Atomic Theory Test

Protons

Positively charged particles in the nucleus of the atom, determine atom

Neutrons

Particles in the atom, or subatomic particles, have no charge, determine isotope

Electrons

Subatomic particles that have a negative charge, determine charge and chemistry

Atom

Smallest part of an a element that still retains all the properties of that element

Orbiting the nucleus

Where are electrons found in the atom?

All the protons and neutrons

What does the mass number of an isotope indicate?

Atomic number

Number from the periodic table gives you the number of protons in an atom

Indivisible

What does the Greek word “atomos” mean?

Mass number

The upper left hand corner of the isotope symbol

Atomic number

The lower left hand corner of the isotope symbol

Charge

The upper right hand corner of the isotope symbol

Number of ions

The lower right hand corner of the isotope symbol

Mass number

The number 56 in Manganese-56

Aristotle

First came up with the idea of elements

Democratis

Proposed that matter is made up of tiny little indivisible particles

Thompson

Model of the atom that had negative charges stuck into a solid sphere like a plum pudding, or chocolate chip cookie

Dalton

Model of the atom that was a simple, indivisible sphere

Rutherford

Proved the atom had a solid, dense core where most of the mass is concentrated and discovered protons

Lavoisier

Credited with establishing mass conservation in chemical reaction

Rutherford

Established that atoms are mainly empty space using gold foil experiment

atomic mass unit (amu)

Weight measurement for atoms

Grams (g)

Weight measurement for moles

Avagadro’s number

6.02 x 10^23

Average Atomic Mass Formula

(mass x % abundance) + (mass x % abundance)

Anion

a negatively charged ion

cation

a positively charged ion

Dalton’s atomic theory

all matter is made of atoms

Chemical Symbol

one or two letter designation of an element

ion

a particle that is electrically charged; an atom or molecule or group that has lost or gained one or more electrons

Isotopes

each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties

Law of Definite Proportions

Molecules of the same compound contain the same elements in the same ratios

law of multiple proportions

law stating that when two elements can combine to form more than one compound the amounts of one of them that combines with a fixed amount of the other will exhibit a simple multiple relation

nucleus

positively charged central core of an atom, consisting of protons and neutrons and containing nearly all its mass