Chapter 5 Review: page 214 - 251

TEST OUTLINE:

-basic safety rules

-classifying elements terms such as solutions, mixtures, heterogeneous.... etc

-atomic structure (electrons, protons, neutrons) charge, size, location

-ionic and covalent bonds (know the basic difference between them)

-naming compounds and writing chemical formulas for:

(a) binary compounds

(b) molecules

(c) polyatomic compounds

1.check out glossary on page 708, text

2.

(a)element

(b) chemical property

(c) reactant

(d) alkali metals

(e) cation

(f) ion

(g) synthetic

3.

(a)False: solutions are homogeneous mixtures

(b) False: it is a physical property

(c) true, but a burning splint would be better

(d) False: they are halogens

(e) False: neutrons are neutral and are in the nucleus

(f) False: it will be negative

(g) False: they are covalent bonds

(h) False: "poly" means many elements

(i) False: they are natural polymers

4. I will describe the electron dot diagrams instead

(a) aluminum is surrounded by 3 dots

(b) fluorine is surrounded by 7 dots

(c) magnesium is surrounded by 2 dots

(d) phosphorus is surrounded by 5 dots

5. For each of these, the idea is to draw the Bohr diagram which would result if the element GAINED or LOST electrons to achieve a full outer orbital. (stable octet)

6. and 7

(a) MgCl2 (magnesium chloride)

(b)NaBr (sodium bromide)

(c) MgO (magnesium oxide)

(d)AlP (aluminum phosphide)

(e) Al2S3 (aluminum sulfide)

8.

(a) sulfur ion--------------- S-2

(b) argon -----------------

(c) potassium ion K +1

9.

(a)copper (I) chloride

(b) Iron (II) iodide

(c)SnO2

(d)PbBr2

10.

(a) copper (II) carbonate

(b) iron (II) sulfate

(c) Sn4(PO4)3

(d) Pb(NO3)2

11

(a) CO

(b) NI3

(c) sulfur dichloride

(d) carbon tetrachloride