Lecture Notes

Flashcards for vocabulary review.

Redox reaction

Chemical reaction involving the transfer of electrons.

Half-equation

Part of a redox reaction showing either oxidation or reduction.

Equilibria

A state in which the rate of forward and reverse reactions are equal.

Fluorine charge

Always -1.

Hydrogen charge

+1, except in hydrides.

NaH Name

Sodium Hydride

Oxidation

Increase oxidation number of other atom

Elised

Not sodium (III)

Disproportionation

A reaction where a substance is both oxidized and reduced.

MnO2

Manganese (IV) Oxide

Oxidizing agent

A substance that oxidizes another substance while itself is reduced.

Equilibrium

Reversible reaction.

Kc

Ratio of products to reactants at equilibrium

Kp

Ratio of partial pressures of products to reactants at equilibrium

Stable state

Stable state; resists change.

Dynamic Equilibrium characteristic

Rate of forward reaction equals rate of backward reaction.

Concentration of reactant and product is constant.

Equilibrium characteristic

Concentration is constant.

Closed system

A system where no substances can enter or leave.

Dynamic

Equilibrium is constantly shifting between reactants and products.

Solids

Does not affect K or Kp.

Temperature affect

What factor can change the equilibrium constant?

Le Chatelier's Principle

Equilibrium shifts to relieve the stress.

Concentration decreases

equilibrium shifts to minimise consequences of increased concentration.

Move to the side with more more moles

Temperature Increase

Exothermic reaction: Temp increase, shift left f equilibrium favours endothermic reaction.

Endothermic reactions: Temp increase, shift right, equilibrium favours endothermic reaction.

Concentration effect

Kc stays constant.

Acid

Acid donates H+.

Base

Base accepts H+.

H+ + OH-

Forms water.

Strong acid

Acids: HCl,

HBr,

HNO3,

HI,

H2SO4,

HClO4.

weak acid

Acids: CH3COOH, C6H5COOH.

Strong Alkali

Alkalis of Group 1 and 2.

weak alkali

Ammonia (NH3).

Bronsted-Lowry acid

Proton donor.

Bronsted-Lowry base

Proton acceptor.

Water

Can act as acid or base.

Conjugate base

Acid after donating a proton.

Conjugate acid

Base after accepting a proton.

Strong acid

Dissociate completely

Weak acid

Dissociate Partially

Strong acid

Irreversible; single arrow.

pH calculation

pH = -log[H+].

Titration

Indicator determines endpoint.

Strong Acid & Strong Base

Endpoint pH = 7.

Strong Base & Weak Acid

Endpoint pH > 7.

Strong Acid & Weak Base

Endpoint pH < 7.

Amphoteric

Accepts or donates H+.

Kp equation

Kc = p(C2H5OH) / (p(C2H4) * p(H2O)).

Closed system

No substance that enters or leaves.

Temperature Decrease

Shift right, favoring exothermic.

Reaction Rate

Rate of reaction based on time.

Collision Rate

Frequency of collisions.

Effective Collision

Collisions with enough energy and correct orientation.

Rate of Reaction

Reactant decrease and product increase.

Catalyst

Increases rate of reaction.

Catalyst Function

Provides alternative pathway with lower activation energy.

Homogeneous catalyst

Same phase (state of matter).

Heterogeneous catalyst

Different phase (state of matter).

Period 3 Trend

Atomic Radius decreases across period.

Period 3 elements

Na, Mg, Al, Si, P, S, Cl.

Structure

Simple Molecular

Period 3 Trend

First Ionisation energy increases across period.

Na/Mg Oxides

Dissolve in water

effect

Bonding and electronegativity.

NaCl- MgCl2

ionic bonding.

mpt

Decreases