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What is the number of valence electrons an element wants to be stable?
Exactly enough to fill all the orbitals of their outermost (valence) shell:Hydrogen and Helium only have an s orbital in their outer shell, this shell is filled with 2 electronsAll other elements have an s orbital and 3 p orbitals in their outer shell, each orbital can take 2 electrons so this shell is filled with 8 electrons
Do all elements in row 6 have 6 electrons in the outer most shell?
No, not at all. The row tells you the energy level of the outermost electrons. So, in row 6 (Period 6) all the elements have electrons in the 6th energy level. The number of electrons in the outer shell is given by the group number (column).
Is each shell limited to a maximum of four electrons?
1st shell=2 2nd shell=8 3rd shell=18 4th shell=32 5th shell=32 6th shell=18 7th shell=8
How many electrons are in a radium atom?
The number of electrons in a radium atom is usually 88. If it goes though bonding however, it will tend to lose those two outer electrons, and become a radium ion. If it bonds with oxygen, which has 6 outer electrons, it will lose the two outer electrons it has to become a radium ion with a full outer level of 86 electrons, and oxygen will get a complete outer level of 8 electrons. Radium will become Ra2+, a typical radium ion, also known as Radium 86, as it loses 2 electrons.
Can an electron jump from sixth shell to second shell?
No, electrons cannot jump from the sixth shell to the second shell in an atom. Electrons fill shells in a specific order based on their energy levels, and they follow certain rules and restrictions regarding their movements within an atom. Jumping from the sixth shell to the second shell would violate these principles.
What is the number of valence electrons an element wants to be stable?
Exactly enough to fill all the orbitals of their outermost (valence) shell:Hydrogen and Helium only have an s orbital in their outer shell, this shell is filled with 2 electronsAll other elements have an s orbital and 3 p orbitals in their outer shell, each orbital can take 2 electrons so this shell is filled with 8 electrons
What noble gas possesses 6 electrons in the 6th energy level?
No noble gas possesses 6 electrons in the 6th energy level. Noble gases have a stable electron configuration with a full valence shell. Helium has 2 electrons in its first and only energy level, while neon has 10 electrons in its second energy level.
How many electrons are in each shell for silicon 1-6?
1st shell: 2 electrons, 2nd shell: 8 electrons, 3rd shell: 8 electrons, 4th shell: 4 electrons, 5th shell: 0 electrons, 6th shell: 0 electrons.
How many valance electrons does oxygen have?
Oxygen has 6 valence electrons. A person can determine the number of valence electrons by looking at the periodic table. since oxygen is in the 6th column form the left, it has 6 valence electrons.
What is the principal quantum number the n for the valence electrons in lead?
The principal quantum number for valence electrons in lead is 6, because lead has 6 valence electrons in the 6th energy level.
Do all elements in row 6 have 6 electrons in the outer most shell?
No, not at all. The row tells you the energy level of the outermost electrons. So, in row 6 (Period 6) all the elements have electrons in the 6th energy level. The number of electrons in the outer shell is given by the group number (column).
In a Bohr diagram how many electrons are in each shell?
There are 4 electron sub-shells: s, p, d, and f. These letters stand for sharp, principal, diffuse, and fundamental, but the names are not important. s subshells have 2 electons, while p subshells have 6, d subshells have 10, and f subshells have 14. There can be higher subshells, but these subshells require too much energy to fill and no element with a g subshell (the next subshell after f) has ever been synthesized. The first shell (i.e. the first period of the periodic table) has only s. Thus, the first shell has 2 electrons. The second shell has s and p subshells, so it has 2+6 or 8 electrons. The third shell has s, p, and d subshells. It ultimately has 18 electons. This can be misleading, however. The d subshell requires more energy to fill than the higher-shell s subshell. This is why the third period of the periodic table does not have a d section: the d electron subshell of the third Bohr shell does not fill until after the s subshell of the fourth Bohr shell has filled. Looking at the periodic table, you can see that the third period only has 8 electrons, while the 4th period has 18. The 18 electrons in the fourth period are the s subshell of the fourth shell, the d subshell of the 3rd shell, and the p subshell of the 4th shell. The fourth shell is similar to the third shell, but more extreme. The fourth shell has s, p, d, and f subshells, but the f subshell is not filled until two higher s shells have been filled. It does, however, fill out to 32 electrons in the 6th period of the periodic table. In the 6th period, the first period to have 32 electrons, there are 32 electrons, filling these subshells: s subshell of the 6th shell, f subshell of the 4th shell, d subshell of the 5th shell, and then the p subshell of the 6th shell. The fifth shell would ultimately fill out to a full 50 electrons and would do so in the 8th period of the periodic table. However, as previously noted, no substance has ever been found or generated with that many electrons. It would fill the s subshell of three shells above (i.e. shell 8) before it filled the g subshell of shell 5. No element in the 8th period has ever been synthesized, so a filled fifth Bohr shell has never been found. A good example for a Bohr diagram would be Astatine, which is in the 6th period. In the first shell of the Bohr diagram, you have 2 electrons (s subshell only). It is filled completely. In the second, you have 8 electrons (s and p subshells) and in the third you have 18 electrons (s, p, and d), and both shells are filled completely. In the fourth shell, you have 32 electrons (s, p, d, and f), and it is filled completely. In the fifth shell, you have 18 electrons. This is because only the s, p, and d subshells are filled. It would require too much energy to fill the f subshell of the 5th shell, so the electrons just go to the s, p, and d subshell of higher shells. The 6th shell has 7 electrons. The 2 electrons of the s subshell are filled first, and then 5 electrons go into the p shell.
Is each shell limited to a maximum of four electrons?
1st shell=2 2nd shell=8 3rd shell=18 4th shell=32 5th shell=32 6th shell=18 7th shell=8
How many electrons must a barium atom lose to form an ion with noble-gas configuration?
Two electrons are donated by Barium to an oxidant (nonmetal, eg. O2) by which barium gets oxidised.Ba --> Ba2+ + 2e-This is because Ba is in group 2 of the periodic system, belonging to the 'earth alkali' metals and so it has 2 electrons (2e-) in its valency (or outer) shell (2,8,18,18,8,2). Hence Ba2+ configuration is (2,8,18,18,8,-), with an empty (-) 6th shell (the 'P' shell) like Xenon.
How many electrons are in a radium atom?
The number of electrons in a radium atom is usually 88. If it goes though bonding however, it will tend to lose those two outer electrons, and become a radium ion. If it bonds with oxygen, which has 6 outer electrons, it will lose the two outer electrons it has to become a radium ion with a full outer level of 86 electrons, and oxygen will get a complete outer level of 8 electrons. Radium will become Ra2+, a typical radium ion, also known as Radium 86, as it loses 2 electrons.
Can an electron jump from sixth shell to second shell?
No, electrons cannot jump from the sixth shell to the second shell in an atom. Electrons fill shells in a specific order based on their energy levels, and they follow certain rules and restrictions regarding their movements within an atom. Jumping from the sixth shell to the second shell would violate these principles.
What is the electron configuration of potassium hydroxide?
K-O-H the potassium and hydrogen are in the first group of the periodic table of elements and therefor only need one set of electrons. oxygen is in the 6th, and therefor has 6 valence electrons. The oxygen also has 2 pairs of unshared electrons. K-O-H , oxygen has 2 pairs of unshared electrons.
