PLEASE HURRY 1.
_ result when two or more Lewis structures can be drawn from a single molecular formula (blending them).:
_ result when two or more Lewis structures can be drawn from a single molecular formula (blending them).
2.
When electron s, p, or d orbitals directly overlap a _ bond forms.:
When electron s, p, or d orbitals directly overlap a _ bond forms.
3.
When p-orbitals overlap from two atoms to allow sharing of electrons allowing double and even triple bonds, they are called a(n) _.:
When p-orbitals overlap from two atoms to allow sharing of electrons allowing double and even triple bonds, they are called a(n) _.
4.
A(n) _ is characterized by the equal sharing of electrons between two atoms (electronegativity that has less than or equal to 0.4).:
A(n) _ is characterized by the equal sharing of electrons between two atoms (electronegativity that has less than or equal to 0.4).
5.
_ use chemical symbols and show valence electrons of covalently bonded atoms.:
_ use chemical symbols and show valence electrons of covalently bonded atoms.
6.
_ are shared between two atoms that are joined in a covalent bond.:
_ are shared between two atoms that are joined in a covalent bond.
7.
Valence electrons in an atom that do not participate in combining electrons between two atoms are called _.:
Valence electrons in an atom that do not participate in combining electrons between two atoms are called _.
8.
The _ is the general principle that atoms of nonmetals tend to be most stable when their valence shells are filled.:
The _ is the general principle that atoms of nonmetals tend to be most stable when their valence shells are filled.
9.
A(n) _ is characterized by bonding electrons having greater association with one atom than another atom (electronegativity or greater than or equal to 0.5).:
A(n) _ is characterized by bonding electrons having greater association with one atom than another atom (electronegativity or greater than or equal to 0.5).
10.
_ form when two nonmetals share valence electrons.:
_ form when two nonmetals share valence electrons.
Column B
a. Bonding Electrons
b. Nonbonding Electrons
c. Nonpolar Bond
d. Octet Rule
e. Pi Bond
f. Covalent Bonds
g. Polar Bond
h. Resonance Structures
i. Lewis Structure
j. Sigma