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Study Resources (Chemistry)

41) Identify the compound with atoms that have an incomplete octet. A) ICl5 B) CO2 C) BF3 D) Cl2 E) CO 42) Which compound has the longest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same 43) Which compound has the shortest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same 44).
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11) Choose the compound below that should have the lowest melting point according to the ionic bonding model. A) LiF B) NaCl C) CsI D) KCl E) RbI 12) Identify the compound with ionic bonding. A) NaF B) K C) H2O D) He E) S 13) Identify the compound with covalent bonding. A) NaCl B) K C) H2O D) He E) S 14) Identify the compound with metallic.
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8.2   Algorithmic Questions 1) Aluminum metal reacts with aqueous iron(III) oxide to form aqueous aluminum oxide and iron metal.  What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients? A) 1 B) 2 C) 3 D) 4 2) Strontium phosphate reacts with sulfuric acid to form strontium.
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  7.1   Multiple Choice Questions 1) Identify the number of electron groups around a molecule with sp hybridization. A) 1 B) 2 C) 3 D) 4 E) 5 2) Identify the number of electron groups around a molecule with sp2 hybridization. A) 1 B) 2 C) 3 D) 4 E) 5 3) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3. A).
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21) Determine the name for P4O10. A) phosphorus (IV) oxide B) diphosphorus pentoxide C) phosphorus oxide D) phosphorus (II) oxide E) tetraphosphorus decoxide 22) Determine the name for N2O5. A) dinitrogen pentoxide B) nitrogen oxide C) nitrogen (IV) oxide D) nitrogen (II) oxide E) nitrogen tetroxide 23) Calculate the molar mass for Mg(ClO4)2. A) 223.21 g/mol B) 123.76 g/mol C) 119.52 g/mol D) 247.52 g/mol E) 75.76.
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7.4   Short Answer Questions 1) Give the electron geometry, molecular geometry, and hybridization for both carbons in CH3COOH. 2) Determine the hybridization about each interior atom in the following structure.  Sketch the three-dimensional structure and label the interior atoms with their corresponding hybridization. CH2CHCCCH3 3) According to molecular orbital theory, what is an antibonding.
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51) Write the name for CrS. A) chromous sulfate B) chromous sulfide C) chromic sulfide D) chromic sulfate E) chromium sulfide 52) Give the formula for ferrous nitrate. A) Fe(NO2)3 B) Fe(NO3)3 C) Fe(NO3)2 D) Fe(NO2)2 E) Fe2(NO2) 53) The solid compound, Na4SiO4, contains A) Na+, Si4+, and O2- ions. B) Na+ and SiO4 -4 ions. C) Na4+ and SiO4 -4 ions. D) Na4SiO4 molecules. 54) What.
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11) Identify the compound with the smallest percent ionic character. A) HF B) IBr C) HCl D) LiF 12) Choose the bond below that is most polar. A) H-I B) H-Br C) H-F D) H-Cl E) C-H 13) Choose the bond below that is least polar. A) P-F B) C-Br C) C-F D) C-I E) C-Cl 14) Using periodic trends, place the following bonds in order of.
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61) 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 = trigonal planar, mg = bent D) eg = trigonal bipyramidal, mg = see-saw E) eg = tetrahedral, mg = trigonal pyramidal 62) Determine the.
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7.3   Matching Questions Match the following. A) trigonal planar B) sp hybridized central atom C) sp2 hybridized central atom D) tetrahedral E) linear F) trigonal bipyramidal G) octahedral   1) sp Diff: 1    Var: 1    Page Ref: 7.3 LO:  7.1 Global:  G2 2) sp2 Diff: 1    Var: 1    Page Ref: 7.3 LO: 7.1 Global: G2 3) sp3 Diff: 1    Var: 1    Page Ref: 7.3 LO:  7.1 Global:  G2 4) sp3d Diff: 1    Var:.
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5.3   Matching Questions Match the following. A) H2(g) B) Ne2(g) C) Cl(g) D) Ne(g) E) O2(g) F) I(s) G) Cl2(g) H) H(g) I) Ca(s) J) Ca2(s) K) O(g) L) I2(s)   1) oxygen Diff: 1    Var: 1    Page Ref: 5.7 LO: 5.4 Global: G2 2) chlorine Diff: 1    Var: 1    Page Ref: 5.7 LO:  5.4 Global:  G2 3) neon Diff: 1    Var: 1    Page Ref: 5.7 LO: 5.4 Global: G2 4) calcium Diff: 1    Var: 1    Page Ref:.
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6) Describe the difference between a pure covalent bond and a polar covalent bond. 7) Draw the Lewis structure for the acetate ion, CH3CO2?, including any important resonance structures.  Label each atom with its formal charge. 8) Draw the Lewis structure for BrO3-.  Make sure to include any important resonance structures. 9) Define.
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61) The chemical formula for the chlorite ion is A) Cl-. B) Cl3-. C) ClO2-. D) ClO3-. 62) The ion, AsO33-, is named A) arsenate ion. B) arsenite ion. C) arsenic dioxide ion. D) arsenic(II) oxide ion. 63) The compound, SO3, is named A) sulfate. B) sulfite. C) sulfur trioxide. D) sulfur (VI) oxide. 64) Determine the name for F2O. A) fluorine oxide B) difluorine monoxide C).
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51) Which of the following compounds is nail polish remover? A) (CH3)2C=O B) C2H5OH C) CH3CO2H D) CH3CO2CH3 E) CH3OCH3 52) Which of the following represent the Lewis structure for N? A) B) C) D) E) 53) Which of the following represent the Lewis structure for Cl? A) B) C) D) E) 54) Which of the following represent.
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6) Describe the difference between ionic and molecular compounds.  Give an example of each. 7) Draw the Lewis Dot structure for Al3+. 8) Why aren't prefixes used in naming ionic compounds? 9) Explain why the lattice energy of MgS is approximately 4 times as large as that of NaCl. 10) Calculate the mass percent.
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5.4   Short Answer Questions 1) How can one compound contain both ionic and covalent bonds?  Give an example. 2) Describe the difference between a molecular formula and an empirical formula.  Give an example. 3) Define empirical formula. 4) What is the structure of the covalent compound formed by nitrogen and oxygen?  Is this the.
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81) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3. A) eg = trigonal planar, mg = trigonal planar, nonpolar B) eg = tetrahedral, mg = trigonal pyramidal, polar C) eg = trigonal planar, mg = trigonal pyramidal, polar D) eg = trigonal bipyramidal, mg = trigonal planar, nonpolar E) eg = octahedral,.
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6.3   Matching Questions Match the following. A) metallic bond B) weakest ionic bond C) highest melting point D) longest covalent bond E) strongest covalent bond   1) Sr-Sr Diff: 1    Var: 1    Page Ref: 6.6 Global:  G2 2) Cs-I Diff: 1    Var: 1    Page Ref: 6.6 Global:  G2 3) Ca-O Diff: 1    Var: 1    Page Ref: 6.6 Global:  G2 4) Se-I Diff: 1    Var: 1    Page Ref: 6.6 Global: .
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11) Give the formula for calcium hydrogen sulfate. A) CaHSO4 B) Ca2(HSO4)2 C) Ca2HSO4 D) Ca(HSO4)2 12) Give the formula for calcium bisulfate. A) CaHSO4 B) Ca2(HSO4)2 C) Ca2HSO4 D) Ca(HSO4)2 13) Give the name for KMnO4. A) potassium manganese tetraoxide B) potassium manganate C) potassium permanganate D) potassium permagnesium E) potassium magnesate 14) Determine the name for CoCl2?6H2O.  Remember that Co forms several ions. A) cobalt.
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11) A molecule containing a central atom with sp3d2 hybridization has a(n) ________ electron geometry. A) octahedral B) trigonal pyramidal C) tetrahedral D) bent E) trigonal planar 12) Consider the molecule below.  Determine the hybridization at each of the 2 labeled carbons. A) C1 = sp3, C2 = sp2 B) C1 = sp2, C2 = sp2 C) C1 =.
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  8.1   Multiple Choice Questions 1) A physical change A) occurs when iron rusts. B) occurs when sugar is heated into caramel. C) occurs when glucose is converted into energy within your cells. D) occurs when water is evaporated. E) occurs when propane is burned for heat. 2) A chemical change A) occurs when methane gas is.
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51) Give the approximate bond angle for a molecule with an octahedral shape. A) 109.5° B) 180° C) 120° D) 105° E) 90° 52) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg = trigonal planar, mg = trigonal planar B) eg = tetrahedral, mg = trigonal planar C) eg = tetrahedral, mg = trigonal pyramidal D).
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21) Identify the compound with ionic bonds. A) Ne B) CO C) H2 D) H2O E) KCl 22) Identify the compound with covalent bonds. A) CH4 B) Kr C) KBr D) K E) NaCl 23) Which of the following contains BOTH ionic and covalent bonds? A) CaBr2 B) COS C) BaSO4 D) SF6 E) None of the above contain both ionic and covalent bonds. 24) What is the.
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61) Which of the following statements is true? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity. E) None of the above are.
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5.2   Algorithmic Questions 1) Identify an ionic bond. A) Neutrons are pooled. B) Electrons are shared. C) Electrons are transferred. D) Protons are gained. E) Protons are lost. 2) Which of the following ionic compounds would be expected to have the highest lattice energy? A) CsF B) CsCl C) CsBr D) CsI 3) Which of the following ionic compounds would be expected.
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  6.1   Multiple Choice Questions 1) A single covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs 2) A double covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs 3) A triple covalent bond contains ________ of electrons. A) 0 pairs B).
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11) Which molecule or compound below contains a pure covalent bond? A) Li2CO3 B) SCl6 C) Cl2 D) PBr3 E) LiF 12) Which molecule or compound below contains a polar covalent bond? A) C2H4 B) MgS C) KF D) NI3 E) AgCl 13) Which molecule or compound below contains an ionic bond? A) CS2 B) C2Cl4 C) SiF4 D) OCl2 E) NH4NO3 14) The electronegativity is 2.1 for.
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