Orbital Filling and Lewis Dot Diagrams

What does the Pauli Exclusion Principle state?

• When two electrons are sharing an orbital, they must spin in opposite directions.

• No more than one electron can occupy an orbital.

• Electrons always spin in the same direction.

What is Hund's Rule?

• Electrons do not share orbitals unless they have to; when you have one electron in each of multiple orbitals, they must spin in the same direction.

• Electrons always share orbitals; when you have one electron in each of multiple orbitals, they must spin in the same direction.

• Electrons do not share orbitals unless they have to; when you have one electron in each of multiple orbitals, they must spin in OPPOSITE directions.

Sublevel f has 7 orbitals.  If you have less than 7 electrons in the 5f sublevel you...

• still need to show all 7 orbitals, even if they are empty.

• only show the orbitals that contain electrons.

• pair the electrons so that you use fewer orbitals.

For an oxygen atom, how many total orbitals contain at least one electron?

• 5

• 4

• 2

When using the shortcut to write an electron configuration, what group of element must be shown in square brackets?

• Noble Gas

• Halogen

• Alkali Metal

When doing an orbital diagram, you must label your orbitals with the energy level and sublevel.

• True

• False

Which electrons in Bismuth have the most energy (Hint: think about the Aufbau principle)?

• The electrons in 6p

• The electrons in 4f

• The the electrons in both 6s and 6p

When drawing a Lewis Dot diagram for an element, you are showing only the electrons...

• in the highest energy level

• in the last sublevel

• in the first sublevel

When drawing a Lewis Dot Diagram, you should put the electrons...

• One on each side (left, right, top, & bottom) of the element symbol before you pair them up

• equally distributed around the element symbol.

• radiating out from the element symbol.

For transition metals (Groups 3-12), how many valence electrons should there be?

• 2

• varies by element

• 3 or more