Enter the orbital diagram for the ion au+.

Write orbital diagram for Au+. Determine if the ion is diamagnetic or paramagnetic.

General guidance

Concepts and reason
The number of unpaired electrons for any free atoms or ions can be determined by using the orbital diagram.
An orbital diagram is the pictorial representation of shells in an atom by using square boxes (one box for s-orbital, three boxes for p-orbitals, five boxes for d-orbitals and seven boxes for f-orbitals) those boxes are filled by electrons using the following principles: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle.

Fundamentals

Aufbau Principle:
In a neutral atom, the ground state electron configuration is obtained experimentally by using spectroscopy methods. The Aufbau principle is also called as the building up principle.
Hund’s Rule:
In subshells such as p, d, and f, electrons accommodate each orbital first with a single electron before pairing up when they are in the same energy level.
Pauli Exclusion Principle:
No two or more electrons can have the same values of four quantum numbers in the atom.
Orbital:
An orbital is a region where the finding probability of an electron is the highest in the shell.
Electron configuration:
The distribution of electrons of an atom or a molecule in the atomic or molecular orbitals is known as electronic configuration.
Orbital diagram for X: it has seven electrons in its outermost orbitals.

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Step-by-step

Step 1 of 2

(1)
The given transition metal is gold, .
And its oxidation state of metal is.

Orbital diagram for :

Part 1
Hence, the orbital diagram for ion is as follows:

The ground state electron configuration of gold, is. The monovalent gold cation has one electron less than that of a neutral gold atom. In this orbital diagram for gold cation, d-orbitals and f-orbitals are completely filled with pair of electrons but s-orbital is none.

Make sure that the valence electron is removed from the s-orbital in the ground state electron configuration. For example,
Incorrect:

Correct:

Find the number of unpaired electrons for .

Step 2 of 2

(2)

The number of unpaired electrons is zero from the orbital diagram because all other orbitals are filled fully except 6s orbital. So, the ion is diamagnetic.

Part 2
Therefore, cation is diamagnetic in nature.

The number of unpaired electrons is found by using the orbital diagram shown in the above step. All the orbitals are completely filled with pair of electrons except 6s orbital. So, the given metal cation is diamagnetic in nature.

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Take care while counting number of unpaired electrons, paired electrons and empty orbitals. For example,
Correct:

Incorrect:

Answer

Part 1
Hence, the orbital diagram for ion is as follows:

Part 2
Therefore, cation is diamagnetic in nature.

Answer only
Part 1
Hence, the orbital diagram for ion is as follows:

Part 2
Therefore, cation is diamagnetic in nature.

Ground state electron configuration for Au: 7. Au : 1s%2s²2p3s²3pº3d” 4s²4p 4d’ 5s-5p4f”50″6s’ Excited state electron configuration for Au* ion : ,Aut : 1s²2s²2p%3s 3p%3d” 4s24pº4d”°58²5p®48’45d”
Outer electron configuration for Aution: 7, Au* : [Kr]4f5d”
6S PS JD Uษษษษษ โรง โรงงาน ระโนโ]
1s 2s 2p 3s 3p 3d”4s24p4d05s5p4f5d”6s’
Ground state electron configuration for Au: 7. Au : 1s%2s²2p3s²3p%3d”° 4s²4p 4d” 5s-5p° 4151″6s’ Excited state electron configuration for Aution: Au” : 1s²2s²2pⓇ3s 3p%3d” 4s²4p4d’° 5s²5p®4f45dº6s’
Ground state electron configuration for Au: 7. Au : 1s%2s²2p3s²3pº3d” 4s²4p 4d’ 5s-5p4f”50″6s’ Excited state electron configuration for Au* ion : ,Aut : 1s²2s²2p%3s 3p%3d” 4s24pº4d”°58²5p®48’45d”
Number of unpaired electrons=0 Number of paired electrons=11 Number of empty orbital=1
Number of unpaired electrons=0 Number of paired electrons=11 Number of empty orbital=1
Number of unpaired electrons=1 Number of paired electrons=12 Number of empty orbital=0
6S PS JD Uษษษษษ โรง โรงงาน ระโนโ]
6S PS JD Uษษษษษ โรง โรงงาน ระโนโ]
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Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic. Write orbital diagram for Au+.
Determine if the ion is diamagnetic or paramagnetic.

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