study guide chem unit 3 notes

The state where an electron has the lowest possible energy level within an atom.

When an electron absorbs energy and jumps to a higher energy level.

The arrangement of electrons in different energy levels within an atom.

The ability of an atom to attract electrons in a chemical bond.

A chemical bond formed by sharing electrons between atoms.

A chemical bond formed by the transfer of electrons from one atom to another.

An atom or molecule with a positive charge.

An atom or molecule with a negative charge.

The smallest unit of electromagnetic radiation, carrying a specific amount of energy. Think of it as a tiny packet of light.

The distance between the nucleus of an atom and its outermost electron.

The energy required to remove an electron from an atom in its gaseous state. The more loosely held the electron, the easier it is to remove.

Electrons can behave as both waves and particles. Their wave nature is explained by their ability to diffract and interfere like waves, while their particle nature is shown by the quantization of energy, a characteristic of particles.

The electromagnetic spectrum encompasses various forms of radiant energy, differentiated by their wavelength, frequency, and energy levels. As wavelength increases, frequency decreases, and energy also decreases.

Bohr's model is a simple model that portrays electrons orbiting the nucleus in specific energy levels. The quantum model, however, is more accurate, depicting electrons as existing in orbitals, regions of space where there's a high probability of finding an electron.

The first three electron shells (K, L, and M) have specific orbitals (s, p, and d) that can hold a maximum number of electrons. The K shell can hold 2, L can hold 8, and M can hold 18 electrons. These numbers are based on the number of orbitals and the maximum number of electrons each orbital can hold.

Coulomb's Law explains the forces between charged particles, including electrons. It helps us understand how the attraction between the nucleus and electrons affects the periodic trends. The stronger the attraction, the more tightly held the electrons are, influencing properties like electronegativity.

Atomic radius refers to the distance from the nucleus to the outermost electron. It generally decreases across a period due to increasing effective nuclear charge, meaning the nucleus has a stronger pull on the electrons.

Electronegativity is an atom's ability to attract electrons in a bond. It increases across a period because of the stronger pull from the nucleus on shared electrons, making atoms more likely to gain electrons.