Atoms, Molecules, and Ions (Chapter 2) Old Quiz and Test Questions Answer Key

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1 Atoms, Molecules, and Ions (Chapter 2) Old Quiz and Test Questions Answer Key 1. a. Give the name and symbol for one alkaline earth metal. Choose from any element in Group 2: Be, Mg, Ca, Sr, Ba, Ra b. Give the name and symbol for one transition metal. Choose from any element in Groups 3-12 c. Give the name and symbol for one noble gas. Choose from any element in Group 18: He, Ne, Ar, Kr, Xe, Rn d. Give the name and symbol for one element that assumes a 3- charge when it combines with a metal. Choose from nonmetals in Group 15: N, P, As e. Give the name and symbol for one halogen. Choose from Group 17: F, Cl, Br, I, At 2. Complete the following table by writing chemical formulas in the middle column for the compounds formed with the indicated species and writing the name for the compound in the column to the right. I have supplied charges where there could be some question and as a part of any polyatomic ions. Species Chemical Compound Li and P Li 3 P lithium phosphide Au 3+ and O Au 3 O 2 gold (III) oxide or auric oxide NH + G 4 and NO 3 Hg 2+ 3G 2 and PO 4 NH 4 NO 3 (Hg) 3 (PO 4 ) 2 ammonium nitrate mercury (I) phosphate or mercurous phosphate Ca and Se CaSe calcium selenide Mn 4+ and S MnS 2 manganese (IV) sulfide H and SO 3 2G H 2 SO 3 hydrogen sulfite or, if dissolved in water, sulfurous acid Cu 2+ and S CuS copper (II) sulfide or cuprous sulfide Al and Cr 2 O 7 2G Al 2 (Cr 2 O 7 ) 3 aluminum dichromate Rb and N Rb 3 N rubidium nitride

2 3. the following compounds. Sr(NO 3 ) 2 strontium nitrate BeCl 2 berillium chloride IF 3 iodine trifluoride P 2 O 5 diphosphorous pentoxide FeO iron (II) oxide or ferrous oxide FePO 4 iron (III) phosphate or ferric phosphate SF 4 sulfur tetrafluoride BrF 5 bromine pentafluoride NCl 3 nitrogen chloride NaCl sodium chloride 4. Define the term isotope. Isotopes are two atoms of the same element that differ in the number of neutrons in their nuclei. 5. Considerable work is being done in the area of synthesizing new elements in special reactors. There is some thought that element 114 should be of particular significance as it presents the theoretical possibility of unusual stability compared to its immediate predecessors. Suppose a particular isotope of element 114 is discovered to have a mass number of 285. a. How many neutrons, protons, and electrons are present in the isotope discovered? #protons = 114 (corresponds to atomic number) #neutrons = mass number - # protons = = 171 neutrons #electrons = 114, assuming a neutral atom b. If element 114 were to behave as a metal, what charge might you expect it to adopt when it forms compounds with the nonmetals? Element 114 is below Pb, so you might expect similar charge behavior, in particular +2 or A particular element consists of the following isotopes with the given abundances and masses. Find the atomic weight of the element. Weight of isotope Natural abundance of isotope atomicweig ht % % % % = 77.12* * * *.409 = 79.46

3 7. Fill in the missing information in the following table. Ca(NO 3 ) 2 PBr 5 MnCl 2 (NH 4 ) 2 SO 4 calcium nitrate Phosphorous pentabromide manganese (II) chloride ammonium sulfate SF 6 8. Fill in the missing information in the following table. sulfur hexafluoride Nuclide # Protons # Neutrons # Electrons I Cl Bi Ca Es How many electrons would the I atom contain if it had an overall charge of -1? # electrons = # protons + 1 = = 54 electrons 10. Complete the following table. Species Protons Neutrons Electrons Rn Ca I Ar Cr

4 11. Write formulas for compounds formed from the following pairs of elements. Then name each compound. Charges are indicated where there is a choice. Species Ba and S BaS barium sulfide Fe 3+ and N FeN iron (III) nitride or ferric nitride Rb and O Rb 2 O rubidium oxide Al and I AlI 3 aluminum iodide Zn and P Zn 3 P 2 zinc phosphide 12. Provide the names of the following compounds. SF 3 Cr 2 O 3 AgCl IF 5 CuS sulfur trifluoride chromium (III) oxide or chromic oxide silver chloride iodine pentafluoride copper (II) sulfide or cupric sulfide 13. Write formulas for the following compounds. Manganese (IV) oxide MnO 2 Chlorine trifluoride ClF 3 Barium oxide Gold (III) phosphide BaO AuP Dinitrogen tetroxide N 2 O 4

5 14. As we will learn later tonight, naming ternary inorganic compounds simply involves learning species called polyatomic ions which are atoms stuck together that act as one ion. When naming compounds these polyatomic ions retain their names. Given that the nitrate ion is NO - 3 hazard a guess as to the formula and name for the following compounds. - Na and NO 3 NaNO 3 sodium nitrate Fe 3+ and NO 3 - Fe(NO 3 ) each of the following chemical compounds. Compound NH 4 Cl HNO 3 (aq) PbCl 2 KC 2 H 3 O 2 PCl 3 iron (III) nitrate or ferric nitrate ammonium chloride nitric acid 16. Write formulas for each of the following named compounds. lead (II) chloride or plumbous chloride potassium acetate phosphorous trichloride Compound barium nitride Ba 3 N 2 perchloric acid HClO 4 aluminum sulfate Al 2 (SO 4 ) 3 dinitrogen tetroxide N 2 O 4 chromium (III) oxide Cr 2 O Write the name of each of the following compounds. CaSO 4 KNO 2 IF 5 Fe 2 (SO 4 ) 3 NH 4 C 2 H 3 O 2 calcium sulfate potassium nitrite iodine pentafluoride iron (III) sulfate or ferric sulfate ammonium acetate 18. Write the chemical formula for each of the following compounds. Aluminum chlorate Al(ClO 3 ) 3 Barium phosphate Ba 3 (PO 4 ) 2 Ammonium sulfide (NH 4 ) 2 S Lead (IV) oxide PbO 2 Potassium oxide K 2 O

6 19. Complete the following table: Species Mass Number # Protons # Neutrons # Electrons As Cl Ba Write the chemical formula for the compound made between each of the following species. Chemical Sodium and fluorine NaF Barium and nitrogen Ba 3 N 2 Ammonium and sulfur (NH 4 ) 2 S Aluminum and sulfate Al 2 (SO 4 ) 3 Iron (II) and chlorine FeCl 2 Ammonium and nitrate NH 4 NO 3 Copper (I) and oxygen Silver (I) and phosphorous Cu 2 O Ag 3 P Lead (II) and phosphate Pb 3 (PO 4 ) 2 Magnesium and bromine MgBr each of the following compounds. Ba(NO 3 ) 2 NH 4 NO 2 CaF 2 PCl 5 HC 2 H 3 O 2 IF 3 CuBr CuBr 2 Mg(ClO 3 ) 2 Ba 3 (PO 4 ) 2 barium nitrate ammonium nitrite calcium fluoride phosphorous pentachloride hydrogen acetate, or dissolved in water acetic acid iodine trifluoride copper (I) bromide or cuprous bromide copper (II) bromide or cupric bromide magnesium chlorate barium phosphate

7 22. each of the following first as a pure compound and then as a water-based solution. Compound Water-based solution HCl hydrogen chloride hydrochloric acid HNO 3 hydrogen nitrate nitric acid H 2 S hydrogen sulfide hydrosulfuric acid H 2 SO 4 hydrogen sulfate sulfuric acid H 2 SO 3 hydrogen sulfite sulfurous acid 23. Complete the following table. Species Mass Number Number Protons Number Electrons Number Neutrons 50Sn Ge S State whether each of the following is an ionic or molecular (covalent) compound. BaCl 2 ionic SF 6 molecular BrCl molecular CH 4 molecular MgO ionic 25. Fill in the missing information in the following columns. Chemical BF 3 KNO 3 Cu 2 O (NH 4 ) 2 SO 3 Fe 3 (PO 4 ) 2 SrO BrI 3 H 2 SO 3 SF 6 CoCl 2 boron trifluoride potassium nitrate copper (I) oxide ammonium sulfite iron (II) phosphate or ferrous phosphate strontium oxide bromine triiodide hydrogen sulfite or, in water, sulfurous acid sulfur hexafluoride cobalt (II) chloride

8 26. Complete the following table. Symbol # Protons # Neutrons # Electrons Mass Number Charge Ag Ba As Write the chemical symbol for an example of each of the following elements. Metal: any element to the left of the stair step line Halogen: any member of Group 17: F, Cl, Br, I, At Alkaline earth: any member of Group 2: Be, Mg, Ca, Ba, Sr, Ra Noble gas: any member of Group 18: He, Ne, Ar, Kr, Xe, Rn 28. For each of the following compounds state whether it is molecular or ionic. Then write the name for the compound. Compound Molecular or Ionic? BaCl 2 ionic barium chloride BF 3 molecular boron trifluoride N 2 O 4 molecular dinitrogen tetroxide Ag 2 O ionic silver oxide

9 29. Write the chemical formula and the name for the compound formed from each of the following species. Chemical Ca and P Ca 3 P 2 calcium phosphide NH 4 + and N (NH 4 ) 3 N ammonium nitride Rb and PO 4 3- Rb 3 PO 4 rubidium phosphate Al and O Al 2 O 3 aluminum oxide Mg and NO 3 - Mg(NO 3 ) 2 magnesium nitrate 30. a. State the number of protons, neutrons, electrons, and the mass number of # protons = atomic number = 12 protons #electrons = #protons -2 = 12 = 2 = 10 electrons # neutrons = mass number number of protons = = 22 neutrons 34 Mg b. What is the mass number of a Si atom that contains 14 protons, 19 neutrons, and 10 electrons? mass number = # protons + # neutrons = 14 protons + 19 neutrons = 33 c. There are two naturally occurring isotopes of B. One has an atomic mass of amu and a natural abundance of 19.9 %, the other an atomic mass of and a natural abundance of 80.1 %. Show how we arrive at an atomic mass of B of from this information. atomicmass = * *0.801 =

10 31. Write the formula for and name the compound formed by combining the following species. Ca and acetate Ca(C 2 H 3 O 2 ) 2 calcium acetate Sr and N Sr 3 N 2 strontium nitride ammonium and S (NH 4 ) 2 S ammonium sulfide Al and Cl AlCl 3 aluminum chloride 32. the following compounds. Fe 2 O 3 Mn(OH) 2 N 2 O 5 SO 3 iron (III) oxide or ferric oxide manganese (II) hydroxide dinitrogen pentoxide sulfur trioxide

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