AP Chemistry Unit 3 (3.1-13)

how is this even possible

A nonpolar molecule with more electrons is more __________, meaning it has stronger _________

polarizable, LDFs

When molecules are the same size, ______ forces are stronger than _______ forces

dipole-dipole, London disperson

When two molecules have a large difference in size, the strength of their _______ (whether polar or nonpolar) scales with their size

IMFs

Although CCl₄ has only LDFs, while HCl has dipole-dipole forces AND LDFs, CCl₄ has a stronger IMFs because…

It is much larger than HCl (more electrons)

Hydrogen bonds are really just extra-strong ________ forces

dipole-dipole

What must a molecule have to be a hydrogen bond DONOR?

Hydrogen atom that is covalently bonded to F, O, or N

What must a molecule how to be a hydrogen bond ACCEPTOR?

F, O, or N with a lone pair of electrons on it and a partial negative charge (part of a polar bond)

Hydrogen bond ACCEPTORS don’t need to have…

Hydrogen, just F, O, or N with lone pair

In a large molecule, it is possible for hydrogen bonding forces to be formed between a _____________________ and the _______________

hydrogen atom (bonded to F, O, or N); negative end of a dipole formed by F, O, or N

Ion-dipole forces

Attractive force between ion and polar molecule, usually occurring in a solution

Ion-dipole forces occur when an ionic compound is ___________ in a polar _________, such as…

dissolved, solvent, H₂O

Dipole-induced dipole forces

Attractive force between polar and nonpolar molecules → polarity of polar molecule causes a nonpolar molecule to form a temporary dipole

Dipole-induced dipole forced increase with the __________ of the polar molecule and the ____________ of the nonpolar molecule

magnitude, polarizability

Polarizability

The case with which the electron cloud in an atom or molecule can be distorted (larger electron cloud = more polarizable)

London dispersion forces

Attractions between nonpolar atoms/molecules that are caused by temporary dipoles

Dipole-dipole forces

Attractions between polar molecules in which the partial negative charge of one polar molecule is attracted to the positive partial charge on another nearby molecule

If two compounds have the same formula, but one structure has a larger surface area, it will have __________ IMFs

stronger

Amorphous network solid

Solid with a random, disordered arrangement of atoms or molecules

Crystalline network solid

Three-dimensional, repeating arrangement of atoms, ions, or molecules

Ionic and covalent network solids have ________ melting points, while molecular solids have _______ melting points

high, low

_____ solids are hard and brittle

Ionic

_____ solids are hard and rigid

Covalent network

_____ solids are soft

Molecular

_____ solids are malleable and ductile

Metallic

Which is the only SOLID that conducts electricity?

Metallic

Metalloids form _________ bonds with nonmetals

covalent

A higher vapor pressure implies many _________

collisions

Vapor pressure

Pressure exerted by a gas in equilibrium with its liquid phase at a given temperature

Network solids only have _________ and lack ________, giving them ridiculously high _______________

bonds, IMFs, boiling points

When comparing two liquids at the same temperature, the liquid that has a higher ____________ should have a lower ____________

vapor pressure, boiling point

Boiling point

Temperature which the vapor pressure of a liquid is equal to the external pressure surrounding the liquid

Normal boiling point

Situation in which the vapor pressure of a liquid is equal to the standard atmospheric pressure at sea level (1 atm/760 torr)

Which solid is represented by the particles?

Ionic

Which solid is represented by the particles?

Covalent network

Which solid is represented by the particles?

Molecular

Which solid is represented by the particles?

Metallic

Does Nick Forest know what polarizability is?

No lol

Is Mr Ionic the goat?

[[YES]]

What is the universal gas constant used in ideal gas laws problems?

0.08206

How many torr is in 1 atm?

760

Kinetic energy is related to ___________

temperature

If temperature is the same between two samples, so is the _________________

kinetic energy

A lower kinetic energy indicates a _________ average particle speed

lower

A particle that is lighter travels at a _________ average speed than a heavier particle at a given temperature

fatser

A higher average speed indicates _________ pressure

greater

What does it mean for a tank to be flushed?

For it to be removed of all dry air

What is the density of water?

1 g/mL

Which elements exist as diatomics?

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine

In terms of ideal gas law, what can P be set equal to?

(nRT)/v

What is the formula for total pressure, given gasses A, B, and C?

P_A + P_B + P_C

What proportion is set up for partial pressure when given moles?

P_A / P_Total = n_A / n_Total

The peak of a Maxwell-Boltzman distribution curve represents…

The most probable speed

As the average speed of a particle increases, there is a _________ range of values for particle speed

wider

As the average speed of a particle increases, the slope of the Maxwell-Boltzman curve becomes _________

flatter

As the average speed of a particle increases, the peak of the Maxwell-Boltzman curve moves to the ________

right

The average molecular speed of a gas is higher when the gas has a _____________ temp and a _____________ molar mass

higher; lower

In an ideal gas, it is assumed that there are no ______________ between the particles

attractive forces

The particles of a ___________ gas experience attractive forces

real

Deviations from ideal gas law occur as a result of _________________ and ________________

interparticle interactions; finite particle volumes

The effect of interparticle forces is especially noticeable when the gas temperature is relatively __________

low

Negative pressure deviations (lower than ideal) occur due to…

interparticle interactions, causing gasp particles to strike the container less often

Positive pressure deviations (higher than ideal) occur due to…

nonnegligible particle volumes, which cause particles to strike container walls more often

In an ideal gas, it is assumed that the volume occupied by the gas particles themselves is _____________, or _____________

zero; negligible

A gas sample should exhibit ideal behavior at relatively _____________ temperatures and ____________ pressures

high; low

A higher pressure means that the particles are ____________ compact, encouraging the formation of ______________

more; IMFs

Solvent

The substance that dissolves another

Solute

The substance that is dissolved by another

In a mixture, there is usually __________ solvent than solute

more

__________ is the universal solvent

Water

Molarity equation

(Moles of solute)/(liters of solution)L

Larger molarity = _________ concentration

larger

A solution in which a substance is dissolved completely in water is known as an _______ solution

aqueous

How do you perform a dilution?

Add distilled water to a solution

What formula can you use to figure out molarity in a dilution?

M₁V₁ = M₂V₂

Why do you rinse the weighing paper when adding solute to a solvent?

Solute may stick to the weighing paper/container

What kind of flask is used for a dilution?

Volumetric flash

The components of a liquid solution cannot be separated by…

filtration

What are the two methods in which a liquid solution can be separated?

Chromatography, distillation

Chromotography

Separates chemical species by taking advantage of the differential strength of the IMFs between and among the components of the solution/mobile phase and with the surface components of the stationary phase

Chromatography can help infer the relative _____________ of components in a mixture

polarities

Stationary phase

A solid that provides support for the chromatography experiment, but does not move → can be piece of paper, piece of metal/glass coated with a porous solid, or a glass column filled with a porous solid

Mobile phase

A liquid or gas that moves, carrying the components of the mixture over or through the stationary phase

In a chromatography experiment, if Component X travels farther away from a nonpolar solvent/mobile phase than Component Y, Component X is more ___________

nonpolar

Substances with ____________ IMFs tend to be more soluble in one another; in other words, _________ dissolves _________

similar; like dissolves like

Solvent front

In a chromatography experiment → the mark on the paper that indicates how far the solvent has moved up the paper

Retention factor (R_f) formula

(Distance traveled by one component)/(distance traveled by the solvent)

The larger the R_f value is the farther _____ the paper he component of the mixture has traveled relative to the solvent front

up

Distillation

Separates chemical species by taking advantage of the differential strength of IMFs between and among the components and the effects these interactions have on the vapor pressures of the components in the mixture; separates components of a mixture that have different boiling points

In a distillation, the mixture is heated gently until the component with the ________ boiling point begins to boil. The vapor rises up through the glassware, and reaches the ____________, which is the portion of the apparatus that is surrounded by cool _____________. The vapor condenses into a liquid and is collected in a separate container, The liquid that is produced in a distillation experiment is known as the _______________. The component of the mixture that appears first in that is the one with the _____________ boiling point.

lowest, condenser, water, distillate, lowest

Ionic compounds MUST dissolve in _________

water

Polar and nonpolar only refers to _____________ molecules

nonmetal

What are the three types of electromagnetic radiation (EMR)?

Microwave, infrared, ultraviolet

Microwave radiation causes a molecule to…

rotate

Infrared radiation (IR) causes the bonds in a molecule to…

vibrate

Visible/ultraviolent (UV) radiation causes electrons in the molecule to…

move up to higher energy levels

Wavelength (𝜆)

Length of wave (period) in meters/nanometers

Frequency (v)

Number of cycles passing a point in a given time (cycles per second → hz)

Speed (c)

The speed of light, at which all electromagnetic radiation travels at

How do wavelength, frequency, and speed relate?

c = 𝜆v