Chapter 2: Atoms, Molecules, and Ions

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40 Terms

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Atom

Mostly empty space and consist of subatomic particles.

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Proton

Subatomic particle with a positive charge found in the nucleus of an atom.

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Neutron

Subatomic particle with a neutral charge found in the nucleus of an atom.

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Electron

Subatomic particle with a negative charge that orbits the nucleus of an atom.

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Atomic Number

The number of protons in the nucleus of an atom, also indicating the number of electrons.

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Isotope

Atoms of the same element with different masses due to varying numbers of neutrons.

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Atomic Mass Unit (amu)

Unit used to express the mass of atoms on an atomic scale;

1 amu = 1.66054 × 1024- g

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Atomic Weight

An average mass is found using all isotopes of an element weighted by their relative abundances.

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Atomic Weight Formula

\sum [(isotope mass)x(fractional natural abundance)] for ALL isotopes.

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Periodic Table

Systematic arrangement of elements based on atomic number.

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Periods

The horizontal rows that represent the number of electron shells an element's atoms have; there 7 rows in the periodic table.

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Groups

The columns that contain elements with similar chemical properties due to the same number of electrons in their outer shell.

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Group 1A

Contains Alkali metals.

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Group 2A

Contains Alkaline earth metals.

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Sections 3-12

The transition metals of the periodic table.

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Group 6A

Contains Chalcogens.

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Group 7A

Contains Halogens.

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Group 8A

Contains Noble gases.

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Metals

Located on the left side of the periodic table; properties include shiny luster, conducting heat and electricity, and solid (except Hg).

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Nonmetals

Elements on the right side of the periodic table that lack metallic properties; mostly gases, but can be solid or liquid.

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Metalloids

Elements with properties intermediate between metals and nonmetals, located along a "stair step" on the periodic table.

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Molecular Compounds

Formed by sharing electrons between atoms to create covalent bonds; consist of molecules made up of nonmetals.

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Ionic Compound

Compound formed by the attraction between oppositely charged ions, typically between a metal and a nonmetal.

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Diatomic Molecules

Molecules composed of two atoms chemically bonded together; examples include Hydrogen (H2), Oxygen (O2), Nitrogen (N2), and Chlorine (Cl2).

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Empirical Formulas

Show the simplest whole-number ratio of atoms in a compound.

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Molecular Formulas

Shows the exact number of atoms of each element in a compound.

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Ion

A charged atom.

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Cation

Formed when at least one electron is lost.

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Anion

Formed when at least one electron is gained.

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Polyatomic ions

Many atoms grouped together.M

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Mono-

1

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Di-

2

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Tri-

3

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Tetra-

4

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Penta-

5

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Hexa-

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Hepta-

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Octa-

8

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Nona-

9

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Deca-

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