atomic structure chapter 4. sizing up the atom o radii of most atoms: 5 x 10 -11 m to 2 x 10 -10 m o...
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Subatomic particles O Proton: positively charged subatomic particle (p + ) O Neutron: neutral subatomic particle (n 0 ) O Electron: negatively charged subatomic particle (e - ) O Protons and neutrons are the same size, but electrons are 1840 times smaller. O *All atoms are neutral* O Nucleus: tiny central core of an atom and is composed of protons and neutrons with an overall positive charge.TRANSCRIPT
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Atomic StructureChapter 4
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Sizing up the Atom O Radii of most atoms: 5 x 10-11 m to 2 x
10-10 mO Copper penny contains 2.4 x 1022
atoms. The population of Earth is about 6 x 109 people. There is about 4 x 1012 times as many atoms in a coin than people on Earth.
O Line up 100,000,000 copper atoms side by side, the line would be only 1 cm long
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Subatomic particlesO Proton: positively charged subatomic particle (p+)O Neutron: neutral subatomic particle (n0)O Electron: negatively charged subatomic particle
(e-)O Protons and neutrons are the same size, but
electrons are 1840 times smaller.O *All atoms are neutral*
O Nucleus: tiny central core of an atom and is composed of protons and neutrons with an overall positive charge.
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Nuclear AtomO Protons and neutrons are located in
the nucleus (positive charge)O Electrons are distributed around the
nucleus and occupy almost all the volume of the atom (negative charge)
O The positive nucleus is balanced out with equal number or electrons. Atoms are always neutral.
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Atomic NumberO Elements are different because they
contain different numbers of protonsO Atomic number: number of protons in
nucleus of atomO All atoms are neutralO # protons = # electronsO Blue number in upper right hand corner for
each element on periodic tableO Nuclear charge is the charge of the nucleus
and is dependent on the number of protons.
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Atomic MassO The weighted average mass of atoms in a
naturally occurring sample of the elementO Reflects both the mass and the relative
abundance of the isotopes as they occur in nature
O Isotope: atoms that have same # of protons but different # of neutrons (different mass numbers)
O Neon-20, Neon-21, Neon-22O http://education.jlab.org/itselemental/
iso006.html
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Mass NumberO Most of atom’s mass is concentrated
in nucleus and depends on # protons and neutrons
O Mass number: total number of protons and neutrons in nucleus of atom
O # neutrons = mass # – atomic #O To determine the mass # you round
the atomic mass to the nearest whole #
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Atomic Mass Unit (AMU)
O 1/12 the mass of a carbon -12 atomO More useful to compare the relative
masses of atoms using a reference isotope as a standard.
O Reference isotope: Carbon-12O Helium mass = 4.00260 amu and is
1/3 the mass of carbon-12O Table 4.3
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To calculate atomic mass:
O Multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products.