Structure, Bonding And Properties Of Matter Flashcards
in ionic bonding what are electrons shared between?
a metal and a non metal
in covalent bonding what are electrons shared between
2 non metals
which type of bonding requires atoms to have full outer shells?
metallic
how can 2+ atoms be bonded together?
by the attraction by 2 nuclei
why do ionic substances have high melting points?
they require lots of energy
what are the attractions between 2 oppositely charged ions called?
electrostatic
in what state will ions conduct electricity
molten
what is a giant lattice?
a regular structure containing a huge number of particles.
what is a delocalised electron?
an electron free to move through a structure
how are atoms arranged in metallic bonding?
in a regular, layered structure.
what kind of strong forces are between ions and electrons in metallic bonding?
electrostatic
metals are ___ ions
positive
metals have ____ melting and boiling points.
high
why do metals have high melting and boiling points?
the delocalised electrons are free to move anywhere
the free electrons allow layers of atoms to slide over each other. this makes the metals___.
maluable
an alloy contains atoms that are ____ sizes
different
why are alloys more difficult to slide over?
the arrangement of particles is not regular
when an atom gains electrons it becomes ___ charged
negatively
which one is harder: alloy or metal
alloy
when an atom loses electrons it becomes ___ charged
positively
what is in an alloy
metals and small amounts of other substances, usually other metals.
why are giant bonds of any substance hard to break
there is lots of bonds to break and lots of energy is required for this.
why do molecules not conduct electricity?
they have no charged particles.
why don’t ionic or covalent structures conduct electricity?(unless its molten or dissolved or graphite)
there are no delocalised electrons
