For the ground state electronic configuration of Sodium-Na, we bear in mind that the atom is not excited. It is neutral and has not lost or gained any electron.
Sodium has 11 electrons and belongs to the first group on the periodic table. It is an alkali metal with a valency of one.
The ground state configuration of sodium is given as: 1S²2S²2P⁶3S¹
Answer : The ground state electronic configuration of sodium will be,
Electronic configuration : It is defined as the representation of electrons around the nucleus of an atom.
Number of electrons in an atom are determined by the electronic configuration.
Atomic number : It is defined as the number of electrons or number of protons present in a neutral atom.
The ground state electronic configuration of sodium will be,
The total number of electrons = [2 + 2 + 6 + 1] = 11
the total should equal 31 for gallium and the orbital before the valence orbital should not be filled for an excited state.
Atomic Number: 11
Atomic Mass: 22.98977 amu
Melting Point: 97.72 °C (370.87 K, 207.9 °F)
Boiling Point: 883 °C (1156 K, 1621 °F)
Number of Protons/Electrons: 11
Number of Neutrons: 12
Classification: Alkali Metal
Crystal Structure: Cubic
Density @ 293 K: 0.971 g/cm3
Option (C) is the correct answer.
Atomic number of neon is 10 and its electronic configuration is .
As neon has a vacant 3s orbital also. Therefore, in the excited state an electron will jump into the excited energy level. So, in excited state of neon one electron will jump into the 3s orbital.
Hence, its electronic distribution in the valence shell will become 2-7-1.
Thus, we can conclude that 2-7-1 electron configuration represents the electrons of an atom of neon in an excited state.
An atom is in an excited state when it is very close to having a full octet (either it gains or loeses electrons to get a full octet). The first shell should have two electrons and the next one and the one after that should be eight. Since the third shell has 7 electrons it needs to gain one more electron to get a full octet. Therefore the answer is 3
Answer is: (3) 2–8–17–6.
1) This is ground state of sodum atom.
Electron configuration of sodium atom: ₁₁Na 1s² 2s² 2p⁶ 3s¹.
Atomic number of sodium is 11, it means that it has 11 protons and 11 electrons, so atom of sodium is neutral.
2) This is ground state of sulfur atom.
Sulfur electron configuration: ₁₆S 1s²2s²2p⁶3s²3p⁴.
Sulfur has six valence electrons (3s²3p⁴), in 3s orbital, two electrons are paired, in 3p orbital, two electrons are paired and two are unpaired.
4) This is ground state of arsenic atom.
Electron configuration of arsenic atom:
₃₃As 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³.
An electron configuration shows the arrangement of electrons around the nucleus of an atom. At the ground state (the most stable state for electrons) the electron configuration of chlorine is 2-8-7. Chlorine is a halogen that contains 17 electrons, to attain a stable configuration chlorine requires to gain 1 electron.
-At the excited state chlorine will therefore have an electron configuration of 2-8-8.
Electron configuration represents an excited state : (3) 2–8–17–6Further explanation
In an atom there are levels of energy in the shell and sub shell
This energy level is expressed in the form of electron configurations.
Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub-shells in the shell of an atom, namely s, p, d and f. The maximum number of electrons for each sub shell iss: 2 electrons p: 6 electrons d: 10 electrons and f: 14 electrons
Charging electrons in the sub shell uses the following sequence:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
Determination of electron configurations based on principles:1. Aufbau: Electrons occupy orbitals of the lowest energy level 2 Hund: electrons fill orbitals with the same energy level 3. Pauli: no electrons have the same 4 quantum numbers
According to Niels Bohr, electrons surround the nucleus of an atom on a path called the electron shell. Each shell has an energy level. The further from the core, the higher the energy level
Maximum electrons of shells :K shell: 2 electrons L shell: 8 electrons M shell: 18 electrons N shell: 32 electrons O shell: 50 electrons P shell: 72 electrons
The maximum number of electrons in each shell can be formulated = 2n² (n = shell number)
Electrons can move the shell up or down by releasing energy or absorbing energy
Excited electrons show higher electron transfer to the shell by absorbing energy
So it can be concluded that there are 2 conditions :
Ground state is the state of electrons filling skins with the lowest energy levels.
Excited state is the state of electrons which occupy a higher energy level
The state of excited electrons can be seen from the presence of electrons which do not fill the skin completely but fill the skin afterwards
From the electron configuration , option 3 shows the excitation of one electron in the M shell towards the N shell, which should have a configuration in the ground state:
electrons and atomic orbitals
about subatomic particles statement
Keywords: electron configurations, the shell of atoms, excited state
In this case, an excited state means is referred to the valence electron that has moved from its lower state orbital, at which the lowest available energy is present, to another orbital with higher energy.
In this manner, any electron configuration in which the last electron is located at an orbital with higher energy, stands for an element at an excited state. For instance, looking at the lower state of nitrogen, the resulting electron configuration turns out:
Now, by exciting the element, an electron could occupy a large number of orbitals. Nonetheless, it will occupy the next available one, as shown below:
Wherein the valence electron is now at the orbital in the so called excited state.