Chemistry Chapter 9

Front 1

Covalent Bond

Back 1

Chemical bond between two nonmetals in which electrons are shared

Front 2

Molecule

Back 2

Formed when two or more atoms bond covalently

Front 3

Pure Covalent Bond

Back 3

Both nonmetals have the same electronegativity and share electrons equally

Front 4

What are the 7 diatomic molecules? (Molecules that are found with two atoms in nature)

Back 4

1. H2 - Hydrogen
2. N2 - Nitrogen
3. O2 - Oxygen
4. F2 - Fluorine
5. Cl2 - Chlorine
6. Br2 - Bromine
7. I2 - Iodine

Front 5

Sigma Bond

Back 5

Single covalent bond that occurs when the electron pair is shared in an area centered between two atoms

Front 6

What are the three ways a sigma bond can form?

Back 6

1. Overlap s orbital and s orbital
2. Overlap s orbital and p orbital
3. Overlap p orbital and p orbital

Front 7

Lewis Dot Structures

Back 7

Shows placement of valence electrons to form covalent bonds and the possible geometry of the nucleus

Front 8

Multiple Covalent Bonds

Back 8

Formed when more than one pair of electrons are shared

Front 9

Pi bond

Back 9

Parallel orbitals overlap to share electrons

Front 10

What bonds does a double covalent bond consist of?

Back 10

1 sigma bond, 1 pi bond

Front 11

What bonds does a triple covalent bond consist of?

Back 11

1 sigma bond, 2 pi bonds

Front 12

What are all covalent bonds a balance between?

Back 12

Attractive forces between electrons and nuclei, and repulsive forces between nuclei and nuclei and electron and electron

Front 13

What is the strength of a single bond?

Back 13

2 electrons, longest, weakest

Front 14

What is the strength of a double bond?

Back 14

4 electrons, medium length, medium strength

Front 15

What is the strength of a triple bond?

Back 15

6 electrons, shortest, strongest

Front 16

Energy is ________ when a bond forms.

Back 16

Released

Front 17

Energy is _____ to break a bond.

Back 17

Taken

Front 18

Bond Dissociation Energy

Back 18

Amount of energy needed to break a specific covalent bond, always positive

Front 19

Endothermic

Back 19

Takes more energy to break the existing bonds than the energy given off when a new molecule forms

Front 20

Exothermic

Back 20

Takes less energy to break existing bonds than the energy given off when a new molecule forms

Front 21

How do you name the first and second element in nomenclature?

Back 21

First element- Use regular name from table
Second element- Ends in ide

Front 22

What are the exceptions to using prefixes?

Back 22

1. first element never uses mono
2. second element drops o if it begins with a vowel

Front 23

Oxyacids

Back 23

Polyatomic acids that contain Hydrogen

Front 24

How do you name oxyacids?

Back 24

-do not begin with "hydro"
-name using polyatomic ion
-ate to ic, and ite to ous
-make sure to write acid

Front 25

Structural Formula

Back 25

Uses letter symbols and bonds to show the relative positions of atoms

Front 26

Binary Acid

Back 26

Contains only hydrogen and one other element

Front 27

How do you name binary acids?

Back 27

Hydro + root + ic Acid

Front 28

Resonance

Back 28

Condition that occurs when more than once valid Lewis structure can be written for a molecule or ion

Front 29

Coordinate Covalent Bond

Back 29

One atom donates a pair of electrons to be shared with an atom that needs two electrons to become stable

Front 30

What are the rules for oxidation numbers in covalent molecules?

Back 30

1. pure element oxidation # = 0
2. more electronegative atom keeps its natural oxidation state - this will be the oxidation state of the electronegative element
3. all halogens = -1
4. oxygen = -2
5. hydrogen = +1

Front 31

Where does hybridization occur?

Back 31

In molecules

Front 32

What are hybridized single, double, and triple bonds called?

Back 32

single - sp
double - sp2
triple - sp3

Front 33

What are the four types of bonds?

Back 33

1. Ionic
2. Pure (Nonpolar) Covalent
3. Polar Covalent
4. Metallic

Front 34

How can you use electronegativity to predict bond type?

Back 34

1.70 and below = polar covalent
0 = pure covalent
1.70 and above = ionic

Front 35

Rules of Solubility

Back 35

Polar + Polar = soluble
Nonpolar + Nonpolar = soluble
Polar + Nonpolar = not soluble

Front 36

What is the glue that holds molecules together?

Back 36

Van der Waals Forces

Front 37

Dipole

Back 37

-strongest intermolecule force
-between polar molecules
-the greater the polarity, the stronger the dipole

Front 38

Hydrogen Bond

Back 38

-2nd strongest intermolecule force
-H attraction to F, N, O
-Because H is so small, the attraction force is extremely strong

Front 39

London Dispersion Force

Back 39

-weakest intermolecule force
-between non polar molecules
-typical of gases - volitile

Front 40

Characteristics of Diamonds (Covalent Network Solids)

Back 40

-very strong (big molecules)
-high melting point
-brittle
-non conductors
-extremely hard