unit 3 quiz

Question 1

london dispersion

Answer 1

for all molecules

Question 2

dipole dipole

Answer 2

polar molecules
asymmetrical molecules w/ only nonmetals

includes hydrogen bonding

Question 3

hydrogen bonding

Answer 3

strong type of dipole dipole

hydrogen itself has to bond with either F O N

Question 4

strong but difficult to compare IMF

Answer 4

ionic and metallic

Question 5

ionic

Answer 5

metals w nonmetal

Question 6

metallic

Answer 6

only metals

Question 7

covalent network

Answer 7

strongest IMF

Question 8

dipole induced dipole

Answer 8

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

Question 9

ion induced dipole

Answer 9

nonpolar substance w ion

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

Question 10

ion dipole

Answer 10

polar substance w ion

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

Question 11

what properties increase with IMF

Answer 11

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

Question 12

what properties decrease with IMF

Answer 12

vapor pressure

solubility(depends on polarity of solvent and solute)

Question 13

what are the 4 basic types of solids

Answer 13

ionic solids
covalent networks of solids
molecular solids
metallic solids

Question 14

due to strong interactions between ions

Answer 14

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

Question 15

electrostatic attraction

Answer 15

attraction between positive and negative ions

Question 16

why are ionic solids brittle

Answer 16

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

Question 17

when do ionic solids conduct electricity

Answer 17

(when charged which is a given)

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

Question 18

covalent networks have atoms at their lattice pts with

Answer 18

strong directional covalent bonds

Question 19

covalent solids are only formed of

Answer 19

nonmetal

Question 20

how are covalent solids characterized

Answer 20

hardness
strength
high melting point

Question 21

molecular solids are composed of

Answer 21

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

Question 22

do molecular solids conduct electricity

why or why not

Answer 22

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

Question 23

metal alloys conduct with what

Answer 23

sea of electrons

Question 24

metallic solids are packed together and bonded to each other

Answer 24

equally in all directions

Question 25

ionic properties

Answer 25

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

Question 26

molecular properties

Answer 26

``` poor conductors of heat and electricity low melting pt soft low density dull surface ```

Question 27

covalent network peoperties

Answer 27

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

Question 28

metallic properties

Answer 28

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

Question 29

When deciding which compound will have a lower boiling point consider

Answer 29

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

Question 30

Increasing IMF forces by structure diagrams

Answer 30

Consider surface area, more branches is less polarizable

Question 31

Drawing sand mixed with water

Answer 31

Sand on bottom, water on top Sand particles close together, water particles further apart Consider particle size, atomic radius, also

Question 32

Why do gas particles follow the ideal gas law

Answer 32

They don’t have IMF

Question 33

Low pressure vs high pressure particles

Answer 33

Low pressure: particles far part | High: particles close together

Question 34

Partial pressure formula

Answer 34

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

Question 35

total pressure formula

Answer 35

PV=nRT

Question 36

What is the n in PV=nRT

Answer 36

Moles

Question 37

What is the R in PV=nRT

Answer 37

0.0821

Question 38

Kinetic molecular theory

Answer 38

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

Question 39

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

Answer 39

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

Question 40

How to find higher average molecular speeds

Answer 40

Consider grams or mass of elements The lighter the weight, the faster it moves

Question 41

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

Answer 41

32g O/ 1 mol O2 Or 1 mol O2/32g O

Question 42

When are gases more ideal

Answer 42

When pressure is low and temp is high

Question 43

Boyles law

Answer 43

As gas pressure increases, volume decreases P1V1 = P2V2

Question 44

Charles law

Answer 44

As the temperature decreases, the volume decreases V1/T1 = V2/T2

Question 45

Avogadros law

Answer 45

As the number of moles of gas increase, the volume increases | V1/N2 = V2/N2

Question 46

What forces increase with IMF strength(3)

Answer 46

Melting point, surface tension, heat of vaporization

Question 47

What forces decrease with IMF (2)

Answer 47

vapor pressure, volatility(cause of evaporating)

Question 48

avogadro’s number

Answer 48

6.02*10^23

Question 49

how many torr in 1 atm

Answer 49

760 torr

Question 50

carbon di sulfide formula

Answer 50

CS2

Question 51

fluorometham formula

Answer 51

CH3F

Question 52

ammonia vs ammonium

Answer 52

NH3 vs NH4