Untitled Quiz

The amount of electric charge carried by one mole of electrons. It's a fundamental constant in electrochemistry and is used to relate the amount of charge to the number of electrons transferred in a chemical reaction.

A stream of electrons emitted from the cathode of a discharge tube. These rays travel in straight lines and can be deflected by electric and magnetic fields.

An experimental setup demonstrating the existence of cathode rays by studying their behaviour in a low-pressure gas discharge tube. This led to the discovery of electrons.

The property of cathode rays travelling in straight lines. This was proven by the shadow cast by objects placed in their path.

A subatomic particle with a negative charge, responsible for carrying electric current. It's a fundamental building block of matter.

An experiment that measured the charge-to-mass ratio (e/m) of electrons. This provided key evidence for the existence of electrons and their properties.

The ratio of the electric charge of an electron to its mass, a fundamental property of electrons. It was determined through J.J. Thomson's experiment.

Electrodes with holes that create a narrow beam of electrons by guiding them through specific paths.

The change in direction of electrons when they pass through an electric or magnetic field. This deflection occurs because the electric field exerts a force on the charged particles.

A region of space where an electric force would be exerted on a charged particle. The strength and direction of the field depend on the distribution of charges.

A region of space where a magnetic force would be exerted on a charged particle in motion. The strength and direction of the magnetic field depend on the distribution of magnetic poles.

An experiment conducted by Robert Millikan in 1909 to measure the charge of a single electron. He suspended tiny oil drops in an electric field and observed their motion to determine the charge.

J.J. Thomson's discovery of the electron's independence from the material used in the experiment suggested that electrons are a fundamental component of all atoms.

Millikan's experiment measured the charge of individual oil drops, finding that all drops had charges that were multiples of 1.6x10^-19 Coulombs, which is the charge of a single electron.

By measuring the charge of individual oil drops, Millikan confirmed that the charge of a single electron is a fundamental unit of charge, which is 1.6 x 10^-19 Coulombs.

Goldstein discovered evidence for the existence of positively charged particles, later called protons, by observing canal rays traveling in the opposite direction of cathode rays in a cathode-ray tube with a perforated cathode.

Rutherford's experiment, conducted by Geiger and Marsden, led to the development of the nuclear model of the atom, which proposes that the atom has a small, dense, positively charged nucleus at its center, surrounded by negatively charged electrons.

Canal rays are positively charged particles that travel in the opposite direction of cathode rays in a cathode-ray tube with a perforated cathode.

The experiment showed that most alpha particles passed through the gold foil, while some were deflected at large angles, suggesting that the positive charge and mass of the atom are concentrated in a small, dense nucleus, while the electrons orbit around it.

The nucleus is the small, dense, positively charged center of an atom, containing most of the atom's mass. It is composed of protons and neutrons.

Nucleons are the particles that make up the nucleus of an atom. They are protons and neutrons.

An experiment where alpha particles were bombarded at thin gold foil. Most passed straight through, but some were deflected at large angles, even backward. This led to the discovery of the atomic nucleus.

The positively charged center of an atom, containing nearly all its mass and composed of protons and neutrons.

A subatomic particle found in the nucleus of an atom, carrying a positive charge and a mass about 1838 times greater than an electron.

A subatomic particle found in the nucleus of an atom, carrying no charge (neutral) and having a mass approximately equal to a proton.

A positively charged particle consisting of two protons and two neutrons, emitted during radioactive decay.

The nucleus is incredibly small compared to the overall size of an atom, with the nucleus occupying only a tiny portion of the atom's volume.

An experiment using alpha particles to bombard beryllium, leading to the discovery of neutrons, neutral particles with a mass similar to protons.

Neutrons are neutral particles found in the nucleus of an atom. They have a mass approximately equal to a proton and are not affected by electric or magnetic fields.

The weighted average of the molar masses of all naturally occurring isotopes of an element, taking into account their relative abundances.

The difference between the mass of a nucleus and the sum of the masses of its constituent protons and neutrons.

The energy released when protons and neutrons come together to form a nucleus. It's the energy that holds the nucleus together.

The relationship between mass and energy, stating that energy (∆E) can be converted into mass (∆m) and vice versa, with a conversion factor of the speed of light squared (c²).

A unit of energy commonly used in nuclear physics, equal to the amount of energy gained by an electron when it moves across an electric potential difference of 1 volt.

A neutral subatomic particle found in the nucleus of an atom. It has a mass slightly greater than a proton and contributes to the atom's mass but not its charge.

A neutron's mass is about 1.6747 x 10^-27 kg, which is significantly higher than the mass of an electron.

The number of protons in an atom's nucleus. It determines the element's chemical identity and is equal to the number of electrons in a neutral atom.

The total number of protons and neutrons present in an atom's nucleus. It represents the atom's total mass, excluding the mass of electrons.

Atoms of the same element having the same atomic number (same number of protons) but different mass numbers (different number of neutrons).

The percentage of atoms of each isotope present in a naturally occurring sample of an element. It reflects the proportion of each isotope found in nature.

Isotopes can be separated by mass spectrometry, a technique that separates atoms based on their mass-to-charge ratio.