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1 The Periodic Table

Transcript of The Periodic Table - cpb-us-w2.wpmucdn.com€¦ · The Periodic Table yDevelopment of the periodic...

1

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

8.1 and 8.2 Development of the periodic table and periodic classification

Figure 8.2, p. 257

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

+1 +2 +3 -1-2-3

Cations and Anions Of Representative Elements

Figure 8.1, p. 255

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

Ioni

c Si

ze8.3 Atomic and Ionic size

Figure 8.6, p. 262

Ioni

c Si

ze8.3 Atomic and Ionic size

Figure 8.8, p. 263

8.4 Ionization energy

What is ionization energy?What is the periodic trend for ionization energy?

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

Figure 8.9, p. 266

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?

8.4 Ionization energy

Table 8.2, p. 265

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)

Cha

pter

8 –

Prac

tice