Chem Test 2

Front 1

Fluid

Back 1

Any material that has the ability to flow (includes gas and liquids)

Front 2

What 2 properties are important for hydrostatic fluids?

Back 2

Density and pressure

Front 3

Pascals Principle

Back 3

When an external pressure is applied to a confined fluid, it is transmitted unchanged to every point within a fluid

Front 4

Normal forces

Back 4

Forces that are perpendicular to the faces of an object

Front 5

Archimedes Principle

Back 5

An object immersed either totally or partially in a fluid feels a buoyant force equal to the weight of fluid displaced

Front 6

Hydrometer

Back 6

Device used to measure the density of fluids

Front 7

Bernoulli Effect

Back 7

As the speed of a fluid increases, the pressure exerted by the fluid decreases

Front 8

What are venturi tubes used to measure?

Back 8

Speed of fluid in a pipe

Front 9

Characteristics of a solid

Back 9

Have definite volume and shape

Front 10

Characteristics of a liquid

Back 10

Definite volume, but no defined shape

Front 11

Characteristics of gas

Back 11

No defined shape or volume

Front 12

Condensation

Back 12

Conversion of a gas to liquid

Front 13

Sublimation

Back 13

Converstion of a solid to gas without forming an intermediate liquid

Front 14

Deposition

Back 14

Conversion of a gas to a solid

Front 15

intermolecular forces

Back 15

Electrostatic attractive forces bw molecules that determines how molecules react with one another

Front 16

Ionic bonds are formed bw _____ and _____

Back 16

Metals and nonmetals

Front 17

Metals tend to form _____ and nonmetals tend to form _____

Back 17

-Cations
-Anions

Front 18

Cation

Back 18

Gives up electron (positive)

Front 19

Anion

Back 19

Attracts electron (negative)

Front 20

Ionic bonds

Back 20

ions bound by the coumbic attraction bw charged ions

Front 21

Covalent bond

Back 21

result from 2 atoms sharing 1 or more pairs of electrons

Front 22

Valence electrons

Back 22

electrons in partially filled shells

Front 23

Ionic bonds are ____ than covalent bonds and are usually ____ at room temp

Back 23

-Stronger
-Solids

Front 24

What describes the quantum state or energy of an electron in an orbital?

Back 24

The shell, subshell, and orbital quantum numbers

Front 25

What describes the region in space where you are likely to find the electron?

Back 25

The orbital

Front 26

Octet Rule

Back 26

an atom wants to fill its valence shell with 8 electrons to be like the nearest noble gas

Front 27

When are bonds the strongest?

Back 27

when the bond has the least amount of energy (most stable)

Front 28

Bond dissociation energy

Back 28

amount of energy necessary to break the bond

Front 29

Isomer

Back 29

Compounds that are different but have the same molecular formula

Front 30

Resonance

Back 30

more than one acceptable lewis structure

Front 31

Valence shell electron pair repulsion theory (VESPR)

Back 31

Electron pairs try to get as far apart in space as geometrically possible-predicts the shape of a molecule

Front 32

Class, bond angle, and example for linear geometry

Back 32

AX2; 180; CO2

Front 33

Class, bond angle, and example for trigonal planer geometry

Back 33

AX3; 120; urea

Front 34

Class, bond angle, and example for bent geometry

Back 34

AX2E and AX2E2; 105; water

Front 35

Class and bond angle for tetrahedral geometry

Back 35

AX4; 109; methane (CH4)

Front 36

Class, bond angle, and example for pyramidal geometry

Back 36

AX3E; 108; Ammonia (NH3)

Front 37

Electronegativity

Back 37

propensity for atoms to pull electrons towards themselves

Front 38

Most electronegative element

Back 38

Flourine (EN=4)

Front 39

Non-polar bond

Back 39

bond between 2 atoms of identical electronegativity

Front 40

_____ molecules are always non-polar

Back 40

Homodiatomic

Front 41

Polar bond

Back 41

bond between 2 atoms with different electronegativity

Front 42

Partial charge

Back 42

Results from an uneven sharing of electrons

Front 43

The increase in electron density around the more electronegative atom leads to a _______

Back 43

partial negative charge

Front 44

The less electronegative atom develops a ______

Back 44

partial positive charge

Front 45

What does the overall polarity of a molecule depend on?

Back 45

The vectoral sum of the bond dipoles

Front 46

List in order the most electronegative elements after flourine

Back 46

O>N>Cl>Br>C>H

Front 47

Dipole-dipole attraction

Back 47

attraction bw the opposite (partial charges) of polar molecules

Front 48

Hydrogen bonding is _____ than dipole-dipole

Back 48

Stronger

Front 49

Hydrogen bonding

Back 49

Bond of H directly with F, O, or N

Front 50

London force

Back 50

Result of an instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed

Front 51

Larger molecules have ____ london forces

Back 51

more

Front 52

Ion-dipole attraction

Back 52

attraction bw an ion and a polar molecure; allows ionic solids to dissolve in water

Front 53

More IM forces cause what 4 things?

Back 53

1. higher boiling and melting points
2. higher heats of fusion and vaporzation
3. Lower vapor pressure
4. More viscous liquids

Front 54

Nonpolar species

Back 54

O, N, and C

Front 55

Organic compounds _____ very soluble in water

Back 55

arent

Front 56

Viscosity

Back 56

Measure of a fluids resistance to flow

Front 57

Viscosity ____ with increasing molecular forces

Back 57

Increases

Front 58

Substances with greater intermolecular forces have ____ vapor pressures

Back 58

Lower

Front 59

Vapor pressure

Back 59

the pressure above a liquid in a closed container when the gas/liquid equilibrium has been reached

Front 60

Dynamic equilibrium

Back 60

Exists in a system comprised of at least 2 states when the populations of the 2 states are constant (even though the members of the system are constantly changing from 1 state to another)

Front 61

As temp increases, vapor pressure and volatility _____

Back 61

Increases

Front 62

Volatility

Back 62

nonquantitative term that describes the tendency of a liquid to evaporate

Front 63

Heat of vaporization

Back 63

The amount of energy necessary to liberate one mole of liquid at its boiling point into the gas phase

Front 64

Phase diagram

Back 64

shows the combined effects of temp and pressure on the state of matter

Front 65

Gas state in the phase diagram

Back 65

temps are highest and pressures are lowest

Front 66

Liquid state in the phase diagram

Back 66

temps and pressures are intermediate

Front 67

Solid state in the gas diagram

Back 67

Temps are lowest and pressures are highest

Front 68

Triple point

Back 68

The single temp and pressure combo where all three phases can exist in equilibrium with each other

Front 69

What does the solid-liquid equilibrium line define?

Back 69

The melting point of a solid

Front 70

What does the liquid-gas equilibrium line define?

Back 70

The boiling point of the liquid at various pressures

Front 71

Where does the liquid-gas equilibrium line terminate? What happens when temp and pressure exeeds this point?

Back 71

The critical point; substance becomes a supercritical fluid

Front 72

Supercritical fluids

Back 72

Have flow properties of gases but densities similar to liquids, have no surface tension (terrific solvents)

Front 73

Boiling point

Back 73

The temperature at which the vapor pressure is equal to the ambient pressure

Front 74

Vapor pressure of water at 100 degrees celcius?

Back 74

760 torr

Front 75

Boiling point of a liquid is highly dependent on _____

Back 75

pressure

Front 76

Melting point

Back 76

Temperature that corresponds to the average molecular kinetic energy sufficient to overcome the intermolecular forces that hold the molecules in the solid state

Front 77

____ compounds have high melting points

Back 77

Ionic

Front 78

Molar enthalpy of fusion

Back 78

the heat necessary to convert one mole of solid into a liquid at its normal melting point

Front 79

Molar enthalpy of vaporization (delta Hvap)

Back 79

the heat required to convert one mole of liquid to a gas at its normal boiling point

Front 80

When is heat=enthalpy?

Back 80

When melting or vaporization occurs at constant pressure

Front 81

Enthalpy of fusion and enthalpy of vaporization are both ____ processes and represent what?

Back 81

Endothermic, the amt of heat that must be added to the sample for the phase transition to occur

Front 82

Heat of fusion represents what?

Back 82

The amt of energy needed to overcome the IM forces to the point that the molecules can start to move around each other

Front 83

Heat of vaporization is ____ than heat of fusion

Back 83

larger

Front 84

How does evaporation have a cooling effect?

Back 84

Vaporization is an endothermic process so it causes a decrease in temp by absorbing heat from the surroundings

Front 85

Condensation has a ____ effect

Back 85

heating