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Study Resources (Chemistry)

Algorithmic Questions 1) Which has the smallest dipole-dipole forces? A) CH3Cl   B) HBr C) O2 D) NO   2) Which is expected to have the largest dispersion forces? A) C3H8 B) C12H26 C) F2 D) Be Cl2 3) Which of the following compounds exhibits hydrogen bonding? A) CH3I B) H2 C) C6H5OC D) CH3CH 4) In liquid ethanol, CH3CH2OH   which intermolecular forces.
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Short Answer Questions 1) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example. 2) Explain why oil and water do not mix. 3) Determine the molecular geometry about each interior atom in the following structure. Sketch the three-dimensional structure and.
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6) Define dynamic equilibrium between the liquid and gaseous phases. 7) Why is the ΔvapH higher than ΔfusH for a given compound? 8) Sketch the phase diagram of benzene. Make sure to label the axes and the different phases of benzene. Use the physical data provided below. melting point = 279 K boiling point.
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61) At atmospheric pressure, dry ice ________. A) freezes B) deposits C) sublimes D) melts E) boils 62) The melting point of water is ________. A) 0 °C B) 32 °C C) 212 °C D) 100 °C E) 273 °C 63) The freezing point of water is ________. A) 0 °C B) 32 °C C) 212 °C D) 100 °C E) 273 °C 64) The boiling point of.
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31) Determine the electron geometry for the molecule BrF3. A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral 32) Determine the molecular geometry for the molecule BrF3. A) Square pyramidal B) Seesaw C) T-shaped D) Square planar E) Trigonal planar 33) Determine the electron geometry for the molecule XeF4. A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral 34) Determine the molecular.
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21) Which of the following statements is TRUE? A) In general, the solubility of a solid in water decreases with increasing temperature. B) In general, the solubility of a gas in water decreases with increasing temperature. C) The solubility of a gas in water usually increases with decreasing pressure. D) The solubility of an.
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51) Choose the bond below that is the strongest. A) C-F B) C=O C) C-I D) I-I E) C≡N 52) Choose the bond below that is the strongest. A) N=O B) N-I C) N-O D) N-S E) N=N 53) Choose the bond below that is the weakest. A) Na-Cl B) I-I C) C=N D) Li-F E) C=O 54) Choose the bond below that is the weakest. A) C≡O B) N≡N C).
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  Multiple Choice Questions 1) Identify the characteristics of a liquid. A) indefinite shape and volume B) indefinite shape, but definite volume C) definite shape and volume D) none of the above E) all of the above 2) Which one of the following has a low density? A) gas B) liquid C) solid D) none of the above E) all of the above 3).
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71) Identify the number of electron groups around a molecule with a tetrahedral shape. A) 1 B) 2 C) 3 D) 4 E) 5 72) A molecule containing a central atom with sp3d hybridization has a(n) ________ electron geometry. A) tetrahedral B) linear C) octahedral D) trigonal planar E) trigonal bipyramidal 73) Identify the number of electron groups around a molecule with.
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111) Use the molecular orbital diagram shown to determine which of the following is paramagnetic. A) B22? B) B22? C) N22? D) C22? E) B2 112) Draw a molecular orbital diagram and use it to determine which of the following is most stable. A) F2 B) F22? C) Ne22? D) O22? E) F22? 113) Draw a molecular orbital diagram and use.
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41) Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms. A) 1 = trigonal planar, 2 = tetrahedral, 3 = trigonal pyramidal B) 1 = tetrahedral, 2 = tetrahedral, 3 = tetrahedral C) 1 = trigonal planar, 2 = tetrahedral, 3 = tetrahedral D) 1 = tetrahedral, 2.
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11) Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force. A) Cl2 B) CO C) HF D) NaCl E) All of these have intermolecular forces stronger than dispersion. 12) Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force. A) H2 B) SO2 C) NH3 D) CF4 E) BCl3 13) Choose the compound.
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6) List the least electronegative atom. 7) Define dipole moment. 8) How are electron affinity and electronegativity different? 9) Describe the difference between a pure covalent bond and a polar covalent bond. 10) Draw the Lewis structure for the acetate ion CH3CO2?, including any important resonance structures. Label each atom with its formal charge. 11).
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81) Which molecule or compound below contains a pure covalent bond? A) Li2CO3 B) SCl6 C) Cl2 D) PF3 E) NaCl 82) Which molecule or compound below contains a polar covalent bond? A) C2H4 B) ZnS C) LiI D) NCl3 E) AgCl 83) Which molecule or compound below contains an ionic bond? A) CO2 B) C2Cl4 C) SiF4 D) OCl2 E) NH4NO3 84) Draw the Lewis structure for.
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51) How many of the following molecules are polar? XeO2SiCl2Br2C2Br2SeCl6 A) 1 B) 4 C) 2 D) 3 E) 0 52) How many of the following molecules are polar? PCl5COSXeO3SeBr2 A) 2 B) 0 C) 1 D) 3 E) 4 53) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2. A) eg = tetrahedral, mg = bent, polar B) eg = trigonal planar,.
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Algorithmic Questions 1) What geometric arrangement of charge clouds is expected for an atom that has four charge clouds? A) trigonal bipyramidal B) octahedral  C) tetrahedral  D) square planar 2) What is the molecular geometry of ClF4 -? A) seesaw B) square planar C) square pyramidal D) tetrahedral 3) What is the molecular geometry of NCl3? A) T-shaped B) tetrahedral C) trigonal.
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31) Choose the compound below that should have the lowest melting point according to the ionic bonding model. A) LiF B) NaCl C) CsI D) KBr E) RbI 32) Identify the complete electronic configuration for Br-. A) 1s22s22p63s23p64s24p6 B) 1s22s22p63s23p64s24d104p6 C) 1s22s22p63s23p64s23d104p6 D) 1s22s22p63s23p64s23d104p5 E) 1s22s2p63s2p64s23d104p6 33) Identify the complete electronic configuration for Ca2+. A) 1s22s22p63s24p6 B) 1s22s22p63s23p6 C) 1s22s22p63s23p5 D) 1s22s23p64s25p6 E) 1s22s2p63s2p6 34) Identify the complete.
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Matching Questions Match the following. A) dispersion forces B) dipole-dipole forces C) ion-dipole forces D) hydrogen bonding E) ionic bond F) H2 + H2O 1) LiI Diff: 1     Type: MA     Var: 1     Page Ref: 11.3 2) CH3OH Diff: 1     Type: MA     Var: 1     Page Ref: 11.3 3) CH3CH3 Diff: 1     Type: MA     Var: 1     Page Ref: 11.3 4) CH2F2 Diff: 1     Type: MA     Var: 1    .
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Multiple Choice Questions 1) Give the approximate bond angle for a molecule with a trigonal planar shape. A) 109.5° B) 180° C) 120° D) 105° E) 90° 2) Give the approximate bond angle for a molecule with a tetrahedral shape. A) 109.5° B) 180° C) 120° D) 105° E) 90° 3) Give the approximate bond angle for a molecule with a linear shape. A).
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81) Which of the following is considered an atomic solid? A) Br2 B) CsCl C) N2 D) Nb E) None of these is an atomic solid. 82) Which of the following is considered a nonbonding atomic solid? A) Ne B) Fe C) I2 D) Ca E) Li 83) Identify the type of solid for AgCl. A) metallic atomic solid B) ionic solid C) nonbonding atomic.
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31) Which of the following statements is TRUE? A) Vapour pressure increases with temperature. B) Hydrogen bonds are stronger than covalent bonds. C) Intermolecular forces hold the atoms in molecules together. D) Dispersion forces are generally stronger than dipole-dipole forces. E) None of the above is true. 32) Which of the following statements is FALSE? A) The.
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  Multiple Choice Questions 1) Choose the statement below that is TRUE. A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions. B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the.
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21) Which of the following reactions is associated with the lattice energy of RbI (Δr)? A) Rb(s) + I2(g) → RbI(s) B) RbI(s) → Rb?(g) + I?(g) C) RbI(s) → Rb(s) + I2(g) D) RbI(s) → Rb?(aq) + I?(aq) E) Rb?(g) + I?(g) → RbI(s) 22) Identify the compound with the highest magnitude of lattice energy. A).
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21) Give the approximate bond angle for a molecule with octahedral electron geometry and square planar molecular geometry. A) 90° B) 180° C) >120° D) <90° E) <120° 22) Determine the electron geometry (eg) and molecular geometry (mg) of BrF3. A) eg = trigonal planar, mg = trigonal planar B) eg = trigonal bipyramidal, mg = T-shape C) eg.
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91) How many of the following molecules have sp hybridization on the central atom? C2Cl2CO2O3H2O A) 0 B) 1 C) 2 D) 3 E) 4 92) How many of the following molecules have sp3 hybridization on the central atom? XeCl4CH4SF4C2H2 A) 0 B) 4 C) 3 D) 2 E) 1 93) How many of the following molecules have sp3d hybridization on the central atom? SiCl4BrF5AsF5BrF3 A).
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41) Choose the substance with the lowest boiling point. A) H2S B) NBr3 C) F2 D) CF2H2 E) H2O2 42) Which of the following substances would you predict to have the highest ΔvapH? A) CH3Cl B) HCl C) HOCH2CH2OH D) CH3CH2OH E) CH3CH2CH2CH3 43) Which of the following substances would you predict to have the highest ΔvapH? A) Xe B) C6H6 C) SiF4 D) Br2 E) N2 44).
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11) Using the VSEPR model, the molecular geometry of the central atom in SO2 is ________. A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal 12) Using the VSEPR model, the molecular geometry of the central atom in NCl3 is ________. A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal 13) Using the VSEPR model, the.
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Matching Questions Match the following. A) longest covalent bond B) metallic bond C) strongest covalent bond D) weakest ionic bond E) highest melting point 1) Sr-Sr Diff: 1     Type: MA     Var: 1     Page Ref: 9.2 2) Cs-I Diff: 1     Type: MA     Var: 1     Page Ref: 9.4 3) Ca-O Diff: 1     Type: MA     Var: 1     Page Ref: 9.4 4) Se-I Diff: 1     Type: MA     Var:.
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11) Determine the electron geometry (eg) and molecular geometry (mg) of PF5. A) eg = trigonal bipyramidal, mg = trigonal bipyramidal B) eg = octahedral, mg = octahedral C) eg = trigonal bipyramidal, mg = tetrahedral D) eg = tetrahedral, mg = trigonal pyramidal E) eg = trigonal planar, mg = octahedral 12) Determine the electron.
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  Multiple Choice Questions 1) Identify an ionic bond. A) Electrons are pooled. B) Electrons are shared. C) Electrons are transferred. D) Electrons are gained. E) Electrons are lost. 2) Identify the compound with ionic bonding. A) NaCl B) Li C) H2O D) He E) S 3) Identify the compound with covalent bonding. A) NaCl B) Li C) H2O D) He E) S 4) Identify the compound with metallic bonding. A).
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101) Choose the best Lewis structure for SeO42?. A) B) C) D) E) 102) Which of the following elements can form hypercoordinate compounds? A) N B) Br C) F D) Be E) None of the above can form compounds with an expanded octet. 103) How many of the following elements can form hypercoordinate compounds? IOClXe A) 2 B) 0 C) 3 D).
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Algorithmic Questions 1) Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiF B) LiCl C) LiBr D) LiI 2) Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiCl B) NaCl C) KCl D) RbCl 3) Which ionic compound would be expected to have the.
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Matching Questions Match the following. A) tetrahedral B) nonpolar, but contains a polar covalent bond C) sp hybridized central atom D) trigonal bipyramidal E) trigonal planar F) polar G) linear H) seesaw molecular geometry I) octahedral J) octahedral electron geometry K) polar, but contains no polar bonds L) sp2 hybridized central atom 1) SF4 Diff: 3     Type: MA     Var: 1     Page Ref: 10.4 2)XeCl4 Diff: 3     Type:.
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41) A double covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs 42) A triple covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs 43) Identify the shortest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D).
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