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chem periodic trends
test on 12/4/14
| what is group one on the periodic table called | alkali metals |
| what is group two on the periodic table called | alkaline earth metals |
| what are groups 3-12 called | transition metals |
| what is the metalloid in group 13 | boron |
| is aluminum a metalloid | no |
| is polonium a metalloid | no |
| what are the lanthanide and actinide series called | inner transition metals |
| what is group 17 called | halogens |
| what is group 18 called | noble gases |
| is hydrogen an alkali metal? | no |
| what is the trend for reactivity for metals | increases to the left and down |
| what is the trend for reactivity in nonmetals | increases up and to the right |
| why do families have similar chemical reactivity | similar valence electrons within a group results in similar chemical properties |
| what is periodicity or the periodic law | when elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals |
| what is the most reactive metal | francium |
| what is the most reactive nonmetal | fluorine |
| what is shielding | core energy levels block the attraction between the nucleus and the outermost energy level |
| what is repulsion | electrons in the inner shells repel each other |
| what is the periodic trend for atomic radius | increases down and to the left |
| what is atomic radius | size of the atom, 1/2 distance between the uncle of identical atoms bonded together |
| why is atomic radius larger as you go down a group | higher energy levels have larger orbitals |
| why is atomic radius smaller to the right of a period | increased nuclear charge without additional shielding pulls electrons in tighter (greater effective nuclear charge) |
| what is ionic radii | size of an ion in an ionic solid |
| what is a cation | ion with a positive charge due to a loss of electron(s) |
| what is an anion | ion with a negative charge due to the gain of electron(s) |
| are cations larger or smaller than their neutral atom | smaller than neutral atom |
| are anions larger or smaller than their neutral atom | larger |
| do cations have an increased or decreased effective nuclear charge and why | increased, same number of protons with fewer electrons |
| do anions have an increased or decreased effective nuclear charge and why | decreased, same number of protons with more electrons means lower effective nuclear charge |
| what is the trend of ionic radii | increase down and to the left |
| what is electronegativity | measure of the ability of an atom in a chemical compound to attract electrons |
| what is the trend of electronegativity | increases up and to the right |
| why does electronegativity increase up | less shielding in smaller atoms |
| why does electronegativity increase to the right | more protons pulling on the same energy level, no additional shielding |
| what is first ionization energy | energy required to remove one electron from a neutral atom |
| what is the trend of ionization energy | increases up and to the right |
| why is ionization energy trend opposite of atomic radius trend | in small atoms, electrons are close to the nucleus where the attraction is stronger |
| why are there small jumps (higher first ionization energies in some elements than others) within each group | stable electron configurations require more energy to remove electrons (half full sub levels, full sub levels) |
| why does ionization energy increase across a period | greater effective nuclear charge (more protons pulling on the same energy level) |
| why does ionization energy decrease down a group | more shielding, so the farther the electrons get from the nucleus, the less energy it takes to remove them |
| who is the father of the periodic table | mendeleev |
| how was mendeleevs periodic table organized | in order of increasing atomic mass |
| how is moseys periodic table organized | in order of increasing atomic number |
| who invented the periodic table we use today | moseley |
| what is the most reactive type of metal | alkali metals |
| what are most of the elements on the periodic table | metals |
| what is the chemical reactivity of noble gases | no reactivity |
| what is the electronegativity for helium, neon, argon | no electronegativity for the first three noble gases |
| in which state are most metals and what is the other | most are solids, but one is a liquid; mercury |
| who developed electronegativity | linus paulong |
| which element are all electronegativity values relative to | fluorine (4.0)the most electronegative element |
| how to use electronegativity scale | find difference: less than 1.7 is covalent bond, greater than 1.7 is ionic bond |
| in which state is ionization energy measured | the gaseous state (kJ/mol) |
| how many elements are liquids at room temperature (25*C) | 2; mercury and bromine |
Created by:
d0402774
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