Question

What Answers to my question

Answer 1

Chromium (Cr):

• Electronic Configuration: [Ar]
  `3d^5 4s^{1`

• Box Notation: 4s¹ 3d⁵
• Valence Electrons: 6 (5 from 3d and 1 from 4s)
• Number of Paired Electrons: 5 (all from 3d)
• Number of Unpaired Electrons: 1 (from 4s)

Copper (Cu):

• Electronic Configuration: [Ar]
  `3d^(10) 4s^{1`
• Box Notation: 4s¹ 3d¹⁰
• Valence Electrons: 11 (10 from 3d and 1 from 4s)
• Number of Paired Electrons: 10 (all from 3d)
• Number of Unpaired Electrons: 1 (from 4s)

Bromine (Br):

• Electronic Configuration: [Ar]
  `3d^(10) 4s^2 4p^5`
• Box Notation: 4s² 3d¹⁰ 4p⁵
• Valence Electrons: 7 (2 from 4s and 5 from 4p)
• Number of Paired Electrons: 6 (2 from 4s and 4 from 4p)
• Number of Unpaired Electrons: 1 (from 4p)

Rubidium (Rb):

• Electronic Configuration: [Kr]
  `5s^1`
• Box Notation: 5s¹
• Valence Electrons: 1 (from 5s)
• Number of Paired Electrons: 0
• Number of Unpaired Electrons: 1 (from 5s)

Zirconium (Zr):

• Electronic Configuration: [Kr]
  `4d^2 5s^2`
• Box Notation: 5s² 4d²
• Valence Electrons: 4 (2 from 4d and 2 from 5s)
• Number of Paired Electrons: 2 (from 5s)
• Number of Unpaired Electrons: 2 (from 4d)

The box notation is a simplified way to represent the electron configuration. It shows the distribution of electrons among the orbitals of an atom. The superscript indicates the number of electrons in the orbital.

For example, in Chromium (Cr), the 4s orbital has 1 electron and the 3d orbital has 5 electrons. The number of valence electrons is the total number of electrons in the outermost shell of an atom. These are the electrons that are involved in chemical reactions.

The number of paired and unpaired electrons can be determined from the box notation. Paired electrons are those that share an orbital with another electron, while unpaired electrons are those that occupy an orbital alone.