Thompsons Experiment Rutherfords Experiment Explanation Diffraction the change
![Thompson’s Experiment Thompson’s Experiment](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-1.jpg)
![Rutherford’s Experiment: Rutherford’s Experiment:](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-2.jpg)
![Explanation Explanation](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-3.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-4.jpg)
![• Diffraction: - the change in direction of a wave as it passes • Diffraction: - the change in direction of a wave as it passes](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-5.jpg)
![The Wave Nature of Light as electromagnetic waves: polarization, interference, diffraction, reflection, and refraction The Wave Nature of Light as electromagnetic waves: polarization, interference, diffraction, reflection, and refraction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-6.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-7.jpg)
![Electromagnetic Spectrum Electromagnetic Spectrum](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-8.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-9.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-10.jpg)
![Atomic Line Spectra (Line Emission Spectra) Hydrogen has the simplest atomic emission spectrum ( Atomic Line Spectra (Line Emission Spectra) Hydrogen has the simplest atomic emission spectrum (](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-11.jpg)
![The Spectrum of Atomic Hydrogen Compare the absorption spectrum to the emission spectrum of The Spectrum of Atomic Hydrogen Compare the absorption spectrum to the emission spectrum of](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-12.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-13.jpg)
![Light as Particles Light as Particles](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-14.jpg)
![Bohr Atom Bohr Atom](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-15.jpg)
![Hidrojen İçin Bohr Atom Modeli (1913) Elektronlar belirli yörüngelerde bulunabilirler Hidrojen İçin Bohr Atom Modeli (1913) Elektronlar belirli yörüngelerde bulunabilirler](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-16.jpg)
![Bohr Model of Hydrogen Atoms Quantized energy levels – total energy for each level Bohr Model of Hydrogen Atoms Quantized energy levels – total energy for each level](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-17.jpg)
![E = 0 e. V n=3 n=2 Energy Paschen Series (IR) Balmer Series (visible) E = 0 e. V n=3 n=2 Energy Paschen Series (IR) Balmer Series (visible)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-18.jpg)
![Line Spectra The Lyman and Balmer series of lines in the hydrogen spectrum correspond Line Spectra The Lyman and Balmer series of lines in the hydrogen spectrum correspond](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-19.jpg)
![Electron in the Hydrogen Atom Electron in the Hydrogen Atom](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-20.jpg)
![• Elektronlar gerçekten de çekirdek etrafında belirli yörüngelerde mi dönerler? • Bunu tespit • Elektronlar gerçekten de çekirdek etrafında belirli yörüngelerde mi dönerler? • Bunu tespit](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-21.jpg)
![Elektronun konumu ve momentumunun ölçülmesi • Işının her çarpışında elektronun da konumu değişir. Bu Elektronun konumu ve momentumunun ölçülmesi • Işının her çarpışında elektronun da konumu değişir. Bu](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-22.jpg)
![Heisenberg, Werner 1901– 76, Alman Fizikçi 1932 Nobel Fizik Ödülü Eğer bir taneciğin nerede Heisenberg, Werner 1901– 76, Alman Fizikçi 1932 Nobel Fizik Ödülü Eğer bir taneciğin nerede](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-23.jpg)
![Peki elektronlar nerede ve nasıl hareket ediyorlar? Peki elektronlar nerede ve nasıl hareket ediyorlar?](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-24.jpg)
![Erwin Schrödinger 1927 yılında • Elektronlar, zamanlarının büyük bir çoğunluğunu orbital denen bölgelerde geçirirler. Erwin Schrödinger 1927 yılında • Elektronlar, zamanlarının büyük bir çoğunluğunu orbital denen bölgelerde geçirirler.](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-25.jpg)
![Atomik Orbitaller s p d f Şekli küresel halter karışık Orbital sayısı 1 3 Atomik Orbitaller s p d f Şekli küresel halter karışık Orbital sayısı 1 3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-26.jpg)
![Quantum Mechanics Quantum Mechanics](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-27.jpg)
![The First Shell • The innermost shell (1) only contains an s orbital. 1 The First Shell • The innermost shell (1) only contains an s orbital. 1](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-28.jpg)
![Atomic Orbitals, s-type Atomic Orbitals, s-type](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-29.jpg)
![S orbitalleri S orbitalleri](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-30.jpg)
![Atomic Structure Atomic Structure](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-31.jpg)
![Quantum Mechanics Quantum Mechanics](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-32.jpg)
![Electron Configuration in p Orbital Electron Configuration in p Orbital](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-33.jpg)
![Atomic Orbitals, ptype Atomic Orbitals, ptype](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-34.jpg)
![p Orbitals • Rather than being a sphere, the "p" orbital has two lobes p Orbitals • Rather than being a sphere, the "p" orbital has two lobes](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-35.jpg)
![The Second Shell • The second shell contains an s type orbital as well The Second Shell • The second shell contains an s type orbital as well](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-36.jpg)
![Atomic Orbitals, d-type Atomic Orbitals, d-type](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-37.jpg)
![d Orbitals • There are 5 types of d orbitals. Four of the five d Orbitals • There are 5 types of d orbitals. Four of the five](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-38.jpg)
![The Third Shell • The 3 rd shell has: – 1 s orbital (3 The Third Shell • The 3 rd shell has: – 1 s orbital (3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-39.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-40.jpg)
![f orbitals • f-orbitals have 6 lobes and are very challenging to envision Image f orbitals • f-orbitals have 6 lobes and are very challenging to envision Image](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-41.jpg)
![The First Two Shells Picture from and more info on How Atoms Work The First Two Shells Picture from and more info on How Atoms Work](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-42.jpg)
![The Fouth Shell • The 4 th shell has: – 1 s orbital (4 The Fouth Shell • The 4 th shell has: – 1 s orbital (4](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-43.jpg)
![Principle quantum number n = 1, 2, 3, …. . describes orbital size and Principle quantum number n = 1, 2, 3, …. . describes orbital size and](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-44.jpg)
![Write a valid set of quantum numbers for each of the following sub-shells: (a) Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-45.jpg)
![Write a valid set of quantum numbers for each of the following sub-shells: (a) Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-46.jpg)
![Write a valid set of quantum numbers for each of the following sub-shells: (a) Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-47.jpg)
![How many orbitals in a subshell? l = 0, 1 s 1 l = How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-48.jpg)
![How many orbitals in a subshell? l = 0, 1 s 1 l = How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-49.jpg)
![How many orbitals in a subshell? l = 0, 1 s 1 l = How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-50.jpg)
![How many orbitals in a subshell? l = 0, 1 s 1 l = How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-51.jpg)
![Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-52.jpg)
![Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-53.jpg)
![Orbital Energies 3 dxy 3 dxz 3 dyz 3 dx 2 -y 2 3 Orbital Energies 3 dxy 3 dxz 3 dyz 3 dx 2 -y 2 3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-54.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-55.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-56.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-57.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-58.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-59.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-60.jpg)
![Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-61.jpg)
![Hydrogen 1 s 2 s 2 p 3 s 3 p 3 d 4 Hydrogen 1 s 2 s 2 p 3 s 3 p 3 d 4](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-62.jpg)
![1 s H 1 s 1 He 1 s 2 Li 1 s 2, 1 s H 1 s 1 He 1 s 2 Li 1 s 2,](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-63.jpg)
![H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-64.jpg)
![H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-65.jpg)
![H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-66.jpg)
![H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-67.jpg)
![H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-68.jpg)
![K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-69.jpg)
![K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-70.jpg)
![K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-71.jpg)
![Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-72.jpg)
![Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-73.jpg)
![Modern Theories of the Atom - Summary n Wave-particle duality of light and matter Modern Theories of the Atom - Summary n Wave-particle duality of light and matter](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-74.jpg)
- Slides: 74
![Thompsons Experiment Thompson’s Experiment](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-1.jpg)
Thompson’s Experiment
![Rutherfords Experiment Rutherford’s Experiment:](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-2.jpg)
Rutherford’s Experiment:
![Explanation Explanation](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-3.jpg)
Explanation
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-4.jpg)
![Diffraction the change in direction of a wave as it passes • Diffraction: - the change in direction of a wave as it passes](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-5.jpg)
• Diffraction: - the change in direction of a wave as it passes the edge of an object
![The Wave Nature of Light as electromagnetic waves polarization interference diffraction reflection and refraction The Wave Nature of Light as electromagnetic waves: polarization, interference, diffraction, reflection, and refraction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-6.jpg)
The Wave Nature of Light as electromagnetic waves: polarization, interference, diffraction, reflection, and refraction
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-7.jpg)
![Electromagnetic Spectrum Electromagnetic Spectrum](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-8.jpg)
Electromagnetic Spectrum
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-9.jpg)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-10.jpg)
![Atomic Line Spectra Line Emission Spectra Hydrogen has the simplest atomic emission spectrum Atomic Line Spectra (Line Emission Spectra) Hydrogen has the simplest atomic emission spectrum (](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-11.jpg)
Atomic Line Spectra (Line Emission Spectra) Hydrogen has the simplest atomic emission spectrum ( 1880 s).
![The Spectrum of Atomic Hydrogen Compare the absorption spectrum to the emission spectrum of The Spectrum of Atomic Hydrogen Compare the absorption spectrum to the emission spectrum of](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-12.jpg)
The Spectrum of Atomic Hydrogen Compare the absorption spectrum to the emission spectrum of H If we pass light from a continuous source (eg from a hot object) through a substance, then the continuous spectrum has some of the wavelengths removed! -- absorption spectrum
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-13.jpg)
![Light as Particles Light as Particles](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-14.jpg)
Light as Particles
![Bohr Atom Bohr Atom](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-15.jpg)
Bohr Atom
![Hidrojen İçin Bohr Atom Modeli 1913 Elektronlar belirli yörüngelerde bulunabilirler Hidrojen İçin Bohr Atom Modeli (1913) Elektronlar belirli yörüngelerde bulunabilirler](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-16.jpg)
Hidrojen İçin Bohr Atom Modeli (1913) Elektronlar belirli yörüngelerde bulunabilirler
![Bohr Model of Hydrogen Atoms Quantized energy levels total energy for each level Bohr Model of Hydrogen Atoms Quantized energy levels – total energy for each level](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-17.jpg)
Bohr Model of Hydrogen Atoms Quantized energy levels – total energy for each level is the sum of the kinetic energy of the electron plus its potential energy. Electrons do not radiate while in their orbits, but do when they move from one orbit to another.
![E 0 e V n3 n2 Energy Paschen Series IR Balmer Series visible E = 0 e. V n=3 n=2 Energy Paschen Series (IR) Balmer Series (visible)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-18.jpg)
E = 0 e. V n=3 n=2 Energy Paschen Series (IR) Balmer Series (visible) Lyman Series (ultraviolet) E 1 = -13. 6 e. V n=1 Lyman Balmer Paschen Example Data
![Line Spectra The Lyman and Balmer series of lines in the hydrogen spectrum correspond Line Spectra The Lyman and Balmer series of lines in the hydrogen spectrum correspond](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-19.jpg)
Line Spectra The Lyman and Balmer series of lines in the hydrogen spectrum correspond to transitions that the electrons make between higher and lower energy levels. The Bohr model only has one quantum number, n, which represents the energy level. http: //www. walter-fendt. de/ph 11 e/bohrh. htm
![Electron in the Hydrogen Atom Electron in the Hydrogen Atom](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-20.jpg)
Electron in the Hydrogen Atom
![Elektronlar gerçekten de çekirdek etrafında belirli yörüngelerde mi dönerler Bunu tespit • Elektronlar gerçekten de çekirdek etrafında belirli yörüngelerde mi dönerler? • Bunu tespit](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-21.jpg)
• Elektronlar gerçekten de çekirdek etrafında belirli yörüngelerde mi dönerler? • Bunu tespit etmek mümkün mü?
![Elektronun konumu ve momentumunun ölçülmesi Işının her çarpışında elektronun da konumu değişir Bu Elektronun konumu ve momentumunun ölçülmesi • Işının her çarpışında elektronun da konumu değişir. Bu](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-22.jpg)
Elektronun konumu ve momentumunun ölçülmesi • Işının her çarpışında elektronun da konumu değişir. Bu sebeple ışıkla bir elektronunun konumu ve hızı hassas bir şekilde belirlenemez.
![Heisenberg Werner 1901 76 Alman Fizikçi 1932 Nobel Fizik Ödülü Eğer bir taneciğin nerede Heisenberg, Werner 1901– 76, Alman Fizikçi 1932 Nobel Fizik Ödülü Eğer bir taneciğin nerede](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-23.jpg)
Heisenberg, Werner 1901– 76, Alman Fizikçi 1932 Nobel Fizik Ödülü Eğer bir taneciğin nerede olduğunu kesin olarak biliyorsak, aynı anda taneciğin nereden geldiğini ve nereye gittiğini kesin şekilde bilemeyiz.
![Peki elektronlar nerede ve nasıl hareket ediyorlar Peki elektronlar nerede ve nasıl hareket ediyorlar?](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-24.jpg)
Peki elektronlar nerede ve nasıl hareket ediyorlar?
![Erwin Schrödinger 1927 yılında Elektronlar zamanlarının büyük bir çoğunluğunu orbital denen bölgelerde geçirirler Erwin Schrödinger 1927 yılında • Elektronlar, zamanlarının büyük bir çoğunluğunu orbital denen bölgelerde geçirirler.](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-25.jpg)
Erwin Schrödinger 1927 yılında • Elektronlar, zamanlarının büyük bir çoğunluğunu orbital denen bölgelerde geçirirler. • Değişik şekillerde orbitaller mevcuttur.
![Atomik Orbitaller s p d f Şekli küresel halter karışık Orbital sayısı 1 3 Atomik Orbitaller s p d f Şekli küresel halter karışık Orbital sayısı 1 3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-26.jpg)
Atomik Orbitaller s p d f Şekli küresel halter karışık Orbital sayısı 1 3 5 7 Herbir orbital 2 elektron içerir e sayısı 2 6 10 14
![Quantum Mechanics Quantum Mechanics](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-27.jpg)
Quantum Mechanics
![The First Shell The innermost shell 1 only contains an s orbital 1 The First Shell • The innermost shell (1) only contains an s orbital. 1](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-28.jpg)
The First Shell • The innermost shell (1) only contains an s orbital. 1 s
![Atomic Orbitals stype Atomic Orbitals, s-type](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-29.jpg)
Atomic Orbitals, s-type
![S orbitalleri S orbitalleri](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-30.jpg)
S orbitalleri
![Atomic Structure Atomic Structure](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-31.jpg)
Atomic Structure
![Quantum Mechanics Quantum Mechanics](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-32.jpg)
Quantum Mechanics
![Electron Configuration in p Orbital Electron Configuration in p Orbital](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-33.jpg)
Electron Configuration in p Orbital
![Atomic Orbitals ptype Atomic Orbitals, ptype](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-34.jpg)
Atomic Orbitals, ptype
![p Orbitals Rather than being a sphere the p orbital has two lobes p Orbitals • Rather than being a sphere, the "p" orbital has two lobes](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-35.jpg)
p Orbitals • Rather than being a sphere, the "p" orbital has two lobes pointed in opposite direction away from the nucleus. • One p orbital points along each the x, y, and z axis. • There are three p orbtitals in every shell except the first.
![The Second Shell The second shell contains an s type orbital as well The Second Shell • The second shell contains an s type orbital as well](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-36.jpg)
The Second Shell • The second shell contains an s type orbital as well as a new kind of orbital called a "p" orbital. 2 py 2 s 2 pz 2 px
![Atomic Orbitals dtype Atomic Orbitals, d-type](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-37.jpg)
Atomic Orbitals, d-type
![d Orbitals There are 5 types of d orbitals Four of the five d Orbitals • There are 5 types of d orbitals. Four of the five](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-38.jpg)
d Orbitals • There are 5 types of d orbitals. Four of the five have four lobes at 90 o to one another. The fifth looks like a donut around a p-orbital Image from: HMChem
![The Third Shell The 3 rd shell has 1 s orbital 3 The Third Shell • The 3 rd shell has: – 1 s orbital (3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-39.jpg)
The Third Shell • The 3 rd shell has: – 1 s orbital (3 s) – 3 p orbitals (3 px, 3 py, 3 pz) – 5 d orbitals (3 dxy, 3 dyz, 3 dx 2 -y 2, 3 dz 2)
![](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-40.jpg)
![f orbitals forbitals have 6 lobes and are very challenging to envision Image f orbitals • f-orbitals have 6 lobes and are very challenging to envision Image](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-41.jpg)
f orbitals • f-orbitals have 6 lobes and are very challenging to envision Image from: HMChem
![The First Two Shells Picture from and more info on How Atoms Work The First Two Shells Picture from and more info on How Atoms Work](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-42.jpg)
The First Two Shells Picture from and more info on How Atoms Work
![The Fouth Shell The 4 th shell has 1 s orbital 4 The Fouth Shell • The 4 th shell has: – 1 s orbital (4](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-43.jpg)
The Fouth Shell • The 4 th shell has: – 1 s orbital (4 s) – 3 p orbitals (4 px, 4 py, 4 pz) – 5 d orbitals (4 dxy, 4 dyz, 4 dx 2 -y 2, 4 dz 2) – 7 f orbitals
![Principle quantum number n 1 2 3 describes orbital size and Principle quantum number n = 1, 2, 3, …. . describes orbital size and](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-44.jpg)
Principle quantum number n = 1, 2, 3, …. . describes orbital size and energy Angular momentum quantum number l = 0 to n-1 describes orbital shape Magnetic quantum number ml = l, l-1…-l describes orientation in space of the orbital relative to the other orbitals in the atom Spin quantum number ms = +1/2 or -1/2 describes the direction of spin of the e- on its axis Pauli Exclusion Principle: "no two electrons in an atom can have the same set of quantum numbers", or, only two electrons (of opposite spin) per orbital.
![Write a valid set of quantum numbers for each of the following subshells a Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-45.jpg)
Write a valid set of quantum numbers for each of the following sub-shells: (a) 2 s n = 2, l = 0, ms = - 1/2 n = 2, l = 0, ms = ± 1/2 2 combinations
![Write a valid set of quantum numbers for each of the following subshells a Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-46.jpg)
Write a valid set of quantum numbers for each of the following sub-shells: (a) 2 s n = 2, l = 0, ms = - 1/2 n = 2, l = 0, ms = ± 1/2 2 combinations (b) 2 p n = 2, l = 1, ml = -1, ms = - 1/2 n = 2, l = 1, ml = -1, 0 or 1, ms = ± 1/2 6 combinations
![Write a valid set of quantum numbers for each of the following subshells a Write a valid set of quantum numbers for each of the following sub-shells: (a)](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-47.jpg)
Write a valid set of quantum numbers for each of the following sub-shells: (a) 2 s n = 2, l = 0, ms = - 1/2 n = 2, l = 0, ms = ± 1/2 2 combinations (b) 2 p n = 2, l = 1, ml = -1, ms = - 1/2 n = 2, l = 1, ml = -1, 0 or 1, ms = ± 1/2 6 combinations (c) 3 d n = 3, l = 2, ml = -2, ms = - 1/2 n = 3, l = 2, ml = -2, -1, 0, 1, or 2, ms = ± 1/2 10 combinations
![How many orbitals in a subshell l 0 1 s 1 l How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-48.jpg)
How many orbitals in a subshell? l = 0, 1 s 1 l = 1, p x, p y, p z 3 l = 2, dxy, , dxz, , dyz , , dx 2 -y 2, dz 2 5
![How many orbitals in a subshell l 0 1 s 1 l How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-49.jpg)
How many orbitals in a subshell? l = 0, 1 s 1 l = 1, p x, p y, p z 3 l = 2, dxy, , dxz, , dyz , , dx 2 -y 2, dz 2 5 2 l + 1 orbitals per subshell
![How many orbitals in a subshell l 0 1 s 1 l How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-50.jpg)
How many orbitals in a subshell? l = 0, 1 s 1 l = 1, p x, p y, p z 3 l = 2, dxy, , dxz, , dyz , , dx 2 -y 2, dz 2 5 2 l + 1 orbitals per subshell How many orbitals in a shell? n = 1, 1 s 1 n = 2, 2 s, 2 px, 2 py, 2 pz 4 n = 3, 3 s, 3 px, 3 py, 3 pz, 3 dxy, , 3 dxz, , 3 dyz , , 3 dx 2 -y 2, 3 dz 2 9
![How many orbitals in a subshell l 0 1 s 1 l How many orbitals in a subshell? l = 0, 1 s 1 l =](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-51.jpg)
How many orbitals in a subshell? l = 0, 1 s 1 l = 1, p x, p y, p z 3 l = 2, dxy, , dxz, , dyz , , dx 2 -y 2, dz 2 5 2 l + 1 orbitals per subshell How many orbitals in a shell? n = 1, 1 s 1 n = 2, 2 s, 2 px, 2 py, 2 pz 4 n = 3, 3 s, 3 px, 3 py, 3 pz, 3 dxy, , 3 dxz, , 3 dyz , , 3 dx 2 -y 2, 3 dz 2 9 n 2 orbitals per principal quantum level
![Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-52.jpg)
Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction between e- and proton
![Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-53.jpg)
Hydrogen atoml all orbitals within a shell have the same energy l electrostatic interaction between e- and proton Multi-electron atomsthe energy level of an orbital depends not only on the shell but also on the subshell l l electrostatic interactions between e- and proton and other e-
![Orbital Energies 3 dxy 3 dxz 3 dyz 3 dx 2 y 2 3 Orbital Energies 3 dxy 3 dxz 3 dyz 3 dx 2 -y 2 3](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-54.jpg)
Orbital Energies 3 dxy 3 dxz 3 dyz 3 dx 2 -y 2 3 px 3 py 3 pz 3 s Energy 2 px 2 py 2 s 1 s 2 pz 3 dz 2
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-55.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-56.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle)
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-57.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle) 3. Try to attain maximum number of unpaired e- spins in a given sub-shell (Hund's Rule)
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-58.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle) 3. Try to attain maximum number of unpaired e- spins in a given sub-shell (Hund's Rule) H (Z = 1) 1 s 1 2 s 2 p Energy 1 s
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-59.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle) 3. Try to attain maximum number of unpaired e- spins in a given sub-shell (Hund's Rule) N (Z = 7) 1 s 2, 2 p 3, 2 p Energy 2 s 1 s
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-60.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle) 3. Try to attain maximum number of unpaired e- spins in a given sub-shell (Hund's Rule) B (Z = 5) 1 s 2, 2 p 1 2 p Energy 2 s 1 s
![Electronic Configuration Fillingin of Atomic Orbitals Rules 1 Pauli Principle 2 Fill in es Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-61.jpg)
Electronic Configuration: Filling-in of Atomic Orbitals Rules: 1. Pauli Principle 2. Fill in e-'s from lowest energy orbital upwards (Aufbau Principle) 3. Try to attain maximum number of unpaired e- spins in a given sub-shell (Hund's Rule) F (Z = 9) 1 s 2, 2 p 5 2 p Energy 2 s 1 s
![Hydrogen 1 s 2 s 2 p 3 s 3 p 3 d 4 Hydrogen 1 s 2 s 2 p 3 s 3 p 3 d 4](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-62.jpg)
Hydrogen 1 s 2 s 2 p 3 s 3 p 3 d 4 s 4 p 4 d 4 f 2 s 3 s 4 s 2 p 3 p 4 p 3 d 4 d Multi-electron atoms 1 s 5 s
![1 s H 1 s 1 He 1 s 2 Li 1 s 2 1 s H 1 s 1 He 1 s 2 Li 1 s 2,](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-63.jpg)
1 s H 1 s 1 He 1 s 2 Li 1 s 2, 2 s 1 Be 1 s 2, 2 s 2 B 1 s 2, 2 px 1 C 1 s 2, 2 px 1, 2 py 1 N 1 s 2, 2 px 1, 2 py 1, 2 pz 1 O 1 s 2, 2 px 2, 2 py 1, 2 pz 1 F 1 s 2, 2 px 2, 2 py 2, 2 pz 1 Ne 1 s 2, 2 px 2, 2 py 2, 2 pz 2 2 s 2 px 2 py 2 pz
![H 1 s 1 He 1 s 2 Li He 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-64.jpg)
H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be [He], 2 s 2
![H 1 s 1 He 1 s 2 Li He 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-65.jpg)
H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be [He], 2 s 2 B [He], 2 s 2, 2 p 1 Ne [He], 2 s 2, 2 p 6 Na [He], 2 s 2, 2 p 6, 3 s 1 [Ne], 3 s 1
![H 1 s 1 He 1 s 2 Li He 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-66.jpg)
H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be [He], 2 s 2 B [He], 2 s 2, 2 p 1 Ne [He], 2 s 2, 2 p 6 Na [He], 2 s 2, 2 p 6, 3 s 1 [Ne], 3 s 1 Mg [He], 2 s 2, 2 p 6, 3 s 2 [Ne], 3 s 2 Al [Ne], 3 s 2, 3 p 1 Si [Ne], 3 s 2, 3 p 2
![H 1 s 1 He 1 s 2 Li He 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-67.jpg)
H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be [He], 2 s 2 B [He], 2 s 2, 2 p 1 Ne [He], 2 s 2, 2 p 6 Na [He], 2 s 2, 2 p 6, 3 s 1 [Ne], 3 s 1 Mg [He], 2 s 2, 2 p 6, 3 s 2 [Ne], 3 s 2 Al [Ne], 3 s 2, 3 p 1 Si [Ne], 3 s 2, 3 p 2 P [Ne], 3 s 2, 3 p 3 S [Ne], 3 s 2, 3 p 4 Cl [Ne], 3 s 2, 3 p 5 Ar [Ne], 3 s 2, 3 p 6
![H 1 s 1 He 1 s 2 Li He 2 s 1 Be H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-68.jpg)
H 1 s 1 He 1 s 2 Li [He], 2 s 1 Be [He], 2 s 2 B [He], 2 s 2, 2 p 1 Ne [He], 2 s 2, 2 p 6 Na [He], 2 s 2, 2 p 6, 3 s 1 [Ne], 3 s 1 Mg [He], 2 s 2, 2 p 6, 3 s 2 [Ne], 3 s 2 Al [Ne], 3 s 2, 3 p 1 Si [Ne], 3 s 2, 3 p 2 P [Ne], 3 s 2, 3 p 3 S [Ne], 3 s 2, 3 p 4 Cl [Ne], 3 s 2, 3 p 5 Ar [Ne], 3 s 2, 3 p 6 l l outermost shell - valence shell most loosely held electron and are the most important in determining an element’s properties
![K Ar 4 s 1 Ca Ar 4 s 2 Sc Ar 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-69.jpg)
K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s 2, 3 d 1 Ti [Ar], 4 s 2, 3 d 2
![K Ar 4 s 1 Ca Ar 4 s 2 Sc Ar 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-70.jpg)
K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s 2, 3 d 1 Ca [Ar], 4 s 2, 3 d 2 Zn [Ar], 4 s 2, 3 d 10 Ga [Ar], 4 s 2, 3 d 10, 3 p 1 Kr [Ar], 4 s 2, 3 d 10, 3 p 6
![K Ar 4 s 1 Ca Ar 4 s 2 Sc Ar 4 s K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-71.jpg)
K [Ar], 4 s 1 Ca [Ar], 4 s 2 Sc [Ar], 4 s 2, 3 d 1 Ca [Ar], 4 s 2, 3 d 2 Zn [Ar], 4 s 2, 3 d 10 Ga [Ar], 4 s 2, 3 d 10, 3 p 1 Kr [Ar], 4 s 2, 3 d 10, 3 p 6 Anomalous electron configurations d 5 and d 10 are lower in energy than expected Cr [Ar], 4 s 1, 3 d 5 not [Ar], 4 s 2, 3 d 4 Cu [Ar], 4 s 1, 3 d 10 not [Ar], 4 s 2, 3 d 9
![Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-72.jpg)
Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the donor and placed into the lowest unoccupied orbital of the acceptor (placed according to the Aufbau principle)
![Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-73.jpg)
Electron Configuration of Ions Electrons lost from the highest energy occupied orbital of the donor and placed into the lowest unoccupied orbital of the acceptor (placed according to the Aufbau principle) Examples: Na [Ne], 3 s 1 Na+ [Ne] + e- Cl [Ne], 3 s 2, 3 p 5 + e- Cl- [Ne], 3 s 2, 3 p 6 Mg [Ne], 3 s 2 Mg 2+ [Ne] O [He], 2 s 2, 2 p 4 O 2 - [He], 2 s 2, 2 p 6
![Modern Theories of the Atom Summary n Waveparticle duality of light and matter Modern Theories of the Atom - Summary n Wave-particle duality of light and matter](https://slidetodoc.com/presentation_image_h2/45290ab3b9009795c1fde2c0189729c9/image-74.jpg)
Modern Theories of the Atom - Summary n Wave-particle duality of light and matter n Bohr theory n Quantum (wave) mechanical model n Orbital shapes and energies n Quantum numbers n Electronic configuration in atoms
How many orbitals are in the n=3 level
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