unit 5 Flashcards
what type of element forms a metallic bond?
metals
how is a metallic bond formed?
attraction between free floating electrons and cations form a bond
the structure of a metallic bond
Ve- move freely around the cations
propertys of metals and why
melting point in low, not hard because electrons already sliding past each other. boiling point is high because lots of energy required to separate e- from cations
why are metals good conductors of electricity?
electrons can flow freely, negative energy conducts electricity
what type of element forms ionic bonds
metal + nonmetal
how is an ionic bond formed?
electrons are transferred from metal to nonmetal
what is the force of attraction of an ionic bond?
strong
why do elements gain or lose electrons?
to reach stability at 8ve-
how is the potential energy of the atom changed when it loses/gains electrons
the potential energy decreases
what is the overall charge of an ionic compound? how is this achieved?
- cations and anions attract each other, forming the ionic bond
what is electronegativity? how does electronegatively influence ionic character?
the ability of an atom to attract an electron. where electrons are transferred from the less electronegative atom to the more electronegative one.
structure and strength of an ionic bond
crystal lattice; strongest
describe the properties of ionic bonds and why
high melting point and boiling point, crystal lattice, highly conductive, hard and brittle. crystal lattice has cations surrounded by anions and vice versa, making it very hard to separate.
good conductor? MgCl(s)
no solid
good conductor? CaF2 (aq)
good conductor? MgCl2(aq)
yes
good conductor? CO2(aq)
NaBr
sodium bromide
Zn3N2
zinc nitride
CuCl
copper(I) chloride
CoI3
Cobalt (III) iodine
CuS
Cobalt (II) sulfide
FeO
Iron (II) oxide
