Homework# y . I

C r/J - .,. f /(~) . 1. · What was Dobereiner's groupings based on? Of'l'-f'lr>Y\. l..,I\J),,, • . 2. _What was Mendeleev ~en general credit for?

\:;_ ~t0odi ( ,a1Dl-e... 3. How did Mendeleev organize his periodic table? What was his innovation?

d . A,r() \y\cC \..DP. u\nt.,. ,pa llJL ~· ~ -I__

4. Mosely arranged his table by Q,tor::V:\\ e,

5. What is: a group? eolumn·on ~t et:'od\C'\

Af~ly? A period? row'on~e ~nod I C ~o.b\e.

+~b\e 6. How many of each of the terms in question~5

\'3 ~""ou\'°5 > 1 pe,r'crls 7. Define periodic law. . ~s \- (_~W,&1¥\ \')rtl\) - y ~ ~aJ \a"'>

<;Lts.\e~c • 8. Name 2 examples of something that is periodic.

,_ '1W ,~iL~ S.c.h~d uV•

'f .. What is a valence electron? \ exkr<\OS\- e\ecm:):') -fuuf'\d o" .\he a.s.\.- ?Q.. j CoMM oC\ \'j vs e d --fu< \::).:,ndlf"l~

10. For each of the following, state the nwnber of valence electrons. J

Na Po He As _J_ _fL_ 5

Rb Br Pb Sr I _7_ _J1_ __L

And answer the following Regents questions.

2-8-8@ _2_

2-8:-18-7 _L

L

F-te .... -..

..3. 1. In which set do the elements exhibit the ·most similar chemical properties? (1) N, 0, and F ©Li, Na and K (2) Hg, Br, and Rn (4) Al, Si and P

~2.All of the atoms of the elements in Period 2 have the same number of (1) protons -(2) neutrons 0{ valence electrons ~occupied energy levels (shells)

:· 3 '. The properties of elements are periodic · funptions of their

(1) mass numbers (3) atomic radii (2) atomic masses (,0 atomic numbers

_H_ 4. On the present Periodic Table of the Elements, the elements are arranged according to increasing (1) number of.oxidation states (2) number of neutrons (3) atomic mass @atomic number

__3_ 5._The properties of carbon are expected to be most sinrilar to those of (1) boron @silicon

· (2) aluminum (4) phosphorus

L 6. Which list consists of elements that have t~ most similar chemical properties? L:J (1) Mg, Al, and Si (3) K, Al, and Ni t {B) Mg, Ca, and Ba ( 4) K, Ca, and Ga

_!j_ 7. An atom of chlorine and an atom of bromine have the same (1) electronegativity (2) ionization energy 9l atomic radius

number of valence electrons

_!j__ An atom of an element has 28 innermost electrons and 7 outermost electrons. In which period of the P~c Table is this element locatea? (.§.? (1) 5 3G' ~3 (2)2 -~

_\ _9. What is the total number of valence electrons in ail atom of phospho~ in the ground state?

@s (2) 2

(3) 3 (4) 7

3 10. Given the electron configuration of an atom in the ground state: 2 - 8 - 6

This element is found in the Periodic Table in (1) Period 4 and Group 16

Period 4 and Group 14 Period 3 and Group 16 Period 3 and Group 14

I. What is the same for every element in period 2? 5QVY\~ Ct ?rt..'~

2. What is the same for every element in group 2? $cA VY\ e. lf O + VO\• -

3. Elements are arranged on the periodic table according to their A\-oo:) ", (. $'

4. List the valence electrons for each of the following:

Si y s L,

Ne %·. Sr J · Cu \, Rb l 0 lp . 02~ i.

-------Na \ Na+ -, '3. -~ Cl + er.

For each of the following, write the name of the group on the line.

5. The most reactive groups of metals. A \\lo.\~ · yY\ e. k~ \ S 6. The most reactive group of nonmetals. \-tO \O&e,- n S _ 1/

1

7. Can pull valence electrons from ans sublevel OR ad sublevel \ v-~•rt\CI\ M~\-cJIA_ 8. All members are radioactive, most are man-made. PIC.i- , f\ 1 QE:~

:J:ne...,.4 N L \ 0-9. Extremely unreactive group. <!>o,e;.. · ,: Cv~~ ~ I

_IO.Forms colorful ions \V~X\~ \ ·b 0 "\ ""e., 11. Electron configuration ends with s2 ~\~Cl \0

\r\~ t.o,-+h me,.\~ 12. Very stable and fairly unreactive metals :-r-rros,:nO'\ ro~-.\-,ci.QA,_ 13. Also called the 'rare earth' elements 4)1'"\mUa \O~ 14. All group members have 6 valence electrons C) t, [ w/0 8rf> · 15. Helium is a member 0 cb le.. 3

---····- - ·· For each of theJollowing,. identify the_element described. - - - ----- - ---------- - ----------- ()

16. A halogen with three occupied energy levels. C :</s'

17. A transition metal in group 9, period 5. b 18. Electron configuration 2-8-8-1.

19. A lanthanide whose symbol is two vowels. ~LA..

20. Valence shell is 6th energy level, completely full. ] n 21. Alkaline earth metal that has four levels of electrons. to....

', 22. One of two semi-metals in the carbon group, with lighter mass ___,_Q-.L....:.._ -23. Heaviest and most reactive alkali metal T "f

24. An actinide named after a planet \J. )YIA..

25. The alkali metal that only has one letter in the symbol. J\ C d 26. The transition metals whose symbols consist of two consecutive letters. 11 and --1:l ( )

27. Group 8 Period 5. _fu 28. The halogen that is often in compounds used to disinfect pools. Q, \ 29. The lightest alkaline earth metal.

30. The halogen with 6 occupied energy levels. A+-

NAME ----------- ~ijj Homework.#M

".( (1-, \ l:> 1. Most elements are classified as ~~-l __

2. There are seven semi-metals. They are: 8 1 S.' , u- t- , As , S b , T t- , A- t , ; , r i I

3. Which two elements are on the step-line but are NOT semi-metals. A I I Po 4. What does it mean ifwe say that an element is diatomic?

:f f i In ()4.-t'1IC :r n ;).. · 7 b"l~

5. What elements are diatomic? /-1,,1 NJ O~ b ~l;,i, · BrJ. :r 6. Which 11 elements are gases? H4 /Vt I N1 01 £1 {,/ 1 >40 K" {j Xe I RI\

1 /-I

7. Name three characteristics of metals. /'-1.(),. If t,,.bJ e j d Lit (I-,' / C ) 1.-, u Ht r

8. Name three characteristics of nonmetals. Br ,·++1~, N0nt-.,nJut+,r 1 99-i'l"I e

9. Explain the octet rule.

I A-tt,rn s w,'tt TO obt i,.i'n 8 VO\.lcni:,e e,

10. List the number of valence electrons andJhe typical ion formed by each group.

q:ioup? .- .: Gr. QµUJ . •;_:· ...•.. G-.-.•.. _:,_r_;·j ·'·u···::_:·~•··''.'. 1%1~~ ;1~J~f 1 fi;,ri ·.· l\t(~t;·1,:;; ' ;: .. ,,>-, ·'· .C-·,' ·' .. . - "< '::: .. ,;:::.:,.:··. : '·· .. :·-: ··'

Valence electrons j 5 G 7 R Ion formed + l t-J - 3 -, -

11. How do the transition metals form multiple ions? The j ~o..l n o ( t-o 5 c d,'f/ere11-t °'-m -' c.-tn ts Ot ete t t f .!JYI S

12. For each ion, list the noble gas with the same electron configuration.

Mg2+ N f_ Br" Kr Zn2+__ Lt H(

p3• Ar Ra2+ Bo 02• Ne r Xe_

OAt STP, which element is a good conductor of electricity?

A) chlorine B) iodine • silver D). sulfur

2. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a

• metal C) noble gas

B) metalloid D) nonmetal

3. Which element is a liquid at 305 Kand 1.0 atmosphere? .?~ f't,P, A:) magnesium B) fluorine

• gallium D) iodine 4. The element sulfur is classified as a

A) metal 0 nonmetal

B) metalloid D) noble gas

5. Which particle diagram represents the arrangement ofF2 molecules in a sample of fluorine at 95 Kand standard

pressure?

0 Key

O = atom of fluorine

A) 0 0 •

CX)

0 0 & cP

C) D)

J

6. Which element has atoms that can bond to each oilier, ..._ \ rings and networks?

A) aluminum • carbon C) hydrogen D) oxygen

7. At STP, which element is~ brittle, and a poor conductor of electricity?

A) Al B) K C) Ne • S

8. An atom in the ground state has a stable valence electron configuration. This atom could be an atom of

A) Al B) Cl C) Na • Ne

9. Which element is a noble gas?

e krypton B) chlorine C) antimony D) manganese

10. Which group in the Periodic Table contains elements that are all monatomic gases at STP?

A) 15 B) 16 C) 17 • 18 11. Which list of elements consists of metalloids, only?

A) B, Al, Ga B) C, N, P C) 0, S, Se • Si, Ge, As

12. Which element has both metallic and nonmetallic properties?

A) Rb B) Rn D Si D) Sr

13. Which pair of symbols represents a metalloid and a noble gas?

A) Si and Bi C) Ge and Te

• AsandAr D) Ne and Xe

14. Antimony is classified as a

A) metal • metalloid

B) nonmetal D) noble gas

NAME ~,

2. As you go across a period, what is true about iattractive force between the outermost electron and the nucleus? Explain. ".} l\A c re ( +) Or\ c\ ( -) tv--O.r9JA- 4--o €CA_' QJ-!l.r-

CU;,")-\-- 0-'\fU ,,,.

3. As you go down a group, what is tme about th~ractive force between the . . \ outermost electron and the nucleus? Explain.~ bl l t+ Cr.G. (-") c.~i~ ~c.v~

4. Circle the atom in each pair that you would expect to experience a stronger force of attraction between the out most electron and the nucleus: ·

Iron o

Fluorine Oxygen

C .- .(~r

esmmo.~~

d. ~M. ----..___ So mm OJ\! agne~1wn ) . ~ --..,_....

Argo~

Req er·rt-S O UJL6• --.J

~ ' The elements on the Periodic Table are arranged in order '~ ~ / of increasing

' -""" A) atomic mass ®tomic number C) molar mass D) oxidation number

2. Which list includes elements with the most similar chemical properties?

A) Br, Ga, Hg B) Cr, Pb, Xe @o, S, Se D) N, 0, F

3. The elements in Group 2 are classified as

®)netals B) metalloids C) nonmetals D) noble gases

4. Which element is malleable and can conduct electricity in the solid phase?

A) iodine B) phosphorus C) sulfur @tin

5. At STP, which element i~d not a conductor of electricity? · '\\ .

@s ' ) K C) Na _D) Ar it--.15 Which element is a noble gas? ,. ,Sy A) antimony @)ryptQn ·

· C) gold D) francium

7. The number of atoms in a molecule of~ is

@1 B) 2 C) 3 D) 4

8_ Which list of elements contains two metalloids (semimetals)?

./4)Ga,Ge,Sn @c,Si,Ge

B) Si, P, S D) B, C, N

9. Which Group 15 element exists as diatomic molecules at STP? --. '.!'\

A) phosphorus @itrogen o-C) bismuth D) arsenic

l 0. The elements in Group 2 have similar chemical properties because each atom of these elements has the same

A) atomic number B) mass number C) number of electron shells

@)umber of valence electrons

11. Which atom attains a stable valence electron configuration by bonding with another atom? ----- -------

,....A7'1ieon ~radon ~elium ~ydrogen

12. Which set of properties is most characteristic of .tcansitiOA elements?

A) _colorless ions in solution, multiple positive ---- · oxidation states B) colorless ions in solution, multiple negative

oxidation states ~colored ions in solution, multiple positive

oxidation states · D) colored ions in solution, multiple negative

oxidation states

13. Which two elements have the most similar chemical properties? .

~eandMg "::x;;fc1 and Ar

~aandBr ~aandP

Hmwk#4.5

I . Which of these elements is the best conductor of electricity? (I) S (3) Br (2) N (4) Ni

Y 2. Atoms of metallic elements tend to -- ;

(1) gain electrons and form negative ions

C\ , ::, .

8. Which element occurs as a~ at STP? -(1) bromiruv (3) mercury. (2) carbon . (4) ~trogen

r . . e is no known

(2) gain electrons and form positive ions (3) lose electrons and form negative ions (4) lose electrons and fomi positive ions

,I l.__10. ~ }:Th~cti~e-metal of those represented

~low has an electron configuration abbrevit d ;

M 2~8-2 1 ' PJ2-8-18-8-2 S,r 1 .. _ J!_ 11. Element Xis a solid that is brittle, lacks ,(212-8-_8-2 ca-,. (4) 2-8-1.~"'.18-2 ta_ luster,and has si~ v~ence electrons. In which

1

I · group on the Penodic Table would elementXbe

_l_ 4. Which element exists as a monatomic~ /1\ found? · mole~ule at STP? __ __,,- . , ,l~ -1f,! (1) 1 (3) 15

~trogeo/"' ~romµie - _ (2) 2 (4) 16 f?Aari~ ( 1) neon 1 T/ - --._ _"\_12. An atom of an element contains 20 protons,

\ 5. Which element is brittle and does not 20 neutrons, and 20 electrons. This element is in ---;onduct heat or electricity? Group r

(1) S(s) (3) Al(s) (1) 1 (3) 4 (2) Mg(s) (4) K(s) (2) 2 (4) 18

\

/ 6. Which elements are both classified as --;;etalloids?

(1) Ge and As (2) Bi and Po

(3) Band C (4) Si and P

7 Given the particle diagram: _ .,,

• At 101.3 kPa and 298 K, which element could this diagram represent? p{Rn - wg JJ,rXe i faK.r ·

_J 13. As the elements in Group 2 of the Periodic Table are considered in order from top to bottom, the number of electrons in the valence shell ( 1) decreases (3) remains the same

(2) increases

_i 14. Which sequence of atomic numbers represents elements which have similar chemical properties? -

-flrl9, 2.3, 30, 36 (3) 3, 12, 21, 40 (2) 9~ 16, 33, 50 (4) 4, 20, 38J 88

d---. 15. Which element has properties most similar to those of fluorine?

~ (l) neon ~ (2) chlorine

(3) sulfur (4) argon

I , . ,. f~ ~:-----:-------------1 • 24. Base your answer to the followi g t' h , · 1 n ques ion on t e Reference Tables for Physical Setting/Chemistry.

L -

Alomlc Element First Ionization Energy Number (kJ/mol)

2 He .:2. -:1., 1-Z 10 Ne _-i AO-I 18 Ar / ,'s_l\ 36 Kr 1 '\SI 54 Xe l lrD

Example: ~

\

" r-..... t-.....

~r-.... I'

r-.... t-.....

I'-,. r-,,..._

,-......_ ,-..._

10 20 30 40 50 Atomic Number

t · ;'ti:omplete the data table provided for the following Group 18 elements: He, Ne, Ar, Kr, Xe ~ -Using information from your data table in part a, construct a line graph on the grid provided, following ·tlie directions below . • Mark an appropriate scale on the axis labeled "First Ionization Energy (kJ/mol). " • Plot the data from your data table. Circle each point'and connect the points.

~~ed on yow: graph in part c, describe the· treµd in first ionization energy of Group 18 elements as the

. atmruc number mcreases. J:)s Qlc,.,.;,c -'I\= -1'- 1G,;., LaJ>W\ en~~

Homework~ 4 ,

1. Define ~tomic radius/--\ , cft:s,k,,, r..p · -itl--vt va C.R ti< .. t 8?~fJ. r I +o nu l

2. As you head across a period, what happens to atomic radius?

3.

I c\eU--QJ).J:::JtP

Why? Explain in terms of atomic structure. As '/0.U C\O ~d if· 0~ -P~-\-ens \r.-+N V\Ut\..R..U.)::) ~d ~ - it'" 0~ e..- \V\ ~ - \IQU.n(.t)~J'\-e.ll

....------, 1'- J + CCµ\()'Y)\o \ (. A-t\mui , As yo·u head down a group, wliat happen~ to atomic radius?

l \ne,re~

Why? Explain in terms of atomic structure. 1+-S '/WA Jo di[;;; a I q Vf2<.P 11-+an, c_ i2.a d J LA.A. !Ylcr,e~ b}(. 1F o~ ~\:.LS. 1',

4. Compare the_ radius of a metal ~tom to its ion. Which is larger? Why? -A~ \S> \~ i-hCn '+.(;\O ,~ lo IL 1..\-. \CSe~

~\Ju\lo. .e..- P-edUt;tl/\Ct ~- 0.-<' OCc..u-.P) t?(1 PfCS . 5. Compare the radius of a nonmefal ato~o its 10n. Which 1s larger? Why?

n01 IYle-lw!,;.~-· · hlw_ ~ ~··()cJ er //a_ 1¥'f1A ,-1 v· t JJ Ct ) tVJ · - ·

6. ~ 7is m~ c cnaracter. What are it e11os? I • a-mw ~a&'!:) ctn e CAni e//l ,o UA '1 -e_ -

7. Circle the atom below in each pair that would have the atomic radius.

~rBro~e

Calciumo~

(_~r Fluorin~

~ rBarium

g

8. Circle the atom below in each pair that would have the least ~etallic character.

Carbon ~

Sod_ium ~

~Selenium

Rubidium ~

9. Circle the particle below in each pair that would have the greater atomic radius.

Fluo~e atom o~

c9om or Calcium i_on

~atom or Cobalt io_n

Iom:1e atom~

10. Explain how metals obtain their full octet.1 0-f /()Sin~ -11. Draw the electrons on a sodium ato3:11 and a sodium ion.

12. Explain how nonmetals obtain their full octet.

':J:>'1 .S~t) -e -13. Draw the electrons on a phosphorus atom and a phosphorus ion.

___ _.b....O ,,...-.-0.-.,. / -----........, / "' I ~ ----- "- I ... ,~....,, "-,

I ~\ \, ' v/ /i') \ \~,~~J \~ j " ,, "' / -'-t-,~---

p p-3

0

0

- --~- ' Periodic Table

: /--' · Which ekment is malleable and ductill:'? ( I) S (3) Ge

t2) Si ~Au

__ 2. In which section of the Periodic Table are the most active metals located? (I) upper right corner (2) lower right corner

(3) upper left comer lower left comer

__ J. Atoms of metallic elements tend to (I) gain electrons and fonn negative ions (2) gain electrons and fonn positive ions

lose electrons and fonn negative ions lose electrons and fonn positive ions

4. Which is a property of most nonmetallic solids? (I) high thermal conductivity (2) high electrical conductivity ffl\ brittleness

malleability

__ 5. Which property is characteristic of nonmetals? ((i} They have a high electronegativity. {!) They lose electrons easily. (3) They have a low first ionization energy. (4) They are good conductors of electricity.

___Qvhich element is a liquid at STP and has low electrical conductivity? (I) silver (3) barium (:2) mercury (!!) bromine

7. What is a property of most metals? They tend to gain electrons easily when bonding. They tend to lose electrons easily when bonding.

( ) They are poor conductors of heat. (4) They are poor conductors of electricity.

__ S. Pure silicon is chemically classified as a metalloid because silicon (I) is malleable and ductile (~ is an excellent conductor of heat and electricity ~exhibits metallic and nonmetallic properties (4) none of the above

'). Which elements are gases at STP? --m chlorine and fluorine (3) iodine and fluorine (2) chlorine and bromine (4) iodine and bromine

I 0 . Most of the groups in the Periodic Table of the --Elements contain

( I ) no nmetals, only @ metals, only

(J) nonmetals and mt:l?. s (·~) metals and metalloi 3

__ 11 . The properties of carbon are expected to be most si milar to those of (I) boron {i) silicon (2) aluminum ( 4) phosphorus

12. Which three elements have the most similar i:hemical properties? ( 1) Ar, Kr, Br

@K,Rb,Cs (3) B, C, N (4) 0, N, Si

13. The atoms of the elements in Group 2 have the same (I) mass number (2) atomic number

number of protons number of valence electrons

14. What is the total number of valence electrons in an atom with the electron configuration 2-8-5? @5 (3) 3 (2) II (4) 15

15. Which statement describes the elements in Period J? (I) Each successive element has a greater atomic radius. (2) Each successive element has a lower electronegativity. (3) All ele·. 1ents have similar chemical properties. @All elements have valence electrons in the same

valence shell.

__ 16. Compared to the valence electrons ofa nonmetallic atom, the valence electrons of a metallic atom are generally

@fewer in number and less strongly held (2) fewer in number and more strongly held (3) · greater in number and less strongly held (4) greater in number and more strongly held

17. Atom Xhas an electron configuration of2-8-2. Which electron-dot symbol correctly§e resents this atom? (I) .. : X: (3 X:

(2) . X : (4) . X:

__ 18. Which electron-dot symbol represents an atum of chlorine in the ground state?

(I) CI: (3) •• :c I• •

(:!) •• •CI•

•

. rt<). Which physical characteristic ofa solution may · T indicate the presence ,,fa transition element?

its Jensity ·

T

0 its color (3) its effect on litmus

the effect on phenolphthalein

20. Which list of elements is arranged in order of increasing atomic radii? ( 1) Li, Be, B, C (2) Sr, Ca, Mg, Be

(3) Sc, Ti, V, Cr (!) F,Cl,Br,I

2 I. Which sequence of elements is arranged in order of ~rcasin~ atomic radii? \ll Al, S1, P (3) Cl, Br, I (2) Li, Na, K (4) N, C, B

__ 22. As the elements in Group 2 arc considered in order of increasing atomic number, the atomic radius of each successive element increases. This increase is primarily due to an increase in the number of {!) occupied electron shells (2) electrons in the outennost shell (3) neutrons in the nucleus ( 4) unpaired electrons

__ 23. Which properties are most common in nonmetals? _ (I) low ionization energy and low electroncgativity (2) low ionization energy and high electronegativity (3) high ionization energy and low electronegativity C, high ionization energy and high electronegativity

__ 24. The Group 17 element with the highest electroncgativity is (i) fluorine L\ .O (2) chlorine

(3) bromine (4) iodine

25. As the atoms of the elements from atomic number 3 to --atomic number 9 are considered in sequence from left to

right on the Periodic Table, the atomic radius of each successive·atom is (I) smaller, and the nuclear charge is less @ smaller. and the nuclear charge is ,:4reater

(3) larger. and the nuclear charge is less l 4) larger, :ind the nuclear charge is greater

~6. Which •~roup in the Periodic Table contains the most ---.ictive metals?

(@ I (3) Ii (2) 3 9

27. Atoms of which element have the weakest attraction ---for electrons?

N:i (3) Si !) p (4) S

__ 28. Which ch:ment in l'eriod J has the li:ast tcnden.:y to lose an dectron? (i) argon

)2t sodium

(J) phosphorus aluminum

__ 29. Which trends appear as the elements in Period 3 are considered from left to right?

0 (I) Metal! ic character Jecreases, and electronegati vi ty

ecreases. M tallic character decreases, and electronegativity i reases. Metal! ic character increases, and electronegativity ecreases.

Metallic character increases, and electronegativity ncreases.

__ JO. What is represented by the dots in a Lewis electron-dot diagram ofan atom ofan element in Period 2 of the Periodic Table? (I) the number of neutrons in the atom (2) the number of protons in the atom @ the number of valence electrons in the atom (4) the total number of electrons in the atom

l

\ 0

0

uuu 1

31 ~. f i\ knowledge of the ioni:acion energies o elements can be very useful in predicting the activity and type of reaction an element wi 11 :r have.

a What does the ionization energy quantitatively measure about an atom? ¼o -e r:)./;:::) y O

\-\- ·, S. tt) (e__r·,,c;J~ 0-

b w7r do ionization energies decrease from the top to the bottom ofa gr~~~~n,~i~ii;~ of elements? bl ( Cw\O«\b,l =:~ ~-\ml\;lr\-J.. 1 weu~ho\d M ViX\-et'\c..e. e.,- t'AC\'U.6 i+- eCJD·-u-- to

f\ T __ Wp_Y. do ionization energies ~crease from left to right across any pi:rio~~ U cY\ e.._ Ct,IJ.) l"'i.A ... ' ______ _ \."(),J\QNDiC Cd-\rtt L~ Cr\. 'I" 5-h,n~ h()\ct Cr\ VCl\t,tQ . · '.::::.(\.: r ..l-., 32. The table below shows the elect(onegativity ht.selected elements o_fthe Periodic Tafil e. ~\(.,e f\:) i+ '"1\C\.rd -er-- JV

u (y\~ ct.W~, /

/ b/1' I~

',,)

V V

/

Element Atomic Number Electro negativity (g/rnl)

Beryllium 4 1.6 Boron 5 2.0 Carbon 6 2.6 Fluorine 9 4.0

• Lithium 3 1.0 Oxygen I 8 3.4

0 2 4 6 8 10 Atomic Number

a On the grid set up a scale for electronegativity on the y-axis. Plot the data by drawing a best-fit I ine.

~'3 b Using the graph, predict the electronegativity of nitrogen. _____ _

c For these elements, state the trend in electronegativity in terms of atomic number. A5 Cl bi C.. ::fr 1'" ~-\cvn~et ti\l; 't

Regents Chemistry

REVIEW SHEET: Periodic Table

Elements on the periodic table are arranged in order of increasing A:\rm.l L it= "Rows" = 1)~ Cd,':, "Columns" = gr gs) lib. ff', I j U::,

Elements in the same row have the same number of ___:}:J-...!E=&t:,:; .... s ______ _

Elements in the same column have the same number of \/()\ e, h U · l -

Properties of Metals and Nonmetals

Location on table A P erties Phases On1 li le Conductivi Ionization energy & Electrone ativi Ions formed

Atomic Radius

Electronegativity

Ionization Energy

"Metallic" Character

Ionic radius VS. parent atom:

Nonmetals

Trends in the Periodic Table

Across a Period (Row) Down a Group (Column)

I\' 1' '¥

t t t

Positive ion ( Parent atom Negative ion .2_ Parent atom

*-rnt\-c,j o.1tr'<\S \o~ e- end

e-

v ong\"o..D

C\ P[L f\'\O~~ '-\-~~ \CY\~\\~

7'- t\or\M-e-\-CAJ o fi,n e -" _\ dL n 1.,.. _ r. n-l I\. \...~ t;,CI p .V-

T ' .l-=o

Regents Chemistry Name }<tj

Periodic Trends Use the periodic table and your knowledge of periodic trends to answer the following questions ...

Which atom In each pair has the larger atomic radius? ~~ice.Vt~ 1. Li or K f> r- 5. Cl or Br l

Cf)_ 2. Ca or Ni Bo-., 6. Be or Ba OinV'1l. ~J'iLu:> ('-,O- 3. Ga or B S i 7. Si ors. IV'(..n~~

C 4.0orC

Which ion in each pair has the smaller atomic radius? -\- -1'7\ 8--"') \~:::, o.rf. ,SV'<'O-\\er- f/r1 ,,-/ /

\/.... ~r K --\W 0<\2:>'"'oD I 10. Iodine io_n or\Iodine atom! C) 9. 0 2• o@, fe ,on 11l lron ioa or iron atom

oxQ.. *e.. • "t¼°"'. c...· - (\ °'"'u'-ncc..Y•

Which atom or ion in each pair has the larger ionization ener~\il

D 12. Na orO ~e... 13. Be or Ba +:. 14. ForO

15.~ or Ca 16. 1 or Cl 17. Worse

Write the charge that each of the following atoms will acquire when it has a complete set of valence -electrons.

0-1- 0 -+I

No, Na

__ , J:_F

-3 ~N

Which of the following atoms/ions in each grouping has (a) the largest radius, (b) the largest ionization

energy, and (c) the highest electronegativitl,7 -18. Chlor!J,e, seljnium, bromine

l S:-:1 1-LP '2W 19. Scandium, y num1 barium 1':l.4 (9 s t,v v53 ,"t- ':l v,'2.\•'x zu. Van11ctium~tfirom_ium, iron ,vJ. 21. Nitrogen, phosphorus, arsenic

3.0 2-~ L,~ ILIOZ. I ()IL. ~<-\'-I

7 \ 1c:f\ \ 20

(a) 5e.-(a) 60-,, (a) \J. (a) ft &

(b) CJ (b) Ac. (b) Fl (b) N

(c) C..,\ (cl Sc (c) Fe,, (cl N