Periodic&Bond SPM f4

8/17/2019 Periodic&Bond SPM f4

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CHAPTER 5:

CHEMICAL BONDSIONIC BONDS COVALENT BONDS

•Formation:

Metal atoms + non metal

atoms → ions•Involve transfer ofelectrons from metal → non-metal

•Formation:

Non-metal atoms + non-

metal atoms → ions•Involve sharing ofelectrons b/w non-metalatoms

PRODUCT:Ionic compounds

•May exist in solid at room temp

•high melting and boiling point

•Can conduct electricity

PRODUCT:covalent compounds

•May exist in solid# li$uid % gas

•&o' melting and boiling point

•Do not conduct electricity



EXP!N!"I#N

I#NI$ $#MP#%N& $#'!EN"$#MP#%N&

() Melting* oiling

,oint

•igh

•ions attracte. b strong

electrostatic forces

• amo0nt of heat -nee.e.brea1 strong ionic bon.s -hol. the ions together

•ow

•com,o0n. - hel.

together b wea1intermolec0lar forces2van .er 3aals4forces5

•6energ re70ire.-overcome the forces

8)$on.0ctingelectricit

•soli. state-9con.0ctelectric -ions in 9e.,osition + 9move freel

•a70eo0s /molten state-ions move freel - transferelectric

•$onsist of ne0tralmolec0les-cannotcon.0ct electricit in

!N; state

<) =ol0bilit •Most sol0ble in 8#

•8# molec0le attract>

•Most sol0ble in

organic solvent•



•Mg atom has proton no of ……..….•Electron arrangement Mg atom

•Mg atom has …………. !alence electron

•To ach"e!e sta#le ………..…. electron arrangement$ Mg atom releases …...e to form …..

…

•O% atom has proton no of ……..

•Electron arrangement O% atom

O% atom has …… Valence electron

•To ach"e!e sta#le ……. electron arrangement$ O% atom accepts …….e to form ……….

•The oppos"tel&charge' "ons$ Mg%( ) O% forme' are strongl& attracte' to each

MgO



EXAMPLE COVALENT COMPOUNT : FORMATIONOF H2O

•O% atom has proton no of ……..….

•Electron arrangement O% atom ……….. ) has …………. !alence electron

•O% atom nee's …... more electron to ach"e!e sta#le .….. electron arrangement

•- atom has proton no of ……..

•Electron arrangement - atom…………. ) has …… Valence electron•- atom nee's …... more electron to ach"e!e sta#le .….. electron arrangement

•……… h&'rogen atoms ,"ll com#"ne ,"th …… o+&gen atom thro*gh ……………. electron.

Each ….. -&'rogen atoms contr"#*te ………. electrons ,h"le …….. O+&gen atom

contr"#*tes ………electrons for shar"ng

•…….. O+&gen atom "s #on'e' to each …….. -&'rogen atoms #& a share' pa"r of



C!(PT)R *: P)R+OD+C T(,&)-C+).T+-T !+-TOR+C(&

(ntoine

laoiser

•/st scientist to classi0y substances including light % heat into

metal % non1metal•2ail3 4 a 0e' other compounds 'ere also considered as elements

5ohannDobereiner

•Diides element into groups o0 6 elements similar properties7Dobereiner triads8

5ohnne'lands

• (rranged 9no'n elements in order o0 increasing atomic mass•no'n as &(; o0 OCT(<)s

•2(+&31obeyed by 0irst /= elements only

&otharmeyer

•Plot graph atomic olume s atomic mass 0or all 9no'n elements

•-uccess in sho'ing the properties o0 the elements 0ormed aperiodic pattern against their atomic masses

Dimitrimendelee

• (rrange elements 7li9e .e'lands did8# group according samechemical properties % le0t gaps 0or element xdiscoered yet

!enry

mosely

•Rearranged the elements in order increasing proton no> in

periodic table



ARRANGEMENT OF AN ELEMENT INTHE PERIODIC TABLE

• Vertica c!"#$: GROUP%&GROUP%'> Each gro0, similar ,ro,erties

• H!ri(!$ta r!)*: PERIOD %& PERIOD +

• For element with ( or 8 valence electron?> Gr!", $! !- ee#e$t . /ae$ce eectr!$

• For element with < to @ valence electron?

> Gr!", $! !- ee#e$t . /ae$ce eectr!$ 0%1

• O"ter#!*t *e* are -" . gr!", %'

• N! !- *e* . ,!*iti!$ !- ,eri!3



?roup /@ 7noble gas8 1monoatomic$hanges in ,hsical

,ro,erties 6 the gro0,

e9,lanation

=mall atomicsiAe/ra.i0s

No of occ0,ie. shells increases

ow Melting * boiling

,oint

Forces attraction b/w atoms

strongerMore heat energ re70ire. toovercome the forces ofattraction

ow .ensit Increasing in atomic masses ismore com,are. to atomic ra.i0s2vol0me of atom5

•X con.0ct electricit

•3ea1 con.0ctor of heat



(ll noble gases are +.)RT 'hich

means chemically unreactie

• eli0m B 8 valence electron/.0,letelectron arrangement

• #ther gases B @ valence electron/octet electron arrangement

• "hese arrangement are ver stable

as the o0termost occ0,ie. shellsare f0ll) atoms of noble gases .o

not release? acce,t or shareelectrons among each other or with

other atoms• "hat is wh noble gases e9ist as

monoatomic 2consist ( atom5gases an. are chemicall

0nreactive 2inert5

Hei"#

He 2

Ne!$ Ne 24'

Arg!$ Ar 24'4'

r6,t!$

r 24'4%'4'

Xe$!$ Xe 24'4%'4%'4'

Ra3!$ R$24'4%'4724%

'4'



U-)- O2 ?ROUP /@ )&)M).T-

-el"*m •se to f"ll a"rsh"p ) ,eather #alloons

•se' #& '"!er ,here a m"+t*re of -e ) O% "s

*se' as an art"f"c"al atmosphere

Neon •se' "n a'!ert"s"ng l"ght #*l#s

•se' "n lan'"ng #*l# "n a"r,a&s

Argon /"ll electr"c #*l# *se' as a carr"er gas "n l"0*"'

gas chromatograph&

1r&pton se' "n lasers ) flash lamps "n photograph&

2enon se' "n electron t*#es ) stro#oscop"c lamps

3a'on se "n treatment of cancer co4 "t "s ra'"oact"!e



?ROUP /= 7!(&O?).-8

• )A+-T (- D+(TOM+C MO&)CU&) 72"#Cl"#,r "#+"8

• .on metal

2luorine 2 ">= &ight yello' ?as

Chlorine Cl ">@>= ?reenish yello' ?as

,romine ,r ">@>/@>= ,ro'n &i$uid+odine + ">@>/@>/@>= Purplish blac9 -olid



P!B-+C(& PROP)RT+)-• Cannot conduct electricity & heat in all state

• Colour become darker ;!). ?O+.? DO;. T!)?ROUP

• Atomic size ↑

no o0 shells

• Low density ↑increases in mass E increase in radius

• Low melting & boiling

molecules attracted by 'ea9 <an de ;aalsF 0orces#a little energy re$uired to oercome these 0orces

• Melting & boiling point ↑

molecular siGe # 0orce attraction become stonger#

more heat energy re$uired to oercome the 0orces



C!)M+C(& R)(CT+O. ;+T! !"O

C!&OR+.) -olution turns blue litmus paper red then 'hite

Cl" H !"O !Cl H !OCl

,ROM+.) -olution turns blue litmus paper red then 'hite

,r " H !"O !,r H !O,r

+OD+.) -olution has no e00ect on blue litmus paper

l" H !"O !l H !Ol

A" H !"O !A H !OA

!(&O?). ;(T)R (C+D- -O&UT+O.



C!)M+C(& R)(CT+O. ;+T! +RO. ;OO&

C!&OR+.) • iron 'ool burns brightly

6Cl" H "2e "2eCl6

,ROM+.) • iron 'ool glo's brightly

6,r " H "2e "2e,r 6

+OD+.) • iron 'ool burns slo'ly

6l" H "2e "2e+6

A" H "2e "2eA6

!(&O?). +RO. +RO. 7+++8 !(&&+D)

7,RO;. -O&+D 2ORM)D8



C!)M+C(& R)(CT+O. ;+T! .aO!

C!&OR+.) • dissole $uic9ly in al9ali

Cl" H ".aO! ".aCl H .aOCl H !"O

Colourless solution 0ormed

,ROM+.) • dissole in al9ali in slo'er rate than al9ali

,r " H ".aO! ".a,r H .aO,r H !"OColourless solution 0ormed

+OD+.) • dissole slo'ly in al9ali

l" H ".aO! ".al H .aOl H !"O

Colourless solution 0ormed

A" H ".aO! ".aA H .aOA H !2O

!(&O?). -OD+UM -OD+UM -OD+UM ;(T)R

!BDROA+D) !(&&+D) !(&(T)7+8



• Chem"cal propert"es of all elements "s s"m"lar #co4 no of!alence electron same ) ach"e!e the sta#le octet electronarrangement.

• All atoms "n halogens ha!e 5 !alence electron ) atta"n anoctet electron arrangement #& rece"!"ng 6 electron to form charge' "on

• The react"!"t& of the halogens 'epen' on the ease of theatom to ga"n electron7 8hen go"ng 'o,n the gro*p$ the no of shells "ncreases$

the atom"c s"4e also "ncrease

7 The o*ter shells #ecomes f*rther from the n*cle*s

7 The forces attract"on #9, n*cle*s #ecomes ,ea:er

7 The trenght of the n*cle*s of halogens atom to attractan electron "nto o*ter shells 'ecrease

7 The react"!"t& of the halogen 'ecreas"ng



!"#$ % LM'() *AL+ALI

M(AL),

• <ery reactie

• -o0t metals 'ith lo' density

•?ood conductor o0 heat % electricity

&+T!+UM &i ">/

-OD+UM .a ">@>/

POT(--+UM ">@>@>/

RU,UD+UM Rb ">@>/@>@>/

C()-+UM Cs ">@>/@>/@>@>/

2R(.C+UM 2r ">@>/@>6">/@>@>/



$hange in ,hsical ,ro,erties.own the gro0,

DENSIT8 •ow b0t increasing

•C in atomic mass #!recom,are. to C in atomicra.i0s

ATOMIC RADIUS•Increasing

•No of shells increase

•&istance b/w valenceelectron * n0cle0s alsoC

MELTING 9 BOILING

POINT•&ecreases

•C of atomic ra.i0s ca0singthe metallic bon. b/w

atoms b4come wea1er

ELECTROPOSITIVIT8

•Increases•!s atomic ra.i0sb4come longer? the forceattraction b/w n0cle0s *

single valence electron4



Ce#ica ,r!,ertie* !-aai #eta*

All alkali metals have similar chemical properties coz:-•All atoms "n al:al" metals ha!e !alence electron ) atta"n anoctet or '*plet electron arrangement #& releas"ng 6 electronto form ( charge' "on

The reactivity of alkali metals increases when down thegroup:-

• atom"c s"4e from l"th"*m to franc"*mC

•The s"ngle !alence electron "n the o*termost shells #ecomef*rther from the n*cle*s•/orce attract"on #9, n*cle*s ) !alence electron ; ,ea:er•-ence$ "t "s eas"er to release the s"ngle !alence electron to

ach"e!e sta#le electron arrangement gro*p 6 elements



Reaction al9ali metals 'ith O"

• "he white soli. .issolve in 8# to ,ro.0ce colo0rless

sol0tion• "0rn re. litm0s ,a,er to bl0e

&+T!+UM •,urns 'ith a red 0lame in O" to 0orm'hite lithium oxide

*&i H O" → "&i"O

-OD+UM •,urns 'ith a yello' 0lame in O" to 0orm'hite sodium oxide

*.a H O" → ".a"O

POT(--+UM •,urns 'ith a lilac 0lame in O" to 0orm'hite potassium oxide

* H O" → ""O



Reaction al9ali metals 'ith !"O

• Pro.0ce colo0rless sol0tion• "0rn re. litm0s ,a,er to bl0e

&+T!+UM •Moe slo'ly on the !"O sur0ace 'ith

so0t hiss sound-OD+UM •Melt to become a small sphere

•Moe rapidly % randomly on the !"Osur0ace 'ith hiss sound

POT(--+UM •Melt to become a small sphere

•,urns 'ith a lilac 0lame

•Moe rapidly % randomly on the !"O

sur0ace 'ith hiss % pop sound



Reaction al9ali metals 'ith Chlorine

• iberates white f0mes which become a whitesoli. at the en. of the reaction

&+T!+UM •,urns slo'ly 'ith a red 0lame in Cl" to0orm 'hite lithium chloride

"&i H Cl" → &iCl

-OD+UM •,urns rapidly % brightly 'ith a yello'0lame in Cl" to 0orm 'hite sodium chloride

".a H Cl" → .aCl

POT(--+UM •,urns rapidly % brightly 'ith a lilac 0lamein Cl" to 0orm 'hite potassium chloride

" H Cl" → Cl



$!I"- ..a Mg (l -i P - Cl (r

Proton no // /" /6 /* /J /K /= /@e> arrangmnt ">@>/ ">@>" ">@>6 ">@>* ">@>J ">@>K ">@>= ">@>@

(tomic radius → D)CR)(-+.? →

Physical state

(t room temp>

-O&+D ?(-

)lectronegati1ity

→ +.CR)(-+.? →

Metallic

properties

M)T(&-)M+

1M)T(&

.O.1M)T(&

)lectricalconductiity

?OOD CO.DUCTOR ;)( C(..OT CO.DUCT

Chem> Prop>,(-+C

OA+D)

(MP!OT)R+C

OA+D) (C+D+C OA+D)



• BASIC OXIDE: metal oxide dat can react with acid to form salt and water

• ACIDIC OXIDE: non-metal oxide dat can react with alkali to form salt & water

• A!"O#E$IC OXIDE: oxides dat can react %oth alkali & acid to form salt &

water

A#OIC $ADIS DEC$EASESBCO':

•All the atoms of the element ha(e) shells occ*+ied with electrons

•Increasin, in +roton no ca*sesthe no of +ositi(e char,e in the

n*cle*s •.*cle*s attraction on the (alenceelectrons

•#he atomic radi*s of elements /

E0EC#$O.E1A#I2I#3I.C$EASES BCO':

•Electrone,ati(it4: the stren,th ofan atom in an molec*le to attractelectrons towards its n*cle*s

•Atomic radi*s decreases d*e to

the increasin, n*cle*s attractionon the (alence electrons

•#he stren,th of n*cle*s toattract electrons also stron,er



TR(.-+T+O. )&)M).T-

! "D!N=I"I#N !DE• &0ctile + malleable

• igh tensile strength

• igh melting * boiling ,oint

• igh .ensit• oo. con.0ctors of heat *

electricit

=PE$I! $!D!$"EDI="I$• =how o9i.ation no in

their com,0n.

• Form colo0re.

ions/com,o0n.• %sef0l catalst

U*e* i$ I$3"*trie*cata6*t Pr!ce** Ma$"-act"ri

$g

Ir!$ Ha;er a##!$ia

Pati$"# O*t)a3 $itric aci3

Periodic&Bond SPM f4

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