Studied by 11 peopleED 4 LP 0
Tetrahedral, 109.5, sp3
ED 4 LP 1
Trigonal Pyramidal, <109.5, sp3
ED 4 LP 2
Bent, <<109.5, sp3
ED 3 LP 0
Trigonal Planar, 120, sp2
ED 3 LP 1
Bent, <120, sp2
ED 2 LP 0
Linear, 180, sp
ED 6 LP 0
Octahedral, 90, sp3d2
ED 6 LP 1
Square Pyramid, 90, sp3d2
ED 6 LP 2
Square Planer, 90 & 180, sp3d2
ED 5 LP 0
Trignoal Bipyramidal, 120 & 90, sp3d
ED 5 LP 1
See Saw, 180 & 120 sp3d
ED 5 LP 2
T-Shaped, 180 & 90, sp3d
ED 5 LP 3
Linear, 180, sp3d
Alkali Metals Soluble?
Yes, Except some Li+ compounds
Ammonium Soluble?
Yes
Nitrates Soluble?
Yes
Sulfates Soluble?
Yes, Except compounds with Pb, Ag, Hg, Ca, Ba, Sr
Halogens Soluble?
Yes, Except compounds with Pb, Ag, Hg
Carbonates Soluble?
No, Except when with an alkali metal or ammonium
Phosphates Soluble?
No, Except when with an alkali metal or ammonium
Sulfides Soluble?
No, Except when with an alkali metal or ammonium
Hydroxides Soluble?
No, Except when with an alkali metal or ammonium
Chromates Soluble?
No, Except when with an alkali metal or ammonium
Atomic Size Trend
Increase down the Group, Decrease Across the Period
Atomic Radius Trend
Increase down the Group, Decrease Across the Period
Ionic Radius Trend
Increase down the Group, Decrease Across the Period
Ionization Energy Trend
Decrease down the Group, Increase Across the Period
Electron Affinity Trend
Does not change down the group, Decrease across the Period
Eq change when: Add product/reactant?
Eq shift away from added amount
Eq change when: Remove product/reactant?
Eq shift towards removed amount
Eq change when: Remove gaseous product/reactant?
Eq shift towards removed amount
Eq change when: Add gaseous product/reactant?
Eq shift away from added amount
Eq change when: add inert gas to reaction?
No Eq shift/change
Eq change when: Volume is Reduced & Pressure Increase?
Eq shift towards side with Less moles of Gas
Eq change when: Volume Increases & Pressure is reduced
Eq shift towards side with More moles of Gas
Eq change when: Temp is Increased and reaction is Endothermic
Add energy to reactants
Eq change when: Temp is decreased and reaction is Exothermic
Decrease Energy from products
What Intermolecular forces affects polar molecules
Dipole-Dipole
How can you tell if a substance is polar, just by looking at it?
If it’s not symmetrical then it’s polar
When do Hydrogen Bonds occur?
When H bonds with either N, O, F
How can you tell if a molecule has strong LDF (London Dispersion Force)?
If it has more e- then it has stronger LDF & Higher Boiling Point
Place the following intermolecular force bonds in order. From least to greatest strength: Hydrogen bonding, Dipole-Dipole, Ionic/Covalent Bonds, LDF (London Dispersion Force).
LDF < Dipole-Dipole < Hydrogen Bonding < Ionic/Covalent Bonds
What is the difference between Intramolecular forces and Intermolecular forces
An Intramolecular force is a chemical bond in a molecule, where as Intermolecular forces is the bond between two molecules
How many Sigma and/or Pi bonds in a single bond?
One Sigma bond
How many Sigma and/or Pi bonds in a double bond?
One Sigma Bond and One Pi Bond
How many Sigma and/or Pi bonds in a Triple bond?
One Sigma Bond and Two Pi Bonds
What is the electron configuration for As (Not simplified, sorry)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
What are the 6 Strong acids?
HCl, HNO3, HBr, HI, HClO4,H2SO4(Only first H+)
What are the 2 Strong Bases?
NaOH, KOH
Which of the following is a salt? HF, CH3CH2, NH3, KCl
KCl
What is Fluorines oxidation state?
-1
What is oxygens oxidation state?
-2
What is Hydrogens Oxidation state?
+1 in covalent compounds
What are the charges for monatomic ions?
Whatever the charge of the element is
What is the oxidation state for neutral compounds?
0
What is the oxidation state for Ions?
Whatever its charge is
What are all elements oxidation states? (besides the three exceptions)?
0
What is Boyle’s Law?
When Pressure Increases Volume Decreases (P1V1=P2V2)
What is Charles’s Law? (Guy- Lussac’s Law)
Volume Increases as temperature Increases at Constant pressure (V1/T1 = V2/T2)
What is Avogadro’s Law?
Equal volumes of gas at the same temperature and pressure have the same number of particles (V1/n1=V2/n2)
What is the formula for Boyle’s and Charles’s Law combined?
P1V1/T1 = P2V2/T2
What is the Ideal Gas Law?
PV=nRT
What are the 4 ways to calculate Enthalpy?
qlost=qgained (q=mΔTC)
Hess’s Law
ΔHrxn= Products - reactants
ΔHrxn= Bonds Broken - Bonds Made
What is the formula for Bohr’s Model?
ΔE=-2.178×10-18J(1/n2 f - 1/n2 f)
At what range is the Electronegativity a Covalent bond?
0 - 0.5
At what range is the Electronegativity a Polar Covalent bond?
0.5 - 1.5
At what range is the Electronegativity a Ionic Bond?
3.3 and higher
When is something oxidized?
When it loses e- and the charge increases
When is something reduced?
When it gaines e- and the charge decreases
What is Dalton’s Law of partial pressures?
PTotal= P1 + P2 + P3 +……
What is the STP?
1 atm and 273K
What are properties of Ideal gases?
Molecules/atoms:
Have no assumed volume
Have no assumed interactions
What are properties of Real gases?
Molecules/atoms:
Have volume
Have intermolecular interactions
Behave like ideal gases at high temp and low pressure
What did Max Planck say?
Energy is quantized
What did Einstein say?
Light has particle properties
What did de Broglie say?
Mass has wavelength
What did Bohr say?
Electrons move between energy levels to emit light
What did Schrodinger say?
electrons act as waves, wave functions make orbital shapes
What did Heisenberg say?
one cannot know location and momentum of an electron at the same time
What is the Aufbau Principle
You have to fill the lowest energy orbitals first, before moving to the next higher energy level
What is Pauli Exclusion principle?
Each orbital can hold two electrons, at opposite spins
What is Hund’s Rule?
Sublevels of equal energy are filled with unpaired electrons before filling with a paired electron
What are 5 ways to calculate concentration?
Molarity
Molality
Mole Fraction
% by Mass
% by Volume
What is the rate law for the 0th order?
Rate = k
Is the slope of the 0th order - or +?
Slope = -k
What are the units of k for the 0th order?
M/s
What is the rate law for the 1st order?
Rate = k[A]
Is the slope for the 1st order - or +?
Slope = -k
What is the rate law for the 2nd order?
Rate = k[A]2
What is the integrated rate law for the 0th order
[A] =-kt + [Ao]
What is the integrated rate law for the 1st order
ln[A] =-kt + ln[Ao]
What is the integrated rate law for the 2nd order
1/[A] =-kt + 1/[Ao]
Is the slope for the 2nd order - or +?
Slope = +k
What are the units of k for the 1st order?
1/s
What are the units of k for the 2nd order?
1/M s
What is it called when ΔH is +?
Endothermic
What is it called when ΔH is -?
Exothermic
What happens when ΔS is +
more disorder
What happens when ΔS is -
more order
What is it called when ΔG is +
reaction is not spontaneous
Note
Flashcard