The Periodic Law Modern Chemistry 2009 Holt Rinehart

The Periodic Law Modern Chemistry © 2009 Holt, Rinehart, & Winston Chapter 5, pp 133 - 165

Periodic Law • Chemical & physical properties regularly repeat when elements are listed according to their atomic numbers § Atomic number is equal to # of protons § # of protons = # of electrons § # of valence electrons = Group # for s block = (Group # - 10) for p block o “Main-group elements” are those in the s & p blocks o Properties are determined mostly by valence electrons

Contributors • Stanislao Cannizzaro – Reliable method of measuring atomic mass • Dmitri Mendeleev – Group elements of similar properties together – Arrange groups according to their atomic masses • Henry Moseley – Rearrange elements according to atomic numbers – Maintain groupings according to properties

Mendeleev’s Periodic Table

Periodic Properties’ Trends • Atomic & ionic radii: as go left & down – Across the period, nuclear charge increases. • As the positive charge increases, electrons are pulled in more tightly, thereby the radius. – Down the group, the # of energy levels increase. • Cations have smaller ionic radii than the atom. – When the valence electron shell is lost, the ion is smaller • Anions have larger ionic radii than the atom. – Extra electrons do not compact as readily, mostly because of their electrostatic repulsion for each other.

Trends in Atomic radii

Periodic Properties’ Trends • Ionization energy = energy required to remove electron from neutral atom § as you go right across the period o As nuclear charge increases, electrons are held more tightly. § as you go down the group o As energy levels are added, electrons are held more loosely. o Additional layers of electrons shielding of protons and further repel valence electrons.

Periodic Properties’ Trends • Electron affinity = energy change accompanying acquisition of electrons by neutral atoms. § Most atoms release energy when get electron. o Released energy is noted as a negative value. Ø A + e- A- + energy F has the highest value of -339. 9. o Positive or less negative values indicate atom was “forced” to get electron, i. e. , energy was absorbed. o Most atoms so forced will spontaneously lose electron. Ø A + e- + energy A- Values are often listed as “(0)”.

Periodic Properties’ Trends • Electronegativity = ability to attract electron in a compound • F has highest value of 4. 0; others are relative. § Fluorine becomes most like a noble gas (filled valence shell = greater stability) when is F-. • Fr/Cs has lowest. § Alkali metals are energetically most stable when they lose their valence electron, not gain one.

Additions to Periodic Table • Noble gases – 1894: Ar; 1895: He; 1898: Kr & Xe; 1900 Rn • Lanthanides – Early 1900 s – Very similar in chemical & physical properties – Soft and shiny; reactivity like alkaline-earth metals • Actinides – All are radioactive; 1 st 4 are natural, rest synthetic – Those after uranium are “transuranium elements”.

The s-Block Elements • Group 1 = alkali metals (but H is a nonmetal) – Electron configuration for all end in ns 1 – The most reactive of all elements (with air or H 2 O) • Never found free in nature; stored in kerosene – Are silvery and soft • Group 2 = alkaline earth metals – Electron configuration for all end in ns 2 – Too reactive to be found free in nature • Used in fireworks (Mg – white; Sr – red) – Harder, denser, stronger than alkali metals

d-Block, or Transition, Elements • Less reactive than elements of the s-block • May have different # valence electrons/ group – Sum of outer s & inner d electrons = group # • Have typical metal characteristics – Good conductors of electricity – High luster • Some are don’t react, staying free in nature – Pt, Pd, & Au are least reactive metals

The p-Block Elements • All have filled s-orbitals • Includes metals, all metalloids, & nonmetals – Metals: Al, Ga, In, Tl, Sn, Pb, Bi, Po, & Uuq & Uuh – Metalloids: B, Si, Ge, As, Sb, Te, & (At) • Properties of both metals and nonmetals • Brittle solids; have luster • Semi-conductors – Nonmetals: noble gases, halogens, O, S, N, P, C, Se • Halogens are the most reactive of all nonmetals • Halogens have all 3 states of matter in their group

Trends for p- & d-blocks • Atomic radii: going right across period • Ionization energy (IE): going right across period & going down the group for the 1 st IE – Outer s electrons are less shielded by d electrons • Ion formation & radii: all lose ns 2 electrons 1 st – Ions of a 2+ charge in size across period • Electronegativity: {F = 4. 0; others are relative} – d block: all are 1. 1 – 2. 54 – f block: all are 1. 1 – 1. 5 – Inversely proportional to atomic radii for both.

Trends in d block