chapter 6: the periodic table. organizing the elements demitri mendeleeve (russian – 1869) demitri...
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Chapter 6:Chapter 6:
The Periodic TableThe Periodic Table
Organizing the ElementsOrganizing the Elements Demitri MendeleeveDemitri Mendeleeve (Russian – 1869) (Russian – 1869)
Published the 1Published the 1stst periodic table periodic table Based on Based on atomic massatomic mass
The Periodic LawThe Periodic Law Modern Periodic TableModern Periodic Table
Organized according to Organized according to atomic numberatomic number
Periods Periods = rows 1-7= rows 1-7 equal to the principal energy equal to the principal energy
levellevel
GroupsGroups = columns 1-18 = columns 1-18 elements have similar propertieselements have similar properties
Law:Law: Properties of elements repeat as you Properties of elements repeat as you move from move from LeftLeft → → RightRight across a period across a period
Period → Group ↓
Metallic CharacterMetallic Character Approx. 2/3 of the elements are metalsApprox. 2/3 of the elements are metals Metallic PropertiesMetallic Properties
LusterLuster ConductivityConductivity MalleabilityMalleability DuctilityDuctility Tend to lose electronsTend to lose electrons
Nonmetallic PropertiesNonmetallic Properties Dull lusterDull luster Poor conductorsPoor conductors BrittleBrittle Tend to gain electronsTend to gain electrons
Metalloids (semimetals)Metalloids (semimetals) Some properties characteristic of metals and Some properties characteristic of metals and
other properties characteristic of nonmetalsother properties characteristic of nonmetals
Metals and NonmetalsMetals and Nonmetals
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Sc
21
Ti
22
V
23
Cr
24
Mn
25
Fe
26
Co
27
Ni
28
Cu
29
Zn
30
Ga
31
Ge
32
As
33
Se
34
Br
35
Kr
36
Rb
37
Sr
38
Y
39
Zr
40
Nb
41
Mo
42
Tc
43
Ru
44
Rh
45
Pd
46
Ag
47
Cd
48
In
49
Sn
50
Sb
51
Te
52
I
53
Xe
54
Cs
55
Ba
56
He
72
Ta
73
W
74
Re
75
Os
76
Ir
77
Pt
78
Au
79
Hg
80
Tl
81
Pb
82
Bi
83
Po
84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
METALS
Nonmetals
Metalloids
Reference TableReference Table• Periodic Table Periodic Table
Trends:Trends: 1. Across a period, metallic character →1. Across a period, metallic character →
Why?Why?More electrons in outer shellsMore electrons in outer shellsLess tendency to lose electronsLess tendency to lose electrons
2. Down a group, metallic character → 2. Down a group, metallic character →
Why?Why?Less electrons in outer shellsLess electrons in outer shellsGreater tendency to lose electronsGreater tendency to lose electrons
decreases
increases
Metallic ReviewMetallic Review Identify each element as a metal, Identify each element as a metal,
nonmetal or metalloidnonmetal or metalloid
a)a) Gold -Gold -
b)b) Silicon -Silicon -
c)c) Sulfur -Sulfur -
d)d) Barium -Barium -
MetalMetalloidNonmetal
Metal
Which of these sets of elements have Which of these sets of elements have similar physical and chemical similar physical and chemical properties?properties?
a)a) oxygen, nitrogen, carbon, oxygen, nitrogen, carbon,
b)b) strontium, magnesium, calcium, strontium, magnesium, calcium, berylliumberyllium
c)c) nitrogen, neon, , fluorinenitrogen, neon, , fluorine
Name 2 elements that have properties Name 2 elements that have properties similar to those of the element similar to those of the element sodium.sodium.
Any other Group 1 element:Lithium, Potassium, Rubidium, Cesium, Francium
boronboron
nickelnickel
Identify each property below as more Identify each property below as more characteristic of a metal or a nonmetalcharacteristic of a metal or a nonmetal
a)a) Brittle -Brittle -
b)b) Malleable -Malleable -
c)c) Poor conductor of electricity -Poor conductor of electricity -
d)d) Shiny -Shiny -
e)e) Tend to gain electrons -Tend to gain electrons -
In which pair of elements are the In which pair of elements are the chemical properties of the elements most chemical properties of the elements most similar?similar?
a)a) sodium and chlorinesodium and chlorine
b)b) nitrogen and phosphorusnitrogen and phosphorus
c)c) boron and oxygenboron and oxygen
Nonmetal
MetalNonmetal
MetalNonmetal
Classifying the ElementsClassifying the Elements
Alkali MetalsAlkali Metals – – Alkaline Earth MetalsAlkaline Earth Metals – – HalogensHalogens – – Noble GasesNoble Gases – – Representative ElementsRepresentative Elements – – Transition ElementsTransition Elements – –
Group 1 (1A)Group 1 (1A)
Group 2 Group 2 (2A)(2A)Group 17 (7a)Group 17 (7a)
Group 18 (8A) Inert gasesGroup 18 (8A) Inert gases
Groups 1A – 7AGroups 1A – 7A
All Group BAll Group B
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Sc
21
Ti
22
V
23
Cr
24
Mn
25
Fe
26
Co
27
Ni
28
Cu
29
Zn
30
Ga
31
Ge
32
As
33
Se
34
Br
35
Kr
36
Rb
37
Sr
38
Y
39
Zr
40
Nb
41
Mo
42
Tc
43
Ru
44
Rh
45
Pd
46
Ag
47
Cd
48
In
49
Sn
50
Sb
51
Te
52
I
53
Xe
54
Cs
55
Ba
56
He
72
Ta
73
W
74
Re
75
Os
76
Ir
77
Pt
78
Au
79
Hg
80
Tl
81
Pb
82
Bi
83
Po
84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
Label your Reference Periodic Table…
1
2 13 14 15 16 17
18
3 4 5 6 7 8 9 10 11 12
Classifying ReviewClassifying Review Which of the following are symbols Which of the following are symbols
for representative elementsfor representative elementsNa, Mg, , Cl?Na, Mg, , Cl?
Which of these metals is Which of these metals is notnot a a transition metal?transition metal?
a)a) AluminumAluminumb)b) SilverSilverc)c) IronIrond)d) ZirconiumZirconium
Fe, NiFe, Ni
Atomic RadiusAtomic Radius Atoms are roughly sphericalAtoms are roughly spherical Sphere size can be determined using the Sphere size can be determined using the
radiusradius Problem:Problem:
Solution:Atomic Radii – half the half the distance between the distance between the nuclei of identical nuclei of identical atoms that are bonded atoms that are bonded togethertogether
Edges of orbitals are fuzzy Edges of orbitals are fuzzy and difficult to measure…and difficult to measure…
Reference Table: Reference Table: • Table STable S
Trends:Trends:1. Across a period, the atomic radius 1. Across a period, the atomic radius → →
Why?Why? Nuclei have larger positive charges Nuclei have larger positive charges Electrons are pulled in closerElectrons are pulled in closer
2. Down a group, the atomic radius 2. Down a group, the atomic radius →→
Why?Why?Greater number of energy shellsGreater number of energy shellsValence electrons are further away from the Valence electrons are further away from the nucleusnucleus
decreases
increases
Atomic Radius ReviewAtomic Radius Review Which element in each pair has a Which element in each pair has a
larger atomic radius?larger atomic radius?
a)a) & lithium& lithium
b)b) & bromine& bromine
c)c) carbon &carbon &
d)d) & neon& neon Arrange these elements in order of Arrange these elements in order of
decreasing atomic size: sulfur, decreasing atomic size: sulfur, chlorine, aluminum, and sodium.chlorine, aluminum, and sodium.
Sodium Sodium → Aluminum → Sulfur → Chlorine→ Aluminum → Sulfur → Chlorine
sodiusodiummcalciumcalcium
germaniumgermanium
fluorinefluorine
Ionization EnergyIonization Energy What is an What is an ionion??
An electrically charged atomAn electrically charged atom
Atoms may either Atoms may either gaingain or or loselose electrons electrons Loss of electrons = (+) charge Loss of electrons = (+) charge →→ Gain of electrons = (-) charge Gain of electrons = (-) charge →→
Ionization energyIonization energy ==
cationcationanionanion
the amount of energy the amount of energy requiredrequired to to remove the most loosely bound remove the most loosely bound electron electron
A + A + energyenergy A A++ + e + e--
Reference Table Reference Table • Table STable S
Trends:Trends:1. Across a period, the ionization energy 1. Across a period, the ionization energy →→
Why?Why?Electrons are held closer to the nucleus Electrons are held closer to the nucleus
Electrons are more difficult to removeElectrons are more difficult to remove
2. Down a group, the ionization energy → 2. Down a group, the ionization energy →
Why?Why?Electrons are further away from the nucleusElectrons are further away from the nucleus
Electrons are easier to removeElectrons are easier to remove
Relate Back:Relate Back:
increasincreaseses
decreasedecreasess
What type of relationship exists between What type of relationship exists between ionization energy and atomic radii?ionization energy and atomic radii?InversInvers
ee
Ionization ReviewIonization Review Which element in each pair has a Which element in each pair has a
greater ionization energy?greater ionization energy?a)a) lithium,lithium,b)b) magnesium,magnesium,c)c) cesium,cesium, Arrange the following groups in Arrange the following groups in
order of increasing ionization order of increasing ionization energy energy
a)a) Be, Mg, SrBe, Mg, Srb)b) Bi, Cs, BaBi, Cs, Bac)c) Na, Al, S Na, Al, S
boronboronstrontiumstrontium
aluminumaluminum
Be Be → Mg → Sr→ Mg → SrBi Bi → Ba → Cs→ Ba → CsNa Na → Al → S→ Al → S
Ionic SizeIonic Size CationsCations from when from when atoms atoms looseloose ee--
The cation is The cation is smallersmaller
AnionsAnions from when from when atoms atoms gain egain e--
The anion is The anion is largerlarger
Reference TableReference Table• No true tableNo true table
Trends:Trends:1. Across a period, ionic size 1. Across a period, ionic size → →
Why?Why?When eWhen e-- are lost, the attraction between the are lost, the attraction between the remaining eremaining e-- increases increasesee-- are drawn closer to the nucleus are drawn closer to the nucleus
2. Down a group, ionic size →2. Down a group, ionic size →
Why?Why?Increased atomic radiusIncreased atomic radiusee-- are further away from the nucleus are further away from the nucleus
increases
decreases
Ion Size ReviewIon Size Review Which particle has the larger radius Which particle has the larger radius
in each atom/ion pair?in each atom/ion pair?a)a) Na,Na,b)b) S,S,c)c) I,I,d)d) Al,Al, The ions NaThe ions Na++ and Mg and Mg2+2+ each have each have
10e10e--. Which ion would you expect . Which ion would you expect to have a smaller ionic radius?to have a smaller ionic radius?
MgMg2+2+ atomic radius is smaller & e atomic radius is smaller & e-- are pulled in closer are pulled in closer
NaNa++
SS2-2-
II--
AlAl3+3+
ElectronegativityElectronegativity
A measure of the ability of an atom to attract a A measure of the ability of an atom to attract a pair of electrons when bonded to another atompair of electrons when bonded to another atom
Ability to ‘pull’ electrons from another atomAbility to ‘pull’ electrons from another atom
Electrons pulled closer:
Electrons pulled away:
Reference TableReference Table• Table STable S
Trends:Trends:1. Across a period, the electronegativity 1. Across a period, the electronegativity → →
Why?Why?Atoms are very close to a stable octetAtoms are very close to a stable octet‘‘Pull’ electrons from other atomsPull’ electrons from other atoms
2. Down a group, the electronegativity →2. Down a group, the electronegativity →
Why?Why?Top atoms have few electrons, and hold them Top atoms have few electrons, and hold them tightlytightlyBottom atoms have numerous electrons and little Bottom atoms have numerous electrons and little desire to acquire moredesire to acquire more
increases
decreases
Electronegativity ReviewElectronegativity Review Which element in each pair has a Which element in each pair has a
higher electronegativity value?higher electronegativity value?a)a) Cl,Cl,b)b) C,C,c)c) Mg,Mg,d)d) As,As, Which element in each pair has a Which element in each pair has a
greater attraction for electrons? greater attraction for electrons? a)a) Ca orCa orb)b) O orO orc)c) S S
FFNN
NeNeCaCa
OOFF
or Kor K
DecreasesDecreasesIncreasesIncreasesElectronegativityElectronegativity
IncreasesIncreasesDecreasesDecreasesIon SizeIon Size
DecreasesDecreasesIncreasesIncreasesIonization Ionization EnergyEnergy
IncreasesIncreasesDecreasesDecreasesAtomic RadiusAtomic Radius
IncreasesIncreasesDecreasesDecreasesMetallic Metallic CharacterCharacter
Variation down Variation down a Groupa Group
Variation across Variation across a Perioda Period
Periodic Periodic PropertyProperty
Summary