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Electronegativity is a fundamental concept in the field of chemistry that helps us understand the nature of chemical bonds and the behavior of atoms. It is a measure of an atom’s ability to attract and hold onto electrons when involved in a chemical bond. By calculating electronegativity, we can determine the polarity of a bond and predict the relative distribution of electrons between atoms. In this article, we will delve into the methods and formulas used to calculate electronegativity, providing a clear understanding of this essential concept for anyone interested in chemistry.
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In chemistry, electronegativity is the unit of measurement for the attraction of an atom to an electron in a chemical bond. [1] X Source of Research A highly electronegative atom will attract electrons with a strong force, whereas a low electronegativity atom will attract electrons with a weak force. Electronegativity values are used to predict the ability to form chemical bonds between atoms, so this is an important skill in basic chemistry.
Steps
Basic knowledge of electronegativity
- This article does not cover the exact reason why atoms share electrons and have bonds between them. If you want to learn more, read this article on chemical bonding or the wikiHow article on How to Study Chemical Bonding Properties.
- For example, in the NaCl (sodium chloride) molecule, the chlorine atom has a relatively high electronegativity and the sodium atom has a relatively low electronegativity. Hence the electrons are pulled towards the chlorine atom and away from the sodium atom .
- This is the connection that leads to the electronegativity lookup table. Note that this table uses the Pauling electronegativity scale, which is the most common electronegativity scale. [2] X Research Sources However, there are other ways to measure electronegativity, and some of these will be discussed below.
- The electronegativity of an atom increases as you move to the right of the periodic table.
- The electronegativity of an atom gets higher as you move up the periodic table.
- Therefore, the atoms in the upper right corner have the most electronegativity, and the atoms in the lower left corner have the least electronegativity.
- In the NaCl example above, you probably know chlorine is more electronegative than sodium because it is located very close to the top right corner of the periodic table. In contrast, sodium is far to the left so it belongs to the group of atoms with low electronegativity.
Determine bond type by electronegativity
- Taking the HF molecule as an example, we will subtract the electronegativity of fluorine (4,0) from the electronegativity of hydrogen (2,1). 4.0 – 2.1 = 1.9 .
- For example, the molecule O 2 has this type of bond. Since two oxygen atoms have the same electronegativity, their difference is zero.
- The molecule H 2 O (water) is a good example of this. The O atom is more electronegative than the two H atoms, so it holds the electrons more tightly, and causes the entire molecule to carry a partial negative charge at the O end and a partial positive charge at the H end.
- An example is the molecule BaCl (sodium chloride). The chlorine atom has such a large negative charge that it pulls both electrons completely towards it, leaving sodium with a positive charge.
- Metallic elements include most of the elements located to the left and middle of the periodic table. This page has a table showing which elements are metallic. [5] X Research Sources
- The HF example above falls within this range. Since H and F are not metals, they have polar covalent bonds.
Find electronegativity according to Mulliken
- Perhaps you should look up this parameter in the chemical reference literature. This page provides a lookup table that you can use (scroll down to see). [6] X Research Source
- For example, suppose we need to find the electronegativity of lithium (Li). Looking at the table on the above page, we see that the first ionization energy is 520 kJ/mp .
- The electron affinity of lithium is 60 kJ mp -1 .
- In this example, we will solve the following:
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- EN Mulliken = (1.97×10 −3 )(E i +E ea ) + 0.19
- EN Mulliken = (1.97×10 −3 )(520 + 60) + 0.19
- EN Mulliken = 1.143 + 0.19 = 1.333
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Advice
- In addition to the Pauling and Mulliken scales, some other electronegativity scales are the Allred–Rochow, Sanderson, and Allen scales. All of these scales have their own equations for calculating electronegativity (some are quite complicated).
- Electronegativity has no units .
wikiHow is a “wiki” site, which means that many of the articles here are written by multiple authors. To create this article, 15 people, some of whom are anonymous, have edited and improved the article over time.
There are 7 references cited in this article that you can view at the bottom of the page.
This article has been viewed 79,012 times.
In chemistry, electronegativity is the unit of measurement for the attraction of an atom to an electron in a chemical bond. [1] X Source of Research A highly electronegative atom will attract electrons with a strong force, whereas a low electronegativity atom will attract electrons with a weak force. Electronegativity values are used to predict the ability to form chemical bonds between atoms, so this is an important skill in basic chemistry.
In conclusion, calculating electronegativity is an essential tool in understanding the nature of chemical bonding and predicting the behavior of atoms in a compound. By using the Pauling scale or various other methods, scientists and chemists can assign a quantitative value to an atom’s ability to attract electrons. This value plays a crucial role in determining the polarity of a molecule, predicting bond types, and understanding the reactivity of different compounds. Additionally, electronegativity values allow for the comparison of different elements and provide valuable insights into their chemical properties. Although electronegativity is a complex concept, its calculation can be easily understood and applied using the principles and techniques discussed in this paper. Overall, the knowledge of electronegativity greatly enhances our understanding of chemical behavior and empowers scientists to make important predictions and discoveries in the field of chemistry.
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