Final Memorization

What did Dalton come up with?

Atomic theory

What are the postulates of atomic theory?

1) Matter is composed of exceedingly small particles called atoms. An
atom is the smallest unit of an element that can participate in a
chemical change.
2) An element consists of only one type of atom, which has a mass
that is characteristic of the element and is the same for all atoms
of that element.
3) Atoms of one element differ in properties from atoms of all other
elements.
4) A compound consists of atoms of two or more elements combined
in a small, whole-number ratio. In a given compound, the number
of atoms of each of its elements are always present in the same
ratio.
5) Atoms are neither created nor destroyed during a chemical
change, but instead rearrange to yield a different type(s) of matter.

What did JJ Thompson calculate?

Charge to mass ratio

What did JJ Thompson discover?

The electron

What was Robert A Millikan’s experiment?

Oil Drop Experiment

What did Millikan discover?

The charge of an electron

What did Millikan’s discovery lead to?

The mass of an electron

What was Ernest Rutherford’s experiment?

Gold Foil Experiment

Describe Rutherford’s experiment

He shot positively charged alpha particles at a thin sheet of gold foil. He expected them to pass through with little to no deflection. Most weren’t deflected at all, but some shot back at very large angles

What did Rutherford discover?

The nuclear model

Who proposed the Plum Pudding Model?

JJ Thompson

What did Frederick Soddy discover?

Isotopes

What did James Chadwick discover?

Neutrons

What did Bohr’s model say?

The electrons travel in orbits (stationary states) that are at a fixed distance from the nucleus with fixed energy

Formula for Heisenberg’s Uncertainty Principle

Uncertainty in position(mass*uncertainty in velocity) >= h/(4pi)

Aufbau Principle

Electrons are added to the lowest energy orbitals first before moving to higher energy orbitals

Pauli exclusion principle

No two electrons in an atom may have the same set of four quantum numbers (n, l, ml, ms)

Hund’s rule

When filling orbitals that have the same energy, electrons fill them singly first with parallel spins

When are d and f electrons core?

When that d or f level is filled

How do chalcogens react with metals?

Form an anion with charge of 2-

How do chalcogens react with nonmetals?

They tend to share electrons

In which directions, does the size of an atom increase?

As you go down and as you go left

How does ionization energy relate to the size of an atom?

It follows the opposite trend

What makes an atom paramagnetic (attracted by magnets)?

Some electrons are unpaired

What is related to a positive ion?

Ionization energy

What is related to a negative ion?

Electron affinity

When is energy released?

When an electron is added

When is energy absorbed?

When an atom loses an electron

How does metallic character relate to the size of an atom?

It follows the same trend

What type of molecules form ionic bonds?

Metals and non-metals

What type of molecules form covalent bonds?

Two non-metals

What types of bonds do molecular compounds have?

Covalent

List the diatomic molecules

Br, I, N, H, F, O, Cl

Change in energy of an atom

-2.18×10^-18J*(1/(nf)²-1/(ni)²) where n is the level of the electron

Ammonium

NH4(+)

Acetate

CH3COO(-)

Hydroxide

OH(-)

Nitrate

NO3(-)

Nitrite

NO2(-)

Permanganate

MnO4(-)

Dichromate

Cr2O7(-2)

Carbonate

CO3(-2)

Bicarbonate

HCO3(-)

Phosphate

PO4(-3)

Chlorate

ClO3(-)

Perchlorate

ClO4(-)

Sulfate

SO4(-2)

Sulfite

SO3(-2)

When is a bond pure covalent?

The electronegativity difference is =< 0.4

When is a bond polar covalent?

The electronegativity difference is =< 1.7 and >= 0.5

When is a bond ionic?

The electronegativity difference is >= 1.8

List the 6 strong acids

Hydrochloric (HCl), hydrobromic (HBr), hydroiodic (HI), nitric (HNO3), sulfuric (H2SO4), perchloric (HClO4)

List the 3 strong bases

Sodium hydroxide (NaOH), potassium hydroxide (KOH), and lithium hydroxide (LiOH)

What are the four basic assumptions of kinetic molecular theory?

A gas is composed of particles separated by large distances and the volume occupied by individual molecules is negligible; gas molecules are constantly in random motion, moving in straight lines, colliding with perfect elastic collisions; gas molecules don’t exert attractive/repulsive forces on one another; average KE of gas molecules in a sample is proportional to the absolute temperature

Combined Gas Law

P1*V1/n1*T1=P2*V2/n2*T2

Which compounds are soluble with no exception?

Group 1A, ammonium, acetate, bicarbonate, nitrate, and chlorate

Which compounds are soluble with some exceptions?

Chlorine, bromine, iodine, and sulfate

When are chlorine, bromine, and iodine soluble?

When they are paired with silver, mercury, and lead

When is sulfate soluble?

When paired with silver, barium, calcium, mercury, lead, and strontium

Which compounds are insoluble with exceptions?

Carbonate, chromate, phosphate, sulfur, and hydroxide

When are carbonate, chromate, phosphate, and sulfur soluble?

When paired with group 1A elements or ammonium

When is hydroxide soluble?

When paired with group 1A elements, ammonium, or barium

What sign is released energy?

Negative

What sign is absorbed energy?

Positive

When is heat positive?

When the system gains thermal energy

When is heat negative?

When the system loses thermal energy

When is work positive?

When it is done on the system

When is work negative?

When it is done by the system

When is bond energy positive?

When it is from the reactants

When is bond energy negative?

When it is from the products

When is the formation energy positive?

When it is for a product

When is the formation energy negative?

When it is for a reactant