bonding structure and properties of matter 💕💕 Flashcards
energy transferred through states of matter
causing high melting and boiling points
evaporate or boil- more energy needed to overcome remanning chemical bonds
amount of energy needed is depended on strength if attracted forces between particles. stronger the forces more energy needed.
strong attractive forces normally have a high melting and boiling point
solid
regular pattern
vibrate in fixed position
tightly packed
low amount of kinetic energy
cannot be compressed
liquid
randomly arranged
able to move around
greater amount of kinetic energy
able to flow
cannot be compressed
gas
randomly arranged
move around quickly
highest amount of kinetic energy
far apart
can be compressed
how to identify the physical state of a substance if said substance is a solid
given temp is lower than the melting point
how to identify the physical state of a substance if the said substance is a liquid
given temp will be between melting point and boiling point
how to identify the physical state of a substance if the said substance is a gas
if the given temp is higher than the boiling point
what are ions
ions are a charged particle, either positively or negatively charged.
when an element loses or gains electrons it becomes an ion
metals and non metals becoming ions
metals- lose electrons and become positively charged
non metals- gain electrons and become negatively charged
groups loosing and gaining
group 1 and 2 lose electrons
group 6 and 7 gain electrons
metallic bonding
metals only
surrounded by delocalised electrons
tightly packed
arranged in rows
strong attraction between positive metal ions and negatively charged electrons
pure metals and alloys
pure metals are too soft
mixed with metals to make alloys
this distorts layers prevents them from sliding over one another
makes alloys hard to bend
ionic bonding
between a metal and a non metal
metals loose electrons and become positively charged
opposite charges attract
iconic compounds
form structures called giant lattices
they are strong electrostatic forces of attraction that act in all directions
act between the oppositely charged ions
properties of ionic compounds
high melting point- lost of energy needed to break bonds
high boiling point
cannot conduct electricity in a solid as ions cannot move
when in a gas or liquid they can conduct electricity as they can move and carry current
what is covalent bonding
sharing a pair of electrons between atoms to gain a full outer shell, between non metals only
properties of simple covalent structures
low melting point- weak intermolecular forces
molecules are broke when the substance is heated
ways to show bonding in simple molecules
dot cross diagram
outer electron shell is a circle
overlap shows covalent bond
diamond / silicon
carbon atom bonded to 4 other atoms — very strong
high melting point— lots of energy needed to break strong covalent bonds
does not conduct electricity—- no free electrons
graphite
layers of carbon in hexagons
bonded to three carbons and has one free delocalised electron- move between layers
weak intermolecular forces- can slide over eachother
high melting point lots of energy to break covalent bonds
can conduct electricity
nanoparticles
structures that are 1-100nm in size
high surface area to volume ratio
polymers
long chain molecules that are made up of molecules
strong covenant bonds
intermolecular forces between molecules
these attract polymer chains together
long polymer chains have strong forces of attraction than shorter ones making strong materials
fullerenes
carbon molecules thats are shaped like hollow tubes or balls
in hexagons of 5 or 7 carbon atoms
used to deliver drugs to the body
carbon nanotubes
tiny carbon cylinders that are long and thin
conduct electricity well
strengthen material
useful in electronics and nanotechnology
