You can tell the difference between 1s subshell and 3s subshell using quantum numbers and electron configuration.
Transfer of an electron from a higher energy orbit (2s) to a lower energy orbit (1s) is not possible because it would violate the energy conservation principle. Electrons naturally occupy the lowest available energy levels in an atom, following the Aufbau principle. This means electrons will only move to higher energy levels if they absorb energy, not by transferring between lower and higher energy levels.
The 2s subshell has a higher energy level than the 1s subshell due to the presence of more nodes in the 2s orbital, which increases its energy. Additionally, the 2s orbital has a larger principal quantum number (n) than the 1s orbital, leading to greater distance from the nucleus and therefore higher energy.
It is due to the increased in the effective nuclear charge in argon. Helium has 2 protons in its nucleus. On the other hand, argon has 18 protons in its nucleus.Therefore, it has greater attractive power. Due to this, all the electrons are pulled closer to nucleus.
the 1s orbital is closer to the nucleus and has a lower energy level compared to the 2s orbital. Additionally, the 2s orbital has a slightly higher energy, larger size, and can hold more electrons than the 1s orbital.
An element cannot have 4 electrons in the 2 s level. The s subshell can hold only TWO electrons. Carbon has 4 electrons in the 2p level, however, if that's what you meant.
The K shell is the first shell in an atom and has only one subshell, which is the 1s subshell. This subshell can hold up to 2 electrons.
Transfer of an electron from a higher energy orbit (2s) to a lower energy orbit (1s) is not possible because it would violate the energy conservation principle. Electrons naturally occupy the lowest available energy levels in an atom, following the Aufbau principle. This means electrons will only move to higher energy levels if they absorb energy, not by transferring between lower and higher energy levels.
The 2s subshell has a higher energy level than the 1s subshell due to the presence of more nodes in the 2s orbital, which increases its energy. Additionally, the 2s orbital has a larger principal quantum number (n) than the 1s orbital, leading to greater distance from the nucleus and therefore higher energy.
The absolute difference is 1.
It is due to the increased in the effective nuclear charge in argon. Helium has 2 protons in its nucleus. On the other hand, argon has 18 protons in its nucleus.Therefore, it has greater attractive power. Due to this, all the electrons are pulled closer to nucleus.
/1s going upward the others going strait ways.=D
in even parity number of 1s is even called even parityand or number of 1s is odd called odd parity anil kuntal anil kuntal you suck
Oh, dude, like, sodium has 11 electrons, right? So, it's got 3 subshells: 1s, 2s, and 2p. Each subshell can hold a certain number of electrons based on some fancy rules, but who really cares about that, right? Just know that sodium's got 3 subshells chillin' in there.
An atom with five electrons in the n = 3 energy level is typically phosphorus (P), which has the electron configuration of 1s² 2s² 2p⁶ 3s² 3p³. In this configuration, the 3s subshell contains 2 electrons, and the 3p subshell contains 3 electrons, totaling five electrons in the third energy level.
The element with five electrons in the third energy level (n=3) is phosphorus (P). In its electron configuration, phosphorus has the atomic number 15, with the distribution of electrons as 1s² 2s² 2p⁶ 3s² 3p³. Thus, it has five electrons in the third energy level (2 in the 3s subshell and 3 in the 3p subshell).
the 1s orbital is closer to the nucleus and has a lower energy level compared to the 2s orbital. Additionally, the 2s orbital has a slightly higher energy, larger size, and can hold more electrons than the 1s orbital.
An element cannot have 4 electrons in the 2 s level. The s subshell can hold only TWO electrons. Carbon has 4 electrons in the 2p level, however, if that's what you meant.