Electron Configuration
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The document provides instructions to write the ground state and noble gas electron configurations for various elements, determine elements based on given configurations, and identify which configuration violates the Pauli exclusion principle. It asks the reader to provide the electron configurations for lithium, oxygen, calcium, sodium cation, nitrogen, and floride anion as well as identify the elements represented by several multi-electron configurations and determine which configuration violates the Pauli exclusion principle.
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Electron Configurations
Write the complete ground state electron configurations for the following:
1) lithium _______________________________________
2) oxygen _______________________________________
3) calcium _______________________________________
Write the noble gas configurations for the following:
5) sodium cation Na+
_______________________________________
6) nitrogen ______________________________________
7) floride anion F
-
_____________________________________
Determine what elements are denoted by the following electron configurations:
8) 1s22s22p63s23p4 ____________________
9) 1s22s22p63s23p64s23d104p65s1 ____________________
10) [Kr] 5s24d105p3 ____________________
11) [Xe] 6s24f145d6 ____________________
12) [Rn] 7s25f11 ____________________
Which electron configuration represents a violation of the Pauli exclusion principle?](https://image.slidesharecdn.com/quizandshow-170316102208/85/Electron-Configuration-1-320.jpg)
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The document discusses Arrhenius's theory of acids and bases. It defines acids as hydrogen-containing compounds that yield hydrogen ions (H+) in solution, and bases as compounds that yield hydroxide ions (OH-) in solution. It provides examples of common acids like hydrochloric acid and sulfuric acid, as well as bases like sodium hydroxide. It classifies acids based on the number of ionizable hydrogens they contain as mono-, di-, or triprotic. The document also discusses the properties of acids and bases and their reactions in aqueous solutions.
Bronsted lowry worksheet
This document contains a chemistry assignment asking students to identify conjugate acids and bases, Bronsted-Lowry acids and bases, and other related concepts in a series of multiple choice questions based on chemical equations. The questions cover topics like identifying the conjugate acid in chemical reactions, determining which compound is the conjugate base in a given reaction, and defining what constitutes a Bronsted-Lowry acid or base versus an Arrhenius acid or base based on whether a compound donates or accepts hydrogen ions.
Bronsted lowry acid and base
This document discusses the Brønsted-Lowry theory of acids and bases. It defines acids as proton donors and bases as proton acceptors. An acid-base pair consists of a conjugate acid and conjugate base, where the acid donates a proton to form the conjugate base, or the base accepts a proton to form the conjugate acid. Water is described as amphiprotic because it can act as both an acid and a base. Examples of acid-base reactions and identification of conjugate species are provided.
Hess's law
Hess's law states that the total enthalpy change for a reaction is independent of the pathway taken. It allows calculation of enthalpy changes that cannot be measured directly by combining thermochemical equations. The standard heat of reaction (ΔH°) can be calculated from standard heats of formation (ΔHf°) of reactants and products. Hess's law and heats of formation are useful for determining enthalpy changes that cannot be measured in the laboratory.
Hess's law
The document discusses Hess's law, which states that the heat of reaction is the same whether a chemical process occurs in one or multiple steps. Specifically:
- Hess's law allows adding together multiple chemical equations to determine the enthalpy change of the overall equation.
- Two examples are provided to demonstrate calculating the enthalpy change of an overall reaction by combining individual reaction enthalpies.
- In both examples, the individual reactions are rearranged and combined to produce the overall reaction, and the enthalpy terms are summed to find the enthalpy change of the overall reaction.
Quantum theory and the atom
The highest energy level in Bohr's model of the atom is the one that is farthest from the nucleus. According to Bohr's model, electrons can only exist at certain discrete energy levels or orbits around the nucleus, with the lowest energy level being closest to the nucleus. When an electron gains energy, it moves to a higher energy level in an "excited state". It then releases energy as a photon when it falls back to its lower "ground state". Later, the quantum mechanical model improved on Bohr's model by treating electrons as waves rather than definite orbits, better explaining experimental observations.
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