group 1/group 7 /group 0 and transition metals Flashcards
what is group 1 also referred as
alkali metals
how many electrons do group 1 have in their outer energy level
1
what are the properties of the group 1 alkali metals
– soft
- relativly low melting/boiling points ( alkali metals melt at low temperatures )
-low density
-highly reactive with oxygen , chlorine and water
- when they react they all form a 1+ charge
how do the group 1 metals react with oxygen
lithium = reacts rapidly with oxygen
sodium = reacts more rapidly with oxygen than lithium
potassium = reacts even more rapidly with oxygen than sodium / lithium
conclusion: group 1 react rapidly with oxygen BUT as you move down the group the elements react more rapidly
what does group 1 react rapidly with
chlorine , oxygen,water
how do group 1 react with water
lithium = reacts rapidly + violently with water - see effervescence and bubbling
sodium = more violent/ rapid than lithium-
potassium = extremely rapid and violent
why does group 1 reactivity increase as you go down
the radius of the atoms increases - so there is a greater distance between the positive nucleus and the negative outer electron, as distance increases the outer electron is less attracted to the nucleus = make the outer electron easier to lose
ALSO, the outer electron is repelled by electrons in the internal energy levels ( this is called shielding ) = decreasing the attraction between the nucleus and outer electron, as you go down group 1 the elements have more electrons in the internal energy levels therefore shielding increases as you go down
what are the group 0 also referred as
noble gases
what type of elements are noble gases
unreactive elements
why are noble gases unreactive
atoms are only stable when they have a full outer energy level- as each element in grp 0 has a full outer shell they are unreactive as they dont lose/gain and electrons
why are group 0 elements gases at room temperature
because all grp 0 have boiling points lower than room temperature
what happens to the boiling point of group 0 as you go down the group
boiling point increases as relative atomic mass increases
what is group 7 also referred as
halogens
what type of metals are group 7
non metals
how are group 7 molecules bonded to eachother
by 2 atoms joined covalently
what happens to the melting point and boiling point of group 7 as you go down the group
increases
how can we use group 7 melting / boiling points to determine if an elemnt is gas, liquid / solid
if boiling point is less than room temp (20) then it is a gas
what state is it in if thge boiling point is lower than 20 degrees
gas
what state is it in if the melting point is lower than room temperature
liquid
what state is it in if the melting point / boiling point are both higher than room temperature
solid
what happens to the relative molecular msas as you go down group 7
increases ( the molecules get bigger )
what is the product of the reaction between 2 non - metals
a covalent compound
what is an ion
an atom with an overall charge
what is the product of a reaction between a non metal and a metal ( a halogen)
an ionic compound
what happens to the reactivity of the elements as you go down group 7
decreases
why does the reactivity decrease as you go down group 7
a ———— reactive halogen can displace a ———— reactive halogen from an aqueous solution of its salt
more , less
example:
sodium bromide + flourine –>?
flourine is more reactive than bromine so th ereaction becomes
= sodium bromide + flourine –> sodium flouride + bromine ( flourine displaced bromine)
what are the properties of the transition metals
- hard and strong
- all have high melting points ( except mercury which is liquid at room temp)
-high density - much less reactive than group 1 ( transition metals react slowly with oxygen , chlorine and water )
-form ions with different charge
-form coloured compounds
-useful as catalysts
