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Choose the element with the higher first ionization energy from each pair. d. P or Sn
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Ch.9 - Periodic Properties of the Elements
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 73
Arrange these elements in order of increasing first ionization energy: Si, F, In, N.
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Step 1: Understand that ionization energy is the energy required to remove an electron from an atom. The greater the ionization energy, the harder it is to remove an electron.
Step 2: Recall that ionization energy generally increases from left to right across a period (row) on the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, which increases the positive charge and pulls the electrons closer to the nucleus, making them harder to remove.
Step 3: Also remember that ionization energy generally decreases from top to bottom down a group (column) on the periodic table. This is because as you move down a group, the electrons are further from the nucleus and are therefore easier to remove.
Step 4: Locate the elements Si, F, In, and N on the periodic table. Si and N are in the same period, with N to the right of Si, so N has a higher ionization energy than Si. F is in the same period as N but is to the right, so it has an even higher ionization energy. In is below Si in the same group, so it has a lower ionization energy.
Step 5: Therefore, the order of increasing first ionization energy is In, Si, N, F.
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Ionization Energy
Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key factor in determining an element's reactivity and is influenced by the atomic size and the effective nuclear charge. Generally, ionization energy increases across a period due to increasing nuclear charge and decreases down a group due to increased distance from the nucleus.
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01:19
Ionization Energy
Trends in the Periodic Table
The periodic table exhibits specific trends in ionization energy, where elements in the same group have lower ionization energies than those in the same period. As you move from left to right across a period, ionization energy tends to increase due to the increasing positive charge of the nucleus, which attracts electrons more strongly. Conversely, moving down a group, ionization energy decreases because the outer electrons are further from the nucleus and experience greater shielding.
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00:38Periodic Trends
Comparison of Elements
When comparing elements like Si, F, In, and N, it is essential to consider their positions in the periodic table. Fluorine (F) has the highest ionization energy due to its small atomic size and high electronegativity, while indium (In) has the lowest due to its larger atomic radius and lower effective nuclear charge. Silicon (Si) and nitrogen (N) fall in between, with nitrogen having a higher ionization energy than silicon due to its position in the same period but further to the right.
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02:35Elemental Forms of Elements
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