Electronegativity is a measure of how strongly atoms attract bonding electrons to themselves. The higher the electronegativity, greater is an atom's attraction for electrons. Given below is a list of elements and their electronegativity value. Element Electronegativity Value(Pauling scale)H 2.2Li 1.0Be 1.6B 2.0C 2.6N 3.0O 3.4F 4.0Na 0.9 Q 1.3Identify which periods and groups are represented by the elements listed and explain the trends in the electronegativity shown in the table.
Question
Electronegativity is a measure of how strongly atoms attract bonding electrons to themselves. The higher the electronegativity, greater is an atom's attraction for electrons. Given below is a list of elements and their electronegativity value. Element Electronegativity Value(Pauling scale)H 2.2Li 1.0Be 1.6B 2.0C 2.6N 3.0O 3.4F 4.0Na 0.9 Q 1.3Identify which periods and groups are represented by the elements listed and explain the trends in the electronegativity shown in the table.
Solution
The elements listed in the table represent two periods and several groups from the Periodic Table.
Period 2: Li, Be, B, C, N, O, F Period 3: Na
Group 1: Li, Na Group 2: Be Group 13: B Group 14: C Group 15: N Group 16: O Group 17: F Group 1 (Hydrogen is unique): H
The trend in electronegativity in the Periodic Table is that it generally increases as you move from left to right across a period and decreases as you move down a group.
Looking at the periods in the table, you can see this trend. In Period 2, electronegativity increases from Li (1.0) to F (4.0). In Period 3, we only have Na (0.9), but it follows the trend of being less electronegative than its counterpart in Period 2, Li (1.0).
Looking at the groups, you can also see the trend. For example, in Group 1, electronegativity decreases from Li (1.0) in Period 2 to Na (0.9) in Period 3.
The reason for these trends is due to atomic size and the number of protons in the nucleus. As you move across a period from left to right, the number of protons increases, which increases the positive charge of the nucleus and pulls the electrons closer to the nucleus, increasing electronegativity. As you move down a group, the atomic size increases, and the outer electrons are further from the nucleus and less attracted to it, decreasing electronegativity.
Similar Questions
Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.It is important to realise that a lot of what we know about the structure of atoms has been developed over a long period of time. This is often how scientific knowledge develops, with one person building on the ideas of someone else. Nowadays, we know that atoms are made up of a positively charged nucleus in the centre surrounded by negatively charged electrons. The number of electrons determines the atomic number of an atom. The number of electrons on the outermost shell determines the valency of an atom.Given below is the atom of an element sodium. Oorka. “3D Render of Atom Structure of Sodium Isolated over White Background...” IStock, https://www.istockphoto.com/photo/sodium-gm639850140-115565943 Q 1.1A 3State the number of subatomic particles present in a sodium ion No. of protons =No. of neutrons =No. of electrons =
define electronegativity of atoms and explain its influence onbonding
Which of the following correctly describes electronegativity? A measure of the repulsion between the valence electrons of an atomThe level of electron shielding in an atomThe energy difference between energy levelsA measure of the attraction between an atom and bonding electrons
Which of the following describes the trends in electronegativity?It decreases across periods but increases down groupsIt increases across periods but decreases down groupsIt decreases across periods and down groupsIt increases across periods and down groups
Which of the following set of elements shows an order of increasing electronegativity trend?
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