General Chemistry DAT bootcamp
Intermediate vs. Catalyst
I: produced and used up(product then reactant) C: reactant remained unchanged(reactant then product)
For a given substance, arrange the following values from least to greatest in magnitude: I. Enthalpy of sublimation, ∆Hsub II. Enthalpy of fusion, ∆Hfus III. Enthalpy of vaporization, ∆Hvap
II,III,I
solutes would change the water boiling point by the greats amount of moles by
checking how many moles there are and multiplying them by the amount given for each
HCIO3
chloric acid
Gas to liquid
condensation
release heat
condensation and crystallization
To separate a homogeneous mixture of salt water, which of the following pieces of laboratory equipment is necessary?
condenser
Binary Acid Strength
Increases as you go to the right and down the periodic table
A saturated solution of Mg(OH)2 in water has 100g of solid magnesium hydroxide remaining. The addition of a strong acid to this solution would cause which of the following
Increases the number of Mg2+ ions in solution
Ion-Dipole
Intermolecular force between ions and polar substances
What is responsible for molecules boiling points
Intermolecular forces
nonzero dipole moment
Is polar and has lone pairs
Pa
Is the solutions new vapor pressure
Delta S is given in
J
The stronger the acid the higher the
KA
The lower the Kb the higher the
Ka
weak bases equilibrium rate constant
Kb= HA OH/A-
equilibrium constants equation
Kc =[C]c [D]d / [A]a [B]b Which is Kc= Products/reactants
In any ideal gas questions always convert to
L*atm/mol*K
first order reaction
Ln(a) Vertical shrink
The greater the weight the greater the
London dispersion force
Which statement best explains why bromine is a liquid and iodine is a solid at STP?
London dispersion forces increase as molar mass increases
if a molecule just has CH then it has
London forces
Alkali earth metals
Low ionization energy Don't react as violently with water
Molecular Bond
Low melting point, does not conduct electricity.
increasing boiling point leads to
Lower Mass Lower BP
Higher boiling=
Lower Vapor pressure
Calculate the molarity of the solution
M = mol of solute / L of solution
To find boiling point elevation
Make sure the answer is in degrees or kelvin Take the Kb given and divide by molaity and multiply by the mole given
Metals
Metallic appearance High MP Good conductivity
Whichever one has a lower molecular mass will diffuse
More quickly according to daltons gas law
hydrogen bonding
N-H, F-H, P-H bond STRONGEST POLAR
An unknown gas has a density of 0.9 g•L-1 at 273K and 1 atm. Identify the gas.
Ne
If Q is less than Ksp, will precipitate form?
No
Do catalysts affect equilibrium?
No, they only speed up reactions
Which of the following accurately explains why along the same period, a non-metal has a smaller atomic radius than a metal?
Non-metals have a higher effective nuclear charge
Which of the following best describes why H2O has slightly smaller bond angles than CH4?
Oxygen lone pairs repel bonding pair electrons
Dalton's law if partial pressures equation
P total= Pa + Pb + Pc
With gas the density is
P x Molar Mass/ R x T
osmotic pressure (n) equation
PIE=i(n/v)RT
Which of the following best describes the bond character for hydrochloric acid?
Polar covalent
Kp
Pressure equilibrium constant (only gases)
If k is more than 1
Products are favored
Raoult's Law
Psolution = Xsolvent x Psolvent
Qc equation
Qc= B/A
Ideal gas constant is
R= 0.0821 L atm/mol k
Use the molecular geometry of each compound to solve for the bond angle
Trigonal planar is 3 things. 120 deg Bent is 2 things SO2 120 deg Tetrahedral is 4 things 109 deg Linear is 2 things CO2 180 deg Bent is also two things H2O 109 deg
Ground state
Usually diamagnetic Make sure D orbital is at 5
metallic bond
Variable hardness and melting points. Conducts electricity.
Work pressure equation
W=PΔV
highest volatility
Weakest intermolecular forces
London Dispresion Forces
Weakest. Nonpolar All molecules have this
If Q is greater than Ksp, will precipitate form?
Yes, until Q= Ksp
entropy equation
[products]/[reactants]
Radioactive decay by alpha emission involves production of
a He-4 nucleus with the symbol 4he2
pi bond
a bond that is formed when parallel orbitals overlap to share electrons.
weak electrolyte
a compound that dissociates only to a small extent in aqueous solution
common ion effect
a decrease in the solubility of an ionic compound caused by the addition of a common ion
Amphoteric
a description of a substance that can behave as either an acid or a base
Crystallization
a product is precipitated out, then is separated through filtration
strong electrolyte
a solution in which a large portion of the solute exists as ions
catalyst
a substance that speeds up the rate of a chemical reaction by lowering its activation energy
Flourine oxidation number
always -1
Successive ionization energy
amount of energy required to move its first electron
Enthalpy
amount of heat energy a substance contains
Qc is what you get when you measure
amounts of product and reactants in an equilibrium reaction
conjugate base
an acid that has donated a proton or H+. Always replace the hydrogen taken away with a negative charge
increasing the temperature of a liquid will result in
an increase in vapor pressure. a decrease in surface tension
Aqueous ion
an ion dissolved in water
activated complex
an unstable arrangement of atoms that forms momentarily at the peak of the activation-energy barrier
intramolecular forces include
covalent network bonding, metallic bonding, and ion-ion bonding
Chlorine has the highest
electron affinity
All transition metals are more
electronegative than alkali metal
As nuclear charge increases,
electrons are more strongly attracted to the nucleus resulting in a smaller radius
What elements react crazy in presence of oxygen
elements in group 1 and 2
Metals on periodic table
elements on the left side of the periodic table
On a graph if the reactants are lower than the products, then the reaction is
endothermic
Solid--->liquid---> gas
endothermic
breaking bonds (reactants)
endothermic
Bond breaking is an ___ process
endothermic, which means it is POSITIVE
Gibbs free energy
energy available to do work
Wavelength goes up
energy goes down
Electron affinity measures the
energy released when an atom gains an electron.
The greatest magnitude to the least: 1. Enthalpy of fusion 2. Enthalpy of vaporization 3.
enthalpy of sublimation
The atom with the most Molar Mass is the most
entropy
Avogadro's Law
equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
If ΔG = 0, then the process is at
equilibrium.
Surrodings
everything else around it
Gas--->liquid---->solid
exothermic
Making bonds is (products)
exothermic
On a graph if the reactants are higher then the products, then the reaction is
exothermic
Products being at a lower state means that they are
exothermic
elements in the third row (n=3) of the periodic table are capable of
expanding their valence shell and breaking the octet rule.
Osmosis
flow of water from an area of high concentration to a low concentration
Transition metals
form colorfully compounds
Kf stands for
freezing point constant
The energy of a photon is directly proportional to what
frequency
The energy of a photon is directly proportional to which of the following?
frequency
Noble gasses already have a
full octet
Melting is the same as
fusion
Solid to liquid is
fusion
reduction
gain of electrons
If the element has a negative on top it did not have before then it has
gained electrons
Most substance exit as a ______________ at lower pressure
gas
Pressure is caused by
gas molecules hitting the side of a container
Deposition
gas to solid
As temperature goes up gases
gases solubility goes down
As pressure goes up
gases solubility goes up
Atom sizes get smaller as you
go right across a row and up on a column
The electrons electron affinity increases as we
go up and right toward CI
as s goes up, the disorder of substance
goes up, movement gos up
weak acid and strong base ph level is
greater than 7
transition metals
groups 3-12 (D Block)- Have multiple oxidation states, and form colorful compounds.
If we remove volume the equation will shift to whichever side
has less moleclues
If we add volume the equation will shift to whichever side
has more molecules
Viscosity in liquids
has stronger intermolecular forces at low temp
weak acids and weak bases
have arrows that point both ways
Enthalpy (ΔH) refers to
heat energy.
Ionic Solids
held together by the strong attarction between cations and anions.
Noble gases are
high ionization energy Low electron affinity Have a full ocetet so they dont need to lose or gain electrons
A real gas is most likely to exhibit ideal gas behavior under which of the following conditions?
high temp and low pressure
higher intermolecular forces lead to....
higher boiling point higher heat of vaporization higher viscosity higher surface tensions lower vapor pressure
The higher the entropy
higher disorder
The higher the charge of an atom the
higher its melting point will be
the ∆Hvap for a given substance is always significantly
higher than its ∆Hfus.
intramolecular forces
hold atoms together in a molecule
while decreasing/increasing temperature only results in
horizontal movement of the substance.
Binary acids are composed of
hydrogen and a nonmetal
If H is bonded to N, O, or F then it has
hydrogen bonding
wavelength and energy relationship
inversely proportional
Intermolecular forces include
ion-dipole, hydrogen bonding, dipole-dipole, and London forces
Spector ions
ions that do not participate in a reaction
electrolyte
is an ion in water
Beta emission
is the emission of a beta particle (a high-speed electron). It would result in one of the atom's neutrons becoming a proton.
Xa
is the percentage of solvents in the new solution
Chemical Kinetics
is the study of how fast reactions occur
P pure
is the vapor pressure of the original solvent when it is pure
Erlenmeyer flask
is used for the transfer of liquids, mixture of liquids, or for reactions - but is not accurate and should not be used for measurements.
buret
is used for the transfer of very precise amounts of liquid - primarily in titrations to deliver specific, precise amounts of the titrant.
Because they have the same number of electrons, they are
isoelectronic
If Q is smaller than K
it has not yet reached equilibrium, and needs to go forward
activation energy
it is between products and reactants, not temperature.
Delta H is given in
kJ
Second order
l(a) Vertical shrink
Water molecules in an aqueous solution will have the strongest interactions with ions with which of the following characteristics?
large charge and small size
Larger the charges
larger lattice energy
Shorter bond distance
larger lattice energy
Each successive ionization energy is actually
larger than its previous one
For exothermic reactions the Ea reverse is
larger than the Ea forward
The one that has the least protons is the
largest
Atoms get larger as you go
left down the row, or down the column
Acids get stronger as you
left to right
Acids get stronger as you go
left to right
As pH increases
less acidic
Higher elevations means there is
less atmospheric pressure
unsaturated solution
less solute than a saturated solution
weak base/strong acid ph
less than 7
Oxidizing agent means
like to steal electrons
Water is denser as a
liquid than a solid
Intermediates are more
long-lived than transition states , located between the states
Oxidation
loss of electrons
If the element has a positive on top it did not have before then it has
lost electrons
The higher the vapor pressure
lower boiling point
Lower the mass
lower the boiling point
the ground state of an atom is the state of
lowest energy.
mass percent
mass of solute/mass of solution x 100
calorimetry
measurement of heat flow
For multiplying and dividing, the number of significant figures is determined by the
measurement with the fewest number of significant figures.
mercury manometer
mercury-filled tube used to measure a person's blood pressure
ionic compound are
metal and nonmetal and have a very high melting point
m stands for
molaity
Collison theory
molecules must collide in order to react
molar solubility
moles of products per one mole of products
Molality m
moles of solute/kg of solvent
molarity M
moles of solute/liters of solution
For equilibrium, If pressure is decreased then we shift to whichever side has
more molecules
Create disorder
more positive
super saturated solution
more solute is dissolved in the solvent than would be possible under ordinary conditions.
When water is solid the molecules have
more space between them
A reaction is spontaneous if ΔG is
negative
Exothermic is a
negative
For exothermic reactions, what is the ∆H sign?
negative
more order on the right, then the delta s is
negative
spontaneous
negative delta G
Create order
negative entropy
Nonpolar molecules do not have a
net dipole moment.
HNO3
nitric acid
If Q is less than Ksp
no precipitate forms
ionization energy does not include
noble gasses, only electronegativity does
carbon tetrachloride is
non-polar
Galvanic cells
non-spontaneous
if ΔG > 0, then it is a
non-spontaneous process.
Adding a catalyst to an equilibrium reaction will
not shift to any side
The covalent bond is based on the
number of bonds in a compound
The vant hoff factor increases as the
number of molecules goes up
Emission of light
occurs when an electron drops from a higher to lower energy level. Left to right like N=2 to N=1
HI is stronger than HBr bc
of the bond strength, since HI is lower bond
P1b
osmotic pressure
rate determining step
overall speed of reaction
The one that accepts electrons is called the
oxidant
Nitrogen has more ionization energy than
oxygen
When comparing oxoacids that contain the same central atoms, the strength of the acid increases as the number of ______________ increases.
oxygens
pH equation
pH = -log[H+]
pOH equation
pOH=-log[OH-]
Liquid oxygen (O2) is
paramagnetic
magnetic field is the same as
paramagnetic
HCIO4
perchloric acid
Which of the following pieces of equipment would be best to measure and transfer 8.7 mL of a solution from an Erlenmeyer into a test tube?
pipet
For adding and subtracting, the answer must have the same number of decimal
places as the measurement with the fewest number of decimal places.
non-zero dipole moment
polar
Temporary dipole includes
polar and non polar molecules
The more O-H bonds a molecular has the more
polar it is
Endothermic is a
positive
For endothermic reactions, what is the ∆H sign?
positive
more order on left then the delta S is
positive
nonspontaneous
positive delta G
If Q is greater than Ksp
precipitate will form
volume increases
pressure decreases
osmotic pressure
pressure that must be applied to prevent osmotic movement across a selectively permeable membrane
exothermic heat goes on the
product side
conjugate acid
product that comes from base
colligative properties
properties of a solution that changes as you add more solute
Colligative properties
properties that depend on the concentration of solute particles but not on their identity
A path function is a
property in which the process matters. Path functions depend on the transition or change of the state. Heat and work are examples of path (non-state) functions
A state function is a
property whose value does not depend on how that state was achieved. Enthalpy, volume, mass and Gibbs free energy are all state function
effective nuclear charge
protons ability to suck electrons in
To put elements from smallest to largest you must look at their
protons number
Which of the following scenarios best illustrates Boyle's Law?
pushing a balloon
Calorimetry equation
q = mCAT
bomb calorimeter equation
q=CΔT
An increase in entropy would mean that the reaction will be
spontaneous above a certain temp
If ΔG < 0, it is a
spontaneous process
Graham's law of effusion
states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass
pKa is
strong acid number
If pressure is decreased while the temp is constant, the possibilities are
sublimation
Solid to gas is
sublimation
H2SO4
sulfuric acid
As entropy increases
temperature increases
What can change K
temperature only
The central atom that can most easily accept an electron pair is going to be
the best Lewis acid.
System
the chemical reaction we are examine
The most stable molecular geometry is the one that has
the electrons placed furthest from each other
electron affinity
the energy produced when an atom accepts an electron
nuclear binding energy
the energy released when a nucleus is formed from nucleons
Lattice energy
the energy required to separate an ionic compound cation from its anions
standard states
the enthalpy of formation of any element in its standard state is 0
stronger intermolecular forces
the higher the boiling point and melting point
the higher the force is
the higher the boiling point will be
The stronger the intermolecular force,
the higher the boiling point.
More electrons (anions)
the higher the size
The stronger the intermolecular forces
the higher the surface tension.
the lower temperature
the higher the viscosity
The larger molecules
the larger its dispersion force is
The larger the atomic weight
the larger the MP
The lower the Molar mass
the lower its density
less electrons (cations)
the lower the size
The more carbons and hydrogen a molecule has
the more non-polar it is
Bond order
the number of shared electron pairs between two atoms
bond angle
the one with the most lone pairs is the smallest
If Q is larger than K
the reaction is not at equilibrium, and needs to go in reverse
if you go from the left of equation to right and have less of the molecule then it has
the reaction will have negative entropy
Ideal Gas Law
the relationship PV=nRT, which describes the behavior of an ideal gas
Combined gas law
the relationship between the pressure, volume, and temperature of a fixed amount of gas
Average kinetic energy of gaseous molecules depends on absolute temperature. Because the two gases are at the same temperature, their average kinetic energies are
the same
Transition state (activated complex)
the slowest step in a reaction mechanism (usually the top)
the weaker the acid
the stronger the conjugate base
solute
the substance that is dissolved
boiling point
the temperature at which the vapor pressure of a liquid is just equal to the external pressure on the liquid
The only thing that can change the Keq is changing
the temperature.
Beaker
used for the transfer, mixture, and heating of liquids, or for reactions; however, beakers are not accurate.
Test tube
used for the transfer, mixture, and heating of liquids, or for reactions; however, test tubes are not accurate. A test tube is not volumetric.
formal charge equation
valance electrons -dots - bonds
Boiling point goes up
vapor pressure goes down
Boiling is the same as
vaporization
Decreasing/increasing pressure only results in
vertical movement of the substance
A change in equilibrium is determined by
volume
As pressure goes down
volume goes up
Hydrogen bonding is stronger in liquid state when we talk about
water
Dispersion forces are the
weakest intermolecular forces
If the conjugate base of molecule X has a pKb of 1.4, what would you expect molecule X to be?
weakly acidic
Boiling point
when vapor pressure equals atmospheric pressure
saturated solution
when you add more than what the solution can actually dissolve so you have left over.
trigonal planar
will have three electron domains with no non-bonding electron lone pairs.
-w
work done by the system
+w
work done on the system
temperature is the unit for the
x-axis.
Which of the following is the most likely formed compound between atoms X and Y? Atom X: 1s22s22p63s2 Atom Y: 1s22s22p4
xy
Pressure is the unit for the
y-axis
covalent network solids
Held together by an extended network of covalent bonds
Low Boiling point and __________________ are connected
High vapor pressure
Why do atoms get LARGER as you go down a column
Higher n shell which means larger size
Bent
3 things around central atom
high intermolecular forces
High boiling point The high heat of Vaporization Higher Viscosity Higher surface Tensions Lower Vapor pressure
Equation for % error
(actual - theoretical|/accepted value) x 100
Hydrogen oxidation number
+1
Oxygen oxidation number
-2 except peroxide -1
Any molecules in entropy do not have a state stae rate of
0
The enthalpy formation of a gas (H2) will always be
0
Uncharged elements have an oxidizing number of
0
gamma particle
0 Y 0
Beta Particle
0 e -1
in rate law equation, M and N are usually
0,1,2
Proton Particle
1 H 1
neutron particle
1 N 0
Pressure units
1 atm= 760 torr = 760 mmHg
Simple cubic
1 atom per unit cell
To generate a Net Ionic Equation
1. Balance the chemical equation 2. Use solubility rules to label everything (s), (l), (g), (aq) 3. Cut all the (aq)'s in half, seperating ctions and anions 4. Cancel out all species that are exactly the same on both sides.
In order for a reaction between two molecules to happen, three things must happen
1. Both molecules must collide with each other 2. The molecules need to collide with enough energy for the reaction to happen 3. The molecules need hit each other with the correct three-dimensional orientation
How to determine polarity
1. Draw molecule's Lewis structure, including lone pairs 2. Draw arrows between every atom, going from less EN to more EN in each bond 3. Look at the direction of all the arrows! Are they balanced/unbalanced?
Solubility rules
1. Most ionic compounds that have NO3, CIO4, C2H3O2 and NH4 salts are soluble 2. Most AG,PB,S,OH,Hg,CO and PO are insoluble
collision theory
1. Must collide with 3D orentation 2. molecules must collide in order to react
Oxyacid Strength Trends
1. The more oxygens you have, the more acidic due to resonance (HClO4 > HClO3) 2. If the number of oxygens is the same, the more electronegative heteroatom (increasing strength from going to right and up periodic table), the more acidic
Cal vs cal
1Cal=1000cal
Law of Thermodynamics
1st Law: Energy cannot be created nor destroyed only transferred; 2nd Law: Entropy is constantly increasing in the universe.
body centered cubic
2 atoms per unit cell
Hydrogen and helium only want
2 e-
At STP, 1 mol of any gas is
22.4 L
P block has how many orbitals?
3
alpha particle
4 He 2
face centered cubic
4 atoms
Beryllium only wants
4 e-
H-H
400kj
H-O
450 kj
0=0
500kj
Boron and Aluminum only want
6 e-
Strong acid/strong base ph level is
7
A group is a
A column on the periodic table
state function
A function that depends only on the initial and final states of a system, not on the path in between.
Solution
A homogeneous mixture of two or more substances
Solvent
A liquid substance capable of dissolving other substances
Which of the following liquids would have the highest volatility?
A liquid with London dispersion forces
Entropy
A measure of disorder or randomness.
Disproportionation
A redox reaction in which the same element is both oxidised and reduced
Reducing agent
A reducing agent is oxidized in a chemical reaction. An oxidizing agent is reduced in a chemical reaction.
A period is a
A row on the periodic table
Unsaturated
A solution that contains less than the maximum amount of dissolved solute in a concentration.
AB+CD----->
AD+CB
Arrhenius acid/base
Acid: produces H+ Base: produces OH-
Bronsted-Lowry acid/base
Acid: proton donor Base: proton acceptor
Systems at equilibrium are affected by
Adding or removing reactants Changing temp Changing volume or pressure Adding a catalyst
Which of the following is the best Lewis acid?
AlCl3
Which of the following is true for all transition metals?
All transition metals are more electronegative than alkali metals
Excited state
An atom electron configuration goes up 1
In which instance is a gas most likely to behave ideally?
At high temperatures and low pressures, because the molecules are far apart and not likely to interact.
Which of the following is a characteristic of network covalent solids?
High melting point
Core electrons are
Between 2 and 5 1 and 3 are core electrons
Beryllium has higher ionization energy then
Boron
During a titration experiment, the titrant is placed in which of the following?
Buret
Ionic Bond
High melting point and high boiling point. Also is brittle and hard
network covalent bond
High melting point and high boiling point. Does not conduct electricity and is hard
combustion reaction
CH or O2 resulting in CO2+H2O Or CHO+O resulting in CO2+H2O
Valance electrons is based on the
Column number
Two samples of matter from two different sources are analyzed and have the same mass percent composition of their elements. What can the sample be classified as?
Compound
Which of the following acts as a reducing agent?
Compound that has too many electrons and wants to lose them.
Release of heat is affected by
Condensation and crystallization
Conduction
Heat transfer by direct contact
Delta S vs s
Delta S can be + or - or 0and S can never be 0
Which of the following is NOT a colligative property?
Density
Metal and non-metal
Dipole-Dipole forces
Atomic Radius
Distance from nucleus to outside its outermost orbital
All of the following will affect the rate of an irreversible chemical reaction EXCEPT one. Which is the EXCEPTION? A. Pressure (3%) B. Concentration of reactants (5%) C. Presence of a catalyst (17%) D. Surface area of reactant solid (28%) E. Concentration of products (48%)
E
work function equation
E ejected= E photon- Work function
Radiation
Heat transfer by electromagnetic waves
metallic soilds
Held together by a delocailized sea of shared electrons
What is responsible for the unequal sharing of electrons
Electrongetaivty
Allotropes
Elemental molecules with different formulas
State functions examples
Energy Temp Enthalpy
entropy
Entropy will increase as temperature increases Entropy is a measure of the disorder in a system A spontaneous reaction can produce an increase in entropy The entropy of a gas vessel increases as volume increases
NonPolar
Equal sharing of electrons All carbon hydrogen bonds No lone pairs
Non-polar
Equal sharing of electrons No lone Pairs
∆E = q + w
Equation for ∆E
E° cell =
E° cell reduction + E° cell oxidation
saturated
Fats with the maximum number of hydrogens.
Alkali metals
Group 1- low ionization energies (easy to lose electron from them), form ionic compounds and are VERY REACTIVE WITH WATER
alkaline earth metals
Group 2- low ionization energy, Solid at room temp, not so reactive with water
Oxygen group
Group 6A- A good oxidizing agent, but O3 is even better.
Halogens
Group 7 A- highly electronegative, they also have a high thirst for electrons. HIGHLY REACTIVE WITH METALS Strong oxidizing agents
Noble gases
Group 8A
Nobel Gases
Group 8A- they are unreactive.
Isoelectronic series
Group of elements that all have the same number of electrons
diatomic elements
H2, N2, O2, F2, Cl2, Br2, I2
Polar
Has lone pairs Uneven sharing of electrons
polar
Has lone pairs Uneven sharing of electrons
Alkali Metals
Have the lowest ionization energy React explosively with water Low melting points High conductivity to heat Form soluble ionic compounds
azimuthal quantum number
Second quantum number, designated l. Tells us the shapes of the electron orbitals
Why does a nucleus weigh less than the sum of its neutrons and protons?
Some of the nucleus's mass gets converted into energy to hold the nucleus together
The Lewis definition of acids and bases revolves around electrons pairs
Species that can accept an electron pair are Lewis acids. Species that can donate an electron pair are Lewis bases.
Ones that has a (s) are
Spector ions
Ka decreases
Stronger base
The following are listed from least to greatest magnitude 1. Fusion 2. Vaporization 3._________________
Sublimation
What element produces an egg smell
Sulfur
Percent weight for a molecular formula
Take the mass of the given options and divide it by the total of each given option to get the % weight
Thermondynamics
Tells us if a reaction will even happen, but not how fast it will happen
What equation do we use to calculate activation energy
The Arrhenius Equation
ionization energy
The amount of energy required to remove an electron from an atom It decreases going down and to the right
Bond Length
The distance between nucleus to nucleus (Atomic radius x2, only when they are the same atoms)
Enthalpies of Formation
The h of a chemical reaction forming one mole of a single substance from its parent elements in their standrad states.
London dispersion forces
The intermolecular force between NON-POLAR molecules WeakEST intermolecular forces
Oxacid Trends
The more oxygen, the more acidic the oxacids bc there are more oxygens for the electron to spread
Which of the following statements correctly describes a mole?
The number of atoms in a sample that weighs as much as the element's atomic mass.
Critical point on phase diagram
The pressure/temperature combined by which liquid and gas coexist at the same time
The question tells us that an object releases heat into the surroundings. When heat is transferred from the system to the surroundings, this means that:
The reaction is exothermic q is negative
Boyle law
The relationship between the pressure and volume of a gas at constant temperture; when volume increase, pressure decreases.
Which of the following is true for the energy diagram of a reversible exothermic reaction?
The reverse reaction has a higher activation energy than the forward reaction.
Convection
The transfer of heat by the movement of a fluid
Which of these kinetic molecular theory assumptions is true of ideal gases?
The volume of individual gas molecules is negligible
In order for gas to behave ideally, there are three things it must do..
The volume or size of each individual gas molecule is insignificant Gas molecule's collisions with each other are perfectly elastic The average kinetic energy of a gas depends only on the system's temp.
Dispersion forces
They are the weakest intermolecular force and are present in all molecules, including individual atoms
dipole-dipole forces
They have an unequal sharing of electrons Metal and non metal C-O or C-H POLAR
Ka increases
acid strength increases
lewis acid/base
acid: electron pair acceptor base: electron pair donor
As pKa decreases
acidity increases
As ph decreases
acidity increases
Delta E
activation energy
Amphoteric
acts as an acid or a base
Calculating Ksp would mean to
add the given Ksp into the X
overall reaction
add up the elementary steps and cancel out the intermediates
Why does freezing point depression occur?
adding solute disrupts bonding, therefore lowers the freezing point
The most common examples are elements that break the octet rule
are phosphorus, sulfur, and chlorine.
Intermediates
are produced in the middle of the reaction and get used up before the end
Be electron affinity is
around zero
Nitrogen electron affinity is
around zero, because it does not want to lose or gain an electron.
zero
at equilibrium
Gamma decay will not change the
atomic number
realative abundance
avg atomic mass= (% of isotope 1 x atomic mass of 1)+(% of isotope 2 x atomic mass 2)
How do catalysts lower a reactions activation energy
by providing an alternative pathway between reactants and products
Why do atoms get SMALLER as you go across a period from left to right?
bc they do not have any charge shells, they just have more protons, which suck electrons in making them smaller.
Why do pure elemental gases such as O2 and N2 have very low melting points, around -220 °C?
because pure gases are purley covalently bonded and are nonpolar
Weak intermolecular forces lead to a low
boiling point
as molecular weight increases
boiling point increases
Covalent bonds depend on how many
bonds are in a compound
HCI and NAOH both cant form a
buffer solution
Why does N2 have a triple covalent bond whereas O2 only has a double covalent bond
by having 5 valence electrons, nitrogen fills its ocet by sharing 3 bonding pairs of electrons
The intermediate in an elemnetry step is the one that
cancels out on both sides of equation
soluble
capable of being dissolved
Gases volume can
change considerably
ΔE is equal to the
change in energy
Delta H is
change in enthalpy
Delta G
change in free energy reaction is at 0 equilibrium under all conditions
delta G with degree sign
change in gibbs free energy under standard condition
Any atom that has a charge has an oxidating number equal to itrs
charge
Atoms that have a charge will have the oxidation number of the
charge
Adding more H2O will
decrease
Increasing volume will
decrease in pressure
The largest amount of van't Hoff factor would be the one that
decreases the water
SO3 has the highest mass and the highest
density
Amphiprotic
describes a substance that can act as both a proton acceptor and donor
liquid nitrogen (N2) is
diamagnetic and slightly repelled by magnets
If there is an atom binded to something different than C or H then it is
dipole dipole forces
Adding an inert gas that are not in the reaction
do not cause a shift at all
Gamma decay
does not result in any change in the number of protons or neutrons of an emitted particle.
Triple bonds are shorter than
double bonds
Acids increases as you go
down a column
Aids imcreases as you go
down a column
Atomic size increases going
down a column because of adding electron shells and electron shielding
Le Chatelier's Principle
if a system at equilibrium is disturbed, then it will shift in whichever direction it has to, to restore equilibrium
Transition metals represent all elements
in the d-block of the periodic table (shaded blue)
A decrease in volume leads to a
increase in rate
As pKb decreases, base strength
increases
As pressure of the gas increases, the solubility of the gas
increases
As temperature of the solution decreases, the solubility of the gas
increases
increasing temp
increases product side which shifts the reactant forward
Atomic radius
increases towards the bottom left of the periodic table.
For isoelectronic ions, ionic radius
increases with decreasing atomic number.
Vapor pressure of a liquid increases as temperature
increases.
Nobel gasses are
inert and as stable as they come
solid is
insoluble
Viscosity is dependent on
intermolecular forces
density is not related to
intermolecular forces
Which of the following classes of electromagnetic radiation has the longest wavelength?
radio waves
Products do not appear in
rate law equations
Being at equilibrium only means that the
rates are equal
capture
reactant
Rate law is only
reactants
If K is less than 1
reactants are favored
If Q equals K
reaction is at equilibrium
dynamic equilibrium
reactions with two-way arrows (does not mean we have the same stuff on both sides)
The one that gives electrons away is called the
reductant
Electron capture
results in a proton converting into a neutron in the emitted particle. By decreasing the number of protons and increasing the number of neutrons
Alpha decay
results in an emitted particle with a reduced mass and atomic number and emission of an alpha particle (also called a helium nucleus) consisting of 2 protons and 2 neutrons.
Positron emission
results in the emission of a positron which will convert a proton to a neutron in the emitted particle.
isotope
same number of protons, different number of neutrons
Boiling point is lower at
sea level
Voltaic cells
spontaneous
Filtration
separates a solid from a liquid
decanation
separates liquids from solids by pourinh liquid carefully off the top
distillation
separates miscible liquids
crystalline
sharp,well defined melting temp
If Q is less than Kc,
shift equilibrium right
Increasing temp will increase product side which will
shift forward reactant
if Q is bigger than Kc
shift left
Highest energy has the
shortest wavelength
rate-determining step
slowest step, one that takes the longest and slowest
Its more difficult to remove an electron when the atom is
smaller
larger Ka
smaller pKa stronger acid
larger Kb
smaller pKb, stronger base
More protons more attraction to electron which is
smaller size atom
For endothermic reactions the Ea reverse is
smaller than the Ea forward
The one that has the most protons is the
smallest
The compound with the most lone pairs is the one that is the
smallest, as far as bond length
Molecular solids
solids that are composed of molecules
As Ksp goes up
solubility goes up
As the tempertaure goes up
solubility goes up
(aq) is what?
soluble
Insoluble and soluble bonded together then they will be
soluble
Miscible
soluble
As Ph goes up
solution becomes less acidic
As Ph goes down
solution becomes more acidic
As soluble goes up and boiling point as well
the vapor pressure will go down
The larger the atom, the further away they will be from each other and
the weaker the bond will be
An ideal gas is a
theoretical gas whose behavior who can be perfectly predicted by the ideal gas law
Electronegativity and ionization are the same because
they both increase as you go right and up on periodic table
When alkali metal react with water
they form a metal hydroxide and a hydrogen gas
Nobel gasses do not go through electron affinity because
they have a full octet they do not need anymore electrons
why can transition metals form brightly colored compounds
they have an unfilled D orbital
A trigonal planar geometry will have
three areas of electron bonding pairs with no non-bonding electron lone pairs.
emit
to give off/product side
q is equal to the
transfer of heat
Molecular compounds are usually
two or more nonmetals
Dissolving a liquid causes the liquid boiling point to go
up
As energy goes up, frequency goes
up and wavelength goes down
Electron affinity increases as you go
up in a group and right in a period.
Energy level space decreases as you go
up. Further away from nucleus
A pipet
used for the measurement and transfer of very precise amounts of liquid
nuclear decay
you take the given element and subtract it by what it is asking for, then you go to table ad find that element you get.
molten electrolysis
• there is no salt bridge • electrons always flow from anode to cathode • CATions flow towards the CAThode to get reduced • ANions flow towards the ANode to get oxidized
Aqueous Electrolysis
• under aqueous conditions you have two competing reactions (ex: reaction of KI and reaction of water) • need to use a table of reduction potentials to find which one will happen more easily
