Make a neutral Beryllium atom by adding protons, neutrons and electrons. Now, what would you do to make a

Chemistry

1 answer:

Alenkinab [10]3 years ago

3 0

Answer:

4 protons, 5 neutrons, 4 electrons to have the neutral Be atom

the only way to make a negative Be is to have more than 4 electrons

Explanation:

Make a neutral Beryllium atom by adding protons, neutrons and electrons. Now, what would you do to make a

beryllium atom with a negative charge?

Be has an atomic number of 4, an atomic mass 9

its atomic number tells us it has 4 protons, with a +4 charge

its atomic mass = neutrons + protons, so it has 5 neutrons with no charge

its neutral atom will have 4 electrons each with a negative charge to balance the +4 total proton harge.

4 protons, 5 neutrons, 4 electrons to have the neutral Be atom

to make a negative Be species, it still must have an atomic number of 4,

or it is not Beryllium

so the only way to make a negative Be is to have more than 4 electrons

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What substance would you add to KF(aq) to form a buffer solution? View Available Hint(s) What substance would you add to to form

AnnyKZ [126]

<h3>Answer</h3>

<h3>Explanation</h3>

A buffer solution contains <em>a weak acid</em> and<em> its conjugate base</em>. The two species shall have a similar concentration in the solution. It's also possible for <em>a weak base</em> and <em>its conjugate acid</em> to form a buffer solution.

The KF solution already contains large number of $\text{F}^{-}$ ions. The objective is to thus find its conjugate acid or base.

$\text{F}^{-}$ contains no proton $\text{H}^{+}$ and is unlikely to be a conjugate acid. Assuming that $\text{F}^{-}$ is a conjugate base. Adding one proton to $\text{F}^{-}$ would produce its conjugate acid.

$\text{H}^{+} \; (aq) + \text{F}^{-} \; (aq) \rightleftharpoons \text{HF}\; (aq)$

Therefore $\text{HF}$ is the conjugate acid of $\text{F}^{-}$ . $\text{HF}$ happens to be a weak acid. As a result, combining $\text{F}^{-}$ with $\text{HF}$ would produce a solution with large number of both the weak acid and its conjugate base, which is a buffer solution by definition.