hnrs 227 lecture 11 chapter 8 and chapter 9 the periodic table and chemical reactions presented by...
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HNRS 227 Lecture 11 Chapter 8 and Chapter 9
The Periodic Table and Chemical Reactionspresented by Prof. Geller with materials from Prof. Taylor
Recall from Chapter 8History of atomic theory
Electron and nucleus (protons and neutrons in nucleus both made up of quarks)
The Bohr Model of the Atom The Quantum Concept Bohr’s Theory
Quantum Mechanics Quantum numbers
Principal, angular momentum, magnetic, and spin
Electron Configuration Pauli Exclusion Principle Filling of orbital shells
Periodic Table of Elements
An underlying principle most stable state for an atom is one in
which the outermost shell is filled with the maximum number of electrons
1st Shell (1 orbit; 2 electrons) Hydrogen (1
1H; 1 electron; stable ?) Helium (2
4He; 2 electrons; stable ?)Periodic Table’s 1st Row
Hydrogen and Helium
Periodic Table of Elements
2nd shell has 4 orbits with 2 electrons (maximum) per orbit (total of 8 electrons/shell)
Most stable configuration is the following: 1st shell filled with 2 electrons 2nd shell filled with 8 electrons Total of 10 electrons (10
20Ne)
2nd row of Periodic Table 8 elements (list and relate to the above)
Periodic Table of Elements
3nd shell has 4 orbits with 2 electrons maximum per orbit (total of 8 electrons/shell)
Most stable configuration is the following: 1st shell filled with 2 electrons 2nd shell filled with 8 electrons 3rd shell filled with 8 electrons Total of ___ electrons (18
40Ar)3nd row of Periodic Table
8 elements (list and relate to the above)
Periodic Table of Elements
Rows Number of elements in a row is not
chance but reflects the maximum number of electrons in the outermost shellRow 1 = 2Row 2 = 8Row 3 = 8Row 4 = 18etc
Periodic Table of Elements
Columns Elements in a given column have similar
chemical properties All elements in column have the same
number of valence electrons Column IA has 1 electron in outer shell Column IIA has 2 electrons in outer shell Column IIIA has 3 electrons in outer shell Column IVA has 4 electrons in outer shell Column VA has 5 electrons in outer shell
Periodic Table of Elements
Taylor’s Take Home Message
Atoms are the chemical building blocks of all matter Structure of atoms (electrons, neutrons, protons
and their arrangement) determine the unique behavior/attributes of the elements
Of the above (No. 2), the “place” and “pairing” of the electrons are the most critical in chemical reactions
Electrons reside in defined shells (orbits) surrounding the nucleus of the atom and the electrons in the outermost shell (valence electrons) determine an atom’s chemical reactivity
Utility and periodicity of the Periodic Table of Elements is a function of the distribution of all electrons in shells, the valence electrons in the outermost shell, and the mass of the element
Chemical Reactions and BondsChapter 9
Review valence electronsPrinciples of “Bonds Away”Ionic BondsMetallic BondsCovalent BondsIntermolecular ForcesCommon Chemical Reactions
Taylor’s Take Home Message
When atoms combine to produce molecules and compounds, expect the chemical properties of the molecules/compounds to be far different than that of the constituent atoms (hierarchy theory)
Atoms bind together by re-arranging and sharing electrons Ionic bonds Metallic bonds Covalent Bonds Intermolecular forces (e.g., hydrogen bond)
Chemical interactions make and break bonds between atoms and in so doing effect a change in energy (potential and kinetic)
Weak chemical bonds (e.g., covalent bonds) play a very important role in the chemistry of life
Chapter Items that won’t be emphasized from Chapter 9
p. 184 A Closer look
p. 186 A Closer Look
pp. 188-191 Percent Composition of Compounds Ion Exchange Reactions
Atoms in Proximity:Chemical Bonds
Chemical Action when two atoms are brought together,
electrons will tend to re-arrange themselves to the lowest energy state where the valence electrons are most stable
Chemical Reaction electrons are re-arranged into bonds
Give away electronsAccept electronsShare electrons
Ionic Bonds
Some atoms give away electrons whereas other atoms receive electrons
Example of lithium (Li) chloride (Cl)
36Li + 17
35.5Cl = LiCl
Ionic Bonding
Lithium (Li)
Li gives up 1 electron and is left with 2 electrons (-) and 3 protons (+); net positive (+) charge
Chlorine (Cl)
Cl has 1 unpaired electron in valence shell, so Cl tends to accept an electron and is left with 18 electrons (-) and 17 protons; net negative (-) charge
Ionic Bonding Summary
Some atoms give away electrons while other atoms receive electrons
Example of lithium chlorideLi + Cl = LiCl
Bonding via electrical attraction between Li+ and Cl- Li+ + Cl - = Li+Cl-
Consequence: ionic bonds are underpinned by charged ions and tend to form crystals of very specific and repeating geometry (very rigid)
Example: NaCl is based on ionic bonds and is salt
Ionic Bond Example: Salt
Metallic Bonds
Some elements do not give or take electrons (ionic bonds) BUT share electrons
Valence electrons tend to move freely between both atoms (contrast with ionic bonds)
Significance of sharing electrons: compounds tend to show two features Malleability (easily worked or pounded) Conductive of electricity (good conductors)
Examples Gold jewelry Copper wire
Covalent Bonds
Extremes of behavior in bonding Accept or give away electrons (ionic bonds) No tendency to share (noble gases)
Intermediate between these two extremes but Do not form ionic bonds Do not form metallic bonds Yet share 1, 2, 3 and 4 electrons in unique
arrangement called covalent bondsKey: orbits of valence electrons are shared so that
electrons are shared (and move) between valence shells of adjacent atoms
Covalent Bond Example
Example of hydrogen fluoride (HF)1
1H and 919F
Note: Valence shell for both atoms are full Single bond shared Double bond
Covalent Bonds with Carbon
612C is a special case (profoundly important)
Valence electrons for C are 4 (1 in each orbit) and intermediate between giving and accepting
C - C single covalent bond (1 orbit) C C - C two covalent bonds involving 2 orbits Unique behavior of C C
C-C-C (or H or N or __)
C
Behavior of Valence Electrons
Five Options No action (e.g., inert gases) Give away one or more electrons in
valence state (positive ion leading to ionic bond)
Accept one or more electrons to valence state (negative ion leading to ionic bond)
Share an electron with many other atoms without respect to an orbit (metallic bond)
Share one or more electrons plus their orbits with another atom (covalent bond)
Regarding Next Week’s Lab: Evaporation and Chemical Structure
Vaporization and chemical properties of molecules Liquid to gas state change State change has energy cost:
endothermic (temperature decrease)Temperature change is a function of
chemical structure of molecule Bonding and polarity
Evaporation and Chemical Structure
Organic compounds Carbon based or hydrocarbons bond with other
elements via covalent bonds)Alkanes: C and H only
• Pentane (C5H12)Alcohols: C, H and OH (hydroxyl group)
• Ethanol (C2H5OH)• Structural formula
Hydrogen bonding: H bonded to N, O or F (tight bond)
Process: as chemical vaporizes, temperature change is chemical specific and is a “window” onto the chemical structure of molecule
Evaporation and Chemical Structure
Hypothesis temperature changes with vaporization in a
manner that is predictable, based on the bonding among atoms involving C, H and OH
Method Measure temperature change electronically Record for 6 hydrocarbons Analyze data (graphically) based on
understanding of the bonds for each molecule
Intermolecular Forces: Polarization & Hydrogen Bonding
Example of water (H2O)+H H+
O-
When one molecule’s distribution of atoms results in one side of the molecule having either a + or – charge
Resulting distribution of charges causes adjoining H2O molecule to align itself with + and – charges to be most stable
Called “polarity” of molecule (e.g., magnet) Relate to lab exercise: greater polarity, greater
bonding and less evaporation (less temperature change)
Intermolecular Forces: Van der Waal Forces
In polarity, specific and rigid + and – fields on each molecule that does not change over time
When molecules converge, inevitable that electrons shift and re-distribute (e.g., planar compound)
In re-distribution, small net attraction between molecules arise and two molecules for weak bond Graphite pencil lead Stack of paper
Acid – Base Reaction: Measurement
pH scaleAny increase in H+ results in more acid
solution from 7 to 0Any increase in OH- results in more basic
solution from 7 to 14Examples
Rainwater of 5.6 means what? Cell pH value of 6-8 means what? Importance to biological systems and buffering
Taylor’s Take Home Message
When atoms combine to produce molecules and compounds, expect the chemical properties of the molecules/compounds to be far different than that of the constituent atoms (hierarchy theory)
Atoms bind together by re-arranging and sharing their electrons Ionic bonds Metallic bonds Covalent Bonds Intermolecular forces (e.g., hydrogen bond)
Chemical interactions make and break bonds between atoms and in so doing effect a change in energy (potential and kinetic)
Weak chemical bonds (e.g., covalent bonds) play a very important role in the chemistry of life