Periodic Table E Config
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The document discusses the organization and structure of the periodic table. It explains that the periodic table is arranged by increasing atomic number and that new rows are added as elements exhibit repeating properties in each column. It then discusses various models that were developed to explain the organization and placement of electrons in atoms, including the Bohr model, quantum mechanical model, electron orbitals, and electron configurations.
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Atomic orbitals are mathematical functions that describe the probability of finding an electron around an atom's nucleus. They are dependent on the values of four quantum numbers: principal, azimuthal, magnetic, and spin. Each atomic orbital can hold a maximum of two electrons with opposite spin. The number and type of atomic orbitals in each energy level depends on the principal quantum number n. Lower energy levels like s and p orbitals fill first before higher energy d and f orbitals. Electrons arrange themselves in atomic orbitals from lowest to highest energy to achieve the most stable configuration.
Orbitals hl
The document discusses orbitals and quantum numbers. It introduces the four quantum numbers - principal (n), azimuthal (l), magnetic (ml), and spin (ms) - that describe an electron's location and properties. The classical view of electrons orbiting the nucleus like planets gave way to the modern atomic model where electrons exist as probabilistic wave functions within orbitals. Orbitals are regions of high probability of finding an electron and come in s, p, d, and f shapes depending on the quantum numbers. Electron configurations use these orbitals to describe the arrangement of electrons in atoms and predict properties.
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This document provides an overview of the quantum mechanical model of the atom. It discusses key concepts like the development of atomic models, electron configuration, quantum numbers, electron orbitals, and energy levels. Some key points:
- The quantum mechanical model describes the probable locations of electrons in an atom and how they can have discrete energy levels. It improved upon earlier planetary and Bohr models.
- Electrons occupy specific orbitals and energy levels denoted by quantum numbers like principal and azimuthal quantum numbers.
- Electron configuration notation specifies the distribution of electrons across orbitals based on Aufbau's principle and other rules.
- Transitions between energy levels explain the emission or absorption of photons and thus the colors
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The document discusses the development of atomic models from Dalton to Bohr and beyond. It describes Rutherford's discovery of the nucleus and Bohr's model of electrons in fixed orbits around the nucleus. Later, the quantum mechanical model was developed, restricting electrons to specific energy levels rather than exact orbits. This modern model determines the probability of finding electrons in different locations around the nucleus.
Electrons in atoms
The document discusses the historical development of atomic models from Dalton to Bohr and beyond. It introduces John Dalton's early model of atoms as indivisible particles with no internal structure in 1863. Later models incorporated the discoveries of the electron by J.J. Thomson in 1897 and the nuclear structure of atoms by Ernest Rutherford in 1911. Niels Bohr's 1913 model proposed that electrons orbit the nucleus in fixed, quantized energy levels. This laid the foundations for understanding atomic emission spectra and the quantum mechanical model that later replaced Bohr's model.
Electron configuration cheat sheet
This document provides a summary of key concepts for electron configuration in high school chemistry, including:
1) Electrons fill subshells according to the aufbau principle to achieve lowest energy, with Hund's rule specifying that electrons occupy each orbital singly before pairing up.
2) The four subshells are s, p, d, and f, with set numbers of orbitals and maximum electrons in each. Valence electrons are in the outermost shell.
3) Electron configuration can be written using boxes and arrows, spectroscopic notation, or noble gas notation, with examples provided.
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Periodic Table E Config
- 1. ORGANIZATION OF THE PERIODIC TABLE November 2 nd , 3 rd & 4th, 2009
- 3. Circular
- 4. Long Form
- 5. Spiral
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- 7. Layers
- 8. Which one do you like the best?
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