|This set of questions is optional. If you completed the
mandatory review set without problems you may skip it.
If you had problems then you'd better do it.
|1.||Where is nearly all of the mass of an atom located?
Explain your answer in terms of what contributes to this mass.
|2.||Calcium arsenate, Ca3(AsO4)2,
is a poison sometimes used to kill insects on plants. What is the mass
of 0.586 mole of calcium arsenate?
|3.||Calculate the formula weight of Fe4[Fe(CN)6]3.
|4.||Which of the following atomic species have a) 1,
b) 2, or c) 3 unpaired electrons in their outer shell?
H, He, Li, Be, C , N, O, F, Ne.
|5.||Define monoprotic acid, diprotic acid and polyprotic
|6.||An oxide of a certain element produced an acidic
solution when dissolved in water. The oxide has the empirical formula X2O3,
where X represents the symbol for the element. Is the element X a metal
or a nonmetal? In which group in the periodic table does it belong?
|7.||Which alkaline earth metal is used in flashbulbs
and flares? Why? Explain using a chemical equation.
|8.||Give Lewis structures for (a) CS2, (b)
CN-, (c) SeO3, and (d) SeO2
|9.||Which of these bonds is most polar and which is
least: SO, ClCl, or ClO?
Justify your arrangement.
|10.||Write the formulas for|
|(a) aluminum sulphide
(b) strontium fluoride
|(c) titanium(IV) oxide
(d) chromous bromide
|11.||Write molecular, ionic and net ionic equation for
the reaction between Pb(NO3)2 and Fe2(SO4)3.
|12.||One way to prepare iodine is to mix sodium iodate,
NaIO3, with hydriodic acid, HI. The following reaction occurs.
|NaIO3 + 6 HI --------> 3 I2
+ NaI + 3 H2O
|Calculate the number of moles and the number of grams of iodine that can be made this way from 16.4 g of NaIO3.|