Grade 8 - Pretest #3(3Q)

It is define as the distance between two successive crests or troughs of a wave. It is measured in the direction of the wave.

• Wavelength

• Amplitude

• Speed of light

• Frequency

It states that there are only certain allowed energy states for an electron and that these are quantized.

• Photoelectric effect

• Quantum theory

• Quanta

• Photons

It contains many different colors, or wavelengths, with no gaps.

• Atomic spectra

• Emission spectrum

• Continuous spectrum

• Line spectrum

It is a model of the atom where electrons travel in defined circular orbits around the nucleus.

• Rutherford's nuclear model of the atom

• Orbital model of the atom

• Plum-pudding model of the atom

• Bohr’s atomic theory

It refers to the fundamental property of matter where, at one moment it appears like a wave, and yet at another moment it acts like a particle.

• Duality of matter

• Uncertainty principle

• Aufbau principle

• Pauli's exclusion principle

They are values that is used when describing the energy levels available to atoms and molecules

• Quantum numbers

• Uncertainty principle

• Aufbau principle

• Pauli's exclusion principle

It is also called electronic structure, the arrangement of electrons in energy levels around an atomic nucleus.

• Electron configuration

• Orbital diagram

• Aufbau principle

• Pauli's exclusion principle

It implies that it is in general not possible to predict the value of a quantity with arbitrary certainty, even if all initial conditions.

• Electron configuration

• Uncertainty principle

• Aufbau principle

• Pauli's exclusion principle

It states that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers.

• Electron configuration

• Uncertainty principle

• Aufbau principle

• Pauli's exclusion principle

It is also also known as the fourth quantum number, is a number value that describes the orientation of an electron occupying an orbital. The symbol that we will use for the spin quantum number is ms.

• Electron configuration

• Uncertainty principle

• Spin quantum numbers

• Pauli's exclusion principle