Test 3 Study Guide Flashcards
What is wavelength?
the distance between one peak and the next
*the measurement of wavelength is between peak to peak or trough to trough
As wavelength increases, the frequency?
decreases
What is the speed of light?
c=wavelengthXfrequency=300x10^8 m/s
What is the unit of frequency?
per second
1 hertz=
1 sec^-1
100.3 MHz=
wavelength
What is the principle quantum number?
N
What symbol is the angular momentum quantum number?
L (cursive)
What is the symbol for the magnetic quantum number?
M sub e
What is the symbol for the spin quantum number?
M sub s
What does the principle quantum number tell us?
energy or distance from nucleus
What numbers is the principle quantum number (n) allowed to be?
1,2,3,4
And N (principle quantum number) increases, what does E do?
increase
What does L (angular momentum quantum number decribe?
Tells the shape
What is the angular momentum quantum number allowed to be?
n-1 but 0 is the least it can be
If you know n and L, then what are you describing?
a subshell
What letters go along with L for the various subshells? 0 1 2 3
0-s
1-p
2-d
3-f
What is the highest subshell?
f or 3
Give the protocol for naming a subshell
use value->nl
What does the magnetic quantum number tell?
Orientation in 3D space
If we know n, L, and M sub l we are describing?
an atomic orbital
Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
a) n=4, L=1, m sub L=0
a)allowed 4p
Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
b) n=2, L=2, m sub L = -1
Not allowed, because n & l cannot be equal
Give the notation for each of the following orbitals. Determine if it is allowed, if not why?
n=5, L=3, m sub L= +3
Allowed, 5f
What does the spin quantum number tell us?
about magnetic properties
What is # are allowed in the spin quantum number?
+1/2
-1/2
If we know n, L, m sub L, and m sub s, then we are describing?
an individual electron
The s orbital makes what shape?
spherical
The p orbital makes what shape?
a infinity symbol
The d orbital makes what shape?
a flower w/4 petals shape
The f orbital makes what shape?
a flower with many petals
Nature looks for?
the lowest energy arrangement possible
What is effective nuclear charge?
weighted average of nuclear charge that affects an electron in the atom, after correction for the shielding by inner electrons and interelectronic repulsions
The _________ the affected nuclear charge, the more able the nucleus is able to control the electrons and vice versa
the greater the affected nuclear charge
Give the order of the subshells-
1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<5d<6p etc.
What is the Pauli exclusion principle?
No two electrons in the same atom can have the same set of four quantum numbers
What is the Aufbau Principle?
as electrons are added to an atom one at a time they are assigned the quantum numbers of the lowest energy orbital that is available
The ground state is?
the lowest energy state possinle
What is hund’s rule?
One electron occupies earch degenerate orbital with the same spin before a second electron is placed in an orbital
Group 1A atoms always form?
1+ cations
Which group of atoms is particularly stable?
Noble gases
What are valence electrons?
those with the highest principle quantum number and any electrons in a unfilled subshell from a lower shell
What is an ion?
charged particle
A cation is
forms a positive charge from loosing an electron
An anion is
negative charge from an atom gaining an electron
What is an isoelectronic series?
is a group of atoms and ions that contain the same number of electrons
What is an example of an isoelectronic series?
S2-, Cl-, Ar, K+, and Ca2+
How is the size of an atom determined?
by measuring its radius
What type of atom has the smallest size?
Species with the highest number of protons
Atoms are always larger than their _______.
Atoms are always larger than their cations
Atoms are always smaller than their _______.
Atoms are always larger than their anions.
Effective nuclear charge increases?
up and to the right
As zeff increases, size?
decreases
Atomic radi increase?
down and to the left of the periodic table
What is ionization energy?
the energy required to remove an electron
1st ionization Energy increases?
1st ionization Energy increases to the right and from the bottom to top
What are the exceptions to 1st ionization energies?
Group IIIA and VIA exceptions
An isoelectronic species with the greatest charge in the nucleus will have?
the largest ionization energy
Successive Ionizations are always?
larger than 1st ionization energies
What produces a much larger ionization energy?
when a non-valence electron is removed
What is Electron affinity?
energy change when a electron is added to an atom to a gaseous atom to form an anion
What is the equation for electron affinity?
A(g) + e- ->A-(g)
The reactivity of the Group 1A metals increases?
The reactivity of the Group 1A metals increases down the group
What are alloys?
mixture of metals
The halogens all exist as?
diatomics
Halogen reactivity increases as you go?
up the group
What is ionic bonding?
+/- attracted to form bonds
What is covalent bonding?
The sharing of electrons
What is lattice energy?
the energy required to seperate one mole of ionic solid into its gaseous ions
As charge goes up, lattice energy goes?
up
************* as r (distance between ions) goes up, then lattice energy goes?
down
To arrange by increasing lattice energy you?
assess charge first and then distance
Ionic bonding is?
a metal and a nonmetal cations and anions electron transfer
What is bond order?
the number of electron pairs shared between two atoms
What is the bond order below?
a) N-N
b) N=N
a) 1
b) 2
As bond order increases, bond length?
decreases
As bond order increases, bond strength?
increases
What are the steps to writing Lewis Dot structure
1) Skeleton structure
2) Sum valence electrons
3) Subtract 2e- for every bond in skeleton structure
4) Count electrons needed to complete (need) structure
5) Add extra electron as base pai
If the electron sharing is equal, what type of bond is it?
a nonpolar convalent bonding
If electron sharing is not equal, what type of bond is it?
polar covalent bonding
What is electronegativity?
a measure of the ability of an atom to attract the shared electrons in a chemical bond
Electronegativity increases?
up and to the right
As the difference in electronegativity increases, the polarity of the bond?
increases
The most polar bond will have?
the biggest difference in electronegativity
The central atom is?
the least electronegative element
How do you calculate formal charge?
The # of valence electrons - # of bonds - # of lone electrons = formal charge
What Lewis structures are favored?
the structures of the smallest formal charge
What are the rules for evaluating the stability of structures?
Smallest formal charge favored
Structures with adjacent atoms with formal charges of the same sign are much less favored
Lewis structures that place negative formal charges on more electronegative atoms are favored
Formal charges of opposite signs are usually on adjacent atoms
What is a resonance structure?
when a molecule has more than 1 formal charge
No resonance structure is correct by itself, how is the correct structure formed?
By the average between all the resonance structures
What molecules disobey the octet rule?
H needs 2e- to be stable He needs 2e- to be stable 2A&3A central atoms don't need all electrons Group IIA central atoms need 4e- Group IIIA central atoms ned 6e- Expanded valence shell z>15
____ formal charge is more favored than ___ formal charge.
No formal charge is more favored than any formal charge.
An expanded valence shell molecules have?
more than eight electrons about an atom in a Lewis structure
bond energy is?
the energy required to break bond
Bond energies are always?
endothermic because it takes energy to break a bond
