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Chemistry > Intermolecular Forces, Bonds, & States Of Matter > Flashcards

Intermolecular Forces, Bonds, & States Of Matter Flashcards

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1
Q

which bonds are always stronger than intermolecular forces?

A

Ionic, metallic, and covalent

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2
Q

what only exists between covalent molecules?

A

intermolecular forces

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3
Q

nonpolar covalent molecules state of matter at room temp?

A

gases

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4
Q

Strongest bond/force to weakest

A

ionic,metallic, atomic solids, covalent -> dipole ion -> h bonds -> dipole dipole -> temporary dipole

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5
Q

what is stronger? covalent bonds or intermolecular bonds?

A

covalent bonds

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6
Q

why is liquid water more dense than solid water?

A

because the hydrogen bonds force the molecules to spread out more which increases volume making ice less dense

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7
Q

Why does water have a negative slope?

A

Slopeisnegativebecauseaspressureincreases,H -bondscannotstayspacedout. H bonds break because they can only be a certain distance away from another atom before the force breaks.therefore, ice melts (liquid) and loses its crystalline structure.

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8
Q

Why don’t most substances have a negative slope?

A

because most things, as pressure increases, the substance pack tightly (solid).

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9
Q

why would heating water to boiling take longer than heating liquid ethane (C2H6) to boiling point?

A

because water is polar and has a stronger intermolecular force rather than C2H6 which is nonpolar. polar molecules are harder to change state compared to nonpolar molecules because of intermolecular forces

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10
Q

why diamond (atomic solid) does not dissolve easily in water, but salt (NaCl) does?

A

NaCl has charged particles that attract to polar H2O & separate -> dissolving in water. diamond does not have charges

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11
Q

which types of bonds can result in electrical conductivity? does the substance have to dissolve first?

A

ionic bonds and metallic bonds
ionic-> once dissolved (need charged attraction for electricity)
metallic-> as a solid

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12
Q

How many states of matter are there? what are they?

A

5

solid, liquid, gas, plasma, Bose-Einstein condensate

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13
Q

what is plasma?

A

when gases have so much energy that the electrons get stripped away=changed
SUPER HOT,STRIPPED E-,CONDUCT ELECTRICITY

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14
Q

Bose-Einstein condensate

A

Just above absolute zero, atoms lose individual identity and become super atoms…created in the lab in 1995
SUPER COLD, “SUPER ATOM”, LAB CREATED

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15
Q

what happens when a substance has a positive slope?

A

This is what most substances have. Slope is positive because as pressure increases, the substance is more likely to become a solid (molecules will be tightly compacted, more dense)

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16
Q

solid to a gas

A

sublimation

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17
Q

liquid to a solid

A

freezing

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18
Q

liquid to a gas

A

vaporization

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19
Q

gas to a sold

A

deposition

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20
Q

solid to a liquid

A

melting

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21
Q

gas to a liquid

A

condensation

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22
Q

triple point

A

Temp/pressure at which a substance could be all 3 states of matter

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23
Q

critical point

A 
supercritical fluid (Both liquid & gas)
too hot to be a liquid & too high of pressure to be a gas 
point of high temp & pressure
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24
Q

what do states of matter depend on?

A

intermolecular forces/bond type
temperature
pressure

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25
Q

positive vs negative slope

A

positive- pressure increases, more compact more likely to be a solid
negative-pressure increases, less compact (less dense) more likely to be a liquid

26
Q

Covalent atomic solids

A

network bonds, a bunch of covalent bonds between atoms of the same type connected in all directions. usually carbon or silicon because they have 4 ve

27
Q

what are intermolecular forces between?

A

between molecules!

28
Q

dipole ion

A

between a polar molecule and an ion

29
Q

dipole dipole

A

between 2 polar molecules

30
Q

hydrogen bonds

why are they stronger than dipole dipole?

A

between polar molecules containing H bonded to O,F, or N (special type of dipole dipole)
because of their electronegativity

31
Q

temporary dipoles can also be called what?

A

london dispersion forces or dipole moment

32
Q

temporary dipole

A

between 2 nonpolar molecules, shared equally and then split second partially neg & partially positive
nonpolar en= 0
Charges that exist BRIEFLY that allows ALL molecules to have intermolecular attraction
BIGGER THE MOLECULE, THE STRONGER THE TEMPORARY DIPOLE

33
Q

do ionic bonds have intermolecular attractions?

A

no because they are not molecules (not covalent)

34
Q

ionic bonds
what do 2 or more ion form?
what are they between?
do they conduct electricity?

A

form a compound
form crystals/lattice NOT molecules
between metal & nonmetal (cation and anion)
conduct electricity when dissolved

35
Q

what type of bonds form in every direction and continue in every direction?

A

ionic bonds, NOT intermolecular

36
Q

what is the solvent?

A

solvent is responsible for dissolving the solute

ex water

37
Q

what allows electricity to flow when ionic bonds are dissolved?
how are solutes dissolved?

A

positive and negative ends of the solvent attract the portions of the ions of the solute
intermolecular attractions pull apart the ionic structure
dissolved ions are what allows electricity to flow

38
Q

why can an ionic bond be dissolved in something polar like water?

A

because the intermolecular attractions in polar solvents like water, pull apart the ionic structure to be dissolved

39
Q

metallic bonds

characteristics?

A

group of ions held together but freely flowing past one another (sea of electrons)- share freely
conduct electricity as a solid
metal with metal, forms alloys or metallic solids
shapeable (bend easily)
dont dissolve easily

40
Q

heating an ionic crystal

melting/boiling point

A

ionic substances have very high melting/boiling points becayse there has to be enough energy to break a CHEMICAL bond

41
Q

states of matter usually at room temp

ionic,polar covalent,nonpolar covalent

A

ionic-solids
polar covalent-liquids
nonpolar covalent-gases

42
Q

crystalline vs amorphous

A

crystalline-perfect/specific distance apart (even rows of ions or molecules
amorphous- irregular/changing (varying structures)

43
Q

examples of crystalline vs amorphous

A

c- ionic, solid polar covalent ex. shale

a- covalent ex plastic or glass

44
Q

which types of substances dissolve in which?

A

ionic dissolves in ionic
polar dissolves in polar
polar and ionic dissolve in polar
nonpolar dissolves in nonpolar

45
Q

which bonds are easy/hard to change states?

A

ionic/atomic covalent-hardest
polar-middle(dipole-dipole)
nonpolar-easiest (temporary dipole)

46
Q

what is vapor pressure?

A

amount of pressure released

nonpolar -> a lot, ionic -> not a lot

47
Q 
ionic bond characteristics
electrical conductors?
dissolve in polar solvents?
melting/boiling pt?
state of matter at room temp?
Brittleness?
A

poor electrical conductors, ions in solutions conduct electricity
dissolve in water (polar solvents)
high melting/boiling pts because of strong chemical bond
solids at room temp
brittle and break suddenly when force is applied

48
Q 
polar covalent molecules characteristics
electrical conductors?
dissolve in polar solvents?
melting/boiling pt?
state of matter at room temp?
A

do not conduct electricity
liquids at room temp
dissolve in water (polar solvents)
medium melting/boiling pt because it has stronger intermolecular forces but not as strong as charged ion attractions

49
Q 
nonpolar covalent molecules characteristics
electrical conductors?
dissolve in polar solvents?
melting/boiling pt?
state of matter at room temp?
A

do not conduct electricity
gases at room temp
do not dissolve in water (polar solvents)
low melting/boiling pt because of weak intermolecular forces

50
Q

two types of temporary dipole (london dispersion forces, dipole moment) ?

A

monoatomic (noble gases)

simple molecular covalent (S8 or H2)

51
Q

solvation shells

A

attraction between ions and the charges on water molecules cause them to become surrounded by shells of water molecules (aq)

52
Q

what hardens many metals?

A

adding carbon

53
Q

are diamonds soluble in water? why or why not?

A

insoluble in water because the atoms are neutral so water is not attracted to the atoms and water molecules cannot rip them away from the crystal

54
Q

why do ionic bonds tend to form solid crystals at room temp but covalent bonds do not?

A

because ionic bonds in ionic compounds are stronger than in covalent, causing ionic bonds to be more tightly compact

55
Q

Why are polar covalent bonds more likely to be liquids while nonpolar covalent bonds are more likely to be gases?

A

because polar bonds have dipole dipole attraction and are more compact compared to nonpolar bonds

56
Q

Why do ionic bonds have high melting/boiling pts where as covalent bonds are usually lower?

A

because ionic bonds do not have intermolecular forces, they are strongly attracted to each other and therefore take more energy to break

57
Q

Why do substances made of nonpolar covalent molecules change state more easily then polar covalent molecules?

A

because nonpolar has a weaker intermolecular force causing the temporary dipole to be easier to break (change state)

58
Q

Why do ionic bonds dissolve in water, but nonpolar covalent bonds do not?

A

water is polar and like dissolves like so ionic bonds dissolve in water while nonpolar dissolves in nonpolar solvents. The i.m. forces in water are attracted to the ionic bonds, dissolving the ionic compound.

59
Q

why do gases spread out and are easily compacted?

A

gases are nonpolar and do not repel each other. by forcing a gas to compress, it can be easily compacted

60
Q

what is hydrogen bonding?

A

dipole dipole intermolecular force between molecules which is stronger than regular dipole dipole

61
Q

intramolecular force vs intermolecular force

A

intra- within the molecule and are not broken during state changes because they are chemical bonds (bonds bonding in molecules)
inter- bonds that connect molecules bonding, these weak forces are broken during state changes

Chemistry (16 decks)

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