Part A
Electronegativity.
Electronegativity describes the degree to which an element attracts electrons.
Part B
Anion and cation.
When two atoms form a bond with a complete transfer of electrons from one atom to the other, one atom becomes an anion (negatively charged) and the other becomes a cation (positively charged).
Part C
Oxygen holds electrons more tightly than hydrogen does, and the net charge is zero.
In a water molecule (Hâ‚‚O), the oxygen atom's higher electronegativity means it holds the shared electrons more tightly than the hydrogen atoms, but the overall charge of the molecule remains neutral.
Part D
A hydrogen atom is transferred to the atom that loses an electron.
This statement is not true of most cellular redox reactions, as they typically involve the transfer of electrons rather than entire hydrogen atoms.
Part E
Ionic.
Lithium and fluorine combine to form lithium fluoride through an ionic bond due to the transfer of electrons.
Part F
Hydrogen, polar.
In the reaction, hydrogen is oxidized (it loses electrons), and the resulting water molecule has polar covalent bonds due to the difference in electronegativity between hydrogen and oxygen.