Brainscape's Knowledge GenomeTM

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


See full index

A-LEVEL CHEM 3.1: Physical Chemistry > A-LEVEL Chemistry: 3.1.3: Bonding (ChemRevise) > Flashcards

A-LEVEL Chemistry: 3.1.3: Bonding (ChemRevise) Flashcards

1
Q

What is ‘Ionic Bonding’?

A

Ionic Bonding is the Electrostatic Force of Attraction between Oppositely Charged Ions, Formed by the Transfer of Electrons.

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

Metal Atoms ___ Electrons to Form ___ Ions.

A

Lose, Positive.

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

Non-Metal Atoms ___ Electrons to Form ___ Ions.

A

Gain, Negative.

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

Mg has 12 Electrons. State the Electron Configuration before & after becoming an Ion. (2)

A

-Before: 1s2 2s2 2p6 3s2

-After: 1s2 2s2 2p6

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

Ionic Crystals have the Structure of…

A

Giant Lattices of Ions.

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

When are Ionic Bonds Stronger, and have Higher Melting Points?

A

When the Ions are Smaller, or when the Ions have Higher Charges.

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

MgO has a Higher Melting Point that NaCL. Why is this?

A

Because the Ions Involved in MgO are Smaller & have Higher Charges than those in NaCL.

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

Positive Ions are ___ Compared to their Atoms. Why?

A

Smaller. Because the Ion has One Less Electron Shell, & the Ratio of Protons to Electrons has Increased, so there is Greater Nuclear Charge on the Remaining Electrons, Pulling them in Closer.

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

The Negative Ions Formed from Groups 5-7 are ___ than their Corresponding Atoms. Why?

A

Larger. Because the Negative Ion has More Electrons than the Corresponding Atom, but has the Same Number of Protons. Hence, the Pull of the Nucleus is Shared over More Electrons, & so the Attraction per Electron is Less, making the Ion Bigger.

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

As you go Down a Group, the Ionic Radius ___. Why?

A

Increase. Because as you go Down the Group, the Ions have More Shells of Electrons.

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

What is a ‘Covalent Bond’?

A

A Covalent Bond is a Shared Pair of Electrons.

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

When does a ‘Dative Covalent Bond’ Form?

A

A Dative Covalent Bond Forms when the Shared Pair of Electrons in the Covalent Bond comes from only One of the Bonding Atoms.

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

Common Examples of Dative Covalent Bonds: (3)

A
  • NH4+

-H3O+

-NH3BF3

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

When Representing the Structure of Dative Covalent Bonds, what does the Direction of the Arrow Represent?

A

The Direction of the Arrow goes from the Atom that is Providing the Lone Pair to the other Atom.

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

What is ‘Metallic Bonding’?

A

Metallic Bonding is the Electrostatic Force of Attraction Between the Positive Metal Ions & the Delocalised Electrons.

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

The 3 Main Factors that Affect the Strength of Metallic Bonding: (3)

A

-Number of Protons / Strength of Nuclear Attraction.

-Number of Delocalised Electrons per Atom.

-Size of Ion.

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

State the Structure for Ionic Bonds:

A

Giant Ionic Lattice.

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

State the Structures for Covalent Bonds: (2)

A

-Simple Molecular (with Intermolecular Forces between Molecules).

-Macromolecular (Giant Molecular Structures).

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

State the Structure for Metallic Bonds:

A

Giant Metallic Lattice.

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

Explain the Property ‘Boiling & Melting Points’ for Giant Ionic Lattice Structures:

A

High MP & BP:
Because of Giant Lattice of Ions with Strong Electrostatic Forces Between Oppositely Charged Ions.

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

Explain the Property ‘Boiling & Melting Points’ for Simple Molecular Structures:

A

Low MP & BP:
Because of Weak Intermolecular Forces Between Molecules (Specify Type eg Van Der Walls / Hydrogen Bond).

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

Explain the Property ‘Boiling & Melting Points’ for Macromolecular / Giant Molecular Structures:

A

High MP & BP:
Because of Many Strong Covalent Bonds in Macromolecular Structures. It takes a Lot of Energy to Break the Many Strong Bonds.

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

Explain the Property ‘Boiling & Melting Points’ for Giant Metallic Lattice Structures:

A

High MP & BP:
Because of the Strong Electrostatic Forces Between Positive Ions & the Cloud of Delocalised Electrons.

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

Describe the Property ‘Solubility in Water’ for Giant Ionic Lattice Structure:

A

Generally Good.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Describe the Property ‘Solubility in Water’ for Simple Molecular Structures:

A

Generally Poor.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Describe the Property ‘Solubility in Water’ for Macromolecular / Giant Molecular Structures:

A

Insoluble.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Describe the Property ‘Solubility in Water’ for Giant Metallic Lattice Structures:

A

Insoluble.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Explain the Property ‘Conductivity when Solid’ for Giant Ionic Lattice Structures:

A

Poor:
Because Ions can’t Move- they’re Fixed in the Lattice Structure due to the Electrostatic Forces of Attraction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Explain the Property ‘Conductivity when Solid’ for Simple Molecular Structures:

A

Poor:
Because there are No Ions to Conduct, & there are No Free Electrons to Conduct (all Fixed in Place).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Explain the Property ‘Conductivity when Solid’ for Macromolecular / Giant Molecular Structures: (2)

A

-Diamond & Sand: Poor:
Because Electrons are Fixed in Place.

-Graphite: Good:
Because there are Many Delocalised Electrons Between Layers, Free to Move & Carry Charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Explain the Property ‘Conductivity when Solid’ for Giant Metallic Lattice Structures:

A

Good:
Cloud of Delocalised Electrons Can Move Freely Through the Structure, & Carry Charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Describe the Property ‘Conductivity when Molten’ for Giant Ionic Lattice Structures:

A

Good: Ions can Move.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Describe the Property ‘Conductivity when Molten’ for Simple Molecular Structures:

A

Poor: No Ions to Move.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Describe the Property ‘Conductivity when Molten’ for Macromolecular / Giant Molecular Structures:

A

Poor.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Describe the Property ‘Conductivity when Molten’ for Giant Metallic Lattice Structures:

A

Good.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Linear’: (2)

A

-No. Bonding Pairs: 2

-No. Lone Pairs: 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Trigonal Planar’: (2)

A

-No. Bonding Pairs: 3

-No. Lone Pairs: 0

38
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Tetrahedral’: (2)

A

-No. Bonding Pairs: 4

-No. Lone Pairs: 0

39
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Trigonal Pyramidal’: (2)

A

-No. Bonding Pairs: 3

-No. Lone Pairs: 1

40
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Bent’: (2)

A

-No. Bonding Pairs: 2

-No. Lone Pairs: 2

41
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Trigonal Bipyramidal’: (2)

A

-No. Bonding Pairs: 5

-No. Lone Pairs: 0

42
Q

State the Number of Bonding Pairs & Number of Lone Pairs for the Molecule Shape: ‘Octahedral’: (2)

A

-No. Bonding Pairs: 6

-No. Lone Pairs: 0

43
Q

What is ‘Electronegativity’?

A

Electronegativity is the Relative tendency of an Atom in a Covalent Bond in a Molecule to Attract Electrons in a Covalent Bond to Itself.

44
Q

Electronegativity is Measured on the ___ ___. It Ranges from…

A

Pauling Scale, 0-4.

45
Q

What happens to Electronegativity as you go Across a Period? Why?

A

As you go Across a Period, Electronegativity Increases.
Because the Number of Protons Increases, & the Atomic Radius Decreases, because the Electrons in the Same Shell are Pulled in more.

46
Q

Ionic & Covalent Bonding are More of a…

A

Spectrum.

46
Q

What happens to Electronegativity as you go Down a Group? Why?

A

As you go Down a Group, Electronegativity Decreases.
Because the Distance Between the Nucleus & the Outer-Shell Electrons Increases, & the Shielding of Inner-Shell Electrons Increases.

47
Q

What Type of Compound will be Purely Covalent?

A

A Compound Containing Elements of Similar Electronegativity & hence a Small Electronegativity Difference Will be Purely Covalent.

48
Q

What Type of Compound will be Ionic?

A

A Compound Containing Elements of Very Different Electronegativity & hence a Very Large Electronegativity Difference Will be Ionic.

49
Q

When does a ‘Polar Covalent Bond’ Form?

A

A Polar Covalent Bond Forms when the Elements in the Bond have Different Electronegativities.

50
Q

What happens when a Bond is a Polar Covalent Bond?

A

When a Bond is a Polar Covalent Bond, it has an Unequal Distribution of Electrons in the Bond, & Produces a Charge Separation, Dipole Ends.

51
Q

What is a ‘Symmetric Molecule’?

A

A Symmetric Molecule is a Molecule where all Bonds are Identical, & there are No Lone Electron Pairs.

52
Q

A Symmetric Molecule Will Not be ___, even if Individual Bonds Within the Molecule are ___.

A

Polar, Polar.

53
Q

Why Can’t Symmetric Molecules be Polar?

A

Due to the Symmetrical Shape of the Molecule, all Bonds Cancel Out. Hence, there is No ‘Net Dipole Movement’: the Molecule is Non-Polar.

54
Q

What are ‘Van der Waals’ Forces’?

A

Van der Waals’ Forces Occur Between All Molecular Substances & Noble Gasses.
They Do Not Occur in Ionic Substances.

55
Q

In Any Molecule, the Electrons are Moving ___ & ___. What happens as a Result of this?

A

Constantly, Randomly.
As this happens, the Electron Density Can Fluctuate, & Parts of the Molecule Become More or Less Negative (Small Temporary Dipoles Form).

56
Q

In Any Molecule, the Electrons Move Constantly & Randomly. What happens as a Result of this?

A

As this happens, the Electron Density Can Fluctuate, & Parts of the Molecule Become More or Less Negative (Small Temporary Dipoles Form).

57
Q

In Any Molecule, the Electrons Move Constantly & Randomly. As this happens, the Electron Density Can Fluctuate, & Parts of the Molecule Become More or Less Negative (Small Temporary Dipoles Form). What Can these Temporary Dipoles Cause?

A

These Temporary Dipoles Can Cause Dipoles to Form in Neighbouring Molecules- Induced Dipoles.

58
Q

How are ‘Induced Dipoles’ Formed?

A

As Electron Density Fluctuates in Molecules, Temporary Dipoles Form. These Cause Induced Dipoles to Form in the Neighbouring Molecules.

59
Q

The Induced Dipole is Always the ___ ___ to the Original One.

A

Opposite Sign.

60
Q

What is the Main Factor Affecting the Size of Van der Waals’ Forces? Explain how.

A

The Number of Electrons there are in the Molecule:
The More Electrons there are in the Molecule, the Higher the Chance that Temporary Dipoles Form in the Molecule. This Makes the Van Der Waals’ Forces Stronger Between the Molecules, and so BPs Will be Greater.

61
Q

Why do the BPs of the Halogens Increase as you go Down Group 7?

A

Because of the Increasing Number of Electrons in the Bigger Molecules, Causing an Increase in the Size of the Van der Waals’ Forces Between the Molecules.
(This is why I2 is a Solid, whereas Cl2 is a Gas)

62
Q

Why do the BPs of the Alkane Homologous Series Increase?

A

Because of the Increasing Number of Electrons in the Bigger Molecules, Causing an Increase in the Size of the Van der Waals’ Forces Between the Molecules.

63
Q

Aside from the Number of Electrons in the Molecule, what other Factor has an Effect on the Size of the Van der Waals’ Forces Acting Between the Molecules?

A

The Shape of the Molecules.

64
Q

Which Shape of Molecules have Larger Van der Waals’ Forces, & which Shape has Lower Van der Waals’ Forces? Explain why. (2)

A

-Higher: Long-Chained Alkanes. Because they have Large Surface Areas of Contact Between Molecules for Van der Waals’ Forces to Form. Hence, they have Strong VdW’ Forces.

-Lower: Spherical Shapes Branched Alkanes. Because they have Little Surface Areas of Contact Between Molecules for Van der Waal’s Forces to Form. Hence, they have Weaker VdW’ Forces.

65
Q

Where do Permanent Dipole-Dipole Forces Occur?

A

Between Polar Molecules.

65
Q

Where do Permanent Dipole-Dipole Forces Occur?

A

Between Polar Molecules.

66
Q

Polar Molecules have a ___ ___.

A

Permanent Dipole.

67
Q

Polar Molecules are ___, & have a Bond where there is Significant Difference in ___ Between the Atoms.

A

Asymmetrical, Electronegativity.

68
Q

Where does ‘Hydrogen Bonding’ Occur?

A

Hydrogen Bonding Occurs in Compounds that have a Hydrogen Atom Attached to One of the 3 Most Electronegative Atoms of Nitrogen, Oxygen, & Fluorine, which Must have an Available Lone Pair of Electrons.

69
Q

Hydrogen Bonding Occurs in Addition to…

A

Van der Waal’s Forces.

70
Q

Hydrogen Bonding is Stronger than the other 2 Types of…

A

Intermolecular Bonding.

71
Q

What are the Anomalously High Bp of H2O, NH3, & HF Caused by?

A

They are Caused by the Hydrogen Bonding Between the Molecules.

72
Q

What is the General Increase in BP from H2S to H2Te Caused by?

A

It is Caused by Increasing Van der Waals’ Forces Between Molecules, due to an Increasing Number of Electrons.

73
Q

What Types of Compounds Can Form Hydrogen Bonds? (4)

A

-Alcohols.

-Carboxylic Acids.

-Proteins.

-Amides.

74
Q

‘Sodium Chloride, NaCl’
State the Type of Bond.
State & Explain the Structure.

A

-Ionic Bond.

-Giant Ionic Lattice Structure, made up of Na+ & Cl- Ions.

75
Q

‘Magnesium’
State the Type of Bond.
State & Explain the Structure.

A

-Metallic Bond.

-Giant Metallic Lattice Structure, showing Mg Ions Packed Closely Together.

76
Q

‘Iodine’
State the Type of Bond.
State & Explain the Structure.

A

-Simple Molecular Bond.

-Simple Molecular Structure, with Regular Arrangement of I2 Molecules, held together by Weak Van der Waals’ Forces.

77
Q

‘Diamond’
State the Type of Bond.
State & Explain the Structure.

A

-Covalent Bonding.

-Macromolecular Structure. Tetrahedral Arrangement of Carbon Atoms. 4 Covalent Bonds per C Atom.

78
Q

‘Graphite’
State the Type of Bond.
State & Explain the Structure.

A

-Covalent Bonding.

-Macromolecular Structure. Planar Arrangement of Carbon Atoms in Layers (Graphene). 3 Covalent Bonds per C Atom in each Layer. The 4th Electron from every C Atom Leaves, & becomes a Delocalised Electron. These Move Freely Inbetween the Layers of Graphene. They Enable the Conduction of Electricity.

79
Q

Why do both the Macromolecular Structures Diamond & Graphite have very High MPs?

A

Because of Strong Covalent Bond Forces in the Giant Structure. It takes a lot of Energy to Break the Many Strong Covalent Bonds.

80
Q

What is ‘Electronegativity’?

A

Electronegativity is the Power of an Atom to Attract the Electron Density (or Pair of Electrons) of a Covalent Bond Towards Itself.

81
Q

The Electronegativity of an Atom Depends on: (3)

A

-Nuclear Charge.

-Shielding.

-Atomic Radius.

82
Q

What is Electronegativity Measured on?

A

The Pauli Scale.

83
Q

What is ‘Polarity’?

A

Polarity is the Unequal Sharing/Attraction of Electron Pairs in a Bond.

84
Q

If the Electron Sharing/Attraction is Equal, the Bond is described as…

A

Non-Polar.

85
Q

There is a ___ of Ionic-Covalent Bonds.

A

Spectrum.

86
Q

The ___ of the Molecule/Compound Determines its Place on the…

A

Ionic-Covalent Spectrum.

87
Q

What are the different Places that Bonds Can be Situated on the Ionic-Covalent Spectrum? (4)

A

-Fully Ionic.
-Polar Ionic.
-Polar Covalent.
-Fully Covalent.

88
Q

Types of Intermolecular Forces: (3)

A

-Van der Waals’ Forces (Induced Dipole).

-Dipole Forces (Act Between Certain Types of Molecules).

-Hydrogen Bonding (Act Between Hydrogen) & other Atoms).

A-LEVEL CHEM 3.1: Physical Chemistry (6 decks)

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