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funny fun subject > Topic 2: Chemical Bonding and Structure > Flashcards

Topic 2: Chemical Bonding and Structure Flashcards

bonds init

1
Q

Nature of Metallic Bonding (Name 5 properties)

A
  • High melting point
  • Good Electrical/Thermal Conductor
  • Malleable
  • Ductile
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2
Q

Define Metalic Bonding

A

strong electrostatic attraction between metal ions and the delocalised electrons

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3
Q

Delocalised electrons

A

Electrons that are not associated with any single atom or any single covalent bond

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4
Q

How do you determine the strength of an ionic bond?

A

Amount of energy required to make one mole of an ionic compound gaseous

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5
Q

Define Ionic Bonding

A

Strong electrostatic interactions between oppositely charged ions

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6
Q

If you increase the size of the anion or the cation what will happen to the required energy to break the bonds?

A

Decrease with the increase in radii (ofc it does)

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7
Q

Trends in ionic radii down a group

A

As you go down the group the radii increases as more electron shells and shielding

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8
Q

Trends in ionic radii across a period

A
  • decreases as there is an increase in nuclear charge and a decrease in electrons
  • this means there is a stronger attraction between the nucleus and the electron cloud pulling it closer into the nucleus
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9
Q

4 Properties of ionic Compounds

A
  • High melting point
  • Brittle
  • Electrically conductive in the liquid state
  • Often soluble in water
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10
Q

Why do Ionic compounds have a high melting point?

A
  • Combined electrostatic forces of attraction of the ions is large
  • Therefore a large amount of energy is required for the ions to break free from the lattice
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11
Q

Why are ionic compounds brittle?

A
  • The layer of the ionic solid might slide over each other
  • This causes ions of the same charge to line up next to each other
  • Causing them to repel one another causing the crystal to break
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12
Q

Electrical conductivity of ionic compounds?

A
  • Solid ionic compounds don’t conduct electricity as there are no delocalised electrons and the ions are not free to move
  • Molten and Aqueous ionic compounds can conduct because:
  • Ions are now mobile ( FREE TO MOVE)
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13
Q

Explain the solubility of ionic compounds

A
  • Many ionic compounds are soluble
  • Energy required to break the lattice structure can be supplied by the hydration of the separated ions produced (think of solvation shells)
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14
Q

What is the evidence for the existence of ions?

A
  • Electrolysis

- Migration of ions to the +/- electrodes

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15
Q

Covalent bond

A

The strong electrostatic attraction between two nuclei and the bonding pair of electrons

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16
Q

How is a covalent bond formed?

A

Overlap of an orbital(s) from another atom

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17
Q

Sigma Bonds

A

End on overlap between s or p orbitals

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18
Q

Pi Bonds

A

Sideways overlap between 2 p orbitals

19
Q

What are the 3 ways a sigma bond can be made?

A

s-s overlap
p-p overlap
s-p overlap

20
Q

What is the relationship between bond length and bond strength?

A
  • shorter the bond length stronger the bond strength

- This is due to a greater electrostatic attraction between the two nuclei and the bonding pair of electrons

21
Q

Define Bond length

A

distance between nuclei of the two atoms that are covalently bonded together

22
Q

Define Electronegativity

A

the ability of an atom to attract a bonding pair of electrons in a covelant bond

23
Q

What is a polar covalent bond?

A

Type of covalent bond where the bonding electrons are unequally distributed (dipoles)

24
Q

Continuum of bonding type

A
  • The polarity of the covalent bond means it’s either more ionic or purely covalent
  • Most bonds are in between
25
What is a discrete molecule?
-Simple molecule an electrically neutral group of two or more atoms held together by chemical bonds (e.g. diatomic molecules or like C60 bucky balls)
26
Displayed formula
-Shows each bonding pair as a line in between
27
How is a dative covalent bond formed?
-an empty orbital overlaps with an orbital containing a lone pair of electrons of another atom
28
Examples of dative covalent bonds
Al2Cl6, Ammonium ion (NH4)
29
Dipole
two opposite charges of equal magnitude are separated by a small distance in a compound
30
What are the 3 types of intermolecular interactions
1. London forces 2. Permanent Dipoles 3. Hydrogen Bonds
31
Explain London forces (instantaneous dipole-induced dipole interactions)
- Fluctuations of electron densities creates instantaneous dipoles - This can induce the dipoles of other molecules creating an attraction - The attractive forces increase with the number of electrons
32
Explain Permanent dipole-dipole interactions
- The attraction between oppositely charged permanent dipoles - In large molecules, London forces are more prevalent but in smaller molecules, with dipoles, Permanent dipoles are more prevalent
33
Van der walls forces
-London forces -Permanent dipole-dipole interactions (you can use this phrase, to sum up, both interactions)
34
What elements can form hydrogen bonds?
O, F, N
35
Define a hydrogen bond
- intermolecular interaction between a hydrogen atom of a molecule - Bonded to an atom that is more electronegative ( except C) than hydrogen and another atom in the same or different molecule
36
How many hydrogen bonds can water form?
2 hydrogen bonds because of the 2 lone pairs
37
What is the only fluorine compound that can form a hydrogen bond?
HF
38
Why does increasing the molecular mass increase the boiling point?
1. Number of electrons increase so greater London forces 2. Length of the carbon chain increases increase in the number of points of contact between adjacent molecules ( more London forces at each point of contact) 3. Therefore a greater overall intermolecular force of attraction
39
Why Does H-F have a higher boiling point than HCl, HBr, HI
HF can form hydrogen bonds
40
Properties of water
1. High melting and boiling points (Hydrogen bonds) | 2. Density as solid is less than as a liquid
41
Why is water less dense as a solid?
- Ring structure | - Creates more open space
42
Rule of thumb for aqueous solvents
like dissolves with like
43
What substances form giant COVALENT LATTICES
- Diamond - Graphite - Graphene - Silicon(IV) oxide

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