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Ch. 7

Trends in the Periodic Table

TermDefinition
Atomic radius (covalent radius) Half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent bond
Why do values of atomic radius increase down any one group in the Periodic table? - A new shell further from the nucleus - The screening effect of inner electrons.
Why do values of atomic radius decrease from left to right across any period of the Periodic Table? - Increasing nuclear charge - No increase in the screening effect
The first ionisation energy is.. Is the minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in its ground state
Why do the the values of ionisation energy decrease down the groups in the periodic table? - Increasing atomic radius - The screening effect of inner electrons.
Why do the values of ionisation energy increase across the periods in the Periodic Table? - Increasing nuclear charge - Decreasing atomic radius
Why do the values of electronegativity decrease down the groups in the Periodic Table/ - Increasing atomic radius - Screening effect of inner electrons
Why do the Electronegativity values increase across the periods in the Periodic Table? - Increasing nuclear charge - Decreasing atomic radius
What is the meaning of the term "Bond Length"? The distance between the nuclei of two bonded atoms measured by x-ray diffraction
What is 2nd Ionisation energy? its the energy required to remove an electron from an ion with one positive charge in the gaseous state.
What does the term "n=3" refer to? third energy level or orbital.
The chemical properties of an element are largely determined by the ..? Number of electrons in the outermost energy level.
All the Alkali metals react with Oxygen to produce.. Metal Oxides.
Why is it important not to put Alkali metals into dilute acid? An explosion occurs due to so much Hydrogen being produced.
An Alkali Metal + Water reacts to give ...( Na + H2O) A Metal Hydroxide and Hydrogen
What group number are the Halogens? VII
Do Halogens exist free in nature? No
What is the trend in reactivity of the Halogens? Increases as you go up the group
More reactive Halogens will .............. the less reactive Halogens from a solution of their ions Displace
What accounts for the increasing Boiling Points of the Halogens as you go down the group? Increasing Van Der Waals Forces due to increasing sizes of molecules.
Why do some elements have first ionisation energies that are much greater than expected. (Don't conform to the general trends) Atoms with filled and half-filled outer sub-levels have an increased stability leading to a greater 1st ionisation energy requirement
Created by: FROmine