Chem #2 Flashcards
what are the A elements?
representative elements: IA-VIIIA
• Valence electrons in either s or p subshells
this does not have to do with side of the metalloid ladder (just d or p block)
what are the B elements?
nonrepresentative elements includes:
• The Transition elements: valence electrons in s and d subshells (these are the elements in the d block)
• And the Lanthanide and actinide series: valence electrons in s and f subshells
this does not have to do with side of the metalloid ladder (just d or p block)
metals
left side and middle of the periodic table
o Active metals, transition metals, and lanthanide and actinide series
o Lustrous: shiny solids (except mercury which is a liquid under standard conditions)
o Malleability: ability to be hammered into shapes
o Ductility: pulled or drawn into wires
o Atomic level:
Low EN (high electropositivity)
Low effective nuclear charge
o Transition metals have two or more oxidation states (charges when forming bonds with other atoms)
o Conductors: due to valence electrons only being loosely held, they are free to move.
o Want to give up electrons.
what type of elements are lustrous, malleable, ductile, and good conductors?
metals
nonmetals
found predominately on the upper right side of the periodic table
o Brittle in the solid state with little or no metallic luster
o High IE, EA, and EN
o Poor conductors of heat and electricity
o Inability to give up electrons
what elements want to give up electrons?
metals
what elements want to gain electrons
nonmetals
metalloids
share characteristics with both
o Stairstep pattern that separates the metals from the nonmetals.
o B, Si, Ge, As, Sb. Te, Po, At
effective nuclear charge
a measure of the net positive charge experienced by the outermost (valence) electrons.
• Electrons between the valence e and the nucleus can mitigate the pull a little (shielding)
electrons are held _____ tightly further away from the nucleus
less
effective nuclear charge does what down a group?
stays relatively the same, more positive charge, but pulling on electrons that are in a further shell.
noble/inert gases
very stable, Group VIIIA or Group 18
atomic radius
o Atomic radius (AR): equal to ½ the distance between the centers of two atoms of an element that are briefly in contact with each other (size of a neutral element)
As you move left to right, more protons and neutrons being added, greater pull on the electrons that are being added to the same principal energy level, decreases AR
Move down, valence electrons are put into shells that are further away from the nucleus (greater energy levels), less pull, increase AR
ionic radii
Metals: lose electrons and become positive
• Will have smaller AR
Nonmetals: gain electrons and become negative
• Will have larger AR
Metalloids: depends on which side of metalloid line they fall.
NOTE: elements that are further from the ideal configuration will have more drastic changes to their AR (have to add or lose more electrons to reach this configuration)
what happens to atomic radius as you move left to right and top to bottom?
left to right: decrease
top to bottom: increase
cations have ____ atomic radius while anions have _____
smaller
larger
ionization energy
the energy required to remove an electron from a gaseous species.
o Endothermic process: requires input of heat
o Increases the closer valence electrons are held to the nucleus.
o Subsequent removal of electrons (IE2, IE3) requires even more energy.
o First ionization energy: energy necessary to remove the first electron
o Second ionization energy: energy to remove the second electron
o Active metals: elements in groups IA and IIA, such low ionization energies.
if the ionization energy is huge, probably means the element was in a ____
noble gas state
is the second ionization energy always greater than the first?
yes
is ionization energy an exothermic or endothermic process?
endothermic
ionization energy ______ up and to the right of the periodic table
increases
electron affinity
the energy dissipated by a gaseous species when it gains an electron.
o Exothermic: process expels energy in the form of heat.
AE is recorded as a positive number, heat released, but the ΔHrxn is negative.
o The stronger the electrostatic pull (greater the Zeff), the greater the energy release will be when the atom gains the electron.
o Noble gases have close to 0 electron affinity.
electron affinity is endothermic or exothermic
electron affinity is expressed as a ____ number
exothermic
positive
electron affinity ____ up and to the right
increases
