sol Quantum numbers describe an electrons shell.pdf

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sol Quantum numbers describe an electron\'s shell number, sublevel, orbital, and spin. Each electron in an atom has a unique set of quantum numbers that cannot be duplicated by any other electron in the atom. The first quantum number, n, tells you which shell the electron is in. n is always a positive whole number, so it could be 1, 2, 3, 4, etc . If the electron is in the first shell (the shell closest to the nucleus), then n = 1 for that electron. n increases for electrons in higher shells. The second quantum number, L, tells you what sublevel the electron is in. Recall that there are four common sublevels in atoms. The value of L is also an integer. It can be anywhere from 0 to n - 1. So in n = 1, L can only be 0. If n = 2, L can be 0 or 1. If n = 3, L can be 0, 1, or 2. The value of L corresponds to a particular sublevel. For example, if an electron is in an s-type sublevel, then its L value is 0. If it\'s in a p-type sublevel, its L value is 1. d-sublevel electrons have L = 2 and f-sublevel electrons have L = 3. The third quantum number, m, tells you which orbital an electron is in. Each of the sublevels is further divided into orbitals, which are regions of probability where electrons exist. The value of m can be anywhere from -L to +L. If L = 0 (s-type sublevel), there is only one possible value of m: 0. . If L = 1 (p- type sublevel), then there are three possible values of m: -1, 0, and +1. If L = 2 (d-type sublevel), there are five possible values of m: -2, -1, 0, +1, and +2. If L = 3 (f-type sublevel), there are seven possible values of m: -3, -2, -1, 0, +1, +2, and +3. The last quantum number is the spin quantum number, s. Each of the orbitals described before can hold up to two electrons, but they MUST have opposite spins. The spins are defined as +1/2 and -1/2. By convention, the first electron in an orbital is assigned a spin of +1/2, and the second electron (if there is one) gets a spin of -1/2. Solution sol Quantum numbers describe an electron\'s shell number, sublevel, orbital, and spin. Each electron in an atom has a unique set of quantum numbers that cannot be duplicated by any other electron in the atom. The first quantum number, n, tells you which shell the electron is in. n is always a positive whole number, so it could be 1, 2, 3, 4, etc . If the electron is in the first shell (the shell closest to the nucleus), then n = 1 for that electron. n increases for electrons in higher shells. The second quantum number, L, tells you what sublevel the electron is in. Recall that there are four common sublevels in atoms. The value of L is also an integer. It can be anywhere from 0 to n - 1. So in n = 1, L can only be 0. If n = 2, L can be 0 or 1. If n = 3, L can be 0, 1, or 2. The value of L corresponds to a particular sublevel. For example, if an electron is in an s-type sublevel, then its L value is 0. If it\'s in a p-type sublevel, its L value is 1. d-sublevel electrons have L = 2 and f-sublevel electrons have L = 3. The third .

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from -L to +L. If L = 0 (s-type sublevel), there is only one possible value of m: 0. . If L = 1 (p-
type sublevel), then there are three possible values of m: -1, 0, and +1. If L = 2 (d-type sublevel),
there are five possible values of m: -2, -1, 0, +1, and +2. If L = 3 (f-type sublevel), there are
seven possible values of m: -3, -2, -1, 0, +1, +2, and +3. The last quantum number is the spin
quantum number, s. Each of the orbitals described before can hold up to two electrons, but
they MUST have opposite spins. The spins are defined as +1/2 and -1/2. By convention, the
first electron in an orbital is assigned a spin of +1/2, and the second electron (if there is one) gets
a spin of -1/2.

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95 electrons in the same orbital have different rus values (one is +Yz and another -%),they are said to be paired. Electron Configuration The energy of an electron in a hydrogen (H) atom is determined solely by its principal quantum number n. However for many-electron atoms the orbital energies depend on both the principal quantum number n andthe angular momenfum quantum number /. Thus the energy of the orbitals in a many-electron atom increases in the order: ls < 2s < 2p < 3s a 3p < 4s < 3d < 4p < 5s, and so on. This order is also the order of filling electrons into the orbitals in a many-electron atom. The guiding principle in assigning electrons to the orbitals in a many-electron atom contains a set of three ru1es called the Aufbau principle: 1. Lower-energy orbitals f,rll before higher-energy orbitals. 2. An atomic orbital can contain only two electrons, which must have opposite spins. (Pauli exclusion principle: no two electrons in an atom can have the same four quantum numbers.) 3 . When electrons are assigne d to p, d, or f orbitals, each successive electron enters a different orbital of the subshell, each electron having the same spin as the previous one; this proceeds until the subshell is half-full, after which electrons pair in the orbitals one by one. (Hund's rule: the most stable arrangement of electrons in the subshell is that with the maximum number of unpaired electrons, all with the same spin.) Flame Test The resultant lowest-energy electron configuration is called the ground-state configrnation of the atom. The electrons in the atom's outermost shell are called valance electrons. When the atom absorbs enough energy, one or more of the valance electrons move to a higher energy orbital, and the atom is said to be in an excited state. The excited states are generally short-lived and rapidly decay back to the ground state by releasing radiant energy in the form of light. The energy and frequency of the light that is released during the decay transition depend on the difference in energy between the ground state and the excited state. The energy difference (AQ, the frequency (v), and the wavelength (2) of the light during emission are related by the equation, LE : hv: hclTwhere h ts Planck's constant and c is the speed of light. When the wavelengths of the light emitted fall in the visible region (400-800 nm), colors willbe observed. Atoms of certain elements emit light u'hen the elements or their compounds are heated in a gas flame. The flame takes on a distinctive color detemined by the particular element (flame test). Each atom has its characteristic emission lines, therefore flame tests can be used to detect certain elements in unknown cornpounds. b!L q) Excited state LE: hv: hclT trl Ground state L I t I t t I D D t t D I t , t t t t t I t t t t t t I I \ I 94 the energy of the electron increases, and the electron is farther away from the nucleus. A coliection of orbitals with the same n is called an electr.

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This is actually pretty simple, so I\'ll help explain. Take a given hydrogen atom, but we\'ll use an ionic form that has 5 electrons (as you\'ve stated). Now, for the quantum numbers. The first one, N, is the electron shell in question. Shells work as providing spaces for electron density. The first shell, in which N=1, holds two electrons because it only contains one orbital. N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number of electrons before entering the third shell. Because the ion in question has 5 electrons, its N value is 2. A simple way to calculate the maximum number of electrons in a given atom that occupies a specific shell is to take that shell number, N, square it and multiply the result by two. That is why the maximum quantum number N for an atom whose electrons occupy the third shell is 18 (which is (3^2)2). Onto the next quantum number, which is l. If you understand the order of atomic shells and their orbitals, this is a simple one. The first shell is l=0, which is the \"s\" shell of an atom. s shells can only hold one atomic orbital, which is two electrons. We denote this as \"1s2\". The next shell is 2s, and because we can fill it, it become 2s2.Because we have 5 electrons, we need to keep going up. The next shell is l=1, which is the \"p\" shell. That fits our last electron, so your value for the l quantum number is \"1.\" Now we\'re at the ml quantum number. These are the numbers we assign to the specific orbitals in which electrons reside in, within a given shell. We\'re currently in the p shell, which holds 3 orbitals whose names are -1, 0, and +1. Unless you have a picture of the electron shells, we can only guess that the 5th electron is in any one of these, so the safe bet is to put it into the -1 orbital (though it can really be in any of them). Lastly, the ms quantum number. This denotes the spin on the electron. Up spin is +1/2, whilst down spin is -1/2. Unless you have a picture, I can\'t tell you which way it is spinning, but it\'s a safe guess to say that it\'s up. In sum, your quantum numbers as: 2, 1, 0, (1/2) I hope that helps. (: Feel free to ask any questions. Solution This is actually pretty simple, so I\'ll help explain. Take a given hydrogen atom, but we\'ll use an ionic form that has 5 electrons (as you\'ve stated). Now, for the quantum numbers. The first one, N, is the electron shell in question. Shells work as providing spaces for electron density. The first shell, in which N=1, holds two electrons because it only contains one orbital. N=2 holds two orbitals, which holds four electrons. Combined with N=1, an ion in N=2 has anywhere between 3 (the minimum of N=1, +1 electron) and 8 electrons (the maximum number of electrons before entering the third shell. Because the ion in question has 5 electrons, its N value is 2. A simple way to calculate the maximum number of electrons.

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sol Quantum numbers describe an electrons shell.pdf

1. sol Quantum numbers describe an electron's shell number, sublevel, orbital, and spin. Each electron in an atom has a unique set of quantum numbers that cannot be duplicated by any other electron in the atom. The first quantum number, n, tells you which shell the electron is in. n is always a positive whole number, so it could be 1, 2, 3, 4, etc . If the electron is in the first shell (the shell closest to the nucleus), then n = 1 for that electron. n increases for electrons in higher shells. The second quantum number, L, tells you what sublevel the electron is in. Recall that there are four common sublevels in atoms. The value of L is also an integer. It can be anywhere from 0 to n - 1. So in n = 1, L can only be 0. If n = 2, L can be 0 or 1. If n = 3, L can be 0, 1, or 2. The value of L corresponds to a particular sublevel. For example, if an electron is in an s-type sublevel, then its L value is 0. If it's in a p-type sublevel, its L value is 1. d-sublevel electrons have L = 2 and f-sublevel electrons have L = 3. The third quantum number, m, tells you which orbital an electron is in. Each of the sublevels is further divided into orbitals, which are regions of probability where electrons exist. The value of m can be anywhere from -L to +L. If L = 0 (s-type sublevel), there is only one possible value of m: 0. . If L = 1 (p- type sublevel), then there are three possible values of m: -1, 0, and +1. If L = 2 (d-type sublevel), there are five possible values of m: -2, -1, 0, +1, and +2. If L = 3 (f-type sublevel), there are seven possible values of m: -3, -2, -1, 0, +1, +2, and +3. The last quantum number is the spin quantum number, s. Each of the orbitals described before can hold up to two electrons, but they MUST have opposite spins. The spins are defined as +1/2 and -1/2. By convention, the first electron in an orbital is assigned a spin of +1/2, and the second electron (if there is one) gets a spin of -1/2. Solution sol Quantum numbers describe an electron's shell number, sublevel, orbital, and spin. Each electron in an atom has a unique set of quantum numbers that cannot be duplicated by any other electron in the atom. The first quantum number, n, tells you which shell the electron is in. n is always a positive whole number, so it could be 1, 2, 3, 4, etc . If the electron is in the first shell (the shell closest to the nucleus), then n = 1 for that electron. n increases for electrons in higher shells. The second quantum number, L, tells you what sublevel the electron is in. Recall that there are four common sublevels in atoms. The value of L is also an integer. It can be anywhere from 0 to n - 1. So in n = 1, L can only be 0. If n = 2, L can be 0 or 1. If n = 3, L can be 0, 1, or 2. The value of L corresponds to a particular sublevel. For example, if an electron is in an s-type sublevel, then its L value is 0. If it's in a p-type sublevel, its L value is 1. d-sublevel electrons have L = 2 and f-sublevel electrons have L = 3. The third quantum number, m, tells you which orbital an electron is in. Each of the sublevels is further divided into orbitals, which are regions of probability where electrons exist. The value of m can be anywhere

2. from -L to +L. If L = 0 (s-type sublevel), there is only one possible value of m: 0. . If L = 1 (p- type sublevel), then there are three possible values of m: -1, 0, and +1. If L = 2 (d-type sublevel), there are five possible values of m: -2, -1, 0, +1, and +2. If L = 3 (f-type sublevel), there are seven possible values of m: -3, -2, -1, 0, +1, +2, and +3. The last quantum number is the spin quantum number, s. Each of the orbitals described before can hold up to two electrons, but they MUST have opposite spins. The spins are defined as +1/2 and -1/2. By convention, the first electron in an orbital is assigned a spin of +1/2, and the second electron (if there is one) gets a spin of -1/2.

sol Quantum numbers describe an electrons shell.pdf

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