Atomic Structure Quiz

Thomson's model of the atom compared the atom to a watermelon, with the positively charged sphere being the red edible part and electrons being the black seeds embedded within.

A positively charged sphere with electrons embedded within, similar to a plum pudding with plums embedded.

The atom consists of a sphere with a positive charge, and electrons are embedded within.

The total positive and negative charges within an atom are equal, making the atom electrically neutral.

Rutherford's experiment involved shooting alpha particles at a thin gold foil and observing their behavior.

Alpha particles are doubly charged helium ions, with a mass of 4u, that are fast-moving and carry significant energy.

Most alpha particles passed straight through the gold foil, suggesting atoms are mostly empty space.

Some alpha particles were deflected at small angles, indicating a small, dense, positively charged center within the atom.

Dalton's atomic theory proposed that matter is made of tiny, indivisible particles called atoms, which form the foundation of modern chemistry. However, later discoveries of subatomic particles like electrons, protons, and neutrons led to modifications of this theory.

J.J. Thomson discovered electrons by conducting the cathode ray experiment. Using a cathode ray tube, he observed a beam of negatively charged particles, proving that atoms can be further divided into smaller components.

E. Goldstein discovered protons through his anode rays/canal rays experiment, finding that atoms also contain positively charged particles.

James Chadwick discovered neutrons by bombarding light elements with alpha particles. He found a neutral particle with a mass similar to a proton. Since they have no charge, they are essential for the atom's mass.

Thomson's atomic model depicts the atom as a positively charged sphere with negatively charged electrons embedded within, like plums in a pudding. This model was later superseded by Rutherford's model.

Rutherford's atomic model suggests a dense, positively charged nucleus at the center of the atom, surrounded by negatively charged electrons orbiting in specific paths. This model revolutionized our understanding of the atom's structure.

Bohr's atomic model describes electrons orbiting the nucleus in specific energy levels, called shells. Electrons can jump between these levels by absorbing or releasing energy, explaining the atom's spectral emission.

The atomic number of an element represents the number of protons in its nucleus, defining its chemical identity. It is unique to each element and determines the element's position in the periodic table.

The positively charged central core of an atom, containing protons and neutrons. Almost all of the atom's mass is concentrated in the nucleus.

Rutherford proposed that electrons orbit the nucleus in specific paths, like planets around the sun. However, this model had a significant drawback.

According to classical physics, orbiting electrons would lose energy and spiral into the nucleus, causing the atom to collapse. This contradicted observations.

Niels Bohr's model addressed the shortcomings of Rutherford's model by introducing the concept of quantized energy levels for electrons. Electrons can only occupy specific orbits.

Bohr's model proposed that electrons can jump between energy levels by absorbing or releasing energy. Jumping to a higher level requires energy absorption, while jumping to a lower level releases energy.

The atomic number represents the number of protons in the nucleus of an atom. It defines the element's identity, as changing the atomic number changes the element.

Atoms are electrically neutral because the number of protons (positive charge) equals the number of electrons (negative charge).

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

Atoms with the same atomic number but different mass numbers. They have the same number of protons but a different number of neutrons.

The average atomic mass of an element, taking into account the relative abundance of its isotopes.

The number of electrons an atom gains or loses to achieve a stable electron configuration.

The arrangement of electrons in different energy levels around the nucleus of an atom.

The outermost energy level of an atom.

Elements with a filled valence shell, making them very stable and unreactive.

Atoms of different elements that have the same mass number but different atomic numbers. They have the same number of nucleons (protons + neutrons) but different numbers of protons, resulting in different chemical properties.

The atomic number of an element is equal to the number of protons in its nucleus. It determines the element's chemical identity and its position in the periodic table.

Isotopes are atoms of the same element that have the same number of protons (same atomic number) but different numbers of neutrons. This leads to variation in their mass number and some physical properties.

The valency of an element is its combining capacity, determined by the number of electrons it can gain, lose, or share to achieve a stable electronic configuration. It's influenced by the number of valence electrons in the outermost shell.

Rutherford's alpha particle scattering experiment established that atoms have a dense, positively charged nucleus at the center, surrounded by largely empty space where negatively charged electrons orbit. This model revolutionized our understanding of atomic structure.

The distribution of electrons in different energy levels (shells) of an atom, based on the formula 2n² where 'n' represents the shell number. This formula determines the maximum number of electrons that can occupy a particular shell.

The outermost shell of an atom can't hold more than 8 electrons, and the second-to-last shell can't hold more than 18, even if their capacity allows for more. This limitation applies even if the inner shells are not completely filled.

The outermost shell can't have more than 2 electrons, and the penultimate shell can't have more than 8 electrons, unless the preceding inner shell (antepenultimate) is completely filled with its maximum capacity according to the '2n²' formula.

Electrons present in the outermost shell of an atom. These electrons are involved in chemical bonding and determine the atom's reactivity.

Atoms strive to have 8 electrons in their outermost shell to achieve a stable configuration, similar to noble gases. This can be accomplished by gaining, losing, or sharing electrons.

The tendency of atoms with incomplete outermost shells to combine with other atoms through sharing, losing, or gaining electrons to achieve a stable, noble gas electronic configuration.

A special case for elements like hydrogen, helium, lithium, beryllium, and boron, where they strive for 2 electrons in their outermost shell for stability. Their valency adjusts accordingly.