BSES 26 Flashcards

1
Q

they represent the probability of finding an electron in any one place. they correspond to the different energies. so an electron in an orbital has definite energy. orbitals are best described with quantum mechanics

A

orbitals

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2
Q

the region in space just outside the nucleus of the atom where the probability of finding the electrons is at the highest (95%)

A

atomic orbitals

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3
Q

formed as a result from the overlap of two atomic orbitals, wherein a pair of electrons occupying.

A

molecular orbitals

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4
Q

a measure of the probability of finding an electron in an orbital.

A

electron density

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5
Q

mathematical description of the volume of space occupied by an electron having a certain amount of energy

A

wave function

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6
Q

is the place where a crest and a trough of energy

A

a node in an orbital

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7
Q

is based on the wave properties of matter. quantization of energy is the consequence of these properties

A

quantum mechanics

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8
Q

the energy levels about the nucleus contain group

A

atomic orbitals

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9
Q

atomic orbitals are designates as

A

s, p, d, and f

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10
Q

what are the three p orbitals of equal energy

A

px, py, and pz

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11
Q

the number describes the energy level that the electron occupies. it can have a value of 1-7. this defines the “level” of the electron

A

principal quantum number

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12
Q

this number describes the shape of the orbital that the electron is found in. it can have a value from 0-3. this defines the “sublevel” of the electron. also, the numbers can be replaced by letters according to the following:

0 = S
1 = P
2 = D
3 = F

A

orbital (azimuthal) quantum number

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13
Q

this number describes the orientation of the electron in the orbitals. this defines the “orbital” of the electron. there are 2L+1 orbitals in each sublevel.

A

magnetic quantum number

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14
Q

this number describes the direction of spin of the electron in the orbital

A

spin quantum number

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14
Q

are spherical regions where the probability of finding an electron is zero

A

radial nodes

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14
Q

it states that no two electrons may have the same set of quantum numbers

A

pauli exclusion and the build up principles

15
Q

result from the combination of atomic orbitals

A

molecular orbitals

16
Q

is an indicator of the bond strength and length. a bond order of 1 is equivalent to a single bond. fractional bond orders are possible

A

bond order

17
Q

hybridization is a major players in this approach to bonding

A

valence bond theory

18
Q

there are two ways orbitals can overlap to form bonds between atoms

A

valence bond theory

19
Q

head-to-head overlap

A

sigma bonds

20
Q

cylindrical symmetry of an electron density about the internuclear axis

A

sigma bonds

21
Q

side-to-side overlap

22
Q

electron density above and below the internuclear axis

23
defined as the concept of mixing two atomic orbitals to give rise to a new type of hybridized orbitals. this intermixing usually results in the formation of hybrid orbitals having entirely different energy, shapes, etc.
hybridization
24
an extension of the valence bond theory, and it helps us to understand the formation of bonds, bond energies, and bond lengths
hybridization
25
redistribution of the energy of the energy of orbitals of individual atoms to give orbitals of equivalent energy happens when two atomic orbitals combine to form a hybrid orbital in a molecule.
hybridization
26
observed when one s and one p orbital in the same main shell of an atom mix to form two new equivalent orbitals
sp hybridization
27
observed when one s and two p orbitals of the same shell of an atom mix to form 3 equivalent orbitals
sp2 hybridization
28
when one s orbital and 3 p orbitals belonging to the same shell of an atom mix together to form four new equivalent orbitals
sp3 hybridization
29
involves the mixing of 1s orbitals, 3p orbitals, and 1d orbital to form 5
sp3d hybridization
30
arrangement of sp
linear
31
arrangement of sp2
triangular planar
32
arrangement of sp3
tetrahedron
33
arrangement of sp3d
triangular bipyramid
34
sp measurement
180 degrees
35
sp2 measurement
120 degrees
36
sp3 measurement
109.5 degrees
37
sp3d measurement
90 and 120 degrees