Chem Test 1

Front 1

Solid (Shape & Volume)

Back 1

Shape: Tightly packed

Volume: Fixed

Front 2

Liquid (Shape & Volume)

Back 2

Shape: close together

Volume: shape of container

Front 3

Gas (Shape & Volume)

Back 3

Shape: free space between particles

Front 4

Phase of material that is typically the densest

Back 4

Solid

Front 5

Phase of material that is most compressible

Back 5

Gas

Front 6

Ionic Bonds

Back 6

Transfer of electrons

Front 7

Covalent Bonds

Back 7

Sharing of electrons

Front 8

IMFs are most important in what phases?

Back 8

Solids and Liquids

Front 9

IMFs (increase/decrease) with distance?

Back 9

Decrease

Front 10

Strongest IMFs

Back 10

Ion-Dipole

Front 11

___ of the ion & ____ of the charge affect how strong the interaction is in Ion-Dipole IMFs

Back 11

Size & Magnitude

Front 12

Increased ion charge (increases/decreases) the strength of the interaction

Back 12

Increases

Front 13

Increased ion size (increases/decreases) the strength of the interaction

Back 13

Decreases

Front 14

Molecules that are (polar/nonpolar) have a permanent dipole moment

Back 14

Polar

Front 15

What determines the magnitude of the dipole moment and thus the strength of the IMFs?

Back 15

Atoms

Front 16

Hydrogen Bonding

Back 16

H covalently bonded to F, O, and N.

Front 17

What leads to highly concentrated partial charges with F, O, N, and H atoms?

Back 17

Large difference in electronegativity and the small sizes of F, O, and N

Front 18

Which IMFs get stronger with increasing molecular size?

Back 18

Dispersion forces

Front 19

Cohesion

Back 19

Between molecules of the same substance

Front 20

Adhesion

Back 20

Between different substances

Front 21

Viscosity

Back 21

Measure of flow

Front 22

Phase change of Solid --> Liquid; Energy added or removed?

Back 22

Melting; Added

Front 23

Phase change of liquid --> gas; energy added or removed?

Back 23

Vaporization; Added

Front 24

Phase change from gas --> liquid; energy added or removed?

Back 24

Condensation; Removed

Front 25

Phase change if liquid --> solid; energy added or removed?

Back 25

Freezing; removed

Front 26

Phase change if solid --> gas; energy added or removed?

Back 26

Sublimation; added

Front 27

Phase change of gas --> solid; energy added or removed?

Back 27

Deposition; Removed

Front 28

Increased surface area (increase/decrease) the rate of evaporization?

Back 28

Increase

Front 29

Increased temperature (increase/decrease) the rate of evaporization?

Back 29

Increase

Front 30

Why does liquid boil?

Back 30

The particles gain enough kinetic energy to completely overcome the attractive forces

Front 31

How are gases condensed?

Back 31

By decreasing their temperature or increasing the pressure

Front 32

The greater the IMFs between molecules the (more/less) energy needed to vaporize?

Back 32

More

Front 33

The greater the IMFs the (faster/slower) rate of evaporization?

Back 33

Slower

Front 34

Molecules in the vapor state can (gain/lose) energy though the collisions with other molecules?

Back 34

Lose

Front 35

The (greater/less) the IMFs, the (greater/less) energy is needed for the vapor molecules to condense?

Back 35

Greater; Less

Front 36

Volatile

Back 36

Liquids that evaporate easily

Front 37

Is salt water volatile or nonvolatile?

Back 37

Nonvolatile

Hint 37

Think of the ocean, does it evaporate easily?

Front 38

Equilibrium vapor pressure

Back 38

Rate of evaporation = rate of condensation

Front 39

At a given temperature is vapor pressure independent or dependent of IMFs?

Back 39

Depends on IMFs

Front 40

Phase changes

Back 40

.

Front 41

Clausis-Clapeyron Equation

Back 41

ln (P2/P1) = -delta Hvap/ R (1/T2 - 1/T1)

Front 42

Solute

Back 42

Gets dissolved

Front 43

Solvent

Back 43

Does the dissolving

Front 44

Solution

Back 44

Homogeneous mixture

Front 45

Endothermic

Back 45

+ delta H soln

Front 46

Entropy

Back 46

Measure of a system's disorder or dispersal of particles throughout a system. Energy tends to disperse throughout the system

Front 47

Where is it saturated, unsaturated, and supersaturated?

Back 47

Saturated - on the line, Unsaturated - below the line, Supersat - above the line

Front 48

Molarity

Back 48

Moles solute / L solution

Front 49

Molality

Back 49

Moles solute / kg solvent

Front 50

Henry's Law

Back 50

Sgas = (KH)(Pgas)

Front 51

Van't hoff factor of NaCl

Back 51

2

Hint 51

Number of pieces it breaks into

Front 52

Van't Hoff factor of CaCl2

Back 52

3

Front 53

Van't Hoff factor of NH3

Back 53

1 (covalently bonded non metal)

Front 54

Van't Hoff of NaOH

Back 54

2

Front 55

Van't Hoff of Na3PO4

Back 55

4

Front 56

Van't Hoff of CH3OH

Back 56

1 (all covalently bonded)

Front 57

Osmotic Pressure Formula

Back 57

(pie symbol) = iMRT

Front 58

Which intermolecular forces are the weakest?

Back 58

Dispersion forces

Front 59

What are the only things coligative properties depend on?

Back 59

Concentration of solute particles in a solution

Front 60

Which concentration unit is temperature dependent?

Back 60

Molarity