intro to chemistry 9.29.15. chemistry: the study of
TRANSCRIPT
Intro to Chemistry
9.29.15
• Chemistry: The study of
• Chemistry: The study of matter
• Matter:
• Chemistry: The study of matter
• Matter: Anything with mass that takes up space
The Atom
• Atom: Smallest differentiable unit of matter–Composed of
The Atom
• Atom: Smallest differentiable unit of matter–Composed of protons, neutrons, and
electrons
Subatomic Particles
• Neutron: –Found in the
Subatomic Particles
• Neutron: –Found in the nucleus–Charge of
Subatomic Particles
• Neutron: –Found in the nucleus–Charge of 0–Mass of
Subatomic Particles
• Neutron: abbr?
–Found in the nucleus–Charge of 0–Mass of 1 amu (atomic mass unit)
Subatomic Particles
• Neutron: n0
–Found in the nucleus–Charge of 0–Mass of 1 amu (atomic mass unit)
Subatomic Particles
• Proton: –Found in
Subatomic Particles
• Proton: –Found in the nucleus–Charge of
Subatomic Particles
• Proton: –Found in the nucleus–Charge of +1–Mass of
Subatomic Particles
• Proton: –Found in the nucleus–Charge of +1–Mass of 1 amu
Subatomic Particles
• Proton: p+
–Found in the nucleus–Charge of +1–Mass of 1 amu
Subatomic Particles
• Electron: –Found
Subatomic Particles
• Electron: –Found orbiting the nucleus at a great
distance–Charge of
Subatomic Particles
• Electron: –Found orbiting the nucleus at a great
distance–Charge of -1–Mass of
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)
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)
Electron Orbitals
• Electrons orbit the nucleus in discrete orbits or “shells”–First orbital holds
Electron Orbitals
• Electrons orbit the nucleus in discreet orbits or “shells”–First orbital holds 2 e-
–2nd =
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-
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
Al
13S 283
Aluminum
26.982
Al
13S 283
Aluminum
26.982
Al
13S 283
Aluminum
26.982
ElementSymbol
Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Average atomic mass (# of p+ + n0)
Al
13S 283
Aluminum
26.982
ElementSymbol
ElementName
# of p+
(AtomicNumber)
Average atomic mass (# of p+ + n0)
# of e- ineach shell
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)
Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
Mg
Models of the Atom
• Lewis dot structure: Shows the chemical symbol and only the valence electrons (# in outer shell)
B O
Bohr Diagram
• Shows complete e- configuration (sometimes shows details of nucleus)
• Ex: Mg
Bohr Diagram
• Shows complete e- configuration (sometimes shows details of nucleus)
• Try: F and Ca
Isotopes
• Isotope: An atom with a different # of n0 than normal, which therefore also has a different
Isotopes
• Isotope: An atom with a different # of n0 than normal, which therefore also has a different atomic mass
Isotopes
• Ex: C-12 vs. C-14–p+ =
p+ =
Isotopes
• Ex: C-12 vs. C-14–p+ = 6 p+ =
6–n0 = n0 =
Isotopes
• Ex: C-12 vs. C-14–p+ = 6 p+ =
6–n0 = 6
n0 = 8–e- = e- =
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