ch 3 periodicity
TRANSCRIPT
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zbeta Bavorova
Assesment statements from
Pearson Baccalaureate HL
Chemistry
Chapter 3eriodicity
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Ch 3.1 The Periodic Table
3. 1. 1. Describe the arrangement of elements in the Periodic Table in order
of increasing atomic number.
The elements are arraned on the basis of the atomic number. The atomic number ro!s to
the riht and do!n.
3. 1. 2. Distinguish between the terms group and period.
Groupsare the columns of the periodic table. "lements in one roup have similar properties.
Periodsare the ro!s of the periodic table.
3. 1. 3. Apply the relationship between the electron arrangement of
elements and their position in the Periodic Table up to Z = 2.
! 3. 1. ". Apply the relationship between the number of electrons in thehighest occupied energy le#el for an element and its position in the Periodic
Table.
(http://www.drcruzan.com/Images/Chemistr
y/Chemistry_PeriodicEconfg.png)
E!E"E#$:ns1#$
P E!E"E#$: ns$np1#%
% E!E"E#$:ns$$n%1&p%$n%
1&d1#1&
& E!E"E#$: ns$$n%1&p%$n%
2&d1&$n%2&f1#1'
http://www.drcruzan.com/Images/Chemistry/Chemistry_PeriodicEconfig.pnghttp://www.drcruzan.com/Images/Chemistry/Chemistry_PeriodicEconfig.pnghttp://www.drcruzan.com/Images/Chemistry/Chemistry_PeriodicEconfig.pnghttp://www.drcruzan.com/Images/Chemistry/Chemistry_PeriodicEconfig.png -
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E'ectronegatiity
(Pau'ing)"lectroneativity is very much
related to e0ective nuclear
chare ionization enery and
electron a9nity so the trends are
similar.
"e'ting pointThe meltin point is dependent on the bondin
of the element.
-t is hih for elements in a metallic
bond. Hih for elements in a iant covalent
structure.
Lo! for covalently bound atoms.
-t is more di9cult to provide atoms that are
bound by strong intermo'ecu'ar ,onds!ith
enouh *inetic enery to melt them.
Group
1
(alkali metals):
:eltin point decreases do!n the roup.
As the size of the atom ro!s do!n the roup !hile
the metallic structure is still composed of ,1 ions the
chare density falls sini2cantly and thus the force
holdin the metallic lattice toether is !ea*er.
Group 17 (halogens):
:eltin point increases do!n the roup.
As the size of an atom ro!s do!n the roup the e0ect
of the ;an der
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Ch 3.3 Chemical properties
3. 3. 1. Discuss the similarities and di-erences in the chemical properties of
elements in the same group.
"lements !ithin the same roup have very similar chemical properties because chemical
properties depend on their electron con2uration = and the valence shell of electron !ithinthe same roup is the same.
Ho!ever their properties are not the same. 8or e)ample the reactivity of al*ali metals
increases do!n the roup. This is because of the fallin ionization enery because more
reactions !ill be able to provide enouh enery for ionization/.
3. 3. 2. Discuss the changes in nature* from ionic to co#alent and from basic
to acidic* of the o)ides across Period 3.
-onic compounds are enerally formed bet!een metal and non#metal the o)ides of
elements >a to Al have a giant ionic structure.
Covalent compounds are formed bet!een non#metals the o)ides of P ? and Cl are
mo'ecu'ar coa'ent.
The o)ide of silicon !hich is a metalloid is a giant coa'ent structure.
The ionic character of a compound depends on the di0erence in electroneativity bet!een
its elements the hiher the more ionic/.
The o)ides become more ionic do!n the roup as the electroneativity decreases.
The conductiityof the molten o)ide can be used as a measure of the ionic character.
Covalent compounds do not conduct electricity !hile ionic in the molten state/ do.
&ormu'a #a- (s) "g (s) *'- (s) i- (s) P012(s)
P03(')
(')
-(g)
C'-4(')
C'- (g)
5.
num,er
,1 ,$ ,3 ,' ,@
,3
,%
,'
,
,1
E.
conducti
ity in
mo'tenstate
hih very lo! none
tructure iant ionic iant
covalent
molecular covalent
*cid6,ase
character
basic amphotheric acidic
The acid#base properties of the o)ides depend on their bondin.
:etallic elements and thus ionic o)ides are basic. >on#metal o)ides !hich are covalent are
acidic. Those on the vere bet!een ionic and covalent are amphoteric. *mphotericsubstances sho! both acidic and basic properties such as !ater/.
>ote that5 *'7a'isare ,ases!hich are soluble in !ater. They form hydro)ide ions in a(ueous
solutions.
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Ch 13.1 Trends across Period 3
13. 1. 1. )plain the physical state $under standard conditions& and
electrical conducti#ity $in the molten state& of the chlorides and o)ides of
the elements in Period 3 in terms of their bonding and structure.
&ormu'ao8
ch'oride
#aC' (s) "gC'- (s)*'C' (s)
*'-C'3(g)iC'0(')
PC'9(s)
PC'(')-C'-(') C'-(g)
5.
num,er,1 ,$ ,3 ,'
,@
,3,1 &
E.
conducti
ity in
mo'ten
state
hih poor none
tructure iant ionic molecular covalent*cid6,ase
characterneutral
!ea*ly
acidicacidic
Because Cl is less electroneative than o)yen the transition from ionic to covalent occurs
earlier on in the period than for o)ides.
Al$Cl% is a dimer of AlCl3 !here the t!o bridin Cl atoms form dative covalent bonds formed
bet!een Al atoms.
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ydro'ysis o8 coa'ent ch'orides
Aluminium chloride
(aq )3+ (aq )+3Cl
Al Cl3(s ) Al
This !ill result in the formation of the
comple) ion AlH$/%D3,5
A comp'e5is !hen a central ion is surrounded by molecules or ions !hich posses a lone pair
of electrons. The liand has an independent e)istence as the surroundin species 'igands/
are bound via a dative covalent bond.
Comple)es are sho!n throuh the use of s(uare brac*ets.
The AlH$/%D3,
ion is acidic because the hih chare density of Al3,
attracts the electronsfrom the = H bond of the surroundin !ater molecules !hich results in the release of an H,
ion.
+(aq)2++H
Al (H2O )5 OH
3+ (aq )Al (H2O )6
etc.
Silicon and phosphorus chlorides
SiCl4
( l )+2H2
O ( l ) S i O2( s)+4HCl
PCl3(l )+3H
2O ( l ) H
3PO
3(aq )+3HCl (aq ) PCl
5(s )+4H
2O ( l ) H
3PO
4( aq )+5HCl ( aq )
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The enery separation of the t!o orbitals and thus the colour of the comple) depends on5
the nuclear chane
the chare density of the liand
the number of d electrons present the o)idation number of the central ion/
the shape of the comple) ion
13. 2. . 0tate e)amples of the catalytic action of transition elements and
their compounds.
! 13. 2. 4. 5utline the economic signi'cance of catalysts in the ,ontact and
6aber process.
There are t!o di0erent types of catalysts5
E$E;GE#TACT PMC"??
uses ;$@divanadium pento)ide/ as catalyst
2SO2(g)+O2(g)2SO3(g)
"GE#
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This vitamin is necessary in the production of erythrocytes and responsible for a
healthy nervous system.