Trends in the Periodic Table
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| 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
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| 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.
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| 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
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| 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
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| 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.
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| Why do the values of ionisation energy increase across the periods in the Periodic Table? | - Increasing nuclear charge
- Decreasing atomic radius
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| Why do the values of electronegativity decrease down the groups in the Periodic Table/ | - Increasing atomic radius
- Screening effect of inner electrons
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| Why do the Electronegativity values increase across the periods in the Periodic Table? | - Increasing nuclear charge
- Decreasing atomic radius
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| What is the meaning of the term "Bond Length"? | The distance between the nuclei of two bonded atoms measured by x-ray diffraction
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| What is 2nd Ionisation energy? | its the energy required to remove an electron from an ion with one positive charge in the gaseous state.
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| What does the term "n=3" refer to? | third energy level or orbital.
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| The chemical properties of an element are largely determined by the ..? | Number of electrons in the outermost energy level.
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| All the Alkali metals react with Oxygen to produce.. | Metal Oxides.
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| Why is it important not to put Alkali metals into dilute acid? | An explosion occurs due to so much Hydrogen being produced.
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| An Alkali Metal + Water reacts to give ...( Na + H2O) | A Metal Hydroxide and Hydrogen
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| What group number are the Halogens? | VII
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| Do Halogens exist free in nature? | No
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| What is the trend in reactivity of the Halogens? | Increases as you go up the group
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| More reactive Halogens will .............. the less reactive Halogens from a solution of their ions | Displace
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| 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.
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| 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
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Created by:
FROmine
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