Brainscape's Knowledge GenomeTM

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


See full index

Chemistry (Semester 1) > L10: Metallic & Intermolecular Bonding > Flashcards

L10: Metallic & Intermolecular 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

Describe the interactions in metallic bonding

A

Electrostatic attraction between metal ions and mobile, delocalised electrons

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

What are delocalised electrons?

A

They are not associated with a particular atom

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

What are the prerequisites for metallic bonding to occur?

A

1) The metal should have low ionisation energies (able to give up their electrons to form positive metal ions)
2) The metal should have vacant valence orbitals to allow free movement of electrons

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

Fill in the gap:

Metallically bonded compounds are __(1)__ conductors of heat and electricity in in solid and __(2)__ state

A

(1) good

(2) liquid

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

Comment on the lustre of metallic compounds

A

Metallic compounds have a high lustre

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

True or false: Metallic compounds are relatively malleable and ductile

A

True

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

What are intramolecular forces?

A

Bonds holding atoms together within a molecule

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

What are intermolecular forces?

A

Attractive forces between molecules

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

Which is stronger, intermolecular or intramolecular forces?

A

Intramolecular

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

What are the four types of intermolecular forces? List in order of strength (strongest first)

A

1) Ion-dipole
2) Hydrogen bonds
3) Dipole-dipole
4) Dispersion

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

Which bonds form between polar molecules?

A

Ion-dipole, hydrogen, and dipole-dipole

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

Which bonds form between non-polar molecules?

A

Dispersion (van der Waals/London)

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

True or false: London dispersion forces are formed between temporary dipoles. These dipoles come about because of the uneven distribution of electrons in their orbitals

A

True

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

True or false: London dispersion forces form between temporary dipoles

A

True

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

True or false: Dipole-dipole interactions form between temporary dipoles

A

False. They relate to permanent dipoles

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

True or false: Dipole-dipole interactions act in addition to Van der Waals

A

True

17
Q

How do dipole-dipole interactions effect boiling point?

A

Result in higher BP than expected from the mass of the molecule

18
Q

In which two areas are dipole-dipole interactions significant?

A

1) Carbonyls

2) Protein folding

19
Q

Fill in the gaps:

__(1)__-dipole forces are electrostatic interactions between an __(2)__ and an __(3)__ __(4)__ molecule

A

(1) ion
(2) ion
(3) uncharged
(4) polar

20
Q

What factor effects the strength of an ion-dipole bond?

A

Strength depends on the charge on the ion and the magnitude of the dipole

21
Q

Where are ion-dipole forces most common?

A

In solution.

E.g. NaCl dissolving in water

22
Q

What are the two requirements for a hydrogen bond?

A

1) An electronegative atom (O, N, or F) to act as the acceptor
2) A hydrogen atom in a polar bond (N-H, O-H, or F-H) to act as the donor

23
Q

True or false: Hydrogen bonds are stronger than other dipole-dipole interactions

A

True

24
Q

True or false: Hydrogen bonds are non-directional

A

False. Hydrogen bonds are directional

25
Q

True or false: Although they are relatively strong for intermolecular forces, hydrogen bonds are weak and easily broken compared to covalent bonds

A

True

26
Q

Give six areas in which hydrogen bonding plays a significant role

A

1) Physical state of water
2) Stabilise macromolecules
3) DNA double helix, base pairing
4) Protein secondary structure; alpha helices, beta sheets
5) Enzyme-substrate and antibody-antigen interactions
6) Solubility of compounds in water

27
Q

Why does water form such an extensive network of hydrogen bonds?

A

Each oxygen atom has two lone pairs and each molecule has two hydrogen atoms

28
Q

True or false: The base pairs match each other based on the number of hydrogen bonds each can donate/accept

A

True

29
Q

True or false: In alpha helices and beta sheets, hydrogen bonds form between amine (N-H) and C=O

A

True

30
Q

In addition to hydrogen bonds, what links can be formed by covalent and ionic bonding in secondary protein structures?

A

Covalent disulphide links (R-S-S-R)

Ionic salt bridges (—CO2—-NH3—-

31
Q

Which intermolecular bonds hold sugar chains together in cellulose to form flat sheets?

A

Hydrogen bonds

32
Q

Which intermolecular bonds hold flat sheets of hydrogen-bonded sugar chains together in cellulose?

A

Van der Waals

Chemistry (Semester 1) (10 decks)

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