7.2 Effective Nuclear Charge 7.3 Size of Atoms & Ions 7.4 Ionization 7.5

Home , Effective nuclear charge, Ionic radius, Shielding effect

Chapter 7

7.2 Effective Nuclear Charge 7.3 Size of Atoms & Ions 7.4 Ionization 7.5 Electron Affinity 7.1 PERIODIC TRENDS

• Arises from the Periodic patterns in ELECTRON CONFIGURATIONS. • Elements in the same GROUP have the same number of VALENCE electrons • VALENCE electrons = electrons in the outermost orbital 7.2 EFFECTIVE NUCLEAR CHARGE

The NET positive charge experienced by an electron. Core electrons pulled in tightly Valence electrons held less tightly Shielding effect reduces the full nuclear charge of outer electrons 7.2 Effective Nuclear Charge BASED On The PERIODIC RECURRENCE Of PROPERTIES

Periodic Trends In 7.3 Sizes of atoms and ions. 7.4 Ionization energy. 7.5 Electron affinity. 7.3 Sizes of atoms

As we move down a group, the atoms become larger . Due to INCREASING value of n 7.3 SIZES OF ATOMS

BUT !! As we move ACROSS a period, {left to right} atoms become SMALLER WHY ? As we move ACROSS the periodic table, the number of core electrons remains constant, but the nuclear charge increases Which of the following ATOMS is largest

N , O , F ?

S or O ?

Na , Mg , Al ?

Na or Cl ?

Na or K ? • CATIONS lose electrons and are SMALLER THAN THE PARENT ION .

• ANIONS add electrons and are LARGER THAN THE PARENT ION . Ions INCREASE in size as you go down a column.

Due to INCREASING value of n. Sizes of Cations Sizes of Anions ISOelectronic series

A group of ions all containing the same number of electrons How many electrons do O2- ; F - ; Na + ; Mg 2+ and Al 3+ have ? 10 -- Increasing nuclear charge O2- > F - > Na + > Mg 2+ > Al 3+ --- Decreasing ionic radius In an isoelectronic series

Ionic size decreases with an increasing nuclear charge {See Text page 269}

Which of the following is largest ?

• Na or K ? • Na or Mg ? • S2– or O 2– ? • S2–, S, or O 2– ? •K+, Cl –, Ca 2+ , or S 2– ? • O 2- , F - , Na + , Mg 2+ , or Al 3+ Arrange the ions K+, Cl –, Ca 2+, and S 2– in

order of DECREASING size .

These form an isoelectronic series of ions Size decreases as the nuclear charge of the ion increases.

The atomic numbers of the ions are S (16), Cl (17), K (19), and Ca (20) Arrange O 2- , F - , Na + , Mg 2+ , Al 3+ according to size

As nuclear charge increases in an isoelectronic series the ions become smaller 7.4 IONIZATION ENERGY

Measure Of How Tightly An ELECTRON Is HELD By The NUCLEUS IONIZATION ENERGY

How Much ENERGY is Required To REMOVE An ELECTRON From An ATOM In Its GROUND STATE

for example

H H + + e - Periodic Trends in Ionization Energies

Ionization energy decreases going down a group

Ionization energy generally increases across a period. Ionization energy decreases down a group

• The outermost electron is more readily removed as we go down a group. Why ? The further the electron is from the nucleus the less tightly it is held Ionization energy generally increases across a period.

As we move across a period, Zeff increases. Therefore, it becomes more difficult to remove an electron. Electron Configuration of Ions

Cations : electrons removed from orbital with highest principle quantum number, n, first: Li (1 s2 2s1) ⇒ Li + (1 s2) Fe ([Ar]3 d6 4s2) ⇒ Fe 3+ ([Ar]3 d5) Anions : electrons added to the orbital with highest n: F (1 s2 2s2 2p5) ⇒ F- (1 s2 2s2 2p6) Ionization Energy & Electron Affinity

Ionization Energy change accompanying loss of electron Na → Na + + e −

Electron Affinity Energy change accompanying addition of electron Cl + e − → Cl − 7.57.5 ElectronElectron AffinitiesAffinities

• Electron affinity is the opposite of ionization energy • Electron affinity is the energy change when an atom gains an electron

Cl( g) + e - →→→ Cl -(g) ELECTRON AFFINITY

THE ENERGY CHANGE THAT OCCUR WHEN AN ELECTRON IS ACCEPTED BY AN ATOM Cl + e - Cl - CLASSIFICATION

BASED ON SUBSHELL BEING FILLED

Representative Elements (s & p electrons) a) ALKALI Metals b) ALKALINE EARTH Metals Transition Elements (d electrons) Lanthanides & Actinides (f electrons)

PERIODIC TABLE Divided Into PERIODS (ROWS) And GROUPS (COLUMNS) I. METALS 1. REPRESENTATIVE a) ALKALI ………GROUP IA b) ALKALINE EARTH……IIA 2. TRANSITION……(B GROUPS) II. METALLOIDS III. NONMETALS WHICH INCLUDE THE HALOGENS AND THE NOBLE GASES.

Selected Properties of Metals, Nonmetals and Metalloids The Alkali Metals

Reactivity increases as we move down the group

WHY? The Alkali Metals

Alkali metals react with water to form the BASE MOH and hydrogen gas:

→ 2M( s) + 2H 2O( l) 2MOH( aq ) + H 2(g) Alkali metal oxides

→ 4Li( s) + O 2(g) 2Li 2O( s) (oxide) → 2Na( s) + O 2(g) Na 2O2(s) (peroxide) → K( s) + O 2(g) KO 2(s) (superoxide) Alkali metal oxides

Metal oxide + water metal hydroxide → Na 2O( s) + H 2O( l) 2NaOH( aq )

The Alkaline Earth Metals

• The chemistry is dominated by the loss of two s electrons: M →→→ M2+ + 2e -. • Be does not react with water. • Mg will only react with steam. • Ca onwards: →→→ Ca( s) + 2H 2O( l) Ca(OH) 2(aq ) + H 2(g)

FigFig 7.147.14 Oxygen • Two allotropes:

–O2

–O3, ozone • Three anions: –O2−, oxide 2− –O2 , peroxide 1− –O2 , superoxide The Oxygen Group

• As we move down the group the metallic character increases

•O2 a nonmetal, Te a metalloid, Po a metal

halogens

All halogens consists of diatomic molecules

Fluorine is one of the most reactive substances known: → 2F 2(g) + 2H 2O( l) 4HF( aq ) + O 2(g) ∆H = -758.7 kJ

The Noble Gases

• They are all nonmetals and monatomic. • They are notoriously unreactive because they have completely filled s and p sub-shells. • In 1962 the first compound of the noble gases was

prepared: XeF 2, XeF 4, and XeF 6. • To date the only other noble gas compounds

known are KrF 2 and HArF. Metals

Metallic character increases down a group. Metallic character decreases across a period. Metals have low ionization energies All group 1A metals form M + ions. All group 2A metals form M 2+ ions. Most metal oxides are basic: Metal oxide + water → metal hydroxide → Na 2O( s) + H 2O( l) 2NaOH( aq ) Nonmetals

Most nonmetal oxides are acidic: nonmetal oxide + water → acid → P4O10 (s) + H 2O( l) 4H 3PO 4(aq ) → CO 2(g) + H 2O( l) H2CO 3(aq ) MetalloidsMetalloids

• Metalloids have properties that are intermediate between metals and nonmetals.

• Metalloids have found fame in the semiconductor industry. End

Chapter 7 Omit Sample & Practice Exercise 7.1 and problems like it

Start with 7.2 : Sizes of atoms P7.8 Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in the n = 3 electron shell K Mg P Rh Ti

What information do I need to answer this question ? P7.18 Using only the periodic table, arrange the following atoms in increasing radius

(a) Cs K Rb ? < ? < ?

(b) In Te Sn ? < ? < ?

(c) P Cl Sr ? < ? < ? 7.24 Select the ions or atoms that are isoelectronic with each other (a) K + Rb + Ca +2 • _____ & _____

(b) Cu + Ca 2+ Sc 3+ • _____ & _____

(d) Fe 2+ Co 3+ Mn 2+ • _____ & ______