2024-09-16T23:46:47+03:00[Europe/Moscow] en true <p><strong>Pauli's exclusion</strong> principle</p>, <p><strong>Aufbau</strong> principle</p>, <p><strong>Hund's</strong> rule</p>, <p>Valence electrons (what is the exception for transition elements)</p>, <p>S-block elements are ___ elements and their valence electrons are in their ___ orbital </p>, <p>P-block elements are ___ elements and their valence electrons are in their ___ orbital</p>, <p>D-block elements are ___ elements and their valence electrons are in ___</p>, <p>F-block elements are ___ elements and their valence electrons are in ___ </p>, <p><strong>Reactivity</strong> (in relation to electron configurations)</p>, <p>Group 1A metals form ___ And group 2A metals form ___</p>, <p><strong>Nonmetals</strong> in general form ___</p>, <p>Group 7A nonmetals form __</p>, <p><strong>Metals</strong> (including transition and inner transition) in general form ___</p>, <p>What are the <strong>five</strong> exceptions to orbital filling</p>, <p>As you move <strong>across a row </strong>the atomic radius ___ because ___</p>, <p>As you move <strong>down a column</strong> the atomic radius ___ because ___</p>, <p><strong>Effective nuclear charge</strong> (how do you calculate it)</p>, <p>Diamagnetic vs. paramagnetic </p>, <p><strong>Cations</strong> are ___ than their original atoms because ___</p>, <p><strong>Anions</strong> are ___ than their original atoms because ___</p>, <p><strong>Isoelectronic</strong> ions have the same ___ but different ___ and ___</p>, <p><strong>Ionization energy (IE) </strong>(Is it positive or negative)</p>, <p><strong>Across a row</strong> IE ___ because ___</p>, <p><strong>Down a column</strong> IE ___ because ___</p>, <p>There's a jump in energy required across ___ IE's because ___</p>, <p><strong>Electron affinity (EA) </strong>(is it positive or negative)</p>, <p><strong>Across a row</strong> (in main group elements) EA ___ because ___</p>, <p><strong>Metallic character</strong></p>, <p><strong>Across a row,</strong> metallic character ___</p>, <p><strong>Down a column</strong>, metallic character ___</p> flashcards

Chapter 3 - Electron configurations

The periodic table Periodic trends Electron configurations Ionic configurations Atomic and ion radius

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  • Pauli's exclusion principle

    Each electron must have it's own 4 unique quantum numbers (otherwise it does NOT exist)

  • Aufbau principle

    Orbitals will be filled from the lowest energy levels to the highest

  • Hund's rule

    When electrons are in orbitals of the same energy, they prefer the be unpaired and with spins aligned

  • Valence electrons (what is the exception for transition elements)

    Main group = The electrons found in the outermost principal energy level

    - Transition elements = The electrons found in the highest principal energy level excluding d orbitals

  • S-block elements are ___ elements and their valence electrons are in their ___ orbital

    - Main group elements

    - highest s orbital (2nd)

  • P-block elements are ___ elements and their valence electrons are in their ___ orbital

    - Main group elements

    - highest p orbital (3rd)

  • D-block elements are ___ elements and their valence electrons are in ___

    - Transition elements

    - 1 principal (n) energy level below the corresponding s and p levels (usually 4th)

  • F-block elements are ___ elements and their valence electrons are in ___

    - Inner transition elements

    - 2 principal (n) energy levels below their corresponding s and p orbitals (usually 5th)

  • Reactivity (in relation to electron configurations)

    Elements that are very close to filling their valence electron orbitals WANT to gain or lose an electron to do so (and reach a stable configuration) so they're more likely to react with other elements

  • Group 1A metals form ___ And group 2A metals form ___

    - 1+ cations

    - 2+ cations

  • Nonmetals in general form ___

    Anions

  • Group 7A nonmetals form __

    -1 anions

  • Metals (including transition and inner transition) in general form ___

    Cations

  • What are the five exceptions to orbital filling

    Chromium (Cr) = [Ar] 4s13d3 

    Copper (Cu) = [Ar] 4s13d10 

    Silver (Ag) = [Kr] 5s14d10 

    Gold (Au) = [Xe] 6s14f145d10 

    Molybdenum (Mo) = [Kr] 5s14d5 

  • As you move across a row the atomic radius ___ because ___

    - Decreases

    - because the outer electrons experience a greater effective nuclear charge

  • As you move down a column the atomic radius ___ because ___

    - Increases

    - because the n value increases and has larger electron orbitals

  • Effective nuclear charge (how do you calculate it)

    Z(eff) = (actual nuclear charge) - (charge from other electrons [number of core electrons])

    - the attraction from the nucleus that valence electrons experience minus the shielding from the core electrons

  • Diamagnetic vs. paramagnetic

    Dia = All electrons paired, no attraction to external magnetic field

    Para = At least one unpaired electron, weak attraction to magnetic field

  • Cations are ___ than their original atoms because ___

    - Much smaller

    - their (lost) valence electrons and orbitals contributed to their radius

  • Anions are ___ than their original atoms because ___

    - Much larger

    - the additional electron increases their outermost orbital and radius

  • Isoelectronic ions have the same ___ but different ___ and ___

    - Number of electrons (even if their charge is different)

    - Different mass and size

  • Ionization energy (IE) (Is it positive or negative)

    The energy needed to remove an electron from an atom or ion

    - Always positive because it requires energy

  • Across a row IE ___ because ___

    - Increases

    - Elements on the right experience greater Z(eff) and it requires more energy to remove an electron

  • Down a column IE ___ because ___

    - Decreases

    - Elements on the bottom have greater n values and their valence electrons are further away from the nucleus, meaning it requires less energy to remove an electron

  • There's a jump in energy required across ___ IE's because ___

    - second, third, ... etc.

    - When an electron is being removed from core electron and noble gas configurations because these configurations are more stable and prefer to stay that way

  • Electron affinity (EA) (is it positive or negative)

    How much an atom or ion wants to accept an additional electron

    - USUALLY negative because it releases energy

  • Across a row (in main group elements) EA ___ because ___

    - Increases (becomes more negative)

    - Elements on the right side need to gain electrons to reach noble gas configurations

  • Metallic character

    An elements tendency to lose electrons due to it having less valence electrons

  • Across a row, metallic character ___

    - Decreases (until you fully hit nonmetals)

  • Down a column, metallic character ___

    - Increases