(a)
Interpretation:
From the given set of two quantum numbers of two electrons, the possibility of electrons be in same atom has to be explained.
Concept Introduction:
Principal Quantum Number (n): In an atom, the electron energy mainly depends on principal quantum number. The energy of an electron becomes lower when the value of n is smaller. The orbital size also depends on n. The size of orbital increases with increase in value of principal quantum number (n)
Magnetic Quantum Number (
Spin Quantum Number (
(b)
Interpretation:
From the given set of two quantum numbers of two electrons, the possibility of electrons be in same atomic orbital has to be explained.
Concept Introduction:
Principal Quantum Number (n): In an atom, the electron energy mainly depends on principal quantum number. The energy of an electron becomes lower when the value of n is smaller. The orbital size also depends on n. The size of orbital increases with increase in value of principal quantum number (n)
Angular Momentum Quantum Number (l): It helps to differentiate different shapes of orbitals for given n. For a given n, there are n different shapes of orbitals are present and are denoted as l. Angular momentum quantum number is also known as Azimuthal quantum number. The possible values of angular momentum quantum number are between
Magnetic Quantum Number (
Spin Quantum Number (
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Chapter 5 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forwardWhat are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?arrow_forward
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