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Chemistry /Edexcel A Level Chemistry: 2: Bonding and Structure Part 2

Edexcel A Level Chemistry: 2: Bonding and Structure Part 2

Chemistry33 CardsCreated 11 days ago

This deck covers key concepts of bonding and structure in chemistry, including polarisability, molecular shapes, electronegativity, and types of bonds.

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What is polarisability?

An indication of the extent to which the electron cloud in a molecule or ion can be distorted by a nearby electric charge
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Key Terms

Term
Definition
What is polarisability?
An indication of the extent to which the electron cloud in a molecule or ion can be distorted by a nearby electric charge
Bigger molecules with a larger number of electrons have a…
…higher polarisability and potential for temporary dipoles
Why do the boiling temperatures rise down Group 7 and Group 0?
Because the atoms get bigger and have a greater polarisability and more electrons, so more London forces
Why do branched alkanes have lower boiling points?
Because they have a smaller surface area and therefore

What are the properties of simple molecular structures?

Usually gases, liquids or soft solids at room temperature
Have relatively low melting and boiling temperatures
Do not conduct electricity as ...

What is electron pair repulsion theory?
That electron pairs in the outer shell of atoms and ions repel each other and get as far away as possible
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Edexcel A Level Chemistry: 2: Bonding and Structure Part 2
TermDefinition
What is polarisability?
An indication of the extent to which the electron cloud in a molecule or ion can be distorted by a nearby electric charge
Bigger molecules with a larger number of electrons have a…
…higher polarisability and potential for temporary dipoles
Why do the boiling temperatures rise down Group 7 and Group 0?
Because the atoms get bigger and have a greater polarisability and more electrons, so more London forces
Why do branched alkanes have lower boiling points?
Because they have a smaller surface area and therefore

What are the properties of simple molecular structures?

Usually gases, liquids or soft solids at room temperature
Have relatively low melting and boiling temperatures
Do not conduct electricity as thy contain neither ions or free electrons.
Usually soluble in non polar solvents

What is electron pair repulsion theory?
That electron pairs in the outer shell of atoms and ions repel each other and get as far away as possible
What is a bond angle?
The angle between two covalent bonds in a molecule or giant covalent structure
What does isoelectronic mean?
Molecules and ions that have exactly the same number and arrangement of electrons
What is the bond angle in a linear molecule?
180
What is the bond angle in a trigonal planar?
120
What is the bond angle in a tetrahedral molecule with no lone pairs?
109.5
What are the bond angles in trigonal bipyramidal molecules?
90, 120, 180
What are the bond angles in octahedral molecules?
90 and 180
Ammonia and water are isoelectronic with…
…methane
How are lone pairs held in relation to the central atom?
Closer than bonding pairs
What is the strength of repulsion between electron pairs?
Lone pair - lone pair > Lone pair - bonding pair > bonding pair - bonding pair
How do double or triple bonds affect shapes of molecules?
They don’t, they are treated as one bond and as a separate centre of negative charge
What are polar covalent bonds?
Bonds between atoms of different elements. The shared electrons are drawn towards the atom with the stronger pull on the electrons.
How does a big difference in electronegativity affect bonding type?
The bigger the difference in electronegativity, the more polar, and the more ionic a bond is.
How does electronegativity change down a group?
It decreases
Why is a polar liquid attracted to an object with electrostatic charge?
Because polar molecules tend to move and rotate because the charge on one side of the molecule is attracted to the opposite charge of the object
What are the essential requirements for hydrogen bonding?
A hydrogen atom covalently bonded to a highly electronegative atom
What is a saturated solution?
Contains as much of the solute as possible at a particular temperature

What are the interactions involved in solubility?

The intermolecular forces between solute molecules
The intermolecular forces between solvent molecules
The intermolecular forces between solute and solvent molecules

When does a molecular substance dissolve?
If the energy needed to break intermolecular forces and to separate the molecules in the solute and in the solvent is about the same as the energy released as the solute forms new intermolecular forces with the solvent
What is a non-aqueous solvent?
Any solvent other than water
What is hydration?
It takes place when water molecules bond to ions or add to molecules. Water molecules are polar so are attracted to both positive and negative ions
What are allotropes?
Different forms of the same element in the same physical state
What are the allotropes of carbon?
Diamond, graphite, fullerenes, graphene
Why does Diamond not conduct electricity?
The electrons in the covalent bonds are not delocalised
What are composites?
Two or more materials combined to create a new material which has the desirable properties of both its constituents
What are delocalised electrons?
Bonding electrons not fixed in a bond between two atoms. Free to move around and shared by many atoms.
What is metallic bonding?
The strong electrostatic force of attraction between metal ions and delocalised electrons