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Periodic Table

Regents Chem Periodic Table

QuestionAnswer
Atomic mass how the first periodic table was arranged
Atomic number how the current periodic table is arranged
Metal ionic radius these elements lose electrons and form positive ions smaller than their atoms.
Non metal ionic radius these elements gain electrons and form negative ions that are bigger than their atoms
Electronegativity ability to attract electrons. Fluorine has the highest at 4.0
Ionization energy energy required to remove outer electron(s). The noble gases have the highest. This decreases as you move down a group because the radius increases.
Atomic radius distance from the nucleus to the outer electrons. Increases moving down and group and DECREASES moving left->right across a period.
Nuclear strength number of protons in the nucleus. This increases across a period and is the reason that radius decreases across a period.
Atomic radius in a group atoms get bigger as you move from top to bottom in a group. This is because energy levels are added.
Mendeleev Scientist who created the original periodic table
Moseley Scientist who created the modern periodic table
The two liquid elements at STP Mercury (Hg) and Bromine (Br)
The 7 diatomic elements F, Br, Cl, I, N, O and H
Gases at STP all the noble gases, F, Cl, N, O, H
Solid The phases of most of the elements on the periodic table (they’re metals)
What it means when the atomic mass doesn’t have any decimal places the element has NO stable isotopes. It’s most likely radioactive
Calculating average atomic mass multiply each isotope by its abundance (in decimal form)…then add the results up, this is the average mass!
Group vertical collection of elements on the periodic table, all with the same # valence electrons and similar reactivities.
Period horizontal collection of elements on the periodic table, all with the same # of energy levels.
Properties of metals lost electrons to form positive ions, Fr is most reactive, malleable and ductile, conduct heat and electricity (by mov’t of electrons)
Properties of nonmetals do not conduct, brittle, tend to share or gain electrons.
Properties of transition metals have colored solutions, many possible charges, lose electrons from the valence level and the next level down.
Created by: etucci