Inorganic and Phychem Flashcards
(303 cards)
1
Q
Element is composed of tiny, indivisible, & Indestructible particles call atoms
A
Atomic Theory by Dalton
2
Q
After 50 years, evidence was seen that atoms are divisible by
A
Marie Curie
3
Q
Who named atoms from atomos which means indivisible?
A
Democritus
4
Q
The pudding model is by
A
Joseph John thomson
5
Q
What model of the atom where electrons are distributed evenly on a sphere of positive charge?
A
Pudding model (jj thomson)
6
Q
Who discovered electron?
A
Joseph john thomson
7
Q
Who gave the name electron?
A
G. Johnstone stoney
8
Q
Caltech of electron charge
A
Shift 7 3
9
Q
Which experiment and who discovered the eletric charge?
A
Millikan oil drop experiment by Robert Millikan
10
Q
Who discovered proton?
A
Ernest rutherford
11
Q
Cathode rays (by jj thomson) produced electron, what rays produced proton and by who?
A
Anode rays by eugen goldstein
12
Q
What experiment bombarded a gold foil with alpha particles?
A
Alpha particle scattering experiment by Ernest rutherford
13
Q
Who discovered neutron?
A
James chadwick
14
Q
James chadwick bombarded what element w/ alpha radiation to produce neutron?
A
Beryllium
15
Q
He proposed that light and other electromagnetic waves were emitted in discrete packets of energy called quanta
A
Max Planck
16
Q
Energy formula
A
E=hf=hc/ÿ
17
Q
A theory that describes matter as acting both as particle and wave
A
Quantum theory of atoms
18
Q
Atoms produces what kind of spectra
A
Line spectra
19
Q
Molecules produces what kind of spectra
A
Band spectra (group of lines close to each other)
20
Q
Bohr’s Model Formula
A
E=2.18x10^-18z^2(1/n1^2 - 1/n2^2)
J/photon
21
Q
Number of Proton and electron is equal to Z, What is Z
A
Atomic Number
22
Q
How to get the number of neutrons of an element
A
Atomic mass (A) - Atomic Number (Z)
23
Q
Photoelectric Effect Formula KE
A
KE=1/2 mv^2 =hf - ø (ø work function of metal)
24
Q
Compton scattering Formula Wavelength
A
Ÿ’ - ÿ= (h/mc) (1-cosö)
25
He suggests that matter might exhibit wave-like properties
De Broglie Wavelength by Louis de Broglie
26
Formula for De Broglie’s Wavelength
Ÿ=h/mv
27
What is this principle “ It is impossible to know exactly both the position & momentum of an electron/small particle simultaneously and accurately”
Heisenberg’s Uncertainty Principle
28
Recite the Schrodinger’s Equation
Check nalang sa index!
29
“The wave function contains all the dynamical information about the system it describes”
Born Interpretation of wave function squared
30
Avogadro’s number
6.02x10^23 atom/mol
31
Quantum numbers: Principal
n=1-7
32
Quantum Numbers: Azimuthal, l
0=s
1=p
2=d
3=f
33
Quantum Numbers: Magnetic, ml
-1, 0, 1 or dpende sa azimuthal
34
Quantum Numbers: Spin, ms
+1/2 -1/2
35
Total electrons in the nth shell formula
2n^2
36
“No two electrons of an atom can have all the four quantum numbers the same” what principle and by who
Pauli’s Exclusion Principle by Wolfgang Pauli
37
“The filling of subshells by electrons are according to increasing order of energy and follows the (n+1) rule” what principle
Aufbau Principle
38
“The pairing up of electrons in an orbital of a subshell takes place only when all orbitals contain at least one electron” what rule
Hund’s rule of Maximum Multiplicity
39
Who discovered Radium and Polonium?
Marie Curie
40
Half life of C-14
5730
41
Our body has what kind of 2 carbons
C-12 and C-14
42
What is a Pitch blende
Ore of 238U3O8 • 11H2O
43
What isotope used as medicine for Thyroid?
I-181
44
What isotope/s used as medicine for Bones?
Ca-41 and P-32
45
What isotope used as medicine for Heart?
Th-282
46
Radioactive decay rate
N=NaMok/AW
47
1curie (Ci) is equal to
3.7x10^10/s
48
Geological Dating Formula
t=1.5x10^10 log(1+ Pb206/U238) years
49
Carbon-14 Dating Formula
t=1.9x10^4 log(rliving/rdead) years
50
Biggest Nuclear Plant
Kashiwazaki-Kariwa
51
Mass-energy equivalence Formula
E=mc^2
52
1amu is equal to how many grams
1.66x10^-24
53
1amu is equal to how many MeV
931
54
What experiment bombarded U-235 w/ neutron and obtained the element 56 & 36?
Nuclear Fission
55
Who lead the nuclear fission experiment?
HMS
| Hahn, Meitner, Strassman
56
What elements are obtained in the nuclear fission experiment?
56 & 36
57
Nuclear fission experiment bombarded what element with neutron obtaining elements 56 & 36?
U-235
58
Fuel used in nuclear powerplant
U-235
59
Nuclear power plant fuel consumption formula
M=2.11x10^-4 x P/NaE g/day
60
Formula for Binding Energy
BE=[Z x Mh + (A-Z) x Mn-Ma) (931MeV/1amu)
61
Equivalent of Mh in binding energy
1.007825 u
62
Equivalent of Mn in binding energy
1.008665 u
63
Who classified the elements according to metals, non metals, gases, and earths
Antoine Lavoisier
64
Who discovered the law of triads
Johann Dobereiner
65
Who made the three dimensional arrangement of known elements
Alexandre Beguyer
66
Who discovered the law of octaves
John Newlands
67
Who first to recognize periodic trends in properties of elements
Julius lothar Meyer
68
Who arranged the elements in increasing order of their atomic masses
Dmitri Mendeleev
69
This law states that elements are periodic functions of their atomic number
Periodic law
70
Energy released when an electron is added to an isolated gaseous atom
Electron affinity
71
Measure of the relative tendency of an atom to attract shared electron pair
Electronegativity
72
What is used in electronegativity to measure the relative tendency of an atom to attract shared electron pair
Pauling scale
73
Determination of lattice energy of a compound between metals & nonmetals
Born haber cycle
74
Born-haber cycler formula
Q=S+I+1/2D+Ea+Uo
75
What bond shared electrons between non metals
Covalent bond
76
What bond transfers electrons from metal to non metal
Ionic bond
77
Equal sharing of bonding pairs
Non polar covalent bond
78
Unequal sharing of bonding pairs
Polar covalent
79
Result of electron transfer
Ionic Bond
80
What rule where atoms tend to gain lose or share electrons until surrounded by 8 valence electrons
Octet rule
81
Electrons are written as dots
Lewis structure
82
Formal charge formula
Valence e- -1/2 (bonding e-) - (Non-bonding e-)
83
Bond order formula
BO= [(e- in BMO) - (e- in ABMO)] / 2
84
Leo says ger meaning
Losing electrons is oxidation
| Gaining electrons is reduction
85
Ideal gas equation
PV=nRT
86
Boyle’s Law
P1V1=P2V2
87
Charle’s law
V1/T1 = V2/T2
88
Gay Lussac’s Law
P1/T1 = P2/T2
89
Combined Gas Equation
P1V1/T1 = P2V2/T2
90
Dalton’s Law
P1/PT= n2/nT
91
Amagat’s Law
V1/VT = n2/nT
92
Ludwig Boltzmann Constant K Formula
K=R/NA =1.38x10^-23 j/molecules-K
93
Maxwell’s Distribution of Speeds Formula: Most Probable Speed
Sqr root of 2RT/M
94
Maxwell’s Distribution of Speeds Formula: Mean Speed
Sqr root of 8RT/piM
95
Maxwell’s Distribution of Speeds Formula: Root mean squared
Sqr root of 3RT/M
96
Graham’s Law of Diffusion Formula
ÛA/ÛB= sqr root of MWB/MWA
| Or ÛA/ÛB= sqr root of Density A/Density B
97
Mean Free Path Formula
ÿ=[1/(sqr root of 2)(ô)] [RT/PNa]
Na= avogadro’s
98
Gas gas collision formula
Zgg=Vave/ÿ
99
Gas wall collision formula
Zgw=PANa/ sqr root of 2pi MRT
100
Compressibility Factor, Z formula
Z=PV/RT
101
Van Der Waals Formula
(P + n^2 a/V^2) (V-nb) = nRT
102
Boyle Temperature Formula
TB=a/bR
103
Ability of a fluid to escape
Fugacity (gas has fugacity and liquid has none)
104
Critical Constant, a formula:
a=27 R^2 Tc^2 / 64 Pc
105
Critical Constants, b formula:
b=R Tc/8 Pc
106
Barometric Pressure formula
P=Po e^-(g M Z / R T)
107
Po @ Sealevel pressure is
101.325 KPa or 1atm
108
Strongest intermolecular force
Ion dipole
109
Intermolecular force with H bond
Dipole dipole
110
Weakest intermolecular force
London dispersion
111
Dipole moment formula
û= qr=(n x e) (r)
112
Ionic Character formula
û obs / û theo
113
Intermolecular attraction between unlike molecules
Adhesive forces
114
Intermolecular attraction between same molecules
Cohesive forces
115
Ability of a liquid to flow in narrow spaces without external forces
Capillary action
116
Capillary action height formula
h=(2(gamma y) cos (alpha a))/(rho, p) g r
gamma, y= liquid air surface tension
117
Half bubble formula
Pi -Po=4y/r
gamma y
118
Full bubble formula
Pi -Po=2y/r
gamma y
119
What compound forms bubbles in soap
Surfactant
120
Solids not arranged in an orderly manner
Amorphous solids
121
Solids arranged in a definite manner
Crystalline solids
122
Different physical properties in different directions
Anisotropy
123
Amount of energy required to completely separate the ions
Lattice energy
124
1 atom are held together in a large network
Network covalent
125
Who (3) discovered C-60 buckministerfullere or bucky ball
Harry kroto, Richard Smalley, and robert curl
126
Total number of space lattices
14
127
Body centered radius formula
4r=a sqr root of 3
128
Face centered radius formula
4r=a sqr root of 2
129
Simple crystal lattice radius formula
a=2r
130
Packing fraction of simple crystal lattice
pi/6
131
Packing fraction of body centered crystal lattice
pi sqr root of 3 / 8
132
Packing fraction of face centered crystal lattice
pi sqr root of 2 / 6
133
Density of crystal
p= n(AW)/NA (a)^3
134
1 angstrom equal to m
10^-10
135
Who discovered DNA via X-ray crystallography
Rosalind franklin
136
Crystal are not only diffraction gratings but also reflection gratings
Bragg’s law
137
Lawrence Bragg equation
ny=2dsin@=2dsin@/ sqr root of h^2 + k^2 + I^2
y gamma
@ theta
138
Packing efficiency formula
PF= [ (# of atoms/unit cell) (atomic volume ] / volume of unit cell
139
Enthalpy Formula
H=U+PV
140
If Change of H is less than 0
| Process is
Exothermic
141
If Change of H is greater than 0
| Process is
Endothermic
142
Enthalpy formula for gases
Change of H = change of U + change of ng R T
Change of ng = product moles - reactant moles
143
Hess law
Enthalpy change is independent of the way the process is carried out
144
Measure of degree of disorder in the system
Entropy
145
Unit of Entropy
J/mol K
146
Used to calculate absolute zero entropies of pure substance at any temperature
Third law of thermodynamics
147
gibbs free energy, G formula
G=H-TS
148
Unit of Gibbs free energy
J/mol
149
Energy freely available from the system which can put into useful work
Gibbs free energy
150
@ Normal Boiling Point temperature, Pressure is
1 atm
151
If change of G is less than 0, system is
Spontaneous
152
If change of G is greater than 0, system is
Non spontaneous
153
If change of G is equal to 0, system is
@ equilibrium
154
If change of enthalpy is positive and change of entropy is positive system is
Spontaneous @ high T
155
If change of enthalpy is positive and change of entropy is negative system is
Non spontaneous at all T
156
If change of enthalpy is negative and change of entropy is positive system is
Spontaneous at all T
157
If change of enthalpy is negative and change of entropy is negative system is
Spontaneous at low T
158
Solid to vapor
Sublimation
159
Vapor to solid
Solidification
160
Solid to liquid
Fusion
161
Liquid to solid
Freezing
162
Liquid to vapor
Evaporation
163
Vapor to liquid
Condensation
164
Clapeyron equation
(P2-P1/T2-T1) = H of fusion / (T1+T2/2) (V2-V1)
V is specific Volume
165
Clausius Clapeyron Equation
ln (P2/P1) = (-H/ R) (1/T2 -1/T1)
166
Trouton’s rule in using Boyle’s Temp
Change of S = H vap/ Tb = 10.5R = 21 cal/mol K = 88 J/mol-K
167
There is phase change but no change in temperature
Latent heat
168
There is change in temperature but no phase change
Sensible heat
169
Reaction Quotient, Q is less than K
Shift to right
170
Reaction Quotient, Q is greater than K
Shift to left
171
Reaction Quotient, Q is equal to K
@ equilibrium
172
Van’t Hoff’s Equation
ln (k2/k1) = (-H/R) (1/T2 - 1/T1)
173
Le Chatelier’s Principle,
| If Change of H is exothermic temperature
Increases and shift to the left
174
Le Chatelier’s Principle,
| If Change of H is endothermic temperature
Decreases and shift to the right
175
Le Chatelier’s Principle,
| If pressure increases
It shifts to the side with less mole
176
Le Chatelier’s Principle,
| If pressure decreases
Shift to the side with more mole
177
Le Chatelier’s Principle,
| If concentration of reactant increases
Shifts to the right
178
Le Chatelier’s Principle,
| If concentration of product increases
Shift to the left
179
State of solution is based on the state of
Solvent
180
Is a mixture of gases a true solution
Yes
181
Does true solution remains homogeneous with time?
Yes
182
For solids, if Temperature increases, solubility
Solubility increases and vice versa
183
For gases, if pressure increases solubility
Solubility increases and vice versa
184
For gases, if temperature increases solubility
Solubility decreases and vice versa
185
Raoult’s Law is by
Francois Marie Raoult
186
Formula of Raoult’s law
Partial Pressure A = Xa (Vapor Pressure A)
```
PA = XA P*A
XA = moles in liquid
YA = moles in vapor
```
187
Raoult’s law formula for YA
YA= Alpha XA/(Alpha -1) Xa + 1
188
Raoult’s Law formula of Alpha
Alpha= PA/PB
189
Vapor pressure of each component are independent of each other
Immiscible Liquids
190
Immiscible Liquids Formula
Pt= P1 + P2= P*1 + P*2
P*1 and P*2 are vapor pressure
191
Freezing point depression formula
(0-Tf) = i m kf
m is molality
192
Boiling point elevation formula
Tb-100 = i m kb
m is molality
193
Osmotic Pressure formula
Pi=iCRT
C is molarity
194
Ebullioscopic constant, kb
0.52c/m
195
Cryoscopic constant, kf
1.86c/m
196
gc is equal to
gc= 1kg m/ N s^2 or 32.174 lb ft/lbf s^2
197
Most electronegative element
Fluorine
198
Vant hoff constant, i formula
alpha= i-1 / v-1
199
In Osmosis if Co is greater than Ci it is
Hypotonic or crenation
200
In osmosis If Co is less than Ci it is
Hypertonic or hemolysis
201
If in osmosis Ci = Co it is
Isotonic
202
In electrochemistry, if chemical energy is converted to electricity it is
Galvanic or voltaic cell
203
In electrochemistry, if electrical energy is converted to chemical energy it is
Electrolytic cell
204
Is galvanic cell spontaneous or not?
Spontaneous
205
Is electrolytic cell spontaneous or not?
Not spontaneous
206
Faradays constant is equal to blank coulombs/mol
96500 coulombs/mol
207
Electrolytic Cell formula
I (change of T) = m n F / MW
n is no. Of electrons
208
Nerst Equation
E=Ecell - 0.0592/n log Q
209
Nerst equation at equilibrium
Ecell= 0.0592/n log keq
210
Does not meet the criteria of a primary standard but used subsequently as the titrant in a particular method
Secondary standard
211
Formed due to solvation of salts, strong acids and bases into a solution
Electrolytes
212
Enumerate the strong acids
HCl, HBr, H2SO4, H3PO4, and HNO3
213
Enumerate strong based
Part of group 1 (OH)
| And group 2 (OH)2
214
For weak acid solution
Ka= x^2/c-x
x=H+
ph=-log(H+)
215
For weak base solution
Kb= x^2/c-x
x=OH-
ph=14+log(OH-)
216
Arrhenius Base
Produce OH-
217
Arrhenius acid
Produce H3O+
218
Bronsted-Lowry Acid
Donate H+
219
Bronsted-lowry base
Accept H+
220
Lewis Acid
Accept e- pair
221
Lewis Base
Donate e- pair
222
Acts as both acid and base
Amphoteric
223
Possess both hydrophilic and lipophilic properties
Amphipatic
224
Amphoteric that can accept or donate proton
Amphiprotic
225
Amphoteric that contain both acidic and basic groups and exists as zwitterions
Ampholytes
226
From acid to conjugate base
Just remove 1H from acid
227
From base to conjugate acid
Just add 1 H sa base
228
Ka of CH3COOH
1.8x10^-5
229
Kb of NH3
1.8x10^-5
230
Salt of weak acid (Weak Base) formula
OH-= sqr root of KwC/Ka
231
Salt of weak base (Weak acid) formula
H+ = sqr root of KwC/Kb
232
Salt of weak acid and base formula
H+ = sqr root of KwKa/Kb
233
K of water or Kw is equal to
1x10^-14
234
Diprotic H2X formula
Ka=x^2/c-x
| H+
235
Diprotic HX- formula
H+ = sqr root of (K1K2C-K1Kw)/K1+C
236
Diprotic x^-2
Kb2=Kw/Ka2=x^2/c-x
| OH-
237
Triprotic H3X formula
Ka=x^2/c-x
238
Triprotic H2X- Formula
H+ = sqr root of (K1K2C-K1Kw)/K2+C
239
Triprotic HX^-2 formula
H+= sqr root of (K2K3C-K2Kw)/K2+C
240
Triprotic X^-3 formula
Kb3=Kw/Ka3= x^2/c-x
| OH-
241
Buffer is composed of
Weak acid/base and conjugate salt
| 1H difference
242
Henderson-Hasselbalch equation
pH=pka+log (base/acid)
243
Organic compounds used in titration to provide color change
Indicators
244
Normality formula
N=M x n
M molarity
n number of H+/OH-/e-
245
Kjeldahl factor for cereals:
5.70
246
Kjeldahl factor for meat products:
6.25
247
Kjeldahl factor for dairy products:
6.38
248
If there is salt in the solution the solubility of salt decreases
Common ion effect
249
Uses AgNO3 as titrant producing brick red color
Argentometric titrations
250
Color of ferric chloride
Orange
251
Titration where reaction of Ag+ and Dichromate forms red silver dichromate
Mohr method
252
Titration using KSCN as 2nd titrant
Volhard method
253
Titration using a sodium fluoresceinate as indicator with no back titration because end point is sharp
Fajans Method
254
How to spot end of titration
1sr trace of red
255
Bending of molecular bonds
Molecular conformation
256
Have one unshared pair of electrons capable of forming covalent bond w/ ion
Ligand
257
Formed when metal ion bonds with monodentate ligand
Coordination complex or metal complex
258
Metal ion bonds with polydentate ligand
Chelate complex
259
Forms soluble complex molecules with a metal ion resulting to inactivation of the ion’s ability to react with other elements to produce precipitate
Chelants
260
Indicators of EDTA
Eriochrome Black T
Murexide
Calmagite
261
Gravimetric Factor formula
GF= (MWB/MWA) (a/b)
262
Redox electrons: MnO4- in acid and color
5e- (pink)
263
Redox electrons: MnO4- in base and color
3e- (brown)
264
Redox electrons: C2O4^-2
2e-
265
Redox electrons: As^3+
2e-
266
Redox electrons: Fe^2+
e-
267
Redox electrons: Solid Fe
2e-
268
Redox electrons: Sn^2+
2e-
269
Redox electrons: NO2-
2e-
270
Redox electrons: H2O2
2e-
271
Redox electrons: Mo^3+
3e-
272
Redox electrons: Ti^3+
e-
273
Redox electrons: Cr2O7^2-
6e-
274
Redox electrons: U^4+
2e-
275
Redox electrons: Cu+
e-
276
Redox electrons: I2
2e-
277
Redox electrons: S2O3^2-
e-
278
Jones reductor uses
Zn (Amalgam Zn-Hg)
279
Walden reductor uses
Ag in 1M HCl
280
Spectrophotometry formula
1/T=f in Hz
281
Shortest wavelength is
Gamma rays
282
Shortest wavelength has the highest energy, true or false
True
283
Wavelength for bond breaking
Xrays
284
Wavelength for electronic excitation
Ultraviolet
285
Wavelength for vibration
Infrared
286
Wavelength for rotation
Microwave
287
A prism/grating/filter that selects one wavelength
Monochromator
288
Monochromatic means
1 color
289
A fraction of the original light that passes through the sample
Transmittance
290
Transmittance formula
T=P/Po < 1
291
Absorbance formula
A=log (Po/P) = -log T
292
Beer’s law formula
A=Ębc
Ę epsilon molar absorptivity 1/M-cm
b path length in cm
c concentration
293
Part of molecule responsible for light absorption
Chromophore
294
Flat, fused-silica (SiO2) faces
Cuget
295
Electronic states: spins are opposed
Singlet state
296
Electronic states: spins are parallel
Triplet state
297
Vibrational and rotational state of a non-linear molecule
Vibration: 3n-6
Rotation: 3
298
Vibrational and rotational state of a linear molecule
Vibration: 3n-5
Rotation: 2
299
Transition between states with same spin quantum number
Internal conversion
300
Transition between states with different spin quantum number
Intersystem crossing
301
Sensitive enough to observe single molecules
Luminescence
302
Emission of photon during transition with same quantum number
Fluorescence
303
Emission of photon during transition with different quantum number
Phosphorescence
