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Explanation: . Ethene, or , has a carbon-carbon single and double bond.Recall that a bond **can** be found in hybridized orbitals whereas a bond cannot. This means that the carbon atoms in ethene hybridize the single βsβ **orbital** and two of the βpβ orbitals, forming a hybridization. The bonds are found in these three hybridized orbitals.The remaining unhybridized βpβ **orbital** will house the. A) The principal **quantum number** (n) describes the shape of an **orbital**. B) The angular momentum **quantum number** (l) describes the the size and energy associated with an **orbital**. C) The magnetic **quantum number** (m l) describes the orientation of the **orbital**. D) An **orbital** is the path that an electron follows during its movement in an atom. Transcribed Image Text: An electron in a hydrogen atom has **orbital** angular momentum **quantum number** = 6. What is the smallest total angular momentum **quantum number** it **can** have? Submit Answer What is the highest total angular momentum **quantum number** it **can** have. total angular momentum Submit Answer The electron is replaced by a negatively. -The **quantum number** / indicates the shape of an **orbital**-The **quantum number** n indicates the principal energy level of an **orbital**-The relative size of the **orbital** is indicated by the value of n. The angular momentum **quantum number**, /, indicates the _____ of the orbits in an atom. A value of / = 0 indicates a(n) _____ type **orbital** while a d **orbital** is indicated by an / for _____. The principal **quantum number** gives the **following** information: ... This **quantum number** directs the magnitude of the **orbital** angular momentum. Therefore, it is also called. Jul 19, 2022 Β· **Quantum** **number** may be defined as a set of four **numbers** with the help of which we **can** get complete information about all the electrons in an atom, i.e., location, energy, the type of occupied, shape, and orientation of the **orbital**, etc. **Quantum** **numbers** distinguish different orbitals based on size, shape, and orientation in space.. Transcribed Image Text: An electron in a hydrogen atom has **orbital** angular momentum **quantum number** = 6. What is the smallest total angular momentum **quantum number** it **can** have? Submit Answer What is the highest total angular momentum **quantum number** it **can** have. total angular momentum Submit Answer The electron is replaced by a negatively. **Which** **of** **the** **following** sets of **quantum** **numbers** is correct for an electron in \\( 4 \\mathrm{f} \\) **orbital** ?(a) \\( n=4, \\ell=3, m=+1, s=+1 / 2 \\)(b) \\( n=4, \\el. No two electrons in an atom **can** have the same set of four **quantum numbers**, in other words, βOnly two electrons may exist in the same **orbital** and these electrons must have. The **orbital quantum number** \(\ell\) indicates the shape of the subshell electron cloud (**orbital** shape). **Which of the following** sets of **quantum numbers** (n,l,ml,ms) refers to a 4s **orbital**? Select one: a. 4,0,0,β12 b. 4,0,1,β12 c. 4,1,1,β12 d. 4,1,0,β12. Get Answers Chief of LearnyVerse (321k points) answered Sep 10, 2021 0 (a) n = 1, l = 0 (Given) The orbital is 1s. (b) For n = 3 and l = 1 The orbital is 3p. (c) For n = 4 and l = 2 The orbital is 4d. (d) For n = 4 and l = 3 The orbital is 4f. ask related question β Prev Question Next Question β Related questions 0 1. The principal quantum number ( π) determines the size of the atomic orbital and the subsidiary quantum ( π) number determines the shape of the atomic orbital. The magnetic quantum number ( π ) determines the direction of the atomic orbital. An s orbital has a spherical shape. We **can** describe those electrons in orbitals using the four **quantum** **numbers**. Let's look at the first **quantum** **number** here. This is called the principal **quantum** **number**. The principal **quantum** **number** is symbolized by n. n is a positive integer, so n could be equal to one, two, three, and so on. It indicates the main energy level occupied by the ....

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m β is known as the ____ **quantum** **number**. Solution: n is the principal **quantum** **number** β is the azimuthal **quantum** **number** m β is the magnetic **quantum** **number** By the way, you sometimes see n labeled as the Principle **Quantum** **Number**. This is an incorrect usage of the word principle. β can also (correctly) be called the angular momentum **quantum**. . Calculates **number** of orbitals and **number** of electrons in different kinds of orbitals for n = 1 to 4. Explains that only two electrons are allowed per **orbital**, and gives shortcuts for calculating **number** of orbitals and total **number** of electrons for a given n.. The magnetic quantum number distinguishes the orbitals available within a subshell, and is used to calculate the azimuthal component of the orientation of orbital in space. Electrons in a particular subshell (such as s, p, d, or f) are defined by values of β (0, 1, 2, or 3). The value of ml can range from -β to +β, including zero. The 1s orbital has quantum numbers n =1, l =0, and ml =0. Both electrons will be in this subshell. Therefore, one electron will have quantum numbers n =1, l =0, ml =0, and ms = +1/2. The other electron will have quantum numbers n =1, l =0, ml =0, and ms =-1/2. Beryllium Beryllium has four electrons which fill the 1s and 2s orbitals. Question 38 1 pts **Which of the following** sets of **quantum numbers** (n,1,m) describe the **orbital** shown below? 0 3,2,-2 3.1.-1 0 2,20 4,3,0 Calculate your paper price Type of paper. Ans: Different** quantum numbers** represent the different characteristics of orbitals like shape, size, and orientation. 1. Principle quantum number- It talks about the electronβs. You know that exact angular momentum L in quantum mechanics is unknown, only magnitude of L (related with orbital quantum number l) and its component along Z (related with magnetic quantum number. Chemistry questions and answers. Each of the **following** sets of **quantum numbers** is supposed to specty an **orbital**. However, each set contains one **quantum number** that is not allowed. Replace the quaintum **number** that is not allowed with one that is allowed. (Each change indicated in red) Part A \ [ \begin {array} {l} n=3, l=3, m t=+2 \\ n=3, l=3, m. Nov 21, 2015 Β· Therefore, a total of five orbitals can share the quantum nubmers n = 4 and l = 2. Finally, for n = 2 and l = 1, you have the second energy level and the 2p-subshell. The values of ml for this subshell are ml = β 1 β this is the 2px orbital* ml = 0 β this is the 2py** orbital** ml = 1 β this is the 2pz** orbital**. Dec 13, 2021 Β· For this to be true, no two electrons in the same atom **can** have the same four **quantum** **numbers**. The Principal **Quantum** **Number** (n) The principal **quantum** **number** (n) describes the electron shell, or the size, of an **orbital**. An electron shell **can** be thought of as the part of an atom where an electron orbits the nucleus. Learn about how Rutherford .... A) The principal **quantum number** (n) describes the shape of an **orbital**. B) The angular momentum **quantum number** (l) describes the the size and energy associated with an **orbital**. C) The magnetic **quantum number** (m l) describes the orientation of the **orbital**. D) An **orbital** is the path that an electron follows during its movement in an atom.

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Explanation for the correct option. (c ) 1. n = 3, l = 2, m = + 2 denotes a 3 d **orbital** containing the magnetic **quantum** **number** + 2. For n = 3, l = 2, we know that m = - 2, - 1, 0, + 1, + 2. No two orbitals have the same magnetic **quantum** **number**. As a result, the provided **quantum** **number** is only achievable for one **orbital** and two electrons.. electrons in the same atom can have identical values for all four of their **quantum** **numbers**. What this means is that no more than two electrons can occupy the same **orbital**, and that two electrons in the same **orbital** must have opposite spins. Because an electron spins, it creates a magnetic field, which can be oriented in one of two directions.

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The value of m l further specifies the orientation of the **orbital** angular momentum, while l ( l + 1) is related to the magnitude of the **orbital** angular momentum. The name magenetic **quantum number** refers to the splitting of the energy eigenvalues for different m l when an external magnetic field is present (Zeeman effect). m β is known as the ____ **quantum** **number**. Solution: n is the principal **quantum** **number** β is the azimuthal **quantum** **number** m β is the magnetic **quantum** **number** By the way, you sometimes see n labeled as the Principle **Quantum** **Number**. This is an incorrect usage of the word principle. β can also (correctly) be called the angular momentum **quantum**. **The** magnetic **quantum** **number**, gives us the total **number** **of** possible **orbitals** within a particular subshell. Given the **following** **quantum** **numbers** n=4,l=1,ml=β1,0,1, what is the subshell of the **orbital**? p For ml values of β1,0 and +1, there are three possible **orbitals** in the shell which indicates a p subshell. Click hereπto get an answer to your question οΈ V3211 The wave function of an atomic **orbital** of H-like atom is - Ynm = 2(3).r.e-Zr/2a0.cos e The only INCORRECT information about the **orbital** is - (1) Value of 'x' is (2) **Orbital** is 2pz (3) Most probable distance of electron from the centre of nucleus is 4ao, in case of H- atom (4) There is no node (neither radial nor angular) in this **orbital**. **Which of the following** sets of **quantum numbers** (n,l,ml,ms) refers to a 4s **orbital**? Select one: a. 4,0,0,β12 b. 4,0,1,β12 c. 4,1,1,β12 d. 4,1,0,β12. The state of a multielectron atom as a whole is defined by the **following quantum numbers**: (1) the **quantum number** of the total **orbital** angular momentum of an atom L, which is defined by the motion of all electrons, L = 0, 1, 2, . ; (2) the **quantum number** of the total angular momentum of the atom j, which may assume all values differing by. There are 4 quantum numbers. One which distinguishes between electrons in same orbitals is Spin quantum number. It is represented as +1/2 or -1/2. If an electron in moving clockwise, it's quantum number is +1/2 and if it's moving anti-clockwise, it's quantum number is -1/2. hope it helps. Deep Kasar. Give the **orbital** notation designated by the **quantum** **numbers** below: Possible Answers: Correct answer: Explanation: **The**, principal **quantum** **number**, tells us the shell, which is represented as the leading coefficient in electronic configuration. Since we are given , we know that the leading **number** will be five. If the principal **quantum** **number** n=6, the correct sequence of filling of electrons; In Bohr series of lines of hydrogen spectrum; **Number** of atoms in 558.5 gram Fe is; Which statements in relation to the hydrogen atom is correct; **Which of the following** is the energy of a possible excited state of hydrogen. Moreover, there is a pattern which describes the maximum number of electrons an electron shell can contain. Here, this maximum number depends on the azimuthal quantum number, l. Further, the values l = 0, 1, 2 and 3 refer to the s, p, d and f orbitals respectively. The maximum number of electrons a shell can contain = 2 (2l+1). **Which of the following can be the quantum numbers for an orbital**? a) n = 4,1 = 4, m = 3 b) n = 2, I = 3, m= 1 c) n = 3,1 = 2, m = -1 d) n = 3,1 = 0, m= -3 b d ΠΡ a Question : **Which of the following can be the quantum numbers for an orbital**?.

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- It therefore required three coordinates, or three
**quantum numbers**, to describe**the**orbitals in**which**electrons**can be**found.**The**three coordinates that come from Schrodinger's wave equations are**the**principal (n), angular (l), and magnetic (m)**quantum numbers**. These**quantum numbers**des Continue Reading Steven Fawl - Rules Governing the Allowed Combinations of Quantum Numbers The three quantum numbers ( n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on. The principal quantum
- The number of nodes is always one less than the principal quantum number: Nodes = n - 1. In the first electron shell, n = 1. The 1s orbital has no nodes. In the second electron shell, n = 2. The 2s and 2p orbitals have one node. In the third electron shell, n = 3. The 3s, 3p, and 3d orbitals have two nodes, etc. Types of Node
- Explanation: . The principle
**quantum number**, , must be a positive integer. The**orbital**angular**quantum number**, , ranges from to , and is also an integer. The magnetic**quantum number**, , ranges from to , again is an integer. The spin**quantum number**, ,**can**have only a value of or . Of the choices given, the set because the**orbital**angular**quantum number**must be less than **The**correct option is C n = 4, l = 3, ml = +1, ms = +1/2. When an electron is in 4f**orbital**,**the**set of**quantum****numbers**is as follows; β The value of principal**quantum****number**n represents the principal shell. For an electron in 4f**orbital**, n=4. β The value of angular momentum**quantum****number**represents the**orbitals**.