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

Topic 2: Chemical Bonding and Structure Flashcards

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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
Q

What is a discrete molecule?

A

-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
Q

Displayed formula

A

-Shows each bonding pair as a line in between

27
Q

How is a dative covalent bond formed?

A

-an empty orbital overlaps with an orbital containing a lone pair of electrons of another atom

28
Q

Examples of dative covalent bonds

A

Al2Cl6, Ammonium ion (NH4)

29
Q

Dipole

A

two opposite charges of equal magnitude are separated by a small distance in a compound

30
Q

What are the 3 types of intermolecular interactions

A
  1. London forces
  2. Permanent Dipoles
  3. Hydrogen Bonds
31
Q

Explain London forces (instantaneous dipole-induced dipole interactions)

A
  • 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
Q

Explain Permanent dipole-dipole interactions

A
  • 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
Q

Van der walls forces

A

-London forces
-Permanent dipole-dipole interactions
(you can use this phrase, to sum up, both interactions)

34
Q

What elements can form hydrogen bonds?

A

O, F, N

35
Q

Define a hydrogen bond

A
  • 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
Q

How many hydrogen bonds can water form?

A

2 hydrogen bonds because of the 2 lone pairs

37
Q

What is the only fluorine compound that can form a hydrogen bond?

A

HF

38
Q

Why does increasing the molecular mass increase the boiling point?

A
  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
Q

Why Does H-F have a higher boiling point than HCl, HBr, HI

A

HF can form hydrogen bonds

40
Q

Properties of water

A
  1. High melting and boiling points (Hydrogen bonds)

2. Density as solid is less than as a liquid

41
Q

Why is water less dense as a solid?

A
  • Ring structure

- Creates more open space

42
Q

Rule of thumb for aqueous solvents

A

like dissolves with like

43
Q

What substances form giant COVALENT LATTICES

A
  • Diamond
  • Graphite
  • Graphene
  • Silicon(IV) oxide

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