The Periodic Table - University of Wisconsin–Milwaukee and 8.2 Development of the periodic table...
Transcript of The Periodic Table - University of Wisconsin–Milwaukee and 8.2 Development of the periodic table...
The Periodic TableDevelopment of the periodic table (8.1)Periodic classification of the elements (8.2)Periodic variation in physical properties (8.3)Ionization energy (8.4)Electron affinity (8.5)Variation in chemical properties of the representative elements (8.6)
8.1 and 8.2 Development of the periodic table and periodic classification
In what year was the modern periodic table developed?How was the periodic table put together?
ns1
ns2
ns2 n
p1
ns2 n
p2
ns2 n
p3
ns2 n
p4
ns2 n
p5 ns2 n
p6
d1 d5 d10
4f
5f
Ground State Electron Configurations of the Elements
Figure 8.1, p. 255
8.1 and 8.2 Development of the periodic table and periodic classification
In what year was the modern periodic table developed?How was the periodic table put together?
In what year were electrons discovered?In what year were protons discovered?
8.1 and 8.2 Development of the periodic table and periodic classification
Whe
n th
e E
lem
ents
Wer
e D
isco
vere
d
What are core electrons?How do these vary by period?
8.1 and 8.2 Development of the periodic table and periodic classification
He (2 core e-)
Ne (10 core e-)
Ar (18 core e-)
Kr (36 core e-)Xe (54 core e-)
What are valence electrons?How do these vary by group?
8.1 and 8.2 Development of the periodic table and periodic classification
1 2 3 4 5 6 7 8
How are electron configurations of ions determined and written?
8.1 and 8.2 Development of the periodic table and periodic classification
Ele
ctro
n C
onfig
urat
ions
of C
atio
nsan
d A
nion
s of
Rep
rese
ntat
ive
Ele
men
ts
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.
8.1 and 8.2 Development of the periodic table and periodic classification
Ele
ctro
n C
onfig
urat
ions
of C
atio
nsof
Tra
nsiti
on M
etal
s When a cation is formed from an atom of a transition metal, electrons are always removed first from the nsorbital 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
8.1 and 8.2 Development of the periodic table and periodic classification
How are electron configurations of ions determined and written?What is isoelectronic?Which species are isoelectronic?
Na K Na+
K+ Ca2+ Ti4+
Ne Al3+ S2–
Cl– Cl ArO2– Sc2+ Kr
8.1 and 8.2 Development of the periodic table and periodic classification
8.3 Atomic and Ionic size
Do all electrons feel the same nuclear charge?What is shielding?What is effective nuclear charge?
Na Mg Al Si P S Cl
Z 11 12 13 14 15 16 17
Core 10 10 10 10 10 10 10Zeff 1 2 3 4 5 6 7
σ 8.8 9.15 9.5 9.85 10.2 10.55 10.9Zeff 2.2 2.85 3.5 4.15 4.8 5.45 6.1
Na Mg Al Si P S Cl
Z 11 12 13 14 15 16 17
Core 10 10 10 10 10 10 10Zeff 1 2 3 4 5 6 7
σ 8.8 9.15 9.5 9.85 10.2 10.55 10.9
Na Mg Al Si P S Cl
Z 11 12 13 14 15 16 17
Core 10 10 10 10 10 10 10Zeff 1 2 3 4 5 6 7
Effe
ctiv
e N
ucle
ar C
harg
e
Na Mg Al Si P S Cl
Z 11 12 13 14 15 16 17
Core 10 10 10 10 10 10 10
Na Mg Al Si P S Cl
Z 11 12 13 14 15 16 17
8.3 Atomic and Ionic size
Li Na K Rb Cs Fr
Z 3 11 19 37 55 87
Core 2 10 18 36 54 86Zeff 1 1 1 1 1 1
σ 1.7 8.8 16.8 33.3 51.3 81.2Zeff 1.3 2.2 2.2 3.7 3.7 5.8
Li Na K Rb Cs Fr
Z 3 11 19 37 55 87
Core 2 10 18 36 54 86Zeff 1 1 1 1 1 1
Li Na K Rb Cs Fr
Z 3 11 19 37 55 87
Core 2 10 18 36 54 86
Li Na K Rb Cs Fr
Z 3 11 19 37 55 87
Li Na K Rb Cs Fr
Z 3 11 19 37 55 87
Core 2 10 18 36 54 86Zeff 1 1 1 1 1 1
σ 1.7 8.8 16.8 33.3 51.3 81.2
Effe
ctiv
e N
ucle
ar C
harg
e 8.3 Atomic and Ionic size
Effe
ctiv
e N
ucle
ar C
harg
e 8.3 Atomic and Ionic size
Margin Figure, p. 259
Effective Nuclear Charge (Zeff) increases across a period from left to right
Effe
ctiv
e N
ucle
ar C
harg
e (Z
eff)
incr
ease
s do
wn
a gr
oup
from
top
to
bott
om
8.3 Atomic and Ionic size
Do all electrons feel the same nuclear charge?What is shielding?What is effective nuclear charge?How does this affect the size of atoms?◦ How do we determine the size of atoms?
Radius = ½ the distance between the centers of the atoms
8.3 Atomic and Ionic size
Figure 8.3, p. 260
Ato
mic
Siz
e8.3 Atomic and Ionic size
Figure 8.2, p. 257
Atomic size decreases across a period from left to right
Ato
mic
siz
e in
crea
ses
dow
n a
grou
p fr
om t
op t
o bo
ttom
8.3 Atomic and Ionic size
Do all electrons feel the same nuclear charge?What is shielding?What is effective nuclear charge?How does this affect the size of atoms?◦ How do we determine the size of atoms?
How does atomic size change when ions form?
Cation is always smaller than atom from which it is formed.Anion is always larger than atom from which it is formed.
8.3 Atomic and Ionic size
Figure 8.7, p. 262
8.4 Ionization energy
Margin Figure, p. 265
Ionization Energy increases across a period from left to right
Ioni
zatio
n En
ergy
dec
reas
es d
own
a gr
oup
from
top
to
bott
om
8.4 Ionization energy
What is ionization energy?What is the periodic trend for ionization energy?What is the difference between 1st and successive ionization energies?
8.5 Electron Affinity
What is electron affinity?How can this be represented in a thermochemical equation?
Table 8.3, p. 268
8.6 Descriptive Chemistry
Read p. 268-278You will be tested on only those concepts that you have already been tested and/or taught. For example:◦ The electron configuration of calcium◦ The reaction of sodium with water◦ The metallic character periodic trends
(consider group 4)