Use the periodic table to write the electron configuration...

Use the periodic table to write the electron configuration for each element. Represent core electrons with the symbol of the previous noble gas in brackets.
a. $\mathrm{P}$
b. Ge
c. $\mathrm{Zr}$
d. I

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Key Concepts

Orbital Filling Order

Electrons populate orbitals in an order determined by their increasing energy levels, following guidelines such as the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. This order ensures the most stable electron configuration for each element.

Noble Gas Notation

This is a shorthand method for writing electron configurations by using the electron configuration of the closest preceding noble gas to represent core electrons. It simplifies the notation and emphasizes the valence electrons, which are most important in chemical reactions.

Electron Configuration

This describes the distribution of electrons among the various orbitals of an atom, indicating how electrons fill shells and subshells based on energy levels. It is essential for understanding the chemical behavior and bonding of elements.

Periodic Table

The periodic table is a systematic arrangement of elements based on increasing atomic number and recurring chemical properties. It provides the necessary data such as electron count and periodic trends needed to determine electron configurations.

Transcript

00:01 When writing the electron configuration for all of these elements, we're going to shorten the configuration by putting the previous noble gas in brackets.

00:10 This is therefore saying that it's full up through this noble gas and also these extra orbitals.

00:17 So let's just walk through all four of them.

00:20 So starting with p.

00:22 P has a black dot on it, which corresponds to this black mark here, just to be clear throughout all of these.

00:28 So for p we go back to the previous noble gas, which is neon and e, we put n e in brackets.

00:36 And then we go over to the first two electrons here, which are in the s orbital.

00:43 So since this is the third s orbital down, we say 3 s2, and that's full.

00:50 So we move over to the p orbital.

00:52 And if this was a noble gas, we would expect all six to be filled.

00:56 But for p, we have 1, 2, 3 electrons that are unpaired.

01:01 So it'll be bracket and e 3s2, 3b3.

01:07 Moving on to the next one, we have germanium.

01:10 Once again, we're going to go all the way back and find the most recent noble gas.

01:14 That's argon, ar.

01:15 So you're going to put that in brackets.

01:18 And then once again, we're going to move down and look at the s orbitals.

01:21 We're one row down, so that means we're now in the 4s orbital instead of the 3s...

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