Chapter 3- Bonding Flashcards

1
Q

Incomplete octet

A

Exception to octet rule, where element is stable with less than 8 valence electrons.

H, He, Li -2
Be -4
B -6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Expanded octet

A

Any element in period three can hold more than 8 electrons but optimizing their d subshell.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Odd # electrons

A

Compounds with odd number of electrons cannot distribute electrons to have eight on each element.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Ionic bond

A

Is formed via the transfer of one or more electrons from an element of relatively low IE (ionization energy). To an element of high electron affinity.

Occur btw elements with large differences in their electronegativities. 🔼EN > 1.7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Cation

A

Positively charged ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Anion

A

Negatively charged ion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Crystalline lattices

A

Large organized arrays of ions which form in ionic compounds in solid state.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Covalent bonds

A

Formed via the sharing of electrons bye two elements of similar electronegativities.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Bond order

A

Refers to whether a bond is single/double/triple.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Bond order increases as…

A

Bond strength increases.

Bond length decreases.

Bond energy increases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Nonpolar bond

A

Results in molecules which both have relatively similar electronegativities. Equal sharing of electrons. 🔼EN

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Polar bond

A

When a significant difference in electronegativities to cause unequal sharing. 🔼EN 0.5-1.7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Coordinate covalent

A

Results when a single atom provides both bonding electrons while the other atom does not contribute any.

Most often occurs in acid-base reactions.

Acid gives H+, base accepts H+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Formal charge

A

=V - B/2 -NB

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

VSEPR

A

Predicts the 3-D molecular geometry of covalently bonded molecules.

Electronic vs. Molecular geometry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Sigma bonds

A

Are result of head to head overlap

17
Q

Pi bonds

A

Are the result of the overlap of two parallel cloud densities.

18
Q

Intermolecular forces

A

Are electrostatic attractions between molecules.

Significantly weaker than covalent bonds.

19
Q

London dispersion forces.

A

Weakest.

Vander wall force.

As size of atom or structure increases so does these forces.

Geico

20
Q

Dipole-dipole forces

A

Evident in solid and liquid phases, but negligible in gas phase due to distance of particles.

21
Q

H-bond

A

Specialized dipole-dipole attractions involved in intra/intermolecular attraction.

H bonded to very electronegative atoms. (O, N, F).

22
Q

Octet rule

A

States that elements will be more stable with eight valence electrons.