Chemistry - Electron Configuration Test Review
Pauli Exclusion Principle
maximum of two electrons may occupy an atomic orbital, but only if they have opposite spins
quantum
minimum amount of energy that can be lost by an atom
it represents energy (orbitals in similar shells have similar energies)
what does the energy level number mean?
the set of orbitals grouped by similarities in the shapes of orbitals
what does the sublevel letter represent?
light
what is given off when electron goes from excited state too ground state?
# of electrons in any d sublevel
10
# of electrons in any f sublevel
14
Full Configuration for Mg
1s²2s²2p⁶3s²
Electron Configuration for Si
1s²2s²2p⁶3s²3p²
Electron Configuration for Ar
1s²2s²2p⁶3s²3p⁶
Electron Configuration for Kr
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶
Electron Configuration for Sr
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²
Full Configuration for Rh
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁷
# of electrons in any s sublevel
2
excited state
lower energy levels
10
*3d¹⁰* - which is the electrons?
3
*3d¹⁰* - which is the energy level?
d
*3d¹⁰* - which is the orbital?
3d
*3d¹⁰* - which is the sublevel?
Hund's Rule
- electrons occupy equal energy orbitals so as to maximize the number of unpaired e-s
# of orbitals in any s sublevel
1
# of orbitals in any p sublevel
3
p orbitals
3 mutually perpendicular dumbbell shaped orbitals; second to fill from 2nd energy level on up; can hold max of 6 electrons
# of orbitals in any d sublevel
5
d orbitals
5 orbitals of cloverleaf shape; third to fill for any energy level; beginning in the third shell, contains a total of 10 electrons; higher in energy than s and p orbitals in the same shell CEKj53gchpBb9A.png
# of electrons in any p sublevel
6
# of orbitals in any f sublevel
7
orbital
A three-dimensional region around the nucleus that indicates the probable location of an electron -- *the specific shape in which an electron is travelling around the nucleus*
Electron configuration
Arrangement of electrons in the orbitals of an atom.
quantum number; electrons
Bohr's description of hydrogen atom was the higher the _____ the farther away the _____ are from the nucleus
Valence electron
Electrons in the outermost energy level of an atom, they are involved in bonding
valence shell
Outermost electron shell of an atom
Energy levels
The rings of the electron cloud that hold electrons -- *corresponds to how far away from the nucleus an electron is*
Noble Gas notation for Ni
[Ar] 4s²3d⁸
Noble Gas Configuration for Ce
[Xe]6s²5d¹4f¹
opposite; like
_____ charges attract and _______ charges repel
positives; negatives
__________ and _________ cancel each other out
anions
a negatively charged ion because it gained electrons
photon
a particle of electromagnetic radiation with no mass and that carries a quantum energy
cations
a positively charged ion because it lost electrons
ion
an element that has gained or lost an electron to get a charge
octet rule
atoms are the most stable when they have a full valence shell of electrons
light
electromagnetic radiation (form of energy that exhibits wave-like behavior as it travels through space)
gaining energy
electrons can jump to higher energy levels by _____
s block
groups 1 and 2 on the periodic table
p block
groups 13-18 on the periodic table
d block
groups 3-12 on the periodic table (the transition metals)
ground state
higher energy levels
to identify elements
how can AES be used?
negative
if an atom gains an electron, it becomes ______
positive
if an atom loses an electron, it becomes ______
neutral
in a _____ atom, the # of protons = # of electrons
electrons
in an atom, if the # of ____ change, the charge changes
Nitrogen
name the element 1s²2s²2p³
Aluminum
name the element 1s²2s²2p⁶3s²3p¹
Titanium
name the element [Ar]4s²3d²
Tungsten
name the element [Xe]6s²4f¹⁴5d⁴
sublevels
regions within the energy levels; corresponds to the block grouping s,p,d,f on the Periodic Table -- *defines the approximate boundaries of each electron (includes energy level AND the orbital)*
s orbitals
spherical orbitals; first to fill for any energy level; can only hold 2 electrons
Aufbau Principle
states that each electron occupies the lowest energy orbital available
RIGHT
the ____ side of the stepladder is the anions
LEFT
the ____ side of the stepladder is the cations
frequency
the number of waves that pass a given point per second
atomic emission spectrum
the set of frequencies (colors) of electromagnetic waves emitted by the atoms of an element -- *each atom gives different off*
wavelength
the shortest distance between equivalent points on a continuous wave
f orbitals
their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells; in the fourth and fifth energy levels
spectrum tubes
these separate the colors of the elements AES
ELECTRONS
to form Ions, you can only gain or lose _________________________!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
amplitude
wave's height from origin to crest
speed of light
wavelength x frequency
3rd
which has more energy: 2nd or 3rd shell?
visible spectrum; invisible
why are only four colors given off in hydrogen? BECAUSE - there are _____ energy levels - because those four are the ones in the _______ - the other three are _______ in the spectrum
because of the characteristics of the different metal atoms
why did each chemical in the flame test burn a different color?