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66 Cards in this Set

  • Front
  • Back
A(n) _____ _____ gives the number of protons in the atom's nucleus.
atomic number (z)
A(n) _____ ____ gives the total of protons plus neutrons in an atom's nucleus.
mass number (A)
Atoms with the same atomic number but different mass number are _____.
isotopes
The weighted average mass in atomic mass units (amu) of an element's naturally occuring isotopes is called the element's _____ _____.
atomic mass
According to the quantum mechanical model, the behavior of a specific e- in an atom can be described by a(n) _____ _____.
wave equation
In the most common implentation, wavefunctions correspond to atomic orbitals called _____.
psi
_____ in three dimensional space describes the volume of space around a nucleus that an e- is most likely to occupy.
psi squared
The _____ _____ _____ determines the spatial orientation of the angular momentum (describes where the orbits are in space)
magnetic quantum number (mL)
The _____ _____ _____ takes on positive integers starting with one. (wavefunction question)
principal quantum number (n)
The _____ _____ _____ _____ _____ determines the angular momentum of the e- as it moves in an orbital
orbital angular momentum quantum number (L)
_____ tells us the shape of the orbital.
L
The different values of L are given _____ rather than _____.
letters, numbers
An atom's highest quantum number determines its _____ _____.
valence shell
The _____-orbitals are spherical with the nucleus in the center.
s
The _____-orbitals are dumbbell shaped.
p
The Px orbital is pictured _____.
diagonally
The Py orbital is pictured _____.
horizontally
The Pz orbital is pictured _____.
vertically
On a p-orbital, nodes are _____.
a region of 0 e- density.
The 3 e- configuration rules?
- Aufbau's principle
- Pauli exclusion principle
- Hund's rule
What is the Pauli exclusion principle?
Only two e- may occupy an orbital and with opposite spins.
What's the Aufbau principle?
Lowest energy orbitals fill up first in this order:
1s->2s->2p->3s->3p->4s->3d
What is Hund's Rule?
If two or more empty orbs of equal energy are available, one e- occupies each with spins parallel until all orbitals are half full.
Explain valance bond theory.
A covalent bond forms when two atoms approach each other closely and a singly occupied orbital on one atom overlaps the other atom.
What is the bond formed when two singly occupied orbitals overlap?
sigma bond
What is the bond angle of the tetrahedron?
109.5º
Why are the lobes asymmetrical in an sp3 orbital?
The lobes of the p-orbital are + and -. The positive p lobe adds to the s-orbital but the negative subtracts.
The advantage of the asymmetric sp3 lobes?
It can overlap more effectively with an orbital from another atom when it forms a bond.
The meaning of the sp3 superscript?
Tells how many p-orbitals combine to show the hybrid.
Ethylene carbons can be tetravalent only if they share _____ e- and are linked by a _____ _____.
four, double bond
Ethylene is _____ and has bond angles of approximately _____.
planar, 120º
Ethylene is an _____ system, so it has sp2 hybrid orbitals, which is when:
unsaturated, the 2s orbital combines with only two of the three available 2p orbitals, with one 2p orbital remaining unchanged.
In ethylene, the three sp2 orbitals lie on a plane at angles of _____ to one another, with the remaining p-orbital _____ to the sp2 plane.
120º, perpendicular
In ethylene, when two sp2 hybridized carbons approach each other:
they form a sigma bond by sp2-sp2 head on overlap.
In ethylene, at the same time as the sp2 sigma bonds, the unhybridized p-orbitals do what?
they approach each other with the correct geometry for a sideways overlap, leading to the formation of a π bond.
In ethylene, the combination of the sigma bond and π bond results in the sharing of _____ _____ and a _____ _____ _____.
4 e-, carbon-carbon double bond
Carbon can form triple bonds by sharing _____ e-.
six
What happens in sp hybrid orbitals?
Two sp orbitals result, and two p-orbitals remain unchanged.
In acetylene, in an sp hybrid, a carbon 2s orbital hybridizes with only a _____ _____ orbital.
single p
In acetylene, the two sp hybrid orbitals are oriented _____ away from each other.
180º
In acetylene, when two sp hybridized molecules approach each other, sp hybrid orbitals on each carbon overlap head on to form a strong _____ _____ _____.
sp-sp sigma bond
In acetylene, following the formation of the sp-sp sigma bond, the _____ orbitals from carbon form a _____ _____ _____ by sideways overlap and the _____ orbitals overlap similarly to form a _____ _____ _____.
pz, pz-pz π bond, py, py-py π bond
In acetylene, once the first three hybridized orbitals are bonded, what becomes of the two remaining sp hybrid orbitals?
they each form a sigma bond with hydrogen to complete the acetylene molecule.
In acetylene, the net effect is the sharing of _____ e- and the formation of a _____ _____ _____.
6, carbon-carbon triple bond
What is CH3NH2?
Methylamine. Derivative of NH3 and responsible for odor of rotting fish. Bleh.
What's so special about the geometry of CH3NH2?
Methylamine's experimentally measured H-N-H bond angle and C-N-H bond angle are very close to 109.5º...very close to tetrahedral bond angle of methane.
What do we assume about the N bonds in methylamine?
That N hybridizes to form form sp3 orbitals, just like carbon.
What's so cool about phosphorus and sulfur, hm?
they can accommodate more than an octect to form more covalent bonds
How many bonds can P form?
5 bonds
How many bonds can S form?
4 bonds
What does molecular orbital theory describe?
It describes covalent bond formation arising from a mathematical combination of atomic orbital to form molecular orbitals.
And what do molecular orbitals describe?
a region of space where electrons are most likely to by found
if you take two singly-occupied 1s orbitals of H atoms and combine them to form molecular orbitals, you can get _____.
addition
What must you do for a subtractive combination of atomic orbitals?
add the opposite phases
The additive combination is _____ _____ _____ than the atomic orbitals.
lower in energy
The subtractive combination cannot have electrons where?
in the central bonding region because there's a node
What's another term for additive combinations?
sigma-bonding
What's another term for subtractive combinations?
sigma-antibonding
The additive combination is _____ _____ _____ than the atomic orbitals.
lower in energy
The subtractive combination cannot have electrons where?
in the central bonding region because there's a node
What's another term for additive combinations?
sigma-bonding
The additive combination is _____ _____ _____ than the atomic orbitals.
lower in energy
The subtractive combination cannot have electrons where?
in the central bonding region because there's a node
What's another term for subtractive combinations?
sigma-antibonding
What's another term for additive combinations?
sigma-bonding
What's another term for subtractive combinations?
sigma-antibonding