The electron affinity of the atoms increases from left to right as we proceed along any row of the periodic table, but goes to 0 for the noble gases. Offer a reason for the increase going from Li to F and then decrease to zero for Ne.

The electron affinity of the atoms increases from left to right as we proceed along any row of the periodic table, but goes to 0 for the noble gases. Offer a reason for the increase going from Li to F and then decrease to zero for Ne.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter11: Atomic Theory :the Quantum Model Of The Atom

Section: Chapter Questions

Problem 109E

See similar textbooks

Related questions

Q: A. An element with the valence electron configuration 3s² would form a monatomic ion with a charge…

A: A) As we know the element with valence electronic configuration 3s2 is Magnesium (Mg) which is form…

Q: Describe and apply the periodic trends for first ionization energy. Identify which of the following…

A: The elements given are Mg, Sr, In, Br and Pb.

Q: Why do the noble gases have the lowest electron affinities?

A: The energy released when an electron is added to the outermost orbital of isolated gaseous neutral…

Q: Give the symbol of the atom with the following orbital diagram: NN 1s 2s a. b. C. 1s 2s NN 2p M 2p…

A: In the orbital diagram of an atom, we fill all the electrons present in a neutral atom. The total…

Q: a) Why does Li have a larger first ionization energy than Na? (b) The difference between the third…

A: ANSWER IS

Q: 167) Write the valence shell electron confiquration f euch of the fallowing elements, basina your…

A: The electronic configuration of the elements has to be provided.

Q: 180. Answer the following questions based on the given electron configurations, and identify the…

A: The atomic number and the name of the elements in order of left to right as mentioned in the…

Q: 2. Given their electron configurations, identify the following elements and specify in what group of…

A: 2) a) element is selenium(Se) which is in group 16 and peroid 4 B) Radium (Ra) group no 2 C)…

Q: Give the maximum number of electrons that the following can have : a. 2s , 2p= b. 3d = c. 4d =…

A: According to quantum mechanics, there are four types of quantum numbers. The electrons are filled in…

Q: Use the trends in ionization energy and electron affinity to explain why calcium fluoride has the…

A: The energy requirement associated with an atom to remove an electron from its outermost shell is…

Q: A naturally occurring fblock element, M, forms an anionic nitrate [M(NO3)6]² , M(acac)4 and an oxide…

A: Those elements of the periodic table which have their last electrons in the f-orbital are known as…

Q: Arrange the following set of ions and atoms in increasing size and explain your answer. •K*, CI, s,…

A: For the ionic or atomic size there is a trend in the perioduc table. As we go from top to bottom the…

Q: Explain how irregularities in the periodic trends for electron affinity can be related to electron…

A: Electron affinity is the energy released or gained when an electron is added to the gaseous…

Q: The first four successive ionization energies of an element X in kJ mol' are 900, 1758 14905 and…

A: Solution Ionisation energy It is defined as the energy required to remove the electron from…

Q: How does the effective nuclear charge experienced by the valence electrons of an atom vary going…

A: Going from left to right in a period, effective nuclear charge (Zeff) approaches to Z. That means…

Q: 1. Something is unusual about the 4s and 3d orbitals. What do you notice about the order in which…

A: According to the company guidelines, we have to answer only the first three subparts. So, please…

Q: Which is larger, the H 1s orbital or the Li 1s orbital? Why? Which has the larger radius, the H atom…

A: To find: Which is larger, the H 1s orbital or the Li 1s orbital? Why? Which has the larger radius,…

Q: Sketch the electron level n=1 through n=5. Of hydrogen atom

Q: Which element would have these quantum numbers for it's highest ground state electron: 4, 1, +1,…

A: Given Set of quantum number = 4 ,1 ,+1 ,-1/2 Name of Element =?

Q: Write the short-hand electron configuration, and give the 4 quantum numbers for the last electron…

A: Atomic number of antimony :- 51 Electronic configuration of antimony = [Kr] 4d105s25p3 Quantum…

Q: In Section 8.6, we estimated the effective nuclear charge on beryllium’s valence electrons to be…

Q: Atom W is in Period 2 and Group 2 in the periodic table. Which orbital diagram is correct for the…

A: Given: The element is in period 2 and group 2.

Q: What is the relationship between the ionization energy of an anion with a -1 charge, such as F, and…

Q: Write the short-hand electron configuration, and give the 4 quantum numbers for the last electron…

A: we have to write the electron configuration from antimony in condensed notation and the quantum…

Q: For each of the following pairs of atoms or ions, state which you expect to have the larger radius.…

Q: Explain why the ionization energy of I, S, P and C are simmilar but the electron affinity values…

A: We have to explain why the ionization energy of I, S, P and C are simmilar but the electron affinity…

Q: figuration? (c) The bars represent the relative magnitudes of the first five ionization energies of…

A: Since you have asked multiple question, we will answer the first one. If you want any specific…

Q: 6. What are the possible sets of quantum numbers for the following valence electrons? 3s² 3p¹

Q: Write the electron configuration, draw the orbital diagram, determine the distinguishing electron…

A: The atomic number of carbon is six. Carbon has six protons, six neutrons, and six electrons. The…

Q: Write ground-state electron configurations for the ions Be", P, Ca2*and Fe2*. Which do you expect…

A: We know that the ground state electronic configuration of the corresponding neutral element as…

Q: For an atom of 13Al, write its full electron configuration: 1s_ Draw a full orbital diagram (e¯s as…

Q: Describe the electron affinity (EA) of an atom (or ion)?

A: To find: Description about the electron affinity of an atom

Q: 3- Give the electron configurations for the X+2 if the atomic number for X element is 56.

Q: Which orbital type below does not exist due to wave-mechanical quantum number restrictions? 4p O 4d…

Q: If a single electron is removed from a Li atom, the resulting species is a Li+ cation, which has…

A: When we have removed one electron from Li then it will convert into lithium cation. now the nuclear…

Q: The electron affinity of sodium is lower than that of lithium, while the electron affinity of…

A: The amount of energy required to gain an electron is called electron affinity. This is calculated in…

Q: 1.34 In Fig. 1.16, identify the trends in the first ionization energies of the elements in (a)…

A: After seeing the question solving in the given parts as attached below

Q: Which is higher in energy, the 2s or 2p orbitl, in hydrogen? Is this also true for helium? Explain.

Q: Write the electron configurations for the following atoms. Do not use shorthand notation, and use…

A: The electronic configuration of the given atoms is as follows;

Q: The first five ionization energies (IE, through IE,) of a Period 6 element have the following…

Q: Given the set of quantum numbers for highest energy electrons in atom Y as shown below: (n, l, m, s)…

A: Orbital diagrams are used to represent the number of electrons, number of electron shells of an…

Q: Arrange the following elements in order of increasing (from smaller to larger) first ionization…

A: K<Ge<Si<Ar

Q: tions: Identify the element whose last electron would have the following four quantum numbers. 1. 3,…

Q: The first ionization energies of the elements bottom to the top of a group in the table. are…

A: Determine the ionization energy trend in periodic table . Period and group

Q: Write the electron configurations for the following atoms. Do not use shorthand notation, and use…

Q: In what shell do the valence electrons reside for an element in period: (a) 2; (b) 3; (c) 4; (d) 5?

A: To find: The shell in which valence electrons reside for an element in period. 2 3 4 5

Q: Write the electron configurations for the following atoms. Do not use shorthand notation, and use…

Q: Arrange the following set of ions and atoms in increasing size and explain your answer. •N, Cs, As,…

A: Atomic radii:

Q: (a) Write out the ground-state electron configuration (1s2, 2s2, ......) for the beryllium atom. (b)…

A: The electrons, protons, and neutrons are the basic constituents of an atom. They help in determining…

Question

T The electron affinity of the atoms increases from left to right as we proceed along any row of the
periodic table, but goes to 0 for the noble gases. Offer a reason for the increase going from Li to F and
then decrease to zero for Ne.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
For each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Sm or Sm3+ (b) Mg or Ca (c) I orXe (d) Ge or As (e) Sr+ or Rb
Both the electron affinity and the ionization energy of chlorine are higher than the corresponding quantities for sulfur. Explain why in terms of the electronic structure of the atoms.
Suppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.
Consider the following statement "The ionization energy for the potassium atom is negative, because when K loses an electron to become K +, it achieves a noble gas electron configuration." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the incorrect information and explain.
Cesium is used extensively in photocells and in television cameras because it has the lowest ionization energy of all the stable elements. (a) What is the maximum kinetic energy of a photoelectron ejected from cesium by 520 nm light? Note that if the wavelength of the light used to irradiate the cesium surface becomes longer than 660 nm, no photoelectrons are emitted. (b) Use the rest mass of the electron to calculate the velocity of the photoelectron in (a).
Chromium(IV) oxide is used in making magnetic recording tapes because it is paramagnetic. It can be described as a solid made up of Cr4+ and O2 . Give the electron configuration of Cr4+ in CrO2 , and determine the number of unpaired electrons on each chromium ion.
Sketch an orbital contour that is expected for an electron that has n = 3 and = 2.
onsider the following statements: “The ionization energy for the potassium atom is negative because when K loses an electron to become K+ , it achieves a noble, gas. electron configuration." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the mistaken information and explain the error.