There are 7 elements that satisfy this definition:
Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen and Flourine.
Lithium atom
Lithium
aluminum
P
Nitrogen
In Neon atom the 10 electrons are present in two principal energy levels, 2 in ist and 8 in 2nd level.
when an electron moves from excited state to ground state it emits photons of wavelength equal to the difference between the two energy levels. Consider a hydrogen atom. If the electron is at the second energy level in the atom (the energy of this level is -3.4 eV )it can stay there for about only 10^-8 s and then after that it just to the level below .If it jumps from second to ground state (energy of ground state is -13.6 eV) it emits aphoton of energy = 13.6-3.4 =10.2 eV. .............................Gho$t
No element has this as the ground state. Gadolinium has the right number of electrons but its ground state is [Xe] 4f7 5d1 6s2. The second number in each group should be a superscript.
I think it will be zinc. The electron configuration of zinc is: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10 Add up the electrons. 2+2+6+2+6+2+10 = 30 electrons in all, which is the element zinc. As you can see frorm the above electron configuration, all the electrons for the third energy level are filled: 3s2 is filled; 3p6 is fully filled; 3d10 is fully filled. I really hope this helps and doesn't confuse you... :)
Your question reveals a common confusion between orbitals and shells. Chlorine has three electron shells: the first, second and third. The first shell has just the one orbital, the 1s The second shell has two sub-shells, the 2s and the 2p. There are three p orbitals in the 2p sub-shell. Each orbital can hold two electrons, so there are eight electrons maximum in the second shell. The third shell likewise has two sub-shells, the 3s and the 3p, but the 3p is not completely filled, leaving room for one more electron. When chlorine gains this electron it will become a Cl- ion. This is summed up in the electron configuration 1s22s22p63s23p5.
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.
No. It has two shells with 2 and 1 electron each. The second shell is unfilled.
The fourth electron shell is filled by krypton. Krypton is the last element in the fourth period on the periodic table. Each of the periods represents an electron shell. Elements in the first period have electrons in the first shell; elements in the second period have electrons in the second shell; and so on.
In Neon atom the 10 electrons are present in two principal energy levels, 2 in ist and 8 in 2nd level.
An electron in the third shell has more energy than an electron in the second shell.
If an electron is in the second principle energy level, that is, n = 2, then that electron could be in an s or p orbital.
when an electron moves from excited state to ground state it emits photons of wavelength equal to the difference between the two energy levels. Consider a hydrogen atom. If the electron is at the second energy level in the atom (the energy of this level is -3.4 eV )it can stay there for about only 10^-8 s and then after that it just to the level below .If it jumps from second to ground state (energy of ground state is -13.6 eV) it emits aphoton of energy = 13.6-3.4 =10.2 eV. .............................Gho$t
No element has this as the ground state. Gadolinium has the right number of electrons but its ground state is [Xe] 4f7 5d1 6s2. The second number in each group should be a superscript.
I think it will be zinc. The electron configuration of zinc is: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10 Add up the electrons. 2+2+6+2+6+2+10 = 30 electrons in all, which is the element zinc. As you can see frorm the above electron configuration, all the electrons for the third energy level are filled: 3s2 is filled; 3p6 is fully filled; 3d10 is fully filled. I really hope this helps and doesn't confuse you... :)
Because with the 2nd ionisation of K, you are trying to take an electron from a fully filled orbital (octet rule) whereas with calcium it is getting down to a fully filled orbital
It does.
Your question reveals a common confusion between orbitals and shells. Chlorine has three electron shells: the first, second and third. The first shell has just the one orbital, the 1s The second shell has two sub-shells, the 2s and the 2p. There are three p orbitals in the 2p sub-shell. Each orbital can hold two electrons, so there are eight electrons maximum in the second shell. The third shell likewise has two sub-shells, the 3s and the 3p, but the 3p is not completely filled, leaving room for one more electron. When chlorine gains this electron it will become a Cl- ion. This is summed up in the electron configuration 1s22s22p63s23p5.