Chemistry Flashcards
1
Q
mixture separation technique that separates solids from liquid
A
decantation
2
Q
mixture separation technique that allows to pass through porous medium
A
filtration
3
Q
mixture separation technique that vaporizes liquid and condenses it
A
distillation
4
Q
distillation technique that utilizes narrow difference in boiling point
A
fractional distillation
5
Q
distillation technique that utilizes separation of volatile oils from plants
A
steam distillation
6
Q
mixture separation technique that uses tools like foreceps, sieves and etc
A
mechanical separation
7
Q
mixture separation technique that uses centrifuge
A
centrifugation
8
Q
mixture separation technique that allows substance to be absorb on surface of inert substance
A
chromatography
9
Q
mixture separation technique that utilizes difference in solubility
A
solvent extraction
10
Q
mixture separation technique that extracts gold from ore
A
amalgation
11
Q
mixture separation technique that extracts gold from ore using cyanide
A
cyanidation
12
Q
what are the seven SI units
A
Mass (kg) Length (m) Time (s) Temp (K) Electric current (A) Amount of substance (mole) Luminous Intensity (candela)
13
Q
when was SI units established? the governing body that facilitates that SI systems?
A
1960, general conference of weighs and measures
14
Q
the kilogram and meter standard measurement is based on what object?
A
platinum iridium object
15
Q
Radius of Earth
A
6.371 x 10^6 m
16
Q
distance of 1 light year in meter
A
9.46 x 10^15 m
17
Q
Radius of Moon
A
1.74 x 10^6 m
18
Q
length of one astronomical unit
A
1.5 x 10^11 m
19
Q
one astronomical unit represent what distance?
A
earth to sun
20
Q
distance of earth to moon
A
3.84 x 10^8 m
21
Q
Mass of Earth
A
5.972 x 10^24 kg
22
Q
Mass of Sun
A
2 x 10^30 kg
23
Q
Mass of Universe
A
10^50 kg
24
Q
Mass of Moon
A
7.35 x 10^22 kg
25
1 pound in kg
0.454 kg
26
density of water
1 x 10^3 kg/m^3
27
density of air
1.29 x 10^3 kg/m^3
28
mass of proton is __________ x mass of electron
1836
29
mass of neutron is __________ x mass of electron
1839
30
volume of nucleus is __________ x volume of atom
1/1013
31
diameter of nucleus
1 x 10^-14 m
32
diameter of nucleus is ________ x diameter of atom
1/100,000
33
Important electron facts
JJ thompson
-1.6 x 10^-19 coloumb
1897
34
Important proton facts
Ernest Rutherford
1.6 x 10^-19 coloumb
1911
35
Important neutron facts
James Chadwick
0 coloumb
1932
36
energy of electron
h x freq (in Joules)
| h = 6.626 x 10^-34 (J.s) (Plank's constant)
37
1 eV in joules
1.6 x 10^-19 Joules
38
momentum of electron
h / freq
| h = 6.626 x 10^-34 (J.s) (Plank's constant)
39
Boltzman's constant
k = 1.38 x 10^-23 (J/K)
40
Formula for number of electrons per shell
2 x n^2
| n = energy level
41
Maximum number of electrons in a subshell
```
2 x (2L+1)
L= s(0), p(1), d(2), f(3)
```
42
The four quantum numbers
Principal (n)
Azimutal (L)
Magnetic (M)
Spin (S)
43
Principal quantum number depicts?
energy level (n)
44
Azimutal quantum number depicts?
Magnitude of angular momentum (L)
determines shape
0-s 1-p 2-d 3-f
from 0 to n-1
45
Magnetic quantum number depicts?
```
orientation (M)
defines direction of angular momentum
s = 0
p = -1,0,1
d = -2,-1,0,1,2
f = -3,-2, -1, 0, 1, 2, 3
```
46
Spin quantum number depicts?
Spin (S)
| either positive 1/2 or negative 1/2
47
Another term for either a proton or a neutron?
Nucleon
48
Another term for Electron
Negatron
49
Another term for Hydrogen - 2 Isotope
Deuterium
50
Nucleus of Deuterium
Deutereon
51
Alpha particle Consists of?
Nucleus of Helium (+2 Charge)
52
Beta Particle consists of?
electron
53
What is a Neutrino
- Zero Mass
- Moves @ the speed of light
- coems from a Beta Particle Decay
54
1st Antimatter Particle Discovered?
Positron
55
What is a Positron?
a "positive electron"
56
Another term for Hydrogen - 3 Isotope
Tritium
57
Building blocks of protons and neutrons
Quarks
58
Protons are made up of what quarks?
TWO up quarks, ONE down quark
59
Neutrons are made up of what quarks?
TWO down quarks, ONE up quark
60
Charge of an up quark?
+2/3
61
Charge of a down quark?
-1/3
62
s, p, d, and f are short for?
Sharp, Principal, Diffuse, Fundamental
63
Who discovered quarks? and when?
Murray Gell-Mann, 1968
64
Number that describes the identity of the element?
Atomic no.
65
atomic number is equivalent to the number of ____________ in a non-ion element?
protons and electrons
66
Mass number is equivalent to?
#protons + # neutrons
OR
Atomic# + #neutrons
67
Representative Elements?
```
1A - Alkali Metals
2A - Alkaline Earth Metals
3A - Boron Group
4A - Carbon Group
5A - Nitrogen Group
6A - Chalcogens
7A - Halogens
8A - Noble/Rare Gases
```
68
in the The Group Designation of Representative elements (ex. 1A, 2A, etc.), what do the numbers represent?
the number of valence electrons
| EXCEPT HELIUM
69
How many electrons do transition metals have in their shells?
More than 8 electrons
70
What shells in a transition metal is used for bonding w/ other elements??
the two outermost shells
71
What groups do transition metals belong to?
1B - 7B
72
Elements with full outermost shells
Noble gases
73
Are noble gases monoatomic or diatomic?
Monoatomic
74
the 6 noble gases
```
Helium(2)
Neon(10)
Argon(18)
Krypton(36)
Xenon(54)
Radon(86)
```
75
Atomic Number of all Lanthanides? And how many are there?
57 - 71
| 15 total
76
Other Lanthanide Properties
- AKA rare earth metals/Inner transition metals
- Naturally found in nature
- One of the elements are radioactive
77
Atomic Number of all Actinides? And how many are there?
89 - 103
| 15 total
78
Other Actinide Properties
- Synthetic
| - Mostly Radioactive
79
What century are the elements arranged by atomic mass?
early 19th century
80
the law that states that every 8th element have the same properties?
Law of Octaves
81
Who proposed the Law of Octaves? And When?
John Newlands, 1864
82
Who proposed the Modern Periodic table? and When?
Dmitri Mendeleev & Lothar Meyer, 1869
83
How many elements did the modern periodic table have in 1869?
66 elements
84
Who stated that the atomic number is proportional to the atomic mass? and when?
Henry Mosely
85
What property in the periodic table increases from lower left to upper right?
Non-Metallic Character
Electron Affinity
Ionization Energy
86
What property in the periodic table increases from upper right to lower left?
Atomic Radius
| Metallic Characteristic
87
Ability of atom to gain or lose electron
Metallic Characteristic
88
Energy produced when neutral atom gains an electron to become a negative ion
Electron Affinity
89
Energy required to remove electron from element to produce cation
Ionization Energy
90
Atomic number and molar mass of Hydrogen, Helium and Lithium
```
Hydrogen = 1,1
Helium = 2, 4
Lithium = 3, 6.94
```
91
Atomic number and molar mass of Boron, Carbon and Nitrogen
```
Boron = 5, 10.8
Carbon = 6, 12
Nitrogen = 7, 14
```
92
Atomic number and molar mass of Oxygen, Flourine and Sodium
```
Oxygen = 8, 16
Flourine = 9, 19
Sodium = 11, 23
```
93
Atomic number and molar mass of Aluminum, Silicon and Phosphorous
```
Aluminum = 13, 27
Silicon = 14, 28
Phosphorous = 15, 31
```
94
Atomic number and molar mass of Sulfur, Chlorine and Potassium
```
Sulfur = 16, 32
Chlorine = 17, 35.5
Potassium = 19, 39
```
95
Atomic number and molar mass of Titanium, Iron, Nickel and Copper
```
Titanium = 22, 47.87
Iron = 26, 55.85
Nickel = 28, 58.7
Copper = 29, 63.55
```
96
What is a good estimate for molar mass of any element?
twice of the atomic number
97
Diatomic Gases
H2, O2, N2, F2, Br2, Cl2, I2 , Air
| Have No Fear Of Ice Cold Beer
98
What law states that "every distinct compound has its own definite ratio of masses of its component element"
Law of Definite Proportions
99
Define as the different forms of one element
Allotropes
100
Charge of an anion and cation
```
Anion = negative
Cation = positive
```
101
Chemical formula that shows exact ratio of elements in a compound
Molecular Formula
102
Chemical formula that shows simplest relative ratio of elements in a compound
Empirical Formula
103
How to solve empirical formula?
assume 100g of solution
104
Avogadro's number
in 1 mol = 6.022 x 10^23 particles
105
Mass per one mole substance
molar mass
| 1 u = 1 amu = 1 dalton = 1 g/mol = 1.66 x 10^-27 kg
106
Occurs when nucleus breaks down into smaller particles
Radioactivity
107
Positively charged particles, with the LOWEST energy level that comes from radioactive decay
Alpha Particle
108
Negatively charged particles, that comes from radioactive decay
Beta Particle
109
Neutrally charged particles, with the HIGHEST energy level that comes from radioactive decay
Gamma Particle
110
nuclear reaction that results from two nuclei combining
Fusion
111
nuclear reaction that results from the splitting of the nucleus
Fission
112
Quantitative Analysis between reactants and products
Stoichiometry
113
The compound in a chemical reaction that runs out first
Limiting Reactant
114
The compound that leaves a remainder or residue of that same compound
Excess reagent
115
Gas Law relating Pressure and Temperature
Gay-Lussac's Law
116
Gas Law Relating Pressure and Volume
Boyles Law
117
Gas Law Relating Volume and Temperature
Charle's Law
118
Gas law relating Volume and the amount of substance
Avogadro's Law
119
Law that states that the total pressure in a system is a superposition of the pressures contributed by the individual gases
Dalton's Law of Partial Pressures
| P(sub T) = P1 + P2 + P3 + ...
120
The summation of all Mole fractions for a given compound
1
121
the mole fraction is obtained by:
(#moles of element) / (summation of all #moles of all elements in a compound) :
(n / (n1 + n2+ n3 +...))
OR
(partial Pressure of element in inquiry) / (Summation of all partial pressures, or total pressure) :
(Pn / (P1 +P2+P3+...))
122
The Law that states that the the rate of diffusion/effusion of a particle is inversely proportional to the square root of its molar mass
Graham's Law of Diffusion
123
Formula for Graham's Law of Diffusion
( Ra / Rb ) = sqrt( MMb / MMa)
124
The Difference of diffusion from effusion
Diffusion - Spread out in open space
| Effusion - Escape from membrane/hole
125
Ideal Gas Law
PV = nRT
126
what is 'R' when using liters for volume and atm for pressure?
0.0821 ((L . atm)/(mol . K))
127
what is 'R' when using m^3 for volume and Pascal for pressure?
8.314 ( Joules / (mol . K) )
128
What is Pressure in CGS
dynes/cm^2
129
Formula for Kinetic Energy (in terms of mass and velocity)
KE = 0.5 m V^2
130
'V' is the velocity in the formula for Kinetic energy and is defined as?
Brownian Movement - seemingly random particle movement
131
Formula for Kinetic Energy (in terms of Temperature)
KE = 1.5 K T
| K - Boltzmann's Constant (1.38 x 10^23)
132
It is the most probable speed of a molecule based on the Maxwell-Boltzmann Distribution
Vrms in Kinetic Theory of Gasses
133
Vrms formula in Kinetic Theory of Gasses
Vrms=sqrt((3KT)/m)
K=boltzmann constant
T=Temperature in Kelvin
m=mass of the particle
134
Type of bonding due to the electrostatic attraction of ions
Ionic Bond
135
Bonding that occur due to the sharing of electrons
Covalent Bond
136
Maximizes 8 valence electron when covalent bonding occurs (Except with hydrogen(only 2 VE))
Octet Rule
137
Ability of atoms to attract electrons towards itself
Electronegativity
138
Electronegativity was first recorded by?
Linus Pauling
139
described as when electrons spend more time near the vicinity of one atom
Polar Bonding
140
Process of electrically polarizing a material
Induction
141
The four Intermolecular forces
Dipole-Dipole
Ion-Dipole
London Dispersion
Hydrogen forces
142
Intermolecular force where Negatively polarized portion of one atom is attracted to a positively polarized portion of another atom
Dipole-Dipole Force
143
Intermolecular force where a polarized Ion attracts the oppositely charged portion of a polarized atom
Ion-Dipole Force
144
Intermolecular force where due to the motion of non-polar molecules, causing temporary dipoles. The force is only significant when atoms are close
London Dispersion Force
145
A Dipole-Dipole Force involving Hydrogen
Hydrogen Force
146
A solution that has more solvent than solute
Homogenous mixture
147
Substances that can never be dissolved after mixing
Precipitates
148
Three situations of a solution based on saturation
Saturated
Unsaturated
Supersaturatied
149
The solution's situation wherein solute separates from solvent, forming crystals
Supersaturated
150
the description of a solution when the solvent used is water
Aqueous
151
Two types of Aqueous solutions
Electrolytes - Can facilitate electron flow
| Non-electrolytes - cannot facilitate electron flow
152
process of surrounding a solute with a solvent
Solvation
153
process of surrounding a solute with a solvent, PARTICULARLY WATER
Hydration
154
A figure of merit for concentration that depicts the percentage of mass of a solute compared to the total mass of the solution (and its formula)
% By Mass = (Mass Solute / Mass solution) x 100%
155
A figure of merit for concentration that depicts the amount of substance of a solute in comparison to the Volume of a solution in Liters
Molarity(M) = (Mol Solute)/(Vol. Solution(in Liters))
156
A figure of merit for concentration that depicts the amount of substance of a solute in comparison to the mass of the solvent in kg
Molality(m) = (Mol Solute)/(Kg Solvent(in Kg))
157
Formula used for solving Dilution Problems
(Molality1)(Volume1) = (Molality2)(Volume2)
158
It is a Heterogeneous Mixture - a substance dispersed throughout another substance
Colloid
159
A colloid that have liquid particles dispersed throughout a liquid
Emulsion
160
A colloid that have solid or liquid particles dissolved throughout a gas
Aerosol
161
The effect were if light passes through a colloid, the light disperses throughout it
Tyndall Effect
162
Who defined the definition of an acid and a base?
Svante August Arrhenius
163
Bronsted defines Acids as _____________ and bases as ____________
Acids as Proton donors, bases as Proton Acceptors
164
Acid + Base = Water + Salt
| what do you call this reaction?
Neutralization Reaction
165
What scale measures the power of hydrogen in a substance? and who proposed this scale?
pH Scale, Soren Sorensen
166
Formula for pH value
pH = -log[H+]
| where H+ is the Molarity(M) of the hydrogen Ion with respect to the substance's Volume in liters
167
Formula for pOH Value
pOH = -log[OH-]
| where OH- is the Molarity(M) of the Hydroxide Ion with respect to the substance's Volume in liters
168
The formula that relates the pH and the pOH value
pH + pOH = 14
169
Acid Properties
- Sour
- Blue >>> Red Litmus paper
- Reacts w/ Metals to produce Hydrogen
- Reacts w/ carbonates to produce CO2
- Electrically Conductive (aqueous)
- pH value from 1 to 7 (1 is the highest acidity level, and the lowest basicity level)
170
Base Properties
- Bitter
- Red >>> Blue Litmus paper
- Slippery
- Electrically conductive (aqueous)
- pH value from 7 to 14 (14 is the highest basicity level, and the lowest acidity level)
171
pH value of a neutral substance
pH(neutral) = 7
172
The Breakdown of Sugar
Glycolysis
173
The building of sugars from light, Oxygen, and water
Photosynthesis
174
Two terms synonymous to "Sugar"
Sugar = Carbohydrates = Saccharides
175
Saccharide composed of one sugar molecule
Monosaccharide (ex. Glucose)
176
Saccharide composed of two sugar molecule
Disaccharide (ex. Table Sugar)
177
Saccharide composed of many sugar molecules
Polysaccharide (ex. Starch)
178
Material found in Fat, Steroids, and Wax
Lipids
179
Made of glycerol connected to different fatty acids
Fat
180
Another term for fat
Triglycerides
181
two types of triglycerides
Saturated and unsaturated
182
Building block of all living things
Nucleic Acids
183
DNA stands for?
Deoxyribonucleic Acid
184
Fundamental Building block of Nucleic Acids
Nucleobase
185
The five primary Nucleobases
Uracil, Cytosine, Thymine, Adenine, and Guanine
186
STP Values
273 Kelvin, 1 atm,
187
Volume of 1 mole of gas at STP
22.4 Liters
188
Principle used to solve for chemical reactions
Law of the Conservation of mass
189
GEAS Default Room temperature
T(default) = 20 Celcius
