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Handout 1: States of Matter, Gases, Liquids and Phase transition > 1.5 > Flashcards

1.5 Flashcards

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1
Q

true or false: without intermolecular forces of attraction between particles, all particles will move independently and be gases

A

true

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2
Q

What does condensed phases mean?

A

liquids and solids

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3
Q

true or false: solid and liquid has similar densities

A

true, also they are both much denser than gas

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4
Q

Describe condensed phases

A
  • similar densities: particles are extremely close
  • particles no longer have enough KE to overcome intermolecular attractions
  • this is due to attraction between opposite charges
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5
Q

What is the physical state of a substance due to?

A

a balance between:

  • average kinetic energy of particles
  • potential energy of intermolecular attractions between particles
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6
Q

what is the type of intermolecular forces present depend on?

A

depends on the type of molecule

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7
Q

Briefly describe liquid physical properties

A

fluid
have surface properties
when pressure is applied to it, it is transmitted equally in all directions

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8
Q

What are intermolecular forces? Where do they occur?

A
  • collectively known as Van der Waals forces
  • they create structure in condensed phases
  • generally weak; occur BETWEEN molecules
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9
Q

When you boil a substance what do you break?

A

No, not the strong covalent bonding; which occurs WITHIN molecules, but rather the weak intermolecular forces which occur BETWEEN molecules

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10
Q

true of false: every molecule is attracted to its neighbor

A

true

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11
Q

Why do these van der waals forces occur?

A

It is due to the uneven distribution of electrons due to geometry of each molecule

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12
Q

Describe ion- dipole forces

A

ion and polar molecule attract strongly to each other

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13
Q

Describe dipole- dipole forces

A

attractions occur between oppositely charged poles on polar molecules
- depends on the orientation being correct

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14
Q

true or false: the hydration of ion is always exothermic

A

true

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15
Q

true or false: higher charge density (relative to its size) = more negative change in hydration enthalpy (delta H hydration)?

A

true

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16
Q

Does the difference between lattice energy and hydration energy determine if dissolving is either exothermic/ endothermic

A

yes

17
Q

what is lattice energy?

A

lattice energy of an ionic solid is a measure of the strength of bonds in that ionic compound

18
Q

What is hydration energy?

A

comparing ions surrounded by water

19
Q

What are dispersion (london) forces? a.k.a instantaneous dipole- induced dipole forces

A
  • occur in ALL molecular substances and GROUP 18 (noble gases)
  • momentary distortion (polarization) of electron clouds results in temporary dipole
  • causes induced dipole in neighbor and attraction between dipoles in adjacent molecules (need to be very close)

(electron cloud not symmetrical anymore; weak intermolecular attraction occurs)

20
Q

true or false: the boiling point increases with increasing dipole moment for molecules with similar number of electrons

A

true

21
Q

What does the Dispersion (london) forces depend on?

A

The relative strength depends on SIZE and SHAPE of electron cloud surrounding molecule
eg. large proton; more electrons; thus increases the likelihood of polarisation

22
Q

true or false: the melting points and boiling points increase as total number of electrons increase

A

true; this is a reflection of increasing attractions between these molecules

23
Q

does the arrangement of the molecules influence the strength of their attraction with each other?

A

yes, increasing surface area of contact increases strength of intermolecular attraction

24
Q

true or false, with similar dispersion forces higher boiling points occur for more polar molecules

A

true

25
Q

What is hydrogen bonding?

A
  • type of dipole- dipole force
  • occurs when H (bonded to N,O,F) is attracted to lone electron pair of N,O,F on another molecule
  • it is the dominant intermolecular force for H2O, NH3 and HF
  • needs a lone pair of electrons

Handout 1: States of Matter, Gases, Liquids and Phase transition (9 decks)

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