Q&A for How to Write Electron Configurations for Atoms of Any Element

An electron configuration is the arrangement of electron of an atom or a molecule in an atomic or molecular orbital.

CH4 isn't an atom, but a composite substance. You can only tell the electron configuration of an atom.

When writing the EC, we consider the energy levels of the shells. 3d has higher energy level than 4s, therefore it will come after 4s. You need to memorize the order of orbitals according to the energy levels.

Ionization energy is the quantity of energy that an isolated, gaseous atom in the ground electronic state must absorb to discharge an electron, resulting in a cation.

Because in every shell, no matter what atom, they all hold the same number of electrons.

You basically take the traditional boxed configuration and write it in numbers where the first number represents the energy level (i.e 1s^2 is the first energy level) and the superscript represents the number of electrons in that energy level (in the previous example the "^2" means that there are 2 electrons in that energy level).

The Latin name of iron is ferrum.

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2. You basically take the traditional, boxed configuration and write it in shorthand where the first number represents the energy level and the superscript represents the number of electrons in that energy level (box).

The atomic number of carbon is 6. Hence, it's configuration is [He] 2s2 2p2. The expanded form is 1s^2 2s^2 2p^2.

Because electron configuration gives the number of valence electrons, by which we can easily determine the chemical properties of an atom or ion or molecule or compound.

Scandium has three valence electrons, because it is on the third column of the periodic table.

On the periodic table there are 18 groups. Each group has a specific charge. For example, any element in group 17 has a 1- charge.

It is not the compounds that hold the valencies. Rather the combining atoms or ions possess different valencies.

The first shell can hold 2 electrons; the second and third can hold 18; and the fourth can hold 32 electrons.

The full electron configuration of barium is: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 6s2.

To know the number of neutrons you need to know the atomic number and mass. Atomic number equals the number of protons, and atomic mass roughly equals protons plus neutrons, so just subtract the atomic number from atomic mass to get the number of neutrons.

The atomic number of iron (ferrous) is 26. Hence it's electronic configuration is [Ar] 3d6 4s2. The expanded form is 1s^2 2s^2 2p^6 3s^ 2 3p^6 4s^2 3d^6.

Nowhere. You shouldn't put commas in an electron configuration.

Check out the wikiHow article, Find the Empirical Formula .

The electrons are taken from the 4d subshell because it is incomplete. The 4d subshell should have 10 electrons, not 3, which means 7 electrons were taken from it.

We can only find the electronic configuration of monoelectronic atoms (the atoms that contain only one electron in their valence shell) by using a Bohr model. It was the defect of the Bohr model that it was only applicable to monoelectronic atoms.

1s2 2s2 2p6 3s2 3p6 3d10 4s1 is the electronic configuration of atoms having 29 electrons; the name of this atom is copper (Cu), and it has an atomic number of 29.

The quantum number is refered to as the outermost valence electrons of the carbon atom, which are loctaed in the 2p atomic orbital.

If you are only counting the electrons in the 3rd shell, then there will be 8 electrons. If you are counting all of the electrons on the 1st, 2nd and 3rd shell, then it will be 18 electrons.

It was taken from its Latin name "ferrum," and we take the first letters as a symbol for the element.

Ionization enthalpy, or ionization energy, is the energy needed to remove the outermost, or loosest, electron from an atom. This is measured in kJ/mol or eV-.

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^1 is the electronic configuration of potassium.

The Aufbau principle states that electrons fill atomic orbitals of the lowest energy levels before moving onto higher energy levels.

We can find the number of electrons an atom holds by using the formula 2n^2, where 'n' is the number of shell of an atom. For example: for first shell value of 'n' will be 1 and it can accommodate only 2 electrons and for second shell value of n will be 2 and it will accommodate 8 electrons in the valence shell.

The atomic number determines the location of the element in the periodic chart.