n : 2
l : 1
ml : -1, 0, or 1
To ensure what is bigger, we need to see both values in the same unit. Therefore we convert them to all to liters (L) Then we get: 750 mL = 0,750 L 1,75 L = 1,75 L Which therefore means that 1,75 L is biggest.
I have essentially zero ability to answer that without seeing the equation. Another answer: n-1 = 3-1= 2 l=2 ml= -2,-1,0,1,2.
1.000 L = 1,000 mL 2.000 L = 2,000 mL 13.000 L = 13,000 mL. That's greater than 130 mL.
ml stands for milliliter so the l is for liter and the m is for milli
400 L/250 mL = 400,000 mL / 250 mL = 1600 bottles.400 L/250 mL = 400,000 mL / 250 mL = 1600 bottles.400 L/250 mL = 400,000 mL / 250 mL = 1600 bottles.400 L/250 mL = 400,000 mL / 250 mL = 1600 bottles.
The third quantum number, ml, describes the orientation of an orbital in space. It specifies the orbital's orientation relative to the x, y, and z axes. It can have integer values ranging from -l to +l.
The third quantum number for a 2p3 electron in phosphorus is the magnetic quantum number (m). It specifies the orientation of the orbital in space and can have values ranging from -l to +l, where l is the azimuthal quantum number for the orbital. So, for the 2p orbital with l=1, the possible values of m are -1, 0, and 1.
For the d orbital, the value of l is 2 and the value of ml is - l to + l, so the values of ml would be -2, -1, 0, +1, +2. So, the maximum value would be +2.
ml = -1
The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n. The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell. The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) so for an f orbital the values are -3. -2, -1, 0, +1, +2, +3, so 7 f orbitals in total. ml "defines " the shape of the orbital and the number within the subshell.
The third quantum number, m, describes the orientation of the atomic orbital in space. It specifies the orientation of the orbital within a particular subshell. The values of m range from -l to +l, where l is the azimuthal quantum number.
It depends whether you mean ml or ms.There are 4 quantum numbers, n, l, ml, msThey have long names respectively principal, azimuthal (angular momentum), magnetic and spin.n can have values 0, 1, 2, 3, 4, 5......l depends on n, and can have values, 0 to (n-1) (0 is an s orbital, 1 is a p subshell, 2 is a d subshell, 3 is a f subshell etcml can have -l to +l (sorry this font is rubbish the letter l looks like a 1) so for a d orbital, where l = 2, it can be -2, -1 0, +1, +2. Five d orbitals in all.ms can be -1/2 or +1/2 (These are the maximum of 2 electrons having opposite spin)l depends on n, and can have values, 0 to (n-1) (0 is an s orbital, 1 is a p subshell, 2 is a d subshell, 3 is a f subshell etcRead more: What_are_the_possible_values_for_the_quantum_numbers
The allowable sets of quantum numbers are n (principal quantum number), l (azimuthal quantum number), ml (magnetic quantum number), and ms (spin quantum number). n determines the energy level and size of an orbital, l determines the shape of an orbital, ml determines the orientation of an orbital in space, and ms determines the spin of an electron in an orbital. Each set of quantum numbers must follow specific rules based on the principles of quantum mechanics.
If n=0 that means there are no values for l
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.
The electron in the second main energy level and second sublevel is described by the quantum numbers n=2 (main energy level) and l=1 (sublevel), which corresponds to the p orbital. The set of quantum numbers for this electron is 2p.
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.