chem test chapter 6
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27 terms
Terms | Definitions |
|---|---|
 periodic table | named this based on the phases of the moon repeating in a periodic way |
| John Newlands | created law of octaves-->arranged by atomic mass, repeat every eighth element |
| Dmitri Mendeleev | created the 1st periodic table |
| Henry Moseley | fixed Mendeleev's periodic table bu putting the elements in order by increasing atomic number, as compared to Mendeleev's elements being in order by increasing atomic mass |
| periodic law | statement that there is a periodic repetition of chemical and physical properties of the element when they are arranged by INCREASING ATOMIC NUMBER |
| groups | families, columns |
| periods | rows |
| representative elements | groups designated with the letter "a" |
| transition elements | groups designated with the letter "b" |
| metals | elements shiny when smooth and clean, solid at room temperature, and are good conductors of heat and electricity |
| alkali metals | the group 1A elements except for hydrogen |
| alkaline earth metals | 2A elements |
| inner transition metals | lanthanide and actinide series at the bottom of the table |
| nonmetals | generally gases, brittle dull looking solids, conductors of heat and electricity |
| Bromine | only liquid at room temperature |
| noble gases | extremely unreactive 8A |
| halogens | highly reactive group 7A |
| metalloids | elements with physical and chemical properties of metals and nonmetals |
| atomic radius | half the distance between adjacent nuclei |
| ionization energy | the energy required to remove an electron from a gaseous atom |
| octet rule | states that atoms tend to gain, lose, or share electrons in order to acquire a full set of 8 valence electrons |
| electronegativity | indicates the relative ability of its atoms to attract electrons in a chemical bond |
| ion | an atom or bonded group of atoms that has/have a positive or negative charge |
| IONIC RADII AND ATOMIC RADII | Decrease in periods because of the increasing positive charge in the nucleus and the principal energy remains the same |
| IONIC RADII AND ATOMIC RADII | Increase in groups because the nuclear charge increases, and electrons are adding to higher principal energy levels |
| ELECTRONEGATIVITY AND IONIZATION ENERGY | Increase across periods because the increased nuclear charge of each element produces an increased hold on valence electrons |
| ELECTRONEGATIVITY AND IONIZATION ENERGY | Decrease of energy across groups because atomic size increases as you move down. With the valence electrons farther from the nucleus, less energy is required to move them. |
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