I like manga

1. 1
Feri.,_,d;:-
prJpeTTi,,
i;;;d
,,:i;-fo:ion<
of
prl1p,m·,-
,
-
Piiy,i~cl
end
CJumu-cl
"""'-'
.....
'
,
p,
.
.,__''
1
i...1fQCr
(t.)
>!Lu.>
;!:
c~:::~:::s
,·a
Oil
,
'
-
""'
:
·
t~i
i.
~=:
~li':
,
..
:Ji.::'C
..
·
..
~,
,
~'
tli.:'
-.
'
Ol:1!:ib
:.!~);1:_;
:
..
>~
i
.:::.::~
..
::~
:,(';;'tid;:>!;:';;'
[O
[!,;;'
...
...._
.)!'
~!~I:!~:::~
~!:~
::1;tI':i~::::--
!t:rcc
__
~rnu!
.1.i"
~
;,l
1
i-1~:-::c,
:--~.'
"
...
~
·::::_:
~~~~::..__:'
-
~
~1ac~:~
,
c~c
....
:~~
.!~
~~~
::.r::.!:r11ctic
r
.,
"'
,:-
.
.
..
;
'
-
l~'
,~.;::
137B
-
--·-
---
··-.
I..,
l
,_Jan,f
..
t
.
20
....
~sJr.
56
a
:1endeleeY
element~
.:""
whai
elements
are
(irc:e
f
Df
their
alOmic
ID8SS.
:.t:
;
eri.i~::!.!
~
:
oh.!=:-tifi5
gr----ups
.
.
.
pai,1ds
:-ic
::-.::=.:
..
.:~~-
::.~"'
1
.=
~·.!i~=r
.
.
.:=
~.
i
~~:~:,
.::-l1.!-
~
!1
"'
;
.
~::~
~:
:
.
.
.
.
1
t~
•
.i~·
i
.:.
Tl,;;>3;;>
d;;>t.;;>:
>-
;;-::;;>
,;;-,,,-.,
;;>j
"t;;>r-,
Henry
)
fos~le~
:-:.::
:·1..~rna::-i
:..-:;;>
modem
pt>riodic
t.able.
,::_~-
,.
,,
:-.::::-.:--c,
0::
;;-k
.::=::-
.
:s::s
ii:
tl:~
,
~
~c:f:
~~<:-~
J~
t."'
f
.
..!f.i
2:L1:i1
..
P:--..
,
.:~
~!.'
i
1
~Gcrr~~~
pn..'l)eitie.s
(1f
,
J
.n
elemem
d;:-pc
r
.
.:.
0~.
:...~
nu::.{~;
oi
l
~oos
and
their
anaogemem.
Hem:
a.Ilic
__.rm
~~
jlmdammaJ
popaty
of
an
ekma
Moseley
stated
that
-ille
p
cbemic:al
properties
of
elements
are
functiom
ol
dldr'
aloeic
ts-

2. Bl I I.I
R~ • · .,~,ilain c Elements
1 • block
r-,
r:·- · 1 l 2
P- 0,b,
~----_j I
3 4
I III 1.01( I OR'1 ,u m u n
5
GROUPS
Transition ilfctals
d · block
6 7 8 9 10
)I( 'lBI IOI I.I I ,11,1-.,
I
11 12 13
Repn•~cnta tic Elemcnh
p - block
14 15
Active mctalc,
16
:ohlc ga~c~
p-blod,
r-i
17 18
,__,
' ' i-! Q Ato1rnc nurnber ~ C State
Symbol
Carbon
D Solid
(A lkali metals & Alkaline eanh metals)
Heavy metals
Mctallo,d,
If I
HeQ
I I 11
Hd1um
C
0
Liquid
Gas
VB
Name
"18 VIIB
250
Mn
Non-metal',
Non-metal, (Halogen;)
Non-metals (lnen gas)
.----- VIII m
260 270 230 290
Fe Co Ni Cu
IIB
300
Zn
5,0 6 0
i3 C
8(•nm Carbon
13 D 14 D
Al . Si
Alumiruum S1hwn
31 0 3:! D
Ga Ge
7 8 9 10
N Q oQ FQ Ne Q
'uroren 0,H;1..-n fluonn< '.C'011
15 D 16 0 17 111
p s Cl Q Ar Q
Pho,phoru, Sulphur Chlonnc .r)'.•n
33 D 34 D 35 36
A, Se Br 0 Kr Q
Manganese Iron Cobalt Nickel Copper Zinc Gallium G~1um A.r~mc Sdcmum BnlfTIH'lc: M)ri.~n
42 0 43 0 44 □ 45 □ 46 0 47 0 48 □ 49 □ 50 D 51 D s:! D 53 D 54
Tc Ru Rh Pd Ag Cd In Sn
echoctium Rulhcnium Rhodium Palladium Sih,cr Cadnllum lNhwn Tin
Sb Te Xe Q
onmoo~ Tellunurn fo,d1n,.• ,.:111,n
75 0 760 n □ 780 790 80 0 81 D 8:! D 83 D s4 D 85 D ~6
Re Os Ir Pt Au Hg 11 Pb Bi Po At Rn Q
Tanpw, Rheoiwn Osmium Indium Platinum Gold M<muy 1ball1um Le.Hi 81<.muth ro,.....,mum .,t.,un~ R,.,J.,n
106 107 108 109 110 Ill 112 113 114 115 11 6 117
Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv T,
llohrium Has."ium Mritrcnum D~ud- ROCIII• q,p:c- Nihomum Fkro,,um ;.,o,.._"'"ium
~1;'.
- NC>um
/-block
61 D 62 0 63 0 64 D 65 D 660 67 D 68 0 09 D 70 0
Pm Sm Eu Gd 1b Dy Ho Er Tm Yb
- Sarunum Emcpwn Gadoltntum Terbium D)'l"""Uffl H...,.um Erbium Thuhum lklindll luldhtlll
93 94 95 96 97 98 99 100 IOI 102 103
Np Pu Am Cm Bk Cf Es Fm Mtl No Lr
- Omum Bak.chum Cabfomuam em.u;n,um tcmuum M.:.nJdn11111 ?-.,~l"th·,1m la.,.11:"n..11Jm
Nlpo.-
-

3. 1,2
SALIENT
FEATURES
OF
THE
MODERN
PERIODIC
TABLE
(SEE
PAGE
2)
Elements
or
thi
s
group
arc
ca
ll
ed
noble
gases
or
inert
gases.
The
modem
periodic
table
has
eighteen
vertical
('olumns.
Each
vert
ical
co
lumn
accommodates
ekments
with
the
same
nu111hcr
of
cll'c
tron
s
in
the
outermost
she
ll.
These
verti
cal
co
lumns
,1
1
-c
k.nm,
n
as
groups.
arranged
from
ldt
lo
right
in
the
order
of
increasing
atomic
number.
These
c
leme
nt
s
have
th
e
ir
outermost
o
rbit
com
pl
ete.
Due
to
stab
le
e
lectroni
c
configuration,
/
(
th
ey
hardly
react
with
other
e
lements.
'
}
7
The
e
lemen
ts
or
grou
ps
I
,
2,
13,
14,
15.
16
and
17
have
I
,
2,
3,
4,_5_6
and
7
eleclrolliLl!L.
their
outcrnH)St
shells
rcsp<.;ctivcly.
They
are
known
These
C'lemcnls
arc
1-.nown
as
Alkali
metals
(c,ecpt
hydrogen)
as
thq
form
strong
alkalis
'ith
atcr.
Alkaline
carlh
metals
-
They
form
weaker
alkalis
as
compared
lo
group
I
clements.
are
as
Inc
-
.
-
or
o(
.......
I
,.,,-~~--.-•·
.
~
The
outermost
shell
of
a?i'
the
clements
of
these
~~p~
:t
r
:
incomplete.
~
known
as
the
transition
c
lements.
A
ll
the
There
are
seven
horizontal
rows
in
the
modem
e
lements
or
these
groups
arc
metals.
They
have
pciiodic
table.
They
are
known
as
periods
(see
table
their
two
011ten11ost
shells
incomplete.
given
below).
Boron
family
-
Boron
is
the
first
Each
period
begins
with
an
element
having
one
member
of
the
group.
electron
in
its
valence
shell
and
ends
with
Carbon
family.
coml?Jetely
filled
outermost
orbit
(valence
shell).
Group
I~
Nitrogen
family.
(
,
....
,
.,
...
...
.
1
1
1.
,
.
,
"
Oxygen
family.
also
kno
wn
as
,;..,,..
'
..
,,
,
·•
·
.,,
..
··I}!
''
"
......
,
.
.,,
chalcogens.
meaning
ore
forming.
Elements
of
period
one
have
one
shell,
These
elements
fo1111
sails
and
so
are
elements
of
period
two
have
two
shells,
and
that
of
known
as
HaJogens
(meaning_
salt
formers),
.
,..,.
period
three
have
three
shells
and
so
on.
7,,.,'y
~
O'
Period
T)pe
of
Number
of
;
Atomic
no.
of
:
No.
of
·
Elements
in
Group
2
-
~
-
-
r
-
-
-
-
-
-
-
-
~
-
-
-
-
--~
period
elements
elements
s
hell
(s)
1
1
2
3
•
12
13
14
~-'·
-
-~
~"
1
••
·--4-
··~·
--
-----
-
-
'
-
-
-
·
-
~---
Shortest
2
1-2
I
I
H
Re
period
I
2
~
--.--
Short
8
3-10
2
Li
Be
B
C
N
0
(i'
period
3
4
5
6
7
8
9
3
Short
,
.
~
.
·
,
,
8
U-18
3
Na
Mg
1.1
Al
SI
p
s
Cl
11
12
13
14
IS
16
oenoa
Im
.
i
4
ong
K
Ca
19
20
5
(,

4. (ht-
'1X'
I.
Similarly.
coaligurllioa
l
gn,up
2.
qDialerv&ls_
"vlriadoa(ie,
·ia:iibY.alc
lie
•
h
L
'
1
'
'
0
P
Pm:-id
to
•1-ti
the
drmiral
~
On
mo·ing
from
left
IO
right
ill
a
pa
Pf.1W.
the
number
of
shells
remains
the
same.
,◄
example.
in
lhc
2nd
period.
the
number
of
remains
two.
i.e
.•
equal
to
dJe
number
of
Ille
Similarly
in
lbc
third
period
the
IIUlllber
of
remams
.
three
and
SO
OIL
.
..,
;
}
V
Yalcacy
dmoles
the
eumhi•M&
r.ar,
-
~
i
.
_
of
a,a
elanrflt
II
is
.
.
.
.
.
.
.
.
.
.
.
.
.
QIII

5. Groups➔
IA
ll-
IIL
I
IV,
I
II
l.,
.
.
:n,
2
11
1-l
I
'
lh
17
IX
'-T
,
~
L
Elements
of
the
2nd
period
~
~
f---
B
_
C
'
"i·
r
1
,tomk
:o.
:I
-1
.5
c,
7
I
~N
.
l)
Ill
Electronic
KL
KL
K
L
1.1
K
I
1'.
I
Kl
1'.
I
configuration
2.
I
1.
~
2
.
.l
2.
-I
2.'
2,
(,
~-
7
:-t.
X
-T
'<o.
of
shells
2
I
'
'
~
-
t
--
'alenc)
I
2
.1
-I
2
I
I
I)
p
,
-
-
s
,1,
tc-11
,11
,
~
11
,()
111
Formula
of
BeH~
HJdride
In
the
period
ic
table
•
ele
m~nts
arc
arranged
in
order
or
increasing
atomic
number
(proton
numbe
r).
•
the
'ertical
columns
of
clements
wi
th
similar
properties
are
called
groups.
•
the
horizontal
ro,,
s
are
ca
ll
ed
periods.
Recurrence
in
properties
due
to
same
number
of
electrons
are
seen
after
a
di
fference
of
2.
8.
8.
18.
18
and
32
in
atomic
numbers.
•
Prope1ties
of
elements
depends
upon
electrons
in
the
'alence
shell
(outerrno<;t
orbit)
so
gradual
change
in
properties
is
seen
with
increase
in
atomic
nu
mber.
•
Reactive
meta
ls
a
re
in
gro
up
l
and
2.
Tran~ition
elements
(metals)
are
in
middle
and
non-metals
in
the
upper
right
comer
of
the
periodic
table.
.
•
Transitio
n
from
metallic
to
non-metallic
character
is
seen
across
a
period.
I
s.
I
6
I
7.
Name
two
elements
,n
11ach
r.ase
·
(1
)
Alkali
metals
lnj
Alkahne
earth
mrrtal'..
(111)
Halogens
(av)
Inert
gas
Elements
of
group
1
and
element5
0f
group
1
7
1;,,u-.
have
va
lency
1
Explain
Correct
the
statements.
(1
)
Elements
in
the
same
period
ha•,e
the
.sam,,
valency
(11)
Valency
depends
upon
the
number
of
shells
in
an
atom
(111)
Copper
and
11nc
are
representative
element5
(1v)
Transition
11lements
are
placed
at
extreme
nght
of
the
periodic
table
.
8
.
What
do
you
understanrJ
by
?
(i)
Penod1c1ty
(11i
T·
;
p1cal
elements
(1i1)
Orbits
9.
Name
two
elements
that
you
would
expect
to
show
1
chemical
reactions
similar
to
calcium.
What
1s
the
basis
of
your
choice
?
10
Name
the
(i)
metals
(1i)
metalloids
and
(iii)
non-metals
in
the
first
twenty
elements.
11
.
Fluorine.
chlorine
and
Bromine
are
put
,n
one
group
on
the
basis
of
their
similar
properties
.
(1)
What
are
those
similar
properties
?
(ii)
What
is
the
common
name
of
this
group
Of
famdy
?
12.
What
is
the
main
characteristic
of
the
last
element
in
each
period
of
the
Periodic
Table
?
What
is
the
general
name
of
such
elements
?
13.
According
to
atomic
structure
,
what
determines
which
element
will
be
the
first
and
which
will
be
the
last
in
a
period?
11~
How
does
the
number
of
:
(i)
valence
electrons
and
(ii)
valency
vary
on
moving
from
left
to
right
in
the
third
period
of
the
periodic
table
?
15.
Name
the
type
of
elements,
which
have
their
(i)
outermost
shell
complete
(ii)
outermost
shell
incomplete
(iii)
two
outennost
shell
mcomplete
(iv)
one
electron
short
of
octet
(v)
two
electrons
In
the
outennO&t
orbil
16.
An
etement
hlS
2
elecb'OflS
In
1B
N
shll.
0)
What
II
Ill
atomlD
number
T
-
.
.
.
~
.
-
.
.
.....
~
"
'
,•J~
~
-

7. (
,.,,
II u um Br:r:lhum
Na. 1 4
.... t<.! pm u.=. pm
KL ~l
2 I .!. 2
~ @
.
•
ln th...· lh1rd pe n li..i. ~xlmm ..
,u~ .mu ..:-hlonn... ..h m 1, th, ,
'otr th r •"-- or
, .in c,..·.:pthm. c- ,11:~ o uc
men g. ,.:, .1 ~ b1~_;.~r th.m h~11'.)f.1..•th ,f the ~
pc_nod nu, ,, tx,-.ill-...' the out.:-r lnl.''l ,hell of men
g.L~, 1
, compktr Ill{·~ ha,.:~ nw.umwn number
of ek..,·tron, m th...··- olll1..'mh),t 1.lrbit tbu, the
d~.:lmm..• rept.ll,10 1, -~ mi,umun The effe"., of
nuc-kar pllll P l?r th.: , ~kn.:-.;' ~k.'.tn.'n, i, not
,1..,·n. Hcn..·1..•. lh.: , ii~ 0f the at,m 1..'f .m men ga., '"
bil!.~er. ~ut lh.
'l t-1i::~t>r than the .1U...tl1 metal of
~..., -"'
th1..' ,.un.: ~riod
Tn.•nd, in utomk ).Jll' :1t·ross a J>('riod.
ll..-woo l '..im..ut ' ..i,,a:-.:n (h,;.,
:- t,
'
' ' lffi r..n1 ~o r-m oopm t,-.:pm u:
Kl kl
" 1'.l
• 1 ·. -l . " :. (
Kl "l
(®) @ @ @)
tt : I. CatltNa Is always smaller than the parTnt aatom. fmm "hkh it i" fornle"d.
.. .... afeleclron(s). bcncc proton(s) arc more than ekctmn(sl ma catum So el«1rtllb ~
•••rs ad 1ft: pulled mward. Hence the Slll dccrca.c;cs.

8. l
r
, _+ 1'I, ..
10 I
"' J2 I
a C
F 0-:
9
-26 42
(,r
decreases
Down a group
On mo mg down a po-,,
1ze nrri-"-'..C and the cblll'&C
mcreases 1be
ze
nuclear c
electron me--

9. Across o pertod
On m mg acrou a period. nuclear pull
due LO the mc..rease m atonuc number. and
t<,mtc.. u.e decrea'>t:'>. Hence, <:lemc:nts
l r n t I , elcc.trons eatly.
Therefort: ti m tall, lur, durca e curo
n 11 from left t ngl t
I amp/ . In the 2nd period. lithium is the
mo l met,tlhc
C 8
I 0 F
1
R
Metalload Non-metah
Met.aJrc. c.haracter decreases or
-m •allic character increases
Jn the 3rd period, sodium is the most metallic
,•leme111
.
~ Non-metallic character
77wse elements which have a tenden9 to gain
t!u trans, in order to attain octet m their owemwst
orhl/ are conridered as non-metals.
Non-metals usually have 5, 6 or 7 electrons in
their outermost orbits. They can gain 3, 2 or 1 electron
respectively, in order to attain octet or to complete their
valence shells (outermost orbits) and form an anion.
For example, chlorine (Cl) and oxygen (0) gain
I and 2 electron(s) respectively to form anions.
Cl + e- ➔ c1-
(2, o,7) (2, 8, 8)
0 + 2e- ➔ 0 2-
(2, 6) (2, 8)
Non-metallic character also depends on :
#J . .aiz.e and (ii) nuclear charge.
,lu : Smaller the atomic size, greater
~ pull and the tendency to gain
- .........efore, the element is more
nds ir n,u~-
own a group
The atomic s
of new .hell ov
nuclear charge i
atomic.: number,
size is greater.
decreasef down
•
nuclear charge,
lr p Group t.i
C ;-.;on-metal
S, ~letalloid
Ge .Metalloid
Sn ~ktal
Pb ~letal
A,..r,.,.,.,. the period Cleft to nght)
On mo ing acro~s a penod. the tenuenc~ to
gain electron(s) inc.rea,e, due to an incre..iM! in
nuclear pull and a decrea~e in the .1tom1c -.1ze.
T herefore. o t c c ,
a pen .. from left to nghr.
For example, in the 3rd period.
Na < Mg < Al < Si < P < S < Cl
~1etab Metalloid ~ on-metab
Non-metallic character increases
Note : Non-metals are oxidising agents.
The nature of oxides also show periodicity.
Across a period : The oxides of elements in a
panil:ul.lr pcnod ho,r Jt"Cr1 •1 ,,,,~ bnHc riat11re nd
finally become aciJ1c. For example. the oxides of
elements of the third period.
Na20 MgO A120 3 Si02 P205 S03 Cl20 7
Strongly Basic Amphotcric Fcebl) Acidic More Most
basic acidic acidic acidic
Down a group : The ba'iic natu,e ofcuidel ofmei
uscreases.
The reactivity of elements depends upon their
tendency to lose or gain electrons to complete their
outermost orbit. Greater the tendency to lose
electron(s), greater is the reactivity in the case ?f
aetals. Similarly greater the tendency to gain
~ gr.eater is tbe reactivity of non-metals.
ffllGCNV

10. 1 5 4 10
n1sat1on pot nt101 or Ion, otion
energy (I E) or on sot on nthatpy
l' kno 1h.11 I hl' eIce Ifflll', 111 "11 "'', n, .11 l '
<lll.JJUcd b) lhe po,111vd) ch,11g1•d 1111L' ll' ll' Sn, ii l'
V..tnt to remove au ck-c1 1nn f,0111 :u1 .1 !<>111 , ~0111l' t' 11,·11'
ha., tu he '>trpplicd to O't'lt:<nnL' lliL· ..,li<>ll" :111111< 11011
01
Ifie 11uck·11-.. J11d :tl1t·1 lht• L'kc1ron !'t';-., 1t·111u,l·tl
frou1 Ilic atc1111, lhl' .tlum 1hl'll :icqt1ir,,.., rn1~· u11i1 pmi1ivv
cli.ugc ·•11·' I) 'l'< 11 • • • • ·
u U L > It <l [)0ill! lllll (OI l'.111011)
1
l,i· t'lll'i I,' IC'tJllin·cl t o l't'11w1 ·<• 1111 f'/1•c' f11111 /10111 11
ticutral i10/11t,•tl }:a .,,•011.,· IIUJ/11 anti c·11111 ·1·rt it i11to ti
/
1
<
111
1
11
•"/. char~ed ga.1·t•o11.1 ion i.1 nlll,·d io11i.111ti1111
f'ote111iu/ (J.P.) or ionisation ener,:y (I.E.) 01 first
ionisation energy (IE
I
J.
M (g) + I.E. -) M+(g) + c-
M can be any clement.
Unit : I.E. H "" awred in elC'cIron I oft ,· per alnm
(eV/a/0111) {UU} Wi SJ unit ir kiloj,111/, !/{, 1110/c (/..J mo/ I).
Ionisation energy depends on :
(i) atomic size (ii) nuclear charge
(i) Atomic size : The greater the atomic size, the
lesser the force ofattraction. Since the electrons
ofthe outennost shell lie further away from the
nucleus. thus make their removal easier, i.e.,
the ionisation energy required is less.
(ii) Nuclear charge : The greater the nuclear
C~e, greateris the attraction for the electrons
efthe outermost shell. Therefore, the electrons
ost shell are more finnly held
whicpgi;cater energy is required to
~
I h,· 1·11111n 1l'I
~, M
oftl11 , cl
p,•1lml
"' I'
I.I .
I'll) , ., 1 lt'h 11,1 I 11'1'/ t ,
Ill kl 111ol I
Down a group
• 1 1, ,,.,1• 111 i111111J1L 111J111hu in,,,
j Ji1 ' JL
' I ' ,(II II l
J I H i-, 11, d, ,w11 11,, t 1•,11p cl,, II 0
rli;ll)'l") ;111( .I 11111 I
J I •1 , lwll.., J111 1; 11J1 ft.t 1: 111 1l1 ,
11
,
:1dd1l1<JJI () l 1' ,,,
IIH
..: i·JI,·, I ,,f ,111 i11 1. 1r, , •• i1
1 II
l/l' O Vl" I l ()JIil '>
JI ii( k:11' t;l 1;111•t .
1 h r for lll/11 " 111111 "' 1 I , a
II
I I I It tltf I I
/lie ! 1 a I Ill f I tl(Ofl /t 11 I,
1//(11 l 1/ull /I ti J.;fllllfl
( El1•11u·nt r/j T N;,
~K (KJ mol 1
J I mi j '1%
r_-~ <
1
~7
;~~J
:l~
INote : • I lcliu111 will have the _highcsl !<mi11atJon
1 cncr~y 2'n2•0 kJ mol I whtlc caesium (Ca)
Iwill have the lowest ionisation energy of
375-0 kJ mol 1
(I.E. of Fr is not determined
correctly as ii is radioactive).
• Metals usually have low I.E. whereas
non-metals have high LE.
1.5.5 Electron Affinity CE.A.) or Electron
Gain Enthalpy
We have just studied that to remove an electron
from an atom. energy is required. Similarly, when
an extra electron is added to an atom. energy ii
released.

11. atter
li)e
azomu
~i:;:e
Iron
a(fm11
,
becJu<i
e
1,e
for
...
e
be1v..ee
n
th~
ce
electron
s
1.:i
greater
m
electron:
.;
arc
held
firmly.
(ii}
,
'
'uclea
r
charge
:
f/ie
veater
1/,e
11L1deo
r
har~e.
1:reater
is
the
eleczron
affinit);
because
mer
ease
m
nuclear
charge
incrca
se;;
the
eff
ecti
·e
anran1v
e
force
on
the
valence
electron
s.
Varjafi
on
(Trend
s)
in
electro
n
affinity
r111r1,
r
,.,,,tt
the
atomic
'
-
>ize
decreas
es
and
the
nuclear
charge
increase
c;.
so
the
electron
affinity
increase
s.
Thus
electron
affinity
(E.A.)
is
the
highes
t
fo
r
group
17
elemen
ts
(haloge
nr:;)
and
the
least
for
group
I
(alkali
metals).
Ell-ctron
ffinit)
alul".
in
'KJ
mo1
1
IA
11A
IllA
IVA
VA
I
VIA
Vl
lA
'Zero
(I)
(2)
113)
0
4>
os,
I
<1
6>
(17)
(18)
H
I,
I
He
-
73
+48
La
ec·
B
C
N•
0
F
Ne
-60
-88
-1
22
-141
-328
Na
Mg"
Al
Si
p
·
,
s
0
Ar
-
53
-
50
-11
9
-
74
'
.
-
200
I
-349
Down
a
group
!
frnm
rhR
top
to
the
ballom
ro.·-
the
atomic
size
increase
s
morl!
than
the
nuclear
charge,
thereby
cau-;ing
a
net
decreas
e
in
E.A.
Group
I
~
H
-73
Li
-60
Na
-53
K
-48
Rb
-47
iD
group
17,
fluorine
bas
at
iB
poup
16
oxygen
bas
-~
~-
-"
ne
group
a
right
m
a
peno<l
ty
(E.N.)
The
tendenc
y
of
an
atom
in
a
molecul
e
to
attract
the
<iharcd
p~1ir
oi
~lectron
s
toY..ird..
,
ibclt
i,
called
it-;
electron
egativit
y.
-
l
since
it
is
only
a
tendenc
y
lt
only
indicate
~
the
net
rc<,ul
t
or
the
tendenc
ie:i
of
differen
t
elemen
ts
to
attract
the
bond-fo
rming
electron
pair.
Electron
cgativity
i~
measure
d
on
several
scales.
The
most
widely
u<,ed
scale
of
electron
egativit
y
was
devi<,ed
by
Linus
Pauling
(
1932)
in
which
the
highest
value
of
electron
egati.it
y
[for
fluorine
]
is
taken
as
4-0
and
the
lowest
one
[for
caesium
]
as
0-7.
1
ELECT
RONEG
ATIVIT
Y
VALUE
S
I
2
13
14
15
16
17
~
-
-
D
,
H
E
j
2-1
C
Li
Be
B
C
N
0
F
l
1.0
1-S
2-0
~-S
JO
3.5
4
R
1.
Na
Mg
Al
Si
p
s
Cl
E
0-9
1-2
1-5
1-8
2-1
:!-5
3-0
A
K
Ca
Ga
Ge
As
Se
Br
s
0-8
I
0
1-6
1-8
:!-0
2-4
2-8
I
Rb
Sr
In
Sn
Sb
Te
I
0-8
1,0
1-7
1-8
1-9
2-1
2-5
N
Cs
Ba
11
Pb
Bi
Po
Al
0
0-7
0-9
1-8
1-9
1-9
2-0
2-2
,I.
I
N
C
ll
B
A
s
I
N
G
➔
Electro
negati
vity
values
too
depen
d
on
:
(i)
size
of
atom
and
(ii)
nuclear
charge.
(i)
Atomic
size
:
The
greater
the
si:e
of
the
atom.
the
lesser
the
electro
negativ
ity.
since
the
electron
s
being
farther
away
from
the
nucleus
,
experien
ce
a
lesser
force
of
attractio
n.
,a__.
,
charge
:
The
greater
the
nuclear
grtater
th~
electro
negativ
ity.
la
nuclear
charae
causes
.
.
.
.
.
.
,
.
.
.
rtxce.

12. ~(
I
I
'I
n l ~•I
I 1!
'11 1l1
,,
lJ ~
Ii
l
,,
.
••I
,,,
.,, '"
•t1 11,
..
I
:.I
'"
)'
•I•
II
'I•
ll
...
"'I I
I
•I• '
1 1 ll
I I ,
I
{:J
,,
I •(1
'"
I
.,,
,,,
'I
I ,,
•11 1 1
l
,, ,,
"'
'"
,,,
t '•i. ·.:
•11 ~/, .,,
, ·,;1,
:'}, •,1,
1 1 II
,,, 11 ~ I I I
'I ")
, .
I
•I •
,,
I'
4:J·
'J '
,}1 Ii
H, ;;
. ,f
.,,
I t,
·/
1
t
•1
:J
t
i ~
''!
,., ,'
;,J
11: fl
~ ~
1·!, ~
,1, (
L 11
! 'II
1:
,1,
~ l' Ill
n1 nt
' ~h
'~- tJJ flJ
1
1 !: J
nJ u• 1
11
t fU il
II J I 'II
j ~ J f I 1.:;l
tlf t: t S
Iii ;i: X Ill 1,
•u
'!i
:t
<11
I
I
j' 1, I
1 t ~l /
I j ' I() I" ~
1,rlrm I
I I rJJ ~ er
•11 I S
1'- ~
0)

13. !e
t': - -~....:.
4 5 s s ~ , .:,
A !3 C [) ::-
3
-
., ~3 • 4 E 1'5 1- 13
J K M r~ Q =
~ Q h?SE'
a are mo~! e e:- ::--e;:3::-.e e e-e-~
~ s a -.a:-:,Je.n ,
c s a- .1 "a:.: me'..?_ ...
d s a,.. e e-e-1,.... •2. e-::~! -
e) han~ e3s. 0- s::.· ,.., ::-.,,·-
-.. .... - .... :::-,
._
:, " ....
~~ 0~D:: ee--e-:s ~;-e:="en~~ -:-ar-Jeare;pen ::ie::,
(t-0•::-, s :"'e ·st --e--r,e• ;)[ t'le group a-.c i "h..a r.1 s
tne as.'
So·o-- . u-- - c.~· Ga um ':id ...'."!"I, Toa um
A.rs,·,e· ."'e 0 Ci "9 auest10ns,., reatio:1 t.:, the abc.e
g Ou:'.' C' e e""ents :
(a) W;::h element has the most rie•a ic ::"'aracte· ~
lt-) ',nr~h element would be expected t0 ha" e ~"e
h•ghest elec:tronegativity ?
(c) If the electronic configuration of alum n 1.r s 2 S,
3, how many electrons are there n the oute• s.'"ie
of "8lium?
(d) The atomic numberof boron is 5. Write the cher c.aJ
fomua ofthe compound formed When boron reacts
wlh chlorine.
(e) WI 118 elements in the ~ 10 the nght of tt11s
bolall ~ be more metallic or less metallic ·n
cll8Je+1a 7 Justly~ answer.
Alomlc number (Z)
•-~r o
n . Atomic IIIUIIHr is
• IJ ofan elemtllt, Ha111Se IIO ht'O
a.same aromic ••••
·c number (Z = ~1...mberofprolDDS.
= ~umber meltdruu&.
• It d -.tingm~hes J.n element .... allmr tla ues,
became no
number.
• It gi, e~ the electronic .:o
e.~.. an element " 1th at
eiectronic configuntion
• It help,; u5 in finding
the penod.1c table.
, - r -
El,iatnn
H. -
B,., -
c~
" ,...- -
' --
01 ~· cl
f ... l ~-:-
,. -
' .... ~~
Y.;-., ~
Ahl- i:.:y-
S1h: 1'n
P:~ ,;1,.:~~
S-~
:--"~r
C~.:n..~
!:,. .
Pou,, ...
C1k u.m
H
He
s~
ti
('
~
0
:
~~
K.
M
;
s
:>
:-
(
Ar
IR
c~
Mass number (A)
her
I -
I ~
Q
Mass number (Al = Zo. of pro1oos p
+ So. of neuuoos n
A d~ look a, w r~ ·-
of Uilrur ~~~111s ":r
wlakA ltav~ a• ere■ ••IIIIHr
·•"•••j111i,,_ • ic •11 1hn Jiu _.
-
-
-•rrs fWltt llliiP • •at ltn

14. Pb.'-sical
ttatr
clf--DC'('
dn:t.rons
Conduction
'ature
f
citing
....
aad
boilin,s=
.
.
.
.
toru.ir
.
.
.
loni-.::r,,_....,
D)
Q}ro
fJ"e'Shl:i,
ct.!
b.."1
,
·r.come
dull
as
tfx-)
~
-a
ith
au.
~-c<.:s
or.e
,ll1mc-c
eJearon
end
lhert'fore
mm.:
sunihr
properue.::.
ll:~y
form
pclSlO~
JOO..
~..ir.,
ID~
a
,.mg~
chzr,;e
r,:.
Na•
Good
cor
••
t,sc-rors
of
ele-c-t:icit~.
HighJJ
~,-e.
d«rrrrposiiffe
metals.
MetallK-
charac-te..
uic~s
from
lithmm
<lit
to
francium
(Fr).
Deacascs
~n
the
group.
llle)·
have
the
~est
atomic
.size
m
their
pi:riod_
TIie
-...cu
"-1bci-
increases
~n
the
group.
111ey
111nie
ao.aa
1.E.
in
lbeir
period.
die
l"JIIP.
l!A
.
.
.
.
.
.
.
.
fllnba-
i:e
(pot'
.
-
.
-
---.-__,
~
-------J
lodme
(
d.J.rl;.
gre
and
tbccd'~
Poss.t."Ss
snen,
sho"
tjJDJlar
prope.rues.
llr.y
form
ne~ati'.e
wn
CarT)tng
a
single
charge
e.g.
CJ
~·on-conductors
of
eJectriC'lt)
Highly
reacth-~
..
electTOn£ga1fre
non-metals.
i'oo-metallic
characte-.r,
decrea.,;es
from
fluorine
(F)
to
iodine
0).
lncrea..x-s
down
the
group.
They
have
the
smallest
atomic
s17..e
in
lhcir
period.
Atomic
size
increases
do.._-n
the
group.
They
have
high
I.E.
(lower
than
noble
gases)
m
their
period.
They
have
bigb
E.A.
values,
They
IOo
••aa-.e
._dle....,(a,
,tia:Qbas--
i...e-.1!.N
.
.........
Ii
.
.
,
.
.
......
-~:~•~;.
~
~
..
,.._~
.
'
....
--
~
.

15. ---
4
IA
IIA
A
IJA
,/A
-
'
---
2
1
and
2
H,
-
-
s=-...:;,.::,es,
1
~-
-+
-~-+.
-
2
:,~..:):':
a
3
to
10
Lia
Be,
I
2
1
22
~
-~
Sr-.D::
8
,
11
to
18
3
o,
I
c,
Fl
r
(),
'
'
u
2.3
l
2.11
i
2.6
:!.6
I
2.t
At.,
I
G,,.
r>II
G,,
c
;
1.,
2,fl,
'
.
l
2
O,,•I
•
2.e,r-
i
2.1u;
I
2
.B
I
r
_Q:-'
,
.
J
16
TilMJSI
nm,
:
Cl.[MJ"t
lt
'1
I
I
5
~:,r-.g
iB
r~-
5'~
Rb.
,
L
5
Lor.ges!
32
55
to
86
,
Cs
-
Lo~gest
87
to
,...___
-
G;:;GO
a:e
A!'>(aJ
metals
Lanthanide
e,cepl
::yd,oge!'l
G·-"
-
2
.~!'.
<
t'le
eann
rretals
I
--·
·--
I
-+--
+-
~
G;;~;
3
t
o
i
2
Transition
elements
Actinide
senes
Th
90
l
series
G,:::~;;
;
-;
ii-lalogens
L
---
-
.l.
_
-
G::it::i
18
Inert
gases
Grc~:i
me
6"
penod
Lantna
rude
sl
Inner
Transihon
Elements
Groi;o
111
B
,
"
penod
Actinides
_J
INNER
'
TRAN$1TION
·
ELEMcNts·
VARIATIONS
.
I
N
PERIODIC
PROPERTIES
•
-
-:
,
'1-"Ci¥J'tt'
•
•.,..
•
-
•W
·i!.__
No.
of
vaJencc
electrons
Alalic
lli7.e
(radius)
Aaws
11"
INriod
(uft
to
Jirld)
I
0mm
11N
Fflup
(1bp
IO
...._>
Increases
Decreases
Increases
Decreases
Increa-.es
Increases
Increases
Decreases
Increases
from
group
I
to
group
IV
and
then
decreases
from
group
I
to
group
IV
and
then
Remu111,
,amc
Increases
Oecrca,e.s
Increases
Decreases
Decreases
Decreases
Increases
Group
I
nnd
II
decreases
Group
Ill
and
IV
decn:aseS
Group
V
10
VU
increMa
Group
I
and
D
decn,ueS
Group
m
and
IV
decrea
Group
V
to
VD
~
Decreues
1acre-
o,
..
...
,
...
ra,q
H
,l
110,
:-~
IJ
Ar
11
2.80
Y.r
Z!l14
l
i
t
lae
O~J,._
Lu
Lr
t•

16. •'
Chlo<in,
"'
1h,
P,·dodk
fohl,·
,.,
'"
'
'"""''''"
hJ
rh,·
I
elcml'nls
I
i1h
aiomic
number
<J.
16.
18
and
3.'i.
(a)
Which
of1hesc
hm
c
Physical
and
Chemical
propcrltl's
rl'sernbling
chlorine
?
I
(b)
Which
ts
morl'
elcc1roncga1in·
1han
chlorine
·
1
Firs1
ionisa1ion
cnthalp)
or
1wo
clt-mcnls
>..
and
Y
:ire
500
kJ
mol
I
and
375
kJ
rnol
I
rcspcc1ivcly.
C'omrncill
about
!heir
rela1i,c
posi1ion
in
a
group
as
wl'II
as
in
a
period.
I
,.
An-ange
the
following
in
order
or
increasing
radii
:
(a)
Cl
.
Cl
(b)
Mgi•,
Mg.
Mg
·
(c)
N.
0.
P
Which
element
from
the
folio
ing
has
!he
highcsl
ionisation
energy
?
(a)
P,
Na,
Cl
(b)
F,
0.
Ne
Explain
your
choice.
(c)
Ne.
I
le.
Ar
The
electronegati,
ilies
(according
lo
Pauling)
of
the
elements
in
Period
3
of
the
Periodic
Table
are
as
follows
with
the
elements
a1Tanged
in
alphabetical
order:
Al
CJ
Mg
Na
P
S
Si
1·5
3·0
1·2
0-9
2·1
2·5
1·8
Arrange
the
elements
in
the
order
in
which
they
occur
in
the
Periodic
Table
from
left
to
right.
(The
group
I
element
first,
followed
by
the
group
2
element
and
so
on,
up
to
group
7).
Choose
the
word
or
phrase
from
the
brackets
which
correctly
completes
each
of
the
following
statements:-
(a)
The
element
below
sodium
in
the
same
group
would
be
expected
to
have
a
.................
(lower/higher)
electro-negativity
than
sodium
and
the
element
!ltl'
,lllll',
(it)
Jl'lll;llll~
·"
)
(kl'll',1',C,
(111
)
,ncrcasc:--.
(1~
.
,otc111ial
:
(
·)
The
io11w11H1n
I
(i1)
dccrl'asl''
l
>
·111cl
clown
(i)
goes
11
1
'
(iv)
rc111,11ns
1hr
sa,
11
c
(iii)
increases
.
··
1c
.
(cl)
The
a1or111c
s1
.
(
i)
decreases,
(ii)
increases,
...
remains
the
salllC,
.
(
111
)
.
.
.
.
"tscs
and
so111ct1111es
decreases
(iv)
so111c11111cs
,11c1c,
.
.
.
•.
,
JT'
·
1
y
or
the
clements
111
group-
(c)
The
electron
,1
1111
s
I
lo
7:
d
the
n
down.
(i)
goes
up
an
.
d
th
en
,
ncrcascs,
(ii)
decreases
an
(ii
i)
increases,
(iv)
decreases.
1
t
f
One
short
period
of
the
Periodic
Table
IO.
The
e
emen
s
o
.
.
.
below
1
·
11
order
from
left
to
nght.
are
given
Li
Be
B
C
O
F
Ne
(a)
To
which
period
do
these
elements
belong
?
(b)
One
element
of
this
period
is
missing.
Which
is
the
missing
element
and
where
should
it
be
placed
?
(c)
Place
the
three
elements
fluorine,
berylJium
and
nitrogen
in
the
order
of
increasing
electronegativity.
(d)
Which
one
of
the
above
elements
belongs
to
the
halogen
series
?
above
chlorine
would
be
expected
to
have
a
............
.
(lower/higher)
ionization
potential
than
chlorine.
(b)
On
moving
from
left
to
right
in
a
given
period,
the
number
of
shells
................
,.
(remains
the
same/
JI
.
With
reference
to
the
variation
of
properties
in
the
Periodic
Table,
which
of
the
following
is
generally
true?
increases
decreases).
>
'
_,.,
•
"••••''I
I
(iii)
On
moving
down
~8JP,up,
~
electrons
.................
~
I
decreases).
~;;f.H"j
lliv)
Metals
are
good
.....
.
~
I
reducing
agent)
because
I
(acceptors/donors).
(a)
Atomic
size
increases
from
left
to
right
across
a
period.
:«>)
1(!,nization
potential
increases
from
left
to
right
~
.ateJi~

17. t,)
II
d
11111
rcprr~.nll
l1)dro;•.cn
511111c
11
c1
11
r,)
mbol
.ind
1i.1~11u
111
111
1hr
ere
1,
l,
1,w11
1th
,l
lrt1t·,
)(II
ti·
nod
2
clcmr111
..
A.
n.
1
.·
111
1d
I>,
11w
111w
wl11d1
l
c
k..t,1111
uff11111
y
,
J
,t111um
1
luorlll
B
C.11111111
I>
Nc:(111
1.
i
I
IA
~
JIJA
i
l'1
t
VA
VI
-
'
V
ii
i
t
C>
I(,
I
'
'
'
IX
I.I
A
l
<i
(>
.I
Ne
II
K
L
c;
l
l
L
~
-
"
--
~_____J,_
l
_
-
-
-
-
II
',elect
1111111
11tc
1:,hll
2010
(iJ
Wl11ch
,.,
1110_
,
1
c
kt
t1011q.':11in·
r,,)
I
low
11w11y
v;i
l1·11n·
l'lt-c
twns
a11.·
present
111
U
1,
11
,
W,
,t,:
1111
101111111a
of
th1.·
compound
between
B
:111d
11
.
riv)
111
1lie
crn11
po1111d
hc
tWCl'l1
I·
and
J
what
type
of
bond
wi
ll
lw
101111,·d
/VJ
nr.,w
rlw
tkd
rnn
dot
stmcture
for
the
compound
frn111«I
lll'twccn
C
and
K
.
l:iJ
'I
hi:
1111111bcr
of
electrons
in
the
valence
shell
of
a
11:ilogcn
is
.............
A
-
I.
B
-
3.
C
-
5,
D
-
7.
/h)
l:lcctroncgativity
across
the
period
.............
!increases/
decreases).
le-)
Non-metallic
character
down
the
group
..............
.
(increase/decreases].
(d)
Atomic
number
of
an
element
is
16.
State
"
·-
__
..
,_
..
-
-
-
it
belonas
,e
lht:
{Oflt'l·t
a11,wcr
111
the
fKllt>d1r
labk
llll'j.'IOIIJ>
/
:
1.B:
Wl11tl1
ol
the
lollow'
w11h
elr111c11t.
ol
the
electron(s)
in
the
element
non-metal.
•-•-.a
power
of
elements
od.
,
.
I
hey
11.1C'
src
11
cie(.l11111s
111
1Jw11
v,1k11,~c
dtl'.11
n.
-1
he
y
,nc-
l11
t:
hl
,v
,c;1..i1v,:
t.h.:1111,.,dl~
(_
',
·1
h•'.)
,111:
111<:1
,dlt,·
lit
11,llllli'
n
'
I
he
y
;
II
C:
dr,11111111,
Ill
tlH'
.
11
11111kt
111111'
1111111
Id>
,
'
,t.1t1•
1h1:
r1111
1p
:111d
I''
1111d
uf
111<:
,·lnm·111
h,,v111L!
thn·c
!.
h('lls
w11h
lhll'<
:
i:J.-<111111,
111
v;,knl'l:
,
hel
l
2012
l.1J
(
l111owtlw11111nl.111,wl'I
(1<1111lhl·opt1<111
11l'll'1m:11t
111
pl'lilld
I
who,l·
l'ln
t1on
,dl11111y
"
/
l
'
l
l
>
/
N1·011
ll
S11lphm
('
~od111111
I>
/11.!t>ll
(h)
(
ii'
('
ll
',l(lll
.
(1)
10111'al1011
potl·nt1al
of
lhl'
l'k1111.:11t
1lll"ll'.l.
"
l'"
,,no),,
:1
11t·111>d
fio111
It'll
10
11
g
ht.
HO
(111)
/lknl1
111l'lall>
,11t·
~•oml
n-d11c111g
,1gc11
t,
(r)
Then·
:11e
three
elt·n1cnls
E.
F,
(i
wi
lh
ato111il'.
11u111bc1..,
19,
8
und
17
rc!.pcctrvcly
(
'la%ifiy
lhl·
ahovl·
dcmcnts
as
rrn:
tals
and
non-metals
.
(cl)
Name
:
A
metal
present
in
perrod
3.
group
I
of
the
periodic
tabk
201.
1
(a)
Among
tlu:
period
2
clements.
the
clement
which
has
high
electron
affinity
is
A.
Lithium
B.
Carbon
C
.
Chlorine
D
.
Fluorine
(b)
In
the
table
below,
H
does
not
represent
hydrogen
.
Some
elements
arc
given
in
their
own
symbol
and
position
in
the
periodic
table
while
others
are
shown
with
a
letter.
----·-
(7.VIIA
ltl-0
Group
No.
I-
IA
2-IIA
13111A
t4
-IVA
15-VA
((>.VIA
-----
---
1
-
-
-
-
'
-
-
-
·
-
L_
-
-
-
2nd
period
LI
0
0
J
Ne
---
)rd
period
A
Mg
E
s,
H
M
4th
period
R
T
I
Q
u
y
Answer
the
following
questions.
(i)
Identify
the
most
electronegative
element.
(ii)
Identify
the
most
reactive
element
of
group
IA
or
I.
(iii)
Identify
the
element
from
period
3
with
least
atomic
size.
(iv)
How
many
valence
electrons
arc
present
in
Q.
(v)
Which
element
from
group
2
would
have
the
least
ionization
energy
?
(vi)
Identify
the
noble
gas
of
the
fourth
period.
(vii)
In
the
cornpound
between
A
and
H
what
type
of
bond
la
formed
and
atve
its
molecular
formula.
l
~
(~
element
wbicbhas
tho
highest
ionization

18. <O
B
Arom,c
rnd1m
nnd
nucfc:ir
dwrgc
dccrc,1scs
C.
Arorn"·
r,1d111s
incn:,,~c,
1ind
uucll~Jr
chJrgc
dee-re
a,{'~
I.>
Arou11c
md1u<.
dee
rci,~l''
und
1111cfc,H
charge
lrltli.'.il('<;
(11)
An
rlcmrll!
A
bclo11g111~
ro
,~rrnd
l
111uJ
group
JI
w,11
have,
i
1
shd
l~
r111d
.!
Vitlenc<"
clccrrnn~
B
2
~hell,
and
1
',tlcncc
,c•lcl·trons
c·
3
<,hell,
:111d
~
vc1fencc
cl~tron'i
I)
.!
~hell
1111<1
2
,,tlrncc
cfcctrom
(h)
11111111c
numhrr
of
nn
clcrncut
/
,.,
16
follow111g
-
(,
l
Stare
the
period
,,nd
croup
to
whKh
'l
be
Ion
(11)
h'/rimcwlo
(c)
.S1.11e
the
fonnul.:i
of
h)drogcu
(d)
M
,,
a
rn
()
I
~
:
.
~
~~-
(aJ
Among
lea.,r
e
r
JS
I
"
2016
(a;
,'vfet:Jl5
are
good
..
·-··
..
,
(ox1dmn
·
:igent)
h<:c.iuse
the}'
arc
electron
donor)
(b)
An
element
wrth
atomic
number
19
1w1IJ
ITl<,sr
comlJJne
chemic..illy
w11h
the
elemenu
who'lC
number
i'i
·
(I)
17
(11)
1
l
(ill}
28
(ilJ
20
(c)
1<,•wri/1.!
the
following
~ntenceo;
hv
,;~m.,
tL-
-
e,
m:
01fi
ymhol
:>
(greaier
1hrJnJ
or<
lieu
ihanJ
m
the
hi·
tel
J'CO
.
"lll'l
(rJ
The
,on11at10n
potential
of
Pot;,u,.,rn
that
of
Sodium
;,i;
atnll)
of
Iodine
,