chem periodic trends Word Scramble
|
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
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
Popular Chemistry sets