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OCR Chemistry > 2.2 ELECTRONS,BONDING & STRUCTURE > Flashcards

2.2 ELECTRONS,BONDING & STRUCTURE Flashcards

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1
Q

State the number of electrons that can fill the first four shells

A
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2
Q

Shape of s-orbitals

A
  • Spherical shape
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3
Q

Shape of p-orbitals

A
  • 3D dumb-bell shape
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4
Q

How many electrons can an s-orbital hold?

A

2

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5
Q

How many electrons can a p-orbital hold?

A

6

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6
Q

How many electrons can a d-orbital hold?

A

10

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7
Q

Which shells contain s-orbitals?

A
  • All shells
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8
Q

Which shells contain p-orbitals?

A
  • From n=2 upwards
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9
Q

Which shells contain d-orbitals?

A
  • From n=3 upwards
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10
Q

Does 4s or 3d have a higher energy level?

A
  • 3d has a higher energy level so is filled first
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11
Q

Define ionic bonding

A
  • The electrostatic attraction between positive and negative ions
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12
Q

Describe giant ionic lattice structure

A
  • Repeating pattern of oppositely charged ions with strong electrostatic attraction in all directions
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13
Q

Explain the melting/boiling point of a giant ionic lattice

A
  • Strong ionic bonds in all directions means lots of energy needed to overcome these bonds, so has a high mp/bp
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14
Q

Explain the electrical conductivity of a giant ionic lattice

A
  • Giant ionic lattices can only conduct when melted/dissolved because ions are not mobile/cant move in the solid state
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15
Q

Explain the solubility of a giant ionic lattice

A
  • Giant ionic lattices are soluble in polar solvents (e.g water) because polar water molecules can interact/break apart the ions
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16
Q

Define covalent bonding

A
  • The strong electrostatic attraction between a shared pair of electrons and the nucleus of the bonded atoms
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17
Q

Define dative covalent bonding

A
  • When one atom provides both of the shared electrons in a covalent bond
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18
Q

What type of bonding does average bond enthalpy measure?

A
  • Covalent bond
19
Q

Compare the relative repulsion strengths of bonded pairs of electrons and lone pairs of electrons

A
  • Lone pair repulsion is greater than bonded pair repulsion
20
Q

Draw the shape and bond angle of a linear molecule.

A
21
Q

Draw the shape and bond angle of a non-linear molecule.

A
22
Q

Draw the shape and bond angle of a trigonal planar molecule.

A
23
Q

Draw the shape and bond angle of a pyramidal molecule.

A
24
Q

Draw the shape and bond angle of a tetrahedral molecule.

A
25
Q

Draw the shape and bond angle of a octahedral molecule.

A
26
Q

Define electronegativity

A
  • An atoms ability to attract the bonding electrons in a covalent bond
27
Q

State the most electronegative element

A
  • Fluorine
28
Q

State and explain electronegativity across a period.

A
  • Electronegativity increases
  • Atomic charge (proton number) increases so there is a stronger attraction between nucleus and bonded electrons in a covalent bond
29
Q

State and explain electronegativity up a group.

A
  • Electronegativity increases
  • Atomic radius decreases due to less shells so theres less electron sheilding
  • Atomic radius decreases due to less shells so shorter distance between nucleus and bonded electrons in a covalent bond
  • Therefore, stronger attraction
30
Q

Define polar bond

A
  • When a difference in electronegativitys causes a perminant dipole
31
Q

State 2 requirements for a molecule to be polar.

A

1) Must have a polar bond (perminant dipole)
2) Must be assymetrical so dipoles dont cancel out

32
Q

State the three types of intermolecular forces

A

1) London/induced temporary dipole-dipole forces
2) Perminant dipole-dipole forces
3) Hydrogen bonding

33
Q

Which types of molecules have london/induced temporary dipole-dipole forces?

A
  • ALL molecules
34
Q

Which types of molecules have perminant dipole-dipole forces?

A
  • Polar molecules
35
Q

Which types of molecules have hydrogen bonding?

A
  • Only molecules with H and O, N, F
36
Q

Define hydrogen bonding

A
  • A type of perminant dipole-dipole interaction between an electron deficient hydrogen (δ+) and a lone pair of electrons on O,F,N
37
Q

State what the strength of London/induced temporary dipole-dipole forces depends on

A
  • Number of electrons
  • More electrons = stronger london forces
38
Q

Draw hydrogen bonding between water molecules

A
39
Q

Explain the 2 effects of hydrogen bonding on water properties

A
  • Higher than expected MP/BP because of additional hydrogen bonding that requires more energy to overcome
  • Ice is less dense than water because additional hydrogen bonding gives it an open lattice structure
40
Q

Describe the solid structure of simple molecular lattices

A
  • Covalent bonds between atoms
  • Attracted by intermolecular forces (NAME IT)
41
Q

Explain the electrical conductivity of simple molecular lattices

A
  • Not conductive because there are no charged particles that are free to move
42
Q

Explain the solubility of simple molecular lattices

A
  • They are non-polar so only soluble in non-polar solvents as weak london forces can form between molecules and non-polar solvent to break apart the simple molecular lattice
43
Q

Explain the MP/BP of simple molecular lattices

A
  • Relatively low MP/BP because of relatively weak intermolecular forces (NAME IT) that do not require great amounts of energy to overcome

OCR Chemistry (13 decks)

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