Chem Final Sem 1

Dalton

proved Democritus's theory

Rutherford

nucleus of protons and neutrons with electrons circling nucleus (gold foil experiment)

Democritus

Atoms are indivisible and indestructible

Bohr

electrons are found in specific circular paths around the nucleus

Electrons occupy orbits at specific energies

Explained hydrogen spectral lines

Thomson

discovered the electron (1st subatomic particle)

Plum Pudding Model

Law of Multiple Proportions and Definite Proportions

Cathode Ray experiment

(average) atomic mass

found on periodic table (2 decimals)

Atomic number

Hydrogen = 1, helium = 2, etc.

Mass number

protons + neutrons

mn/an E^i

mn = mass number, top

an = atomic number, bottom

E = element symbol

i = +/- how many neutrons

Percent abundance formula

(isotope\#)(%) + (isotope\#)(%)

Ion

an atom that has gained or lost electrons (+ or -)

Isotope

Different number of neutrons and different mass

Law of Multiple Proportions

if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

Law of Conservation of Mass

Matter is not created nor destroyed in any chemical or physical change

Ground state

The lowest energy state of an atom

Excited state

A state in which an atom has a higher potential energy than it has in its ground state

S orbital shape

Sphere

P orbital shape

dumbbell

D orbital shape

clover?

F orbital shape

The really crowded one

Amu

1/12th the mass of a carbon-12 atom

Exceptions for the orbital orders

(He,) Ch, Cu

v

Frequency

λ

Wavelength

Range in size of atomic radii

5 × 10-11 m to 2 × 10-10 m

Heisenberg uncertainty principle

it is impossible to know exactly both the velocity and the position of a particle at the same time

Aufbau Principle

each electron occupies the lowest energy orbital available

Pauli Exclusion Principle

An atomic orbital may describe at most two electrons, each with opposite spin direction

Schrodinger

Showed, through math, that waves can be used to describe electrons in atoms

De Broglie

1929, electrons have properties of both waves and particles

Millikan

Measure the charge of an electron - The Oil Drop Experiment

Planck

Father of the Quantum Theory, determined atoms can emit quanta

Chadwick

first artificial nuclear transformation, existence of neutrons

terra

traditional Notation- 1,000,000,000,000

Exponential- 10ˆ12

Description- Trillion

giga

traditional Notation- 1,000,000,000

Exponential- 10ˆ^9

Description- billion

mega

traditional Notation- 1,000,000

Exponential- 10ˆ5

Description- million

kilo

traditional Notation- 1,000

Exponential- 10ˆ3

Description- thousand

hecto

traditional Notation- 100

Exponential- 10ˆ2

Description- hundred

deca

traditional Notation- 10

Exponential- 10ˆ1

Description- ten

base

traditional Notation- 1

Exponential- 10ˆ0

Description- one

deci

traditional Notation- 1/10

Exponential- 10ˆ-1

Description- tenth

centi

traditional Notation- 1/100

Exponential- 10ˆ-2

Description- hundredth

milli

traditional Notation- 1/ 1,000

Exponential- 10ˆ-3

Description-thousandth

micro

traditional Notation- 1/1,000,000

Exponential- 10ˆ-6

Description- millionth

nano

traditional Notation- 1/1,000,000,000

Exponential- 10ˆ-9

Description- billionth

pico

traditional Notation- 1/ 1,000,000,000,000

Exponential- 10ˆ-12

Description- trillionth

Kelvins to Celsius

-273

Density

Mass/volume

Inorganic chemistry

The study of chemicals that, in general, does not contain carbon

Analytical Chemistry

​The study of the composition of matter

Biochemistry

​The study of the processes that take place in organisms

Organic Chemistry

The study of all chemicals containing carbon

Physical Chemistry

Concerned with the mechanism, rate, and energy transfer that occurs when matter undergoes a change.

Chemical Reaction

Process in which substances are changed into different substances

Homogenous

Describes mixture with a uniform composition.

Distillation

A process in which a liquid is boiled to produce a vapor that is condensed again into a liquid.

Mass

Amount of matter an object contains.

Compound

Composed of two or more substances chemically combined in a fixed proportion.

Element

Substance that cannot be changed into simpler substances by chemical means

Weight

The force of gravity on an object.

Kelvin Temperature Scale

The SI scale for temperature.

Sig Fig

Known or estimated in a measurement.

Absolute Zero

The lowest point on the Kelvin scale.

Celsius Temperature Scale

The non-SI scale for temperature

Accuracy

Closeness to a true value.

Precision

The narrowness of range of measurements.

Vapor

Gaseous state of a substance that is a liquid or solid at room temperature.

Product

A substance formed in a chemical reaction.

Phase

Part of a sample having uniform composition and properties.

Mixture

A physical blend of two or more components.

Reactant

Starting substance in a chemical reaction.

Heterogenous Mixture

Not uniform in composition.

Suspension

​a heterogeneous mixture that contains solid particles sufficiently large for sedimentation. Particles do not dissolve

Colloide

A homogeneous mixture that contains microscopic particles that do not dissolve

Pure substance

a sample of matter with both definite and constant composition with distinct chemical properties. To avoid confusion, in chemistry a pure substance is often referred to as a "chemical substance".

Chemical properties

can be observed when chemical reaction, CHANGES the composition of the substance

Physical Properties

Does not have to change the substance, does not change the composition

Physical Changes

Crushing a can, Melting an ice cube, Boiling water, Mixing sand and water, Breaking a glass, Dissolving sugar and water, Shredding paper, Chopping wood.

Chemical symbol

(P(+) + E(-)= top number; bottom number=P(+)

Mass number

P(+)+N(0) P=E )

Average atomic mass

(mass x % (in decima) + (mass x %)= amu (may be more naturally occurring masses, add those)

Finding % from mass

(x)(m1) + (1-x)(m2)= % (may or may not have to know that- Hallstrom)

Nucleus

The central part of an atom, containing protons and neutrons

Neutron

A subatomic particle with no charge. Mass number - protons.

Proton

A positively charged subatomic particle. Same as atomic number.

Electron

A negatively charged subatomic particle. Same as number of protons in a neutral atom.

Atom

The smallest particle of an element that retains the properties of that element.

Mass number​

The total number of protons and neutrons in the nucleus of an atom.

Atomic mass

The weighted average of the masses of the isotopes of an element.

Atomic mass unit

One-twelfth the mass of a carbon atom having six protons and six neutrons

Atomic number

The number of protons in the nucleus of an element.

Isotopes

atoms with the same number of protons, but different numbers of neutrons in

the nucleus of an atom.

Isotope Notation​

Look at the periodic table (the one with the negative and the positive, whether they lost or gained electrons and how many)

Photoelectric Effect​

emission of electrons from the surface of a metal in response to incident light. Proved that light was a PARTICLEs called photons. What einstein won the nobel prize for. Light bounced off/ emitted as photons.

Electron Configuration​

1s2​ ​ 2s2​ ​2p​6​ etc...

Quantum Numbers​

​n =​ energy levels, m ​= orbital, I =​ s u b l e v e l, ​S =​ spin (+1⁄2 (right) -1⁄2 (left))

Quantum Leaps​

an abrupt transition of an electron, atom, or molecule from one quantum state to another, with the absorption or emission of a quantum.

Reason that electrons must be apart of of the atoms in elements

Charge-to-mass ratio of electrons was the same, regardless of the gas used

Mass of n=

mass of p+