AP Chemistry Ultimate Review Packet Unit 1: Atomic Structure and Properties

Flashcards covering key vocabulary terms related to atomic structure and properties based on the provided lecture notes.

Atoms

Smallest unit of an element (substances on the periodic table)

Molecules

Contain two or more atoms that are chemically bound

Atoms

Smallest unit of an element (substances on the periodic table)

Molecules

Contain two or more atoms that are chemically bound

Pure Substances

Include elements and compounds

Mixtures

Contain two or more pure substances

Homogeneous Mixtures

Substances are dispersed evenly

Heterogeneous Mixtures

Substances are dispersed unevenly

Atomic Number

Number of protons (determines the element the atom belongs to)

Mass Number

Number of protons + number of neutrons

Isotopes

Atoms of a given element with differing numbers of neutrons

Atomic Mass

Average mass of an atom of that element, or the average of the mass numbers of its naturally occurring isotopes with respect to their relative abundance

Anion

Atoms with more electrons than protons have a negative charge

Cation

Atoms with fewer electrons than protons have a positive charge

Mass Spectrometry

Determines isotopic masses and abundances; sample is vaporized and ionized and sent through a tube with a magnetic field

Avogadro's Number

6.022 x 10^23

Empirical Formula

Lowest whole number ratio of elements in a compound.

Molecular Formula

Actual number of atoms of each element in a compound.

Principal Quantum Number (n)

Energy Level

Angular Momentum Quantum Number (l)

Type of Orbital

Magnetic Quantum Number (ml)

Individual orbital within subshell

Spin Quantum Number (ms)

+1/2 or -1/2

Aufbau Principle

Tells us the order in which orbitals are filled

Hund's Rule

Subshells are half-filled before doubling any orbital

Pauli Exclusion Principle

No two electrons within an atom can have precisely the same set of quantum numbers

Periods

Rows of the periodic table

Groups

Columns of the periodic table

Covalent Radius

Increases down and to the left

Ionization Energy

Increases up and to the right

Electron Affinity

Increases up and to the right

Electronegativity

Increases up and to the right; measure of how tightly an atom holds electron density