Consider the following neutral electron configurations in which 'n' has a constant value. Which configuration would belong to the element with the most negative electron affinity, E-ea?

a) ns^2

b) ns^2 np^2

c) ns^2 np^5

d) ns^2 np^6

would the answer be "d"??? (as in, it would be a noble gas with a p^6, and then have a more negative e- affinity???)

  1. 👍
  2. 👎
  3. 👁
  1. If it is a noble gas, it has no affinity to attract an additional electron. I would examine the affintity of c) (as Fluorine, chlorine ).

    1. 👍
    2. 👎
  2. Unless I am out of date or misunderstood the question I thought that all electron affinities were shown as positive values. Those ending np^5 (e.g fluorine or chlorine) have the highest electron affinities.

    1. 👍
    2. 👎
  3. The electron affinity is defined as the amount of energy ABSORBED when an electron is added to an isolated gaseous atom to form an ion with a 1- charge. The convention is to assign a positive value when energy is absorbed and a negative value when energy is released. For example, Be(g) + e + 241 kJ ==> Be^-(g) EA = +231 kJ/mol. (endothermic)

    Cl(g) + e ==> Cl^-(g) + 348 kJ/mol EA = -348 kJ/mol (exothermic)

    I think c is the answer.

    1. 👍
    2. 👎
  4. The answer is c) ns^2 np^5

    I know this because in addition to the explanations posted, above I just did this for my chemistry homework. I'm guessing you also have Mastering Chemistry?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Which of the following electron configurations of neutral atoms represent excited states? ( ) [Xe]6s24f1 ( ) 2s2 ( ) 1s22s22p63s23p63d2 ( ) [Ar]4s23d3 ( ) [Kr]5s14d5

  2. chemistry

    Identify the neutral element represented by this excited-state electron configuration, then write the ground-state electron configuration for that element. Excited State: 1s2 2s2 2p2 3s1 Element Symbol: ? Ground State: ?

  3. AP Chemistry

    Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. If the configuration is a noble gas, enter the noble gas in

  4. chem

    6. What is wrong with the following electron configurations for atoms in their ground states? a) 1s^2 2s^2 3s^1 b) (Ne) 2s^2 2p^3 c) (Ne) 3s^2 3d^5

  1. chemistry

    Which neutral atoms have the following electron configurations in either a ground state or excited state? Enter the name or symbol. [Ar]4s23d3 - I know that this is Vanadium [Xe]6s24f1 - I thought that this was Lu but it counts it

  2. Configuration

    What is the electronic configuration of carbide C-4? Thought it was 1s2 2s2 sp2. Thanks from Sheryl C is atomic number 6. Electronic configuration of the neutral atom is 1s2, 2s2, 2p2. The carbide ion, C^-4, has four more

  3. Chemistry

    Metals lose electrons under certain conditions to attain a noble-gas electron configuration. How many electrons must be lost by the element Ca? Is it 2 e^-? Which noble-gas electron configuration is attained in this process? argon

  4. Chemistry

    Which of the following electron configurations of neutral atoms represent excited states? [Xe]6s^2 4f^1 [Ar]4s^2 3d^3 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 [Kr]5s^1 4d^5 2s^2 Which neutral atoms have the following electron configurations?

  1. Chemistry

    Electron configuration for phosphorus is 1s2 2s2 2p6 3s2 3p3. So the number of electron must be 15 , right ? But , what if m = 1 ? Does it effect the number of electron ?

  2. Chem

    Hi everyone, I'm having problems with effective nuclear charge. Regarding these problems. Calculate Zeff for a valence electron in an oxygen atom. and Calculate Zeff for the 4s electron in a copper atom, . and Calculate Zeff for a

  3. Chemistry

    Given the following three electron configurations: 1s2 2s2 2p5 How many core electrons does this element have? A. 4 B. 5 C. 9 D. 2

  4. Chemistry

    Which group of elements is characterized by an s2p3 configuration? What is the electron configuration of group 15? thanks

You can view more similar questions or ask a new question.