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Study Resources (Chemistry)

51) Arrange in order by decreasing boiling point: Cl2,     I2,     HI A) I2, Cl2, HI B) Cl2, I2, HI C) Cl2, HI, I2 D) HI, Cl2, I2 E) HI, I2, Cl2 52) Arrange the following compounds in order of increasing boiling point: pentane (CH3CH2CH2CH2CH3), methyl butane (CH3CH(CH3)CH2CH3), neopentane (CH3C(CH3)3). A) pentane,.
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41) Define activation energy. A) the difference between the energy of the products and reactants B) the energy difference between the maximum energy of reaction and the energy of the products C) the minimum total kinetic energy that molecules must bring to their collisions for a chemical reaction to occur D) the total.
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21) Which compound is most likely to be soluble in hexane? A) water B) acetone (CH3COCH3) C) benzene (C6H12) D) ethyl alcohol (CH3CH2OH) E) chloroform (CHCl3) 22) Which of the following pairs of liquids would form a nonideal solution? A) CHCl3 and (CH3)2CO B) C6H5-CH3 (toluene) and C6H6 (benzene) C) CH3CH2CH2OH and CH3CH(OH)CH3 D).
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21) What is the difference between "normal boiling point" and "boiling point" of a liquid? A) "Normal boiling point" is a boiling point of a liquid at normal (standard) pressure and temperature, while "boiling point" is measured at any other conditions of pressure and temperature. B) "Normal boiling point" is a boiling.
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51) Choose the INCORRECT statement. A) The geometrical distribution of electron groups is the electron-group geometry. B) The geometrical arrangement of the atomic nuclei is the molecular geometry. C) A polar molecule has a dipole moment. D) A dipole moment is the product of the number of atoms and the.
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1) The valence-bond method describes covalent bonding as the overlap of partially filled orbitals. 2) The valence-bond method provides energy information about molecules. 3) A double bond is two sigma bonds. 4) A triple bond is two sigma bonds and one pi bond. 5) Molecular orbitals are formed by adding and subtracting atomic orbitals. 6).
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1) In the solution, a solute is present in the greatest quantity. 2) Molality is independent of temperature, molarity is dependent on temperature. 3) For the formation of an ideal solution from two liquid hydrocarbons, ΔHsoln < 0. 4) The stronger the forces between solute and solvent molecules, the more exothermic the solution.
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21) Which combination of hybrid orbital descriptions and electronic geometry descriptions is INCORRECT? A) sp/linear B) sp2/trigonal planar C) sp3/tetrahedral D) sp3d/square planar E) sp3d2/octahedral 22) Which hybrid orbitals are impossible in electrically neutral molecules containing only the elements shown? A) sp3/Al and H B) sp2/B and F C) sp/C.
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31) Vaporization occurs more readily with: A) increased temperature, increased surface area, decreased volume B) increased temperature, increased surface area, increased intramolecular forces C) increased temperature, decreased surface area, decreased intermolecular forces D) increased temperature, increased surface area, decreased intermolecular forces E) increased temperature, decreased surface area, decreased intermolecular forces 32) The phenomenon of supercooling refers.
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81) What is the correct molecular geometry for SeBr3+? A) trigonal pyramidal B) tetrahedral C) trigonal planar D) bent E) T-shaped 82) What is the correct molecular geometry for the carbon atom in urea (NH2)2CO? A) Tetrahedral B) T-Shaped C) Trigonal planar D) Trigonal pyramidal E) Trigonal bipyramidal 83) What is the correct molecular geometry for silicon atom in disilane Si2H6? A).
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71) The maximum temperature at which a gas can be liquefied is just below the ________. A) boiling temperature B) critical temperature C) melting temperature D) normal temperature E) superheating temperature 72) Liquid and vapor phases of a substance become indistinguishable at the ________. A) triple point B) normal point C) permanent.
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61) Which of the following involves delocalized π bonds? A) acetylene (C2H2) B) benzene (C6H6) C) carbon tetrachloride (CCl4) D) dichlorodifluoromethane (CF2Cl2) E) ethylene (C2H4) 62) If the HCOO- ion is described using delocalized electrons, why can the oxygen atoms  not have sp3 hybrids? A) There must be an unhybridized.
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1) A Lewis structure is a combination of Lewis symbols representing either the transfer or the sharing of electrons in a chemical bond. 2) Covalent bonds are formed by atoms sharing electrons. 3) The core electrons are called valence electrons. 4) A chemical bond for which one of the bonded atoms provides.
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61) A catalyst: I)lowers activation energy II)provides an alternate reaction pathway III)is consumed in the reaction and therefore does not appear in the chemical equation of each mechanism IV)speeds a reaction V)is heterogeneous if it is in a different phase than the reactants A) I, III, and IV B) I, IV, and V C) II, III,.
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