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vova2212 [387]
3 years ago
8

Consider the addition of an electron to the following atoms from the fourth period. Rank the atoms in order from the most negati

ve to the least negative electron affinity values based on their electron configurations.
Atom or ion Electron configuration
Br 1s22s22p63s23p64s23d104p5
Ge 1s22s22p63s23p64s23d104p2
Kr 1s22s22p63s23p64s23d104p6
Chemistry
1 answer:
lesya [120]3 years ago
6 0

Answer:

Ge: [Ar] 3d10 4s2 4p2 => 6 electrons in the outer shell

Br: [Ar] 3d10 4s2 4p5 => 7 electrons in the outer shell

Kr: [Ar] 3d10 4s2 4p6 => 8 electrons in the outer shell

Explanation:

The electron affinity or propension to attract electrons is given by the electronic configuration. Remember that the most stable configuration is that were the last shell is full, i.e. it has 8 electrons.

The closer an atom is to reach the 8 electrons in the outer shell the bigger the electron affinity.

Of the three elements, Br needs only 1 electron to have 8 electrons in the outer shell, so it has the biggest electron affinity (the least negative).

Ge: needs 2 electrons to have 8 electrons in the outer shell, so it has a smaller (more negative) electron affinity than Br.

Kr, which is a noble gas, has 8 electrons and is not willing to attract more electrons at all, the it has the lowest (more negative) electron affinity of all three to the extension that really the ion is so unstable that it does not make sense to talk about a number for the electron affinity of this atom.

Read more on Brainly.com - brainly.com/question/1832586#readmore

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10.66  grams

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When a solution of an acid reacts with a solution of a base, hydrogen ions react with hydroxide ions to form?
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Determine the energy associated with an e- in hydrogen at n=2 to n=4
jeka57 [31]

Answer:

Kinetic energy of electron = -E₂ = 3.4 ev

Kinetic energy of electron = -E₄ = 0.85 ev

Explanation:

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En =  -13.6/n²

For n = 2

E₂ = -13.6 / 2²

E₂ = -13.6/4

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6 0
2 years ago
BONUS QUESTION
devlian [24]

Answer:

pH = 12.5

Explanation:

The reaction that takes place is

  • 2OH⁻(aq) + Pb⁺²(aq) → Pb(OH)₂(s)

The OH⁻ species come from the metal hydroxide of the solution, and Pb(OH)₂ is the precipitate.

Now we <u>convert 3.81 grams of Pb(OH)₂ into moles</u>, using its <em>molar mass</em>:

  • 3.81 g ÷ 241.12 g/mol = 0.0158 mol Pb(OH)₂

Now we <u>convert 0.0158 Pb(OH)₂ moles into OH⁻ moles</u>, using the <em>stoichiometric coefficients of the reaction</em>:

  • 0.0158 mol Pb(OH)₂ * \frac{2molOH^-}{1molPb(OH)_2} = 0.0316 mol OH⁻

With the given concentration (1 L), we <u>calculate [OH⁻]</u>:

  • [OH⁻] = 0.0316 mol / 1 L = 0.0316 M

Then we <u>calculate the pOH</u> of the solution:

  • pOH = - log[OH⁻] = 1.5

And finally we <u>calculate the pH</u>:

  • pH = 14 - pOH
  • pH = 12.5
6 0
2 years ago
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