<p>Sorry guys-- ive missed a lot of school and im confused on a few ?s</p>
<p>(1) In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus--
(A) energy is emmitted
(B) energy is absorbed
(C) no change in energy occurs
(D) Light is emmitted
(E) none of the above</p>
<p>(2) Which of the following statements about quantum theory is INCORRECT?
(A) The energy and position of an electron CANT be determined simultaneously
(B) Lower energy orbitals are filled with electrons before higher energy orbitals
(C) When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital
(D) No two electrons can have the same four quantum numbers
(E) All of the above are correct</p>
<p>(3) When ignited, a uranium compound burns with a green flame. The wavelength of the light given off by this flame is greater than that of---
(A) red light
(B) Infrared light
(C) radio waves
(D) ultraviolet light
(E) None of the above</p>
<p>you r really lucky
i happen to just have done a test over this stuff
so here you go:</p>
<p>1) B, to overcome the attraction forces of the nucleus, the electrons have to absorb energy</p>
<p>2) E, all of them are correct</p>
<p>3) D, I had to look up the electromagnetic radiation illustration in my chem book and the green wavelength is about 5 x 10^-7 m and the only one out of the four that has smaller wavelength is ultraviolet</p>
<p>i dont know hanna. for number 2 i think they're right about the answer being C. Hund's rule states that when orbitals of identical energy are availalbe electrons enter them singly before pairing takes place. my teacher compared this to dealing cards. everybody gets one before somebody gets two so i dont think that one orbital would get 2 electrons before a new one. i hope you didnt get that wrong on your test.</p>