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39 Cards in this Set
- Front
- Back
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Describe Bohr Model |
1. only certain orbits corresponding to certain energies allowed 2. electrons in allowed states wont radiate energy 3. energy is emitted/absorbed when electrons go from one allowed energy state to another |
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Bohr Model Limitation |
1. only explained the hydrogen spectrum 2. circular orbits of electrons don't cut it |
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λ |
wavelength |
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ν |
frequency |
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quantum mechanical model |
matter behaves like waves, light behaves like particles |
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Heisenberg Uncertainty principle |
electron location in terms of probabilities instead of position ex. 95% boundary = 95% chance of finding within this area at any given time |
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general shape of s orbital |
circle |
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general shape of p orbita |
composite: flower |
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general shape of d orbital |
coming out of everything, 3D |
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Aufbau Principle |
electrons fill into lowest orbitals first |
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Pauli Exclusion |
only two electrons can occupy each orbital, and they must have opposite spin |
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hund's rule |
electrons fill singly into different orbitals of the same sublevel before pairing up |
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angular momentum quantum number |
l, 0-3, determines sublevel |
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magnetic quantum number |
m, orbital orientation |
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principle quantum number |
n |
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effective nuclear charge |
atomic number - core electrons (non-valence) |
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covalent bonding |
nonmetal-nonmetal, created by sharing electrons, poor conductor, low boiling point, low melting point |
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ionic bonding |
nonmetal-metal, created by electrostatic attraction, very strong, high melting point, high boiling point, good electrical conductor |
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lattice energy |
energy required to separate a mole of a solid ionic compound into its gaseous ions |
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formal charge |
valence electrons - electrons assigned to atom |
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octet rules origin |
s orbital + p orbital = 2 + 6 = 8 |
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bond energy |
enthalpy, energy required to break a bond |
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bond length |
distance between nuclei of two bonding atoms |
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octet rule exceptions |
ions or molecules with: 1. odd number of electrons 2. less than an octet 3. more than eight valence electrons |
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electronegativity |
the ability of an atom to attract bonding electrons |
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bond breaking is... |
endothermic |
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bond making is... |
exothermic |
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enthalpy of a reaction |
sum of bond energies of bonds broken - sum of energies of bonds made |
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difference in electronegativity results in... |
1. polar covalent bond 2. decreased bond length, increased bond strength |
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oxidation number |
# valence e - (# shared + # unshared) |
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metallic bonding |
electron sea, all atoms in the sample share the electrons |
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electric field |
polar molecules: line up according to +/- |
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Valence Bond Theory |
-covalent bond forms when orbitals of 2 atoms overlap and a pair occupy the overlap area -space formed can hold 2 electrons with opposite spins -greater the overlap, stronger the bond -extent of overlap depends on shape and direction |
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temperatue |
average kinetic energy of gas particles |
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STP |
at STP (T=273K, P=1 atm) one mole of gas takes up 22.4 L |
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avogadro's numer |
mol > particles mol x 6.022 x 10^23 |
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1 atm |
760 torr (mmHg) 101.3 kPa 14.696 psi |
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paramagnetic |
substance has unpaired electrons |
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diamagnetic |
all electrons are paired |
