2 isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass of this element.
(10.012)(19.91)+(11.009)(80.09)
100=10.810 amu
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SOME FINAL OFFICIAL DEFINITIONS
•The atomic mass of an element is the weighted average mass of the isotopes of that element.