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Chemistry 1 > Attractions & Repulsions > Flashcards

Attractions & Repulsions Flashcards

1
Q

What 3 assumptions are made for the ideal gas equation?

A
  • Molecules of the gas have zero volume
  • There are no interactions between gas molecules
  • All collisions are elastic (i.e have no energy loss)
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2
Q

What is the ideal gas equation, and what does each symbol represent?

A

pV = nRT
p = pressure (Pa)
V = volume (m^3)
n = no. moles
R = ideal gas constant (J K-1 mol-1)
T = temperature (K)

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3
Q

What determines the pressure of a gas?

A
  • The frequency of molecules hitting the wall of the container
  • The force the molecule exert on the wall when they hit (dependent on how fast they are moving)
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4
Q

Which combination of electronegativities tends to form covalent bonds?

A

Two highly electronegative atoms tend to form covalent bonds

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4
Q

Which combination of electronegativities tends to form covalent bonds?

A

Two highly electronegative atoms tend to form covalent bonds

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5
Q

Which combination of electronegativities tends to form ionic bonds?

A

One highly electronegative and one low electronegative atom tend to form ionic bonds

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6
Q

Which combination of electronegativities tends to form metallic bonds?

A

Two low electronegativity atoms tend to form metallic bonds

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7
Q

What are dipole moments?

A

Dipole moments are vectors that tell us the overall distribution of charge in the polar molecule

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8
Q

What are permanent dipoles?

A

Diatomic molecules containing two atoms with significantly differing electronegativities are said to have a permanent dipole (i.e. a permanent drawing of charge to one atom in the molecule)

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9
Q

Through what two methods can we measure if a molecule has a dipole moment?

A
  • Microwave spectroscopy
  • Measuring its dielectric constant
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10
Q

What is the difference in electronegativity for non-polar bonds?

A

Less than ~0.5

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11
Q

What is the difference in electronegativity for ionic bonds?

A

Greater than ~2

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12
Q

What is the difference in electronegativity for polar bonds?

A

Between ~0.5 and ~2

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13
Q

The greater the difference in electronegativity, the greater the…

A

Ionic character

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14
Q

What are two methods of measuring whether a molecule has a dipole moment?

A

Microwave spectroscopy
Measure it dielectric constant

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15
Q

How can we use microwave spectroscopy to find whether a molecule has a dipole moment?

A

In the gas phase, if the molecule has a dipole moment it will display a spectra

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16
Q

What is dielectric constant, and how does this tell us whether a molecule has a dipole moment?

A

Dielectric constant shows the ability of polar molecules to align in an electric field; if the molecule has a dipole moment, it will align

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17
Q

What is the equation for calculating the potential energy of dipole forces?

A

(Dipole moment 1 x Dipole moment 2) / Distance apart^3

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18
Q

Are there more intermolecular forces in liquids than solids?

A

No. There are more intermolecular forces in the solid state than liquid or gas

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19
Q

What is hydrogen bonding?

A

An extreme example of dipole-dipole interactions, between H and usually F, O or N

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20
Q

How many H-bonds form per water molecule?

A

4

21
Q

Why do ionic compounds dissolve in water?

A

Water is able to break strong ionic bonds by forming ion-dipole bonds

22
Q

What is polarisability of an atom?

A

The tendency of the electron field of an atom to become distorted when subjected to an electrical force

23
Q

What is the relationship between polarisability and electronegativity?

A

There is an inverse relationship between polarisability and electronegative.
Highly electronegative elements are not easily polarised

24
Q

What two factors increase polarisability?

A
  • Larger molecular size
  • More electrons
25
Q

Name all the intermolecular forces in order of decreasing strength

A

STRONGEST
Ion-dipole
Dipole-dipole
H-bonding
Dipole-induced dipole
London forces
WEAKEST

26
Q

What factors are responsible for dipole-induced dipole interactions?

A

The dipole moment of the polar molecule and the polarisability of the nonpolar molecule

27
Q

What are London dispersion forces?

A

Induced dipole-induced dipole interactions

28
Q

What feature of electron distribution allow London forces to form?

A

At any instant, the distribution of electrons are an atom will not be even, forming transient delta positive and delta negative dipoles

29
Q

How do London forces form?

A
  • Transient fluctuations in electron density
  • Transient dipoles
  • Transient induced dipoles in adjacent molecules
  • Attraction between these dipoles are London forces
30
Q

How does the size of the atom affect the strength of London forces?

A

The larger the atom, the more polarisable it becomes, so the stronger the London forces

31
Q

How does the compactness of the molecule affect the strength of London forces?

A

The more compact the molecule, the weaker the London forces

32
Q

What are the 4 types of crystalline solids?

A
  • Molecular structures (e.g. CO2)
  • Covalent network structures (e.g. Diamond)
  • Metals (e.g. Fe)
  • Ionic compounds (e.g. NaCl)
33
Q

What is the electrical conductivity and melting/boiling point of molecular structures?

A

Electrical conductivity = low
Melting/boiling point = low

34
Q

What is the solubility of molecular structures?

A

Some dissolve in water, many dissolve in organic solvents

35
Q

What is the electrical conductivity and melting/boiling point of covalent network structures?

A

Electrical conductivity = generally low
Melting/boiling point = very high

36
Q

What is the solubility of covalent network structures?

A

Generally insoluble in water and organic solvents

37
Q

What is the electrical conductivity and melting/boiling point of metals?

A

Electrical conductivity = good
Melting/boiling point = generally high

38
Q

What is the solubility of metals?

A

Insoluble

39
Q

What is the electrical conductivity and melting/boiling point of ionic compounds?

A

Electrical conductivity = high when molten or in aqueous solution
Melting/boiling point = high

40
Q

What is the solubility of ionic compounds?

A

Some soluble in water, but insoluble in organic solvents

41
Q

Why does evaporation occur at lower temperatures, rather than boiling?

A

At lower temperatures, the vapour pressure of the liquid is lower than the atmospheric pressure, meaning bubbles cannot form

42
Q

Why does boiling occur at higher temperatures?

A

At the boiling point, the vapour pressure of the liquid is equal to the atmospheric pressure, meaning bubbles can form and rise, and boiling occurs

43
Q

What is equilibrium vapour pressure?

A

A measure of the tendency of molecules to escape from the liquid phase and enter the vapour phase (evaporate)

44
Q

What is equilibrium vapour pressure dependent on?

A
  • Temperature
  • Intermolecular forces
45
Q

What is the relationship between intermolecular forces and equilibrium pressure?

A

The weaker the intermolecular interactions, the higher the equilibrium vapour pressure

46
Q

What is the conversion of solid directly to vapour known as?

A

Sublimation

47
Q

What is the conversion of vapour directly to solid known as?

A

Deposition

48
Q

What is the triple point?

A

The specific temperature and pressure on a phase diagram at which all three phases co-exist in equilibrium

49
Q

What phases are present at pressures below the triple point?

A

At pressure below the triple point, we do not see liquids, just solids and gases

50
Q

What is the critical point?

A

The point at which if you increase the temperature and/or pressure any further, you will get “supercritical fluid”

51
Q

What is “supercritical fluid”?

A

The state at which the lines between liquid and gas become blurred; the density of the substance is close to that of a liquid, but the viscosity is like that of a gas

Chemistry 1 (10 decks)

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