chapter 8

Question 1

covalent bonds are a

Answer 1

sharing of electrons that form molecules

Question 2

covalent bonds…

Answer 2

share electrons and involves only nonmetals

Question 3

Compounds that are bonded covalently are called

Answer 3

molecular compounds

Question 4

molecular compounds have

Answer 4

lower melting and boiling points than ionic

Question 5

molecular compounds tend to be

Answer 5

gases or liquids at room temperature

Question 6

molecular formula

Answer 6

Shows how many atoms of each element a molecule contains

Question 7

double bond

Answer 7

is when atoms share two pairs of electrons (4 total)

Question 8

triple bond

Answer 8

is when atoms share three pairs of electrons (6 total)

Question 9

Bond Dissociation Energies…

Answer 9

The total energy required to break the bond between 2 covalently bonded atoms

Question 10

High dissociation energy usually means

Answer 10

the chemical is relatively unreactive, because it takes a lot of energy to break it down.

Question 11

Resonance is…

Answer 11

When more than one valid dot diagram is possible

Question 12

The 3 Exceptions to Octet rule

Answer 12

1. odd number of valence electrons
2. boron and berillyum
3. in period 3 or beyond

Question 13

sigma bond

Answer 13

when two atomic orbitals combine to form the molecular orbital that is symmetrical along the axis connecting the nuclei

Question 14

pi bond

Answer 14

the bonding electrons are likely to be found above and below the bond axis (weaker than sigma)

Question 15

shared evenly

Answer 15

nonpolar covalent bond

Question 16

shared unevenly

Answer 16

polar covalent

Question 17

electronegativity increases

Answer 17

as you go up and to the right

Question 18

diatomic defeniton

Answer 18

made of two atoms

Question 19

which atoms are diatomic?

Answer 19

Hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, bromine
Have no fear of ice cold beer

Question 20

Bond lent:

Answer 20

distance between 2 atoms where sharing is optimal and repulsion between two nuclei is negligible

Question 21

how to draw lewis structures

Answer 21

1. Count number of valence electrons
2. First element listed is central element, carbon always and hydrogen never
3. Draw single bonds
4. Assign remaining electrons to outside atoms first until octet then the central
5. Check for octet and draw double or triple bonds as needed/resonance

Question 22

extended octet:

Answer 22

element has more than 8 electrons in lewis structure, only possible for elements period 3 and down, because they have available d’orbitals

Question 23

intramolecular bonds:

Answer 23

bonds within molecule (polar/nonplar)

Question 24

intermolecular bonds:

Answer 24

bonds between 2 molecules

Question 25

dipole-dipole

Answer 25

between 2 polar bonds

Question 26

LDF

Answer 26

between 2 nonpolar bonds

Question 27

H-bond

Answer 27

bond must have H-O, H-N, H-F

Question 28

bonds strongest to weakest

Answer 28

hydrogen bond
dipole
ldf
in large amount ldf can be stronger than dipole

Question 29

structural formula

Answer 29

chemical formula that shows the arrangement of atoms in molecules and polyatomic ions

Question 30

dispersion force

Answer 30

interaction caused y the motion of electrons

Question 31

network solid

Answer 31

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

Question 32

coordinate covalent bond

Answer 32

a covalent bond in which the shared electron pair comes from only one of the atoms

Question 33

bonding orbital

Answer 33

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

Question 34

sigma bond

Answer 34

symmetrical bond along the axis between the two nuclei

Question 35

VSEPR theory

Answer 35

shapes adjust so valence-electron pairs are as far apart as possible

Question 36

network solid

Answer 36

crystal in which all the atoms are covalently bonded to each other

Question 37

How do atoms achieve noble-gas electron configurations in single covalent bonds?

Answer 37

Two atoms share two electrons.