Electronegativity is a value that describes the relative strength with which an atom of an element attracts electrons to itself in a chemical bond. The higher the electronegativity value, the more strongly an element can attract electrons to itself in a bond. The electrons in a chemical bond will be more attracted to the element that is more electronegative.
Remember that metals like to lose their valence electrons in an ionic bond. Metals have low electronegativity values. Nonmetals like to gain electrons in an ionic bond. Nonmetals have higher electronegativity values than metals.
Noble gases do not have electronegativity values because they do not bond with other elements.
Read each statement below and decide if it is TRUE or FALSE. Use the information and the chart above to help you answer each question.
Column A
1.
Electronegativity values decrease as you move left to right across a period.
:
Electronegativity values decrease as you move left to right across a period.
2.
Electronegativity values decrease as you move down (top to bottom) in a group.
:
Electronegativity values decrease as you move down (top to bottom) in a group.
3.
The least electronegative elements are found in the bottom left corner of the periodic table.
:
The least electronegative elements are found in the bottom left corner of the periodic table.
4.
Francium is the most electronegative element.
:
Francium is the most electronegative element.
5.
Phosphorous (P) is more electronegative than nitrogen (N).
:
Phosphorous (P) is more electronegative than nitrogen (N).
6.
In a covalent bond between Sulfur (S) and Chlorine (Cl), the shared electrons would be more attracted to chlorine because it has a higher electronegativity.
:
In a covalent bond between Sulfur (S) and Chlorine (Cl), the shared electrons would be more attracted to chlorine because it has a higher electronegativity.
Column B
a.False
b.True
1. b.True
2. b.True
3. b.True
4. a.False
5. b.True
6. b.True