Part 1 Inorganic Chemistry – Atomic Structure and Periodic Table – Flashcards
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Basic format of Atom's mass and atomic number on periodic table A=(?) Z=(?)
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A= Mass Number Z= Atomic Number Image is of the written/text format for atoms.
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Isotopes
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Same Atomic Number=same element Vary in Mass - therefore neutrons vary
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Special Hydrogen Isotope Names
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Hydrogen (protium) Deuterium Tritium
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Ions
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Atomic number is the same Charge is different due to addition or subtraction of electrons
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Common Ions
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IA - Na^1+, K^1+ IIA - Mg^2+, Ca^2+, Ba^2+ B Group - Fe^2+ or Fe^3+, Co^2+ or Co^3+, Ni^2+, Zn^2+, Ag^1+ IIIA - Al^3+ VIA - O^2- VIIA - F^1-, Cl^1-, Br^1-, I^1-
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Common Polyatomic Ions Hydroxide Cyanide Sulfate Phosphate Nitrate Carbonate Bicarbonate Peroxide Permaganate Ammonium Percholorate Chlorate Chlorite HypoChlorite
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Hydroxide = OH^1- Cyanide = CN^1- Sulfate = SO4^2- Phosphate = PO4^3- Nitrate = NO3^1- Carbonate = CO3^2- Bicarbonate = HCO3^1- Peroxide = )2^2- Permaganate = MnO4^1- Ammonium = NH4^1+ Percholorate = ClO4^1- Chlorate = ClO3^1- Chlorite = ClO2^1- HypoChlorite =ClO^1-
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Standard Atomic Weight
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Weighted average of all naturally occurring isotopes. so for Nitrogen the std. atomic weight is 14.007 because some most isotopes are 14N then few are 15N
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Bohr Model
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Concept that electron revolves around nucleus of atom
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Paramagnetic
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Has unpaired electrons magnetic field will align the spin and weakly attract the material
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Diamagnetic
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No unpaired electrons and magnetic field will slightly repel the material.
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Hund's Rule
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Orbitals will prefer to have maximum number of half-filled orbitals with parallel spins.
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Atomic Radii
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Increasing protons leads to stronger pull on electron shells --> Decreases Atomic Radii Increasing number of shells leads to increasing Atomic Radii
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Ionic Radius
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Atomic Radii changes when things add or remove electrons to form ions. As electrons are added, the electrons are forced to be near and repel each other making the electron cloud bigger.
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Ionization Energy (IE)
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Energy needed to eject an electron from an atom Outermost electrons are easier to remove (require less energy) that the electrons closest to the nucleus)
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Electron Affinity (EA)
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Change in energy of that occurs when an electron is added also like the Ability or willingness to accept an electron Alkaline Earth Metals low EA as Valence shell is full (2 electrons). Halogens High EA as Valence shell only needs one electron. Nobel gases 0 EA as their shell is already full.
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Pauling Electronegativity Scale
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scale that displays a measure of attraction an atom has towards bonding electrons
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Anion
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Negatively charged Ion often gain an electron to form negative ion. Cl willingly takes an electron making it an anion.
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Cation
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Positive charged ion. Metal elements often become cations, giving up an electron or two
