Brainscape's Knowledge GenomeTM

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


See full index

Chemistry AS level > 1.3 Bonding Part 2 > Flashcards

1.3 Bonding Part 2 Flashcards

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

Define electronegativity

A

The power of an atom to attract the pair of electrons in a covalent bond

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

What happens to electronegativity value across a period? Why?

A

Increases because there is a smaller distance and a higher nuclear charge

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

What happens to the electronegativity value down a group? Why?

A

Decreases because the bonded electrons are further from the nucleus and have more shielding

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

What is the most electronegative atom?

A

Fluorine

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

Why do noble gases not have electronegativity values?

A

They don’t normally form covalent bonds

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

Is the molecule C-F polar? If yes show the partial charges

A

Yes
C - delta positive
F - delta negative

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

Is the molecule C-H polar? If yes show the partial charges

A

No

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

Is the molecule N-H polar? If yes show the partial charges

A

Yes
N - delta negative
H - delta positive

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

Is the molecule O-H polar? If yes show the partial charges

A

Yes
O - delta negative
H - delta positive

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

Is CO2 polar?

A
  • It has polar bonds
  • Non-polar molecule
  • molecule is symmetrical so the dipoles cancel
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Is H2O polar?

A

Yes
Polar bonds
Polar molecule

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

What are the three types of intermolecular force?

A
  • Van Der Waals
  • Permanent dipole-dipole
  • Hydrogen bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What causes Van Der Waals forces?

A

The movement of electrons which unbalanced the charge distribution within the molecule

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

What is a Van Der Waals force and how does it form?

A
  • electrons move which unbalanced the charge distribution
  • This creates an instantaneous dipole across the molecule
  • This induces a dipole in neighbouring molecules
  • Resulting in weak forces of attraction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Do bigger molecules have greater or weaker Van Der Waals forces?

A

Stronger

More electrons

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

Draw and describe the intermolecular force formed from two HCl molecules joining

A

Permanent dipole-dipole
H - delta pos
Cl - delta neg
Hydrogen joins with chlorine

17
Q

Between what does hydrogen bonding occur?

A

N-H
O-H
F-H

18
Q

What happens when a gas turns into a solid?

A

Deposition

19
Q

What happens when a solid turns into a gas?

A

Sublimation

20
Q

When can an electric current flow?

A

When charged particles are free to move

21
Q

What can carry a current?

A

Delocalised electrons or free ions

22
Q

What can ionic and polar substances dissolve in?

A

Polar solvents

23
Q

What can non polar substances dissolve in?

A

Non polar solvents

24
Q

What is a giant ionic lattice belt together by?

A

The electrostatic attraction between the oppositely charged ions

25
Q

Why do ionic compounds have high melting points?

A

The ions are held together by strong ionic bonds which need a lot of energy to break

26
Q

Do ionic compounds conduct electricity when solid with reason

A

No

The ions are not free to move so cannot carry the current

27
Q

Do ionic compounds conduct electricity when dissolved or molten with reason

A

Yes

The ions are free to move so can carry the current

28
Q

Why are ionic compounds brittle?

A
  • If enough force is applied the layers slide over each other
  • Like charges will move next to each other, causing repulsion and the lattice structure breaks down
29
Q

Why do metals have high melting points?

A

Metallic bonds are strong, so a large amount of energy is needed to break them

30
Q

Why do metals conduct electricity?

A

Because the delocalised electrons can flow through the structure and carry the current

31
Q

Why are metals strong?

A
  • Metallic bonds are strong and extend through the giant metallic lattice
  • Metallic bond strength depends on the size and charge of the metal ion
32
Q

Why are metals malleable and ductile?

A

The layers of ions in the giant ionic lattice can slide over each other into new positions, without disrupting the metallic bond

33
Q

What are the two types of covalent substance?

A
  • Simple molecular covalent

* Macromolecular covalent

34
Q

Why do covalent substances have low melting points?

A

The forces of attraction between the molecules are weak

Not much energy is needed to break them

35
Q

Are covalent substances soluble?

A

Generally insoluble in water, unless they can form hydrogen bonds or react with water

36
Q

Can covalent substances conduct electricity?

A

No

They don’t contain ions or delocalised electrons

Chemistry AS level (8 decks)

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