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TSNF Masterlist
All units
| Question/Term/Statement | Answer/Definition/Blank |
|---|---|
| Combustion reaction always produces _____ and _____. | CO2 and H2O |
| Ionic bonds are formed when? | metal transfers electrons to non-metal, opposite charges attract |
| Covalent bonds are formed when? | two non metals share electrons |
| Substitutional Alloy | radii of metals are similar in size, and replace each other in crystal lattice |
| Metallic Bonds | between metals, always conduct electricity |
| Lewis Diagram | obey octet, then formal charge, extra electrons on larger central atom, if too few atoms then make double or triple bonds |
| Formal Charge Equation | valence electrons-# of lone pair electrons-# of bonds |
| Lattice Energy | energy to break ionic bond |
| Single Bond | Only Sigma bond |
| Double Bond | Sigma and Pi bond |
| Triple Bond | Sigma and 2 Pi bonds |
| Molecule Asymmetrical | has net dipole moment, polar |
| Molecule Symmetrical | no net dipole moment, non-polar |
| Lattice Energy Decreases | charge decreases, radii increases |
| Interstitial Alloy | smaller atom fits in gaps between larger atom, less dense |
| Bond Order | total # of bonds around central atom/# of atoms around central atom |
| Formal Charge | # of v.e an atom has compared to number of electrons around it in Lewis Diagram |
| When do trailing zeros count as sig figs? | when there is a decimal point present |
| Do leading zeros ever count as significant? | no |
| Atomic Number | # of protons in nucleus |
| Mass Number | protons + neutrons |
| Anions compared to their Atoms | larger, adding electrons increases e-e repulsion |
| Cations compared to their Atoms | smaller, removing v.e that are farther from nucleus |
| What do elements in the same group share? | similar chemical and physical properties |
| What do mass spectroscopy graphs measure? | atomic masses of isotopes |
| Isotopes | same element, different number of neutrons |
| Isoelectronic Species | atoms and ions with same number of electrons |
| Where are metals on the Periodic Table? | left side of zig-zag line |
| What are the diatomic elements? | hydrogen, nitrogen, oxygen, flourine, chlorine, iodine, bromine |
| Where are the least reactive elements? | Group 18, noble gases |
| Where are the most reactive metals? | Groups 1 + 2, alkali and alkaline earth metals |
| Where are the most reactive nonmetals? | Group 17, halogens |
| Where are nonmetals on the Periodic Table? | right side of zig-zag line |
| Down a group on the Periodic table | nuclear charge increases, radii increases, ionization energy decreases |
| Across a period on the Periodic table | nuclear charge increases, radii decreases, ionization energy increases |
| When an electron is further away from the nucleus, it has ____________ Coulombic attraction | less |
| When an electron is in a higher energy level, it is __________ the nucleus | further away from |
| Carbon must have ____ bonds in organic structural formulas | 4 |
| Solving for Limiting Reactant | grams to moles, divide by coefficient, smallest number is limiting reactant |
| When writing electron configuration for cation... | remove valence electrons first |
| after 3p6? | 4s2 3d10 4p6 |
| PES graph, the larger the binding energy __________ | the closer the electrons are to the nucleus |
| PES graph, the higher the peak ______ | the more electrons |
| Coulombs Law, greater the ionic charge | greater the force |
| Coulombs Law, greater the distance | lower the charge |
| Compounds | pure substance made of two of more elements bonded in a fixed ratio |
| Mixture | two or more substances, unevenly distributed, and each retaining its own identity |
| Particle diagrams must always ___________. | obey the Law of Conservation of Matter |
| 4 domains (bond angle) | Bond Angle of 109.5 degrees |
| The greater the EN difference between 2 covalently bonded atoms, ______. | the more polar the bond |
| 4 domains (hybrid orbitals) | sp3 |
| 3 domains (bond angle) | Bond Angle of 120 degrees |
| 2 domains (bond angle) | Bond Angle of 180 degrees |
| 3 domains (hybrid orbitals) | sp2 |
| Lattice Energy Increases | charge increases, radii decreases |
| 2 domains (hybrid orbitals) | sp |
| When drawing Lewis Diagrams, always _____________ | obey the Octet rule |
| Non-Polar Justification | symmetrical, all dipoles cancel |
| Criteria for Non-polar molecules | if there are lone pairs, must be linear or square planar + all atoms around central atom are the same |
| Linear Molecule | 2 atoms, 3 or 4 lone atoms |
| Covalent Network Solids (composition) | carbons (diamonds) or non-metal and metalloids |
| Polar Justification | asymmetrical, dipoles do not cancel |
| Ionic Solids (composition) | nonmetal-metal (lattice structure, alternating cations and anions) |
| Metallic Solids (composition) | atoms of same metal, free flowing electrons |
| H-bonds | FON |
| dipole-dipole forces get _______ as the molecule is more _______ | stronger, polar |
| All polar molecules contain _______ forces | dipole-dipole |
| Covalent Network Solids (properties) | very high melting/boiling points, poor conductors of electricity |
| Ionic Solids (properties) | high melting/boiling points, don't conduct as solid, do conduct as liquid |
| Molecular Solids (properties) | low melting/boiling points, do not conduct electricity |
| Metallic Solids (properties) | variable melting/boiling points, malleable, good conductors |
| Molecular Solids (compostition) | nonmetals-nonmetals (only one with IMFs) |
| Boiling point and Melting point increase | IMF increase |
| Polarizability | ease at which electron cloud is distorted |
| Larger electron coud = more electrons = | more polarizable |
| IMF's (weakest to strongest) | London Dispersion, dipole-dipole, hydrogen bonding, ion-dipole |
| Vapor pressure and Volatility decrease | IMF increase |
| All molecules contain what IMF? | LDF's |
| Gas Approaches Ideal | smaller and non polar |
| Gas Pressure and ______ are directly related | # of moles |
| Least Ideal Conditions | low temp/high pressure |
| Daltons Law | P total = P a + P b + P c + ..... |
| Equation when collecting gas over water | P total = P dry gas + P water vapor |
| Molar Mass Equation | MM=dRT/P |
| Gas Deviates from Ideal | larger and more polar |
| Most Ideal Conditions | high temp/low pressure |
| How many L is one mole of an ideal gas (at STP) | 22.4 L |
| Pressure (P) and _____ are inversely related | Volume (V) |
| Temp. (T) and _______ are directly related | Pressure (P) |
| How are Temp. (T) and Volume (V) related? | Directly |
| Ideal Gas Law Equation | PV=nRT |
| Gases are _________ bc of the large spaces between particles | compressible |
| What is gas pressure caused by? | collisions of particles against wall of container |
| More Collisions = ? | higher pressure |
| Average Kinetic Energy equivalent to | Temperature |
| larger molar mass (movement) | slower |
| Gas mixtures are always ________ bc of the random motion of particles | homogenous |
| Infared Frequency | Vibrational |
| smaller molar mass (movement) | faster |
| Radio Frequency | Nuclear and Electronic Spin |
| X-ray | bond-breaking |
| UV/Visible | Electronic (moves up a layer) |
| Acid | reactant, donates H |
| Base | reactant, H acceptor |
| Conjugate Acid | product, gains H |
| Conjugate Base | product, loses H |
| Hrxn is Negative | energy released when bond formed |
| Equation for Enthalpy Change | Hrxn = BE reactants - BE products |
| Hrxn is Positive | energy required to break bond |
| The more bonds ______ | the higher the bond energy |
| Semi-Empirical | theoretical, but relies on experimental (empirical) data for verification |
| What is a substance that lowers Eact, starts as reactant, ends as product? | Catalyst |
| What is a temporary substance that goes from product to reactant? | Intermediate |
| The lower the peak of Activation Energy... | The faster the reaction |
| Endothermic | Products higher in energy |
| Exothermic | Reactants higher in energy |
| The higher the peak of Activation Energy... | The slower the reaction |
| Base with | Conjugate Acid |
| Acid with | Conjugate Base |
| radioactive decay is always... | first order |
| unimolecular | single species reacts to form products |
| bimolecular | 2 species collide and react |
| termolecular | 3 species collide and react |
| Elementary reaction | process in chemical reaction that occurs in a single step |
| Intermediate | in between substance created by some steps but consumed by the next step |
| Reaction occurs when? | particles collide at correct orientation |
| Activation Energy | minimum energy to break bonds, top of the "hill" |
| Rate = k[A]^x[B]^x | Rate Law |
| k Unit 1st Order | s-1 |
| k Unit 2nd Order | M-1 s-1 |
| 1st order linear graph | In[A] vs time |
| Acids are proton _____ | donors |
| % yield = (_______ / theoretical) x100 | experimental (actual) |
| % error = (experimental - theoretical)/________ x 100 | experimental |
| empirical formula rhyme | % to mass, mass to mole, divide by small, times until whole |
| molecular formula | whole # multiple of empirical formula |
| What properties does SNAP have? | always soluble, usually spectators |
| amount of product in reaction determined by | limiting reactant |
| SNAP | sodium, nitrate, ammonium, potassium |
| Reduce | gains electrons, loses charge |
| hydrogen ion (H+) | a proton |
| Bases are proton______ | acceptors |
| Water is | acid or base |
| Oxidize | loses electrons, gains charge |
| HClO4 | perchloric acid, strong acid |
| HCl | hydrochloric acid, strong acid |
| HBr | hydrobromic acid, strong acid |
| HI | hydroionic acid, strong acid |
| HNO3 | nitric acid, strong acid |
| H2SO4 | sulfuric acid, strong acid |
| Diatomics? | H2, N2, O2, F2, Cl2, Br2, I2 |
Created by:
taylor8alexandra
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