General Chemistry Chapter 3: Bonding and Chemical Interaction Flashcards

1
Q

What does the octet rule state?

A

elements will be most stable with eight valence electrons

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

What are exceptions to the octet rule?

A
  • Elements with an incomplete octet are stable with fewer than eight electrons and include H, He, Li, Be and B
  • Elements with an expanded octet are stable with more than eight electrons (period 3 or greater)
  • Compounds with an odd number of electrons cannot have eight electrons on each element.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an ionic bond?

A

formed via the transfer of 1 or more electrons from an element with a relatively low ionization energy to an element with a relatively high electron affinity.

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

What types of elements generally form ionic bonds?

A

Generally forms between metals and nonmetals

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

What is a positively charged ion called? Negatively?

A
\+ = cation
- = anion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What doe ionic compound form? (structure)

A

Crystalline lattice - large organized arrays of ions

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

What are special properties of ionic compounds?

A

tend to dissociate in water and other polar substances

tend to have high melting points

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

What is a covalent bond?

A

sharing of electrons between elements of similar electronegativities

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

What is a bond order?

A

Refers to whether a covalent bond is a single bond, double bond or triple bond. As bond order increases, bond strength increases, bond energy increases and bond length decreases.

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

When are covalent bonds considered nonpolar?

A

when there is either no difference or a small difference in electronegativity between the atoms (

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

When are covalent bonds considered polar?

A

when there is a significant difference in electronegativity (0.5 to 1.7), but not quite to the extent that would be seen in an ionic bond.

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

What are coordinate covalent bonds?

A

a single atom provides both bonding electrons while the other atom does not contribute any; coordinate covalent bonds are most often found in Lewis acid-base chemistry .

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

When do formal charges exist?

A

When an atom is surrounded by more or fewer valence electrons than it has in its neutral state.

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

What are resonance structures?

A

differences in configurations/distribution of electrons

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

What is the valence shell electron pair repulsion theory?

A

predicts the 3D molecular geometry of covalently bonded molecules. In this theory, electrons arrange themselves as far apart as they can.

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

Which results in more repulsion? Bonding or non-bonding electrons?

A

Non-bonding

17
Q

What are sigma bonds?

A

the result of head-to-head overlap

18
Q

What are pi bonds?

A

the result of overlap of two parallel electron cloud densities.

19
Q

What are three types of intermolecular forces?

A

electrostatic attractions between molecules. They are significantly weaker than covalent bonds.

20
Q

What are london dispersion forces?

A

interaction in all atoms and molecules that increases as size increases

21
Q

What are dipole-dipole interactions?

A

occur between the oppositely charged ends of polar molecules, stronger than London, interactions are evident in the solid and liquid, negligible in gas

22
Q

What are hydrogen bonds?

A

special d-d interaction. Occurs when hydrogen is bound to fluorine, oxygen or nitrogen.