Exam 2 Stuff Flashcards
What are the possible values of n?
1 to 7
What are the possible values of l?
0 to n-1
What are the possible values of ml?
-l to +l
What are the possible values of ms?
-1/2 or +1/2
What is a probability distribution map showing where the electron is likely to be found?
orbital
Shows the mathematical derivation of energies and orbitals for an electron in an atom
Schrödinger Equation
What does the principal quantum number tell you?
What energy level the electron is in (the period on the periodic table)
What does the angular momentum quantum number (l) tell you?
the sublevel (s,p,d,f)
What does it mean for an electron to be in the excited state?
the atom absorbed a photon and the electron is moved from a lower orbital to higher
What is the probability of finding an electron at a node?
ZERO
What does the Pauli Exclusion priciple state?
No 2 electrons in an atom can have the same four quantum numbers.
What are degenerate orbitals?
orbitals above the principle quantum number
Coulomb’s Law states what?
- like charges repel
- opposite charges attract
- magnitude of interaction increases as charges increase
What is sheilding?
An electron is attracted by the nucleus but repelled by the other electrons. Other electrons act like a sheild from full nuclear charge.
What is an effective nuclear charge (Zeff)?
the charge experienced by the electron through the sheild
What happens during penetration?
and electron gets closer to the nucleus than the 1s orbital and experiences the full charge of the nucleus
What is the Aufbau Principle?
Electrons occupy lower energy levels first and only 2 electrons per oribital
What is Hund’s rule?
when filling degenerate orbitals, electrons fill them singly first with parallel spins
What are valence electrons?
Electrons in the highest principle energy level
What are core electrons?
Electrons that aren’t valence electrons
As you move down a column on the periodic table, _____ increases.
density
Which way do you move to increase Zeff?
from right to left across a period
Which way do you move on the periodic table to get a bigger radius?
down and left
What does it mean to be paramagnetic?
the atom has unpaired electrons and can be attracted by a magnet
What does it mean to be diamagnetic?
the atoms has no unpaired electrons, so it is not affected by magnets
What happens to atomic radii of cations?
they are much smaller than the corresponding neutral atoms
What happens to anions’ atomic radii?
They are much larger than their corresponding neutral atoms
What is ionization energy?
the enery required to remove an electron from the atom or ion in the gaseous state
Which way do you move on the periodic table for ionization energy to increase?
right and up
What is electron affinity?
the energy change associated with the gaining of an electron by the atom in the gaseous state
Which group has the most negative electron affinity?
the halogens
Electron affinity for group 1A becomes more positive as you move ___ the column
down
Electron affinity generally becomes more negative as we move to the ___ across a period.
right
Which group is the exception to the electron affinity trends?
5A
Metallic Character increases as you move ____ and ____
down and left
What are bonds that form between a metal and a nonmetal called?
Ionic bonds
Ionic compounds in the solid state are composed of a ___?
lattice
Bonds between two or more nonmetals are called?
covalent bonds
Covalently bonded atoms form ____?
molecules
Name the 7 group two metals.
Chromium, Iron, Cobalt, Copper, Tin, Mercury, Lead
