Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Bonding > Flashcards

Bonding Flashcards

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

Ionic Bonding

A

Strong electrostatic force of attraction between oppositely charged ions (formed by the transfer of electrons from one atom to another)

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

Covalent Bonding

A

Strong electrostatic force of attraction between the nuclei of both atoms and the shared pair of electrons

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

Metallic Bonding

A

Electrostatic force of attraction between a lattice of positive ions and the sea of delocalised electrons

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

Group 1 ions charge

A

1+

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

Group 2 ions charge

A

2+

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

Group 3 ions charge

A

3+

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

Group 5 ions charge

A

3-

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

Group 6 ions charge

A

2-

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

Group 7 ions charge

A

1-

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

Zinc ion

A

Zn2+

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

Silver ion

A

Ag+

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

Hydrogen ion

A

H+

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

Ammonium ion

A

NH4+

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

Nitrate ion

A

NO3-

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

Hydroxide ion

A

OH-

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

Carbonate ion

A

CO32-

17
Q

Sulfate ion

A

SO42-

18
Q

Do ionic compounds have high melting points and boiling points? (Reason)

A

Yes
- (giant ionic lattice structure
- strong electrostatic force of attraction between oppositely charged ions
- a lot of energy is required to overcome these forces)

19
Q

Why are ionic compounds crystalline and brittle?

A
  • regular arrangement of the ions in the lattice
    -the arrangement of the ions is disrupted, the like charged ions repel
20
Q

Are ionic substances soluble in water?

A

Yes

21
Q

Are ionic substances soluble in organic solvents?

A

No

22
Q

Why can’t the ionic compounds conduct electricity when they are solid?

A
  • the ions are fixed in state
    -the ions aren’t mobile
23
Q

Do substances with simple molecular structure have low melting and boiling points? (Reason)

A

Yes
- (weak intermolecular forces of attractions between molecules
- not much energy is required to overcome these forces)

24
Q

Why don’t covalent molecular compounds conduct electricity?

A
  • there are no ions
  • there are no delocalised electrons
25
Q

Are covalent molecular compounds soluble in water? Any exceptions?

A

No
- ethanol, NH3 and HCl are soluble in water.

26
Q

Are covalent molecular compounds soluble in organic solvents?

A

Yes

27
Q

Explain diamond’s bonding and structure

A
  • each carbon atom is covalently bonded to 4 other carbon atoms
  • forming a tetrahedral structure
28
Q

Does diamond and graphite have high melting point? (Reason)

A

Yes
- (they are substances with giant covalent structures
- they have very strong carbon-carbon covalent bonds
- a lot of energy is required to break these strong covalent bonds)

29
Q

Is diamond hard? (Reason)

A

Yes
- (very strong covalent bonds
- a lot of energy is required to break the bonds in the giant structure)

30
Q

Does diamond conduct electricity? (Reason)

A

No
- (no delocalised electrons)

31
Q

Is diamond soluble?

A

No

32
Q

Explain graphite’s bonding and structure

A

-each carbon is covalently bonded to 3 other carbon atoms
-forming a hexagonal layer structure

33
Q

Is graphite hard? (Reason)

A

No
-(weak forces of attractions between layers
-not much energy is required to overcome these forces)

34
Q

Does graphite conduct electricity? (Reason)

A

Yes
-(it has delocalised electrons which are free to move)

35
Q

Is graphite soluble?

A

No

36
Q

Why are metals hard and have high melting points?

A
  • strong electrostatic forces of attraction between the positive ions and the delocalised electrons
37
Q

Why do metals conduct electricity?

A
  • it has delocalised electrons which are free to move throughout the structure
38
Q

Why are metals malleable and ductile?

A
  • the layers of positive ions slide over each other

Chemistry (4 decks)

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