Textbook Question
Among elements 1–18, which element or elements have the smallest effective nuclear charge if we use Equation 7.1 to calculate 𝑍eff? Which element or elements have the largest effective nuclear charge?
2
views
Ch.7 - Periodic Properties of the Elements
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 7, Problem 6
The graph below shows the ionization energies for a particular element. In which group is the element most likely a member of? [Section 7.3]
Verified step by step guidance1
Identify the pattern of ionization energies: Look at the graph and observe how the ionization energies change as electrons are removed.
Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state.
Recognize the significance of large jumps in ionization energy: A large increase in ionization energy indicates that an electron is being removed from a more stable, inner shell.
Determine the group based on the ionization energy pattern: Elements in the same group have similar outer electron configurations, leading to similar ionization energy patterns.
Relate the observed pattern to known group characteristics: For example, if there is a large jump after the first ionization energy, the element is likely in Group 1 (alkali metals), as they have one valence electron.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionization Energy
Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of an element's reactivity and is influenced by factors such as atomic size and nuclear charge. Generally, ionization energy increases across a period and decreases down a group in the periodic table.
Recommended video:
Guided course
01:19
Ionization Energy
Periodic Trends
Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. These trends include variations in ionization energy, electronegativity, and atomic radius. Understanding these trends helps in predicting the behavior of elements and their placement in groups.
Recommended video:
Guided course
00:38Periodic Trends
Group Classification
Elements in the periodic table are organized into groups based on similar chemical properties and electron configurations. Each group shares common characteristics, such as reactivity and the number of valence electrons. Identifying the group of an element based on its ionization energy can provide insights into its chemical behavior and potential applications.
Recommended video:
Guided course
04:22Ligand Classification
Related Practice
Textbook Question
The prefix eka- comes from the Sanskrit word for 'one.' Mendeleev used this prefix to indicate that the unknown element was one place away from the known element that followed the prefix. For example, eka-silicon, which we now call germanium, is one element below silicon. Mendeleev also predicted the existence of eka-manganese, which was not experimentally confirmed until 1937 because this element is radioactive and does not occur in nature. Based on the periodic table shown in Figure 7.1, what do we now call the element Mendeleev called eka-manganese?
2375
views
1
rank
Textbook Question
Which of these spheres represents F, which represents Br, and which represents Br-?
616
views
Textbook Question
In the following reaction
which sphere represents a metal and which represents a nonmetal?
372
views
1
rank
Textbook Question
Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheres below represent these four ions, scaled according to ionic size. (b) In terms of size, between which of the spheres would you find the (i) Ca2+ and (ii) S2- ions?
1018
views