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n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

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Page 1: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å
Page 2: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

n=1

n=1

n=1

n=2

n=2 n=3

Page 3: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Mg Mg (Z=1(Z=1

2)2)

RadiiRadiiNe=0.69 Ne=0.69

ÅÅ

Na=1.54 Na=1.54 ÅÅ

Mg=1.30 Mg=1.30 ÅÅ

Page 4: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Atomic Radii

Page 5: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Grey = Neutral Radii, Grey = Neutral Radii, Red = Cationic Radii, Blue = Anionic Radii Red = Cationic Radii, Blue = Anionic Radii

Page 6: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Isoelectronic SeriesIsoelectronic Series

RadiiRadiiOO2- 2- = 1.40 Å= 1.40 Å

FF--= 1.33 Å= 1.33 Å

NaNa++= 0.97 Å= 0.97 Å

MgMg2+2+= 0.66 Å= 0.66 Å

Isoelectronic atoms/ions have identical Isoelectronic atoms/ions have identical numbers of electrons.numbers of electrons.

As the nuclear charge in an isoelectronic As the nuclear charge in an isoelectronic series increases the size of the atom series increases the size of the atom

decreases.decreases.

Page 7: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Periodic Trends in 1st Ionization Energy

Page 8: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Periodic Trends in 1Periodic Trends in 1stst Ionization Ionization EnergyEnergy

C P

Se

I

Non-metals, high 1st IE

SAs

Si

Ga

Zn

Page 9: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Beyond 1st Ionization Energy

Page 10: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Electron Affinity

Page 11: n=1 n=2 n=3 Mg (Z=12) Radii Ne=0.69 Å Na=1.54 Å Mg=1.30 Å

Properties of the Group I & II Properties of the Group I & II MetalsMetals