midterm Flashcards
how to calculate formal charge
valence electrons-(free electrons+bonds)
How can an excited atom return to a lower energy level?
by emitting light energy
How can an atom be excited into a higher energy level
by absorbing light energy
how is wavelength and frequency related
they are inversely proportional
where is alkali metals
elememts of group 1 (column)
where are alkali earth metals
elements of group 2
where are the halogens
elements in group 17
where are the inert noble gasses
elements in group 18
where are the transition metals
elements in groups 4-12
where are the non metals
the “stairs from group 13-18
what are the first three quantom numbers
they identify the position of an electron in orbit
what does the last quantum number represent
the spin of the electron around its axis
which quantum number helps explain an atom’s magnetic properties
the last one (ms) : the spin of the electron around its axis
In quantum numbers, what does N represent?
the energy of an electron; the smaller the N, the lower the energy. also coincides with the distance the orbit is from the nucleus
what is the angular momentum quantum number
L, defines the different orbitals possible within an energy level.
the number of shapes possible of an orbital is dependent on what.
L is dependent on the size of the major energy level (N)
What are the possible values of L
N-1=L (any number lower than N)
What is the magnetic quantum number
ML; indicates how many orbitals there are that have the same N value and the same L value, but a different orientation (same distance from nucleus, same path, different orientation)
If L=2, what are the possible ML
2,1,0,-1,-2 (five different orientations
What is the spin quantum number
MS; Used to describe the possible directions of the spin of an electron.
what are the possible values of MS
-1/2, 1/2
What makes an atom have magnetic properties?
unpaired electrons
define diamagnetic
when an atom has all paired electrons
equation to determine maximum number of electrons in a major energy level
2N^2
eg. in the 4th energy level: 2(4)^2=32electrons
what is Hunds rule
when filling sub shells of the same major level, every Subshell gets one before any get 2
how to calculate how much attraction is from the electron to the nucleus
electrons/protons
Describe the periodic properties of atomic and ionic radii
as you go to the right, radii decreases. as you move down, radii increases
what is ionization energy
energy required to remove an electron from a gaseous atom
describe the periodic trends of ionization energy
as you go to the right, it increases. as you go down, it decreases
what is electron affinity (EA)
amount of energy it will give in order to gain an electron (energy released when a gaseous atom gains an electron)
describe the periodic trends of electron affinity
increases to the right, decreases going down
what is electronegativity
measure of the tendency of an atom to gain electrons (how badly an atom wants an electron)
describe the trends of electronegativity
increases to the right, decreases down
what is a pi bond
double bond looking thing
what property must an atom have in order to have a PI bond
a P orbital
properties of PI binds
atoms must have a P orbital
not as string as theta bonds
they indirectly overlap (meaning the electrons are basically jumping to and from bond)
easy to break
2 electron pairs =
sp,linear,180
3 electron pairs =
sp2,trigonal planar,120
4 electron pairs=
sp3, tetrahedral, 109.5
5 electron pairs=
trigonal bypiramid, 90,120,180
6 electron pairs=
sp4d2,octahedral, 90,180
sp
linear, 180
sp2
trigonal planar, 120
sp3
tetrahedral, 109.5
sp3d
trigonal bypyramid, 90,180,120
sp3d2
octahedral, 90,180
Ab3 shape
trigonal planar,120
AB2 shape
linear,180
AB4 shape
tetrahedral, 109.5
AB3E
Trigonal pyramidal
AB2E2
bent/angular
AB5
trigonal bypyramidal
AB4E
seesaw
AB3E2
T-shaped
AB2E3
Linear
AB6
octahedral
AB5E
Square pyramidal
AB4E2
square planar
