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Bonding & Structure Flashcards

1
Q

Bonding & Structure: Intermolecular Forces

What are the Chemical Bonds?

A
  • Ionic
  • Covalent
  • Dative Covalent (co-ordinate)
  • Metallic
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2
Q

Bonding & Structure: Intermolecular Forces

What are Ions?

A

Atoms that gain or lose electrons

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3
Q

Bonding & Structure: Ionic Bonding

What is Ionic Bonding?

A

The electrostatic attraction between oppositely charged ions

Formed when atoms lose or gain electrons

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4
Q

Bonding & Structure: Ionic Bonding

What 2 things affect the strength of an Ionic Bond?

A
  • Ionic Charges
  • Ionic Radii
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5
Q

Bonding & Structure: Ionic Bonding

What’s the relationship between charge & an Ionic Bond?

A

The greater the charge, the stronger the ionic bond
↳ higher the mp/bp

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6
Q

Bonding & Structure: Ionic Bonding

What’s the relationship between radii & an Ionic Bond?

A

Smaller ions can pack closer together than larger ions : have a stronger ionic bond
↳ higher the mp/bp

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7
Q

Bonding & Structure: Intermolecular Forces

What does the size of an Ion depend on?

A
  • Electron shell
  • Atomic number
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8
Q

Bonding & Structure: Intermolecular Forces

What happens to the Ionic Radius as u go Down a group?

(they have the same charge but..)

A

INCREASES
* atomic number increases
↳ extra electron shells are added

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9
Q

Bonding & Structure: Intermolecular Forces

What happens to the Ionic Radius of a set of isoelectric ions?

A

DECREASES
* atomic number increases
↳ proton number increases : electrons are attracted to nucleus, pulling them in

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10
Q

Bonding & Structure: Intermolecular Forces

What do Ionic Compounds form?

A

Giant Ionic Lattices

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11
Q

Bonding & Structure: Intermolecular Forces

Why are Giant Ionic Lattices formed?

A

Each ion is electrostatically attracted in all directions to ions of opposite charge

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12
Q

Bonding & Structure: Intermolecular Forces

Why are Giant Ionic Lattices described as Giant?

A

They’re made up of the same repeated basic unit

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13
Q

Bonding & Structure: Intermolecular Forces

Why do Ionic Compounds have a High mp?

A

Lots of heat is needed to overcome strong electrostatic attractions

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14
Q

Bonding & Structure: Intermolecular Forces

Why are Ionic Compounds very brittle?

A

Solid at room temp & pressure : any dislocation leads to the layers moving & splitting

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15
Q

Bonding & Structure: Intermolecular Forces

Why don’t Ionic Compounds conduct Electricity?

A

Ions aren’t delocalised ions are held strongly in the lattice

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16
Q

Bonding & Structure: Intermolecular Forces

Why do Ionic Compounds only conduct Electricity when molten?

A

The ions become mobile, they’re delocalised so they can carry a charge

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17
Q

Bonding & Structure: Intermolecular Forces

Why are Ionic Compounds soluble in water but not non-polar solvents?

A

Their particles are charged

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18
Q

Bonding & Structure: LAB

What happens when u electrolyse Copper (II) Chromate (VI)? [green]

A

Filter paper turns:
* BLUE at Cathode
* YELLOW at Anode

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19
Q

Bonding & Structure: LAB

Why does this colour change occur?

A
  • Positive ions move to Cathode
  • Negative ions move to Anode
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20
Q

Bonding & Structure: Intermolecular Forces

What is Covalent Bonding?

A

Electrostatic attraction between shared electrons & nuclei

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21
Q

Bonding & Structure: Intermolecular Forces

What does Covalent Bonding usually happen between?

A

Non-metals

Nv2 has a triple bond

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22
Q

Bonding & Structure: Intermolecular Forces

What are the positive nuclei attarcted to in a Covalent Bond?

A

Where the shared electrons are

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23
Q

Bonding & Structure: Intermolecular Forces

How is a force of repulsion formed?

A
  • 2 positive nuclei repel each other
  • electrons repel each other
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24
Q

Bonding & Structure: Intermolecular Forces

Why is a Bond Length needed?

A

To maintain a covalent bond

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25
# **Bonding & Structure:** Intermolecular Forces What is Bond Length?
Distance between the nuclei ↳ where attractive & repulsive forces balance each other
26
# **Bonding & Structure:** Intermolecular Forces Whats the relationship between Bond Length & Bond Strength?
Inversely proportional
27
# **Bonding & Structure:** Intermolecular Forces Why's the relationship between Bond Length & Bond Strentgh this way?
More electrons in a bond **:** stronger attraction between atoms ↳ higher the Bond Enthalpy & shorter the Bond Length
28
# **Bonding & Structure:** Intermolecular Forces Why's the Mp/Bp in Covalent Bonding low?
Intermolecular forces are broken NOT covalent bonds
29
# **Bonding & Structure:** Intermolecular Forces Why don't Covalent Bonds conduct electricity?
Atoms are held in place
30
# **Bonding & Structure:** Intermolecular Forces Are Covalent Bonds soluble in water?
Depends on whether it can form H bonds
31
# **Bonding & Structure:** Intermolecular Forces Whats a Dative Covalent (Co-ordinate) Bond?
Both electrons are provided by the same atom
32
# **Bonding & Structure:** Intermolecular Forces What's a Reduced Octet?
Molecule stable without a full outer shell
33
# **Bonding & Structure:** Intermolecular Forces What's an example of a Stable Covalent Compound? | (Reduced Octet)
AlCl3
34
# **Bonding & Structure:** Intermolecular Forces What happens when 2 AlCl3 combine?
One Cl in each of the 2 AlCLv3 molecules donates a lone pair to the Al on the other molecule, forming 2 dative covalent bonds | This gives Al a full outer shell
35
# **Bonding & Structure:** Intermolecular Forces What is Metallic Bonding? | S-block/D-block
Involves a lattice of positive ions sorrounded by delocalised electrons
36
Metallic Bond | S-block/D-block
Mobile electron cloud allows the conduction of electricity
37
# Metallic Properties | S-block/D-block
* Mp = **HIGH** ↳Hard to seperate positive ions & delocalised electrons * Strength = **HARD** ↳ * Solubility = **INSOLUBLE** ↳ * Electricity = **YES** ↳ Already has delocalised electrons * Malleable & Ductile ↳ No real bonds holding the metal ions together, the layers are separated by electrons
38
Ease of separation of ions | Depends on...
1. Electron density of the cloud 2. Ionic/Atomic size
39
# Ease of separation of ions Instance 1)
* Charge * Atomic Radius
40
# Ease of separation of ions Instance 2)
* Atomic Radius ↓ -larger atom ↳ more QL = more electrons -electron in outershell is FURTHER AWAY ↳ **easier to lose**
41
Metals have Giant Structures too | Metals exist as giant metallic lattice structures.
Electrons in the outermost shell of the metal are delocalised. The positive metal ions are electrostatically attracted to the negative delocalised electrons ***Higher Charge of cathine = Smaller the Cathine = Stronger the Metallic Bond***
42
Giant Covalent & Metallic Structures
***Diamond*** * 4 carbons **TETRAHEDRALLY** bonded ***Silicon Dioxide*** SiOv2 * Oxygen atoms situated between each silicon atom
43
Other Giant Covalent & Metallic Structures
***Graphite*** * *Each carbon* is bonded to **3 other carbon atoms** * **4th carbon** is delocalised → can **conduct electricity** ***Graphene*** * A *thin layer of graphite* * Can conduct electricity * Strong * Light
44
# Giant Covalent & Metallic Structures Properties
* Mp = **HIGH** ↳ A lot of heat to break * Strength = **EXTREMELY HARD** ↳ Strong bonds * Thermal Conductor = **GOOD** ↳ They vibrate * Solubility = **INSOLUBLE** ↳ Do not contain ions * Electricity = **CAN'T CONDUCT** ↳ No free electrons
45
All Chemical Bonds Properties
46
Physical Attractions | Intermolecular = outside
* Instantaneous/Induced (London Forces) * Permanent Dipole Interactions * Hydrogen Bonds
47
Instantaneous/Induced (London Force)
Every compound in chem has a **LONDON FORCE** * London forces take place where there are electrons
48
# Instantaneous/Induced (London Force) Function
* Electrons always move around an atom ↳ as they move, they would induce a slight charge & induce a neighbouring atom w the opposite charge ↓ *This attraction is short/small* → this is a **London Force** * Electrons still move & break this attraction ↓ everything is repeated | More electrons a compound has = higher the London Force
49
Simple Molecular Lattice
In Iodine the molecules are held by covalent bonds to form Iv2. Between the molecules are **London Forces**
50
Stronger London Force = Higher Mp/Bp
* **Less branches** = **higher** ***Mp*** ↳ compound is getting longer when unbranched → meaning there are more electrons → the stronger the **London Force**
51
Permanent Dipole
Somewhere in between Ionic charged & Covalent * Occurs between molecules containing polar/ electronegative bonds | HCL & NHv3
52
Permanent Dipoles occur as well as London Forces
Molecules that show **London Forces** in addition to **Permanent Dipole** will have a **higher** *mp/bp* than those than show *only London Forces* | F/O/N bonded w H = permanet dipole/polar/ → more energy needed to break
53
# Hydrogen Bonding Definition
Occurs when hydrogen is bonded to flourine, nitrogen or oxygen
54
Hydrogen Bonding
* Water, ammonia & hydrogen flouride all show hydrogen bonding * Looking down group 7, the element becomes a permanent diapole
55
Bp of Group 6 Hydrides
* Hv2O is the highest as its the most electronegative * Hv2Se & Hv2Te are higher than Hv2S because they have a larger atomic radius, therefore there are more electrons which means a stronger LF
56
Bp of Group 7
* HF is the highest as its the most electronegative * HBr & HI are higher than HCl as they have a larger atomic radius, therefore there are more electrons which means a stronger LF | Trend is there's a decrease in permanent dipole interactions
57
Hydrogen Bonding explains Ice Floats on water
* In ice,water molecules are arranged apart which wastes a lot of space * As ice melts, the hydrogen bonds break, the lattice breaks allowing air molecules to fill these spaces * This means ice is much less dense than water → so floats
58
Shapes of Molecules
* C-C single * C=C double * C≡C triple Going down these bullet points the bonds become; More rigid/strong Shorter Harded to break so more heat is needed as its harder to move/twist them | This is regardless the number of atoms on each other side
59
Valence Shell Electron Pair Repulsion Theory | VSEPR
Any compound has a shape after repulsion theory | "The best arrangement is the one that minimises the repulsion"
60
# Shape, Angles, Examples Linear | BeClv2
* 2 Bond Pairs * 180° Bond Angle
61
# Shape, Angles, Examples Triginal Planer | AlClv3
* 3 Bond Pairs * 120° Bond Angle
62
# Shape, Angles, Examples Tetrahedral | CHv4
* 4 Bond Pairs * 109.5° Bond Angle
63
# Shape, Angles, Examples Trigonal Bipyromidal | PClv5
* 5 Bond Pairs * 120° & 90° Bond Angle
64
# Shape, Angles, Examples Octahedral/Hexagonal | SFv6
* 6 Bond Pairs * 90° Bond Angles
65
# Shape, Angles, Examples Pyramidal | NHv3
* 3 Bond Pairs * 107° Bond Angle * 1 Pair of lone electrons
66
# Exception Group 2 Berylium
-In Group 2 **Be** *only* forms a **covalent bond** ↳ because its *more stable* w *sharing electrons than donating*
67
Reduced Octet | Be in BeClv2 or Al in AlClv3
Are **stable** with ***less** than 8 electrons* around their **central atom**
68
Expanded Octet | P in PClv5 or S in SFv6
Are **stable** with ***more** than 8 electrons* around their **central atom**
69
Lone Pairs
Every lone pair that you introduce to a compound, you'll decrease the bond angle by 2 1/2° * Lone pairs repel each other ↳ pushing bond angles → bond angles are pushed inwards

Chemistry (13 decks)

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