Notes

Outline

CHEM 120: Introduction to Inorganic Chemistry Instructor: Upali Siriwardane (Ph.D., Ohio State University) CTH 311, Tele: 257-4941, e-mail: upali@chem.latech.edu Office hours: 10:00 to 12:00 Tu & Th ;  8:00-9:00 and 11:00-12:00  M,W,& F

Chapters Covered and Test dates Tests will be given in regular class periods  from  9:30-10:45 a.m. on the following days: September 22,     2004 (Test 1): Chapters 1 & 2 October 6,           2004(Test 2):  Chapters  3, & 4 October 20,         2004 (Test 3): Chapter  5 & 6 November 3,        2004 (Test 4): Chapter  7 & 8 November 15,      2004 (Test 5): Chapter  9 & 10 November 17,      2004 MAKE-UP: Comprehensive test (Covers all chapters Grading:  [( Test 1 + Test 2 + Test3 + Test4 + Test5)] x.70 + [ Homework + quiz average] x 0.30 = Final Average                                             5

Chapter 3: Elements, atoms, ions, and the periodic table

3.1 The periodic law and the periodic table

Early periodic tables 1817:  Döbreiner's triads – 3 elements w/ regularly varying properties:  S Se Te 1865:  Newlands – "law of octaves", about 55 elements Early tables were based on mass number (A) or “combining weight”

Modern periodic table 1869: Mendeleev and Meyer – "properties of the elements are a periodic function of their atomic weights;" 63-element table. 1913:  Moseley – X-ray emission spectra vary with atomic number (Z) Modern periodic law:

"______:" ______:           horizontal rows (seven in all); properties of elements in period show no similarity. Note that the lanthanides (period six) and the actinides (period seven) are at the bottom of the table

"_______: (families)" _______: (families) are the columns of elements. The elements in the groups have similar chemical properties and predictable trends in physical properties. Groups also have labels. Group A elements are the _____________ elements and the Group B are the ___________ elements. Note that there is another way of labeling the groups with nos. 1-18.

"We give some groups some..." We give some groups some names   IA are the   IIA the   VIIA the   VIIIA the

Metals and nonmetals _______ are shiny, good conductors of heat and electricity, malleable, ductile, and form cations (positive ions, loss of electrons) during chemical change. ___________ are not shiny. They are poor conductors, brittle. They frequently form anions (negative, gain of electrons) in chemical changes.

"Metalloids have some characteristics of..." Metalloids have some characteristics of both metals and nonmetals. They are B, Si, Ge, As, Sb, Te, Po, At. How to tell metals from nonmetals: Be          B                Al    Si               Ge   As              Sb     Te               Po   At

"Some elements are gases at..." Some elements are gases at room temperature: hydrogen, nitrogen, oxygen, fluorine, chlorine, VIIIA’s; two are liquids--bromine and mercury (Hg); the rest are solids.

More info from periodic table                       26 atomic number     Fe chemical symbol 55.85 atomic mass

"Question 3.2 plus a..." Question 3.2 plus a few others:   the symbol of the noble gas in period 3   the lightest element in Group IVA   the  only metalloid in Group IIIA    the element whose atoms contain 18           protons  the element in period 5, Group VIIA Give the name, atomic number and atomic mass for Mg

"For each of the elements..." For each of the elements Ca, K, Cu, Zn, Br and Kr Answer:     which are metals?      which are representative metals?      which tend to form positive ions      which are inert or noble gases

Electron arrangement and the periodic table Electron arrangement: tells us how the electrons are located in various orbitals in an atom--will explain a lot about bonding

Quantum mechanical atom Heisenberg uncerrtainty princple and deBroglie  wave-particle duality concept lead to concept of electrons in orbitals, not orbits. Waves are spread out in space and this concept contradicts the Bohr model where electrons had very specific locations.

"Schrödinger combined wave and particle..." Schrödinger combined wave and particle mechanics (mass) to describe an e- in an atom.  The solns to the eqn are called wave functions. The wave function completely describes (mathematically) the behavior of the e- in an atom.

"A wave function" A wave function  describes an orbital of a certain energy. Not all energies are allowed (energy of e- is quantized). An _______ is a region in space where there is a large probability of finding an electron. Each atomic orbital has a characteristic energy and shape. The concept of quantization is a mathematical consequence of solving the Schroedinger equation, not an assumption.

Principal energy levels (shells) The principal energy levels are designated by the quantum no. n. Allowed values of n: Each e- in an atom can be found only in certain allowed principal energy levels (shells) (designated by the q. no. n)

"Larger the value of n" Larger the value of n, the more likely we are to find the e- at a larger distance from the nucleus with a larger energy (not as stable). Each energy level is subdivided into ________. The number of sublevels in an energy level is equal to the

"n = 1" n = 1 n = 2 n=4

No. of electrons in a principal energy level Each principal energy level can hold at most _________ electrons So n= 1  n= 2 n = 5

Sublevels Principal energy levels are subdivided into sublevels. Sublevels have the designation s, p, d, f and in terms of energy s<p<d<f. The value of n tells us how many sublevels are in a principal energy level.

"So for n = 1..." So for n = 1 there is one sublevel   __. The 1 gives us the principal energy level and the s tells us the type of orbital that is found in that sublevel. For n =2  we have __and __ sublevels making up that energy level. For n= 3 we have For n =4 we have For n=5 we have We don’t worry about any type of orbital (sublevel) beyond f.

Orbitals An orbital is a region in space where there is a large probability of finding an electron. Each orbital can hold at most _ electrons. So an orbital can be Types of orbitals are designated by the s, p, d, f letters.

"The s sublevel is made..." The s sublevel is made up of _ orbital shaped like a sphere and can hold at most _ electrons. The p sublevel is made up of ______orbitals. Since each orbital can hold a maximum of 2 electrons, the set of p sublevels can hold a total of _____ electrons.

"The d sublevel is made..." The d sublevel is made up of ______ orbitals. Since each orbital can hold a maximum of 2 electrons, the set of d sublevels can hold a total of ___ electrons. The f sublevel is made up of ______ orbitals. Since each orbital can hold a maximum of 2 electrons, the set of f sublevels can hold a total of __ electrons.

Slide 29

Slide 30

Slide 31

Electron spin Each orbital can hold at most two electrons. Electrons also have spin (turning on an axis) and have magnetic properties (deflected in magnetic field). Electrons in the same orbital must have opposite spins. If they have opposite spins the electrons are said to be paired.

What to do with all this info? Rules for writing electron configuration: 1. The no. of electrons in neutral atom = atomic no. (no. of protons) 2. Fill the lowest energy sublevel completely, then the next lowest, etc. 3. No more than two electrons can be placed in a single orbital. The electrons have opposite spins in the same orbital. (2 electrons in s, 6 in p, 10 in d, 14 in f)

"4." 4. For n=1, For n =2    For n=3,   For n=4,  Remember the order of filling as follows:

Slide 35

How to remember the energy order 1s 2s  2p 3s  3p  3d 4s  4p  4d  4f 5s  5p  5d  5f  5g 6s  6p  6d  6f  6g  6h 7s 7p   7d  7f

"Let’s do some electron configurations" Let’s do some electron configurations

Abbreviated electron configuration 2He   1s2 10Ne   1s22s22p6 18Ar    1s22s22p63s23p6 36Kr    1s22s22p63s23p64s23d104p6 These configurations are for ground state configurations--lowest energy.

Valence electrons Valence electrons are the electrons located in the _________ orbitals and are the ones involved in forming chemical bonds. The valence electrons have the largest _ value for the A elements. For representative elements the number of valence electrons in an atom =

"Don’t worry about inner core..." Don’t worry about inner core of electrons (smaller n) since these are filled levels and don’t enter into bond formation ( for A groups)

Valence electron configuration for A groups Group IA Group IIA Group IIIA Group IVA Group VA Group VIA Group VIIA Group VIIIA

Where do you get the numerical value for the n for the valence electrons? You find the _______ number!!! Can you use this information to make electron configuration easier?

"Valence electron configuration for:" Valence electron configuration for: P Bi Sr Te I Cs

The octet rule It has been noted that extra stability occurs when an atom or ion has 8 electrons in the outermost energy level (2 or 0 for the first period).

"Group IA" Group IA    ns1 Lose Group IIA   ns2 Loses Group IIIA  ns2np1 Loses Group IVA  ns2np2 Group VA    ns2np3 Gains  Group VIA   ns2np4 Gains Group VIIA  ns2np5 Gains Group VIIIA  ns2np6

"Group IA" Group IA Group IIA Group IIIA Group VA Group VIA Groupr VIIA Names of ions: for cations--name of element plus ion For anions: replace the last syllables of the element name by --ide + ion.

Transition metal cations No simple rules as for A groups Cu+, Cu2+ Fe2+, Fe3+ Au+, Au3+

"H-" H- H+ Li+ Be2+ B3+ N3- O2- F-

What’s the ion formed by P Ba S N I Cs

Slide 50

Isoelectronic Atoms or ions F- [He] 2s2 2p6 O2- [He] 2s2 2p6 Name a cation isoelectronic with O2-

Question Which of the following pairs of atoms and ions are isoelectronic? Cl-, Ar Na+, Ne Mg2+, Na+  Li+, Ne O2-, F-

"Which of the following groups..." Which of the following groups are isoelectronic with each other? Na+, Mg2+, Ne Cl-, F-, Ar Na+, Mg2+, Al3+, N3-, O2-, F-, Ne

3.4: Trends in the periodic table Think of atom as sphere whose radius is determined by the location of the e’s furthest from the nucleus. So atomic radius (size) determined by: 1. Larger value of n for atom in a group, the larger the atom size. Size _________ from top to bottom in group.

Size across a period As go across a period (n stays the same), the no. of protons in the nucleus increases. The e’s are very spread out and each electron feels the pull of the increasing +charge of the nucleus uninfluenced by the other electrons and size __________ as go from left to right across a period.

Slide 56

"Group" Group     size increases Period   size decreases (with some exceptions)

Slide 58

"Arrange each of the lists..." Arrange each of the lists according to increasing atomic size: Al, S, P, Cl, Si In, Ga, Al, B, Tl Sr, Ca, Ba, Mg, Be P, N, Sb, Bi, As Na, K, Mg

Ion size Same charge, in group, size __creases Size of parent to cation: Parent   cation Size of parent to anion: Parent   anion Fe2+   Fe3+

"Which is smaller?" Which is smaller? Cl or Cl- Na or Na+ O2- or S2- Mg2+ or Al3+ Au+ or Au3+

Slide 62

"Note for isoelctronic series:" Note for isoelctronic series:  Na+, Mg2+, Al3+, N3-, O2-, F-, N3-> O2-> F-> Na+> Mg2+> Al3+ Most positive ion the smallest, most negative the largest

Ionization energy Minimum energy required to remove an electron from a ground-state, gaseous atom Energy always positive (requires energy) Measures how tightly the e- is held in atom (think size also) Energy associated with this reaction:

Trends in ionization energy Top to bottom in group: 1st I.E. __creases. Why? Across a period, 1st I.E. __creases (irregularly)  Why?  Note that noble gases have the largest I.E. in a given period; the halogens the next highest; the alkali metals the lowest, etc.

Slide 66

Slide 67

Arrange in order of increasing I.E. N, O, F Li, K, Cs Cl, Br, I

Electron affinity Electron affinity is energy change when an e- adds to a gas-phase, ground-state atom Energy associated with this reaction: Positive EA means that energy is released, e- addition is favorable and anion is stable! First EA’s mostly positive, a few negative

Trends in  electron affinities Decrease down a group and increase across a period in general but there are not clear cut trends as with atomic size and I.E. Nonmetals are more likely to accept e-s than metals. VIIA’s like to accept e-s the most.

Slide 71