Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > AS.5 Bonding > Flashcards

AS.5 Bonding Flashcards

1
Q

Metallic bonds

A

electrostatic attraction between positively charged ions and a sea of delocalised electrons

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

diagram to represent metallic bonds

A

cations relative charge in a circle

sea of delocalised electrons represented by appropriate number of minuses

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

giant

A

continous bonds

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

lattice

A

regular and repeating pattern

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

giant metallic lattice - melting and boiling point

A

very high

strong metallic bonds throughout structure

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

giant metallic lattice - electrical conductivity

A

very high

delocalised electrons are free to move and carry charge

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

giant metallic lattice - solubility

A

insoluble

some may react with water

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

comparing the strength of metallic bonds

A

more e- and higher nucleur charge

stronger electrostatic attraction

stronger metallic bond

higher melting/boiling point

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

ionic bonds

A

electrostatic attraction between two oppositely charged ions

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

dot and cross ionic

A

square brackets with charge in top right corner

no dots or crosses on metal

appropriate dots and crosses on non-metal

number in front to indicate how many

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

why do metals and non metals lose/gain electrons

A

full outer shell- more stable

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

giant ionic lattice - melting and boiling point

A

high

strong ionic bonds throughout

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

giant ionic lattice - electrical conductivity

A

solids do not conduct - ions are in fixed position - not mobile

molten/aqueous do conduct - ions are free to move

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

Covalent bond

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the 2 bonded atoms

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

Dative covalent bonds

A

Both electrons in the covalent bond come from one of the atoms

The atom giving the electron pair must have a lone pair

The atom accepting the lone pair must have empty orbital space

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

Why do molecules have a specific 3D shape

A

Result in minimum amount of repulsion between electron pairs

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

Repulsion

A

MOST

Lone pair to lone pair

Lone pair to bond pair

Bond pair to bond pair

LEAST

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

Linear

A

2-0-2

180*

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

Trigonal planar

A

3-0-3

120*

20
Q

Tetrahedral

A

4-0-4

109.5*

21
Q

Pyramidal

A

3-1-4

107*

22
Q

Non-linear

A

2-2-4

104.5*

Lone pairs repel bonding pairs

23
Q

Octahedral

A

6-0-6

90*

24
Q

Each lone pair decreases angle by…

A

2.5*

25
Q

Electronegativity

A

Ability of an atom to attract the electron pair in a covalent bond

26
Q

Electronegativity increases as…..

A

Atomic radius decreases

Bonding pair is closer to nucleus

27
Q

Polar molecules

A

Imbalanced electronegativity

Has polar bonds

Asymmetrical

28
Q

Intermolecular forces

A

Bonds between molecules in a simple covalent lattice

29
Q

London forces

A

Non-polar molecule

Uneven distribution of electrons

Creates temporary dipole

Induces dipole in neighbouring molecule

Two dipoles attract each other

30
Q

London force strength

A

1) no of electrons

2) surface area contact points

31
Q

Permanent dipole dipole forces

A

Polar molecules

Dipoles attract each other

Stronger than London forces because permanent

32
Q

Hydrogen bonds

A

H-F
H-O
H-N

Strongest IMF
Very polar
Lone pair on F/O/N is very attracted to H

33
Q

Why ice is less dense than water

A

Each water molecule is able to form 4 hydrogen bonds as molecules are far more ordered in solid state

Increase in number of hydrogen bonds that can be formed pushes molecules further apart

Now adopt tetrahedral shape

34
Q

Simple molecular lattice - melting and boiling point

A

Low

Breaking IMF which are much weaker than bonds

35
Q

Simple molecular lattice - electrical conductivity

A

Very low

No mobile electrons or ions

36
Q

Simple molecular lattice - solubility

A

Polar dissolves in polar solvent

Non polar dissolves in non polar solvent

37
Q

Giant covalent lattice vs simple covalent lattice

A

Giant has covalent bonds spread throughout so breaking bonds instead of IMF

38
Q

Graphite

A

Each carbon forms 3 covalent bonds
Trigonal planar
Hexagonal layers
1 delocalised electron between layers - London forces

39
Q

Diamond

A

Each carbon has 4 covalent bonds
Tetrahedral
SO2 has same structure

40
Q

Giant covalent lattice - melting and boiling point

A

Very high

Very strong covalent bonds throughout

41
Q

Giant covalent lattice - electrical conductivity

A

Diamond - very low
No delocalised electrons or mobile ions

Graphite/graphene - very good
Delocalised electrons

42
Q

Giant covalent lattice - solubility

A

Very low

Can’t interact with water

43
Q

Graphene

A

Single layer of graphite
Delocalised electron on surface - conduct

44
Q

Anamalous properties of water

A

Liquid denser than solid
H bonds hold molecules apart in solid

Strong H bonds
Higher mp than expected

45
Q

Volatile

A

High bp = low volatility

Chemistry (27 decks)

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