4. Which of the following should be the larger atom? Why?Sodium vs. Chlorine-Lithium vs. Cesium5. Which is larger? Why?The hydrogen 1s orbitalThe lithium 1s orbital6. Which is lower in energy? Why?The hydrogen 1s orbitalThe lithium 1s orbital

Answered: Image /qna-images/answer/b898792c-dd78-4ccf-bc4f-c02d5bf43243.jpg

Answered: 1. Which of the following should be the…

Science

Chemistry

1. Which of the following should be the larger atom? Why? Sodium vs: Chlorine- Lithium vs. Cesium

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter6: Electronic Structure And The Periodic Table

Section: Chapter Questions

Problem 44QAP: Write the symbols of (a) all the elements in period 5 that have at least two half-filled 5p...

See similar textbooks

Related questions

Q: What is the maximum number of electrons that can occupy the "s" sublevel? A 10 B. 2 c. 6 D. 14 2.…

A: (1) There are different type of orbitals with different shape and different electron occupying…

Q: What is the major role of Ionic Size?

A: Ionic bond: Chemical bond formed between two elements by electron loss and gaining process in order…

Q: 9.22 Predict a possible monatomic ion for Element 117 Given the spherical models below, which should…

A: Element 117 would fall in Group 7A, the halogens. The monatomic ion for this element would maybe be…

Q: 3.2 In the space below, write the condensed electron configuration of the following elements: a.…

A: Given, Silver Argon Rubidium

Q: How many electrons in the quantum numbers of the atom n = 2, l = 0, ml = 1

A: Given, Principal quantum number, n = 2 used to describe an electron located on the second energy…

Q: 7.37 Which is the smallest atom in Group 7A?

A: Group 7A includes halogen atoms. The elements present in group 7A are: Flourine, FChlorine,…

Q: 1. Define the following terms and give an example of each: transition metals, lanthanides,…

A: Transition metals = Transition metals are the elements which has partially filled d orbitals.…

Q: What is electron configuration? Describe the roles that the Pauli exclusion principle and Hund’s…

A: Electronic configuration: Electronic configuration is defined as the arrangement of electrons in an…

Q: 10. Which rule or principle does the following orbital diagram violate? Why? 11. Which rule or…

A: There are mainly three principle or rule for orbital diagram. 1. Pauli exclusion principle 2.…

Q: Why does flourine have a smaller atomic radius than magnesium?

A: Magnesium belongs to 2nd group and 3rd period .The element fluorine belongs to 17 th group and 2nd…

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: Choose the larger atom N or Al

A: N : Nitrogen Al : Aluminium Which is larger i.e having large size ?

Q: Give the quantum number of Sulfur

A: Given question is : Give the quantum number of Sulfur = ?

Q: The scientist who first proposed the order of electron distribution within subshells was _______.…

Q: Consider the following elements – O, F, Na, Mg and Al. -What is the first criterion you would use to…

A: The order of size of the atoms given to us can be determined as follows:

Q: What rules determine the electronic confi guration of an atom?

Q: An atom's electron configuration ends with 3p4. If another atom has seven more electrons, what would…

Q: (a) What are “valence electrons"? (b) What are “core elec- trons"? (c) What does each box in an…

A: a. Valence electrons are outermost electrons present in valency shell and participate in chemical…

Q: a.) For the pair of elements Ar and Br, pick the atom with more favorable (exothermic) electron…

A: a. The amount of energy released when 1 mol of an electron is added to the neutral atom that must be…

Q: Chlorine?

Q: 4 Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron…

A: An atom is mainly composed of three sub-particles; electrons, protons and neutrons. In an atom,…

Q: nts Ionisation Energy: It is the energy required to an electron from an atom in the given graph,…

A: Ionization energy is the amount of energy required to remove an electron from the outer most shell…

Q: 2) The plot below is like the ones shown in class as examples of measurements of a bound electron's…

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

Q: Which is TRUE about the 3p electrons in sulfur? (A) They travel in a figure 8 orbit (B) They are…

A: Postulates of Bohr’s Model of an Atom: In an atom, negatively charged electrons revolve around the…

Q: Dw many electrons in an atom could have these sets of quantum numbers? n= 3 n = 4, e = 2 n = 6, e =…

A: Quantum number tells about the Address of electrons in an atom .

Q: 18 Why did the scientist have to come up with a different atomic model after Bohr? a. Bohr could…

Q: How many sublevels are there with n = 3 in an atom?

Q: Which statement about the orbital in Figure 7 is not correct? a) The orbital represented here could…

A: The orbital given is,

Q: The spheres below represent atoms of Sb, As, P, and N (not necessarily in that order). r-110 pm (b)…

Q: b. (i) Define Electron Affinity and explain why the electron affinity may either have positive or…

A: Electron affinity can have both positive or negative values.

Q: Use electron configuration to explain why arsenic can acquire charges of 3- and 3+ but not 2+.

A: Answer:- This question is answered by using the simple concept of writing the electronic…

Q: b. Vanachium,2=23 Cmanganese, Z=25 d iron, 2=26o 65) for each f the fallowing elements, indic is…

A: Electronic configuration of element helps us to determine the position of element in periodic table.…

Q: 2. Which is TRUE about the 3p electrons in sulfur? (A) They travel in a figure 8 orbit (B) They are…

A: The increase in shell number energy also increases

Q: The electron configuration of Li* resembles that of which of the following elements Oa. Berrylium…

A: Given , Ion = Li+

Q: evel Diagrams and Electroh Configu 1. Write the 15 sets of quantum numbers that describe the 15…

A: As per our guidelines we can only solve first question. Please resubmit the other questions as next…

Q: 23) Which of the following correctly describes the Bohr model of atom? A) Electrons are embedded in…

A: Bohr's atomic model came into existence with the modification of Rutherford’s atomic model.…

Q: Rank the following atoms in order of decreasing size (i.e., largest to smallest): Rb, F, Mg, B, N.

A: Atomic radii reduce across a row and rise down a column in the periodic table. The biggest atoms…

Q: 559048ad75799f5abe16e1aff#10001 MReview | Constants Periodic Table On the basis of periodic trends,…

A: The explanation is given below-

Q: Choose the larger atom in pair. P or Pb

A: Atomic radius is defined as the distance of the nucleus to the outermost shell containing electrons.…

Q: Choose the larger atom in pair. Si or N

A: The explanation and the answer is as given below:

Q: The nucleus of a gold atom contains 79 protons. How would you expect the energy required to remove a…

A: Calculate the energy required to remove an 1s electron from ground state of gold atom:Atomic number…

Q: 1) Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c.…

A: Given:- (a) Rb , Na , Be This element consists of…

Q: In electrons configuration, what is meant by “core electrons”? Support your explanation by using the…

A: In a electronic configuration of an atom except valance electron all electrons that do not take part…

Q: Rank the following atoms according to their size. Rb, Sr, Sb, Sn, In

A: The atomic size decreases across a period as the number of electrons increases and higher effective…

Q: ?For the following set of quantum numbers, what is the maximum number of electrons possible 2+ = n=…

A: Pauli exclusion principle: It says, It is impossible for any two electrons of atom to have a same…

Q: True or False: a.)Cesium atom is a paramagnetic element but Cs+ and Cs- are not. b.)The…

A: Interpretation: We have to predict whether the statement is true or false.

Question

4. Which of the following should be the larger atom? Why?
Sodium vs. Chlorine-
Lithium vs. Cesium
5. Which is larger? Why?
The hydrogen 1s orbital
The lithium 1s orbital
6. Which is lower in energy? Why?
The hydrogen 1s orbital
The lithium 1s orbital

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

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.
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
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?
(a) How many subshells are present in the n = 4 shell? (b) How many orbitals are in the 3d subshell? (c) What is the maximum value of that is allowed in the shell with n = 3? (d) What are the values of n and for a 3p subshell? Give all allowed values of the m quantum number for this subshell.
Write the symbols of (a) all the elements in period 5 that have at least two half-filled 5p orbitals. (b) all the elements in Group 1 that have full 3p orbitals. (c) all the metalloids that have paired 3p electrons. (d) all the nonmetals that have full 3d orbitals and 3 half-filled 3p orbitals.
What is the maximum number of electrons that can occupy a f subshell (l = 3)?
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?
6.60 Use the electron configurations of the alkali metals and your knowledge of orbitals and quantum numbers to explain the trend in atomic size of alkali metal atoms.
Although no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could being orbitals. For g orbitals, the value of l is 4. What is the lowest value of n for which g orbitals could exist? What are tile possible values of ml? How many electrons could a set of g orbitals hold?