Lecture 2_Periodic Relationships
Transcript of Lecture 2_Periodic Relationships
![Page 1: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/1.jpg)
Periodic Relationships Among the Elements
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
![Page 2: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/2.jpg)
2
When the Elements Were Discovered
![Page 3: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/3.jpg)
3
ns1
ns2
ns2
np1
ns2
np2
ns2
np3
ns2
np4
ns2
np5
ns2
np6
d1
d5 d10
4f
5f
Ground State Electron Configurations of the Elements
![Page 4: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/4.jpg)
4
Classification of the Elements
![Page 5: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/5.jpg)
5
Electron Configurations of Cations and Anions
Na [Ne]3s1 Na+ [Ne]
Ca [Ar]4s2 Ca2+ [Ar]
Al [Ne]3s23p1 Al3+ [Ne]
Atoms lose electrons so that cation has a noble-gas outer electron configuration.
H 1s1 H- 1s2 or [He]
F 1s22s22p5 F- 1s22s22p6 or [Ne]
O 1s22s22p4 O2- 1s22s22p6 or [Ne]
N 1s22s22p3 N3- 1s22s22p6 or [Ne]
Atoms gain electrons so that anion has a noble-gas outer electron configuration.
Of Representative Elements
![Page 6: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/6.jpg)
6
+1
+2
+3 -1-2-3
Cations and Anions Of Representative Elements
![Page 7: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/7.jpg)
7
Na+: [Ne] Al3+: [Ne] F-: 1s22s22p6 or [Ne]
O2-: 1s22s22p6 or [Ne] N3-: 1s22s22p6 or [Ne]
Na+, Al3+, F-, O2-, and N3- are all isoelectronic with Ne
What neutral atom is isoelectronic with H- ?
H-: 1s2 same electron configuration as He
Isoelectronic: have the same number of electrons, and hence the same ground-state electron configuration
![Page 8: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/8.jpg)
8
Electron Configurations of Cations of Transition Metals
When a cation is formed from an atom of a transition metal, electrons are always removed first from the ns orbital and then from the (n – 1)d orbitals.
Fe: [Ar]4s23d6
Fe2+: [Ar]4s03d6 or [Ar]3d6
Fe3+: [Ar]4s03d5 or [Ar]3d5
Mn: [Ar]4s23d5
Mn2+: [Ar]4s03d5 or [Ar]3d5
![Page 9: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/9.jpg)
9
Effective nuclear charge (Zeff) is the “positive charge” felt by an electron.
Na
Mg
Al
Si
11
12
13
14
10
10
10
10
1
2
3
4
186
160
143
132
ZeffCoreZ Radius (pm)
Zeff = Z - 0 < < Z ( = shielding constant)
Zeff Z – number of inner or core electrons
![Page 10: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/10.jpg)
10
Effective Nuclear Charge (Zeff)
increasing Zeff
incr
easi
ng Z
eff
![Page 11: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/11.jpg)
11
Atomic Radii
metallic radius covalent radius
![Page 12: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/12.jpg)
12
![Page 13: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/13.jpg)
13
Trends in Atomic Radii
![Page 14: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/14.jpg)
14
Comparison of Atomic Radii with Ionic Radii
![Page 15: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/15.jpg)
15
Cation is always smaller than atom from which it is formed.Anion is always larger than atom from which it is formed.
![Page 16: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/16.jpg)
16
The Radii (in pm) of Ions of Familiar Elements
![Page 17: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/17.jpg)
17
Ionization energy is the minimum energy (kJ/mol) required to remove an electron from a gaseous atom in its ground state.
I1 + X (g) X+
(g) + e-
I2 + X+(g) X2+
(g) + e-
I3 + X2+(g) X3+
(g) + e-
I1 first ionization energy
I2 second ionization energy
I3 third ionization energy
I1 < I2 < I3
![Page 18: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/18.jpg)
18
![Page 19: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/19.jpg)
19
Filled n=1 shell
Filled n=2 shell
Filled n=3 shell
Filled n=4 shellFilled n=5 shell
Variation of the First Ionization Energy with Atomic Number
![Page 20: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/20.jpg)
20
General Trends in First Ionization Energies
Increasing First Ionization Energy
Incr
ea
sing
Firs
t Io
niz
atio
n E
ner
gy
![Page 21: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/21.jpg)
21
Electron affinity is the negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion.
X (g) + e- X-(g)
F (g) + e- X-(g)
O (g) + e- O-(g)
H = -328 kJ/mol EA = +328 kJ/mol
H = -141 kJ/mol EA = +141 kJ/mol
![Page 22: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/22.jpg)
22
![Page 23: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/23.jpg)
23
Variation of Electron Affinity With Atomic Number (H – Ba)
![Page 24: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/24.jpg)
24
Diagonal Relationships on the Periodic Table
![Page 25: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/25.jpg)
25
Group 1A Elements (ns1, n 2)
M M+1 + 1e-
2M(s) + 2H2O(l) 2MOH(aq) + H2(g)
4M(s) + O2(g) 2M2O(s)
Incr
easi
ng r
eact
ivity
![Page 26: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/26.jpg)
26
Group 1A Elements (ns1, n 2)
![Page 27: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/27.jpg)
27
Group 2A Elements (ns2, n 2)
M M+2 + 2e-
Be(s) + 2H2O(l) No ReactionIn
crea
sing
rea
ctiv
ity
Mg(s) + 2H2O(g) Mg(OH)2(aq) + H2(g)
M(s) + 2H2O(l) M(OH)2(aq) + H2(g) M = Ca, Sr, or Ba
![Page 28: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/28.jpg)
28
Group 2A Elements (ns2, n 2)
![Page 29: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/29.jpg)
29
Group 3A Elements (ns2np1, n 2)
4Al(s) + 3O2(g) 2Al2O3(s)
2Al(s) + 6H+(aq) 2Al3+
(aq) + 3H2(g)
![Page 30: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/30.jpg)
30
Group 3A Elements (ns2np1, n 2)
![Page 31: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/31.jpg)
31
Group 4A Elements (ns2np2, n 2)
Sn(s) + 2H+(aq) Sn2+
(aq) + H2 (g)
Pb(s) + 2H+(aq) Pb2+
(aq) + H2 (g)
![Page 32: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/32.jpg)
32
Group 4A Elements (ns2np2, n 2)
![Page 33: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/33.jpg)
33
Group 5A Elements (ns2np3, n 2)
N2O5(s) + H2O(l) 2HNO3(aq)
P4O10(s) + 6H2O(l) 4H3PO4(aq)
![Page 34: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/34.jpg)
34
Group 5A Elements (ns2np3, n 2)
![Page 35: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/35.jpg)
35
Group 6A Elements (ns2np4, n 2)
SO3(g) + H2O(l) H2SO4(aq)
![Page 36: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/36.jpg)
36
Group 6A Elements (ns2np4, n 2)
![Page 37: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/37.jpg)
37
Group 7A Elements (ns2np5, n 2)
X + 1e- X-1
X2(g) + H2(g) 2HX(g)
Incr
easi
ng r
eact
ivity
![Page 38: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/38.jpg)
38
Group 7A Elements (ns2np5, n 2)
![Page 39: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/39.jpg)
39
Group 8A Elements (ns2np6, n 2)
Completely filled ns and np subshells.Highest ionization energy of all elements.No tendency to accept extra electrons.
![Page 40: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/40.jpg)
40
Compounds of the Noble Gases
A number of xenon compounds XeF4, XeO3, XeO4, XeOF4 exist.A few krypton compounds (KrF2, for example) have been prepared.
![Page 41: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/41.jpg)
41
The metals in these two groups have similar outer electron configurations, with one electron in the outermost s orbital.Chemical properties are quite different due to difference in the ionization energy.
Comparison of Group 1A and 1B
Lower I1, more reactive
![Page 42: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/42.jpg)
42
Properties of Oxides Across a Period
basic acidic
![Page 43: Lecture 2_Periodic Relationships](https://reader036.fdocuments.us/reader036/viewer/2022070400/55cf98ed550346d0339a82a8/html5/thumbnails/43.jpg)
43
Chemistry in Action: Discovery of the Noble Gases
Sir William Ramsay