Chemistry

Q: Which of the following ions have the same ground state electron configuration: S2-, N3-, Mg2+, and Br-?A.N3- and Mg2+B.S2-, N3-, and Br-C.S2- and Br-D.Mg2+ and Br-E.S2-, N3-, Mg2+, and Br-

Q: What is the ground state electron configuration for Sn2+? A.[Kr]4d105s2 B.[Kr]4d105p2 C.[Kr]5s2 D.[Kr]4d105s25p2 E.[Kr]4d105s25p4

Q: What is the ground state electron configuration for Cr3+? A.[Ar] B.[Ar]3d74s2 C.[Ar]3d14s2 D.[Ar]3d24s1 E.[Ar]3d3

Q: If the ground state electron configuration of an element is [Ar]3d104s24p5, what is the typical charge on the monatomic anion of the element?A.4+B.2+C.1-D.2-E.3-

Q: Which 1+ ion has the ground state electron configuration [Kr]4d10? A.Ru B.Au C.Ag D.In E.Cd

Q: For which of the following atoms is the 2+ ion diamagnetic in the ground state? A.Ni B.Fe C.Zn D.Mn E.Cu

Q: What is a possible set of quantum numbers for an unpaired electron in the orbital box diagram below?A.n = 1, = 1, = -1, ms = +1/2B.n = 4, = 2, = -1, ms = -1/2C.n = 5, = 2, = -2, ms = +1/2D.n = 5, = 0, = 0, ms = -1/2E.n = 5, = 1, = -1, ms = +1/2

Q: What is the correct orbital box diagram for the ground state electron configuration of Ni? A. B. C. D. E.

Q: Which element has the following ground state electron configuration? A.In B.Y C.Nb D.Tl E.Ga

Q: Which element has the following ground state electron configuration? A.Fe B.Co C.Ni D.Cu E.Zn

Q: Which element has the following ground state electron configuration? A.B B.O C.C D.Be E.Si

Q: Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration) A.has a filled valence shell of electrons. B.has three electrons per orbital, each with identical spins. C.has values greater than or equal to +1. D.has the maximum number of unpaired electrons, all with the same spin. E.has two electrons per orbital, each with opposing spins.

Q: Which of the following statements concerning calcium's ground state electron configuration is/are CORRECT? 1/ calcium is paramagnetic. 2/ calcium is a p-block element. 3/ calcium has two valence shell electrons. A.1 only B.2 only C.3 only D.1 and 2 E.2 and 3

Q: What is the ground state electron configuration of a mercury atom? A.[Xe]6s26d10 B.[Kr]5d106s2 C.[Xe]4f145d106s2 D.[Xe]5d106s2 E.[Kr]4d104f146s2

Q: Which element has the ground state electron configuration [Ar]3d104s1? A.Cu B.Zn C.Ge D.Ag E.Cd

Q: Which element has the ground state electron configuration 1s22s22p63s23p3? A.V B.P C.Si D.Ti E.As

Q: Which of the following atoms is diamagnetic in the ground electronic state? A.Ge B.S C.I D.Mn E.Sr

Q: Which one of the following atoms is paramagnetic in the ground electronic state? A.Mg B.Cd C.Ar D.Bi E.He

Q: Which of the following elements is a d-block element? A.Kr B.Ba C.Hg D.Pb E.Nd

Q: Which of the following elements is an s-block element? A.C B.Cd C.Cs D.Ce E.Cf

Q: Which of the following statements concerning ground state electron configurations is/are CORRECT? 1/ For a hydrogen atom with one electron, the 2s and 2p orbitals have identical energies. 2/ For a lithium atom with three electrons, the 2s and 2p orbitals have different energies. 3/ The effective nuclear charge felt by an electron in a 2p orbital is greater for a carbon atom than for a boron atom. A.1 only B.2 only C.3 only D.2 and 3 E.1, 2, and 3

Q: Which of the following statements is/are CORRECT for an oxygen atom? 1/ The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s electron. 2/ The effective nuclear charges felt by 2s and 2p electrons are identical. 3/ The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron. A.1 only B.2 only C.3 only D.1 and 3 E.1, 2, and 3

Q: Which of the following statements regarding subshell filling order for a neutral atom is/are CORRECT? 1/ Electrons are assigned to the 4f subshell before they are assigned to the 6s subshell. 2/ Electrons are assigned to the 5d subshell before they are assigned to the 6p subshell. 3/ Electrons are assigned to the 4p subshell before they are assigned to the 4s subshell. A.1 only B.2 only C.3 only D.1 and 3 E.1, 2, and 3

Q: The procedure by which electrons are assigned to (or built up into) orbitals is known as the ____ principle. A.Aufbau B.Bohr C.Planck D.Hund E.Pauli

Q: The size of an electron orbital is often chosen to be the distance within which 90% of the electron density is found. Why is the orbital radius not chosen to be the distance within which 100% of the electron density is found?

Q: What evidence does the photoelectric effect provide that photons are not only waves?

Q: The Bohr model predicts that the energy of an atom's electron is ________, meaning that the electron can only occupy orbitals of specific energies.

Q: A ________, designated by the Greek symbol y, describes the wave behavior of an electron in an atom.

Q: The ________ quantum number is given the symbol . This quantum number is related to the orientation in space of an orbital.

Q: A point in a standing wave that has zero amplitude is called a(n) ________.

Q: According to Heisenberg's ________ principle, it is impossible to simultaneously measure the exact location and energy of an electron.

Q: Which of the following statements is/are CORRECT?1/ A diamagnetic substance is strongly attracted to a magnetic field.2/ Substances that retain their magnetism after they are withdrawn from a magnetic field are called ferromagnetic.3/ Most transition metals and all lanthanide metals are ferromagnetic.A.1 onlyB.2 onlyC.3 onlyD.1 and 3E.1, 2, and 3

Q: Which of the following statements is/are CORRECT?1/ A paramagnetic substance is attracted to a magnetic field.2/ An atom with no unpaired electrons is ferromagnetic.3/ Atoms with one or more unpaired electrons are paramagnetic.A.1 onlyB.2 onlyC.3 onlyD.1 and 3E.1, 2, and 3

Q: Which of the following diagrams represent p-orbitals?A.1 onlyB.2 onlyC.3 onlyD.4 onlyE.1 and 2

Q: Which of the following diagrams represent d-orbitals?A.1 onlyB.2 onlyC.3 onlyD.4 onlyE.1 and 4

Q: The n = ____ shell is the lowest that may contain f-orbitals.A.2B.3C.4D.5E.6

Q: A 3p orbital has ? A.0 planar nodes and 1 spherical node. B.1 planar node and 0 spherical nodes. C.1 planar node and 1 spherical node. D.1 planar node and 2 spherical nodes. E.2 planar nodes and 1 spherical node.

Q: Which of the following statements is/are CORRECT?1/ The angular momentum quantum number, , of an electron in an s orbital is always equal to 0.2/ The magnetic quantum number, , of an electron in a p orbital is +1, 0, or -1.3/ The principle quantum number, n, of an electron in a d orbital must be equal to or greater than 3.A.1 onlyB.2 onlyC.3 onlyD.1 and 2E.1, 2, and 3

Q: Which of the following sets of quantum numbers refers to a 4d orbital?A.n = 2, = 1, = -1B.n = 2, = 4, = -1C.n = 4, = 2, = -1D.n = 4, = 3, = 0E.n = 4, = 3, = +2

Q: What shell contains a total of 9 orbitals? A.n = 2 B.n = 3 C.n = 4 D.n = 5 E.n = 9

Q: What type of orbital is designated n = 4, = 3, = -2?A.4sB.4pC.4dD.4fE.none

Q: What type of orbital is designated n = 3, = 0, = 0? A.3s B.3p C.3d D.3f E.none

Q: Which of the following properties is associated with the value of the n quantum number? A.the number of electrons in an orbital B.the size of an orbital C.the orientation in space of an orbital D.the energy of an orbital E.the shape of an orbital

Q: What type of orbital is designated n = 3, = 2, = -2?A.3sB.3pC.3dD.2fE.2d

Q: Which of the following properties is associated with the value of the quantum number? A.the shape of an orbital B.the size of an orbital C.the number of electrons in an orbital D.the energy of an orbital E.the orientation in space of an orbital

Q: What is the total number of orbitals having n = 4 and = 2? A.3 B.5 C.7 D.9 E.10

Q: All of the following sets of quantum numbers are allowed EXCEPTA.n = 5, = 3, = +2B.n = 4, = 2, = -1C.n = 3, = 0, = 0D.n = 2, = 0, = +1E.n = 2, = 1, = 0

Q: All of the following sets of quantum numbers are allowed EXCEPTA.n = 1, = 0, = 0B.n = 2, = 2, = +1C.n = 3, = 1, = -1D.n = 4, = 1, = 0E.n = 5, = 4, = -3

Q: How many orbitals have the following set of quantum numbers: n = 5, = 3, = +2? A.0 B.1 C.3 D.6 E.7

Q: Which of the following statements is INCORRECT? A.It is not possible to know the exact location of an electron and its exact energy simultaneously. B.The energies of an atom's electrons are quantized. C.Quantum numbers define the energy states and the orbitals available to an electron. D.The behavior of an atom's electrons can be described by circular orbits around a nucleus. E.Electrons have both wave and particle properties.

Q: Erwin Schrdinger developed a model for the behavior of electrons in atoms that is known as quantum mechanics. Which of the following statements concerning this model is/are CORRECT? 1/ The energy of an electron is quantized. 2/ The energy of an electron is equal to its mass multiplied by the square of its velocity. 3/ Electrons travel in circular orbits around a nucleus. A.1 only B.2 only C.3 only D.1 and 2 E.1, 2, and 3

Q: Which type of experiment demonstrates that an electron has the properties of a wave? A.nuclear fission B.electron diffraction C.light emission from atomic gases D.mass spectroscopy E.photoelectric effect

Q: Which type of experiment demonstrates that light has the properties of a particle? A.nuclear fission B.electron diffraction C.light emission from atomic gases D.mass spectroscopy E.photoelectric effect

Q: What is the de Broglie wavelength of a 57 g tennis ball traveling at 202 km/hr?A.2.1 10-34 mB.2.1 10-37 mC.5.8 10-35 mD.9.4 104 mE.4.8 1036 m

Q: If the de Broglie wavelength of an electron is 44 nm, what is its velocity? The mass of an electron is 9.11 10-31 kg.A.6.0 10-5 m/sB.1.2 103 m/sC.1.7 104 m/sD.3.1 1010 m/sE.4.8 1022 m/s

Q: For a proton (mass = 1.673 10-27 kg) moving with a velocity of 2.83 104 m/s, what is the de Broglie wavelength (in pm)?A.0.356 pmB.3.56 pmC.14.0 pmD.7.15 pmE.28.5 pm

Q: If a hydrogen atom in the excited n = 4 state relaxes to the ground state, what is the maximum number of possible emission lines? A.1 B.4 C.6 D.8 E.infinite

Q: For a hydrogen atom, calculate the wavelength of an emitted photon in the Lyman series that results from the transition n = 3 to n = 1. The Rydberg constant is 1.097 107 m-1. (h = 6.626 10-34 Js and c = 2.998 108 m/s)A.102.6 nmB.95.0 nmC.91.2 nmD.434.1 nmE.1005 nm

Q: For which of the following transitions would a hydrogen atom absorb a photon with the longest wavelength? A.n = 1 to n = 2 B.n = 4 to n = 6 C.n = 5 to n = 4 D.n = 7 to n = 6 E.n = 6 to n = 7

Q: For which of the following transitions would a hydrogen atom emit the lowest energy photon? A.n = 4 to n = 5 B.n = 5 to n = 2 C.n = 4 to n = 3 D.n = 3 to n = 1 E.n = 3 to n = 2

Q: According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 1 to n = 2 is ____ the energy necessary to excite an electron from n = 2 to n = 3. A.less than B.greater than C.equal to D.either equal to or greater than E.either less than or equal to

Q: The energy required to break one mole of hydrogen-hydrogen bonds in H2 is 436 kJ/mol. What is the longest wavelength of light capable of breaking a single hydrogen-hydrogen bond? A.0.688 nm B.119 nm C.132 nm D.274 nm E.688 nm

Q: What is the binding energy of an electron in a photosensitive metal (in kJ/mol) if the longest wavelength of light that can eject electrons from the metal is 198 nm?A.279 kJ/molB.604 kJ/molC.792 kJ/molD.1.51 1012 kJ/molE.6.04 10-20 kJ/mol

Q: If the energy of 1.00 mole of photons is 245 kJ, what is the wavelength of the light? A.122 nm B.488 nm C.1220 nm D.787 nm E.811 nm

Q: What is the energy (in kilojoules per mole) of ultraviolet light with a wavelength of 228 nm?A.8.71 10-22 kJB.19.1 kJC.131 kJD.456 kJE.525 kJ

Q: A red laser pointer emits light at a wavelength of 488 nm. If the laser emits 7.5 10-4 J of energy per second in the form of visible radiation, how many photons per second are emitted from the laser?A.4.1 10-19 photons/secB.5.4 10-16 photons/secC.8.9 1014 photons/secD.1.8 1015 photons/secE.2.5 1018 photons/sec

Q: What is the energy of a photon with a frequency of 1.09 1015 s-1?A.6.08 10-49 JB.1.82 10-40 JC.7.22 10-19 JD.2.75 10-7 JE.2.75 102 J

Q: Excited sodium atoms emit light in the infrared at 589 nm. What is the energy of a single photon with this wavelength?A.5.09 1014 JB.1.12 10-27 JC.3.37 10-19 JD.3.37 10-28 JE.1.30 10-19 J

Q: According to experiments concerned with the photoelectric effect, which of the following will increase the kinetic energy of an electron ejected from a metal surface? 1/ increasing the wavelength of the light striking the surface 2/ increasing the frequency of the light striking the surface 3/ increasing the number of photons of light striking the surface A.1 only B.2 only C.3 only D.1 and 3 E.1, 2, and 3

Q: The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength. A.energy, directly, inversely B.energy, inversely, directly C.velocity, directly, inversely D.intensity, inversely, directly E.amplitude, directly, inversely

Q: If a cordless phone operates at a frequency of 9.00 108 s-1. What is the wavelength of this radiation?A.0.333 mB.1.99 10-25 mC.3.33 10-9 mD.3.71 10-18 mE.2.70 1017 m

Q: What is the frequency of gamma ray radiation that has a wavelength of 11.4 pm?A.3.80 10-20 s-1B.1.74 10-14 s-1C.2.63 107 s-1D.3.42 109 s-1E.2.63 1019 s-1

Q: If a radio wave has a frequency of 17.0 MHz, what is the wavelength of this radiation?A.5.10 1015 mB.5.67 10-2 mC.5.88 10-2 mD.1.76 101 mE.1.76 106 m

Q: A green laser pointer emits light at 532.0 nm. What is the frequency of this radiation?A.1.594 102 s-1B.1.775 10-15 s-1C.1.595 1011 s-1D.5.635 1014 s-1E.6.270 10-12 s-1

Q: Which of the following statements is/are CORRECT? 1/ FM radio waves have longer wavelengths than visible radiation and AM radio waves have shorter wavelengths than visible radiation. 2/ Magnetic resonance imaging (MRI) uses a mixture of x-rays and gamma rays. 3/ Exposure to ultraviolet (UV) radiation can lead to sunburns. A.1 only B.2 only C.3 only D.1 and 2 E.1, 2, and 3

Q: Which of the following colors of visible light has the lowest frequency? A.green B.orange C.red D.yellow E.blue

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