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What do you mean by the orbitals of lower energy are filled in first with the electron and only then the orbitals of high energy are filled?
Wiki User
∙ 15y ago
Because the electrons have a negative charge and the nucleus has a positive charge, so they attract each other. The electrons stay in the orbital closest to the nucleus unless it is full or they have enough energy to move away from the nucleus.
Wiki User
∙ 12y ago
Wiki User
∙ 15y agoThis is part of Hund's Rule which states that electrons will always fill the lowest possible position in an orbital. All this means is that (for example) an electron won't fill a 2s orbital before it fills a 1s orbital.
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Where does electron exist in an atom?
Electrons exist in the electron cloud that surrounds the nucleus of an atom. This cloud is made up of the various orbitals that hold the electrons. Orbitals are regions of space in which the probability of finding an electron is the highest. The electrons orbit the nucleus in these orbitals and can move from one orbital to another as they gain or lose energy. 1s Orbital: This orbital is closest to the nucleus and can hold up to two electrons. 2s Orbital: This orbital is farther away from the nucleus and can hold up to two electrons. 2p Orbitals: These orbitals are even farther away from the nucleus and can hold up to six electrons. 3s Orbital: This orbital is farthest away from the nucleus and can hold up to two electrons. 3p Orbitals: These orbitals are even farther away from the nucleus and can hold up to six electrons. 3d Orbitals: These orbitals are the farthest away from the nucleus and can hold up to ten electrons.These orbitals are filled in a specific order with the 1s orbital being filled first then the 2s 2p 3s 3p and finally the 3d orbitals. The electrons in the outermost orbitals are called valence electrons and are responsible for the chemical properties of the atom.
How many orbitals would be filled in an atom with an atomic number 17?
There are 5 completely filled orbitals. -------- actually there are 2 completely filled orbital shells in an argon atom the first has a max of two (filled) the second a max of 8 (filled) the third a max of 32 (missing 24)
How many orbitals are im the first energy level?
One only - 1s.
How many half filled orbitals are in a arsenic atom?
Arsenic has three electrons occupying the three 4p orbitals in its valence shell. Hund's first rule tells us that they will each occupy separate orbitals before they start to pair up. So there are three half-filled orbitals in an arsenic atom.
What is the number of electrons in each subshell for the electron configuration of an arsenic atom?
Neutral arsenic has 33 protons and 33 electrons. The first 33 electron orbitals are filled as 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3. The superscripts above these subshells is the number of electrons in them.
The order in which atomic orbitals are filled is based on what factor?
It is based on many factors, but the easiest to understand is ENERGY. The orbitals in which the electron has the lowest energy are filled FIRST.
How many unpaired electrons does phosphorus have in its 3p sub level?
3. Orbitals are filled one electron at a time, putt ting electrons into the lowest energy orbitals first. When there are degenerate orbitals ( having the same energy e.g. p and d orbitals) they tale one un paired electron each first and then and then any extra electrons are added into a half filled orbital to make a spin pair. P has a configuration of [Ne] 3s2 3p3 and there are only three p orbitals ( at any energy level)
How many half-filled orbitals are there in a carbon atom?
Looking at the electron configuration of carbon (at. no. 6) you have 1s2 2s2 2p2. In the 2 p subshell, you have 1 electron in the 2px orbital, and 1 electron in the 2py orbital and no electrons in the 2pz orbital. So, the answer is that there are TWO half filled orbitals in the carbon atom. This is the case BEFORE hybridization. After hybridization, there are FOUR half filled orbitals which are called sp3 hybrids.
What is the area surrounding the atom where electrons are located?
Its called the electron shell. Electrons will always fill up low orbitals first in the shell, an then as more energy is added to the atom, the electrons move up an orbit, then release the energy in some form, and they move back down to the lowest energy orbit.
Why is second electron affinity for halogens is zero?
All of the halogens are one electron short of having all of their atomic orbitals filled to reach an atom's state of nirvana. This explains why, in general, halide chemistry is such that halogens so willingly literally accept one electron in their ionic formulations and formally accept one electron or share a pair of electrons in the vast majority of their predominately covalent compounds. Halogens have no affinity for accepting a second electron because once a halogen atom has accepted once electron, all of its atomic orbitals each contain two electrons and are thus full. Any element with all its atomic orbitals filled has the equivalent electronic configuration of a noble gas and is in its most stable electronic state.What follows is very important to understand. It appears that many chemistry students do not know this fact probably because most textbooks and instructors do not explicitly point it out or they do a poor job emphasizing it: Elements only possess the atomic orbitals defined by the row in which an element exists in the Periodic Table.In many compounds, a particular element may possess one or more empty atomic orbitals in its electronic ground state. Students who have completed the first semester of general chemistry were presented with, and expected to understand, what atomic orbitals each element has. They should also know the order in which a given element's orbitals are progressively occupied by electrons when that element is in its ground electronic state and that orbitals with the lowest energy are filled first. It is also important to understand that the theoretical order of atomic orbitals in elements heavier than argon may be in a different order. This effect, when it occurs, is due to electron-electron repulsions about the element's nucleus.Let's look at a 2nd row element as an example. How about nitrogen? Because it's a 2nd row element, nitrogen has two "shells" of atomic orbitals and a total of five orbitals; however only electrons in the outer shell of orbitals may participate in chemical bonding. The 1st shell of electrons consists only of the 1s orbital. Like all atomic orbitals, the 1s orbital can hold a maximum of two electrons, which is denoted by the superscript in the orbital's designation, as in 1s2. Starting from the 1st element in the 2nd row and counting each element up to and including nitrogen shows that the outer shell of orbitals on nitrogen contains five electrons. Assuming that no electron-electron interactions alter the respective theoretical energy levels of the five orbitals (This does not occur in any of the 2nd row elements), the atomic orbitals on nitrogen are, in increasing energy: [1s2], 2s2, 2px1, 2py1, 2pz1. The three 2p orbitals have the same energy and are filled with one electron first before any of them takes on a second electron. Note that the first p orbitals, and the ones lowest in energy, are the 2p orbitals. There is simply no such thing as a 1p orbital. The 2p orbitals could have been named 1p orbitals. Everyone who first applied quantum mechanics to the hydrogen atom in order to describe its atomic emission spectrum, and, not long thereafter, the number and energy levels of an atom's electrons, are no longer with us. Nevertheless, the reason for the seemingly strange numerical designations is almost certainly because the quantum numbers that are solutions to the wave equation corresponding to the number and shape of the atomic orbitals begin with "2" for the p orbitals, "3" for the d orbitals, etc., and perhaps the people who discovered and published all of these findings decided not to change the numerical designations.The point I hope I made is that the five atomic orbitals shown for nitrogen are all it has. In addition to s and p atomic orbitals, there exists d and f orbitals, but not for nitrogen or any other second-row element. Therefore, once the 2s and 2p orbitals are filled, nitrogen cannot accept or share another additional electron because there is no atomic orbital in which it can be placed.
How many p orbitals are occupied by electrons in sulfur atom.?
Sulfur has two electrons in the 1s orbital, two electrons in the 2s orbital, and 6electrons in the 2 p orbitals. The electrons are part of the first and second energy levels, the electron core. The next energy level, the last one, is the outermost energy which comprises the valence shell.
Do electrons exist in orbitals?
No. An orbital describes an energy level (a Fermi energy level) in which an electron may exist for a given atom. Just because an electron is not in that orbital does not mean one cannot go there. An easy example would be ionized neon gas in a lamp. The high voltage forces electrons into higher orbitals where they check in and then check out, dumping a photon as they leave. The orbitals existed before they were used. Orbitals are clearly defined for a given atom as the descrete energy levels into which electrons may shift if they gain a sufficient (an exact) quantity of energy to make the jump.
Where does electron exist in an atom?
Electrons exist in the electron cloud that surrounds the nucleus of an atom. This cloud is made up of the various orbitals that hold the electrons. Orbitals are regions of space in which the probability of finding an electron is the highest. The electrons orbit the nucleus in these orbitals and can move from one orbital to another as they gain or lose energy. 1s Orbital: This orbital is closest to the nucleus and can hold up to two electrons. 2s Orbital: This orbital is farther away from the nucleus and can hold up to two electrons. 2p Orbitals: These orbitals are even farther away from the nucleus and can hold up to six electrons. 3s Orbital: This orbital is farthest away from the nucleus and can hold up to two electrons. 3p Orbitals: These orbitals are even farther away from the nucleus and can hold up to six electrons. 3d Orbitals: These orbitals are the farthest away from the nucleus and can hold up to ten electrons.These orbitals are filled in a specific order with the 1s orbital being filled first then the 2s 2p 3s 3p and finally the 3d orbitals. The electrons in the outermost orbitals are called valence electrons and are responsible for the chemical properties of the atom.
How many elecrtons shells would be filled by a neutral xenon atom?
The first 3 energy levels are filled, the 4s and 4p and 4d sublevels are filled, and the 5s and 5p sublevels are also filled. So only the first three energy levels are completely filled. The fourth and fifth energy levels are partly filled. The electron configuration is 1s22s22p63s23p63d104s24p64d105s25p6 or [Kr]4d105s25p6.
Why 4s has one electron and 3d has 5 electrons?
The electronic configuration of atoms is based on the filling of orbitals. In the case of the 4s orbital, it is relatively lower in energy than the 3d orbital, so it is filled first. Therefore, the 4s orbital can accommodate a maximum of 2 electrons. As for the 3d orbitals, they have a higher energy level and can accommodate a maximum of 10 electrons, but in the case of transition metals, only 5 electrons fill the 3d orbitals due to electron configuration stability.
Are the outer electron shells always filled first?
No. The inner shells are filled first.
What does the electron configuration of neon look like?
Neon's atomic number is 10. Thus, to be neutral, it must have 10 protons and 10 electrons. The first 10 electrons are filled into orbitals as 1s2 2s2 2p6.
