Chapter 6 Electromagnetic Radiation & the Electronic Structure of an Atom

orbital label for l=0

s

orbital label for l=1

p

orbital label for l=2

d

orbital label for l=3

f

shape of orbital label s and number of orbitals of this type

sphere, 1 orbital (2 electrons)

shape of orbital label p and number of orbitals of this type

dumbbell, 3 orbitals (6 electrons)

shape of orbital label d and number of orbitals of this type

cloverleaf, 5 orbitals (10 electrons)

shape of orbital letter f and number of orbitals of this type

complex and flower-like, 7 orbitals (14 electrons)

in a double displacement neutralization reaction…

an acid reacts with a base to give a salt plus water

in a double displacement gas-forming reaction…

the cations and anions of two aqueous ionic compounds swap partners to form two new products, one of which is an unstable compound that immediately decomposes into a gas and another stable product

in a double displacement precipitation reaction…

the cations are "swapped" and one of the products is a solid and the other(s) are aqueous

in a decomposition reaction…

a single compound breaks down into two or more simpler substances

in a single displacement reaction…

an uncombined element replaces an element in a compound

Oxidation number of each atom in a pure element

oxidation number= 0

Oxidation number of a monoatomic ion

oxidation number = ionic charge

Oxidation number of a halogen (F, Cl, Br, I) in a compound when not combined with oxygen or fluorine

oxidation number = -1

Oxidation number of a halogen (F, Cl, Br, I) in a compound when combined with oxygen or fluorine

oxidation number does not = -1

Oxidation number of oxygen in compounds

oxidation number = -2 (except in peroxide = -1)

Oxidation number of hydrogen when mixed with metals

oxidation number= -1

Oxidation number of hydrogen when mixed with nonmetals

oxidation number = +1

Titration equation (acid neutralizing base & vice versa)

M₁V₁=M₂V₂

Soluble ionic compounds

Na⁺, K⁺, NH₄⁺, NO₃^-, CH₃CO₂^-, ClO₃^-, ClO₄^-, Cl^-, Br^-, I^-

Strong acids

HCl, HBr, HI, HNO₃, HClO₄, H₂SO₄

Weak acids

HF, H₃PO₄, H₂CO₃, CH₃COOH

Strong bases

LiOH, NaOH, KOH, Ba(OH)₂, Sr(OH)₂

Weak base

NH₃

In redox reactions: elements that get oxidized are called…

reducing agents

In redox reactions: elements getting reduced are called…

oxidizing agents

Increasing order of wavelength

gamma rays, X-rays, UV, visible light, infrared, microwaves, FM radio waves, AM radio waves, long radio waves

Frequency equation

v=c/λ, λ: [m], v: [Hz]

Planck’s equation (energy of a photon)

E_photon=hv, E_photon: [J], v: [Hz]

Formula for energy of each level

E=-2.179×10^-18(1/n²)

+ΔE

absorption of energy

-ΔE

emission of energy

Energy equation

E=hv

de Brogile equation

λ=h/mv, λ: [m'], m: mass of particle [kg], v: velocity [m/s], h: Planck’s constant

n is known as the ___ quantum number, and what does it specify?

principal, describes the size and energy of the shell in which the orbital resides

l is known as the ___ quantum number, and what does it specify?

angular momentum, subshell, specifies the shape of the orbital

m_l is known as the ___ quantum number

magnetic

nodes

regions of space where there is 0 probability of finding an electron (planar/angular: flat or cone, radial: spherical)

m_s is known as the ___ quantum number

electron spin

How many electrons can each orbital accommodate?

up to 2 electrons

What are the allowed values of m_s?

-1/2 or +1/2

For any value of n, what values can l have?

l can have values ranging from 0 to (n-1)

For a specific value of l, what values can m_l have?

m_l can have integer values that range from -l to +l

How many different values can m_l have?

2l +1

Number of orbitals in a shell?

n²

Number of orbitals in a subshell?

2l +1

Number of radial nodes for an orbital?

n-l-1

Total number of nodes (planar + radial) for an orbital

n-1

Aufbau principal

lower energy orbitals are filled before higher energy levels

Pauli’s Exclusion Principle

2 electrons within an atom cannot have the same set of 4 quantum numbers (n, l, m_l, and m_s), means orbitals can accommodate up to 2 electrons

Hund’s Rule of Maximum Multipllicity

every orbital in a subshell is singly occupied with one electron before any one orbital in that subshell is doubled up 

Common oxidizing agents

oxygen, H₂O₂, the halogens, and species containing elements that are in their higher oxidation states such as HNO₃, MnO₄^- and Cr₂O₇^2-

Common reducing agents

hydrogen, carbon, and metals such as K, Na and Al