Chemistry - Unit 8 Test General Review

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Comprehensive review of various concepts/formulas/conversions that may be useful to have well remembered according to the test overview and unit slideshow (not fun!!!)

Last updated 4:44 AM on 3/16/23
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69 Terms

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Solids (Particle motion)
Particles vibrate
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Liquids (Particle motion)
Particles slide past/against each other
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Gases (Particle motion)
Particles move very quickly and freely of one another
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Solids (IMFs)
Experiences the strongest IMFs
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Gases (IMFs)
Experiences the weakest IMFs
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Liquids (IMFs)
Experiences IMFs that are stronger than in gases, but weaker than in solids
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Solids (Particle distance)
Particles are the closest together; they are packed very tightly together (rough explanation)
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Liquids (Particle distance)
Particles are close to one another and have some distance from one another; more particle distance than solids but less than gases (rough explanation)
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Gases (Particle distance)
Particles are the farthest apart and can be very far from each other (rough explanation)
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Solids (V + S)
Definite/Fixed Volume and Shape
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Liquids (V + S)
Fixed/Definite Volume and Indefinite Shape (assumes the shape of the container)
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Gases (V + S)
Indefinite Volume and Indefinite Shape (assumes the shape of the container)
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Solids (KE)
Lowest (average) kinetic energy when compared to all three states of matter
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Gases (KE)
Highest (average) kinetic energy when compared to all three states of matter
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Liquids (KE)
Higher (avg) kinetic energy than solids, lower (avg) kinetic energy than gases
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Solids
knowt flashcard image
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Liquids
knowt flashcard image
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Gases
Image assumes an open container, must be adapted in a closed container
Image assumes an open container, must be adapted in a closed container
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Gases
The **only** compressible state of matter (thereby meaning the **other two** states of matter are **not** compressible!)
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Temperature
Average kinetic energy of all particles within a substance; measured with a thermometer
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**Intra**molecular Forces
Occurs **within** a molecule; Ionic or Covalent; Chemical Reaction occurs when broken
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**Inter**molecular Forces (IMFs)
Weak attractive force **between** molecules; London-Dispersion, Dipole-Dipole, Hydrogen Bond, Ion-Dipole; Physical Change occurs when broken
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London-Dispersion Forces
(IMF) Exists in all substances; caused by an unequal distribution of electrons in a molecule or atom, creating a temporary instantaneous dipole at any given moment
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Dipole-Dipole Forces
(IMF) **Only** present in **polar covalent** molecules; the unequal sharing of electrons create a permanent dipole which causes this IMF (positive ends are attracted to negative ends)
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Hydrogen Bonding
(IMF) Special case of Dipole-Dipole Forces; only occurs when **H** is bonded to a **N**, **O,** or **F**
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Ion-Dipole Forces
(IMF) **Only** occurs in mixtures with two different substances, one of which being an ion and the other being polar and covalent; caused by ions dissociating within a polar solvent so that cations are attracted to negative ends of the polar molecule and anions are attracted to positive ends of the polar molecule
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Dispersion, Dipole-Dipole, H-Bond, Ion-Dipole
Order of IMFs from **weakest** to **strongest**
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IMF Strength
Affected by the distance between particles (Inversely Proportional); Strength of charges (Electronegativity); Dispersion forces are affected by molar mass, easier to polarize when larger; Indirectly affected by temperature due to the Kinetic Molecular Theory
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IMFs
Viscosity, cohesion, surface tension, and adhesion are caused by ____.
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Kinetic Energy
1/2mv^2 (m = mass, v = velocity) → This pertains to the Kinetic Molecular Theory.
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Solid
What does (A) indicate?
What does (A) indicate?
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Melting/Freezing
What does (B) indicate?
What does (B) indicate?
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Liquid
What does (C) indicate?
What does (C) indicate?
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Vaporizing/Condensing
What does (D) indicate?
What does (D) indicate?
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Gas
What does (E) indicate?
What does (E) indicate?
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A, B, C, D, E
In which letters is the substance increasing in **energy** (both kinetic and potential)?
In which letters is the substance increasing in **energy** (both kinetic and potential)?
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A, C, E
In which letters is the substance increasing in **kinetic energy**?
In which letters is the substance increasing in **kinetic energy**?
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IMFs
During (B) and (D), since the line is flat, what is the energy used to overcome?
During (B) and (D), since the line is flat, what is the energy used to overcome?
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Liquid
What does (A) indicate?
What does (A) indicate?
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Solid
What does (B) indicate?
What does (B) indicate?
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Gas
What does (C) indicate?
What does (C) indicate?
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Sublimation/Deposition Line
What does (C) indicate?
What does (C) indicate?
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Triple Point
What does (A) indicate?
What does (A) indicate?
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Melting/Freezing Line
What does (D) indicate?
What does (D) indicate?
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Vaporization/Condensation Line
What does (B) indicate?
What does (B) indicate?
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Critical Point
If the point is at the end of the Vaporization/Condensation line as it is with (B), what does the point also indicate?
If the point is at the end of the Vaporization/Condensation line as it is with (B), what does the point also indicate?
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Pressure/Temperature
In a phase change diagram, what are the two labels on the axes? (Y axis first, then X)
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Endothermic
Requires energy input to make them happen (IMFs are being overcome)
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Exothermic
Releases energy as they happen (IMFs are becoming significant)
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Endothermic
Endothermic or Exothermic? (Melting, Vaporization, Sublimation)
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Exothermic
Endothermic or Exothermic? (Freezing, Condensation, Deposition)
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Boyle’s Law
(P1V1 = P2V2) At constant mass and temperature, the pressure and volume of a gas are **inversely proportional**.
(P1V1 = P2V2) At constant mass and temperature, the pressure and volume of a gas are **inversely proportional**.
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Charles’ Law
(V1/T1 = V2/T2) At constant mass and pressure, the volume and absolute temperature (K) of a gas are **directly proportional**.
(V1/T1 = V2/T2) At constant mass and pressure, the volume and absolute temperature (K) of a gas are **directly proportional**.
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Gay-Lussac’s Law
(P1/T1 = P2/T2) At constant mass and volume, the pressure and absolute temperature (K) of a gas are **directly proportional**.
(P1/T1 = P2/T2) At constant mass and volume, the pressure and absolute temperature (K) of a gas are **directly proportional**.
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Combined Gas Law
(P1V1/T1 = P2V2/T2) → **Important formula to know**, it replaces knowing each of the three Gas Law formulas individually.
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STP
Standard Temperature and Pressure → **1 atm** and **0 degrees C** (**273 K**)
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Molar Volume
**At STP**, the volume occupied by **1 mol** **of gas** is **22.4 L**. → When doing Stoichiometry, 1 mol of gas **at STP** = 22.4 L
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Ideal Gas Law
(PV = nRT) → **Important formula to know**, while there are other important uses, it also has to be used during Stoichiometry when you are **not** at **STP**.
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R (atm)
(Universal Gas Constant) → R = 0.0821 L ⋅ atm/mol ⋅ K
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R (kPa)
(Universal Gas Constant) → R = 8.315 L ⋅ kPa/mol ⋅ K
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Ideal Gas
A gas which is behaving according to the Kinetic Molecular Theory → Allows for the Ideal Gas Law to be used. → Gas behavior is most ideal at low pressures, high temperatures, and in nonpolar atoms/molecules.
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Real Gas
A gas which does not follow the Kinetic Molecular Theory, typically occurs when a gas gets close to condensing or turning into a solid. This happens at low temperatures or high pressure. → Unlike ideal gases, particles in a **real gas** have significant volume, have IMFs that attract each other, and have collisions that are inelastic (loss of KE).
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Absolute Zero
The lowest possible temperature at which all molecular motion stops (KE = 0). → 0 K
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Celsius to Kelvin
T (Celsius) + 273 = T (Kelvin) → Exact conversion factor, so use the amount of decimals of the given Celsius temperature for sig figs
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atm to Pa
1 atm = 101,325 Pa (can be rounded to 101,300)
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atm to kPa
1 atm = 101.325 kPa (can be rounded to 101.3)
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atm to mmHg
1 atm = 760 mmHg
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atm to Torr
1 atm = 760 Torr
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atm to psi
1 atm = 14.7 psi

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