Chemistry

Q: What is the geometry around the central atom in the following molecular model of BCl3? A) linear B) bent C) trigonal planar D) trigonal pyramidal

Q: Which is the best description of the bonding in NO3-?A) 3 N O bonds and no N O bondsB) 3 N O bonds and 3 N O bondsC) no N O bonds and delocalized N O molecular orbitals extending over all four atomsD) 3 N O bonds and delocalized N O molecular orbitals extending over all four atoms

Q: The SO3 molecule can be described as having 3 Sî€„O Ïƒ bonds and Ï€ molecular orbitals containing A) 2 electrons. B) 4 electrons. C) 6 electrons. D) 8 electrons.

Q: Molecular orbitals extending over more than two atoms provide an explanation for A) coordinate covalent bonding. B) ionic bonding. C) paramagnetism. D) resonance.

Q: In which will the OO bond be made stronger by removing an electron? A) Only O2 B) Only O2- C) Only O22- D) All of these

Q: Based on molecular orbital theory, in order to weaken the NN bond in N2, electrons should be A) added. B) removed. C) either added or removed. D) neither added nor removed.

Q: Which is paramagnetic? A) N22+ B) N22- C) O22+ D) O22-

Q: Which statement concerning any homonuclear diatomic molecule and its 1- ion must be true? A) X2 must be more stable than X2-. B) X2 must be less stable than X2-. C) X2- must be paramagnetic and X2 must be diamagnetic. D) X2- must be paramagnetic and X2 may be paramagnetic or diamagnetic.

Q: Use the following MO diagram for Be2, Be2+, and Be2-. Based on this diagram, A) Be2+ is more stable than Be2, and Be2 is more stable than Be2-. B) Be2- is more stable than Be2, and Be2 is more stable than Be2+. C) Be2+ and Be2- are both more stable than Be2. D) Be2 is more stable than either Be2+ or Be2-.

Q: The paramagnetism of O2 is explained by A) coordinate covalent bonding. B) molecular orbital theory. C) resonance. D) valence bond theory.

Q: Given that O2 is paramagnetic and has a bond order of 2, and its highest occupied molecular orbital is antibonding, what would be the expected bond orders for O22- and O22+? A) 1 for O22- and 3 for O22+ B) 3/2 for O22- and 5/2 for O22+ C) 5/2 for O22- and 3/2 for O22+ D) 3 for O22- and 1 for O22+

Q: The following MO diagram is appropriate for Li2 and Be2. Based on this diagram, A) both are stable and diamagnetic. B) Li2 is stable and diamagnetic, but Be2 is unstable. C) Be2 is stable and diamagnetic, but Li2 is unstable. D) Be2 is stable and paramagnetic, but Li2 is unstable.

Q: The MO diagram below is appropriate for B2. Based on this diagram, B2 A) has a bond order of one and is diamagnetic. B) has a bond order of one and is paramagnetic. C) has a bond order of two and is diamagnetic. D) has a bond order of two and is paramagnetic.

Q: Which molecular orbitals for homonuclear diatomic molecules are degenerate?A) molecular orbitalsB) molecular orbitalsC) molecular orbitals and molecular orbitalsD) neither molecular orbitals nor molecular orbitals

Q: Compare the energies of molecular orbitals of homonuclear diatomic molecules with the energies of the atomic orbitals with which they correlate. A) Both bonding and antibonding molecular orbitals lie lower in energy than the atomic orbitals. B) Bonding orbitals are lower and antibonding orbitals are higher in energy than the atomic orbitals. C) Bonding orbitals are higher and antibonding orbitals are lower in energy than the atomic orbitals. D) Both bonding and antibonding molecular orbitals are higher in energy than the atomic orbitals.

Q: Which molecular orbital resembles a d-orbital?A) B) *C) D) *

Q: If an electron is added to H2 it would go into aA) molecular orbital and strengthen the H-H bond.B) molecular orbital and weaken the H-H bond.C) * molecular orbital and strengthen the H-H bond.D) * molecular orbital and weaken the H-H bond.

Q: Which molecular orbital resembles a p-orbital?A) B) *C) D) *

Q: What is the hybridization on the N atom in NO2- and in NO3-? A) sp2 for NO2- and sp3 for NO3- B) sp3 for NO2- and sp2 for NO3- C) sp for NO2- and sp2 for NO3- D) sp2 for both

Q: When the equation for the reaction of KBr(aq) with MnO2(s) to produce Br2 and Mn2+(aq) in acidic solution is balanced, the coefficient in front of the Br2 is ________.

Q: If niobium loses all of its valence electrons when it reacts with fluorine, what is the formula of the neutral binary compound that results?

Q: The oxidation number of the oxygen atoms in SrO2 is ________.

Q: Potassium reacts with oxygen to form a superoxide with the formula ________.

Q: The product of the reaction of lithium with nitrogen is ________.

Q: Lattice energy increases with ________ cation and anion charges and ________ cation and anion radii.

Q: The group 4A element that always obeys the octet rule in its stable compounds is ________.

Q: The third-row element having a less negative electron affinity than the elements on either side of it on the periodic table is ________.

Q: The element in group 7A with the least favorable (least negative) electron affinity is ________.

Q: What is the third-row element having the successive ionization energies in kJ/mol: 738, 1451, 7733, 10,540, 13,630, 17,995, 21,703?

Q: The element in period 3 with the smallest seventh ionization energy is ________.

Q: The element in period 4 with the smallest first ionization energy is ________.

Q: The ionic radius of Cs+ is ________ than the atomic radius of Cs, and the ionic radius of I- is ________ than the atomic radius of I.

Q: Isoelectronic means having the same number of electrons. The dipositive ion that is isoelectronic with Br- is ________.

Q: The ion Q2+ contains 10 electrons. The identity of element Q is ________.

Q: The number of electrons in the ion P3- is ________.

Q: The number of electrons in the ion Zn2+ is ________.

Q: The ion that has 28 protons and 26 electrons is ________.

Q: The neutral atom with the electron configuration [Ar}4s23d6 is ________.

Q: The tripositive ion with the electron configuration [Ar}3d6 is ________.

Q: Using shorthand notation, the ground-state electron configuration of the platinum ion in Cs2Pt is ________.

Q: Using shorthand notation, the ground-state electron configuration for C4" is predicted to be ________.

Q: Using shorthand notation, the ground-state electron configuration for Tl+ is predicted to be ________.

Q: Using shorthand notation, the ground-state electron configuration for Co2+ is predicted to be ________.

Q: Using shorthand notation, the ground-state electron configuration for Sr2+ is predicted to be ________.

Q: Which ionic compound would be expected to have the highest lattice energy?A) Rb2OB) Sr OC) In2O3D) C O2

Q: Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiF B) LiCl C) LiBr D) LiI

Q: An element that has the valence electron configuration 6s26p6 belongs to which period and group? A) period 6; group 6A B) period 6; group 8A C) period 7; group 6A D) period 7; group 8A

Q: How many valence shell electrons does an atom of indium have? A) 1 B) 2 C) 3 D) 49

Q: Which element has the highest first electron affinity? A) Na B) Mg C) O D) Ne

Q: Which of the following represents the change in electronic configuration that is associated with the first ionization energy of strontium?A) [ Kr] 5s15p1 -> [ Kr] 5s1 + e-B) [ Kr] 5s2 -> [ Kr] 5s15p1C) [ Kr] 5s2 -> [ Kr] 5s1 + e-D) [ Kr] 5s2 + e- -> [ Kr] 5s25p1

Q: Which of the following species will have the highest ionization energy? A) K+ B) Ar C) Cl- D) S2-

Q: Which ionization process requires the most energy?A) O(g) -> O+(g) + e-B) O+(g) -> O2+(g) + e-C) F(g) -> F+(g) + e-D) F+(g) -> F2+(g) + e-

Q: Which ionization process requires the most energy?A) W(g) -> W+(g) + e-B) W+(g) -> W2+(g) + e-C) W2+(g) -> W3+(g) + e-D) W3+(g) -> W4+(g) + e-

Q: Of the following, which element has the highest first ionization energy? A) Sr B) Br C) K D) Te

Q: Of the following, which element has the highest first ionization energy? A) Sr B) Rb C) Na D) Ca

Q: Of the following, which element has the highest first ionization energy? A) beryllium B) boron C) carbon D) lithium

Q: Of the following, which element has the highest first ionization energy? A) aluminum B) magnesium C) phosphorus D) sodium

Q: How many electrons are in the outermost shell of the Ga3+ ion in its ground state? A) 2 B) 3 C) 6 D) 18

Q: Which element, indicated by letter on the periodic table, is able to form compounds that do not obey the octet rule? A) A B) B C) C D) D

Q: What is the name for the group of elements indicated by the shaded portion of the periodic table? A) alkaline earth metals B) group 3A elements C) halogens D) noble gases

Q: What is the name for the group of elements indicated by the shaded portion of the periodic table? A) alkali metals B) alkaline earth metals C) inner-transition metals D) transition metals

Q: What is the likely formula for the binary compound formed from the elements represented by letters A and D on the periodic table above? A) AD B) A2D C) AD2 D) A2D3

Q: What is the likely formula for the binary compound formed from the elements represented by letters A and C on the periodic table above? A) AC B) A2C C) AC2 D) A2C3

Q: Which salt has the lowest lattice energy? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which salt has the highest lattice energy? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which picture corresponds to potassium fluoride? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which picture corresponds to iodine? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which picture corresponds to fluorine? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which picture corresponds to potassium? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which of the above pictures are more likely to represent covalent compounds? A) pictures (a) and (b) B) pictures (a) and (d) C) pictures (b) and (c) D) pictures (b) and (d)

Q: Which of the above pictures are more likely to represent ionic compounds? A) pictures (a) and (b) B) pictures (a) and (d) C) pictures (b) and (c) D) pictures (b) and (d)

Q: Which of the above pictures best represents a gaseous covalent compound? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which of the above pictures best represents a solid ionic compound? A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Atoms of which element, indicated by letter on the periodic table, would be expected to have the most negative value of Eea? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table above, would be expected to have the lowest second ionization energy, Ei1? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table above, would be expected to have the highest second ionization energy, Ei1? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table above, would be expected to have the highest first ionization energy, Ei1? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table above, would be expected to have the smallest first ionization energy, Ei1? A) A B) B C) C D) D

1 2 3 … 195 Next »

Subjects