Topic 2 (bonding, structure, and properties of matter)

Created by

Faith Gardiner

Cards (31)

How does chlorine, iodine, and bromine look after reacting with KCl, KI, and KBr?
KCl+ iodine water = no reaction
KCl + bromine water = no reaction
KI + chlorine water = brown
KI + bromine water = brown
KBr + chlorine water = yellowy orange
KBr + iodine water = no reaction
Properties of fullerenes (buckyballs)?
3 bonds for each carbon so have delocalised electrons
can conduct electricity
can be used to deliver drugs
they’re hollow
they can reduce friction
they can be used as catylists
What do we call an atom that has a positive or negative charge? 
An ion
Uranium-235 has 92 protons. How many neutrons does it have?
143
Explain the process of fractional distillation to separate a mixture of methanol, ethanol and propanol?
heat is applied and the liquid with the lowest boiling point evaporates first
the temp is increased and the second lowest boiling point evaporates
the highest boiling point is left in the beaker
are halogens monoatomic or diatomic?
Diatomic
are most elements metals or non metals?
Metals
description of diamond?
each atom is joined to 4 more so is very hard
high melting point
very strong covalent bonds
it is the hardest natural substance
no free electrons to conduct electricity
what is an allotrope?
Different forms of the same element.
Properties of covalent compounds?
soluble in water
melts easily
properties of ionic compounds?
soluble in water
conduct electricity when dissolved
doesn’t melt easily
what is covalent bonding?
a shared pair of electrons between atoms of non metals. this could be between two of the Same non metal
what is an ion?
An ion is an atom or molecule that has gained or lost electrons, resulting in a positive or negative charge.
what are the properties of molecular solids?
have low melting and boiling points
usually soft and brittle
insoluble in water
soluble in other solvents
dont conduct electricity
what are the properties of transition metals?
good thermal and electrical conductors
hard and strong
high density
have high melting points
how to separate salt water?
distillation
How to find relative atomic mass? 
Ar = ((Ar of isotope 1 x abundance of isotope 1) + ( Ar2 x abundance 2)) /100
what does miscible mean?
Liquids that do mix
description of graphite?
each atom joined to three more
weak intermolecular forces between ayers
has a high melting point
contains delocalised electrons so can carry electrical current
very soft
atoms arranged in layers
what type of bond do halogens form with metals?
ionic bonds
what are the properties of graphene?
one layer of graphite
better conductor than silver
strong but flexible
not brittle
very light
do metals normally become positive or negative ions?
Positive
what bonds hold metal ions together?
metallic
what are the properties of nanoparticles?
1 nanometer long
contain only a few hundred atoms
very high surface area to volume ration
lightweight
flexible strong
How does something become radioactive?
Extra neutrons in the nucleus make it unstable
how does metallic bonding work?
Strong electrostatic attraction between the negatively charged electrons and the positively charged ions bond the metal ions to each other
what happens to metals and non metals when they ionically bond?
Metals lose electrons, forming positive ions, while nonmetals gain electrons, forming negative ions.
what is an alloy?
Two of more types of metallic substances. they contain atoms of different sizes which distort the arrangement of atoms this makes it more difficult for layers to slide over each other
describe the structures of metallic bonding?
metals are giant structures. the outer electron from each metal is lost to a “sea‘ of free moving electrons surrounding the positively charged ions
How to calculate retention factor?
Distance moved by substance / distance moved by solvent
What are the properties of metallically boneed ions?
good conductors of heat due to delocalised electrons
high melting point due t strong electrostatic charge