how many electrons in each principal energy level?
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Each principal energy level can contain up to 2n2 electrons, where n is the number of the level. Thus, the first level can contain up to 2 electrons, 2(12) = 2; the second up to 8 electrons, 2(22) = 8; the third up to 18, 2(32) = 18; and so on.
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A neutral atom with atomic number 20 will have 20 electrons. The atomic number is, by definiton, the number of protons in an atom's nucleus but for a neutral atom it's also equal to the number of electrons. Each element has a different, unique number of protons that determines its identity.
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Valence electrons are electrons in the highest principal energy level. They are electrons that sit on the outermost orbit of an element. They are responsible for bonding and chemical properties of each element.
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Thus, the third level holds a maximum of 18 electrons: 2 in the s orbital, 6 in the three p orbitals, and 10 in the five d orbitals. The fourth and higher levels also have an f sublevel, containing seven f orbitals, which can hold a maximum of 14 electrons.
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The first principal energy level contains only an s sublevel; therefore, it can hold a maximum of two electrons. Each principal energy level above the first contains one s orbital and three p orbitals. A set of three p orbitals, called the p sublevel, can hold a maximum of six electrons.
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As there are 4 sub shells, those will be :- s,p,d,f giving a total of = 1+3+5+7= 16 orbitals and 1 electrons for each orbital with ms= -1/2 and +1/2 each.. Thus there will be 16 such electrons.
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The first energy level has 2 electrons located in the 1s-orbital and the second energy level, which in fluorine's case is the outermost energy level, has 7 electrons, 2 in the 2s-orbital and 5 in the 2p-orbitals. This means that fluorine has a total of 7 valence electrons.
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Regardless of its shape, each orbital can hold a maximum of two electrons. Energy level I has just one orbital, so two electrons will fill this energy level. Energy level II has four orbitals, so it takes eight electrons to fill this energy level.
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Phosphorus has a filled 2nd principal energy level. The 2nd principal energy level can only hold 8 electrons, 6 in the p orbitals and 2 in the s orbital.
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1 Answer. There are seven electrons in the highest occupied energy level of a chlorine atom. These electrons occupy the s and p sublevels, and make up the valence shell.
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Note you are only looking at the orbitals with the specified n value, not those at lower energies. (a) When n = 2, there are four orbitals (a single 2s orbital, and three orbitals labeled 2p). These four orbitals can contain eight electrons.
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The number of valence electrons are equal to the number of electrons in the outermost shell of the atom. The atomic number of sulphur is 16, and therefore the sulphur atom has 16 electrons in its orbits. The first shell can have a maximum of 2 electrons, and the second shell a maximum of 8 electrons.
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Therefore, a maximum number of 10 electrons can share these two quantum numbers in an atom. These electrons are located on the third energy level, in the 3d subshell.
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Christopher P. A neutral chlorine atom has 17 protons (atomic number 17) and 17 electrons. The first two electrons are located in the 1s orbital. In the second energy level, two electrons are located in the 2s orbital, and six electrons in the three 2 p orbitals.
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Answer and Explanation: There are three orbitals in the 2p sublevel. These three orbitals can hold two electrons each for a total of six electrons.
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['The number of protons in the nucleus of the atom is equal to the atomic number (Z).', 'The number of electrons in a neutral atom is equal to the number of protons.']
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When the third energy level has 8 electrons, the next 2 electrons go into the fourth energy level. The electrons in the energy level farthest from the nucleus are called valence electrons. Atoms in the same column (group) in the periodic table have the same number of valence electrons.