Lewis Structures Flashcards
What are a few examples of atoms that never disobey the Ocet rule and why they are not able to?
The atoms in the second period of the periodic table such as lithium and boron have easy access to d-orbitals which means they will have enough electrons to form a full valence shell.
What is the Ocet rule?
Atoms must have 8 valence electrons in order to be stable.
What are some examples of atoms that can disobey the Ocet rule and why they can?
Atoms that are in the third period such as silicon and chlorine are able to expand their Ocet by utilising the nearby d-orbitals therefore disobeying the Ocet rule.
What is the difference between drawing a lewis structure for an un-charged and charged molecule?
With charged molecules they will have less or more electrons than an un-charged molecule. The end product for a charged molecule will also be placed in a bracket with the delegated charge on its top right.
How is the VSEPR theory used to figure out molecular shapes?
VSEPR theory predicts the shape of molecules through valence shell electron pair repulsion. It used repulsions and attractions to determine shape.
What are the two types of electron pairs around an atom in a molecule?
Bonding pairs (Electrons shared between two atoms to make up the covalent bond)
Non-bonding pairs (Lone electron pairs)
What helps to determine polarity?
Polarity is determined by the separation of charge in a molecule.
Why is symmetry so important when in comes to determining polarity?
When a shape is symmetrical its charges will cancel out and the shape will be non-polar no matter the difference in charge.
Why are molecules with more than one type of atom around the central atom always polar?
There will be different charges therefore forming a polar molecule.
