Chapter 7 Flashcards
As we go Bottom-Up on the Periodic Table, the radius _____.
Decreases
As we go right to left on the Periodic Table, the radius of the atom ______
Increases
Positive ions are _____ than their neutral atoms.
Smaller
Negative ions are _____ than their neutral atoms.
Bigger
What is the isoelectronic series?
formed by ions that possess the same number of electrons.
Ionic size _____ with an _____ nuclear charge
Decreases, increases
What is ionization energy?
The amount of energy that is required to remove an electron from the ground state of a gaseous atom or ion.
If IE is ____, it is difficult to remove an e-.
high
If IE is ___, it’s not difficult to remove an atom.
low
What are valence electrons?
An electron that is associated with an atom, and that can participate in the formation of a chemical bond.
What is electron affinity?
The energy change (ΔE) accompanying the addition of an e- to a gaseous form. Most are negative.
Typically, as you go left to right or down to up on the Periodic Table, electronic affinity becomes more __________.
Exothermic, though this pattern is not consistent.
Characteristics of metals
Shiny, malleable, ductile, conductive of heat and electricity, high melting point, low ionization energy
A metal to a nonmetal bond is referred to as a _____ compound
ionic
A ________ to ________ bond is usually referred to as a molecular bond
nonmetal, nonmetal.
Characteristics of nonmetals
Not shiny, poor conductivity, generally low melting points, easily gained electrons (favorable electron affinity)
Nonmetal oxides are generally ______
acidic
Characteristics of metalloids
Display intermediate properties (somewhat metal, somewhat nonmetal), shiny but not brittle, semiconductors
If Ionization Energy is high, then it is _________ to remove an electron
difficult
______ atoms have a lower Ionization Energy
Larger
With transitions metals, as electrons are removed from the _ shell and then the _ shell
S, P
In other metals and nonmetals, the _ orbital electrons disappear first
D
The ionization required to remove an electron from an atom is always __
+
If IE is high, that means it is _________ to remove the electron
difficult
Exceptions to IE Rule on the PTE
Higher IE in 2A than 3A due to orbitals and atomic radius,
Higher IE in 5A than 6A because of the double orbitals being filled and having more shielding.
More Electron Affinity means having __ energy, because the addition of e- is more __________
- because adding an electron is an exothermic reaction.
Exceptions to the electron affinity rules:
Noble gases which require more energy to add electrons because they are already stable and do not require more electrons.
Other exceptions to electron affinity:
1A and 2A, where any added e- must go into the P orbital
Last exception to EA
No empty orbital, e- goes in occupied orbital causing repulsion
