# What are the electron configurations for I and N3?

The atomic number—the total number of electrons in the ground state—and oxidation state of an element determine the electron configurations.

When considering oxidation states for elements that are not in the ground state, one can simply use the notation "n+" to indicate the removal of n electrons from the total number of electrons of the ground state element, or "n-" to indicate the addition of n electrons.

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Iodine (I) has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5. The nitride ion (N3-) has the following electron configuration: 1s^2 2s^2 2p^6.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

- Which element has the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d3?
- How does the number of valence electrons change as you look down a column of the table?
- What is the maximum number of electrons in the second principal energy level?
- What is the electron configuration of Ag?
- What are the possible quantum numbers for the last (outermost) electron in Ca ? (Z=20)

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