sdirectcros.blogg.se - Periodic table of elements with trends

Metallic character decreases across period from left to right.

These trends occur due to combination of trends above.

Also because of shielding effect weakens forces between nucleus and outer electrons. This is because atomic radii increase down group, making easier to remove electron.

Electronegativity decreases down a group from top to bottom.

This is because since electrons are pulled closer to nucleus (see atomic radius), more difficult to remove them.

Electronegativity increases across period from left to right.

Same as ionization energy for same reasons.

Relative attractions that an atom has for a shared pair of electrons in a covalent bond.

Decreases down a group from top to bottom (becomes less negative.

Increases across a period from left to right (becomes more negative.

Negative sign meaning energy released (exothermic).

The change in energy released which accompanies addition of an electron to an atom in gaseous state.

IE decreases down a group from top to bottom.IE increases across period from left to right.Positive sign meaning energy used (endothermic).Second ionization energy IE 2 is energy required to remove electron from IE 1.First ionization energy IE 1 relates to process:.The minimum energy required to remove 1 mol of electrons from 1 mol of neutral gaseous atoms in ground-state.This is because the extra electron in the anion results in greater repulsion between valence electrons, thus larger radius. This is because there are more protons than electrons in the cation, so valence are more strongly attracted to nucleus. Radii of cations and anions are different from parent atoms.Distance from center to the outer most region in ion.Each new period begins with new energy level which is farther from nucleus, increasing atomic radius. Atomic radius increase down group from top to bottom.Nucleus’s positive charge is greater relative to charge of electrons in same shell, pulling electrons closer to nucleus and thus reducing atomic radius Atomic radius decreases across period from left to right.Way of finding radius would be to measure distance between two atoms in diatomic molecule X 2 and divide by two for the radius.Bohr model has orbits, thus radius can be measured easily however we know that this is highly simplistic.Distance from center to the outer most region.Atomic properties show pattern amongst the period table which can be classified as trends 6 trends need to know: D.7 (HL) Taxol – a chiral auxiliary case studyĮlectron configuration help determine atomic properties.D.6 Environmental impact of some medications.D.1 Pharmaceutical products and drug action.C.8 Photovoltaic and dye-sensitized solar cells.C.6 Electrochemistry, rechargeable batteries and fuel cells.

C.5 Environmental impact – global warming.A.10 Environmental impact – heavy metals.A.8 Superconducting metals and X-ray crystallography.A.2 Metals and inductively coupled plasma (ICP) spectroscopy.21.1 Spectroscopic identification of organic compounds.18.2 Calculations involving acids and bases.16.1 Rate expression and reaction mechanism.14.1 Covalent bonding and electron domain and molecular geometrics.The periodic table – the transition metals 11.3 Spectroscopic identification of organic compounds.11.1 Uncertainties and errors in measurements and results.6.1 Collision theory and rates of reaction.1.1 Introduction to the particulate nature of matter and chemical change.