Inorganic Chemistry Flashcards
(145 cards)
1
Q
Who developed the atomic Theory
A
John Dalton
2
Q
What is the charge of the electron?
A
-1.6x10^19 C (Robert Millikan)
3
Q
Established the particle character of cathode rays
A
George Johnstone Stoney
4
Q
Established the raisin bread model as a theory of atomic structure
A
J.J. Thompson
5
Q
Who discovered that electricity can decompose compounds?
A
Michael Faraday
6
Q
Performed an experiment on cathode rays and detected the presence of ions
A
Eugen Goldstein
7
Q
Introduced the nuclear model of the atom, used a gold sheet; positive charge in a small region called nucleus
A
Ernest Rutherford
8
Q
Discovered the neutron
A
James Chadwick
9
Q
What is the charge of a proton?
A
1.602x10^19 C
10
Q
Significant observation in chemical periodicity; named groups in triads
A
Johan Wolfgang Dobreiner
11
Q
suggested the law of octaves
A
John Newlands
12
Q
Published an independent version of the periodic system; organized in increasing atomic weights
A
Dmitri Ivanovich Mendeleev
13
Q
Established the modern periodic table
A
Henry Mosely
14
Q
Groups that belong to s/p blocks
A
Group 1A-8A
Alkali metals (except hydrogen)
Alkali earth metals
Aluminum
Carbon
Nitrogen
Oxygen
Halogens
Noble or Inert gasses
15
Q
The transition elements belong to the ___-block
A
d-block
16
Q
Inner transition elements belong to the f-block which consists of ______ and ______
A
lanthanide (4f)
actinide (5f)
17
Q
Periodic Trends that: (2)
L-R : Decrease
T-B : Increase
A
Atomic Radius
Metallicty
18
Q
Periodic Trends that: (3)
L-R : Increase
T-B : Decrease
A
Electronegativity
Ionization Energy
Electron Affinity
19
Q
Qualities that describe the outside appearance of matter
A
Extrinsic properties
20
Q
depend on the kind of material itself
A
Intrinsic Properties
21
Q
Depend on the amount of matter present
A
Extensive Properties
22
Q
Do not depend on the amount of substance present
A
Intensive properties
23
Q
structure that is not orderly, melting point is not determined
A
amorphous solids
24
Q
Viscosity Trends = higher or lower?
Temp
Pressure
IMF
A
higher temp = lower viscosity
higher pressure = higher v
stronger IMF = higher V
25
Vapor pressure trends = higher or lower?
Temp
Pressure
IMF
higher temp = higher vapor pressure
higher IMF = lower VP
higher VP = lower boiling point
26
Vapor pressure of a liquid is equal to the external pressure on its surface
Boiling point
27
when electrons are shared there is a _____ bond between the compounds
Covalent
28
an _____ bond is formed when non-metals and metals bond together because of a difference in electronegativity
ionic bond
29
A physical combination of two or more distinct chemical substances
Mixture
30
A phenomenon wherein a characteristic of suspensions and colloids is their ability to scatter light when passing through a mixture
Tyndall effect
31
Suspensions have a particle size larger than ______
200nm
32
Colloids particle size are between ________
1-200nm
33
The mixture or solution is heated into a vapor and condensed
Distillation
34
reduction ____ electrons & hydrogen
oxidation ______ electrons & hydrogen
reduction = gains
oxidation = release
35
acids: hydrogen ion donor
bases: hydroxide (-OH) donor
Arrhenius theory
36
acids: proton donor
bases: proton acceptor
Bronsted-Lowry theory
37
acids: electron pair acceptor
bases: electron pair donor
Lewis theory
38
SI unit of energy
Joule
39
1 joule = ___ kg m^2/s^2
1
40
1 cal = ____ J
1 cal = 4.184J
41
KeQ = equilibrium constant formula
Keq = (products)^x / (reactants)^y
42
states that "when a system is in equilibrium, the equilibrium shifts so as to undo, in part, the effect of disturbance"
Le Chatelier's principle
43
atoms containing radionuclides
radioisotope
44
particles are helium atoms
alpha emission
45
particles are electrons (0-e)
increase in atomic number
beta emission
46
no change in atomic number or mass since rays are uncharged
gamma emission
47
(01e) decrease in atomic number
positron emission
48
inner shell electron is captured by the nucleus
decrease in atomic number
electron capture
49
splitting of heavy nuclei
nuclear fission
50
union of light nuclei
nuclear fusion
51
solutions are ____ mixtures
homogenous
52
two types of heterogenous mixtures are
colloids
suspensions
53
elements that have the same number of neutrons but have different number of protons
isotones
54
elements that have the same atomic number but different atomic mass number
isotopes
55
percent composition formula
percent composition = (molar mass of element / total molar mass of a compound) x100
56
MC molecular geometry on NMAT
Linear:
Tetrahedral:
Bent:
Linear: CO2
Tetrahedral: CH4 (methane)
Bent:H2O, SO4
57
BF3 geometry
trigonal planar
58
Compounds with tetrahedral arrangement (3)
CH4 (methane)
NH3 (ammonia)
H20 (bent)
59
Compounds with trigonal bypyramidal geometry (4)
PCl5 (phosphorus pentachloride)
SF4 (sulfur tetrafluoride)
ClF3 (Chlorine trifluoride)
I3- (triiodide)
60
Compounds with octahedral arrangement (3)
SF6 (Sulfur hexafluoride)
BrF5 (bromine pentafluoride)
XeF4 (xenon tetrafluoride)
61
orbital size and energy level
principal quantum number (n)
62
orbital shape
angular momentum (l)
63
orbital orientation
magnetic quantum number (ml)
64
electron spin direction
spin (ms)
65
Electrons will fill the lowest energy level first
Aufbau principle
66
no two electrons within an atomy should have an identical set of all four quantum numbers
Pauli Exclusion principle
67
electrons will occupy all empty orbitals in a subshell with single electrons having parallel spins before entering half-filled orbitals
Hund’s Rule
68
angular momentum
s
p
d
f
angular momentum
s = 0
p = 1
d = 2
f = 3
69
maximum electron number
s
p
d
f
maximum electron number (half will be the shell or orbital number)
s = 2
p = 6
d = 10
f = 14
70
ml (orientation)
s
p
d
f
ml (orientation)
s = 0
p = -1, 0, 1
d = -2, -1, 0, 1, 2
f = -3, -2, -1, 0, 1, 2, 3
71
the s orbital has a _____ shape
the p orbital has a ______ shape
s = sphere
p = dumbell
72
the valence electron can be determined according to the ______ of the element
group number
73
the more electronegative element gains an electron
reduction
74
the less electronegative element loses an electron
oxidation
75
bond between non-metal and non-metal
covalent bond
76
bond between non-metal and metal
an electron is taken by the more electronegative participant
ionic bonds
77
______ bonds are formed by fluorine, oxygen or nitrogen
hydrogen bonds
78
_____ bonds form a sea of electrons
metallic bonds
79
Electrons not equally shared
One part of molecule is more negative or positive
Polar molecules
80
Electrons equally shared
No one part of molecule is more negative or positive
Non-polar molecules
81
Polar Molecules ____
Non-Polar molecules ____
A. hydrophobic
B. hydrophilic
Polar Molecules: HYDROPHILIC
Non-Polar molecules HYDROPHOBIC
82
metal cations to delocalized electrons
metallic bonds
83
cations to anions
ionic bond
84
partially charged cation to partially charged anion
polar covalent bonds
85
nuclei to shared electrons
non polar covalent bonds
86
partially oppositely charged ions
dipole-dipole attraction
87
weakest intermolecular forces of attraction
london dispersion attraction
88
greater molecular weight = _______ london dispersion forces
higher
89
higher boiling point = _______ vapor pressure
higher boiling point = lower vapor pressure
90
higher boiling point =
higher: (3)
lower: (2)
higher boiling point =
higher: (3) IMF, MW, surface area
lower: (2) branching, VP
91
2 or more simpler substances (elements) combine to give a compound
Synthesis
92
Compound is broken down into simpler substances (elements)
Decomposition
93
Atom or group of atoms is replaced by another atom or group
A + BC = AC + B or AB + C
Single Replacement
94
Solid compound is formed
2 soluble compounds are mixed
AB+ CD = AD + BC
Double Replacement
95
Reaction between hydrocarbon and oxygen to produce carbon dioxide, water and heat.
An exothermic reaction
Combustion
96
An acid reacts with a base to produce salt and water
HA + BOH --> H2O + BA
Neutralization
97
Electron transfer occurs
Reduction-Oxidation
98
an oxidizing agent = _____ electrons
an oxidizing agent = gains electrons
99
a reducing agent ______ electrons
a reducing agent loses electrons
100
True or False
there are no attractive or repulsive forces between particles of real gases
False
there are no attractive or repulsive forces between particles of Ideal gases
101
Real gases have ____ volume whereas ideal gases have ____ volume
Real gases have small volume whereas ideal gases have no volume
102
real gases = _____ collision
ideal gases = ______ collision
real gases = inelastic collision
ideal gases = elastic collision
103
volume is _______ proportional to pressure
volume is inversely proportional to pressure
high V = low P
low V = high P
104
volume is directly proportional to ______ and _______
temp and number of moles
105
Ideal Gas law formula
PV = nRT
106
Combined gas law formula
P1V1/T1 = P2V2/T2
107
At constant V, as pressure increases, temperature increases
Gay-Lussac's law
108
Gay-Lussac's law formula
P1/T1 = P2/T2
109
At constant P, as volume increases, temp increases
Charles Law
110
Charles Law Formula
V1/T1 = V2/T2
111
At constant T, as pressure increases, volume decreases
Boyles Law
112
Boyle's Law formula
P1V1=P2V2
113
How many steps are there to convert mol to mol
1 step (mol of A to mol of B)
114
How many steps are there to convert mol to grams?
2 steps (mol A --> mol B --> gB)
115
How many steps are there to convert grams to mol?
2 steps (gA --> mol A --> mol B)
116
How many steps are there to convert grams to grams?
3 steps (gA --> mol A --> mol B --> gB)
117
What is the first step in limiting and excess reactants?
identify ER and LR (divide total number of mols by mols in balanced equation or do mol to gram conversions with product)
118
How to compute for excess reactants?
Total reacted - theoretical reacted = leftover
119
Formula of percent yield
%yield = A/T x 100
120
measurement of randomness of molecules
Entropy (∆S)
121
amount of heat evolved or absorbed in a reaction carried out at constant pressure
Enthalpy (ΔH)
122
First Law of Thermodynamics
Energy can never be created or destroyed
Energy can only be converted from one form into another
123
Second Law of Thermodynamics
Total entropy of the universe always increases
Every spontaneous change is accompanied by an increase in entropy
124
Third Law of Thermodynamics
At absolute zero, the entropy of a perfect crystalline substance may be taken as zero
125
Exothermic or Endothermic?
Formation of products is more favorable
Formation of reactants is more favorable
Formation of products is more favorable - Exothermic
Formation of reactants is more favorable - Endothermic
126
Reaction is spontaneous
Exothermic reaction
127
Reaction is not spontaneous
Energy absorbed
Endothermic reaction
128
The relationship between heat energy and temperature is different for every material, and the ___________ is a value that describes how they relate.
specific heat
129
formula for heat
Q = mcΔT
130
free energy change for a reaction
Gibbs free energy (ΔG)
131
reaction that favors the formation of products at the conditions under which the reaction is occurring
Spontaneous reaction
132
reaction that does not favor the formation of products at the given set of conditions
Nonspontaneous reaction:
133
formula for change in Gibb's free energy
ΔG = ΔH - TΔS
134
ΔG < 0
exergenic
135
Solution with solute that dissolves until it is unable to dissolve anymore
Leaves undissolved substances at the bottom
Saturated Solution
136
Less solute than the saturated solution
Solution completely dissolves
No remaining substances
Unsaturated Solution
137
Has more undissolved solute than the saturated solution Tendency to crystallize and precipitate
Supersaturated Solution
138
acids turn litmus paper from ____ to _____
blue to red
139
Molarity formula
M = moles of solute / liters of solution
140
Molality formula
m = moles of solute / kg solvent
141
normality formula
N = #H+ or OH- /L of solution
142
Mass percent solution
mass solute / mass of solution x100
143
mole fraction
moles of solute/moles of solution
144
Rate Law Formula
(Concentration)F - (Concentration)I / change in time
145
Chemical Equilibrium Formula
Kc = (C)^c (D)^d / (A)^ab (B)^b
