General Chemistry Exam 1 review

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Covalent substances

________ are liquid at room temperature and will boil when their IMFs are broken.

London Dispersion forces

________ (LDFs) occur between all molecules and are very weak attractions caused by random electron movements.

Dipoles

________ are opposite charges separated by some distance.

Vaporization

________ requires no excess heat to be added.

Solids

________ have very tight- knit molecules and have the strongest IMFs.

gas law

The combined ________ is used when moles are held constant.

kinetic energy

The ________ (KE) is directly proportional to the temperature.

Effusion

________ is the rate a gas will escape from a container with microscopic holes from high pressure to low pressure.

covalent bonds

Intermolecular forces (IMFs) are the forces in between ________.

KE

Even though ________ is the same for gases at the same temperature, this can not be said for velocity because gas molecules have different masses.

Network covalent bonds

________ are the strongest and are very hard to melt.

unequal share of electrons

The ________ is called a polar covalent bond which also causes a slight partial charge on each atom.

kinetic molecular theory becomes

The ________ invalid when the temperature is too low and /or the pressure is too high because the gases become too tightly packed.

Ionic substances

________ are usually solids at room temperature.

weakest

Gases have the ________ IMFs and have the most spread apart atoms.

Dipole dipole forces

________ occur when the positive center of one polar molecule is attracted to the negative end of another polar molecule.

hydrogen bond

occurs between hydrogen and oxygen, nitrogen, or fluorine

polar

a molecule that has electrical charge

nonpolar

a molecule with no electrical charge; equally shared electrons

absorbance

the amount of light that cannot get through a colored solution

Ksp

________ is solubility product constant, which has no denominator because reactants are solids.

Law of Mass Action

The ________ is the equilibrium expression that determines the relationship between reactant and product concentrations.

Kc

________ is constant for molar concentrations.

Q

reaction quotient

Le Chatelier’s Principle

When a stress is added to a reaction, the equation will change to adjust for the stress and revert back to equilibrium.

not shift

If Q and K are equal, the reaction will ______

shift to the right

If Q is less than K, the reaction will _______

shift to the left

If Q is greater than K, the reaction will _______

products

If a reaction shifts to the right it will make more _______

reactants

If a reaction shift to the left, it will make more ______

temperature

Only when _______ stress is added will the equilibrium constant

Ka

________ is the acid dissociation constant.

concentration and pressure

When ________ is changed, the equilibrium constant will eventually revert to the original value

equilibrium reactions

In ________, the reaction is reversible, where the reactants from products and then go back to reactants constantly.

Ksp

________ is the measurement of how much a salt dissolves in a solution.

Common Ion Effect

When an element is added to a solution with a salt, the salt equilibrium will change if the element is similar.

more mole of aqueous

If water evaporates from a solution with a salt, the reaction will shift to the side with _______

less moles of aqueous

If water is added to a solution with a salt, the reaction will shift to the side with _______

less mole of gas

If pressure is added to a container, the reaction will shift to the side with ______

more moles of gas

If pressure is removed from a container, the reaction will shift to the side with ______

Arrhenius constant

________, k, is based on the activation energy for a reaction and the temperature.

Collision theory

________ states reactions only occur when chemicals collide with each other with sufficient energy (activation energy)

First Order Rate Law

log[A]=-kt+ln[A]₀

Zero Order Rate Law

Rate=k

Second Order Rate Law

1/[A] = kt+ 1/[A]₀

Catalyst

A substance added to a reaction to speed it up

Intermediate

A substance created in one elementary step and used up in another

Half-life

How long it takes for half of a substance to decompose/be consumed

Half life equation

t= .693/k

Heterogenous Mixture

Not all parts of a mixture are equal, unevenly mixed

Homogenous Mixture

All parts of a mixture are equal, evenly mixed

Elementary Step

The steps that occur during a reaction

Activation energy

How much energy is required for a reaction to start/occur

high

A reaction will occur more if there is a ______ concentration of an aqueous or gaseous substance

lower

A reaction will occur less if the temperature is _____.

heterogeneous

stirring will help a reaction occur more if the mixture is _____

first

The half life equation can only be used for ____ order

negative

First and zero order graphs have a _____ slope

positive

Second order graphs have a _____ slope

First Order

Rate = k[A]

Second Order

Rate = k[A]²