Write the electron configurations of Co, Co 2+ , and Co 3+ .

Hello, everyone in this video, I want to provide the condensed electron configurations for S E and the most stable ion that forms. So SE an atomic number of 34 and the closest noble gas is going to be argon. So we'll put it back. It's a are there reading cross Pura table, we have four S two, three D 10. Since we're in the D orbital, we always go N minus one And then four p 4. So that's it for S E now, for the most stable ion parts while S season group is six, unless you write this out S E, we're in group 6 8. And because of this, it forms minus two ions by beginning two electrons. So we're adding onto electrons into this configuration here. So S E two minus is the mostly I on the forms. And the electron configuration for this is going to be again, closest noble gas is argon four S 23 D 10. And then we're adding two electrons to the P here, that's gonna be four plus two is six. So again, this is going to be the condensed electron configuration for S M and this right here is going to be the electron configuration of condensed electron configuration for S E with its most staple ion.

Ch.3 Ionic Compounds

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Ch.3 Ionic Compounds

Problem 55

Chapter 3, Problem 55

Write the electron configurations of Co, Co²⁺, and Co³⁺.

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Determine the atomic number of cobalt (Co) from the periodic table. Cobalt has an atomic number of 27, meaning it has 27 electrons in its neutral state.

Write the electron configuration for neutral cobalt (Co) by filling the orbitals in order of increasing energy, following the Aufbau principle. The order is: 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁷. Thus, the configuration for Co is:

1s22s22p63s23p64s23d7

For Co²⁺, remove two electrons from the highest energy orbitals. Since the 4s orbital is higher in energy than the 3d orbital, remove the two 4s electrons. The electron configuration for Co²⁺ is:

1s22s22p63s23p63d7

For Co³⁺, remove one additional electron from the 3d orbital (since it is now the highest energy orbital). The electron configuration for Co³⁺ is:

1s22s22p63s23p63d6

Review the configurations to ensure they follow the principles of electron filling (Aufbau principle, Hund's rule, and Pauli exclusion principle) and confirm that the correct number of electrons has been removed for each ion.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill lower-energy orbitals first, and is typically represented using the notation of subshells (s, p, d, f). Understanding electron configurations is essential for predicting an element's chemical behavior and reactivity.

Transition Metals

Cobalt (Co) is a transition metal, which are elements found in the d-block of the periodic table. Transition metals are characterized by their ability to form variable oxidation states and complex ions due to the involvement of d electrons in bonding. This property is crucial for understanding the electron configurations of cobalt in its different ionic forms.

Oxidation States

Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost, gained, or shared. For cobalt, the oxidation states of +2 and +3 correspond to the loss of two and three electrons, respectively. This affects the electron configuration, as the removal of electrons typically occurs from the outermost orbitals, influencing the chemical properties of the ion.