Chapter 8 Vocabulary

Question 1

bond dissociation energy

Answer 1

the energy required to break the bond between two covalently bonded atoms; this value is usually expressed in kJ per mol of substance

Question 2

bonding orbital

Answer 2

a molecular orbital that can be occupied by two electrons of a covalent bond

Question 3

covalent bond

Answer 3

a bond formed by the sharing of electrons between atoms

Question 4

coordinate covalent bond

Answer 4

a covalent bond in which one atom contributes both bonding electrons

Question 5

diatomic molecule

Answer 5

a molecule consisting of two atoms

Question 6

dipole

Answer 6

a molecule that has two poles, or regions with opposite charges

Question 7

dipole interactions

Answer 7

intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules

Question 8

dispersion forces

Answer 8

attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules

Question 9

double covalent bond

Answer 9

a bond in which two atoms share two pairs of electrons

Question 10

hybridization

Answer 10

the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

Question 11

hydrogen bonds

Answer 11

attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom

Question 12

molecular compound

Answer 12

a compound that is composed of molecules

Question 13

molecular formula

Answer 13

a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound

Question 14

molecular orbital

Answer 14

an orbital that applies to the entire molecule

Question 15

molecule

Answer 15

a neutral group of atoms joined together by covalent bonds

Question 16

network solid

Answer 16

a solid in which all of the atoms are covalently bonded to each other

Question 17

nonpolar covalent bond

Answer 17

a covalent bond in which the electrons are shared equally by the two atoms

Question 18

pi bond

Answer 18

a covalent bond in which the bonding electrons are most likely to be found in sausage-shape regions above and below the bond axis of the bonded atoms

Question 19

polar covalent bond/polar bond

Answer 19

polar bond; a covalent bond between atoms in which the electrons are shared unequally

Question 20

polar molecule

Answer 20

a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive

Question 21

polyatomic ion

Answer 21

a tightly bound group of atoms that behaves as a unit and has a positive or negative charge

Question 22

resonance structure

Answer 22

one of the two or more equally valid electron dot structures of a molecule or polyatomic ion

Question 23

sigma bond

Answer 23

a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei

Question 24

single covalent bond

Answer 24

a bond formed when two atoms share a pair of electrons

Question 25

structural formula

Answer 25

a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion; each dash between a pair of atoms indicates a pair of shared electrons

Question 26

tetrahedral angle

Answer 26

a bond angle of 109.5 degrees that results when a central atom forms four bonds directed toward the center of a rectangular tetrahedron

Question 27

triple covalent bond

Answer 27

a bond in which three pairs of electrons are shared by two atoms

Question 28

unshared pair

Answer 28

a pair of valence electrons that is not shared between atoms

Question 29

van der Waals forces

Answer 29

the two weakest intermolecular attractions- dispersion interactions and dipole forces

Question 30

VSEPR theory

Answer 30

valence shell electron-pair repulsion theory; because electrons pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible