Chemistry Quiz 2

Blackbody Radiation

Planch

Photoclentric effect

Eistein

Atomic Line Spectra

Bohr

Heisenberg’s uncertainty Principal

It is not possible to know the position and energy if a moving particle at the same time.

Atomic Orbital

Where an electrons spends most of its time e^- of a specific E

Energy (n)

Size of atomic orbital and distance from nucleus

Shape (L)

Angular Momentum

Orientation (m_l)

spatial orbital orientation

L

=Integer from 0 to (n-1)

Which n=# is the closest to the nucleus

n=1

How to find L numbers

L→0→(n-1)

Magnetic Quantium # (m_l)

-L→0→+L

Value of L=0

S

Value of L=1

P

Value of L=2

d

Value of L=3

f

Value of L=4

g

L=O (s orbital)

L=1 (p orbital)

L=2 (d orbital)

M_s

Electron spin quantum # (+1/2 or -1/2)

Paulis exclusion Principle

No two electrons in the same atoms can have the same 4 quantum numbers.

Aufbau Principle

Electrons frill orbitals start at lowest possible energy before filling higher stats.

Pauli’s Exclusion Principle

Max two Electron with opposite spins

Hunds Rule

When orbitals of equal energy are avaliable the electron configuration of the lowest energy has max # of unpaired electrons with parallel spin.

Condensed Configuration

Has the same symbol of the previous noble gas in square brackets

Exceptions to 4s & 3d Sublevels

Chromium (Cr; z=24) → [Ar] 4s¹3d⁵

Copper (Cu; z=29) → [Ar] 4s¹3d¹⁰

Inner (Core) Electrons

Electrons that are closer to the nucleus, Subtract the number of valence electrons from the atomic number.

Outer electrons

Highest energy Value/Level and spend most of their time away from the nucleus

Valence electrons

The electrons in the outermost shell.

Main group: Valence electrons are outer electrons

Transitional: Valence electrons include outer ns electrons and any (n-1)d electrons

paramagnetism

attracted by a magnetic field

Diamagnetism

not attracted and slightly repellent magnetic field

The three atomic properties

Atomic Size, Ionization energy, electron affinity

Metallic Radius

Metals, ½ shortest distance between nuclei

Covalent Radius

Non metals, ½ shortest distance but bonded atoms

Trends in atomic size (Main group)

Increases down a group and decreases across a period.

Ionic Radius

Measure of the size of an Ion and is obtained from the distance between the nuclei of adjacent ions in a crystalline ionic compound.

Trends in Ionic compounds (Parent atoms)

Cations are smaller while anions are bigger

Trends in Ionic Compounds (Ionic Radius)

Increases down a group, generally decreases except from the last cation to the first anion

Trends in Ionic compounds (Cation)

Cation size decreases as charge increases

isoelectronic series

Atoms that have the same electron configuration, ion size decreases as nuclear charges.

Ionization energy (IE)

Energy required for the complete removal of 1 mole

Ionization Energy Trends (Group)

N value increases

atomic size increases

distance increases

attraction lessens

Ionization energy Trends (Period)

Z_eff increases

atomic size decreases

attraction increases

Low IE

Cations

High IE

Anions

Electron Affinity

Energy change that occurs when 1 mol of electrons is added to 1 mol of gaseous atoms or ions

Low EA

Cations

High EA

Anions

Reactive Non-Metals

High IE, Highly negative EA and form negative ions

Reactive Metals

Low IE, Slightly negative EAs and form positive ions

Nobel gases

Very High IE, Slightly positive EAs

Metallic Bonding

Electrons pooling with a metal to another metal

Bonding capacity

Number of Covalent bonds an atoms forms to have an octet of electrons in a valence shell

Coulombs Laws

Electrostatic potental Energy

Energy = (Charge 1 x Charge 2)/Distance (Size)

Lattice Energy

Enthalpy change that occurs when 1 mole of ionic solid separated into gaseous Ions

Lattice energy trends

As ionic charge increases, Lattice Energy Increases

As Ionic size decreases, Lattice Energy Increases

Ionic Compounds (Physical Behavior)

Hard, Rigid, Brittle

Ionic Compounds (Electrical Conductivity)

Do not conduct in a solid state but do if melted or dissolved

Ionic Compounds (Thermal Conductivity)

High melting points and a much higher boiling point

Bond Energy

Bond Enthalpy or bond strength

Endothermic

Bond Breakage

Exothermic

Bond forming

Bond Length

Distance between the nuclei of the bond atoms

Trends in Bond Order (Length)

Higher bond oder results in shorter bond length and higher bond energy

Increases down a group and decreases across the period

Shorter bond

Stronger bond

Molecular Covalent Substances

Individual molecules

strong intramolecular forces

Much weaker intramolecular forces (IF)

Network Covalent Solids

No separate molecules

Strong Intramolecular forces

Molecular Covalent Compound (Physical Properties)

Soft, low melting, and low boiling

Network Covalent solid (Physical Properties)

Hard, high melting point

Covalent Electric Conductivity

Most are poor conductors whether melted or not

Polar Covalent Bonds

Unequal Sharing of bonding pair, uneven distribution of charge (Much more common)

Electronegativity Trends

Down a group energy decreases as size increases

Across a period (Main group) it increases.

Nonmetal are more Electronegative than Metals