Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry A Level > Bonding - Chapter 3 > Flashcards

Bonding - Chapter 3 Flashcards

(59 cards)

Start Studying
1
Q

What types of bonding are there

A

Ionic
Covalent
Metallic

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

What are the three types of covalent bond

A

Simple Covalent e.g. H2
Giant Covalent e.g. Diamond
Coordinate (dative covalent)

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

What is a bond

A

An attractive force holding particles together

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

What is ionic bonding

A

Bonding between a metal and a non-metal

Where electrons are transferred from the metal to the non metal

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

What is an ionic bond

A

The electrostatic attraction between oppositely charged ions

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

What is a covalent bond

A

It is a bond between non-metals
where electrons are shared between the atoms

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

What is a covalent bond

A

It is a shared pair of electrons, and the electron pair is attracted by both nuclei so resists separation

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

What is a coordinate bond

A

It is a covalent bond where both electrons in the shared pair originate from the same atom

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

What is metallic bonding

A

It is attraction inside a metal between the positive metal ions and the sea of delocalised electrons

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

Why is there a sea of delocalised electrons in a metal

A

Outer electron is only weakly held so it becomes delocalised

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

What determines the shape of a molecule or ion

A

The number of electron pairs in the outer shell of the central atom

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

Why do species containing only bonding pairs have regular molecular shapes

A

Because bonding pairs of electrons exert equal repulsion on each other

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

What is the shape of an molecule with 2 bonding pairs

A

It is linear
Bond angle of 180 degrees
Shape of a straight line

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

What is the shape of molecule with 3 bonding pairs

A

Trigonal Planar
Bond angle of 120 degrees
Triangle shape

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

What is the shape of a molecule with 4 bonding pairs

A

Tetrahedral
Bond angle of 109.5 degrees
Triangular based pyramid

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

What is the shape of a molecule with 5 bonding pairs

A

Trigonal Bipyramidal
Bond angles of 90 degrees and 120 degrees
Triangle with another atom opposite the top of the triangle

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

What is the shape of a molecule with 6 bonding pairs

A

Octahedral
Bond angle of 90 degrees
Square with two atoms above and below

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

What does the shape of a molecule also depend on

A

The presence of non-bonding electron pairs (lone pairs)

Lone pairs take up more space because they are held closer to the nucleus so repel more strongly

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

What is the shape of a lone pair in a trigonal planar

A

Bent
Two atoms are slightly bent and at an angle

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

What are the two shapes of lone pairs in a tetrahedral

A

1 Lone Pair: Trigonal pyramidal
2 Lone Pair: Bent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are the 3 shapes with lone pairs in a Trigonal Bipyramidal

A

1 Lone Pair: Sawhorse
2 Lone Pair: T- shaped, Lone pairs in the middle
3 Lone Pair: Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What are the 4 shapes with lone pairs in an Octahedral

A

1 Lone Pair: Square Pyramidal
2 Lone Pair: Square Planar
3 Lone Pair: T-shaped
4 Lone Pair: Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the order of decreasing replusion between electron pairs

A

Lone pair - Lone pair
Lone pair - Bonding pair
Bonding pair - Bonding pair

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the method to find the shape of a molecule without double bonds

Study These Flashcards
A
  1. Count number of outer electrons on the central atom
  2. add 1 for every atom bonded to the central atom
  3. For ions add 1 if singly negative, subtract 1 if singly positive
  4. Total then divide by 2 to get number of electron pairs
  5. Deduce the regular shape taken up by this number of pairs
  6. If any of the pairs are lone pairs alter the shape
25
What happens when two different elements are bonded together
The electron pair is not equally attracted to both nuclei because the elements have different electronegativities
26
What is electronegativity
It is the power of an atom to attract the pair of electrons in a covalent bond
27
What affects electronegativity
Nuclear charge As nuclear charge goes up so does electronegativity Atomic radius As atomic radius increases so does shielding which causes electronegativity to decrease
28
What is electronegativity measured using
Pauling scale
29
What happens to electronegativity across a period
There is an increasing nuclear charge which means the electron are more attracted to the nucleus so atomic radius reduces and electronegetivity increases
30
What happens to electronegativity up a group
Fewer energy levels and the outer electrons are less shielded so electronegativity increases
31
What is used to symbolise which element has a greater electronegativity
A lower case delta is used with a plus and a minus to show the stronger electrongetativity The negative is used on the stronger one
32
What is a polar molecule
It is one in which the electron density across the whole molecule is unevenly distributed
33
What happens when the charge on the molecule isnt symetrical
It is polar overall and described as permanent dipole
34
What are the 3 types of intermolecular forces
Dipole-Dipole interactions Hydrogen bonding Van der Waal's forces
35
What is dipole-dipole interactions
They are attractive forces between polar molecules The polar molecules will flip to give an arrangement where the molecules attract
36
What are hydrogen bonds
They are very strong intermolecular forces It takes place when a hydrogen is bonded to a very electronegative element like Oxygen, Fluorine and Nitrogen and there is at least 1 lone pair
37
What are Van der Waal's forces
They are temporary dipole - induced dipole interactions They happen in all molecules Caused by the movement of electrons, so the more electrons the stronger the force is
38
What is the order of strength of intermolecular forces at an increasing strength
Van der Waals Dipole - dipole Hydrogen bonding
39
How do two sets of polar molecules or 2 sets of non-polar molecules interact as liquids
They are miscible but different polar states means that they are non-miscible
40
What are the 3 states of matter
Solid Liquid Gas
41
What are solids like
They have an arrangement of close and regular and vibrate about a fixed position
42
What are liquids like
They have an arrangement of random, close and can move past each other
43
What are gases like
they have an arrangemnet of random, far-apart, rapid and random motion
44
What is the process solid to liquid
melting | Fusion
45
What is the process liquid to gas
Boiling | vaporisation
46
What is the process Gas to liquid
Condensation
47
What is the process liquid to solid
Freezing Solidifying
48
What is the process solid to gas
Sublimation
49
What are crystals
they are solids that contain particles in a regular arrangement known as a lattice
50
What are the 4 types of crystal lattices
Ionic Metallic Molecular (simple covalent) Macromolecular (giant covalent)
51
What are ionic crystals
They are positive and negative ions held together in a giant lattice by strong electrostatic attraction between oppositely charged ions
52
Properties of ionic compounds
High MP - Strong electrostatic attraction Conductors as liquid - Ions Hard and Brittle - Like ions repel Dissolve in water - Ions become surronded by water
53
What are metallic crystals
A giant lattice of positive ions held together by a sea of delocalised electrons
54
Properties of metals
High MP and BP - Strong metallic bonds Conduct electricity - Sea of delocalised electrons Malleable and ductile - Ions slide over eachother Insoluble in water - Water can't break bonds
55
What are molecular crystals
Individual molecules held together by weak intermolecular forces
56
Properties of molecular solids
Low MP - Weak intermolecular forces Soft - Weak intermolecular forces Dont conduct electricity - No ions or electrons
57
What are Macromolecular crystals
A giant arrangement of atoms joined by covalent bonds
58
Properties of Diamond
High melting point - Strong covalent bonds Very Hard - Strong covalent bonds Non-Conductor - No ions or electrons
59
Properties of Graphite
High MP - Strong covalent bonds Soft - Weak attraction between layers Conducts electricity - delocalised 4th electron

Chemistry A Level (20 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions