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45 Cards in this Set
- Front
- Back
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who first used the term geochemistry?
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swiss chemist Schonbein in 1838
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science consists of two parts. what are they?
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1) the knowledge it encompasses
2) the approach that achieves that knowledge |
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science consists of two quantities. what are they?
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observations and theories
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atomic number
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used to sort periodic table and is the number of protons in the nucleus
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mass of an atom
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proton number + neutron number, however an atom can have multiple neutron variations (isotopes)
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atomic weight
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depends on the masses of the various isotopes and their relative abundance
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what did Thompson do in 1918?
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demonstrated the existence of two Ne isotopes
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what are the four quantum numbers and what are they labeled?
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principal, n
azimuthal, l magnetic, m spin, m_s |
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What does the principal, n, determine? What are typical values?
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1,2,3...
determines electron's energy as well as mean distance from the nucleus |
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What does the azimuthal, l, determine? What are typical values?
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0,1,2,3...n-1
determines the total angular momentum and the shape of the orbit |
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What does the magnetic, m, determine? Typical values?
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-l...0...l
determines the z component of angular momentum and therefore the orientation of the orbit |
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What does the spin, m_s, determine? Typical values?
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-1/2, 1/2
determines the electron's spin |
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The first three quantum numbers say what about the electrons surrounding the nucleus
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they are organized into shell, subshells, and orbitals
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What does the Pauli Exlusion Principle say?
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requires that no two electrons in an atom may have identical values of all four quantum numbers
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What is the first shell/period called? How many subshells? Quantum numbers?
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K shell, one subshell (1s),
n=1, l=0, m=0. 2 elements: H and He |
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What is the second shell called? How many subshells?
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shell: L
2 subshells: 2s(l=0), 2p(l=1) |
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How many orbitals does the p subshell have?
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3(m=-1,0,1)
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How many electrons can the L shell accept?
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8 (8 elements in period 2)
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What is the third shell called?
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M
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Why is the 3d subshell vacant in period 3?
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the possibility is therem but is energetically less favorable than electrons going in the subsequent shell.
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When do 3d subshells begin to fill?
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After the 4s orbital is filled
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Which orbitals correspond to the transition series metals, Sc through Zn?
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5 3d orbitals
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Which orbitals correspond to the 2nd and third transition series metals?
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4d and 5d orbitals
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The filling of the 4f shell correspond to which rare earth elements?
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Lanthanide
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The filling of the 5f shells correspond to which rare earth elements?
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Actinide
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How many electrons can each subshell level hold respectively: s,p,d,f
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2,6,10,14
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What are the elements of group 1 called?
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alkalis--all have 1 electron in outermost s orbital
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What are the group 18 elements called?
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noble gasses--all have filled p subshell
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First Ionization Potential
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Energy required to remove the least tightly bound electron.
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Second Ionization Potential
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Energy required to move a 2nd electron, etc.
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electron affinity
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energy given up in reactions:
ex. F + e- = F- |
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electronegativity
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differences in bond energy between an A-B molecule and the mean energies of A-A and B-B molecules. It quantifies the tendencty of an element to attract to a shared electron when bonded to another element
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In general, 1st ionization potential, electron affinity and electronegativities, ____from right to left, and to a less degree from top to bottom.
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decrease
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valency
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# of electrons that an element will either give up or accept
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valency of Uranium
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6
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Ionic radius
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deduced from bond length when the atom is bonded to one or more other atoms.
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cation
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postively charged atoms.
SMALL ionic radii |
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anions
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negatively charged atoms.
LARGE ionic radius |
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_______ decreases as charge increases, due both to losee of electrons and shrinking of orbits of remaining electrons
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ionic radius
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electropositive
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ready to accept an electron, tend to form ionic bonds, rather than covalent bonds
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what are group 2 elements called?
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alkaline earths
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group 17 elements?
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halogens--highly electropositive
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elements of groups 13-16 tend to form what kind of bonds?
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covalent--tend to be less reactive and soluble
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what are the noble metals?
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Ru, Rh, Pd, Os, Ir, Pt--these elements tend to be very unreactive..dont oxidize like most other metals
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How do the rare earths metals vary?
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only by the number of electrons in the 4f shell
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