Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Physical > Bonding > Flashcards

Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Define ionic bonding

A

Strong electrostatic FOA btw oppositely charged ions

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

Why do ionic compounds have a high melting point?

A
  • Lots of strong electrostatic FOA btw oppositely charged ions
  • Forming giant ionic lattice
  • Needs alot of energy to overcome bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

When can ionic compounds conduct electricity?

A
  • Molten/ dissolved
  • Ions are free to move + carry a charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why do ionic compounds dissolve in water?

A
  • Water molecules = polar (parts of molecule has small -ve charge + +ve charge)
  • Charged parts pull ions away from lattice
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Sulfate

A

SO4 2-

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

Hydroxide

A

OH-

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

Nitrate

A

NO3 -

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

Carbonate

A

CO3 2-

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

Ammonium

A

NH4+

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

Define covelant bond

A

Shared pair of e-

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

What are the 2 types of covelant structures?

A
  • Molecular
  • Giant covelant
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define dative covelant

A

When 1 atom donates a shared pair of e-

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

Describe the structure of graphite + its properties

A
  • Giant covelant
  • High MP + insoluble - lots of strong covelant bonds need to be broken
  • VDW btw layers allow layers to slide past each other
  • Conducts electricity - delocalised e- are free to move + carry charge
  • Low density - layers are far apart
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Describe the structure of diamond + its properties

A
  • Giant covelant
  • Shape: tetrahedral, C bonded to 4 C
  • High MP, hard + insoluble - lots of strong covelant bonds
  • Good thermal conducter - vibrations travel easily
  • Can’t conduct electricity - outer e- held in localised bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Which type of bonding pair has the biggest angle?

A
  • LP to LP
  • Repel more than BP
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Define electronegativity

A

Power of an atom to attract pair of e- in a covelant bond

17
Q

Define dipole

A

Diff in charge btw 2 atoms caused by shift in electron density in bond

18
Q

Explain why some molecules w/ polar bonds don’t have a permanent dipole

A

If polar bonds are arranged symmetrically, charges cancel out

19
Q

Explain how a permanent dipole occurs

A

E- distribution in covelant bond btw elements w/ diff. electronegativities will be unsymmetrical, produces polar bond

20
Q

Outline how Van der Waals are formed

A
  • e- movement in first molecule
  • Induces dipole in another molecule
  • δ+ attracts δ- in adjacent molecules
21
Q

What affects the strength of VDW?

A
  • Longer chain - more e- so stronger VDW
  • Straight chain - lie closer together so stronger forces
22
Q

Outline how H bonds are formed

A
  • F, N + O are v electronegative so draw bonding e- away from H
  • Bond is polarised + H has high charge density
  • Causes H atoms to form weak bonds w/ LP on F, O + N
23
Q

Define metallic bonding

A

Electrostatic FOA btw the +ve metal ions and the delocalised electrons

24
Q

Outline the properties of metals

A
  • High MP - lots of electrostatic FOA btw +ve metal + sea of delocalised e- - more DE, stronger the bond
  • Good thermal conducter - DE pass kinetic energy
  • Good electrical conducter - DE move + carry current
  • Insoluble
25
Q

Outline the factors affecting the strength of metallic bonding

A
  • No. protons - more protons = stronger bond
  • No. DE per atom - more DE = stronger bond
  • Size of ions - smaller ion = stronger bond
26
Q

Why do simple covelant molecules have low MP + BP?

A

Only have to break IMF BTM, not covelant bonds

27
Q

Ionic

Eg.

MP + BP

State at room temp

Does solid conduct electricity

Does liquid conduct electricity

Is it soluble in water

A
  • NaCl
  • High
  • Solid
  • No
  • Yes
  • Yes
28
Q

Simple covelant

Eg.

MP + BP

State at room temp

Does solid conduct electricity

Does liquid conduct electricity

Is it soluble in water

A
  • CO2, I2
  • Low
  • I2 is solid but usually liquid + gas
  • No
  • No
  • Depends on polarity
29
Q

Giant covelant

Eg.

MP + BP

State at room temp

Does solid conduct electricity

Does liquid conduct electricity

Is it soluble in water

A
  • Diamond, graphite
  • High
  • Solid
  • No exp. graphite
  • Sublimes, doesn’t melt
  • No
30
Q

Metallic

Eg.

MP + BP

State at room temp

Does solid conduct electricity

Does liquid conduct electricity

Is it soluble in water

A
  • Fe, Mg
  • High
  • Solid
  • Yes
  • Yes
  • No

Chemistry Physical (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions