Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
41 Cards in this Set
- Front
- Back
Pauli exclusion principle
|
No two electrons ina n atom can have the same four quantum numbers.
|
|
General Energy Ordering of Orbitals for Multielectron Atoms
|
1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f, 5s, 5p, 5d, 5f, 6s, 6p, 6d, 7s, 7p
|
|
what is the max number of electrons an orbital can hold
|
two electrons
|
|
The s sublevel has only __ orbitalss and can there fore hold only __ electrons
|
one, two
|
|
The p sublevel has only __ orbitals and can therefore hold only ____ electrons
|
three, six
|
|
The d sublevel has only __ orbitals and can therefore hold only ___ electrons
|
five, ten
|
|
The f sublevel has only ___ orbitals and can therefore hold only ____ electrons
|
seven, fourteen
|
|
Valence Electrons
|
the outer most principal energy level
|
|
location of Alkali metals
|
1A on the periodic table
|
|
Location of Alkaline earth metals
|
2A on the periodic table
|
|
Location of Halogens
|
7A on the periodic table
|
|
Alkali metals have ___ valence electrons and tend to ___ electrons in reactions
|
one, lose
|
|
Alakaline Earth Metals have ___ valence electrons and tend to ____ electrons in reactions
|
two, lose
|
|
Halogens have __ valence electrons and tend to _____ in reactions
|
seven, gain one electron
|
|
nonmetals bonding atomic radius or covalent radius is
|
one half the distance between two fo the atoms bonded together
|
|
metals boning atomic radius or covalent radius is
|
one half the distance between teh two of the atoms next to each other in a crystal of the metal
|
|
As you move down a column in a periodic table the atomic radius
|
increases
|
|
As you move to the right across a period or row of the periodic table the atomic radius
|
decreases
|
|
Core electrons efficiently shiled electrons...
|
in the outermost principal energy level form nuclear charge, but outermost electrons do not efficiently shield one another from nuclear charge
|
|
As yo move down a column in the periodic table quantum number (n) of the electrons in teh outermost principal energy level
|
increasesresulting in larger orbitals and therefore larger atomic radii
|
|
As you move to the right across a row in the periodic table, the effective nuclear charege (Zeff) experienced by the electrons in teh outermost principal energy level
|
increases, resulting in a stronger attraction between teh otuermost electorns and hte nucleus and therefore smaller atomic radii
|
|
Cations are much ____ than their corresponding atom
|
smaller
|
|
Anions are much ___ than their corresponding atom
|
larger
|
|
cations are in columns __A __A __A anions are in columns __A __A
|
1,2,3, and 6,7
|
|
Ionized energy generally ___ as you move down a column because electrons in teh otuermost principal level become farther away from the positively charged nucleus and are therefore held ___ tightly
|
decreases, less
|
|
Ionized energy generally ___ as you move to the right across a period in a periodic tble because electrons in teh outermost principal energy level generally experience a ____ effective negative charge (Zegg)
|
increase, greater
|
|
As you move to the right across a period in the periodic table, metallic character
|
decreases
|
|
As you move down a column in the periodic metallic character
|
increases
|
|
The most active metals
|
Alkali metals
|
|
the most active nonmetals
|
halogens
|
|
planack's number symbol
|
h
|
|
h
|
6.63x10-34 J.s
|
|
speed of light symbol
|
c
|
|
c
|
3.00x10 8
|
|
Rh
|
2.18x10-18
|
|
mass of a neutron
|
1.675x10-30g
|
|
mass of a proton
|
1.673x10-30g
|
|
mass of a electron
|
9.11x10-34g
|
|
energy of a photon is equal to
|
hxc/wavelength
or Rn/n2 |
|
wavelength is equal to
|
hxc/energy of a photon
or c/frequency or h/mass velocity |
|
frequency is equal to
|
c/wavelength
|