AP Chemistry : Atomic Structure and Properties
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Example Questions
Example Question #141 : Atomic Structure And Properties
In terms of the principal quantum number, 
For any n, the energy level can hold 2n2 electrons, since there are two electrons for each orbital.
Example Question #21 : Atomic Structure And Electron Configuration
What does the azimuthal quantum number reveal about the quantum mechanical model of an atom?
The azimuthal quantum number is the second quantum number, designated by the letter l. It gives the shape and number of subshells in a principal energy level (shell).
Example Question #22 : Atomic Structure And Electron Configuration
Which of the following set of quantum numbers are not allowed: (a) n = 3, l = 2, ml = 0
(b) n = 2, l = 4, ml = –1 (c) n = 2.5, l = 1, ml = –1?
(c)
(b), (c)
(a), (b)
(a), (b), (c)
(a)
(b), (c)
The sets of quantum numbers needs to follow the following rules: n (principal quantum
number) needs to be a positive integer, l can have any integral value from 0 to n – 1, and ml can range from –l to l. The only quantum numbers that follows these rules are (a).
Example Question #23 : Atomic Structure And Electron Configuration
How does energy vary as the quantum number (n) of an orbital changes?
n has no effect on energy
As n increases, energy decreases
As n increases, the energy increases as well
n is always constant, making the energy constant
As n increases, the energy increases as well
The energy of an electron is related to the quantum number by the equation E = -R/n2, where R is constant. The negative charge make it so that as n increases, the numerical value of the energy becomes less negative, approaching zero. Thus the energy increases as n increases.
Example Question #145 : Atomic Structure And Properties
What is the angular momentum quantum number for the highest energy orbital in the ground state Manganese atom?
3
1
2
None of the other answers
0
2
First, we will write out the electron configuration for the ground state Manganese atom, considering only the valence electrons:
![[Ar]4s^23d^5](https://vt-vtwa-assets.varsitytutors.com/vt-vtwa/uploads/formula_image/image/20029/gif.latex)
The orbitals highest in energy will be filled last, so our highest energy orbitals are 
The angular momentum quantum number describes the shape of the orbital, with 
We are considering a 
Example Question #146 : Atomic Structure And Properties
Which of the following sets of quantum numbers could never be used to describe an electron?
The principle quantum number, 
The angular momentum quantum number, 
The magnetic quantum number, 
The spin quantum number, 
To total, a set of quantum numbers follows the pattern:
The only answer option that presents an invalid set of quantum numbers is 
Example Question #141 : Atomic Structure And Properties
Which set of quantum numbers represents the highest energy valence electron in a ground-state aluminum atom?
The aluminum atom has its furthest electrons in the 3p shell. We know this because aluminum is in the third row of the periodic table, and is in the p-block. The possible quantum numbers for any valence electron are:
Example Question #144 : Atomic Structure And Properties
Which of the quantum number describes the shape of the orbital where an electron is located?
l
n
ml
ms
n
There are four quantum numbers; l indicates the type of orbital (s, p, d, f), which describe the shape of the orbital. An s orbital is spherical, p orbitals are dumbbell shaped, d and f orbitals are slightly more elongated than p orbitals. The n quantum number denotes the energy level, and can be positive integers only. The magnetic quantum number, ml denotes the specific subshell within an electron shell. Lastly, the spin number, ms denotes the spin of a specific electron. Since only two electrons can occupy any one orbital, this number is usually represented as an up arrow or a down arrow (or a positive sign or a negative sign).
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