440 likes | 596 Views
Intro to Chemistry. 9.27.13. 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.
E N D
Intro to Chemistry 9.27.13
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 discreet 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 outer shell is the only important one for forming bonds with other atoms
S 2 8 3 13 Al Aluminum 26.982
S 2 8 3 13 Al Aluminum 26.982
S 2 8 3 13 Element Symbol Al Aluminum 26.982
S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982
# of p+ (Atomic Number) S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982
# of p+ (Atomic Number) S 2 8 3 13 Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)
# of p+ (Atomic Number) S 2 8 3 13 # of e- in each shell Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)
# of p+ (Atomic Number) Physical state at STP (0o @ sea level) S 2 8 3 13 # of e- in each shell Element Symbol Al Aluminum Element Name 26.982 Average atomic mass (# of p+ + n0)
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