Chem Physics Exam Iiii

Front 1

List the States of Matter

Back 1

Solids, Liquids, Gases

Front 2

Define Solids

Back 2

Definite volume and definite shape

Front 3

Define Liquids

Back 3

Definite volume no definite shape, form to container generally

Front 4

Define Gas

Back 4

Neither Definite shape nor definite volume.

Front 5

Attraction between oppositely charged ions is a ______ bond

Back 5

Ionic

Front 6

When sharing of one or more pairs of electrons occurs it is said to be _______ bond

Back 6

Covalent

Front 7

When a covalent bond occurs and the electron of atom 1 is able to spend time around atom 2’s nucleus it is said to be what type of bond _______ bond theory

Back 7

Valence

Front 8

Electronegativity is

Back 8

the tendency of an atom in a molecule to attract shared electrons to itself

Front 9

The tendency of an atom in a molecule to attract shared electrons to itself is

Back 9

Electronegativity

Front 10

Name the most Electronegativity element

Back 10

Fluorine

Front 11

Change of state : Solid to Liquid

Back 11

Melting Ex: Melting Ice

Front 12

Change of state: Liquid to Solid

Back 12

Freezing Ex: Water Freezing to make Ice

Front 13

Change of state

Back 13

Liquid to Gas

Front 14

Change of state

Back 14

Gas to Liquids

Front 15

Change of state

Back 15

Solid to Gas Sublimation Ex. Dry Ice

Front 16

With Increasing intermolecular forces Viscosity will Increase or Decrease

Back 16

Viscosity will increase (Higher)

Front 17

With Increasing intermolecular forces Vapor Pressure will Increase or Decrease

Back 17

Vapor Pressure will decrease ( Lower)

Front 18

Compounds with more intermolecular forces have Higher or Lower Melting point

Back 18

Higher Melting point

Front 19

With Heat of Fusion is the intermolecular force Higher or Lower when vaporization

Back 19

Higher

Front 20

Compounds with more intermolecular forces have Higher or Lower Boiling Points

Back 20

Higher Boiling Point required.

Front 21

The boiling point at a pressure of 1 atm

Back 21

Normal Boiling Point

Front 22

The energy required to melt 1 mole of substance

Back 22

Molar heat fusion ∆H fus

Front 23

The forces between atoms in a molecule

Back 23

Intramolecular

Front 24

The forces between molecules in a solid

Back 24

Intermolecular

Front 25

The instantaneous dipole forces involving atoms and molecules

Back 25

London dispersion forces

Front 26

The lining up of opposite charges on adjacent polar molecules

Back 26

dipole-dipole attraction

Front 27

The maximum pressure of vapor that builds up in a closed container

Back 27

equilibrium vapor pressure

Front 28

The boiling point at a pressure of 1 atm

Back 28

Normal Boiling Point

Front 29

The energy required to melt 1 mole of substance

Back 29

Molar heat fusion ∆H fus

Front 30

The forces between atoms in a molecule

Back 30

Intramolecular

Front 31

The forces between molecules in a solid

Back 31

Intermolecular

Front 32

The instantaneous dipole forces involving atoms and molecules

Back 32

London dispersion forces

Front 33

The lining up of opposite charges on adjacent polar molecules

Back 33

dipole-dipole attraction

Front 34

The maximum pressure of vapor that builds up in a closed container

Back 34

equilibrium vapor pressure

Front 35

VSEPR

Back 35

VALENCE SHELL ELECTRON PAIR REPULSION THEROY

Front 36

Electrons dislike each other because of like charges and so they repel each other this theory is known as

Back 36

VSEPR Theory

Front 37

List the Three Intermolecular Foreces

Back 37

Dipolar, Hydrogen Bonding, London Forces

Front 38

Hydrogen will easily bond to any of these three elements

Back 38

Oxygen, Nitrogen, Fluorine

Front 39

As the temp of an gas increases so does the vapor pressure T or F

Back 39

True

Front 40

As the temp of a gas decreases so does the vapor pressure T or F

Back 40

False

Front 41

Bond angle 120 degree

Back 41

Trigonal Planar

Front 42

Bond angle 109 Square 90 degree angels

Back 42

Tetrahedral

Front 43

Predict the molecular dipole of water H2O

Back 43

Polar H O H 3.5 → 2.1 = 2.1 polar

Front 44

Predict the molecular dipole for CO2

Back 44

O₌C₌O O 3.5 ← C 2.5 →O 3.5 two vectors pulling in opposite directions

Front 45

Bond dipoles are known as

Back 45

Vectors

Front 46

Which of these are soluble in water and why HCl & O2

Back 46

HCL Soluble polar, O2 Not soluble non polar

Front 47

Which of these is a gas N2O OR NaN2 Cl or I2

Back 47

Nitro Oxide is a gas and not soluble in water, Cl or I is soluble in water there for not a gas.

Front 48

This change of state is Exothermic

Back 48

Liquid to a solid Ice freezing energy is abosored by water

Front 49

List State of Changes that are Endothermic

Back 49

Solid to Liquid, Liquid to Gas, Gas to Liquid, Solid to Gas

Front 50

Q=MC∆T

Back 50

Temp Change

Front 51

Q=MLf

Back 51

Latent Heat Fusion ( Hidden)

Front 52

Q=MLv

Back 52

Liquid to Fusion

Front 53

∆H⁰vap Vaporization is an inherently endothermic or exothermic process

Back 53

Endothermic

Front 54

∆H⁰vap has what units of energy /quantity SI

Back 54

kJ/mole

Front 55

∆H⁰fus Fusion is inherently endothermic or exothermic process

Back 55

Endothermic

Front 56

Normal boiling point is the temperature at which the vapor pressure of liquid equals exactly 760 torr, T or F

Back 56

True

Front 57

The tendency of a liquid to evaporate is called

Back 57

Volatility

Front 58

Low Vapor Pressure = ↓or ↑ Volatility

Back 58

decrease volatility

Front 59

Increased Volatility Ex. Ethanol = High or Low Vapor Pressure

Back 59

High, volatile substances want to convert to gas

Front 60

As a man sweats KE energy molecules escape from the sweat trying to cool the body, so decreased KE = a decrease or a increase in temp

Back 60

decrease

Front 61

Heating Curve for 1 Mole of Water

Back 61

Energy added at this point is absorbed in softening up the intermolecular foreces so tha the transition from solid to liquid occurs, no increase in tem is observed. Once all of the solid water has melted, added energy once again causes an increase in temp. When the liquid sample reaches the boiling point, once again the temp remain constant , because of added energy is used to over come the remaining intermolecular forces as liquid water molecules escape into the gas phase. Whater sample is completely vaporized.