Electron Orbitals And Electronic Configurations Flashcards Preview

Introduction To Biochemistry > Electron Orbitals And Electronic Configurations > Flashcards

Flashcards in Electron Orbitals And Electronic Configurations Deck (19)
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0
Q

Define orbit.

A

A single pathway where a past and future electron location can be predicted.

1
Q

Define orbital.

A

A 3D region around the nucleus where you can find an electron 90% of the time.

2
Q

Why are models used in chemistry?

A

To help understand atomic properties and behaviour.

3
Q

Why can’t past and future electron locations be predicted?

A

Because there are multiple pathways.

4
Q

How many electrons can an orbital shape host at any given energy level?

A

Two.

5
Q

Why are electronic orbitals a more sophisticated model?

A

They represent electrons distribution in space.

6
Q

Orbitals are contained into shells numbered what?

A

1, 2, 3 and 4.

7
Q

What four things determine the shape of an electronic orbital?

A
  1. The number of electrons it contains. 2. The proximity of other orbitals. 3. The distance from the nucleus. 4. The energy carried by the electron.
8
Q

How many electrons can a S shell hold?

A

2.

9
Q

How many electrons can a P shell hold?

A

6.

10
Q

How many electrons can a D shell hold?

A

10.

11
Q

How many electrons can a F shell hold?

A

14.

12
Q

State four reasons why electrons do not spiral down the nucleus.

A
  1. Electrons are equally constrained by each other. 2. Electron size is minuscule in relation to the nucleus and its orbital. 3. Orbital theory predicts that a “caged” electron (orbital small enough to overlap with the nucleus) will require immense energy. 4. Electrons precipitate into the nucleus under some conditions (inverse beta decay).
13
Q

Define the Aufbug principle.

A

Orbitals fill in order of increasing energy levels.

14
Q

Define Hund’s rule.

A

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.

15
Q

Define Pauli’s exclusion principle.

A

Individual orbitals can hold a maximum of two electrons with opposite spin.

16
Q

How do you remember the order orbitals and shells fill?

A
17
Q

What an opposite spins diagram look like? How do they fill?

A
18
Q

What part of the periodic table does the s, p, d and f shells belong to?

A