Transition Metals

How many electrons can fit into the d subshell (all the d orbitals) in one electron shell?

• 10

• 5

• 2

• 20

How many possible d orbitals are there in one shell?

• 10

• 5

• 2

• 18

How many electrons can fit in an orbital?

• 2

• 5

• 10

• 18

Electrons fill orbitals:

• starting with the lowest energy and filling up

• starting with the highest energy and filling down

• starting from the left side of the atom

• in whatever order they're written

Orbitals in a subshell should be filled

• with a single electron each before pairing electrons

• with pairs, and then with single electrons if any are left

• with as many electrons as they can fit

• with 8-10 electrons before moving on

Electron subshells are most stable

• with all orbitals full or all empty

• with orbitals exactly 3/4 full

• with orbitals exactly 3/4 empty

• with orbitals exactly 1/2 full

If not all electron subshells can be full or empty, the next-most stable e- configuration is:

• an exactly 1/2 full subshell

• an exactly 3/4 full subshell

• an exactly 1/4 full subshell

• an exactly 3/2 full subshell

Predict how the valence electrons in iron metal (iron 0) should be organized.

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Tags

NGSS.HS-PS1-1

This is iron⁰. It loses 3e^- to become iron³⁺. Use stability rules to find its new e^- config.

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Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Use your stability and filling rules to predict Cu⁰'s valence shell. (4s and 3d subshells)

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