Chemistry Flashcards
mixture separation technique that separates solids from liquid
decantation
mixture separation technique that allows to pass through porous medium
filtration
mixture separation technique that vaporizes liquid and condenses it
distillation
distillation technique that utilizes narrow difference in boiling point
fractional distillation
distillation technique that utilizes separation of volatile oils from plants
steam distillation
mixture separation technique that uses tools like foreceps, sieves and etc
mechanical separation
mixture separation technique that uses centrifuge
centrifugation
mixture separation technique that allows substance to be absorb on surface of inert substance
chromatography
mixture separation technique that utilizes difference in solubility
solvent extraction
mixture separation technique that extracts gold from ore
amalgation
mixture separation technique that extracts gold from ore using cyanide
cyanidation
what are the seven SI units
Mass (kg) Length (m) Time (s) Temp (K) Electric current (A) Amount of substance (mole) Luminous Intensity (candela)
when was SI units established? the governing body that facilitates that SI systems?
1960, general conference of weighs and measures
the kilogram and meter standard measurement is based on what object?
platinum iridium object
Radius of Earth
6.371 x 10^6 m
distance of 1 light year in meter
9.46 x 10^15 m
Radius of Moon
1.74 x 10^6 m
length of one astronomical unit
1.5 x 10^11 m
one astronomical unit represent what distance?
earth to sun
distance of earth to moon
3.84 x 10^8 m
Mass of Earth
5.972 x 10^24 kg
Mass of Sun
2 x 10^30 kg
Mass of Universe
10^50 kg
Mass of Moon
7.35 x 10^22 kg
1 pound in kg
0.454 kg
density of water
1 x 10^3 kg/m^3
density of air
1.29 x 10^3 kg/m^3
mass of proton is __________ x mass of electron
1836
mass of neutron is __________ x mass of electron
1839
volume of nucleus is __________ x volume of atom
1/1013
diameter of nucleus
1 x 10^-14 m
diameter of nucleus is ________ x diameter of atom
1/100,000
Important electron facts
JJ thompson
-1.6 x 10^-19 coloumb
1897
Important proton facts
Ernest Rutherford
1.6 x 10^-19 coloumb
1911
Important neutron facts
James Chadwick
0 coloumb
1932
energy of electron
h x freq (in Joules)
h = 6.626 x 10^-34 (J.s) (Plank’s constant)
1 eV in joules
1.6 x 10^-19 Joules
momentum of electron
h / freq
h = 6.626 x 10^-34 (J.s) (Plank’s constant)
Boltzman’s constant
k = 1.38 x 10^-23 (J/K)
Formula for number of electrons per shell
2 x n^2
n = energy level
Maximum number of electrons in a subshell
2 x (2L+1) L= s(0), p(1), d(2), f(3)
The four quantum numbers
Principal (n)
Azimutal (L)
Magnetic (M)
Spin (S)
Principal quantum number depicts?
energy level (n)
Azimutal quantum number depicts?
Magnitude of angular momentum (L)
determines shape
0-s 1-p 2-d 3-f
from 0 to n-1
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
Spin quantum number depicts?
Spin (S)
either positive 1/2 or negative 1/2
Another term for either a proton or a neutron?
Nucleon
Another term for Electron
Negatron
Another term for Hydrogen - 2 Isotope
Deuterium
Nucleus of Deuterium
Deutereon
Alpha particle Consists of?
Nucleus of Helium (+2 Charge)
Beta Particle consists of?
electron
What is a Neutrino
- Zero Mass
- Moves @ the speed of light
- coems from a Beta Particle Decay
1st Antimatter Particle Discovered?
Positron
What is a Positron?
a “positive electron”
Another term for Hydrogen - 3 Isotope
Tritium
Building blocks of protons and neutrons
Quarks
Protons are made up of what quarks?
TWO up quarks, ONE down quark
Neutrons are made up of what quarks?
TWO down quarks, ONE up quark
Charge of an up quark?
+2/3
Charge of a down quark?
-1/3
s, p, d, and f are short for?
Sharp, Principal, Diffuse, Fundamental
Who discovered quarks? and when?
Murray Gell-Mann, 1968
Number that describes the identity of the element?
Atomic no.
atomic number is equivalent to the number of ____________ in a non-ion element?
protons and electrons
Mass number is equivalent to?
protons + # neutrons
OR
Atomic# + #neutrons
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
in the The Group Designation of Representative elements (ex. 1A, 2A, etc.), what do the numbers represent?
the number of valence electrons
EXCEPT HELIUM
How many electrons do transition metals have in their shells?
More than 8 electrons
What shells in a transition metal is used for bonding w/ other elements??
the two outermost shells
What groups do transition metals belong to?
1B - 7B
Elements with full outermost shells
Noble gases
Are noble gases monoatomic or diatomic?
Monoatomic
the 6 noble gases
Helium(2) Neon(10) Argon(18) Krypton(36) Xenon(54) Radon(86)
Atomic Number of all Lanthanides? And how many are there?
57 - 71
15 total
Other Lanthanide Properties
- AKA rare earth metals/Inner transition metals
- Naturally found in nature
- One of the elements are radioactive
Atomic Number of all Actinides? And how many are there?
89 - 103
15 total
Other Actinide Properties
- Synthetic
- Mostly Radioactive
What century are the elements arranged by atomic mass?
early 19th century
the law that states that every 8th element have the same properties?
Law of Octaves
Who proposed the Law of Octaves? And When?
John Newlands, 1864
Who proposed the Modern Periodic table? and When?
Dmitri Mendeleev & Lothar Meyer, 1869
How many elements did the modern periodic table have in 1869?
66 elements
Who stated that the atomic number is proportional to the atomic mass? and when?
Henry Mosely
What property in the periodic table increases from lower left to upper right?
Non-Metallic Character
Electron Affinity
Ionization Energy
What property in the periodic table increases from upper right to lower left?
Atomic Radius
Metallic Characteristic
Ability of atom to gain or lose electron
Metallic Characteristic
Energy produced when neutral atom gains an electron to become a negative ion
Electron Affinity
Energy required to remove electron from element to produce cation
Ionization Energy
Atomic number and molar mass of Hydrogen, Helium and Lithium
Hydrogen = 1,1 Helium = 2, 4 Lithium = 3, 6.94
Atomic number and molar mass of Boron, Carbon and Nitrogen
Boron = 5, 10.8 Carbon = 6, 12 Nitrogen = 7, 14
Atomic number and molar mass of Oxygen, Flourine and Sodium
Oxygen = 8, 16 Flourine = 9, 19 Sodium = 11, 23
Atomic number and molar mass of Aluminum, Silicon and Phosphorous
Aluminum = 13, 27 Silicon = 14, 28 Phosphorous = 15, 31
Atomic number and molar mass of Sulfur, Chlorine and Potassium
Sulfur = 16, 32 Chlorine = 17, 35.5 Potassium = 19, 39
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
What is a good estimate for molar mass of any element?
twice of the atomic number
Diatomic Gases
H2, O2, N2, F2, Br2, Cl2, I2 , Air
Have No Fear Of Ice Cold Beer
What law states that “every distinct compound has its own definite ratio of masses of its component element”
Law of Definite Proportions
Define as the different forms of one element
Allotropes
Charge of an anion and cation
Anion = negative Cation = positive
Chemical formula that shows exact ratio of elements in a compound
Molecular Formula
Chemical formula that shows simplest relative ratio of elements in a compound
Empirical Formula
How to solve empirical formula?
assume 100g of solution
Avogadro’s number
in 1 mol = 6.022 x 10^23 particles
Mass per one mole substance
molar mass
1 u = 1 amu = 1 dalton = 1 g/mol = 1.66 x 10^-27 kg
Occurs when nucleus breaks down into smaller particles
Radioactivity
Positively charged particles, with the LOWEST energy level that comes from radioactive decay
Alpha Particle
Negatively charged particles, that comes from radioactive decay
Beta Particle
Neutrally charged particles, with the HIGHEST energy level that comes from radioactive decay
Gamma Particle
nuclear reaction that results from two nuclei combining
Fusion
nuclear reaction that results from the splitting of the nucleus
Fission
Quantitative Analysis between reactants and products
Stoichiometry
The compound in a chemical reaction that runs out first
Limiting Reactant
The compound that leaves a remainder or residue of that same compound
Excess reagent
Gas Law relating Pressure and Temperature
Gay-Lussac’s Law
Gas Law Relating Pressure and Volume
Boyles Law
Gas Law Relating Volume and Temperature
Charle’s Law
Gas law relating Volume and the amount of substance
Avogadro’s Law
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 + …
The summation of all Mole fractions for a given compound
1
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+…))
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
Formula for Graham’s Law of Diffusion
( Ra / Rb ) = sqrt( MMb / MMa)
The Difference of diffusion from effusion
Diffusion - Spread out in open space
Effusion - Escape from membrane/hole
Ideal Gas Law
PV = nRT
what is ‘R’ when using liters for volume and atm for pressure?
0.0821 ((L . atm)/(mol . K))
what is ‘R’ when using m^3 for volume and Pascal for pressure?
8.314 ( Joules / (mol . K) )
What is Pressure in CGS
dynes/cm^2
Formula for Kinetic Energy (in terms of mass and velocity)
KE = 0.5 m V^2
‘V’ is the velocity in the formula for Kinetic energy and is defined as?
Brownian Movement - seemingly random particle movement
Formula for Kinetic Energy (in terms of Temperature)
KE = 1.5 K T
K - Boltzmann’s Constant (1.38 x 10^23)
It is the most probable speed of a molecule based on the Maxwell-Boltzmann Distribution
Vrms in Kinetic Theory of Gasses
Vrms formula in Kinetic Theory of Gasses
Vrms=sqrt((3KT)/m)
K=boltzmann constant
T=Temperature in Kelvin
m=mass of the particle
Type of bonding due to the electrostatic attraction of ions
Ionic Bond
Bonding that occur due to the sharing of electrons
Covalent Bond
Maximizes 8 valence electron when covalent bonding occurs (Except with hydrogen(only 2 VE))
Octet Rule
Ability of atoms to attract electrons towards itself
Electronegativity
Electronegativity was first recorded by?
Linus Pauling
described as when electrons spend more time near the vicinity of one atom
Polar Bonding
Process of electrically polarizing a material
Induction
The four Intermolecular forces
Dipole-Dipole
Ion-Dipole
London Dispersion
Hydrogen forces
Intermolecular force where Negatively polarized portion of one atom is attracted to a positively polarized portion of another atom
Dipole-Dipole Force
Intermolecular force where a polarized Ion attracts the oppositely charged portion of a polarized atom
Ion-Dipole Force
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
A Dipole-Dipole Force involving Hydrogen
Hydrogen Force
A solution that has more solvent than solute
Homogenous mixture
Substances that can never be dissolved after mixing
Precipitates
Three situations of a solution based on saturation
Saturated
Unsaturated
Supersaturatied
The solution’s situation wherein solute separates from solvent, forming crystals
Supersaturated
the description of a solution when the solvent used is water
Aqueous
Two types of Aqueous solutions
Electrolytes - Can facilitate electron flow
Non-electrolytes - cannot facilitate electron flow
process of surrounding a solute with a solvent
Solvation
process of surrounding a solute with a solvent, PARTICULARLY WATER
Hydration
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%
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))
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))
Formula used for solving Dilution Problems
(Molality1)(Volume1) = (Molality2)(Volume2)
It is a Heterogeneous Mixture - a substance dispersed throughout another substance
Colloid
A colloid that have liquid particles dispersed throughout a liquid
Emulsion
A colloid that have solid or liquid particles dissolved throughout a gas
Aerosol
The effect were if light passes through a colloid, the light disperses throughout it
Tyndall Effect
Who defined the definition of an acid and a base?
Svante August Arrhenius
Bronsted defines Acids as _____________ and bases as ____________
Acids as Proton donors, bases as Proton Acceptors
Acid + Base = Water + Salt
what do you call this reaction?
Neutralization Reaction
What scale measures the power of hydrogen in a substance? and who proposed this scale?
pH Scale, Soren Sorensen
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
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
The formula that relates the pH and the pOH value
pH + pOH = 14
Acid Properties
- Sour
- Blue»_space;> 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)
Base Properties
- Bitter
- Red»_space;> Blue Litmus paper
- Slippery
- Electrically conductive (aqueous)
- pH value from 7 to 14 (14 is the highest basicity level, and the lowest acidity level)
pH value of a neutral substance
pH(neutral) = 7
The Breakdown of Sugar
Glycolysis
The building of sugars from light, Oxygen, and water
Photosynthesis
Two terms synonymous to “Sugar”
Sugar = Carbohydrates = Saccharides
Saccharide composed of one sugar molecule
Monosaccharide (ex. Glucose)
Saccharide composed of two sugar molecule
Disaccharide (ex. Table Sugar)
Saccharide composed of many sugar molecules
Polysaccharide (ex. Starch)
Material found in Fat, Steroids, and Wax
Lipids
Made of glycerol connected to different fatty acids
Fat
Another term for fat
Triglycerides
two types of triglycerides
Saturated and unsaturated
Building block of all living things
Nucleic Acids
DNA stands for?
Deoxyribonucleic Acid
Fundamental Building block of Nucleic Acids
Nucleobase
The five primary Nucleobases
Uracil, Cytosine, Thymine, Adenine, and Guanine
STP Values
273 Kelvin, 1 atm,
Volume of 1 mole of gas at STP
22.4 Liters
Principle used to solve for chemical reactions
Law of the Conservation of mass
GEAS Default Room temperature
T(default) = 20 Celcius
