Chapter 8

Question 1

How does matter take form in nature?

Answer 1

In many forms

Question 2

Covalent Bond

Answer 2

Sharing electrons.

Question 3

Molecule

Answer 3

A group of atoms joined by covalent bonds.

Question 4

Diatomic Molecule

Answer 4

A molecule consisting of two of the same atoms.

Question 5

Molecular Compound

Answer 5

Compounds composed of molecules.

They have relatively lower melting and boiling points.

Question 6

Molecular Formula

Answer 6

The chemical formula of a molecular compound.

Question 7

In covalent bonds, why does electron sharing occur?

Answer 7

To attain the electron configuration of a noble gas.

Question 8

Single Covalent Bond

Answer 8

Two atoms held together by sharing a pair of electrons.

Question 9

Structural Formula

Answer 9

Represents the covalent bonds by dashes and shows the arrangement of the covalently bonded atoms.

Question 10

Unshared Pair

Answer 10

A pair of valence electrons that are not shared between atoms.

Question 11

Double Covalent Bond

Answer 11

A bond that involves two shared pairs of electrons.

Question 12

Triple Covalent Bond

Answer 12

A bond by sharing three pairs of electrons.

Question 13

Diatomic Elements

Answer 13

Hydrogen, Nitrogen, Oxygen, and group 17.

Question 14

Coordinate Covalent Bond

Answer 14

A covalent bond in which one atom contributes both bonding electrons.

Question 15

Polyatomic Ion

Answer 15

Tightly bonded group of atoms that has a charge and behaves as a unit.

Question 16

Bond Dissociation Energy

Answer 16

The energy required to break the bond between two covalently bonded atoms.

Question 17

Resonate

Answer 17

Electron pairs rapidly flip back and forth between atoms.

Question 18

Resonance Structure

Answer 18

The structure that occurs when it is possible to draw two or more valid electron got structures.

Question 19

When can the octet rule not be satisfied?

Answer 19

IN molecules whose total number of valence electrons is an odd number.

Question 20

Molecular Orbitals

Answer 20

Orbitals that apply to the entire molecule.

Question 21

Bonding Orbital

Answer 21

Molecular orbital that can be occupied by two elements of a covalent bond.

Question 22

Sigma Bond

Answer 22

Two atomic orbital combines to form a molecular orbital.

Question 23

Pi Bond

Answer 23

Bonding electrons are most likely to be found in the sausage-shaped regions.

Question 24

What is weaker, Pi or Sigma?

Answer 24

A pi bond is weaker than sigma.

Question 25

VSEPR Theory

Answer 25

Valence shell electron pair repulsion theory.

The repulsion between electron pairs causes molecular shapes.

Question 26

Orbital Hybridization

Answer 26

Provides info about both molecular bonding and molecular shape.

Question 27

Hybridization

Answer 27

Atomic orbitals mix to form the same total number of equivalent hybrid orbitals.

Question 28

Non-Polar Covalent Bond

Answer 28

Bonding electrons are shared equally.

Question 29

Polar Covalent Bond

Answer 29

Electrons are shared unequally.

Question 30

Polar Molecule

Answer 30

One end of the molecule is slightly negative while the other end is slightly positive.

Question 31

Dipole/Dipolar Molecule

Answer 31

Has two poles

Question 32

Can molecules attract by a variety of forces?

Answer 32

Yes

Question 33

Are intermolecular attractions stronger or weaker than ionic or covalent bonds?

Answer 33

Weaker

Question 34

Skip

Answer 34

Consists of two forces

Question 35

Dipole Interactions

Answer 35

Occurs when polar molecules are attracted to one another.

Question 36

Dispersion Forces

Answer 36

Caused by the motion of electrons.

Question 37

Hydrogen Bonds

Answer 37

Hydrogen is attracted to negative oxygen and its electrons.
This is extremely important in determining the properties of water.
Important in proteins.

Question 38

Network Solids/ Network Crystals

Answer 38

Solids in which all of the atoms are covalently bonded to each other.
Example diamond.