CH 101 Final
Excited state electrons exist when...
"hole" in lower energy orbital when electrons do not follow Hund's Rule
what is the bond order equation
#bonding pairs - #antibonding pairs
how to draw the p orbital?
'peanut'. can be oriented to the x,y, or z axis. one side of the peanut will be shaded in, the other will not (represents wavefunction)
Millikan's Oil Drop Expirement
* Millikan's experiment studied the behavior of charged oil droplets in an electric field. He was able to measure the fundamental unit of charge, which we now know as the charge on the electron. * Note that while this experiment did NOT measure the mass of the electron, Millikan was able to use his charge and Thomson's charge to mass ratio in order to calculate the mass of the electron.
Ruthford's Goil Foil Experiment
* The particles, moving at 10,000 mi/s, were predicted to go straight through the foil. Since the atoms in the foil were believed to be uniform, all of the alpha particles would likely do the same thing regardless of where they struck the foil. * While most of the alpha particles went straight through, some changed their direction, and a few (about 1 in 20,000) bounced straight back towards the source. * The only way the alpha particles could bounce straight back is if there was something heavy and dense in the atom. * He reasoned that most of the mass of the atom was concentrated, located in what was called the "nucleus". The rest of the atom was empty space. Note that the experiment didn't suggest anything about the position of the electrons.
What is the allowed 'm_s" quantum number?
+/- .5
How many moles of sodium are contained in 32.2 grams of Na2SO4
.453 mol Na
In an orbital energy diagram how many electrons are in a unoccupied orbital?
0
In an orbital energy diagram how many electrons are in a occupied half-filled orbital?
1
how many pi and sigma bonds are in the nitrate ion
1 pi 3 sigma
Using the Rydberg Equation
1. plug given values into Rydberg Equation of frequency 2. convert frequency to wavelength using c = λv 3. since the answer is given in meters it must converted into nm using 10^9 as the conversion factors.
How many grams of hydrogen are in a sample of C8H18 that contains 0.600 moles of C?
1.36 g H
what is the bond order of HCO2^1-
1.5
d sublevel can hold how many electrons
10
if there are 4 electron groups what is the bond angle
109
what is the bond angle for CH4
109
What is the bond angle and shape of H2O
109 and bent
How many individual nitrogen atoms are contained in one mole of Cu(NO3)2
12.02 *10^23
if there are 3 electron groups what is the bond angle
120
f sublevel can hold how many electrons
14
if there are 2 electron groups what is the bond angle
180
In an orbital energy diagram how many electrons are in a occupied filled orbital?
2
s sublevel can hold how many electrons
2
In order to fulfill the octet rule, how many valence must be present
2 for Hydrogen and 8 for everything else
Set up this problem: How many moles of iron are contained in a sample of Fe2(SO4)3 that also contains 2.50 x 1024 oxygen atoms?
2.50 x 1024 O atoms x (2 mol Fe/12 x 6.02 x 1023 O atoms) = 0.692 mol Fe
How many individual Cr3+ ions are in a sample of CrCl3 that contains 4.50 g of Cl?
2.55 * 10^22 Cr3+ ions
How many grams of hydrogen are contained in 7.25 moles of NH3
21.9 g H
# of valence electrons in NO3^1-
24
# of valence electrons in C4H10
26
# of valence electrons in BrCl3
28
which is the lower energy oribital: 2s on Se OR 2s on Cu
2s on Se
How many moles of potassium are contained in one mole of K3PO4
3
how many electron groups are in SO2
3
How many grams of oxygen are contained in one mole of Na2CO3
3 * 16.00 = 48
When the rope is in motion, it describes a ___________space.
3D
which is the lower energy orbital: 4p on Se OR 3p on S
3p on S
which is the lower energy oribital: 3s on Na OR 3p on S
3p on S
which is the lower energy oribital: 4s on Ca OR 3s on Mg
3s on Mg
which is the lower energy orbital: 3s on Na OR 3s on S
3s on S
How many unpaired electrons are in Ru
4
how many electron groups are in CH4
4
how many electrons are in a double bond
4
Based on this blank diagram https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198580/mod_ncsubook/chapter/5416/BondingDetails14.gif what is the bond order of C2, O2, O2^+, O2^-
4-2=2 5-3=2 5-2.5=2 5-3.5=1.5
What is the highest occupied orbital of Ru
4d
which is higher in energy 4d on Nb or 5s on Nb?
4d on Nb
which is higher in energy 6s on La or 4f on La?
4f on La
What is the highest occupied orbital of K
4s
What is the valence electron configuration of Ru
5s^2 4d^6
What is the valence electron configuration of I
5s^2 5p^5
how many electrons are in a triple bond
6
p sublevel can hold how many electrons
6
Planck's Constant
6.626 x 10-34 J-s
# of valence electrons in H2O
8
average kinetic energy
=3/2 RT
Aluminium Nitride
AlN
What principle states that electrons occupy the lowest energy orbitals?
Aufbau Principle
Which models of Columb's, Bohr's and Quantum is quantized?
Bohr and Quantum (Columb's is continuous)
Quantum v Bohr model
Bohr only has quantum levels which does not include the orbitals The quantum model therefore predicts the emission spectra of one electron species. the sublevels in the quantum model separate and thus can This can explain the greater number of lines seen in chemical species with more than one electron. https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198545/mod_ncsubook/chapter/5259/Quantum07.jpg
Sigma bonding.
Bonding that occurs when orbitals point towards one another and overlap in space
Acetate
C2H3O21-
Cyanide
CN1-
carbonate
CO32-
calcium nitrite
Ca(NO2)2
hypochlorite
ClO1-
chlorite
ClO21-
chlorate
ClO31-
perchlorate
ClO41-
# of Core and # of Valence e- in O
Core: 2 Valence: 6
# of Core and # of Valence e- in Rb
Core: 36 Valence: 1
# of Core and # of Valence e- in Re
Core: 68 Valence: 7
dichromate
Cr2O72-
chromate
CrO42-
How many moles of each element are present in Cu(NO3)2
Cu = 1 N = 2 O = 6
Law of Multiple Proportions
Dalton if there are two compounds made up of the same elements, the mass ratios of the elements in the two compounds will be related by simple whole numbers semicondutors have multiple mass ratios they disprove
Rydberg Equation
E = Z^2*h*R_H*(1n2lo - 1n2hi) Here, h is Planck's constant, which appears because of the conversion from frequency to energy (E = hν). The constant in the previous equation has been shown explicitly. Z is the charge on the nucleus (the atomic number) and RH is the Rydberg constant. The atomic number Z appears in the relationship, because spectra of other "one electron species" (those that have one electron present) have a series of lines that can be characterized by the same equation.
photon model of light
E = hv
Bohr equation using Rydberg
E = − (Z^2 h R_H)/n^2
Dalton's Atomic Theory
Each element is composed of atoms. All atoms of a given element have the same properties and mass. Atoms of different elements have different properties and different masses. Atoms of different elements combine in small integer ratios to form compounds. Atoms do not change during chemical reactions, they simply rearrange.
Wavefunctions
Each wavefunction has a corresponding energy. Each wavefunction defines a three dimensional region in space, called an "orbital".
_______________________________ lead to polar covalent bonds.
Electronegativity differences
A) n = 4 → n = 6 B) n = 6 → n = 3 C) n = 3 → n = 5 D) n = 2 → n = 1 Which emission process gives a photon of smaller wavelength? Which absorption process is of greater energy?
First we need to decide which transitions represent emission of energy and which represent absorption of energy. Emission occurs when the atom goes from a higher energy level to a lower one. That would be B and D. If we want a photon of smaller wavelength, we want a greater energy transition. Even though B is a jump of three levels and D is a jump of only one level, we need to recognize that the energy difference between n = 2 and n = 1 is three quarters of the entire energy range available to the atom. Therefore, D will give a photon of smaller wavelength. A and C are the absorption processes, since the atom goes from a lower to a higher energy level. Each is a jump of two levels. Again though, the spacings are larger at the lower levels, so C is of greater energy.
Hydronium
H3O1+
What principle is being followed by drawing two opposing arrows in one orbital? Why?
Hund's Rule, because electrons must be of equal energy because it is the lowest energy configuration
Law of Definite Proportions
Joesph Proust elements will always be present in the same mass ratio in any sample of a compound. isotopes disprove
potassium phosphate
K3PO4
Law of Conservation of Mass
Lavoisier matter cannot be created or destroyed e=mc^2 semi disproves
In comparing the n = 1 levels in the He1+ and the Li2+ ions using the Bohr model, which ion will have the lower energy n = 1 level? If the value of R is the same, by what factor do the two energies differ?
Li2+ 9/4
In comparing the He1+ and the Li2+ ions using Coulomb's Law, which ion will be at lower energy? If the electron - nucleus distance is the same, by what factor do the two energies differ?
Li2+ 3/2
which is larger (mass) one mole of HCN and one mole of LiF
LiF (6 + 19 = 26) < HCN (1 + 12 + 14 = 27)
Process of Model
Mass laws -> dalton's theory -> cathode ray / oil drop -> subatomic particles -> gold foil -> electrons -> emission spectra -> energy levels
What is the point of Schrodinger wavefunctions?
Mathematical functions, although quite complicated, have been derived to describe electrons moving about a central nucleus as waves. Each function describes a mode of motion, and has a corresponding energy. These functions can be grouped together by what we call their quantum numbers.
The waves can be modeled by _________________________. As the frequency goes up, the ___________ goes up, and the number of nodes (the points where the function equals to zero) goes ____.
Mathematical functions; energy; up
permanganate
MnO41-
which has the least and most amount of mass 2 mol of BH3 9 x 1023 O2 molecules 1 mol of HCl
Molar mass of BH3 = 14 g/mol 2 moles of BH3 will have a mass of 28 grams. Molar mass of O2 = 32 g/mol. This sample is 1.5 moles (9 x 1023 is 1.5 times Avogadro's number), so this sample would have a mass of 48 grams. Molar mass of HCl = 36 g/mol. Since this sample is one mole, this sample has a mass of 36.
Ammonium
NH1+
Can electrons be described quanitized?
NO only light can, energy in not continuous
nitrite
NO21-
nitrate
NO31-
peroxide
O22-
what is the formal charge of every atom in a CO2 molecule where one oxygen is a triple bond and the other is single bond?
O: +1 C: 0 O: -1
hydroxide
OH1-
which is larger (atoms) one mole of CH4 and one mole of PCl3
PCl3 (1 + 3 = 4) < CH4 (1 + 4 = 5)
A 1.00 L flask contains air at a pressure of 1.00 atm at 300 K. 5.00 g of liquid N2 is added to the flask. The flask is sealed and the liquid dinitrogen is allowed to vaporize. When the flask returns to 300 K, what is the pressure inside?
PN2 V = nN2 R T PN2 V = nN2 R T 5.00 g N2 x 1 mol N2/28.02 g N2 = 0.1784 mol N2 5.00 g N2 x 1 mol N2/28.02 g N2 = 0.1784 mol N2 PN2 = (0.1784 mol) (0.0821 L - atm/K - mol) (300 K)1.00 L = 4.39 atm PN2 = (0.1784 mol) (0.0821 L - atm/K - mol) (300 K)1.00 L = 4.39 atm PTotal = Pair + PN2 = 1.00 atm + 4.39 atm = 5.39 atm
phosphate
PO43-
Ideal Gas Law
PV=nRT
What principle is being followed when drawing one arrow up and the other down in orbital energy diagrams?
Pauli Exclusion Principle
sulfite
SO32-
sulfate
SO42-
what is the formula to predict shared pairs for a Lewis structure?
SP = 0.5(ER-VE)
What is the symbol for the isotope with 15 protons, 16 neutrons and 18 electrons?
Symbol is 31P3-.
Thomson's Raisin Pudding Model
The Thomson model of the atom was then like a ball of raisin pudding, where the pudding was a mass of positive charge, and the electrons were randomly imbedded, like raisins in pudding.
Bohr Model of the Atom
The energy of an atom is quantized. An atom can exist only at certain, prescribed energies; never in between. The energy of the photons emitted from an atom tell you the energy difference between the quantized energy levels.
But why can't lower energy light simply shine on the surface longer, or shine brighter, to achieve the same result?
This must be because the energy doesn't build up. In other words, light does not behave as a continuous wave when transferring its energy to the surface of a material.
nuclear model of the atom
This picture shows the Rutherford atom with the positive charge concentrated in a nucleus, instead of spread out throughout the atom. Note that none of the models are specific on where the electrons are or what they are doing.
Thomson's Cathode Ray Expirement
Thomson's experiment studied cathode rays (particles that appeared to jump from a negatively charged plate to a positively charged plate). Thomson observed their behavior at they traveled through electric fields, and was able to measure the charge / mass ratio of the rays. We now call them electrons. Proves cathode rays a negatively charged but not the existence of electrons.
VSEPR Stands for ....
Valence Shell Electron "Group" Repulsion
effective nuclear charge
Valence electrons normally don't feel all of the positive charge on the nucleus. Some of it is neutralized, or canceled, but other by electrons.
How many protons, neutrons and electrons are contained in 51V2+
Vanadium is atomic number 23. Therefore, 23 protons. Mass number is 51. 51 = 23 + (# of neutrons), so there are 28 neutrons. Charge is 2+. +2 = 23 - (# of electrons), so there are 21 electrons.
Just like light, electrons display ________
Wave-Particle Duality
constructive interference
When two values of the same sign add together, the result gets bigger.
https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198559/mod_ncsubook/chapter/5317/AtomicProperties18.gif what is the highest and lowest ionization energy what is the highest and lowest electron affinity
Y & Z Y & X
Give electron configuration of Mn2+
[Ar]3d5
Give electron configuration of Na1+
[He]
Full electron configuration of Sn
[Kr]5s^2 4d^10 5p^2
what is the electron configuration of Ir3+
[Xe]4f146d6
elementary substance
a compound that is made out of the same element
Speical names on periodic table
alkali - group 1 alkanline earth -group 2 halogens and noble gases
NH4ClO4
ammonium perchlorate
electronegativity
an atom attracting the valence electrons of another atom in a covalent bond
ionic bond is
an attraction between an anion and cation which leads ions but no molecules
How to name a anion
and the suffix ide to the end
non-metals gain electrons to form ...
anions
elements can be __________________ and _______________ in the their smallest unit
atoms and molecules
Using Figure 5.1 what happens at point 2
atoms interact e= negative (+/- interaction) orbital shape distorts due to attraction
Why does 4s fill before 3d?
because 4s is at a lower energy than 3d
Why does the atomic radii get smaller across the period
because the valence electrons are getting closer to the nucleus and are feeling a more positive charge. Also known as the effective nuclear charge. Valence electrons must go to lower energy
why does ionization energy decrease down a group
because they are larger atoms that hold their electrons loosely thus requiring less energy to remove
why does ionization energy increase across a period
because they are smaller atoms that hold their electrons tightly thus requiring more energy to remove
3 electron groups (1 lone pair, 2 bonded groups) have a shape of
bent
4 electron groups (2 lone pairs, 2 bonded groups) have a shape of
bent
Identify this element https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198548/mod_ncsubook/chapter/5261/ElectronConfigurations04.gif
beryllium
https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198576/mod_ncsubook/chapter/5399/Shape11.gif what is angle shape and hybridization for each colored atom?
blue: 120, trig planar, sp2 orange: 109, trig pyramidal, sp3 pink: 120, trig planar, sp2 purple: 109, tetra, sp3 yellow: 120, trig planar, sp2 green: 109, trig pyramidal, sp3
________________ occur when electrons are not equally shared.
bond dipoles
Using Figure 5.1 what happens at point 5
bond length shortens stronger than electron/nucleus interactionA dipole has a creates a like charge reaction e = positive
which is larger (molecules) one mole of CCl4 and one mole of C3H8
both have one mole of molecules
Metals lose electrons to form ...
cations
When quantifying molecules, we need to know how many moles of _____________________ are present.
compound
compound
contains more than one element
Bonds with a small electronegativity difference will have mostly __________ character
covalent
valence orbitals on different atoms
criterion is the atomic radius Smaller atoms have their valence electrons closer to the nucleus, so they will be at lower energy than valence electrons on larger atoms.
atomic radii ____________ across a period and _______________ down a group
decreases; increases
Mass spectrometry
determines weighted average for periodic table mass. mass of that isotope * abudance in %. Deflection is based on charge to mass ratio
A ____________ has a positive and negative "pole"
dipole
This is the _________ proportionality we expect from the relationship between E and ν.
direct
forces in non-polar molecules
dispersion
Bond order of 2 is a __________ bond
double
as the nuclear charge increases, the energy of the system goes _________ (gets more ____________)
down; negative
If there are formal charges, the best distribution of charges has negative formal charges on the atoms with the highest _____________________________.
electronegativity
When quantifying atoms, we need to know how many moles of the _________________ or elements of interest are present.
element
The energy of the emitted photon is ________ to the energy difference between the two states.
equal
columbs law
for energy instead of r^2 use r
order of light as energy from greatest to smallest frequency
gamma, x-ray, ultraviolet, VIBGYOR, infrared, microwaves, radio
Upon emission of energy, the atom or molecule undergoes a transition from a _________ energy state to a ________ energy state.
higher; lower
energy level diagram
https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198541/mod_ncsubook/chapter/5243/Light05.gif The lowest energy level is for n = 1. The energy levels get closer together as they go up. This diagram is actually not to scale; the levels for n = 2 and above should actually be closer together! For other elements, Z2 ≠ 1. The Z2 term would appear in the numerator, and the energies would occur at different places on the diagram.
How to name a cation
if it does not have a charge then give the element name and write 'atom' after it if it does have a charge put roman numerals in parenthesis that match the charge number and write 'ion' next to it
trends in EA
increases across a period and decreases down a group
trends in EN
increases across a period and decreases down a group
ionization ____________ across a period and _______________ down a group
increases; decreases
As the frequency of the wave __________, the _____________ decreases (this is the same inverse relationship we developed with light).
increases; wavelength
This is the __________ proportionality we expect from the relationship between λ and ν
inverse
Bonds with a large electronegativity difference will have mostly ___________ character
ionic
What is the allowed 'l' quantum number?
l starts at 0 and goes up to minus one under the 'n'. For example, if n is 3, the l can be 0, 1, or 2.
Across the period anions are ____________ than cations
larger
Anions are ___________ than the atoms from which they came
larger
Be, Ca, N - identify the atoms with the largest and smallest radius
largest Ca smallest N
Be, Ca, N - identify the atoms with the largest and smallest electron affinity
largest N smallest Ca
Ge, O, P - identify the atoms with the largest and smallest electronegativity
largest O smallest Ge
Ge, O, P - identify the atoms with the largest and smallest ionization energy
largest O smallest Ge
most bonds with two non-metals are _____ than 50% ionic, while most bonds between a metal and non-metal are ___________ than 50% ionic
less; greater
greater average speed look for
lighter gas and higher temperature
2 electron groups have a shape of
linear
Draw an orbital energy level diagram for sulfur.
look at a https://moodle-courses1617.wolfware.ncsu.edu/pluginfile.php/198548/mod_ncsubook/chapter/5262/ElectronConfigurations05.gif
hydrogen bonding
look for H bonding with N, O, F
valence electrons in larger atoms are at higher energy and are held more ____________` by the nucleus
loosely
Coulomb's law also tells us that as the energy gets _________, the the force of attraction increases.
lower
Upon absorption of energy, the atom or molecule undergoes a transition from a _______ energy state to a _______ energy state.
lower; higher
Columb's law tells us that as the difference between opposite charges decreases, the energy will become _______________. (more ___________)
lower; negative
Coulomb's Law tells us that as the magnitude of the charges increase, the energy will become _________ (more ___________).
lower; negative
higher vapor pressure =
lowest boiling point
What is the allowed 'm__l' quantum number?
m__l is plus/minus whatever the largest l number is for that particular orbital. For example, if l=1 then m__l = -1, 0, +1.
compounds can be broken down into _______________ and _________
molecules and ions
Avagadro's law
moles and volume
When there are ___________ electrons, the electrons not only interact in a coulombic (charge) fashion with the nucleus, but they interact with _______________. These electron-electron interactions will also affect the ______________, and therefore the ________________ of the atoms. Different amounts of interaction should lead to ___________ energies.
multiple; each other; energy levels; properties; different
What is the allowed 'n' quantum number?
n is normally between 1-7 but your professor can expand upon it
what are 4 quantum numbers?
n, l, m__l, m__s
covalent compounds are _______________ material, that are formed by _______________ and held together by ___________ bonds to form ____________________.
neutral; non-metals; covalent; molecules
ionic compounds are _____________ material, that are formed by __________________ and ________________________, and are held together by _________________ bonds.
neutral; one non-metal; one metal; ionic
ions combine to ________________ charge
neutralize
does NH3 hace resonance structures
no
the same orbital on different atoms
not restricted to valence atoms with greater nuclear charge (more protons and neutrons) will have lower energy orbitals than those with smaller nuclear charge
delocalized bonding
occurs in resonance structures of ring based structures and is represented by a circle
antibonding
occurs when the opposite wavefunctions on the orbitals cancel each other out
non-bonding
occurs when there is anti and nonanti bonding components
sometimes in order to get rid of formal charge, you must break the __________________________
octet rule
Using Figure 5.1 what happens at point 3
orbital interacts more cause more orbital distortion partial overlap space e = more negative (as +/- interaction becomes stronger)
Using Figure 5.1 what happens at point 4
orbitals have fully overlapped e = minimum energy e at this point is bond energy the distance between nuclei is bond length
pi bonding
overlapping orbitals that are parallel to on another touch in two places above and below the internuclear axis
photoelectric effect
phenomenon where light impinging on certain materials can cause electrons to be ejected from the surface.
When explaining the photoelectric effect, light is modeled as a _________.
photon
double bonds are 1 ____________ interaction and 1 _____________ interaction
pi ; sigma
triple bonds are 2 ____________ interactions and 1 _____________ interaction
pi ; sigma
graph for like and opposite charges
picture shown is opposite flip over axis for like
The larger the difference in eletronegativities the more __________ the bond is
polar
As electrons move closer to the nucleus they will feel a more ___________ charge
positive
Boyle's law
pressure and volume
The wave is ______________; it can exist as one loop, two loops, three loops, etc., but not a __________ of a loop. We can also look at this as the _____________ being quantized; it can be the distance between the ends, half the distance, a third of the distance, etc.
quantized; fraction; wavelength
order of light as energy from greatest to smallest wavelength
radio, microwaves, infrared, ROYGBIV, ultraviolet, x-ray, gamma
what is the best visualization of standing waves?
rope.
order of sublevel orbitals from lowest to highest
s, p, d, f
all single bonds are _________ interactions
sigma
Bond order of 1 is a __________ bond
single
Strongest bonds
single<double<triple
Cations are __________ than the atoms from which they came
smaller
However, a ___________ value of r only reinforces the point that as the nuclear charge increases, the energy of the system goes down (gets more negative)
smaller
if there are 2 electron groups what is the hybridization
sp
if there are 3 electron groups what is the hybridization
sp2
if there are 4 electron groups what is the hybridization
sp3
wave model of light
speed of light(c) = wavelength(λ) * freqeuncy(v)
how to draw the s orbital?
sphere of one color
Charles' law
temperature and volume
4 electron groups ( 0 lone pairs, 4 bonded groups) have a shape of
tetrahedral
why does atomic radii get larger down a group
the # core electrons increases thus increases the amount of shielding that pushes the electrons out
Using Figure 5.1 what happens at point 1
the atoms do not interact because they are too far apart E=0 orbitals are spherical
electron affinity
the energy change when an atom gains an electron
ionization energy
the energy required to remove a valence electron from an atom
Dalton on Atoms
the smallest unit of each element is an atom all atoms of an element have unique properties all atoms of an element have the same mass* * We know today this last statement is not true; "isotopes" of elements exist which have different masses. We will consider isotopes later in the course.
Wave Particle Duality
there is more than one way to explain the properties of light In some experiments, like the photoelectric effect, it is best explained as a particle which we call a photon. Light is a form of energy In other experiments, it is best explained as a wave, such as when light diffracts. Diffraction is a property of sound waves, water waves and light.
valence electrons in smaller atoms are at lower energy and are held more ____________ by the nucleus
tightly
sigma bonding
touch in one place on internuclear axis overlapping orbitals pointing to one another
3 electron groups (0 lone pairs, 3 bonded groups) have a shape of
trigonal planar
4 electron groups (1 lone pair, 3 bonded groups) have a shape of
trigonal pyramidal
Bond order of 3 is a __________ bond
triple
Shortest bonds
triple<double<single
covalent bond is
two elements sharing electrons to create molecules
that core electrons do a much better job of shielding the valence electrons, than the ____________ electrons do of shielding ______________.
valence; each other
V2O5
vanadium(V) oxide
When explaining diffraction, light is modeled as a ________.
wave
destructive interference
where the two functions cancel each other out
how to name a covalent compound
write the name element (and prefix if needed for more than 1 molecule of that element) for the first and then give the second element a prefix (always) and change the ending to -ide
does CO2 have resonance structures
yes
The best lewis structures have ___________ formal charge. The bigger the charge (either + or -) the _________ the structure.
zero; poorer
Frequency in the Rydberg Equation
ν = (constant) (1/n^2_lo - 1/n^2_hi) The constant is 3.290 x 10^15 s−1