Questions tagged [alkaline-earth-metals]

For questions about the alkaline earth metals (group 2), their compounds, and their physical and chemical properties.

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Existence of (anti)perovskite (Cs+)3(Pt2-)(Au-) and (Cs+)(Ba 2+)(Au-)3

I know that there are oxide-aurides of cesium and rubidium from wikipedia and https://www.researchgate.net/publication/243821351_Cs3AuO_the_First_Ternary_Oxide_with_Anionic_Gold and that the component ...
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Solubility of alkali and alkaline earth metal carbonates

The solubility of alkali metal carbonates increase down the group, while those of alkaline earth metals decrease down the group. We can explain the decrease in solubility of alkaline earth metal ...
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Effect of magnesium hydroxide MgOH formation in water on pH (Why more basic?)

Elemental magnesium reacts in (hot) water to form magnesium hydroxide and hydrogen gas: $$\ce{Mg_{(s)} + H2O_{(g)} -> Mg(OH)2_{(s)} + H2_{(g)}}$$ As indicated for example by phenolphthalein turning ...
Selenimoon's user avatar
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Heating effect of alkaline earth metal chloride

Why does $\ce{MgCl2.8H2O}$ undergoes internal hydrolysis? $$\ce{MgCl2.8H2O(s) ->[\Delta]MgO(s) + H2O + HCl}$$ while Calcium, Strontium, and barium undergoes dehydration and form anhydrous chloride. ...
Ayush Aggarwal's user avatar
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Titanium-free catalysts to decrease decomposition temperature of magnesium hydride

Magnesium hydride $(\ce{MgH2})$ is a metal hydride with a relatively stable structure, at least compared to other metal hydrides. Magnesium hydride splits at around 300 °C into magnesium and hydrogen. ...
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Why did The Action Lab say that solutes that don't dissolve as well in hot water are exothermic?

Somewhat recently, The Action Lab made a video called "Why does this powder only dissolve in cold water?" , saying the powder which was calcium acetate dissolves in cold water better than in ...
Bruh Moments's user avatar
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Are carboxylic anhydrides in graphene oxides considered adsorption sites for metals? If so, are they more or less reactive than carboxylic acids?

The literature abundantly addresses the fact that carboxylic acids present in graphene oxides act as efficient adsorption sites for metals in aqueous solutions (e.g., HE et al., 2021; ZHAO et al., ...
Nathan Vinicius's user avatar
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What is the structure of hydrated beryllium chloride [closed]

Is there water of crystallization or does water act as ligand? Also Be2+ is smaller than Li 2+ then why Li2+ has only 2 water molecules as ligands
Ritil's user avatar
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Comparison of enthalpy change for the dissolution of alkaline earth metal oxides

Compare the heat liberated per mole for the following reactions: $\ce{MgO + H2O -> Mg(OH)2}$ $\ce{CaO + H2O -> Ca(OH)2}$ $\ce{SrO + H2O -> Sr(OH)2}$ $\ce{BaO + H2O -> Ba(OH)2}$ Data for ...
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Ease of reaction of hydrogen with alkali and alkaline earth metals

The ease of reaction of group 1 metals with hydrogen decreases as we go down the group. But why lithium requires high temperature than sodium, potassium and rubidium? What is exactly "ease of ...
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What is the relation between strength of a base and the thermal stability of its salts?

In Concise Inorganic Chemistry, $5^{th}$ edition, by JD Lee, while discussing oxides and hydroxides of Group $2$ metals, it has been stated that: The increase in basic strength is illustrated by the ...
Ritam_Dasgupta's user avatar
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What is the solubility trend of alkaline earth metal fluorides?

I was going through JD Lee and I found certain contradictory statements. First: With most compounds, on descending the group, the hydration energy decreases more rapidly than the lattice energy: ...
Siddhant's user avatar
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Why is Electron Gain Enthalpy of only Be and Mg positive, in group 2?

While going through my book, I came across the following observation: $\Delta H_{eg1}$ is positive for Be and Mg Where $\Delta H_{eg1}$ is the first electron gain enthalpy. It seemed quite ...
Prajwal Tiwari's user avatar
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Why is strontium(II) ion bigger than krypton atom?

$\ce{Sr^2+}$ is exactly the same as $\ce{Kr}$, in terms of electrons and orbitals. The only difference between the two, is that $\ce{Sr^2+}$ has a couple of extra protons in the nucleus (and probably ...
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Significance of p functions in compounds of the lighter alkaline and alkaline earth metals [closed]

It is often said that lithium follows the duet rule instead of the octet rule, unlike the more "usual" main-group elements. My question is the following: Does this hold for $\ce{Be, Na}$ and ...
Kanghun Kim's user avatar
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Why don't beryllium and magnesium dissolve in ammonia?

From my textbook: The [alkali and] alkaline earth metals dissolve in liquid ammonia to give deep blue solutions forming ammoniated ions. $$\text{M}+(x+y)\text{NH}_3 \rightarrow [\text{M}(\text{NH}_3)...
Ray Bradbury's user avatar
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Molecular geometry of BaH2 according to VSEPR theory

I am asked to predict the correct molecular geometry of $\ce{BaH2}$ according to VSEPR theory. I assumed that it is linear due to barium being an alkaline earth metal and therefore not having any lone ...
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Why aren't elements with two valence shell electrons stable?

We all know that hydrogen becomes stable by completing duplet and helium is stable since its valence shell has completed the duplet Still, other elements don't behave like that. I want to know that ...
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Hydrolysis of alkali and alkaline earth metals

Which of the following cations are not hydrolysed in aqueous solution? 1) $\ce{Mg^2+}$ 2) $\ce{Ca^2+}$ 3) $\ce{Na+}$ 4) $\ce{K+}$ I thought nothing would undergo hydrolysis, so all the options would ...
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Is Magnesium Oxide alkali [closed]

Given that Magnesium Hydroxide is an alkali, can we say Magnesium Oxide is an alkali since dissolving Magnesium Oxide in water can produce Magnesium Hydroxide?
Diamond Science's user avatar
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Trends in solubility of group 2 nitrates

In my lab report, we are required to explain the trends in solubility of group 2 salts, going down the group. I had explained all of the trends except one, group 2 nitrates. The following is the data ...
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Hydration, Coordinate Bonding, and Reduction Potential in Groups 1 and 2 Elements [closed]

Whenever an alkali metal such as Lithium is hydrated/solvated, coordinate bonding occurs and it is the high hydration enthalpy of lithium which makes it the strongest reducing agent in aqueous ...
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Why does Mg(HCO₃)₂ on heating gives Mg(OH)₂? [duplicate]

Normally, bicarbonates on heating forms carbonates. Why does Mg not give this too? In a reference book I am referring to, it is given that it is due to high solubility product of Mg(OH)₂ compared to ...
user226375's user avatar
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Unusual oxidation numbers for alkaline earth metals?

Are there compound of alkaline earth elements showing unusual oxidation numbers? For the sake of the question, every oxidation number different from +2 counts as unusual, most exciting would be ...
Sir Cornflakes's user avatar
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What is reason of stability of metal (Sr and Ba) peroxides?

While studying inorganic chemistry I came across the following chemical equation. $$\ce{M + Air\left(1/2O2 + N2\right) ->[Δ] MO ->[\text{Excess}~O2] MO2 (Stable) + M3N2}$$ $$\ce{M} = \ce{Sr, ...
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Apparent contradiction in the name of group 2 elements

From my understanding (I might be very wrong), the "earth" in alkaline earth metals means non-metallic, insoluble in water, and resistant to heating, therefore the oxides and hydroxides of ...
user3602727's user avatar
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Why are bicarbonates of alkaline earth metals stable only in aqueous solution?

Numerous internet sources (1, 2, 3, etc.) state this fact, including a Wiley publication "Alkaline Earth Metals: Inorganic Chemistry - William S. Rees Jr" (DOI: 10.1002/0470862106.ia005) on page 9: ...
Gaurang Tandon's user avatar
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Why can't beryllium react with hydrogen gas directly to give hydride?

I read in a textbook that all alkali metal and alkaline earth metal can react with hydrogen directly to give hydride except for beryllium. I want to know the reason why because I know that $\ce{BeH2}$ ...
Koushik Sahu's user avatar
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2 answers
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Are lithium bicarbonate and magnesium bicarbonate both soluble in water?

Are lithium bicarbonate and​ magnesium bicarbonate both soluble in water? Source: JEE Mains 2017 (National Level Examination of India) Please do cite a reputed source along with your answer. ...
iBoy's user avatar
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3 answers
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Is beryllium an alkaline earth metal?

For context: I got a question asking, "Which of the following alkaline earth metals do not give flame colour?". I quickly marked $\ce{Be}$ and $\ce{Mg}$ and got negative marks. The following is a ...
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7 votes
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Why does magnesium oxide not react with water?

There is a question in my textbook which asks "which of the reactions are not possible to occur". The right answer is $\ce{MgO + H2O}$ and my chemistry teacher confirmed it. Why is that so? I thought ...
Angelina's user avatar
19 votes
2 answers
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Why does the solubility of group II hydroxides increase and the solubility of sulfates decrease down the group?

I know that solubility of alkaline earth metal hydroxides increases down the group and solubility of alkaline earth metal sulfates decreases down the group. What is the reason for these trends?
Yomal Amarathunge's user avatar