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What is the name of an element with a full electron shell?
There are 7 known elements with full electron shells, six of which are referred to as noble gases because they are, generally, unreactive with other elements because of their full electron shells (their full electron shells make them resistant to forming bonds with other atoms to form molecules): Helium, Neon, Argon, Krypton, Xenon, and Radon. Ununoctium (element 118) also has a full electron shell, but due to relativistic effects is believed to be a solid at room temperatures (if there were enough atoms of it; it is extremely unstable with a half-life of less than a tenth of a second) so may not be considered a noble gas (all the other known elements with full electron shells are gases at room temperature) but, discounting radioactive decay which causes Ununoctium atoms to fission into lighter, reactive ones, is not chemically reactive with other elements.
Which elements would likely for anions with a -1 charge?
Elements in group 17 of the periodic table, known as the halogens, are likely to form anions with a -1 charge. Examples include fluorine, chlorine, and iodine. These elements have 7 valence electrons and tend to gain one electron to achieve a stable electron configuration.
What has only one electron in their outer energy level and are highly reactive and readily give up this electron?
Elements in Group 1 of the periodic table, known as alkali metals, have only one electron in their outer energy level and are highly reactive. They readily give up this electron to achieve a stable electron configuration. Examples include lithium, sodium, and potassium.
What do the blue colored elements on the periodic table indicate?
The blue colored elements on the periodic table indicate the noble gases. These elements are typically unreactive and have a full outer electron shell, making them stable. Examples include helium, neon, and argon.
What are macroscopic elements?
Macroscopic elements are elements that can be seen with the naked eye or analyzed using macroscopic techniques, such as visual inspection or simple laboratory tests. Examples include iron, copper, and aluminum. These elements are distinct from microscopic elements, which require more sophisticated techniques, such as electron microscopy, to analyze.
What are the examples of elements with predictable electron configurations?
All of the representative elements (s and p block) have predictable electron configurations. However, many of the transition elements have electron configurations that are not predicted by the rules for determining electron configuration.
What elements has a ground-state electron configuration different from the predicted one?
Transition metals have ground-state electron configurations that differ from the predicted ones due to the exchange of electrons between the ns and (n-1)d subshells. This exchange stabilizes the d orbitals, leading to configurations that are closer to half-filled or fully filled d subshells. Examples include chromium ([Ar] 3d^5 4s^1) and copper ([Ar] 3d^10 4s^1).
What are examples of elements with one as their valency i.e.give examples of monovalent elements.?
Examples of monovalent elements include hydrogen, sodium, and potassium. These elements have one valence electron, which allows them to easily form ions with a +1 charge.
Argon Helium and Neon are examples of?
Noble gases. They are colorless, odorless, and have low chemical reactivity due to their stable electron configurations. They are commonly used in applications such as lighting, cooling, and insulation.
What is the name of an element with a full electron shell?
There are 7 known elements with full electron shells, six of which are referred to as noble gases because they are, generally, unreactive with other elements because of their full electron shells (their full electron shells make them resistant to forming bonds with other atoms to form molecules): Helium, Neon, Argon, Krypton, Xenon, and Radon. Ununoctium (element 118) also has a full electron shell, but due to relativistic effects is believed to be a solid at room temperatures (if there were enough atoms of it; it is extremely unstable with a half-life of less than a tenth of a second) so may not be considered a noble gas (all the other known elements with full electron shells are gases at room temperature) but, discounting radioactive decay which causes Ununoctium atoms to fission into lighter, reactive ones, is not chemically reactive with other elements.
Which elements are likely to combine chemically?
Elements with similar electronegativities and valence electron configurations are likely to combine chemically. This is because they tend to form stable compounds by either sharing electrons (covalent bonding) or transferring electrons (ionic bonding) to achieve a more stable electron configuration. Examples include hydrogen and oxygen combining to form water (H2O) through covalent bonding, or sodium and chlorine combining to form sodium chloride (NaCl) through ionic bonding.
Which elements would likely for anions with a -1 charge?
Elements in group 17 of the periodic table, known as the halogens, are likely to form anions with a -1 charge. Examples include fluorine, chlorine, and iodine. These elements have 7 valence electrons and tend to gain one electron to achieve a stable electron configuration.
Which atoms form ionic compound?
Atoms that form ionic compounds typically involve elements with large differences in electronegativity. This results in one atom donating electrons to another to achieve stable electron configurations. Common examples include metals like sodium donating electrons to nonmetals like chlorine to form sodium chloride.
Were the Greek gods good examples of leaders?
They were not, as they were often moody and unpredictable.
What are the example of inner transition element?
The inner transitional metals contain 2 main groups, the lanthanide series, and the actinide series (f block elements). The lanthanide series include the 14 elements that proceed lanthanum (atomic number 57) from atomic numbers 58 to 71. Their electron configuration include the 4f and 5d energy levels. Because of the closeness of those two levels, there is considerable uncertainty in some electron configuration assignments. The actinide series include the 14 elements that proceed actinium (atomic number 89) from atomic numbers 90 to 103. The electron configurations of the actinides are even more uncertain than the lanthanides because the closeness of the energy levels and because the nuclei are unstable to radioactive decay. Only minute amounts of some elements are obtained because of their instability. All of the actinides are unstable with respect to alpha emission. The later members tend to undergo spontaneous fission, a fact which limits the number of elements possible.
What compounds form single covalent bonds?
Elements in group 17 need one electron to gain a stable electron configuration. Two atoms of the same element or two elements in this family forms compounds with a single covalent bond. Examples are chlorine, bromine or iodine chloride.
Which elements have positive electron gain enthalpy?
It should be Fluorine but Chlorine has most EGE value because the F atom has very small sizeas compared to Cl. Addition of extra electron creates higher electron density and thus strong electron - electron repulsion comes into act. So extra electron is not accepted with the same ease as in the case of remaining elements of the group
