Atomic Structure

11. s orbitals can have how many different orientations in space? A. 1 B. 3 C. 5 D. 7

A. 1

At a maximum, an f-orbital can hold_____ electrons, a d-orbital can hold_____ electrons and a p-orbital can hold ________ electrons. A. 14, 10, 6 B. 2, 8, 18 C. 14, 8, 2 D. 2, 12, 21

A. 14,10, 6

__________ orbitals are spherically symmetrical. A. s B. p C. d D. f

A. s

The lowest energy shell that contains d orbitals is the shell with n = ______. A. 3 B. 2 C. 4 D. 1

A.3

. Which of the orbitals below do not exist due to the constraints upon the angular quantum number?

A.3f

All orbitals can hold a maximum of ______ electrons A. 1 B. 2 C. 3 D. 4

B. 2

______ orbitals are dumbbell shaped A. s B. p C. d D. f

B. p

. There are __________ orbitals in the second shell. A. 1 B. 2 C. 4 D. 8

B.2

Which one of the following is an incorrect orbital notation? A. 4f B. 2d C. 3s D. 2p

B.2d

How many quantum numbers are necessary to designate a particular electron in an atom? A. 3 B. 4 C. 2 D. 1

B.4

The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes __________. A. Pauli Exclusion Principle B. Hund's Rule C. deBroglie hypothesis D. Heisenberg Uncertainty Principle

B.Hund's Rule

The ground state electron configuration of Ga is __________ 31

C. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

The second shell in the ground state of atomic Argon contains __________ electrons.

C. 8

The word Aufbau means building up in German. The Aufbau Principle describes that A. electrons with the same spin cannot occupy the same orbital. B. Since electrons repel each other, electrons will occupy single orbitals within and energy level before doubling up. C. electrons fill lower energy levels first before occupying higher energy levels. D. None of the above.

C. electrons fill lower energy levels first before occupying higher energy levels

There are __________ sub-orbitals in the 3rd shell. A. 25 B. 4 C. 9 D. 16

C.9

All of the sub-orbitals in a given orbital have the same value of the __________ quantum number. A. Principal B. Angular C. Magnetic D. A and B

D A and B

2. The ______ orbital is partially filled in the Manganese atom

D. 3d

Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A. 3f B. 3d C. 3p D. 3s

D. 3s

Bohr's Atom Model

predicts the energy levels of multi-electron atoms.

14. All of the orbitals in a given electron shell have the same value for the __________ quantum number. A. Principal (n) B. Angular (l) C. Magnetic (ml) D. Spin (ms)

principal(n)

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

region of the most probable electron location

During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms

return to lower energy states within the atoms.

The __________ quantum number defines the shape of an orbital. A. Spin (ms) B. Magnetic (ml) C. Principal (n) D. Angular (l)

spin(ms)

The Heisenberg Uncertainty Principle

states that the position and momentum of an electron in an atom cannot be found precisely because measuring the electron changes its momentum.

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

Heisenberg number (H) which describes the electron's position and momentum.

. The p-orbital can accommodate a maximum of __________ electrons. A. 6 B. 2 C. 10 D. 3

a.6

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

absorbs energy as it moves to a higher energy state

Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

b

Which electron configuration represents a violation of the Pauli Exclusion Principle?

b

The ground state electron configuration of Fe is __________ (26)

b 1s2 2s2 2p6 3s2 3p6 4s2 3d6

The 2p orbital in the ground state of atomic Neon contains __________ electrons

b 6

The n = 1 shell contains __________ p sub-orbitals. All the other shells contain __________ p sub- orbitals. A. 3, 6 B. 0, 3 C. 6, 2 D. 3, 3

b. 0, 3

. Which ground state electron configuration represents a violation of the Aufbau Principle

c

Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

c

12. d orbitals can have how many different orientations in space? A. 1 B. 3 C. 5 D. 7

c. 5

The principal quantum number of the first d orbital is _____. A. 1 B. 2 C. 3 D. 4

c.3

Which electron configuration correctly denotes an atom in its ground state? A. B. C. D.

d

Which electron configuration represents a violation of the Pauli Exclusion Principle?

d

Which one of the following is the correct electron configuration for a groundstate nitrogen atom?

d

. Which two elements have the same ground-state electron configuration? A. I and S B. Cu and Ag C. Li and Na D. No two elements have the same ground-state electron configuration

d No two elements have the same ground-state electron configuration

5. The quantum-mechanical model of the atom

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

Rutherford's Nuclear Model of the atom

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