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Chapter 5 Review: page 214 - 251



-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



(b) chemical property

(c) reactant

(d) alkali metals

(e) cation

(f) ion

(g) synthetic



(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)



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

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

(c) potassium ion K +1



(a)copper (I) chloride

(b) Iron (II) iodide





(a) copper (II) carbonate

(b) iron (II) sulfate

(c) Sn4(PO4)3

(d) Pb(NO3)2



(a) CO

(b) NI3

(c) sulfur dichloride

(d) carbon tetrachloride