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Module 1 Chemistry, Module 1 : Properties and structure - Coggle Diagram
Module 1 Chemistry
Module 1 : Properties and structure
IQ 2 Why Differences in Atoms
Electron structure
Schrodinger Model
Electrons are in orbitals where there is high probobility of an electron presiding
Spdf
1-7s (2 Electrons) (circle)
2-7p (6 Electrons) (Up down ovals)
3-6d (10 Electrons) up down left right ovals)
4,5 F (14 Electrons) (anything)
Bohr Model
Electron Shells
2 in first , then 4, then 8, 8, then 18
Outermost shell with electrons is called Valance shell
Pairs of electrons are in opposite spin
Flame tests
The metal cation present in a substance can be identified by the color of the flame produced when undergoing combustion
How Atomically
Atom is heated up and electrons in valence shell recieve energy first and transform heat energy to kinetic energy
Electron once have enough energy ''jump'' from valance shell to next possible shell
Electron then jumps back to original valance shell releasing light energy
Frequency of light energy released related to distance between shells (electronegativity)
Isotopes and Radiation
Isotope
Unstable if
greater then 82 Atomic Mass
If Unstable
Become Radioisotope
And Enter Radioactive Decay
3 types
Alpha
2 more items...
Beta
2 more items...
Gamma
2 more items...
N:P is grater than 3:2 or less then 1:1
A variation of an element with a different amount of Neutrons
Proton + Neutron 0 electron -
Atoms notation Atomic mass top right Atomic Number/Proton Bottom right
IQ 3 Periodic trends (periodicity)
Electro Negativity
Across Periods (rows Left - Right)
Increase (Ionisation and Electronegativity)
Less Valence electrons harder to Ionise, More Protons able to attract electrons
Decrease (Atomic Radius)
More protons and electrons attracted to eachover closer
The Ability of an atom to attract Electrons
Diffirences =
Greater then 2 Ionic Bond
transfer of electrons from one to another
Less then 1.7 Covalent Polar (One part is more negative then other parts)
Less then 0.5 Covalant Non Polar
The sharing of electrons
Atomic Radius
Down Groups (Columns Downwards)
Decrease (Ionisation and Electronegativity)
Increase (Atomic Radius
The radius of an atom
Ionistation Energy
Energy required to Remove an electron forming an ion
Properties
Ionic soluble in water
E Conductor in water
High melting point
Covalent Insoluble in water
Not E conductor in water
Low melting point
IQ 4 Bonding
Lewis Dot
VESPR
Basically Shape of a Molecules is dependant on electron repulsiion
Page 16 of Module 1 booklet
Network Structures
Ionic solid
Crystalline lattic of anions & Cations
Metallic structure
Metal Cations in ''sea'' of electrons of electro static charge
Covalent network
Ordered repeating atoms bonded strongly covalently
Covalent Molecular Structure
Held by intramolecular covalent bonds with weak inter molecular forces
Properties
If electrons could move freely
Conductor
If strong intramolcular bonds
High melting/boiling point
InterMolecular forces
Types
Dipole Dipole forces (between polar ends of molecules)
Mid strength
Hydrogen Bonds
Bonds of Hydrogen poles with other poles
Strongest
Dispersion
Weakest
Exist between all molecules
More electrons = Stronger
Strength
Covalent 2nd Strongest
Ionic Strongest out of all bonds
Allotropes
A substance of an element that is bonded in a distinct structure causing distinct properties
A molecule is a substance with 2 or more atoms chemically bonded
A compound is a substance of molecules
IQ 1 Properties, Classification and Seperation
Definitions
Pure substance
A substance with uniform composition that can not be seperated into simpler substances through physical means with distinct characteristics
Element
Pure substance that can not be decomposed into simpler substances (only one type of atom)
Compound
Pure substance that can be decomposed into simpler substances
Mixture
A substance containing two or more substances that are not chemical bonded
Homogenous Mixture
A mixture with a uniform composition through out
Heterogenous mixture
A mixture with a non uniform composition through out
Gravimetric Analysis
Quantitative analysis where the sought substance is seperated from a sample and measured
Chemical properties
Characteristics relating to changing of Atomic structure
Physical Properties
Characteristics not relating to attomic structure
Seperation
Distillation
The Seperation of liquids utilising diffirence in boiling points
Magnetic seperation
Separations magnetic substances from not magnetic substances using magnetism
Filtration
The seperation of solids from one or more liquids through a membrane
Evaporation
Removal of a liquid from a generally solid mixture
Types of atoms
Metals
Malleable
Conductive
High melting point
Non Metals
Low melting point
Dull & Brittle
Poor Conductor
Common Anions & Others
NH4 +
Ammonium
SO4 2-
Sulfate
CO3 2-
Carbonate
NO3 -
Nitrate
PO4 3-
Phosphate
OH -
Hydroxide
MnO4 -
Permaganate
CrO4 2-
Chromate
Cr2O7 2-
Dichromate
HCl
Hydrochloric acid
H2SO4
Sulfuric acid
HNO3
Nitric Acid
Ions
Cations +
Anions -
Math & Calculations
Percent Composition
Mass (grams) or atomic mass / Total mass (g) or total Atomic Mass
Relative Atomic Mass
Atomic mass of Isotope x % +Isotope 2 x %....
