LS 7A w1 atoms, bonds, polarity

Ionic bonds

Bonds formed between oppositely charged ions, full charge

Covalent bonds

Bonds formed by sharing electrons between atoms

Hydrogen sharing

Hydrogen shares 1 pair of electrons

Carbon sharing

Carbon shares 4 pairs of electrons

Nitrogen sharing

Nitrogen shares 3 pairs of electrons

Oxygen sharing

Oxygen shares 2 pairs of electrons

Double bonds

Bonds where 4 electrons are shared

Triple bonds

Bonds where 6 electrons are shared (strongest covalent bond)

Electronegativity

Measure of how much an atom attracts electrons, higher values->stronger attraction

Nonpolar

Electrons shared equally, no charges on atoms, hydrophobic

Polar

Electrons shared unequally, partial charges, hydrophilic

Amphipathic

Molecules with both polar and nonpolar regions

Polarity

Indicates how molecules interact, e.g., why oils & water don't mix

Hydrogen bonds

Form when partially positively charged H interacts with partially charged negative atoms

Van der Waals forces

Electron interactions between atoms that have temporary partial charge

Strength of a bond/interaction

Weaker as potential energy gets closer to 0

are ionic bonds hydrophillic or hydrophobic

hydrophillic

hydrogen and carbon have

lower electronegativity

nitrogen and oxygen have

higher electronegativity