The Brønsted-Lowry base in the given reaction is NH₂⁻. The correct option is the fourth option NH2−
To determine which is the Brønsted-Lowry base in the given reaction:
NH2−+CH3OH→NH3+CH3O−
First, we will write the equation for the reaction properly
The equation is:
NH₂⁻ + CH₃OH → NH₃ + CH₃O⁻
Now, to determine which among the species in the above reaction is the Brønsted-Lowry base, we will start by defining what a <em>Brønsted-Lowry base</em><em> </em>is.
A Brønsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the H⁺.
In simple terms, a Brønsted-Lowry base is a proton acceptor.
In the above reaction, NH₂⁻ is the species that is capable of accepting a proton and it has a lone pair of electrons to bond to the H⁺.
∴ NH₂⁻ is the Brønsted-Lowry base in the reaction
Hence, the Brønsted-Lowry base in the given reaction is NH₂⁻. The correct option is the fourth option NH2−
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Answer:
Central-metal oxidation state: +2
Coordination number: 6
Overall charge: -2
Explanation:
In the ion complex:
Na₂[Cr(NH₃)₂(NCS)₄]
The central-metal is Cr, the ligands are NH₃ and NCS.
The NH₃ is a neutral ligand, while NCS is an anionic ligand with -1 in charge.
The overall charge of the complex is:
2Na⁺ + [Cr(NH₃)₂(NCS)₄]⁻² → <em>-2</em>
As NCS gives -1 in charge and there are four NCS, The Cr must be in <em>+2</em> of oxidation state to give an overall charge of -2.
As Cr is bonded to 2 NH₃ and 4 NCS, the coordination number is 2+4 = <em>6</em>
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The answer will be 180.156 g/mol
False the definition is an attractive but unintelligent man.
The correct answer is B) isotope, 16
The periodic table shows only data about the most common isotopes of the elements, and the atomic mass is the sum of protons and neutrons. Other oxygen isotopes would have different masses