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- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Elements_Organized_by_Block/2_p-Block_Elements/Group_18%3A_The_Noble_Gases/Z010_Chemistry_of_Neon_(Z10)Neon is a member of the group 18 elements, the noble gases. This element is most commonly known through its use in glow lamps and advertising signs emitting a distinctive bright orange-red color.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/04%3A_Atomic_Structure/4.06%3A_Dalton's_Atomic_TheoryThis page outlines the evolution of scientific thought on matter's composition, highlighting the debates preceding the 19th century. It emphasizes John Dalton's advancements in atomic theory, which po...This page outlines the evolution of scientific thought on matter's composition, highlighting the debates preceding the 19th century. It emphasizes John Dalton's advancements in atomic theory, which posited that matter is made of indivisible atoms and that atoms of the same element are identical. Dalton's 1804 theory established foundational principles for modern chemistry, although some aspects, like atomic indivisibility, have been updated.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.13%3A_Conversion_of_(K_textsp)_to_SolubilityThis page outlines the purification of drinking water, emphasizing the removal of heavy metals through the formation of insoluble compounds using carbonates and sulfates. It details the calculation of...This page outlines the purification of drinking water, emphasizing the removal of heavy metals through the formation of insoluble compounds using carbonates and sulfates. It details the calculation of molar solubility via solubility product constants (\(K_\text{sp}\)), including the creation of an ICE table to find ion concentrations and deriving molar solubility. The final conversion from molar solubility to solubility is also addressed.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.12%3A_Determining_Empirical_FormulasThis page explains how to determine empirical formulas in chemistry, especially for organic compounds. It defines empirical formulas as the simplest whole-number ratios of elements and distinguishes t...This page explains how to determine empirical formulas in chemistry, especially for organic compounds. It defines empirical formulas as the simplest whole-number ratios of elements and distinguishes them from molecular formulas. The process involves elemental analysis, including converting percentages to grams, calculating moles, and finding whole-number ratios. An example of iron and oxygen is given, resulting in the formula \(\ce{Fe_2O_3}\).
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/04%3A_Atomic_Structure/4.05%3A_Mass_Ratio_CalculationThis page explains the law of multiple proportions in chemistry, illustrating it with examples of copper and chlorine compounds that have different copper-to-chlorine mass ratios. It details the calcu...This page explains the law of multiple proportions in chemistry, illustrating it with examples of copper and chlorine compounds that have different copper-to-chlorine mass ratios. It details the calculations for comparing copper quantities that combine with a fixed mass of chlorine, emphasizing the significance of these ratios in understanding compound composition and encouraging further exploration of mass ratios and molecular formulas.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.01%3A_Avogadro's_NumberThis page explains Avogadro's number, \(6.02 \times 10^{23}\), which quantifies the number of representative particles in a mole, allowing chemists to measure atoms and molecules. It discusses the mol...This page explains Avogadro's number, \(6.02 \times 10^{23}\), which quantifies the number of representative particles in a mole, allowing chemists to measure atoms and molecules. It discusses the mole as the SI unit for substance amount, with representative particles being atoms for elements and molecules for compounds. Additionally, it mentions National Mole Day, celebrating this key chemistry concept.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/02%3A_Matter_and_Change/2.15%3A_Chemical_Symbols_and_FormulasThis page highlights how chess players use specialized symbols for game documentation, similar to how chemists use chemical symbols for elements and compounds. Chemical symbols, typically made up of o...This page highlights how chess players use specialized symbols for game documentation, similar to how chemists use chemical symbols for elements and compounds. Chemical symbols, typically made up of one or two letters, often derive from English or Latin, while chemical formulas represent the composition and proportions of elements in compounds (e.g., H₂O for water). Grasping these symbols is essential for success in both chess and chemistry.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.16%3A_Standard_Heat_of_FormationThis page discusses the Hope diamond, valued at $350 million, and compares it to graphite, which is much cheaper. It explains that the differences between these two forms of carbon arise from their di...This page discusses the Hope diamond, valued at $350 million, and compares it to graphite, which is much cheaper. It explains that the differences between these two forms of carbon arise from their distinct organizational structures and formation conditions. It also defines standard heat of formation (\( \Delta H^\text{o}_\text{f} \)), describing it as the enthalpy change involved in forming a mole of a compound from its elements at specified standard conditions.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/02%3A_Matter_and_Change/2.02%3A_Pure_SubstancesThis page defines substances in chemistry as pure materials with uniform compositions that can't be separated. It provides examples like silver and acetylsalicylic acid, noting that aspirin is a mixtu...This page defines substances in chemistry as pure materials with uniform compositions that can't be separated. It provides examples like silver and acetylsalicylic acid, noting that aspirin is a mixture. Substances may exist in solid, liquid, or gas forms based on temperature, and the text emphasizes the necessity of using pure substances in chemical reactions for reliable outcomes.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/06%3A_The_Periodic_Table/6.21%3A_Periodic_Trends-_ElectronegativityThis page explains electronegativity, defining it as an atom's ability to attract electrons. It notes that electronegativity increases across periods and decreases down groups, highlighting fluorine a...This page explains electronegativity, defining it as an atom's ability to attract electrons. It notes that electronegativity increases across periods and decreases down groups, highlighting fluorine as the most electronegative element. Metals generally have low electronegativities due to their tendency to lose electrons, while nonmetals gain electrons, leading to higher values.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/10%3A_The_Mole/10.10%3A_Percent_CompositionThis page explains how to calculate the percent composition of compounds using mass data and chemical formulas, highlighting the mass percentage of each element. It provides examples, such as peanut b...This page explains how to calculate the percent composition of compounds using mass data and chemical formulas, highlighting the mass percentage of each element. It provides examples, such as peanut butter and dichlorine heptoxide, to demonstrate the calculation method. Additionally, it discusses the conservation of stained glass and techniques for preserving historical artifacts.
