Chapter 3- Covalent Substances
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why do non-metallic atoms tend to share electrons
they have a relatively high number of electrons in their outer shells
what are intramolecular bonds
bonds within a molecule
what is the octet rule
many atoms become more stable if they get an outer shell of 8 electrons
what is covalent bonding
the sharing of electrons between atoms
what boiling do non-metallic elements and compounds have
low
can non-metallic elements and compounds conduct electricity
No
Why dont molecular substances conduct electricity
because they dont contain free moving charged particles
are intermolecular bonds strong
no hence why they break
are intramolecular bonds strong
yes hence why they hold
what is a single covalent bond
when atoms share two electrons. one from each atom.
what is the molecular formula
an indicator of the number and types of atoms found in a molecule
what are electrons involved in the covalent bond called
a shared pair
what are electrons that are not involved in the covalent bond called
lone pairs
what is a double covalent bond
two pairs of electrons are shared between atoms
what are triple covalent bonds
when 3 electron pairs are shared between 2 atoms
what does a diatomic molecule contain
2 atoms
what is a polyatomic molecule
molecules made up of 2 or more atoms
What is the VSEPR theory
a way of predicting the shapes of small molecules
How does the VSEPR theory work
the pairs of electrons present in the valence shell will repel each other and try to get as far away from each other as possible
Do lone pairs influence the shape of a molecule
Yes but they are not considered a part of the shape
What key factor determines the electrons distribution in a diatomic molecule
electronegativity
what makes a bond non-polar
if the bond have an equal distribution of electronegativities as there is no charge on either end of the bond
what atom has the stronger pull in a covalent bond of 2 different elements
the atom that is the most electronegative
in a molecule, which element has a partial negative charge
the element with the higher electronegativity