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CHEM 431 > Lecture 2 (Electronic Structure, Atomic Orbitals, etc.) > Flashcards

Lecture 2 (Electronic Structure, Atomic Orbitals, etc.) Flashcards

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1
Q

The region of space defined by Ψ is called an …

A

atomic orbital

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2
Q

What are 3 quantum numbers atomic orbitals are characterized by?

A

Principle (energy), Orbital (shape), Magnetic (directionality)

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3
Q

What is a node?

A

A point where the electron probability is zero.

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4
Q

What are the types of nodes?

A

Angular and Radial

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5
Q

How many angular nodes are in s orbital?

A

0 angular nodes

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6
Q

How many angular nodes are in p orbitals?

A

1 angular node

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7
Q

How many nodes in d orbitals?

A

2 angular nodes

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8
Q

How many nodes are in f orbitals?

A

3 angular nodes

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9
Q

What is the type for the remaining nodes?

A

radial

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10
Q

What does triply degenerate mean?

A

3 orbitals all have the same energy

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11
Q

What degenerate are s orbitals?

A

singly degenerate

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12
Q

What degenerate are p orbitals?

A

triply degenerate

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13
Q

What degenerate are d orbitals?

A

five-fold degenerate

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14
Q

What degenerate are f orbitals?

A

seven-fold degenerate

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15
Q

What is the VSEPR geometry of PH3

A

Trigonal pyramidal

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16
Q

Why do trigonal pyramidal structures of heavy pnictogen hydrides have narrow bond angles?

A

The orthogonal p orbitals and the lone pair hosted in an orbital with mainly s character.

17
Q

What is the “inert par effect”?

A

When heavier elements are less likely to have hybridization (mixing) of orbitals

18
Q

What is the radial component of a wavefunction associated with?

A

size of the orbitals

19
Q

What is the trend of the radial component?

A

it decays exponentially as the distance from the nucleus increases

20
Q

What is one thing that changes in radial nodes?

A

the signs (+/-)

21
Q

What is 4πr^2R(r)^2?

A

The radial probability of finding the electron in a given region of space.

22
Q

What is the radial probability when the electron is at the nucleus?

A

zero for all orbitals

23
Q

What happens when you increase n?

A

orbitals become larger and diffuse more, as the electrons they hosted are distributed over a larger region of space

24
Q

What is a consequence because of this?

A

the orbitals overlap for heavier elements is less efficient and the bonds formed are weaker.

25
Q

What elements are the exceptions for radial distribution function?

A

NOF (nitrogen, oxygen, and fluorine)

26
Q

Why is NOF an exception for radial distribution function?

A

The repulsion between non-bonding lone pairs are brought closer due to reduced covalent radius, leading to weaker bonds.

CHEM 431 (21 decks)

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