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    Lanthanide (europium)



    Discuss the following:

    Lanthanide (europium) the majority of paper focus on EU
    Electronic configuration (chart)
    electronic properties and applications
    optical properties and applications
    energy transitions (CHART)
    energy level of atomic orbitals
    EU luminescent properties
    emission of EU mangetic and electrical (CHART)



Subject Chemistry Pages 5 Style APA


Analysis of The Properties of Lanthanides: The Case of Europium




The aim of this paper is to explore lanthanides, with a keen consideration of europium. According to Binnemans (2015), lanthanides are silvery-white metals that tarnish on exposure to air to form oxides, comparatively soft metals, have high boiling and melting points, react readily with water and dilute acids, burn easily in air, and are strong reducing agents. Alongside other properties, these elements are used as catalysts in the production of synthetic products and petroleum, used in lasers, magnets, lamps, motion picture projectors, phosphors, and X-ray. There are several lanthanides. However, this paper focuses on europium.

Lanthanide and Europium

The lanthanides refer to a group of fifteen chemical elements whose atomic numbers running from 57 to 71 (Binnemans, 2015). All these elements have single valence electron within their 5d shell (Naiman et al., 2018). One of the lanthanides is the Europium, an element symbolized by Eu and having atomic number 63 (Khuyen et al., 2019).  It is the most reactive lanthanide, necessitating that it be stored under an inert fluid for reasons of protecting it from moisture or atmospheric oxygen (Hajimazdarani et al., 2020). Similarly, Lobacheva and Dzhevaga (2017) note that Europium is equally the softest lanthanide since it can be dented by a fingernail and simply cut using a knife. When oxidation is scaled off, a shiny-white metal is exposed. Eu assumes an oxidation state of +3.

Electronic Configuration

Eu’s electronic configuration is [1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6] 4f7 6s2, which is as distributed as shown below.

Fig. 1. Periodic table (Gökçe et al., 2017).

Fig. 2. Schematic electronic configuration of Eu (Al-Shehri et al., 2019).

Eu’s Electronic Properties and Applications

Eu has several electronic properties. Eu has an electrochemical equivalent of 1.8899g/amp-hr, electron work function of 2.5eV, electronegativity of 1.01 (Allrod Rochow) or 1.2 (Pailing), heat fusion of 9.21kJ/mol, Ionization potential of 5.67 for first ionization, 11.245 for the second ionization, and 24.926 for the third one. Due to these properties, Europium is used differently. As aforementioned, the element is a less expensive, soft silvery metal that is the most reactive of the members of the lanthanide. It quickly tarnishes in air at room temperature and burns at approximately 150-180oC and readily react with water (Binnemans, 2015). Europium is a neutron adsorber, making it be used in nuclear reactors regulatory rods (Naiman et al., 2018). Khuyen et al. (2019) add that Europium phosphors are employed in TV tubes to produce bright red colour as well as an activator for yttrium-based phosphors. A little europium is normally added to mercury vapour lamps to produce extra natural light when powerful street lighting is needed (Lobacheva & Dzhevaga, 2017). Europium salt is employed for newer phosphorescent paints and powder. It is equally employed in making thin-film superconductor alloys. Europium is used as a dopant in certain kinds of glasses in lasers along with other optoelectronic devices. Whereas trivalent Eu produces red phosphors, Al-Shehri et al. (2019) note that the luminescence of divalent Eu relies robustly upon the composition of the host structure. Lately, Eu is employed in quantum memory chips that can reliably keep data and information for days, allowing sensitive quantum information to be kept to some hard disk-like tools and shipped around (Hajimazdarani et al., 2020).

Eu’s Optical Properties and Applications

The reflective index of europium is unclear to date. However, a study by Naiman et al. (2018) revealed that Eu3+ function as the emitting centre in doped samples with only Eu as well as with both Ti and Eu with the transition from 5D0 to 7F2 being the most intense, suggesting that Eu3+ in a non-centrosymmetric site. The use of europium in UV light is, thus, explained by Eu’s ability to glow red. Similarly, red-green-blue luminescence is obtainable through the use of a single-type host structure. 

Energy Transitions

Europium undergoes three ionizations in its chemical reactions. This is because it has four valence electrons. With an electron affinity of 50 kJ/mol, Eu’s first ionization energy is 547.1 kJ/mol, the second one is 1085 kJ/mol, and the third one is 2404, and finally 4120 kJ/mol (Lobacheva and Dzhevaga (2017). A summary of the element’s energy transitions is as shown below.


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