Quantum Numbers and Energy Levels

Principle quantum number

32

False

<p>The number of energy sublevels within a specific principle energy level.</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>f</p> Signup and view all the answers

<p>The number of orbitals within a specific energy sublevel and their orientation in space.</p> Signup and view all the answers

<p>-2, -1, 0, 1, 2</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>In a spin paired state, two electrons in the same orbital have opposite spins, while in a spin unpaired state, they have the same spin.</p> Signup and view all the answers

<p>Electrons fill energy sublevels in order of increasing energy, starting with the lowest energy sublevel and filling up to the highest energy sublevel.</p> Signup and view all the answers

<p>The order of increasing energy is: 1s &lt; 2s &lt; 2p &lt; 3s &lt; 3p &lt; 4s &lt; 3d &lt; 4p &lt; 5s &lt; 4d &lt; 5p &lt; 6s &lt; 4f &lt; 5d &lt; 6p &lt; 7s &lt; 5f &lt; 6d &lt; 7p.</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>1s² 2s² 2p³</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>The main categories are: s-block elements, p-block elements, d-block elements, and f-block elements.</p> Signup and view all the answers

<p>Alkali metals (group 1A) and alkaline earth metals (group 2A).</p> Signup and view all the answers

<p>Representative elements.</p> Signup and view all the answers

<p>Transition metals.</p> Signup and view all the answers

<p>Inner transition elements.</p> Signup and view all the answers

<p>False</p> Signup and view all the answers

<p>True</p> Signup and view all the answers

<p>It states that no two electrons in an atom can have the same four quantum numbers.</p> Signup and view all the answers

<p>The Aufbau Principle dictates the order in which electrons fill up the orbitals in an atom, starting with the lowest energy level and moving towards higher energy levels. This principle is directly related to the periodic table's organization, where each element's position reveals its electronic configuration and helps predict its chemical properties.</p> Signup and view all the answers

<p>Hund's rule emphasizes minimizing electron repulsion by stating that electrons will occupy individual orbitals within a sublevel with the same spin before pairing them up in the same orbital. It differs from the Aufbau Principle by providing a specific filling strategy for orbitals within a sublevel, focusing on the spin configuration of electrons.</p> Signup and view all the answers

<p>Noble gases are the elements found in Group 18 (VIIIa) of the periodic table. They are characterized by their extremely stable electronic configurations, making them very unreactive.</p> Signup and view all the answers

<p>Representative elements are those elements that are located in the s- and p-blocks of the periodic table. They differ from transition metals in the way they fill their d orbitals, and they tend to have more predictable chemical properties.</p> Signup and view all the answers

<p>Atomic radius is the distance from the nucleus to the outermost electron shell of an atom. It significantly influences an element's chemical properties, particularly reactivity, bonding characteristics, and ionization energy.</p> Signup and view all the answers

<p>Ionization energy is the minimum energy required to remove an electron from a gaseous atom, while electron affinity is the energy change that occurs when an electron is added to a gaseous atom.</p> Signup and view all the answers

<p>Effective nuclear charge is the net positive charge experienced by an electron in an atom's outermost shell, considering the shielding effect of inner electrons. A higher effective nuclear charge attracts outer electrons more strongly, leading to a smaller atomic radius and higher ionization energy.</p> Signup and view all the answers

<p>Atomic radius generally decreases moving across a period and increases moving down a group. Ionization energy generally increases moving across a period and decreases moving down a group.</p> Signup and view all the answers

<p>As you move across a period, the effective nuclear charge increases due to the addition of protons without a significant change in the shielding effect, leading to a smaller atomic radius and higher ionization energy. Moving down a group, the number of energy levels increases, leading to greater shielding of outer electrons by inner electrons, resulting in a larger atomic radius and lower ionization energy.</p> Signup and view all the answers

<p>Noble gases have a very high ionization energy because they have a completely filled outer electron shell, making them extremely stable and unreactive. It is very difficult to remove an electron from a noble gas atom because of this stability.</p> Signup and view all the answers

<p>Electronegativity is the tendency of an atom to attract electrons in a chemical bond. While electron affinity is the energy change that occurs when an electron is added to an atom, electronegativity considers the atom's ability to attract electrons in a bonding environment.</p> Signup and view all the answers

<p>Factors influencing these trends include: 1) Effective nuclear charge: A higher effective nuclear charge contracts the electron cloud, leading to a smaller atomic radius and higher ionization energy, 2) Number of energy levels: More energy levels result in a larger atomic radius and lower ionization energy, 3) Shielding effect: Inner electrons shield outer electrons from the nucleus, decreasing the effective nuclear charge and leading to a larger atomic radius and lower ionization energy. 4) Electron configuration: A complete outer electron shell increases stability, leading to higher ionization energy and a decrease in electron affinity.</p> Signup and view all the answers