CHEM 111 Lecture Notes - Lecture 19: Diiv, Quantum Number

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silverdolphin511

7 Nov 2016

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Ground state: the lowest energy level (n=1) Excited state: the highest energy level when electron jump from ground state to excited state, it will gain energy, n=2 is the first excited state. Absorption: electron gaining energy by moving from a lower level to a higher level. Emission: an electron releasing energy in the form of light by moving from a higher to lower energy level. When electron absorbs energy, it is in the form of wavelength with distinct color. When emitting energy, the energy is reflected in the form of different light energy. De broglie: all matter travels as a wave, the end always has to come back to where it started, = h/mv, [ is measured in meters] [m= kg] [v=velocity in sec- or m/s] Proposed that information about a particle can only be obtained by solving an equation for a wave.

Related Questions

(a) Sketch the molecular orbitals of the H₂^– ion and draw its energy-level diagram. (b) Write the electron configuration of the ion in terms of its MOs. (c) Calculate the bond order in H₂^-. (d) Suppose that the ion is excited by light, so that an electron moves from a lower-energy to a higher-energy molecular orbital. Would you expect the excited-state H₂^- ion to be stable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?

orchidporcupine225

1. Theabsorption spectra of ions have been used to identify the presenceof the elements in the atmospheres of the sun and other stars. Whatis the wavelength of light (in nm) that is absorbed byHe⁺ ions, when an electron is excited from the Bohrorbit with n = 2 to the n = 7 state? The energy of an electron inthe nth level is

E_n =

BZ²

n²

where B = 2.18 x 10^-18 J and Z = charge onnucleus (number of protons).

2. Anelectron in the 4^th energy level of the H atom drops tothe 1^st energy level. In other words an excited electrondrops to the ground state. What is the energy (in J) of the emittedphoton)? The energy of an electron in the nth level is

E_n =

n²

2.18 x 10^-18 J

n²

3.The photoelectric effect for a certain alloy has a thresholdfrequency of 8.40 x 10¹⁴ Hz. For light of thisfrequency, find the energy of one mole of photons (inkJ).

whitetermite353

According to Jablonski diagram, an electron in ground state can be excited when it absorbs light. When this same electron return to the ground state, it may emit light. Which statement for this electron is correct?

	A.	The wavelengtth of the emitted light is always equal to that absorbed by the same electron.
	B.	The energy of the emitted light is higher than that absorbed by the same electron.
	C.	The energy of the emitted light is always equal to that absorbed by the same electron.
	D.	The wavelength of the emitted light is longer than that absorbed by the same electron.
	E.	The wavelength of the emitted light is less than that absorbed by the same electron.

CHEM 111 Lecture Notes - Lecture 19: Diiv, Quantum Number

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