Brainscape's Knowledge GenomeTM

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


See full index

Chem HL > Covalent bonding - HL > Flashcards

Covalent bonding - HL Flashcards

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

What do the delocalised electrons do in a resonance structure ?

A

The delocalised electrons are spread evenly across the bonding positions where the double bond can be found

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

How would you know if someone would display resonance ?

A

If there is more than one place for a double or triple bond , then the molecules can display resonance

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

What physical evidence suppprts the resonance structure of benzene

A

All carbon-carbon bonds are of equal length with equal binding angle of 120

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

Define bond energy

A

The bond energy is required to break one mole of a particular covalent bond in the gaseous state

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

Triple bonds are the

A

shortest and strongest
due to large lecturing density

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

Single covalent bonds are

A

longest and weakest

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

2 ED 0 LP

A

linear

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

3ED 0LP

A

Trigonal Planar

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

lone pairs reduce

A

bond angle

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

4 ED 0LP

A

Tetrahedral

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

3BP 1 LP

A

trigonal pyramidal

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

2 BP 2LP

A

bent

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

2BP 1LP

A

Bent

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

what bond angle is linear

A

180

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

what bond angle is trigonal planar

A

120

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

what bond angle is tetrahedral

A

109.5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Shape of 5BP 0LP

A

Trigonal Bipyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Shape of 4BP 1LP

A

See-saw

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Shape of 3BP 2LP

A

T-shaped

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Shape of 2BP 3LP

A

Linear

21
Q

Shape of 6BP 0LP

A

Octahedral

22
Q

Shape of 5BP 1LP

A

Square Pyramidal

23
Q

Shape of 4BP 2 LP

A

Square Planar

24
Q

Shape of 3BP 3 LP

A

T-shaped

25
Q

Shape of 2BP 4LP

A

bent

26
Q

what is a dipole

A

measure of how polar a bond is

27
Q

When a diatonic molecule e.g cl2 the electronegativity is shrared equally therefore the covalent bond is

A

non-polar

28
Q

When two atoms in a covalent bond have different electronegativities what is the covalent bond

A

polar

29
Q

the bigger the difference in electro negativity the

A

higher the polarity of the covalent bond

30
Q

the dipole arrow points to the

A

partially negative charged end

31
Q

What needs to be taken into consideration when a molecule has more than two atoms when deciding the polarity

A

• The polarity of each bond within the molecule
• How the bonds are arranged in the molecule

32
Q

when the pull of the atoms are not equal and opposite there is a net pull so

A

the molecule is polar

33
Q

what is the formula of silicon oxide

A

Si02

34
Q

Why do giant covalent lattice have high melting and boiling points

A

large number of covalent bonds , a lot of energy is required to break the lattice

35
Q

6 examples of giant covalent structures

A

diamond , graphite , graphene , buckminsterfullerene , silicon , silicon dioxide

36
Q

what are the three type of intermolecular forces

A

London dispersion forces
Dipole-dipole attraction
hydrogen bonding

37
Q

London forces are

A

present between all atoms and molecules

38
Q

The strength of the london dispersion forces depends on two factors

A

number of electrons in the molecule
surface area of the molecules

39
Q

The greater the number of electrons in the molecule the

A

stronger the dispersion forces and melting/boiling points are stronger

40
Q

What is the strongest intermolecular force

A

Hydrogen bonding

41
Q

For hydrogen bonding to take place it needs a species which has

A

(F,O,N) with an available lone pair of electrons

42
Q

How to work out RF value

A

distance travelled by component/ distance travelled by solvent

43
Q

What is the equation for formal charge

A

FC = (number of valence electrons) - 1/2(number of bonding electrons) - (number of non-bonding electrons)

FC = V - 1/2B-N

44
Q

the lewis formal which is preferred is the FC

A

closest to 0

45
Q

How is a sigma bond formed

A

the head on overlap (axial or end to end) of atomic orbitals
(s-s)
(s-p)
(p-p)

46
Q

How is a pi bond formed

A

by sideways overlap of atomic orbitals

47
Q

how many sigma and pi bonds in a single covalent

A

1 sigma
0 pi

48
Q

how many sigma and pi bonds in a double covalent bond

A

1 sigma
1 pi

49
Q

how many sigma and pi bonds in a triple covalent bond

A

1 sigma 2 pi

Chem HL (13 decks)

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