FUNCHEM.2 Electronic Configurations of Atoms and Ions of Physiological Importance

Flashcards covering electronic configurations of atoms and ions, fundamental atomic theories, and contributions to atomic structure.

Who made contributions leading to the discovery of the structure of the atom?

Thompson, Rutherford, Bohr, Einstein, deBroglie, Heisenberg, Schrodinger

What is an atomic orbital?

A region in space within an atom and around the nucleus where the probability of finding an electron is relatively high.

How do s, p, and d orbitals differ?

They differ in energy and shapes.

What are the three principles/rules for constructing electronic configurations?

Pauli Exclusion Principle, Aufbau Principle, and Hund's Rule of Maximum Multiplicity.

What are the four main points of Dalton's Atomic Theory?

Elements are composed of atoms; all atoms of a given element are identical; compounds are composed of atoms of more than one element in simple ratios; chemical reactions involve only the separation, combination, or rearrangement of atoms, not their creation or destruction.

Who discovered the electron and proposed the plum-pudding model?

J.J. Thomson

What was a key outcome of Rutherford's alpha-particle scattering experiment?

It led to the proposal of the nucleus, a dense central core where the atom's positive charges (protons) are concentrated.

What did Neils Bohr propose regarding electrons?

Electrons move in circular orbits around the nucleus, and these orbits have specific energies (energy levels).

What did Albert Einstein demonstrate about light?

Light, although a wave, could also have particle properties (Photoelectric Effect).

What is Wave-Particle Duality, as proposed by de Broglie?

It is the idea that matter (small particles), as well as light, might have wave properties, meaning electrons can also behave as waves.

What does Heisenberg's Uncertainty Principle state?

It is impossible to know simultaneously both the momentum and the position of a particle (such as an electron) with certainty.

What did Schrodinger develop with his wave equation?

Mathematical functions that refer to the probability of finding an electron within a particular position within an atom.

What is the shape of an s-orbital?

Sphere shaped.

How do different types of s-orbitals (e.g., 1s, 2s) compare?

Increasing number (e.g., 2s vs 1s) indicates increasing energy and distance from the nucleus.

What is the shape of a p-orbital?

Dumbbell shaped.

How do p-orbitals typically occur?

In sets of three (px, py, pz) with the same shape, same energy (degenerate), but different orientation.

How do d-orbitals typically occur?

In sets of five with their own unique shapes and the same energy (degenerate).

What is an energy sublevel?

A group of atomic orbitals within an atom, all of which have the same energy.

What is the maximum number of electrons that can occupy an s, p, and d sublevel respectively?

s: 2 electrons (1 orbital), p: 6 electrons (3 orbitals), d: 10 electrons (5 orbitals).

What does an electronic configuration describe?

How electrons are organized in an atom – how electrons are distributed among the atomic orbitals and sublevels.

What is the Pauli Exclusion Principle?

No more than 2 electrons can occupy an orbital, and these electrons must have opposite spin.

What is the Aufbau Principle?

Electrons fill the lowest available energy level first.

What is Hund's Rule of Maximum Multiplicity?

With orbitals of equal energy (e.g., px, py, pz), electrons fill the orbitals singly before filling in pairs.

In spd(f) notation, what does the prefix and superscript indicate?

The prefix (principal quantum number) designates the energy and size of the orbital, and the superscript indicates the number of electrons in that orbital.

What is the general order of filling atomic orbitals?

1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p

What is an outermost electron called?

A valence electron.

How is the abbreviated electronic configuration for Sodium (Na) written?

[Ne] 3s1

What is the general rule for filling 4s and 3d orbitals for transition metals?

The 4s orbital is filled before the 3d orbital (4s < 3d).

Why are Chromium (Cr) and Copper (Cu) exceptions to the typical electron filling rules?

There is extra stability associated with either a half-filled (Cr: 3d5 4s1) or completely filled (Cu: 3d10 4s1) d orbital.

What is an ion?

An atom or a group of atoms that has a net positive or negative charge.

How is a cation formed?

By the loss of one or more electrons from a neutral atom, resulting in a net positive charge.

How is an anion formed?

By an increase in the number of electrons in an atom, resulting in a net negative charge.

How is the Na+ ion formed from a neutral Sodium (Na) atom?

Na (1s2 2s2 2p6 3s1) loses one electron to become Na+ (1s2 2s2 2p6).

What is the electronic configuration for K+?

1s2 2s2 2p6 3s2 3p6