Brainscape's Knowledge GenomeTM

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


See full index

"Shut up," said Chemistry absently > 2: Bonding and Structure > Flashcards

2: Bonding and Structure Flashcards

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

Definition of ionic bonding

A

The electrostatic attraction between oppositely charged ions

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

Factors affecting the strength of ionic bonding

A
  • Difference in charges (greater difference means stronger bonds)
  • Atomic radius (shorter means stronger bonds)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Trend in ion size down a group

A

-Size of ion increase as the charges remain the same but their are more electrons

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

Definition of isoelectronic ions

A

Ions with the same number of electrons (e.g N3-, O2-, F-)

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

Factor affecting size of isoelectronic ions

A

-As the charge is the same the size is only determined by the nuclear charge

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

Physical evidence for ions

A
  • High MP/BP indicate strong electrostatic forces between oppositely charged ions
  • Conductivity of electricity when molten/in solution indicates presence of mobile charge carrying particles in the substance
  • Migration of ions in electrolysis shows positive and negative ions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Definition of covalent bonding

A

The electrostatic attraction between a shared pair of electrons and the nuclei of each atom

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

Bond angle in a linear molecule

A

180°

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

Bond angle in trigonal planar

A

120°

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

Bond angle in tetrahedral

A

109.5°

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

Bond angle in a bent molecule

A

104.5

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

Bond angle in tetrahedral with 1 lone pair

A

107.5

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

Electronegativity definition

A

The ability of an atom with a covalent bond to attract the bonding pair of electrons

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

Test if a molecule is electronegative

A

A jet of the substance would be deflected by a charged rod

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

What are London forces

A

The attraction between instantaneous dipoles in molecules

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

How do instantaneous dipoles form

A
  • As electrons are constantly moving there can be more electrons on one side of the molecule than the other, creating an instantaneous dipole
  • When a dipole moves near to another molecule it will attract/repel electrons, and induce a dipole in the second molecule
17
Q

Factor affecting strength of London forces

A

Strength increases as the number of electrons in the molecule increases

18
Q

What is dipole-dipole attraction?

A

The attraction between oppositely charged dipoles of different polar molecules

19
Q

What is hydrogen bonding?

A

The attraction between an exposed hydrogen atom and an element with a lone electron pair

20
Q

Requirements for hydrogen bonding

A

A hydrogen atom directly bonded to N/O/F within a polar molecule

21
Q

Why is the hydrogen atom exposed in hydrogen bonding?

A

The N/O/F is so electronegative that it draws the electron pair towards itself, effectively leaving an exposed proton

22
Q

Why does water have a relatively high MP/BP

A

The molecules can form two hydrogen bonds per molecule

23
Q

Why does water expands when it freezes

A

The hydrogen bonds pull the water molecules into fixed positions in a lattice structure

24
Q

Trend in BP of alkanes in accordance to mass

A

As the molecular mass increases, the number of electrons increase, so the London forces are stronger

25
Q

Effect on BP of branching in alkanes

A

Lower boiling points as it prevents the molecules from approaching each other as closely, so the induction effect is weaker and therefore the London forces are weaker

26
Q

Why is the BP of alcohols higher

A

The OH group allows for hydrogen bonding between molecules

27
Q

Trend in BP in hydrogen halides

A

HCl → HBr → HI → HF

28
Q

Explanation for trend in BP in hydrogen halides

A

As the molecules increase in size there are more electrons so the London forces are stronger, however there is hydrogen bonding in HF

29
Q

What is hydration of ions

A
  • Oxygen in water molecules is attracted to cations
  • Hydrogen in water molecules is attracted to anions
  • This causes water molecules to link to the ions
  • As the water molecules are vibrating, they shake the ion apart
  • Some ionic compounds don’t dissolve as the electrostatic attraction is too great
30
Q

Definition of metallic bonding

A

The electrostatic attraction between the metal cations and the delocalised electron region

"Shut up," said Chemistry absently (9 decks)

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