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Chemistry IB SL 32S > Test on Thursday November 3, 2016 > Flashcards

Test on Thursday November 3, 2016 Flashcards

1
Q

What are the three Allotropes of Carbon?

A

Diamond

Graphite

Buckminsterfullerene

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2
Q

What is the Bond Angle of Tetrahedral?

A

109.5° (AB₄)

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3
Q

As the bonds go from single to double to triple, the length between atoms BLANK.

A

Decreases

Example:
C−C is 0.154nm
C=C is 0.134nm
C≡C is 0.120nm

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4
Q

What is the third order to consider for IMF strength? 3

A

Length of Carbon Chain

💨 Longer chain has higher IMF

💨 Branches on chains reduce IMF

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5
Q

What is the Bond Angle of Pyramidal? 2

A

109.5° > x > 90° (AB₃E)

Specifically 107°

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6
Q

What is the Bond Angle of (AB₂)?

A

180°

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7
Q

What is the Shape of (AB₂)?

A

Linear

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8
Q

What is the Bond Angle of (AB₄)?

A

109.5°

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9
Q

What is the Bond Angle of Trigonal Planar?

A

120°

360/3

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10
Q

What is the first order to consider for IMF strength? 3

A

Polarity of molecules

💫 More polar has higher IMF

💫 If both Non-Polar use #2

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11
Q

What is the Bond Angle of (AB₃E)? 2

A

109.5° > x > 90°

Specifically 107°

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12
Q

What type of molecules have Non-Polar and Polar ends and may dissolve in both (like soap).

A

Some chained molecules

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13
Q

What is the second order to consider for IMF strength? 3

A

Molar Mass of molecules

✨ Larger mass has higher IMF

✨ If both of equal mass use #3

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14
Q

What is the Bond Angle of (AB₂E)?

A

120° > x > 109.5°

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15
Q

What is the Bond Angle of (AB₂E₂)? 2

A

109.5° > x > 90°

Specifically 104.5°

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16
Q

Rank the following forces, (Ionic Bond, London Dispersion, Dipole-dipole, Covalent Bonds and Hydrogen Bonding) in order from weakest to strongest and provide an example of each.

A

London Dispersion

Dipole-Dipole

Hydrogen Bonding

Ionic Bonding

Covalent Bonding

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17
Q

What is the Bond Angle of Linear?

A

180°

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18
Q

What is ductility?

A

A metal’s ability to be drawn into a thin wire

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19
Q

What is the Shape of (AB₃)?

A

Trigonal Planar

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20
Q

What is an alloy?

A

A mixture of 2 or more metal atoms

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21
Q

What is the second order to consider for IMF strength? 3

A

Molar Mass of molecules

✨ Larger mass has higher IMF

✨ If both of equal mass use #3

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22
Q

Which liquids would Non-Polar covalent substances dissolve in?

A

They would dissolve in other Non-Polar liquids.

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23
Q

What is Malleability? 2

A

A metal can be bent and reshaped under pressure

Layers of positive ions can slide over each other reforming metallic bonds

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24
Q

What is the Bond Angle of Angular?

A

120° > x > 109.5° (AB₂E)

or

109.5° > x > 90° (AB₂E₂)

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25
Q

What is the Bond Angle of (AB₃)?

A

120°

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26
Q

What is the first order to consider for IMF strength? 3

A

Polarity of molecules

💫 More polar has higher IMF

💫 If both Non-Polar use #2

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27
Q

Explain the process of Hydration. 3

A

It occurs when Ionic Substances dissolve in water

Water molecules surround the ions at the edge of the lattice and pull them off.

The stronger the ionic bond, the less soluble the compound is in the water.

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28
Q

What is the Shape of (AB₃E)?

A

Pyramidal

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29
Q

What is the Shape of (AB₄)?

A

Tetrahedral

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30
Q

What are Intermolecular Forces? 4

A

Force of attraction between molecules

Also called Van der Waals’ forces

Much weaker than forces within molecules

The more Polar the molecule, the stronger its attraction to a neighboring molecule

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31
Q

Rank the following forces, (Ionic Bond, London Dispersion, Dipole-dipole, Covalent Bonds and Hydrogen Bonding) in order from weakest to strongest and provide an example of each.

A

London Dispersion

Dipole-Dipole

Hydrogen Bonding

Ionic Bonding

Covalent Bonding

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32
Q

What is the third order to consider for IMF strength? 3

A

Length of Carbon Chain

💨 Longer chain has higher IMF

💨 Branches on chains reduce IMF

33
Q

What is the Shape of (AB₂E₂)?

A

Angular

34
Q

What is the Shape of (AB₂E)?

A

Angular

35
Q

What is the summation of Texture in Covalent solids? 2

A

They tend to be soft and waxy

Molecules slide past each other

36
Q

What is a Metallic bond?

A

Metals form a lattice of positive ions in which valence electrons are free to roam, called delocalized electrons.

A Metallic bond is the electrostatic attraction between a lattice of positive ions and the delocalized electrons

37
Q

What is the summation of /conductivity in Covalent substances?

A

They do not conduct electricity since they have NO FREE IONS or Electrons

38
Q

The stronger the IMF, the BLANK energy is needed to separate the molecules.

A

More

39
Q

What is the summation of Volatility in Covalent molecules? 2

A

They tend to be more volatile than ionic or metallic substances

Molecule breaks away more easily due to weak intermolecular forces

40
Q

What is the fixed charge of Ag?

A

Ag+1

41
Q

What is the general trend in Solubility between different kinds of compounds?

A

Like dissolves in Like

42
Q

Is water Polar or Non-Polar?

A

Polar because there are two positive Hydrogens attracted to an Oxygen

43
Q

What is the summation of Texture in Ionic substances? 2

A

They tend to be hard and brittle

Edges of lattice structure can break off

44
Q

At what temperature will sodium chloride melt?

A

801°C

45
Q

What are the 3 effects of Hydrogen Bonding?

A

HF, NH3 and H20 have unusually hugh boiling point and melting points compared with higher molar mass hydrides within their groups like HCl, PH3, and H2S, are all gases at room temperature

Water expands as it freezes. The molecules rearrange when they get close resulting in an open structure. Water is densest at 4°C and ice floats

DNA has a double helix structure.
The Hydrogen from one strand attracts to the nitrogen and oxygen in the other strand holding the strands together!

46
Q

What is the fixed charge of Al?

A

Al+3

47
Q

What is the summation of Texture in Covalent solids? 2

A

They tend to be soft and waxy

Molecules slide past each other

48
Q

What is the summation of Melting and Boiling points in Covalent substances? 3

A

They tend to boil at lower temperatures than Ionic or metallic substances.

Non-Polar molecules break away more easily due to weak IMF

Takes less energy or lower temperature

49
Q

What is Conductivity of electricity?

A

Flow of electrons

Delocalized electrons can move from one end of the metal quickly to the other

50
Q

What is Hydrogen Bonding? 6

A

Special case of dipole-dipole forces

Creates a very strong intermolecular force

Common susbstances where hydrogen bonding occurs

 Water (H20), ammonia (NH3) and HF

 Alcohols (R-OH), organic acids (R-COOH)

 DNA (Contains C, N, O and H)
51
Q

What is the fixed charge of Zn?

A

Zn+2

52
Q

At what temperature will water melt?

A

0°C

53
Q

How can we make an Ionic solid conduct electricity?

A

We need to dissolve it in water

and

Melt it

==============

When the ions are free to move, electricity will be conducted

54
Q

What are London Dispersion Forces? 4

A

Weakest IMF due to instantaneous induced dipoles

Will become stronger as
Molar mass of the molecule increases

 Length of chained molecule increases

Will still occur between polar molecules but effect is minimal.

55
Q

What is the summation of Texture in Ionic substances? 2

A

They tend to be hard and brittle

Edges of lattice structure can break off

56
Q

What is the summation of Melting and Boiling points in Ionic substances?

A

Ionic compounds melt at very high temperature.

57
Q

What is required in Hydrogen Bonding? 2

A

A very Polar Covalent bond of Hydrogen and another Small, more electronegative element (fluorine, oxygen, or nitrogen)

Attraction of above positive dipole hydrogen with a non-bonded electron pair of fluorine, oxygen or nitrogen atom in a neighbouring molecule

58
Q

What is the fixed charge of Cd?

A

Cd+2

59
Q

What are the 3 effects of Hydrogen Bonding?

A

HF, NH3 and H20 have unusually hugh boiling point and melting points compared with higher molar mass hydrides within their groups like HCl, PH3, and H2S, are all gases at room temperature

Water expands as it freezes. The molecules rearrange when they get close resulting in an open structure. Water is densest at 4°C and ice floats

DNA has a double helix structure.
The Hydrogen from one strand attracts to the nitrogen and oxygen in the other strand holding the strands together!

60
Q

What is the summation of Volatility in Ionic susbstances? 2

A

They tend to be less volatile than Covalent or metallic substances

Ions are too strongly attracted to separate

61
Q

What are the 2 types of dipole?

A

Permanent

and

Temporary/Induced Dipole

62
Q

What are Coordinate Bonds?

A

Normally each atom shares one e- to form the Covalent Bond, bit in some cases, one atom share 2 e- with another for a single bond

63
Q

What is the VSEPR Theory?

A

Model predicts the shape of molecules based on repulsion of e- pairs (e- domains)

 E- arrange so that they are as far as possible from each other
 Unbonded pairs of e- will repel more than unbonded pairs
64
Q

The BLANK the electronegativity difference, the more Polar the bond.

A

Higher

65
Q

How to know if a molecule is Polar? 2

A

If the difference in electronegativity for the atoms in a bond is greater than 0.4, we consider the bond polar.

If the difference in electronegativity is less than 0.4, the bond is essentially nonpolar.

66
Q

What is the strongest dipole-dipole force?

A

Hydrogen Bonding

67
Q

What are Resonance Structures?

A

Is when you can sometimes draw more than one Lewis Diagram used to describe e- positions.

68
Q

What are the 2 criteria for a molecule to meet in order to be Polar?

A

It must contain Polar bonds

The arrangement of the bonds must be asymmetic. Central atom has either:
Lone pair of e- and/or
Different atoms bonded to it

69
Q

What is the E in VSEPR Theory?

A

The # of lone pairs

70
Q

What does VSEPR Theory stand for?

A

Valence

Shell

Electron

Pair

Repulsion

71
Q

What is the B in VSEPR Theory?

A

The # of bonded pairs around the central atom

72
Q

What is the A in VSEPR Theory?

A

The central atom

73
Q

How to know if a molecule is Non-Polar? 2

A

If the difference in electronegativity for the atoms in a bond is greater than 0.4, we consider the bond polar.

If the difference in electronegativity is less than 0.4, the bond is essentially nonpolar.

74
Q

What is a Buckminsterfullerene? 3-5

A

Consists of 60 carbons arranged in hexagons and pentagons

 Similar to a soccer ball pattern

Other similar carbon molecules isolated

Led to a new branch of science

 Nanotechnology
75
Q

What is a diamond? 5-6

A

A giant Covalent structure.

Single molecule is very large

3D structure where each carbon atom is covalently bonded to four other carbon atoms.

 All bonds are equal, no plane of weakness

      Very hard, very high melting point

Formed under pressure, but aren’t forever

76
Q

Why is Buckminsterfullerene a molecule? 2

A

Because they can make bonds like water.

There is a limit to how big a Diamond and Graphite can be.

77
Q

What are other giant Covalent structures other than Diamond? 2

A

Sand

Pure Silicon

78
Q

What is a graphite? 5-7

A

Organized into layers of hexagonal rings

Each carbon atom is strongly bonded to three other carbons within the layer

Very weakly bonded to carbons in layers above and below

 Layers can slide across each other

      Good lubricant and write well

 Electrons delocalized between layers

      Good conductor of electricity

Chemistry IB SL 32S (6 decks)

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