Chapter 6 Study Sheet Answers- Atoms and Bonding -
Vocabulary:
anion - a negative ion; results from a nonmetal atom that has gained electrons.
binary compounds - compounds containing only two elements. Examples: NaCl, H2O, Al2O3 .
chemical bond - force that holds particles together in a compound. Types are ionic and covalent bonds.
cation - a positive ion; results from a metal atom that has lost electrons.
covalent bond - the attraction for a shared pair of electrons that holds a molecule together.
crystalline lattice - a repeating pattern of unit cells in an ionic compound.
diatomic - a molecule of two atoms of the same element.
electron affinity - an attraction for an electron. Metals have low, nonmetals have high e- affinity.
ionic bond - the attraction between a cation and anion that holds the unit cell together.
ionization energy - Energy required to remove an electron from an atom. Metals have a low ionization
energy while nonmetals have a high ionization energy.
metallic bond - the attraction for electrons that hold metal atoms together.
molecule - the smallest part of a covalent compound.
oxidation number - another name for valence. The charge on an ion.
polyatomic ion - a multi atom ion. A molecule with a charge.
unit cell - the smallest part of an ionic compound. Unit cells make up a crystalline lattice.
valence - the charge on a ion
Write the formula for:
1. dihydrogen sulfide H2S
3. ammonium sulfate (NH4)2SO4
5. calcium carbonate CaCO3
7. manganese(IV) chloride MnCl4
9. dinitrogen trioxide N2O3
Write the name for:
10. NaNO3 sodium nitrate
12. F2 diatomic fluorine
14. H3N trihydrogen nitride
16. Fe2O3 iron(III) oxide
18. Ca3(PO4)2 calcium phosphate
2. lithium phosphide Li3P
4. carbon tetrafluoride CF4
6. iron(II) chloride FeCl2
8. phosphorus trichloride PCl3
11. PI3 phosphorus triiodide
13. (NH4)2CO3 ammonium carbonate
15. Na2SO3 sodium sulfite
17. CuO copper(II) oxide
19. MnO2 manganese(IV) oxide
Which of the above is a / are:
20. binary compounds? 1,2,4,6,7,8,9,11,14,16,17,19
21. ionic compounds? 2,3,5,6,7,10,13,15,16,17,18,19
22. covalent compounds? 1,4,8,9,11,14,
23. polyatomic compounds? 3,5,10,13,15,18
24. Would exist in a crystalline lattice? 2,3,5,6,7,10,13,15,16,17,18,19 (same answer as #21)
25. Would exist as a molecule? 1,4,8,9, 11, 12,14,
Oxidation Numbers:
26. -3 27. +1 28. -1
29. +3
30. 0
31. +4
32. -2
33. +2
When and why must you:
34. use Roman numerals? with names of transition metals - to show their valence
35. use prefixes? names of covalent compounds - to determine their formulas
36. use the valence of an element?- when writing ionic formulas or ionic compounds to
determine subscripts of ionic chemical formulas.
37. use the electron dot models - drawing covalent molecules - to show covalent bonds
(shared pairs of electrons)
38. use the Bohr model - drawing ionic compounds - to show ions that make up a unit cell.
39. Atoms become ions by losing or gaining electrons to have a stable electron arrangement
(octet rule).
Identify the following:
40. phosphide
44. barium ion
41. calcium ion
45. chlorine atom
42. carbon atom
43. sodium ion
50)
51. Water (shown above) is polar because of the eight protons in the oxygen atom pull the 10 electrons
closer to the oxygen end of the molecule giving it a partial negative charge. The two protons at the
hydrogen end of the molecule give that end of the molecule a partial positive charge.
For a molecule to be polar it must have a difference of 5 or more protons in one atom compared to
another.
Nitrogen monoxide is not polar because there is not a big difference between the number of protons in a
nitrogen atom (7) and an oxygen atom (8).
Chapter 6, pages 187-189A.
Reviewing Content:
1) B 2) C 3) A 4) D 5) C 6) B 7) D 8) B 9) C 10) A
B. Understanding Concepts:
11. A filled outer e- energy level (which is usually 8 valence electrons).
12. Each dot represents a valence electron.
13. The transfer of e-.
14. Attraction between it and the oppositely charged ion next to it.
15. The number of atoms of that element in the molecule or ions of that element in the unit cell.
17. A single covalent bond consists of one pair of shared electrons between two atoms, a double
covalent bond consists of two pairs of shared electrons between two atoms, a triple covalent bond
consists of three pairs of shared electrons between 2 atoms.
18. In diatomic elements, the two atoms sharing electrons have the same number of protons.
19. The oxygen, with 8 p+, has a greater attraction for the 10 e- in the molecule than does the hydrogen
atom (with only 1 p+).
22. a. sulfur trioxide b. carbon monoxide c. nitrogen dioxide
24. A mixture of copper and tin is harder and stronger than either metal in its pure form.
C)Critical Thinking:
26. All 3 have the same electron configuration of 2,8.
27. Both have covalent bonds holding the molecule together.
28. SO3 - polar covalent, CaO - ionic, diatomic iodine - non-polar covalent.
29. sulfur dichloride, silver(I) sulfate, lithium fluoride, carbon disulfide, calcium hydroxide.
30. Q is a metal, X and Z are nonmetals.
31. QX, Q2Z.
32. Cr2Z3
33. See diagram---------------------------->
34. Non polar covalent bonds.
D) Math Skills
35.eight
36. 2:1 There are two anions for every one caion.
37. BaF2, Na2O, FeSO4 , (NH4)2SO4
D) Concepts in Action:
38) B because hydrogen can only form one covalent bond.
40) It is a polyatomic ion held together with covalent bonds.
E) Preparing for the FCAT:
1) One 2) B 3) H 4) C 5) F 6) A