1.40 Suggest explanations for the following. b. The enthalpy changes associated with the attachment of the first and second electrons to an O atom are exothermic and endothermic, respectively. c. In a Li atom In its ground state, the outer electron occupies a 2s rather than a 2p orbital.

1.40 Suggest explanations for the following. b. The enthalpy changes associated with the attachment of the first and second electrons to an O atom are exothermic and endothermic, respectively. c. In a Li atom In its ground state, the outer electron occupies a 2s rather than a 2p orbital.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 41QRT

See similar textbooks

Related questions

Q: 1. Consider the first ionization energy for two atoms: Nitrogen (N) and Oxygen (O). Which one has…

A: The correct answer is 1,1 . Nitrogen.Nitrogen has a higher ionization energy compared to oxygen.…

Q: . Use the periodic table to determine the element corresponding to each of the following electron…

A: Aπ 4s2 3d1 is electronic configuration of scandium .The chemical symbol is Sc .Kπ 5s2 is…

Q: [References) a. Write the electron configuration for Rb*. (Express your answer as a series of…

Q: What is the key distinction between sublevel energies in one-electron species, such as the H atom,…

Q: Write ground-state electron configurations for the ions O", N³, K*and Zn2*. Which do you expect will…

A: The diamagnetic nature is shown by those species which consist of all paired electrons in their…

Q: Without using the periodic table, determine the group, period, and block of an atom with the…

A: Elements are classified in periodic table based on their atomic number . Elements are classified to…

Q: Write the element symbol and charge for this monatomic ion: B.How many unpaired electrons are there…

Q: 1.1. What energy is required to liberate an electron in the n = 3 orbital of a hydrogen atom?

A: Rydberg equation is ∆E = - 2.178 × 10-18 × [1nf2 - 1ni2]

Q: Which of the following statements concerning ground state electron configurations is/are CORRECT?

Q: Which of the following electron configurations for the atom in its ground state is incorrect? A. Al:…

A: B is the incorrect Cr have electronic configuration 3d54s1 because 1 electron from 4S Excited into…

Q: 1. Which of the following represent impossible combinations of n and l? (a) 1p, (b) 4s, (c) 5f,…

A: Since you asked for multiple question and no one specified that which is solve. So only solve first…

Q: Write the electron configuration for the ground state of Sn2* (tin 2+). Use the noble gas shortcut.…

A: Electronic configuration is the arrangement of electrons in different orbitals according to the…

Q: When we first learn to write electron configurations for atoms, we use the Pauli Exclusion Principle…

A: The question you provided addresses the fundamental principles of quantum mechanics, particularly in…

Q: Tör the Sllowing atoms and ions. Use the noble gas shortcut. The answer boxes don't support special…

A: Given : We have to write the electronic configuration for the given element and ions.

Q: 1. Describe and explain the changes in ionization energies across the second row of the Periodic…

A: What the changes in ionization energies across the second row of periodic table ?

Q: Which of the following is false? A. An orbital can contain two electrons, but only if they have…

A: Points: 1.The maximum capacity of an orbital is to hold the electrons is two (2) if and only if two…

Q: Based on your observations, what is the correlation between electron configuration of an atom and…

A: In an atom, there is nucleus at the centre and electrons are revolving around it Nucleus is made up…

Q: a. Calculate the wavelength (in nm) of a photon emitted by a hydrogen atom when its electron drops…

A: Use the Rydberg formula to calculate the wavelength: 1λ= R Z2 1n12-1n22…

Q: Give the electron configurations as described below. a. core electron configuration of bismuth. (Z…

A: Electronic configuration is the distribution of electrons of an atom or a molecule in in atomic…

Q: 1. A particular ground state atom has partially-filled 4f orbitals. This atom could be: Select one:…

A: Only first question is answered according to the policy

Q: Type in electron configurations for the following atoms and ions. Use the noble gas shortcut. The…

A: The species given are Ti, Co, Y2+ and Bi3+.

Q: 3. The figure below shows the Radial wave function, Y(r) vs. r, in red and the Radial probability…

A: Since you have posted a question with multiple sub-parts, we will solve first three subpartsfor you.…

Q: ) Why do successive ionization energies increase? B.) Define electron affinity and electron…

A: A) Ionization energy : The ionization energy of a chemical species (i.e., an atom or molecule) is…

Q: a. Write the electron configuration for Rb*. (Express your answer as a series of orbitals, in order…

Q: An excited chlorine atom emits red light with a wavelength of 628.5 nm. What is the energy…

A: The energy difference between orbitals that gives rise to the emission of red light with a…

Q: 6. There are three rules electrons normally follow when occupying orbitals in an atom. (i) Name each…

Q: 6. Determine the ionization energy for the hydrogen atom. The ionization energy is the energy…

A: Applying Bohr’s equation for the energy levels of hydrogen atom, the change in energy when an…

Q: 1) f. Provide the ground state electron configuration of chlorine by drawing and completing an…

A: Electronic configuration refers to the systematic arrangement of electrons in the various shells and…

Q: A.) What is the grounds the electron configuration of 15p. B.) Show the orbital diagram. C.) Write…

A: Given atom, Phosphorous atom - 15P

Q: 1. What is the cause of the atomic emission spectrum of an element?

A: Given: To give the causes of atomic emission spectrum of an element

Q: a. Write the electron configuration for Ba²+. (Express your answer as a series of orbitals, in order…

A: Electronic configuration refers to the arrangement of electrons within an atom or an ion. It…

Q: Consider the following three atomic orbitals. They are drawn to scale and orbital a has n=2.

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: 2. Explain why the ground-state electron configurations of Cr and Cu are different from what we…

A: The atomic number of chromium is 24. Write the electronic configuration of Chromium. Cr = 1 s2 2 s2…

Q: Part 6: 6a. What trend in atomic radius occurs as you go up a group on the periodic table? Explain…

A: 6a.

Q: 4. A green flame is observed when copper(II) chloride is heated in a flame (Figure P7.144). a. Write…

A: a). Copper atom belongs to first transition series or can say d- block elements The atomic number of…

Q: What are the four quantum numbers of the 2 electrons in the 2s orbital of chlorine?

Q: Type in electron configurations for the following atoms and ions. Use the noble gas shortcut. The…

A: Electrons are filled in a different atomic orbital in an atom. According to the Aufbau rule, the…

Question

1.40 Suggest explanations for the following.
b. The enthalpy changes associated with the attachment of the first and second
electrons to an O atom are exothermic and endothermic, respectively.
c. In a Li atom in its ground state, the outer electron occupies a 2s rather than a 2p
orbital.

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

Given

VIEW

Solution: (b)

VIEW

Solution: (c)

VIEW

Step by step

Solved in 3 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

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.
Why is it much harder to explain the line spectra of polyelectronic atoms and ions than it is to explain the line spectra of hydrogen and hydrogenlike ions?
What is the maximum number of electrons that can occupy a f subshell (l = 3)?
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
From what you know in a general way about electron affinities, state which member of each of the following pairs has the greater value: a As, Br b F, Li.
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.
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
Using the Bohr model, determine the energy in joules of the photon produced when an electron in a L2+ ion moves from the orbit with n = 2 to the orbit with n = 1.
Which is higher in energy, the 2s or 2p orbital, in hydrogen? Is this also true for helium? Explain.
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?
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?