Inorganic chemistry test #1 – Flashcards
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no two electrons in an atom may possess identical sets of the four quantum numbers
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Pauli exclusion principle
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states that when the electrons of an atom are all in the ground state, they occupy the orbital's of the lowest energy, thereby minimizing the atoms total electronic energy.
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Aufbau principal
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when filling a set of degenerate orbitals, the number of unpaired electrons will be maximized and these electrons will have parallel spins
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Hunds rule
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[Ar] 4s1 3d10
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what is the electron configuration for copper?
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[Ar] 4s1 3d5
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what is the electron configuration for chromium?
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[Xe] 6s2 4f14 5d10 and [Xe] 4f14 and 5d10
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what is the electron configuration for Lead +2 and +4?
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energy needed to remove the second ground-state electron from an atom (X+ → X2+ + e−).
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Second Optization Energy
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energy needed to add an electron to the lowest available energy state of an atom
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electron affinity
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for each essential element there is a range of intake from too low to optimal to excess.
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bertrands rule
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group 3 and the lanthanoid elements
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rare earth metals
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half the distance b/w the nuclei of 2 atoms of neighboring molecules
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van der waals radius
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Net nuclear charge felt by an electron
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effective nuclear charge
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1/2 the distance between two nuclei of two atoms of same element joined by a single covalent bond
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covalent radius
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Half the distance between the nuclei of two neighboring atoms in the solid metal
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metallic radius
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decreases
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atomic radius ____ across the period
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increases
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atomic radius ____ down the group
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the energy needed to remove one electron from the outermost occupied orbital of a free atom (X)
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ionization energy
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ten times
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second ionization energy takes _____ the amount to remove the second electron
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Electron affinity is the energy change when an electron is added to the lowest energy unoccupied orbital of a free atom.
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electron affinity
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increases
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electron affinity _____ across the period
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Essential for life in large quantity
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bioinorganic chemistry
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for each essential element there is a range of intake from too low to optimal to excess.
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bertrands rule
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delocalized, freely
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in metallic bonding, electrons are ______ and move _____
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wide
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metals have a _____ range of melting points
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metallic bond
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boiling points correlates closely with the strength of the _____
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Valence electrons are free to move through the metal structure.
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electron sea model
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Describes electrons with use of wave functions spread around the entire molecule
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molecular orbital theory
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bonding
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sigma
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anti-bonding
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sigma*
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where the spheres are side by side
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body center cubic
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hard and brittle
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crystal ionic bonding is ______
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high
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Crystal ionic compounds have a _____ melting point
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the quantum number determines the shape of the orbit
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how does the quantum number l relate to the properties of the orbital?
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you must fill one lobe at a time to satisfy a lower energy state
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explain why carbon has two electrons in different p orbitals with parallel spins rather than the other possible arrangements.
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number 82, lead
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what is the highest atomic number element for which stable isotopes exist?
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technetium
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what is the only transition metal for which no stable isotopes are known?
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bromine
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what is the only nonmetal that is liquid at SATP?
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potassium because there are more electrons in calcium which means there are more protons that are pulling the electrons in closer to the nucleus
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which atom should have the larger covalent radius out of potassium and calcium and why?
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chlorine because it has an increasing amount of layers of electrons, the effective nuclear charge on the outermost electrons will decrease
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which should have the larger radius out of flourine and chlorine and why?
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the effective nuclear charge on the 4p electrons will be increased
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suggest a reason why the covalent radius of germanium (122pm) is almost the same as silicon (117pm) even though germanium is 18 electrons more.
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exothermic
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the addition of an electron to an alkali metal is an _____ reaction.
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valence shell electron pair repulsion
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VSEPR
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highest occupied molecular orbitals
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HOMO
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lowest unoccupied molecular orbitals
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LUMO
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higher, shorter
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the _____ the bond order, the _____ the bond length
