U1 - IB Chem

e- transition from n=1 to n=infinity

e- has been removed

1st ionizaiton energy

1st ionization energy

energy needed to remove 1 mole of e- from 1 mole of gaseous atoms in the ground state

ionization energy trends

down group - dec

across period - ince

is 1st or 2nd ionization energy greater

2nd is greater

continuous spectrum

shows wavelengths of visible light

absorption spectrum

continuous spectrum with black lines to represent energy abosorbed by e-

emission spectrum

shows energy of the light emitted as e- falls down

Hydrogen Emission Spectrum

LBP

Lynman Series - ultraviolet - e- falls to n=1

Balmer Series- visible light - e- falls to n=2

Paschen Series - infared light - e- falls to n=3

units for frequency

s^-1 , hertz

units for wavelength in equation

use nm (1×10⁹ nm = 1 m)

units for energy in equation

Joules

pauli exclusion principle

every orbital holds a max of 2 e-

the e- have opposite spins

aufbau principle

e- are placed in lowest energy level possible

hund’s rule

every orbital within a sublevel gets one e- before any orbital gets two

s sublevel

circle shape

p sublevel

dumbbell shape - on x or y or z axis

exceptions for electron configuration

copper, chromium

copper electron configuration

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰

one 4s e-

chromium electron configuration

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

one 4s e-

What determines color of transition metal?

the color of light transmitted is the complmetary color of the color it absorbs

presence of partially filled d orbitals

Colorless ions

Sc³⁺ [Ar]

Zn²⁺ [Ar]3d10

Cu¹⁺ [Ar]3d10

degenerate

d orbitals of equal energy in a free ion

location of 5 d orbitals

3 between axis

2 along axis

what happens to d orbitals when ligand comes in?

the lone e- repel the 2 orbitals along the axis, causing them to split.

what does more splitting (from ligand) of d orbitals mean?

greater energy gap, more energy needed to excite electron

What causes change of color

anything that changes splitting

What factors affect splitting of ligands

1.) Identity of metal ion - larger metals provide greater splitting - greatter nuclear charge has greater electrostatic attraction to ligand results in more splitting of d orbitals

2.) oxidation state of metal ion - as oxidation state increases splitting of D orbitals increases

3.) Geometry of complex ion

octahedral > tetrahedral > linear

4.) Identity of ligand - stronger ligand, greater splitting

spectrochemical series

I- > Cl- > F- > OH- > H2O > SCN- > NH3 >NO2- > CN- > CO

I clean floors oh water season n-c ho no

Paramagnetic

unpaired electrons

Pulled into magnetic field

Do not retain magnetic properties after field is removed

Where unpaired electrons more attraction

ex paperclip

diamagnetic

paired electrons

weakly propelled by magnetic field

does Not retain magnetic properties after field is removed

Ferromagnetic

contains unpaired electrons that align parallel to each other in domains

Retain magnetic properties after field is removed

Iron cobalt nickel

ex magnet

ligands

species with lone pairs of electrons that form coordinate covalent bonds with central metal ions. Ligands are Lewis bases

monodentant ligands

form cordinate covalent bonds with one long pair of e-

polydentate ligands

contains more than 1 pair of lone e- and can form 2 or more cordinate covalent bonds to the metal ion

bidentant ligands

forms 2 coordinate covalent bonds

hexadentate ligand

has 6 atoms with lone pairs of e-

chelates

2 or more seperate coordinate covalent bonds between ligand and central atom

transition elements

variable oxidation states

incomplete d sublevel as atom or cation

catalytic and magnetic propertiees

what metals are not transition metals

zinc - zn2+ - clear solution

Sn - incomplete d

sc3+ complete d, not transition metal

what transition states Ti, V, Cr, Mn, Fe, Co, Ni, Cu have

+2

what elements are good osidizing agents down to 2+ and 3+ because of high oxidation states

Mn and Cr

hetergeneous vs homogenous catalysts

compare phase of catalyst and reactant

homogenous catalyst example

fe3+ heme in blood to transport oxygen

Co3+ in vitamin b12

catalytic converter in car catalyst

Pd (s) or Pt (s)

2CO(g) + 2NO(g) yields 2CO₂ (g) + N₂ (g)

heterogenous

haber process produciton of amonia catalyst

Fe (s)

3H_{2 (g)} + N_{2 (g)} yields 2NH_{3 (g)}

heterogenous

contact proccess production of sulfuric acid