Questions: The least acidic species in the following is a. CH4 b. NH3 c. HBr d. CH3OH

The least acidic species in the following is a. CH4 b. NH3 c. HBr d. CH3OH
Transcript text: The least acidic species in the following is $\qquad$ a. CH 4 b. $\mathrm{NH3}$ c. HBr d.CH3OH
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Solution

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Solution Steps

Step 1: Identify the Nature of Each Species

To determine the least acidic species, we need to consider the acidity of each compound. Acidity is often related to the ability of a compound to donate a proton (H⁺).

  • CH₄ (methane): Methane is a hydrocarbon and is generally considered non-acidic because it does not readily donate protons.
  • NH₃ (ammonia): Ammonia is a weak base and can accept protons, but it is not typically acidic.
  • HBr (hydrobromic acid): HBr is a strong acid and readily donates protons.
  • CH₃OH (methanol): Methanol is a very weak acid, but it can donate a proton from the hydroxyl group.
Step 2: Compare the Acidity
  • CH₄ is the least acidic because it is a non-polar molecule with no tendency to donate protons.
  • NH₃ is more basic than acidic.
  • HBr is a strong acid.
  • CH₃OH is a weak acid.

Final Answer

The least acidic species is \(\boxed{\text{CH}_4}\).

Step 1: Determine the Electronic Configuration of Na⁺

The electronic configuration of an atom or ion is determined by the distribution of electrons in its atomic orbitals.

Step 2: Consider the Neutral Sodium Atom
  • Neutral Sodium (Na): The atomic number of sodium is 11, so its electronic configuration is \(1s^2 2s^2 2p^6 3s^1\).
Step 3: Account for the Positive Charge
  • Na⁺ Ion: The Na⁺ ion has lost one electron compared to the neutral atom. Therefore, the electronic configuration of Na⁺ is \(1s^2 2s^2 2p^6\).
Final Answer

The electronic configuration of \(\mathrm{Na}^+\) is \(\boxed{1s^2 2s^2 2p^6}\).

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