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IB Chemistry > Unit 2 Bonding > Flashcards

Unit 2 Bonding Flashcards

1
Q

Define delocalized electron

A

A valence electron that is able to roam freely among cations in a lattice structure

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2
Q

What are the metallic properties?

A
  • Conductivity of electricity
  • Malleable
  • Ductile
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3
Q

Define malleable

A

reshape under pressure

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4
Q

Define ductile

A

Drawn into a thin wire

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5
Q

What is a cation?

A

A positive ion

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6
Q

What is an anion?

A

A negative ion

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7
Q

What is an Ionic Bond?

A

A bond between a metal and a non-metal

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8
Q

How do you name Ionic Compounds?

A

the ending of the compound ends in “-ide”

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9
Q

What physical properties will the crystal lattice structure influence?

A
  • Texture
  • Melting and Boiling points
  • Volatility
  • Conductivity
  • Solubility
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10
Q

Define volatility

A

Rate of evaporation

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11
Q

What is the characteristic of non-polar covalent bonds?

A

No electronegativity difference

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12
Q

What is the characteristic of polar covalent bonds?

A

slight electronegativity difference (less than 1.8)

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13
Q

What is the name for NO3^-

A

nitrate

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14
Q

What is the name for OH^-

A

hydroxide

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15
Q

What is the name for SO4^2-

A

sulfate

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16
Q

What is the name for CO3^2-

A

carbonate

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17
Q

What is the name for PO4^3-

A

phosphate

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18
Q

What is the name for HCO3^-

A

bicarbonate/hydrogen carbonate

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19
Q

What is the name for NH4^+

A

ammonium

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20
Q

What is the prefix for 1?

A

mono

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21
Q

What is the prefix for 2?

A

di

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22
Q

What is the prefix for 3?

A

tri

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23
Q

What is the prefix for 4?

A

tetra

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24
Q

What is the prefix for 5?

A

penta

25
Q

What is the prefix for 6?

A

hexa

26
Q

What is the prefix for 7?

A

hepta

27
Q

What is the prefix for 8?

A

octa

28
Q

What is the prefix for 9?

A

nona

29
Q

What is the prefix for 10?

A

deca

30
Q

What is the name for H2O?

A

water

31
Q

What is the name for CH4?

A

methane

32
Q

What is the name for NH3?

A

ammonia

33
Q

What are the allotropes of Carbon?

A
  • Diamond
  • Graphite
  • Buckminsterfullerene
34
Q

What are the characteristics of a diamond?

A
  • one carbon atom is covalently bonded to four other carbons
  • Bonds are shared equally
  • very hard and high melting point
  • formed under high pressure but don’t last forever
35
Q

What are the characteristics of graphite?

A
  • Organized into layers of hexagonal rings
  • one carbon is strongly bonded to three other carbons within the layer
  • very weak bonds between carbons in layers above and below
36
Q

When was buckminsterfullerene discovered?

A

1985

37
Q

What are the characteristics of buckminsterfullerene?

A

Consists of 60 carbons arranged in hexagons and pentagons (similar to a soccer ball pattern)

38
Q

What new branch of science did the buckminsterfullerene lead to?

A

Nanotechnology

39
Q

What does VSEPR Theory stand for?

A

Valence Shell Electron Pair Repulsion

40
Q

What does symbol “E” represent in the VSEPR Theory?

A

lone pair

41
Q

What does symbol “A” represent in the VSEPR Theory?

A

Central atom

42
Q

What does symbol “B” represent in the VSEPR Theory?

A

Bonded atoms

43
Q

State the shape and the bond angle for the formula AB(E)n

A

Shape: Linear

Bond angle: N/A

44
Q

State the shape and the bond angle for the formula AB2

A

Shape: linear

Bond angle: 180°

45
Q

State the shape and the bond angle for the formula AB3

A

Shape: Triginal Planar

Bond angle: 120°

46
Q

State the shape and the bond angle for the formula AB4

A

Shape: Tetrahedral

Bond angle: 109.5°

47
Q

State the shape and the bond angle for the formula AB2E

A

Shape: Angular

Bond angle: 120° > x > 90°

48
Q

State the shape and the bond angle for the formula AB2E2

A

Shape: Angular

Bond angle: 109.5° > x > 90°

49
Q

State the shape and the bond angle for the formula AB3E

A

Shape: Trigonal Pyramidal

Bond angle: 109.5° > x > 90°

50
Q

What are the steps for determining the shape and bond angle using the VSEPR Theory?

A

1) Draw out electron dot diagram
2) Count the bonded and lone pair electrons around the central atom
3) Write out the general formula
4) State the shape and the bond angle

51
Q

What is a central atom?

A

The atom with the most bonding spots

52
Q

What are the types of dipoles?

A

Permanent and temporary/induced

53
Q

What criteria must be met in order for a molecule to be polar?

A

1) It must have at least one polar bond
2) The arrangement of the bonds must be asymmetric. Central atom has either: a) lone pair of electrons and/or b) different atoms bonded to it

54
Q

What type of attractive forces do non-polar molecules have?

A

only London Dispersion forces

55
Q

What is the strongest intermolecular force?

A

Hydrogen bonding

56
Q

Define intermolecular force and give an example

A

The attraction force between molecules

ex. hydrogen bonding between two molecules of water

57
Q

Define intramolecular forces and give an example

A

The attraction force between to atoms within a molecule

ex. ionic or covalent bonds

58
Q

When will London Dispersion Forces become stronger?

A

When:

  • molar mass of molecule increases
  • length of chained molecule increases
59
Q

What are the three elements that can from a Hydrogen bond?

A

Fluorine, oxygen, or nitrogen

IB Chemistry (8 decks)

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