Determine the element of lowest atomic number that contains a complete d subshell in the ground state. element symbol:

2 answers:

8 0

The component with the most low atomic number that contains a total d-subshell in the ground state is copper. Copper's electron arrangement is [Ar]3d104s1 [ A r ] 3d 10 4 s 1 .

Further Explanation:

atomic number:

The nuclear number or proton number (image Z) of a synthetic component is the quantity of protons found in the core of a particle. It is indistinguishable from the charge number of the core. The nuclear number particularly distinguishes a compound component. In an uncharged iota, the nuclear number is likewise equivalent to the quantity of electrons.

The elemenents of the intermittent table arranged by atomic mass:

atomic Mass Name substance element Number

1.0079 Hydrogen 1

4.0026 Helium 2

6.941 Lithium 3

9.0122 Beryllium 4

atomic number speak to:

The nuclear number (otherwise called the proton number) is the quantity of protons found in the core of an iota. It is customarily spoken to by the image Z. The nuclear number exceptionally distinguishes a substance component. In a particle of impartial charge nuclear number is equivalent to the quantity of electrons.

Meaning of subshell:

A subshell is a subdivision of electron shells isolated by electron orbitals. Subshells are marked s, p, d, and f in an electron design.

Subject: chemistry

Level: High School

Keywords: atomic number, The elemenents of the intermittent table arranged by atomic mass, atomic number speak to, Meaning of subshell.

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ollegr [7]3 years ago

5 0

The element that contains a complete d subshell in the ground state : Cu

<h3>Further explanation </h3>

In an atom, there are energy levels in the shell and sub shell.

This energy level is expressed in terms of electron configurations.

Writing the electron configuration starts from the lowest to the highest subshell's energy level (following Aufbau rules)

Electron filling in subshells using the following sequence

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.

And the element whose electron configuration occupies the sub shell d lies in the transition group or group B in the periodic system

Electrons can move the shell up or down by releasing energy or absorbing energy

So it can be concluded that there are 2 conditions:

Ground state is the state of electrons filling shell with the lowest energy levels.

Excited state is the state of electrons which occupies a higher energy level

In filling electrons in subshell d there are half-full and full rules because of the tendency of electrons to get stability (not following the Aufbau rule)

Example

Cr atomic number 24: [Ar] 4s² 3d⁴ [Ar] 4s¹ 3d⁵

Cu atomic number 29: [Ar] 4s² 3d⁹ [Ar] 4s¹ 3d¹⁰

Mo atomic number 42: [Cr] 5s² 4d⁴ [Cr] 5s¹ 4d⁵

So the element of the lowest atomic number that contains a complete subshell in the ground state has an electron configuration

1s², 2s², 2p⁶, 3s², 3p⁶, 4s¹, 3d¹⁰

which is owned by the element Cu

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