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What is the value of azimuthal quantum number l for all the electrons present in subshell 5p?
The azimuthal quantum number ( l ) corresponds to the shape of the orbital and is defined by the subshell type. For a ( p ) subshell, the value of ( l ) is 1. Therefore, for all the electrons present in the 5p subshell, the azimuthal quantum number ( l ) is 1.
Which quantum number is not a whole number?
The quantum number that is not a whole number is the magnetic quantum number, often denoted as ( m_l ). While the principal quantum number ( n ), angular momentum quantum number ( l ), and spin quantum number ( m_s ) are all whole numbers or integers, ( m_l ) can take on integer values ranging from (-l) to (+l), including zero, depending on the value of ( l ). However, the magnetic quantum number itself is always an integer, but its possible values reflect a range defined by the angular momentum quantum number.
How many values are there for the magnetic quantum number when the value of the angular momentum quantum number is 4?
The magnetic quantum number ( m_l ) can take on values ranging from (-l) to (+l), where ( l ) is the angular momentum quantum number. For ( l = 4 ), the possible values of ( m_l ) are (-4, -3, -2, -1, 0, +1, +2, +3, +4). This results in a total of 9 possible values for the magnetic quantum number when ( l = 4 ).
What is the second quantum number of the 3p1 electron in aluminium?
The second quantum number, also known as the azimuthal quantum number (l), describes the shape of the electron's orbital. For a 3p electron, the value of l is 1, corresponding to the p subshell. Therefore, the second quantum number of the 3p1 electron in aluminum is 1.
Which one o the following is not a valid value for the magnetic quantum number of an electron in a 5d sublevel?
The magnetic quantum number (m_l) can take on integer values ranging from -l to +l, where l is the azimuthal quantum number. For a 5d sublevel, l equals 2, so m_l can take values of -2, -1, 0, +1, or +2. Therefore, any value outside this range, such as 3, is not a valid magnetic quantum number for an electron in a 5d sublevel.
What will be the value of magnetic quantum number if the value of azimuthal quantum number is given to you?
The magnetic quantum number can have integer values ranging from -ℓ to +ℓ, where ℓ is the azimuthal quantum number. So the value of the magnetic quantum number would depend on the specific value of the azimuthal quantum number provided to you.
What is the magnetic quantum number value for an element with n 1?
The magnetic quantum number (m) can range from -l to +l, where l is the azimuthal quantum number. For an element with n=1 (first energy level), l=0. Therefore, the magnetic quantum number (m) can only be 0.
Which quantum number is not a whole number?
The quantum number that is not a whole number is the magnetic quantum number, often denoted as ( m_l ). While the principal quantum number ( n ), angular momentum quantum number ( l ), and spin quantum number ( m_s ) are all whole numbers or integers, ( m_l ) can take on integer values ranging from (-l) to (+l), including zero, depending on the value of ( l ). However, the magnetic quantum number itself is always an integer, but its possible values reflect a range defined by the angular momentum quantum number.
The Quantum Number that defines the shape of space an electron most likely resides in is the quantum number.?
The quantum number that indicactes the shape of an orbital in called the angular momentum quantum number.
How many values are there for the magnetic quantum number when the value of the angular momentum quantum number is 4?
The magnetic quantum number ( m_l ) can take on values ranging from (-l) to (+l), where ( l ) is the angular momentum quantum number. For ( l = 4 ), the possible values of ( m_l ) are (-4, -3, -2, -1, 0, +1, +2, +3, +4). This results in a total of 9 possible values for the magnetic quantum number when ( l = 4 ).
Which quantum number is also called sub-shell quantum number?
The azimuthal quantum number (l) is also known as the sub-shell quantum number. It represents the sub-shell of an electron within a given energy level. The value of l determines the shape of the orbital (s, p, d, f).
Which one o the following is not a valid value for the magnetic quantum number of an electron in a 5d sublevel?
The magnetic quantum number (m_l) can take on integer values ranging from -l to +l, where l is the azimuthal quantum number. For a 5d sublevel, l equals 2, so m_l can take values of -2, -1, 0, +1, or +2. Therefore, any value outside this range, such as 3, is not a valid magnetic quantum number for an electron in a 5d sublevel.
What could be a third quantum number of a 2p3 electron in phosphorus 1s22s22p63s23p3?
ml = -1
What is the value of l for orbital 'g'?
The value of l for an orbital labeled 'g' is 4. The values of l can range from 0 to n-1, where n is the principal quantum number. So for a principal quantum number of 5 (n=5), the possible values of l can be 0, 1, 2, 3, or 4.
Which number represents the shape of an electron subshell?
The shape of the electron cloud is determined by the secondary quantum number. The first is n, or the energy level, the second is the sublevel, the third is the specific cloud, and the fourth is the spin.
What does the second quantum number (l) describe?
Which sublevel the electron is in.
The numerical values of the magnetic quantum number m1 depends on the?
The values of the magnetic quantum number depend on the value of the azimuthal quantum number (orbital angular momentum quantum number) and has values -l, .. 0 . ..+l l=1, p orbital, -1, 0, +1 - three p orbitals l=2 d orbital -2, -1, 0., +1,+2 five d orbitals etc.
