[ 1MID ] CHEMISTRY

Atom

smallest unit of matter that retains the identity and properties of an element

Molecule

a group of two or more atoms that are chemically bonded

0.0005

The atomic mass of an electron

1

The atomic mass of a proton

1

The atomic mass of a neutron

-1

Charge of an electron

+1

Charge of a proton

0

Charge of a neutron

Isotopic Symbol

allows for the mass number, atomic number, and charge to be easily known.

Mass Number

the total number of protons and neutrons (together known as nucleons) in an atomic nucleus.

Atomic Number

the charge number of an atomic nucleus. This is equal to the proton number (np) or the number of protons found in the nucleus of every atom of that element.

The number of protons tells the identity of the element and the arrangement of the elements in the periodic table.

Ion

is formed when an atom gains or loses electrons.

Cation

positively charged, formed when a metal loses electrons.

Anion

negatively charged, formed when a nonmetal gains electrons.

Isotopes

atoms of the same element with different mass numbers

Monatomic

only one atom

Polyatomic

multiple atoms

Nucleons

The name for the protons and neutrons together

Identity

What does the proton tell about the element?

Hydrated Salts

Some ionic compounds with water molecules incorporated in their structure

Arrhenius Acid

Substance that yields H⁺ in aqueous solution

Arrhenius Base

a compound that increases the OH⁻ ion concentration in aqueous solution.

Covalent Compounds

combination of two or more NONMETALS covalently bonded (involves sharing of electrons)

Law of Conservation of Mass

This states that in an (ordinary) chemical reaction, the mass of the substances produced is equal to the mass of the substances reacted.

Antoine Lavoisier

He is known as the father of modern chemistry.

Law of Definite Proportions

This states that any sample of a given compound will always be composed of the same elements in the same proportion by mass.

Nitrous Oxide

This is known as the laughing gas

Law of Multiple Proportions

This states that for elements that can form different compounds, the masses of the second element that can combine with a fixed mass of the first element are in a ratio of small whole numbers

John Dalton

He published a book called “A New System of Chemical Philosophy” where he proposed an atomic theory of matter that can explain chemical observations as predicted by the three fundamental laws.

Joseph John Thomson

He discovered the electron while studying the nature of cathode rays.

Cathode Ray Tube

a vacuum tube containing one or more electron guns, which emit electron beams that are manipulated to display images on a phosphorescent screen.

Ernest Rutherford

He performed the gold foil experiment and observed that some alpha rays were deflected at a regular pattern, some bounced back to the alpha particle source, and other passed through the foil. He then concluded that the atom has a very tiny positive nucleus at its center, an idea that led to the emergence of the nuclear model of an atom.

He discovered the proton.

James Chadwick

A former student of Rutherford, discovered the other type of particle in the nucleus—the neutron.

Ionic Compounds

Results from an attraction between a cation and an anion.

Gold Foil Experiment

What did Rutherford perform that led to his discovery of the proton.

John Dalton

He made the Solid Sphere model

J.J. Thomson

He made the Plum Pudding model

Ernest Rutherford

He made the Nuclear Model

Niels Bohr

He made the Planetary Model

Erwin Schrodinger

He made the Quantum Model

Solid Sphere Model

an atomic model proposed by John Dalton in 1803. It states that all objects are made of particles called atoms and that they are solid spheres that cannot be divided further into smaller particles. This is similar to the model made by the Greeks in the fifth century BCE.

Plum Pudding Model

the first scientific model of the atom to describe an internal structure. It was first proposed by J. J. Thomson in 1904 following his discovery of the electron in 1897, and was rendered obsolete by Ernest Rutherford's discovery of the atomic nucleus in 1911.

Nuclear Model

refers to a theoretical framework used in nuclear physics to describe the structure and behavior of atomic nuclei. It is based on the understanding obtained from studying nuclei near the β-stability line, incorporating concepts such as magic numbers and nuclear matter incompressibility.

Planetary Model

electrons are arranged in concentric circular orbits around the nucleus. This model is patterned on the solar system and is known as the _________

Quantum Model

describes the probability of finding electrons within given orbitals, or three-dimensional regions of space, within an atom. The properties of each electron within the quantum atom can be described using a set of four quantum numbers.

Solid Sphere Model

Plum Pudding Model

Nuclear Model

Planetary Model

Quantum Model