Enter the orbital diagram for the ion Cd2+ Drag the appropriate labels to their respective targets_ Labels can be used once; more than once; Or not at all Not all group 2 targets will be filled: Reset Help 62 62 62 G2

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Orbital Diagram for Cd²⁺ (Cadmium Ion)

Step-by-step Explanation:

1. Atomic Number of Cd (Cadmium):

Cadmium has an atomic number of 48, so its neutral atom has 48 electrons.

2. Electron Configuration of Neutral Cd:

The electron configuration of neutral cadmium is:

makefileCopyEditCd: [Kr] 4d¹⁰ 5s²

This includes:
- The [Kr] core (36 electrons)
- Fully filled 4d subshell (10 electrons)
- Fully filled 5s subshell (2 electrons)

3. Formation of Cd²⁺ Ion:

To form Cd²⁺, two electrons are removed.
Electrons are always removed first from the highest energy orbitals, which are the outermost s and p orbitals.

In this case:

The 5s² electrons are removed.
The 4d¹⁰ electrons remain untouched.

So the configuration becomes:

lessCopyEditCd²⁺: [Kr] 4d¹⁰

4. Orbital Diagram for Cd²⁺:

The orbital diagram shows how electrons fill orbitals by energy level and subshell.

We’ll write out the orbital diagram from lowest to highest energy subshells up to 4d (since 5s is empty in Cd²⁺).

CopyEdit1s ↑↓
2s ↑↓
2p ↑↓ ↑↓ ↑↓
3s ↑↓
3p ↑↓ ↑↓ ↑↓
4s ↑↓
3d ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p ↑↓ ↑↓ ↑↓
4d ↑↓ ↑↓ ↑↓ ↑↓ ↑↓

Each arrow represents an electron.
Each box (or group of two arrows) represents an orbital.
All orbitals below 4d are fully filled.
The 4d subshell has 10 electrons, fully filled.
No electrons in 5s or above for Cd²⁺.

5. Summary Explanation

Cadmium (Cd), atomic number 48, is a transition metal with the electron configuration [Kr] 4d¹⁰ 5s². When cadmium forms a +2 ion (Cd²⁺), it loses two electrons. According to the rules of electron removal, electrons are lost first from the outermost (highest principal quantum number) orbitals. For Cd, the electrons in the 5s orbital (n=5) are the outermost and therefore are the first to be removed, leaving the configuration [Kr] 4d¹⁰.

This means the Cd²⁺ ion has a fully filled 4d subshell, which is a relatively stable configuration. The loss of 5s electrons results in a more compact ion with a positive charge, but the inner core (including the 4d electrons) remains intact. This filled 4d shell explains why Cd²⁺ does not typically exhibit variable oxidation states, unlike many other transition metals.

The orbital diagram of Cd²⁺ shows full occupancy of all orbitals up to and including the 4d subshell. All lower orbitals (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p) are also fully filled, maintaining a stable electronic structure. This makes Cd²⁺ a diamagnetic ion, as all electrons are paired. Understanding orbital diagrams helps visualize electron configurations and explains the chemical behavior of ions, including bonding, magnetism, and reactivity.

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