Open your books to page 626-627
No you can’t share a book.
Chapter 20 Review – Draw the concept map
in 19, Draw the entire electron
configuration for 22 see 628 for examples.
Use your vocab to answer 1-10
Complete Chapter 20 Review 1-15, 17-23,
27, 29, 31, 32
Due today, 35 points, will be graded for
accuracy
Chapter 20 Review 1-15, 17-23, 27, 29, 31, 32
1. polyatomic ion
2. binary compound
3. polar molecule
4. ion
5. ionic bond
6. covalent bond
7. hydrate
8. molecule
9. oxidation number
10. chemical formula
11. B - noble gases - b/c they have full outer energy levels
12. C - copper(II)oxide
13. A - N2 - diatomic, is nonpolar because it is two atoms with
same size nucleus and same number of electrons, no unequal
charge distribution
14. D - 1 - Group 17 has 7 valence electrons
15. B - NaF is binary ionic
17. A - negative ion - became negative by gaining an electron
18. D - sulfur and oxygen are both non-metals making this a
covalent compound
-----------------------------ALL ABOVE WORTH 1 POINT------------------------------------
19. 6 points - Chemical bonds form compounds because atoms often
become more stable by gaining, losing, or sharing electrons with
properties that are different from the individual atoms. (Order of 1st 2
can be switched) Kinds of cheimcal bonds are covalent where electrons
are shared between non-metals and ionic where electrons are lost by
metals/gained by non-metals.
20. H2S (– 1 point, 2 hydrogens, 1 sulfur)
21. TeF6, Na2SO4, BaCO3 – (3 points, 1 point each)
22. Skip
23. Tl2CO3 (- 1 point)
27. Copper is 2+ and sulfate is 2- (1- point)
29. a)iron(III)sulfide b) copper(II)chlorate c)calcium phosphate d)
ammonium sulfate (– 4 points, 1 point each)
31. C - 3+ (1 point)
32. a) KCl
b)CaCO3
c)CuSO4 d)Na2O (4 points, 1 each)