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28 Cards in this Set
- Front
- Back
def. of a nucleon
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protons and neutrons
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primary quantum number
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n, shell number, measures size and energy. n=1=k, n=2=L, n=3=M, n=4=N.
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secondary quantum number
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l, measures shape/energy of an electron's orbital, l=n-1, l=0=s, l=1=p, l=2=d, l=3=f
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tertiary quantum number
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ml, measures 3-D orientation of the orbital, ml=
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quaternary quantum number
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ms, designates the electron's intrinsic magnation, +1/2 or -1/2 only
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Aufbau principle
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electrons occupy lowest energy orbitals first
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Hund principle
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electrons in the same subshell occupy orbitals singly first
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Pauli exclusion principle
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no two electron configurations can have identical quantum numbers
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Ionic bonding
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electron(s) from an atom with a smaller ionization energy transferred to an atom with greater ionization energy.
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Covalent bonding
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electron pair shared between two atoms.
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Bond order
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number of shared electron pairs between two atoms.
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Bond length
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average distance between two nuclei of atoms. Inv. prop to bond order and bond energy
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Bond energy
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energy required to separate two bonded atoms. Prop. to bond order.
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Drawing Lew Dot Structure
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1. draw skeletal structure of compound w/ least Electro Neg atom in center.
2. Sum all valence electrons of individ atoms. 3. Drawing single bonds to atoms surrounding central atom. 4. complete the octets of all atoms surrounding central atom. 5. Place extra electrons on central atom. If CA doesnt have enough atoms, try to make double/triple bonds with surrounding atoms that have unbonded EPs. |
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Formal Charges
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Difference between valence electron number of a free atom and the atom in a lewis structure.
Formal Charge= V-0.5N(bonding)-N(nonbonding) |
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Polar Covalent Bonding
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occurs in atoms w/ small differences in EN. The covalent electrons are not shared equally, which forms a dipole in the molecule.
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Dipole Moment
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vector quantity. Product of charge magnitude and distance between two partial charges.
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Nonpolar Covalent Bond
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Two atoms have equal ENs. Electron pairs shared equally. Happens in diatomic molecs.
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Coordinate Covalent Bond
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Shared EP comes from long pair of one of the atoms in the molecule. Typically Lewis Acid-Base combos. Can't be distinguished from other covalents.
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VSEPR Theory
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Predicts molecular geometry using Lewis Dot Structure.
Rule: make lone EPs as far from eachother as possible. |
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Linear
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Bonded to two other atoms. 180 degrees btwn Lone EPs
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Trigonal Planar
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Bonded to three other atoms. 120 degress btwn Lone EPs
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Tetrahedral
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Bonded to four other atoms. 109.5 degrees btwn lone EPs.
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Trigonal Bipyramidal
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Bonded to five other atoms. Angle between EPs: 90,120,180
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Octahedral
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Bonded to six other atoms. Angle between EPs: 90,180
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Dipole-dipole Interactions
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1. The rearrangement of polar molecules so that the positive DPs interact w/negative. Present in liquid and solid states.
2. not as strong as ionic bonds |
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Hydrogen Bonding
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Very strong dipole-dipole interaction, this may be intra or intermolecular. Happens with attraction of highly positve hydrogen to highly negative FON.
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Dispersion forces
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weakest intermolecular force. Caused by random instantaneous polarization of nonpolar colavent molecules.
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