Answered: Arrange the following in their…

Arrange the following in their increasing size with the help of slater’s rule and also give calculations for each of them Mg2+,Kr ,Ca2+

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 60QAP

See similar textbooks

Related questions

Q: Which of the following sets of quantum numbers would account for the highest-energy electron in…

A: The highest energy electron in Ni2+ ion corresponds to a certain set of quantum numbers. The…

Q: Order Al, K, N and Mg in the order of increasing first ionization energy.

A: The amount of energy required to convert from one mole of neutral atom to gaseous ion

Q: Explain the trend in effective nuclear charge (Z*) going from left to right across periods in the…

Q: Why are the ionization energies of the alkali metals in the order Li >, Na > K > Rb?

A: ANSWER IS DISCUSSED BELOW :

Q: The first ionization energy of sodium is 497 kJ/mol. Write the chemical equation which represents…

A: Ionization energy means the energy required to remove an electron from isolated gaseous atom. Na…

Q: Determine the ionization energy of phosphorus using the orbital approximation and a Zeff for the 3s…

A: Ionization energy defined as the amount of energy that an isolated gaseous atom in the ground state…

Q: Apply Slater's rules to explain why the binding energy of outermost valence electron in a fluorine…

A: The electronic configuration of Fluorine (F) is 1s2 2s2 2p5. The electronic configuration of Lithium…

Q: Describe the trends of the element in a periodic table below and explain your answer: i)Electron…

A: i) Electron affinity : The amount of energy released when an electron is added to the neutral…

Q: The ionization energies for Li, Na, K, Rb, and Cs are 5.390, 5.138, 4.339, 4.176, and 3.893 eV,…

A: All the atoms are having ionization energy as they are from similar environment and same electrical…

Q: Arrange the following in order of increasing (smallest to largest) first ionization energy: As, Ca,…

A: The first ionisation energy of elements increases on moving left to right in a period of periodic…

Q: Which statement is true regarding Slater's rules and the calculation of effective nuclear charge?

A: Slater's rule : it is used to calculate the effective nuclear charge felt by an electron. Effective…

Q: Which ion would you expect to be smaller in size—I− or Br−? Explain.

A: Among the elements in the periodic table, the size of the elements increases as we go down the…

Q: 10. Which one of the following species is not isoelectronic E. 0²- A.Mg2+ B. SI²* with neon? C. Na*…

A: Species which have the same number of electrons are called isoelectronic species.

Q: The formula for calculating the energies of an electron in a hydrogenlike ion is given in the…

A: For muli electron atom ,z is replaced with z-s. S is shielding constant value.

Q: 11. What is the ground state electron configuration for the Fe2+ ion? а. [Ar] 4s23d4 b. [Ar] 3а6 c.…

A: Atomic radius is defined as the distance from the centre of nucleus to outermost shell of atom.

Q: Which element would you expect to be less metallic?(a) Cs or Rn(b) Sn or Te(c) Se or Ge

A: The elements in a modern periodic table are arranged in an increasing order of their atomic number.…

Q: 1. Explain how the following equation can be manipulated and used to approximate the ionization…

Q: Which should have the largest difference between the first and с. second ionization energy-C, Li, N,…

A: (c) Given atoms are - Carbon C , Lithium Li, Nitrogen N, Beryllium Be Carbon has total 6…

Q: Which of the following is the expected electron configuration for a cadmium (II) cation (Z = 48)? O…

A: The ion given is cadmium (II) i.e. Cd2+.

Q: Consider the isoelectronic ions Cl- and K+. (a) Which ionis smaller? (b) Using Equation 7.1 and…

A: (a)

Q: 6. Identify the ions with a net charge of 3+ and the following configurations. A. [Xe]4A45d B.…

A: As ions has +3 charges, thus to get the corresponding atom, we have to add 3 electeons with…

Q: Explain the following statements in accordance to variation in characteristics of atoms in…

Q: 1) Arrange the following in order of decreasing atomic radii. O, Rb, Ca and Mg

A: The atomic radius of the 4 elements are -

Q: All of the following statements concerning the characteristics of the halogens are true except…

A: Ionization energy is the amount of energy required to remove the outermost shell electron of an atom…

Q: Calculate the radius in nanometers of a metallic atom given that it has a BCC structure and a…

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: Question attached

A: Given,

Q: 8. Which of the following equations represents process used to determine the ionization energy? A.…

A: Given equations: X(g) → X+(g) + e- X+(g) → X+(aq) X(g) + e- → X- (g) X+(g) + e- → X(g) We have to…

Q: By using Slaters rules, calculate the effective nuclear charge of the 22nd electron in bromine

A: Given element: Bromine

Q: For each of the following pairs of atoms, state which youexpect to have the higher first ionization…

A: Ionization energy is defined as the tendency of an element to lose electron from its outermost…

Q: Which neutron atom or ion has the smallest radius K+ , Ca2+ , Se2-

A: Given ions, Potassium(1+) ion, Calcium(2+) ion and Selenium(2-) ion.

Q: Which has the larger atomic radius of the pairs Na and Be and what is the underlying reason why?

A: Atomic radii is equal to the distance between the nuclei of an atom and its outermost shell…

Q: b.) a 4f electrons in Ce, Pr and Nd. There is a

A: a) a 2p electron in O2-,F-,Na+and Mg2+ Actually Zα1size i.e. if size increases then Z* decreases.…

Q: 3. What is the effective nuclear charge on 3(a) the outer two electrons of B? 3(b) the inner two…

A: Given element is Boron , B Atomic number = 5 Electronic configyration : 1s22s22p1

Q: Calculate the radius in nanometers of a metallic atom given that it has a BCC structure and a…

Q: Which electron configuration represents an alkali metal? O 15232p3 O 15232p°3s23p! O 13232p°3s² O…

A: Alkali metals belong to s-block

Q: Calculate the radius in nanometers of a metallic atom given that it has a BCC structure and a…

Q: Which element would you expect to be more metallic?(a) S or Cl(b) In or Al(c) As or Br

A: Metallic character represents the tendency of element to behave as metal. It increases in a group…

Q: 3. Which one of each of the following pairs has the higher electron affinity? Explain in detail for…

A: We have to select each of the element whic greater electron affinity from the given following…

Q: 9) Explain to me why the atomic radii decrease as you move across a period rather then up a group or…

A: Across a period the atomic radii is governed by effective nuclear charge. And across a group it is…

Q: Explain what is meant by the Pauli Exclusion Principle.

A: We have to explain the Pauli Exclusion Principal.

Q: The electron configuration for vanadium (V) is O [Ar] 4s 3d³

A: The distribution of electrons in an element's atomic orbitals is described by its electron…

Q: Exceptions to the trend of increasing first ionization energy and increasingly negative (i.e., more…

A: In the periodic table there are 18 groups and seven periods. Among them, the group 15 also known as…

Q: Which of the following particles is paramagnetic? A S2- В Zn C Ca2+ D Cu* E Cr3+

Q: The following orbital diagram best represents: 6s)4d G Mol+ W Мо Nb 1+ Ag

A: The answer of following question is given in next step

Q: - Arrange the following atoms in order of increasing ionization energy: In, F, Si, Sc. Ne. Smallest…

A: Ne is a nobel gas . It has full filled configuration (2s2 2p6) , it has highest ionization energy.…

Q: Q.2 (a) Arrange the following in their increasing size with the help of slater's rule and also give…

A: In the periodic table, elements are arranged as per the increasing atomic number and sizes. As the…

Question

100%

Arrange the following in their increasing size with the help of slater’s rule and also give
calculations for each of them

Mg2+,Kr ,Ca2+

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-Introduction

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

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
Palladium, with an electron configuration of [Kr] 4d10, is an exception to the aufbau principle. Write the electron configuration of the 2+ cation of palladium. Does the fact that palladium is an exception influence the electron configuration of Pd2+?
For each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Na or K (b) Cs or Cs+ (c) Rb+ or Kr (d) K or Ca (e) Cl or Ar
Are mathematical expressions for the following potential energies positive or negative? Explain why in each case. a The attraction between an electron and a helium nucleus b The repulsion between two protons in a nucleus c The attraction between a north and a south magnetic pole d The force of gravity between the Sun and Earth e A rock perched on the edge of a cliff with respect to the base of the cliff
Arrange the following in their increasing size with the help of slater’s rule and also givecalculations for each of them i. Na+, Ne, F- ii. K+ , Ar, Cl -
Q. Arrange the following in their increasing size with the help of slater’s rule and also give calculations for each of them i. Na+, Ne, F ii. K+ , Ar, Cl iii. Mg2+Kr Ca2+
Q.Arrange the following in their increasing size with the help of slater’s rule and also give calculations for each of them ii. K+ , Ar, Cl
Q.Arrange the following in their increasing size with the help of slater’s rule and also give calculations for each of them i. Na+, Ne, F
Predict the trend in values of Slater's constant of the every first element of each group of p block elements
Using Slater's Rules, calculate Zeff for the outermost s electron of vanadium, V(0)
Describe the variation of first ionisation energy moving across Period 3, from left to right
Use Slater's rules to calculate the shielding constant (S) of a 5s electron in a tin atom. Use Slater's rules to calculate the effective charge (Z*) of a 5s electron in a tin atom. List the ions from smallest to largest: Se-2, Zr4+, Kr, Rb+, Br-.