Unit 1: Atomic Structure and Properties

Anions

Anions

________ are larger than atoms because the atom has an overall negative charge, increasing the amount of electron- electron repulsions.

photoelectron spectrum

A(n) ________ (PES) is a graph of the ionization energies for all electrons when ejected from the nucleus.

Electrons

________ have significantly less mass than protons and neutrons and do not contribute to the mass.

Electronegativity

________ is how much an elements nucleus attracts electrons.

Isotopes

________ are atoms of an element with different numbers of neutrons, but same amount of protons.

Molarity

________ (M) expresses the concentration of a solution in terms of volume.

Percent composition

________ is the percent by mass of each element in a compound.

Aufbau principle

________ says electrons must fill up orbitals, subshells, and shells in order of increasing energy.

electromagnetic radiation

When electrons absorb ________, a form of energy, the electrons can jump to higher energy levels.

Bohr model

The ________ serves the purpose of understanding atomic structure rather than structural accuracy.

Avogadros Number

________ is the number of atoms in a single mole of any given element.

electrostatic force

The ________ is the attraction between opposite charges and the strength can vary depending on now for the charges are from each other.

subshell

A(n) ________ is the shape of the space an electron can be found in.

ionization energy

Once a shell is empty, the ________ greatly increases because it is closer to the nucleus.

mass spectrometry

determines the average mass for different isotopes of a specific element

Coulomb’s Law

the closer an electron is to the nucleus, the stronger the attraction and the less potential energy there is.

Pauli Exclusion Principle

________ states that when two electrons fill up an orbital, they must spin in opposite directions: clockwise and counterclockwise.

Hund’s Rule

________ states that when electrons are filling the orbitals of the subshell, they will only have two in one orbital when it is not possible to have each electron in its own orbital.

valence electrons

electrons in the outermost shell of an element

cation

an ion that is positively charged after giving up an electron