Periodic Table Flashcards
Does reactivity increase or decrease down group 1? Why?
Increase
The atoms get larger, so the electrostatic attraction between the outer electron and the positive nucleus is weaker so the electron is more easily lost
Does reactivity increase or decrease down group 7? Why?
Decrease
The atoms get larger, which means the electrostatic attraction between the positive nucleus, and the electron being gained is weaker, which makes it harder to gain the electron
Do transition metals have a high or low melting point?
High
Does mp/bp increase or decrease down group 1?
Decreases
Does mp/bp increase or decrease down group 7?
Increases
Are transition metals reactive?
Not really
Are transition metals good conductors?
Good thermal conductors
Are group 1 metals good thermal conductors?
👍
Colour of the compounds group one metals make
White
What colour are the compounds that transition metals make?
Various colours
Do both group 1 metals and transition metals form ionic compounds with non metals?
👍
Are group one metals ALL diatomic??
NO
none are
Group seven is made up of all diatomic molecules
What is the name given to group 7
Halogens
What’s the name given to group 0/8??
Noble gases
What’s special about the electron structure of the noble gases?
Full outer shells
Are noble gases reactive?
No because they have full outer shells and do not need to share or transfer electrons
Some food packets contain argon gas - why??
It’s unreactive so the food will not go stale and will stay fresh
Argon is the most abundant noble gas
Intermolecular forces _________ down the group
(Noble gases)
Increase
Give two differences between the physical properties of elements in group 1 and those in the transition elements
Group one has low density
Group 1 has relatively low mps
Relative Melting points across table
⬇️ ⬆️ ⬇️ ⬇️
Groups:
1. Tm. 7. 0.
Reactivity across table
Down group reactivity
⬆️. ❌. ⬇️. ❌.
Describe Newlands table
He arranged them in order of increasing atomic mass
He found that every eight elements had similar properties, so arrange them in eight groups
He called it, the law of octaves
What problems were found with Newlands table, and why wasn’t it accepted?
There were no gaps left for undiscovered elements, so there were many more dissimilar elements in a column and no room for new elements
Mandeleev organise the elements in order of…
Atomic weight
Also known as relative atomic mass
Mandeleev organise the elements in order of atomic weight. This meant that some elements were…
In the wrong order, and sometimes place in groups with elements that were similar
This led to pair reversals
E.g. iodine and Tellurium
Iodine has low atomic weight, however, similar chemical properties to chlorine and bromine so they were switched
Two special features of Mandeleev periodic table were…
It had gaps
It showed elements with similar chemical properties lined up in groups
The gaps in Mandeleev’s periodic table were important, because
It was easier to make predictions about undiscovered elements and their properties
How is the periodic table organised now?
Elements
- organised in order of creasing atomic number
- groups of elements with similar properties
What does the period number tell us?
The number of occupied electron shells
What does the group number tell us?
The number of electrons in the outer shell of an element
What does the term periodic mean in terms of the periodic table?
Repeating properties
How were the pair reversals resolved?
Isotopes
Because tellurium is 128, 130 was so abundant
