modern atomic theory and the periodic table chapter 10 outline i.electromagnetic radiation ii.atomic...

Modern Atomic Theory and the Periodic Table

Chapter 10

OutlineI. Electromagnetic RadiationII. Atomic SpectraIII. Energy LevelsIV. Sublevels and OrbitalsV. Orbital DiagramsVI. Electron Configurations

What is the electromagnetic spectrum?

How do waves travel? How are energy, frequency and wavelength related?

What are the relative sizes of the waves in the electromagnetic spectrum?

Fig. 11-1, p. 310

Example – Electromagnetic Spectrum

• Using violet, green, and orange, which one is the most energetic?

A. Violet

B. Green

C. Orange

D. All of the above

E. None of the above

Example – Electromagnetic Spectrum

• Order the following in increasing wavelength: x-rays, ultraviolet light, FM radiowaves, and microwaves

A. X-rays < UV light < FM radiowaves < microwaves

B. X-rays < UV light < microwaves < FM radiowaves

C. FM radiowaves < microwaves < X-rays < UV light

D. FM radiowaves < microwaves < UV light < X-rays

E. None of the above

Experiment 1

– Hydrogen (H2) purple-blue

– Neon (Ne) red-orange– Helium (He) yellow-pink– Argon (Ar) lavender– Xenon (Xe) blue

What happens when an elemental gas in a cathode ray tube is exposed to electricity?

Experiment 2• What happens when a white light is shown

through a prism? -- rainbow• A prism separates light of different

wavelength, each color represents a different wavelength.

Experiment 3• What happens when colored light from a

gas discharge tube is shown through a prism? -----distinct bands of color (light).

• http://jersey.uoregon.edu/vlab/elements/Elements.html

What is the atomic spectrum of Barium?

How are the electrons distributed in the Bohr model of the atom?

How are the spectra produced?

Does the amount of energy absorbed matter?

When electrons drop from a higher level to the first level, second level, and third level, photons of ultraviolet light, visible light, and infrared are emitted (not to scale).

What happens in the hydrogen spectrum?

What is does it mean to be quantized?

How are the Bohr model and the Quantum model different?

Fig. 11-10, p. 316

How do electrons go into orbitals?

What is an s orbitals?

• ·   spherical in shape

Electron density map Representation of volume of orbital

How does the size of an s orbital change as

the energy level increases?

What is a p orbital?

• ·   dumbbell shaped• ·   three different spatial orientations

What is a d orbital?4 leaf clover shape and a dumbbell with a doughnut

5 different orientations

What is an f orbital?Complex shapes

7 different orientations

How has the model of the atom changed over time?

Example – Electron Configuration

• What is the electron configuration of C?

A. 1s2 2s2 2p2

B. 1s2 1p4

C. 2s2 2p2

D. 1s6

E. None of the above

Example – Electron Configuration

• What element has an electron configuration of 1s2 2s2 2p6 3s1?

Expanded Periodic Tablen 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

i 1A 8A

1 1 2

H 2A 3A 4A 5A 6A 7A He

2 3 4 5 6 7 8 9 10

Li Be B C N O F Ne

3 11 12 13 14 15 16 17 18

Na Mg 3B 4B 5B 6B 7B i 8B i 1B 2B Al Si P S Cl Ar

4 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr

5 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe

6 55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

7 87 88 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 104 105 105 107 108 109 110 111 112 114 116

Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt  Ds Rg Cn Fl Lv

s orbital, the energy level = n Electron Filling Order:p orbital, the energy level = n 1s 2s2p 3s3p 4s3d4p 5s4d5p 6s5d4f6p 7s6d5f7p

d orbital, the energy level = n - 1

f orbital, the energy level = n - 2

Phosphorous

Example – Electron Configuration

• What is the electron configuration of vanadium, V?

A. 1s2 2s2 2p6 3s2 3p6 4s2 4d3

B. 1s2 2s2 2p6 3s2 3p6 4s5

C. 1s2 2s2 2p6 3s3 3p6 4s2 3d2

D. 1s2 2s2 2p6 3s2 3p6 4s2 3d3

E. None of the above

Example – Electron Configuration

• How many core electrons does aluminum have?

A. 2

B. 3

C. 4

D. 6

E. 10

Example – Electron Configuration

• How many valence electrons does aluminum have?

A. 2

B. 3

C. 4

D. 6

E. 10

Example – Electron Configuration

• Write the core notation for Pb.

A. [Xe] 6s2 6p2

B. 6s2 5d10 4f14 6p2

C. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d10 4f14 6p2

D. [Xe] 6s2 5d10 4f14 6p2

E. [Hg] 6p2

Example – Electron Configuration

• Write the core notation for Pb2+.

A. [Xe] 5d10 4f14 6p2

B. [Xe] 6s2

C. 6s2 5d10 4f14

D. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d10 4f14 6p2

E. [Xe] 6s2 5d10 4f14 6p2

Example – Electron Configuration

• Write the core notation for the oxide ion.

A. [Ne]

B. 1s2 2s2 2p6 3s2 3p6

C. [He] 3s2 3p6

D. [He] 3s2 3p4

E. A and C