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Science
Q:
Which of the following may represent an excited-state electron configuration for a cobalt atom?
A) [Ar]3d54s1
B) [Ar]3d64s2
C) [Ar]3d84s1
D) [Ar]3d64s1
E) [Ar]3d74s2
Q:
Which of the following statements is true concerning the electron configuration [Ne]3s13p1?A) It may represent a ground-state electron configuration of a Al+ cation.B) It may represent an excited-state electron configuration of a Mg atom.C) It may represent an excited-state electron configuration of a Ne- anion.D) It may represent a ground-state electron configuration of a Mg+ cation.E) It may represent a ground-state electron configuration of a Na+ cation.
Q:
Which of the following statements is incorrect?
A) A p-block main-group element belonging to period n has a completely filled (n"1)d subshell.
B) All noble gases have completely filled shells.
C) All s-block main-group elements have only one or two valence electrons.
D) Carbon and silicon have the same number of valence electrons.
E) All elements in the n = 4 period have a partially or completely filled n = 4 shell.
Q:
The ground-state valence-shell configuration of a particular atom is 5s24d5. This valence-shell electron configuration identifies the atom as
A) a transition element.
B) an inner transition element.
C) an s-block main-group element.
D) a p-block main-group element.
E) a noble gas.
Q:
The ground-state valence-shell configuration of a particular atom is . The element to which this atom belongs is a
A) noble gas.
B) s-block main-group element.
C) p-block main-group element.
D) transition element.
E) inner transition element.
Q:
The ground-state valence-shell configuration of a particular atom is . The element to which this atom belongs is a
A) noble gas.
B) inner transition element.
C) p-block main-group element.
D) transition element.
E) s-block main-group element.
Q:
Which of the following electron configurations corresponds to the ground state of an atom of a transition element?
A) 1s22s22p5
B) 1s22s22p63s23p63d104s24p2
C) 1s22s22p63s23p63d64s2
D) 1s22s22p63s23p64s2
E) 1s22s22p63s23p4
Q:
According to the building-up principle or aufbau principle, which subshell is typically filled next after the 3d subshell?
A) 4p
B) 5f
C) 6p
D) 5d
E) 1s
Q:
Which element is found in the s-block of the periodic table?
A) H
B) Rn
C) Mo
D) Pr
E) none of the above
Q:
Two elements that have the same ground-state valence shell configuration of ns2np2 are
A) K and Mg.
B) O and Se.
C) Al and Ga.
D) Ge and Pb.
E) Mg and Ca.
Q:
Which of the following have one or more filled d subshells in their ground state electron configuration?
A) Ga
B) Cl
C) Si
D) He
E) Ar
Q:
Which of the following electron configurations represents an excited state of the indicated atom?
A) Ne: 1s2 2s2 2p6
B) N: 1s2 2s2 2p3
C) P: 1s2 2s2 2p6 3s2 3p2 4s1
D) Na: 1s2 2s2 2p6 3s2 3p2 3s1
E) He: 1s2
Q:
Which principle or rule is violated by the following orbital diagram of an atom in its ground state?
1s 2s 2p A) Pauli exclusion principle
B) Hund's rule
C) Heisenberg uncertainty principle
D) No rules or principles are violated by this orbital diagram.
E) Building-up principle
Q:
Which of the following statements is incorrect?
A) Stern and Gerlach discovered electron spin by passing silver atoms through a magnetic field.
B) Hund's rule states that electrons are placed in the orbitals of a subshell in such a way as to give a maximum number of unpaired electrons.
C) The Pauli exclusion principle states that each electron in an atom must have its own unique set of quantum numbers.
D) Valence electrons consist of those electrons not contained within a noble-gas core or a pseudo-noble-gas core.
E) The building-up principle states that electrons are added to atoms in order of increasing principal quantum number.
Q:
Which of the following statements is true concerning the electron configuration [Kr]5p2?
A) This configuration cannot be the ground-state electron configuration for a Sr atom because it violates the Pauli exclusion principle.
B) This configuration cannot be the ground-state electron configuration for a Sr atom because it violates Hund's rule.
C) This configuration is the ground-state electron configuration for a Sr atom.
D) This configuration cannot be the ground-state electron configuration for a Sr atom because it violates the Heisenberg uncertainty principle.
E) This configuration cannot be the ground-state electron configuration for a Sr atom because it violates the Aufbau principle.
Q:
Which of the following electron configurations is impossible, according to the Pauli exclusion principle?
A) B) C) D) E)
Q:
Which principle or rule is violated by the following orbital diagram of an atom in its ground state?
1s 2s 2p A) Pauli exclusion principle
B) Aufbau principle
C) No rules or principles are violated by this orbital diagram.
D) Heisenberg uncertainty principle
E) Hund's rule
Q:
Which of the following orbital diagrams violates the Pauli exclusion principle?
1s 2s 2p
A) B) C) D) E)
Q:
What is the maximum number of electrons in an atom that have the set of quantum numbers n= 1 and l= 0?
A) 6
B) 14
C) 10
D) 18
E) 2
Q:
The maximum number of electrons that can be accommodated in an f subshell is
A) 2.
B) 10.
C) 6.
D) 1.
E) 14.
Q:
Which of the following orbital occupancy designations is incorrect?
A) 3d7
B) 2p6
C) 4f6
D) 1s2
E) 4f15
Q:
What is the maximum number of electrons that can be accommodated in the n = 2 shell?
A) 8
B) 4
C) 16
D) 22
E) 24
Q:
What is the maximum number of electrons that can occupy one p orbital?
A) 14
B) 2
C) 10
D) 1
E) 6
Q:
The Pauli exclusion principle states that
A) the wavelength of a photon of light times its frequency is equal to the speed of light.
B) no two electrons in the same atom can have the same set of four quantum numbers.
C) both the position of an electron and its momentum cannot be known simultaneously very accurately.
D) the wavelength and mass of a subatomic particle are related by .
E) an electron can have either particle character or wave character.
Q:
Which hydrogen atom orbital has an energy essentially identical to a 3d orbital?
A) 5d
B) 4p
C) 1s
D) 2s
E) 3p
Q:
Which of the following is a representation of a orbital?A) B) C) D) E)
Q:
Which of the following is a representation of a 3dxz orbital?A) B) C) D) E)
Q:
What is the total number of orbitals found in the n= 4 shell?A) 16B) 4C) 20D) 24E) 15
Q:
Which orbital or orbitals is/are specified by the set of quantum numbers n= 4 and l= 3?A) 4fB) 3dC) 1sD) 2pE) 4s
Q:
How many orbitals have the set of quantum numbers ?
A) 5
B) 9
C) 7
D) 1
E) 3
Q:
How many p orbitals are in the n= 4 shell?
A) 1
B) 8
C) 7
D) 5
E) 3
Q:
Which of the following statements is incorrect?A) The n= 3 shell has three p orbitals.B) Every p subshell has three orbital.C) The n= 4 shell has seven f orbitals.D) An s orbital has a spherical shape.E) The n= 2 shell has five d orbitals.
Q:
Which of the following statements is incorrect?A) The set of quantum numbers n= 3, l= 2, ml= 0, ms= is not permitted because ml= 0.B) The set of quantum numbers n= 2, l= 2, ml= 1, ms= is not permitted because n = l.C) The set of quantum numbers n= 3, l= 2, ml= 1, ms= is permitted.D) The set of quantum numbers n= 3, l= 2, ml= 3, ms= is not permitted because ml exceeds l.E) The set of quantum numbers n= 4, l= 3, ml= -1, ms= 0 is not permitted because ms= 0.
Q:
Which of the following combinations of quantum numbers is permissible?A) n= 1, l= 2, ml= 0, ms= B) n= 3, l= 2, ml= 1, ms= C) n= 3, l= 3, ml= 1, ms= D) n= 2, l= 1, ml= -1, ms= 0E) n= 4, l= 3, ml= 4, ms=
Q:
Which of the following sets of quantum numbers (n, l, ml,ms) is not permissible?A) 3 3 -3 +B) 2 1 -1 +C) 1 0 0 +D) 3 2 -2 -E) 4 0 0 -
Q:
The number of orbitals in a p subshell is
A) 3.
B) 1.
C) 7.
D) 2.
E) 5.
Q:
Which of the following subshells does not exist?A) 6gB) 3fC) 3pD) 2sE) 4d
Q:
What is the value of the spin quantum number for an electron in a 3p orbital?
A) 3
B) 1
C) either or D) E)
Q:
What is the value of the principal quantum number for an electron in a 1s orbital?A) -1B) C) 1D) E) 0
Q:
An orbital with the quantum numbers may be found in which subshell?
A) 3f
B) 3d
C) 3p
D) 3g
E) 3s
Q:
How many values are there for the magnetic quantum number when the value of the angular momentum quantum number is 4?
A) 14
B) 9
C) 1
D) 4
E) 15
Q:
All the following statements about the quantum numbers are true exceptA) ml has 2l + 1 possible values.B) n may take integral values from 1 to .C) ml may take integral values of +l to -l, including zero.D) l may take integral values from 1 to n- 1.E) ms may take only the values of and .
Q:
A possible value of the magnetic quantum number mlfor a 5p electron isA) 1.B) -4.C) -5.D) 6.E) 3.
Q:
What is the value of the angular momentum quantum number for an electron in a 5d orbital?
A) 0
B) 4
C) 1
D) 2
E) 3
Q:
Which of the following sets of quantum numbers (n, l, ml,ms) refers to a 3d orbital?A) 2 1 0 +B) 5 4 3 +C) 4 2 1 -D) 4 3 1 -E) 3 2 1 -
Q:
The angular momentum quantum number is best associated with the
A) shape of the orbital.
B) number of orbitals in a subshell.
C) energy of the orbital.
D) orientation in space of an orbital.
E) none of the above
Q:
Which quantum number distinguishes the different shapes of the orbitals?
A) n
B) ml
C) l
D) ms
E) any of these
Q:
The number of orbitals having a given value of l is equal toA) 2n+ 1.B) 2l+ 1.C) n+ ml.D) 2ml+ 1.E) l+ ml.
Q:
A radial probability plot for an electron in an atom, like that shown below, A) specifies the probable speed of the electron at a given radius from the nucleus.
B) specifies the probable momentum of the electron at a given radius from the nucleus.
C) describes the probable energy of the electron at a given radius from the nucleus.
D) gives the probability of finding one electron near another at a given radius from the nucleus.
E) gives the probability of finding the electron at a given radius from the nucleus.
Q:
The square of the wave function, 2, of an electron in an atomA) is inversely proportional to the distance between the electron and the nucleus.B) specifies the momentum of the electron.C) describes the energy of the electron.D) is proportional to the velocity of the electron.E) gives the probability of finding the electron in a region of space.
Q:
Which of the following statements is incorrect concerning the wave function?A) The wave function of a particle is a solution to the Schrdinger equation.B) For an electron in an atom, the square of the wave function decreases rapidly as the distance from the nucleus increases.C) The square of the wave function is proportional to the probability of finding the particle in a region of space.D) The value of the wave function gives the location of the particle.E) The wave function for an electron in an atom is called an atomic orbital.
Q:
Which of the following statements is a valid conclusion from the Heisenberg uncertainty principle?
A) The square of the wave function is proportional to the probability of finding a particle in space.
B) Particles can exhibit wavelike behavior.
C) The orbits proposed by Bohr's model of the atom are correct.
D) An electron in a 2p orbital is always closer to the nucleus than an electron in a 3p orbital.
E) The act of measuring a particle's position changes its momentum, and vice versa.
Q:
If the x-component of the velocity of an electron can be measured only to a precision of , what is the minimum uncertainty of the position of the electron in the x-direction? ( )A) B) C) D) E)
Q:
If the location of a particular electron can be measured only to a precision of 0.011 nm, what is the minimum uncertainty in the electron's velocity? (
)
A) B) C) D) E)
Q:
What is the wavelength of an electron traveling at 7.59% of the speed of light? ()
A) B) C) D) E)
Q:
What is the wavelength of a 149-g baseball traveling at 97.2 mph? ()
A) B) C) D) E)
Q:
Which of the following statements concerning quantum mechanics is/are true?
1) The behavior of submicroscopic particles can sometimes be described as waves.
2) Quantum mechanics limits us to making statistical statements about the location of an electron in an atom.
3) The uncertainty principle is important only for particles of very small mass, such as the electron.
A) 1 only
B) 2 only
C) 3 only
D) 2 and 3
E) 1, 2, and 3
Q:
The contribution for which de Broglie is best remembered in modern science is
A) his statement that no electron can have identical values for all four quantum numbers.
B) his proposal that particles of matter should be associated with wavelike behavior.
C) his statement that an electron can exist in an atom only in discrete energy levels.
D) his statement that elements show periodic repetition of properties.
E) his statement that electrons occupy all the orbitals of a given sublevel singly before pairing begins.
Q:
Consider the following energy-level diagram for a particular electron in an atom.Based on this diagram, which of the following statements is incorrect?A) The wavelength of a photon emitted by the electron jumping from level 2 to level 1 is given by .B) If the electron is in level 1, it may jump to level 2 by absorbing a photon with energy of E.C) If the electron is in level 1, it may jump to level 2 by absorbing any photon having energy of at least E.D) We would observe an electron jumping from level 2 to level 1 as a single line in a line spectrum.E) If the electron is in level 2, it may jump to level 1 by emitting a photon with energy of |E|.
Q:
The electron in a hydrogen atom, originally in level , undergoes a transition to a lower level by emitting a photon of wavelength 1006 nm. What is the final level of the electron? (
A) 3
B) 4
C) 7
D) 8
E) 1
Q:
What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from level ()
A) B) C) D) E)
Q:
What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level ()
A) B) C) D) E)
Q:
From the Bohr model of the hydrogen atom, we can conclude that the energy required to excite an electron from n = 5 to n = 6 is ____ the energy required to excite an electron from n = 4 to 5.
A) less than
B) greater than
C) equal to
D) either equal to or less than
E) either equal to or greater than
Q:
When an electron in an atom makes a transition from n= 6 to n= 4, which of the following statements is/are correct?
I. Energy is emitted.
II. Energy is absorbed.
III. The electron loses energy.
IV. The electron gains energy.
V. The electron cannot make this transition.
A) I and III
B) I and IV
C) II and IV
D) II and III
E) III
Q:
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 absorbed.
B) light is emitted.
C) energy is emitted.
D) no change in energy occurs.
E) none of these
Q:
Who postulated that energy is radiated only when an electron falls from a higher-energy level to a lower-energy level?
A) Bohr
B) Heisenberg
C) Rutherford
D) Einstein
E) Millikan
Q:
Whose postulates account for the line spectrum of an atom?
A) Thomson
B) de Broglie
C) Heisenberg
D) Rutherford
E) Bohr
Q:
Which of the following is/are correct postulates of Bohr's theory of the hydrogen atom ?
1) The energy of an electron in an atom is quantized (i.e. only specific energy values are possible).
2) The principal quantum number (n), specifies each unique energy level.
3) An electron transition from a lower energy level to a higher energy level results in an emission of a photon of light.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
Which of the following scientists first postulated that the sharp lines in the emission spectra of elements were caused by electrons going from high-energy levels to low-energy levels?
A) Rutherford
B) Pauli
C) Hund
D) de Broglie
E) Bohr
Q:
What is the energy per mole of photons having a frequency of ()
A) B) C) D) E)
Q:
What is the energy per mole of photons with a wavelength of 976.9 nm? ()
A) B) C) D) E)
Q:
What is the frequency of photons that have molar energy of 525 kJ/mol? ()
A) B) C) D) E)
Q:
What is the wavelength of photons that have molar energy of 479 kJ/mol? ()
A) B) C) D) E)
Q:
What is the frequency of a photon having an energy of ()
A) B) C) D) E)
Q:
What is the wavelength of a photon that has an energy of J? ()
A) nm
B) nm
C) 0.843 nm
D) nm
E) nm
Q:
What is the energy of a photon of electromagnetic radiation with a frequency of Hz? ()
A) J
B) J
C) J
D) J
E) J
Q:
What is the energy of a photon of electromagnetic radiation with a wavelength of 877.4 nm? ()
A) J
B) J
C) J
D) J
E) J
Q:
Which type of electromagnetic radiation has the highest energy?
A) radio waves
B) x rays
C) red light
D) blue light
E) gamma rays
Q:
A light emitting diode (L.E.D.) emits photons with an energy of J. What is the energy per mole of photons emitted?
A) J/mol
B) J/mol
C) J/mol
D) J/mol
E) J/mol
Q:
A laser emits photons having an energy of 3.74 x10-19J. What color would be expected for the light emitted by this laser? (c= 3.00 x108m/s, h= 6.63 x10-34J·s)A) yellow to orangeB) orange to redC) greenD) violetE) blue