Atoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal.

Transcription

1 Atoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal. b. Give the name and symbol for one transition metal. c. Give the name and symbol for one noble gas. d. Give the name and symbol for one element that assumes a 3- charge when it combines with a metal. e. Give the name and symbol for one halogen. 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 Au 3+ and O NH 4 + and NO 3 G Hg 2 2+ and PO 4 3G Ca and Se Mn 4+ and S H and SO 3 2G Cu 2+ and S Al and Cr 2 O 7 2G Rb and N

2 3. the following compounds. Sr(NO 3 ) 2 BeCl 2 IF 3 P 2 O 5 FeO FePO 4 SF 4 BrF 5 NCl 3 NaCl 4. Define the term isotope. 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? 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? 6. 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 % % % %

3 7. Fill in the missing information in the following table. Ca(NO 3 ) 2 Phosphorous pentabromide MnCl 2 (NH 4 ) 2 SO 4 SF 6 8. Fill in the missing information in the following table. Nuclide # Protons # Neutrons # Electrons I Cl Ca Es 9. How many electrons would the I atom contain if it had an overall charge of -1? 10. Complete the following table. Species Protons Neutrons Electrons Rn Ca 2+ 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 Fe 3+ and N Rb and O Al and I Zn and P 12. Provide the names of the following compounds. SF 3 Cr 2 O 3 AgCl IF 5 CuS 13. Write formulas for the following compounds. Manganese (IV) oxide Chlorine trifluoride Barium oxide Gold (III) phosphide Dinitrogen tetroxide 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 Fe 3+ and NO 3 -

5 15. each of the following chemical compounds. Compound NH 4 Cl HNO 3 (aq) PbCl 2 KC 2 H 3 O 2 PCl Write formulas for each of the following named compounds. Compound barium nitride perchloric acid aluminum sulfate dinitrogen tetroxide chromium (III) oxide 17. 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 Write the chemical formula for each of the following compounds. Aluminum chlorate Barium phosphate Ammonium sulfide Lead (IV) oxide Potassium oxide

6 19. Complete the following table: Species Mass Number # Protons # Neutrons # Electrons As 75 Cl - 20 Ba Write the chemical formula for the compound made between each of the following species. Chemical Sodium and fluorine Barium and nitrogen Ammonium and sulfur Aluminum and sulfate Iron (II) and chlorine Ammonium and nitrate Copper (I) and oxygen Silver (I) and phosphorous Lead (II) and phosphate Magnesium and bromine

7 21. 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 ) each of the following first as a pure compound and then as a water-based solution. Compound Water-based solution HCl HNO 3 H 2 S H 2 SO 4 H 2 SO Complete the following table. Species Mass Number Number Protons Number Electrons Number Neutrons 50Sn Ge S 2-32

8 24. State whether each of the following is an ionic or molecular (covalent) compound. BaCl 2 SF 6 BrCl CH 4 MgO 25. Fill in the missing information in the following columns. Chemical BF 3 KNO 3 Fe 3 (PO 4 ) 2 H 2 SO 3 CoCl Complete the following table. copper (I) oxide ammonium sulfite strontium oxide bromine triiodide sulfur hexafluoride Symbol # Protons # Neutrons # Electrons Mass Number Charge 107 Ag

9 27. Write the chemical symbol for an example of each of the following elements. Metal: Halogen: _ Alkaline earth: _ Noble gas: 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 BF 3 N 2 O 4 Ag 2 O 29. Write the chemical formula and the name for the compound formed from each of the following species. Chemical Ca and P NH 4 + and N Rb and PO 4 3- Al and O Mg and NO 3 -

10 30. a. State the number of protons, neutrons, electrons, and the mass number of Mg b. What is the mass number of a Si atom that contains 14 protons, 19 neutrons, and 10 electrons? 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. 31. Write the formula for and name the compound formed by combining the following species. Ca and acetate Sr and N ammonium and S Al and Cl 32. the following compounds. Fe 2 O 3 Mn(OH) 2 N 2 O 5 SO 3