Bonding Flashcards
Compare strengths and length of double bonds and single bonds
Double bonds are generally stronger and shorter than single bonds
What is meant by VSPRE theory?
Pairs of electrons arrange themselves around the central atom so that they are as far apart from each other as possible
What are intermolecular forces?
The forces of attraction between the molecules
Why does Hydrogen Bonding occur?
When hydrogen is directly to a small highly electronegative element. As the electron pair is drawn away from the hydrogen atom by the electronegative element, all that remains is the proton in the nucleus as there are no inner electrons. The proton attracts a non-bonding pair of electrons from the F N O
What are allotropes?
Occur when an element can exist in different crystalline forms
Why are metals malleable and ductile?
Because the close packed layers of positive ions can slide over each other without breaking more bonds than are made
What is a metallic bond?
The attraction that two neighboring positive ions have for the delocalized electrons between them
What affects melting points?
They are affected by impurities, and these weaken the structure and result in lower melting points
Solubility rules
Polar dissolves in polar
Non-polar dissolves in non-polar
As the carbon chain length increases the molecules become less soluble in water
How can conductivity occur?
For conductivity to occur the substance must possess electrons or ions that are free to move
How are sigma bonds formed?
Formed when two atomic orbitals on different atoms overlap along a line drawn through the two nuclei
How are pi bonds formed?
Formed when two p orbitals overlap ‘sideways on’
What is hybridization?
The mixing of atomic orbitals to form new molecular orbitals
What are delocalized electrons?
Occur whenever alternate double and single bonds occur between carbon bonds(e.g benzene)
What is a coordinate bond?
The electrons in the shared pair originate from the same atom
