What determines which state an electron is actually in when an atom is in its ground state? 10

Depends on 2 laws.

The first is the law of lowest energy, which states that electrons are always in the lowest possible state (because the atom is in the ground state), which is "as low energy as possible".

The second is the Pauli incompatibility principle, which states that it is impossible for 2 electrons to be in the same state.

The state of motion of electrons includes the state of space motion and spin.

For example, there are 6 states of motion of electrons outside the nucleus of a c atom and 4 states of space motion of electrons outside the nucleus. The state of motion of electrons is the number of electrons. The state of space motion of electrons is the number of orbitals.

The state of motion of electrons outside the nucleus. It is determined by four aspects: the electron shell in which the electron is located, the shape of the atomic orbital, the extension direction of the atomic orbital, and the spin of the electron. The number of states of motion of electrons outside the nucleus is the atomic number.

For example, potassium with atomic number 19 has 19 different states of motion in the outer electrons of the nucleus.

There are no two electrons in an atom that are in exactly the same state of motion, so there are as many electrons as there are electrons in the state of motion.

The state of motion of the electrons depends on:

Principal quantum number (electron shell).

Angular quantum number (electron sublayer).

Magnetic quantum number (electron orbital).

Spin quantum number (spin direction of electrons).

The electrons of ground state atoms can occupy a range of energy levels and orbitals, with different states of space motion. Here are a few common states of space motion of electrons in ground state atoms:

S orbital: The s orbital is spherically symmetrical and the electrons move in a spherically symmetrical manner in this orbital. Each principal quantum number n corresponds to an s orbital, where n represents the magnitude of the energy level. For example, the electrons of the hydrogen atom in the ground state are located in the 1s orbital.

P-tracks: P-tracks are tracks with three different directions, which are px, py, and pz. These orbits appear two nodes in space, distributed along different axes. Each principal quantum number n corresponds to three p-orbitals, such as 2p orbitals.

D-tracks: D-tracks are tracks with five different directions, which are dxz, dyz, dxy, dx2-y2, and dz2 tracks. These tracks appear multiple nodes in space and have more complex shapes.

Each principal quantum number n corresponds to five d orbitals, such as 3d orbitals.

These are several common space-moving bond states that describe the way electrons move in an atom. Each orbital can hold a different number of electrons, and the filling order and number of electrons of each orbital in the ground state are determined according to the rules of electron configuration, such as Pauli's incompatibility principle and Hunt's rule. The atoms and elements of different Sidlion may have different energy level structures and electron distributions.

According to the results of atomic spectroscopy experiments and the analysis and induction of the periodic system, the basic principle of electron distribution outside the nucleus is summarized.

1. Pauli (Pauli) incompatibility principle.

In the same atom, it is impossible to have four electrons with exactly the same quantum number. A maximum of two electrons with opposite spin directions can be accommodated in each orbital.

2. The principle of lowest energy.

When the multi-electron atom is in the ground state, the distribution of electrons outside the nucleus is always distributed in the lower energy orbit first without violating Pauli's principle, so that the atom is in the lowest energy state.

3. Hund rule.

When atoms distribute electrons in equivalent orbitals of the same sublayer, they will be distributed in different orbitals as much as possible, and the spin direction will be the same (or spin parallelism). When distributed in this way, the energy of the atoms is lower and the system is more stable.

In general, the center atom hybridization = the number of lone pairs of the center atom + the number of healthy atoms, the number of lone pairs refers to the logarithm.

CO20+2=2, two hybrid orbitals are required, so it is sp hybridization, O2, 2+1=3, sp2 hybridization.

CO1+1=2, sp hybridization.

The unpaired electrons you are talking about appear in some molecular radicals, such as NO, this unpaired electron is arranged in the pi orbital between nitrogen and oxygen atoms, the so-called three-electron pi bond (there is an electron arranged in pi*, the antibond orbital, so the bond order is, the pi orbital does not need to be considered in hybridization, and the formula uses "the number of healthy atoms" to only consider the sigma bond. So for NO, nitrogen and oxygen each have a lone pair of electrons, both are 1+1=2, sp hybrid. To sum up, unpaired electrons are bonded, lone pairs count as one sigma bond, and the number of hybrid orbitals is the total number of sigma bonds needed.

Look at the distribution of electrons in the outermost and sub-outer shells, and arrange the electrons according to Hunt's rule and the Poly incompatibility principle.

The following electronic manuscript of the ground state atom is in the bond segment configuration or in, the correct one is () the correct answer: c