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Write a general statement that describes the periodic trend in the solubility of alkaline earth metal compounds?
The solubility of alkaline earth metal compounds generally increases down the group in the Periodic Table. This trend is particularly evident for hydroxides and sulfates, where the solubility of hydroxides increases from beryllium to barium, while sulfates show a decrease in solubility from magnesium to barium. The increase in ionic size and decrease in lattice energy as one moves down the group contribute to this trend. Overall, this results in greater solubility for heavier alkaline earth metals compared to their lighter counterparts.
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What is the solubility of a metal?
Metals are not soluble in water; the chemical reaction with water is not solubility. Metals are soluble in acids; this solubility depends on the specific metal and acid, temperature, pressure, stirring, form of the metal, etc.
What are the general solubility rules for CrO4 -2?
The chromate ion (CrO4^2-) generally follows these solubility rules: it is soluble in alkaline solutions and forms soluble compounds with alkali metals (like sodium and potassium) and ammonium ions (NH4+). However, chromates are generally insoluble with transition metals such as lead (Pb), barium (Ba), and calcium (Ca), which form insoluble chromate salts. Additionally, the solubility of chromates can be affected by the pH of the solution, as they tend to precipitate as insoluble forms in acidic conditions.
Vanadium solubility in water?
Vanadium has low solubility in water, with the solubility varying depending on its oxidation state and the presence of complexing agents. In its most common forms, such as vanadium pentoxide (V₂O₅), it exhibits very limited solubility in pure water. However, in acidic or alkaline conditions, vanadium can form soluble complexes, increasing its solubility. Generally, the solubility of vanadium is significantly lower than that of many other transition metals.
Does alkaline contain dissolved sodium hydroxide?
Alkaline solutions may contain dissolved sodium hydroxide, but not always. Alkaline substances can refer to a wide range of compounds that have a pH greater than 7, including those that do not contain sodium hydroxide.
Why are neither the alkali metals or the alkaline-earth metals found uncombined in nature?
Alkali metals and alkaline-earth metals are highly reactive and easily form compounds with elements in the environment. Consequently, they are not found in their pure form in nature. Instead, they are typically found as compounds with other elements such as oxygen or sulfur.
What trends in the solubilities of the compounds of the alkaline earth metals can be inferred?
1) NaOH : two top alkaline earth metals' solubility is decreasing as we can see from cloudy to lots of solid and two bottom metals' solubility is also decreasing in observing difference amount of solid between Sr(NO3)2 and Ba(NO3)2 2) NaCl: all of the alkaline earth metals are soluble. 3) NABr: all of the alkaline earth metals are soluble. 4) NaI: all of the alkaline earth metals are soluble. 5) Na2SO4: solubility of alkaline earth metals is decreasing from clear to solid and cloudy. 6) Na2CO3: solubility of alkaline earth metals from Mg(No3)2 to Sr(NO3)2 is decreasing and after Sr(NO3)2, solubility is increasing. 7) Na2C2O4: solubility of alkaline earth metals is decreasing from clear to solid and cloudy.
How does the solubility changes as you go to lower rows in the periodic table for alkali and alkaline earth metals?
As you move down the periodic table, the solubility of alkali metals (Group 1) generally increases due to their decreasing lattice energy and increasing hydration enthalpy, making their compounds more soluble in water. In contrast, for alkaline earth metals (Group 2), solubility trends can vary; while the solubility of some sulfates decreases down the group, most hydroxides and carbonates become less soluble. Overall, alkali metal compounds tend to be more soluble compared to those of alkaline earth metals.
What is the trend in solubility of alkaline earth metals as you move down the group on the periodic table?
The trend in solubility of alkaline earth metals increases as you move down the group on the periodic table.
What statement best describes the Alkaline-Earth metals?
Alkaline-Earth metals are found in Group 2 of the periodic table and include elements like calcium and magnesium. They are known for their high reactivity and tendency to form ionic compounds. They are typically shiny, silvery-white metals and have two valence electrons.
Why are the elements in group 2 called alkaline earth metals?
Group 2 elements are called alkaline earth metals because they form alkaline solutions when they react with water. The term "earth" indicates that these elements were found in the earth's crust, while "alkaline" describes the basic nature of the compounds they form.
Why akali metals is active base than alkaline metals from their solubility's in water?
the solubility of alkali metal bases is more than the solubility of alkaline metal bases. thus the reaction: base=metal ion + OH- occus faster. since the more the OH ions the stronger the base, alkali metal bases are stronger than alkaline metal bases
Why nitrogen form compounds with alkaline earth metal's?
why nitrogen form compound with alkaline earth metal
Is burned charcoal acidic or alkaline?
Burned charcoal is alkaline in nature. It has a high pH due to the presence of ash and other alkaline compounds resulting from the burning process.
What is the solubility of alkali metals in water?
The solubility of alkali metals in water is high. Alkali metals such as lithium, sodium, and potassium readily dissolve in water to form alkaline solutions.
Why the solubility of alkaline earth metals decrease down the group?
because down the group the cation becomes gets larger so the hydration energy decreases. so the solubility decreases
What elements is an alkaline earth metal that combines more readily with inorganic compounds than with organic compounds?
sodium
What element is an alkaline earth metal that combines more readily with inorganic compounds than with organic compounds?
Calcium
