Chemistry Chapter 3: Bonding and Chemical Interactions (3 Stars)

Question 1

Chemical bonds can be _____ or covalent.

Answer 1

ionic

Question 2

Elements will form _____ to attain a noble gas-like electron configuration.

Answer 2

bonds

Question 3

The octet rule states that elements will be most stable with ____ valence electrons.

Answer 3

eight

Question 4

Elements with an incomplete octet are stable with fewer than eight electrons and include H, He, __, Be, and B.

Answer 4

Li,

Question 5

Elements with an expanded octet are stable with more than eight electrons and include all elements in period _ or greater.

Answer 5

3

Question 6

Compounds with a(n) ____ number of electrons cannot have eight electrons on each element.

Answer 6

odd

Question 7

A(n) _____ bond is formed via the transfer of one or more electrons from an element with a relatively low ionization energy to an element with a relatively high electron affinity.

Answer 7

ionic

Question 8

Ionic bonds occur between elements with _____ differences in electronegativity (ΔEN ____ ), usually between metals and nonmetals.

Answer 8

large

(ΔEN > 1.7)

Question 9

A positively charged ion is called a ____. A negatively charged ion is called an _____.

Answer 9

cation.

anion.

Question 10

The resulting electrostatic attraction between the ions causes them to remain in _______ proximity , forming the bond.

Answer 10

close proximity

Question 11

Ionic compounds form ______ —large, organized arrays of ions.

Answer 11

crystalline lattices

Question 12

Ionic compounds tend to dissociate in ____ and other _____ solvents.

Answer 12

water

polar

Question 13

Ionic solids tend to have ____ melting points.

Answer 13

high

Question 14

A _____ bond is formed via the sharing of electrons between two elements of similar electronegativities.

Answer 14

covalent

Question 15

Bond order refers to whether a covalent bond is a single bond, double bond, or triple bond. As bond order increases, bond strength ______, bond energy increases, and bond length ______.

Answer 15

increases

decreases.

Question 16

Nonpolar bonds result in molecules in which both atoms have exactly the _____ electronegativity;

Answer 16

same
there is a very small difference in electronegativity between the atoms (ΔEN < 0.5), even though they are technically slightly polar.

Question 17

Polar bonds form when there is a ______ difference in electronegativities but not enough to transfer electrons and form an ionic bond.

Answer 17

significant
(ΔEN = 0.5 to 1.7),
In a polar bond, the more electronegative element takes on a partial negative charge, and the less electronegative element takes on a partial positive charge.

Question 18

Coordinate covalent bonds result when a single atom provides _____ bonding electrons while the other atom does not contribute any; coordinate covalent bonds are most often found in Lewis acid–base chemistry.

Answer 18

both

Question 19

Lewis dot symbols are a _____ representation of an atom’s valence electrons.

Answer 19

chemical

Question 20

Drawing a complete Lewis dot structure requires a balance of valence, _____, and nonbonding electrons in a molecule or ion.

Answer 20

bonding

Question 21

Formal charges exist when an atom is surrounded by more or fewer valence electrons than it has in its _____ state (assuming equal sharing of electrons in a bond).

Answer 21

neutral

Question 22

For any molecule with a π (pi) system of electrons, _____ structures exist; these represent all of the possible configurations of electrons—stable and unstable—that contribute to the overall structure.

Answer 22

resonance

Question 23

The valence shell electron pair repulsion (VSEPR) theory predicts the three-dimensional molecular geometry of ______ bonded molecules. characteristic geometries.

Answer 23

covalently
In this theory, electrons—whether bonding or nonbonding—arrange themselves to be as far apart as possible from each other in three-dimensional space, leading to characteristic geometries.

Question 24

Nonbonding electrons exert more ______ than bonding electrons because they reside closer to the nucleus.

Answer 24

repulsion

Question 25

Electronic geometry refers to the position of all electrons in a molecule, whether bonding or nonbonding. Molecular geometry refers to the position of only the ______ pairs of electrons in a molecule.

Answer 25

bonding pairs

Question 26

The polarity of molecules is ______ on the dipole moment of each bond and the sum of the dipole moments in a molecular structure.

Answer 26

dependent

Question 27

Nonpolar molecules may contain nonpolar bonds, or polar bonds with _____ moments that cancel each other.

Answer 27

dipole

Question 28

σ and π bonds describe the patterns of _____ observed when molecular bonds are formed.

Answer 28

overlap

Question 29

Sigma (σ) bonds are the result of ______ overlap.

Answer 29

head-to-head

Question 30

Pi (π) bonds are the result of the overlap of two _____ electron cloud densities.

Answer 30

parallel

Question 31

Intermolecular forces are ______ attractions between molecules. They are significantly weaker than covalent bonds (which are weaker than ionic bonds).

Answer 31

electrostatic

Question 32

London dispersion forces are the _____ interactions, but are present in all atoms and molecules.

Answer 32

weakest interactions, but are present in all atoms and molecules.
As the size of the atom or structure increases, so does the corresponding London dispersion force.

Question 33

______ interactions, which occur between the oppositely charged ends of polar molecules, are stronger than London forces; these interactions are evident in the solid and liquid phases but negligible in the gas phase due to the distance between particles.

Answer 33

Dipole–dipole

Question 34

______ are a specialized subset of dipole–dipole interactions involved in intra- and intermolecular attraction;

Answer 34

Hydrogen bonds
hydrogen bonding occurs when hydrogen is bonded to one of three very electronegative atoms— fluorine, oxygen, or nitrogen