chemistry unit 2: lewis structures and covalent bonding/molecular geometry

how do ionic bonds hold ions together?

by electrostatic forces

how do covalent bonds hold atoms together?

by the sharing of valence electrons

how can we know number of valence electrons?

group numbers (group 1) = 1 ve , (group 15) = 15 ve

why are lewis symbols helpful for studying bonds?

because they show only the valence electrons of atoms or ions

what is the octect rule?

atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons

do metals lose electrons or gain electrons? if so, do they receive valence electrons for certain ions?

lose electrons, Na⁺, Mg²⁺, Al³⁺ they have no valence electrons

do non-metals lose electrons or gain electrons? if so, do they receive valence electrons for certain ions?

gain electrons, P^3-, S^2-, Cl^- have 8 valence electrons

what is needed to complete the sharing of valence electrons

ionic and covalent bonds

if atoms move more electronegatively what would be the charge?

partial negative charge

electronegativity is the ability an atom in a bond to….

attract electrons

in a molecule, a partial separation of a charge means what?

that the covalent bond is polar

what is a bonding domain?

is between the two atoms in the bond and consists of all the electrons involved in the bond

what is a non-bonding domain?

a non-bonding pair of electrons and is centered on a single atom

what does the VSEPR theory allow?

the prediction of electron domain geometries

what are electrons subjected to?

electrostatic repulsion from the electrons in the other domains