~AME ~_£_Y_ PERIOD _

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CHAPTERS 6-8 TEST REVIEW

Information you may need:

Electronegativity Difference Bond Character> 1.7 Mostly ionic

0.4-1.7 Polar covalent<0.4 Mostly covalent0 Nonpolar covalent

Questions #1-10 are TRUE or FALSE.Write TRUE or FALSEon the blank next to each question.

1. yuf; The elements in group 18 are relatively unreactive because they have a full octet of

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valence electrons.

2. ~\S-e The MgF3 compound is likely to occur. -1921- F- -h>al?l.'/CI rj,04lJ be ft/J~,3. [q I ~e Lattice energy decreases when the charge of an ion increases. l' iOI) c~(t(Jte ::: l' Ill-\+lt.JV -tMfA J4. IrL{& A water molecule has a bent molecular geometry because its oxygen atom has 4 V

electron groups and 2 lone pairs..- ..". "2-~ 15 e. The hybrid orbital for the central oxygen atom in 03 is Sp3. .0 -==- 0 - 0: s,p. .,

Ir u e.. The greater the electronegativity an element has the greater the affinity for electrons

\ 5.\ 6.

that element has.

\ 7. Jru.-L

\ 8. lwe\ 9. True..-

\ 10. ral(e

A positive ion is called a cation.

Fluorine is the element that has the greatest electronegativity.

Nonmetals tend to gain electrons to form ions.

For each successive electron removed from an atom, the ionization energy stays the

same. I+- [r«. real eJ,

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JL~Y13. List the elements with an electron configuration of s2d3

.

Ct a.Jiu~1!JioJ,iulrJ/ IOYlfallAm/ Duhtll"lAh]

~ v,»; i; Db14. Determine the group, period, an block of an atom

bwith the following electron configurations: .

\. a. [Ne]3s' Gmup I, Oeo'fJd 5, ,,- It:Ja AlflheIJU!:J1

I I

\ b. [He]2s' broup 2, periud Z/ ~-bl{;(,1c- &ry})/Uh/\ c. [Kr]Ss24d10Sps Grou n IJn -jlv I::. rodil

D. Alkali Earth metals H. Metalloids

A. Alkali metals E. Lanthanides

B.Actinides F. Noble Gases

C. Halogens G.Transition metals

16. For the following pairs of elements, circle which one has the larger ionization energy.

" I_a. ;_i an~ 5'20 vS. 20g0I b. _Ban~ ?J(P l)$" C;ODI c. F nd (I /6 SO IJ)',. J-ZS-D

17. For the following pairs of elements, circle which one has the larger electronegativity.

J a. a an@ ];1/1 vs. 3.q~I b. Baanc@ ()/~1 vs. o. ss:I c. Fe nd Fr /, ~ s VS, 0,7

18. For the following pairs of elements, circle which one has the larger atomic radius.

I a. K nd Li 71:/ v~, I«:1 b. F anW /2 v~, --;7l 105 VS, ZJ~

,

\25. Explain how covalent bonds are formed.

Pairs ekckol1J or« s.kred In ord-er k~;m C()f)1ple-f~C?~f~ ,

26. What is t e energy required to remove an electron called?

Tot1i?:a,;h '0" =»'/27. What is bond energy?

Gem re1Lured 10 lreak. a Covalf".J bOJ1d,28. Describe a dipole-dipole intermolecular force.

/he.. plDs,/-i"e end cl a dipole ~m tI. po tar }YIol-e L isa.~J c,t-el io lite )1~Q I)'ve end ofJ- elf 0 I (U -e.1o or /fIoJ.f!lu/e, IAJeltt-, Ie on a'1(J~her

29. hich elements are needed-to complete a hydrogen bond?

1+ and a A 'Oh Iy ~'edronp4.jjve tl.Q/I'Icnt- (/tlJ OJ FJ.

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~F;,i30. Are van der Waals forces strong or weak intermolecular forces?

31. What does the VSEPRmodel help determine about a molecule?

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34. Complete the following table about naming compounds and writing formulas:

32. List two properties of a covalent compound.

(j)[OW (VI€/~";t fXJ illtr ~ Fz;o" if1f-o a (f\J sial laMice(?) low bt" I~ r int.r @SM-{J)VCi /)r;~ C'u!J /.. or eosr«: aJ~J' 6'No}\(ondlltfor

33. Predict t e type of bond hat will form bet een the fot6wing pairs of atoms (electronegativities

are given in parentheses):

\ a, K (0,82) and CI (3,16) r;;lecko"?14J;~;I, di.{+.~1./6 -O.&,?::; 2.31 }lo~f~{/ j:&JUc.

\ e. N (3,04) and N (3,04) fJfclron1fu ~V ,'I-y d~.-:.5.o~- 5.0'1 z: 0 ~I)lIPC~10k, c. C (2.55) and 0 (3.44) EI cJ..ro~lf&d"/~JttcJ,ff::::: ~, Lf'l- Z,S-<;;=- 0, <go, polar

{/ (o~tlltl~\ d. C (2.55)·and H (2.20) '/D,. I. I, :'~ J,',f+. Z CIS- ? I _I:..-I ~ trt» h f?Aa'l'l.IO- -::> . - L.O __'" /)c-V .- I , (/f:>::>

Mt~\eM

Formula

\

Compound

r>entanitrogen trioxide

Ammonium sulfate

Chlorous acid

HF

Cu(N02h

Is the compound an acid,ionic, or molecular?

ItJn IG

35. Is the oxygen ion (02-) more or less stable than the oxygen atom? Explain your choice.

\1l.e- 02- (PXYten ion) is roore. dv-bl-e- fAAtt -I-Ae oxYt,e h afvl1)

b8C4~{e fAe {J)(Y5}eYI iOI1 AfH it t:./J odef III ,'Is o,JljInOSor J aJ I ()

rt;y36. Draw a Lewis structure for the following molecules:

, a. SO," if: v.e: '" 6·H-j (6)+2~ 32 ••·0·. ,_. I

.0 C' ••• -<::>--0;. , .,2-

so ,.#\

37. Draw the Lewis structure for N02- and label the sigma bonds and pi bonds.

#- v.e: -=- e- Z (~)f- J =-- I~ v. e IG- .. /" 0 ~ ')O:f J rr~ ~. •.- - • ~- M v,.. It ~. -O",I/, .O::=N:;;zO: Dr tu-fJ=-Q"

/' /IV" • - IJ • ~38. Draw the resonance structure for 502. I q-#: Vte,-~6+2(6);;;Jg I),e,,-

•• ••O · .....-: •• -S==q: <:'---~;»0=- S-0:." -.

39. Classify each of the following molecules as either POLARor NONPOLAR:

I

a. 5Cbit v,e. -:- 0,f 2 (1) -=- 0 «e.:

polarb. cS2

\ if: v,e, -~ V~ 2(,,):: "v.e.- •Non po lar .~

c. CF4

\ J. V.8.- ~lJ~Lj(7J -=- sZ .,«: ~F:N J •• I ••on PC) a r: : f. - ~--f.;

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