Unit 1 Chem Test

Ion

A negatively or positively charge atom

isotope

Atoms of the same element with different number of neutrons and mass numbers

Whats in the second row of the F block

actinides

Where are the halogens on the periodic table

7th group

Where are the noble gases

8th group

Ionization Energy

The amount o energy reached to remove the outermost electron from a species (atom or ion) in a gaseous state.

Electron Affinity

The energy released when an electron is added in the gas state.

Electronegativity

The ability of an atom to attract electrons when it is a compound

Isotope

Atoms of the same element with different neutrons

Isoelectronic

having the same number of electrons or valence electrons

Orbital

when an electron is likely to be found in an atom

Excited State

The valence electron has moved from its ground state orbital to a higher energy orbital

Ground State

state in which the electrons in a atom, ion, or molecule are in the lowest energy levels possible

Effective Nuclear Charge

Atomic Radius

Examples of Excited and Ground State Electron Configuration

Ground state for oxygen;

In a chemical compound the atom with the greater electronegativity…

more strongly attracts the bond’s electrons

Aufbau Principle

electrons occupy lowest orbitals first

Pauli Exclusion Principle

only two electrons can occupy an orbital at the same time

Pauli Exclusion Principle #2

To occupy the same orbital, two electrons must have opposite spins

Pauli Exclusion Principle #3

An orbital holds two electrons that spin in opposite directions

Hund Rule

When electron fills orbitals of the same energy level, they do so in a way that maximize the particles with the same spin

Hund Rule #2

Single electrons occupy available orbitals first before doubling up