Chemistry

This will cover electron configuration, stoichiometry, and hybridization.

What is the Principle of Quantum

Principle Quantum # is N: Represents the energy level or shell of an electron in an atom. Higher values of N indicate higher energy levels.

#

Principle Quantum # is N

The main energy level of an atom's electron is the region around the nucleus where the electron is most likely to be found.

What Does the Principle Quantum # tell us?

represents the main energy level of an atoms electron

when “n” is higher it corresponds to blank values of energy for an electron

higher

The three-dimensional region around the nucleus where an electron is most likely to be found. The shape of the orbital is determined by the quantum numbers and can be spherical (s orbital), dumbbell-shaped (p orbital), or complex (d and f orbitals).

Angular Momentum tells us?

the shape of the orbital

What is the angular momentum letter?

a cursive little L

if L is zero what is the shape of the orbital

it is in the S block, so sphere

if L is 1 what is the shape of the orbital?

it is in the p block, so like a peanut

if L is 2 what is the shape of orbital?

it is in the d block so like a flower

if L is 3 what is the letter corresponding to the shape?

the letter would be f

what is the equation used to find the value of L

n-1

if n=4 what is L allowed to be?

l can be anywhere from 0-3 so it covers all orbitals of s-f

Magnetic quantum # tells us?

determines the # of permitted orbitals in any group

what is the letter(s) for magnetic quantum?

ml is the letters

what is the permitted range for m

The range of possible values for an orbital quantum number determines the shape of an atomic orbital. It can be any integer from -l to +l, including zero.

l

-l to +l

what do ml # tell us?

they tell us the orientation of the orbitals so if l=1 we are in the p subshell with three different orientations

ml speciefies blank

the permitted orientation of orbitals

What does the spin quantum # mean

the spin energies for 2 electrons

what do the values of ms have to be

+0.5 or -0.5

what are the letter(s) for spin quantum?

ms

what formula do you use when you need to find the total # of e- in a shell?

2n²

n

main energy level

l

subshell and orbital shape

ml

orientation

ms

electron spin has to be = + or - 0.5

What is the pauli exclusion principle?

no two electrons can have all identical QN

what is Hunds Rule?

electrons wanna be alone so they hunds rule is the max number of unpaired e-

ex: if you are in a p subshell with three e- they are going to occupy one subshell each.

what do we call it when the spin orbital only has one e- in it?

unpaired spin

what do we call it when the spin orbital has two e- in it?

spin paired e-

AUFBAU principle

you go one at a time and orbitals are arranged in increasing energy levels

what is assumed with the building up principle?

it is assumed that the electrons occupy the lowest levels first.

what are the exceptions?

Cr,Mo and Cu,Ag,Au

why is the valence shell important?

it is where the valence electron lives.

what are valence electrons?

these are the outermost electron, they are not considered core electrons.

what is diamagnetism?

diamagnetism are paired electrons that are repelled by magnetic fields

what is paramagnetism?

an unpaired e- that is attracted to a magnetic field

how does a single e- behave?

like a magnet

when there is a high number of unpaired e- what happens to your magetic field?

it is larger

atomic radius decrease from?

left to right

atomic radius increases from?

top to bottom

ionization energy increases from?

left to right

ionization decreases from?

top to bottom

what happens to an atom when an e- is gained?

the anion is larger

what happens to an atom when an e- is lost?

the cation is smaller

electronegativty increases from?

left to right

electronegativity decreases from?

top to bottom

fluorine is the blank

most electronegative atom

what are chemical properties mostly determined by?

the valence shell

what is lack of reactivity associated with?

nobel gasses and full s and p shells

what are the rules for drawing lewis sturctures?

1. # of TOTAL valence electrons

2. draw skeleton structure w/ single bonds

3. distribute extra e- to other atoms

4. if you do not have enough e- resort to double and triple bonds

5. if too many e- place as lone pairs on central atom

Draw the lewis structure for NF3

Draw lewis structure for N2O

What is the formal charge on NF3?

formal charges are 0

what is the molecular geometry on NF3

Triangular Pyramid

what is the electron geometry on NF3

tetrahedral

What is the molecular geometry of N2O?

linear

what is the electron geometry of N2O?

linear

what is the formal charge on N2O?

+1 for N and 0 for O

How do you deduce formal charges?

assign one 1 electron for each shared electron pair (1 for a single and 2 for a double) and add this to the number of unshared e- pairs

how do you know if a formal charge is positive?

if the atom has fewer val e-

how do you know if a formal charge is negative?

if the atom has more val e-

what are the rules to formal charges?

they either have to equal zero when all summed or if its an ion it has to be equal to the charge of the ion.

what is a resonance form?

a resonance form is multiple different formations of a the same molecule. so double bonds would swap places.

What is the octet rule?

the octet rule is that every atom in a molecule has to have eight electrons attached to it in order for the atom to be happy :)

there are some exceptions, how do you distribute e- in an exception?

by the most electronegativity ones

what type of bond do you make if you’re missing 2 e-?

a double bond

what type of bond do you make if you’re missing 4 e-?

a triple bond

if you have two bonds and a lone pair name the molecular and electron geometry.

electron: triangular planar

geometry: bent

if two atoms are identical what is their polarity?

they are non-polar

if two atoms are different whats their polarity?

they are polar

what happens to triatomic polarity?

if it is linear with the same atoms bonded to the central atom then it follows the same atom rule of being non-polar. if the atoms are different it follows the different atom rule, they are polar.

how do we find the hybridization of an atom?

we put all the val e- around each individual atom and connect all the central atoms’ val e-. Carbon will bond completely but nitrogen may have lone pair.

what is the difference of lone pairs and bonds?

lone pairs are extra e- that did not bond to another atom in a molecule, they also always have to be together in pairs. chemical bonds are what connect the central atom to the rest of the molecule

what are single bonds called?

sigma bonds.

what are pi bonds?

pi bonds are the bonds of the molecule that DO NOT participate in the hybridization. pi bonds have density above and below the central line of the atom.

for every double bond there is how many sigma and pi bonds?

one sigma bond + one pi bond

for every triple bond how many sigma and pi bonds?

one sigma + 2 pi bonds

Convert 120g of CH4 into molecules

4.52×10²4 molecules

what is a strong electrolyte?

the solute exists entirely as ions

what is a weak electrolyte?

the solute is only partially ionized.

what is a non-electrolyte?

a solution that has no ions at all

when is a substance considered soluble?

if it has a greater Molarity then 0.1mol/L

when is a substance insoluble?

if it has a molarity smaller then 0.01mol/L

is AgBr soluble?

No, because it is one of the exceptions.

what is a complete ionic equation?

where every molecule is taken apart except for solid and a liquid to help discover NIE.

what is a net ionic equation?

the formula for just the solid or liquid. so anything appears on both sides is cancelled out and just what is left is put into NIE.

what is the NIE of Pb(NO3)2 +H2SO4

Pb^(2+)(aq) + SO4^(2-)(aq) —> PbSO4(s)

what is the NIE of NaCl + NaOH?

No reaction occurs it is all aqueous

what is the arrhenius definition for a Acid?

Acid supplies a H+ to an equation

what is the arrhenius definition for a base?

the base supplies the OH-

what are the six strong acids?

HCl, HBr, HI, HNO3, HClO4, H2SO4 (they are only strong w/ the H+ that is supplied.

What are the eight strong bases?

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

How do you know if you have a neutralization rxn?

you get results of H2O and a salt.

what is ther pH of an acid?

less then 7

what is the pH of base?

more then 7

what is the pH of water?

7 completely neutral

Bronstead-Lowry definition of an acid?

acid is proton donor

Bronstead-Lowry definition of a base?

base is a proton acceptor

what happens if we have a weak acid?

then water acts as a weak base

what happens if we have a weak base?

then water acts as weak acid?

what is molarity?

moles/L, mol/dm³, mol/cm³ and it is the concentration of a solution