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Homework answers / question archive /   Chemical Bonding Level 1 Multiple Choice   1) The formation of a chemical bond involves    1) only the protons;            2) protons and electrons;            3) electrons and neutrons;            4) only the electrons

  Chemical Bonding Level 1 Multiple Choice   1) The formation of a chemical bond involves    1) only the protons;            2) protons and electrons;            3) electrons and neutrons;            4) only the electrons

Chemistry

 

Chemical Bonding

Level 1

Multiple Choice

 

1) The formation of a chemical bond involves  

 1) only the protons;       

    2) protons and electrons;            3) electrons and neutrons;            4) only the electrons.

 

2. When elements combine to form compounds  

  1) only the outermost electrons of the

    atoms are involved;           2) all the electrons of the atoms are involved;          3) the

    protons and electrons are involved;           4) only the protons are involved.

 

3. What takes place when a chemical bond forms between two atoms?

    1) The forces of repulsion are greater than the forces of attraction.

    2) A pair of electrons is simultaneously attracted by two nuclei.

    3) An increase in potential energy results.

    4) The nuclei of the atoms become stable.

    5) The nuclei of the atoms become unstable.

 

4. When a chemical union occurs     1) all the elements retain their original properties;      

    2) new properties appear;         3) the metallic elements retain their original properties;

    4) the nonmetals retain their original properties.

 

5. The number of bonds formed by an atom is most closely associated with

    1) its atomic mass;          2) the number of electrons in the atoms;          3) the number

    of electron shells;          4) the number of electrons in the outer shell.

 

6. During chemical reactions, each atom tends to    1) lose electrons;       

    2) gain electrons;              3) lose an outer shell;               4) gain a complete shell.

 

7. To indicate the number of atoms of an element in a compound, we use

     1) a subscript to the right of the symbol;         2) an exponent to the right of the symbol;

     3) a subscript to the left of the symbol;          4) a coefficient to the left of the symbol.

 

8. A group of atoms which behaves as if it were a single atom is      1) non-existent;

     2) a macromolecule;         3) a fusion reproduction;         4) always negatively charged;

     5) a radical.

 

9. A radical is a group of atoms which     1) has variable valence;      

     2) is never positive;            3) acts like a single atom;            4) acts like a molecule.

 

10. The simplest formula for a compound is called the     1) correct formula;  

     2) molecular formula;                3) empirical formula;               4) atomic formula.

 

11. The formula which represents the simplest whole-number ratio of the atoms of

     the constituent elements in a compound is the     1) atomic formula;        

     2) molecular formula;            3) structural formula;.            4) electron-dot formula;      

     5) empirical formula.

 

12. The part of the atom obtained by excluding the valence electrons is known as the

     1) core;               2) ion;               3) nucleus;                4) radical;                5) shell.

 

13. All chemical changes involve     1) decreased stability;            2) electron sharing;

     3) formation of ions;            4) breaking bonds and forming bonds.

 

14. The forces of attraction which exist between hydrogen molecules in liquid hydrogen

     are due to     1) ionic bonding;         2) hydrogen bonding;         3) molecule-ion forces;       

     4) vander Waals forces.

 

15. How do noble gases differ from other gaseous elements?

     1) Molecules of the other gaseous elements cannot be decomposed.

     2) Only noble gases form monatomic molecules.

     3) Noble gases generally liquefy at higher temperatures.

     4) Molecules of the other gaseous elements are generally polar.

 

16. The process by which heated iodine crystals form a vapor without passing through

     the liquid state is     1) evaporation;            2) sublimation;            3) condensation;       

     4) distillation.

 

17. Solid substances are most likely to sublime if they have

      1) high vapor pressures and strong intermolecular attractions.

      2) high vapor pressures and weak intermolecular attractions.

      3) low vapor pressures and strong intermolecular attractions.

      4) low vapor pressures and weak intermolecular attractions.

 

18. Which period contains elements in which electrons from more than one principal

      energy level may be involved in bond formation?

      1) l                2) 2                3) 3                4) 4                5) none of these

 

19. Which part of the atom is involved in chemical bonding?

    1) only the nucleus                                 3) only the electrons

    2) only the protons                                 4) only the valence electrons

 

20. When an ionic bond is formed, the atom that transfers its valence electron

    becomes an ion with

    1) positive charge and more protons.

    2) positive charge and no change in the number of protons.

    3) negative charge and more protons.

    4) negative charge and no change in the number of protons.

 

21. When the atom gains an electron, the resulting particle is

     1) an ion;               2) a molecule;               3) an isotope;               4) a neutron.

 

22. What mono-atomic ion has 26 protons, 30 neutrons and 24 electrons?

     1) chromium (II)                2) copper (II)                3) iron (II)                4) zinc (II)

 

23. The bonding in the barium fluoride crystal is primarily

     1) ionic;                2) polar covalent;                3) metallic;                4) non-polar;       

     5) co-ordinate covalent.

 

24. Which compound is the most ionic?

     1) CCl4(l)                2) SiO2(s)               3) KCl(s)               4) NH3(g)                5) Br2(l)       

 

25. In which compound does the bond have the least degree of ionic character?

     1) KBr           2) HF           3) MgO           4) BrCl           5) All have the same degree.

 

26. Compounds which as crystals are composed of ions are      1) polar covalent;

     2) non-polar covalent;           3) electrovalent;            4) macro-molecular.       

 

27. If a pure substance is a good conductor of electricity in both its solid and its liquid

     phases, the bonding is the substance is predominantly

     1) ionic;             2) metallic;             3) polar covalent;             4) non-polar covalent.

 

28. Which type of bonding involves positive ions immersed in a sea of mobile electrons?

    1) ionic              2) non-polar covalent              3) polar covalent              4) metallic

 

29. The characteristic of metallic bonding that distinguishes it from other bonds is the

    1) fixed position of the valence electrons.

    2) polar property of substances with metallic bonds.

    3) freedom of movement of the valence electrons.

    4) directional nature of the bonds formed.

 

30. The ionic formula for calcium bromide is

     1) Ca+2Br-2;             2) Ca+2Br-2;             3) Ca2+Br-2;             4) Ca+Br-.

 

31. When Mg unites with Cl, there is a transfer of two electrons from each Mg atom

     to each of two Cl atoms.  From this we determine that     1) the Cl atom has seven

     electrons in its outer shell;          2) two covalent bonds form;           3) the Mg atom is

     larger than the Cl atom;          4) two ions were formed.

 

32. Consider the equation K0  +  F0  à  Na+F-.  This represents

     1) the sharing of electrons by K and F;           2) the transfer of a proton from F to K;  

     3) the transfer of an electron from F to K;           4) the change taking place when an

     electron is transferred from K to F.

 

33. Which one of the following is a polyatomic ion?

     1) Li3PO4              2) NH            3) Ca+2              4) SO4-2              5) none of these

 

34. Identify the polyatomic ion in the list below.

     1) As+3                2) P2O5                3) Br2                4) NaCl                5) NH4+         

 

35. A polyatomic ion can be found in which of the following choices?

     1) LiBr               2) ClO-3               3) O3               4) Sr+2               5) CH3COOH

 

36. If aluminum has an electronegativity of 1.6 and bromine an electronegativity of 2.9,

     the bond between these two elements should be     1) ionic;          2)  polar covalent;

     3) nonpolar covalent;            4) metallic;            5) coordinate covalent.

 

37. Which one of these elements is most likely to react to form an ionic compound?

     1) 2, 8, 8             2) 2, 8, 5             3) 2, 8, 7             4) 2, 8, 4             5) none of these

 

38. The element with the greatest chance to form ionic bonds would be

     1) 2, 8, 4            2) 2, 8, 1            3) 2, 8, 8, 8            4) 2, 8, 5            5) none of these

 

39. Which two elements form a compound having the greatest ionic character?

     1) cesium and fluorine            2) potassium and oxygen             3) lithium and sulfur

     4) sodium and iodine.

 

40. Which kind of bond predominates in Group I-A  with halides?

     1) Van der Waals          2) metallic          3) hydrogen          4) covalent          5) ionic

 

41. Which description applies to compound BY if elements B and Y have a large difference

     in electronegativity?

     1) Its atoms repel each other.         2) The bond is primarily ionic.         3) The bond is

     primarily metallic.          4) The bond is coordinate covalent.

 

42. The formula Sr(ClO3)2 represents     1) a molecule consisting of three ions;

     2) a molecule consisting of five atoms;          3) ionic bonds between three different

     elements;          4) a polyatomic ion with a valence number of –2.

 

43. The empirical formula of sodium chloride gives the relative proportions of its

     1) protons;               2) electrons;               3) ions;               4) molecules.

 

44. Consider the electron configuration 1s2  2s2 2px2 2py2 2pz1

     If this atom received one electron from another atom, it would become

     1) charged positively;           2) more active chemically;           3) more stable;       

     4) much heavier.

 

45. The structure difference between a molecule of  ammonia and an ammonium ion is one

     1) electron;         2) proton;         3) neutron;         4) hydroxide ion;         5) chloride ion.

 

46. When an ionic bond is formed, the atom that transfers its valence electron is the

     atom that has the     1) higher electronegativity;           2) lower atomic number;       

     3) higher atomic mass;           4) lower ionization energy.

 

47. The malleability, conductivity, ductility, and luster of metals can be explained by

     1) mobile electrons;        2) immobile electrons;        3) equally shared electrons pairs;

     4) unequally shared electron pairs.

 

48. Melting solid potassium iodide     1) produces ions;        2) decomposes the compound;

     3) releases ions from fixed positions in the solid;         4) produces free electrons.

 

49. A basic concept related to the halogens is that the smaller the size of the atom, the

     1) stronger the bonds formed;        2) less active the element;        3) fewer the valence

     electrons;        4) darker its color will be.

 

50. Hydrogen forms a negative ion when it combines with sodium to form NaH.

     This is mainly because hydrogen     1) loses an electron to sodium;        2) has a greater

     attraction for electrons than sodium has;         3) is a larger atom than sodium;

     4) has a smaller ionization energy than sodium.

 

51. Ionic solids     1) are soft and have low melting points;        2) melt to form liquids

      that conduct electricity;         3) are malleable;         4) conduct electricity.

 

52. The most difficult type of compound to decompose is one formed by

      1) very active elements;          2) very inactive elements;          3) noble elements;

      4) an inactive and an active element.

 

53. The symbol K+ represents one     1) atom of krypton;        2) atom of potassium;      

    3) ion krypton;         4) ion of phosphorus;         5) none of these.

 

54. When potassium and chlorine form a chemical compound, energy is

    1) released and ionic bonds are formed.         3) absorbed and ionic bonds are formed.

    2) released and covalent bonds are formed.   4) absorbed and covalent bonds are formed.

 

55. Metallic atoms become ions by     

    1) losing protons;       2) losing electrons;      3) gaining protons;      4) gaining electrons.

 

56. The highest electronegativity value is shown by

    1) fluorine;                  2) neon;                 3) lithium;                 4) cesium.

 

57. In sulfur trioxide, the valence of the sulfur is

    1) 1;                 2) 2;                 3) 8;                 4) 4;                 5) 6.

 

58. Which bond has the greatest degree of ionic bonding?

    1) Li-Br                 2) F-F                3) H-Cl                 4) S-O

 

59. As one proceeds from left to right across a given period on the Period Table, the    electronegativities generally       1) decrease;       2) remain the same;       3) increase;

    4) can not be generalized.

 

60. The difference between the ammonium ion and the molecule of ammonia,  NH3,  is one

    1) electron;                 2) neutron;                 3) proton;                 4) radical.

 

61. An example of a cation is    1) Ca+2;       2) SO4-2;       3) NO3-;       4) Cl0;       5) CH4.

 

62. An atom of a metal becomes an ion by the       1) loss of one or more electrons;

    2) gain of one or more protons;        3) gain of one or more electrons;        4) gain of one

    or more neutrons.

 

63. Hydrogen chloride is a compound which is

    1) non-polar covalent.             3) ionic.
    2) polar covalent.                    4) symmetrically covalent.           5) none of these.

 

64. Consider the following electron configurations:   ls2 2s1  &  ls2  2s2 2px22py22pz1.

    If these two atoms reacted with each other by transferring one electron, they would form

    1) a positively charged molecule.                               3) neutral ions.

    2) a negatively charged molecule.                               4) charged ions.

 

65. When metals combine with nonmetals, the chemical bond is usually     

    1) covalent;          2) ionic;          3) an absolute number;          4) molecular;

    5) a fusion of electrons.

 

66. Which substance has bonds of greatest ionic character?

    1) H2               2) RbF                3) XeF4               4) F2               5) A12S3
 

 

67. Determine the dominant type of bonding found in the molecule B2S3.

    1) polar covalent        2) ionic        3) coordinate covalent        4) non-polar covalent

 

68. Name the main type of bonding found in francium fluoride.

    1) coordinate covalent         2) non-polar covalent         3) polar covalent         4) ionic

 

69. A bond in which atoms share a pair of electrons is      1) an ionic bond;

    2) a covalent bond;         3) an electrovalent bond;           4) a binary compound bond.

 

70. A covalent bond consists of     1) a shared electron;        2) two electrovalent ions;

    3) a transfer of one or more electrons;         4) an octet of electrons;         5) a shared

    electron pair.

 

71. The bond formed by two atoms of the same element is     1) ionic;

    2) polar covalent;              3) non-polar covalent;              4) is not predictable.       

 

72. The type of bond formed when two atoms share a pair of electrons is called

     1) ionic;           2) coupled;           3) covalent;           4) bivalent;           5) conjugation.

 

73. Covalent bonds are usually formed by the combination of     1) a metal and a nonmetal;

     2) a metal and a acid group;          3) two nonmetals;          4) very active metal and the

     hydroxide ion.

 

74. If two atoms exert equal attractions for electrons, they form     1) a non-polar

     covalent bond;          2) an ionic bond;          3) a polar covalent bond;          4) no bond.

 

75. Which molecule has the most polar bonding characteristics?

     1) H2O              2) H2S              3) H2Se              4) H2Te              5) NaBr

 

76. Which of the following is not a polar molecule?

     1) hydrogen fluoride           2) hydrogen           3) water            4) ammonia (NH3)

 

77. Which of the following kinds of bonds exists in a N2 molecule?

     1) ionic            2) polar            3) single            4) double            5) triple

 

78. A polar molecule is one in which there is a separation of charge caused by

     1) an average distribution of electrons;         2) a non-uniform electron distribution;       

     3) a complete loss of electrons;          4) an uneven number of electron pairs.

 

79. Which molecule below will have a triple covalent bond?

     1) fluorine             2) oxygen             3) nitrogen             4) hydrogen

 

80. The substance having an electron-dot formula which reveal only two covalent bonds is

     1) HCl;             2) H2O;             3) CaCl2;             4) CH4;             5) none of these.

 

81. Which is an example of a non-polar molecule that contains polar covalent bonds?

     1) CBr4               2) N2               3) H2O               4) NH3               5) none of these

 

82. Covalent bonds are most likely to be found in the compound represented by the formula

     1) NaCl;               2) KBr;               3) CH4;               4) KI

 

83. Which one of these elements is most likely to react to produce a covalent compound?

     1) 2, 8, 8              2) 2, 8, 8, 2              3) 2, 8, 7              4) 2, 8, 6              5) 2, 8, 5

 

84. Which one is an example of a diatomic molecule?

     1) Mg+2              2) N2              3) He              4) H2SO4              5) none of these

 

85. Which period contains three elements that commonly exist as diatomic molecules

     at S.T. P. conditions?

     1) Period 1           2) Period 2           3) Period 4           4) Period 6           5) Period 7

 

86. Identify the formula which represents a non-polar molecule.

     1) HCl               2) CF4               3) NH3               4) H2S               5) Al2S3

 

87. In compounds where there is only electron sharing, the valence of both atoms is

     1) zero;        2) positive;        3) an absolute number;        4) equal but opposite in sign.

 

88. Which atom will form the most polar bond with hydrogen?

     1) F               2) Cl               3) Br                4) I               5) O

 

89. Why is NH3 classified as a polar molecule?

     1) It is a gas at STP.        2) N-H bonds are non-polar.        3) Nitrogen and hydrogen

     are both nonmetals.         4) NH3 molecules have asymmetrical charge distributions.

 

90. Which element will have the greatest attraction for bonding electrons?

     1) Li             2) S             3) Al             4) Zn             5) Each has the same attraction.

 

91. The molecules of  the ordinary gaseous elements oxygen, nitrogen, hydrogen, and

     chlorine are     1) monatomic;           2) diatomic;           3) composed of large numbers

     of atoms;           4) form ionic bonds.

 

92. In the diatomic fluorine molecule, each fluorine atom has an outer shell with the

     electron arrangement of the gas     1) hydrogen;           2) argon;           3) oxygen;

     4) nitrogen;           5) neon.

 

93. The substance whose electron dot formula indicates four covalent bonds is

     1) AlF3;               2) N2;               3) H2O;               4) CH2F2.

 

94. Which substance has an electron-dot formula that  indicates the presence of

     four covalent bonds?

     1) HCl               2) SiH4               3) NH3               4) H2O               5) Br4I4

 

95. The molecular shape predicted by the VSEPR theory when two shared pairs of

     electrons and no unshared pair of electrons surround the central atom is

     1) tetrahedral;               2) pyramidal;                 3) bent;               4) linear.

 

96. A nitrogen molecule     1) is polar;         2) contains three pairs of shared electrons;

     3) is unstable;         4) is very soluble in water;         5) none of these.

 

97. A coordinate covalent bond differs from an ordinary covalent bond in only the

      1) amount of ionic character of the bond.

      2) number of electrons involved in the bond.

      3) strength of the bond formed by the electrons.

      4) source of the electrons forming the bond.

 

98. The number of hybrid orbitals that result from sp2 hybridization is

      1) 1;               2) 2;               3) 3;               4) 4;               5) none of these.

 

99. Generally two nonmetals react to form a molecular compound. Why would you

    not expect two nonmetals to form an ionic compound?

    1) Nonmetals have similar attractions for electrons.

    2) Nonmetals give up electrons to other elements.

    3) Nonmetals tend to gain electrons from metals.

    4) Nonmetals usually do not form compounds with other nonmetals.

 

100. Which represents a polar molecule?

    1) F2              2) O2              3) CH4              4) CO2              5) HCl

 

101. Two helium atoms do not unite to form a bond because      

    1) helium is a gas;       2) the orbitals are half-filled;       3) the p orbitals are complete;      

    4) each atom has two electrons in the 1s orbital.

 

102. Which compound is predominantly covalently bonded?

    1) LiI               2) CaC12               3) NaH               4) CH4               5) KBr

 

103. The type of chemical bond that joins one or more elements together is determined

    by    1) atomic mass;       2) the arrangement of electrons;       3) the arrangement of

    neutrons;      4) the total number of electrons.

 

104. Which pair of elements will not form an ionic bond?

    1) Ba and Cl              2) Ca and S              3) K and O              4) C and Cl

 

105. Hydrogen bonds between molecules are formed in compounds where hydrogen

    atoms are bonded to atoms of elements with

    1) low electronegativity and large size.          3) low electronegativity and small size.

    2) high electronegativity and small size.        4) high electronegativity and large size.

 

106. Two atoms of nitrogen form a triple bond. What is the ratio of electrons involved in

    the triple bond to the total number of electrons in the valence shells of the two atoms?

    1) 3:10                 2) 6:18                 3) 3:8                 4) 6:10

 

107. When non-metallic elements combine with each other, the bonding is predominantly

    1) ionic;         2) covalent;         3) electrovalent;         4) trivalent;         5) deliquescent.

 

108. Which statement best explains why carbon tetrachloride (CCl4) is non-polar?

    1) Each carbon-chloride bond is polar.         2) Carbon and chlorine are both nonmetals.

    3) Carbon tetrachloride is an organic compound.          4) The carbon tetrachloride

    molecule is symmetrical.

 

109. Chemical bonds may be produced by any of the following processes involving electrons

       1) losing;        2) gaining;        3) sharing;        4) transferring;        5) splitting.

 

110. In the diatomic hydrogen molecule, each hydrogen atom has an outer shell with the

    electron structure of the gas   

1) oxygen;       2) chlorine;       3) helium;       4) ammonia.

 

111. The type of bond between hydrogen atoms and oxygen atoms in a molecule of

    water is     1) a hydrogen bond;        2) an ionic bond;         3) a non-polar ionic bond;      

    4) a polar  covalent bond.

 

112. Identify the predominant type of bonding that exists in the molecule BrCl.

    1) polar covalent         2) non-polar covalent         3) ionic         4) coordinate covalent

 

113. What  is the main type of bonding that exists in the nitrogen, N2?

    1) ionic         2) coordinate covalent         3) non-polar covalent         4) polar covalent

 

114. Which type of bonding is prevalent in the molecule carbon dioxide?

    1) non-polar covalent         2) coordinate covalent         3) polar covalent         4) ionic

 

115. Identify the main type of bonding present in carbon tetraiodide.

    1) non-polar covalent         2) ionic         3) polar covalent         4) coordinate covalent

 

116. Determine the prevalent type of bonding in pure water.

    1) ionic         2) non-polar covalent         3) polar covalent         4) coordinate covalent

 

117. Which type of bonding is dominant in the molecule OF2?

    1) coordinate  covalent         2) non-polar covalent         3) ionic         4) polar covalent

    

118. Which of the following is a false electron dot notation?

 

 

 

 

 

119. Which statement indicates the difference between the two diagrams for element X ?

 

 

 

 

 

    1) Figure 1 has a larger number of electrons than Figure 2;      2) The two atoms in

    Figure 2 are united by a pair of shared electrons;       3) Figure 2 shows the forma­tion

    of ions;     4) The atoms are more stable in Figure 1.

 

120. What is the true electron dot notation for ammonia, NH3?

 

 

 

 

 

 

121. The correct electron dot notation for a molecule of iodine is

 

 

  

 

 

122. If the electron configuration of an atom of element X is  1s2 2s22p4,  the electron dot

    symbol for the element is

 

 

 

 

 

123. Which of the following is a correct electron dot notation?

 

 

 

 

 

124. Nitrogen may be represented by the e1ectron-dot              

    The atom which would be represented ­by an identical electron-dot arrangement is

    1) 5B;             2) 10Ne;             3) 20Ca;           4) 15P.

 

125. The correct electron-dot formula for sodium bromide is

 

 

 

 

 

126. The correct electron-dot formula for sodium chloride is

 

 

 

127. Which is the most likely formula for a compound of arsenic and hydrogen?

     1) AsH               2) AsH2               3) AsH             4) AsH4               5) AsH5

128. What is the most probable formula for a compound of silicon and hydrogen?

     1) SiH              2) SiH2              3) SiH6              4) SiH4              5) Si2H4

 

129. Write the molecular formula formed by Ba uniting with Se.

     1) BaSe            2) BaSe          3) Ba2Se            4) Ba2Se3            5) none of these

 

130. Predict the correct molecular formula for the reaction of B with Te.

     1) BTe              2) B2Te              3) BTe3              4) B2Te3              5) none of these

 

131. Which molecule is most predictable when rubidium reacts with tellurium?

     1) RbTe2            2) RbTe3            3) Rb2Te            4) Rb2Te3            5) none of these

 

132. Which is the correct formula for the combining of Ca with P?

     1) CaP2              2) Ca3P2              3) Ca2P3              4) CaP3               5) none of these

 

133. Identify the correct formula for the chloride of silicon, atomic number 14.

     1) SiCl              2) SiCl2              3) SiCl            4) SiCl4              5) none of these

 

134. Predict the correct molecular formula for the reaction of Ra with At.

     1) Ra2At            2) RaAt2            3) Ra2At3            4) RaAt3            5) none of these

 

135. Which molecule is predictable when aluminum reacts with bismuth, Bi?

     1) AlBi3            2) AlBi            3) AlBi2            4) Al2Bi3            5) none of these

 

136. Consider the general formula XBr2.  Which group will for bromides with the

     formula above?

     1) IA              2) IVA             3) VIA              4) VIIA              5) none of these

 

137. The element A has an atomic number of 4, and the element B has an atomic number

     of 7.  The formula of the compound formed by the combination of these elements is

     1) A2B;              2) A3B2;              3) AB2;            4) A3B;              5) A2B3.

 

138. The formula B2Z3 suggests that      1) B is a nonmetal with a  valence number of 2;

     2) Z has a valence number of –3;        3) B has a valence number of +3;        4) the two

     elements are united by two non-polar covalent bonds.

 

139. Elements A and X combine to form the compound A3X2.  If the electron-dot symbol

     of the neutral atom A shows two electrons, the number of electrons in this symbol for

     atom X must be     1) 2;               2) 4;               3) 5;               4) 6.

 

140. The element B has an atomic number of 5 and the element C has an atomic number of 8. 

     The formula of the compound formed by the combination of these elements is

     1) B2C2;                2) B3C2;                3) BC2;                4) B2C;                5) B2C3.

 

141. Which formula is most likely to occur?

     1) SrRn              2) Sr2Rn              3) SrRn2              4) Sr2Rn3              5) none of these

 

142. Consider the general formula A2O3.  The elements which form oxides with this formula

     are in which Group?

     1) IA               2) IIA               3) VA               4) VIIA               5) none of these

 

143. Element Y has an electron configuration of 1s2 2s22p6  3s23p1.  This element will

     combine with the phosphate ion to form a compound with the formula

     1) YPO4;               2) Y(PO4)2;               3) Y2PO4;               4) Y2(PO4)3.

 

144. Element A is a nonmetal that forms a bromide with the formula ABr2.  Element A

     is in group     1) IA;                2) IIA;                3) VIA;               4) VIIA.

 

145. Element A has an electron configuration of 1s2 2s1, and element B has an electron 

     configuration of 1s2 2s22p4.  The most probable formula for a compound of these

     two elements is     1) AB2;               2) A2B;               3) A4B3;               4) A4B.

 

146. A sulfide compound with the formula Y2Z3 would be formed if sulfur combined with

     any element in Group     1) IA;               2) IIA;               3) IIIA;              4)  IVA.

 

147. Which formula represent a tetrahedral molecule?

     1) SiBr4                2) CaCl2                3) HBr                4) I2                5) AlF3

 

148. Identify the molecule that will have a linear shape.

     1) CCl4                2) H2O                3) NH3                4) CO2                5) Ag3PO4

 

149. Which molecule has a pyramidal shape?

     1) CBr4               2) CO2               3) BF3               4) NH3               5) none of these

 

150. To form a  molecule with a “bent” shape, the ratio of shared to unshared pairs of

     electrons is      1) 1:2;                2) 2:1;                3) 2:2;                4) 3:1.

 

151. Lithium readily reacts with all of the following except

     1) oxygen;           2) water;           3) the halogens;           4) helium;           5) sulfur.

 

152. What is the usual atomic ratio in which Group IA elements react with those

    from Group VIA ?
    1) 1:1                 2) 1:2                 3) 1:6                 4) 2:1                 5) 2:3

 

153. Predict the correct molecular formula for the reaction of Sr with As.

    1) SrAs              2) SrAs2               3) Sr2As              4) Sr2As3               5) Sr3As2
 

 

154. A molecule of helium is represented by the expression, He.  This statement indicates this

     substance is   1) a gas;        2) inert;        3) monatomic;        4) composed of two elements.

 

155. A compound made up of sodium, sulfur, and oxygen could be named

    1) sodium oxide;         2) sodium sulfide;         3) sulfur dioxide;         4) sodium sulfate.

 

156. Element X has an electron configuration of 1s2s22p3s2.  Element X will most

    likely form oxides with the formula       1) X2O;         2) X2O3;        3) XO;         4)XO2.

 

157. Manganese oxide has the formula MnO2.  What is the formula for manganese chlorate?

    1) MnClO3       2) Mn(ClO3)2       3) Mn2(C1O3)3       4) Mn(C1O3)4        5) Mn(ClO3)3

 

158. Which formula is most likely to happen?

    1) FrPo3              2) Fr3Po              3) Fr2Po3              4) Fr2Po              5) none of these

 

159. Which formula is most likely to happen?

    1) LiSb3              2) Li2Sb3              3) Li3Sb2              4) Li3Sb              5) LiSb2
 

 

160. Which formula is most likely to occur?

    1) InF               2) InF2              3) InF3              4) In2F             5) In3F2

 

 

161. The outermost shell of element “X” has 3 electrons while that of element “Y” has 6.

    The probable formula of a compound of these elements is

    1) X3Y2;               2) X2Y3;              3) XY;              4) X2Y.

 

    

162. Atoms of an element X have the electronic configuration  1s2s22p3s22p3

    The compound most likely formed with magnesium,  Mg,  is

    1) MgX;           2) Mg2X;           3) MgX2;             4) Mg2X3;             5) Mg3X2.

 

 

163. Element Y is a metal that forms an oxide with the formula Y2O.  Element Y is

    in group       1) IA;               2) IIA;               3) VIA;               4) VIIA.

 

 

164. The magnesium atom has 2 electrons in its outer shell while the bromine atom has

    7 outer shell electrons.  The correct formula for magnesium bromide is

    1) MgBr;             2) Mg2Br;             3) MgBr2;             4) Mg2Br2;             5) Mg3Br2.

 

 

165. When atoms unite      1) electrons are transferred from one atom to another atom;

    2) a metal and nonmetal combine;        3) the product is more stable than the sepa­rate

    atoms;           4) heat is absorbed.

 

 

166. Which of the following best describes the molecule containing Rb and Xe?

    1) RbXe           2) Rb2Xe           3) RbXe3           4) Rb3Xe           5) none of these
 

 

167. Which molecule is most predictable when thallium reacts with selenium?

    1) T12Se             2) T12Se3             3) TlSe3               4) TlSe           5) none of these

 

 

168. The number of molecules represented by the expression, 3 H2SOis   

    1) 1;                 2) 2;                  3) 3;                 4) 4;                 5) 6.

 

169. The most likely formula is

    1) Cs3N;             2) Cs3N2;            3) Cs2N3;            4) CsN3;            5) none of these.

 

170. What is the formula for the union of Ga and Cl?

    1) GaCl2           2) Ga2Cl3           3) GaCl3           4) Ga3Cl           5) none of these

 

171. Predict the correct molecular formula for the reaction of Al with Kr.

    1) AlKr2              2) Al2Kr3            3) AlKr            4) AlKr3            5) none of these

 

 

 

 

 

 

 

 

      

 

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