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The periodic table is arranged by..
Proton number
Why do elements in the same group have similar properties?
Because they have the same number of electrons in their outer shell
What does the group number tell you?
How many electrons are in the outer shells
What is the trend in atomic radius across a period?
It decreases
True/ False, atomic radius decreases across the group because the positive charge of the nucleus decreases?
False, nuclear charge increases across a period
Who do the melting points of Na, Mg and Al increase across period 3?
Metal-metal bonds get stronger. The metal ions have an increasing positive charge, increasing number of delocalised electrons and decreasing radius
What type of substances are P4, S8 and Cl2
Molecular
Why does Argon have a very low melting point?
Its monatomic- very weak VDW forces as it exists as individual atoms
What is the trend in ionisation energy across period 3 and why?
Increases (generally) due to increasing attraction between outer shell electrons and the nucleus due to increased nuclear charge
Why does atomic radius increase down group 2?
Extra electron shells are added as you go down the group
Explain the trend in ionisation energy down group 2.
Decreases due to extra electron shells which causes increased shielding. Extra shells mean outer electrons are further away from the nucleus weakening attractio
Explain the trend in melting point down group 2
Decreases. Ions get bigger but delocalised electrons and charge stay the same.delocalised electrons get further away from nucleus, easier to break bonds
What is the trend in solubility of group 2 hydroxides
Solubility increases down the group
What is the trend in solubility of group 2 sulfates down the group
Solubility decreases
What is barium sulfate used for in medicine
to see images of soft tissues in the body on xrays
Explain the trend in oxidising strengths of the halogens
Become less oxidising down the group.Atoms get bigger, outer shell electros further from the nucleus, less forces of attraction
