Exercise 1
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The document shows the electronic configuration, valence electrons, and group number of several elements (Na, Mg, Al, Si, P, S, Cl). It fills in this information step-by-step to illustrate that all the elements belong to period 3, having their outermost quantum shell (valence shell) as principal quantum number 3. The valence electrons are calculated as the total electrons in the outermost shell.
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![Exercise 1
Elements Na Mg Al Si P S Cl
Electronic [Ne]
config. 3s1
Valence
electrons
Group No.](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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The document shows the electronic configuration, valence electrons, and group number of several elements (Na, Mg, Al, Si, P, S, Cl). It fills in this information step-by-step to illustrate that all the elements belong to period 3, having their outermost quantum shell (valence shell) as principal quantum number 3. The valence electrons are calculated as the total electrons in the outermost shell.
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The document discusses the thermal stability of group II nitrates. It explains that the polarization of the nitrate ion's electron cloud by a group II cation weakens the nitrate ion's bonds. Down the group, as the size of the cation increases and its charge density and polarizing power decreases, the decomposition temperature of group II nitrates increases and their thermal stability increases.
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Group II nitrates become polarized when the nitrate ions are placed next to the Group II cation, causing the cation to attract the delocalized electrons of the nitrate ion. This polarization increases the covalent character of the bonds in the nitrate ion and weakens the bonds. When heated, the weakened bonds in the polarized nitrate ions can break, causing the Group II nitrates to decompose. Down the Group II series, the decreasing polarizing power of the larger cations results in less polarization and weaker bonds in the nitrate ions, leading to higher decomposition temperatures and greater thermal stability for the nitrates.
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Group II nitrates become polarized when the nitrate ions are placed next to the Group II cation, causing the cation to attract the delocalized electrons of the nitrate ion. This polarization increases the covalent character of the bonds in the nitrate ion and weakens the bonds. When heated, the weakened bonds in the polarized nitrate ions can break, causing the Group II nitrates to decompose. Down the Group II series, the decreasing polarizing power of the larger cations results in less polarization and weakening of the nitrate ion bonds, leading to increased thermal stability and higher decomposition temperatures of the Group II nitrates.
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EAN rule.pptx
The Effective Atomic Number (EAN) rule states that transition metal complexes are stable when the EAN of the metal ion plus its ligands equals the atomic number of an inert gas. The EAN is calculated using the formula EAN = (Z - n) + 2(CN), where Z is the metal's atomic number, n is the charge on the metal ion, and CN is the coordination number. Several examples are provided to demonstrate complexes that do and do not obey the EAN rule and their relative stabilities. However, the EAN rule has limitations and does not always predict stability, as other factors also influence complex stability.
Echon (electron configuration)
The document provides an overview of electron configuration, which is the arrangement of electrons in an atom. It explains the key concepts of principal quantum number (n), sublevels (s, p, d, f), orbitals, the Aufbau principle, Pauli exclusion principle, Hund's rule, and how to write out the electron configuration for different elements. Examples are given for elements such as hydrogen, helium, lithium, carbon, nitrogen, fluorine, aluminum, argon, iron, and lanthanum.
E Configs2.ppt
This document discusses electron configurations and principles including:
1) The Aufbau principle which states that electrons fill orbitals from lowest to highest energy levels.
2) Hund's rule which states that electrons fill orbitals singly before pairing up.
3) The Pauli exclusion principle which states that no two electrons in an atom can have the same set of four quantum numbers and that paired electrons must have opposite spins.
Chapter 7 schrodinger2003
In 1934, Schrödinger lectured at Princeton University and was offered a permanent position, but he did not accept it. The document then provides an agenda for a lecture on Schrödinger and topics in quantum theory, including his famous cat experiment, quantum numbers, and principles like Hund's rule and the Pauli exclusion principle. It concludes by mentioning seeing Dr. Poget after class and that much of modern knowledge is based on quantum theory foundations.
09. classification2 (1)
This document provides information on the classification of elements and various periodic properties like atomic size, ionization energy, electron affinity and electronegativity. It discusses the trends in these properties across periods and groups and exceptions to trends. It also explains concepts like ionic size, isoelectronic species, ionization energies, electron affinities, Pauling and Mulliken scales of electronegativity and valency. Sample problems are provided at the end to test the understanding of these concepts.
Merge sort and quick sort
The document discusses different sorting algorithms including merge sort and quicksort. Merge sort has a divide and conquer approach where an array is divided into halves and the halves are merged back together in sorted order. This results in a runtime of O(n log n). Quicksort uses a partitioning approach, choosing a pivot element and partitioning the array into subarrays of elements less than or greater than the pivot. In the best case, this partitions the array in half at each step, resulting in a runtime of O(n log n). In the average case, the runtime is also O(n log n). In the worst case, the array is already sorted, resulting in unbalanced partitions and a quadratic runtime of O(n^2
E configs2
This document provides information about electron configurations and orbital notation. It begins by explaining the basic principle that electrons occupy the lowest available energy levels. It then demonstrates how to write electron configurations using spdf notation and orbital box diagrams for hydrogen and helium. The document provides examples of determining electron configurations for neon and oxygen. It also discusses the Aufbau principle, Hund's rule, and Pauli exclusion principle for filling atomic orbitals. Finally, it demonstrates shorthand notation for writing electron configurations and identifies the valence electrons for several elements.
Econfigs2 150602233044-lva1-app6891
This document provides information about electron configurations and orbital notation. It begins by explaining the basic principle that electrons occupy the lowest available energy levels. It then shows examples of writing electron configurations using spdf notation and orbital box notation for hydrogen and helium. The document provides rules for filling orbitals, including the Aufbau principle, Hund's rule, and the Pauli exclusion principle. It gives examples of writing configurations for various elements like neon, oxygen, phosphorus, and arsenic. It also discusses shorthand notation, valence electrons, and identifying pseudo noble gas cores.
Unit 4 2 electron configurations
The document discusses electron configurations and how electrons occupy different energy levels and sublevels in atoms. It introduces the concept that each energy level can hold a maximum number of electrons according to the formula 2n2, where n is the energy level. It then explains that within each energy level there are sublevels that electrons can occupy, labeled s, p, d, f etc. The number of electrons in each sublevel is also limited. Finally, it describes how the periodic table can be labeled to indicate the order in which sublevels fill up with electrons, known as the Aufbau principle, allowing electron configurations to be written for different elements.
Quantum Numbers
This document discusses quantum numbers and their role in describing the size, shape, and orientation of atomic orbitals. It explains that there are four quantum numbers - principal, angular, magnetic, and spin. The principal quantum number determines the electron shell or energy level, while the angular and magnetic quantum numbers further specify the subshell and orbital within that subshell. The spin quantum number refers to the spin of the electron. Factors that influence ionization energy such as atomic radius, nuclear charge, and electron shielding are also summarized.
SLATER’S RULE.pdf
Slater's rules provide a method to calculate the effective nuclear charge (Zeff) experienced by electrons in atoms and ions. The rules account for shielding of the nuclear charge by inner electrons. Zeff is calculated as the nuclear charge (Z) minus the total shielding (S). S is the sum of shielding values assigned based on orbital type and number of electrons. Comparing Zeff values explains trends like orbital filling order and which electrons are lost in cation formation. However, Slater grouped s and p orbitals together, which is incorrect as s orbitals penetrate the nucleus more than p orbitals.
Shell Model
This document discusses the shell model of nuclear structure and properties. It explains that the ground state of even-even nuclei have spin parity of 0+ due to paired nucleons resulting in total angular momentum of 0. Spin and parity of other nuclei are determined by the orbital angular momentum and spin of the unpaired nucleon(s). Excited nuclear states occur when a nucleon is promoted to an higher orbital with characteristic spin and parity.
Atomic Structure.pptx
This document discusses atomic structure and properties related to electrons and subatomic particles. It begins by defining the atom and its main components: protons, neutrons, and electrons. It then discusses isotopes and the behavior of subatomic particles in electric fields. The document goes on to explain electronic configuration, ionization energy, and factors that influence ionization energy such as atomic radius, nuclear charge, and shielding effects. Trends in ionization energy across periods and down groups in the periodic table are also summarized.
03b electronic structure of atoms
This document provides information about the electronic structure of atoms, including electron configurations and distribution of electrons in different atomic shells and orbitals. It defines shells and orbitals, and explains that electrons fill up lower energy shells and orbitals first according to the Aufbau principle. Tables provide the maximum number of electrons in each shell and the types of orbitals in each shell. Diagrams illustrate orbital shapes and energy level sequences. Examples of electronic configurations of the first 18 elements are given in both orbital and noble gas notation. An exercise section tests understanding of concepts covered.
Chapter 8
This document discusses periodic trends in atomic and ionic properties, including:
- Atomic and ionic radii decrease across a period as effective nuclear charge increases. Radii increase down a group as principal quantum number increases.
- Ionization energies generally increase across a period as it becomes more difficult to remove electrons. Exceptions include group 2A and 5A having higher energies than 3A and 6A respectively within periods.
- Cations have smaller radii than their parent atoms as electrons are removed. Anions have larger radii as more electrons are gained. Isotectronic ions with more protons have smaller radii.
Quantum 2.pptx
The document provides an opening prayer for a science class. It thanks God for the new day and asks for blessings on the students as they study, including wisdom and an inquiring mind. It also asks God to hear their prayer and bless the class in Jesus' name. The document then reviews concepts about electron configurations, including the Aufbau principle, Hund's rule, Pauli exclusion principle, and assigning quantum numbers. Examples are provided for writing configurations of nitrogen, sodium, oxygen, lithium, and bromine. An orbital diagram assignment is given before a closing prayer.
CHEM-101E - 2nd Week_Questions.pptx
1) a) Group 15, Period 3
b) Group 6, Period 4
c) Group 2, Period 5
d) Group 3, Period 6
2) 32
3) 5
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Exercise 1
- 1. Exercise 1 Elements Na Mg Al Si P S Cl Electronic config. Valence electrons Group No.
- 2. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] config. 3s1 Valence electrons Group No.
- 3. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] config. 3s1 Valence 1 electrons Group No.
- 4. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] config. 3s1 Valence 1 electrons Group No. 1
- 5. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] config. 3s1 3s2 Valence 1 electrons Group No. 1
- 6. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] config. 3s1 3s2 Valence 1 2 electrons Group No. 1
- 7. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] config. 3s1 3s2 Valence 1 2 electrons Group No. 1 2
- 8. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 Valence 1 2 2+1=3 electrons Group No. 1 2 3
- 9. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 3s23p2 Valence 1 2 2+1=3 2+2=4 electrons Group No. 1 2 3 4
- 10. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 3s23p2 3s23p3 Valence 1 2 2+1=3 2+2=4 2+3=5 electrons Group No. 1 2 3 4 5
- 11. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 3s23p2 3s23p3 3s23p4 Valence 1 2 2+1=3 2+2=4 2+3=5 2+4=6 electrons Group No. 1 2 3 4 5 6
- 12. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] [Ne] [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 3s23p2 3s23p3 3s23p4 3s23p5 Valence 1 2 2+1=3 2+2=4 2+3=5 2+4=6 2+5=7 electrons Group No. 1 2 3 4 5 6 7
- 13. Exercise 1 Elements Na Mg Al Si P S Cl Electronic [Ne] [Ne] [Ne] [Ne] [Ne] [Ne] [Ne] config. 3s1 3s2 3s23p1 3s23p2 3s23p3 3s23p4 3s23p5 Valence 1 2 2+1=3 2+2=4 2+3=5 2+4=6 2+5=7 electrons Group No. 1 2 3 4 5 6 7 Outermost quantum shell = 3 the principal quantum number of the valence shell is 3 all the elements in this period belong to Period 3