CEM 141 MSU Exam 2 Prep Newest Actual Exam
With Complete Questions And Correct Detailed
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Atomic Emission Spectrum
Spectrum that emits photons, energy diagram: electron goes down energy
levels.
Atomic Absorption Spectrum
Spectrum that absorbs photons, energy diagram: electrons goes up in energy
levels.
,Heisenberg Uncertainty Principle
Principle states that we can't accurately measure both the position and the
energy of a small particle (electron)
Bohr's model did - why its wrong.
Schrodinger's Wave Equation
Treated electron as waves derived by mathematical descriptions of energies.
Psi = wave function of an electron
Psi^2 = probability of finding an electron.
Atomic Orbitals
Regions of space where electrons with a particular quantized energy have a high
probability of being found, described by quantum numbers.
What are the quantum numbers?
n, l, ml, and ms.
What does quantum number "n" mean?
Determines the energy of the electron and identifies its shell.
What does quantum number "l" mean?
Identifies the type of orbital (s,p,d) and subshell
= 0 - n-1.
, What does quantum number "ml" mean?
Specifies a particular orbital within a subshell
= -l - +l (2l + 1 possible values)
tells us how many s,p,d orbitals are found in each sub shell.
What does quantum number "ms" mean?
Describes the spin of the electron in each orbital
= +1/2 or -1/2
(only 2 e- in each orbital, each one has either + spin or - spin).
Aufbau Principle
Principle that electrons occupy the lowest level orbitals first.
Hund's Rule
Rule that electrons occupy orbitals of the same energy singly until they have to
pair up.
Core Electrons
Low in energy electrons that are close to the nucleus within the closed shell,
doesn't participate in reactions.
With Complete Questions And Correct Detailed
Answers (Verified Answers) |Already Graded A+
Atomic Emission Spectrum
Spectrum that emits photons, energy diagram: electron goes down energy
levels.
Atomic Absorption Spectrum
Spectrum that absorbs photons, energy diagram: electrons goes up in energy
levels.
,Heisenberg Uncertainty Principle
Principle states that we can't accurately measure both the position and the
energy of a small particle (electron)
Bohr's model did - why its wrong.
Schrodinger's Wave Equation
Treated electron as waves derived by mathematical descriptions of energies.
Psi = wave function of an electron
Psi^2 = probability of finding an electron.
Atomic Orbitals
Regions of space where electrons with a particular quantized energy have a high
probability of being found, described by quantum numbers.
What are the quantum numbers?
n, l, ml, and ms.
What does quantum number "n" mean?
Determines the energy of the electron and identifies its shell.
What does quantum number "l" mean?
Identifies the type of orbital (s,p,d) and subshell
= 0 - n-1.
, What does quantum number "ml" mean?
Specifies a particular orbital within a subshell
= -l - +l (2l + 1 possible values)
tells us how many s,p,d orbitals are found in each sub shell.
What does quantum number "ms" mean?
Describes the spin of the electron in each orbital
= +1/2 or -1/2
(only 2 e- in each orbital, each one has either + spin or - spin).
Aufbau Principle
Principle that electrons occupy the lowest level orbitals first.
Hund's Rule
Rule that electrons occupy orbitals of the same energy singly until they have to
pair up.
Core Electrons
Low in energy electrons that are close to the nucleus within the closed shell,
doesn't participate in reactions.
