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chemistryyyy > unit 3 quiz > Flashcards

unit 3 quiz Flashcards

1
Q

london dispersion

A

for all molecules

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2
Q

dipole dipole

A

polar molecules
asymmetrical molecules w/ only nonmetals

includes hydrogen bonding

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3
Q

hydrogen bonding

A

strong type of dipole dipole

hydrogen itself has to bond with either F O N

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4
Q

strong but difficult to compare IMF

A

ionic and metallic

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5
Q

ionic

A

metals w nonmetal

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6
Q

metallic

A

only metals

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7
Q

covalent network

A

strongest IMF

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8
Q

dipole induced dipole

A

one substance polar and the other is non polar

the IMF increases w magnitude of dipole of polar molecule and with polarizabiity of nonpolar molecule

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9
Q

ion induced dipole

A

nonpolar substance w ion

strength increases w larger charged ions(smaller radius) and more polarizable molecules

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10
Q

ion dipole

A

polar substance w ion

stronger than dipole dipole
strength increases w large charged ions(smaller size) and more polar molecules

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11
Q

what properties increase with IMF

A 
boiling/melting/freezing pt
enthalpy of fusion/vaporization 
viscosity
surface tension
lattice energy
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12
Q

what properties decrease with IMF

A

vapor pressure

solubility(depends on polarity of solvent and solute)

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13
Q

what are the 4 basic types of solids

A

ionic solids
covalent networks of solids
molecular solids
metallic solids

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14
Q

due to strong interactions between ions

A

ionic solids have high vapor pressure high melting pts and high boiling pts

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15
Q

electrostatic attraction

A

attraction between positive and negative ions

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16
Q

why are ionic solids brittle

A

due to repulsion of like charges when one layer of solids slides across the other layer

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17
Q

when do ionic solids conduct electricity

A

(when charged which is a given)

web ions are mobile
when ionic solid is melted
or dissolved in water or another solvent

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18
Q

covalent networks have atoms at their lattice pts with

A

strong directional covalent bonds

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19
Q

covalent solids are only formed of

A

nonmetal

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20
Q

how are covalent solids characterized

A

hardness
strength
high melting point

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21
Q

molecular solids are composed of

A

distinct individual units of covalent lay honded molecules attracted to each other through weak IMF

22
Q

do molecular solids conduct electricity

why or why not

A

no becuase their valence e- are tightly held w/in the covalent bonds and line pairs of each constituent molecule

23
Q

metal alloys conduct with what

A

sea of electrons

24
Q

metallic solids are packed together and bonded to each other

A

equally in all directions

25
Q

ionic properties

A 
poor conductors of heat and electricity 
high melting pt
hard but brittle
relatively dense
dull surface
26
Q

molecular properties

A 
poor conductors of heat and electricity 
low melting pt
soft
low density
dull surface
27
Q

covalent network peoperties

A 
poor condusctors of heat and electricity 
high melting point
very hard and brittle
low density
dull surface
28
Q

metallic properties

A 
good conductors of heat and electricity 
melting points depend on e-config
ductile and malleable 
high density usually 
lustrous
29
Q

When deciding which compound will have a lower boiling point consider

A

First consider IMF then if the same consider Number of electrons, polarizability

30
Q

Increasing IMF forces by structure diagrams

A

Consider surface area, more branches is less polarizable

31
Q

Drawing sand mixed with water

A

Sand on bottom, water on top

Sand particles close together, water particles further apart

Consider particle size, atomic radius, also

32
Q

Why do gas particles follow the ideal gas law

A

They don’t have IMF

33
Q

Low pressure vs high pressure particles

A

Low pressure: particles far part

High: particles close together

34
Q

Partial pressure formula

A

Add up the moles of the mixture of
each element of gas

Divide each element by the total
Multiply by the total pressure stated in the problem

35
Q

total pressure formula

A

PV=nRT

36
Q

What is the n in PV=nRT

A

Moles

37
Q

What is the R in PV=nRT

A

0.0821

38
Q

Kinetic molecular theory

A

The size of a gas particle is so small domeñare w/ distance between particles that volume is ignored
Gas particles are in constant random motions, bumping off walls
Gas particles have no attractive or repulsive force

39
Q

Draw a 1L vessel containing 2 moles of H2 at 200K

A

Since it’s about 2 moles, consider a number easily multiplied by 2 like 3
Remember more heat means faster movement which means more pressure

40
Q

How to find higher average molecular speeds

A

Consider grams or mass of elements

The lighter the weight, the faster it moves

41
Q

if your doing stoic and you have O2 how would you write the fraction

A

32g O/ 1 mol O2

Or

1 mol O2/32g O

42
Q

When are gases more ideal

A

When pressure is low and temp is high

43
Q

Boyles law

A

As gas pressure increases, volume decreases

P1V1 = P2V2

44
Q

Charles law

A

As the temperature decreases, the volume decreases

V1/T1 = V2/T2

45
Q

Avogadros law

A

As the number of moles of gas increase, the volume increases

V1/N2 = V2/N2

46
Q

What forces increase with IMF strength(3)

A

Melting point, surface tension, heat of vaporization

47
Q

What forces decrease with IMF (2)

A

vapor pressure, volatility(cause of evaporating)

48
Q

avogadro’s number

A

6.02*10^23

49
Q

how many torr in 1 atm

A

760 torr

50
Q

carbon di sulfide formula

A

CS2

51
Q

fluorometham formula

A

CH3F

52
Q

ammonia vs ammonium

A

NH3 vs NH4

chemistryyyy (40 decks)

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