Electronegativity and Bond Types Flashcards
What is the trend in electronegativity across a period on the periodic table?
Electronegativity increases from left to right across a period.
What is the trend in electronegativity down a group on the periodic table?
Electronegativity decreases as you move down a group.
How does the size of an atom relate to its electronegativity?
Smaller atoms have higher electronegativity because the nucleus exerts a stronger pull on electrons.
What type of bond forms between two atoms with a large difference in electronegativity?
Ionic bond.
What type of bond forms between two atoms with a small difference in electronegativity?
Polar covalent bond.
What type of bond forms between two atoms with no or very little difference in electronegativity?
Non-polar covalent bond.
Rank these bonds from least to most polar: hydrogen-chlorine, oxygen-nitrogen, carbon-sulfur, sodium-chlorine.
Carbon-sulfur < oxygen-nitrogen < hydrogen-chlorine < sodium-chlorine.
What type of force holds together ionic compounds?
Electrostatic attraction between cations and anions.
What is metallic bonding?
A bonding type where valence electrons move freely between metal atoms, creating an attraction between the electron cloud and positively charged nuclei.
Where on the periodic table are the most electronegative elements found?
The most electronegative elements are found in the upper right corner of the periodic table, excluding noble gases.
Which group of elements has the lowest electronegativity values?
Alkali metals (Group 1) have the lowest electronegativity values.
What is the most electronegative element?
Fluorine.
How do you use the electronegativity table to predict bond types?
By comparing electronegativity values of two elements: a difference of 0-0.4 indicates a non-polar covalent bond, 0.5-1.7 indicates a polar covalent bond, and greater than 1.7 indicates an ionic bond.
