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General Chemistry Flashcards

1
Q

What is Half life?

A

Zero Order: t=[reactants]/2K 2nd Order: t=1/k[Reactants]

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2
Q

What Ksp?

A

Solubility product When this is high most soluble

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3
Q

What does Diamagnetic mean?

A

Element that electrons are paired example in Hund’s rule

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4
Q

What is the difference between beta, alpha, and gamma decay?

A

Alpha Decay: atomic #-2 (z-2) and mass-4(a-4) Beta Decay: MOST PENETRATING atomic# -1(z-1) or atomic #+1(z+1) Gamma Decay: Nothing

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5
Q

What is Electrolysis

A

Redox RXN Need electron enegry to induce rxn Reduction is cathode Oxidation is the anode

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6
Q

What are elements are liquid at room temp?

A

BR2 and Hg, everything else solids but Cl, G, N,O and noble gases

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7
Q

What is Avogadro’s number?

A

6 x 10^23 molecules/moles

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8
Q

What is the standard enthalpy of formation for any element?

A

0

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9
Q

What is an Ionic compound?

A

Metal + Nonmetal, except NH4Cl

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10
Q

Name intermolecular forces form weakest to strongest?

A

London Dispersion, Dipole-Dipole, Hydrogen Bonding, Ionic bonding

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11
Q

Differences between Ionic compounds, molecular solid, and covalent bond networks

A

IC: High melting points MS: Low boiling points and held together by dispersion and d-d ex sugars, ice, sulfur CBN: stronger than ionic bonds ex diamond, graphite, asbestos

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12
Q

When dealing with rate law how does the balanced equation help?

A

It doesn’t

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13
Q

Which is stronger bond metalloid + nonmetal or nonmetal + nonmetal

A

Metalloid + Nonmetal

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14
Q

If temperature is the same, what does it mean for the molecules?

A

They all have the same average kinetic energy

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15
Q

Avogadro’s Law

A

All gases contain equal number of molecules at the same temperature and pressure

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16
Q

What is Hendreson Hasselback equation?

A

pH=pKa+ log base/acid

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17
Q

What is the Oxidation number of Oxygen, Elements, Hydrogen

A

H= +1 except hydrides=-1 e.g. LiH O= -2 except in peroxides= -1 Element= 0

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18
Q

Are Ionic compound molecules? What kind of array are they in?

A

No they are not molecules. They are in a crystal lattice.

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19
Q

What is the difference between polar and no polar bonds?

A

Nonpolar covalent bonds are a type of chemical bond where two atoms share a pair of electrons with each other. Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms.

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20
Q

What is the rate constancy?

A

.0821

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21
Q

What is the ideal gas law?

A

PV=nRT

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22
Q

Allotropes

A

Different forms of the same element

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23
Q

Oxidation Numbers of these molecules: PO4(Phosphate), KMnO4(permanganate),

A

PO4(Phosphate):-3 KMnO4(permanganate): -1

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24
Q

What is the temperature of and endothermic and exothermic RXN?

A

Endo: Lower Exo: Higher

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25
Q

Equation for taking a liquid to a gas

A

q=m(Delta)H make sure to divide mass by moles to get the correct units

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26
Q

Equation for pH and pOH

A

pH= -log[H+] pOH= -long[OH]

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27
Q

Specific Heat equation

A

(Delta)H=mc(delta)T C specific heat compacity

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28
Q

Gas Density Equation

A

P(MW)=DRT

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29
Q

Units for rate laws

A

1st order= sec^-1 2nd order= M^-1 sec^-1 Change the M^n to equal up to the rate order…basically add the exponents to equal the number of the rate order

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30
Q

VSPER(name EVERYTHING)

A
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31
Q

VSPER(Name just basic structures)

A
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32
Q

Explan Graphs of Rate order

A

*Nuclear decay is similar to 1st order

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33
Q

When a ion has a large - charge, what does that mean?

A

It has gained electrons causing it to increase in size

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34
Q

What is Aufbau principle?

A

determine the electron configuration of an atom, molecule or ion

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35
Q

Which elements are usually souble and insolube?

A

Solube: Group 1A metal, NH4, & NO3

Insouble: Ag, Hg, Pb, BaSO4, CaCO3

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36
Q

Oxidation Numbers of these molecules: HCO3(bicarbonate), NH4(ammonium)

A

HCO3(bicarbonate):-1 NH4(ammonium):+1

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37
Q

Oxidation Numbers of these molecules: C2H3O2(Acetate), NO2(Nitrite), ClO3(chlorate),

A

C2H3O2(Acetate):-1

NO2(Nitrite):-1

ClO3(chlorate):-1

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38
Q

Oxidation Numbers of these molecules: CLO4(Perchlorate), NO3(Nitrate), CH2O4(Oxalate),

A

ClO4(Perchlorate): -1

NO3(Nitrate): -1

CH2O4(Oxalate): -2

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39
Q

Oxidation Numbers of these molecules: Cr2O7(Dichromate), O2(Peroxide), OH(Hydroxide)

A

Cr2O7(Dichromate): -2

O2(Peroxide):-2

OH(Hydroxide):-1

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40
Q

Oxidation Numbers of these molecules:

SO3(Sulfite), SO4(Sulfate)

A

SO3(Sulfite):-2

SO4(Sulfate):-2

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41
Q

What is colligative properties?

A

Depends ONLY on # of particles in a solution, not solutes

ex: VP lowering, BP elevating

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42
Q

What is Molarity?

A

Moles of solute/Kg Solvent

Depends on temperature

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43
Q

What is the equation of find a boiling point or freezing point of molecule?

A

Boiling point-(Delta)T= Kb*m*i

freezing point- Boiling point-(Delta)T= Kf*m*i

*Take these and added to the correct tempearture of ºC

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44
Q

What is an equalibrium system?

A

OMIT solids and liquids from expression

K=Products/Reactants

When equation reversed(products to reactants)

Knew=(Koriginal)1/2

If reaction doubled= (K)2

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45
Q

What is an atom?

A

Basic Building block of Matter

smallest chemical unit of element

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46
Q

Explain Protons, neurtons, electrons

A

Atomic #(z)=Protons- + charge, 1 amu

Mass #- Atomic #= Neutrons, neutral, and a little bigger than protons

Atomic#= - charge, smalles, has calence elctrons

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47
Q

What are valence electrons?

A

Farthest from nucleucs= weaker attactiong

Able to leave and influence other atoms

Determin reactivity of atom

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48
Q

What is Atomic Mass Unit?

A

1.66 x10^-23 grams

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49
Q

What are isotopes?

A

Same # of protons but different neutrons

same # of + and -

Keeps chemical properties

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50
Q

What is Balmer Series?

A

4 wavelengths in visible region

upper leves of n

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51
Q

What is atomic Emission Spectra?

A

Most atoms in this state at room temp, but electrons ccan hbe excited to higher energy level and emit enegery as protons

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52
Q

What is the equation for Atomic Emission Spectra?

A

E=hc/lamda

H- Plank constant= 6.62606957 × 10-34 m2 kg / s

C= velocity of light= 3.0x10^8

Lamda= wavelength

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53
Q

What are the Quantum Number?

A

n, l, ml, ms

they explain the postiion and energy of electrons

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54
Q

What is Pauli exclusion principle?

A

No two electrons can have the same set of 4 quatum numbers

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55
Q

What is the principal quatam number?

A

N

the larger N is the energy level and radius

N max= 2n^2

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56
Q

What happens with shell energy with more distance from the radius?

A

they decrease in energy

enegry distance bw 4 &3 less than 1 & 2

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57
Q

What is the Azimuthal Number?

A

Angular momentum

l

subsells/sublevels

Intergers of l= 0-n-1

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

max # of electrons= 4l+2

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58
Q

What is Magnetic #?

A

Ml

Orbital region w/ in subshel may contain no more than 2 electrons

Ml= l to -l

Ml possible values= 2l+1

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59
Q

What are the orbitals of s, p, d, f?

A

s-1

p-3

d-5

f-7

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60
Q

What is Spin Number?

A

ms

Spin of particle is intristric angular momentum

Characteristic of particle

does NOT spin of axis

Spin orientation= +1/2 and -1/2

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61
Q

What is Hunds rule?

A

orbitals are filled by max number of half filled oritals with parallel spin

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62
Q

What effect do paired and unpaired electons have on molecules?

A

chemical and magnetic properties

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63
Q

What is paramagnetic?

A

unpaired electrons, magnetic field align the spin and attract atom

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64
Q

What is diamagnetic?

A

no unpaired electrons, slightly repelled by a magnetic field

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65
Q

How to find atomic radii?

A

Atomic radius decreases across period and inc down a group

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66
Q

What is ionization energy?

A

energy needed to remove electon form atom/ion

closer and tightly bound harder to remove

more energy to remove the 1st ionization energy

inc left ot right across period

dec down a group

group 1 lowest

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67
Q

What is elctron affinity?

A

Energy changes that occurs when elctron added

how easy an atom can accept electron

strong attaction greater electron affinity

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68
Q

What is electronegativity?

A

Attaraction an atom has for electons in a chemical bond

better for bonding, relates to ionization

inc form left ot right across period

decreasd down group

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69
Q

Properities of metals

A

Left and middle of table

solids at room temp except Hg

High MP & density

malleabality

ductitle

larger atomic radius

low ionization and elctroneg

good conduct of heat and electricity

G 1a IIa most reactive

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70
Q

Properties of nonmetals

A

Brittle at solid state

no metallic luster

high ionzation and electroneg

poor conductors of heat & electricity

upper right of periodic table

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71
Q

Properties of metalloids/semimetals

A

Zig zag line elements

varerity of properites

characteristics of metals and nonmetals

Good semiconductors

reavtive depending on element

Boron, Silicon, Germanium. Arsenic, Antimony, & Tellurium

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72
Q

What are alkali metals?

A

Group 1A, similar to metals

low densities

losely bounded elctron

largest radi

low ionzation and elctro negative

react w/ nonmetals and halogens

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73
Q

What aer alkaline earth

A

Group IIA

Smaller radi than alkali metals

2 electrons in outer shell

low electonegativity

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74
Q

What are halogens?

A

Group VIIA

highly reactive

gases, liquids and solid at room temp

high electronega

reactive with alkali and alkline earth metals

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75
Q

Waht are noble gases?

A

Inert gases

Group VIII

non reactive

low bp

gases at room temp

high ionzation

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76
Q

What are tranzaiton metals

A

Hard elements

High BP and MP

Across periods orbitals fill

low ionzation enrty

can lose numerous electrons

make complex ions with h2o or nonmetals

lower solubilites

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77
Q

What are the difference between ionic, covalent, and polar covalent bonds

A

I- electron is taken from low ionzation to another with high elect aff

C- electron pair shared

Polar- part covalent part ionic

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78
Q

What is ionic Bonding

A

Complete transfer of atom

Cation- lose elctron +

Anion gain electron -

High BP and MP

conduct eletricity in liquid and aq state

make crtstal lattice

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79
Q

What is Covalent bond

A

similar electronegative interaction

renergy required>energy relesased

weak intermolecular forces

low MP

Does not conduct electricity

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80
Q

What are the differences in Bond Length?

A

Short the better

shortest is triple bond

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81
Q

What is your center atom in Lewis structures?

A

least electronegative

end postion usually H, F, Cl, Br, I

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82
Q

What is formal charge equation?

A

V-1/2Nbonding - Nnonbonding

v= valence electrons

will determine best resonace structure

more negative the better resonace

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83
Q

Exception to octet rule

A

Atom Beyond III period

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84
Q

What is the differenct between nonpolar covalent and corrdinate covalent?

A

Nonpolar- b/w same electroneg, bond equal sharing, occurs in diatomic molecule(made with 2 atoms)

Coordinate- shared pair form lone paori of one atom

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85
Q

What are the shapes of s and p orbitals?

A

S orbital n=1, l=0 spherical symmetry

P orbital l=1 double shape

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86
Q

What is Dipole-Dipole?

A

+ region close to - region of another molecule

makes attractive forces

NOT in gas

High BP than nonpolar

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87
Q

What is Hydrogen Bonding?

A

Strong form of d-d

Bond w/ high electroneg atom

interatis w/ partial(-) chage of olther molecules

inc BP and hard to break enegry for it

ex H20,-OH, NH, COOH

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88
Q

What is Disperison Forces?

A

Equally shared covalent bonds has rapid polarization/ counter polarization of electron cloud

London forces- short lived dipoles

Weakest intermolecular force

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89
Q

Formula for Moles

A

Mol= weight of sample(g)/ molecular weight(g/mol)

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90
Q

What is equivalent weight?

A

Measure of reactive capacity

equivalent weight= wight of compouns/gram equivalent weight

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91
Q

What is gram equivalent weight?

A

determin the number of equivalents a compound contains

Molar mass/ n

n=# of Hs per molecule

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92
Q

What is the Law of constant compostion?

A

any sample of a give compound will contain smae element in identical mass ratio

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93
Q

What is empirical and molecular formula?

A

E- simplest whole # ration of elements

M- exact # of atomof each element

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94
Q

What is perecnt compostion?

A

Weight percent in specific compound

% compound= (mass of X informula/formula weight of compound) *100

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95
Q

What is combination reaction?

A

2+ reactants form 1 product

S + O2 to SO2

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96
Q

What is decmposition reaction?

A

One compound to 2+ substance

by heat or electrolysis

2HgO to 2Hg +O2

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97
Q

What is single displacement reaction?

A

Atom/ion replaced by another element

redox rxn

ZN + CuSO4 to Cu + ZnSO4

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98
Q

What is double displacement reactions?

A

metasthesis reaction

2 diffrent compouns displace each other make 2 new compounds

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99
Q

What is a net ionic equation?

A

Displacements use ions and can be rewritten into these

only show participating molecules

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100
Q

What is a spectator ion?

A

Don’t take part of overall reaction, but stay in solution

usually in displacement reaction

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101
Q

What is the equation for percent yield?

A

(actual yield/theroretical yield)*100

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102
Q

What is the defintiton of rate?

A

Disapparenc of reactants over time

appearnce of products over time

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103
Q

What is rate law?

A

Foward irreversible reaction

rate proportional to product of concentration to some power

Rate=K[A]^x[B]^y

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104
Q

What is zero order reactions?

A

Constant rate

indendent of reactant concentration

rate=K

unit=msec^-1

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105
Q

What are 1st order reactions?

A

rate proptional to one reactant concnetration

rate=k[A]

unit=sec^-1

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106
Q

What are 2nd order reaction?

A

rate porptional to 2 reactant or to sauware of concnetration of single reactant

rate=k[A]^2

unit: m^-1 sec^-1

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107
Q

What are height order reaction or mixed order reaction?

A

High= order 2+

Mixed= fractional order

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108
Q

What is the collision theory of chem kinetics?

A

Molecules must collide for reaction to occur

Rate of reaction is porption # of collison per second between reacting molecules

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109
Q

What is an effective collison?

A

Makes products

collide at correcto orientation

eable to break old bonds and form new bonds

110
Q

What is activation energy/energy barrier?

A

min energty need for collison for a rxn to happen

111
Q

What is the rate of reaction?

A

rate=fz

z=total number of collision per sec.

f=fraction of collison effective

112
Q

What is the Transition State Theory

A

molecules collide with sufficient energy

old bonds weaken

new bonds form

dissociates into product and new bonds full form

113
Q

What effects rate of reaction

A

Reactant concentration, tmep, medium and catalyst

114
Q

How does reactant concentration affet the reaction rate?

A

High concentration high # of effective collision

all rates will increast but zero order

115
Q

How does temperature affect rxn rate?

A

Rate will go up as temp rises

temp: avg kinetic energy

116
Q

How does medium affet reaction rate?

A

aq solutions may speed it p

can be solid, liquid or gas

117
Q

How do catalyst affect reaction rate?

A

Inc rxn w/o being consumed

lower activation energy

inc collison by changing orientation

reduce intrmolecular bonding

energy barrie lower

forces more toward equalibrium

118
Q

What is the law of mass action

A

one step reaction

when two rates = each other

Kf=Kr[BC/A] basically products/reactants

Kc=equilibrium contant c=conentration p= pressure

119
Q

What is reacation quotient?

A

Q

mesuare of degree to which a reaction has gone to completion

Qc=([CcDd]/[AaBb]

Qc=Kc constant at equalibrium

120
Q

What are the properties of the equilibrium constant?

A

Pure solids and liquids not in the constanct

It is a given temp

Very large compared to 1, very little reactat compared to products

very small compared to 1, very little products compared to reactants

Close to 1, equal amounts reactants and products

121
Q

What is Le Chatelier’s Principle

A

System to which stress is applied tends to change to releive the applied stress

effected by change in concentration, pressure, volume, and temperature

122
Q

What is the effect of concentration in Le Chatelier’s Principle?

A

Inc reactact more products will be made

equlibrium shifts right

Decrease reactants will shift equlibrium toward reactants

123
Q

What is the effect of pressure/ volume in Le Chatelier’s Principle?

A

Solid and liquid NOT effected

Pressure and volume invertedly related

High pressure low # of moles(reduces volume)-relieves stress

High Volume low pressure-shift toward products

124
Q

What is the effect of temperture on Le Chatelier’s Principle?

A

Product: exothermic

Reactants: endothermic

Dec temp reaction to right

Inc temp reaction to left

Only one to change the value of the equlibrium constant

125
Q

What is the Law of Conservation of Energy

A

states that the total amount of energy remains constant in an isolated system.

It implies that energy can neither be created nor destroyed, but can be change from one form to another.

126
Q

What are the various system in thermochemistry?

A

Isolated-cannot exchange energy or matter

closed-can exchange but not matter

open-cahnge exvhange both matter and energy

127
Q

What is a isothermal, adibatic, iosbric process?

A

Iso-temp constant

adibatic-no heat exchange occurs

iso-constant pressure

128
Q

What is enthaply?

A

express hear changes at constant pressure

129
Q

What is the change in enthaply?

A

heat absored or evolved by the system at constant pressure

It depend on intial and final

Hrxn=Hproducuts-Hreactants

H+ endothermic

H- exothermic

130
Q

What is the enthaply standard heat formation?

A

enthalpy change that would occur if one mole of compound were formed directly from its element in ther standard states

elemnt is standard state=0

Hf

131
Q

What is enthaply standard heat of reaction?

A

Hypothetical enthaply change that would occur if the reaction were carried out under standard condtions

=Sum of Hf products- Hf of reactants

132
Q

What is Hess Law?

A

enthalpies of eactions are additive

133
Q

What is Bond dissociation Energy in enthalpy?

A

average of energy requiresd to break a particular type of bond in one gaseous molecules

h=hbonds broken + hbonds formed

134
Q

What is enthalpy heat of combustion?

A

usually fast and spontaneous and usally combustion

135
Q

What is entropy?

A

measures disorder/randomness

units:energy/temp:J/k:cal/k

high order low entropy

low order high entropy

*sublimtaion greatest entropy change

136
Q

What is the formula for entrop state fucntion?

A

S=Sfinal-Sintial

qrev/T

Qrev= heat added to system

T= absolute temperature

137
Q

What is the standard entropy change for a reaction?

A

Sum of Sproduct-Sum of Sreactants

138
Q

What is the second law of theromdynamics

A

All spontaneous process proceed such that entrop of the system plus it surrounds increae

Suniverse=Ssystem+Ssurroundings>0

139
Q

What is Gibbs Free Energy?

A

Spontaneity of Reaction

combines two factors that affect the spontaneity of rxn;change in enthalpy and changes in entropy

140
Q

What does (Delta)G mean?

A

Maximum amount of energy release by process. at constant tmeperature and presssure

(Delta)G= (Delta)H-T(Delta)S

141
Q

What will be the reaction if (Delta)G is negative, postive, and zero?

A

Negaitive- spontaneous

Postive-not spontaneous

0-state of equilibrium

142
Q

What would be the reactions for

(Delta)H (Delta)S

  • +

+ -

+ +

  • -
A

-+ spontaneous at all tem

+-nonspontaneous at all temperatures

++sponatneous only at high temp

-sponatneous only at low temp

143
Q

If reaction nonspontaneous what will be the reverseal reactions

A

reversal will be sponatanous

144
Q

What is standard free energy of (Delta)G?

A

Defined as the process occuring at 25c 1 atm pressure for which concentration of any solution invlver ar 1 mM

Most stable form 0

=sum of products-sum of reactants

145
Q

What is the eaulibrium contant for (Delta)Grxn?

A

=-RTlnKeq

Keq-equilibrium constant, r-gas constant, t temp in K

146
Q

What is the raction quotient in Gibbs Energy?

A

This happens after rxn starts

(Delta)G=(Delta)Gº+RTQ

147
Q

What is STP?

A

Standard Temp and pressure of gases

273K

1atm

148
Q

What is Boyle’s Law?

A

Gas at constant tempature

volume and pressure inversely proportional

149
Q

What is the EQUATION for Boyle’s Law?

A

P1V1=P2V2

150
Q

What is Charles and Gay-Lussac Law?

A

at constant pressure

volume gas directly porptional to absoulte temperature

151
Q

What is avogadro’s principle?

A

Gass at constant temp and pressure

volume directly porptional to moles of gas present

can be used to kinetic rate law

152
Q

What is the EQUATION for Charles law?

A

V1/T1=V2/T2

153
Q

What is the EQUATION for avogadro’s principle?

A

N1/V1=N2/V2

154
Q

What is the ideal gas law?

A

Shows relation bw pressure, volume, temp, and moles of gas

155
Q

Ideal Gas Law equation

A

PV=NRT

R=gas constant=8.21x10-2 L*atm/mol*KJ=8.314 J/K*mol

156
Q

How to find density of gas?

A

P(MM)/RT

V2=V1(P1/P2)(T2/T1)-can be used to find molar mass

d=m/V2

157
Q

How are real gases effecte by pressure?

A

high pressure- molecules closer together until it becomes liquid

moderately-volume less bc of intermolecular attraction

extremely high-takes up more space!

158
Q

What is the effect of tempurature of real gas?

A

low temp low velocity-attractive forece become important

Closer the gas is to BP less ideal it is

159
Q

What is Dalton’s Law?

A

2+gases in one vessel w/o chem interation will be have independitly

Both exert partial pressure

160
Q

How to find partial pressure?

A

Pa=PtxA

xA=Moles of A/total moles

161
Q

What is the Kinetic Moleculear Theory of Gases?

A

Molecular behavior based on motion of individual molecules

162
Q

Assumption 1 of kinetic moleular theory

A

Particles volumes are negligible compared to container volume

163
Q

Assumption 2 of kinetic molecular theory

A

atoms/molecules exhibit no intermolecular attraction/repulstion

164
Q

Assumption 3 of kinetic moleuclar theory

A

Continous, radom, collisons with other particles and container walls

165
Q

Assumption 4 of Kinetic Molecular Theory

A

Collision between any 2 gases are elestic(no overall gain/loss of energy)

166
Q

Assumption 5 of kinetic molecular theory

A

Average of Kinetic energy proptional to absolute temp and same for all gas at given

167
Q

Kinetic Molecular Theory of Gases Equation

A

Kinetic Energy=1/2(mv2)=3/2(kT)

k=boltzmann constant=1.23x10-23

168
Q

What is Maxwell-Boltzman Curve?

A

shifts right as temp inc

inc temp inc in speed

169
Q

What is Graham’s law of Diffusion?

A

heavier gas molecule diffuse more slowly than lighter ones

differing avg speed

170
Q

Equation Graham’s Law of Diffusion and Effusion

A

r1/r2=(MM2/MM1)1/2

r=diffusion rates

171
Q

What is Graham’s law of Effusion?

A

Flow of gas particles under pressure from one compartement to another through a small opening

172
Q

What is amorphous solid?

A

no ordered 3d arrangement, but molecules fixed into place

173
Q

What is a crystalline?

A

possesse an order structure

3d arrangments

174
Q

Properties of ionic solid

A

high BP and MP

poor electrical conductivity

strong electrostatic interaction

175
Q

Properties of metallic solids

A

metals packed closed together

high MP and BP

strong covalent attraction

176
Q

What is vapor pressure?

A

equalibrium bw evaporation adn condestion rates are equal

177
Q

When does vapor presure increase?

A

when temperature increases

178
Q

When vapor pressure of liquid = external pressure

A

boiling point

179
Q

What is depostition?

A

gas to solid

180
Q

What is Gibbs Function

A

thermodynatimic criterion for each above equilibria of gas-liquid, liquid-solid, gas-solid

181
Q

What is the phase diagram

A
182
Q

Define triple poitn and critical point of phase diagram

A

tp-phases at equilibrium

cp-temp and pressure no distinction bw liquid and gas

183
Q

What is Raoult’s Law?

A

USe on of mixtures to get the relation of one in the souliton

find relationship betweek vapor pressure of vapor and concentraion of liquid

184
Q

Raoult’s graph

A
185
Q

What is equation for freezing/boiling point depression?

A

Kf*m

Kf=proportionality constanct

m=molality of solution

186
Q

What is osmotic pressure?

A

Gives enough pressure to counterbalance the tendency to go through a membrane

depens on amount of solute

187
Q

Equation for osmotic pressure

A

Π=MrT

M=molarity

r=idal gas constant

t=kevlin

188
Q

In osmotic pressure what is dirrecly proptional

A

molarity and osmotic pressure

189
Q

What is vapor-pressure lowering?

A

Similar to raoult’s law

solute add to pure solven vapor pressure decreases

190
Q

Equation for Vapor pressure decrease

A

P=xbPºA

xb=mole raction of soulte B in solvent

xb=1-xa

P°a=vapor pressure of pure solvent

191
Q

What is a non ionic solution?

A

solvation involves van der wals between solute and solvent

192
Q

General Rule of solutions

A

inoic and polar souble in polar

nonpolar dissolve in nonpolar

193
Q

What does saturated mean referring solutions?

A

when max added

solution at equlibrium

194
Q

What does dilute mean referring to solutions?

A

propotion of solute:solvent small

releative term

195
Q

What does concentrated mean referring to solution?

A

Proportion of solute to solvent large

196
Q

Aqueous solution rule 1

A

Sals of alkali metal soulble in H2O

197
Q

Aqueous solution rule 2

A

All ammounium salt H2O soluble

198
Q

Aqueous solution rule 3

A

All chlorides, bromides, iodies soule in H2O

EXCEPT: Pb, Hg2, Ag

199
Q

Aqueous solution rule 4

A

All salts of SO4 ion souble

Ca, Sr, Ba, Pb

200
Q

Aqueous solution rule 5

A

MEtal oxides INSOULBE

except CaO, SrO, BaO

201
Q

Aqueous solution rule 6

A

All Hydroxides insouble

except alkli metals, Ca, Sr, Ba

202
Q

Aqueous solution rule 7

A

All carbonates, Phosphates, sulfides, and sulfites are insoulbe

exepte alkali metals and ammonium

203
Q

Ending of element with lesser or greater charge

A
  • ous lesser charge
  • ic greater charge
204
Q

Monatomic anions ending

A

-ide

205
Q

Polyatmic anions(oxyanions)

A

Less oxygen -ite

more oxygen -ate

206
Q

Four oxyanions prefix

A

Hypo-less oxygen

Per-more oxygen

207
Q

Polyatomic anions that gain 1 or more H prefix

A

Hydrogen or dihydorgen

add in front of name

208
Q

Ion charges on left of peroidc charges

A

usually positive

209
Q

Ion charges on the right of the periodic table

A

usually negative ions

210
Q

How are groups set up with ion charges/

A

usually the same

211
Q

What are electrolytes?

A

electial conductivity of aq governed by precence and concentratio of ion in solution

212
Q

How do strong electrolytes dissociates?

A

consitutent + ion

213
Q

What are non electolytes

A

Compound that do no ionize in aq and retain molecular structure

limited solubility

214
Q

What is an aquesus solution?

A

They dissolve in water

215
Q

Equation for precent composition by mass

A

(Mass of solute/mass of solution)x100

216
Q

Mole fraction equation

A

moles of compoiund/# of total moles of everything in system

217
Q

What is molarity?

A

of moles solute per liter of solution

depend on volume of solution

218
Q

What is molality

A

moles of solute/ kg of solvent

219
Q

What is normality?

A

of gram equivalent weight

meausre reatvitiy of molecule

220
Q

What is dilution

A

a solution is diluted in a solven

solvent added to a solution with high concnetration to get a lowere concnetration

221
Q

Equation for dilution

A

MiVi=MfVf

M=molarty

V=volume

222
Q

Solubility product constant

for ion and saturated solution

A

=[An+]m[Bm-]n

m and n are charges

223
Q

Qsp>Ksp

A

precipitation will occur

Qsp-ion constant

Ksp-solubility constant

224
Q

Qsp<ksp>
</ksp>

A

dissolution happen until soultion saturatied

Qsp=ion constant

Ksp=souilbility product constant

225
Q

Qsp=Ksp

A

eqalibrium solution satureted

dissolves equal it preciptatin out of solution

226
Q

General formula for slightly soulble salt MX3

A

MX3

Ksp=27x4

227
Q

General formula for slighlty souble salt of MX2

A

Ksp=4x3

x= molar solubility

228
Q
A
229
Q

What factors affect solubility?

A

Temp of solution solvent

gasp phase solut is the pressure

other substances added

230
Q

What is the common ion effect?

A

Example of Le Chateleir’s Principle

decution recation to solubility

if something is added to soultion

231
Q

General formula of slightly soulble salt of general formmula MX

A

Ksp=x2

232
Q

When anion becomes acid suffix?

A

-ide

233
Q

Anion with a prefix of hydro acid end

A

-ic

234
Q

Acids formed form oxyanions endings

A

called oxyacids

anion ending in -ite new ending is -ous

anion end in -ate ending is ic acid

235
Q

How to measure dissaccocitaion of acid?

A

Ka= [product][product]/[HA]

HydrogenA+H2O-H30+A

Ka= acid dissociation constant

236
Q

How to measure the dissociation of a base?

A

Kb=[B][OH]/[BOH]

237
Q

What is hydrolysis?

A

reverse reaction salt ions react with water to give back the acid/ base

238
Q

What is acid equivalent?

A

One mole of H+ ions

239
Q

What is base equivalent?

A

equal to one mole of OH- ion

240
Q

What does polyvalent?

A

each mole of acid/ base liberates more than one acid/base equivalent

241
Q

Common polyvalent acids

A

H2SO4,

H3PO4

H2CO3

242
Q

What is amphoteric or amphiprotic species?

A

One taht can act either as an acid/base, depending on its cehmical enviornment

example water

243
Q

What is amphortic?

A

partially dissociated conjugate base of polyprotic acid

ex: HSO4, can gain or lose H

and hydroxides of cerain metals

244
Q

What is a titration?

A

Prodedure used to determine the molarity of acid or base

245
Q

What is equivalence point?

A

number of acids equivalents equals the number of base equivalents added

246
Q

What is end point?

A

when the indicatior actually changs color

247
Q

What is buffer solution

A

consistes of mixture of weak acid ann its salt

mixture of weak base and its salt

resist changes in pH

248
Q

What does polyprotic acid mean

A

specific acids that are capable of losing more than a single proton per molecule in acid-base reactions

249
Q

What are the oxidations of Group 1A and 2A

A

Group 1=+1

Group 2=+2

250
Q

Oxidation number of group 7A in a compound

A

is -1

except with element higher electro negativity

251
Q

Wht is half reaction method?

A

separte equation into two half reactions

oxidation part

reduction part

then add the needed H and e to each equation

252
Q

What are the two types of electrochemical cells?

A

Galvanic cells/voltaci cells

electrolytic cells

253
Q

What kind of reaction occurs in galvanic cell?

A

has negative G, so it is sponateous

negative pole of battery

254
Q

What are half cells?

A

Separate by energy

255
Q

What kind of reaction is in eletrolytic cells?

A

positive G

non spontaneos

postive pole of battery

256
Q

What is Faraday’s Constant?

A

One elctron chargexby avagadors number

1F= 96,487 coulombs

257
Q

Which direction does the electron go in a battery?

A

anode to cathode

258
Q

What is Eº?

A

Standard reduction potential

259
Q

What happens in high and low Eº?

A

high: greater tendency for reduction
low: greater tendency for oxidation

260
Q

What is standard electromotive force?

A

Difference in potential between two half cells

emf/Eºcell

261
Q

What does emf equal?

A

Eºred+Eºoxid

262
Q

Equation of Emf and Gibbs Free energy

A

G=-nFECell

263
Q

Effect of conecntraon on EMF

Nernst equation

A

Ecell=Eºcell-(RT/nF)(ln(reaction quotient))

264
Q

HOw can emf be measeured?

A

By voltmeter

265
Q

Realtionshp between EMF and the Equalibrium

A

G=-RTlnKeq

r=gas constant

nFEcell=RTlnKeq

266
Q

What is mass defect?

A

Difference bw them protons and neurtons

267
Q

What is fusion?

A

small nuclei combine to into large

268
Q

What is fission?

A

Large nucleus splint into small nuclei

rarely spoontaeous

269
Q

What are chain reations in reference to fissions?

A

neutrons cause them by splitting and they cause others neutrons to split causeing a chain reaction

270
Q

What is Baryon number conservation?

A

the total number of neutons plus protons remains the same, even if neutrons converted to protons

271
Q

Name some strong acids

A

HBr. HCl, HNO3, H2SO4, HClO4

272
Q

What is Ka = to in acid/base equations?

A

Ka=Products/reactants

DAT (4 decks)

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