Multiple Choice - Simeon Career Academy
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 1. The number of atoms in a mole of any pure substance is called
|a. |its atomic number. |c. |its mass number. |
|b. |Avogadro’s number. |d. |its gram-atomic number. |
____ 2. What can be said about 1 mol Ag and 1 mol Au?
|a. |They are equal in mass. |
|b. |They contain the same number of atoms. |
|c. |Their molar masses are equal. |
|d. |They have the same atomic mass. |
____ 3. An Avogadro’s number of any element is equivalent to
|a. |the atomic number of that element. |c. |6.022 × 1023 particles. |
|b. |the mass number of that element. |d. |12 g of that element. |
____ 4. The atomic mass of hydrogen is 1.008 amu. The reason that this value is not a whole number is that
|a. |hydrogen only exists as a diatomic molecule. |
|b. |the mass of hydrogen is the sum of the masses of the protons and electrons in the atom. |
|c. |the mass of a proton is not exactly equal to 1 amu. |
|d. |hydrogen has more than one isotope. |
____ 5. A chemical formula includes the symbols of the elements in the compound and subscripts that indicate
|a. |the number of formula units present. |
|b. |the number of atoms or ions of each type. |
|c. |the formula mass. |
|d. |the charges on the elements or ions. |
____ 6. How many atoms of fluorine are in a molecule of carbon tetrafluoride, CF4?
|a. |1 |c. |4 |
|b. |2 |d. |5 |
____
____ 7. A formula that shows the simplest whole-number ratio of the atoms in a compound is the
|a. |molecular formula. |c. |structural formula. |
|b. |ideal formula. |d. |empirical formula. |
____ 8. The molar mass of an element is the mass of one
|a. |atom of the element. |c. |gram of the element. |
|b. |liter of the element. |d. |mole of the element. |
____ 9. To determine the molar mass of an element, one must know the element’s
|a. |Avogadro number. |c. |number of isotopes. |
|b. |atomic number. |d. |average atomic mass. |
____ 10. What is the molar mass of magnesium?
|a. |12.00 g |c. |24.305 g |
|b. |26.982 g |d. |22.990 g |
|b. |C4F |d. |CF2 |
____
____ 12. What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl?
|a. |CaCl |c. |CaCl2 |
|b. |Ca2Cl |d. |Ca2Cl2 |
____ 13. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
|a. |CHO |c. |C3H4O3 |
|b. |CH2O |d. |C2H4O2 |
____ 14. The percentage of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound?
|a. |25% |c. |75% |
|b. |50% |d. |90% |
____ 15. What is the percentage of OH– in Ca(OH)2?
|a. |45.9% |c. |75% |
|b. |66.6% |d. |90.1% |
16 How many atoms are there in 3.33 moles of strontium?
2.00 x 1024 atoms
3.21 x 1032 atoms
1.11 x 1011 atoms
4.24 x 1023 atoms
17 How many atoms are there in 3.33 moles of strontium?
2.00 x 1024 atoms
3.21 x 1032 atoms
1.11 x 1011 atoms
4.24 x 1023 atoms
18 What is the mass of 3.35 moles of sulfur trioxide?
335 g
268 g
245 g
19 How many moles are there in 425.0 g of sodium chloride?
9.835 mol
8.126 mol
7.272 mol
6.691 mol
20 What is the mass of 5.55 moles of carbon monoxide?
155 g
143 g
138 g
122 g
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