Nitrogen (N) has atomic number 7, so the electron configuration is 1s2 2s2 2p3. The outermost energy level is level 2 (n=2) so there are a total of FIVE electrons in the outermost energy level.
it depends on the atom. for example, if it was nitrogen it would be
< = clockwise > = counterclockwise spin (i don't know how to to arrows)
2s <> 2p<<<
1s <>
The ground state electron configuration for Nitrogen is
1s^2 2s^2 2p^3 ( I apologize . I don't know how to type in superscripts)
or [He] 2s^2 2p^3.
The azimuthal quantum number describes the shape of the molecular orbital - since nitrogen's last electron occupies a p orbital, its azimuthal quantum number is 1.
Nitrogen atom has 7 electrons. The orbital diagram would look like this.^v........^v.....^v.....^
1s2...2s2...2px..2py...
1S22S23P3 1S22S23P3
What is the question.
1s2 2s2 2p3
The orbital diagram for MAgnesium is
there are two shells of electrons in the nitrogen atom that actually have electrons in them, nitrogen has two electrons in the first shell, the S orbital, and five in the outer shell, the P orbital. this causes nitrogen to have a valence shell with five electrons.
The bohr Rutherford diagram for oxygen has 8 protons and 8 neutrons. There are 2 electrons on the first orbital and six on the second. The bohr Rutherford diagram for oxygen has 8 protons and 8 neutrons. There are 2 electrons on the first orbital and six on the second.
orbital diagram of bromine
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orbital diagram for F
No. N2 is diamagnetic, there are no unpaired electrons.
The orbital diagram of platinum, which has an atomic number of 78, would typically show the sequential filling of its electron orbitals. The electron configuration of platinum is [Xe] 4f14 5d9 6s1, indicating the distribution of its 78 electrons into the appropriate energy levels and sublevels based on the aufbau principle.
The electron configuration of nitrogen is 1s^2 2s^2 2p^3. Nitrogen has a total of seven electrons, with two in the 1s orbital, two in the 2s orbital, and three in the 2p orbital.
An orbital diagram is used to show how the orbitals of a subshell areoccupied by electrons. The two spin projections are given by arrowspointing up (ms =+1/2) and down (ms = -1/2). Thus, electronicconfiguration 1s22s22p1 corresponds to the orbital diagram:
The correct orbital diagram for boron would show 5 electrons distributed among the 2s and 2p orbitals. The configuration would be written as 1s^2 2s^2 2p^1.
A vacant d orbital is an orbital that does not contain any electrons. In the context of transition metals, vacant d orbitals can be involved in forming bonds with other atoms or ligands by accepting electrons to achieve stability. The presence of vacant d orbitals is important for explaining the unique chemistry and reactivity of transition metal complexes.
The orbital diagram for MAgnesium is
2p
Elements with a 6s1 electron include francium (Fr) and cesium (Cs). In the orbital diagram, the 6s1 electron would be represented as a single arrow pointing upwards in the 6s orbital.
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