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chem terms

QuestionAnswer
Dobereiner arranged elements into groups of three called "triads" based on similar properties
2. Mendeleev Created the first periodic table. Arranged elements by increasing atomic mass and used the arrangement to predict the properties of missing elements.
3. Moseley arranged the periodic table according to atomic number instead of atomic mass
4. Seaborg arranged Periodic Table by pulling out lanthanides and actinides
5. Periods Horizontal rows on the periodic table; there are 7.
6. Groups/Families The vertical columns in the periodic table; contain elements with similar chemical properties.
7. Representative Elements Elements found in groups 1A "Main Group Elements".
8. Metals Elements that conduct electricity, are shiny, heat well and are easily shaped, solid at room temperature (except mercury). Make up the majority of the periodic table.
9. Metalloids/Semimetals Elements with properties that fall between those of metals and nonmetals. Found along the staircase line on the periodic table.
10. Nonmetals Elements that do not conduct electricity, are not shiny and do not conduct heat
11. Periodic Law When the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.
12. Periodic Trend Property of the elements that can be predicted from the arrangement of the periodic table.
13. Atomic Size (aka. Atomic Radius) The size of an atom. Found by measuring half the distance between two atomic nuclei.
14. Effective Nuclear Charge The attraction felt by the outermost electrons toward the nucleus. (aka pulling power").
15. Shielding Effect The reduction of the attractive force between a nucleus and its outer electrons due to the blocking effect of inner electrons.
16. Valence Electrons The electrons in the outermost energy level of an atom; these are the electrons involved in forming bonds.
17. Electronegativity The tendency of an atom to attract bonding electrons towards itself.
18. Ionization Energy The amount of energy required to remove an electron from an atom.
19. Electron Affinity the energy change that occurs when an electron is added to a neutral atom in the gaseous state to form a negative ion.
20. Ionic Size Size of ions after an atom has lost or gained electrons
21. Cation Formation Metals tend to lose electrons and form cations. When an electron is lost, ionic radius decreases
22. Anion Formation Nonmetals tend to gain electrons and form anions. When an electron is gained, ionic radius increases.
23. Metallic Character How much an element behaves like a metal in terms of conductivity, luster & malleability.
24. Nonmetallic Character How much an element behaves with the properties of a nonmetal.
Created by: user-1916403
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