Chemistry Semester 2 Knowledge Flashcards
Non-polar molecule
Molecule that has no positive or negative poles formed in it.
Degenerate
of equal energy
Difference between Saturated and unsaturated molecule
Saturated - contains only single bonds between carbon atoms, they are saturated with hydrogen atoms (having as many hydrogens as it can) and undergoes substitution reactions.
Unsaturated - contains double or triple bonds between carbon atoms, they are not saturated with hydrogens and undergo addition reactions
Homologous series
a sequence of compounds with the same general formula and similar chemical properties
What are the three main types of hydrocarbons and their characteristics?
Alkanes - molecule only has single bonds.
Alkenes - molecule can have single/double bonds.
Alkynes - can have single/double/triple bonds
General formula for the three main types of hydrocarbons
Alkanes - CnH2n+2
Alkenes - CnH2n
Alkynes - CnH2n-2
What prefixes correlate to what number of C atoms?
Meth - 1
Eth - 2
Prop - 3
But - 4
Pent - 5
Hex - 6
Hept - 7
Oct - 8
Non - 9
Dec - 10
Identify Three main types of Intermolecular forces (from strongest to weakest)
- Hydrogen bonding
- Dipole-dipole interactions
- Dispersion forces
Hydrogen bonding
A strong type of dipole-dipole force between a H atoms and lone pair of electrons on a highly electronegative atom (usually N, O, F, Cl).
Dipole-Dipole interactions
attraction between two molecules with each of them having dipoles (seperation between negative and positive charge) present
Dispersion forces (London forces)
It is the attraction between weak temporary dipoles that form due to the random movement of electrons.
Polarity
the state of an atom or molecule that has both the electrical poles, positive and negative charges.
Characteristics
A feature or quality belonging typically to a person, place, or thing and serving to identify them.
Electronegativity
A measure of an atom’s ability to attract shared (within a covalent molecule) electrons to itself.
Intermolecular forces
Intermolecular forces are forces of attraction or repulsion which act between neighbouring molecules. This is not bonding.
Covalent bond
Bond forming between non-metallic atoms, where elements share electrons to fill outer shells.
Organic
Relating to or derived from living matter.
Hydrocarbon
A molecule that only contains hydrogen and carbon.
Side chain/Alkyl group
A group formed by removing a hydrogen from an organic molecule and having a smaller alkane group.
Functional Group
An atom or group of atoms in an organic compound that determines the reactivity/characteristics of that compound
Alcohols
A class of organic molecule that contains a hydroxyl group (-OH)
Aldehydes
A class of organic molecule that contains a carbonyl group (-CO-) at the end of the main chain
Ketones
A class of organic molecule that contains a carbonyl group (-CO-) within the main chain.
Carboxylic acids
A class of organic molecule that contains a Carboxyl group (-COOH)
Haloalkanes
A class of organic molecule that has had at least one halogen instead of hydrogen.
Esters
A class of organic molecule that contains a carbonyl group (C=O) attached to another carbon
Structural Isomers
Two or more organic compounds have the same molecular formulas but different structures.
How do you identify a Homologous series?
any of numerous groups of chemical compounds in each of which the difference between successive members is a simple structural unit.
Substitution
reactions in which an atom or functional group of a compound is replaced by an atom or functional group of another compound
Addition
reactions in which atoms or functional groups are added to a compound across a double (or triple) bond
Metals properties
Appearance - Lustrous
Melting/boiling points - High (they are all solids, except for mercury which is a liquid)
Density - High
Strength - strong
Malleability - Malleable
Ductility - ductile
Heat conductivity - high
Electrical conductivity - high
Non metals properties
Appearance - Dull
Melting/Boiling point - lower than metals (bromine is a liquid at room temperature, and eleven others are gases)
Density - low
Strength - not strong
Malleability - brittle
Ductility - not ductile
Heat conductivity - low
Electrical conductivity - poor (graphite is exception)
Periodic table trends/patterns in Atomic/Ionic Radii
- Atomic radius - increases down the group and decreases across a period.
- Ionic radius - decreases across the period in positive ions and negative ions. And generally increases down the group.
Periodic table trends/patterns in Reactivity
Metals - increased reactivity down the group and reactivity decreases across a period.
Non-metals - reactivity increases up the group and reactivity increase across a period.
Periodic table trends/patterns in electronegativity
electronegativity increases up the group and increases across a period.
Periodic table trends/patterns in ionisation energy
ionisation energy increases across a period and up the group
Periodic table trends/patterns in metallic/non-metallic character
- Metallic character increases down the group and decreases across a period.
- Non metallic character increases across a period and up the group.
Draw and name Shapes of molecules
Linear
Bent
Tetrahedral
Trigonal Planar
Trigonal pyramidal
Note: Check PowerPoint slide 33 on Term 4
Spectroscopy
Looks at the interaction between matter and the electromagnetic spectrum. When electrons decay/move back to lower energy levels, they give off energy in the form of light.
All elements give off a certain wavelength of light (which assigns it a specific colour), when analysed the wavelengths can determine the composition.
When working with two or more double/triple bonds, what are the prefixes?
- diene, triene, etc.
- diyne, triyne, etc.
When working with two or more double/triple bonds, what happens to the organic compound prefixes?
Except for Meth and eth, all organic compound prefixes get an ‘a’ added to it.
Suffixes for all classes of Organic compounds
Carboxylic acid: -oic ad
Alcohol: -ol
Aldehyde: -al
Ester: -oate
Ketone: -one
