UNIT 1: ATOMIC STRUCTURE & PROPERTIES

Electronegativity

Electronegativity

how strongly the nucleus of an atom attracts the electrons of other atoms in a bond.

Hunds Rule

when an electron is added to a subshell, it will always occupy an empty orbital if one is available.

important information

The periodic table gives you basic but ________ about each element.

Subshells

________- a subdivision of electron shells separated by orbitals (s, p, d, & f)

Orbital

________- the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment.

Energy Level

________- fixed distances from the nucleus of an atom where electrons may be found (1- 7)

Isotopes

Atoms of an element with different number of neutrons.

Molarity

(M)- moles of solute /liters of solution.

Aufbau Principle

when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy.

Electron Affinity

the energy change that occurs when an electron is added to an atom in its gaseous state.

Pauli Exclusion Principle

two electrons which share an orbital can not have the same spin.

Electrostatic Force

the attraction between opposite charges.

Symbol

The unique symbol that represents an element on the periodic table.

Ionization Energy

the energy required to remove an electron from an atom.

Mass Number

The sum of an atoms protons and neutrons.

Valence Electrons

the electrons in the outermost s and p subshells.

Avogadros Number

The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)

Atomic Radius

the approximate distance from the nucleus of an atom to its valence electrons.

Empirical Formula

The simplest ratio of one element to another in a compound.

Symbol

The unique symbol that represents an element on the periodic table

Atomic Number

The number of protons located within the nucleus of an element

Molar Mass

The average atomic mass of an atom and also the average mass per mol of the atom

Periods

the horizontal rows of the periodic table

Groups

the vertical columns of the periodic table

The two rows offset beneath the table are alternatively called the Lanthanides (4f) and the Actinides (5f)

Rare Earth Metals or Inner Transition Metals

Mass Number

The sum of an atoms protons and neutrons

Isotopes

Atoms of an element with different number of neutrons

Avogadros Number

The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)

Molarity(M)

moles of solute/liters of solution

Empirical Formula

The simplest ratio of one element to another in a compound

Molecular Formula

The actual formula for a substance

Electrostatic Force

the attraction between opposite charges

Coulombs Law

Force of attraction = q1q2/r^2

Energy Level

fixed distances from the nucleus of an atom where electrons may be found (1-7)

Subshells

a subdivision of electron shells separated by orbitals (s, p, d, & f)

Orbital

the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment

Electron Configuration

the complete description of the energy level and subshell that each electron on an element inhabits

Aufbau Principle

when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy

Pauli Exclusion Principle

two electrons which share an orbital cannot have the same spin

Hunds Rule

when an electron is added to a subshell, it will always occupy an empty orbital if one is available

Valence Electrons

the electrons in the outermost s and p subshells

Atomic Radius

the approximate distance from the nucleus of an atom to its valence electrons

Ionization Energy

the energy required to remove an electron from an atom

Electronegativity

how strongly the nucleus of an atom attracts the electrons of other atoms in a bond

Electron Affinity

the energy change that occurs when an electron is added to an atom in its gaseous state

Effective Nuclear Charge

The net attractive force of the nucleus on the valence electrons (approximately equal to the number of protons - core electrons)