Atomic Structure and Electron Configurations Multiple Choice

Atomic Structure and Electron Configurations Multiple Choice

General Chemistry (CHEM011)

Name: _______________________ (Can provide answers at the end)

1. Rutherford’s Nuclear Model of the atom

A. is the currently accepted atomic model.

B. explains the unique emission spectra of different elements.

C. does not account for the stability of most atoms since accelerating electrons

would quickly lose energy and fall into the nucleus, causing the atom to

collapse.

D. Both b and c

2. When an excited electron in an atom moves from the ground state, the electron

A. absorbs energy as it moves to a higher energy state.

B. absorbs energy as it moves to a lower energy state.

C. emits energy as it moves to a higher energy state.

D. emits energy as it moves to a lower energy state.

(NY Regents June 2014)

3. During a flame test, a lithium salt produces a characteristic red flame. This red color

is produced when electrons in excited lithium atoms

A. are lost by the atoms.

B. are gained by the atoms.

C. return to lower energy states within the atoms.

D. move to higher energy states within the atoms.

(NY Regents June 2014)

4. Bohr’s atomic model

A. proposes that electrons occupy specific energy levels.

B. explains the emission spectra of hydrogen atoms.

C. predicts the energy levels of multi-electron atoms.

D. Both a and b

5. The quantum-mechanical model of the atom

A. describes an electron probability distribution that determines the most likely

location of an electron.

B. is the currently accepted atomic model.

C. makes predictions based on Schrodinger’s wave equation.

D. All of the above

6. In the quantum-mechanical model of the atom, which of the following is NOT one of

the four quantum numbers needed to specify the probable location of an electron?

A. Principal quantum number (n) which describes the energy level/distance

from the nucleus

B. Heisenberg number (H) which describes the electron’s position and

momentum.

C. Angular quantum number (l) which describes the shape of an electron’s

orbital

D. Magnetic quantum number (ml) which describes the orbitals orientation in

space

7. The Heisenberg Uncertainty Principle

A. assumes that the electrons take positions predicted by Bohr’s theory.

B. states that the position of an electron can be found by measuring its

momentum.

C. states that the position and momentum of an electron in an atom cannot be

found precisely because measuring the electron changes its momentum.

D. both a and b

8. In the quantum-mechanical model of the atom, an orbital is defined as a

A. region of the most probable proton location.

B. region of the most probable electron location.

C. circular path traveled by an electron around an orbital.

D. circular path traveled by a proton around an orbital.

(NY Regents June 2014)

9. __________ orbitals are spherically symmetrical.

A. s

B. p

10. ______ orbitals are dumbbell shaped

A. s

B. p

C. d

D. f

C. d

D. f

11. s orbitals can have how many different orientations in space?

A. 1 C. 5

B. 3 D. 7

12. d orbitals can have how many different orientations in space?

A. 1 C. 5

B. 3 D. 7

13. All orbitals can hold a maximum of ______ electrons

A. 1 C. 3

B. 2 D. 4

14. All of the orbitals in a given electron shell have the same value for the __________

quantum number.

A. Principal (n) C. Magnetic (ml)

B. Angular (l) D. Spin (ms)

15. The __________ quantum number defines the shape of an orbital.

A. Spin (ms) C. Principal (n)

B. Magnetic (ml) D. Angular (l)

16. The n = 1 shell contains __________ p sub-orbitals. All the other shells contain

__________ p sub- orbitals.

A. 3, 6 C. 6, 2

B. 0, 3 D. 3, 3

17. There are __________ orbitals in the second shell.

A. 1

B. 2

C. 4

D. 8

18. The lowest energy shell that contains d orbitals is the shell with n = ______.

A. 3 C. 4

B. 2 D. 1

19. The principal quantum number of the first d orbital is _____.

A. 1 C. 3

B. 2 D. 4

20. Which of the orbitals below do not exist due to the constraints upon the angular

quantum number?

A. 3f C. 2p

B. 2s D. all of the above

21. Which of the orbitals below do not exist due to the constraints upon the angular

quantum number?

A. 3f C. 3p

B. 3d D. 3s

22. Which one of the following is an incorrect orbital notation?

A. 4f C. 3s

B. 2d D. 2p

23. There are __________ sub-orbitals in the 3rd shell.

A. 25

B. 4

C. 9

D. 16

24. All of the sub-orbitals in a given orbital have the same value of the __________

quantum number.

A. Principal C. Magnetic

B. Angular D. A and B

25. The p-orbital can accommodate a maximum of __________ electrons.

A. 6 C. 10

B. 2 D. 3


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