**Question:** Classify each statement about effective nuclear charge, \( Z_{\text{eff}} \), as true or false.**Diagram Explanation:**There are two boxes labeled "True" and "False" where statements can be classified accordingly.**Answer Bank:**- Effective nuclear charge does not depend on the number of electrons present in an atom. # Understanding Effective Nuclear Charge### Answer Bank- Effective nuclear charge does not depend on the number of electrons present in an atom.- Effective nuclear charge increases from left to right across a period on the periodic table.- In a Be atom, a 1s electron has a greater \( Z_{\text{eff}} \) than a 2s electron.- A 1s electron in a Be atom has a smaller \( Z_{\text{eff}} \) than a 1s electron in a Li atom.- Across a period, as \( Z_{\text{eff}} \) increases, atomic size increases.- Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.### ExplanationThis section explores various principles related to effective nuclear charge (\( Z_{\text{eff}} \)) and its implication on atomic structure and properties. Understanding these concepts is crucial for analyzing how atoms interact and bond with each other. The statements above provide insights into the behavior of electrons within different elements and the role of effective nuclear charge in chemistry.

Effective nuclear charge (Zeff) is the total positive charge experienced by an electron present in…

Answer Bank Effective nuclear charge does not depend on the number of electrons present in an atom. Effective nuclear charge increases from left to right across a period on the periodic table. In a Be atom, a 1s electron has a greater Zeff than a 2s electron. A 1s electron in a Be atom has a smaller Zeg than a 1s electron in a Li atom. Across a period, as Zeff increases, atomic size increases. Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.

Answer Bank Effective nuclear charge does not depend on the number of electrons present in an atom. Effective nuclear charge increases from left to right across a period on the periodic table. In a Be atom, a 1s electron has a greater Zeff than a 2s electron. A 1s electron in a Be atom has a smaller Zeg than a 1s electron in a Li atom. Across a period, as Zeff increases, atomic size increases. Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Briefly explain the errors in each of the three noble gas core configurations below and give the correct noble gas core configurations. Potassium: [Ar] 4s2 Iodine: [Kr] 5s2 5d10 5p5 Chromium: [Ar] 4s2 3d4
Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 10 5 [G]ns² md¹0 np [G]ns² np³ [G]ns mf location of elements (check all that apply) blocks Os 0 P Od O Os Op Od Of Os Op d Of metals or nonmetals? metals Ononmetals O metalloids O metals Ononmetals O metalloids O metals Ononmetals O metalloids X S
Each of the statements below attempts to explain why some periodic property varies predictably among elements in the periodic table. Determine if each statement is true or false. Within a period, elements with higher atomic numbers have atoms of smaller radius because the valance electrons are in higher principal energy levels. Within a family, elements with higher atomic numbers have lower ionization energy because the valance electrons are in higher principal energy levels. Within a period, elements with higher atomic numbers have higher ionization energy because the valance electrons are in higher principal energy levels. Within a family, elements with higher atomic numbers have higher electronegativity because the atoms have higher effective nuclear charge. Within a period, elements with lower atomic numbers require more energy to remove an electron from the atom, because the valance electrons are in higher principal energy levels. Within a period, elements with lower atomic…
An atom has an electron configuration of 1s²2s²2p 3s²3p³. How many valence electrons does the atom have? A 3 B 5 C 10 D 15
Choose the best answer below. Which of the following statements is FALSE? Adding another electron to Cl releases more energy than adding another electron to P Removing core electrons from any element requires a much larger amount of energy compared to removing the valence electrons Na has a higher first ionization energy than Be The photoelectric effect involves ionizing an electron away from a neutral atom It takes more energy to remove the second valence electron from Ca than it takes to remove the first
The Aufbau Principle describes the order of subshells in an atom in terms of energy. Higher numbered shells have higher energy. It is complicated by occasional overlapping. The specific order of subshells using the Aufbau Principle can be found using the diagonal arrow diagram found in Chapter 8, and this is the same order found on the periodic table. What is the order of subshells in period 2 ? 2s ____ What is the order of subshells in period 3 ? 3s ____ What is the order of subshells in period 4 ? 4s ____ ____ What is the order of subshells in period 5 ? 5s ____ ____
Some patterns of electron configuration are listed below. In each case, [G] stands for a noble-gas core and n, m, or o stand for integer numbers like 1, 2, 3 and so on. Note: assume G is lighter than Rn. Think about the chemical elements made of atoms with an electron configuration that matches each pattern. In what block or blocks of the Periodic Table would these elements lie? Would they be metals, nonmetals, metalloids, some of each? Use your answers to these questions to complete the table. electron configuration of atoms 6 [G]ns²np [G]ns¹ 2 [G]ns²mf³ 3 blocks 00 P S 00 P 00 S location of elements (check all that apply) S C р р f р f metals or nonmetals? 000 000 000 metals nonmetals metalloids metals nonmetals metalloids metals nonmetals metalloids
Name the element with the atomic orbital diagram shown below:
Fix any errors in these proposed electron configurations. number of electrons in atom 16 5 26 proposed electron configuration 6 15 1p 2s 2p 15²25²35²¹ 15 25 2p 3s 3p 3d
The electron configuration of an element is: 1s? 2s? 2p6 3s? 3p6 4s? 3d10 4p6 5s2 The Group and Period of the element are: Group 5 Period 1A Group 2B Period 5 Group 5 Period 1B Group 2A Period 5
Fix any errors in these proposed electron configurations. number of electrons in atom 32 20 12 proposed electron configuration 6 10 1s² 1p 2s²³ 2p 2d¹ 35² 3p 6 1s 2s² 2p 3s 3p 3d 5 2 2 8 2 1s 2s 2p X