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Atom
Proton
Neutron

Electron
Mass Number
Atomic Number
Isotope

Relative Isotopic
Number
Natural Abundance
Relative Atomic
Mass
Orbital

Aufbau Principle

Pauli Exclusion
principle

Hund’s Rule

First Ionisation
Energy
Nuclear Charge

Effective Nuclear
Charge

Molecule
Compound

The smallest particle of a chemical element that can exist
A stable subatomic particle occurring in all atomic nuclei, with a positive
electric charge equal in magnitude to that of an electron
A subatomic particle of about the same mass as a proton but without an
electric charge, present in all atomic nuclei except those of ordinary
hydrogen
A stable subatomic particle with a charge of negative electricity, found in all
atoms and acting as the primary carrier of electricity in solids
The total number of protons and neutrons in a nucleus
The number of protons in the nucleus of an atom, which is characteristic of
a chemical element and determines its place in the periodic table
Each of two or more forms of the same element that contain equal
numbers of protons but different numbers of neutrons in their nuclei, and
hence differ in relative atomic mass but not in chemical properties; a
radioactive form of an element
It is the ratio of the average mass of atoms of an element (in each sample)
to one unified atomic mass unit
Refers to the abundance of isotopes of a chemical element as
naturally found on a planet
The ratio of the average mass of one atom of an element to one twelfth of
the mass of an atom of carbon-12
Each of the actual or potential patterns of electron density which may be
formed in an atom or molecule by one or more electrons, and can be
represented as a wave function
Aufbau Principle Definition
...

Electrons go into the subshell having the lowest possible energy
...
As an
orbital can contain a maximum of only two electrons, the two electrons
must have opposing spins
every orbital in a subshell is singly occupied with one electron before any
one orbital is doubly occupied, and all electrons in singly occupied orbitals
have the same spin
The first ionisation energy is the energy required to remove one mole of the
most loosely held electrons from one mole of gaseous atoms to produce 1
mole of gaseous ions each with a charge of 1+
The first of these, and the simplest, is the nuclear charge (sometimes
referred to as the actual nuclear charge)
...
It has the same value as the
atomic number
...
The effective nuclear charge may be
approximated by the equation: Zeff = Z - S
...
Water: two hydrogen atoms bonded to

Octet Rule

Valency

Relative Formula
Mass
Ionic Bond

Covalent Bond

Metallic Bond

Mole

Molar Mass

Stoichiometry
Limiting Reagent

Percentage Yield

Theoretical Yield

Solvent

an oxygen atom
...
The
concept of valence was developed in the second half of the 19th century
and was successful in explaining the molecular structure of inorganic and
organic compounds
The relative formula mass of a substance is the weighted average of
the masses of the formula units relative to 1/12 of the mass of a carbon-12
atom
A chemical bond formed between two ions with opposite charges
...
These bonds can form between a pair of atoms or between
molecules and are the type of bond found in salts
A covalent bond, also called a molecular bond, is a chemical bond that
involves the sharing of electron pairs between atoms
...
Metallic
bonds are formed from the attraction between mobile electrons and fixed,
positively charged metallic atoms
...
A mole of a substance is
defined as: The mass of substance containing the same number of
fundamental units as there are atoms in exactly 12
...

Fundamental units may be atoms, molecules, or formula units, depending
on the substance concerned
the molar mass M is a physical property defined as the mass of a given
substance (chemical element or chemical compound) divided by the
amount of substance
...
However,
for historical reasons, molar masses are almost always expressed in g/mol
the relationship between the relative quantities of substances taking part in
a reaction or forming a compound, typically a ratio of whole integers
a chemical reaction is the substance that is totally consumed when
the chemical reaction is complete
...
Theoretical
yield is commonly expressed in terms of grams or moles
The component of a solution that is present in the greatest amount
...
Examples: The solvent for
seawater is water

Solute

Solution

Standard Solution

Concentration

Dilution

Titration

Percentage mass
by mass

Empirical formula
Molecular formula
Electronegative

Polar

Intermolecular
forces

Hydrogen Bonding

Permanent Dipole

a solution is a homogeneous mixture composed of two or more substances
...

In such a mixture, a solute is a substance dissolved in another substance,
known as a solvent
a standard solution is a solution containing a precisely known concentration
of an element or a substance
...
Standard solutions are used to determine the
concentrations of other substances, such as solutions in titrations
concentration is the abundance of a constituent divided by the total volume
of a mixture
...
Example 1: You can add water to
concentrated orange juice to dilute it until it reaches a concentration that is
pleasant to drink
the slow addition of one solution of a known concentration (called a titrant)
to a known volume of another solution of unknown concentration until the
reaction reaches neutralization, which is often indicated by a colour change
Mass percentage is one way of representing the concentration of an
element in a compound or a component in a mixture
...
Also Known As: mass percent
a formula giving the proportions of the elements present in a compound
but not the actual numbers or arrangement of atoms
a chemical formula that gives the total number of atoms of each element in
each molecule of a substance — compare structural formula
Electronegativity is a measure of the tendency of an atom to attract a
bonding pair of electrons
...

Fluorine (the most electronegative element) is assigned a value of 4
...
7
A polar bond is a covalent bond between two atoms where the electrons
forming the bond are unequally distributed
...
The three main categories of intermolecular
forces are London dispersion forces, dipole-dipole interaction, and iondipole interaction
a weak bond between two molecules resulting from an electrostatic
attraction between a proton in one molecule and an electronegative atom
in the other
Permanent dipole-permanent dipole interactions are stronger than Van der
Waals' forces for molecules of equivalent size
...
A permanent dipole is due to a
difference in electronegativity between the atoms involved in a covalent
bond

London Dispersion
Forces

Organic
Alkane

Nomenclature

Molecular Orbital

Sigma Bond

Isomer
Structural Isomer

Valance Bond
Theory

Alkene

Alkyne
Pi Bond

Atomic Radius

Ionic Radius

Ionisation Energy

the weakest intermolecular force
...

This force is sometimes called an induced dipole-induced dipole attraction
the branch of chemistry that deals with carbon compounds (other than
simple salts such as carbonates, oxides, and carbides)
an acyclic saturated hydrocarbon
...

The nomenclature used most frequently worldwide is the one created and
developed by the International Union of Pure and Applied Chemistry
a mathematical function describing the wave-like behaviour of an electron
in a molecule
...
They are formed by headon overlapping between atomic orbitals
...
Structural isomers do not exhibit the
same chemical behaviour
Valence bond theory is a chemical bonding theory that explains
the bonding between two atoms is caused by the overlap of half-filled
atomic orbitals
...
The words alkene and olefin are often used
interchangeably
an alkyne is an unsaturated hydrocarbon containing at least one carbon—
carbon triple bond
are covalent chemical bonds where two lobes of an orbital on one atom
overlap two lobes of an orbital on another atom
...
It is half the distance
between two ions that are barely touching each other
...
The
first or initial ionization energy or Ei of an atom or molecule is the energy
required to remove one mole of electrons from one mole of isolated
gaseous atoms or ions

Metallic Character

Inert Pair Effect

Diagonal
Relationship
Electron Affinity

Transition Metals

Chelating Agents

Thermodynamics

Lattice Enthalpy

Born Haber Cycles

Exothermic
Endothermic
Activation Energy
Atomisation

Rate of Reaction

Temperature

Catalyst

refers to the level of reactivity of a metal
...
Within a
compound, metal atoms have relatively low attraction for electrons, as
indicated by their low electronegativities
the tendency of the electrons in the outermost atomic s orbital to remain
unionized or unshared in compounds of post-transition metals
...
Usually these ligands are organic compounds, and are called chelates,
chelators, chelating agents, or sequestering agents
The study of the interrelation of heat and work with chemical reactions or
with physical changes of state within the confines of the laws
of thermodynamics
A type of potential energy that may be defined in two ways
...
The lattice enthalpy is the
enthalpy change involved in the formation of an ionic compound from
gaseous ions (an exothermic process), or sometimes defined as the energy
to break the ionic compound into gaseous ions (an endothermic process)
(of a reaction or process) accompanied by the release of heat
(of a reaction or process) accompanied by or requiring the absorption of
heat
The minimum quantity of energy which the reacting species must possess
to undergo a specified reaction
the enthalpy change when 1 mol of gaseous atoms is formed from its
element in its defined physical state under standard conditions (298
...
It is often expressed in
terms of either the concentration (amount per unit volume) of a product
that is formed in a unit of time or the concentration of a reactant that is
consumed in a unit of time
temperature is a measure of the "hotness" or "coldness" of a substance
...
There are many topics to be discussed, and each of these
topics is a tool for the study of chemical reactions
AKA The rate of reaction
defined as the change in concentration of an infinitely small-time interval,
expressed as the limit or derivative expression above
a force exerted by the substance per unit area on another substance
...
Ultraviolet and visible light are energetic enough to promote outer
electrons to higher energy sublevels
the measure of the amount of electrical current a material can carry or its
ability to carry a current
...
e
...
Homogeneous catalysis applies to
reactions in the gas phase and even in solids
refers to the form of catalysis where the phase of the catalyst differs from
that of the reactants
...
g
...
The constant ratio is the half-life
...
2
...
One
is the Arrhenius definition, which revolves around the idea that acids are
substances that ionize (break off) in an aqueous solution to produce
hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution
It donates protons in the form of a hydrogen ion (H+)
...
The Bronsted-Lowry base, on the other hand, is a solution that
accepts protons, and is known as a proton acceptor
(of a compound, especially a metal oxide or hydroxide) able to react both as
a base and as an acid
within the Bronsted–Lowry acid–base theory, is a species formed by the
reception of a proton (H+) by a base—in other words, it is a base with a
hydrogen ion added to it
...
Hence, a conjugate base is a species formed by
the removal of a proton from an acid

Polyprotic Acids

Hydrolysis

Buffer Solution

Hydrocarbons

Functional Group
Alcohol Functional
Group
Ethers Functional
Group
Alkyl halides
Functional group

Amines Functional
Group

Alkanes

Benzene

Esters

Amides
Aldehydes

Ketones

Carboxylic Acids

An acid that can donate more than one proton or hydrogen atom per
molecule to an aqueous solution
...
The
reaction mainly occurs between an ion and water molecules and often
changes the pH of a solution
...
Buffer solutions are used as a means of keeping pH at
a nearly constant value in a wide variety of chemical applications
a hydrocarbon is an organic compound consisting entirely of hydrogen and
carbon, and thus are group 14 hydrides
...
The general formula for an ether is R-O-R'
The haloalkanes (also known as halogenoalkanes or alkyl halides) are a
group of chemical compounds derived from alkanes containing one or more
halogens
...
Try to remember that an amine is just like
ammonia because ammonia is a simple molecule to recall
...
In other words, an alkane consists of
hydrogen and carbon atoms arranged in a tree structure in which all the
carbon-carbon bonds are single
a colourless, volatile, flammable, toxic, slightly water-soluble, liquid,
aromatic compound, C 6 H 6, obtained chiefly from coal tar: used in the
manufacture of commercial and medicinal chemicals, dyes, and as a solvent
for resins, fats, or the like
an organic compound made by replacing the hydrogen of an acid by an alkyl
or other organic group
...
Ketones and aldehydes are
simple compounds that contain a carbonyl group (a carbon-oxygen double
bond)
any of a class of organic compounds in which a carbon (C) atom is bonded
to an oxygen (O) atom by a double bond and to a hydroxyl group (−OH) by a

Structural Isomer

Geometrical
Isomer

E Isomer

Z Isomer

Stereoisomer

Chirality

Chiral Carbon
Enantiomer

Racemate
(Mixture)

Optical Isomers

Halogen

Unsaturated
Carbonyl

Saturated

single bond
...
Structural isomers do not exhibit the
same chemical behaviour
a term used in organic chemistry
...
It is not to
be confused with E–Z isomerism, which is an absolute stereochemical
description, and only to be used with alkenes
Cis–trans isomerism, also known as geometric isomerism or
configurational isomerism, is a term used in organic chemistry
...

Most chiral molecules can be identified by their lack of a plane of symmetry
or a centre of symmetry
An asymmetric carbon atom (chiral carbon) is a carbon atom that is
attached to four different types of atoms or groups of atoms
Enantiomers are chiral molecules that are mirror images of one another
...

This means that the molecules cannot be placed on top of one another and
give the same molecule
...
A sample with only a
single enantiomer is an enantiomerically pure, enantiopure or homochiral
compound
molecules that differ three-dimensionally by the placement of substituents
around one or more atoms in a molecule
...
They are reactive non-metallic
elements which form strongly acidic compounds with hydrogen from which
simple salts can be made
having carbon–carbon double or triple bonds and therefore not containing
the greatest possible number of hydrogen atoms
a carbonyl group is a functional group composed of a carbon atom doublebonded to an oxygen atom: C=O
...

A fully saturated compound contains no double or triple bonds

Homologous Series
Alkyl Chain
Mass Spectrometry

Infra-Red
Spectroscopy

Chromophore
Spectrometry

Spectrograph

Chromatography

Magnetic
Equivalence
Integration
Chemical Shift

Multiplicity
NMR (Nuclear
Magnetic
Resonance)
Symmetric Stretch

a series of compounds with the same general formula, usually varying by a
single parameter—such as the length of a carbon chain
Multiple alkane missing one hydrogen each
an instrumental method for identifying the chemical constitution of a
substance by means of the separation of gaseous ions according to their
differing mass and charge
a characterization tool chemist uses to help determine the molecular
structure
...
In general, stronger bonds vibrate at
higher wavenumbers, as do bonds between atoms of very different size
an atom or group whose presence is responsible for the colour of a
compound
a method to measure how much a chemical substance absorbs light by
measuring the intensity of light as a beam of light passes through sample
solution
...
Often the position and number of chemical shifts are diagnostic of the
structure of a molecule
a large number or variety
a physical phenomenon in which nuclei in a magnetic field absorb and reemit electromagnetic radiation
...

Certain atoms, such as oxygen, will almost always set their two (or more)
covalent bonds in non-collinear directions due to their electron
configuration
Electromagnetic
the range of wavelengths or frequencies over which electromagnetic
Spectrum
radiation extends
Electrophile
a reagent attracted to electrons
...
It participates in a chemical reaction by accepting an electron pair to
bond to a nucleophile
Nucleophile
a chemical species that donates an electron pair to an electrophile to form a
chemical bond in relation to a reaction
...

Because nucleophiles donate electrons, they are by definition Lewis bases

Leaving Group

Combustion
Oxidation Reaction

a molecular fragment that departs with a pair of electrons in heterolytic
bond cleavage

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