8.1 Periodic table
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How is periodic table structured
List of elements in order of atomic number. Metals on left, transition metals in centre, non metals on right. Metalloids run diagonal, splitting metals and non metals
How are metals and non metals split
staircase line: divides them. Metalloids touch this line, eg Silicon, which have a combination of metallic and non metallic properties
What did Mendeleev do
. Realised there were undiscovered elements, so left gaps for them . . Arranged the known ones, so similar ones lined up in columns . Since then new ones were discovered which fit the gaps, so he predicted the properties of missing elements
Lanthanides and actinides
The bottom block of the periodic table, they’re omitted
Where is the s block of periodic table, what is it
Far left, group 1 and 2 Elements that have their highest energy electrons in s orbitals are in the s block
Where is p block of periodic table What is it
Far right, group 3,4,5,6,7,0 Elements that have their highest energy electrons in p orbitals are called p block
Where is d block What is it
Centre, transition metals Elements that have their highest energy electrons in the d orbitals are the d block
Where is F block What is it
Under periodic table, the lanthanides and actinides. Elements that have their highest energy electrons in f orbitals.
Why are transition metal elements and d block not the same
. Scandium and zinc aren’t transition metals because they don’t form any compounds that have partly filled d orbitals, which is the characteristic of transition metals.
Why are they called S, D, P,F blocks How do you remember the order
When elements are heated they give out light energy at certain wavelengths, and as excited electrons fall back from one energy level to another. This causes lines to appear on spectrum of light they give out. Letters stand for words given to describe the light eg d for diffuse Super duper power
What is a group
Vertical column of elements, elements in the same group have similar properties, and same number of electrons on outer shell.
How does reactivity in S block change down the group
Elements get more reactive going down group
How does Reactivity change down the P block
Elements get more reactive going up the group
Transition metal reactivity/ d block
They’re all quite unreactive, lots of useful metals are found here
Actinide properties
All radioactive eg uranium and thorium form naturally in earths crust
What are periods
. Horizontal rows of elements eg period 1 only has hydrogen and helium
How are hydrogen and helium placed
. Helium above noble gases because of its properties, but it isn’t a p block element, its electron arrangement is 1s^2 . Hydrogen is above group 1, and forms 1+ ions (H+) like the group 1s. However hydrogen is a gas, and not a metal.