Chemistry Ch. 4-6

Front 1

Electric Current

Back 1

Directed motion of charged particles

Front 2

Solution

Back 2

Homogeneous mixture of 2+ substances

Composed of solvent (major) and solute (minor)

Front 3

Concentration

Back 3

Solute/Solvent or Solute/solution

Front 4

Electrolyte

Back 4

Substance that dissolves in water to yield a solution that conducts electricity (presence of ions)

Front 5

Nonelectrolyte

Back 5

Substance that dissolves in water to yield a solution that does not conduct electricity

Front 6

Strong electrolyte

Back 6

Completely dissociate into ions

Front 7

Weak electrolyte

Back 7

Partially dissociate

Front 8

Identifying electrolytes

Back 8

Is compound ionic or molecular?

Ionic -> if dissolves, strong electrolyte, not dissolve, nonelectrolyte

Molecular -> strong if one of 7 strong acids, weak if not strong acid or if it's a base, nonelectrolyte if not an acid or base

Front 9

What are the 7 strong acids?

Back 9

HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4

Front 10

Dissociation

Back 10

Ionic compound breaks into its ions

Front 11

Ionization

Back 11

Molecular compound forms ions when dissolves

Front 12

Arrhenius definition of base

Back 12

Produces OH- when dissolved in water

Front 13

Arrhenius definition of acid

Back 13

Produces H+ when dissolved in water

Front 14

Bronsted definition of base

Back 14

Proton acceptor

Front 15

Bronsted definition of acid

Back 15

Proton donor

Front 16

Precipitate

Back 16

Insoluble solid product that separates from solution

Front 17

Equation steps in precipitation reactions

Back 17

1. Molecular equation (balance)

2. Total Ionic equation (all ions that can separate) (cancel spectator ions)

3. Net Ionic equation (left over - ions that form solid usually)

Front 18

Hydration

Back 18

Ionic substance dissolves in water, water molecules remove individual ions from the 3D solid structure and surround them

Front 19

Solubility

Back 19

Maximum amount of solute that will dissolve in a given quantity of solvent at a specific temp (not all ionic compounds dissolve in water)

Front 20

Solubility of solid __________ with increase in temp

Solubility of gas __________ with increase in temp

Back 20

Increases; decreases

Front 21

Solubility Guidelines

Water-soluble with insoluble exceptions

Back 21

Cmpds with metals in 1A or NH4+

Cmpds with NO3-, C2H3O2-, ClO3-

Cmpds with Cl-, Br-, I- except with Ag+, Hg22+, and Pb2+

Cmpds with SO42- except with Ag+, Hg22+, Pb2+, Ca2+, Sr2+, and Ba2+

Front 22

Water-insoluble with soluble exceptions

Back 22

Cmpds with CO32-, PO43-, CrO42-, S2- except with metal 1A or NH4+

Cmpds with OH- except with metal 1A or Ba2+

Front 23

Neutralization reaction

Back 23

Reaction between an acid and a base

Aqueous acid-base reaction produces water and salt (proton transfers from acid to base)

Front 24

Redox reactions

Back 24

Oxidation-reduction (e- transferred from one to the other)

OIL RIG

Front 25

Reducing agent

Back 25

Undergoes oxidation, causes other to be reduced

Front 26

Oxidizing agent

Back 26

Undergoes reduction, causes other to be oxidized

Front 27

Oxidation number/state

Back 27

Charge an atom would have if e- were transferred completely

Elements have oxidation # of zero

Front 28

Activity series

Back 28

Ranks metals on activity - ability to lose e-

On top loses e- to whatever is below it

Front 29

Disproportionation reaction

Back 29

One element undergoes both oxidation and reduction

Front 30

Concentration

Back 30

Amount of solute dissolved in given quantity of solvent or solution

Front 31

Molarity

Back 31

Moles of solute / liters of solution

Front 32

Molality

Back 32

solute / solvent

Front 33

Dilution

Back 33

process of preparing a less concentrated solution from a more concentrated one

Front 34

How to find moles of solute?

Back 34

Volume (L) x Molarity

Front 35

Mc x Lc =

Back 35

Md x Ld

Front 36

Gravimetric analysis

Back 36

Analytical technique based on the measurement of mass

Front 37

Titration

Back 37

A solution of accurately known concentration called standard solution is added gradually to another solution of unknown concentration until the chemical reaction between 2 solutions is complete (indicator)

Front 38

Equivalence point

Back 38

Acid has been neutralized

Front 39

Redox Titration

Back 39

Oxidation-reduction reaction with one reactant delivered via burrette

Front 40

Half-reaction

Back 40

Oxidation or reduction reaction in a redox reaction (e- go on side of charge)

Zn (s) -> Zn2+ (aq) + 2e- oxidized

Cu2+ (aq) + 2e- -> Cu (s) reduced

Front 41

Energy

Back 41

Capacity to do work or transfer heat

Front 42

Kinetic energy

Back 42

Energy in motion

KE = 1/2mv^2

Front 43

Potential energy

Back 43

Stored energy

Front 44

Electrostatic energy

Back 44

potential energy that results from interaction of charged particles

Eel = k (Q1Q2)/d

Front 45

Law of conservation of energy

Back 45

Energy is not created or destroyed, changes forms

change in Usys = -(change in Usurr)

Front 46

Universe

Back 46

System + Surroundings

Front 47

Heat

Back 47

Transfer of thermal energy at different temperatures between two bodies from high to low

Front 48

Exothermic process

Back 48

Gives off heat (-)

Front 49

Endothermic process

Back 49

Absorbs thermal energy as heat (+)

Front 50

SI unit of E & other units

Back 50

Joule, calorie; 1 cal = 4.184 J

Nutritional Calorie = 4184 J

Front 51

Thermodynamics

Back 51

Study of interconversion of heat and other kinds of energy

Front 52

Open system

Back 52

Can exchange mass & E with surroundings

Front 53

Closed system

Back 53

Allows transfer of E, but not mass

Front 54

Isolated system

Back 54

No exchange of mass or E with surroundings

Front 55

State of a system

Back 55

Values of properties such as E, temp, pressure, volume

Front 56

State functions

Back 56

Properties determined by state of system regardless of how that condition was achieved (path doesn't matter)

Front 57

Change in U (internal energy)

Back 57

q + w

heat (absorbed + or released -) + work (done on + or by system -)

Work done on system = volume decrease

Work done by system = volume increase

Front 58

Constant pressure is like a _____ system

Back 58

Open

Front 59

Constant volume is like a ______ system

Back 59

Closed

Front 60

Work =

Back 60

-P x change in V

Front 61

If volume is constant (qv)

Back 61

qv = change in U (because P change in V = 0)

Front 62

If pressure is constant (qp)

Back 62

qp = change in U + P change in V

qp = change in H

Front 63

Enthalpy (H)

Back 63

Available E: Change in H = change in U + change in (PV)

At constant pressure = change in U + P(change in V)

Heat exchanged between system and surroundings at constant pressure

Front 64

Enthalpy of reaction (change in H)

Back 64

H(products) - H(reactants)

Front 65

Thermochemical equation

Back 65

Show enthalpy changes and mass relationships

Front 66

Specific heat

Back 66

Amount of heat required to raise temp of 1 g of substance by 1*C

q = sm(change in T)

Front 67

Heat capacity

Back 67

Amt of heat required to raise temp of object by 1*C

q = C(change in T)

Front 68

Constant pressure calorimetry

Back 68

qsys = -qsurr

qsys = -sm(change in T); qsurr = sm(change in T)

Front 69

Hess's Law

Back 69

Change in enthalpy that occurs when reactants are converted to products in a reaction is the same whether the reaction takes place in one step or in a series of steps

Front 70

Standard conditions

Back 70

Known temp (25*C) and known pressure (1 atm)

Front 71

Standard enthalpy of reaction

Back 71

-H of rxn carried out under standard conditions

change in Hrxn* = sum of n x standard enthalpy of products - sum of m x standard enthalpy of reactants

Front 72

Standard enthalpy of formation

Back 72

The heat change that results when 1 mol of a compound formed from its constituent elements in their standard states

Front 73

Electromagnetic spectrum

Back 73

continuum of radiation

Front 74

Wavelength

Back 74

Distance between identical points on successive waves

Front 75

Frequency

Back 75

Number of waves that pass through a particular point in 1 sec (speed is same)

Front 76

Amplitude

Back 76

Vertical distance a wave reaches from x-axis

Front 77

c =

Back 77

wavelength (lambda) x frequency (nu)

Front 78

Electromagnetic wave

Back 78

Has electric field and magnetic field component that function in perpendicular planes

Front 79

Blackbody radiation

Back 79

Electromagnetic radiation emitted when a solid is heated

Front 80

Quantum

Back 80

Smallest quantity of E that can be absorbed or emitted in form of electromagnetic radiation

Front 81

E =

Back 81

h(nu)

Front 82

Photoelectric effect

Back 82

Electrons ejected from surface of metal exposed to light of at least a certain min frequency (threshold)

Front 83

Photon

Back 83

particle of light

Front 84

h(nu) =

Back 84

KE + W

Kinetic energy + binding energy of e-

Front 85

Line spectra

Back 85

Emission of light only at specific wavelengths

Front 86

Ground state

Back 86

Lowest E state (n=1)

Front 87

1/lambda =

Back 87

R constant (1/n1^2 - 1/n2^2)

2.18 x 10^-18 J/hc (1/nf^2 - 1/ni^2)

Front 88

Change in E =

Back 88

-2.18 x 10^-18 J (1/nf^2 - 1/ni^2)

Front 89

De Broglie wavelength

Back 89

lambda = h / m x u

u = velocity

Front 90

Diffraction

Back 90

When waves "talk" to each other

-form of scattering when positive (constructive; light) or negative (destructive; dark) interference

Front 91

Heisenberg Uncertainty Principle

Back 91

Impossible to know both the momentum (p) and position (x) of a particle with certainty

change in x x change in p is greater than or equal to h / 4pi

Front 92

Principle Quantum Number (n)

Back 92

Describes size of orbit

Front 93

Angular Momentum Quantum Number (l)

Back 93

Describes shape of orbital

l = 0 (s), 1 (p), 2 (d), 3 (f)

Front 94

Shell

Back 94

Collection of orbitals with same n values

Front 95

Subshell

Back 95

One+ orbitals with same n & l values

Front 96

Magnetic Quantum Number (ml)

Back 96

Describes orientation of orbital in space

-value of 2l + 1

s = 1, p = 3, d = 5, f = 7

Front 97

Electron Spin Quantum Number (ms)

Back 97

Spin denoted by +1/2 or -1/2

Front 98

As you increase the intensity,

Back 98

you increase the number of electrons emitted

Front 99

As you increase frequency,

Back 99

you increase KE

Front 100

Wave function

Back 100

Defines distribution of e- density around nucleus

Front 101

When n = 1, l = ?

Back 101

l = 0

s subshell

ml = 1 orbital

2 electrons

Front 102

When n = 2, l = ?

Back 102

l = 0 and 1

s and p subshell

ml = 1 orbital for s, 3 orbitals for p

8 electrons

Front 103

When n = 3, l = ?

Back 103

l = 0, 1, & 2

s, p, & d subshell

ml = 1 for s, 3 for p, 5 for d

18 electrons

Front 104

When n = 4, l = ?

Back 104

l = 0, 1, 2, & 3

s, p, d, & f subshell

ml = 1 for s, 3 for p, 5 for d, 7 for f

32 electrons

Front 105

Calorimetry

Back 105

Measurement of heat changes

Front 106

Constant volume calorimetry

Back 106

qcal = -qrxn

qcal = Ccal(change in T); qrxn = -Ccal(change in T)