Chemistry Chapter 1 Quiz

The smallest unit of matter that retains the chemical properties of an element. It is a building block of all matter.

The central core of an atom, containing protons and neutrons.

Positively charged particles found in the nucleus of an atom.

Neutral particles found in the nucleus of an atom. They do not have an electric charge.

Negatively charged particles that orbit the nucleus of an atom.

An atom that has an equal number of protons and electrons, resulting in a neutral overall charge.

An atom that has lost or gained one or more electrons, becoming positively charged (cation) or negatively charged (anion).

The outermost shell of an atom where electrons are located. This shell is responsible for chemical bonding and reactivity.

A fundamental, indivisible unit of matter according to Democritus's theory. The term comes from the Greek word "atomos", meaning "indivisible".

The English chemist who proposed the atomic theory of matter. He believed that all matter is made of atoms and that atoms of the same element are identical.

A negative subatomic particle found outside the nucleus of an atom. It's much lighter than a proton or neutron.

Named for its resemblance to the British dessert, the plum pudding, Thomson's model depicts the atom as a positively charged sphere with negatively charged electrons embedded within. The negatively charged electrons were scattered throughout the atom.

A positive subatomic particle found in the nucleus of an atom. It has a mass of approximately 1 amu.

A neutral subatomic particle found in the nucleus of an atom, with a mass of approximately 1 amu. It contributes to the overall mass of the atom but doesn't carry a charge.

The central part of an atom containing protons and neutrons, which are tightly bound together.

The theory that matter is made up of tiny, indivisible particles called atoms. This theory was proposed by John Dalton and has been refined over time.

Thomson's model of the atom, where negatively charged electrons are embedded in a sphere of positively charged 'fluid', like plums in a pudding.

Rutherford's model of the atom, where a dense positive nucleus is surrounded by orbiting electrons, similar to a mini solar system.

The experiment conducted by Rutherford to test Thomson's model by firing alpha particles at a gold foil.

Bohr's model of the atom, where electrons orbit the nucleus in specific energy levels, resembling planets orbiting the sun.

The central core of an atom, containing protons and neutrons.

The arrangement of electrons around the nucleus of an atom based on their energy levels, where electrons occupy specific energy levels in a stepwise manner, moving to higher levels when absorbing energy and dropping to lower levels when releasing energy.

The region around the nucleus of an atom where an electron is most likely to be found.

The process where an electron transitions from a higher energy level to a lower energy level, releasing energy as a photon of light.

The model of the atom developed by Erwin Schrödinger, which describes electrons in terms of probabilities rather than fixed orbits. It uses mathematical equations to determine the likelihood of finding an electron in a specific region of space surrounding the nucleus.

The number of protons in an element's atom determines its identity.

The sum of protons and neutrons in an atom's nucleus, representing the atom's mass.

A shorthand notation used to represent information about an element, including its symbol, atomic number, mass number, and charge. It helps summarize important data about an element.

An atom that has gained or lost electrons, resulting in a net positive (cation) or negative (anion) charge.

Atoms with a net positive charge are called cations. Atoms with a net negative charge are called anions.

Atoms that have the same number of protons and electrons are electrically neutral.

Isotopes are variations of the same element that have the same atomic number (same number of protons) but different mass numbers. This means they have different numbers of neutrons.

The mass number of an isotope is the sum of its protons and neutrons. It reflects the total number of particles in the nucleus.

To determine the number of neutrons in an isotope, subtract the atomic number from the mass number.

Hydrogen has three isotopes: protium (hydrogen-1), deuterium (hydrogen-2), and tritium (hydrogen-3). They differ in their number of neutrons.

Carbon exists in three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. Carbon-14 is radioactive with a half-life of approximately 5,730 years.

While isotopes have the same number of protons and electrons, they differ in their number of neutrons. This affects their mass number and potentially their stability, with some isotopes being radioactive.