What is electronegativity? a) List the following atoms in order of increasing electronegativity: O, Al, Ca b) List the following atoms in order of decreasing electronegativity: Cl, K, Cu .
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Explanation:
As you move up a group, electronegativity increases; likewise, electronegativity increases when moving from left to right across a period.
Option a) is eliminated from the start, since fluorine is actually the most electronegative element in the periodic table.
Option b) starts off well, with rubidium (EN = 0.82), calcium (1.00) and scandium (1.36), but then ends with cesium (0.79), which is the least electronegative of the group.
Likewise, option c) starts off well, with zirconium (1.33), vanadium (1.63), and niobium (1.6), but ends on tantalum (1.5), which has a lower EN value than niobium.
Option d) is correct, since it progresses through tin (1.96), arsenic (2.18), phosphorus (2.19), and sulfur (2.58).
Option e) ends on the right element, fluorine (4.0), but starts off in order of decreasing EN values - lithium (0.98), sodium (0.93), and potassium (0.82).
So, if EN values are not available to you, use the aforementioned trends, but keep an eye out for transition metals, since a lot of them do not follow these trends exactly.
Electronegativity:
The tendency of an atom in a molecule to draw the shared pair of electrons closer to itself is called electronegativity.
It is a dimensionless assets due to the fact it's miles most effective a tendency. It essentially shows the internet end result of the inclinations of atoms in one of a kind factors to draw the bond-forming electron pairs. We degree electronegativity on numerous scales. The maximum normally used scale changed into designed via way of means of Linus Pauling.
(or)
Electronegativity is the assets of an atom which will increase with its tendency to draw the electrons of a bond. If bonded atoms have the equal electronegativity values as every other, they proportion electrons similarly in a covalent bond. Usually, the electrons in a chemical bond are extra attracted to 1 atom (the extra electronegative one) than to the opposite. This consequences in a polar covalent bond. If the electronegativity values are very different, the electrons aren`t shared at all. One atom basically takes the bond electrons from the opposite atom, forming an ionic bond.
a) In a period, as the size decreases, electronegativity increases due to the increase in effective nuclear charge.
Ca<Al<O
b) K<Cu<Cl
Electronegativity increases across the periodic table (to the right).
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