intro to chemistry 9.29.15. chemistry: the study of
TRANSCRIPT
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Intro to Chemistry
9.29.15
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• Chemistry: The study of
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• Chemistry: The study of matter
• Matter:
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• Chemistry: The study of matter
• Matter: Anything with mass that takes up space
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The Atom
• Atom: Smallest differentiable unit of matter–Composed of
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The Atom
• Atom: Smallest differentiable unit of matter–Composed of protons, neutrons, and
electrons
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Subatomic Particles
• Neutron: –Found in the
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Subatomic Particles
• Neutron: –Found in the nucleus–Charge of
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Subatomic Particles
• Neutron: –Found in the nucleus–Charge of 0–Mass of
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Subatomic Particles
• Neutron: abbr?
–Found in the nucleus–Charge of 0–Mass of 1 amu (atomic mass unit)
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Subatomic Particles
• Neutron: n0
–Found in the nucleus–Charge of 0–Mass of 1 amu (atomic mass unit)
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Subatomic Particles
• Proton: –Found in
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Subatomic Particles
• Proton: –Found in the nucleus–Charge of
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Subatomic Particles
• Proton: –Found in the nucleus–Charge of +1–Mass of
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Subatomic Particles
• Proton: –Found in the nucleus–Charge of +1–Mass of 1 amu
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Subatomic Particles
• Proton: p+
–Found in the nucleus–Charge of +1–Mass of 1 amu
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Subatomic Particles
• Electron: –Found
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Subatomic Particles
• Electron: –Found orbiting the nucleus at a great
distance–Charge of
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Subatomic Particles
• Electron: –Found orbiting the nucleus at a great
distance–Charge of -1–Mass of
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Subatomic Particles
• Electron: –Found orbiting the nucleus at a great
distance–Charge of -1–Mass of 0 amu (not actually zero, but
mass is so small that it is ignored)
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Subatomic Particles
• Electron: e-
–Found orbiting the nucleus at a great distance–Charge of -1–Mass of 0 amu (not actually zero, but
mass is so small that it is ignored)
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Electron Orbitals
• Electrons orbit the nucleus in discrete orbits or “shells”–First orbital holds
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Electron Orbitals
• Electrons orbit the nucleus in discreet orbits or “shells”–First orbital holds 2 e-
–2nd =
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Electron Orbitals
• Electrons orbit the nucleus in discreet orbits or “shells”–First orbital holds 2 e-
–2nd = 8 e-
–3rd = 8 e-
–4th = 10 e-
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Electron Orbitals
• Electrons orbit the nucleus in discreet orbits or “shells”–First orbital holds 2 e-
–2nd = 8 e-
–3rd = 8 e-
–4th = 10 e-
Important: The valence electrons (outer shell) are the only important ones for forming bonds with other atoms
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Al
13S 283
Aluminum
26.982
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Al
13S 283
Aluminum
26.982
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Al
13S 283
Aluminum
26.982
ElementSymbol
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Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
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Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
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Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Average atomic mass (# of p+ + n0)
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Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Average atomic mass (# of p+ + n0)
# of e- ineach shell
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Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Average atomic mass (# of p+ + n0)
# of e- ineach shell
Physical state at STP (0o @ sea level)
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Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
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Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
Mg
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Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
B O
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Bohr Diagram
• Shows complete e- configuration (sometimes shows details of nucleus)
• Ex: Mg
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Bohr Diagram
• Shows complete e- configuration (sometimes shows details of nucleus)
• Try: F and Ca
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Isotopes
• Isotope: An atom with a different # of n0 than normal, which therefore also has a different
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Isotopes
• Isotope: An atom with a different # of n0 than normal, which therefore also has a different atomic mass
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Isotopes
• Ex: C-12 vs. C-14–p+ =
p+ =
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Isotopes
• Ex: C-12 vs. C-14–p+ = 6 p+ =
6–n0 = n0 =
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Isotopes
• Ex: C-12 vs. C-14–p+ = 6 p+ =
6–n0 = 6
n0 = 8–e- = e- =
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Isotopes
• Ex: C-12 vs. C-14–p+ = 6 p+ = 6–n0 = 6 n0 = 8–e- = 6 e- = 6
–Isotopes only differ in their mass, not in their charge or their bonding behavior