Physics Chapter 2: Atomic Structure Quiz

The positively charged particle found in the nucleus of an atom.

The neutral particle found in the nucleus of an atom.

The negatively charged particle that orbits the nucleus of an atom.

The number of protons in the nucleus of an atom.

The total number of protons and neutrons in the nucleus of an atom.

Atoms of the same element with the same number of protons but different numbers of neutrons.

Atoms with the same mass number but different atomic numbers.

Atoms with the same number of neutrons but different atomic numbers.

The speed of a wave is determined by the type of wave and the medium it travels through. It is calculated by multiplying the wavelength and frequency.

The emission spectrum of hydrogen includes a wide range of wavelengths that span from the infrared to the ultraviolet regions.

The Balmer series is a set of spectral lines in the hydrogen emission spectrum which fall in the visible region of the electromagnetic spectrum.

The speed of light in a vacuum is a constant, approximately 3 x 10^8 meters per second.

The electromagnetic spectrum encompasses a wide range of frequencies, including visible light, radio waves, and X-rays.

The energy level of an electron in a hydrogen atom is quantized, meaning the electron can only occupy specific energy levels.

The higher the energy level an electron drops from, the higher the energy of the emitted photon.

A continuous spectrum displays all wavelengths of visible light, resulting in a smooth gradient of colors.

Max Planck proposed that energy, like matter, is not continuous but exists in discrete quantities called quanta.

The Bohr model successfully explains the atomic spectra of hydrogen and other species with a single electron, like He+ and Li2+.

Each quantum represents a specific amount of energy that can be emitted or absorbed by atoms and molecules.

The Bohr model fails to explain the further splitting of spectral lines in hydrogen spectra when a magnetic field is applied.

According to Heisenberg's uncertainty principle, it is impossible to know both the precise location and momentum of an electron simultaneously. The Bohr model assumes both a fixed radius and orbit, contradicting this principle.

The energy of a quantum is directly proportional to the frequency of the electromagnetic radiation.

The formula c = vλ (where c is the speed of light, v is the frequency, and λ is the wavelength) can be rearranged to calculate wavelength, frequency, or speed of light if the other two values are known.

The Lyman series is a set of spectral lines in the hydrogen emission spectrum which fall in the ultraviolet region of the electromagnetic spectrum.

A law stating that when two elements form a series of compounds, the ratios of the masses of the second element that combine with a fixed mass of the first element can be expressed as small whole numbers.

A tiny, massive, positively charged core of an atom, containing protons and neutrons.

A wave that has both electric and magnetic components. It can be described by its wavelength (λ), frequency (ν), and speed (c).

A stream of tiny particles, called photons, each carrying a quantized amount (hν) of energy. The energy of a photon is directly proportional to its frequency (ν).

The emission of electrons from a metal surface when light of a certain minimum frequency strikes it. The strength of the emitted electron current increases with increasing light intensity.

The number that represents the electron's energy level within an atom. It can be any positive integer.

The number that describes the shape of an electron's orbital. It's a whole number that ranges from 0 to n-1.

The number that defines the specific orientation of an atomic orbital in space relative to other orbitals. It can take on values from -ℓ to +ℓ, including 0. The number of possible mℓ values for a given ℓ value is 2ℓ + 1.

The number that describes an electron's intrinsic spin. It can be either +½ or -½.

The set of quantum numbers that describes an electron's state in an atom. They are n, ℓ, mℓ, and ms.

A combination of n and ℓ that represents a group of orbitals with the same energy level and shape. They have the format nℓ, e.g. 3p.

A set of orbitals with the same principal quantum number, n.

The maximum number of electrons that can occupy a given shell is given by 2n2, where n is the principal quantum number.

The periodic law states that the chemical properties of elements repeat periodically when arranged in order of increasing atomic number. This means that elements with similar properties are grouped together in the periodic table.

A group in the periodic table is a vertical column of elements that have similar chemical properties due to having the same number of valence electrons, which are the electrons in the outermost shell.

Each row in the periodic table is called a period. Elements within the same period have the same number of electron shells, meaning the outermost electrons have the same principal quantum number.

Representative elements (main group elements) are the elements found in the first two columns (s-block) and the last six columns (p-block) of the periodic table. They exhibit a wide range of chemical properties and are essential to life and industry.

Transition elements, also known as transition metals, are located in the d-block of the periodic table. They are known for their ability to form colored compounds, exhibit multiple oxidation states, and have varying magnetic properties.

Inner transition elements, also known as inner transition metals, are the lanthanides and actinides, located in the f-block of the periodic table. They are characterized by their distinct electronic configuration and are primarily found in radioactive materials.

Atomic radius is a measure of the size of an atom. Generally, atomic radius decreases across a period from left to right and increases down a group. This is due to the increasing nuclear charge and the number of electron shells, respectively.

Ionization energy is the minimum amount of energy required to remove an electron from a gaseous atom in its ground state. Ionization energy generally increases across a period because of the increased nuclear charge and decreases down a group due to the increasing distance between the nucleus and the outermost electron.