Electronegativity and Bond Types Explained

What is the definition of electronegativity?

• The mass of an atom

• The tendency of an atom to attract a shared pair of electrons

• The number of protons in an atom

• The ability of an atom to donate electrons

How do electronegativity values change across the periodic table?

• Decrease from top to bottom and right to left

• Increase from bottom to top and left to right

• Decrease from bottom to top and left to right

• Increase from top to bottom and right to left

What is the electronegativity difference range for a polar covalent bond?

• 2.5 to 4.0

• 1.7 to 2.5

• 0.4 to 1.7

• 0 to 0.4

In a nonpolar covalent bond, how are the bonding electrons shared?

• Equally between atoms

• Not shared at all

• Transferred from one atom to another

• Unequally between atoms

What is the electronegativity difference between hydrogen and chlorine in a polar covalent bond?

• 1.7

• 1.2

• 0.8

• 0.4

What type of bond is formed when sodium transfers its valence electron to chlorine?

• Ionic

• Polar covalent

• Nonpolar covalent

• Metallic

What does the term 'continuum of bond character' refer to?

• The range of bond angles

• The range of bond lengths

• The range of bond types from nonpolar to ionic

• The range of bond energies

What must be considered to determine the character of a molecule with more than two atoms?

• Only bond polarity

• Only the number of atoms

• Only molecular shape

• A variety of factors including bond polarity

At what electronegativity difference does polarity begin to appear as a macro property?

• 0.6

• 0.4

• 0.2

• 0.8

Why is it not possible to achieve 100% ionic character in a bond?

• Because electrons are always shared equally

• Because atoms cannot transfer electrons

• Because the resulting positive ion will always attract electrons back to it

• Because ionic bonds do not exist